Chemistry term 1 review sheet- Vacation homework 50 Pts

Chemistry term 1 review sheet- Vacation homework 50 Pts

Name: Date:

1. In the modern Periodic Table, the elements arearranged in order of increasing

A. atomic number B. mass number

C. oxidation number D. valence number

2. Which symbol represents an alkaline earthelement?

A. Na B. Mg C. Ne D. Ag

3. More than two-thirds of the elements are classifiedas

A. nonmetals B. metals

C. metalloids D. noble gases

4. In the reaction Zn + Cu2+ → Zn2+ + Cu, the Cu2+

ions

A. gain electrons B. lose electrons

C. gain protons D. lose protons

5. Which particle has the largest radius?

A. F− B. Ne C. Cl− D. Ar

6. As the elements in Group IA are considered inorder of increasing atomic number, the atomicradius of each successive element increases. Thisis primarily due to an increase in the number of

A. neutrons in the nucleus

B. electrons in the outermost shell

C. unpaired electrons

D. principal energy levels

7. Which is the most active nonmetal in the PeriodicTable of the Elements?

A. Na B. F C. I D. Cl

8. Which of the following atoms has the smallestcovalent atomic radius?

A. Li B. Be C. C D. F

9. As the elements of Group 16 (VIA) are consideredfrom top to bottom on the Periodic Table, thecovalent radii

A. increase and the ionization energies decrease

B. increase and the ionization energies increase

C. decrease and the ionization energies increase

D. decrease and the ionization energies decrease

10. Which element in Period 2 has the greatesttendency to form a negative ion?

A. lithium B. carbon

C. neon D. fluorine

11. The most active metal in Group 2 (IIA) is

A. Mg B. Sr C. Ba D. Ca

12. Which element in Period 3 has the greatesttendency to gain electrons?

A. Na B. Si C. Cl D. Ar

13. The highest ionization energies in any period arefound in Group

A. 1 (IA) B. 2 (IIA)

C. 17 (VIIA) D. 18 (O)

page 1

14. Element M is a metal and its chloride has theformula MCl2. To which group of the PeriodicTable does element M most likely belong?

A. 1 (IA) B. 2 (IIA)

C. 15 (VA) D. 17 (VIIA)

15. As the elements in Group 2 (IIA) of the PeriodicTable are considered in order from top to bottom,the number of electrons in the valence shell

A. decreases B. increases

C. remains the same

16. As the elements of Group 17 (VIIA) are consideredin order of increasing atomic number, thenonmetallic character of each successive element


C. remains the same

17. Which diagram correctly shows the relationshipbetween electronegativity and atomic number forthe elements of Period 3?

A.

B.

C.

D.

18. Which properties are characteristic of the Group 1(IA) metals?

A. high reactivity and the formation of stablecompounds

B. high reactivity and the formation of unstablecompounds

C. low reactivity and the formation of stablecompounds

D. low reactivity and the formation of unstablecompounds

50 Pts page 2 Chemistry term 1 review sheet- Vacation homework

19. In which category of elements in the PeriodicTable do all of the atoms have valence electronsin the second principal energy level?

A. Group 2 (IIA)

B. Period 2

C. the alkaline earth family

D. the alkali metals family

20. Which element in Period 2 of the Periodic Tableis the most reactive nonmetal?

A. carbon B. nitrogen

C. oxygen D. fluorine

21. Which sequence of Group 18 elementsdemonstrates a gradual decrease in the strength ofthe van der Waals forces?

A. Ar(`), Kr(`), Ne(`), Xe(`)

B. Kr(`), Xe(`), Ar(`), Ne(`)

C. Ne(`), Ar(`), Kr(`), Xe(`)

D. Xe(`), Kr(`), Ar(`), Ne(`)

22. Which of these elements in Period 3 has the leasttendency to attract electrons?

A. Mg B. Al C. S D. Cl

23. The data table below shows elements Xx, Yy,and Zz from the same group on the Periodic Table.

Element Atomic Mass(atomic mass unit)

Atomic Radius(pm)

Xx 69.7 141

Yy 114.8 ?

Zz 204.4 171

What is the most likely atomic radius ofelement Yy?

A. 103 pm B. 127 pm

C. 166 pm D. 185 pm

24. Element X reacts with iron to form two differentcompounds with the formulas FeX and Fe2X3. Towhich group on the Periodic Table does element Xbelong?

A. Group 8 B. Group 2

C. Group 13 D. Group 16

25. As the elements of Group 17 are considered inorder of increasing atomic number, there is anincrease in

A. atomic radius

B. electronegativity

C. first ionization energy

D. number of electrons in the first shell


26. Base your answer(s) to the following question(s) on the information below.

The atomic number and corresponding atomic radius of the Period 3 elements are shown in the datatable below.

Data Table

AtomicNumber

AtomicRadius(pm)

11 160.

12 140.

13 124

14 114

15 109

16 104

17 100.

18 101

On the grid below, mark an appropriate scale on the axis labeled “Atomic Radius (pm).”


27. State the general relationship between the atomicnumber and the atomic radius for the Period 3elements.

28. Base your answer(s) to the following question(s)on the information below and on your knowledgeof chemistry.

Before atomic numbers were known,Mendeleev developed a classification systemfor the 63 elements known in l872, usingoxide formulas and atomic masses. He usedan R in the oxide formulas to represent anyelement in each group. The atomic mass waslisted in parentheses after the symbol of eachelement. A modified version of Mendeleev’sclassification system is shown in the tablebelow.

Identify one characteristic used by Mendeleev todevelop his classification system of the elements.

29. Based on Table J, identify the least active metallisted in Group I on Mendeleev’s table.

30. A piece of copper metal is correctly placed on atriple-beam balance. The riders at the zero markexcept for the rider on 0–10 gram beam which islocated at the position shown. What is the massof the copper metal?

A. 0.455 g

B. 4.56 g

C. 0.55 g

D. 5.50 g

31. The diagram shown represents a portion of atriple-beam balance. If the beams are in balance,with the riders in the position shown, what is thetotal mass in grams of the object being massed?

A. 460.62 B. 466.20

C. 466.62 D. 460.20

32. Which device should be used to accuratelymeasure a volume of 16.30 milliliters?

A. B.

C. D.

33. A student has to measure the diameter of a testtube in order to calculate the tube’s volume.Based on the diagram shown, the tube’s diameteris closest to

A. 1.25 cm

B. 2.32 cm

C. 3.25 cm

D. 12.5 cm


34. If the rules for significant figures are observed inthe addition example shown, how should the totalfor this addition be rewritten?

