General, Organic, & Biological Chemistry 4th Edition by Janice Smith – Test Bank

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General, Organic, & Biological Chemistry 4th Edition by Janice Smith – Test Bank

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General, Organic and Biological Chemistry, 4e (Smith)

Chapter 2   Atoms and the Periodic Table

 

1) Which element is a nonmetal?

1. A) K
2. B) Co
3. C) Br
4. D) Al

 

2) Which element is a metal?

1. A) Li
2. B) Si
3. C) Cl
4. D) Ar
5. E) More than one of the elements is a metal.

 

3) Which element is a metalloid?

1. A) B
2. B) C
3. C) Ar
4. D) Al

 

4) What is the mass number of the isotope with the symbol ?

1. A) 17
2. B) 18
3. C) 35.45
4. D) 37

 

5) What is the atomic number of the isotope with the symbol ?

1. A) 17
2. B) 18
3. C) 35.45
4. D) 37

 

6) How many protons are in the isotope with the symbol ?

1. A) 17
2. B) 18
3. C) 35.45
4. D) 37

 

7) Silicon has three naturally occurring isotopes: Si-28, Si-29, and Si-30. If the average atomic mass of silicon is 28.09, which isotope has the highest isotopic abundance?

1. A) Si-28
2. B) Si-29
3. C) Si-30
4. D) All isotopes have the same isotopic abundance.

 

8) The active ingredient in the drug Fosamax is a compound with the chemical formula C4H18NNaO10P2. Which statement concerning the chemical formula of this compound is FALSE?

1. A) Atoms of six different elements make up this compound.
2. B) Carbon, hydrogen, nitrogen, sodium, oxygen, and potassium atoms are present in this compound.
3. C) The ratio of carbon atoms to oxygen atoms is 4:10.
4. D) There is only one atom of nitrogen present in this compound.

 

9) Which element is a transition metal in period 4?

1. A) K
2. B) Hf
3. C) Sn
4. D) Sc

 

10) Which element is a noble gas?

1. A) H
2. B) Ne
3. C) Pr
4. D) Ra
5. E) More than one of the elements listed is a noble gas.

 

11) Which element is not an alkali metal?

1. A) Li
2. B) K
3. C) Rb
4. D) H
5. E) All of these elements are alkali metals.

 

12) Which element is not an alkali metal?

1. A) Li
2. B) Kr
3. C) Rb
4. D) Na
5. E) All of these elements are alkali metals.

 

13) The chemical reactivity of an element is determined by which of the following?

1. A) The number of protons in an atom of the element
2. B) The number of valence electrons in an atom of the element
3. C) The number of neutrons in an atom of the element
4. D) The number of protons and neutrons in an atom of the element

 

14) The element symbol for manganese is ________.

1. A) M
2. B) Ma
3. C) Mg
4. D) Mn

 

15) The element symbol for sulfur is ________.

1. A) S
2. B) Su
3. C) Sf
4. D) Sl

 

16) Which statement is not part of the modern description of the electronic structure of an atom?

1. A) Electrons occupy discrete energy levels.
2. B) Electrons move freely in space.
3. C) The energy of electrons is quantized.
4. D) The energy of electrons is restricted to specific values.

 

17) What is the maximum number of electrons that can occupy the third (n=3) shell?

1. A) 2
2. B) 3
3. C) 6
4. D) 8
5. E) 18

 

18) Which of the following properly represents the order of orbital filling based on the relative energy of the orbitals?

1. A) 1s,2s,2p,3s,3p,3d,4s,4p
2. B) 1s,2s,3s,4s,2p,3p,4p,3d
3. C) 1s,2s,2p,3s,3p,4s,3d,4p
4. D) 1s,2s,2p,3s,3d,3p,4s,4p

 

19) Which atom has the largest atomic radius?

1. A) K
2. B) Ga
3. C) Br
4. D) Rb

 

20) Which atom has the smallest atomic radius?

1. A) K
2. B) Ga
3. C) Br
4. D) Rb

 

21) Which element has the smallest ionization energy?

1. A) K
2. B) Ga
3. C) Br
4. D) Rb

 

22) How many protons are in the isotope  ?

