Periodic Table, Chemical Bonds, Chemical Reactions

Periodic Table, Chemical Bonds, Chemical Reactions

The Periodic Table of the Elements

1H

Hydrogen1.00794

2HeHelium4.003

3Li

Lithium6.941

4Be

Beryllium9.012182

5B

Boron10.811

6C

Carbon12.0107

7N

Nitrogen14.00674

8O

Oxygen15.9994

9F

Fluorine18.9984032

10NeNeon

20.1797

11NaSodium

22.989770

12Mg

Magnesium24.3050

13Al

Aluminum26.981538

14Si

Silicon28.0855

15P

Phosphorus30.973761

16S

Sulfur32.066

17Cl

Chlorine35.4527

18ArArgon

39.948

19K

Potassium39.0983

20Ca

Calcium40.078

21Sc

Scandium44.955910

22Ti

Titanium47.867

23V

Vanadium50.9415

24Cr

Chromium51.9961

25Mn

Manganese54.938049

26FeIron

55.845

27CoCobalt

58.933200

28NiNickel

58.6934

29CuCopper

63.546

30Zn

Zinc65.39

31GaGallium69.723

32Ge

Germanium72.61

33AsArsenic

74.92160

34Se

Selenium78.96

35Br

Bromine79.904

36Kr

Krypton83.80

37Rb

Rubidium85.4678

38Sr

Strontium87.62

39Y

Yttrium88.90585

40Zr

Zirconium91.224

41Nb

Niobium92.90638

42Mo

Molybdenum95.94

43Tc

Technetium(98)

44Ru

Ruthenium101.07

45Rh

Rhodium102.90550

46Pd

Palladium106.42

47AgSilver

107.8682

48Cd

Cadmium112.411

49In

Indium114.818

50Sn

Tin118.710

51Sb

Antimony121.760

52Te

Tellurium127.60

53I

Iodine126.90447

54XeXenon

131.29

55CsCesium

132.90545

56BaBarium

137.327

57La

Lanthanum138.9055

72Hf

Hafnium178.49

73Ta

Tantalum180.9479

74W

Tungsten183.84

75Re

Rhenium186.207

76Os

Osmium190.23

77Ir

Iridium192.217

78Pt

Platinum195.078

79AuGold

196.96655

80HgMercury200.59

81Tl

Thallium204.3833

82PbLead

207.2

83Bi

Bismuth208.98038

84Po

Polonium(209)

85At

Astatine(210)

86RnRadon(222)

87Fr

Francium(223)

88RaRadium(226)

89Ac

Actinium(227)

104Rf

Rutherfordium(261)

105Db

Dubnium(262)

106Sg

Seaborgium(263)

107Bh

Bohrium(262)

108Hs

Hassium(265)

109Mt

Meitnerium(266)

110

(269)

111

(272)

112

(277)

113 114

58CeCerium

140.116

59Pr

Praseodymium140.90765

60Nd

Neodymium144.24

61Pm

Promethium(145)

62Sm

Samarium150.36

63Eu

Europium151.964

64Gd

Gadolinium157.25

65Tb

Terbium158.92534

66Dy

Dysprosium162.50

67Ho

Holmium164.93032

68ErErbium

167.26

69TmThulium

168.93421

70Yb

Ytterbium173.04

71Lu

Lutetium174.967

90Th

Thorium232.0381

91Pa

Protactinium231.03588

92U

Uranium238.0289

93Np

Neptunium(237)

94Pu

Plutonium(244)

95Am

Americium(243)

96CmCurium(247)

97Bk

Berkelium(247)

98Cf

Californium(251)

99Es

Einsteinium(252)

100FmFermium(257)

101Md

Mendelevium(258)

102No

Nobelium(259)

103Lr

Lawrencium(262)

1995 IUPAC masses and Approved Names from http://www.chem.qmw.ac.uk/iupac/AtWt/masses for 107-111 from C&EN, March 13, 1995, p. 35112 from http://www.gsi.de/z112e.html

2

SSR = Science Skills Reading WS LCL = Library Computer Lab WS = Worksheet CW/HW = ClassWork/HomeWork TB = Textbook

FPS: Rice/Sankovich/Rabatin December 2011 & January 2012

Sunday Monday Tuesday Wednesday Thursday Friday Saturday

27 28 Applications and problems associated with nuclear decay, fusion and fission

29 C 10 review

30 C10 test(10.1,10.2 & 10.4)

Dec 1 Flame Tests Li, Na, K demos variations/val e DUE: SSR 5.3 p4-5

2 PT coloring DUE: SSR 5.1&5.2 p8-11, PT coloring at end of period p14-15

3

4 5 Early Dismissal Element search 1&2-253, 4/5&10 LCL Due: p16-17 at end of period

6 c5 PT quiz Lewis dot diagrams

7 ionic bonds and properties DUE: lewis dot ws p21 & SSR 6.1 p22-23

8 chem. think- ionic and covlatent bonding LCL

9 covalent bonding and properties DUE: SSR 6.2 p30-31

10

11

FACEBOOK PROJECT!!!! *****************

12 bonding practice DUE: FACEBOOK PROJECT

13 ionic naming DUE: SSR 6.3 p36-37

14 covalent naming DUE: Ionic Naming p38-39

15 review DUE: chemthink p26-29 and covalent naming p 40-41

16 c6 Test

17 NO SCHOOL WINTER BREAK

Jan 1 2 NO SCHOOL WINTER BREAK

3 reaction demo day

4 reaction lab DUE: SSR 7.1 p44-45

5 chemthink : rxn LCL

6 balancing and rxn practice

7

8 9 acid and base lab

10 life and death of a star video DUE: Acid and base lab p54-55

11 review DUE: Chemthink p46-48, balancing equation ws p52

12 review Study Island 253B DUE: reference sheet p60-61

13 Exams 8:30-10:30 Social Studies 1-4 Math

14

15 16 No School MLK Day

17 Exams 8:30-10:30 English 1-4 Science

18 Exams 8:30-10:30 World Language

19 20 21

SSR = Science Skills Reading WS LCL = Library Computer Lab WS = Worksheet CW/HW = ClassWork/HomeWork TB = Textbook

Name ___________________________ Class ___________________ Date _____________

Chapter 5 The Periodic Table

Physical Science Reading and Study Workbook ! Chapter 5

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Section 5.3 Representative Groups (pages 139–145)This section discusses how the number of valence electrons affectsthe properties of elements. It also describes properties of elementsin Groups 1A through 8A.

Reading Strategy (page 139)

Monitoring Your Understanding As you read, record an importantfact about each element listed in the table. For more information onthis reading strategy, see the Reading and Study Skills in the Skillsand Reference Handbook at the end of your textbook.

Element Important Fact

Magnesium

Aluminum

Chlorine

Valence Electrons (page 139)

1. An electron that is in the highest occupied energy level of an atom isa(n) electron.

2. Elements within a group have the number ofvalence electrons.

The Alkali Metals (page 140)

3. The reactivity of alkali metals from the top ofGroup 1A to the bottom.

4. Sodium is stored under oil because it .

The Alkaline Earth Metals (page 141)

5. Differences in reactivity among alkaline earth metals are shown bythe way they react with .

Find and match two properties to each element listed.Alkaline Earth Metal Property

6. magnesium7. calcium

a. Helps build strong teeth and bonesb. Helps plants produce sugarc. Is used to make lightweight bicycle framesd. Is the main ingredient in limestone

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Name ___________________________ Class ___________________ Date _____________



© Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reser ved.