A. 5,610.00 B. 5,610.340

C. 5,610.34 D. 5,610.3

35.7432.33

5,142.312+

5,610.342

35. Which measurement contains a total of threesignificant figures?

A. 0.01 g B. 0.010 g

C. 0.0100 g D. 0.01000 g

36. The following weighings were made during alaboratory exercise:

Mass of evaporating dish . . . . . . . . . . . 59.260 gMass of sugar sample . . . . . . . . . . . . . . . . . 1.61 g

What is the total mass of the evaporating dishplus the sample, expressed to the proper numberof significant figures?

A. 60.870 g B. 60.87 g

C. 60.9 g D. 61 g

37. Which volume measurement is expressed in foursignificant figures?

A. 5.50 mL B. 550 mL

C. 5,500 mL D. 55,000 mL

38. The diagram shows a section of a 100-millilitergraduated cylinder. When the meniscus is readto the correct number of significant figures, thevolume of water in the cylinder would be recordedas

A. 75.7 mL

B. 75.70 mL

C. 84.3 mL

D. 84.30 mL

39. Base your answer(s) to the following question(s)on the table below.

Physical Properties of Four Gases

Name of Gas hydrogen hydrogenchloride

hydrogenbromide

hydrogeniodide

Molecular Structure H-H H-Cl H-Br H-I

Boiling Point (K) at 1 Atm 20. 188 207 237

Density (g/L) at STP 0.0899 1.64 ? 5.66

The density of hydrogen at STP is 0.0899 gramper liter. Express this density to two significantfigures.

40. Of the following groups, the element with thelowest ionization energy would be found in Group

A. IIA B. O C. VIIA D. IVA

41. Which group contains elements that are obtainedby the electrolytic reduction of their fused salts?

A. 1 (IA) B. 12 (IIB)

C. 14 (IVA) D. 16 (VIA)

42. Which group in the Periodic Table containselements that are all monatomic gases at STP?

A. 15 B. 16 C. 17 D. 18


43. Which element is a noble gas?

A. krypton B. chlorine

C. antimony D. manganese

44. Base your answer(s) to the following question(s)on the information below, which describes theproposed discovery of element 118.

In 1999, a nuclear chemist and histeam announced they had discovered a newelement by crashing krypton atoms into lead.The new element, number 118, was assignedthe name ununoctium and the symbol Uuo.One possible isotope of ununoctium couldhave been Uuo-291.

However, the discovery of Uuo was notconfirmed because other scientists couldnot reproduce the experimental resultspublished by the nuclear chemist and histeam. In 2006, another team of scientistsclaimed that they produced Uuo. This claimhas yet to be confirmed.

Adapted from Discover January 2002

Based on atomic number, in which group on thePeriodic Table would element 118 be placed?

45. All the elements in Period 3 have the samenumber of

A. occupied sublevels

B. principal energy levels

C. electrons

D. protons

46. Which element in Period 3 exists as diatomicmolecules at STP?

A. argon B. chlorine

C. aluminum D. sodium


The diagram below represents threeelements in Group 13 and three elements inPeriod 3 and their relative positions on thePeriodic Table.

Some elements in the solid phaseexist in different forms that vary in theirphysical properties. For example, at roomtemperature, red phosphorus has a densityof 2.16 g/cm3 and white phosphorus has adensity of 1.823 g/cm3.

Identify one element from the diagram that willcombine with phosphorus in the same ratio ofatoms as the ratio in aluminum phosphide.

48. Consider the Period 3 elements in the diagram inorder of increasing atomic number. State the trendin electronegativity for these elements.

49. Identify the element from the diagram that willreact with chlorine to form a compound with thegeneral formula XCl4.

50. Which element would have properties characteristicof both a metal and a nonmetal?

A. Ag B. K C. Si D. Xe

51. At STP, which of the following elements has themost metallic character?

A. iodine B. bromine

C. chlorine D. fluorine


52. Which noble gas would most likely form acompound with fluorine?

A. helium B. neon

C. argon D. xenon

53. Which list of particles is in order of increasingmass?

A. proton → electron → alpha particle

B. proton → alpha particle → electron

C. electron → proton → alpha particle

D. alpha particle → electron → proton

54. Which element is a solid at STP?

A. H2 B. I2 C. N2 D. O2

55. What is conserved during a chemical reaction?

A. mass, only

B. charge, only

C. both mass and charge

D. neither mass nor charge

56. Given the particle diagram:

At 101.3 kPa and 298 K, which element could thisdiagram represent?

A. Rn B. Xe C. Ag D. Kr

57. Base your answer(s) to the following question(s)on the information below.

A substance is a solid at 15◦C. Astudent heated a sample of the solidsubstance and recorded the temperature atone-minute intervals in the data table below.

Time (min) 0 1 2 3 4 5 6 7 8 9 10 11 12

Temperature (◦C) 15 32 46 53 53 53 53 53 53 53 53 60 65

Based on the data table, what is the melting pointof this substance?

58. Which set of procedures and observations indicatesa chemical change?

A. Ethanol is added to an empty beaker and theethanol eventually disappears.

B. A solid is gently heated in a crucible and thesolid slowly turns to liquid.

C. Large crystals are crushed with a mortar andpestle and become powder.

D. A cool, shiny metal is added to water in abeaker and rapid bubbling occurs.

59. Base your answer(s) to the following question(s)on the graph below, which represents the coolingof a substance starting at a temperature above itsboiling point.

What is the melting point of this substance?



Archimedes (287-212 BC), a Greek inventorand mathematician, made several discoveriesimportant to science today. According to alegend, Hiero, the king of Syracuse, commandedArchimedes to find out if the royal crown wasmade of gold, only. The king suspected that thecrown consisted of a mixture of gold, tin, andcopper.

Archimedes measured the mass of the crownand the total amount of water displaced by thecrown when it was completely submerged. Herepeated the procedure using individual samples,one of gold, one of tin, and one of copper.Archimedes was able to determine that the crownwas not made entirely of gold without damaging it.

Identify one physical property that Archimedesused in his comparison of the metal samples.

61. Determine the volume of a 75-gram sample ofgold at STP.


A glass tube is filled with hydrogen gasat low pressure. An electric current is passedthrough the gas, causing it to emit light. Thislight is passed through a prism to separate thelight into the bright, colored lines of hydrogen’svisible spectrum. Each colored line correspondsto a particular wavelength of light. One ofhydrogen’s spectral lines is red light with awavelength of 656 nanometers.

Tubes filled with other gases producedifferent bright-line spectra that are characteristicof each kind of gas. These spectra have beenobserved and recorded.

Explain how the elements present on the surfaceof a star can be identified using bright-line spectra.


The particle diagrams below representthe reaction between two nonmetals, A2 andQ2.

Compare the total mass of the reactants to thetotal mass of the product.