1. A) 238
2. B) 146
3. C) 92
4. D) 330

 

23) How many neutrons are in the isotope ?

1. A) 238
2. B) 146
3. C) 92
4. D) 330

 

24) How many electrons are in the isotope ?

1. A) 238
2. B) 146
3. C) 92
4. D) 330

 

25) Which isotope is not possible?

A)

B)

C)

D)

1. E) More than one of the isotopes is not possible.

26) An atom of the isotope chlorine-37 consists of how many protons, neutrons, and electrons? (p = proton, n = neutron, e = electron)

1. A) 18 p, 37 n, 18 e
2. B) 17 p, 20 n, 17 e
3. C) 17 p, 20 n, 18 e
4. D) 37 p, 37 n, 17 e
5. E) 37 p, 20 n, 37 e

27) The elements in a column of the periodic table are collectively referred to as ________.

1. A) metals
2. B) a period
3. C) a group
4. D) a series
5. E) metalloids

 

28) Which element is most likely to be a good conductor of electricity?

1. A) Ar
2. B) N
3. C) F
4. D) Ni
5. E) O

 

29) Which element is chemically similar to lithium?

1. A) Sulfur
2. B) Magnesium
3. C) Iron
4. D) Lanthanum
5. E) Potassium

 

30) Which element is chemically similar to chlorine?

1. A) Sulfur
2. B) Calcium
3. C) Oxygen
4. D) Bromine
5. E) Argon

 

31) Which element is an s block element?

1. A) S
2. B) Ar
3. C) He
4. D) La
5. E) None of these elements is an s block element.

32) Which element is a d block element?

1. A) S
2. B) Ar
3. C) Ag
4. D) As
5. E) None of these elements is a d block element.

 

 

33) Which element has the following orbital diagram?

 

1. A) Li
2. B) Be
3. C) Na
4. D) Mg

 

34) Which element has the following orbital diagram?

 

1. A) O
2. B) N
3. C) C
4. D) Li

 

35) Which element has the following orbital diagram?

 

1. A) Ar
2. B) Cl
3. C) F
4. D) S

36) Which element has the following orbital diagram?

 

1. A) Mg
2. B) K
3. C) Na
4. D) S

 

 

37) The proper electron-dot symbol for aluminum is ________.

A)

B)

C)

D)

 

38) The electron configuration of chlorine is 1s22s22p63s23p5. Which statement about chlorine is incorrect?

1. A) Chlorine has five valence electrons
2. B) Chlorine’s valence shell is the third shell
3. C) Chlorine has five electrons in the 3p subshell
4. D) Chlorine has 17 total electrons

 

39) What is the symbol for the isotope with A = 31 and Z = 15?

A)

B)

C)

D)

40) In the diagram below, which highlighted element is an f block element?

1. A) A
2. B) B
3. C) C
4. D) D
5. E) E

 

 

41) Which statement describing atoms is FALSE?

1. A) The number of protons in an atom is referred to as the atomic number of the atom.
2. B) The total number of protons, neutrons, and electrons in an atom is referred to as the mass number of the atom.
3. C) Protons and neutrons are located in the nucleus of an atom.
4. D) Electrons are located in the space outside the nucleus called the electron cloud.

 

42) Antimony is a metalloid containing 51 protons that is alloyed with lead and used in car batteries. What is the element symbol for antimony?

1. A) A
2. B) An
3. C) At
4. D) Sb
5. E) Cr

 

43) Which statement concerning the elements fluorine, chlorine, bromine, and iodine is INCORRECT?

1. A) These elements are all halogens.
2. B) These elements all have the same valence shell.
3. C) These elements are all nonmetals.
4. D) These elements all have the same number of valence electrons.

44) A sulfur atom has a larger atomic radius than an oxygen atom. Which statement best explains why?

1. A) Sulfur contains more electrons than oxygen does.
2. B) Sulfur contains more protons than oxygen does.
3. C) The valence shell of sulfur is farther away from the nucleus than the valence shell of oxygen is.
4. D) The larger number of protons in an oxygen atom pulls its electrons closer to the nucleus than a sulfur atom.

