Chemistry In Action - Wikispacesmrstorie.wikispaces.com/file/view/Terrill+Grade+10... · Web viewChemistry in Action- Periodic Table Worksheet List three typical physical properties

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Mr. Storie 20S Science Student Package – Chem Unit

ChemistryIn

Action

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Chemistry In ActionM Y X E L Z E K C A S C X G B M D I P UB A L A N C E O C W N P Y T H M Q N P BU R Q Y N P V A S J O N H S F C Y S S EA U R E C A T D X S R E O N M X S F M IL W L B L I N D I F T G E I X V D S G IU A J E O O M A S S C C W A N I O S W CV O N N B N N O Z M E E U Z M A I H C EV T Y R O E H T T K L D Q D R J R E I WQ X R K Z C U G G A E Z U U O V E L N US V G D E G T T R F Y Q F N A R P L O OT N E I C I F F E O C L W B V T P S I HE L U C E L O M S Q U D O N A S I C O BE K W Y K L T L U U E P X P T C J O I DQ I E R A R E X U A G R S N Y O S E N CH C S O Y F S B K K S K A J Q M U D Q RJ J C H E M I C A L D T T S B P K H F IF B K J L N U O G F C J C C I O H A S UE R C X J V N E N A H D Q W E U P A Q HI W H D Q U C B E F I A C S A N N D M LG A P Z L K B R C A J K R M N D M Y Q N

ANION PRODUCTS IONIC BALANCE BONDSCATION POLYATOMIC PERIODS CHEMICAL COEFFICIENTCOMPOUND SHELLS REACTANTS COVALENT ELECTRONSEQUATION MOLECULE VALENCE GROUPS IONUse your understanding of mass number and atomic number to calculate the values for the blank spaces in the table below. Place the proper symbol for the elements in the brackets.

Refer to the periodic table.

Iron (_____) Krypton (_____) Uranium (_____) Sodium (_____)

Atomic Number

Number of Protons

Lithium (_____) Chlorine (_____) Copper (_____) Silver (_____)

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Number of Protons 3 17 47

Number of Neutrons 4 34 61

Mass number 35 63

1. What is the unit of atomic mass called and what is its symbol?

2. An atom of uranium has an atomic number of 92 and an atomic mass of 238u. a. How many protons are there in one atom of uranium?

b. How many electrons are there in one atom of uranium?

c. How many neutrons are there in one atom of uranium?

d. How many protons are there in 10 atoms of uranium?

e. What is the atomic mass of uranium?

f. What is the mass number of uranium?

3. Concept maps show connections between ideas. The start of a concept map is shown below. Complete the concept map using the terms below.

One u (+) charge Very small mass no charge travels around nucleusNeutron (-) charge energy levels Electron located in nucleus Proton One u located in nucleus

ATOMNucleus

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Chemistry in Action- Periodic Table Worksheet

1. List three typical physical properties of (a) metals, (b) non-metals.

2. How are elements arranged in the periodic table organized?

3. What do we mean by a “group” of elements? Name the first and last element in group VIA (6A).

4. What do we mean by a “period” of elements? Name the first and last element in period 3.

5. What types of changes do we see of the elements in the Periodic Table from left to right?

6. What are the rules about the arrangement of electrons in energy levels?

7. What is the relationship between an element's electron arrangement and its Group number?

8. Draw Bohr diagrams for Lithium, Sodium and Potassium. What is the relationship between an element's electron arrangement and its Period number?

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9. Use the Periodic table on this page to label:

a. Where metals and non-metals are located.b. The 5 element familiesc. The number of valence electrons for each family.

PERIODIC TABLE SEARCH

OK detectives, grab your periodic tables and proceed to solve the mystery of the missing elements. You can use your textbook and notes if you think it will help.

1. Find and write down the names and the atomic number of the following elements:a. Sc h. Re o. Wb. Mg i. Tl p. Hec. Bi j. Tc q. Pbd. Ni k. U r. Sie. Pt l. Ne s. Agf. Sn m. Cs t. Sg. Cf n. Zn

2. Find and write down all the elements whose name begins with an R.

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3. Find and write down at least 4 elements that are named after countries, states, or other places on Earth.

