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Chemistry, Chapter 5, Electron Configuration Review Flashcards | StudBud
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Chemistry, Chapter 5, Electron Configuration Review
Chemistry, Chapter 5, Electron Configuration Review
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Electron Configuration Quiz, Chapter 5
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Answers
1
Which of the following sets of quantum numbers cannot exist?
n=3, l=3, ml=0, ms=-½
n=2, l=0, ml=0, ms=-½
n=4, l=3, ml=-2, ms=½
n=3, l=2, ml=0, ms=½
2
Using the equations c=𝛌v and E=hv, when frequency increases, what happens to planks constant?
it increases
it does not change
we can't figure that out with this information
it decreases
3
According to the aufbau principle, ____.
an orbital may be occupied by only two electrons
electrons enter orbitals of highest energy first
electrons enter orbitals of lowest energy first
electrons in the same orbital must have opposite spins
4
Using the equations c=𝛌v and E=hv, when frequency increases, what happens to frequency?
it decreases
it does not change
we can't figure that out with this information
it increases
5
What is the wavelength: frequency of 60 MHz and speed 3 x 10
8
m/s? (1 MHz = 1,000,000 Hz)
60 MHz ´ 300,000,000 m/s
60,000,000 hz/300,000,000
not enough information
300,000,000/60,000,000 hz
6
A wave has a frequency of 100 Hz and a wavelength of 5 m. What is the speed of the wave?
5 m/s
500 m/s
5000 m/s
50 m/s
7
Stable electron configurations are likely to contain ____.
electrons with a clockwise spin
fewer electrons than unstable configurations
unfilled s orbitals
filled energy sublevels
8
What is an ion?
atoms with an overall neutral charge
an atom that creates a new substance every time
atoms that become charged through the gain/loss of electrons
an atom that has the ability to change its charges
9
The quantum theory.
describes the physical properties of nature at small scales
determines that the laws of physics are the same for non-accelerating thing
that the Earth's solid outer crust, the lithosphere, is separated in plates
energy cannot be created or destroyed
10
How does the energy of an electron change when the electron moves closer to the nucleus?
It stays the same.
It decreases.
It doubles.
It increases.
11
What types of atomic orbitals are in the third principal energy level?
s and p only
s, p, and d only
s, p, d, and f
p and d only
12
ionization energy
required to remove one electron
required to remove three electron
required to remove four electron
required to remove two electron
13
To calculate the frequency of a wave, you need to know the speed of the wave and its
color
wavelength
frequency
intensity.
14
If 3 electrons fill three 2
p
orbitals, how will electrons be distributed in the 3 orbitals?
one electron in each orbital
2 electrons in 1 orbital, one in another, none in the third
Three electrons cannot fill three empty 2p atomic orbitals.
three in one orbital, none in the other two
15
In Bohr's model of the atom, where are the electrons and protons located?
Electrons and protons are throughout atom, but aren't free
Electrons are in fixed spots around protons
Electrons move around protons, which are at center of atom.
The electrons and protons move throughout the atom.
16
What is the electron configuration of potassium?
1s2s2p3s3p4s
1s2s2p3s3p
1s2s2p3s3p4s
1s2s3s3p3d
17
Difference between absorption spectra and emission spectra?
absorption appear as bright lines
Absorption has electrons losing energy
Emission involves electrons increasing energy.
Emission bright lines. Absorption dark lines
18
What is the maximum number of orbitals in the
p
sublevel?
3
2
4
5
19
The quantum numbers (4,1,0,+1/2) correspond to:
Nb
Ge
Sn
Br
20
If a wave has a speed of 10m/s and a frequency of 2 Hz, what is the wavelength?
2 m
12 m
20 m
0.2 m
21
Which of the following sets of quantum numbers would not occur?
n=1, l=0, ml=0, ms= -1/2
n=3, l=0, ml=0, ms=+1/2
n=7, l=1, ml=1, ms= -1/2
n=4, l=2, ml =-3, ms= +1/2
22
Which orbital does Scandium fall under?
3d
3b
4s
4d
23
Which of the following electron configurations of outer sublevels is the most stable?
4d25s4
4d55s1
4d35s3
4d45s2
24
Select the shape that represents a 'p orbital'
Shell
Dumbbell
Sphere
Clover leaf
25
Bohr's model is not complete because...