 

45) Zirconium (Zr) is an element classified as a metal. Which property cannot be assumed based on its classification as a metal?

1. A) Zr has a relatively high density
2. B) Zr is a trace element in the body
3. C) Zr is a good conductor of electricity
4. D) Zr is a shiny solid

 

46) Which element is located in period 3, Group 3A?

1. A) Al
2. B) S
3. C) Si
4. D) B

 

 

47) What is the Period and Group for the element Bromine?

1. A) Period 4, Group 7A
2. B) Period 7, Group 4A
3. C) Period 2, Group 3A
4. D) Period 6, Group 2A

 

48) What is the period and Group for the element Boron?

1. A) Period 2, Group 13A
2. B) Period 3, Group 3A
3. C) Period 2, Group 3A
4. D) Period 4, Group 8A

 

49) Protons and electrons reside in the nucleus of an atom.

 

50) Electrons are negatively charged and have the smallest mass of the three subatomic particles.

 

51) The nucleus contains most of the mass of an atom and is positively charged.

 

52) All atoms of the same element contain the same number of protons.

 

53) An alloy is a mixture of two or more elements that has metallic properties.

 

54) Fl is the element symbol for fluorine.

55) The element symbol S represents sodium.

 

56) Hydrogen is located in group 1A but it is not considered an alkali metal.

 

57) The element symbol for iron is Fe.

 

58) Helium is an s block element.

 

59) Nonmetals have a shiny appearance, and they are generally poor conductors of heat and electricity.

 

60) All elements have at least two naturally occurring isotopes.

 

61) Oxygen, carbon, hydrogen, and nitrogen are called the building-block elements because they make up the majority of the mass of the human body.

 

62) A compound is a pure substance formed by chemically combining two or more elements together.

 

63) The farther a shell is from the nucleus, the larger its volume becomes, and the more electrons it can hold.

 

64) The mass of a neutron is equal to the mass of a proton plus the mass of an electron.

 

65) The 5s orbital is lower in energy than the 4d orbital.

 

66) The electron-dot symbol for barium is .

 

67) Magnesium is a metal.

 

68) Sulfur is a metal.

 

69) All metals are solids at room temperature.

 

70) The maximum number of electrons that can occupy the 3d subshell is ten (10).

 

71) Phosphorus has 15 valence electrons.

 

72) A bromine atom is smaller than a potassium atom.

 

73) Iodine has smaller ionization energy than chlorine.

 

74) The electron configuration for calcium is 1s22s22p63s23p64s2.

 

75) When orbitals are equal in energy, one electron is added to each orbital until the orbitals are half-filled, before any orbital is completely filled.

76) When two electrons occupy the same orbital they have paired spins—that is, the spins are opposite in direction.

 

77) Group 6A elements have the general electron configuration of ns2np6.

 

78) The electron cloud contains most of the volume of an atom.

 

79) Bromine is abbreviated by the two-letter symbol BR.

 

80) A column in the periodic table is called a period.

 

81) An atom with A = 21 and Z = 10 is an isotope of an atom with A = 20 and Z = 10.

 

82) The atomic weight of an element is the sum of the masses of the naturally occurring isotopes of the element.

 

83) Strontium and barium have similar chemical properties.

 

84) The number of electrons that an orbital can contain depends on the type of orbital.

 

85) Fluorine has higher ionization energy than neon.

86) An iodine atom is larger than both a krypton atom and a tellurium atom.

 

87) Radium is a noble gas.

 

88) The chemical formula S8 represents a compound.

 

89) Identify the element with the ground state electron configuration 1s22s22p63s23p6.

1. A) argon, Ar
2. B) calcium ion, Ca2+
3. C) chlorine, Cl
4. D) krypton, Kr
5. E) potassium ion, K+

 

90) Identify ground state electron configuration for the element aluminum. Select all that apply.

1. A) 1s22s83s3
2. B) 1s22s22p63s23p1
3. C) 3s23p1
4. D) [Mg]3p1
5. E) [Ne]3s3
6. F) [Ne]3s23p1

 

91) The electrons in the outermost shell of an atom are called the ________ electrons.

