Summer II Chemistry Final Review B

Which is a typical characteristic of an ionic compound?

• Electron pairs are shared among atoms

• The ionic compound has a low solubility in water

• The ionic compound is described as a molecule

• The ionic compound has a high melting point

Which of these elements does not exist as a diatomic molecule?

• Ne

• F

• H

• I

Why do atoms share electrons in covalent bonds?

• to become ions and attract each other

• to attain a noble-gas electron configuration

• to become more polar

• to increase their atomic numbers

Which elements can form diatomic molecules joined by a single covalent bond?

• hydrogen only

• halogens only

• halogens and members of the oxygen group only

• hydrogen and the halogens only

Which of the following diatomic molecules is joined by a double covalent bond?

• O₂

• Cl₂

• N₂

• He₂

How many electrons can occupy a single molecular orbital?

• 0

• 1

• 2

• 4

According to VSEPR theory, molecules adjust their shapes to keep which of the following as far apart as

possible?

• pairs of valence electrons

• inner shell electrons

• inner shell electrons

• he electrons closest to the nuclei

What causes water molecules to have a bent shape, according to VSEPR theory?

• repulsive forces between unshared pairs of electrons

• interaction between the fixed orbitals of the unshared pairs of oxygen

• ionic attraction and repulsion

• the unusual location of the free electrons

What are the weakest attractions between molecules?

• ionic forces

• Van der Waals forces

• covalent forces

• hydrogen forces

What causes hydrogen bonding?

• attraction between ions

• motion of electrons

• sharing of electron pairs

• bonding of a covalently bonded hydrogen atom with an unshared electron pair