The table below lists physical andchemical properties of six elements atstandard pressure that correspond to knownelements on the Periodic Table. Theelements are identified by the code letters, D,E, G, J, L, and Q.

Properties of Six Elements at Standard Pressure

Element DDensity 0.00018 g/cm3

Melting point −272◦CBoiling point -269◦COxide formula (none)

Element EDensity 1.82 g/cm3

Melting point 4◦CBoiling point 280◦COxide formula E2O5

Element GDensity 0.53 g/cm3

Melting point 181◦CBoiling point 1347◦COxide formula G2O

Element JDensity 0.0013 g/cm3

Melting point −210◦CBoiling point −196◦COxide formula J2O5

Element LDensity 0.86 g/cm3

Melting point 64◦CBoiling point 774◦COxide formula L2O

Element QDensity 0.97 g/cm3

Melting point 98◦CBoiling point 883◦COxide formula Q2O

What is the total number of elements in the“Properties of Six Elements at Standard Pressure”table that are solids at STP?


65. The table below shows mass and volume datafor four samples of substances at 298 K and1 atmosphere.

Masses and Volumesof Four Samples

Sample Mass(g)

Volume(mL)

A 30. 60.

B 40. 50.

C 45 90.

D 90. 120.

Which two samples could consist of the samesubstance?

A. A and B B. A and C

C. B and C D. C and D


An unlit candle is secured to the bottomof a 200-milliliter glass beaker. Baking soda(sodium hydrogen carbonate) is added aroundthe base of the candle as shown below.

The candle is lit and dilute ethanoicacid is poured down the inside of the beaker.As the acid reacts with the baking soda,bubbles of CO2 gas form. After a fewseconds, the air in the beaker is replaced by0.20 liter of CO2 gas, causing the candleflame to go out. The density of CO2 gas is1.8 grams per liter at room temperature.

Calculate the mass of the CO2 gas that replacedthe air in the beaker. Your response must includeboth a correct numerical setup and the calculatedresult.

67. Base your answers to the following question(s) onthe information below.

Starting as a gas at 206◦C, a sample ofa substance is allowed to cool for 16 minutes.This process is represented by the coolingcurve below.

At what time do the particles of this sample havethe lowest average kinetic energy?

68. According to an accepted chemistry reference, theheat of vaporization of water is 540 calories pergram. A student determined in the laboratory thatthe heat of vaporization of water was 620 caloriesper gram. The student’s results had a percent errorof

A. 12.9 B. 14.8 C. 80.0 D. 87.1

69. A student determined the percentage of water ofhydration in BaCl2 · 2H2O by using the data in theaccompanying table.

Quantity Measured Value Obtained

mass of BaCl2 · 2H2O 3.80 grams

mass of BaCl2 3.20 grams

% of water calculated 15.79%

The accepted percentage value for the water ofhydration is 14.75%. What is the student’s percenterror?

A. 1.04% B. 6.00% C. 6.59% D. 7.05%

70. Which is the correct electron dot representation ofan atom of sulfur in the ground state?

A. S : B. ..S : C. .

...S : D. :

..

..S :


71. Which electron dot formula represents a moleculethat can combine with a proton (H+)?

A. H :H B. H :C :C : H

C. HH :

..

..C : HH

D. H :....N : HH

72. The correct electron dot formula for hydrogenchloride is

A. H :Cl B. :....H : Cl

C. H :....Cl : D. :H :

..Cl :

73. Which electron dot diagram represents a moleculethat has a polar covalent bond?

A. B.

C. D.

74. In the box provided below, draw the electron-dot(Lewis) structure of an atom of calcium.

75. In the box provided below, draw the electron-dot(Lewis) structure of an atom of chlorine.

76. In the box provided below, draw the electron-dot(Lewis) structure of calcium chloride.


Each molecule listed below is formedby sharing electrons between atoms whenthe atoms within the molecule are bondedtogether.

Molecule A: Cl2Molecule B: CCl4Molecule C: NH3

In the box below, draw the electron-dot (Lewis)structure for the NH3 molecule.

78. Which Lewis electron-dot diagram is correct forCO2?

A. B.

C. D.



Key

• = electron

Atomic Diagrams of Magnesium and Aluminum

Element Lewis Electron-DotDiagram

Electron-ShellDiagram

magnesium

aluminum

Identify one piece of information shown in theelectron-shell diagrams that is not shown in theLewis electron-dot diagrams.

80. Explain why Lewis electron-dot diagrams aregenerally more suitable than electron-shelldiagrams for illustrating chemical bonding.


Naturally Occurring Isotopes of Sulfur

Isotope Atomic Mass(atomic mass units, u)

Natural Abundance(%)

32S 31.97 94.9333S 32.97 0.7634S 33.97 4.2936S 35.97 0.02

Draw a Lewis electron-dot diagram for an atom ofsulfur-33.

82. The electron dot symbol X : represents

A. an alkali metal

B. an alkaline earth metal

C. a halogen

D. a transition element


Before atomic numbers were known,Mendeleev developed a classification systemfor the 63 elements known in l872, usingoxide formulas and atomic masses. He usedan R in the oxide formulas to represent anyelement in each group. The atomic mass waslisted in parentheses after the symbol of eachelement. A modified version of Mendeleev’sclassification system is shown in the tablebelow.

Based on Mendeleev’s oxide formula, what is thenumber of electrons lost by each atom of theelements in Group III?

84. Compared to a sodium atom in the ground state, asodium atom in the excited state must have

A. a greater number of electrons

B. a smaller number of electrons

C. an electron with greater energy

D. an electron with less energy

85. Which is an electron configuration for an atom ofchlorine in the excited state?

A. 2–8–7 B. 2–8–8

C. 2–8–6–1 D. 2–8–7–1


86. Base your answer(s) to the following question(s)on the diagram below, which shows bright-linespectra of selected elements.

Explain how a bright-line spectrum is produced,in terms of excited state, energy transitions, andground state.

87. Base your answer(s) to the following question(s)on the diagram below, which represents an atomof magnesium-26 in the ground state.

On the diagram below, write an appropriatenumber of electrons in each shell to represent aMg-26 atom in an excited state. Your answer mayinclude additional shells.
















An atom of element G is in the ground state.What is the total number of valence electrons inthis atom?


A fluorescent light tube contains anoble gas and a drop of mercury. Whenthe fluorescent light operates, the Hg is avapor and there are free-flowing Hg ions andelectrons in the tube. The electrons collidewith Hg atoms that then emit ultraviolet(UV) radiation.

The inside of the tube is coatedwith a mixture of several compounds thatabsorbs UV radiation. Ions in the coatingemit a blend of red, green, and blue lightthat together appears as white light. Thecompound that produces red light is Y2O3.The compound that produces green light isCeMgAl11O19. The compound that producesblue light is BaMgAl10O17.