 

92) The name of the halogen in period 3 is ________.

93) Identify the isotope where A equals 49 and Z equals 22.

1. A) Indium-22
2. B) Indium-27
3. C) Indium-49
4. D) Titanium-22
5. E) Titanium-27
6. F) Titanium-49
7. G) None of the choices are correct.

 

94) Isotopes of the same element have the same number of ________.

 

95) Elements in the same group have the same number of ________.

1. A) core electrons
2. B) electrons
3. C) neutrons
4. D) protons
5. E) valence electrons

 

 

96) Iron-56 contains ________ neutrons.

1. A) 56
2. B) 53
3. C) 30
4. D) 26
5. E) 3

 

97) Tungsten is a metal containing 74 protons that is widely used in the electronics industry. What is the elemental symbol for tungsten?

 

General, Organic and Biological Chemistry, 4e (Smith)

Chapter 4   Covalent Compounds

 

1) Covalent bonds result from the ________ electrons between two atoms.

1. A) transfer of
2. B) equal sharing of
3. C) unequal sharing of
4. D) Transfer of, equal sharing of, and unequal sharing of are correct.
5. E) Equal sharing of and unequal sharing of are correct.

 

2) A diatomic molecule contains ________.

1. atoms of two different elements bonded together with a covalent bond
2. two atoms of the same element bonded together with a covalent bond

III. two lone pairs of electrons

1. A) I only
2. B) II only
3. C) III only
4. D) I or II only
5. E) I and III only

 

3) Identify the diatomic element from the given choices.

1. A) Chlorine
2. B) Carbon
3. C) Boron
4. D) Sulfur
5. E) Lithium

 

4) Identify the diatomic element from the given choices.

1. A) Phosphorus
2. B) Helium
3. C) Nitrogen
4. D) Silicon
5. E) Sodium

 

5) Which of the following compounds is classified as covalent?

1. A) KCl
2. B) LiBr
3. C) HCl
4. D) NaBr
5. E) None of the choices are correct.

 

6) Which of the following compounds is not classified as covalent?

1. A) CH4
2. B) SF6
3. C) PBr3
4. D) MgCl2
5. E) None of the choices are correct.

 

7) What is another name for an unshared pair of electrons in a covalent compound?

1. A) Lone pair of electrons
2. B) Nonbonded electron pair
3. C) Bonding pair of electrons
4. D) Lone pair of electrons or nonbonded electron pair

 

8) Which of the statements concerning chemical bonds is false?

1. A) The sharing of electrons between two nonmetal atoms results in a covalent bond.
2. B) The attraction between oppositely charged ions results in an ionic bond.
3. C) The term nonpolar is used to describe a covalent bond in which electrons are not shared equally.
4. D) A bond dipole is the separation of charge that results when atoms sharing electrons have different electronegativities.

 

9) How many covalent bonds are generally formed by atoms with five valence electrons?

1. A) 1
2. B) 2
3. C) 3
4. D) 4
5. E) 5

 

10) How many covalent bonds are generally formed by an oxygen atom?

1. A) 1
2. B) 2
3. C) 3
4. D) 4
5. E) 5

 

11) Which of the following elements will generally form only one covalent bond?

1. A) Sulfur
2. B) Carbon
3. C) Hydrogen
4. D) Argon
5. E) Nitrogen

 

12) How many lone pairs of electrons are present in the Lewis structure of ammonia, NH3?

1. A) 0
2. B) 1
3. C) 2
4. D) 3
5. E) 4

 

13) How many nonbonded electron pairs are in the Lewis structure below?

 

1. A) 2
2. B) 4
3. C) 6
4. D) 8
5. E) 16

 

14) What is the Lewis structure for chloroethylene (C2H3Cl)?

A)

B)

C)

D)

 

15) How many valence electrons are in a molecule of formaldehyde (CH2O)?

1. A) 16
2. B) 12
3. C) 10
4. D) 8
5. E) 0

 

16) Identify the correct name for the compound NO2.

