Deck 9: Chemical Bonds

Question 1

The Lewis electron diagram of an atom is shown below. This atom has a valence shell configuration of ns²np¹.

Answer 1

True

Question 2

Electronegativity is a unitless number

Answer 2

True

Question 3

The following is the accurate Lewis electron diagram for a P atom.

Answer 3

False

Question 4

When electrons are transferred to a central atom to form a compound, a covalent bond is formed.

Question 5

Lone electron pairs are electrons that do not make covalent bonds.

Question 6

BeCl₂ is an example of an electron deficient molecule.

Question 7

O is the central atom in an H₂O molecule.

Question 8

The equal sharing of electrons in a covalent bond is called a nonpolar covalent bond.

Question 9

Most odd electron compounds are chemically inactive.

Question 10

The measured strength of ionic bonding is called the lattice energy.

Question 11

A Cl^- ion has fulfilled the octet rule of valence electrons.

Question 12

NO₂ is an example of an odd electron molecule.

Question 13

A Na atom needs to gain two electrons to fulfill the octet rule.

Question 14

The H−H bond is an example of a covalent bond.

Question 15

A C-H bond is a nonpolar covalent bond.

Question 16

A Lewis electron dot diagram represents only the protons of an atom.

Question 17

The following is the accurate Lewis electron diagram for a carbon atom.

Question 18

A bond will definitely be polar covalent if the electronegativity difference between the atoms involved is 1.4.

Question 19

An ionic bond is formed between two atoms with the same charge.

Question 20

Strength of an ionic bond decreases with an increase in the magnitude of the charge.

Question 21

Two hydrogen atoms share electrons to form a stable compound. This type of a bond is called a(n)_____ bond.

A) ionic
B) hydrogen
C) dipole
D) covalent
E) metallic

Question 22

Which of the following ions contain an octet of valence electrons?

A) N^2-
B) O^-
C) Na²⁺
D) F^-
E) Ba⁺

Question 23

How many electrons should a Ca atom lose to satisfy the octet rule?

A) 1
B) 2
C) 3
D) 4
E) 8

Question 24

The molecule CH₂O takes a trigonal pyramidal shape.

Question 25

The measured strength of ionic bonding is called the _____ energy.

A) kinetic
B) valence
C) covalent
D) lattice
E) latent

Question 26

A molecule with four surrounding atoms takes a bent molecular shape.

Question 27

How many electrons should a Zn atom lose to satisfy the octet rule?

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

Question 28

Which of the following ions do not contain an octet of valence electrons?

A) Na⁺
B) Rb²⁺
C) S^2-
D) Cl^-
E) Ba²⁺

Question 29

Which of the following occurs when Ca reacts with Cl₂ to form CaCl₂?

A) Ca gains two electrons to become Ca²⁺
B) Cl₂ loses two electrons to become Cl₂^2-
C) Ca loses two electrons to become Ca²⁺
D) Cl₂ gains two electrons to become Cl₂²⁺
E) Cl atoms loses 2 electrons each to become Cl^2-

Question 30

Which of the following is used to represent the Na atom using the Lewis electron dot diagram?

A)
B)
C)
D)
E)

Question 31

NaCl remains stable due to the attraction between the Na⁺ and Cl^- ions. This attraction is called a(n)_____.

A) chemical bond
B) ionic bond
C) covalent bond
D) metallic bond
E) dipole attraction

Question 32

For a chlorine atom to complete an octet, it must _____.

A) lose an electron
B) gain two electrons
C) gain an electron
D) gain five electrons
E) lose two electrons

Question 33

Which of the following is the common convention to represent a helium atom using the Lewis electron dot diagram?

A)
B)
C)
D)
E)

Question 34

A(n) _____ is a representation of the valence electrons of an atom that uses dots around the symbol of the element.

A) Lewis electron dot diagram
B) molecular electron graph
C) structural electron formula
D) HYPERLINK "http://en.wikipedia.org/wiki/Molecular_geometry" molecular electron geometry
E) orbital electron diagram

Question 35

CH₃OH is an example of a molecule that violates the octet rule.

Question 36

Which of the following compounds is characterized by the strongest ionic bond?

A) LiCl
B) NaCl
C) NaBr
D) LiF
E) MgO

Question 37

A GeF₂ molecule has linear geometry.

Question 38

Any molecule with only two atoms has a linear shape.

Question 39

What column of the periodic table has Lewis electron dot diagrams that have four electrons in them?

A) the column headed by oxygen
B) the column headed by fluorine
C) the column headed by carbon
D) the column headed by nitrogen
E) the column headed by boron

Question 40

Which of the following bonds is formed when electrons are shared between atoms?

A) ionic bond
B) covalent bond
C) dipole interaction
D) valence bond
E) metallic bond

Question 41

What is the polarity of a Na-Br bond?

A) likely ionic
B) slightly polar covalent
C) definitely polar covalent
D) slightly ionic
E) nonpolar covalent

Question 42

What is the energy change for this reaction? (Refer to Table 9.2 in the text.)

A) -183 kJ/mol
B) -477 kJ/mol
C) 477 kJ/mol
D) -129 kJ/mol
E) -4.00 kJ/mol

Question 43

What is the polarity of a C-Si bond?

