Liquids and Solids

Question 1

Intermolecular Forces

Answer 1

Attractive or repulsive interactions between neighboring molecules

Question 2

What can intermolecular forces determine?

Answer 2

Physical properties such as boiling point, melting point, solubility and density

Question 3

Intramolecular forces

Answer 3

Interactions within a molecule that hold atoms together in a molecule

Question 4

Types of intermolecular forces

Answer 4

London dispersion
Dipole- Dipole
Hydrogen Bonding

Question 5

Intermolecular force type

London dispersion

Answer 5

Exist between all molecules
Weakest IMF
Temporary attractive force

Question 6

Which intermolecular forces exist between all molecules?

Answer 6

London dispersion

Question 7

Dipole- Dipole

Answer 7

Attractive forces between two polar molecules containing permanent dipoles

Question 8

Permanent dipole

Answer 8

Molecules composed of atoms with different electronegativities

Question 9

What determines the boiling point?

Answer 9

Strength of intermolecular force

Question 10

Hydrogen bonds

Answer 10

Strong dipole- dipole interactions betweent a molecules containing a hydrogen atom bonded to N, O, or F

Question 11

What is the rule for hydrogen bonding

Answer 11

Only a hydrogen bond if bonded to a Hydrogen, Oxygen, or Fluorine

Question 12

Types of intramolecular forces

Answer 12

Polar covalent
nonpolar covalent
ionic
metallic bonds

Question 13

Polar covalent

Answer 13

forms between two non metals of slightly different electronegativities

Question 14

What type of intermolecular interactions are present in polar covalent compounds apart of?

Answer 14

dipole-dipole and london dispersion

Question 15

Nonpolar covalent

Answer 15

Form between the same non metals or non metals with similiar electronegativities

Question 16

What type of intermolecular interaction is present in nonpolar covalent bonds?

Answer 16

London dispersion

Question 17

Ionic bonds

Answer 17

Formed between metal and non metal
Transfer of valence e’s from metal to non metal

Question 18

Cation

Answer 18

Postively charged ion

Question 19

Anion

Answer 19

Negativiely charged ion

Question 21

Metallic bonds

Answer 21

Form between metal cations and the valence e’s moving freely through lattice

Question 22

Which are weaker type of forces intermolecular or intramoelcular?

Answer 22

Intermolecular

Question 23

Weakest to strongest intermolecular forces

Answer 23

London dispersion < dipole-dipole< H- bonding

Question 24

Weakest to strongest intramolecular force

Answer 24

covalent< ionic < metallic (strongest)

Question 25

Endothermic

Answer 25

Heat required

Question 26

Exothermic

Answer 26

Heat released

Question 27

Draw the endothermic process of phase changes **(solid to gas)**

Question 28

Draw the exothermic process for phase change **(gas to solid)**

Question 29

What is the process called for a solid to a liquid?

Answer 29

Fusion

Question 30

What is the process from liquid to gas?

Answer 30

Vaporization

Question 31

What is the process from a solid to a gas?

Answer 31

Sublimation

Question 32

Process from gas to liquid

Answer 32

Condensation

Question 33

Process from a liquid to solid

Answer 33

Freezing

Question 34

Process from gas to solid

Answer 34

Deposition

Question 35

Entropy (S)

Answer 35

The disorder or randomness in a system

Question 36

Positive ΔS

Answer 36

Increase in randomness

Question 37

Negative ΔS

Answer 37

Decrease in randomness

Question 38

Enthalpy (H)

Answer 38

Measures the heat in a system

Question 39

What does ΔH represent

Answer 39

Amount of hear gained or lost b a system when a reaction is carried out at constant pressure

Question 40

ΔH > 0 means what

Answer 40

Heat moves into the system so the reaction is **endothermic**

Question 41

ΔH < 0 means what

Answer 41

Heat moves out of the system and the reaction is **exothermic**

Question 42

Phase diagram

Answer 42

Draw out this diagram and label

Question 43

Triple point

Answer 43

Point where all substances exists in the liquid, gas, and solid phase

Question 44

Critical point

Answer 44

Point at which the liquid and gas phase become indistinguishbale

Question 45

What is the point called passed the critical point?

Answer 45

Supercritical fluid

Question 46

# Properties of liquids Miscibility

Answer 46

Degree to which a liquid mixes with another liquid

Question 47

# Properties of liquids Viscosity

Answer 47

Measure of a fluid's resistance to flow

Question 48

# Properties of liquids Surface tension

Answer 48

Ability of a liquid surface to resist external forces

Question 49

# Properties of liquids Vapor Pressure

Answer 49

equilibrium pressure exerted by a vapor above its liquid

Question 50

# Properties of liquids Which has a lower density liquids or solids

Answer 50

Liquids

Question 51

# Properties of solids Ionic solids

Answer 51

Hard, non conductive, brittle and have a high melting point

Question 52

Example of ionic solids

Answer 52

Table salt (NaCl)

Question 53

Metallic solids

Answer 53

Malleable, ductile, conductive, high luster, variable melting pts and hardness

Question 54

Covalent network solids

Answer 54

Hard, non coductive, high melting points

Question 55

Example of covalent network solids

Answer 55

Diamonds

Question 56

Molecular solids

Answer 56

Soft, non conductive, and low melting points

Question 57

Types of unit cells

Answer 57

Simple cubic Body centered cubic Face centerd cubic

Question 58

Simple cubic

Answer 58

1 atom per unit cell At every corner of the cube

Question 59

Body centered cubic

Answer 59

2 atoms per unit cell with 1 atom in the center

Question 60

Face centered cubic

Answer 60

4 atoms per unit cell