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Chapter 4 Review: Arrangement of Electrons in Atoms Flashcards | StudBud
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Chapter 4 Review: Arrangement of Electrons in Atoms
Chapter 4 Review: Arrangement of Electrons in Atoms
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1
How many TOTAL electrons can reside in the 4th energy level?
8
32
2
18
2
All orbitals of equal energy are occupied by 1 electron before any orbital is occupied by 2
Shrodinger's Model
Pauli Exclusion Principle
Hund's Rule
Aufbau principle
3
At which point can an electron NOT reside?
c
d
a
b
4
When you increase wavelength, what happens to the frequency?
frequency doubles
frequency increases
frequency decreases
frequency stays the same
5
What does the principal quantum number refer to?
main energy level of an electron
spin state of an electron
orientation of an orbital around the nucleus
shape of an orbital
6
A photon is emitted from an atom when an electron moves to its ground state from a(n)
less energetic state
inner shell
excited state
n=0 state
7
A single orbital can hold how many electrons?
2
4
3
1
8
What are the 2 possible spin states of an electron?
+1 or -1
+1/4 or -1/4
+1/2 or -1/2
+2 or -2
9
Just as light has a dual nature, so do electrons. They can behave as both: ____ & ______
wave & energized particle
wave & beam
electrons & protons
particle & proton
10
What is the lowest energy state than an electron can occupy?
elevated state
excited state
ground state
Ohio
11
What is a particle of light that has zero mass, but a quantum of energy?
neutron
ion
photon
proton
12
An orbital that would never exist in the quantum description of an atom is
3f
7s
6d
3d
13
The highlighted portion of the periodic table represents which block?
p block
f block
s block
d block
14
The highlighted portion of the periodic table represents which block?
p block
s block
f block
d block
15
The electron configuration below represents a ground state atom of which element?
Beryllium (Be)
Titanium (Ti)
Carbon (C)
Helium (He)
16
How many electrons are present in an atom of calcium that has the following electron config?
30
20
25
15
17
Compared with an electron for which
n
= 3, an electron for which
n
= 1 has
can't be determined
more energy
the same amount of energy
less energy
18
Which of the following electron movements emits the most energy?
a
c
b
d
19
Which states that it's impossible to determine both the speed & location of an electron at once
Heisenberg Uncertainty Principle
Aufbau Principle
Bohr's Rule
Hund's Rule
20
which of the following is not a quantum number?
magnetic quantum number
angular momentum quantum number
orbital quantum number
principal quantum number
21
how many electrons can a p sublevel contain?
2
6
10
14
22
The following electron configuration represents which element?
Argon (Ar)
sulfur (S)
magnesium (Mg)
Chromium (Cr)
23
According to the Aufbau principle, which of the following sublevels is lowest in energy?
4s
5s
4p
3d
24
What are the possible sublevels in an energy level of n=2
s
s, p, d
s, p, d, f
s, p
25
Which of the following states that no atoms can have the same set of quantum numbers?
Pauli Exclusion Principle
Hund's Rule
Bohr's Model
Heisenberg Uncertainty Principle
26
Quantum numbers are sets of numbers that
relate the energies of protons in the atomic nucleus.
specify properties of electrons.
are characteristic only of the hydrogen atom.
consist of multiples of two
27
The highlighted portion of the periodic table represents which block?
f block
s block
p block
d block
28
The highlighted portion of the periodic table represents which block?
f block
d block
s block
p block
29
In the following equation, what does c represent?
wavelength
speed of light
frequency
volume
30
What element is this the electron configuration for?
Silicon (Si)
Magnesium (Mg)
Germanium (Ge)
Titanium (Ti)
31
What shape is a p orbital?
complicated
clover
dumbell
spherical
32
Who proposed the Quantum Theory of the atom, showing orbitals within energy levels?
Aufbau
Bohr
Pauli
Schrodinger
33
What does the angular momentum quantum number refer to?
orientation of an orbital around the nucleus
main energy level of an electron
shape of an orbital
spin state of an electron
34
Which of the following states an electron will occupy the lowest energy orbital that it can
Aufbau Principle
Pauli Exclusion Principle
Heisenberg Uncertainty Principle
Bohr's Rule