The Boron Family (page 142)

8. List the four metals in Group 3A. a. b.c. d.

9. Circle the letter of each sentence that is true about aluminum.a. It is the most abundant metal in Earth’s crust. b. It is often found combined with oxygen in bauxite. c. It is more reactive than sodium and magnesium. d. It is a good conductor of electric current.

The Carbon Family (page 142)

10. List the two metalloids in Group 4A. a. b.

11. Except for water, most of the compounds in your body contain.

The Nitrogen Family (page 143)

12. List the nonmetals in Group 5A. a. b.

13. Name two elements in the nitrogen family that are contained in fertilizer. a. b.

The Oxygen Family (page 143)

14. List the nonmetals in Group 6A. a. b. c.

15. Name the most abundant element in Earth’s crust.

The Halogens (page 144)

16. List the four nonmetals in Group 7A. a. b.c. d.

17. Halogens have similar properties butdifferent properties.

The Noble Gases (page 145)

18. Name three characteristics of noble gases.a. b. c.

19. How can an element that does not react easily with other elementsbe useful?

5

Alkali Metals Reactivity Demo/video

Class Notes________________

Define: Group/family

Period

Element Observations of reaction with water

Lithium

Sodium

Potassium

Cesium(video only)

Francium(video only)

Alkali metals are located where on the periodic table?

As you go down a group of element, the chemical reactivity ______________________________. Why?

Element Observations of flame tests

Lithium

Sodium

Potassium

6

7

Name ___________________________ Class ___________________ Date _____________



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Section 5.1 Organizing the Elements (pages 126–129)This section explains how Mendeleev organized elements into a periodic table.It also discusses the predictions he made about undiscovered elements and howthe discovery of those elements supported his version of the table of the table.


Identifying Main Ideas As you read, complete the table byidentifying the main idea for each topic. For more information on thisreading strategy, see the Reading and Study Skills in the Skills andReference Handbook at the end of your textbook.

Topic Main Idea

Mendeleev’s proposal

Mendeleev’s prediction

Evidence supportingMendeleev’s table

The Search for Order (page 126)

1. Is the following sentence true or false? The first elements to beidentified were mainly gases.

2. As the number of known elements grew, so did the need to organizethem into groups based on their .

3. Circle the letter of each category that the French chemist AntoineLavoisier used to classify elements.a. gases b. metalsc. liquids d. nonmetals

Mendeleev’s Periodic Table (pages 127–129)

4. Is the following sentence true or false? Mendeleev needed toorganize information about 63 elements.

5. Mendeleev’s strategy for classifying elements was modeled on a(n).

6. Circle the letter of each type of information Mendeleev knew abouteach element.a. nameb. number of protonsc. relative massd. properties

8

Name ___________________________ Class ___________________ Date _____________




7. Mendeleev arranged the elements into rows in order ofso that elements with similar properties

were in the same column.8. Is the following sentence true or false? A periodic table is an

arrangement of elements in columns, based on a set of propertiesthat repeat from row to row.

9. Mendeleev published the table above in 1872. Why did Mendeleev leave somelocations in his periodic table blank?

10. Circle the letters of two elements that have similar properties.a. zinc (Zn) b. chlorine (Cl)c. nitrogen (N) d. bromine (Br)

11. How did Mendeleev decide where to place arsenic (As) and selenium (Se)?

12. Is the following sentence true or false? Mendeleev was the firstscientist to arrange elements in a periodic table.

13. Describe a test for the correctness of a scientific model.

14. Mendeleev used the located near the spacesin his table to predict properties for undiscovered elements.

15. The close match between Mendeleev’s predictions and the actual properties of new elements showed .

16. Circle the letter of each element that was discovered after Mendeleevpublished his periodic table that supported Mendeleev’s predictionsand provided evidence validating the table.a. gallium b. scandiumc. germanium d. aluminum

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Name ___________________________ Class ___________________ Date _____________



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Section 5.2 The Modern Periodic Table(pages 130–138)This section explains the organization of the modern periodic table anddiscusses the general properties of metals, nonmetals, and metalloids.


Previewing Before you read, complete the table by writing twoquestions about the periodic table on pages 132–133. As you read,write answers to your questions. For more information on this readingstrategy, see the Reading and Study Skills in the Skills andReference Handbook at the end of your textbook.

Questions About the Periodic Table

Question Answer

The Periodic Law (pages 131–133)

1. Is the following sentence true or false? In the modern periodic table,elements are arranged by increasing number of protons.

2. Explain why the number of elements per period varies.

3. Properties of elements repeat in a predictable way when atomicnumbers are used to arrange elements into groups. This pattern ofrepeating properties is called the .

Atomic Mass (page 134)

4. Label the four types of information supplied for chlorine in the diagram.

a. b.c. d.

17

ClChlorine35.453

a.

b.

d.c.

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Name ___________________________ Class ___________________ Date _____________


50 Physical Science Reading and Study Workbook ! Chapter 5


5. Define atomic mass.

6. Circle the letter of each sentence that is true about a carbon-12atom.a. It has 6 protons and 6 neutrons.b. Scientists assigned a mass of 6 atomic mass units to the

carbon-12 atom.c. It is used as a standard for comparing the masses of atoms.d. An atomic mass unit is defined as one twelfth the mass of a

carbon-12 atom.7. Is the following sentence true or false? Most elements exist as a

mixture of two or more isotopes. 8. The mass of an atom of chlorine-37 is than

the mass of an atom of chlorine-35.9. Is the following sentence true or false? All values are equally

important in a weighted average.

Classes of Elements (pages 135–136)

10. Name the three categories into which elements are classified basedon their general properties.a.b.c.

11. Is the following sentence true or false? All metals react withoxygen in the same way.

12. An important property of transition elements is their ability toform compounds .

13. Circle the letter of each sentence that is true about nonmetals.a. Nonmetals are poor conductors of heat and electric current. b. Many nonmetals are gases at room temperature. c. Some nonmetals are extremely reactive and others hardly

react at all. d. Nonmetals that are solids tend to be malleable.

Variation Across a Period (page 138)

14. Across a period from left to right, the elements becomemetallic and

nonmetallic in their properties.15. Circle the letter of each Period 3 element that is highly reactive.

a. sodium b. siliconc. chlorine d. argon

11

Tour of the Periodic table

Foundation Physical Science Name ___________________________________________________Period____________

YOU WILL NEED YOUR TEXTBOOK & Colored pencils FOR THIS ACTIVITY!!!

1. Obtain the following colored pencils from the location described by

your teacher: Red, Blue, Green, Yellow, Orange, Purple, Pink,

Brown.

2. Define the term period as it applies to the periodic table on your data sheet. On the blank period table found on your data sheet, number the periods.

3. Define the term group as it applies to the periodic table on your data sheet. On the blank period table found on your data sheet, number the groups:1-18.

Color the Noble gases, RED;

the alkali metals, BLUE; the alkaline earth metals, GREEN; the transition metals, YELLOW;

the Lanthnoids/Lanthanides, ORANGE; the Actinoids/Actinides, PURPLE;

the halogens, PINK. 4. Outline the semiconductors in BROWN. 5. Return your colored pencils to the box making sure you have the

pencils in the correct color cubbies of the box.

