WorksheetsChapter 4: Electron Configuration
Total questions: 20
Worksheet time: 11mins
Name
Class
Date
1.
The diagram above represents two electrons with
a)
a. opposite spins.
b)
b. the same spin.
c)
c. different energies.
d)
d. different energy levels.
2.
The electron configuration above violates
a)
a. the Pauli exclusion principle.
b)
b. the Aufbau principle.
c)
c. Hund’s rule.
d)
d. None of the above
3.
A photon is emitted from a gaseous atom when an electron moves to its ground state from a(n)
a)
a. inner shell.
b)
b. excited state.
c)
c. n=0 state.
d)
d. less energetic state.
4.
What is the frequency of light whose wavelength is 633 nm?
a)
a. 4.74 x 104 Hz
b)
b. 4.74 x 102 Hz
c)
c. 4.74 x 1014 Hz
d)
d. 4.74 x 1016 Hz
5.
What is the frequency of a photon whose energy is 3.4 x 10-19 J? (h = 6.626 x 10-34 J·s)
a)
a. 8.8 x 1026 Hz
b)
b. 5.1 x 1014 Hz
c)
c. 1.9 x 10-15 Hz
d)
d. 2.3 x 10-52 Hz
6.
What is the correct electron configuration for a ground-state atom with 7 electrons?
a)
a. 1s2 2s2 2p3
b)
b. 1s2 2s2 2p2 3s1
c)
c. 1s2 2s3 2p2
d)
d. 1s2 2s5
7.
What is the correct noble-gas notation for the electron configuration of an atom of chlorine?
a)
a. [Ar]3s2 3p5
b)
b. [Ne]3s2 3p4
c)
c. [Ar]3s2 3p4
d)
d. [Ne]3s2 3p5
8.
What is the atomic number of the element with the noble-gas notation [Kr]5s1 ?
a)
a. 35
b)
b. 36
c)
c. 37
d)
d. 38
9.
In which orbital(s) are all the inner-shell electrons located in an atom of magnesium that is in the ground state?
a)
a. 1s
b)
b. 1s, 2s
c)
c. 1s, 2s, 2p
d)
d. 1s, 2s, 2p, 3s
10.
Which of the following types of electromagnetic radiation has the lowest frequency?
a)
a. x-rays
b)
b. infrared
c)
c. UV
d)
d. microwaves
11.
The total number of orbitals that can exist at a given main energy level, n, is equal to
a)
a. n.
b)
b. 2n2 .
c)
c. n2 .
d)
d. n -1.
12.
How many possible values are there for the spin quantum number?
a)
a. 2
b)
b. 3
c)
c. 4
d)
d. 0
13.
How many possible orientations does an s orbital have?
a)
a. 1
b)
b. 3
c)
c. 5
d)
d. 7
14.
The electron configuration below represents a ground-state atom of which element?
1s2 2s2 2p6 3s2 3p4
1s2 2s2 2p6 3s2 3p4
a)
a. Se
b)
b. O
c)
c. S
d)
d. Si
15.
What is the total number of electrons needed to fill the fourth main energy level?
a)
a. 4
b)
b. 8
c)
c. 16
d)
d. 32
16.
Which of the following requires that each of the p orbitals at a particular level have one electron before any of them can have two electrons?
a)
a. Aufbau Principle
b)
b. Hund's Rule
c)
c. Pauli Exclusion Principle
d)
d. both a and c.
17.
Max Planck proposed that “hot” objects radiate energy in small, specific amounts called
a)
a. waves
b)
b. electrons
c)
e. hertz
d)
d. quanta
18.
What is the shape of the p orbital?
a)
a. spherical.
b)
b. dumbbell shaped.
c)
c. four-leaf clover shaped.
d)
d. none of the above.
19.
How many degenerate orbitals does the f level have?
a)
a. 1
b)
b. 3
c)
c. 5
d)
d. 7
20.
What rule states that an electron fills the lowest energy orbital first?
a)
a. Hund's Rule
b)
b. Pauli Exclusion Principle
c)
c. Aufbau Principle
d)
d. quantum theory
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