Chemistry Final

Front 1

What are the names and charges of all of the particles in the nucleus?

Back 1

Protons (+)
Neutrons (-)

Front 2

What is an isotope

Back 2

a isotope is an atom that has the same number of protons but a different number of neutrons

Front 3

Isotope Notation

Back 3

(A/Z) X → (3/1) H

A= Mass number
Z= Atomic number

Front 4

Hypen Notation

Back 4

Hydrogen - 3

Front 5

Mass Number

Back 5

sum of the numbers of protons and neutrons in the nucleus of an atom

Front 6

Atomic Number

Back 6

Number of protons and neutrons of an atom; that atomic number is the same for all atoms of an element

Front 7

What is the Relationship between grams and atomic mass units

Back 7

1 amu = 1.66 x 10^-27

Front 8

What is avogadros number?

Back 8

6.022 x 10^23

Front 9

What is avogadros number used for

Back 9

fundamental physical constant used to convert moles of a substance to a quantity of particles which make up that sucstanc

Front 10

What is the relationship between c, λ and v?

Back 10

λ = wavelength
v = frequency
c = speed of light (3.0 x 10^8)
c = λv of v =C/λ

Front 11

What happens to an atom when it moves to its excited state?

Back 11

Absorbs energy

Front 12

Ground state

Back 12

lowest possible enenergy level

Front 13

Excited State

Back 13

High energy level

Front 14

Principal energy level

Back 14

the principle energy level means a value indicating the distance that an electron may move away from the nucleus of an atom

Front 15

Sublevel

Back 15

orbital with a principal energy level

Front 16

Orbital

Back 16

region in an atom where there is a high probabilty of finding electrons

Front 17

For a given energy level how many electrons are in s, p, f, d sublevel?

Back 17

s = 2
P= 6
d= 10
f= 14

Front 18

How many orbitals in s p f d

Back 18

s = 1
p = 3
d = 5
f= 7

Front 19

what are two forces in the nucleus?

Back 19

Electrostatic Force and Strong Nuclear force

Front 20

electrostatic force

Back 20

pulls nuclei apart

Front 21

strong nuclear force

Back 21

holds nuclei together

Front 22

alpha emission

Back 22

(4/2) He
Restricted to heavy nuclei

Front 23

Beta emission

Back 23

(0/-1)β

Front 24

Gamma Emission

Back 24

0/0 Y
highest energy
no charge

Front 25

Group numbers represent

Back 25

number of valence electrons

Front 26

Trend for ionization energy

Back 26

increases left to right
decreases top to bottom

Front 27

Trend for Atomic Radius

Back 27

Decreases moving left to right
Increases moving top to bottom

Front 28

Trend for electronegativity

Back 28

increases left to right
decreases top to bottm

Front 29

cations

Back 29

positive

Front 30

anions

Back 30

negetive

Front 31

Isoelectronic

Back 31

species that have the same number of electrons and the same electron configuration

Front 32

high ionization energy

Back 32

positive ion

Front 33

chemical bond

Back 33

attractive forve that holds atoms or ions

Front 34

Polarity

Back 34

a property of a system in which two points have opposite characteristics such as chargers

Front 35

Characteristics of Ionic Bonds

Back 35

-High melting point
-Bonds are strong
-hard brittle
-good insulators
-conduct electricity

Front 36

Dipole-dipole forces

Back 36

polar

Front 37

london dispersion

Back 37

all forces

Front 38

Aufbau Principle

Back 38

Aufbau is German for Building up; its the principle that electrons fill energy levels from the bottom up

Front 39

Hunds Rule

Back 39

maximum multiplicity describes the order in which electrons fill subshells. It states that they will add into degerate orbitals to create the greatest multitude of orbitals having an electron in them

Front 40

Pauli Exclusion principle

Back 40

No two electrons or protons or neutrons in a given system can be in states characterized by the same set of quantum numbers

Front 41

saturated hydrocarbons

Back 41

organic compound formed only by carbon and hydrogen linked by single bonds

Front 42

Percent Composition

Back 42

percentage by mass of each element in a compound

Front 43

Empirical Formula

Back 43

chemical formula that shows the composition of a compound in terms of the relative numbers and kinds of atoms in the simplest ration

Front 44

molecular formular

Back 44

chemical formula that shows the number and kids of atoms in a molecule but not the arrangement of the atoms

Front 45

Unsaturated solution

Back 45

solution that contains less solute than a saturated solution does and thus is able to dissolve additional solute

Front 46

Saturated Solution

Back 46

solution that cannot dissolve any more solute under given conditions

Front 47

supersaturated solution

Back 47

solution that holds more dissolved solute than required to reach equilibrium

Front 48

Solute

Back 48

substance that dissolves in the solvent

Front 49

solvent

Back 49

substance in which the solute dissolves

Front 50

hydrates

Back 50

molecule that contains some type of water

Front 51

Electrolytes

Back 51

Any of various ions, such as sodium, potassium, or chloride, required by cells to regulate the electric charge and flow of water molecules across the cell membrane