6. Answer all the questions posed on your data sheet using your now colored periodic table.

7. Submit your completed data sheet to your teacher by the end of the period

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13

Touring the Periodic Table

Foundation Physical Science

Data Sheet

Name _____________________________________________________________________Period_____________

1. What is a period on the periodic table?

2. How many periods are in the current periodic table?_______ 3. What is a group on the periodic table?

4. How many groups are in the current periodic table?_______ 5. What element found in the alkali metal group is NOT a metal? ________

6. Why is this element is found in the alkali metal group? 7. In general, are metallic elements located on the left side or the right side of the periodic table?

8. What is another name for semiconductors? _________________________Define semiconductor.

9. Where are the most unreactive and most stable atoms in the periodic table called? __________________

14

10. In what group are the noble gases located? ___________

11. How many valence electrons do the noble gases have? ___________

12. Is oxygen an example of a metal,non-metal or a semiconductor? Defend your answer. 13. Alkali metal atoms have how many valence electrons? _______________ Do these atoms tend to gain or lose electrons when bonding? _______________ This makes these atoms form what type of IONS (cation or anion) _______________ 14. Alkali earth metal atoms have how many valence electrons? _______________ Do these atoms tend to gain or lose electrons when bonding? _______________ This makes these atoms form what type of IONS? _______________

15. Halogen atoms have how many valence electrons? _______________ Do these atoms tend to gain or lose electrons when bonding? _______________ This makes these atoms form what type of IONS? _______________ 16. Which group of elements would have 3 valence electrons in their outermost shells? _______________ Do these atoms tend to gain or lose electrons when bonding? _______________ This makes these atoms form what type of IONS? _______________

17. Write the Isotopic symbol for the halogen with the smallest atomic number. ______________

18. Write the Isotopic symbol for the noble with the greatest average atomic mass. ______________

19. Write the Isotopic symbol for the alkaline earth metal with 38 p+, 50 no and 36 e-. ______________

20. Write the Isotopic symbol for the alkali metal with 55 p+, 73 no and 54 e-. ______________

21. Write the Isotopic symbol for the transition metal with 79 p+, 118 no and 196 e-. ______________

22. Write the Isotopic symbol for the metalloid with 33 p+, 42 no and 36 e-. ______________

15

Place the symbol and name of the element in the room where it belongs.

16

Castle Mendeleev

Across

3. Compound consisting of two atoms of the same element. (ex: O2, H2)

6. Force that attracts chemical elements to other elements and keeps them joined (bonded)

together.

9. Smallest part of a compound.

10. Inactive; ex. He,Ne; do not actively combine with other elements.

Down

1. Easily transfer the flow of electrons (electricity).

2. Compounds consisting of the elements carbon and hydrogen.

4. Electron(s)in the outer orbit of an atom that will either be gained, lost, or shared

when combining with another atom to form a compound.

5. A metal made by mixing two or more metals; ex. copper + zinc ----> brass

6. Orbit of electrons around the nucleus of an atom.

7. A charged particle; the result of an atom either gaining or losing electrons.

8. Atoms of an element that have a different than normal number of electrons.

17

Physical Science

Bonding & Lewis Dot---Class notes

Periodic table is needed—Get yours from your notebook or open up your student planner .

Review—

Example 1--Lithium:

Bohr diagram of the ATOM Bohr diagram of the ION

Notes:

Example 2--Phosphorus:

Bohr diagram of the ATOM Bohr diagram of the ION

Notes:

18

More examples—Chlorine, Hydrogen, Calcium, Carbon (yes you have to draw the templates yourself, you don’t have to

make them so big but if you like big then use your own paper!)

19

In Summary:

Below is a outline of the first three periods of the periodic table. In each box, draw the electron dot for the element

belonging there. Several are done for you as an example.

Group

1

*Group 18

H• Group

2

*Group 13 *Group

14 *Group

15 *Group

16 *Group

17

3 4 5 6 7 8 9 10 11 12

(X represents the chemical symbol of whatever element you are working with.)

Group 1 element has ______ valence electrons and a general electron dot diagram of ________________ (REVIEW!

This group is called?_____________________________________)

Group 2 element has ______ valence electrons and a general electron dot diagram of ________________(This group is

called?_____________________________________)

In general, Group 3-12 element have ______ valence electrons and a general electron dot diagram of

________________ (This block of elements is called?_____________________________________)

Group 13 element has ______ valence electrons and a general electron dot diagram of ________________





(This group is called?_____________________________________)

Group 18 element has ______ valence electrons and a general electron dot diagram of ________________ EXCEPT

_________ Why? (this group is called? _____________________________________)

Chemical reactions involves __________________________whereas Nuclear reactions involve___________________.

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Name_________________________________ Period______ Date__________________

Lewis Dot Structures

Lewis dot structures are a way to indicate the number of valence electrons. Draw Lewis dot structures of the following atoms.

1. Calcium

2. Potassium

3. Argon

4. Aluminum

5. Bromine

6. Carbon

7. Helium

8. Oxygen

9. Phosphorus

10. Hydrogen

11. Chlorine

12. Nitrogen

13. Sodium

14. Neon

15. Lithium

16. Sulfur

17. Arsenic

18. Krypton

19. Iodine

20. Radon

21

Name ___________________________ Class ___________________ Date _____________

Chapter 6 Chemical Bonds©

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Section 6.1 Ionic Bonding (pages 158–164)This section describes the formation of ionic bonds and the properties of ioniccompounds.


Sequencing As you read, complete the concept map to show whathappens to atoms during ionic bonding. For more information on thisReading Strategy, see the Reading and Study Skills in the Skills andReference Handbook at the end of your textbook.

Stable Electron Configurations (page 158)

1. Describe the type of electron configuration that makes an atom stable and not likely to react.

2. Describe an electron dot diagram.

Ionic Bonds (pages 159–161)

3. Some elements achieve stable electron configurations through thetransfer of between atoms.

4. By losing one valence electron, a sodium atom achieves the sameelectron arrangement as an atom of .

5. Circle the letter that states the result of a sodium atom transferringan electron to a chlorine atom. a. Each atom ends up with a more stable electron arrangement.b. The sodium atom becomes more stable, but the chlorine atom

becomes less stable.c. The chlorine atom becomes more stable, but the sodium atom

becomes less stable.d. Each atom ends up with a less stable electron arrangement.

6. Is the following sentence true or false? An ion is an atom that has anet positive or negative electric charge.

7. An ion with a negative charge is called a(n) .

Atom

loseselectrons

to

gainselectrons

to

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Name ___________________________ Class ___________________ Date _____________

Chapter 6 Chemical Bonds


8. An ionic bond forms when are transferredfrom one atom to another.

9. Is the following sentence true or false? The lower the ionizationenergy, the easier it is to remove an electron from an atom.

Ionic Compounds (pages 161–164)

10. Circle the letter of each piece of information provided by thechemical formula of an ionic compound.a. which elements the compound containsb. the charge on each ion in the compoundc. how the ions are arranged in the compoundd. the ratio of ions in the compound

11. Circle the letter of the correct answer. The formula for magnesiumchloride is MgCl2. The charge on the magnesium ion is 2!. What isthe charge on each chloride ion?a. 2" b. 1"

c. 0 d. 1!

