Chem nal review sheet with answers Name: Datelmghs.org/ourpages/auto/2013/1/11/42626310/Chem final exam review sheet.pdf · Chem nal review sheet with answers 40. Base your answer(s)

Chem final review sheet with answers

Name: Date:

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

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

2. Which substance is an ionic solid?

A. LiCl B. HCl C. Ne D. Fe

3. Molecule-ion attractions are found in

A. Cu(s) B. CO(g)

C. KBr(`) D. NaCl(aq)

4. When a reaction occurs between atoms withground state electron configurations 1s22s1 and1s22s22p5 the predominant type of bond formed is

A. polar covalent B. nonpolar covalent

C. ionic D. metallic

5. The greatest degree of ionic character would befound in a bond between sulfur and

A. oxygen B. chlorine

C. bromine D. phosphorus

6. Which atom listed has the greatest ability toattract the electrons that form a bond between itand another atom?

A. sodium B. magnesium

C. aluminum D. chlorine

7. An ionic bond forms between atoms of

A. I and Cl B. K and Cl

C. P and Cl D. H and Cl

8. A characteristic of ionic solids is that they

A. have high melting points

B. have low boiling points

C. conduct electricity

D. are noncrystalline

9. Which of the following compounds contains abond with the greatest degrees of ionic character?

A. CaO B. MgBr2

C. PH3 D. CCL4

10. Which of the following bonds exhibits the greatestionic character?

A. H–F B. H–Cl C. H–Br D. H–I

page 1


11. Which type of bond is formed by the transfer ofelectrons from one atom to another?

A. a covalent bond

B. a coordinate covalent bond

C. a hydrogen bond

D. an ionic bond

12. Which element can react with fluorine to formmore than one binary compound?

A. K B. Mg C. Co D. Na

13. Which compound contains a bond with the leastionic character?

A. CO B. CaO C. K2O D. Li2O

14. Which type of bonds are formed when calciumatoms react with oxygen atoms?

A. polar covalent B. coordinate covalent

C. ionic D. hydrogen

15. Which compound contains both covalent bondsand ionic bonds?

A. NaCl(s) B. HCl(g)

C. NaNO3(s) D. N2O5(g)

16. Which two atoms will form an ionic bond?

A. K and H B. I and H

C. N and H D. C and H

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

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

18. 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

19. Which bond has the greatest ionic character?

A. H−Cl B. H−F C. H−O D. H−N

20. Which compound contains ionic bonds?

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

21. Which compound has the least ionic character?

A. KCl B. CaCl2 C. AlCl3 D. CCl4

page 2


22. Which element would most likely form an ionicbond with chlorine?

A. O B. N C. S D. K

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

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

24. When a metal atom combines with a nonmetalatom, the nonmetal atom will

A. lose electrons and decrease in size

B. lose electrons and increase in size

C. gain electrons and decrease in size

D. gain electrons and increase in size

25. When ionic bonds are formed, metallic atoms tendto

A. lose electrons and become negative ions

B. lose electrons and become positive ions

C. gain electrons and become negative ions

D. gain electrons and become positive ions

26. When a potassium atom reacts with bromine, thepottasium atom will

A. lose only 1 electron

B. lose 2 electrons

C. gain only 1 electron

D. gain 2 electrons

27. Which atom will form an ionic bond with a Bratom?

A. N B. Li C. O D. C

28. Element X is in Group 2 and element Y is inGroup 17. What happens when a compound isformed between these two atoms?

