Chemistry Final

Front 1

Atomic Theory

Back 1

1. Dalton
2. Each element composed of tiny indestructable particles called atoms.
3. All atoms of a given element have the same mass and other properties.
4. Atoms combine in simple, whole-number ratios to form compounds.

Front 2

Physical Vs Chemical Properties

Back 2

1. Physical: No change in composition
2. Chemical: Change in composition via chemical reaction
3. Physical: odor, taste, color, appearance, melting/boiling point, density
4. Chemical: Corrosiveness, flammability, acidity, toxicity.

Front 3

How many sig figs?
1. .04450
2. 10 dm = 1 m
3. .00002 mm
4. 5.0003

Back 3

1. 4 sig figs
2. unlimited
3. 1 sig fig
4. 5 sig figs

Front 4

Atomic Structure (protons/neutrons/electrons)

Back 4

1. Protons in nucleus with neutrons
2. Electrons orbit around in an electron cloud
3. Majority of mass in center
4. JJ Thomson - plum pudding
5. Rutherford - gold foil experiment

Front 5

Nobel gases

Back 5

1. 8th column
2. Stable gases

Front 6

Alkali Metals

Back 6

1. Group 1A
2. REACTIVE metals

Front 7

Alkali-Earth Metals

Back 7

1. Group 2A
2. fairly reactive

Front 8

Halogens

Back 8

1. Group 7A
2. Highly reactive non-metals

Front 9

Avogadro's Number

Back 9

6.022 X 10^23

Front 10

Mole

Back 10

1 mole = 6.022 X 10 ^23 particles

Front 11

Molar Mass

Back 11

1. Mass of 1 mol of atoms of an element

Front 12

Mass Number

Back 12

1. Sum of neutrons and protons in an atom

Front 13

Isotopes

Back 13

1. Atoms with same number of protons, but different number of neutrons.

Front 14

Atomic Number

Back 14

1. Number of protons in an atom's nucleus

Front 15

Cathode Rays

Back 15

1. Produced when high voltage applied between two electrodes.
2. Thomson discovered electrons through this

Front 16

Law of Conservation of Matter

Back 16

1. In a chemical reaction, matter is neither created nor destroyed.

Front 17

Law of definite proportions

Back 17

1. All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements.

Front 18

Law of multiple proportions

Back 18

1. When two elements form two different compounds, the masses of element B that combine with 1 g of element A can be expressed as a whole number ratio.
2. Mass of oxygen to 1 g carbon in CO2/Mass of oxygen to 1 g carbon in CO = 2

Front 19

Cations versus anions

Back 19

1. Cations: Positively charged ions
2. Anions: negatively charged ions

Front 20

Ions

Back 20

1. Positively or negatively charged particles.

Front 21

Nuclear Theory

Back 21

1. Theory that most of the atom's mass and all of its positive charge is contained in a small, dense nucleus.

Front 22

Ionic Bond versus covalent bond

Back 22

1. Metals with Non metals = Ionic - transfer
2. Non-metal with Non-metal = Covalent - sharing

Front 23

Molecular Models

Back 23

1. Ball and Stick model - reflect shape
2. Space-filling model - shows approximate space atom/electrons take up.

Front 24

Atomic Versus Molecular Elements

Back 24

1. Atomic: those that exist in nature with single atoms as their basic units.
2. Molecular: those that exist in nature with two or more atoms bonded together.

Front 25

Polyatomic molecules

Back 25

1. P4, S8

Front 26

Diatomic molecules

Back 26

1. N, O, F, Cl, Br, I, H

Front 27

Acids versus bases

Back 27

1. Acids: molecular compounds that release H+ ions when dissolved in water.
2. Bases: Creates OH- ions

Front 28

Oxyacids

Back 28

1. Contain hydrogen and an oxyanion (anion containing nonmetal and oxygen)

Front 29

Combustion Analysis

Back 29

1. Convert grams into moles and then determine the empirical formula.

Front 30

Hydrocarbons

Back 30

1. Organic compounds that contain only carbon and hydrogen.
2. Alkanes - single bonds
3. Alkenes - double bonds
4. Alkynes - triple bonds

Front 31

Functional group

Back 31

1. Characteristic atom or group of atoms.

Front 32

Stoichiometry

Back 32

1. Numerical relationships between chemical amounts in a balanced equation.

Front 33

Limiting Reactant

Back 33

1. Reactant that limits the amount of product in reaction.

Front 34

Theoretical Yield

Back 34

1. Amount of product that can be made based on limiting reactant.

Front 35

Actual Yield

Back 35

1. Amount of product actually produced by reaction

Front 36

Percent Yield

Back 36

1. Actual/Theoretical X100

Front 37

Aqueous

Back 37

1. Solution in which water acts as the solvent

Front 38

Solvent versus solute

Back 38

1. Solvent = MAJORITY
2. Solute = MINORITY

Front 39

Molarity

Back 39

1. Solution concentration
2. Mol over liters

Front 40

Strong electrolytes versus weak electrolytes

Back 40

1. Substances that completely dissolve into ions when they dissolve in water = STRONG
2. If no dissociation occurs - nonelectrolyte

Front 41

Strong acid versus weak acid

Back 41

1. HCl - strong - completely ionizes in water
2. C2H4O2 - acetic acid - weak acid - doesn't ionize completely in water

Front 42

Spectator ions

Back 42

1. Do not participate in the reaction

Front 43

Net-Ionic reactions

Back 43

1. equation showing only the species that actually change during reaction

Front 44

Acid-Base Reactions

Back 44

1. Also called neutralization reaction
2. Acid reacts with base, produce water!

Front 45

Gas-Evolution

Back 45

1. Reactions occurs and a gas forms, resulting in bubbling.

Front 46

Hydronium Ions

Back 46

1. H+ ions bind with water in acids to form H3O+
2. H3O+

Front 47

Arrhenius Definitions

Back 47

1. definitions of acid/base by Svante Arrhenius
2. Acid: produces H+ ions in aqueous
3. Base: produces OH- ions in aqueous

Front 48

Polyprotic acids

Back 48

1. Contain more than one ionizable proton and release them sequentially.

Front 49

Diprotic acids

Back 49

1. Two ionizable protons (H2SO4)
2. Strong in first ionizable proton, but weak in second.

Front 50

NH3 - base or acid?

