Deck 9: Bonding and Molecular Structure

Question 1

An atom of Se has ____ valence electrons.

A) 2
B) 6
C) 4
D) 3
E) 8

Answer 1

6

Question 2

Which of the following is a correct Lewis structure for H₂SO₄?

A)
B)
C)
D)
E)

Answer 2

Question 3

Which of the following groups contains no ionic compounds?

A) HCN,NO₂,Ca(NO₃)₂
B) PCl₅,LiBr,Zn(OH)₂
C) KOH,CCl₄,SF₄
D) NaH,CaF₂,NaNH₂
E) CH₂O,H₂S,NH₃

Answer 3

CH₂O,H₂S,NH₃

Question 4

Which of the following statements is/are CORRECT?
1)Ionic bonds form when one or more valence electrons are transferred from one atom to another.
2)Covalent bonds involve sharing of electrons between atoms.
3)In most covalently bonded compounds,electrons are NOT shared equally between the atoms.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1,2,and 3

Question 5

In which pair do $\underline{\text{ both }}$ compounds exhibit predominantly ionic bonding?

A) KI and O₃
B) NaF and H₂O
C) PCl₃ and HF
D) Na₂SO₃ and CH₄
E) RbBr and CaO

Question 6

Which of the following molecules or ions will have a Lewis structure most like that of phosphorus trichloride,PCl₃?

A) ClO₃^-
B) SO₃
C) CO₃^2-
D) BF₃
E) Cl₂CO

Question 7

Which of the following molecules or ions are isoelectronic: SO₃,NF₃,NO₃^-,CO₃^2-?

A) SO₃ and NF₃
B) NF₃ and CO₃^2-
C) SO₃,NF₃ and CO₃^2-
D) SO₃,NO₃^- and CO₃^2-
E) SO₃,NF₃,NO₃^-,and CO₃^2-

Question 8

Which of the following has a Lewis structure similar to CS₂?

A) NH₂^-
B) O₃
C) NO₂^-
D) SO₂
E) ClO₂^-

Question 9

In the Lewis formula for sulfur dioxide,SO₂,the number of lone pairs of electrons around the sulfur atom is

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

Question 10

If two or more species have the same number of electrons,resulting in similar Lewis structures,they are said to be ____.

A) isoelectronic
B) resonant structures
C) ionic
D) neutral
E) covalent

Question 11

How many lone pairs of electrons are assigned to the iodine atom in ICl?

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

Question 12

How many valence electrons are present in the Lewis formula for the hypochlorite ion, ?

A) 20
B) 12
C) 18
D) 14
E) 16

Question 13

Which of the following is a correct Lewis electron-dot formula for CO?

A)
B)
C)
D)
E)

Question 14

Which combination of atoms is most likely to produce a compound with ionic bonds?

A) B and C
B) S and O
C) N and F
D) Si and Cl
E) Mg and O

Question 15

The correct Lewis structure for Cl₂CO is (the 2 Cl's and the O are bound to the C and not to each other):

A)
B)
C)
D)
E) none of these

Question 16

Which of the following is a correct Lewis structure for sulfate ion?

A)

B)

C)

D)

E)

Question 17

Which of the following statements is/are CORRECT?
1)Chemical reactions result in the gain,loss,or rearrangement of valence electrons.
2)For main group elements,the number of valence electrons equals eight minus the element's group number.
3)Core electrons are not involved in bonding or in chemical reactions.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 3
E) 1,2,and 3

Question 18

What is the total number of electrons (both lone and bond pairs)in the Lewis structure of C₂O₄2-?

A) 30
B) 34
C) 32
D) 46
E) 44

Question 19

Which combination of atoms is most likely to produce a compound with covalent bonds?

A) K and Br
B) Al and S
C) S and Cl
D) Sn and F
E) Li and I

Question 20

The following representation of an atom is called

A) a Lewis dot structure.
B) an ion.
C) a structural formula.
D) an electrostatic potential map.
E) an ionic bond.

Question 21

What is the formal charge on atom N in the following Lewis structure?

A) 2
B) 1
C) 0
D) -1
E) -2

Question 22

Which of the following exhibits resonance?

A) SCl₆
B) H₂O
C) SO₂
D) NH₃
E) none

Question 23

One resonance structure for OCN^- ion is drawn below.What is the formal charge on each atom?

A) O atom = 0,C atom = 0,and N atom = 0
B) O atom = 0,C atom = 0,and N atom = -1
C) O atom = -1,C atom = 0,and N atom = 0
D) O atom = -1,C atom = -1,and N atom = +1
E) O atom = +1,C atom = 0,and N atom = -2

Question 24

Which of the following is a correct Lewis structure for oxygen?