It can't explain sodium
Couldn't expl. why some orbits are allowed and others not.
none of these
It only works for Hydrogen.
26
What type of orbital is defined by the quantum numbers 4 2 1
4d
4s
4f
4p
27
Who predicted that all matter can behave as waves as well as particles?
Louis de Broglie
Erwin Schrodinger
Max Planck
Albert Einstein
28
How many electrons can the p orbital hold?
One
Four
Six
Two
29
Which type of electromagnetic radiation includes the wavelength 10 m?
gamma ray
visible light
radio wave
microwave
30
Which element has a smaller atomic size?
Sulfur
Tellurium
31
What is the shortcut electron configuration for Scandium?
[Ar] 4s3
[K] 4s13d1
[Ar] 3d1 4s2
[K] 4s2
32
How many energy sublevels are in the second principal energy level?
18
3
1
2
33
Which electron is represented by the quantum numbers 4,2,2,1/2?
4f5
4d5
4d10
4p4
34
Ground state of highest-energy electron of rubidium atom can have which quantum numbers?
n=4; l=0; ml = 0; ms=+1/2
n=5; l=1; ml = 1; ms=+1/2
n=5; l=1; ml = 0; ms=+1/2
n=5; l=0; ml = 1; ms=+1/2
35
The four quantum numbers are, in order:
{n, l, ml, mn}
{n, l, m, s}
{n, ml, l, ms}
{n, l, ml, ms}
36
What family does the element with the following set of quantum numbers belong to? 3;0;0;-1/2
alkali metals
alkaline earth metals
transition metals
halogens
37
As frequency of a wave _________, wavelength decreases.
moves
decreases
increases
equalizes
38
Choose the orbital shape of the s sublevel?
spherical
squared
L shaped
dumbbell
39
What is the wavelength of a wave at 3 x 10
8
m/s withfrequency of 60 MHz? (1 MHz = 1,000,000 Hz)
60 MHz ´ 300,000,000 m/s
60,000,000 hz/300,000,000
No answer can be determined from the information given.
300,000,000/60,000,000 hz
40
Which of the following electromagnetic waves have the highest frequencies?
microwaves
X-rays
gamma rays
ultraviolet light waves
41
How many
unpaired
electrons are in a sulfur atom (atomic number 16)?
0
1
2
3
42
What element has this specific quantum number?
Sulfur
Silicon
Not a valid Quantum Number
Chlorine
43
What happens to the size of atomic radi across a period?
They decrease
Nothing
They increase
they explode
44
As atomic radius increases, ionization energy___
Decreases
Increases
Remains he same
45
If a wave has a speed of 100m/s and a wavelength of 10 m, what is the frequency?
10 Hz
0.1 m
110 m
110 Hz
46
Which of the following sets of quantum numbers represents the highest energy of an atom?
n = 4, l = 0,m = 0, s = +1/ 2
n = 3, l = 0,m = 0, s = +1/ 2
n = 3, l = 1,m = 1, s = +1/ 2
n = 3, l = 2,m = 1, s = +1/ 2
47
What is Planck's Constant?
6.626 x 1034 Js
3.0 x 10-8 mHz
6.626 x 10-34 Js
3.0 x 108 mHz
48
What are the four quantum numbers?
energy level, angular momentum, atomic mass, spin
energy level, angular momentum, magnetic, spin
magnet, isotope, protons, neutrons
atomic number, angle, spin, magnet
49
What is the maximum number of electrons in the second principal energy level?
32
2
18
8
50
What is the next atomic orbital in the series 1
s
, 2
s
, 2
p
, 3
s
, 3
p
?
4s
3f
3d
2d
51
What is the (l) quantum number of the d orbital?
1
2
3
0
52
The electron configuration of the phosphide ion(P3-) is
[Ne]3s2 3p6
[Ne]3s2 3p3
[Ne]3s2 3p1
[Ne]3s2
53
If the spin of one electron is clockwise, what is the spin of the other electron?
counterclockwise
both clockwise and counterclockwise
clockwise
zero
54
0 belong to which set of numbers?
