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CHEM131 > Exam 1 Review > Flashcards

Exam 1 Review Flashcards

1
Q

matter

A

that which has mass and volume

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2
Q

law of conservation of mass

A

mass is neither created or destroyed in a normal chemical rxn

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3
Q

law of definite proportions

A

all samples of a pure compound have the same proportions by mass of their constituent elements

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4
Q

law of multiple proportions

A

when atoms of 2 elements combine to make 2 different compounds, the mass of the element A that combine with B in the 2 can be expressed as a ratio of small whole numbers

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5
Q

extensive property

A

depends on amount

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6
Q

intensive property

A

independent of amount

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7
Q

femto (f)

A

10^-15

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8
Q

pico(p)

A

10^-12

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9
Q

nano(n)

A

10^-9

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10
Q

micro(u)

A

10^-6

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11
Q

milli(m)

A

10^3

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12
Q

centi(c)

A

10^-2

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13
Q

deci(d)

A

10^-1

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14
Q

kilo(k)

A

10^3

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15
Q

mega(M)

A

10^6

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16
Q

giga(G)

A

10^9

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17
Q

tera(T)

A

10^12

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18
Q

Cathode ray experiment

A

discovers electron, negative charge, and charge to mass ratio

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19
Q

Oil drop experiment

A

measured the strength of E-field necessary to halt the free fall oil droplets deducing the charge of an electron and thus the mass

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20
Q

Gold foil experiment

A

alpha particles passed through gold foil, most went straight though, some deflected, evidence for nuclear theory of the atom

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21
Q

nuclear theory of the atom

A

-most of atom’s mass and all its positive charge are in a dense region called nucleus

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22
Q

frequency equation

A

f=c/wavelength

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23
Q

KE of ejected electron

A

Ephoton - Ebinding

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24
Q

Ephoton

A

hf

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25
Q

de broglie wavelength

A

a moving e- has a wavelength = h/mv

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26
Q

Heinsberg Uncertainty

A

we cannot simultaneously observe the wave and particle nature of electrons, the act of observation forced the electron into one state or another. (uncertainty in position)(m*uncertainty in velocity) >= h/4pi

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27
Q

indeterminancy

A

the present doe not determine the future; one can only know probability of finding electron in a certain region

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28
Q

principle quantum number (n)

A

overall size and energy level of an orbital, n=1,2,3,…

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29
Q

angular momentum quantum number (l)

A

determines the shape of the orbital, l=0…(n-1).

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30
Q

l=0

A

s

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31
Q

l=1

A

p

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32
Q

l=2

A

d

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33
Q

l=3

A

f

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34
Q

magnetic quantum number(ml)

A

specifies orientation of orbital, ml = -l to +l (integers)

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35
Q

spin quantum number (ms)

A

ms= -1/2 or +1/2

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36
Q

group 1a

A

alkali earth metals

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37
Q

group 2a

A

alkaline earth metals

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38
Q

group 7a

A

halogens

39
Q

group 8a

A

noble gases

40
Q

pauli exclusion principle

A

no 2 electrons in an atom can have the same 4 quantum numbers

41
Q

aufbau principle

A

lowest energy orbitals are filled first

42
Q

hunds rule

A

electrons first fill singly with II spins, then they pair

43
Q

metals

A

tend to lose e, good conductors of heat and electricity, malleable, ductile

44
Q

nonmetals

A

tend to gain electrons, poor conductors

45
Q

metalloids

A

semiconductors

46
Q

atomic radius

A

increases down a group bc n increases resulting in larger orbitals, decreases across a period bc Zeff increases. remains roughly constant in transition elements bc outermost principle energy level remain constant after 1st 2 groups of transition

47
Q

transition cations

A

ns electrons removed before (n-1)d

48
Q

paramagnetic

A

an atom that contains one or more unpaired electrons is attracted to external magnetic field

49
Q

diamagnetic

A

an atom with all electrons paired is slightly repelled by external magnetic field. proof of how transition cations are formed

50
Q

ionic radii

A

cations are smaller than original element, anions are larger

51
Q

ionization energy

A

energy required to remove an electron; 1st ie decreases down a group, increases across a period . successive ionization energies - increase, then really increase once noble gas config is reached

52
Q

exceptions to ie trends

A

when going from s to p orbital, half filled shell (N and O)

53
Q

electron affinity

A

energy change associated with the gaining of an electron; only 1a has a group trend, becomes more positive. across period ea becomes more negative (adding electron would release more energy into the atmosphere)

54
Q

chemical bonds

A

form bc they lower pe of charged particles that compose atoms

55
Q

ionic bond

A

btwn metal and nonmetal, transfer of electrons, forms a lattice of alternating cations and anions

56
Q

covalent compounds

A

2 or more nonmetals, share electrons

57
Q

lattice energy

A

formation of ionic compounds gives off energy bc pe decreases with the formation of crystalline lattice of cations and anions

58
Q

ionic formulas

A

charges must balance

59
Q

naming ionic compounds

A

name of cation + base name of anion and -ide; if cation can form multiple charge add that

60
Q

metals that form cations with different charges

A

chromium, iron, cobalt, copper, tin, mercury, lead

61
Q

acetate

A

C2H3O2(-)

62
Q

carbonate

A

CO3(2-)

63
Q

hydrogen carbonate

A

HCO3(-)

64
Q

hydroxide

A

OH(-)

65
Q

Nitrite

A

NO2(-)

66
Q

Nitrate

A

NO3(-)

67
Q

Chromate

A

CrO4(2-)

68
Q

Dichromate

A

Cr2O7(2-)

69
Q

phosphate

A

PO4(3-)

70
Q

Hydrogen phosphate

A

HPO4(2-)

71
Q

dihydrogen phosphate

A

H2PO4(-)

72
Q

ammonium

A

NH4(+)

73
Q

hypochlorite

A

ClO(-)

74
Q

chlorite

A

ClO2(-)

75
Q

chlorate

A

ClO3(-)

76
Q

perchlorate

A

ClO4(-)

77
Q

permanganate

A

MnO4(-)

78
Q

Sulfite

A

SO3(2-)

79
Q

hydrogen sulfite

A

HSO3(-)

80
Q

sulfate

A

SO4(2-)

81
Q

hydrogen sulfate

A

HSO4(-)

82
Q

cyanide

A

CN(-)

83
Q

peroxide

A

O2(2-)

84
Q

hemi

A

0.50

85
Q

mono

A

1

86
Q

di

A

2

87
Q

tri

A

3

88
Q

tera

A

4

89
Q

penta

A

5

90
Q

hexa

A

6

91
Q

hepta

A

7

92
Q

octa

A

8

93
Q

nona

A

9

94
Q

deca

A

10

CHEM131 (3 decks)

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