A)
B)
C)
D)
E)

Question 25

The molecule H₂S has

A) 2 bonding pairs and 3 lone pairs
B) 2 bonding pairs and 2 lone pairs
C) 3 bonding pairs and 1 lone pair
D) 3 bonding pairs and 3 lone pairs
E) none of these

Question 26

All of the following Lewis structures of nitrogen oxides are possible EXCEPT

A) N₂O.
B) N₂O₄.
C) N₂O₃.
D) N₂O₅.
E) All of the above are correct structures.

Question 27

Which of the following molecules or ions does not have one or more resonance structures?

A) O₃
B) OCN^-
C) SO₂
D) H₂CO
E) NO₃^-

Question 28

What is the formal charge on carbon in CH₂Cl₂?

A) +2
B) +1
C) 0
D) -1
E) -2

Question 29

The central atom in N₂O is a nitrogen atom.This nitrogen atom is surrounded by

A) two single bonds and two lone pairs of electrons.
B) two single bonds and one lone pair of electrons.
C) one single bond,one double bond,and one lone pairs of electrons.
D) one single bond,one double bond,and one lone pair of electrons.
E) two double bonds and no lone pairs of electrons.

Question 30

Which is the best Lewis structure of CH₂FCO₂H (connectivity correct as given)?

A)
B)
C)
D)
E) none of these is acceptable

Question 31

How many different molecules have the molecular formula C₆H₁₄?

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

Question 32

Which of the following are possible Lewis structures for C₂H₆O?

A) 1
B) 2
C) 3
D) 2 and 3
E) 1,2,and 3

Question 33

Which of the following is/are true concerning formal charge?
1)The formal charge of each individual atom in a molecule or ion is an actual atomic charge that can be experimentally determined.
2)The formal charge of each individual atom is always the same for each possible resonance form.
3)The sum of the formal charges of each atom in a molecule or ion equal the overall charge of the molecule or ion.

A) 1 only
B) 2 only
C) 3 only
D) 1 and 2
E) 1 and 3

Question 34

Which of the following are resonance structures for formate ion,HCO₂^-?

A) 1 and 2
B) 2 and 3
C) 3 and 4
D) 1,3,and 4
E) 2,3,and 4

Question 35

Which of the following is the correct Lewis dash formula for carbon diselenide?

A)
B)
C)
D)
E)

Question 36

The nitrogen atom in cyanide ion,CN^-,is surrounded by

A) one single bond and three lone pairs of electrons.
B) one double bond and one lone pair of electrons.
C) one double bond and two lone pairs of electrons.
D) one triple bond and one lone pair of electrons.
E) one triple bond and no lone pairs of electrons.

Question 37

What is the formal charge on each atom in dichloromethane,CH₂Cl₂?

A) C atom = 0,each H atom = 0,and each Cl atom = 0
B) C atom = -2,each H atom = +1,and two Cl atoms = 0
C) C atom = +4,each H = -1,and each Cl atom = -1
D) C atom = +4,each H = +1,and each Cl atom = -1
E) C atom = -4,each H = +1,and each Cl atom = +1

Question 38

What is the formal charge of the $\underline{\text{ carbon }}$ atom in the Lewis structure for isocyanate shown below?

A) 0
B) (-2)
C) +1
D) (-1)
E) -3

Question 39

How many hydrogen atoms are needed to complete the following hydrocarbon structure?

A) 4
B) 6
C) 2
D) 8
E) 3

Question 40

Which of the following is not a valid resonance structure for N₃^-?

A)
B)
C)
D)
E) all are correct

Question 41

What is the molecular geometry around an atom in a molecule or ion which is surrounded by zero lone pairs of electrons and four single bonds.

A) tetrahedral
B) linear
C) bent
D) trigonal pyramidal
E) trigonal planar

Question 42

What is the molecular geometry around carbon atom C₃?

A) linear
B) tetrahedral
C) trigonal planar
D) trigonal pyramidal
E) square planar

Question 43

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of sulfur dioxide,SO₂.

A) The electron-pair geometry is trigonal-planar,the molecular geometry is trigonal-planar.
B) The electron-pair geometry is trigonal-planar,the molecular geometry is bent.
C) The electron-pair geometry is tetrahedral,the molecular geometry is bent.
D) The electron-pair geometry is tetrahedral,the molecular geometry is linear.
E) The electron-pair geometry is trigonal-bipyramidal,the molecular geometry is linear.

Question 44

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of nitrogen trichloride,NCl₃.

