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Chapter 4 and 5 Test Review

Total questions: 55

Worksheet time: 51mins

Name
Class
Date
1.

What color of light has the greatest energy per photon?

a)

Red

b)

Green

c)

Blue

d)

Violet

2.

What color of light has the shortest wavelength?

a)

Red

b)

Green

c)

Blue

d)

Violet

3.

Put the following regions of electromagnetic radiation in order of longest to shortest wavelength

a)

Radio, Micro, Infra, Visible, Ultra, X-ray, Gamma

b)

Gamma, X-ray, Ultra, Vis, Infra, Micro, Radio

c)

Vis, Micro, Infra, Ultra, X-ray, Gamma, Radio

d)

Micro, Radio, Vis, Infra, Ultra, X-ray, Gamma

4.

What is the energy of a quantum of light with a frequency of 7.39x1014Hz.

a)

4.88x1019

b)

4.88x10-19

c)

2.22x1023

d)

2.22x10-23

5.

A light has a wavelength of 506 nm. What is the frequency of the light? What is the color of light?

a)

16.87Hz, Red

b)

5.93Hz, Orange

c)

5.93x10-14Hz, Blue

d)

5.93x1014Hz, Green

6.

_____________________ is the lowest energy level an electron will occupy in an atom at an ordinary condition

a)

the ground state

b)

the excited state

7.

13. A theory stating that it is forbidden for 2 electrons having the same value of atomic quantum numbers is explained by... .

a)

Hund

b)

Aufbau

c)

Pauli

d)

Schrodinger

8.
Identify the following element:
1s22s22p63s23p64s23d10
a)
nickel
b)
copper
c)
zinc
d)
gallium
9.
According to the Aufbau Principle, which sublevel should starting filling with electrons before the 3p sublevel?
a)
3s
b)
2p
c)
4s
d)
4p
10.

Choose the correct noble gas configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

11.
Which element is depicted from this orbital diagram
a)
Fluorine
b)
Neon
c)
Chlorine
d)
Argon
12.

Which (if any) principles are being violated in this orbital diagram for oxygen?

a)

Aufbau

b)

Pauli

c)

Hund

d)

Both Pauli and Hund

e)

Both Aufbau and Hund

13.

Which choice lists the orbital shapes in order from lowest to highest energy?

a)

s, p, d, f

b)

p, s, d, f

c)

d, f, s, p

d)

they all have the same energy

14.

Which periodic table family could have valence electrons filling orbitals in the s-block?

a)

Alkaline Earth

b)

Halogens

c)

Noble Gases

d)

Transition Metals

15.

Vertical columns on the periodic table are called ___?

a)

groups

b)

periods

c)

rows

16.

Which color on the image of the periodic table corresponds with the halogens.

a)

red

b)

black

c)

blue

d)

orange

17.

Which color on the image of the periodic table corresponds with the noble gases.

a)

red

b)

black

c)

blue

d)

orange

18.

Which color on the image of the periodic table corresponds with the transition metals.

a)

red

b)

black

c)

blue

d)

orange

19.

Which color on the image of the periodic table corresponds with the metalloids.

a)

bright yellow

b)

gold

c)

teal

d)

light blue

20.

Which color on the image of the periodic table corresponds with the alkaline earth metals.

a)

yellow

b)

dark yellow

c)

blue/green

d)

teal

21.

Mendeleev first ordered the periodic table of elements by increasing

a)

atomic number

b)

atomic mass

c)

atomic symbol

d)

atomic weight

22.

Horizontal rows on the periodic table are called ___?

a)

groups

b)

periods

c)

rows

d)

families

23.

The periodic table is mostly comprised of what type of element?

a)

Metals

b)

Nonmetals

c)

Metalloids

24.

period

a)

Elements that occur in vertical columns on the periodic table.

b)

A horizontal row of elements in the periodic table

c)

Found in group two of the periodic table; highly reactive

d)

A subatomic particle that has a negative charge

25.

found in group one of the periodic table; highly reactive

a)

Non-metals

b)

Transition Metals

c)

alkali metals

d)

metalloids

26.

Found in group two of the periodic table; highly reactive

a)

period

b)

Alkali Earth Metals

c)

metalloids

d)

alkali metals

27.