1. A) Nitrogen oxide
2. B) Dinitrogen monoxide
3. C) Nitrogen dioxide
4. D) Nitrogen oxate
5. E) Nitrate

 

17) Which choice would be named dinitrogen pentoxide?

1. A) N2O5
2. B) N5O2
3. C) N3O2
4. D) N2O3
5. E) NO

 

18) Which choice would be named carbon tetrachloride?

1. A) CCl
2. B) C4Cl
3. C) CCl4
4. D) CCl3
5. E) C3Cl

 

19) Predict the bond angles around the carbon atom in the structure of carbonic acid shown below. Don’t forget to draw in lone pairs where needed to give octets.

 

1. A) 180°
2. B) 120°
3. C) 109.5°
4. D) 90°
5. E) 60°

 

20) What is the molecular shape around the phosphorus atom in PH3?

1. A) Linear
2. B) Bent
3. C) Trigonal planar
4. D) Tetrahedral
5. E) Trigonal pyramidal

 

21) What are the bond angles in a tetrahedral geometry?

1. A) 180°
2. B) 120°
3. C) 109.5°
4. D) 90°
5. E) 60°

 

22) Aspartic acid is an amino acid used to synthesize proteins. How many lone pairs of electrons need to be added to complete the aspartic acid structure shown below?

 

1. A) 4
2. B) 6
3. C) 8
4. D) 9
5. E) 11

 

23) Which of the following molecule(s) is(are) polar?

1. A) CO2
2. B) CH4
3. C) CBr4
4. D) CHBr3
5. E) More than one of the molecules are polar.

 

24) Rank the atoms Br, Cl, and K in order of increasing electronegativity.

1. A) K < Br < Cl
2. B) Cl < Br < K
3. C) Br < Cl < K
4. D) K < Cl < Br
5. E) Cl < K < Br

 

25) Rank the atoms Br, Cl, and F in order of increasing electronegativity.

1. A) F < Br < Cl
2. B) Cl < Br < F
3. C) Br < Cl < F
4. D) F < Cl < Br
5. E) Cl < F < Br

 

26) Which atom has the lowest electronegativity?

1. A) Al
2. B) S
3. C) Se
4. D) Rb
5. E) F

 

27) Which bond is the MOST polar?

1. A) C–N
2. B) C–O
3. C) C–C
4. D) C–Cl
5. E) C–F

 

28) Which bond is the LEAST polar?

1. A) C–N
2. B) C–O
3. C) C–C
4. D) C–Cl
5. E) C–F

 

29) Aspartic acid is an amino acid used to synthesize proteins. How many polar bonds are in the aspartic acid structure shown below?

 

1. A) 4
2. B) 6
3. C) 9
4. D) 12
5. E) 15

 

30) What is the correct chemical formula of selenium dioxide?

1. A) SO2
2. B) SeO2
3. C) Se2O
4. D) OS2

 

31) Which bond has the polarity incorrectly labeled?

1. A) δ+H–Cl δ–
2. B) δ+O–C δ–
3. C) δ+Cl–F δ–
4. D) δ–Cl–Br δ+
5. E) δ–F–O δ+

 

32) What is the chemical formula for dinitrogen tetroxide?

1. A) N4O2
2. B) O4N2
3. C) N2O4
4. D) O2N4
5. E) NO2

 

33) Which is the correct Lewis structure for OBr–?

A)

B)

C)

D)

E)

 

34) Estimate the bond angles around the sulfur atom in the structure shown below.

 

1. A) 90°
2. B) 109.5°
3. C) 120°
4. D) 180°

 

35) What is the molecular shape around the nitrogen atom in the structure shown below?

 

1. A) linear
2. B) bent
3. C) trigonal planar
4. D) tetrahedral
5. E) trigonal pyramidal

 

36) What is the molecular shape around the oxygen atom in the structure shown below?

 

1. A) linear
2. B) bent
3. C) trigonal planar
4. D) tetrahedral
5. E) trigonal pyramidal

 

37) Which element may have more than eight valence electrons around it when present in a covalent compound?

1. A) C
2. B) B
3. C) N
4. D) P
5. E) O

 

38) Which molecule or ion has ONLY two resonance structures to describe its bonding?