A) The electron-pair geometry is linear,the molecular geometry is linear.
B) The electron-pair geometry is trigonal-planar,the molecular geometry is trigonal-planar.
C) The electron-pair geometry is trigonal-planar,the molecular geometry is bent.
D) The electron-pair geometry is tetrahedral,the molecular geometry is tetrahedral.
E) The electron-pair geometry is tetrahedral,the molecular geometry is trigonal-pyramidal.

Question 45

The Lewis structure of which of the following formula violates the octet rule?

A) SF₆
B) NF₃
C) OF₂
D) HF
E) SiF₄

Question 46

What is the bond angle in a trigonal planar molecule or ion?

A) 109°
B) 180°
C) 90°
D) 72°
E) 120°

Question 47

Which of the following elements is most likely to form a molecular structure that disobeys the octet rule?

A) B
B) C
C) N
D) O
E) F

Question 48

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of boron tribromide,BBr₃.

A) The electron-pair geometry is trigonal-pyramidal,the molecular geometry is trigonal-pyramidal.
B) The electron-pair geometry is trigonal-planar,the molecular geometry is trigonal-planar.
C) The electron-pair geometry is trigonal-planar,the molecular geometry is bent.
D) The electron-pair geometry is tetrahedral,the molecular geometry is trigonal-pyramidal.
E) The electron-pair geometry is trigonal-pyramidal,the molecular geometry is t-shaped.

Question 49

Which of the following species will have a Lewis structure most like that of IF₄^-?

A) XeF₄
B) SO₄^2-
C) PF₄⁺
D) SF₄
E) IO₄^-

Question 50

What is the correct Lewis structure for IF₃?

A)
B)
C)
D)
E)

Question 51

Which of the following elements is able to form a molecular structure that exceeds the octet rule?

A) F
B) N
C) C
D) B
E) Sb

Question 52

Which of the following has an incomplete octet in its Lewis structure?

A) SO₂
B) F₂
C) NO₂
D) ICl
E) CO₂

Question 53

What is the correct Lewis structure for SF₄?

A)
B)
C)
D)
E)

Question 54

When you draw the Lewis structure for PF₂Cl₃,how many single bonds,double bonds,and lone pair electrons reside on the central phosphorus atom?

A) 5 single bonds,0 double bonds,0 lone pairs
B) 4 single bonds,1 double bond,0 lone pairs
C) 5 single bonds,0 double bonds,1 lone pair
D) 4 single bonds,1 double bond,1 lone pair
E) 3 single bonds,2 double bonds,0 lone pairs

Question 55

What is the electron-pair geometry around an atom in a molecule or ion which is surrounded by zero lone pairs of electrons and five single bonds.

A) trigonal bipyramidal
B) see-saw or distorted tetrahedron
C) T-shaped
D) linear
E) trigonal planar

Question 56

What is the molecular geometry around oxygen atom O₂?

A) linear
B) trigonal pyramidal
C) trigonal planar
D) T-shaped
E) tetrahedral

Question 57

The central atom in SF₆ is surrounded by

A) six single bonds and no lone pairs of electrons.
B) six single bonds and one lone pair of electrons.
C) six single bonds and two lone pairs of electrons.
D) five single bonds,one double bond,and one lone pair of electrons.
E) four single bonds,two double bonds,and no lone pairs of electrons.

Question 58

When both of the electrons in a molecular bond originate from the same atom,the bond is called a(n)

A) sigma bond.
B) coordinate covalent bond.
C) pi bond.
D) metallic bond.
E) ionic bond.

Question 59

Which of the following molecules or ions are likely to be free radicals: N₂O,NO,and NO₂?

A) N₂O only
B) NO only
C) NO₂ only
D) N₂O and NO
E) NO and NO₂

Question 60

In the Lewis structure of SF₆,how many lone pairs are around the central atom?

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

Question 61

Place the following molecules in order from smallest to largest H-N-H bond angles: NH₄⁺,NH₃,and NH₂^-.

A) NH₄⁺ < NH₃ < NH₂^-
B) NH₄⁺ < NH₂^- < NH₃
C) NH₂^- < NH₃ < NH₄⁺
D) NH₂^- < NH₄⁺ < NH₃
E) NH₃ < NH₂^- < NH₄⁺

Question 62

Which of the following bonds would be the most polar?

A) N-N
B) N-P
C) N-C
D) N-As
E) N-Ge

Question 63

Based on electron geometries,which of the following molecules has the smallest bond angle between any two adjacent hydrogen atoms?

A) CH₄
B) H₂O
C) BH₃
D) PH₃
E) SF₆

Question 64

Choose which central atom in the following molecules is most electronegative.

A) PH₃
B) CH₄
C) H₂S
D) H₂O
E) NH₃

Question 65

Use VSEPR theory to predict the molecular geometry of BrO₃^-.

