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college chem 117 > midterm exam 1 > Flashcards

midterm exam 1 Flashcards

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1
Q

what unit is used for average atomic weight

A

Dalton (Da)

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2
Q

although avagrados number works for all elements, what element is the number based off of

A

Carbon - 12

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3
Q

units of molar mass

A

g/mol

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4
Q

how many atoms are there in 3 moles O2

A

36.12 * 10^23 atoms

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5
Q

how many atoms are there in 3 moles of O

A

18.09 * 10^23 atoms

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6
Q

what is the definition for mole regarding avogrados number

A

a collection of avogrados number of atoms is a mole of atoms

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7
Q

what is matter

A

anything that occupies space and has mass

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8
Q

what determines the properties of matter

A

the structure of particles

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9
Q

what is the smallest unit of an element

A

an atom

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10
Q

what is a substance that can’t be broken into a simpler substance by any means

A

element

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11
Q

what is the mass of protons and neutrons

A

1.67262 * 10^-24

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12
Q

what is the mass of an electron

A

9.10936 * 10^-28

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13
Q

why aren’t atomic masses whole numbers

A

they are the averages of all known isotopes weights

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14
Q

Peta (size, symbol)

A

10^15, P

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15
Q

Tera (size, symbol)

A

10^12, T

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16
Q

Giga (size, symbol)

A

10^9, G

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17
Q

Mega (size, symbol)

A

10^6, M

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18
Q

Kilo (size, symbol)

A

10^3, K

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19
Q

Deci (size, symbol)

A

10^-1, d

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20
Q

Centi (size, symbol)

A

10^-2, c

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21
Q

Milli (size, symbol)

A

10^-3, m

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22
Q

Micro (size, symbol)

A

10^-6, μ

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23
Q

Nano (size, symbol)

A

10^-9, n

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24
Q

Pico (size, symbol)

A

10^-12, p

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25
Q

Femto (size, symbol)

A

10^-15, f

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26
Q

Atto (size, symbol)

A

10^-18, a

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27
Q

what are the two waves light consists of

A

magnetic (red) and electric (blue)

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28
Q

light is an electromagnetic _____ phenomenon, consisting of oscillating ________________ through space.

A

wave, electric and magnetic fields

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29
Q

what can light act as

A

a wave and a particle

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30
Q

all types of of electromagnetic waves travel with the same _____, what is it?

A

velocity, speed of light 2.88 * 10^8 m/s

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31
Q

how are frequency and wavelength related? explain

A

inversely, if wavelength goes up the frequency goes down

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32
Q

what does hertz stand for

A

per second

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33
Q

how are frequency and energy related? explain

A

parallel, when frequency goes up, the energy goes up

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34
Q

what is it called when light is acting as stream of particles

A

photon

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35
Q

when a photon interacts with an electron, how much energy does it transfer to the electron

A

ALL OF IT

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36
Q

define wave-particle dualality

A

behaves like a wave and particle at same time

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37
Q

how many photons can interact with an electron at a time

A

only one

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38
Q

describe a discrete interaction when energy is quantized, give example

A

the photon of the light must be transferred as a solid, not just part of it, for example you can’t just go up a half of a stair, you have to go up the whole thing

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39
Q

whats an eV, whats it equal to

A

amount of energy gained by an electron falling through an electric potential drop of one volt, 1.6 * 10^-19 J

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40
Q

all matter is _______ a wave and a particle

A

simultaneously

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41
Q

how do atomic particles emulate light

A

they act as waves and particles

42
Q

what is linear momentum

A

the product of mass and speed (mv)

43
Q

why is matter, like electromagnetic radiation, thought of as quantized?

A

you can’t make a wave w 2.58 wavelengths, it has to be whole integer

44
Q

both matter and electromagnetic radiation have _____ and ______ properties, and their energies are _______

A

wave, particle, quantized

45
Q

what is the most important factor in determining properties of electrons

A

their wave nature

46
Q

if an electron or particle is acting as a wave, can we precisely determine the location

A

no

47
Q

do electrons satellite the nucleus like planets

A

NOOOOO

48
Q

What is Heisenbergs uncertainty principle

A

both position and momentum cannot be known simultaneously

49
Q

what is schrodingers equation represent

A

it describes an electron as a wave

50
Q

what do wavefunctions, ψ, specify

A

the energy states of an electron in an atom, provides info about the probability of finding the location of the e- in the allowed energy state

51
Q

how is an orbital defined

A

by wave functions and the wave nature of an e-

52
Q

can wave functions specify the precise location of a function?