1. A) CO32–
2. B) NO3–
3. C) HCO31–
4. D) SO3

 

39) Which of the following is classified as a group in the valence shell electron pair repulsion (VSEPR) theory?

1. A) An atom
2. B) A lone pair of electrons
3. C) A valence electron
4. D) Either an atom or a valence electron
5. E) Either an atom or a lone pair of electrons

 

40) Which molecule’s Lewis structure contains an atom that violates the octet rule?

1. A) H2O
2. B) BeH2
3. C) PCl3
4. D) H2Se

 

41) Which compound has the greatest number of valence electrons?

1. A) H2S
2. B) CH4
3. C) NH3
4. D) H2O
5. E) All of the molecules have the same number of valence electrons.

 

42) How many total valence electrons does the polyatomic ion NH4+ possess?

1. A) 8
2. B) 9
3. C) 10
4. D) 11
5. E) 7

 

43) How many total valence electrons does the polyatomic ion OBr– possess?

1. A) 11
2. B) 12
3. C) 13
4. D) 14
5. E) 15

 

44) Which atom(s) in the structure below has(have) a partial negative charge (δ–)?

 

1. A) Carbon
2. B) Fluorine
3. C) Hydrogen
4. D) Nitrogen
5. E) Nitrogen and fluorine

 

45) How many lone pairs of electrons need to be added to the Lewis structure of carbonic acid shown below?

 

1. A) 0
2. B) 3
3. C) 4
4. D) 6
5. E) 7

 

46) What is the total number of bonding electrons in the structure below?

 

1. A) 5
2. B) 10
3. C) 20
4. D) 30

 

47) Which Lewis structure is incorrect?

A)

B)

C)

D)

 

48) The Lewis structure shown below is not a valid Lewis structure. What statement best describes the error in the structure?

 

1. A) The nitrogen atoms violate the octet rule.
2. B) The chlorine atoms violate the octet rule.
3. C) The structure contains an incorrect number of valence electrons.
4. D) Chlorine atoms and nitrogen atoms do not typically form bonds with each other.

 

49) Which of the statements concerning compounds is INCORRECT?

1. A) Compounds are formed when atoms of two or more different elements are chemically bonded.
2. B) Ionic compounds are composed of cations and anions.
3. C) Covalent compounds are composed of metals and nonmetals.
4. D) Covalent compounds are composed of individual molecules.

 

50) Which statement concerning chemical bonds is FALSE?

1. A) A covalent bond involves the sharing of electrons between two nonmetal atoms.
2. B) An ionic bond is the attraction between oppositely charged ions.
3. C) A nonpolar bond is a covalent bond in which electrons are not shared equally between the atoms.
4. D) Electronegativity is a measure of the attraction an atom has for the electrons it shares in a bond.

 

51) Considering the electronegativity values indicated for each element, which covalent bond has the LEAST degree of polarity?

 

 

C	Cl	F	O	N	H
2.5	3.0	4.0	3.5	3.0	2.1

 

1. A) C–N
2. B) N–O
3. C) F–F
4. D) H–Cl

 

52) The covalent bond between chlorine and iodine is a polar one. Which of the following properly represents the direction of polarity in this bond?

1. A) δ+Cl–I δ–
2. B) δ–Cl–I δ+
3. C) +Cl–I –
4. D) –Cl–I +

 

53) The Lewis structure of formaldehyde is shown below. Which statement concerning this structure is INCORRECT?

 

1. A) Two electrons are being shared between the carbon atom and the oxygen atom.
2. B) The oxygen atom has four valence electrons that are not being shared with another atom.
3. C) The oxygen and carbon atoms each have an octet of electrons in their valence shells.
4. D) The hydrogen atoms have filled valence shells.

 

54) A molecule is a discrete group of atoms held together by covalent bonds.

55) A Lewis structure shows the connectivity between atoms in a molecule, as well as where all the bonding and nonbonding valence electrons reside.

 

56) Bonding is the joining of two atoms in a stable arrangement.

 

57) Atoms with three valence electrons generally form five bonds.

58) Atoms with seven valence electrons typically form one covalent bond.

