midterm exam 1 Flashcards
(100 cards)
1
Q
what unit is used for average atomic weight
A
Dalton (Da)
2
Q
although avagrados number works for all elements, what element is the number based off of
A
Carbon - 12
3
Q
units of molar mass
A
g/mol
4
Q
how many atoms are there in 3 moles O2
A
36.12 * 10^23 atoms
5
Q
how many atoms are there in 3 moles of O
A
18.09 * 10^23 atoms
6
Q
what is the definition for mole regarding avogrados number
A
a collection of avogrados number of atoms is a mole of atoms
7
Q
what is matter
A
anything that occupies space and has mass
8
Q
what determines the properties of matter
A
the structure of particles
9
Q
what is the smallest unit of an element
A
an atom
10
Q
what is a substance that can’t be broken into a simpler substance by any means
A
element
11
Q
what is the mass of protons and neutrons
A
1.67262 * 10^-24
12
Q
what is the mass of an electron
A
9.10936 * 10^-28
13
Q
why aren’t atomic masses whole numbers
A
they are the averages of all known isotopes weights
14
Q
Peta (size, symbol)
A
10^15, P
15
Q
Tera (size, symbol)
A
10^12, T
16
Q
Giga (size, symbol)
A
10^9, G
17
Q
Mega (size, symbol)
A
10^6, M
18
Q
Kilo (size, symbol)
A
10^3, K
19
Q
Deci (size, symbol)
A
10^-1, d
20
Q
Centi (size, symbol)
A
10^-2, c
21
Q
Milli (size, symbol)
A
10^-3, m
22
Q
Micro (size, symbol)
A
10^-6, μ
23
Q
Nano (size, symbol)
A
10^-9, n
24
Q
Pico (size, symbol)
A
10^-12, p
25
Femto (size, symbol)
10^-15, f
26
Atto (size, symbol)
10^-18, a
27
what are the two waves light consists of
magnetic (red) and electric (blue)
28
light is an electromagnetic _____ phenomenon, consisting of oscillating ________________ through space.
wave, electric and magnetic fields
29
what can light act as
a wave and a particle
30
all types of of electromagnetic waves travel with the same _____, what is it?
velocity, speed of light 2.88 * 10^8 m/s
31
how are frequency and wavelength related? explain
inversely, if wavelength goes up the frequency goes down
32
what does hertz stand for
per second
33
how are frequency and energy related? explain
parallel, when frequency goes up, the energy goes up
34
what is it called when light is acting as stream of particles
photon
35
when a photon interacts with an electron, how much energy does it transfer to the electron
ALL OF IT
36
define wave-particle dualality
behaves like a wave and particle at same time
37
how many photons can interact with an electron at a time
only one
38
describe a discrete interaction when energy is quantized, give example
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
39
whats an eV, whats it equal to
amount of energy gained by an electron falling through an electric potential drop of one volt, 1.6 * 10^-19 J
40
all matter is _______ a wave and a particle
simultaneously
41
how do atomic particles emulate light
they act as waves and particles
42
what is linear momentum
the product of mass and speed (mv)
43
why is matter, like electromagnetic radiation, thought of as quantized?
you can't make a wave w 2.58 wavelengths, it has to be whole integer
44
both matter and electromagnetic radiation have _____ and ______ properties, and their energies are _______
wave, particle, quantized
45
what is the most important factor in determining properties of electrons
their wave nature
46
if an electron or particle is acting as a wave, can we precisely determine the location
no
47
do electrons satellite the nucleus like planets
NOOOOO
48
What is Heisenbergs uncertainty principle
both position and momentum cannot be known simultaneously
49
what is schrodingers equation represent
it describes an electron as a wave
50
what do wavefunctions, ψ, specify
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
how is an orbital defined
by wave functions and the wave nature of an e-
52
can wave functions specify the precise location of a function?
NOOO
53
what makes up a full set of quantum numbers
(n,l,m(l),m(s))
54
in quantum numbers, whats the definition of "n", possible values, and what does it effect
the principal quantum number, (n= 1,2,3,4,5,6,7), defines the size and energy of an atomic orbital
55
in quantum numbers, whats the definition of "l", possible values, and what does it effect
the angular momentum quantum number, (s=0, p=1, d=2, f=3), defines the shape in 3 space
56
in quantum numbers, whats the definition of "m(l)", possible values, and what does it effect
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
what is a collection of orbitals with the same principle quantum number
electron shell
58
what is the collection of orbitals that have the same n and l value
sub shell
59
how many atomic orbitals does each element have
an infinite number
60
what is probability density, and whats the symbol
the probability of finding the electron in the small region of space divided by the volume of that region of space, ψ
61
besides probability density, what can wave functions define
the energy of an electron in a particular atomic orbital
62
what defines an atomic orbital
quantum numbers
63
the energies of all orbitals within a shell have (same or different) energies?
SAME
64
does an electron have more energy in the nucleus or far from the nucleus?
far from the nucleus
65
what is a free e-
an electron not in the nucleus
66
why is the energy of an e- in an atomic orbital negative
it is lower in energy than a free e-
67
in an orbital, where are you most likely to find an e-
near the nucleus
68
what does it mean that an s orbital is spherically symmetrical
it doesn't matter what direction you go, the probability of finding an e- is based of only distance from nucleus
69
what are peaks in a radial probability function based off of
n
70
what does the peak w the highest probability correspond to in a radial probability function
the distance from the nucleus where an e- is MOST likely to be found
71
what is a node
a place where there is NO probability of finding an electron
72
how do you find the number of nodes
n-1
73
when n increases, what happens to the size of the ns orbital
the orbital gets larger
74
in a boundary surface, or contour representation, around what % of the chance of finding an e- is represented?
90
75
what is the overall shape of a p orbital
a dumbell
76
is the boundary of an orbital representation the most likely place to find an e-
NOOO, the nucleus is most likely
77
what is a radial node
distance from the nucleus at which no e- density is found
78
how to find amount of radial nodes
(n-l)-1
79
in Shrodingers equation, whats the only kind of atom that it can be solved for, why
hydrogen, because 1 e- systems are unique and can be solved for exactly
80
in a hydrogen atom, what does it mean if atomic orbitals within a shell with the same "n" are degenerate
they have the same energy
81
Describe Pauli exclusion principle
no two electrons can have the same spin in an orbital, one goes up and one goes down
82
describe hunds rules
an electron will go into each orbital once with parallel spins before filling up an orbital with a second e-
83
describe Aufbaus principle
e- occupy atomic orbitals in order of increasing energy with no more than 2 e- in a single orbital.
84
what is the arrangement of e- in the orbitals of an atom
electronic configuration
85
what is a paired e-
same orbital w opposite spins
86
what are core e-
electrons in an element with full shells before the valance e-
87
what are valance e-
e- on the outer shell
88
how many core e- in Al
10
89
how many valance e- in Al
3
90
what are the exceptions to a normal electron configuration
(3-4)d4 or (3-4)d9 elements
91
what is the electron configuration of Cr
[Ar] 4s^1 3d^5
92
group name of Nitrogen group?
pnictogens
93
group name of Oxygen group
Chalogens
94
which group isn't a transition metal in the d block
zinc group
95
what is a requirement to be a transition metal
a partially filled d orbital
96
which side of the periodic table are metals on?
left
97
which quantum numbers describe an orbital
(n,l,m(l))
98
which quantum numbers describe an e-
(n,l,m(l),m(s))
99
if n decreases, what does size and and energy of an s orbital do?
decrease
100
if n decreases, what does size and and energy of an p, d, or f orbital do?
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