Gen Chem 1101 Chapter 1

Front 1

homogeneous or hetereogenous;
can be separated physically

Back 1

mixture

Front 2

elements or compounds;
chemical change required to separate

Back 2

substance

Front 3

smallest unit of a pure element while still retaining that element's chemical properties

Back 3

atom

Front 4

smallest unit of a compound that still retains the chemical properties of that compound

Back 4

molecule

Front 5

particles are arranged regularly

Back 5

solid

Front 6

particles are not confined to one location

Back 6

liquid

Front 7

particles are far apart and collide randomly

Back 7

gas

Front 8

theory that explains properties of a substance according to the motion of its basic particles

Back 8

Kinetic Molecular Theory

Front 9

occupies space and has mass

Back 9

matter

Front 10

has a uniform composition

Back 10

homogeneous mix

Front 11

nonuniform composition

Back 11

heterogeneous mix

Front 12

homogeneous mixture;
uniform composition that may vary widely

Back 12

solution

Front 13

electrically charged atoms or groups of atoms

Back 13

ion

Front 14

mass/volume

Back 14

density

Front 15

properties that depend on the amount of substance
Ex: mass, volume, energy

Back 15

extensive

Front 16

properties that don't depend on the amount of substance
Ex: melting point, density

Back 16

intensive

Front 17

a substance's identity is preserved even though it may have changed its physical state

Back 17

physical change

Front 18

one or more substances are transformed into one or more different substances

Back 18

chemical change

Front 19

an observation that gives unitless information
Ex: the chairs are blue

Back 19

qualitative

Front 20

an observation that gives a numerical value
Ex: there are 36 chairs

Back 20

quantitative

Front 21

the values agree with an accepted or known value of a quantity

Back 21

accuracy

Front 22

the values have a high degree of reproducibility

Back 22

precision

Front 23

indicates the precision of the measurement and therefore the precision of the measuring instrument

Back 23

significant figures

Front 24

did the Cathode Ray experiment

Back 24

Sir Joseph John Thomson

Front 25

experiment used to determine the charge to mass ratio for electrons

Back 25

Cathode Ray Experiment

Front 26

did the Oil Drop experiment

Back 26

Robert Andrew Millikan

Front 27

experiment used to determine the charge of an electron

Back 27

Oil Drop Experiment

Front 28

did the Gold Foil experiment

Back 28

Earnest Rutherford

Front 29

experiment used to determine that atoms contain a small, positively charged nucleus that contains most of the atom's mass

Back 29

Gold Foil Experiment

Front 30

number of protons in an atom

Back 30

atomic number (z)

Front 31

1/12 of the mass of an atom of carbon-12

Back 31

atomic mass unit (u)

Front 32

sum of number of protons and neutrons for an atom

Back 32

mass number (A)

Front 33

atoms with the same number of protons but different masses

Back 33

isotope

Front 34

# of atoms of a given isotope/total # of atoms of all isotopes of that element

Back 34

percent abundance formula

Front 35

the average weight of a representative sample of atoms

Back 35

atomic weight

Front 36

(% abundance of isotope 1)/100 x the mass of isotope 1 + ...

Back 36

atomic weight formula

Front 37

the amount of particles of a substance equal to the amount of atoms in 12g of carbon-12

Back 37

mole

Front 38

6.0221415 x 10^23 particles

Back 38

Avogadro's Number

Front 39

consists of protons and nuetrons;
contains most of the atom's mass

Back 39

nucleus

Front 40

Mass is converted to energy in the nuclear reaction that forms atoms.

Back 40

Mass Defect

Front 41

the rows in a periodic table

Back 41

periods

Front 42

the columns in a periodic table

Back 42

groups or families

Front 43

metallic character increases down a column and decreases from left to right

Back 43

trend