Explain, in terms of both electrons and energy,how ions in the coating emit light.



Bond energy is the amount of energyrequired to break a chemical bond. Thetable below gives a formula and thecarbon-nitrogen bond energy for selectednitrogen compounds.

Selected Nitrogen Compounds

Compound Formula Carbon-NitrogenBond Energy

(kJ/mol)

hydrogen cyanide 890.

isocyanic acid 615

methanamine 293

Identify the noble gas that has atoms in the groundstate with the same electron configuration as thenitrogen in a molecule of isocyanic acid.

91. The diagram below represents the bright-linespectra of four elements and a bright-line spectrumproduced by a mixture of three of these elements.

Which element is not present in the mixture?

A. A B. D C. X D. Z

92. The bright-line spectra produced by four elementsare represented in the diagram below.

Given the bright-line spectrum of a mixtureformed from two of these elements:

Which elements are present in this mixture?

A. A and D B. A and X

C. Z and D D. Z and X

93. Which pair of elements form an ionic bond witheach other?

A. KCl B. ICl C. PCl D. HCl

94. In which compound does the bond between theatoms have the least ionic character?

A. HF B. HCl C. HBr D. HI

95. A white crystalline salt conducts electricity whenit is melted and when it is dissolved in water.Which type of bond does this salt contain?

A. ionic B. metallic

C. covalent D. network

96. In which compound have electrons been transferredto the oxygen atom?

A. CO2 B. NO2 C. N2O D. Na2O


97. A chemist performs the same tests on twohomogeneous white crystalline solids, A and B.The results are shown in the accompanying table.

The results of these tests suggest that

A. both solids contain only ionic bonds

B. both solids contain only covalent bonds

C. solid A contains only covalent bonds andsolid B contains only ionic bonds

D. solid A contains only ionic bonds and solid Bcontains only covalent bonds

98. Base your answers to the following question(s) onthe information below.

During a fireworks display, salts are heatedto very high temperatures. Ions in the salts absorbenergy and become excited. Spectacular colors areproduced as energy is emitted from the ions in theform of light.

The color of the emitted light is characteristicof the metal ion in each salt. For example, thelithium ion in lithium carbonate, Li2CO3, producesa deep-red color. The strontium ion in strontiumcarbonate, SrCO3, produces a bright-red color.Similarly, calcium chloride is used for orangelight, sodium chloride for yellow light, and bariumchloride for green light.

Identify the two types of chemical bonds found inthe salt used to produce a deep-red color.

99. Given the reaction:

H .x...N .x H

H+ H+ →

HH .x

...N .x H

H

+

The bond formed between the NH3 and the H+ is

A. electrovalent B. ionic

C. metallic D. coordinate covalent

100. Which could form a coordinate covalent bond?

A. Hx. ..

.Nx. H

H

B. HH x

. ..C .x H

H

C. HH .x

...N .x H

H

+ D. Hx. H

101.

H :....O :H

+ H+→

HH :

..

..O :H

+

What kind of bond is formed in the reactionshown?

A. metallic bond

B. hydrogen bond

C. network bond

D. coordinate covalent bond


The particle diagrams below representthe reaction between two nonmetals, A2 andQ2.

Identify the type of chemical bond between anatom of element A and an atom of element Q.


103. Given the formula of a substance:

What is the total number of shared electrons in amolecule of this substance?

A. 22 B. 11 C. 9 D. 6

104. As a bond between a hydrogen atom and a sulfuratom is formed, electrons are

A. shared to form an ionic bond

B. shared to form a covalent bond

C. transferred to form an ionic bond

D. transferred to form a covalent bond


A piece of magnesium ribbon is reactedwith excess hydrochloric acid to produceaqueous magnesium chloride and hydrogengas. The volume of the dry hydrogen gasproduced is 45.6 milliliters. The temperatureof the gas is 293 K, and the pressure is99.5 kilopascals.

Identify the type of bond between the atoms in amolecule of the gas produced in this laboratoryinvestigation.

106. Which formula represents a molecule having anonpolar covalent bond?

A. B.

C. D.

107. What is the total number of electron pairs sharedbetween the carbon atom and one of the oxygenatoms in a carbon dioxide molecule?

108. What is the total number of electrons shared in adouble covalent bond?

A. 1 B. 2 C. 3 D. 4

109. Which molecule has a nonpolar covalent bond?

A. B.

C. D.


One type of soap is produced whenethyl stearate and sodium hydroxide react.The soap produced by this reaction is calledsodium stearate. The other product ofthe reaction is ethanol. This reaction isrepresented by the balanced equation below.

Identify the two types of bonds in the compoundsodium stearate.


Ethene and hydrogen can react at afaster rate in the presence of the catalystplatinum. The equation below represents areaction between ethene and hydrogen.

State the number of electrons shared between thecarbon atoms in one molecule of the reactantethene.

112. Metallic bonding occurs between atoms of

A. fluorine B. neon

C. sulfur D. copper


113. Mobile electrons are a distinguishing characteristicof

A. an ionic bond

B. an electrovalent bond

C. a metallic bond

D. a covalent bond

114. When combining with nonmetallic atoms, metallicatoms generally will

A. lose electrons and form negative ions

B. lose electrons and form positive ions

C. gain electrons and form negative ions

D. gain electrons and form positive ions

115. Hydrogen bonds are strongest between moleculesof

A. H2O(`) B. H2S(`)

C. H2Se(`) D. H2Te(`)

116. In which of the following liquids are hydrogenbonds between molecules the strongest?

A. HI(`) B. HBr(`)

C. HCl(`) D. HF(`)

117. Hydrogen bonding is strongest between moleculesof

A. H2S B. H2O C. H2Se D. H2Te

118. Compared to the boiling point of H2S, the boilingpoint of H2O is relatively high. Which type ofbonding causes this difference?

A. covalent B. hydrogen

C. ionic D. network

119. The accompanying table shows four compoundsand the boiling point of each.

Compound Boiling Point

H2O 100. ◦C

H2S −67.7◦C

H2Se −41.5◦C

H2Te −2.2◦C

Which type of molecular attraction accounts forthe high boiling point of H2O?

A. molecule-ion

B. ion-ion

C. hydrogen bonding

D. van der Waals forces



Have you ever seen an insect called awater strider “skating” across the surfaceof a calm pond? Have you ever “floated”a sewing needle on the water in a glass?If you have, then you’ve observed one ofwater’s many amazing properties.

Water’s surface tension keeps the waterstrider and the sewing needle from sinkinginto the water. Simply stated, the surfacetension is due to the forces that hold thewater molecules together. Without theseintermolecular forces, the water strider andthe sewing needle would sink below thesurface of the water.