Irrational
All
Natural
Whole
55
Which of the quantum leaps would be associated with the greatest energy of emitted light?
n = 4 to n = 5
n = 5 to n = 1
n = 5 to n = 4
n = 2 to n = 5
56
The emission spectra of a sodium atom on Earth and a sodium atom in the sun would be ____.
different from each other
the same as each other only in the ultraviolet range
the same
the same as those of several other elements
57
What is the maximum number of
f
orbitals in any single energy level in an atom?
1
3
7
5
58
What is the number of electrons in the outermost energy level of an oxygen atom?
8
2
6
4
59
What does the angular momentum quantum number identify?
energy level
orbital shape
orientation
spin
60
How does the speed of visible light compare with speed of gamma rays, in a vacuum?
The speed of visible light is greater.
The speeds are the same.
No answer can be determined from the information given.
The speed of gamma rays is greater.
61
What is the total spin quantum number for a neutral boron
2
1/2
1
7
62
How can we find speed of the wave?
wavelength x frequency
speed / frequency
frequency / wavelength
wavelength / frequency
63
How many half-filled orbitals are in a bromine atom?
3
1
4
2
64
The quantum numbers tell us:
The size of the atom
The EMR of the electron
The location of the electron
The wavelength of light
65
How are the frequency and wavelength of light related?
They are inversely proportional to each other.
Wavelength is found by dividing frequency by speed of light.
Frequency equals wavelength divided by the speed of light.
They are directly proportional to each other.
66
The principal quantum number indicates what property of an electron?
energy level
speed
electron cloud shape
position
67
Which element has the highest ionization energy
O
Cn
Sr
Cl
68
What is the approximate frequency of a photon with an energy 5 x 10
-24
J? (
h
= 6.6 x 10
-34
Js)
8 x 109 Hz
3 x 10-58 Hz
3 x 10-57 Hz
1 x 10-10 Hz
69
As changes in energy levels increase, the frequencies of atomic line spectra they emit ____.
cannot be determined
increase
decrease
remain the same
70
This picture is what orbital?
s
p
f
d
71
When an electron moves from a lower to a higher energy level, the electron ____.
absorbs a quantum of energy
moves closer to the nucleus
always doubles its energy
absorbs a continuously variable amount of energy
72
An orbital that could never exist any time is:
3d
6d
8s
3f
73
What is the approximate energy of a photon with a frequency of 4 x 10
7
Hz? (
h
= 6.6 x 10
-34
Js)
3 x 10-26 J
2 x 10-41 J
3 x 1042 J
3 x 10-27 J
74
Which of the following set of quantum numbers belong to highest energy?
n = 2, l = 1, m = 1, s = + 1/2
n = 3, l = 0, m = 0, s = + 1/2
n = 4, l = 0, m = 0, s = + 1/2
n = 3, l = 2, m = 1, s = + 1/2
75
Emissionand absorption spectra provide evidence for
A
B
D
C
76
The quantum numbers for Zirconium (40 electrons)
5,2,-1,+1/2
4,2,-1,+1/2
5,2,-2,-1/2
4,2,-2,-1/2
77
Emission of light from an atom occurs when an electron ____.
falls into the nucleus
jumps from a lower to a higher energy level
drops from a higher to a lower energy level
moves within its atomic orbital
78
How many configurations, or sub-levels, can an d orbital have?
1
7
5
3
79
What is the basis for exceptions to the aufbau diagram?
Some elements have unusual atomic orbitals.
Electron spins are more important than energy levels
Electron configurations are only probable.
Full/half-full sublevels are more stable than part-full
80
Which color of visible light has the shortest wavelength?
yellow
violet
blue
green
81
Which element is identified by the quantum numbers (3, 2, 2, -1/2) ?
zinc
nickel
manganese
iron
82
Does Sodium or Oxygen have a higher ionization energy?
Sodium
Oxygen
yes
Neither
83
What is the maximum number of
d
orbitals in a principal energy level?
1
2
3
5
84
This picture is what orbital?
s
p
f
d
85
Which electron configuration of the 4
f
energy sublevel is the most stable?
4f 14
4f 7
4f 13
4f
86
How many electrons can fit in an d orbital?
6
18
10
8
87
What elemenet has an electron configuration of 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
9
?
Silver
Copper
Zinc
Nickel
88
What element has this specific quantum number?
Sulfur
Not a valid Quantum Number
Chlorine
Silicon
