Unit 3.03 - 3.06

Question 1

What happens when intermolecular forces of two substances are similar?

Answer 1

the substances tend to be miscible (they mix).

Question 2

What are the requirements for any solute to dissolve in any solvant?

Answer 2

1. Solute-solute and solvent-solvent attractions must be broken
2. solute-solvent attractions must be made

Question 3

Define vapor pressure

Answer 3

When a few molecules possess enough energy to overcome the intermolecular forces holding them together and escape, even if the liquid is below its boiling point

Question 4

What do weak intermolecular forces cause liquids to have?

Answer 4

Causes liquids to have low boiling points, which means they are volatile (does not mean explosive) and will have high vapor pressures

Question 5

What was low boiling points mean when it comes to vapor pressure?

Answer 5

Low boiling points = high vapor pressures

Question 6

The more IMF, the less ____________

Answer 6

vapor pressure

Question 7

Define Metallic Solids

Answer 7

Solids that are held together by a delocalized sea of electrons
- electrons are collectively shared between all atoms
- leads to properties of metals

Question 8

Define Ionic solids

Answer 8

Held together by an ionic bond between CATIONS AND ANIONS (metal and nonmetal)
- The repulsion between like (cation/cation) leads to ionic solids being brittle (breakable)
- cannot conduct electricity

Question 9

Define Covalent-network solids

Answer 9

held together by covalent bonds
- Can lead to extremely hard substances
- Do not conduct electricity

Question 10

Define molecular solids

Answer 10

held together by intermolecular forces
- tend to be soft
- have low melting points
- cannot conduct electricity

Question 11

What are the properties of ions present in an ionic solid?

Answer 11

Ions are held rigidly in fixed positions

Question 12

Examples of Covalent solids?

Answer 12

diamond, graphite, silicon dioxide, and silicon carbide (elements of group 14)

Question 13

Molecular solids are made from __________

Answer 13

non-metals ONLY

Question 14

1 atm = ___ mm Hg = ____ torr

Answer 14

760mm Hg: 760 torr

Question 15

Define kinetic molecular theory

Answer 15

The basis for many properties of gas.

Question 16

Gases are composed of __________

Answer 16

tiny particles whose size is negligible, which means the volume of the actual individual particles can be assumed to be negligible (incredibly small)

Question 17

Gas particles move randomly in _____________________

Answer 17

straight lines at various speeds

Question 18

The forces of attraction and repulsion between two gases particles are _____

Answer 18

negligible

Question 19

What do the collisions with the walls of the container create?

Answer 19

gas pressure

Question 20

What is proportional to the average kinetic energy of a gas particle

Answer 20

Kelvin temperature

Question 21

Define P1V1/T1 = P2V1/T2

Answer 21

An equation used for when the gas changes

Question 22

Define PV = nRT

Answer 22

The equation used to describe a gas in a constant state
r = 0.0821
- Temp is K
- Volume is L
- Pressure is atm

Question 23

When should you use r = 0.0821?

Answer 23

What describing a gas at a constant state

Question 24

When should you use r = 8.314?

Answer 24

When it deals with energy

Question 25

As velocity increases, temperature (K) ___________

Answer 25

Increases

Question 26

As velocity increases, molar mass _____

Answer 26

Decreases

Question 27

How many kPa in 1 atm

Answer 27

101.325

Question 28

How do you know if a substance is saturated?

Answer 28

If more solute is added but does not dissolve

Question 29

How do you know if a substance is unsaturated?

Answer 29

If the solute added is dissolved