12. Look at the arrangement of ions in a sodium chloride crystal. How many sodium ions surround each chloride ion in this three-dimensional structure?a. 3 b. 4c. 6 d. 8

13. The shape of an ionic crystal depends on .14. Identify two factors that determine the arrangement of ions in an

ionic crystal. a. b.

15. Is the following sentence true or false? The attractions among ionswithin a crystal lattice are weak.

Na! Cl"


23

Ionic Bonding

Class Notes:_____________ Periodic Table required.

Animation:

http://www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/bom1s2_11.swf and http://www.visionlearning.com/library/module_viewer.php?mid=55 (reaction between sodium chloride) Using a periodic table, I will

1. Draw the electron dot(Lewis Dot) for the cation and the anion and their respective atoms. 2. Identify the symbol of the Noble gas whose valence electron configuration matches the cation

& anion. 3. Draw the electron dot(Lewis Dot) for the ionic compound formed, 4. Predict the chemical formula from the drawn electron dot and name of compound.

(Note the following should be completed in class, if you need more space/paper you must use your

own so get it out quietly. There is NO need to disrupt the class to ask what to do. If we do not get to

finish all these in class due to some type of disruption, then it is your responsibility to finish them

before the next test as practice)

Beryllium and oxygen Potassium and bromide Lithium and sulfur Calcium and iodine aluminum and phosphorus magnesium and nitrogen

24

http://www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/bom1s2_11.swf

http://www.visionlearning.com/library/module_viewer.php?mid=55

25

name per date BULGRIN Integrated Physical Science

Chemthink: IONIC BONDING TUTORIAL a) Go to www.chemthink.com. Log in using your user name and password. (If you forgot, you need to WAIT

QUIETLY until your teacher is done introducing the lesson) b) Scroll to IONIC BONDING then the tutorial under the Ionic Bonding menu. c) Complete the tutorial. As you complete the tutorial, write down the answers to the questions below. d) Once you have successfully completed the tutorial and this worksheet, complete the Question Set.

IONIC BONDING TUTORIAL QUESTIONS:

NOTE: The numbers to the left refer to the page of the tutorial on which the information is found.

4) Oppositely charged ions each other and stick together. 5) Charges that are will repel each other: a) Two charged ions (anions) will each other. b) Two charged ions (cations) will each other. In order to build an ionic compound that will stick together, you will need both

. 6) Since atoms easily lose , the positive ion (cation) will usually be

a .

Atoms on the side of the periodic table (to the of the zig-zag line) form positive

ions. 7) Since atoms form ions by , the ion (anion) will

usually be a .

NOTE: One group of nonmetal atoms doesn’t form ions. They are Group __A = gases. 10) The symbol for = Na. The symbol for = Cl Sometimes Cl will take from Na. 11) This will form _____ ions (cations) and _____ ions (anions) which are to each other. 12) AN IONIC BOND is the

17) A positive ion (cation) will attract any nearby ions (anions) and

each negative ion (anion) will attract any nearby ions (cations).

18) All of these attractions together forms an .

20) In an ionic compound there are no distinct . There is just a regular arrangement

of positive and negative ions called a crystal lattice. This is shown in the 3-D model.

(NOTE: 3-D means )

26

22) Since the sodium chloride crystal contains each ion in a one-to-one ratio (1:1 ratio of Na+:Cl-), we write the

formula for sodium chloride as

NOTE ON NAMING:

A) Anions are named differently than the neutral nonmetal atom they came from.

Take the beginning part of the neutral atom’s name and add “-ide”:

Example: Neutral atom name of Cl = chlorine;

Ion name of Cl- =

B) Cations are named just like the neutral metal atoms they came from:

Example: Neutral atom name of Na = sodium;

Ion name of Na+ =

23) In ionic compounds the formula tells us the between ions in the crystal lattice.

The formula does NOT mean that there are individual

For example, NaCl does NOT mean we have individual molecules that contain 1 Na+ and 1 Cl-. We have a 3-D

crystal lattice that contains ____ Na+ ion for every ____ Cl- ion.

24) Calcium fluoride is an ionic compound because it has metal cations and nonmetal anions .

It contains a ratio of _____ metal Ca2+ cations to _____ nonmetal F- anions.

25) This ratio can be simplified to a _________ ratio of Ca2+:F- so we write the formula for calcium chloride as

____________

Chemthink: COVALENT BONDING TUTORIAL a) Go to www.chemthink.com. Log in using your user name and password. (If you forgot, you need to WAIT

QUIETLY until your teacher is done introducing the lesson) b) Scroll to COVALENT BONDING then the tutorial under the Covalent Bonding menu. c) Complete the tutorial. As you complete the tutorial, write down the answers to the questions below. d) Once you have successfully completed the tutorial and this worksheet, complete the Question Set.

e) Finish early? Double-check your records to make sure all ChemThink assignments are completed. COVALENT BONDING TUTORIAL QUESTIONS:

NOTE: The numbers to the left refer to the page of the tutorial on which the information is found.

2) Describe the movement of the electrons in each separate atom: 3) a) How is the movement of electrons different when the two atoms are close? b) What happens if you try to move the atoms very close together?

27

7) a) When two atoms get close enough, the of one atom has a strong attraction for its own

electrons and also for the electron of the atom.

b) At this point, both atoms are attracting .

c) Where do the two electrons spend most of their time now? 9) In a , two atoms are over each other’s

electrons. Both atoms stay because of this tug-of-war. 11) What family of atoms never forms a bond?

12) Covalent bonds will form between two atoms. Each atom holds onto its

own electrons while trying to take .

13) What nonmetal is on the left side of the periodic table?

WHY DO ATOMS FORM COVALENT BONDS?

16) a) What happens to the potential energy (PE = the energy of position) of the atoms as they move closer together?

b) If the two atoms get too close to each other, the potential energy (PE) because the

positive-charged nuclei start to repel each other.

18) The of a covalent bond is the distance between two nonmetal atoms that

creates the potential energy.

19) The two nonmetal atoms are more (i.e., lower in energy) when they form a covalent bond than

when they are far apart and exist as separate atoms.

20) Lower energy = atoms

Therefore, nonmetal atoms form covalent bonds to become more stable than the separate atoms. 21) A single solid line connecting two atomic symbols represents a . We say the two electrons are being shared. A molecule of hydrogen gas (H2) would be shown as: 22) Some atoms form bonds by sharing ____ pairs of electrons when they bond.

Oxygen gas (O2) can be shown as

A double covalent bond represents a total of ____ shared electrons.

23) A covalent bond id formed when 2 atoms share ____ electrons between them.

Nitrogen gas (N2) is an example and can be shown as

24) Put each type of covalent bond (single, double, or triple bond) in order from weakest to strongest:

< < weakest strongest

28

NAMING SIMPLE COVALENT COMPOUNDS:

27) When covalent compounds are made from only two elements, the ending of the name of the 2nd element is

changed to “-ide”.

examples: oxygen becomes & chlorine becomes

29) Prefixes are added in front of each element’s name to tell us of

that element are present in the molecule.

30) The following prefixes are used in naming covalent compounds:

means 1 means 6

means 2 hepta means 7

means 3 octa means 8

means 4 nona means 9

means 5 deca means 10

The only exception is you never use to name the first element!