The surface tension of water at varioustemperatures is given in the data table below.

Surface Tension at DifferentWater Temperatures

Water Temperature(◦C)

Surface Tension(mN/m)

10. 74.2

25 72.0

50. 67.9

75 63.6

100. 58.9

The surface tension of liquid tetrachloromethane,CCl4, at 25◦C is 26.3 millinewtons/meter (mN/m).Compare the intermolecular forces betweenmolecules of CCl4 to the intermolecular forcesbetween molecules of water, H2O, at 25◦C.

121. The boiling points, at standard pressure, of fourcompounds are given in the table below.

Boiling Points ofFour Compounds

Compound Boiling Point (◦C)

H2O 100.0

H2S −59.6

H2Se −41.3

H2Te −2.0

Which type of attraction can be used to explainthe unusually high boiling point of H2O?

A. ionic bonding

B. hydrogen bonding

C. polar covalent bonding

D. nonpolar covalent bonding

122. Which molecule is a dipole?

A. He B. H2 C. NH3 D. CH4

123. Which molecule contains a nonpolar covalentbond?

A. H x. ....N .x H B. H x

. ....Cl :

C. H x. ...O :H

D. H x.H

124. Which type of bond is contained in a watermolecule?

A. nonpolar covalent B. polar covalent

C. ionic D. electrovalent


125. Base your answer(s) to the following question(s)on the table below.

Physical Properties of Four Gases

Name of Gas hydrogen hydrogenchloride

hydrogenbromide

hydrogeniodide

Molecular Structure H-H H-Cl H-Br H-I

Boiling Point (K) at 1 Atm 20. 188 207 237

Density (g/L) at STP 0.0899 1.64 ? 5.66

Explain, in terms of electronegativity difference,why the bond in H-Cl is more polar than the bondin H-I.


Rubbing alcohol is a product availableat most pharmacies and supermarkets. Onerubbing alcohol solution contains 2-propanoland water. The boiling point of 2-propanol is82.3◦C at standard pressure.

Explain, in terms of electronegativity differences,why a C—O bond is more polar than a C—Hbond.

127. The correct formula for sodium oxide is

A. SO2 B. S2O C. NaO2 D. Na2O

128. Which formula represents tetrahedral molecule?

A. CH4 B. CaCl2 C. HBr D. Br2

129. Which is the formula of a binary compound?

A. KOH B. NaClO3

C. Al2S3 D. Bi(NO3)3

130. Which is the formula for sodium perchlorate?

A. NaClO B. NaClO2

C. NaClO3 D. NaClO4

131. Which substance is classified as a salt?

A. Ca(OH)2 B. C2H4(OH)2

C. CCl4 D. CaCl2

132. Which is the correct formula for nitrogen (I)oxide?

A. NO B. N2O C. NO2 D. N2O3

133. What is the chemical formula for copper (II)chlorate?

A. Cu2Cl B. CuCl2

C. Cu2ClO3 D. Cu(ClO3)2

134. Which of the following compounds has the leastionic character?

A. KI B. NO C. HCl D. MgS

135. Which formula represents an ionic compound?

A. H2O(`) B. NaCl(s)

C. NH3(g) D. CCl4(`)

136. The maximum number of electrons that canoccupy a principal energy level (n) of an atom isequal to

A. n2 B. 2n2 C. n + 2 D. n2 + 2

137. What is the maximum number of electrons thatcan be contained in the n = 4 principal energylevel?

A. 8 B. 18 C. 32 D. 50


138. The characteristic bright-line spectrum of anelement is produced when electrons

A. absorb quanta and return to lower energylevels

B. absorb quanta and move to higher energylevels

C. release quanta and return to lower energylevels

D. release quanta and move to higher energylevels


An atom in an excited state has an electronconfiguration of 2-7-2.

Explain, in terms of subatomic particles, why thisexcited atom is electrically neutral.

140. Element M has an electronegativity of less than1.2 and reacts with bromine to form the compoundM Br2. Element M could be

A. Al B. Na C. Ca D. K

141. Which element has atoms with the strongestattraction for electrons in a chemical bond?

A. chlorine B. nitrogen

C. fluorine D. oxygen

142. A substance has a high melting point and conductselectricity in the liquid phase. This substance is

A. Ne B. Hg C. NaCl D. SiC

143. Which molecule is relatively inactive and containsa triple bond?

A. N2 B. O2 C. Cl2 D. H2

144. The accompanying graph represents the relationshipbetween atomic radii, in picometers, and increasingatomic number for elements in Group 15.

Which element is most metallic?

A. A B. B C. D D. E

145. The element in Period 4 and Group 1 of thePeriodic Table would be classified as a

A. metal B. metalloid

C. nonmetal D. noble gas


146. Base your answer(s) to the following question(s)on the article below, the Reference Tables forPhysical Setting/Chemistry, and your knowledge ofchemistry.

In the 1920s, paint used to inscribe thenumbers on watch dials was composed of aluminescent (glow-in-the-dark) mixture. Thepowdered-paint base was a mixture of radiumsalts and zinc sulfide. As the paint wasmixed, the powdered base became airborneand drifted throughout the workroom causingthe contents of the workroom, including thepainters’ clothes and bodies, to glow in thedark.

The paint is luminescent becauseradiation from the radium salts strikes ascintillator. A scintillator is a material thatemits visible light in response to ionizingradiation. In watchdial paint, zinc sulfideacts as the scintillator.

Radium present in the radium saltsdecomposes spontaneously, emitting alphaparticles. These particles can cause damageto the body when they enter human tissue.Alpha particles are especially harmful tothe blood, liver, lungs, and spleen becausethey can alter genetic information in thecells. Radium can be deposited in the bonesbecause it substitutes for calcium.

Why does radium substitute for calcium in bones?

147. A sample composed only of atoms having thesame atomic number is classified as

A. a compound B. a solution

C. an element D. an isomer

148. Which grouping of circles, when considered inorder from the top to the bottom, best representsthe relative size of the atoms of Li, Na, K, andRb, respectively?

A. B. C. D.

149. Ozone is an allotropic form of the element

A. oxygen B. phosphorous

C. sulfur D. carbon

150. An aqueous solution of XCl2 contains coloredions. Element X is most likely

A. an alkaline earth B. a halogen

C. a transition metal D. an alkali metal


Densities ofGroup 14 Elements

Element Density at STP(g/cm3)

C 3.51

Si 2.33

Ge 5.32

Sn 7.31

Pb 11.35

Identify one element from this table for each typeof element: metal, metalloid, and nonmetal.


