1) Match each of the substances in the left column with the strongest type of in

Question

1) Match each of the substances in the left column with the strongest type of intermolecular force that it exhibits.

water

hydrogen chloride

carbon tetrabromide

hydrogen fluoride

Carbon tetrachloride

nitrogen

ammonia

2) Compare ethanol, CH3CH2OH, and diethyl ether, CH3CH2OCH2CH3, and decide which has the characteristic in the left column.

stronger intermolecular attraction

higher equilibrium vapor pressure at a given temperature

higher boiling point

3. Increasing the surface area of solid solutes will increase the rate of solute particles being able to move out into the solvent.

A) True
B) False

4. When two liquids are totally miscible, they become more dispersed (they achieve the highest-disorder/entropy state available).

A) True
B) False

5. The molecules of an ideal gas have no size and exert no attractive forces on each other.

A) True
B) False

6. The molecules of an ideal gas are small, but they tend to cluster together.

A) True
B) False

Explanation / Answer

First consider Hydrogen bonding

we know that

hydrogen forms a bond with the three highly electronegative atoms given below

1) nitrogen

2) oxygen

3) fluorine

so from the given list

the substances that satisfy this condition are

i) water (H20)

it contains a hydrogen bond between H and O

ii) hydrogen fluoride (HF)

contains a hydrogen bond between H and F

iii) ammonia (NH3)

contians a hydrogen bond between H and N

now

dipole-dipole interaction are seen in covalent molecules with ionic character

HCl is predominantly covalent but it has some ionic character

so

the forces in HCl are dipole dipole

consider nitrogen (N2)

two N atoms are bonded together by the weak attraction forces

these are called london forces

consider CCl4 and CBr4

the C-Cl and C-Br bonds are ionic

but CCl4 and Cbr4 molecules are symmetric

so there is zero dipole moment and they are non polar

as a result

Carbon tetrachloride and carbon tetra bromide are molecules with weak intermolecular forces

so the forces in these molecules are also london forces

finally the table is

Hydrogen bonding : -- water , hydrogen fluoride , ammonia

dipole -dipole : --- hydrogen chloride

london forces : --- carbon tetrachloride, carbon tetra bromide , nitrogen

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