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Chemistry ch. 4 Electron Configuration - VANN Flashcards | StudBud
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Chemistry ch. 4 Electron Configuration - VANN
Chemistry ch. 4 Electron Configuration - VANN
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Electron Configuration
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Answers
1
According the Aufbau Principle
electrons fill low energy orbitals first
electrons must have opposite spins in the same orbital
electrons fill orbitals strictly in order by shell number
electrons fill high energy orbitals first
2
What is the maximum number of electrons that can fit in the "d" subshell?
2
14
6
10
3
Using the line-emission spectra, what 2 gases are in the unknown mixture?
Gas B & C
Gas A & C
Gas B & D
Gas A & B
4
How many total electrons can a d sublevel accommodate?
14
2
10
6
5
Filling in 1s
2
prior to 2s
2
relates to which rule or principle?
Pauli Exclusion
Hund's
Aufbau
Bohr
6
An electron found in a 2p suborbital will have _______ energy than an electron in 3p.
the same
less
greater potential
more
7
What is the highest energy level shown on the periodic table?
4
7
9
6
8
How many possible orientations exist with p orbitals?
7
3
5
1
9
What is the maximum number of electrons that can fit in the "s" subshell?
2
6
14
10
10
How many electrons does arsenic (As) have in its 4th energy level?
15
3
5
6
11
Two electrons in the same orbital must have
opposing viewpoints
opposite spins
the same quantum numbers
the same direction of spin
12
Which element has the following electron configuration?
silver
copper
zinc
gallium
13
What is the electron configuration of nitrogen?
1s2 2s5
1s2 2s3 2p2
1s2 2s2 2p3
2s2 2p3 3s2
14
the frequency of any electromagnetic radiation is�
directly proportional to its wavelength.�
inversely proportional to is energy
equal to its wavelength.�
inversely proportional to its wavelength
15
What element is represented by the following orbital notation?
oxygen
nitrogen
carbon
fluorine
16
Electrons moving in clockwise and counterclockwise directions indicates the
spin quantum number
magnetic quantum number
principal quantum number
angular momentum quantum number
17
Which element is represented by the following orbital notation?
S (sulfur)
F (fluorine)
Cl (chlorine)
O (oxygen)
18
All elements ALWAYS fill up orbitals exactly the same way without any exceptions.�
True
False
19
All noble gases (except Helium) have electron configurations ending in
s6
p8
s2
p6
20
How many TOTAL orbitals are there in energy level 2?
2
4
1
3
21
What is the correct noble gas configuration for Niobium (atomic #41)?
[Kr] 5s25d3
[Kr] 3d10 4s2 4p6
[Kr] 5s2 4d3
[Ar] 3s10 4s2 4p6 5s2 4d3
22
Which element is 1s
2
2s
2
2p
2
?
helium
carbon
nitrogen
boron
23
According to the Pauli Exclusion Principle
Only two electrons are allowed per orbital
Electrons' locations are unknown
Electrons must have parallel spins
Only one electron is allowed per orbital
24
What is the correct noble gas configuration for nickel (Ni)?
[Ca] 4d8
[Kr] 4s2 3d8
[Ar] 4s1 3d9
[Ar] 4s2 3d8
25
Units of frequency
minute
1/s
seconds
Columbs
26
What element is represented by the orbital notation?
krypton
neon
chlorine
argon
27
[Ar]4s
2
3d
10
4p
6
is the electron configuration for
Bromine
None of the above
Krypton
Rubidium
28
The number of electrons in a neutral atom of oxygen is
8
16
15.999
6
29
Quantum number representing the main energy level.
principal quantum number
spin quantum number
magnetic quantum number
angular momentum number
30
Radio waves, gamma waves, light waves, and ultraviolet waves all have the same _________.
energy
wavelength
speed
frequency
31
Which element has 3 unpaired up arrows in its p sublevel?
aluminum
scandium
nitrogen
argon
32
What is the electron configuration of iron?
1s2 2s2 2p33s23p64d8
1s2 2s2 2p63s23p64s23d6
1s2 2s2 2p6 3s2 3p6 4s2 4d6
[Ar]1s22s23s23d2
33
The lowest energy level is ___________ state but the highest energy level is the _______ state.
ground; excited
neutral; charged
neutral; excited
absorbed; emission
34
Who said it's impossible to know an electron's exact location and velocity at the same time?
Dalton
Schrodinger
Bohr
Heisenberg
35
An orbital can hold _____ electrons.
1
2
8
18
36
All elements in group 15 have an electron configuration ending in
p5
s2
p6
p3
37
The type of electron distribution diagram shown for the element is called
molecular orbitals
orbital notation
noble gas configuration
electron configuration
38
All elements in group 1 have electron configurations that end in
s1
p1
s2
d2
39
What is the maximum number of electrons that can fit in an orbital?
3
1
2
4
40
Which of the following is an impossible electron configuration?