A) likely ionic
B) slightly polar covalent
C) definitely polar covalent
D) slightly ionic
E) nonpolar covalent

Question 44

Which of the following bonds is most likely ionic?

A) C-C
B) Li-F
C) P-H
D) H-I
E) H-Br

Question 45

In the molecule CO₂, how many electrons are shared by C and the two O atoms?

A) 4
B) 5
C) 8
D) 6
E) 10

Question 46

Which of the following molecules is not linear in shape?

A) PCl₃
B) O₂
C) CO₂
D) NO
E) BeH₂

Question 47

Which of the following molecules is likely to have a trigonal planar electron group distribution?

A) H₂O
B) CO₂
C) NO
D) NO₂
E) BF₃

Question 48

Which of the following bonds is most likely to be nonpolar covalent bond?

A) P-H
B) C-H
C) O-H (electronegativity chart in text shows a "D" instead of "O" for oxygen
D) Na-Cl
E) Li-Cl

Question 49

Covalent compounds of _____ usually form electron deficient molecules.

A) hydrogen
B) boron
C) chlorine
D) lithium
E) sodium

Question 50

Which of the following is a stable odd-electron molecule?

A) N₃
B) HF
C) CO₂
D) HCl
E) NO

Question 51

Which of the following molecules is formed by triple bonds alone?

A) F₂
B) N₂
C) O₂
D) O₃
E) CO₂

Question 52

Which of the following has the strongest covalent bond?

A) HF
B) H₂S
C) H₂
D) N₂
E) CO₂

Question 53

A covalent bond of any type is called a(n)_____.

A) neutron group
B) proton group
C) core group
D) nucleus group
E) electron group

Question 54

Identify the correct Lewis electron diagram for CO₂.

A)
B)
C)
D)
E)

Question 55

From the following identify the molecule which has a bent or angular shape.

A) CO₂
B) CaCl₂
C) GeF₂
D) CaF₂
E) SiO₂

Question 56

If the electronegativity of a bond formed between two atoms is 0.15, it is likely to be a(n)_____ bond.

A) likely ionic
B) slightly polar covalent
C) definitely polar covalent
D) slightly ionic
E) nonpolar covalent

Question 57

Diatomic molecules are linear because _____.

A) they form odd-electron molecules around the central atom
B) electron-deficient molecules cannot be formed of only two electron groups
C) only polar covalent bonds are formed in such molecules
D) electron groups repel to get as far away from each other
E) bonds in such compounds have a polarity of less than 0.4

Question 58

Which of the following compounds is characterized by electron deficient molecules?

A) NaCl
B) NO₂
C) NO
D) CO₂
E) BeF₂

Question 59

What is the energy change when one carbon-carbon double bond is broken to form a carbon-carbon single bond and two H-H single bonds? (Refer to Table 9.2 in the text.)

A) -565 kJ/mol
B) -129 kJ/mol
C) 609 kJ/mol
D) -1,176 kJ/mol
E) 129 kJ/mol

Question 60

_____ is a scale for judging how much atoms of any element attract electrons.

A) Electron density
B) Reactivity
C) Electron affinity
D) Magnetivity
E) Electronegetavity

Question 61

A molecule has three electron groups on the central atom and has two surrounding atoms. What is the likely shape of the atom?

A) Trigonal pyramidal
B) Bent
C) Trigonal planar
D) Linear
E) Tetrahedral

Question 62

What is a single bond? Provide an example.

Question 63

What are the factors that determine the strength of ionic bonds?

Question 64

Explain why it is difficult to violate the octet rule.

Question 65

What are Lewis electron dot diagrams?

Question 66

Explain the concept of valence shell electron pair repulsion?

Question 67

What are polar covalent bonds and nonpolar covalent bonds?

Question 68

Identify the molecule with a tetrahedral molecular structure.

A) NOF
B) CH₂O
C) NH₃
D) CH₄
E) PCl₃

Question 69

How many electron groups can likely be found on the central atom of a molecule with a trigonal planar shape?

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

Question 70

What are odd-electron molecules?

Question 71

Explain the steps for determining the Lewis electron dot diagram of a simple molecule.

Question 72

Which of the following molecules will likely have a bent molecular shape?

A) NOF
B) CH₂O
C) CH₂Cl₂
D) CH₄
E) PCl₃

Question 73

What are electron-deficient molecules and expanded valence shell molecules?

Question 74

Draw the Lewis electron diagram of a boron atom. Explain the diagram.

Question 75

What is the octet rule? Do atoms always follow the octet rule when forming compounds?

Question 76

Draw the electron diagram for an atom with the valence shell electron configuration of ns²np³.

Question 77

Which of the following molecules will have a trigonal pyramidal molecular structure?

A) PCl₃
B) NO₂
C) CH₄
D) CaCl₂
E) NaCl

Question 78

Explain the concept of electronegativity.

Question 79

What is the most likely shape for a molecule with a central atom and only one atom surrounding it?

A) Angular
B) Linear
C) Trigonal planar
D) Trigonal pyramidal
E) Tetrahedral

Question 80

What is a covalent bond? What is an ionic bond? Give an example that demonstrates each type of bond.