Chem Final

Front 1

matter

Back 1

that which occupies space and has mass

Front 2

physical change

Back 2

a change in the physical form of a substance without changing its chemical identity

Front 3

physical properties

Back 3

properties of a substance that can be observed without changing the substance chemically

Front 4

pure substance

Back 4

a sample consisting of only one kind of matter, either compound or element

Front 5

phase

Back 5

a visibly distinct part of a heterogenous sample of matter

Front 6

potential energy

Back 6

energy possessed by a body of virtue of its position in an attractive and or repulsive force field

Front 7

chemical change

Back 7

a change in which one or more substances dissapear and one or more new substances form

Front 8

chemical property

Back 8

the types of chemical change a substance is able to experience

Front 9

compound

Back 9

a pure substance that can be broken down into two or more pure substances by a chemical change

Front 10

distillation

Back 10

the process of seperating components of a mixture by boiling off and condensing the more volatile component

Front 11

element

Back 11

a pure substance that can't be decomposed into other pure substances by ordinary chemical means

Front 12

endothermic reaction

Back 12

a change that absorbs energy from the surroundings, having a positive delta H, an increase in enthalpy

Front 13

exothermic reaction

Back 13

a reaction that gives off energy to its surroundings

Front 14

electrostatic force

Back 14

the force of attraction or repulsion between electrically charged objects

Front 15

mixture

Back 15

sample of matter that consists of two or more chemicals

Front 16

homogenous solution

Back 16

sample that has a uniform appearence and composition throughout

Front 17

heterogenous mixture

Back 17

having a non-uniform composition usually with visually different parts or phases

Front 18

atom

Back 18

smallest unit particle of an element

Front 19

law of constant composition

Back 19

any compound is always made up of the same elements in the same proportion by mass

Front 20

force field

Back 20

a region of space where a force is effective

Front 21

static electricity

Back 21

objects acquiring an electrical charge that is not moving

Front 22

law of conservation of mass

Back 22

in a nonnuclear change mass is conserved

Front 23

law of conservation of energy

Back 23

in a nonnuclear change energy is conserved

Front 24

dalton's atomic theory

Back 24

All objects are made up of atoms. All atoms are identical. Atoms of two different elements have two different atoms. Atoms can't be destroyed or created. Atoms of different elements can combine to form compounds

Front 25

atomic number

Back 25

number of protons in a nucleus

Front 26

mass number

Back 26

number of protons and neutrons in a nucleus

Front 27

anion

Back 27

negatively charged ion with one more electron than protons

Front 28

cation

Back 28

positively charged ion with one less electron than protons

Front 29

viscosity

Back 29

how quickly a liquid flows

Front 30

specific heat

Back 30

amount of energy required to raise one gram of substance by 1 degree celcius

Front 31

calorimetry

Back 31

environment from which there is a minimum energy leakage

Front 32

like disolves like

Back 32

if forces between molecules of A are about the same as the forces between molecules of B then A+B will probably dissolve in each other

Front 33

misclible

Back 33

dissolves and mixes

Front 34

immiscible

Back 34

doesn't mix

Front 35

weight percent of solute

Back 35

mass of solute/mass of solute+solvent x 100

Front 36

molarity

Back 36

expressed as mol solute/L solution

Front 37

standardization of solution

Back 37

uses a solution of known molarity to react with a component in a solution of unknown concentration. (titration)

Front 38

molality

Back 38

moles of solute per kg of solution

Front 39

colligative properties

Back 39

solution properties that are dtermined only by the number of solute particles dissolved in s fixed quantity of solvent

Front 40

Le Chatelier's principle

Back 40

if a system at equilibrium is subjected to change then the system will adjust and find a predictable new equilibrium

Front 41

combustion reactions

Back 41

carbon containing compounds. Oxygen will always be a reactant. Water and Carbon Dioxide will always be products

Front 42

limiting reagent

Back 42

starting materials corresponding to the least number of moles

Front 43

theoretical yield

Back 43

gram quantity of product theoretically possible if the reaction went to 100% completion

Front 44

actual yield

Back 44

gram quantity actually physically in a reaction

Front 45

quantom concept

Back 45

electrons are stacked around the nucleus at discrete quantinized energy levels

Front 46

ionization energy

Back 46

energy required to remove one electron from a gaseous atom of an element

Front 47

metal

Back 47

an element whose atoms tend to lose electrons in chemical reactions forming cations

Front 48

ionic bonding

Back 48

involves full electron exchange between atoms. Electrostatic bond based on attraction of opposite charge

Front 49

ionic compound

Back 49

molecule. No molecular boundary

Front 50

covalent bonding

Back 50

sharing electrons between nuclei of atoms. Electron sharing allows both atoms a noble gas configuration

Front 51

molecular formula

Back 51

number of atoms of each element in a unit molecule

Front 52

empirical formula

Back 52

smallest whole number ratio of one atom to another in a compound

Front 53

acid

Back 53

any compound which can donate a hydrogen cation to another compound ina pair

Front 54

base

Back 54

any compound which recieves a hydrogen cation from anoter compound in a pair