Chemistry in Focus A Molecular View of Our World 5th Edition by Nivaldo J. Tro - Test Bank
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Chemistry in Focus A Molecular View of Our World 5th Edition by Nivaldo J. Tro - Test Bank

Chemistry in Focus A Molecular View of Our World 5th Edition by Nivaldo J. Tro - Test Bank   Instant Download - Complete Test Bank With Answers     Sample Questions Are Posted Below   Chapter 5—Chemical Bonding   MULTIPLE CHOICE   Which of these theories is utilized in the prediction of molecular shapes? a. …

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Chemistry in Focus A Molecular View of Our World 5th Edition by Nivaldo J. Tro – Test Bank

 

Instant Download – Complete Test Bank With Answers

 

 

Sample Questions Are Posted Below

 

Chapter 5—Chemical Bonding

 

MULTIPLE CHOICE

 

  1. Which of these theories is utilized in the prediction of molecular shapes?
a. Dalton’s Theory
b. VSEPR Theory
c. Bohr’s Atomic Theory
d. Lewis Bonding Theory
e. Einstein’s Theory of Relativity

 

 

ANS:  B                    PTS:   1

 

  1. What does the V in VSEPR theory stand for?
a. very
b. variable
c. valence
d. vanadium
e. volume

 

 

ANS:  C                    PTS:   1

 

  1. Which of these substances is an ionic compound?

 

I. NCl3
II. MgF2
III. AlBr3
IV. CH4

 

a. I and II
b. II and III
c. II and IV
d. II, III and IV
e. II only

 

 

ANS:  B                    PTS:   1

 

  1. Which of the following is true for sodium?
a. It is most stable as an atom.
b. It is most stable as a negatively charged ion.
c. It is most stable as a positively charged ion.
d. All forms of sodium are very stable.
e. All forms of sodium are very unstable.

 

 

ANS:  C                    PTS:   1

 

  1. Which of these substances is covalent compound?

 

I. CaO
II. H20
III. PF3
IV. CH4

 

 

 

a. I and II
b. II and III
c. II and IV
d. II, III and IV
e. II only

 

 

ANS:  D                    PTS:   1

 

  1. Which of these is not a fundamental postulate of bonding proposed by Lewis?
a. Valence electrons are shared in covalent bonding.
b. The valence shell is involved in chemical bonding.
c. Atoms bond to achieve a more stable configuration.
d. Atoms bond to achieve an octet of electrons in the valence shell.
e. A stable electron configuration has six electrons in the valence shell.

 

 

ANS:  E                    PTS:   1

 

  1. Which of these is the correct Lewis dot structure for chlorine?
a.
b.
c.
d.
e.

 

 

ANS:  C                    PTS:   1

 

  1. Which of these is the correct Lewis dot structure for sulfur?
a.
b.
c.
d.
e.

 

 

ANS:  D                    PTS:   1

 

  1. Which of these is the most likely identity of element A in the Lewis dot structure?

 

a. Ca
b. Li
c. Al
d. Cs
e. P

 

 

ANS:  A                    PTS:   1

 

 

  1. Which of these is the most likely identity of element A in the Lewis dot structure?

 

a. Ca
b. K
c. N
d. Cl
e. O

 

 

ANS:  D                    PTS:   1

 

  1. Which of these will not form a positive ion in an ionic compound?
a. Ba
b. Rb
c. P
d. Sn
e. Mg

 

 

ANS:  C                    PTS:   1

 

  1. An element which has two valence electrons as an atom will most likely:
a. Lose 2 electrons to become negatively charged and combine with a cation.
b. Lose 2 electrons to become positively charged and combine with an anion.
c. Gain 2 electrons to become negatively charged and combine with a cation.
d. Gain 2 electrons to become positively charged and combine with an anion.
e. All of the above can occur.