In the late 19th century, theHall-Herroult process was invented as aninexpensive way to produce aluminum.In this process, Al2O3(`) extracted frombauxite is dissolved in Na3AlF6(`) in agraphite—lined tank, as shown in thediagram below. The products are carbondioxide and molten aluminum metal.

What is the melting point of the substance thatcollects at the bottom of the tank?


153. What is the net charge of an ion that consists of10 electrons, 11 protons, and 12 neutrons?

A. 1+ B. 2+ C. 1− D. 2−

154. Water containing dissolved electrolyte conductselectricity because the solution contains mobile

A. electrons B. molecules

C. atoms D. ions

155. As an Na atom forms an Na2+ ion, the number ofprotons in its nucleus


C. remains the same

156. Given the reaction between two different elementsin the gaseous state:

After a neutral sulfur atom gains two electrons,what is the resulting charge of the ion?

157. At 298 K, the vapor pressure of H2O is less thanthe vapor pressure of CS2. The best explanationfor this is that H2O has

A. larger molecules

B. a larger molecular mass

C. stronger ionic bonds

D. stronger intermolecular forces

158. The chart given shows the change in vaporpressure of four pure liquids with increasingtemperature. Which liquid has the lowest normalboiling point?

A. A B. B C. C D. D

159. Liquid A is confined in a container as shown inthe diagram. The equilibrium vapor pressure ofliquid A depends on the

A. amount of vapor in the container

B. amount of liquid in the container

C. temperature of liquid A

D. size of the confining container

160. A closed system is shown in the diagram. Therate of vapor formation at equilibrium is

A. less than the rate of liquid formation

B. greater than the rate of liquid formation

C. equal to the rate of liquid formation


161. The accompanying graph shows the relationshipbetween vapor pressure and temperature forsubstance X.

What is the normal boiling point for substance X?

A. 50◦C B. 20◦C C. 30◦C D. 40◦C

162. The graph shows the relationship betweentemperature and time as heat is added to onemole of a substance at a rate of 100 calories perminute. The substance is in the solid phase atTime = 0 minutes.

The temperature at which the substance begins toboil is

A. 10◦C B. 40◦C

C. 80◦C D. 110◦C

163. A student collected data in an experiment inwhich the uniform cooling of a water sample wasobserved from 50◦C to −32◦C. Which graphmost likely represents the results obtained by thestudent?

A. B.

C. D.

164. When a substance melts, it undergoes the processcalled

A. condensation B. fusion

C. sublimation D. vaporization

165. The temperature at which the solid and liquidphases of matter exist in equilibrium is called its

A. melting point

B. boiling point

C. heat of fusion

D. heat of vaporization


166. The accompanying graph represents the heatingcurve of a substance that starts as a solid belowits freezing point.

What is the melting point of this substance?

A. 30◦C B. 55◦C

C. 90◦C D. 120◦C

167. Base your answer(s) to the following question(s)on the information and diagram below and onyour knowledge of chemistry.

Crude oil is a mixture of many hydrocarbonsthat have different numbers of carbon atoms. Theuse of a fractionating tower allows the separationof this mixture based on the boiling points of thehydrocarbons.

To begin the separation process, the crude oilis heated to about 400◦C in a furnace, causingmany of the hydrocarbons of the crude oil tovaporize. The vaporized mixture is pumped intoa fractionating tower that is usually more than30 meters tall. The temperature of the tower ishighest at the bottom. As vaporized samples ofhydrocarbons travel up the tower, they cool andcondense. The liquid hydrocarbons are collectedon trays and removed from the tower. Thediagram below illustrates the fractional distillationof the crude oil and the temperature ranges inwhich the different hydrocarbons condense.

State the trend between the boiling point of thehydrocarbons contained in the crude oil and thenumber of carbon atoms in these molecules.

















Letter Z corresponds to an element on thePeriodic Table other than the six listed elements.Elements G, Q, L, and Z are in the same group onthe Periodic Table, as shown in the diagram below.

Based on the trend in the melting points forelements G, Q, L, and Z listed in the “Propertiesof Six Elements at Standard Pressure” table,estimate the melting point of element Z, in degreesCelsius.

169. Some physical properties of two samples ofiodine-127 at two different temperatures are shownin the table below.

Selected Physical Properties of Iodine-127 Samples at 1 atm

Sample Sample Temperature(K)

Description Density(g/cm3)

1 298 dark-gray crystals 4.933

2 525 dark-purple gas 0.006

These two samples are two different

A. mixtures B. substances

C. phases of matter D. isotopes of iodine

170. Compared to a 1 mole sample of hydrogen at273 K and 1 atmosphere, a 1 mole sample ofhydrogen at 298 K and 1 atmosphere contains

A. more molecules

B. fewer molecules

C. molecules having higher average kineticenergy

D. molecules having lower average kinetic energy

171. A 1 liter flask of CO2(g) and a 1 liter flask ofH2(g) are both at STP. The ratio of the number ofmolecules of CO2(g) to the number of moleculesof H2(g) in the flasks is

A. 1 : 1 B. 2 : 3 C. 3 : 2 D. 1 : 3

172. A flask containing molecules of gas A and aseparate flask containing molecules of gas B areboth at the same temperature. Gases A and Bmust have equal

A. volumes

B. masses

C. pressures

D. average kinetic energies

173. When the average kinetic energy of a gaseoussystem is increased, the average molecular velocityof the system

A. increases and the molecular mass increases

B. decreases and the molecular mass increases

C. increases and the molecular mass remains thesame

D. decreases and the molecular mass remains thesame


174. The diagrams shown represent four 500-milliliterflasks. Each flask contains the gas represented byits symbol. All gas samples are at STP. Each flaskcontains the same number of

A. atoms, only

B. molecules, only

C. atoms and molecules

D. atoms, but different numbers of molecules

175. P (atm) V (mL)

0.5 1000

1.0 500

2.0 250

The table shows the changes in the volume of gasas the pressure changes at constant temperature.Which equation best expresses the relationshipbetween pressure and volume for the gas?

A.PV

= 500 atm ·mL B. PV = 500 atm ·mL

C.VP

= 500 atm ·mL D. PV =1

500atm ·mL

176. Sample Substance Temp.(K)

Pressure(atm)

Volume(L)

A He 273 1 22.4

B O2 273 1 22.4

C Ne 273 2 22.4

D N2 546 2 44.8

E Ar 546 2 44.8

The table here shows the temperature, pressure, and volume of five samples. Which sample contains the samenumber of molecules as sample A ?

A. E B. B C. C D. D


177. The accompanying graph represents the relationshipbetween pressure and volume of a given mass of agas at constant temperature.

The product of pressure and volume is constant.According to the graph, what is the product inatm ·mL?