A. X loses electrons to Y to form an ionic bond.

B. X loses electrons to Y to form a covalentbond.

C. X gains electrons from Y to form an ionicbond.

D. X gains electrons from Y to form a covalentbond.

page 3


29. The forces between atoms that create chemicalbonds are the result of interactions between

A. nuclei

B. electrons

C. protons and electrons

D. protons and nuclei

30. Which type of bond is formed when an atom ofpotassium transfers an electron to a bromine atom?

A. metallic B. ionic

C. nonpolar covalent D. polar covalent

31. Which substance contains a bond with the greatestionic character?

A. KCl B. HCl C. Cl2 D. F2

32. Which elements combine by forming an ionicbond?

A. sodium and potassium

B. sodium and oxygen

C. carbon and oxygen

D. carbon and sulfur

33. Which statement best describes the substance thatresults when electrons are transferred from a metalto a nonmetal?

A. It contains ionic bonds and has a low meltingpoint.

B. It contains ionic bonds and has a highmelting point.

C. It contains covalent bonds and has a lowmelting point.

D. It contains covalent bonds and has a highmelting point.

34. A hard substance that has a high melting pointand is a poor conductor of electricity in the solidphase could be

A. CO2 B. Mg C. NaCl D. CCl4

page 4


35. 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

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

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

Molecule A: Cl2Molecule B: CCl4Molecule C: NH3

Explain how the bonding in KCl is different fromthe bonding in molecules A, B, and C.

37. The bonds in the compound MgSO4 can bedescribed as

A. ionic, only

B. covalent, only

C. both ionic and covalent

D. neither ionic nor covalent


Given the equation for the dissolvingof sodium chloride in water:

NaCl(s) Na + (aq) + Cl − (aq)

Explain, in terms of particles, why NaCl(s) doesnot conduct electricity.

39. The data table below represents the propertiesdetermined by the analysis of substances A, B, C,and D.

Which substance is an ionic compound?

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

page 5


40. Base your answer(s) to the following question(s)on the balanced equation below.

2Na(s) + Cl2(g) − 2NaCl(s)

Explain, in terms of electrons, why the bonding inNaCl is ionic.

41. Which type of bond is found in sodium bromide?

A. covalent B. hydrogen


42. An ionic bond can be formed when one or moreelectrons are

A. equally shared by two atoms

B. unequally shared by two atoms

C. transferred from the nucleus of one atom tothe nucleus of another atom

D. transferred from the valence shell of one atomto the valence shell of another atom

43. 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,the lithium ion in lithium carbonate, Li2CO3,produces a deep-red color. The strontium ion instrontium carbonate, SrCO3, produces a bright-redcolor. Similarly, calcium chloride is used fororange light, sodium chloride for yellow light, andbarium chloride for green light.

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

44. Which kind of bond is formed when two atomsshare electrons to form a molecule?

A. ionic B. metallic

C. electrovalent D. covalent

45. The distance between two adjacent nuclei of anelement in the solid phase is 2.04 A. The covalentatomic radius of an atom of this element is closestto

A. 0.51 A B. 1.02 A

C. 2.04 A D. 4.08 A

page 6


46. According to Reference Table E, which compoundforms spontaneously from its elements?

TABLE OF SOLUBILITIES IN WATER

i — nearly insoluabless — slightly soluables — soluabled — decomposesn — not isolated ac