4. Find at least 3 elements that are named after scientists (write element and scientist names).

5. Find the number of metals in the periodic table in your science book.

6. Find the number of non-metals in the periodic table in your science book.

7. Find the number of elements that have only one letter for their symbol.

8. Find at least 3 elements that are named after planets or outer-space objects (write element and object).

9. What is the symbol for an important mineral in your body that is found in milk, cheese, bones and teeth?

10. The element found in Period 3, Group VIA (16) –

11. The element found in Period 2, Group 13 –

12. The gas element used in good party balloons –

13. The gas element found in fancy restaurant lights –

14. The element used to purify water –

15. A liquid element used in old thermometers –

16. The element used to shield your body during x-rays –

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17. The element used most in electrical wiring –

18. The solid elements used in most common pencils (not lead) –

19. The radioactive element used as a fuel in nuclear reactors -

20. Some element symbols are based on the Greek and Latin names given when discovered. Use the Latin names listed below to try and find what elements they are:

Element Symbol Latin NameStibiumCuprumAurumFerrum

PlumbumHydragyrum

KaliumArgentumNatriumStannumWolfram

Do the practice questions below to build your skill in writing formulas for ionic compounds.

1. Use the periodic table to complete the table.

Element Number of Electrons Lost or Gained

Positive or Negative Ion Charge on Ion

Sulphur

Boron

Calcium

Chlorine

Phosphorus

Iodine

Nitrogen

Potassium

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Mr. Storie 20S Science Student Package – Chem Unit2. Use the diagram below to answer the following questions.

a. Use the periodic table to name this element. b. To which family does this element belong? c. Would you classify this element as a metal or non-metal? d. How many electrons would you expect this element to lose when it becomes an ion? e. What is the charge of this element when it becomes an ion? f. Would this element be more likely to combine with chlorine or lithium? g. Draw a Bohr diagram for the ion that is normally formed from the atom shown above.

3. Use Bohr model diagrams to illustrate the compounds formed from the following ion. a. Li1+ and Cl1- b. Ca2+ and O2-

c. Na1+ and S2- d. Al3+ and F1-

COMPLETE THE FOLLOWING TABLE ON LEWIS DOT DIAGRAMS

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COMPLETE THE FOLLOWING TABLE ON LEWIS DOT DIAGRAMS AND IONS

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Using the ions above: Construct 3 ionic compounds using the Dot diagrams to show how they fit together.

ANSWER THE FOLLOWING QUESTIONS ABOUT IONS and IONIC BONDING:

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Mr. Storie 20S Science Student Package – Chem Unit1. Complete the following table:

Element Atomic Number

Metal or Nonmetal

Group(Family Name)

# Of Valence Electrons

Electrons Gained or Lost

Ion Formed

Sodium 11 Metal 1A (Alkali metal) 1 1 lost Na+

37Phosphorus

Br -

Sulfur19

N-3

Krypton34

Calcium56

Iodine

2. Name the following binary ionic compounds.

These questions are straight forward with no metal ions with more than one possible valence.

Formula Name Formula Name

MgS SrF2

KBr Li2S

Ba3N2 SrCl2

Al2O3 CaO

NaI AlP

3. Use Lewis Dot Diagrams to illustrate the formation of the following compounds.

Beryllium fluoride

Lithium chloride

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Mr. Storie 20S Science Student Package – Chem Unit4. Name the following binary ionic compounds.

These questions require the use of brackets for the names of metal ions with more than one possible valence.

Formula Name Formula Name

Cr2S3 CuF2

FeBr2 CuS

Pb3N2 CoCl2

Co2O3 PbO

CuI CrP

5. Write formulas for the following compounds that are named using the Criss-Cross method. You will need to use the periodic table plus the table of combining capacity.

Name Formula Name Formula

Magnesium nitride Bismuth(V) fluoride

Lithium sulfide Manganese(II) bromide

Strontium bromide Iron(III) chloride

Aluminum chloride Lead(IV) oxide

Potassium phosphide Potassium chloride

Barium oxide Sodium oxide

Chromium (III) sulfide Calcium bromide

Tin (IV) nitride Magnesium oxide

Tin (II) oxide Aluminum fluoride

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6. Write formulas for compounds formed from the following elements, and provide a compound name. a. Sodium and bromine

b. Potassium and oxygen

c. Aluminum and sulfur

d. Barium and chlorine

e. Lithium and oxygen

f. Silver (I) and chlorine

7. Use the diagram below to answer the following questions.

a. Use the periodic table to name this element. b. What family does this element belong to?

c. Would you classify this element as a metal or non-metal?

d. How many electrons would you expect this element to lose when it becomes an ion?

e. What is the charge of this element when it becomes an ion?

f. Would this element be more likely to combine with chlorine or lithium?

g. Draw the ion that is normally formed from the atom depicted above.

