The boiling point of bromine is 59 °C. Which of the following best predicts the boiling point of iodine monochloride, a polar compound?
Higher than 59 °C because dipole-dipole interactions in iodine monochloride are stronger than dispersion forces in bromine.
Lower than 59 °C because ionic bonding in bromine is stronger than covalent bonding in iodine monochloride.
Lower than 59 °C because dipole-dipole interactions in iodine monochloride are weaker than in bromine.
Higher than 59 °C because ionic bond in iodine monochloride is stronger than H-bonding in bromine.

Question 5(Multiple Choice Worth 1 points)

(03.02 MC)

What happens when the compound MgO is formed?
Oxygen transfers two electrons to magnesium.
Oxygen receives two electrons from magnesium.
Magnesium forms an ion with −1 charge; oxygen forms an ion with +1 charge.
Magnesium forms an ion with +1 charge; oxygen forms an ion with −1 charge.

Question 6(Multiple Choice Worth 1 points)

(03.03 MC)

What best describes the bonding in a carbon dioxide molecule?
Carbon shares two of its electrons, and each oxygen shares four of its electrons.
Carbon shares four of its electrons, and each oxygen shares two of its electrons.
Carbon receives two electrons from each of the two oxygen atoms.
Carbon transfers two electrons to each of the two oxygen atoms.

Question 7(Multiple Choice Worth 1 points)

(03.01 LC)

The electron configuration of an element is 1s22s22p1. How many valence electrons does the element have?
1
2
3
4

Question 8(Multiple Choice Worth 1 points)

(03.06 MC)

A certain intermolecular force is created when hydrogen bonds with a highly electronegative atom. Which of the following best explains the strength of this intermolecular force?
Very strong, because it is a result of interactions between highly polar molecules.
Negligible, because it is a result of interaction between ions and polarized molecules.
Very strong, because it is a result of interactions between molecules with instantaneous dipoles.
Negligible, because it is a result of interactions between symmetrical molecules causing cancelling of dipoles.

Question 9(Multiple Choice Worth 1 points)

(03.03 LC)

At most, how many covalent bonds can a carbon atom form?
1
2
3
4

Question 10(Multiple Choice Worth 1 points)

(03.01 MC)

The electron configurations of two unknown elements X and Y are shown.

X: 1s22s22p6
Y: 1s22s22p63s23p6

Which statement is most likely correct about the two elements?
They will react because X can give up two electrons and Y needs two electrons to become stable.
They will react because X and Y can share two pairs of electrons to become stable.
They will not react because both have a complete outermost shell and are stable.
They will not react because both will give up one electron to become stable.

Question 11(Multiple Choice Worth 1 points)

(03.03 MC)

A diatomic molecule shares a single pair of electrons. What type of bond is present in the molecule?
A single covalent bond because each atom requires one more electron to complete its octet.
A single covalent bond because each atom requires two more electrons to complete its octet.
A double covalent bond because each atom requires four more electrons to complete its octet.
A double covalent bond because each atom requires two more electrons to complete its octet.

Question 12(Multiple Choice Worth 1 points)

(03.01 MC)

The table shows the total number of electrons in Atom A and Atom B.

Atom
Number of Electrons
A
10
B
12

Which statement is correct?

A will give up two electrons to form bonds.
B will give up two electrons to form bonds.
Both A and B will be chemically unreactive.
Both A and B will gain electrons to become stable.

Question 13(Multiple Choice Worth 1 points)

(03.03 LC)

Which of the following is true about the Lewis dot representation in a covalently bonded molecule?
The least electronegative atom is shown in the middle.
The bonded pairs of valence electrons are shown by dots.
The inner shell electrons are shown using small cross marks.
The non-bonded pairs of valence electrons are shown using lines.

Question 14(Multiple Choice Worth 1 points)

(03.02 MC)

The table shows the electronegativity values of four unknown elements on the Pauling scale.

Electronegativity Values
Unknown Element
Electronegativity
A
3.44
B
0.79
C
1.8
D
2.0

Which two elements are most likely to form an ionic bond together?

A and B
B and C
A and D
C and D

Question 15(Multiple Choice Worth 1 points)

(03.06 MC)

The characteristics of two unknown intermolecular forces, X and Y, are compared in the table.

Intermolecular Forces
X
Y
Occurs between molecules with instantaneous dipoles
Occurs between molecules with permanent dipoles and ions