 

 

ANS:  B                    PTS:   1

 

  1. Which of these is the correct formula for aluminum oxide?
a. AlO
b. Al2O
c. AlO2
d. Al2O3
e. Al2O2

 

 

ANS:  D                    PTS:   1

 

  1. Which of these is the correct formula for strontium iodide?
a. SrI
b. SrI2
c. Sr2I
d. SrI3
e. Sr2I2

 

 

ANS:  B                    PTS:   1

 

  1. Which of these is the correct formula for sodium phosphide?
a. NaP
b. NaP2
c. Na3P
d. NaP3
e. Na3P2

 

 

ANS:  C                    PTS:   1

 

  1. Ionic bonds are formed when electrons are ____.
a. transferred
b. split
c. shared
d. destroyed
e. heated

 

 

ANS:  A                    PTS:   1

 

  1. Covalent bonds are formed when electrons are ____.
a. transferred
b. split
c. shared
d. destroyed
e. heated

 

 

ANS:  C                    PTS:   1

 

  1. Which of these is the correct Lewis dot structure for carbon monoxide?
a.
b.
c.
d.
e.

 

 

ANS:  D                    PTS:   1

 

  1. How many total valence electrons are there in the Lewis structure of NO3–1?
a. 32
b. 30
c. 20
d. 22
e. None of these.

 

 

ANS:  E                    PTS:   1

 

  1. The total number of valence electrons in NO2– is
a. 16
b. 17
c. 18
d. none of the above

 

 

ANS:  C                    PTS:   1

 

 

  1. Which of these is the correct Lewis dot structure for sulfur trioxide?
a.
b.
c.
d.
e.

 

 

ANS:  C                    PTS:   1

 

  1. Which of these is the correct Lewis dot structure for nitrogen, N2?
a.
b.
c.
d.

 

 

ANS:  A                    PTS:   1

 

  1. How many lone pairs of electrons are around the central atom in PCl3?
a. 0
b. 1
c. 2
d. 3
e. 20

 

 

ANS:  B                    PTS:   1

 

  1. How many lone pairs of electrons are around the central atom in CO2?
a. 0
b. 1
c. 2
d. 3
e. 4

 

 

ANS:  A                    PTS:   1

 

 

  1. How many lone pairs of electrons are around the central atom in H2O?
a. 0
b. 1
c. 2
d. 3
e. 4

 

 

ANS:  C                    PTS:   1

 

  1. Barium fluoride is often used in glass manufacturing. Which of these is the correct formula and bonding type for barium fluoride?
a. BaF, ionic
b. BaF, covalent
c. BaF2, ionic
d. BaF2, covalent
e. Ba2F, ionic

 

 

ANS:  C                    PTS:   1

 

  1. How many bonding pairs of electrons are around the central atom in CO2?
a. 0
b. 1
c. 2
d. 3
e. 4

 

 

ANS:  E                    PTS:   1

 

  1. How many bonding pairs of electrons are around the central atom in HCN?
a. 0
b. 1
c. 2
d. 3
e. 4

 

 

ANS:  E                    PTS:   1

 

  1. Identify the third-row element X which forms the compound

 

a. S
b. Cl
c. P
d. Si
e. Al

 

 

ANS:  A                    PTS:   1

 

 

  1. Identify the fourth-row element X that forms the ion

 

a. Ge
b. As
c. Se
d. Kr
e. Br

 

 

ANS:  C                    PTS:   1

 

  1. How many lone pairs of electrons are around the central atom in SO2?
a. 0
b. 1
c. 2
d. 3
e. 4

 

 

ANS:  B                    PTS:   1

 

  1. How many lone pairs of electrons are around the central atom in CH4?
a. 0
b. 1
c. 2
d. 3
e. 4

 

 

ANS:  A                    PTS:   1

 

  1. Which of these molecules contains a triple bond?
a. PCl3
b. N2
c. SO2
d. H2O
e. CO2

 

 

ANS:  B                    PTS:   1

 

  1. Which of these molecules contains two double bonds?
a. PCl3
b. N2
c. SO2
d. H2O
e. CO2

 

 

ANS:  E                    PTS:   1

 

 

  1. Which of these molecules contains 1 double bond and 1 single bond?
a. PCl3
b. NH3
c. SO2
d. H2O
e. CO2

 

 

ANS:  C                    PTS:   1

 

  1. Which of these molecules contains a triple bond?
a. NH3
b. OCl2
c. C2H2
d. H2O
e. MgO

 

 

ANS:  C                    PTS:   1

 

  1. Which of the following is true about ozone?
a. Its Lewis structure is best represented with resonance structures.
b. It reduces the amount of ultraviolet radiation that reached the earth’s surface.
c. It can be broken down by ultraviolet radiation.
d. All of the above.
e. None of the above.

 

 

ANS:  D                    PTS:   1

 

  1. The molecular geometry of a two atom molecule:
a. is always bent.
b. is always tetrahedral.
c. is always linear.
d. depends on the atoms involved.

