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Atomic Theory Review

Total questions: 90

Worksheet time: 1hrs 2mins

Name
Class
Date
1.

Match the Following

a)

Element

1.

A substance that cannot be broken down into simpler substances by chemical means.

b)

Atom

2.

The smallest unit of an element that keeps the element’s chemical properties.

c)

Nucleus

3.

The dense center of an atom containing protons and neutrons.

d)

Proton

4.

Positively charged particles found in the nucleus of an atom.

e)

Neutron

5.

Particles with a neutral charge found in the nucleus of an atom.

2.

Match the following

a)

Electron

1.

A negatively charged subatomic particle located around the nucleus of an atom.

b)

Electron Shell

2.

Areas around the nucleus filled with electrons. 

c)

Valence Electron

3.

The electrons filling the outermost shell; react with other atoms.

d)

Compound

4.

A substance formed from two or more atoms chemically united in fixed proportions.

e)

Molecule

5.

A group of atoms held together by chemical forces.

3.

Match the following

a)

Periodic Table

1.

All known elements arranged in order by atomic number.

b)

Family/Group

2.

Vertical columns of elements that have the same amount of valence electrons.

c)

Period

3.

Horizontal rows of elements that have the same number of electron shells. 

d)

Atomic Mass/Mass Number

4.

The average number of protons and neutrons in one atom of an element.

e)

15) Metal

5.

Elements that are malleable, ductile, and good conductors; typically shiny.

4.

Match the following

a)

Metalloid

1.

An element that has properties that fall between metals and nonmetals.

b)

 Nonmetal

2.

Elements that are brittle, poor conductors, and have low melting and boiling points.

c)

Noble Gas

3.

Elements in group 18 that have very low reactivity.

5.

Using a periodic table (you can use the one in the textbook) order the following elements by mass number, least to greatest.

a)

Hydrogen

b)

Boron

c)

Gallium

d)

Thallium

e)

Radon

1)
2)
3)
4)
5)
6.

Using a periodic table (you can use the one in the textbook) order the following elements by # of Electron Shells, least to greatest.

a)

Sodium

b)

Calcium

c)

Strontium

d)

Barium

e)

Dubnium

1)
2)
3)
4)
5)
7.

Using a periodic table (you can use the one in the textbook) order the following elements by # of valence electrons, least to greatest.

a)

Potassium

b)

Barium

c)

Carbon

d)

Oxygen

e)

Neon

1)
2)
3)
4)
5)
8.

How many electron shells does the pictured atom have?

a)

1

b)

2

c)

3

d)

4

9.

How many valence electrons does the pictured atom have?

a)

20

b)

3

c)

2

d)

4

10.

Which TWO particles can be changed within an element without changing what the element is?

a)

Neutrons

b)

Electrons

c)

Protons

11.

How is an ionic bond formed?

a)

Sharing of electrons

b)

Delocalised electrons

c)

Transfer of electrons

12.

Ionic bonds are formed between...

a)

Non - metals

b)

A metal and a non-metal

c)

Metals

13.
Mg2+ and Cl- create...
a)
Mg2Cl
b)
MgCl2
c)
Mg2Cl2
d)
MgCl
14.
Ca2+ and N3- create...
a)
Ca2N3
b)
Ca3N2
c)
CaN3
d)
Ca2N
15.

An example of an ionic compound is Sodium Chloride, which is made from Na+ and Cl- ions. Why do these ions form an ionic bond?

a)

They have like charges

b)

They are from the same group

c)

They are from the same period

d)

They have opposite charges

16.

Lead Chloride is an ionic compound, made up from Pb2+ ions and Cl- ions. Which is the correct formula for this compound?

a)

PbCl3

b)

PbCl

c)

PbCl4

d)

PbCl2

17.

Select all the true statements:

a)

Each outer shell electron in Cl is represented by a cross.

b)

In Na, the total charge is -2.

c)

Na+ and Cl- are held together by electrostatic attraction.

d)

Na+ has a full outer shell of electrons.

18.

Sodium Oxide is Na2O. Meaning there are 2 Na present for every O in the ionic compound. As the Oxygen ion has a charge of -2, what charge does each Sodium ion have?

a)

-1

b)

-2

c)

+2

d)

+1

19.

What is the correct formula for aluminium oxide? Aluminium is in group 3 and oxygen is in group 6.

a)

Al₂O₃

b)

AlO

c)

AlO₄

d)

Al₂O

e)

Al₃O₂

20.

Which of the following could NOT form an ionic compound? Check all that apply.

a)

Li+ and Cl-

b)

F- and O2-

c)

Ba2+ and Ag+

d)

Mg2+ and S2-

21.

Calcium Fluoride has a chemical formula of CaF2. What does the chemical formula tell you?

a)

There are 2 Calcium ions for every 1 Fluoride ion in the crystal

b)

There is 1 Calcium ion for every 2 Fluoride ions in the crystal

22.

