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Chapter 5 Review Chem

Total questions: 25

Worksheet time: 17mins

Name
Class
Date
1.

The pattern for colored lines that was discovered while analyzing light produced by heating elements is called?

a)

Emission Spectrum

b)

Ground State

c)

Color Spectrum

d)

Excited State

2.

Which of the following accurately describes the Bohr Model?

a)
The Bohr Model is a model of the atom in which electrons move in straight lines around the nucleus
b)
The Bohr Model is a model of the atom in which electrons move in circular orbits around the nucleus, with each orbit representing a specific energy level.
c)
The Bohr Model states that electrons move randomly around the nucleus
d)
The Bohr Model suggests that electrons are located within the nucleus of the atom
3.

Light is made up of massless particles called?

a)

Photons

b)

Waves

c)

Electrons

d)

Orbitals

4.

The wave-particle theory describes how an electron can act as both a particle and a

a)

Electron

b)

Photon

c)

Wave

d)

Proton

5.

Orbitals with low energies predict that an electrons ___________ distance is small.

a)

Visual

b)

Total

c)

Short

d)

Average

6.

What is the maximum number of electrons in a 3p orbital?

a)

6

b)
2
c)
7
d)
5
7.

What principal energy level has both s and p sublevels but no others?

a)

first

b)

second

c)

fourth

d)

fifth

8.

How many electrons are present in the third principal energy level in an atom at full capacity?

a)

2

b)

8

c)

18

d)

32

9.

What principle/rule states that each orbital must receive one electron with the same spin before pairing up with another electron?

a)
Bohr's Principle
b)
Hund's Rule
c)
Heisenberg Uncertainty Principle
d)
Pauli Exclusion Principle
10.

What electron configuration best matches Neon?

a)
1s2 2s2 2p6
b)
1s2 2s1 2p6
c)

1s2 2s2 2p6 3s2

d)

1s2 2s2 2p4

11.

What is the best orbital notation for Carbon?

a)
b)
c)
d)
12.

What is the abbreviated electron configuration for Phosphorus?

a)
1s2 2s2 2p6 3s2 3p3
b)
1s2 2s2 2p6 3s2 3p2
c)

[Ne] 3s2 3p3

d)

[Ar] 3s2 3p3

13.

How many valence electrons does Silicon have?

a)
8
b)
4
c)

3

d)
6
14.

If an atom loses an electron it will have a ________ charge.

a)

Negative

b)

Positive

c)

Neutral

d)

Periodic

15.

Each element has __________ line spectrum.

a)

the same

b)

a continuous

c)

a blurred

d)

a unique

16.

What is the maximum number of electrons can that each orbital hold?

a)
8
b)
2
c)
5
d)
10
17.

How many orbitals are in the s energy level?

a)

6

b)

2

c)

3

d)

1

18.

What does Aufbau's principle state?

a)
Aufbau's principle states that electrons fill the energy levels based on their mass.
b)
Aufbau's principle states that electrons fill the energy levels randomly.
c)
Aufbau's principle states that electrons fill the lowest energy levels first before moving to higher energy levels.
d)
Aufbau's principle states that electrons fill the highest energy levels first before moving to lower energy levels.
19.

Which of the following can be used to help explain line spectra?

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli exclusion principle

d)

Bohr Model

20.

Which principle states that it is impossible to know both the energy and the exact position of an electron at the same time?

a)
Bohr's Atomic Model
b)

Pauli exclusion principle

c)

Hund's Rule

d)
Heisenberg Uncertainty Principle
21.

What does Hund's rule do?

a)
Hund's rule dictates that electrons will fill orbitals of different energy singly before pairing up.
b)
Hund's rule dictates that electrons will fill orbitals of equal energy in pairs before filling singly.
c)
Hund's rule dictates that electrons will fill orbitals of different energy in pairs before filling singly.
d)
Hund's rule dictates that electrons will fill orbitals of equal energy singly before pairing up.
22.

States that two electrons in the same orbital must have opposite spins.

a)

Hund's Rule

b)

Aufbau Principle

c)

Pauli exclusion principle

d)

Heisenberg Uncertainty Principle

23.

Which sublevel has a spherical shape?

a)
The d sublevel
b)
The p sublevel
c)
The f sublevel
d)

The s sublevel.

24.

Which sublevel holds the greatest amount of electrons?

a)

The s sublevel

b)

The p sublevel

c)

The f sublevel

d)

The d sublevel

25.

What do the dots on the electron dot notation represent?

a)
The dots represent the valence electrons of an atom.
b)

The dots represent the electrons of an atom.

c)
The dots represent the neutrons of an atom.
d)
The dots represent the protons of an atom.

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