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Electrons in Atoms

Total questions: 31

Worksheet time: 2hrs 33mins

Name
Class
Date
1.

1. What atom matches this electron configuration?

1s2 2s2 2p6 3s23p4

a)

sodium

b)

sulfur

c)

silicon

d)

potassium

2.

What is the correct electron configuration for oxygen?

a)

1s22s22p63s23p64s2

b)

1s22s22p63s23p4

c)

1s12s22p5

d)

1s22s22p4

3.

What is the maximum number of electrons that an orbital can have?

a)

2

b)

6

c)

8

d)

10

4.

How many d orbitals are there?

a)

2

b)

5

c)

7

d)

10

5.

How many electrons can the p sublevel hold?

a)

2

b)

3

c)

6

d)

8

6.

What is this element?

1s22s22p63s23p63d54s2

a)

magnesium

b)

iron

c)

manganese

d)

chromium

7.

What atom matches this electron configuration?

[Xe] 4f145d96s2

a)

tungsten

b)

gold

c)

silver

d)

copper

8.

What is the noble gas configuration for a sulfur atom?

a)

[Ar] 3p4

b)

[Ne] 3p4

c)

[Ne] 3s23p4

d)

[He] 3s23p4

9.

Which of the following is a correct configuration for aluminum?

a)

1s2 2s2 3s2 3p1

b)

1s2 2s2 2p2 2s2 3p1

c)

[Ne] 3s2 3p1

d)

[Ne] 3p1

10.

How many total electrons can an f orbital contain?

a)

2

b)

7

c)

8

d)

14

11.

Which rule says orbitals are filled from lowest energy to highest?

a)

Aufbau's principle

b)

Hund's principle

c)

Pauli exclusion principle

d)

Law of conservation of mass

12.

True or False: The ground state is the highest energy state of an atom.

a)

True

b)

False

13.
For an electron to change from ground state to an excited stated it must...
a)
Absorb energy
b)
Release energy
14.

What is the light that you can see called?

a)

observatory light

b)

ultraviolet light

c)

visible light

d)

infrared light

15.
Line emission spectrum shown below happens when
a)
Electron transition from lower to higher energy level.
b)
Electron transition from higher to lower energy level.
c)
Electron exist in fixed energy states
d)
Electron transition between different energy levels.
16.
Emission of light from an atom occurs when an electron
a)
drops from a higher to a lower energy level.
b)
   jumps from a lower to a higher energy level.   
c)
   moves within its atomic orbital.
d)
falls into the nucleus.
17.
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
18.

All stars are composed of a mixture of elements. When these elements are heated they emit specific amounts of electromagnetic radiation, known as an emission spectrum. Each element emits a unique, identifiable, spectrum.


Using the Bright-line emission spectrum chart below, identify the elements present in this modeled star (found in the line labeled “mixture”).

a)

Lithium and cadmium are in the mixture. Strontium is not in the mixture.

b)

Lithium and strontium are in the mixture. Cadmium is not in the mixture

c)

Cadmium and strontium are in the mixture. Lithium is not in the mixture

d)

All of the shown elements are present in the mixture.

19.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

20.

The unknown emissions spectra belongs to the element

a)

Hydrogen

b)

Mercury

c)

Neon

d)

Sodium

21.
What gases are in the unknown mixture?
a)
Gas B & Gas D
b)
Gas C & Gas B
c)
Gas A & Gas D
d)
Gas D & Gas C
22.

If an electron moves from n=4 to n=2 it ____

a)

absorbs energy

b)

releases energy

23.

Look carefully at the picture. It shows an electron in the excited state on the left, and the electron returning to its ground state on the right. When the electron return to the ground state it emits a_______________________.

a)

blast of cold air

b)

electrostatic charge

c)

proton

d)

photon (light)

24.

The picture shows an atom in the ground state absorbing energy and the electron jumps to the excited state. Which state has higher energy?

a)

Ground State

b)

Excited State

25.

Each element produces its own pattern of emission spectra lines because each element has its own distinct

a)

Speed of light

b)

Electron configuration

c)

Number of neutrons

d)

None of these

26.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
27.
Electrons occupy orbitals of lowest energy first is part of what electron configuration rule?
a)
Hund’s Rule
b)
Aufbau Principle
c)
Pauli Exclusion Principle
28.

What does Pauli exclusion principle state ?

a)

states that each electron occupies the lowest energy orbital available

b)

states that -no two electrons in the same orbital can have the same spin

c)

states that single electrons electrons with the same spin must occupy each-energy orbital before additional electrons with opposite spins can occupy the same orbitals

29.

How many electrons can the d sublevel(orbital) hold?

a)

8

b)

10

c)

2

d)

4

30.
Which of the following is a p block element?
a)
Ca
b)
Ar
c)
Re
d)
Au
31.

There are 4 different types of subshells(orbitals) s,p,d,f

a)

true

b)

false

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