8. Use the Bohr diagram of the element below to answer the following questions.

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a. Use the periodic table to name this element. b. What family does this element belong to?

c. Would you classify this element as a metal or non-metal?

d. How many electrons would you expect this element to gain when it becomes an ion?

e. What is the charge of this element when it becomes an ion?

f. Would this element be more likely to combine with sodium or calcium?

Naming Ionic CompoundsI. Binary compounds: two elements have reacted.

a. Write the name of the positive ion (metal) first and change the ending of the second element (non-metal) to ide.

Name the following binary compounds:

NaI

Na2S

AgCl

CaS2

K2O

Li2O

Mg3N2

Cs3P

CaBr2

KF

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Mr. Storie 20S Science Student Package – Chem UnitBeCl2

MgO

BeO

BaS

MgS

RbF

Fr2O

RaCl2

SrSe

Give the formula for the following binary compounds:

Aluminum chloride

Lithium oxide

Magnesium sulphide

Sodium bromide

Calcium phosphide

Silicon oxide

Cesium sulphide

Rubidium nitride

Potassium carbide

Sodium chloride

Strontium oxide

Barium fluoride

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Mr. Storie 20S Science Student Package – Chem UnitCalcium selenide

Aluminum iodide

Calcium carbide

Francium nitride

Beryllium sulphide

Radium phosphide

b. If a metal has more than one combining power (charge), put a Roman numeral after the name of the metal to show which charge it is:Copper (I) or Copper (II) - Cu1+ or Cu2+

Lead (II) or Lead (IV) - Pb2+ or Pb4+

Give the formula for the following binary compounds:

Iron (II) oxide

Germanium (III) bromide

Cobalt (III) chloride

Chromium (II) iodide

Mercury (I) phosphide

Mercury (II) bromide

Lead (IV) fluoride

Tin (IV) sulphide

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Mr. Storie 20S Science Student Package – Chem UnitCopper (II) selenide

Chromium (III) sulphide

Tin (II) oxide

Iron (III) iodide

Gold (III) iodide

Vanadium (II) sulphide

Thallium (III) bromide

Uranium (VI) oxide

Bismuth (V) phosphide

Determine the combining capacity of the metal by using the reverse criss-cross rule:

Cu2O

CrCl2

CuO

CrS

CuS

CrI3

VCl5

BiBr5

CuI

PbO2

HgO

PbS

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Mr. Storie 20S Science Student Package – Chem UnitHgCl

PbCl4

HgF2

SnO

FeO

CoCl2

Fe2S3

CoCl3

FeS

Au2O3

CoO

Covalent Bonding - Worksheet

1. How does a covalent bond differ from an ionic bond?

2. How are positive ions formed? Give with an example.

3. What is the octet rule?

4. What is a diatomic molecule?

5. Name all the diatomic elements without referring to your notes or any of the pages.

6. What is one covalent compound called (eg. one H20) ?

7. A list of pairs of atoms is shown below. Indicate whether each pair would form a compound using an ionic bond or a covalent bond.

Reacting atoms Type of bond (ionic or covalent) Calcium and bromineHydrogen and oxygen

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Mr. Storie 20S Science Student Package – Chem UnitCarbon and oxygenLithium and oxygenPhosphorus and chlorine

8. Which subatomic particles actually participate in the events during chemical bonding?

9. Is Cs3N the formula of a covalent compound? __________ 10. Is C3N4 the formula of a covalent compound? __________ 11. How did you make your decision?

12. State a rule for predicting which element combinations form covalent compounds.

13. Why is it difficult to write correct formulas for the following compounds: chalk, gasoline, alcohol, and rust?

14. Identify the type of substance formed by the atom pair (ionic compound, covalent compound, or element) and the smallest part of that substance (formula unit, molecule).