etat

e

brom

ide

carb

onat

e

chlo

ride

chro

mat

e

hydr

oxid

e

iodi

de

nitrat

e

phos

phat

e

sulfat

e

sulfi

de

Aluminum ss s n s n i s s i s d

Ammonium s s s s s s s s s s s

Barium s s i s i s s s i i d

Calcium s s i s s ss s s i ss d

Copper II s s i s i i n s i s i

Iron II s s i s n i s s i s i

Iron III s s n s i i n s i ss d

Lead s ss i ss i i ss s i i i

Magnesium s s i s s i s s i s d

Mercury I ss i i i ss n i s i ss i

Mercury II s ss i s ss i i s i d i

Potassium s s s s s s s s s s s

Silver ss i i i ss n i s i ss i

Sodium s s s s s s s s s s s

Zinc s s i s s i s s i s i

A. C2H4 B. C2H2 C. NO2 D. CO2

47. Which kind of bond is formed between a proton(H+) and a water molecule in the production of ahydronium ion?

A. nonpolar covalent B. coordinate covalent

C. electrovalent D. ionic

48. 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

49. What type of bond is present in diamonds?

A. covalent B. ionic

C. electrovalent D. metallic

50. The bonds present in silicon carbid (SiC) are


C. metallic D. van der Waals

51. A diamond consists of covalently bonded carbonatoms. The diamond is an example of

A. a metallic solid B. a molecular solid

C. a network solid D. an ionic solid

page 7


52. One atom of A forms a coordinate covalent bondwith one atom of B. This bond could have beenformed by an atom of B

A. sharing two electrons belonging to an atom ofA

B. sharing only one electron belonging to anatom of A

C. transferring two electrons to an atom of A

D. transferring only one electron to an atom ofA

53. Which type of bond exists between the carbonatoms in diamond?

A. ionic B. covalent

C. metallic D. hydrogen

54. Which compound contains both covalent and ionicbonds?

A. KCl B. NH4Cl

C. MgCl2 D. CCl4

55. Which kinds of bonds are found in a sample ofH2O(s)?

A. hydrogen bonds, only

B. covalent bonds, only

C. both ionic and hydrogen bonds

D. both covalent and hydrogen bonds

56. The bonds in all network solids are


C. metallic D. nonpolar

57. Given the reaction:

H+

Proton

+

H.:N −−H/

HAmmonia

→

H.

H :N−−H/H

Ammonium Ion

Which type of bond is formed between the proton(H+) and the ammonia molecule?

A. ionic B. network

C. coordinate covalent D. nonpolar covalent

58. Substance Melting ConductivityIn SolidState

Solubility inWater

A high no soluble

B high yes insoluble

C high no insoluble

D low no insoluble

The table shows properties of four solids, A, B, C,and D. Which substance could represent diamond,a network solid?

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

page 8


59. What is the maximum number of covalent bondsthat a carbon atom can form?

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

60. Metallic bonding occurs between atoms of

A. fluorine B. neon

C. sulfur D. copper

61. Mobile electrons are a distinguishing characteristicof

A. an ionic bond

B. an electrovalent bond

C. a metallic bond

D. a covalent bond

62. Which element consists of positive ions immersedin a “sea” of mobile electrons?

A. sulfur B. nitrogen

C. calcium D. chlorine

63. Which substance contains particles held togetherby metallic bonds?

A. Ni(s) B. Ne(s) C. N2(s) D. L2(s)

64. 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

65. Metallic bonding occurs between metal atoms thathave

A. full valence orbitals and low ionizationenergies

B. full valence orbitals and high ionizationenergies

C. vacant valence orbitals and low ionizationenergies

D. vacant valence orbitals and high ionizationenergies

66. The high electrical conductivity of metals isprimarily due to

A. high ionization energies

B. filled energy levels

C. mobile electrons

D. high electronegativities

page 9


67. Conductivity in a metal results from the metalatoms having

A. high electronegativity

B. high ionization energy

C. highly mobile protons in the nucleus

D. highly mobile electrons in the valence shell


Element X is a solid metal that reacts withchlorine to form a water-soluble binary compound.

State one physical property of element X thatmakes it a good material for making pots andpans.

69. A solid substance is an excellent conductor ofelectricity. The chemical bonds in this substanceare most likely

A. ionic, because the valence electrons are sharedbetween atoms

B. ionic, because the valence electrons aremobile

C. metallic, because the valence electrons arestationary

D. metallic, because the valence electrons aremobile

70. An element that has a low first ionization energyand good conductivity of heat and electricity isclassified as a

A. metal B. metalloid

C. nonmetal D. noble gas

71. Hydrogen bonds are strongest between moleculesof

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

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

72. Which is the predominate type of attractionbetween molecules of HF in the liquid state?

A. hydrogen bonding

B. electrocovalent bonding

C. ionic bonding

D. covalent bonding

73. Hydrogen bonds are strongest between themolecules of

A. HF(`) B. HCl(`)

C. HBr(`) D. HI(`)

page 10


74. The strongest hydrogen bonds are formed betweenmolecules in which hydrogen is covalently bondedto an element with

A. high electronegativity and large atomic radius

B. high electronegativity and small atomic radius

C. low electronegativity and large atomic radius

D. low electronegativity and small atomic radius

75. Hydrogen bonds are strongest between moleculesof

A. HCl(`) B. HF(`)

C. HBr(`) D. HI(`)

76. Which atom has the least attraction for theelectrons in a bond between that atom and anatom of hydrogen?

A. carbon B. nitrogen

C. oxygen D. fluorine

77. The relatively high boiling point of water isprimarily due to the presence of

A. hydrogen bonds

B. van der Waals forces

C. molecule-ion attractions

D. ion-ion attractions

78. As a chemical bond forms between two hydrogenatoms, the potential energy of the atoms

A. decreases B. increases

C. remains the same

79. Which molecule is a dipole?

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

80. The bonding in NH3 is most similar to thebonding in

A. H2O B. NaCl C. MgO D. KF

81. Which electron dot formula represents a moleculethat contains a nonpolar covalent bond?

A. xxBr .x....Br : B. H .x

..