Examples: NO2 =

and CO2 =

but CO = carbon monoxide (note: NOT mono-oxide! Drop one oxygen)

and NO =

29

Name ___________________________ Class ___________________ Date _____________

Chapter 6 Chemical Bonds


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Section 6.2 Covalent Bonding(pages 165–169)This section discusses the formation of covalent bonds and the factors thatdetermine whether a molecule is polar or nonpolar. It also discussesattractions between molecules.


Relating Text and Visuals As you read the section, look closely atFigure 9. Complete the table by describing each type of model shown.For more information on this Reading Strategy, see the Reading andStudy Skills in the Skills and Reference Handbook at the end ofyour textbook.

Molecular Models

Model Description

Electron dot

Structural formula

Space-filling

Electron cloud

Covalent Bonds (pages 165–167)

1. Describe a covalent bond.

2. Circle the letters of molecular models that show orbitals of atomsoverlapping when a covalent bond forms. a. electron dot b. structural formulac. space-filling d. electron cloud

3. Describe a molecule.

4. Is the following sentence true or false? In a covalent bond, the atomsare held together by the attractions between the shared electronsand the protons in each nucleus.

5. Circle the correct answer. Nitrogen has five valence electrons. Howmany pairs of electrons must two nitrogen atoms share in order foreach atom to have eight valence electrons?

a. zero b. onec. two d. three

30

Name ___________________________ Class ___________________ Date _____________


Pearson Education, Inc., publishing as Pearson Prentice Hall. All rights reser ved.


Unequal Sharing of Electrons (pages 167–168)

6. In general, elements at the of a group have a greater attraction for electrons than elements at the

of a group have.7. In a hydrogen chloride molecule, the shared electrons spend

more time near the atom than near theatom.

8. Describe a polar covalent bond.

9. When atoms form a polar covalent bond, the atom with the greaterattraction for electrons has a partial charge.

10. Is the following sentence true or false? In a molecule of acompound, electrons are always shared equally by both atoms.

11. Circle the letter of each factor that determines whether a moleculeis polar or nonpolar.a. the number of atoms in the moleculeb. the type of atoms in the moleculec. the number of bonds in the moleculed. the shape of the molecule

12. Compare the shapes of carbon dioxide and water molecules. Circlethe letter of the polar molecule. a. carbon dioxide b. water

13. Is the following sentence true or false? In a water molecule, thehydrogen side of the molecule has a partial positive charge, andthe oxygen side has a partial negative charge.

Attraction Between Molecules (page 169)

14. Water has a higher boiling point than carbon dioxide becauseattractions between polar molecules are thanattractions between nonpolar molecules.

15. Is the following sentence true or false? Attractions amongnonpolar molecules explain why nitrogen can be stored as a liquidat low temperatures and high pressures.

CO2 H2O

31

FPS: Covalent Bonding Class Notes_____________________________ Animation Notes: http://www.kentchemistry.com/links/bonding/bondingflashes/bond_types.swf http://www.mhhe.com/physsci/chemistry/animations/chang_7e_esp/bom1s2_11.swf Practice: For each of the following substances, complete the following

1. Draw the electron dot/Lewis dot structure for each element in the substance. 2. Draw the electron dot/Lewis dot for the compound. 3. Identify the types of covalent bonds formed 4. Predict the chemical formula from the electron dot/Lewis dot structure.

Diatomic hydrogen, chlorine, oxygen, and nitrogen. Water, 2 carbon atoms and 2 hydrogen atoms. Use the space that is left, if necessary use your own paper to continue with the notes.

32

33

HW10:

34

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Name ___________________________ Class ___________________ Date _____________


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Section 6.3 Naming Compounds and Writing Formulas(pages 170–175)This section explains how to name and write formulas for ionic andmolecular compounds.


Predicting Before you read, predict the meaning of the termpolyatomic ion, and write your prediction in the table. After you read, if your prediction was incorrect, revise your definition. For more information on this Reading Strategy, see the Reading andStudy Skills in the Skills and Reference Handbook at the end of your textbook.

Vocabulary Term Before You Read After You Read

Polyatomic ion

Describing Ionic Compounds (pages 171–173)

1. Is the following sentence true or false? The name of an ioniccompound must distinguish the compound from other ioniccompounds containing the same elements.

2. What information is provided by the formula for an ionic compound?

3. Circle the letter of the word that describes a compound made fromonly two elements.a. ionic b. binary c. diatomic d. polar

4. Is the following sentence true or false? Names of anions are formedby placing the suffix -ide after part of the name of the nonmetal.

5. When a metal forms more than one ion, the name of the ion containsa Roman numeral to indicate the on the ion.

6. What is a polyatomic ion?

7. Is the following sentence true or false? Because all compounds areneutral, the total charges on the cations and anions in the formula ofan ionic compound must add up to zero.

36

Name ___________________________ Class ___________________ Date _____________




8. Circle the letter of the correct answer. The formula for sodiumsulfide is Na2S. The sodium ion has a charge of 1!. What must thecharge on the sulfide ion be?a. 1! b. 0c. 1" d. 2"

9. Circle the letter that identifies the number of ammonium ionsneeded to form a compound with one phosphate ion.a. one b. twoc. three d. four

Describing Molecular Compounds (pages 174–175)

10. What information is provided by the name and formula of a molecular compound?

11. Describe the general rule for naming molecular compounds.

12. Is the following sentence true or false? The formula for a molecularcompound is written with the symbols for the elements in thesame order as the elements appear in the name of the compound.

13. Circle the letter that identifies the method of naming the numberof atoms in molecular compounds.a. prefix b. suffixc. number d. symbol

14. In the formula of a molecular compound, the number of atoms ofan element in the molecule is represented by a(n)

.

Name Formula FormulaName

Some Polyatomic Ions

Ammonium

Hydroxide

Nitrate

Sulfate

Carbonate

Phosphate

Acetate

Peroxide

Permanganate

Hydrogen sulfate

Hydrogen carbonate

Hydrogen phosphate

C2H3O2!

O22!

MnO4!

HSO4!

HCO3!

HPO42!

NH4"

OH!

NO3!

SO42!

CO32!

PO43!

37

Writing Ionic Formulas Name:____________________________Date:____________ Write the formulas for the following ionic compounds

1. Sodium Chloride ________________

2. Calcium Flouride ________________

3. Zinc Sulfide ________________

4. Sodium phosphate ________________

5. Potassium oxide ________________

6. Aluminum bromide ________________

7. Calcium iodide ________________

8. Magnesium chloride ________________

9. Ammonium chloride ________________

10. Sodium Nitrate ________________

11. Aluminum hydroxide ________________

12. Magnesium carbonate ________________

13. Litium nitride ________________

14. Litium nitrate ________________

15. Aluminum oxide ________________

38

Naming Ionic Compounds Name:____________________________Date:____________ Name the following ionic compounds

1. KCl _____________________________________________

2. AlCl3 _____________________________________________

3. NaF _____________________________________________

4. NaOH _____________________________________________

5. Mg(OH)2 _____________________________________________

6. NH4OH _____________________________________________

7. MgCl2 _____________________________________________

8. K2O _____________________________________________

9. BaCl2 _____________________________________________

10. Ba(OH)2 _____________________________________________

11. Al2(SO4)3 _____________________________________________

12. Al(OH)3 _____________________________________________

13. CaSO4 _____________________________________________

14. CaCO3 _____________________________________________

15. MgCl2 _____________________________________________

39

Naming and Writing Covalent/Molecular Compounds Name:____________________________Date:____________ Write the formulas for the following covalent compounds