Atoms Type of Substance Smallest Particle of the SubstanceNitrogen, ChlorineMagnesium, OxygenCalcium, NitrogenCarbon, BromineTin, FluorinePhosphorus, IodineIodine, Iodine

15. Write names for the following covalent compounds.

PBr3

HF

CF4

P2O3

16. Write formulas for the following covalent compounds

Phosphorus pentasulfide

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Nitrogen monoxide

Carbon tetraiodide

Nitrogen dioxide

Carbon tetrafluoride

Nitrogen monoxide

Dinitrogen tetroxide

Silicon disulfide

17. Write the names for the following compounds

H2S

As2O3

CBr4

OI2

Na2O

ANSWER THE FOLLOWING QUESTIONS ABOUT CHEMICAL COMPOUNDS:

1. List the names of the 5 families of the periodic table and write their combining capacity.

2. A new element has been discovered. It is named element X. It is known to be an alkali metal. What is the formula when X combines with

iodine? ______ sulfur? ______

3. A new element has been discovered. It is named element Z. It is known to be a halogen. What is the formula when Z combines with

sodium? ______ calcium? ______

4. Identify the type of compound (ionic or covalent) for each of the following. Write the name according to IUPAC rules. Type your answer in the table below.

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Formula Type of Compound Name of Compound

CBr4

CaS

PI3

SO2

AlF3

Na2S

BN

SiF4

CoCl2

CuO

5. Identify the type of compound (ionic or covalent) for each of the following. Write the formula according to IUPAC rules. Type your answer in the table below.

Name of Compound Type of Compound Formula

Phosphorus pentoxide

Chromium (III) chloride

Iron (II) oxide

Tin (IV) sulfide

Carbon monoxide

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Trisilicon tetranitride

Aluminum sulfide

Dichlorine monoxide

Dinitrogen tetrahydride

Barium nitride

6. Draw a Lewis Dot diagram for a covalent bond involving oxygen and chlorine.

7. Draw a Lewis Dot diagram for an ionic bond involving oxygen and magnesium.

Counting Atoms Sheet

Name each of the following chemical compounds (make sure you use the right naming scheme!) and determine how many atoms of each element are present:

Use the key at the bottom of the page for the polyatomic ions (in brackets).

1) CaF2 ______________________________________________________

2) Be(OH)2 ____________________________________________________

3) NO2 ______________________________________________________

4) Al2(SO4)3 ___________________________________________________

5) NH4NO3 ____________________________________________________

6) S2F2 ______________________________________________________

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Mr. Storie 20S Science Student Package – Chem Unit7) Na2CO3 ____________________________________________________

8) CH4 ______________________________________________________

Write the formulas for each of the following chemical compounds (make sure you use the right naming scheme!) and determine how many atoms of each element are present:

9) phosphorus trichloride _________________________________________

10) magnesium hydroxide _________________________________________

11) potassium phosphate _________________________________________

12) diphosphorus tetrabromide _____________________________________

13) nitrogen trihydride (ammonia) _________________________________________

14) germanium (IV) phosphate ________________________________________

15) ammonium sulfate _________________________________________

16) diphosphorus pentoxide _______________________________________

Polyatomic Ions:ION Charge ION ChargeHydroxide (OH) -1 Nitrate (NO3) -1Sulphate (SO4) -2 Carbonate (CO3) -2Phosphate (PO4) -3 Ammonium (NH4) +1

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Mr. Storie 20S Science Student Package – Chem UnitBALANCE THE FOLLOWING CHEMICAL REACTIONS:**Name all compounds highlighted **

1. _____ Fe + _____ S _____ FeS

2. _____ H2 + _____ Cl2 _____ HCl

3. _____ Mg + _____ O2 _____ MgO

4. _____ O2 + _____ H2 _____ H2O

5. _____ HgO _____ Hg + _____ O2

6. _____ CH4 + _____ O2 _____ CO2 +____ H2O

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Mr. Storie 20S Science Student Package – Chem Unit7. _____ N2 + _____ H2 _____ NH3

8. _____ Al + _____ O2 _____ Al2O3

9. _____ Na + _____ H2O _____ NaOH + _____ H2

10. _____ Ca + _____ H2O _____ Ca(OH)2 + _____ H2

11. _____ Na2O2 + _____ H2SO4 _____ Na2SO4 + _____ H2O2

12. _____ KMnO4 _____ K2O + _____ MnO + _____ O2

BALANCE THE FOLLOWING CHEMICAL REACTIONS:**Name all compounds highlighted **

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1) ____ N2 + ____ H2 ____ NH3

