Physics Ch.3 Review

Front 1

Mass

Back 1

quantity of matter. measured in kilograms

Front 2

Weight

Back 2

Force that an object exerts under the influence of gravity

Front 3

Atom

Back 3

smallest particle or unit of element that still possesses chemical properties of that element

Front 4

Element

Back 4

group of identical atoms that possess same chemical properties

Front 5

Molecule

Back 5

two of more atoms chemically bonded

Front 6

Compound

Back 6

group of identical molecules that possess same chemical properties

Front 7

Mixture

Back 7

combination of two or more simple and/or complex substances.

Simple substance= pure O2
Complex substance= H2O

Front 8

Greek Atomic theory

Back 8

The first ones to do it.

Matter had 4 basic components: Air, Water, Earth, Fire

Components had 4 basic essences: Wet, Dry, Hot, Cold

Front 9

Dalton Atomic theory

Back 9

(1808)
-Atoms could be differentiated by mass.
-Figured out element was identical atoms that react the same

Front 10

J.J. Thompson Atomic Theory

Back 10

(1890)
-Plum pudding model
- Electrons integral part of all atoms
-Electrons suspended in uniform mas of positive electrification, understood there were different charges

Front 11

Rutherford atomic theory

Back 11

-Nuclear model
-Atom contains small positively charged nucleus (+)
-surrounded by negative cloud of randomly placed electrons (-)
-didn't understand orbiting shells

Front 12

Bohr atomic theory

Back 12

(1913)
-what WE use, expanded on Rutherford's.
-atom resembles solar system
-negative electrons circle positive nucleus
-closer electron to nucleus, stronger the bond

Front 13

Nucleus

Back 13

-contains protons and neutrons (together = Nucleons)
- Atomic # = # of protons in nucleus and determines element

Front 14

Proton

Back 14

(+)
made up of quarks
mass=1

Front 15

Neutron

Back 15

(=) no charge!
Made up of gluons
mass=1

Front 16

Electron

Back 16

(-) doesn't weight anything

Front 17

Centripedal Force

Back 17

Force of nucleus pulling towards itself

Front 18

Centrifugal Force

Back 18

Force of electron flying out

Front 19

Atomic Number AKA Z number

Back 19

number of protons in an atom, defines element
i.e. Tungsten Z=74

Front 20

Atomic Mass Number

Back 20

number of protons and neutrons in atom

*Atomic Mass-Atomic Number = Number of Neutrons

Front 21

Isotopes

Back 21

Atoms with same number of protons but different number of neutrons. (Z=same, Atomic Mass=different)

Front 22

Carbon

Back 22

(C)
Z=6, A=12

Elemental Mass= 12.01

K-shell binding energy= 0.28keV

Front 23

Tungsten

Back 23

(W)
Z=74, A=184

Elemental Mass= 183.8

K-Shell Electron binding energy= 69.5 keV

Front 24

# of Orbital Electrons per Shell

Back 24

N= 2(n)^2
where n = shell number

Front 25

Octet rule

Back 25

Outermost shell (valence shell) never exceeds 8 potential electrons

Front 26

Ionization

Back 26

Complete removal of an electron from its orbital shell

Ion pair is negative = ANION
Ion pair is positive = CATION

Front 27

Electron binding energy

Back 27

Eb
-The closer an electron to the nucleus, the higher the binding energy, measured in eV.
-Part of characteristic radiation within tube. Electron from cathode strikes electron on anode and creates photon

Front 28

Characteristic radiation

Back 28

Photon and electron exit and photon's energy dependent on what shell electron comes in to fill it's place within shell

Front 29

Periodic table: Periods

Back 29

Rows. Each period starts new shell of electrons

Front 30

Periodic table: Groups

Back 30

Columns. Each group has similar chemical properties.

Front 31

Electron arrangement

Back 31

Number of electrons in outermost shell = group (column)
-also determines valence of electron
-also determines period (row) in periodic table

Front 32

Covalent bond

Back 32

two or more atoms share electrons to fill their shells

Front 33

Ionic bond

Back 33

one atom donates its electron, but electronegativity is different for each
-strong, but vulnerable to chemical attack
-one cation and one anion, formed molecule is NEUTRAL

Front 34

Ionic bonds: Cation and Anion and their charges

Back 34

Cation donates e-, is now positive

Anion attracts e-, is now negative

Front 35

What is radioactivity?

Back 35

Decay or disintegration of unstable atomic nucleus as it attempts to become stable.
-emission of energy is radiation

Front 36

Beta emission

Back 36

Electron formed within nucleus by breakdown of neutron into proton and electron. Electron released along with radiation, proton stays and changes element
-More penetrating than Alpha!

Front 37

Alpha emission

Back 37

Emission of alpha particle from nucleus. Alpha particles contain 2 protons and 2 neutrons. Emission of alpha particle means atomic mass decreases by 4 and atomic number decreases by 2, while element becomes another element.

-only happens with heavy radioisotopes. larger than Beta emission, but does more damage

Front 38

Gamma emission

Back 38

High energy EM radiation sometimes given off with Alpha OR Beta particle emission

Doesn't change isotope or element

Front 39

Half-life

Back 39

time required for radioactive element to be reduced to one half of original value

Front 40

Particulate Radiation

Back 40

Alpha, Beta

Front 41

EM Radiation

Back 41

Photons: X-rays, Gamma radiation