Chemistry Multiple Choice Mid-Terms Study Guide

The following molecules contain polar bonds. The only polar molecule is

• CH₄.

• CCl₄.

• CO₂.

• NH₃.

Which substance can you predict will conduct electricity based on the formula and phase of matter?

• H₂O (l)

• C₁₀H₂₂ (l)

• Ag (s)

• MgCl₂ (s)

A chemical bond formed by the attraction between positive ions and surrounding mobile electrons is a(n)

• nonpolar covalent bond.

• metallic bond.

• ionic bond.

• polar covalent bond.

Tags

NGSS.HS-PS1-3

Compared with ionic compounds, molecular compounds

• are harder.

• are brittle.

• have higher boiling points.

• have lower melting points.

Tags

NGSS.HS-PS1-3

Methanol (CH₃OH) dissolves easily in water.  Which is the correct explanation for this?

• Methanol is nonpolar and water is polar, so the molecules are not attracted to each other.

• Methanol is nonpolar and water is polar, so the molecules are attracted to each other.

• Methanol is polar and water is polar, so the molecules are attracted to each other.

• Methanol is polar and water is polar, so the molecules are not attracted to each other.

Metals are malleable because the metallic bonding

• allows one plane of ions to slide past another.

• does not produce ions.

• holds the layers of ions in rigid positions.

• is easily broken.

If two covalently bonded atoms are identical, the bond is

• coordinate covalent.

• nonionic.

• polar covalent.

• nonpolar covalent.

Which of these does not readily conduct electricity?

• a copper wire

• the human body

• pure water

• salt dissolved in water

The boiling point of water (H₂O) is substantially higher than the boiling point of hydrogen sulfide (H₂S). This difference in boiling point can be partially explained by

• ionic bonding.

• hydrogen bonding.

• London forces.

• covalent bonding.

A compound that vaporizes readily at room temperature is most likely to be a(n)

• molecular compound.

• brittle compound.

• metal.

• ionic compound.