 

 

ANS:  C                    PTS:   1

 

  1. Which of these molecules will have a tetrahedral molecular geometry?
a. NH3
b. N2O
c. C2H2
d. CH3Cl
e. MgO

 

 

ANS:  D                    PTS:   1

 

  1. What is the molecular geometry of NH3?
a. tetrahedral
b. bent
c. trigonal pyramidal
d. trigonal planar
e. linear

 

 

ANS:  C                    PTS:   1

 

 

  1. Which of the following results in bent molecular geometry?
a. 4 bonding groups and no lone pair on the central atom.
b. 2 bonding groups and one lone pair on the central atom.
c. 2 bonding groups and 2 lone pairs on the central atom.
d. Both B + C
e. Both A + C

 

 

ANS:  D                    PTS:   1

 

  1. Which of these molecules will have a trigonal pyramidal molecular geometry?
a. PCl3
b. N2O
c. C2H2
d. CH3Cl
e. SO2

 

 

ANS:  A                    PTS:   1

 

  1. Which of these would be expected to have a trigonal planar electron geometry?

 

a. I and II
b. II and III
c. I, II, and III
d. I and III
e. I only

 

 

ANS:  E                    PTS:   1

 

  1. Which of these would be expected to have a linear molecular geometry?

 

a. I and II
b. II and IV
c. I, II, and IV
d. I, and III
e. IV only

 

 

ANS:  B                    PTS:   1

 

  1. Which of these molecules will have a trigonal planar electron geometry and a bent molecular geometry?
a. PCl3
b. H2O
c. C2H2
d. CH3Cl
e. SO2

 

 

ANS:  E                    PTS:   1

 

  1. Which of these molecules will have a tetrahedral electron geometry and a tetrahedral molecular geometry?
a. PCl3
b. H2O
c. C2H2
d. CH3Cl
e. SO2

 

 

ANS:  D                    PTS:   1

 

  1. Which of these molecules will have a tetrahedral electron geometry and a bent molecular geometry?
a. PCl3
b. H2O
c. C2H2
d. CH3Cl
e. SO2

 

 

ANS:  B                    PTS:   1

 

  1. Which of these molecules will have a tetrahedral electron geometry and a trigonal pyramidal molecular geometry?
a. PCl3
b. H2O
c. C2H2
d. CH3Cl
e. SO2

 

 

ANS:  A                    PTS:   1

 

  1. Which of these molecules will have a linear electron geometry and a trigonal pyramidal molecular geometry?
a. PCl3
b. H2O
c. C2H2
d. CH3Cl
e. None of these.

 

 

ANS:  E                    PTS:   1

 

  1. Which of these molecules will have a linear electron geometry and a linear molecular geometry?
a. PCl3
b. H2O
c. CO
d. CH3Cl
e. BF3

 

 

ANS:  C                    PTS:   1

 

  1. Which of these is the correct molecular geometry of CCl4?
a. linear
b. trigonal planar
c. tetrahedral
d. trigonal pyramidal
e. bent

 

 

ANS:  C                    PTS:   1

 

  1. Which of these is the correct molecular geometry of PCl3?
a. linear
b. trigonal planar
c. tetrahedral
d. trigonal pyramidal
e. bent

 

 

ANS:  D                    PTS:   1

 

  1. Which of these is the correct molecular geometry of SO2?
a. linear
b. trigonal planar
c. tetrahedral
d. trigonal pyramidal
e. bent

 

 

ANS:  E                    PTS:   1

 

  1. Which of these is the correct molecular geometry of CO2?
a. linear
b. trigonal planar
c. tetrahedral
d. trigonal pyramidal
e. bent

 

 

ANS:  A                    PTS:   1

 

  1. Which of these is the correct molecular geometry of BF3?
a. linear
b. trigonal planar
c. tetrahedral
d. trigonal pyramidal
e. bent

 

 

ANS:  B                    PTS:   1

 

  1. What is the molecular geometry of NH4+?
a. trigonal planar
b. tetrahedral
c. trigonal pyramidal
d. bent

 

 

ANS:  B                    PTS:   1

 

  1. A molecule with tetrahedral electron geometry could which of the following molecular geometry?
a. tetrahedral
b. trigonal pyramidal
c. bent
d. All of the above.

