Chemistry Final

Front 1

Chemistry

Back 1

the central science, which deals with all the matter in the universe and the changes it undergoes

Front 2

Matter

Back 2

anything which has mass and takes up space(volume)

Front 3

Solid

Back 3

definite shape, and volume and is not easily compressed

Front 4

Liquid

Back 4

indefinite shape and volume, and not easily compressed

Front 5

Gas

Back 5

indefinite shape and volume and is easily compressed

Front 6

Homogeneous Mixture

Back 6

a mixture that is visually the sample throughout the entire sample

Front 7

Heterogeneous Mixture

Back 7

a mixture that is visually different throughout the sample

Front 8

Element

Back 8

contains only one type of atom

Front 9

Compound

Back 9

can be broken down to simpler substances by chemical means

Front 10

Physical Change

Back 10

can be observed without changing the identity of the substance

Front 11

Chemical Change

Back 11

the substance identity is different after the change

Front 12

Density

Back 12

the ratio of the mass of an object to its volume

Front 13

Dalton

Back 13

1808-Dalton’s Atomic Theory
1.All elements are composed of invisible parts called atoms
2.Atoms of the same element are identical-False because of isotopes
3.Atoms can combine, separate, and rearrange in a Chemical Reaction
4.Atoms combine in simple whole number ratios

Front 14

Proton

Back 14

a positively charged subatomic particle found in a nucleolus of an atom

Front 15

Electron

Back 15

“-” charged subatomic particle outside the nucleus

Front 16

Nucleus

Back 16

a time dense central portion of an atom, composed of protons and neutrons.

Front 17

Atom

Back 17

the smallest particle of an element that retains its identity in a chemical reaction

Front 18

Atomic Number

Back 18

is equal to the number of protons found in the nucleus of the atom

Front 19

Mass Number

Back 19

is the sum of protons and neutrons in the nucleus of the atom

Front 20

Chemistry

Back 20

the central science, which deals with all the matter in the universe and the changes it undergoes

Front 21

Matter

Back 21

anything which has mass and takes up space(volume)

Front 22

Solid

Back 22

definite shape, and volume and is not easily compressed

Front 23

Liquid

Back 23

indefinite shape and volume, and not easily compressed

Front 24

Gas

Back 24

indefinite shape and volume and is easily compressed

Front 25

Homogeneous Mixture

Back 25

a mixture that is visually the sample throughout the entire sample

Front 26

Heterogeneous Mixture

Back 26

a mixture that is visually different throughout the sample

Front 27

Element

Back 27

contains only one type of atom

Front 28

Compound

Back 28

can be broken down to simpler substances by chemical means

Front 29

Physical Change

Back 29

can be observed without changing the identity of the substance

Front 30

Chemical Change

Back 30

the substance identity is different after the change

Hint 30

literaly chemical change

Front 31

Isotopes

Back 31

atoms of the same element that have the same atomic number but different atomic masses due to a different number of neutrons

Front 32

Electron configuration

Back 32

the arrangement of electrons of an atom in its ground state into various orbitals around the nuclei of atoms

Front 33

Valence Electrons

Back 33

electrons in the highest energy level

Front 34

Aufbau Principle

Back 34

states that we must occupy the lowest energy level orbital that can receive it

Front 35

Hund’s Rule

Back 35

states that each orientation of an orbital must be occupied by one electron before electron before a second electron is added to any orbital orientation.

Front 36

Pauli Exclusion Principle

Back 36

states that no two electrons in any one atom can have the same set of four quantum numbers

Front 37

Octet Rule

Back 37

atoms react by gaining or losing electrons so as to acquire the stable electron structure of a noble gas, usually eight valence electrons.

Front 38

Photon

Back 38

a quantum of light; a discrete bundle of electromagnetic energy that interacts with matter similarly to particles

Front 39

Nonmetal

Back 39

no luster, not malleable, not ductile, not good conductor of heat and electricity

Front 40

Metalloid

Back 40

semi-metal

Front 41

Ion

Back 41

charged atom-gained or loss electrons

Front 42

Anion

Back 42

a negative ion

Front 43

Cation

Back 43

a positive ion

Front 44

Ionization Energy

Back 44

the energy required removing an electron from an atom in its gaseous state

Front 45

Electronegativity

Back 45

an ability of an atom in a bond to attract an electron

Front 46

Atomic Radius

Back 46

one-half the distance between the nuclei of the two atoms of the same element when the atoms are joined

Hint 46

↓,←

Front 47

Lewis/ Electron Dot Structure

Back 47

a notation that depicts valence electrons as dots around the atomic symbol of the element; the symbol represents the inner electrons and atomic nucleus; also called Lewis dot Structure

Front 48

Covalent

Back 48

sharing of electrons between two atoms

Front 49

Diatomic molecule

Back 49

a molecule consisting of two atoms

Front 50

Polar molecule

Back 50

a molecule in which one side of the molecule is slightly negative and the opposite side is slightly positive.

Front 51

Non-polar covalent bond

Back 51

a covalent bond in which the electrons are shared equally by two atoms.