A) trigonal-pyramidal
B) trigonal-planar
C) bent
D) T-shaped
E) linear

Question 66

Rank the following covalent bonds in order of decreasing polarity:
C-H,N-H,O-H,F-H.

A) F-H,O-H,N-H,C-H
B) O-H,F-H,N-H,C-H
C) N-H,F-H,O-H,C-H
D) C-H,N-H,O-H,F-H
E) C-H,F-H,O-H,N-H

Question 67

What is the O-C-N bond angle in OCN^-?

A) 90 ^$\circ$
B) 107 ^$\circ$
C) 109.5 ^$\circ$
D) 120 ^$\circ$
E) 180 ^$\circ$

Question 68

Which of the following compounds has polar covalent bonds: CCl₄,Cl₂,HCl,and KCl?

A) CCl₄ only
B) Cl₂ only
C) HCl and KCl
D) Cl₂ and KCl
E) CCl₄ and HCl

Question 69

Use VSEPR theory to predict the molecular geometry of BrF₅.

A) tetrahedral
B) see-saw
C) trigonal-bipyramidal
D) square-pyramidal
E) octahedral

Question 70

What are the approximate F-Br-F bond angles in BrF₅?

A) 90 ^$\circ$ and 180 ^$\circ$
B) 109.5 ^$\circ$
C) 90 ^$\circ$ and 120 ^$\circ$
D) 120 ^$\circ$
E) 180 ^$\circ$

Question 71

Which of the following molecules is nonpolar?

A) sulfur dioxide,SO₂
B) phosphorus trifluoride,PF₃
C) hydrogen fluoride,HF
D) phosphorus pentafluoride,PF₅
E) nitrogen trifluoride,NF₃

Question 72

Three non-equivalent Lewis structures for carbonyl sulfide,SCO,are given below.Use the concepts of formal charge and electronegativity to choose the structure that is the best representation.

$~~~~~~~~$ A $~~~~~~~~$$~~~~~~~~$$~~~~~~~~$$~~~~~~~~$$~~~~~~~~$ B $~~~~~~~~$$~~~~~~~~$$~~~~~~~~$$~~~~~~~~$ C

A) Structure A,because all the formal charges equal 0.
B) Structure B,because all the formal charges equal 0.
C) Structure C,because all the formal charges equal 0.
D) Structure A,because the negative formal charge resides on the most electronegative atom.
E) Structure C,because the negative formal charge resides on the most electronegative atom.

Question 73

Use VSEPR theory to predict the molecular geometry around the carbon atom in formaldehyde,H₂CO.

A) linear
B) bent
C) trigonal-planar
D) tetrahedral
E) octahedral

Question 74

What are the approximate H-N-H bond angles in NH₄⁺?

A) 109.5 ^$\circ$
B) 120 ^$\circ$
C) 109.5 ^$\circ$ and 120 ^$\circ$
D) 90 ^$\circ$
E) 90 ^$\circ$ and 120 ^$\circ$

Question 75

Use VSEPR theory to predict the electron-pair geometry and the molecular geometry of sulfur dioxide,XeF₄.

A) The electron-pair geometry is tetrahedral,the molecular geometry is tetrahedral.
B) The electron-pair geometry is octahedral,the molecular geometry is tetrahedral.
C) The electron-pair geometry is tetrahedral,the molecular geometry is octahedral.
D) The electron-pair geometry is octahedral,the molecular geometry is square-planar.
E) The electron-pair geometry is square-planar,the molecular geometry is tetrahedral.

Question 76

Atoms having equal or nearly equal electronegativities are expected to form

A) no bonds
B) polar covalent bonds
C) nonpolar covalent bonds
D) ionic bonds
E) covalent bonds

Question 77

Electronegativity is a measure of

A) the ability of a substance to conduct electricity.
B) the charge on a polyatomic cation.
C) the charge on a polyatomic anion.
D) the ability of an atom in a molecule to attract electrons to itself.
E) the oxidation number of an atom in a molecule or polyatomic anion.

Question 78

Use VSEPR theory to predict the molecular geometry around the nitrogen atom in nitrite ion,NO₂^-.

A) trigonal-planar
B) tetrahedral
C) trigonal-pyramidal
D) T-shaped
E) bent

Question 79

Use VSEPR theory to predict the molecular geometry around either carbon atom in acetylene,C₂H₂.

A) linear
B) bent
C) trigonal-planar
D) tetrahedral
E) octahedral

Question 80

What are the approximate O-S-O bond angles in SO₃^2-?

A) 90 ^$\circ$
B) 109.5 ^$\circ$
C) 120 ^$\circ$
D) 180 ^$\circ$
E) 90 ^$\circ$ and 180 ^$\circ$