 

 

ANS:  D                    PTS:   1

 

 

  1. Which of these theories is utilized in the prediction of molecular polarity?
a. Dalton’s Theory
b. VSEPR Theory
c. Electronegativity
d. Einstein’s Relativity Theory
e. Both B and C

 

 

ANS:  E                    PTS:   1

 

  1. Electronegativity is:
a. The ability of an atom to form positively charged ions.
b. The ability of an atom to form negatively charged ions.
c. Also called a dipole
d. The ability of an atom to attract bonding electrons.
e. The ability of an atom to form polar molecules.

 

 

ANS:  D                    PTS:   1

 

  1. The element with the highest electronegativity is_________.
a. fluorine
b. hydrogen
c. helium
d. neon

 

 

ANS:  A                    PTS:   1

 

  1. List the elements Na, K, Al, Cl, Cs in order of decreasing electronegativity.(from greatest to least)
a. Na > Cl > Al > K > Cs
b. Cs > Na > K > Cl > Al
c. Cl > Na > Al > K > Cs
d. Cl > Al > Na > K > Cs
e. Na > Cs > K > Al > Cl

 

 

ANS:  D                    PTS:   1

 

  1. Which of these elements has the highest electronegativity?
a. Ca
b. N
c. Se
d. P
e. O

 

 

ANS:  E                    PTS:   1

 

  1. Which of these elements has the lowest electronegativity?
a. Ca
b. N
c. Se
d. P
e. O

 

 

ANS:  A                    PTS:   1

 

 

  1. List the elements Na, K, Al, Cl, Cs in order of increasing electronegativity.(from least to greatest)
a. Na < Cs < Al < K < Cl
b. Cs < Na < K < Cl < Al
c. Cl < Na < Al < K < Cs
d. Cl < Al < Na < K < Cs
e. Cs < K < Na < Al < Cl

 

 

ANS:  E                    PTS:   1

 

  1. A nonpolar bond would most likely result when:
a. a metal bonds to a nonmetal.
b. a nonmetal bonds to a metal.
c. two identical nonmetal atoms bond.
d. an atom bonds to hydrogen.

 

 

ANS:  C                    PTS:   1

 

  1. Of the bonds below, the most polar bond would be:
a. C-C c. C-O
b. C-N d. C-F

 

 

ANS:  D                    PTS:   1

 

  1. Water:
a. Is a polar molecule.
b. Has tetrahedral electron geometry.
c. Has bent molecular geometry.
d. Has two lone pairs of electrons on the central atom.
e. All of the above.

 

 

ANS:  E                    PTS:   1

 

  1. Which of the following molecules is nonpolar?
a. CO2
b. N2
c. CH4
d. CCl4
e. All of the above.

 

 

ANS:  E                    PTS:   1

 

  1. Which of these is a polar molecule?

 

I. PCl3
II. H2O
III. CO2
IV. BF3

 

a. I only
b. I and II
c. I, II and IV
d. II only
e. II and IV

 

 

ANS:  B                    PTS:   1

 

 

  1. Element A has an electronegativity of 0.8 and element B has an electronegativity of 2.0. Which statement best describes the bonding in A3B?
a. The AB bond is largely covalent with a d– on A.
b. The AB bond is largely covalent with a d+ on A.
c. The compound is largely ionic with no polar bonds.
d. The compound is largely covalent with no polar bonds.
e. There is insufficient information.

 

 

ANS:  B                    PTS:   1

 

  1. Which of these contains polar bonds but is a nonpolar molecule?

 

I. NCl3
II. H2
III. CO2
IV. BF3

 

a. I only
b. I and III
c. III and IV
d. III only
e. I, III and IV

 

 

ANS:  C                    PTS:   1

 

  1. Which of these is a polar molecule with a tetrahedral electron geometry?

 

I. NCl3
II. H2O
III. CH3Cl
IV. SiH4

 

a. I only
b. I and III
c. I,II and III
d. III only
e. II and III

 

 

ANS:  E                    PTS:   1

 

  1. The [NO2]–molecule has ____ double bonds, ____ single bond(s), and ____ lone (nonbonding) pair(s) of electrons and ____ resonance forms.
a. 2, 0, 8, 2
b. 1, 1, 8, 3
c. 1, 1, 6, 2
d. 0, 2, 10, 0
e. 2, 0, 12, 2

 

 

ANS:  C                    PTS:   1

 

 

  1. Which of these is a nonpolar molecule?
a. CO
b. H2O
c. O3
d. PCl3
e. SO3

 

 

ANS:  E                    PTS:   1

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