Bonding and Forces

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AP Chemistry › Bonding and Forces

Questions 1 - 10
1

Which of the following statements best describes ionic compounds?

3-D arrays of charged particles

Formed when molecules share electrons

Neutral particles that donate electrons

Malleable compounds that lack structural stability

Explanation

The definition of ionic compounds are three-dimensional arrays of atoms held together by strong ionic bonds. Ions are charged particles that have either gained or lost a certain number of electrons. They have great crystalline strength because of the strong electrostatic forces between the ions.

2

Which of the following statements best describes ionic compounds?

3-D arrays of charged particles

Formed when molecules share electrons

Neutral particles that donate electrons

Malleable compounds that lack structural stability

Explanation

The definition of ionic compounds are three-dimensional arrays of atoms held together by strong ionic bonds. Ions are charged particles that have either gained or lost a certain number of electrons. They have great crystalline strength because of the strong electrostatic forces between the ions.

3

Which of the following compounds contains the most π bonds?

CO2

H2O

CH4

NH3

C2H6

Explanation

π bonds occur when there is greater than a single bond (double or triple bond). The only compound listed with double bonds or greater is CO2, meaning it is the one that contains the most π bonds.

4

Which of the following compounds contains the most π bonds?

CO2

H2O

CH4

NH3

C2H6

Explanation

π bonds occur when there is greater than a single bond (double or triple bond). The only compound listed with double bonds or greater is CO2, meaning it is the one that contains the most π bonds.

5

Which of the following compounds has the greatest amount of sigma bonds?

Butane

Ethane

Benzene

Lithium Hydroxide

Water

Explanation

Butane has 13 sigma bonds. Ethane has 7 sigma bonds. Benzene has 12 sigma bonds. Lithium Hydroxide has 2 sigma bonds and water has 2 sigma bonds.

6

Which of the following best explains hydrogen bonding?

Electronegative atoms carry most of the electrons in the shared pairs when they are bonded to hydrogen

Hydrogen does not have any electrons

The covalent bonds between other atoms are hydrogen are called hydrogen bonds

There are too many electrons in a solution, so H atoms interact with them

Explanation

Electronegative atoms disproportionately pull covalently bonded electrons toward themselves, which leaves hydrogen with partial positive character.

7

Find the bond angle present in sulfur dioxide.

Explanation

Sulfur dioxide has the formula and takes on a trigonal planar electronic geometry, with the two oxygen atoms and the lone pair in the same plane. The molecular geometry will be bent, resulting in a oxygen-sulfur-oxygen bond angle of 120 degrees.

8

Which of the following compounds has the greatest amount of sigma bonds?

Butane

Ethane

Benzene

Lithium Hydroxide

Water

Explanation

Butane has 13 sigma bonds. Ethane has 7 sigma bonds. Benzene has 12 sigma bonds. Lithium Hydroxide has 2 sigma bonds and water has 2 sigma bonds.

9

Find the bond angle present in sulfur dioxide.

Explanation

Sulfur dioxide has the formula and takes on a trigonal planar electronic geometry, with the two oxygen atoms and the lone pair in the same plane. The molecular geometry will be bent, resulting in a oxygen-sulfur-oxygen bond angle of 120 degrees.

10

Which of the following best explains hydrogen bonding?

Electronegative atoms carry most of the electrons in the shared pairs when they are bonded to hydrogen

Hydrogen does not have any electrons

The covalent bonds between other atoms are hydrogen are called hydrogen bonds

There are too many electrons in a solution, so H atoms interact with them

Explanation

Electronegative atoms disproportionately pull covalently bonded electrons toward themselves, which leaves hydrogen with partial positive character.

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