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Chem CH 4 - Arrangement of Electrons in Atoms

Total questions: 46

Worksheet time: 2hrs 37mins

Name
Class
Date
1.

In order to go from ground state to an excited state, an electron must

a)

emit energy

b)

absorb energy

c)

wiggle

2.

When an electron returns to ground state from an excited state, the atom will (a)  

Choose from the below words
emit energy
absorb energy
rotate
wiggle
3.

In which state does an electron have the least amount of energy?

a)

Excited state

b)

Ground state

c)

Orbital

d)

Bohr model

4.
Which elements are in the unknown sample?
a)
A and B
b)
B and C
c)
A and D
d)
B and D
5.
Why are line emission spectra of elements called "atomic fingerprints"?
a)
They are all the same
b)
They are all unique
c)
They are all similar
d)
They all contain colored light
6.

Flame tests can be used to identify an element. Each element emits characteristic waves of light when it is heated in a flame. What describes how the light is produced?

a)

Protons in the ground state lose energy and give off light.

b)

Protons in the ground state gain energy and are emitted from the nucleus, giving off light.

c)

Electrons in the ground state lose energy and move to an excited state, giving off light.

d)

Electrons in the ground state gain energy, move to an excited state, and give off light when they return to the ground state.

7.
How much of the electromagnetic spectrum is visible?
a)
All of it
b)
None of it
c)
Most of it
d)
Only a small part
8.
What is the frequency of UV light that has an energy of 2.39 × 10 -18 J? 
a)
2.32 x 109 Hz
b)
3.60 x 1015 Hz
c)
1.58 x 10-51 Hz
d)
3 x 108  m/s
9.
What is the energy of an X-ray with a frequency of 1.0 x 1017 Hz?
a)
6.63 x 10-34 J
b)
6.63 x 10-17 J
c)
1.51 x 1016 J
d)
1.51 x 10-16 J
10.

What is the typical units of measurement for the "E" in the following equation: 
Ephoton= h x v

a)
joules
b)
meters
c)
meters/seconds
d)
hertz
11.
What is the energy of light whose wavelength is 4.06 x 10-11 m? 
a)
2.69 x 10-44 J
b)
1.63 x 10-23 J
c)
4.90 x 10-15 J
d)
8.97 x 10-53 J
12.

The number of waves that pass a given point every second

a)

Frequency

b)

Wavelength

c)

Energy

d)

Electromagnetic Spectrum

13.

Broad range of radiation that carries energy as waves

a)

Frequency

b)

Wavelength

c)

Energy

d)

Electromagnetic Spectrum

14.

Which two variables of the electromagnetic spectrum have a direct relationship?

a)

Crests and trough

b)

energy and frequency

c)

wavelength and energy

d)

frequency and wavelength

15.

As wavelength increases: frequency,_____________ and energy ______________.

a)

Increases; decrease

b)

Increases; increases

c)

Decreases; decreases

d)

Decrease; increases

16.

What is the speed of light?

a)

3.0x108 ms

b)

3.0x108 m/s

c)

6.626x10-34 Js

d)

6.626x10-34 J/s

17.

The frequency of violet light is 7.5x1014 Hz. What is its wavelength?

a)

4.0x10-7 m

b)

4.0x107 m

c)

2.25x1023m

d)

2.25x1023 Hz

18.
When an atom has all of its electrons in the lowest energy orbitals available, the atom is  
a)
in ground state
b)
in excited state
c)
giving off light energy
d)
unstable
19.

Which principal energy level change by the electron of a

hydrogen atom will cause the greatest amount of energy to be absorbed?

a)

n = 2 to n = 4

b)

n = 2 to n = 5

c)

n = 4 to n = 2

d)

n = 5 to n = 2

20.
This is the _____ for helium.
a)
emission spectrum
b)
absorption spectrum
c)
continuous spectrum
d)
black body spectrum
21.
Which rule shows us that we have to add electrons singly to orbitals until each has one before we start pairing?
a)
Hund's Rule
b)
Pauli Exclusion
c)
Aufbau Principle
d)
Paschen Series
22.

The angular momentum quantum number (l), describe..

a)

energy level of electron.

b)

the orientation of the orbital in space.

c)

the shape of orbital.

d)

the behavior of electrons as spinning clockwise or anticlockwise in orbital.

23.
How many orbitals in the d subshell? 
a)
1
b)
7
c)
3
d)
5
24.

Which of the following is NOT a possible pair of quantum numbers?

a)

2p

b)

2d

c)

4p

d)

4f

25.

Identify the element (symbol only) with the electron configuration

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f9

a)

Tb

b)

V

c)

As

d)

Nd

26.

The principle quantum number, n, represents the:

a)

spin

b)

subshell

c)

Energy level

d)

orbital

27.

This orbital shape corresponds to a

a)

s orbital

b)

d orbital

c)

p orbital

d)

f orbital

28.

There may be a maximum of ____ p orbitals at a given energy level.

a)

2

b)

6

c)

3

d)

8

29.

This is a ____ orbital

a)

s

b)

d

c)

p

d)

d

30.

Orbital sublevels, or L, represents:

a)

orbital color

b)

orbital shape

c)

electron spin

d)

energy level

31.

What does the 1 in "1s" stand for?

a)

energy level

b)

s orbitals

c)

p orbitals

d)

the number of electrons

32.

n=5 l=2

a)

3s

b)

4sp

c)

5d

d)

5p

33.
An electron occupies the lowest energy orbital that can receive it.
a)
Hund’s rule
b)
Pauli exclusion principle
c)
Bohr model of the atom
d)
Aufbau principle
34.
All orbitals of equal energy are occupied by one electron before any single orbital is occupied by a second electron.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Core Notation
35.
No two electrons in the same atom can have the same four quantum numbers.
a)
Aufbau principle
b)
Pauli exclusion principle
c)
Hund’s rule
d)
Noble gas notation
36.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
37.
 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.
38.

What element's orbital notation is pictured here?

a)

Ar

b)

Br

c)

Cu

d)

Cl

39.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
40.
This orbital diagram represents:  
a)
C
b)
B
c)
N
d)
O
41.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
42.
What is the noble gas configuration for beryllium?
a)
[He]1s2
b)
[He]2s2
c)
[Li]2s1
d)
[Li]2s2
43.
What is the noble gas configuration for Sulfur?
a)
[Ar] 3p4
b)
[He] 3s2 3p4
c)
[Ne] 3s2 3p4
d)
[Na] 3s2 3p4
44.

Atoms tend to lose or gain electrons to be ____________ a noble gas, their 'octet' of 8 valence electrons is very stable.

a)

exclusive with

b)

identical to

c)

isoelectric to

d)

the same charge as

45.

How many valence electrons does carbon have?

a)

4

b)

5

c)

6

d)

7

46.

Valence electrons are the

a)

electrons in the highest energy level with electrons in it

b)

total electrons in an atom

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