2) ____ H2 + ___ O2 ____ H2O

3) ____ KClO3 ____ KCl + ____ O2

4) ____ NaCl + ____ F2 ____ NaF + ____ Cl2

5) ____ H2O + ____ O2 ____ H2O2

6) ____ P4 + ____ O2 ____ P2O5

7) ____ S8 + ____ O2 ____ SO3

8) ____ NaBr + ____ CaF2 ____ NaF + ____ CaBr2

9) ____ Na + ____ H2O ____ NaOH + ____ H2

10) ____ Ag2O ____ Ag + ____ O2

11) ____ CH4 + ____ O2 ____ CO2 + ____ H2O

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12) ____ FeCl3 + ____ NaOH ____ Fe(OH)3 + ____ NaCl

13) ____ C3H8 + ____ O2 ____ CO2 + ____ H2O

14) ____ AgNO3 + ____ MgCl2 ____ AgCl + ____ Mg(NO3)2

15) ____ AlBr3 + ____ K2SO4 ____ KBr + ____ Al2(SO4)3

16) ____ CO2 + ____ H2O ____ C6H12O6 + ____ O2

17) ____ K + ____ MgBr2 ____ KBr + ____ Mg

18) ____ KCl + ____ CaCO3 ____ CaCl2 + ____ K2CO3

19) ____ HNO3 + ____ NaHCO3 ____ NaNO3 + ____ H2O + ____ CO2

20) ____ C8H18 + ____ O2 ____ CO2 + ____ H2O

21) ____ Pb(OH)2 + ____ HCl ____ H2O + ____ PbCl2

22) ____ H2SO4 + ____ NaNO2 ____ HNO2 + ____ Na2SO4

COMPLETE THE FOLLOWING QUESTIONS ABOUT REACTION TYPES:

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Mr. Storie 20S Science Student Package – Chem Unit1. Identify which type of reaction has the following reactants.

Types of Reactants Type of Reaction

Two compounds

One element and one compound

Two elements

One compound

2. Balance and classify each of the following reactions.

Reaction Type of Reaction

C6H12 + O2 → CO2 + H2O

Ag + S → Ag2S

Mg + HCl → MgCl2 + H2

KNO3 → KNO + O2

HCl + NaOH → H2O + NaCl

Cl2 + KBr → KCl + Br2

Fe + O2 → Fe2O3

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C7H16 + O2 → CO2 + H2O

KClO3 → KCl + O2

SiO2 + HF → SiF4 + H2O

Ca + AlCl3 CaCl2 + Al

Si + S8 Si2S4

C2H5OH + O2 CO2 + H2O

Ca + AlCl3 CaCl2 + Al

N2 + H2 NH3

Fe(s) + O2(g) FeO(s)

Cl2(aq) + KBr(aq) KCl(aq) + Br2(aq)

Ag2O(s) Ag(s) + O2(g)

CH4(g) + O2(g) CO2(g) + H2O(g)

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3. Name each reactant and product properly underneath, then identify the type of reaction. a. Fe(s) + CuS(aq) FeS(aq) + Cu(s)

b. 4 Fe(s) + 3 O2(g) 2 Fe2O3(s)

c. BaF2(aq) + 2 LiBr(aq) BaBr2(aq) + 2 LiF(aq)

d. CH4(g) + 2 O2(g) CO2(g) + 2 H2O(g)

e. 2 MgO(s) 2 Mg(s) + O2(g)

4. Complete and balance the following equations. a. C8H8(l) + O2(g) (combustion)

b. Al(s) + I2(g) (synthesis)

c. BeF2(aq) + K2O(aq) (double displacement)

d. Cl2(g) + NaBr(aq) (single displacement)

e. NaCl(l) (decomposition)

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5. Predict and write the product(s) and identify the type of reaction. The formula must be correct and balanced to receive credit.

a. Ca + O2 →

b. C9H20 + O2 →

c. Na + MgBr2 →

d. ZnCl2 + AgF →

6. Write a balance equation from the description given and identify the reaction type: a. Solid magnesium and oxygen gas produce solid magnesium oxide.

b. Aqueous hydrogen monochloride and solid zinc produce hydrogen gas and solid zinc (II) chloride.

c. Tetracarbon octahydride (butane) gas burns with oxygen gas to yield carbon dioxide gas and water vapour.

