phys ch23 questions

N2 has a triple bond and is a gas at room temperature. The triple bond is a very strong bond. True False

True

. Which of the following pairs would you expect to be covalently bonded? P and Ca Ar and Cl Co and Al S and Br

S and Br

Which of the following would best describe the characteristics of the material formed? -a non-conducting material with low melting and boiling points, likely liquid or gas at room temperature. -a brittle, opaque solid with a very high melting point. -a brittle, transparent solid with a very high melting point. -a shiny, malleable solid with a very high melting point. -a non-conducting solid at room temperature that will conduct if melted or dissolved.

a non-conducting material with low melting and boiling points, likely liquid or gas at room temperature.

Which of the following set of properties is most likely those associated with methane, a covalently bonded compound? gas at room temperature, colorless, does not conduct electricity when solid solid at room temperature, opaque, good electrical conductor solid at room temperature, transparent, electrical conductor when dissolved in water

gas at room temperature, colorless, does not conduct electricity when solid

Dispersion forces are stronger than covalent bonds. True False

False

The forces between the N2 molecules are very strong. True False

False

Which of the following is a true statement about melting and boiling points in materials made of covalent molecules? -Molecules that are polar have lower melting and boiling points than nonpolar molecules. -Molecules that contain triple bonds are the most likely to be gases at room temperature. -Molecules that contain double bonds melt and boil at higher temperatures because the bonds are stronger. -Van der Waals (dispersion) forces lower melting and boiling points. -Hydrogen bonding between molecules increases melting and boiling points.

Hydrogen bonding between molecules increases melting and boiling points.

What best describes how the oxygen molecules would behave if mixed with water? -They would dissolve poorly or not at all because they are polar. -They would dissolve well because they are not polar. -They would dissolve poorly or not at all because they are not polar. -They would dissolve well because they are polar. -They would dissolve well because they are ionic.

They would dissolve poorly or not at all because they are not polar.

What type of bond would exist between the carbon and the oxygen? ionic metallic covalent

covalent

Rank the following according to their strength, weakest first, strongest last. -dipole-dipole interactions, dispersion forces, covalent bonding, hydrogen bonding -hydrogen bonding, covalent bonding, dispersion forces, dipole-dipole interactions -hydrogen bonding, dipole-dipole interactions, dispersion bonding, covalent bonding -dispersion forces, dipole-dipole interactions, hydrogen bonding, covalent bonding -covalent bonding, hydrogen bonding, dipole-dipole interactions, dispersion forces

dispersion forces, dipole-dipole interactions, hydrogen bonding, covalent bonding