Chem Exam 1

Front 1

micro

Back 1

ten negative six

Front 2

NANO

Back 2

ten negative nine

Front 3

pico

Back 3

ten negative 12

Front 4

femto

Back 4

ten negative 15

Front 5

attractive and repulsive forces that act between either electrically charged or magnetic objects

Back 5

electromagnetic forces

Front 6

same number of protons but different number of neutrons

Back 6

isotope

Front 7

atomic weight = ??

Back 7

abundance of isotope x mass + abundance of isotope2 x mass2

Front 8

intrument used to measure precise masses and relative amounts of atomic and molecular ions

Back 8

mass spectrometer

Front 9

group 1a

Back 9

alkali metals

Front 10

group 2a

Back 10

alkaline earth metals

Front 11

group 6a

Back 11

chalcogens

Front 12

group 7a

Back 12

halogens

Front 13

group 8a

Back 13

noble gases(rare gases)

Front 14

rutherford experiment

Back 14

shot particles at gold foil, discovered the nucleus

Front 15

unit of frequency

Back 15

hertz, or cycles per second

Front 16

light or dark: wave crests arrive together

Back 16

light

Front 17

light or dark: wave crest and trough arrive together

Back 17

dark

Front 18

atoms emit or absorb energy in quanta; energy of light is quantized as photons

Back 18

quantum theory

Front 19

energy of a photon is what number?

Back 19

planck's constant 6.606e-34 j s

Front 20

Electrons are emitted by metal only if light has freq greater than certain min. value, not matter how intense the light

Back 20

photoelectric effect

Front 21

light emitted by excited atoms

Back 21

line spectra

Front 22

distance between two adjacent peaks

Back 22

wavelength

Front 23

distance of wave from center line to crest or trough

Back 23

amplitude

Front 24

smallest wavelength

Back 24

gamma rays

Front 25

largest wavelength

Back 25

radio

Front 26

electromagnetic spectrum from smallest to greatest wavelength

Back 26

gamma x uv visible infrared microwaves radio

Front 27

visible light range

Back 27

400 to 700

Front 28

visible light order from smallest to largest wavelength

Back 28

vibgyor

Front 29

emission of light from hot objects

Back 29

black body effect

Front 30

emission of electrons from metal surfaces on which light shines

Back 30

photoelectric effect

Front 31

emission of light from electronically excited gas atoms

Back 31

emission spectra

Front 32

a fixed amount

Back 32

quantum

Front 33

quantum??

Back 33

a fixed amount

Front 34

said energy can only be released or absorbed by atoms only in discrete chunks of some minimum size

Back 34

planck

Front 35

radiation composed of a single wavelenght

Back 35

monochromatic

Front 36

when radiation from a source is seperated into its different wavelength components

Back 36

spectrum

Front 37

spectrum containing radiation of only specific wavelengths

Back 37

line spectrum

Front 38

when n is infinity, energy is

Back 38

zero

Front 39

limitation of the bohr model

Back 39

can only explain line spectrum for H atom

Front 40

describes the wave characteristics of material particles

Back 40

matter waves

Front 41

it is inherently impossible for us to know simultaneously both the exact momentum of the e and its exact location in space

Back 41

uncertainty principle

Front 42

no two e in an atom can have the same set of four quantum numbers

Back 42

pauli exclusion principle

Front 43

all orbitals filled unpaired first

Back 43

Hund's rule

Front 44

quantum number, measures size

Back 44

n

Front 45

quantum number, measures shape

Back 45

l

Front 46

quantum number, measures orientation

Back 46

ml

Front 47

quantum number, measures spin

Back 47

ms

Front 48

L values correspond to these subshells

Back 48

0 s 1 p 2 d 3 f

Front 49

region of space with size, shape, characteristic energy

Back 49

orbitals

Front 50

shape of s orbital number 1

Back 50

spherical

Front 51

shape of p orbital number 3

Back 51

dumbbell

Front 52

shape of d orbital number 5

Back 52

5 shapes

Front 53

principal quantum number

Back 53

n

Front 54

asimuthal quantum number

Back 54

L

Front 55

magnetic quantum number

Back 55

mL

Front 56

these control the chemistry of the elements

Back 56

valence electrons

Front 57

organization of periodic table determined by

Back 57

electron configurations

Front 58

elemental properties determined by

Back 58

size and shape of orbitals and atomic number

Front 59

atomic size across a group, atomic size down a period

Back 59

decreases and increases

Front 60

effective nuclear charge across a group, effective nuclear charge down a period

Back 60

increases and increases

Front 61

net positive charge experienced by an electron in a many-electron atom

Back 61

effective nuclear charge

Front 62

charge equal to the charge minus the shielding

Back 62

effective nuclear charge

Front 63

is cation or anion smaller?

Back 63

cation because has same charge but less e, so each e pulled closer

Front 64

ionic size across a period, ionic size down a group

Back 64

decreases and increases

Front 65

same number of electrons

Back 65

isoelectronic series

Front 66

energy needed to remove an electron

Back 66

ionization energy

Front 67

these electrons are more easily removed, outer or inner

Back 67

outer

Front 68

ionization energy across a period, ionization energy down a group

Back 68

increases and decreases

Front 69

it takes extra energy to remove an electron when?

Back 69

when subshell filled or half filled

Front 70

energy needed to add an electron to an atom or ion in gas phase

Back 70

electron affinity

Front 71

when you add an e to an element

Back 71

electron affinity

Front 72

electron affinity across a period, down a group

Back 72

becomes more negative, very little change

Front 73

electronegativity across a period and down a group

Back 73

increases across, decreases down

Front 74

metallic character across and down

Back 74

metallic character decreases across, increases down

Front 75

measures the ease with which an atom gains an electron

Back 75

electron affinity

Front 76

force holding atom or ions together

Back 76

chemical bond

Front 77

electrostatic force between ions of opposite charge

Back 77

ionic bond

Front 78

sharing of electrons between two bonded atoms

Back 78

covalent bond

Front 79

bond found in metals

Back 79

metallic bond

Front 80

NH4

Back 80

1+

Front 81

OH

Back 81

-1

Front 82

CN

Back 82

-1

Front 83

NO3

Back 83

-1

Front 84

MnO4

Back 84

-1

Front 85

CO3

Back 85

-2

Front 86

CrO4

Back 86

-2

Front 87

SO4

Back 87

-2

Front 88

PO4

Back 88

-3

Front 89

the change in energy when an ionic solid is seperated into isolated ions in the gas phase

Back 89

lattice energy

Front 90

melting point depends on

Back 90

smaller radius means larger lattice means higher meltingg point

Front 91

simplest compounds, contain only H and C

Back 91

hydrocarbons

Front 92

class of hydrocarbons, contains all single bonds

Back 92

alkanes

Front 93

class of hydrocarbons, contains double bond

Back 93

alkenes

Front 94

class of hydrocarbons with a triple bond

Back 94

alkynes

Front 95

equal sharing of electrons

Back 95

nonpolar bond

Front 96

unequal sharing of electrons

Back 96

polar bond

Front 97

tendency of an atom to attract electrons to itself in a bond

Back 97

electronegativity

Front 98

this is the purest covalent bond

Back 98

between two identical atoms

Front 99

formal charge is equal to

Back 99

number of valence minus (num lone pairs + 1/2 num bonding Es)

Front 100

more than one lewis structure for fixed nuclear arrangement

Back 100

resonance

Front 101

1 and a half bonds

Back 101

aromatic bonds