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COMPLETE THE FOLLOWING WORD EQUATIONS:

1. Balance the following skeleton equations: a. C + S CS2 b. Al + Cl2 AlCl3

c. Ba + O2 BaO d. Na + O2 Na2O

e. B + O2 B2O3

2. Write word equations for the skeleton equations in question #1. Include the representative particles (atom, molecule or formula unit) for each substance.

a. C + 2 S CS2

One atom of carbon plus two atoms of sulfur will produce one molecule of carbon disulfide.

3. Translate the following word equations to balanced chemical equations. Include the states for each substance. a. Solid sodium metal combines with chlorine gas to produce sodium chloride crystals.

b. Solid magnesium reacts with aqueous hydrogen chloride to produce a aqueous magnesium chloride solution and hydrogen gas.

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Mr. Storie 20S Science Student Package – Chem Unitc. Aqueous potassium iodide reacts with solid calcium sulfide to produce solid potassium sulfide

and aqueous calcium iodide.

d. Solid silver oxide decomposes to produce silver metal and oxygen gas.

4. Translate the following chemical equations to word equations. Include the states and representative particles for each substance.

a. Fe (s) + CuS (aq) FeS (aq) + Cu (s) One atom of solid iron plus one formula unit of aqueous copper (II) sulfide reacts to produce one aqueous formula unit of iron (II) sulfide and one atom of solid copper.

b. 4 Fe (s) + 3 O2 (g) 2 Fe2O3 (s)

c. BaF2 (aq) + 2 LiBr (aq) BaBr2 (aq) + 2 LiF (aq)

d. CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)

e. 2 MgO (s) 2 Mg (s) + O2 (g)

5. Label the following parts of a chemical equation on the equation given below:

Reactants Products Subscripts Phases Coefficients

CH4 (g) + 2 O2 (g) CO2 (g) + 2 H2O (g)

6. Why can you change the value of a coefficient but not a subscript when balancing an equation.

7. What is meant when we say calcium chloride is in an aqueous state?

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ANSWER THE FOLLOWING QUESTIONS ON ACIDS AND BASES:

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ANSWER THE FOLLOWING QUESTIONS ON ACIDS AND BASES:

1. Compare and contrast the terms “acids” and “bases”.

How are they the same?

How are they different?

2. State whether the liquids in the following examples illustrate an acid (A) or a base(B).

Has a pH of 12. A liquid feels slippery between your fingers. You taste a beverage and it has a pleasant sour taste It tastes bitter.It is used as a household cleanser.A liquid is added to colourless phenolphthalein, causing it to turn pink. A liquid turns blue litmus red Has a pH of 6

3. Place the formulas of the acids under the heading ”acids” and the formulas for bases under the heading “bases”. If it is not an acid or a base, do not place it under either heading.

NH4OH KCl H2SO4 Mg(OH)2 AlCl3 HCl H2CO3 KOH HNO3 H2O HBr Al(OH)3

Acid Base

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HCl(aq) + NaOH(aq) NaCl(aq) + H2O

1. Name the reactants and products in the above reaction.

Reactants

Products

What does the subscript “(aq)” mean?

2. Balance the neutralization reactions shown below. Name each of the compounds (except water) in each equation.

HBr + KOH KBr + H2O

HI + NaOH NaI + H2O

7. For each of the following neutralization reactions, write the formulas of the products, balance the equation.

HF + Ca(OH)2

HI + Al(OH)3

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Complete the following questions on acids, bases and neutralization:

1. The diagram below is a word cycle. Read the list of words in the middle. Select one word and place it in any oval. In the next oval place another word that is related to the first. Plan ahead; the last few words will be tricky to place. You may wish to add some linking comments between words to make the ideas flow better.

2. A double replacement reaction in general form is shown below.

Compound + compound → compound + compound

Use the neutralization reaction between hydrochloric acid and sodium hydroxide to illustrate how a neutralization reaction is a double displacement reaction.

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3. Balance the following neutralization reactions.

HNO3 + RbOH → RbNO3 + H2O

HI + Mg(OH)2 → MgI2 + H2O

H2SO4 + Ba(OH)2 → BaSO4 + H2O

4. For each of the following neutralization reactions, write the formulas of the products, balance the equation and name the salt produced.