..Br :

C. Na+[.xFxx]− D. H .xFxx

82. Which substance contains a polar covalent bond?

A. Na3N B. Mg3N2

C. NH3 D. N2

page 11


83. Which substance contains a polar covalent bond?

A. H2 B. HCl C. Cl2 D. KCl

84. Which molecule contains a nonpolar covalentbond?

A. I2 B. NH3 C. H2O D. CO

85. Two fluorine atoms are held together by a covalentbond. Which statement correctly describes thisbond?

A. It is polar and forms a polar molecule.

B. It is polar and forms a nonpolar molecule.

C. It is nonpolar and forms a polar molecule.

D. It is nonpolar and forms a nonpolar molecule.

86. The bonds between hydrogen and oxygen in awater molecule are classified as

A. polar covalent B. nonpolar covalent


87. Which molecule contains a nonpolar covalentbond?

A. B.

C. D.

88. The chemical bond between which two atoms ismost polar?

A. C–N B. H–H C. S–Cl D. Si–O

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

A. atomic number B. mass number

C. oxidation number D. valence number

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

ions

A. gain electrons B. lose electrons

C. gain protons D. lose protons

page 12


91. 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

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

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

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

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

94. 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

95. The arrangement of the elements in the presentPeriodic Table is based on atomic

A. mass B. number

C. radius D. density

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

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

97. In Period 4 of the Periodic Table, the atom withthe largest covalent radius is located in Group

A. 1 (IA) B. 13 (IIIA)

C. 3 (IIIB) D. 18 (O)

98. The greatest difference in electronegativity betweenan element in Group 2 (IIA) and an element inGroup 16 (VIA) occurs in Period

A. 5 B. 2 C. 3 D. 4

99. The elements in the modern Periodic Table arearranged according to their

A. atomic number B. oxidation number

C. atomic mass D. nuclear mass

page 13


100. As elements in Group 15 of the Periodic Tableare considered in order from top to bottom, themetallic character of each successive elementgenerally

A. decreases B. increases

C. remains the same

101. 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(`)

102. As the elements in Period 3 are considered fromleft to right, they tend to

A. lose electrons more readily and increase inmetallic character

B. lose electrons more readily and increase innonmetallic character

C. gain electrons more readily and increase inmetallic character

D. gain electrons more readily and increase innonmetallic character

103. Which element in Group 15 has the greatestmetallic character?

A. nitrogen B. phosphorus

C. antimony D. bismuth

104. According to the Periodic Table, which elementhas more than one positive oxidation state?

A. cadmium B. iron

C. silver D. zinc

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

A. iodine B. bromine

C. chlorine D. fluorine

106. Which group contains elements that form chlorideshaving the formula MCl24 ?

A. IA B. IIA C. IIIA D. IVA

page 14


107. A student determining the percent by mass ofwater in a hydrated crystal obtained the followingdata.

Mass of crystal before heating . . . . . . . . . .5.0 gMass of crystal after 1st heating . . . . . . . .4.0 gMass of crystal after 2nd heating . . . . . . . 4.0 g

What is the percent by mass of water hydrate?

A. 0.80% B. 0.20% C. 80.0% D. 20.0%

108. Which element is a liquid at room temperature?

A. K B. I2 C. Hg D. Mg

109. The solid block shown here has a mass of146 grams. What is the block’s density?

A. 0.37 g/cm3

B. 2.7 g/cm3

C. 8.1 g/cm3

D. 54 g/cm3

110. How does the ground state electron configurationof the hydrogen atom differ from that of a groundstate helium atom?

A. Hydrogen has one electron in a higher energylevel.

B. Hydrogen has two electrons in a lower energylevel.

C. Hydrogen contains a half-filled orbital.

D. Hydrogen contains a completely filled orbital.

111. The light produced by signs using neon gas resultsfrom electrons that are

A. moving from a higher to a lower principalenergy level

B. moving from a lower to a higher principalenergy level

C. being lost by the Ne(g) atoms

D. being gained by the Ne(g) atoms

112. 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

page 15


113. 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.

