Chem Final

Question 1

Kinetic molecular theory

Answer 1

Used to predict the main properties of gases

Question 2

Boyles law

Answer 2

Relationship between volume and pressure.

Inversely proportional.

^Volume less pressure

Formula:

P1V1=P2V2

Question 3

Charles law

Answer 3

Relationship between volume and temperature.

Volume and Temprature a directly proportional.

As Temp increases Volume increases

V1 = V2

T1 T2

Question 4

Avogadros Law

Answer 4

Volume and Moles of gas–> n

N^ V^ are directly proportional

Increasing the amount of gas increases the amount of moles.

Formula:

V1=V2

N1 N2

Question 5

Ideal gas law

Answer 5

Gases behave ideally at ^Temperature and low Pressure

PV=NRT

R is a constant = 0.082

Question 6

Molar volume

Answer 6

Volume occupied by 1 Mol of gas

1 Mol of gas = 22.4 L (at STP)

Example:

1 mol He = 22.4L

1 mol CO = 22.4L

1 mol Ne = 22.4L

Question 7

IMF Intermolecular forces

Answer 7

The force of attraction between particles

Question 8

Dispersion Forces (London forces)

Answer 8

Present in all molecules

Dispersion forces depend on the size. The bigger or heavier a substance is, the stronger the dispersion forces.

Question 9

Dipole

Answer 9

2 opposite charges

Temporary or induced

Question 10

Dipole-Dipole

Answer 10

Perminent Dipole

Question 11

Polar Bonds

Answer 11

Significant difference in eletronegativity

Example

C-N H-N

C-O H-O

C-F H-F

C-Cl

Question 12

Hydrogen Bond

Answer 12

Strongest IMF

H-N

H-O

H-F

Question 13

Ion Dipole

Answer 13

Ionic -Polar bonds

Compound of Metal and Non-Metal

NaCl

Question 14

Solutions

Answer 14

Homogenous mixtures of two or more substances Physically mixed together

Question 15

Solute

Answer 15

Substances that get dissolved

Question 16

Solvent

Answer 16

Substance that does the dissolving

Question 17

Electrolytes

Answer 17

Type of solvent. Ionic compound (metal + non-metal)

Question 18

Strong electrolyte

Answer 18

Soluble ionic compound (metal+Non-metal)

Dissociate completely in water (only ions)

Example:

NaCl—> Na⁺ + Cl^-

Question 19

Weak Electrolytes

Answer 19

Insouble ionic compounds

Only partial dissociation

Example:

Ag⁺ +Cl^-

Question 20

NonElectrolytes

Answer 20

Covalent or molecular compounds (two non metals)

Example:

CH₃OH

Question 21

Solubility of solid in water

Answer 21

Depends on temperature

In general ^ temperature ^ the solubility of a solid

Higher the temperature higher solubility

Question 22

Solubility of gases

Answer 22

Depend on temperature and Pressure

The higher the temperture the lower the solubility

The higher the pressure the higher the solubility

Question 23

Saturated

Answer 23

A solution that has the solute and solvent in dynamic equilibrium.

***It holds the maximum amount of solute***

Question 24

Unsaturated

Answer 24

A solution that has less solute that is saturated

room for more solute to be dissolved

Question 25

Super Saturated

Answer 25

A solution that contain more solute than saturation Some of the solute is undissolved

Question 26

Vant hoff factor

Answer 26

how many ions you have Example: Na₂CO₃------\> 2 Na⁺¹ + CO₃^-2 = 3 Ions Covalent bonds (two non metals) (non Electrolytes) Always 1 Ion

Question 27

Colligative properties

Answer 27

Properties of all solutions that depend on the number of particles dissolved.

Question 28

Boiling point

Answer 28

The more particles the higher the BP

Question 29

Vapor pressure

Answer 29

The more particles/ higher IMF the lower the VP

Question 30

Freezing point

Answer 30

The more particles/Higher the IMF the lower the FP Freezing point and number of particles are inversly related