A. 20. B. 40. C. 60. D. 80.

178. A cylinder with a tightly fitted piston is shown inthe accompanying diagram.

As the piston moves downward, the number ofmolecules of air in the cylinder


C. remains the same

179. Base your answer(s) to the following question(s)on the diagram, which shows a piston confining agas in a cylinder.

Using the set of axes provided below, sketch thegeneral relationship between the pressure and thevolume of an ideal gas at constant temperature.

180. Which diagram best represents a gas in a closedcontainer?

A. B.

C. D.

181. The table below shows data for the temperature,pressure, and volume of four gas samples.

Data for Four Gas Samples

GasSample

Temperature(K)

Pressure(atm)

Volume(mL)

A 100. 2 400.

B 200. 2 200.

C 100. 2 400.

D 200. 4 200.

Which two gas samples have the same totalnumber of molecules?

A. A and B B. A and C

C. B and C D. B and D


182. The diagram represents a gas confined in a cylinderfitted with a movable piston. As the piston movestoward point A at constant temperature, whichrelationship involving pressure (P) and volume (V)is correct?

A. P + V = k B. P − V = k

C. P ÷ V = k D. P × V = k


A rigid cylinder is fitted with a movablepiston. The cylinder contains a sample ofhelium gas, He(g), which has an initialvolume of 125.0 milliliters and an initialpressure of 1.0 atmosphere, as shown below.The temperature of the helium gas sample is20.0◦C.

Express the initial volume of the helium gassample, in liters.


Cylinder A has a movable pistonand contains hydrogen gas. An identicalcylinder, B, contains methane gas. Thediagram below represents these cylindersand the conditions of pressure, volume, andtemperature of the gas in each cylinder.

Compare the total number of gas molecules incylinder A to the total number of gas molecules incylinder B.

185. State a change in temperature and a change inpressure that will cause the gas in cylinder A tobehave more like an ideal gas.

Temperature:

Pressure:

186. A given sample of a gas has a volume of 3 litersat a pressure of 4 atmospheres. If the temperatureremains constant and the pressure is changed to6 atmospheres, the P × V product will equal

A. 9 B. 12 C. 18 D. 24

187. At constant pressure, 50 milliliters (mL) of a gasat 20◦C is heated to 30◦C. The new volume ofthe gas in milliliters (mL) is equal

A. 50 ×20

30B. 50 ×

30

20

C. 50 ×293

303D. 50 ×

303

293


188. A gas has a volume of 2 liters at 323 K and3 atmospheres. When its temperature is changed to273 K and the pressure is changed to 1 atmosphere,the new volume of the gas would be equal to

A. 2 L ×273 K

323 K×

1 atm

3 atm

B. 2 L ×323 K

273 K×

1 atm

3 atm

C. 2 L ×273 K

323 K×

3 atm

1 atm

D. 2 L ×323 K

273 K×

3 atm

1 atm

189. Base your answer(s) to the following question(s)on the diagram, which shows a piston confining agas in a cylinder.

The gas volume in the cylinder is 6.2 millilitersand its pressure is 1.4 atmospheres. The pistonis then pushed in until the gas volume is3.1 milliliters while the temperature remainsconstant.

a) In the space provided below, calculate thepressure, in atmospheres, after the change involume. Show all work.

b) Record your answer.

190. Base your answer(s) to the following question(s)on the information and diagrams below.

Cylinder A contains 22.0 grams ofCO2(g) and cylinder B contains N2(g). Thevolumes, pressures, and temperatures of thetwo gases are indicated under each cylinder.

The temperature of the CO2(g) is increased to450. K and the volume of cylinder A remainsconstant. Show a correct numerical setup forcalculating the new pressure of the CO2(g) incylinder A.


A rigid cylinder is fitted with a movablepiston. The cylinder contains a sample ofhelium gas, He(g), which has an initialvolume of 125.0 milliliters and an initialpressure of 1.0 atmosphere, as shown below.The temperature of the helium gas sample is20.0◦C.

The piston is pushed further into the cylinder.Show a correct numerical setup for calculatingthe volume of the helium gas that is anticipatedwhen the reading on the pressure gauge is1.5 atmospheres. The temperature of the heliumgas remains constant.


192. The behavior of a real gas would be most similarto the behavior of an ideal gas under conditions of

A. high pressure and high temperature

B. high pressure and low temperature

C. low pressure and high temperature

D. low pressure and low temperature

193. A sample of chlorine gas is at 300. K and1.00 atmosphere. At which temperature andpressure would the sample behave more like anideal gas?

A. 0 K and 1.00 atm

B. 150. K and 0.50 atm

C. 273 K and 1.00 atm

D. 600. K and 0.50 atm

194. What is the total mass of a 10 gram sample of42K that will remain unchanged after 12.4 hours?

A. 2.5 g B. 5.0 g C. 7.5 g D. 10 g

195. An original sample of a radioisotope had a massof 10 grams. After 2 days, 5 grams of theradioisotope remains unchanged. What is thehalf-life of this radioisotope?

A. 1 day B. 2 days

C. 5 days D. 4 days

196. How many grams of a 32-gram sample of 32P willremain after 71.5 days?

A. 1 B. 2 C. 8 D. 4

197. In the reaction 23892U + 1

0n→ 23993Np + X, the species

represented by X is

A. 11H B. 1

0n C. 42He D. 0

−1e

198. The graph shown represents the decay of aradioactive isotope. What is the half-life of thisisotope?

A. 1 hour

B. 2 hours

C. 3 hours

D. 6 hours

199. Which of the following 10-grain samples ofradioisotope will decay to the greatest extent in28 days?

A. 3215P B. 85

36Kr C. 22087Fr D. 131

53I

200. In the equation 22890Th→ 228

88Ra + X, which particleis represented by the letter X?

A. an alpha particle B. a beta particle

C. a positron D. a deuteron


Problem-Attic format version 4.4.279c_ 2011–2016 EducAide Software

Licensed for use by Simone ShakerTerms of Use at www.problem-attic.com

50 Pts Chemistry term 1 review sheet- Vacation homework 01/27/2017

1.Answer: A

2.Answer: B

3.Answer: B

4.Answer: A

5.Answer: C

6.Answer: D

7.Answer: B

8.Answer: D

9.Answer: A

10.Answer: D

11.Answer: C

12.Answer: C

13.Answer: D

14.Answer: B

15.Answer: C

16.Answer: A

17.Answer: A

18.Answer: A

19.Answer: B

20.Answer: D

21.Answer: D

22.Answer: A

23.Answer: C

24.Answer: D

25.Answer: A

26.Answer: Allow credit for marking an appropriate

scale.

27.Answer: As atomic number increases, there is a

decrease in atomic radius.