1. Diphosphorus pentoxide ________________

2. Nitrogen trioxide ________________

3. Phosphorus pentabromide ________________

4. Oxygen difluoride ________________

5. Dinitrogen tetroxide ________________

6. Nitrogen triiodide ________________

7. Dichlorine trioxide ________________

8. antimony tribromide ________________

9. hexaboron silicide ________________

10. chlorine dioxide ________________

11. iodine pentafluoride ________________

12. nitrogen trihydride (ammonia ) ________________

13. dihydrogen monoxide (water) ________________

14. phosphorus triiodide ________________

40

Write the name of the following molecular compounds

1. CO2 _______________________________________________

2. NH3 _______________________________________________

3. N2O3 _______________________________________________

4. CCl4 _______________________________________________

5. NO _______________________________________________

6. PCl5 _______________________________________________

7. PBr3 _______________________________________________

8. P4S5 _______________________________________________

9. O2 _______________________________________________

10. SeF6 _______________________________________________

11. Si2Br6 _______________________________________________

12. SCl4 _______________________________________________

13. B2Si _______________________________________________

41

Naming and Writing Formulas Mixed Practice Name:____________________________Date:____________ First identify the compound as either ionic (I) or covalent (C). Then write the formula or name the compound depending on what’s given. The first one is done for you. 1. Phosphorus pentafluoride PF5

2. Bromine hexafluoride

3. Calcium chloride

4. CS2

5. PCl5

6. Na2CO3

7. CO

8. dinitrogen trioxide

9. phosphorus trifluoride

10. aluminum hydroxide

11. CaSO4

12. C2Br6

13. MgS

14. N2O3

15. tetraphosphorus triselenide

16. potassium chloride

17. tetrasulfur dinitride

18. NaOH

19. Ca(OH)2

20. BaSO4

21. ammonium carbonate

22. sulfur trioxide

23. A12O3

C

42

24. carbon tetrachloride

25. NH4Cl

26. NaBr

27. CaCO3

28. calcium bromide

29. potassium hydroxide

30. Na2CO3

31. NaBr

32. nitrogen tribromide

33. sulfur hexachloride

34. NaOH

35. CaBr2

36. AlI3

37. lithium oxide

38. Strontium nitrate

39. Sodium Phosphide

40. Aluminum Oxide

41. K2S

42. CO2

43. K2O

44. Be3P2

45. FrF

43

Name ___________________________ Class ___________________ Date _____________

Chapter 7 Chemical Reactions©

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Section 7.1 Describing Reactions (pages 192–198)This section discusses the use of chemical equations and how to balance them.It also demonstrates the use of calculations in chemistry.


Monitoring Your Understanding Preview the Key Concepts, topicheadings, vocabulary, and figures in this section. List two thingsyou expect to learn. After reading, state what you learned abouteach item you listed. For more information on this Reading Strategy,see the Reading and Study Skills in the Skills and ReferenceHandbook at the end of your textbook.

What I Expect to Learn What I Learned

Chemical Equations (pages 192–193)

1. Is the following sentence true or false? The new substances formedas a result of a chemical reaction are called products.

2. Circle the letter of each sentence that is a correct interpretation ofthe chemical equation C ! O2 h CO2.a. Carbon and oxygen react and form carbon monoxide.b. Carbon and oxygen react and form carbon dioxide.c. Carbon dioxide yields carbon and oxygen.d. The reaction of carbon and oxygen yields carbon dioxide.

3. Is the following sentence true or false? The law of conservationof mass states that mass is neither created nor destroyed in achemical reaction.

4. Circle the letter of the correct answer. According to the equationC ! O2 h CO2, how many carbon atoms react with 14 moleculesof oxygen to form 14 molecules of carbon dioxide?a. 1 b. 7c. 14 d. 28

5. In the reaction represented by the equation C ! O2 h CO2, the mass of carbon dioxide produced equals

.

44

Name ___________________________ Class ___________________ Date _____________

Chapter 7 Chemical Reactions©



Balancing Equations (pages 194–195)

6. Is the following sentence true or false? A chemical equation mustbe balanced in order to show that mass is conserved during areaction.

7. Circle the letter of the name given to the numbers that appearbefore the formulas in a chemical equation.a. subscripts b. mass numbersc. atomic numbers d. coefficients

8. Is the following sentence true or false? Because the equationN2H4 ! O2 h N2 ! H2O has two nitrogen atoms on each side,the equation is balanced.

Counting With Moles (pages 195–196)

9. Chemists use a counting unit called a(n) tomeasure amounts of a substance because chemical reactions ofteninvolve large numbers of small particles.

10. Circle the letter of the correct answer. If one carbon atom has anatomic mass of 12.0 amu and one oxygen atom has an atomic massof 16.0 amu, what is the molar mass of carbon dioxide?a. 28.0 amu b. 44.0 amuc. 28.0 g d. 44.0 g

11. Circle the letter of the correct answer. To convert grams of carbondioxide to moles of carbon dioxide, you must multiply by whichconversion factor?

a. b.

c. d.

Chemical Calculations (pages 197–198)

12. Complete the table.

Formation of Water

Equation 2H2 + O2 h 2H2O

Amount 2 mol 1 mol

Molar Mass 2.0 g/mol 18.0 g/mol

Mass (Moles " Molar Mass) 32.0 g 36.0 g

13. Circle the letter of the correct answer. One mole of oxygen has amass of 32 grams. What is the mass of four moles of oxygen?a. 128 g b. 144 gc. 128 amu d. 144 amu

1 mol CO2

28.0 g CO2

28.0 g CO2

1 mol CO2

1 mol CO2

44.0 g CO2

44.0 g CO2

1 mol CO2

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name per date BULGRIN Integrated Physical Science

Chemthink: CHEMICAL REACTIONS a) Go to www.chemthink.com. Log in using your user name and password. (If you forgot, you need to WAIT

QUIETLY until your teacher is done introducing the lesson) b) Scroll to CHEMICAL REACTIONS then the tutorial under the Chemical Reactions menu. c) Complete the tutorial. As you complete the tutorial, write down the answers to the questions below. d) Once you have successfully completed the tutorial and this worksheet, complete the Question Set.

CHEMICAL REACTIONS TUTORIAL QUESTIONS:

1. Starting materials in a chemical reaction are called 2. The ending materials in a chemical reaction are called 3. The arrow indicates a has taken place. 4. All reactions have one thing in common: there is a of chemical bonds. 5. Chemical reactions always involve old bonds, new bonds, or both. 6. In all reactions we still have all of the at the end that we had at the start. 7. In every reaction there can never be any atoms or 8. Chemical reactions only in the atoms that are already

there. 9. Let’s represent a reaction on paper. For example, hydrogen gas (H2) reacts with oxygen gas (O2) to form water

(H2O): H2 + O2 H2O If we use only the atoms shown, we’d have atoms of H and atoms of O as reactants. This would

make molecule of H2O, but we’d have atom of O leftover. However, this reaction only makes H2O.

Remember: reactions are not limited to 1 molecule each of reactants. We can use as many as we need to balance the chemical equation. A balanced chemical reaction shows:

a) What atoms are present before (in the reactants) and after (in the products) b) How many of each reactant and product is present before and after.

