Ch.2

Front 1

Forms of energy: Chemical energy (definition?)

Back 1

form of energy stored int eh bonds of chemical substances.

Ex. It the type of energy stored in our foods.

Front 2

Forms of energy: Electrical energy (definition?)

Back 2

results from the movement of charged particles.

Ex. our nervous system uses electrical energy to to send signals to our body.

Front 3

Forms of energy: Mechanical energy (definiton?)

Back 3

energy that is directly involved in moving matter.

Ex. our legs provide the mechanical energy necessary to move the pedals on a bike.

Front 4

Forms of energy: Radiant energy or Electromagnetic energy (definition?)

Back 4

energy that travels in waves; collectively called electromagnetic spectrum.

Ex. visible light, infrared waves, radio waves, ultraviolet waves, and X-rays.

Front 5

Atomic orbital model: orbitals (definition?)

Back 5

regions around the nucleus in which a given electron or electron pair is likely to be found. Not a fixed circular orbit.

Front 6

Atomic orbital model: electron cloud (definition?)

Back 6

probably regions of greatest electron density

Front 7

Atomic structure: Radioactivity (definition?)

Back 7

the process of unstable, heavier isotopes of atoms that decompose spontaneously into more stable forms.

Process of atomic decay.

Front 8

Atomic structure: Radioisotopes (definition?)

Back 8

isotopes that exhibit radioactivity.

Front 9

Mixtures: Solutions (definitions?)

Back 9

homogeneous mixtures of components that may be gases, liquids, or solids.

Ex. mineral water

Front 10

Mixtures: Solvent (definitions?)

Back 10

substance present in the greatest amount;

the medium that is doing the dissolving.

Ex. in mineral water, the water is the solvent.

Front 11

Mixtures: Solute (definitions?)

Back 11

substances present in smaller amounts;

the medium that is being dissolved.

Ex.in mineral water, the minerals are the solute.

Front 12

Mixture concentrations: Molarity (definition?)

Back 12

moles per liter; indicated by M

Front 13

Mixture concentrations: Mole (definition?)

Back 13

and element or compound is equal to its atomic weight or molecular weight weighed out in grams.

Front 14

Mixture concentrations: Molecular weight (definition?)

Back 14

the sum of atomic weights weighed out in grams. (molecule is made up different atoms; the molecular weight is the sum of the atom's weight)

Front 15

Mixtures: Colloid (definition?)

Back 15

also called emulsions; are heterogeneous mixtures with solute particles that are larger than those in a solution, but do not settle out.

Ex. jello

Front 16

Mixtures: Suspensions (definition?)

Back 16

heterogeneous mixtures with large, often visible solutes that tend to settle out.

Ex. mixture of sand and water, or blood (plasma separates from red blood cells)

Front 17

What is the difference between a compound and a mixture?

Back 17

no chemical bonding occurs between the components of a mixture; they do occur in compounds.

mixtures can be separated by physical means (filtering, straining, etc.) and compounds can only be separated by chemical means.

Front 18

Ionic bond (definition?)

Back 18

a chemical bond between atoms formed by the transfer of one or more electrons from one atom to the other.

Ex. the formation of table salt uses ionic bonds.

Front 19

Anion (definition?)

Back 19

the atom that gains one or more electrons, and has a net negative charge. The atom that accepts an electron (the anion) is an electron acceptor.

Front 20

Cation (definition?)

Back 20

the atom that loses electrons is the electron donor and has a positive charge.

think of the "t" in cation as "+" sign for positive charge.

Front 21

Covalent bond (definition?)

Back 21

a bond where two atoms share electrons so they each fill their outer shell part of the time.

Front 22

Hydrogen bond (definition?)

Back 22

see textbook

Front 23

Chemical reaction (definition?)

Back 23

occurs whenever chemical bonds are formed, rearranged, formed, or broken.

Front 24

Reactants (definition?)

Back 24

the number and kinds of reacting substance in a chemical reaction.

Front 25

Products (definition?)

Back 25

the chemical composition of a substance resulting from a chemical reaction.

Front 26

Chemical Reaction Patterns: Synthesis Reaction or Combination Reaction (definition?)

Back 26

when atoms or molecules combine to form a larger, more complex molecule.

it always involves bond formation.

A + B -> AB

Front 27

Chemical Reaction Patterns: Anabolic

Back 27

constructive activities in body cells.

Ex. joining small molecules called amino acids into large protein molecules.

Front 28

Chemical Reaction Patterns: Decomposition Reaction (definition?)

Back 28

occurs when a molecule is broken down into smaller molecules or its constituent parts.

bonds are always broken.

AB -> A + B

Front 29

Chemical Reaction Patterns: Catabolic (definition?)

Back 29

degradative

Front 30

Chemical Reaction Patterns: Exchange Reaction or Displacement Reaction

Back 30

involves both synthesis and decomposition.

bonds are both made and broken.

AB + C -> AC + B and AB + CD -> AD + BC

a molecule is broken up (AB and/or CD) and a new one is formed (AC, AD, and/or BC)

Front 31

Chemical Reaction Patterns: Oxidation - Reduction Reactions or Redox Reactions

Back 31

See textbook

Front 32

Chemical Reaction Patterns: Oxidized

Back 32

process of losing an electron.

Front 33

Chemical Reaction Patterns: Reduced

Back 33

process of reactant taking up the transferred electrons.

Front 34

Exergonic Reactions (definition?)

Back 34

a reaction that releases energy.

Front 35

Endergonic Reactions (definition?)

Back 35

a reaction that absorbs energy.