HBr + KOH →

HF + Mg(OH)2 →

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Chemistry Unit Review

1. What color does litmus paper turn in a. acids? b. bases?

2. The number of protons in an atom can be determined from the ________________.

3. How many of each type of atom is in the compound dinitrogen pentoxide?

4. Write the formula for the above compound

5. Ionic compounds form between __________ and ______________.

6. Covalent compounds from between two ______________.

7. Define the following terms:a. period b. family

8. Name 5 families on the periodic table.

9. Which of the above families does not react?

10. Give an example for each of the following reaction types:a. Addition (synthesis)

b. Decomposition

c. Single replacement

d. Double replacement

e. Combustion

11. Name 4 characteristics for acids and 4 characteristics for basesoo

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Mr. Storie 20S Science Student Package – Chem Unitoooooo

12. The element lithium has an atomic number of 3 and a mass number of 7. How many neutrons does it have?

13. How many electrons are in the outer orbit of rubidium (atomic number 37, atomic mass 85), a member of the alkali metals?

14. What is a chemical family?

15. How are ionic compounds formed? What subatomic particle is involved?

16. How do covalent compounds form?

17. What is the charge on calcium when it forms an ion?

18. What information does the combining capacity of an element provide?

19. What is the charge that results when a halogen forms an ion?

20. What are the characteristics of acids?

21. How do you carry out a neutralization reaction? (what do you mix)

22. What family is the most unreactive. Why?

23. Which chemical bonds are the result of electron transfer?

24. When sodium and chlorine react together to produce sodium chloride, what type of reaction is occurring?

25. Which of the following is a correctly balanced chemical equation?a. H2 + O2 H2Ob. H2 + 2 O2 H2O2

c. H2 + O2 2 H2Od. 2 H2 + O2 2 H2O

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Mr. Storie 20S Science Student Package – Chem Unit26. What is an endothermic reaction?

27. What is the general form of a single replacement reaction?

28. When performing a chemistry lab for Mr. Storie, you mix two solutions together. You observe that the beaker containing the solutions felt hot to the touch. What kind of a reaction is this?

29. What is the general form of a double replacement reaction?

30. You add aluminum to a blue solution of CuCl2 , after some evidence that a chemical reaction has occurred, you notice a reddy-brown solid forming on the bottom of the beaker. What is this brown substance? What kind of a reaction is this?

31. What happens in a chemical reaction?

32. What kind of information is provided by a chemical equation?

33. Match the following terms:

___1. Ion a. results from electron sharing___2. Atom b. a reaction that gives of heat___3. Electron c. the attraction between positive and negative ions___4. Proton d. a positively charged particle___5. Ionic bond e. a reaction that absorbs energy___6. Covalent bond f. an atom/group with a charge on it___7. Isotopes g. a negatively charged particle___8. Endothermic reaction h. the smallest particle of an element that exists by itself

i. atoms of the same element with different massesj. a neutral particle

34. Use the following information to answer the following questions: Mr. Storie spends his free time trying to find new elements. Recently she discoved a new element called Storium – its symbol is St. The only Thing we know about this new element is that it is an alkali metal.

Write the formula when it combines with the following:a. Iodine:b. Sulphur:c. Carbonate (polyatomic – look through your notes)

35. The following are covalent compounds. Write the formula for the following element pairs:

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Mr. Storie 20S Science Student Package – Chem Unita. dinitrogen trioxide – b. carbon tetrachloride –

36. Name the following covalent compounds:a. CF4

b. P2O3

37. Write the products of the following reaction:Acid + base +

38. Balance the following equations. Leave the space blank or add a “1” if no coefficient is required.a. HgO Hg + O2

b. Fe + H2O Fe3O4 + H2

c. Pb3O4 PbO + O2

39. Name all of the above compounds in each reaction:a.b.c.

40. How many sulfur atoms are in disulphur trioxide?

41. What is a mass number?

42. What is a period?

43. What are diatomic molecules? What elements does this apply to?

44. List the characteristics of a base. Give some examples?

45. What is phenolphthalein? What does it do?

46. Name the following ionic compounds:a. NaClb. BeCl2

c. Fe2O3

47. Write formulas for the following ionic compounds:a. Potassium iodideb. Silver nitratec. Gold (II) oxide

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48. What is combustion? What are the products?

49. What is a cation? How is it different from an anion?

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Chemistry In Action - Wikispacesmrstorie.wikispaces.com/file/view/Terrill+Grade+10... · Web viewChemistry in Action- Periodic Table Worksheet List three typical physical properties