Front 52

Molarity

Back 52

The concentration unit of solution expressed as moles of solute dissolved per liter of solution

M = mol/Liter

Front 53

Molality

Back 53

The concentration of a solution expressed in moles of solute per kilograms of solvent
m = mol / Kg

Front 54

PPT

Back 54

parts per thousand

1 x 10 ^ -3

Front 55

PPM

Back 55

Parts per million

1 x 10 ^-6

Front 56

PPB

Back 56

Parts per Billion 1 x 10^-9

Front 57

Dilution

Back 57

Process of reducing the concentration of a solute in solution
M1V1 = M2V2

Front 58

What is Kc

Back 58

Products over Reactants

Front 59

What is oxidation states

Back 59

the condition of an atom expressed by the number of electrons that that atom needs to reach its elemental form

Front 60

Oxidation Numbers

Back 60

indicate the general distribution of electrons among the bonded atoms in a molecular compound of molecular ion

Front 61

What is Oxidation?

Back 61

Loss of Electrons
Half Reaction
Na --> Na(+) + e-

Front 62

Reduction

Back 62

Gain
Half Reaction
Cl2 + 2e- --> 2Cl-

Front 63

Binary Synthesis

Back 63

Two elements mis to form a compound (always redox)
A + X --> AX

Front 64

Metal Oxides in water (synthesis

Back 64

Never redox
Format: MO (s) + H20(l) -> M(OH)2(s)

Front 65

Binary Decomposition

Back 65

Always redox
Format: AX-->A + X

Front 66

What is Oxidation?

Back 66

Loss of Electrons
Half Reaction
Na --> Na(+) + e-

Front 67

Reduction

Back 67

Gain
Half Reaction
Cl2 + 2e- --> 2Cl-

Front 68

Binary Synthesis

Back 68

Two elements mis to form a compound (always redox)
A + X --> AX

Front 69

Metal Oxides in water (synthesis

Back 69

Never redox
Format: MO (s) + H20(l) -> M(OH)2(s)

Front 70

Binary Decomposition

Back 70

Always redox
Format: AX-->A + X

Front 71

Metal Carbonate Decomposistion

Back 71

Never Redox
Format: MCO3 --> MO (s) + CO2(g)

Front 72

Metal Hydroxide Decomposition

Back 72

Never Redox
Format: M(OH)2(s) --> MO + H2O

Front 73

Metal Chlorate Decomposition

Back 73

Always redox

MCLO3 (S) --> MCL (s) + O2

Front 74

Acid decomp (oxyacids only)

Back 74

Sometimes redox
HXOy (aq) --> XOy-1 (g) + H2O (l)

Front 75

Single replacement
Metal Replacement

Back 75

A+BX --> AX (aq) + B2 (g)

Front 76

Single Replacement Halogen Replacement

Back 76

Y2 (g) + BX (s) --> BY (s) + B2 (g)

Front 77

Double replacement with no precipitate

Back 77

No Reaction occurs

Front 78

Double Replacement Precipitate

Back 78

Never redox
AX (aq) + BY (aq) --> AY (s) + BX (aq)

Front 79

Carbon Combustion

Back 79

Products are always oxygen gas and water vapor
EX: C4H10 (l) + O2 --> CO2 (g) +H2) (g)

Front 80

Equations associated with pH and pOH

Back 80

pH + pOH = 14
[H+][OH-] = 1 x 10^-14
pH = -log [H+]
[H+] = 10^-pH
pOH = -log [OH-]
[OH-] = 10^-pOH

Front 81

Characteristics of acids

Back 81

sour, react with bases to produce salt and water, react with metals to produce hydrogen gas and conduct electric current

Front 82

Svante Arrhenius Definition of Acid

Back 82

substances that ionize in water and increase the number of hydrogen ions

Front 83

Bronsted-Lowry Def. Acids

Back 83

H+ donors

Front 84

Characteristics of Bases

Back 84

bitter, slippery, react with acids to produce salt and water and conduct electric current

Front 85

Svante Arrenius Definition of Bases

Back 85

substance that ionizes in water and increases the number of hydroxide ions

Front 86

Bronsted Lowry Definition of Base

Back 86

H+ Acceptors

Front 87

How to convert between Pressure Units

Back 87

1 atm = 760 torr = 14.7 lb/in = 101.325 kPascal

Front 88

Boyle's Law

Back 88

p1V1=P2V2

Front 89

Charles law

Back 89

V1/T1=V2/T2

Front 90

Gay-lussacs Law

Back 90

P1T2=P2T1

Front 91

Combines Gas Law

Back 91

V2 = (p1)(T2)(V1)/(p2)(t1)

Front 92

Dalton's law of partial pressure

Back 92

states that the total pressure exerted by a gaseous mixture is equal to the sum of the partial pressures of each individual component in a gas mixture
p1+p2+p3....=ptotal

Front 93

Graham's law of Effusion

Back 93

Rate1 / Rate2 = square root of (Mass2 / Mass 1)