10. So to make H2O from oxygen gas and hydrogen gas, the balanced equation would be:

____ H2 + _____ O2 _____ H2O Which is the same as:

# of atoms in Reactants Element # of atoms in

Products H

O

11. This idea is called the 12. There must be the same and the same number of before the reaction (in the reactants)

and after the reaction (in the products). 13. What is the balanced equation for this reaction? ____ Cu + _____ O2 ____ CuO

46

14. In the unbalanced equation there are: Reactants Products

Cu atoms _____ Cu atoms ______

O atoms _____ O atoms ______

15. To balance this equation, we have to add ______ molecules to the products, because this reaction doesn’t make

lone _____ atoms. 16. When we added a molecule of CuO, now the number of _____ atoms is balanced but the number of ____ atoms

don’t match. Now we have to add more _____ atoms to the reactants. 17. The balanced equation for this reaction is

____ Cu + _____ O2 ____ CuO This is the same thing as saying: Reactants Products

# Cu atoms _____ = # Cu atoms ______

# O atoms _____ = # O atoms ______

18. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.) _____ CH4 + _____ O2 _____ H2O + _____ CO2


Products 1 C 1

4 H 2

2 O 3 19. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.) _____ N2 + _____ H2 _____ NH3


Products 2 N 1

2 H 3

47

20. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.) _____ KClO3 _____ KCl + _____ O2


Products 1 K 1

1 Cl 1

3 O 2 21. What is the balanced equation for this reaction? (Use the table to keep track of the atoms on each side.) _____ Al + _____ O2 _____ Al2O3


Products 1 Al 2

2 O 3 SUMMARY

1) Chemical reactions always involve 2) The Law of Conservation of Mass says that the same atoms must be

3) To balance a chemical equation, you change the in front of each substance

until there are the same number of each type of in both reactants and products

48

49

FPS: Intro to Balancing equations

Class notes(date)_____________

Several examples will be completed in class. The first several you can follow along using the template below. After

these first few, we will continue but you will need to complete on your own paper. Make sure you end your notes with

a summary of the key points to balancing equations.

Example 1:

Unbalanced equation(UB):

Particle diagram (PD)

Atom tally:

Final Balanced equations(BE):

Example 2:



Atom tally:


50

Example 3:



Atom tally:


Example 4:



Atom tally:


51

Balancing Equation Worksheet

Name _______________________________ Directions: For each of the skeletal equations below, write the coefficients that would balance the equation in front of each substance. Remember no Coefficient written is assumed to be 1.

1. _____H2 + _____ O2 ---> _____ H2O 27. _____ N2 + _____H2 ---> _____ NH3

2. _____S8 + _____O2 ---> _____SO3 28. _____N2 + _____O2 ---> _____N2O 3. _____HgO ---> _____Hg + _____O2 29. _____CO2 + _____ H2O ---> _____ C6H12O6 + _____O2

4. _____Zn + _____ HCl ---> _____ZnCl2 + _____H2

5._____SiCl4 + _____H2O ---> _____H4SiO4 + _____HCl

6. _____Na + _____H2O ---> _____NaOH + _____H2

7. _____C10H16 + _____Cl2 ---> _____C + _____ HCl 8. _____Si2H3 + _____O2 ---> _____SiO2 + _____H2O 9. _____Fe + _____ O2 ---> _____ Fe2O3 10. _____C7H6O2 + _____ O2 ---> _____ CO2 + _____ H2O 11. _____FeS2 + _____O2 ---> _____ Fe2O3 + _____SO2

12. _____Fe2O3 + _____ H2 ---> _____Fe + _____ H2O 13. _____K + _____Br2 ---> _____ KBr 14. _____C2H2 + _____O2 ---> _____ CO2 + _____H2O 15. _____H2O2 ---> _____H2O + _____ O2

16. _____C7H16 + _____O2 ---> _____CO2 + _____ H2O 17. _____SiO2 + _____HF ---> _____SiF4 + _____H2O 18. _____KClO3 ---> _____KCl + _____O2

19. _____KClO3 ---> _____KClO4 + _____KCl 20. _____P4O10 + _____H2O ---> _____H3PO4

21. _____Sb + _____O2 ---> _____Sb4O6

22. _____C3H8 + _____O2 ---> _____CO2 + _____H2O 23. _____Fe2O3 + _____CO ---> _____Fe + _____ CO2 24. _____PCl5 + _____H2O ---> _____HCl + _____ H3PO4

25. _____H2S + _____Cl2 ---> _____S8 + _____HCl 26. _____Fe + _____ H2O ---> _____Fe3O4 + _____H2

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53

Laboratory Activity

AT At Exploring pH

Acids are materials that have certain properties in common. Bases (also called alkalis) are other substances with a different set of properties. Chemists use the pH scale to express how acidic (like an acid) or basic (like a base) a substance is. A pH value below 7 means that a substance is acidic, and the smaller the number, the more acidic it is. A pH value above 7 means that a substance is basic, and the larger the number, the more basic it is.

The most striking property of both acids and bases is their ability to change the color of certain vegetable materials. A common vegetable whose color responds to acids and bases is red cabbage. The first step in this experiment is to prepare an extract of red cabbage, so you can investigate its color changes.

OBJECTIVES

In this experiments, you will investigate some of these properties with materials that are found around your home. In addition, you will learn how chemists use the pH scale to describe acids and bases. MATERIALS

PROCEDURE

1. Obtain a spot plate. If clear place on a white sheet of paper. 2. Use a the stock solutions found at your station ADD 3 drops of ONE solution to 3 different

wells. 3. Take your red litmus paper and stick into WELL 1. Record your observations. Throw the

paper in the trash. 4. Take your blue litmus paper and stick into WELL 2. Record your observations. Throw the

paper in the trash. 5. Take your Universal indicator paper and stick into WELL 3. Record both the COLOR and

the pH found on the canister. Throw the paper in the trash. 6. Rinse your spot plate in the sink. 7. Repeat procedures 1 through 6 for each stock solution found at your station. 8. Answer the conclusions/application questions which follow.

54

Exploring pH Data Sheet NAME ____________________________________

OBSERVATIONS

SUBSTANCE RED LITMUS

COLOR

BLUE LITMUS

COLOR

UNIVERSAL INDICATOR COLOR

PH

BAKING SODA

SHAMPOO

VINEGAR

WATER

DETERGENT

ALKA SELTZER

BLEACH

SPRITE/7UP

QUESTIONS: Using complete sentences, answer the following base on your observation and knowledge of polymers. Identify the household substances that would be classified as an acid. Identify the household substances that would be classified as a base. Do you have any substance that would be NOT be classified as a base or an acid? How did you conclude this?

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Total running time approximately 45 minutes.

