Chemistry Final Semester 1

Front 1

Pure Substance

Back 1

All particles are the same and can't be broken down by physical process; one type of material.
ex: elements and compounds

Front 2

Mixtures

Back 2

Two or more pure substances

Front 3

heterogeneous mixture

Back 3

contains phases; chocolate chip cookie

Front 4

homogeneous mixture

Back 4

same appearance through out; also called solution

Front 5

Tera (T)

Back 5

10^12

Front 6

Giga (G)

Back 6

10^9

Front 7

Mega (M)

Back 7

10^6

Front 8

Kilo (K)

Back 8

10^3

Front 9

Hecto (h)

Back 9

10^2

Front 10

Deca (da or dk)

Back 10

10^1

Front 11

Deci (d)

Back 11

10^-1

Front 12

Centi (c)

Back 12

10^-2

Front 13

Milli (m)

Back 13

10^-3

Front 14

Micro

Back 14

10^-6

Front 15

Nano (n)

Back 15

10^-9

Front 16

Pico (p)

Back 16

10^-12

Front 17

Democtritus

Back 17

originally named the atom; solid homogeneous sphere

Front 18

Dalton

Back 18

proposed the atomic theory; solid homogeneous sphere

Front 19

Thompson

Back 19

Plum pudding model; proved existence of negative particles. (surrounded by positive material.

Front 20

Rutherford

Back 20

nucleus with gold foil experiment; positive particles in the nucleus with electrons surrounding

Front 21

Bohr

Back 21

model was like planets orbiting the sun with protons and neutrons in the nucleus with electrons orbiting

Front 22

Atomic Number

Back 22

number of protons (and electrons), bottom number in the nuclear symbol, and top left corner on each element on the periodic table

Front 23

Mass number

Back 23

mass of protons and neutrons

Front 24

atomic mass

Back 24

bottom # on elements on the periodic table

Front 25

isotope

Back 25

different forms of the same atom

Front 26

Ion

Back 26

atoms that gain or lose electrons

Front 27

Father of the periodic table

Back 27

Mendeleev

Front 28

Characteristics of metals

Back 28

shiny, conduct heat and electricity, malleable, and ductile

Front 29

Characteristics of nonmetals

Back 29

don't conduct, dull solids or gases, brittle

Front 30

Seven diatomic elements

Back 30

Hydrogen, nitrogen, oxygen, fluorine, Chlorine, Bromine, and Iodine

Front 31

Ionization energy

Back 31

energy needed to remove an electron from an atom

Front 32

Nuclear fission

Back 32

large nuclei being split into smaller ones; fuels nuclear bombs and power plants

Front 33

Nuclear Fusion

Back 33

Small nuclei being combined to former a larger nucleus; fuels hydrogen bombs and stars

Front 34

Transmutation

Back 34

elements being changed into a different one during a nuclear reaction

Front 35

ionic bonds

Back 35

bonds between a metal and non-metal; electrons are gained and lost

Front 36

Polar Covalent Bonds

Back 36

two different non-metals bonded

Front 37

Non-Polar Covalent Bonds

Back 37

two of the same non-metals bonded

Front 38

Electronegativity

Back 38

the measure of how much an element attracts an electron; increases up and to the right

Front 39

Dispersion force

Back 39

attraction between molecules because of a random unbalance

Front 40

Critical Point

Back 40

where a liquid and a gas become indistinguishable

Front 41

Triple Point

Back 41

where a substance is a solid, liquid, and gas at one time

Front 42

Nuclear Reaction

Back 42

Atom is changed, can involve one or multiple atoms, and can create a new element

Front 43

Chemical Reaction

Back 43

Nucleus remains unchanged, always involves multiple atoms, new compounds are made when elements are rearranged.

Front 44

C

Back 44

3.00 x 10^8 m/s

Front 45

ionizing radiation

Back 45

radiation powerful enough to knock electrons out of the atom; can damage molecules including DNA

Front 46

alpha decay

Back 46

a product; can be blocked by paper

Front 47

beta decay

Back 47

product; can be blocked by small amounts of lead

Front 48

electron capture

Back 48

reactant

Front 49

positron emission

Back 49

product

Front 50

gamma ray (radiation)

Back 50

product; can be blocked with thick lead