Front 52

Intermolecular Forces

Back 52

are forces of attraction between molecules

Front 53

London Dispersion Forces

Back 53

an intermolecular force between two Non Polar molecules

Front 54

Dipole-Dipole Factors

Back 54

an attractive force between two polar molecules

Front 55

Hydrogen Bonding

Back 55

a intermolecular force between Hydrogen and a highly electronegative atom. (FONS)

Front 56

Resonance

Back 56

when a single Lewis Dot cannot explain the observed Bonding

Front 57

Metallic Bonding

Back 57

the force of attraction that holds metals together; it consists of the attraction of free-floating valence electrons for positively charged metal ions.

Front 58

VESPER

Back 58

a valance-shell electron-pair repulsion theory; because electron pairs repeal, molecules adjust their shapes so that valence electron pairs are as far apart as possible.

Front 59

Hybridization

Back 59

the mixing of several atomic orbitals to form the same total number of equivalent hybrid orbitals.

Front 60

Single Replacement

Back 60

a chemical equation that does not indicate the relative amounts of reactants and products

Front 61

Double Replacement

Back 61

a chemical change that involves an exchange of positive ions between two compounds.

Front 62

Synthesis

Back 62

a chemical change in which two or more substances react to form a single new substance

Front 63

Decomposition

Back 63

a chemical change in which a single compound is broken down into tow or more simpler products

Front 64

Combustion

Back 64

a chemical change in which an element or a compound reacts with oxygen, often producing energy in the form of heat and light

Front 65

Oxidation Number

Back 65

a positive or negative number assigned to an atom to indicate its degree of oxidation or reduction; the oxidation number of an uncombined element is zero

Front 66

Molar Mass

Back 66

a term used to refer to the mass of a mole of any substance

Front 67

Percent Composition

Back 67

the percent by mass of each element in a compound

Front 68

Empirical Formula

Back 68

a formula with the lowest whole-number ratio of elements in a compound; the empirical formula of hydrogen peroxide (H2O2 → HO)

Front 69

Molecular Formula

Back 69

represents the exact number of atoms in a molecule

Front 70

Reactant

Back 70

a substance present at the start of a reaction

Front 71

Product

Back 71

a substance produced in a chemical reaction

Front 72

Theoretical Yield

Back 72

the amount of product that could form during a reaction calculated from a balanced chemical equation; it represents the maximum amount of product that could be formed from a given amount of reactant.

Front 73

Percent Yield

Back 73

the ration of the actual yield to the theoretical yield for a chemical reaction expressed as a percentage; a measure of the efficiency of a reaction

Front 74

Ideal Gas Law

Back 74

the relationship PV=nRT, which describes the behavior of an ideal gas

Front 75

Boyle’s Law

Back 75

for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure.

Front 76

Charles Law

Back 76

the volume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant.

Hint 76

V up T up

Front 77

Combined Gas Law

Back 77

the law that describes the relationship among the pressure, temperature, and the volume of an enclosed gas.

Front 78

Dalton’s Law of Partial Pressure

Back 78

at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressure of the component of gas.

Hint 78

V=constant
T=constant
P=sum of partial pressure of gas

Front 79

Kinetic Molecular Theory

Back 79

the theory explaining the states of matter, based on the concept that all matter consists of tiny particles that are in constant motion

Front 80

Effusion

Back 80

the process that occurs when a gas escapes through a tiny hole in its container

Front 81

Diffusion

Back 81

the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout

Front 82

Vaporization

Back 82

the conversion of a liquid to a gas or a vapor

Front 83

Standard temperature and pressure (STP)

Back 83

the conditions under which the volume of a gas is usually measured; standard temperature is 0°C, and the standard pressure is 101.3kPA, or 1 atmosphere(atm).

Front 84

Phase Diagram

Back 84

a graph showing the conditions at which a substance exists as a solid, liquid, or vapor.

Front 85

Kinetic Energy

Back 85

the energy an object has because of its motion

Front 86

Equilibrium

Back 86

the relative concentrations of reactants and products of a reaction that has reached equilibrium; indicates whether the reactants or products are favored in the reversible reaction

Front 87

Molar Heat of Vaporization (Δhvap)

Back 87

the amount of heat absorbed by one mole of a liquid as it vaporizes at a constant temperature.

Front 88

Molar Heat of Fusion- (Δhfus)

Back 88

the amount of the hat absorbed by one mole of a solid substances as it melts to a liquid a constant temperature

Front 89

Molar Heat of Condensation- (ΔHcond)

Back 89

the amount of heat released by one mole of a vapor as it condenses to a liquid at a constant temperature

Front 90

Enthalpy (H)

Back 90

the heat content of a system at constant pressure

Front 91

Entropy (S)

Back 91

a measure of the disorder of a system; systems tend to go from a state of order (low entropy) to a state of disorder (high entropy)

Front 92

Solubility

Back 92

the amount of a substance that dissolves in a given quantity of solvent at specified conditions of temperature and pressure to produce a saturated solution
Solute- dissolved particles in a solution

Front 93

Solute

Back 93

dissolved particles in a solution

Front 94

Solvent

Back 94

the dissolving medium in a solution

Front 95

Molarity (M)

Back 95

the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 liter of solution

Front 96

Molality(m)

Back 96

the concentration of solute in a solution expressed as the number of moles of solute dissolved in 1 kilogram (1000g) of solvent.

Front 97

Aqueous Solution

Back 97

water that contains dissolved substances