All atoms are most stable with (or would "prefer") how many electrons in their valence shell?

a)

1

b)

2

c)

8

d)

18

23.

The electronic configuration of an ion is 2.8.8.

What could this ion be?

a)

A

b)

B

c)

C

d)

D

24.

Valence electrons are the

a)

outer most electrons in an atom

b)

total electrons in an atom

25.

This is a correct dot diagram for nitrogen (N)

a)

true

b)

false

26.

Which of these is incorrect?

a)
b)
27.

This could be the dot diagram of

a)

Mg

b)

Cl

c)

C

d)

O

28.

Based on this Lewis Dot diagram, what will a Beryllium atom do to become more stable?

a)

gain two electrons

b)

lose (transfer) two electrons

c)

gain six electrons

d)

lose (transfer) six electrons

29.

Why does the Silver ion have a +1 charge? It

a)

gains one electron

b)

gains seven electrons

c)

transfers (loses) one electron

d)

transfers (loses) seven electrons

30.

Why does the Oxygen ion have a -2 charge? It

a)

gains two electrons

b)

transfers (loses) two electrons

c)

gains six electrons

d)

transfers (loses) six electrons

31.

Based on this Lewis Dot diagram, which is the correct ion that would form and why?

a)
b)
c)
d)
32.

Based on the Lewis Dot diagram, which is the correct ion that would form?

a)
b)
c)
d)
33.

Which diagram correctly illustrates the electron transfer between Sodium and Selenium?

a)
b)
c)
d)
34.

Which diagram correctly illustrates the electron transfer between Aluminum and Iodine?

a)
b)
c)
d)
35.
How many electrons can the d sublevel hold?
a)
14
b)
10
c)
2
d)
6
36.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
37.

Each row on the periodic table represents:

a)

an energy level

b)

a sublevel

c)

an electron

d)

an orbital

38.

Which area on the periodic table represents the electrons in the "d" sublevel?

a)

representative elements

b)

columns 3-8

c)

rare earth elements

d)

transition elements

39.
Which electron configuration belongs to Chlorine (Cl)?
a)
1s2 2s2 2p6 3s2 3p5
b)
1s2 2s2 2p6 3s2 3p6
c)
1s2 2s2 2p6 3s2 3p7
40.
What atom matches this electron configuration?
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
41.
The electron configuration of an atom is 1s22s22p6.  The number of electrons in the atom is 
a)
3
b)
6
c)
8
d)
10
42.
What atom matches this electron configuration?
1s22s22p63s2
a)
Neon
b)
Magnesium
c)
Aluminum
d)
Potassium
43.

Choose the correct shortcut configuration for iodine.

a)

[Ar]4s24d104p5

b)

[Kr]5s24d105p5

c)

[Xe]5s25d105p5

d)

none of the above

44.

Energy levels are denoted by:

a)

letters

b)

numbers

c)

a combination of letters and numbers

d)

subscripts

45.
How many electrons can the s sublevel hold?
a)
14
b)
10
c)
2
d)
6
46.

Choose the correct electron configuration for Beryllium (Be).

a)

1s1

b)

1s2 2s2

c)

1s2 2s2 2p1

47.

Choose the correct electron configuration for Chlorine (Cl).

a)

1s2 2s2 2p1

b)

1s2 2s2 2p6 3s2

c)

1s2 2s2 2p6 3s2 3p5

48.

Choose the correct electron configuration for Nickel (Ni).

a)

1s2 2s2 2p6 3s2 3p6 4s2 3d8

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d2

c)

1s2 2s2 2p6 3s2 3p6 4s10

49.

Choose the correct electron configuration for Krypton (Kr).

a)

1s2 2s2 2p6 3s2 3p6 4s8 3d8

b)

1s2 2s2 2p6 3s2 3p6 4s2 3d8 4p3

c)

1s2 2s2 2p6 3s2 3p6 4s2 3d8 4p6

50.
What is Half-life?
a)
The amount of time it takes for some of the nuclei in a sample of the isotope to decay
b)
The amount of time it takes for half the electrons in a sample of the isotope to decay
c)
The amount of time it takes for half the nuclei in a sample of the isotope to decay
d)
the amount of time it takes to double the nuclei in a sample of the isotope to decay
51.
Is the process in which an unstable atomic nucleus emits charged particles and energy 
a)
radioactivity 
b)
radioisotope
c)
beta decay
d)
background radiation 
52.
Any atom containing an unstable nucleus is called
a)
radioisotope
b)
unisotope
c)
particles
d)
nuclei
53.
Charged particles and energy that are emitted from the nuclei of radioisotopes.
a)
nuclear radiation
b)
nuclear decay
c)
beta particles
d)
alpha particles
54.
What would two different isotopes of an atom have in common?
a)
Number of neutrons 
b)
Number of protons
c)
Atomic weight 
d)
Atomic mass
55.
This is the type of radiation that naturally occurs in the environment and is generally safe.
a)
background radiation
b)
environment radiation
c)
ionizing radiation
56.
True or False:  During nuclear decay atoms of one element can change into atoms of a different element altogether. 
a)
True
b)
False
57.
What is the half-life of iodine-131?
a)
32 days
b)
8 days
c)
16 days
d)
24 days
58.

