Chemistry Chapter 3

Front 1

law of conservation of mass

Back 1

states that matter is neither created nor destroyed during ordinary chemical reactions, but it can be rearranged

Front 2

law of definite proportions

Back 2

chemical compound contains the same elements in exactly the same proportions by mass regardless of the size or source of the chemical

Front 3

law of multiple proportions

Back 3

elements combine in simple whole number ratios

Front 4

John Dalton

Back 4

english schoolteacher who came up with a theory to explain the laws of conservation of mass, definite proportions, and multiple proportions

Front 5

Dalton's Atomic Theory

Back 5

1) all matter is composed of atoms
2)atoms of an element are identical in size, mass, & other properties; atoms of different elements differ in size, etc.
3) atoms can't be subdivided, created, or destroyed
4) atoms of different elements combine in simple whole-number ratios to form chemical compounds
5) In chemical reactions, atoms are combined, separated, or rearranged

Front 6

atom

Back 6

smallest particle of an element that retains the properties of that element

Front 7

isotopes

Back 7

havae an unusual number of neutrons

Front 8

1 amu

Back 8

weight of protons / neutrons

Front 9

0 amu

Back 9

weight of electrons

Front 10

nuclear forces

Back 10

proton-neutron / proton-proton / neutron-neutron forces that hold the nuclear particles together

Front 11

atomic number

Back 11

number of protons in each atom of an element
[located above abbrev]

Front 12

isotopes

Back 12

atoms of the same element that have different masses

Front 13

mass number

Back 13

total number of protons and neutrons that make up the nucleus of an isotope

Front 14

nuclide

Back 14

general term for a specific isotope of an element

Front 15

average atomic mass

Back 15

the weighted average of the atomicm asses of the naturally occurring isotopes of an element

Front 16

mole

Back 16

the amount of a substance that contains as many particles as there are atoms in 12 g of carbon-12

Front 17

molar mass

Back 17

mass of one mole of a pure substance

Front 18

democritus

Back 18

greek thinker who named the atom, meaning "indivisible"

Front 19

aristotle

Back 19

thinker who did not believe in atoms, thinking that all matter was continuous

Front 20

cathode

Back 20

part of the cathode ray connected to the negative terminal

Front 21

anode

Back 21

part of the cathode ray connected to the positive terminal

Front 22

jj thompson

Back 22

english physicist who discovered electrons
with cathode ray tube

Front 23

ernest rutherford

Back 23

scientist from new zealand who discovered the nucleus