Lab Final

Question 1

Intermolecular Forces

Answer 1

the attractive forces between particles that are not bonded to each other.

Question 2

Freezing point

Answer 2

the temperature at which a liquid becomes a solid

Question 3

Boiling point

Answer 3

the temperature at which a liquid becomes a gas

Question 4

Vapor pressure

Answer 4

the pressure exerted by the equilibrium concentration of a vapor in equilibrium with its liquid

Question 5

Surface tension

Answer 5

a measure of how strongly molecules on the surface of a liquid attract to each other. The energy needed to pull liquid apart from itself to make a new surface.

Question 6

Viscosity

Answer 6

a measure of how readily a fluid flows against itself. Thick fluids have high viscosity and move slowly.

Question 7

Dipole

Answer 7

an uneven distribution of charge in a molecule

Question 8

Dispersion forces

Answer 8

occur when an atom or molecule come near each other and the electron of one species are attracted to the protons of the other.

Question 9

Dipole-Dipole

Answer 9

forces occur between species that have a permanent dipole, such as water molecules.

Question 10

Hydrogen Bonding

Answer 10

a very strong form of dipole-dipole interaction that occurs in species that have H-F H-O or H-N bonds

Question 11

Ion-Dipole forces

Answer 11

occur between permanent ions and dipoles, such as sodium ions and water.

Question 12

Specific heat capacity

Answer 12

the amount of energy needed to raise 1g of water by 1 degree Celsius

Question 13

Heat of vaporization

Answer 13

energy needed per mole of substance converted from liquid to gas at its boiling point, units J/mol or KJ/ mol.

Question 14

Solution

Answer 14

Homogenous mixture of two or more substances or components containing a solvent and a solute.

Question 15

solvent

Answer 15

majority component of a solution, which does the dissolving of a solute.

Question 16

solute

Answer 16

minority component of a solution, which are dissolved by the solvent.

Question 17

Aqueous solutions

Answer 17

water is the solvent and a solid, liquid or gas is the solute

Question 18

solubility

Answer 18

the amount of a substance that can be dissolved in a given amount of solvent

Question 19

miscible

Answer 19

two substances that are soluble in each other.

Question 20

immiscible

Answer 20

two substances that are not soluble in each other.

Question 21

Henry’s law

Answer 21

the higher the pressure in a gas, the more soluble the gas is in the solvent.

Question 22

Buffers

Answer 22

anything that resists change. weak acid and conjugate base or weak base and conjugate acid.

Question 23

Henderson-Hasselbalch equation

Answer 23

pH=pKa+log (10) {[base]/[acid]}

Question 24

buffer capacity

Answer 24

the number of moles or added acid or base that the buffer can neutralize before it gets overwhelmed.

Question 25

solubility product constant

Answer 25

Ksp, the equilibrium between a solids and its respective ions in a solution. Its value indicates the degree to which a compound dissociates in water

Question 26

common ion effect

Answer 26

if [I-] is increased then [Pb+] must decrease for the Ksp to stay the same

Question 27

formation constant

Answer 27

Kf, the stability of a complex ion can be judged by the magnitude of the equilibrium constant corresponding to the formation of the complex

Question 28

Gibbs free energy

Answer 28

the available energy that can be used for any process.

Question 29

enthalpy

Answer 29

the heat evolved in a chemical reaction at constant pressure.

Question 30

calorimeter

Answer 30

measures temperature change in order to determine heat.

Question 31

reduction

Answer 31

a chemical change where a reagent gains one or more electron, the charge becomes more negative as a result

Question 32

oxidation

Answer 32

chemical change in which a reagent loses one or more electrons, the charge becomes more positive as a result.

Question 33

anode

Answer 33

site of oxidation

Question 34

cathode

Answer 34

the site of the reduction

Question 35

oxidizing agent

Answer 35

a species that causes another to be oxidized

Question 36

reducing agent

Answer 36

a species that causes another to be reduced

Question 37

potential ( electromotive force)

Answer 37

the driving force for the reaction

Question 38

salt bridge

Answer 38

allows the passage of ions to balance the electron flow

Question 39

electrode

Answer 39

the conductor placed in each half cell

Question 40

know the chemicals used in experiments

Answer 40

like iodine

Question 41

spontaneous reaction

Answer 41

occurs without being driven by an outside source

Question 42

Entropy

Answer 42

The number of specific ways where a system may be arranged

Question 43

Solubility product

Answer 43

the equilibrium constant for a chemical equation

Question 44

Colligative property

Answer 44

Properties of solutions that depend on the number of particles dissolved in solution, not on the type of particles

Question 45

LeChatelier’s principle

Answer 45

When temperature, pressure, on concentration increase, equilibrium shifts to accommodate the temperature, pressure, or concentration.