Chemistry Test 2

Front 1

reactants

Back 1

written to the left

Front 2

products

Back 2

written to the right

Front 3

balanced equation

Back 3

has the same number of each type of atom on each side of the reaction arrow

Front 4

synthesis reactions

Back 4

2 or more reactants combine to form one product
CO2+H20 --->H2CO3

Front 5

decomposition reactions

Back 5

1 reactant breaks apart to form two or more products
CaCO3-----> CaO+CO2

Front 6

Single replacement reactions

Back 6

an element moves from one reactant to another
Fe+CuSO4---->Cu+FeSO4

Front 7

double replacement reactions

Back 7

parts of 2 reactants trade places
NaCl+AgNO3--->NaNO3+AgCl

Front 8

hydrolysis reactions

Back 8

water breaks the other reactant apart

Front 9

hydration reactions

Back 9

water adds to a double bond

Front 10

dehydration reactions

Back 10

a double bond is formed when water is eliminated from a reactant

Front 11

Oxidation

Back 11

the loss of electrons, gain of oxygen atoms, and/or loss of hydrogen atoms
2Na+Cl2---->2NaCl

Front 12

Reduction

Back 12

the gain of electrons, loss of oxygen atoms, and/or gain of hydrogen atoms
2Na+Cl2--->2NaCl

Front 13

combustion

Back 13

an oxidation reaction that involves O2
CH4+2O2---> CO2+2H2O

Front 14

hydrogenation

Back 14

a reduction reaction that involves H2 see page 166

Front 15

coefficients

Back 15

in a balanced chemical equation describe, in terms of moles, the various relationships between reactants and products. If mass of reactants is specified, the amount of reactant must be converted to moles before hte balanced equation can be interpreted

Front 16

Limiting Reactant

Back 16

the reactant that runs out first

Front 17

theoretical yield

Back 17

the amount of product expected, based on the amount of limiting reactant, the maximum amount of product that can be obtained

Front 18

percent yield

Back 18

compares the actual yield of a reaction to the theoretical yield
Percent yield=Actual yield over Theoretical yield x 100

Front 19

free energy

Back 19

the energy released or gained in a reaction (G);(delta g) is the change in the free energy for the reaction

Front 20

Reaction rate

Back 20

a measure of how quickly products forms

Front 21

activation energy

Back 21

the energy barrier that must be crossed to go from reactants to products

Front 22

spontaneous reaction

Back 22

continues by itself once it has started

Front 23

nonspontaneous reaction

Back 23

will not take place unless something starts it and keeps it going

Front 24

actual yield

Back 24

the amount of product obtained from a reaction

Front 25

Heat of fusion

Back 25

the energy required at the melting point of a solid to converty a solid into a liquid

Front 26

Heat of Vaporization

Back 26

is the energy required at the boiling point of a liquid to convert a liquid into a gas

Front 27

1 atm

Back 27

14.7 psi, 760 Torr

Front 28

Boyle's Law

Back 28

P1V1=P2V2

Front 29

Gay-Lussac's Law

Back 29

P1/T1=P2/T2

Front 30

Charles' Law

Back 30

V1/T1=V2/T2

Front 31

Avogadro's law

Back 31

V1/n1=V2/n2

Front 32

Combined gas law

Back 32

P1V1/T1=P2V2/T2

Front 33

Ideal gas law

Back 33

PV=nRT

Front 34

Dalton's law of partial pressure

Back 34

the total pressure of mixture of gases is the sum of the individual (partial) pressures of each gas

Front 35

sublimation

Back 35

the conversion of a solid directly into a gas

Front 36

deposition

Back 36

the conversion of a gas directly into a solid

Front 37

barometer

Back 37

measures atmospheric pressure

Front 38

manometer

Back 38

when dealing with enclosed gases, can be used to measure pressure

Front 39

sphygmomanometer

Back 39

used to measure blood pressure

Front 40

boiling point

Back 40

the temperature at which the vapor pressure of the liquid equals the atmospheric pressure

Front 41

pure substance

Back 41

consists of just one element or compound

Front 42

homogeneous

Back 42

uniformly distributed

Front 43

heterogeneous

Back 43

not uniformly distributed

Front 44

solvent

Back 44

the solution component present in the greatest amount

Front 45

solute

Back 45

components dissolved in the solvent

Front 46

precipitate

Back 46

a solid reaction product

Front 47

hydrophilic

Back 47

water liking

Front 48

hydrophobic

Back 48

water fearing

Front 49

amphipathic

Back 49

have both hydrophilic and hydrophobic parts

Front 50

concentration

Back 50

the amount of solute that is dissolved in a solvent

Front 51

saturated

Back 51

holds the maximum amount of solute that can be dissolved at a particular temperature

Front 52

unsaturated

Back 52

holds less than a saturation amount of solute

Front 53

weight/volume percent

Back 53

grams of a solute over mL x 100

Front 54

parts per thousand

Back 54

grams of solute over mL of a solution x10^3

Front 55

parts per million

Back 55

grams of a solute over mL of a solution x 10^6

Front 56

parts per billion

Back 56

grams of solute over mL of a solution x 10^9

Front 57

Molarity(M)

Back 57

the number of moles of solute present in each liter of solution

M= moles of solute over liters of solution

Front 58

suspension

Back 58

large particles suspended in a liquid

Front 59

colloid

Back 59

the particles are larger than the solutes in a solution but smaller than the particles that make up a suspension

Front 60

acids

Back 60

dissolve some metals, turn litmus pink, and have a sour taste

Front 61

bases

Back 61

feel slippery or soapy, turn litmus blue, and have a bitter test

Front 62

Bronsted-Lowry

Back 62

acids release H+ and bases accept H+

Front 63

equilibrium

Back 63

when the rates of the forward and reverse are the same

Front 64

Le Chatelier's Principle

Back 64

states that when a reversible reaction is pushed out of a equilibrium, the reaction responds to restore equilibrium