28.Answer: increasing atomic mass, atomic mass,

oxide formulas

29.Answer: Ag silver

30.Answer: D

31.Answer: B

32.Answer: B

33.Answer: A

34.Answer: D

35.Answer: C

36.Answer: B

37.Answer: C

38.Answer: B

39.Answer: 0.090 g/L

Teacher’s Key Page 2

40.Answer: A

41.Answer: A

42.Answer: D

43.Answer: A

44.Answer: Group 18 or the noble gases

45.Answer: B

46.Answer: B

47.Answer: Acceptable responses include, but are

not limited to: Ga; indium; element 31;element 49


not limited to: As atomic numberincreases, the electronegativity increases;Electronegativity increases; from lower tohigher

49.Answer: Acceptable responses include, but are not

limited to: Si; silicon; element 14

50.Answer: C

51.Answer: A

52.Answer: D

53.Answer: C

54.Answer: B

55.Answer: C

56.Answer: C

57.Answer: 53◦C

58.Answer: D

59.Answer: 50◦C

60.Answer: density, mass, or volume.

61.Answer: 3.9 cm3 or 3.88 cm3

62.Answer: The spectrum from a star is compared to

spectra of known elements.

63.Answer: The total mass of reactants equals the

total mass of product.

64.Answer: 4 or four.

65.Answer: B

66.Answer: m = Vd = (0.20L)(1.8g/L)

(0.2)(1.8)

Allow 1 credit for 0.36 g or for aresponse consistent with the student’snumerical setup. Significant figures donot need to be shown.

Note: Do not allow credit for a numericalsetup and calculated result that are notrelated to the concept assessed by thequestion.

67.Answer: minute 16

at 16 minutes

68.Answer: B

69.Answer: D

70.Answer: C

71.Answer: D

72.Answer: C

73.Answer: A

74.Answer:

75.Answer:


76.Answer:

77.Answer:

78.Answer: C

79.Answer: The electron-shell diagram shows the total

number of protons and the total numberof neutrons in an atom.

shows number of electrons in each innershell

shows total number of protons in an atom

shows the number of electron shells

80.Answer: Lewis electron-dot diagrams only show

valence electrons, which are involved inbonding.

shows only electrons involved in bonding

81.Answer:

82.Answer: B

83.Answer: three electrons

84.Answer: C

85.Answer: C

86.Answer: Excited state to ground state releases

energy.

energy released - excited to ground

An electron absorbs energy and moves toa higher shell (energy level). As theelectron returns to a lower shell (energylevel), it releases energy in the form of abright-line spectrum.

87.Answer:

88.Answer: 1 or one.

89.Answer: Acceptable answers but not limited to:

Electrons move from the ground state toan excited state as the compounds gainenergy. Light energy is released when theelectrons return to lower states.

Electrons lose energy as they move tolower shells.

Light is emitted as electrons return fromhigher to lower energy states.

90.Answer: Ne

neon

element 10

91.Answer: C

92.Answer: A

93.Answer: A

94.Answer: D

95.Answer: A


96.Answer: D

97.Answer: D

98.Answer: ionic bonds and polar covalent bonds

covalent and ionic

99.Answer: D

100.Answer: A

101.Answer: D

102.Answer: polar covalent

103.Answer: A

104.Answer: B

105.Answer: nonpolar covalent bond

covalent bond

nonpolar

106.Answer: C

107.Answer: 2

108.Answer: D

109.Answer: A

110.Answer: covalent bonds and ionic bonds polar and

nonpolar single and double

111.Answer: 4 or four

112.Answer: D

113.Answer: C

114.Answer: B

115.Answer: A

116.Answer: D

117.Answer: B

118.Answer: B

119.Answer: C

120.Answer: Tetrachloromethane, CCl4, has weaker

intermolecular forces than water, H20.

121.Answer: B

122.Answer: C

123.Answer: D

124.Answer: B

125.Answer: The electronegativity difference for HCl is

1.1, which is higher than the 0.6 for HI.


not limited to: There is a greaterelectronegativity difference in a C—Obond than in a C—H bond; TheC—O bond is more polar because theelectronegativity difference for a C—Obond is 0.8, and the electronegativitydifference for a C—H bond is 0.4; TheC—H bond has a smaller difference; TheC—O is .8 and the C—H is .4.

127.Answer: D

128.Answer: A

129.Answer: C

130.Answer: D

131.Answer: D

132.Answer: B

133.Answer: D

134.Answer: B


135.Answer: B

136.Answer: B

137.Answer: C

138.Answer: C

139.Answer: The number of protons equals the number

of electrons.

The atom has 11 protons and 11 electrons.

140.Answer: C

141.Answer: C

142.Answer: C

143.Answer: A

144.Answer: D

145.Answer: A

146.Answer: both Group 2 metals

Radium is a more active metal.

similar chemical properties

They are both alkaline earth metals.

It also has two valence electrons.

147.Answer: C

148.Answer: A

149.Answer: A

150.Answer: C

151.Answer: Metal: tin or Sn or lead or Pb Metalloid:

silicon or Si or germanium or GeNonmetal: carbon or C

152.Answer: 933 K

153.Answer: A

154.Answer: D

155.Answer: C

156.Answer: −2

negative

157.Answer: D

158.Answer: A

159.Answer: C

160.Answer: C

161.Answer: C

162.Answer: C

163.Answer: B

164.Answer: B

165.Answer: A

166.Answer: B

167.Answer: As the number of carbon atoms in these

molecules increases, the boiling pointincreases.

168.Answer: Temperature value below 64◦C.

169.Answer: C

170.Answer: C

171.Answer: A

172.Answer: D

173.Answer: C

174.Answer: B


175.Answer: B

176.Answer: B

177.Answer: D

178.Answer: C

179.Answer:

180.Answer: A

181.Answer: B

182.Answer: D

183.Answer: 0.1250 L

184.Answer: The number of gas molecules in

cylinder A is the same as the number ofgas molecules in cylinder B.

185.Answer: Temperature: above 293 K; Pressure:

below 1.2 atm

OR

Temperature: higher; Pressure: lower

186.Answer: B

187.Answer: D

188.Answer: C

189.Answer: (6.2 mL)(1.4 atm) = (3.1 mL)(P2),

P2 =6.2 mL(1.4 atm)

3.1 mL,

The volume is halved so pressure mustdouble.;

2.8

190.Answer: 1

300 = x450

191.

Answer: V2 =(1.0 atm)(125.0 mL)

1.5 atm

192.Answer: C

193.Answer: D

194.Answer: B

195.Answer: B

196.Answer: A

197.Answer: D

198.Answer: B

199.Answer: C

200.Answer: A

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Chemistry term 1 review sheet- Vacation homework 50 Pts