The Universe—The History Channel

The Life and Death of a Star

Semester 1 Worksheet #2

Class Notes ________ Objective: Upon completion of this lesson, the student should be able to—

describe that stars produce energy from nuclear reactions and that processes in stars have led to the formation of all elements beyond hydrogen and helium.(grade 9, Ohio Academic Benchmark)

explain that gravitational forces govern the characteristics and movement patterns of the planets, comets and asteroids in the solar system. (grade 9, Ohio Academic Benchmark)

examine the life cycle of a star and predict the next likely stage of a star.(grade 8, Ohio Academic Benchmark)

name and describe tools used to study the universe.(grade 8, Ohio Academic Benchmark)

Directions: As you view the video, glean the important information by answering the questions that follow: Introduction & Forces of Gravity (16 minutes)

1. How many stars are in just our galaxy?____________________________________________________ 2. What is so special about the “Pillars of Creation”? What are the main elements that make up the “Pillars

of Creation”? 3. What element is the key component of stars?______________________________________________ 4. What is the most important force in the universe?___________________________________________ 5. The most basic unit of mass produced in the universe due to this force is a

___________________________. Describe how this happens. (make sure to include the following terms—gravity, protostar, star, gas/dust, temperature, compression, thermonuclear fusion,)

6. Once a star is born it is in a constant battle with what force to stay

alive!_____________________________. Describe what “weapon” the star uses to fight this force.

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7. When the star is in a state of equilibrium, it is classified as a ___________ __________________star. 8. Describe how can you tell the temperature of star just by looking at it? 9. Differentiate between the types of main sequence stars by completing the table below: Type of Star Mass of sun Surface Temperature Luminance

Red Dwarf

Blue main Sequence

10. Why do the more massive stars have a shorter life span than the small mass stars? What does this say

about the life span of our own sun? 11. Describe what must be true for a star to die. 12. What can a star do when it’s core temperature reaches 180, 000,000 degrees that can extend its lifespan? 13. Describe how a planetary nebular form? White Dwarfs(9:52minute) 14. How do electrons found in a star help the star fight the force of gravity?

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15. The final stage of a star or a “retired star” is classified as a ________________ _____________ . 16. What is the advantage companion star provides to the life of a white dwarf star? Will our sun be able to

do this? 17. How many supernovas have been found in this last decade? _________________________________ 18. Describe why this is so unusual and what tool allows finding them easier. 19. How are Type 2 supernovas different from Type 1 supernovas? 20. What does it say about the star if you find a lot of iron in its core? 21. Where does all the iron in the universe and elements heavier than iron originally come from? All from the Stars(6:01 minutes) 22. Where do the elements in our body come from? 23. Describe how gravity finally destroys the core of a collapsed star. 24. List at least two differences between a neutron stars and a regular stars? 25. What is a pulsar?

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26. Describe how a black hole is formed and provide two characteristics associated with a black hole.

Collisions of Stars(6:37 minutes)

27. Describe what astronomical event occurred in the fall of 2006. What information did this provide to astronomers?

28. Describe what happens when stars collide and identify the tool astronomers use to help model this

phenomena. Failed Stars(5:35 minutes)

29. Describe how a globular cluster galaxy is different from our spiral galaxy, the Milky Way. 30. Where do the “blue stragglers” come from? 31. List several characteristics about a brown dwarf? 32. Is a brown dwarf a star or a planet? Defend your answer.

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Teacher use only: _____Submitted by the due date _____followed above instructions _____ approved to use

My Semester Final Reference Sheet

Name ________________________________________________________________ The back of this sheet is your periodic table which you will be allowed to use on your final exam, January 17 at 1 am. The rest of this page is for YOU to HANDWRITE any notes you want to have available to you for the final exam. YOU must stay within this PAGE. You may write on the back where the periodic table is, you may NOT attach anything to this page, you may not type this page. Although there may be similarities in the content, all work should be originally and not copied from any else. This will count as a 20

point HW grade and is due by the end of the period on the Last Day of Scheduled classes.. Failure to submit this assignment will result in you only receiving a periodic table to use for the final grade and 0/20 for a HW effort grade.

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The Periodic Table of the Elements

1H

Hydrogen1.00794

2HeHelium4.003

3Li

Lithium6.941

4Be

Beryllium9.012182

5B

Boron10.811

6C

Carbon12.0107

7N

Nitrogen14.00674

8O

Oxygen15.9994

9F

Fluorine18.9984032

10NeNeon

20.1797

11NaSodium

22.989770

12Mg

Magnesium24.3050

13Al

Aluminum26.981538

14Si

Silicon28.0855

15P

Phosphorus30.973761

16S

Sulfur32.066

17Cl

Chlorine35.4527

18ArArgon

39.948

19K

Potassium39.0983

20Ca

Calcium40.078

21Sc

Scandium44.955910

22Ti

Titanium47.867

23V

Vanadium50.9415

24Cr

Chromium51.9961

25Mn

Manganese54.938049

26FeIron

55.845

27CoCobalt

58.933200

28NiNickel

58.6934

29CuCopper

63.546

30Zn

Zinc65.39

31GaGallium69.723

32Ge

Germanium72.61

33AsArsenic

74.92160

34Se

Selenium78.96

35Br

Bromine79.904

36Kr

Krypton83.80

37Rb

Rubidium85.4678

38Sr

Strontium87.62

39Y

Yttrium88.90585

40Zr

Zirconium91.224

41Nb

Niobium92.90638

42Mo

Molybdenum95.94

43Tc

Technetium(98)

44Ru

Ruthenium101.07

45Rh

Rhodium102.90550

46Pd

Palladium106.42

47AgSilver

107.8682

48Cd

Cadmium112.411

49In

Indium114.818

50Sn

Tin118.710

51Sb

Antimony121.760

52Te

Tellurium127.60

53I

Iodine126.90447

54XeXenon

131.29

55CsCesium

132.90545

56BaBarium

137.327

57La

Lanthanum138.9055

72Hf

Hafnium178.49

73Ta

Tantalum180.9479

74W

Tungsten183.84

75Re

Rhenium186.207

76Os

Osmium190.23

77Ir

Iridium192.217

78Pt

Platinum195.078

79AuGold

196.96655

80HgMercury200.59

81Tl

Thallium204.3833

82PbLead

207.2

83Bi

Bismuth208.98038

84Po

Polonium(209)

85At

Astatine(210)

86RnRadon(222)

87Fr

Francium(223)

88RaRadium(226)

89Ac

Actinium(227)

104Rf

Rutherfordium(261)

105Db

Dubnium(262)

106Sg

Seaborgium(263)

107Bh

Bohrium(262)

108Hs

Hassium(265)

109Mt

Meitnerium(266)

110

(269)

111

(272)

112

(277)

113 114

58CeCerium

140.116

59Pr

Praseodymium140.90765

60Nd

Neodymium144.24

61Pm

Promethium(145)

62Sm

Samarium150.36

63Eu

Europium151.964

64Gd

Gadolinium157.25

65Tb

Terbium158.92534

66Dy

Dysprosium162.50

67Ho

Holmium164.93032

68ErErbium

167.26

69TmThulium

168.93421

70Yb

Ytterbium173.04

71Lu

Lutetium174.967

90Th

Thorium232.0381

91Pa

Protactinium231.03588

92U

Uranium238.0289

93Np

Neptunium(237)

94Pu

Plutonium(244)

95Am

Americium(243)

96CmCurium(247)

97Bk

Berkelium(247)

98Cf

Californium(251)

99Es

Einsteinium(252)

100FmFermium(257)

101Md

Mendelevium(258)

102No

Nobelium(259)

103Lr

Lawrencium(262)

1995 IUPAC masses and Approved Names from http://www.chem.qmw.ac.uk/iupac/AtWt/masses for 107-111 from C&EN, March 13, 1995, p. 35112 from http://www.gsi.de/z112e.html

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Documents

Periodic Table, Chemical Bonds, Chemical Reactions