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Chapter 5 Electrons

Total questions: 57

Worksheet time: 55mins

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.
 The electron configuration below represents a ground-state atom of which element? 
1s2 2s2 2p6 3s2 3p4
a)
a. Se
b)
b. O
c)
c. S
d)
d. Si
14.
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
15.
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
16.
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.
17.
How many degenerate orbitals does the f level have?
a)
a. 1
b)
b. 3
c)
c. 5
d)
d. 7
18.
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
19.

the height of a wave from the origin to a crest, or from the origin to a trough

a)

amplitude

b)

frequency

c)

wavelength

d)

crest

20.

a set of frequencies of electromagnetic waves given off by atoms of an element; consists of a series of fine lines of individual colors

a)

atomic orbital

b)

atomic emission spectrum

c)

de Broglie equation

d)

electromagnetic radiation

21.

a three-dimensional region around the nucleus of an atom that describes an electron's probable location

a)

atomic emission spectrum

b)

aufbau principle

c)

atomic orbital

d)

electromagnetic radiation

22.

states that each electron occupies the lowest energy orbital available

a)

de Broglie equation

b)

electron configuration

c)

electron-dot structure

d)

aufbau principle

23.

predicts that all moving particles have wave characteristics and relates each particle's wavelength to its frequency, its mass, and Planck's constant

a)

de Broglie equation

b)

electron configuration

c)

Heisenberg uncertainty principle

d)

Pauli exclusion principle

24.

a form of energy exhibiting wavelike behavior as it travels through space; can be described by wavelength, frequency, amplitude, and speed

a)

atomic emission spectrum

b)

electromagnetic radiation

c)

atomic orbital

d)

electromagnetic spectrum

25.

includes all forms of electromagnetic radiation, with the only differences in the types of radiation being their frequencies and wavelengths

a)

atomic orbital

b)

atomic emission spectrum

c)

electromagnetic spectrum

d)

photoelectric effect

26.

the arrangement of electrons in an atom, which is prescribed by three rules--the Aufbau principle, the Pauli exclusion principle, and Hund's rule

a)

atomic orbital

b)

energy sublevels

c)

ground state

d)

electron configuration

27.

consists of an element's symbol, representing the atomic nucleus and inner-level electrons, that is surrounded by dots, representing the atom's valence electrons

a)

electron-dot structure

b)

photon

c)

principle energy levels

d)

quantum

28.

the energy levels contained within a principal energy level

a)

atomic orbital

b)

energy sublevels

c)

principal energy levels

d)

principal quantum number

29.

the number of waves that pass a given point per second

a)

wavelength

b)

amplitude

c)

frequency

d)

quantum number

30.

the lowest allowable energy state of an atom

a)

photoelectric effect

b)

photon

c)

principal energy levels

d)

ground state

31.

states that it is not possible to know precisely both the velocity and the position of a particle at the same time

a)

Heisenberg uncertainty principle

b)

Pauli exclusion principle

c)

Aufbau principle

d)

quantum mechanical model of the atom

32.
A region of space around the nucleus where an electron with a particular energy is likely to be found
a)
atomic orbital
b)
electron density
c)
principal energy level
d)
quantum
33.
A number that provides information about the energy level possessed by an electron around an atom
a)
principal quantum number
b)
orbital
c)
electron configuration
d)
orbital diagram
34.
This states that each orbital in an atom can hold at most 2 electrons, which must have opposite spins
a)
Pauli exclusion principle
b)
Hund's rule
c)
Aufbau principle
d)
quantum mechanical model
35.
This explains the properties of atoms by treating the electron as a wave and quantizing its energy
a)
quantum mechanical model
b)
Bohr's model
c)
plum-pudding model
d)
Rutherford's nuclear model
36.
The clockwise or counterclockwise motion of an electron
a)
electron spin
b)
quantum
c)
Hund's rule
d)
orbital
37.
This states that orbitals of equal energy are occupied by one electron each before any of those orbitals are occupied by a second electron (split 'em up before you pair 'em up)
a)
Hund's rule
b)
Pauli exclusion principle
c)
Aufbau principle
d)
quantum mechanical model
38.
Describes the most stable arrangement of electrons around the nucleus of an atom, using superscripts with sublevels
a)
electron configuration
b)
orbital diagram
c)
Bohr model of the atom
d)
quantum
39.
This says that electrons enter orbitals of lowest energy first
a)
Aufbau principle
b)
Hund's rule
c)
Pauli exclusion principle
40.
The amount of energy required to move an electron from its present energy level to the next higher one
a)
quantum
b)
orbital
c)
energy level
d)
photon
41.
A particle of light
a)
photon
b)
quantum
c)
electromagnetic radiation
d)
wave
42.

Write the electronic configuration for sodium Na (Z=11)

a)

1s2 2s2 2p6

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s1

d)

1s2 2s2 2p6 3s2 3p4

43.

State the valence electronic configuration for Mg (Z=12)

a)

3s2

b)

3s2 3p1

c)

3s2 3p3

d)

3s2 3p4

44.

Determine the element that has valence electron 3s23p1

a)

Na

b)

Al

c)

Cl

d)

Mg

45.

Which of the orbital is call 'dumbell shaped'

a)

s

b)

p

c)

d

d)

f

46.

Write the set quantum number for 3p.

a)

(3, 0, 0, +1/2)

b)

(3, 1, 0, +1/2)

c)

(3, 2, 0, +1/2)

d)

(3, 0, 1, +1/2)

47.

Which of the following element has this orbital in its electronic configuration.

a)

Ar (Z=18)

b)

K (Z=19)

c)

Ca (Z=20)

d)

Sc (Z=21)

48.

How many unpaired electron of electronic configuration for Sulphur, S (Z=16)

a)

1

b)

2

c)

3

d)

4

49.

What is the symbol for angular quantum number?

a)

n

b)

l

c)

m

d)

s

50.

How many electrons if l=1 for electronic configuration of Mg (Z=12)

a)

12

b)

6

c)

3

d)

2

51.

Electron must be arrange from lowest energy to highest energy.

State the rule/principle?

a)

Hund's Rule

b)

Pauli Exclusion Principle

c)

Aufbau Principle

d)

Zuhaizi Principle

52.
What is this element?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
53.
What is this element?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
54.
How many electrons can the first energy level hold?
a)
1
b)
2
c)
8
d)
0
55.
How many electrons can the d sublevel hold?
a)
8
b)
10
c)
2
d)
4
56.
How many valence electrons does Si contain? (click to see image)
a)
14
b)
28
c)
2
d)
4
57.
An orbital can at most hold how many electrons?
a)
1 electron
b)
2 electrons
c)
3 electrons
d)
4 electrons

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