Ch3 Compounds And Chemical Bonding Bringing Exam Questions

Chapter 3: Compounds and chemical bonding: bringing atoms together

Test Bank

Type: multiple choice question

Title: Chapter 03 - Question 01

1) A double bond comprises which of the following orbitals?

a. one pi orbital

b. two sigma orbitals

c. two pi orbitals

d. two sigma orbitals and one pi orbital

e. one sigma orbital and one pi orbital

Type: multiple choice question

Title: Chapter 03 - Question 02

2) A triple bond comprises which of the following orbitals?

a. one sigma orbital and one pi orbital

b. two pi orbitals

c. two sigma orbitals

d. one sigma orbital and two pi orbitals

e. two sigma orbitals and one pi orbital

Type: multiple response question

Title: Chapter 03 - Question 03

3) Which of the following compounds features a triple bond? Select all that apply.

a. CH₄

b. CHCH

c. CH₂CHCH₃

d. CH₃Cl

e. N₂

Type: multiple choice question

Title: Chapter 03 - Question 04

4) Which of the following best describes a coordinate bond?

a. A highly-polarized covalent bond.

b. A bond comprising only one valence electron.

c. A bond containing two valence electrons, both of which have been donated by the same atom.

d. A bond containing two valence electrons, one donated from each of the atoms joined by the bond.

e. A bond that is stronger than a ‘regular’ covalent bond.

Type: multiple choice question

Title: Chapter 03 - Question 05

5) Which of the following is a noble gas configuration?

a. 1s² 2s²

b. 1s² 2s² 2p⁴

c. 1s² 2s² 2p⁶ 3s² 3p⁶

d. 1s² 2s² 2p⁶ 3s¹

e. 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹

Type: multiple response question

Title: Chapter 03 - Question 06

6) Carbon has a valency of four. Which of the following are correct deductions based on this information? Select all that apply.

a. Carbon needs to share two pairs of valence electrons to achieve a full valence shell.

b. Carbon needs to share four pairs of valence electrons to achieve a full valence shell.

c. One atom of carbon can form four single covalent bonds.

d. One atom of carbon can form one double bond and two single bonds.

e. One atom of carbon can form two single bonds and two double bonds.

Type: multiple response question

Title: Chapter 03 - Question 07

7) Which of the following carry zero charge overall? Select all that apply.

a. An ionic compound

b. A polyatomic ionic compound

c. A covalent compound

d. A molecule

e. An ion

Type: multiple choice question

Title: Chapter 03 - Question 08

8) Two atomic orbitals will overlap to form how many molecular orbitals?

a. One

b. Two

c. Four

Type: multiple response question

Title: Chapter 03 - Question 09

9) Which of the following statements are true? Select all that apply.

a. The overlap of two atomic orbitals generates two bonding orbitals and two anti-bonding orbitals.

b. Electrons in anti-bonding orbitals inhibit covalent bond formation.

c. Electrons in bonding orbitals favour covalent bond formation.

d. More electrons must occupy a molecule’s anti-bonding orbitals than its bonding orbitals for covalent bonding to occur.

e. A non-bonding orbital does not contribute to covalent bonding.

Type: multiple choice question

Title: Chapter 03 - Question 10

10) A full valence shell (except shell 1) is considered to be occupied by how many electrons?

a. 2

b. 8

c. 10

d. 18

e. 24

Type: matching question

Title: Chapter 03 - Question 11

11) Match the movement of electrons with the type of bonding associated with it.

Feedback: Ionic and covalent bonding are distinguished by the extent to which valence electrons are shared between atoms. At one extreme, there is no bonding if no transfer occurs. At the other extreme, ionic bonding occurs if total transfer occurs. Covalent bonding sits in the middle: electrons are partially transferred. Look at Figure 3.4 to see this represented visually.

a. Electrons shared equally between two atoms = Covalent bonding

b. Electrons fully transferred from one atom to another = Ionic bonding

c. Electrons not transferred from one atom to another = No bonding

Type: multiple choice question

Title: Chapter 03 - Question 12

12) Atoms of elements that are unable to undergo chemical bonding are called which of the following?

a. Volatile

b. Inert

c. Conjugated

d. Metallic

e. Radioactive

Type: multiple response question

Title: Chapter 03 - Question 13

13) Which of the following statements about delocalized electrons are true? Select all that apply.

a. Delocalized electrons are valence electrons that are shared between more than one pair of atoms.

b. Delocalized electrons occupy extended sigma orbitals.

c. Delocalized electrons are a characteristic feature of aromatic compounds.

d. Delocalized electrons are found only in cyclic compounds.

Type: multiple choice question

Title: Chapter 03 - Question 14

14) Which of the following elements has the highest electronegativity?

a. Oxygen

See Figure 3.5 to compare oxygen’s electronegativity to that of the other elements listed in this question.

b. Sodium

See Figure 3.5 to compare sodium’s electronegativity to that of the other elements listed in this question.

c. Carbon

d. Hydrogen

e. Sulfur

Type: matching question

Title: Chapter 03 - Question 15

15) Match an element’s electronegativity value with the strength with which the element attracts an electron.

Feedback: An element’s electronegativity is directly proportional to the extent to which it attracts electrons to itself: an element with a high electronegativity attracts electrons strongly; an element with a low electronegativity attracts electrons only weakly.

Page reference: section 3.2, page 58

a. High electronegativity value = Electron strongly attracted

b. Low electronegativity value = Electron weakly attracted

Type: matching question

Title: Chapter 03 - Question 16

16) Match the difference in electronegativity between the atoms of two elements with the type of bonding the atoms are most likely to undergo.

Feedback: If there is a large difference in electronegativity between two atoms, then an electron will be attracted more strongly to one atom than another, favouring total transfer of that electron and, hence, ionic bonding. If there is a small difference in electronegativity, an electron will be attracted to the same extent by both atoms, and so will end up only partially transferred (that is, shared between the atoms), leading to covalent bonding.

Page reference: section 3.2, page 57

a. Large difference in electronegativity = Ionic bonding

b. Small difference in electronegativity = Covalent bonding

Type: multiple response question

Title: Chapter 03 - Question 17

17) Which of the following are non-polar bonds? Select all that apply.

a. C–H

b. C=C

c. C–C

d. C–O

e. C=O

Type: matching question

Title: Chapter 03 - Question 18

18) Rank the following bonds in order of the extent of their polarization, with 1 being the least polarized, and 4 being the most polarized.

Feedback: The degree of polarization of a bond is proportional to the difference in electronegativity values of the elements joined by the bond. A bond joining atoms of the same element is non-polar – that is, it is not polarized. So, the C-C bond ranks lowest. The other bonds should then be ranked in order of the electronegativity of H, N, and O.

Page reference: section 3.5, page 73

a. C–H = 2

b. C–N = 3

c. C–C = 1

d. C–O = 4