Chem Final Review

Front 1

Evaporation

Back 1

process by which molecules of a liquid escape from the surface of the liquid and enter the gaseous, or vapor state

Front 2

Oxidation

Back 2

reaction in which the atoms or ions of an element lose one or more electrons and thus attain a more positive oxidation state (higher oxidation number)

Front 3

Ionization

Back 3

the formation of or separation into ions by heat, electrical discharge, radiation, or chemical reaction

Front 4

Tarnish

Back 4

a thin layer of corrosion that forms over copper, brass, silver, aluminum, and other similar metals as their outermost layer undergoes a chemical reaction. Does not always result from the sole effects of oxygen in the air

Front 5

Filtration

Back 5

a mechanical or physical process to separate solids from fluids

Front 6

Solvent

Back 6

substance that does the dissolving in a solution

Front 7

Oxidation Number

Back 7

number assigned to the atoms in a molecule that show the general distribution of electrons among bonded atoms; equal to the charge in ionic compounds and the charge assigned to the atom according to electronegativity rules for covalent compunds

Front 8

Atomic Mass

Back 8

weighted average of the masses of the existing isotopes of an element

Front 9

Family

Back 9

vertical column of the periodic table that contains elements with similar electron configurations, also known as a group

Front 10

Period

Back 10

horizontal row of elements in the periodic table

Front 11

Ion

Back 11

atom or a group of atoms that has a positive or negative charge because it has lost or gained electrons

Front 12

Alkane

Back 12

hydrocarbon molecule with only single bonds

Front 13

Alkene

Back 13

unsaturated hydrocarbon that contains at least one double bond

Front 14

Alkyne

Back 14

unsaturated hydrocarbon that contains at least one triple bond

Front 15

Reducing Agent

Back 15

substance that loses electrons or attains a more positive oxidation state (higher oxidation number) during an oxidation-reduction reaction

Front 16

Precipitate

Back 16

the creation of a solid in a solution or inside another solid during another chemical reaction or by diffusion in a solid. When the reaction occurs in a liquid solution, the solid formed is this

Front 17

Condensation

Back 17

change of state from gas to liquid

Front 18

Fermentation

Back 18

a chemical reaction in which sugars are broken down into smaller molecules that can be used in living plant systems

Front 19

Dissociation

Back 19

a general process in which ionic compounds separate or split into smaller particles, ions, or radicals, usually in a reversible manner

Front 20

Melting

Back 20

the process by which a substance changes from the solid phase to the liquid phase

Front 21

Decantation

Back 21

a process to separate mixtures can separate particles from a liquid by allowing the solids to settle to the bottom of the mixture and pouring off the particle free part of the liquid

Front 22

Solute

Back 22

substance that is dissolved in a solvent to form a solution

Front 23

Mass Number

Back 23

sum of the number of protons and neutrons in the nucleus of a given atom

Front 24

Group

Back 24

vertical column of the periodic table that contains elements with similar electron configurations, also known as a family

Front 25

Transition Elements

Back 25

any metallic element in columns 3-12 on the periodic table

Front 26

Isotope

Back 26

atom that has the same number of protons as another atom, but has a different number of neutrons

Front 27

Bright-line Spectra

Back 27

an emission spectrum consisting of light lines against a dark background

Front 28

Oxidizing Agent

Back 28

substance that gains electrons or attains a more negative oxidation state (lower oxidation number) during an oxidation-reduction reaction

Front 29

Distillation

Back 29

the separation of a liquid mixture into its separate elements based on different boiling points

Front 30

Electrolysis

Back 30

the passage of an electric current through an electrolyte with subsequent migration of positively and negatively charged ions to the negative and positive electrodes

Front 31

Sublimation

Back 31

the transition of a substance directly from the solid to the gas phase without passing through an intermediate liquid phase, an endothermic process that occurs when temperatures and pressures below a substance’s triple point on the phase diagram

Front 32

Dissolving

Back 32

the process by which a solute forms a solution in a solvent

Front 33

Chromatography

Back 33

a technique used to separate the components of a chemical mixture by moving the mixture along a stationary material like gelatin; different parts of the mixture are caught by the material at different rates and make isolated bands that can be analyzed

Front 34

Solution

Back 34

homogeneous mixture of two or more substances in a single physical state

Front 35

Activation Energy

Back 35

difference between the energy of an activated complex and the energy of the reactants of a chemical reaction, which is produced by an effective collision of particles

Front 36

Atomic Number

Back 36

number of protons in the nucleus of an atom

Front 37

Vapor Pressure

Back 37

the pressure exerted by a vapor in equilibrium with the solid or liquid phase of the same substance, the partial pressure of the substance in the atmosphere above the solid or liquid

Front 38

Vapor Pressure Equilibrium

Back 38

the pressure of vapor in equilibrium with its non-vapor phases

Front 39

First Ionization Energy

Back 39

the energy needed to remove one or more electrons from a neutral atom to form a positively charged ion is a physical property that influences the chemical behavior of an atom

Front 40

Excited State

Back 40

energy level attained by an electron that absorbs additional energy and jumps from its normal level to a higher energy level

Front 41

Democritus

Back 41

an ancient Greek philosopher who said that all matter is made up of tiny particles, he said that an atom is the tiniest particle of matter

Front 42

Dalton

Back 42

wrote the atomic theory (basically took information we already knew about atoms and put it all together) 1. Atoms are made up of spherical, tiny, indivisible particles (false) 2.atoms of the same element are the same; atoms of different elements are different (false) 3. In a chemical reaction, atoms are conserved (true) 4. For any given compound, you always have the same atoms in the same ratios (true) except for a few exceptions

Front 43

Bohr

Back 43

separated light into different colors, prism effect is diffraction grating

Front 44

Lavoisier

Back 44

considered the father of modern chemistry; wrote the first list of most elements, created the metric system

Front 45

Thomson

Back 45

used a cathode ray tube to do experiments on atoms and found out about charges such as the fact that the charge to mass ratio was the same in all of his experiments

Front 46

Avogadro

Back 46

came up with the Avogadro constant (6.022 X 10`23) which is the number of particles for a mole of a given substance. Also came up with Avogadro’s Law which states that equal volumes of gases at the same temperature and pressure contain an equal number of particles.

Front 47

Rutherford

Back 47

discovered radioactive half-life; he proved that radioactivity involved the transmutation of one chemical element to another, and also differentiated and named alpha, beta, and gamma radiation (Alpha is positive 4 and 2, gamma is neutral, and beta is negative 0 and 1)

Front 48

Franklin

Back 48

did stuff electricity, realized lightning could be used as energy and conducted, also found out things like charge repel and opposites attract