An electron that is available to be lost, gained, or shared in the formation of chemical compounds is called a(n)

a)

inner-shell electrons

b)

protons

c)

neutrons

d)

valence electrons

28.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)

Argon

29.
Electronegativity is...
a)

the ability of an atom in a chemical bond to attract electrons

b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)

the energy required to add an electron to a specific atom

30.

List the following in order of lowest to highest ionization energy.

P, Cs, Co, Sr

a)

P, Co, Sr, Cs

b)

Cs, Sr, Co, P

c)

Sr, Cs, Co, P

d)

P, Co, Cs, Sr

31.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

32.

Which of the following will have a higher electronegativity than arsenic (As)?

a)

Carbon (C)

b)

Neon (Ne)

c)

Antimony (Sb)

d)

Germanium (Ge)

33.
Atomic radius generally increases as we move __________.  
a)
down a group and from right to left across a period 
b)
up a group and from left to right across a period 
c)
down a group and from left to right across a period 
d)
up a group and from right to left across a period 
34.
Ionization energy is...
a)
the energy required to add an electron to a specific atom
b)
how much energy it takes to remove an electron from an atom
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
35.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration
36.

Periodic law states that

a)

the chemical properties of elements can be grouped according to appearance.

b)

the physical and chemical properties of the elements are functions of their atomic number.

c)

no two electrons with the same spin can be found in the same place in an atom

d)

wave patterns repeat at regular intervals.

37.

How many valence electrons does oxygen have?

a)

2

b)

8

c)

6

d)

18

38.

Which of these is the correct orbital diagram for oxygen?

a)
b)
c)
d)
39.

Which portion(s) of the periodic table are called "main group" elements?

a)

transition elements

b)

s and p group elements

c)

d and f group elements

d)

alkali and ahlogens

40.

nonmetals are located

a)

on the right side of the periodic table

b)

on the left side of the periodic table

c)

all over the periodic table

d)

in the middle of the periodic table

41.

The molar mass of (NH4)2CO3 is:

a)

96.11

b)

98.54

c)

97.21

d)

95.02

42.

What would be the mass of 5 moles of CO2? 

a)

220.05 g

b)

220.05 mol

c)

0.11 mol

d)

8.80 g

43.

What is the mass of 3.56 moles of H2? 

a)

7.18 g

b)

1.77 mol

c)

1.77 g

d)

0.57 mol

44.

How many moles would make up a sample of 32.7 grams of NH3?

a)

19.19 mol

b)

19.19 g

c)

557.21 mol

d)

0.43 g

45.

How many molecules are present in 1.75 moles CO2?

a)

1.05 X 1024 molecules

b)

1.28 X 10-22 molecules

c)

2.91 X 10-24 molecules

d)

2.39 X 10222 molecules

46.
a)
Amplitude
b)
Crest
c)
Trough
d)
Wavelength
47.
a)
Frequency
b)
Amplitude
c)
Wavelength
d)
Trough
48.
a)
Crest
b)
Trough
c)
Height
d)
Frequency
49.

If the wavelength of a wave increased, what would happen to the frequency?

a)

decrease

b)

increase

c)

stay the same

50.

The number of waves that pass somewhere in a second is:

a)

amplitude

b)

frequency

c)

wavelength

51.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Hund's
b)
Aufbau's
c)
Pauli's Exclusive
52.
Which guideline, Hund’s rule or the Pauli exclusion principle, is violated in the following orbital diagrams?
a)
Aufbau's
b)
Hund's
c)
Pauli exclusive
53.
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
54.

Match the rule to the correct definition

a)

No two electrons in the same atom can have the same four quantum numbers

1.

Pauli Exclusion Principle

b)

we cannot know both the position and speed of a particle, such as a photon or electron

2.

Heisenberg uncertainty principle

c)

in the ground state of an atom or ion, electrons fill atomic orbitals of the lowest available energy level before occupying higher-energy levels

3.

Aufbau Principle

d)

every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied

4.

Hund's Rule

55.

Match the Quantum Number to its description

a)

energy level, size, row number of the periodic table

1.

Principle, n

b)

shape of the subshell

2.

angular momentum quantum number, l

c)

orientation of the orbital

3.

mgnetic quantum number, Ml

d)

spin of the electron

4.

Ms

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