A

NOOO

53
Q

what makes up a full set of quantum numbers

A

(n,l,m(l),m(s))

54
Q

in quantum numbers, whats the definition of “n”, possible values, and what does it effect

A

the principal quantum number, (n= 1,2,3,4,5,6,7), defines the size and energy of an atomic orbital

55
Q

in quantum numbers, whats the definition of “l”, possible values, and what does it effect

A

the angular momentum quantum number, (s=0, p=1, d=2, f=3), defines the shape in 3 space

56
Q

in quantum numbers, whats the definition of “m(l)”, possible values, and what does it effect

A

the magnetic quantum number, (it goes from -l to +l, so for a d orbital, it can be [-2,2]), defines the orientation/direction of the orbital in 3 space and the number of orbitals in a shell/subshell

57
Q

what is a collection of orbitals with the same principle quantum number

A

electron shell

58
Q

what is the collection of orbitals that have the same n and l value

A

sub shell

59
Q

how many atomic orbitals does each element have

A

an infinite number

60
Q

what is probability density, and whats the symbol

A

the probability of finding the electron in the small region of space divided by the volume of that region of space, ψ

61
Q

besides probability density, what can wave functions define

A

the energy of an electron in a particular atomic orbital

62
Q

what defines an atomic orbital

A

quantum numbers

63
Q

the energies of all orbitals within a shell have (same or different) energies?

A

SAME

64
Q

does an electron have more energy in the nucleus or far from the nucleus?

A

far from the nucleus

65
Q

what is a free e-

A

an electron not in the nucleus

66
Q

why is the energy of an e- in an atomic orbital negative

A

it is lower in energy than a free e-

67
Q

in an orbital, where are you most likely to find an e-

A

near the nucleus

68
Q

what does it mean that an s orbital is spherically symmetrical

A

it doesn’t matter what direction you go, the probability of finding an e- is based of only distance from nucleus

69
Q

what are peaks in a radial probability function based off of

A

n

70
Q

what does the peak w the highest probability correspond to in a radial probability function

A

the distance from the nucleus where an e- is MOST likely to be found

71
Q

what is a node

A

a place where there is NO probability of finding an electron

72
Q

how do you find the number of nodes

A

n-1

73
Q

when n increases, what happens to the size of the ns orbital

A

the orbital gets larger

74
Q

in a boundary surface, or contour representation, around what % of the chance of finding an e- is represented?

A

90

75
Q

what is the overall shape of a p orbital

A

a dumbell

76
Q

is the boundary of an orbital representation the most likely place to find an e-

A

NOOO, the nucleus is most likely

77
Q

what is a radial node

A

distance from the nucleus at which no e- density is found

78
Q

how to find amount of radial nodes

A

(n-l)-1

79
Q

in Shrodingers equation, whats the only kind of atom that it can be solved for, why

A

hydrogen, because 1 e- systems are unique and can be solved for exactly

80
Q

in a hydrogen atom, what does it mean if atomic orbitals within a shell with the same “n” are degenerate

A

they have the same energy

81
Q

Describe Pauli exclusion principle

A

no two electrons can have the same spin in an orbital, one goes up and one goes down

82
Q

describe hunds rules

A

an electron will go into each orbital once with parallel spins before filling up an orbital with a second e-

83
Q

describe Aufbaus principle

A

e- occupy atomic orbitals in order of increasing energy with no more than 2 e- in a single orbital.

84
Q

what is the arrangement of e- in the orbitals of an atom

A

electronic configuration

85
Q

what is a paired e-

A

same orbital w opposite spins

86
Q

what are core e-

A

electrons in an element with full shells before the valance e-

87
Q

what are valance e-

A

e- on the outer shell

88
Q

how many core e- in Al

A

10

89
Q

how many valance e- in Al

A

3

90
Q

what are the exceptions to a normal electron configuration

A

(3-4)d4 or (3-4)d9 elements

91
Q

what is the electron configuration of Cr

A

[Ar] 4s^1 3d^5

92
Q

group name of Nitrogen group?

A

pnictogens

93
Q

group name of Oxygen group

A

Chalogens

94
Q

which group isn’t a transition metal in the d block

A

zinc group

95
Q

what is a requirement to be a transition metal

A

a partially filled d orbital

96
Q

which side of the periodic table are metals on?

A

left

97
Q

which quantum numbers describe an orbital

A

(n,l,m(l))

98
Q

which quantum numbers describe an e-

A

(n,l,m(l),m(s))

99
Q

if n decreases, what does size and and energy of an s orbital do?

A

decrease

100
Q

if n decreases, what does size and and energy of an p, d, or f orbital do?

A

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college chem 117 (7 decks)

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