 

59) Every atom must have an octet of electrons in order for a Lewis structure to be considered valid.

 

60) Phosphorus usually forms two covalent bonds in a molecule.

 

61) A double bond consists of four electrons shared between two atoms.

 

62) The Lewis structure for BH3 contains an atom that does not follow the octet rule.

 

63) The Lewis structure for PH3 contains an atom that does not follow the octet rule.

 

64) Resonance structures for a substance differ only in the location of multiple bonds and the position of lone electron pairs.

 

65) There can be a no more than two resonance structures for a molecule.

 

66) The correct name for SF6 is sulfur heptafluoride.

 

67) The formula for dinitrogen pentoxide is N5O2.

 

68) A bond formed between the elements hydrogen and bromine would be considered an ionic bond.

 

69) Unequal sharing of electrons in a covalent bond results in a polar bond.

 

70) Nonpolar molecules may contain polar bonds.

 

71) Some covalent compounds are solids, some are liquids, and some are gases at room temperature.

 

72) C–H bonds are considered to be nonpolar, because the electronegativity difference between carbon and hydrogen is small.

 

73) The symbol δ– is given to the more electronegative atom in a polar bond.

 

74) The structures shown below are resonance structures of sulfur dioxide.

 

and

75) The structures shown below are resonance structures of sulfur dioxide.

 

and

 

76) In the valence shell electron pair repulsion (VSEPR) theory, a group is defined as an atom or a lone pair of electrons.

 

77) A molecule that contains only one polar bond is a polar molecule.

 

78) Ethane (C2H6) is a polar molecule.

 

79) A resonance hybrid is a composite of all resonance structures that spreads out electron pairs in multiple bonds and lone pairs.

 

80) A bond between a carbon atom and a nitrogen atom is a polar covalent bond.

 

81) The molecule below is a polar molecule.

 

 

82) Double bonds and triple bonds are never polar bonds.

 

83) A N–O bond is more polar than a P–O bond.

 

84) The molecule below is a polar molecule.

 

 

85) The shape around each carbon atom in the molecule below is trigonal planar.

 

 

86) The Lewis structure for the molecule below is incomplete because it is missing six pairs of nonbonding electrons.

 

 

87) The shapes around the left and right carbon atoms in the structure below are tetrahedral and linear, respectively.

 

 

88) A double bond is counted as two groups in the valence shell electron pair repulsion (VSEPR) theory.

 

89) Dibromomethane (CH2Br2) is a nonpolar molecule.

 

90) When writing Lewis structures, the symbol below is placed between resonance structures.

 

 

91) The molecular shape around the boron atom in BCl3 is different than the molecular shape around the nitrogen atom in NCl3.

 

92) In Lewis structures, fluorine atoms generally do not obey the octet rule.

 

93) In general, a ________ bond will be one in which the electronegativity difference between two atoms is 0.5 units or greater.

 

94) Electronegativity ________ down a column of the periodic table as the atomic radius increases.

 

95) In the Lewis structure of a molecule, oxygen atoms typically have ________ lone pair(s) of electrons.

 

96) Aspartic acid is an amino acid used to synthesize proteins. There are ________ atoms with a trigonal planar geometry in the aspartic acid structure shown here.

 

1. A) 1
2. B) 2
3. C) 3
4. D) 4
5. E) 5

97) What is the chemical formula for the following Lewis structure?

 

 

98) The chemical formula for phosphorus pentachloride is ________.

 

99) Carbon tetrachloride has ________ valence electrons.

1. A) 4 (four)
2. B) 8 (eight)
3. C) 24 (twenty-four)
4. D) 32 (thirty-two)
5. E) 40 (forty)

 

100) To represent the three-dimensional geometry of a tetrahedron on a two-dimensional piece of paper, a solid line is used for the two bonds in the plane of the paper; a ________ is used to show a bond that extends in front of the plane; and a ________ is used to show a bond that extends behind the plane.

 

101) Carbon usually forms four bonds in stable molecules. However unstable carbon compounds with less than four bonds are known. The methyl carbanion shown below is an example. The molecular shape around the carbon atom in this structure is ________.