Back 50

1. BASE!!!!!
2. Weak base
3. Tricky!!

Front 51

Salt

Back 51

1. Ionic compound that is formed from acid-base reactions - that is left dissolved in solution.

Front 52

Redox (oxidation-reduction) reactions

Back 52

1. Electrons transferred from one reactant to another
2. Oxidation is Loss
3. Reduction is Gain

Front 53

Oxidation State

Back 53

H = +1
F= -1
O = -2
Group 7A = -1
Group 6A = -2
Group 5A = -3

Front 54

Precipitation reactions

Back 54

1.

Front 55

Identifying Redox Reactions

Back 55

1. Oxidation - increase in oxidation state
2. Reduction - decrease in oxidation state

3. Reducing agent: always oxidized
4. Oxidizing agent: always reduced

Front 56

PV=nRT

Back 56

1. Ideal Gas Equation
2. R = .08206

Front 57

Pressure

Back 57

1 atm = average at sea level = 760 mmHg = 760 torr
1 atm = 101325 Pa
2. Force exerted on container walls by gas particles.

Front 58

Barometer

Back 58

1. Evacuated tube who tip is submerged in mercury - forced up by air pressure and measured.

Front 59

STP

Back 59

1 atm --------- 273.15 K

Front 60

Boyle's Law

Back 60

1. Pressure and Volume are inversely related
2. PV=PV

Front 61

Charle's Law

Back 61

1. Volume and Temperature are directly related
2. V/T=V/T

Front 62

Avogadro's Law

Back 62

1. Volume and Amount of Particles are directly related
2. V/n=V/n

Front 63

Ideal Gas Law

Back 63

PV=nRT

Front 64

Dalton's Law of Partial Pressure

Back 64

1. Sum of partial pressures of the components in a gas mixture must equal the total pressure.

Front 65

Energy

Back 65

1. Capacity to do work

Front 66

Work

Back 66

1. Force over distance
2. W= P* Change in Volume

Front 67

Kinetic Theory of Gases

Back 67

1. Volume of particle is negligible
2. Average kinetic energy is same for all gases at same temp - ideal
3. Collisions of particle are elastic
4. Pressure arises from collisions with container walls
5. No attraction/repulsion forces

Front 68

Heat

Back 68

1. Flow of energy caused by a temperature difference

Front 69

Kinetic energy

Back 69

1. Energy due to motion (thermal energy - molecules vibrate give off heat)

Front 70

Potential Energy

Back 70

1. Energy associated with position or composition

Front 71

Chemical Energy

Back 71

1. Energy associated with BONDS!!!!
2. When bonds are broken, chemical energy released.

Front 72

System

Back 72

1. Thing being studied
2. Heat coming into system = +q
3. Heat leaving system = -q

Front 73

Surroundings

Back 73

1. Everything outside of the system that can interact.

Front 74

Joules

Back 74

1. SI unit of energy

Front 75

calories versus Calories

Back 75

1. calorie: amount of energy required to raise 1 g of water by 1 degree Celcius.
2. Calories = 1000 calories - basically 1kcal

Front 76

1st Law of Thermodynamics

Back 76

1. Total energy of the universe is constant

Front 77

State Function

Back 77

1. Value depends only on the state on the system, not how the system arrived at that value.

Front 78

Heat Capacity

Back 78

1. Quantity of heat required to change temp by 1 degree Celcius

Front 79

Specific heat capacity

Back 79

1. Amount of heat required to raise 1 g of substance by 1 celcius
2. Intrinsic measure of ability to absorb heat.

Front 80

Pressure-Volume Work

Back 80

1. Force is a result of a volume change against an external pressure.
2. Such as a piston in a car motor

Front 81

Make sure to convert work from L*atm into Joules by ___________.

Back 81

1. L*atm * 101.3 J

Front 82

Molar Heat Capacity

Back 82

1. Amount of heat required to raise 1 mole of a substance by 1 degree Celcius

Front 83

Bomb Calorimeter

Back 83

1. Combustion reactions - measures heat change
2. Constant Volume, Temp Increase, Mass stays same
3. qcal=-qrxn

Front 84

Enthalpy

Back 84

1. Sum of Internal Energy + W

Front 85

Exothermic Vs Endothermic

Back 85

1. Exothermic - gives heat off - negative q
2. Endothermic - brings heat in - positive q

Front 86

Standard State

Back 86

1. Pure gas at 1 atm
2. Solution - exactly 1 M concentration
3. Liquid/solid - most stable form at 1 atm

Front 87

Coffee-Cup Calorimeter

Back 87

1. No pressure change
2. Measures heat change in solution reactions
3. qrxn=-qsol

Front 88

Hess's Law

Back 88

1. Change in enthalpy for a stepwise process is the sum of the enthalpy changes of the steps.

Front 89

Standard Enthalpy Change

Back 89

1. The change of enthalpy for a process where all reactants and products are in standard states.

Front 90

Standard enthalpy of formation

Back 90

1. Change of enthalpy when 1 mole of a compound forms from its constituent elements in standard states.

Front 91

Volume of an ideal gas is ______ at STP

Back 91

22.4 Liters

Front 92

Volume of an ideal gas is _______ L at absolute zero.

Back 92

0 L