1s2 2s22p63s23p63d5
1s2 2s22p53s23p5
1s2 2s22p63s23p6
1s2 2s22p62d103s23p6
41
The following would best be described as a
p orbital
s orbital
four leaf clover
d orbital
42
A 3D region in space where an electron is likely to be found is called
an orbital
an electron spin
an orbit
an energy level
43
Using the diagram below, which move EMITS the SMALLEST amount of energy?
E3 to E1
E5 to E1
E3 to E2
E6 to E1
44
What are two exceptions to the general electron configuration rules?
Cu and Cl
Cu and Cr
Ca and Ag
Cl and Fe
45
What are the four sub levels called?
f,d,p,s
s,p,c,f
s,d,k,l
s,p,d,r
46
How many unpaired electrons does magnesium (Mg) have in its orbital notation?
0
8
1
2
47
The equation E = hν helped Louis de Broglie determine�
how electron wave frequencies relate to specific energies.�
how protons and neutrons behave in the nucleus.�
Electrons exist in a limited number of orbits.�
whether electrons behave as particles.�
48
What neutral element has the electron configuration of 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
4p
2
?
As
Ga
Zn
Ge
49
What is the maximum number of electrons that can fit in the "p" subshell?
14
2
6
10
50
What is the formula for determining the maximum number of electrons in a
energy level (shell)
?
n2/2
2n2
E=hv
1n2
51
The order in which energy sublevels are filled is determined by
Aufbau's Principle
Hund's Rule
Paulie Exclusion Principle
Quantum Theory
52
Electromagnetic radiation A has a shorter wavelength than B so the frequency of A is�_______.
higher than <br>B
cannot be determined without values
the same as B
lower than B
53
As a deviation to the rules, what is the correct ground state electron configuration of Cu?
1s2 2s2 2p6 3s2 3p6 3d6 4s2 4p3
1s2 2s2 2p6 3s2 3p6 3d9 4s2
1s2 2s2 2p6 3s2 3p6 3d10 4s1
1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 5p1
54
Which orbital type only has one possible orientation?
f orbital
s orbital
p orbital
d orbital
55
Where are the valence electrons located?
All electrons are valence electrons
In the outer energy level
In the nucleus
inner shells
56
How many orbitals are in the highest principal energy level of Chlorine?
2
3
5
4
57
What orbital is represented by the following shape?
d
p
f
s
58
Which orbital could never exists?
6d
2f
3d
8s
59
Element in excited state with electron configuration 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
4p
6
5s
1
4d
10
5p
6
?
Iodine
Xenon
Bromine
Tellurium
60
Quantum number for the orientation of an orbital about the three axes in space i.e. p
x
p
y
&p
z
angular momentum quantum number.�
spin quantum number.�
magnetic quantum number.�
principal quantum number.�
61
Which of the following is not a unit of frequency?
1/s
s-1
second
Hertz
62
According to Hund's Rule
Electrons never have parallel spin
Electrons must have parallel spin, if possible
electrons fill in lower energy levels first
Orbitals must fill before moving to orbital in same sublevel
63
What is the maximum number of
orbitals
that can fit in the "f" subshell?
7
1
3
5
64
Who developed mathematical expressions predicting the probable location of electrons?
Linus Pauling
Aufbau
Hund
Schrodinger
65
The emission of electrons from metals that have absorbed photons is called the�
photoelectric effect
photosynthesis
absorption
ground state
66
Which element has the following orbital notation?
cesium
barium
radium
strontium
67
Which of these violates Bohr's theory that electrons must reside at specific energy levels?
C
D
B
A
68
How many unpaired electrons are in the orbital diagram for sulfur?
3
2
1
0
69
The angular momentum quantum number represents the _________________ of the orbital.
orientation
energy level
shape
spin
70
[Ne]3s
2
is the electron configuration for this element:
magnesium
sodium
neon
calcium
71
Having three up arrows in an orbital notation of a 3p subgroup would relate to __________?
Heisenberg's Uncertainty Principle
Aufbau Principle
Hund's Rule
Pauli Exclusion Principle
72
What is the maximum number of
orbitals
that can fit in the "p" subshell?
7
5
3
1
73
Which groups are in the p-block?
the elements below the main table
3 through 12
13 through 18
1 and 2
74
Which of the following is the ground-state configuration for the atoms of a transition element?
1s2 2s22p63s23p63d3 4s2
1s2 2s22p63s23p63d5
1s2 2s22p62d103s23p6
1s2 2s22p53s23p5
75
Higher freqencies correspond to ______________________.
less Hertz
higher energy
lower energy
longer wavelengths
76
Which orbitals can exist in energy level 3?
s, p, & d only
s only
s, p, d, and f
s and p only
77
What is the maximum number of electrons that can fit in the "f" subshell?
14
10
2
6
78
The rule where each p orbital receives one electron before any of them can have two electrons?�
the Pauli exclusion principle�
Hund's rule�
the quantum rule�
the Aufbau principle�
79
When an electron spins on its axis, it generates
an unhappy hog
an electrostatic array
a magnetic field
a solar flare
80
What neutral element has the electron configuration of 1s
2
2s
2
2p
6
3s
2
3p
6
4s
2
3d
10
4p
6
?
Ar
Xe
Kr
Br