The % of the parent isotope remaining after 1 Half Life.

a)

50%

b)

25%

c)

12.5%

d)

6.25%

59.

The % of the parent isotope remaining after 2 Half Lives.

a)

50%

b)

25%

c)

12.5%

d)

6.25%

60.

What is the Half life of this isotope?

a)

5 seconds

b)

10 seconds

c)

15 seconds

d)

20 seconds

61.
If one-fourth of the carbon-14 is remaining then how many half-lives have passed?
a)
1
b)
2
c)
3
d)
4
62.
An isotope of an element has the same number of _________, but a different number of _________.
a)
Protons, electrons
b)
Protons, neutrons
c)
Electrons, neutrons
63.
Which process involves the splitting of large nuclei?
a)
alpha decay
b)
nuclear fusion
c)
beta decay
d)
nuclear fission
64.
What type of nuclear reaction occurs in the Sun?
a)
Nuclear fission
b)
beta decay
c)
alpha decay
d)
Nuclear fusion
65.
What makes something radioactive?
a)
elements with an atomic number above 81
b)
an unstable nucleus
c)
contaminated sewage
d)
It decays over time
66.

The three types of nuclear radiation are _______ radiation, _________radiation, and _____________ radiation.

a)

alpha, beta, and gamma

b)

theta, beta, and kappa

c)

alpha, beta, positron

67.

emitted helium nucleus

a)

positron

b)

radioactivity

c)

alpha particle

d)

gamma radiation

e)

beta particle

68.

energetic electron from decomposed neutron

a)

positron

b)

radioactivity

c)

alpha particle

d)

gamma radiation

e)

beta particle

69.

high-energy photons emitted by a radioisotope

a)

positron

b)

radioactivity

c)

alpha particle

d)

gamma radiation

e)

beta particle

70.

Which type of radiation has the charge and mass of an electron?

a)

Alpha radiation

b)

Beta radiation

c)

gamma radiation

71.

What type of radiation can be stopped by clothing or a piece of paper?

a)

Alpha radiation

b)

Beta radiation

c)

gamma radiation

72.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
73.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
74.

Elements in the same group have : (2 correct answers)

a)

Similar chemical properties

b)

Similar names

c)

Same number of outer (valence) electrons)

d)

The same number of protons

75.

The blue elements (left side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
76.

The yellow elements (right side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
77.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
78.

Match the following elements to the group they belong to.

a)

sodium

1.

alkali metal

b)

calcium

2.

alkaline earth metal

c)

chlorine

3.

halogen

d)

argon

4.

noble gas

79.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
80.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
81.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
82.
The Periodic Table of the Elements is useful for revealing patterns and trends in the elements. Which statement accurately describes a pattern in the size of atomic radii in the Periodic Table of the Elements?
a)
Atomic radii decrease from left to right across a period and decrease from top to bottom in a group.
b)
Atomic radii increase from left to right across a period and increase from top to bottom in a group.
c)
Atomic radii decrease from left to right across a period and increase from top to bottom in a group.
d)
Atomic radii increase from left to right across a period and decrease from top to bottom in a group.
83.
The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest electronegativity?

a)
W
b)
X
c)
Y
d)
Z
84.
Fluorine, chlorine, bromine, and iodine all have the same number of valence electrons and have a tendency to gain electrons. Which element has the greatest ionization energy and electronegativity?
a)
fluorine
b)
chlorine 
c)
bromine 
d)
iodine 
85.
The ionization potential of an element is the amount of energy required to remove an electron from an isolated atom or molecule. According to the periodic table, which of the following indicates the correct decreasing order of ionization energy?
a)
Li > Na > K > Cs
b)
Na > K > Li > Cs
c)
Li > K > Na > Cs 
d)
Cs > K > Na > Li 
86.
The number of valence electrons in an element affects the reactivity of that element. Which element listed has the fewest valence electrons?
a)
beryllium (Be)
b)
sodium (Na) 
c)
oxygen (O) 
d)
neon (Ne)
87.
Which element has 2 valence electrons? 
a)
cesium (Cs) 
b)
magnesium (Mg)
c)
boron (B)
d)
argon (Ar) 
88.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
89.
Which of the following will have a lower ionization energy than Scandium (Sc)?
a)
Helium (He)
b)
Titanium (Ti)
c)
Calcium (Ca)
d)
Magnesium (Mg)
90.
Electronegativity is...
a)
how good an atom is at attracting electrons
b)
the ability of an atom to lose electrons
c)
the energy required to remove an electron from a specific atom
d)
how easy it is to make friends. 

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