Chemistry Chapters 3-6

Front 1

atom:

Back 1

the smallest particle of an element that retains its identity in a chemical reactions

Front 2

Dalton's Atomic Theory (now we know it's not all correct):

Back 2

1. all elements have atoms 2. atoms of the same element are the same, atoms o different elements are different 3.atoms can form compounds 4. chemical rxns occur when atoms are seperated, joined, or rearrainged, but they are never changed into atoms of another chemical

Front 3

Rutherford's experiment:

Back 3

The gold foil experiment. He sent alpha particles at a very thin sheet of gold foil, some particles went through, but others bounced back at angles. This proved existence of a nucleus and disproved the plum-pudding model

Front 4

nucleus:

Back 4

the tiny core of an atom, it has protons and neutrons

Front 5

isotopes

Back 5

atoms that have the same number of protons but different numbers of neutrons

Front 6

atomic mass:

Back 6

a weighted average mass of the atoms in a naturally occuring sample of the element

Front 7

period:

Back 7

a row in the periodic table, there are 7

Front 8

group

Back 8

each vertical column of the periodic table

Front 9

What is the basic difference between elements?

Back 9

they have different numbers of protons

Front 10

# of neutrons= ?

Back 10

mass#-atomic #

Front 11

J J THomson's atom

Back 11

the plum-pudding model (a mass of positive stuff with electrons inside)

Front 12

Robert Miliken's Experiment

Back 12

the oil-drop experiment, foudn the charge of an electron

Front 13

charge of proton, electron, neutron

Back 13

+1, -1, 0

Front 14

atomic number (z):

Back 14

an atoms # of protons

Front 15

mass # (A)

Back 15

everything in the nucleus (protons and neutrons)

Front 16

cathode ray experiment:

Back 16

an experiment that discovered electrons, a cathode ray was sent between two metal disks in a vaccum, when magnetic things wer placed near the ray, the angle changed

Front 17

energy levels:

Back 17

the fixed energies an electron can have

Front 18

quantum:

Back 18

teh amount of energy needed to make an electron move from one energy level to the next

Front 19

atomic orbital:

Back 19

a region in space in which there is likely an electon

Front 20

Bohr postulate 1

Back 20

the atom only has certain allowable energy levels- stationary states

Front 21

Bohr postulate 2

Back 21

the atom does nto radiate energy while in a stationary state

Front 22

Bohr postulate 3

Back 22

the atom changes to another stationary state (which means the electron moves orbit) only by absorbing or emitting a photon whose energy is equal to the

Front 23

How are quantum mumbers and energy levels related?

Back 23

The quantum muber corresponds to the electrons a sublevel can hold Q(0) = s(2electrons) 1=p(6 electrons) 2=d 3=f

Front 24

What is the equation that determines the change in energy when an electron changes levels?

Back 24

-2.18x10^-18Joules(1/nfinal squared-1/n initial squared

Front 25

electron configurations:

Back 25

the ways electrons are arrainged in orbitals around the nucleus

Front 26

aufbau principle:

Back 26

says electrons occupy the orbitals of the lowest energy first

Front 27

pauli exclusion principle:

Back 27

says an atomic orbital may describe at most two electrons, one spinning in each direction

Front 28

Hund's rule

Back 28

says one electron must be in each possible orbital before there can be two in one

Front 29

what are the five exceptions to standard electron configuration rules

Back 29

cr, mo, cu, ag, au

Front 30

What is the equation relating wavelength and frequency?

Back 30

c= lamda v or speed of light = wavelngthxfrequency

Front 31

spectrum:

Back 31

a spctrum of colors form when light is sent through a prism

Front 32

atomic emission spectrum:

Back 32

the frecuencies of light emitted by an element

Front 33

ground state:

Back 33

the lowest possible energy level of an electron

Front 34

photons

Back 34

light qunta

Front 35

Heisenberg uncertainty principle:

Back 35

it is impssible to know the position and velocity of an electron at the same time

Front 36

What do electrons do when they drop an energy level?

Back 36

they release light

Front 37

What does the eauation E=hv tell u (energy = planck's constantxfrequency)

Back 37

it tells you the energy change of the electron or the frequency of the light released when an electron drops a level

Front 38

valence electrons

Back 38

outermost electrons, they participate in bonding, always from s and p, maximum of 8 valence electrons

Front 39

What are the valence electrons in flourine?

Back 39

1s2 2s2 2p5 so the valence are 2s2 and 2p5

Front 40

core electrons:

Back 40

inner electrons ( not valence)

Front 41

atomic radius:

Back 41

one half the distance between the nuclei of two atoms of the same element when the atoms are joined

Front 42

ion:

Back 42

an atom of group of atoms that has a positive or negative charge

Front 43

anion

Back 43

a negatively charged ion (gained electron)

Front 44

cation

Back 44

a positively charged ion

Front 45

ionization energy

Back 45

the energy required to remove an electron from an atom

Front 46

Are anions and cations bigger than the original atom?

Back 46

cations are always smaller and anions are always bigger

Front 47

periodic law

Back 47

when elements are arrainged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties

Front 48

metals:

Back 48

most elements are metals, they are malleable, ductile, shiny

Front 49

nonmetals:

Back 49

usually gases, are brittle, and can't conduct electricity well, except for Carbon

Front 50

metalloids:

Back 50

sometiems act like metals, sometimes don't