114. 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

115. 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.

page 16



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

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

117. What is the total number of valence electrons in asulfide ion in the ground state?

A. 8 B. 2 C. 16 D. 18


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 coated witha 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 theground state with the same electron configurationas the nitrogen in a molecule of isocyanic acid.

page 17



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

Write the electron configuration of this atom inthe ground state.

page 18

Acces format version 4.4.158c_ 1997–2011 EducAide Software

Licensed for use by Problem-Attic

Chem final review sheet with answers 01/11/2013

1.Answer: A

2.Answer: A

3.Answer: D

4.Answer: C

5.Answer: A

6.Answer: D

7.Answer: B

8.Answer: A

9.Answer: A

10.Answer: A

11.Answer: D

12.Answer: C

13.Answer: A

14.Answer: C

15.Answer: C

16.Answer: A

17.Answer: D

18.Answer: A

19.Answer: B

20.Answer: B

21.Answer: D

22.Answer: D

23.Answer: D

24.Answer: D

25.Answer: B

26.Answer: A

27.Answer: B

28.Answer: A

29.Answer: C

30.Answer: B

31.Answer: A

32.Answer: B

33.Answer: B

34.Answer: C

35.Answer: D

36.Answer: KCl — ionic bond; A, B, C — no

ionic bonds

Atoms do not share electrons whenbonding.

There is a transfer of electrons from Kto Cl.

KCl forms by electrostatic attraction.

Bonding involves a metal with anonmetal.

Teacher’s Key Page 2

37.Answer: C

38.Answer: NaCl(s) ions cannot move (are not

mobile).

no charged particles free to move

39.Answer: D

40.Answer: The sodium atom transfers its one

valence electron to the chlorine atom.

41.Answer: C

42.Answer: D

43.Answer: ionic bonds and polar covalent bonds

covalent and ionic

44.Answer: D

45.Answer: B

46.Answer: D

47.Answer: B

48.Answer: D

49.Answer: A

50.Answer: A

51.Answer: C

52.Answer: A

53.Answer: B

54.Answer: B

55.Answer: D

56.Answer: A

57.Answer: C

58.Answer: C

59.Answer: D

60.Answer: D

61.Answer: C

62.Answer: C

63.Answer: A

64.Answer: B

65.Answer: C

66.Answer: C

67.Answer: D

68.Answer: conducts heat, high melting point,

malleable

69.Answer: D

70.Answer: A

71.Answer: A

72.Answer: A

73.Answer: A

74.Answer: B

75.Answer: B

76.Answer: A

77.Answer: A


78.Answer: B

79.Answer: C

80.Answer: A

81.Answer: A

82.Answer: C

83.Answer: B

84.Answer: A

85.Answer: D

86.Answer: A

87.Answer: C

88.Answer: D

89.Answer: A

90.Answer: A

91.Answer: D

92.Answer: B

93.Answer: D

94.Answer: A

95.Answer: B

96.Answer: C

97.Answer: A

98.Answer: B

99.Answer: A

100.Answer: B

101.Answer: D

102.Answer: D

103.Answer: D

104.Answer: B

105.Answer: A

106.Answer: D

107.Answer: D

108.Answer: C

109.Answer: B

110.Answer: C

111.Answer: A

112.Answer: C

113.Answer: Excited state to ground state releases

energy.

energy released - excited to ground

An electron absorbs energy and movesto a higher shell (energy level). Asthe electron returns to a lower shell(energy level), it releases energy in theform of a bright-line spectrum.

114.Answer: C

115.Answer:


116.Answer: 1 or one.

117.Answer: A

118.Answer: Acceptable answers but not limited to:

Electrons move from the ground stateto an excited state as the compoundsgain energy. Light energy is releasedwhen the electrons return to lowerstates.

Electrons lose energy as they move tolower shells.

Light is emitted as electrons returnfrom higher to lower energy states.

119.Answer: Ne

neon

element 10

120.Answer: 2-8-1.

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Chem nal review sheet with answers Name: Datelmghs.org/ourpages/auto/2013/1/11/42626310/Chem final exam review sheet.pdf · Chem nal review sheet with answers 40. Base your answer(s)