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Atomic Radius, Ionization Energy, & Electronegativity

Total questions: 127

Worksheet time: 2hrs 51mins

Name
Class
Date
1.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
2.
As you move across the periodic table from left to right, the atomic radius decreases.  This is because - 
a)
the number of protons increases, so attraction to electrons increases
b)
the number of energy levels increases
c)
the number of electrons increases
d)
the atomic mass increases
3.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
4.
Francium (Fr) has the lowest ionization energy in Group 1 because - 
a)
it has the smallest number of valence electrons
b)
it has the greatest atomic mass
c)
it has the greatest number of protons, so it attracts its electrons the strongest
d)
its 1 valence electron is very far from the nucleus, so little energy is needed to remove it
5.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
6.
The energy required to remove electrons is the definition of: 
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
7.

What is the name of group 1

a)

Alkaline Earth Metals

b)

Boron Family

c)

Alkali Metals

d)

Halogen Family

8.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
9.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
10.
Electronegativity is...
a)
the ability of an atom to attract/ accept 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. 
11.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
12.
As you move across the periodic table atoms tend to get smaller because, ______________.
a)
the atoms have more mass.
b)
the atoms have less mass
c)
the atoms have more protons.
d)
the atoms have less electrons.
13.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
14.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
15.

Which periodic group has the smallest atomic radius?

a)

Alkali metals

b)

Halogens

c)

Alkaline Earth metals

d)

Transition metals

16.
Atoms that have a high electronegativity, _______________.
a)
give up their electrons more easily.
b)
hold on to their electrons more tightly.
c)
have more electron shells.
17.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
18.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
19.
Which has the greater EN: 
N or C?
a)
C
b)
N
20.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
21.
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)
22.

The common charge on an atom in group 17 would be....

a)

+1

b)

+7

c)

-7

d)

-1

e)

17

23.

Which of the following is the term for a substance in which all the atoms have the same number of protons

a)

a compound

b)

An element

c)

a molecule

d)

a solid

e)

a gas

24.

Which of the following reasons explains why there is a decimal for most atomic masses?

a)

The mass of one atom can have a fraction.

b)

Since electrons are very small mass they only add a little bit, usually only a decimals worth.

c)

It is the average mass of all the potential isotopes of an atom.

d)

Neutrons have a mass of 1.1 meaning that fractions are common.

25.
Which particle has a positive charge?
a)
electron
b)
orbital
c)
proton
d)
neutron
26.
Choose the particle that has no charge.
a)
nucleus
b)
neutron
c)
proton
d)
electron
27.
This particle determines what element you have - the elements identity.
a)
electron
b)
proton
c)
neutron
d)
valence shell
28.
An electron has a _____ charge.
a)
negative
b)
positive
c)
neutral
29.
Which particles make up the nucleus of an atom?
a)
protons and neutrons
b)
electrons and protons
c)
electrons, protons, and neutrons
d)
electrons and neutrons
30.
What is the mass number and name of an element with 8 protons and 8 neutrons?
a)
16 - Carbon
b)
16 - Oxygen
c)
24 - Oxygen
d)
8 - Neon
31.
An element with a mass number of 10 and an atomic number of 6 has how many protons?
a)
5
b)
8
c)
6
d)
10
32.
What is the atomic number of the atom pictured? 
a)
11
b)
12
c)
22
d)
23
33.
How many electrons are in the atom pictured? 
a)
1
b)
2
c)
3
d)
0
34.
What is the number of protons that the element in this image contain?
a)
14
b)
7
c)
15
d)
18
35.
How many protons, electrons and neutrons does an neutral atom of Calcium have?  Its atomic number is 20 and the mass number is 40.
a)
20 protons, 18 electrons and 40 neutrons
b)
20 protons, 20 electrons and 20 neutrons
c)
40 protons, 40 electrons and 20 neutrons
d)
20 protons, 18 electrons and 20 neutrons
36.
Which of the following people said the atom was a solid sphere?
a)
Dalton
b)
Thompson
c)
Rutherford
d)
Bohr
37.
Ag--110 and Ag--112 are two forms of silver with different mass # so they are
a)
compounds
b)
isotopes
c)
orbitals
d)
neutrons
38.
In Dalton's Atomic Theory, all elements consist of __________ that cannot be divided.
a)
Atoms
b)
Parts
c)
Molecules
d)
Hydrogen
39.
In the Thomson Model, he discovered the existence of what particle?
a)
Electrons
b)
Protons
c)
Neutrons
d)
Quarks
40.
Which model is this?
a)
Thomson Model
b)
Cloud Model
c)
Bohr Model
d)
Rutherford Model
41.
Which model involved gold foil?
a)
Thomson Model
b)
Rutherford Model
c)
Cloud Model
d)
Bohr Model
42.
While making his model of an atom, what structure did Rutherford discover (containing protons and neutrons)?
a)
the Nucleus
b)
the Electron Cloud
c)
the quarks
d)
the atomic mass
43.
According to the Bohr Model, electrons are only found in specific orbits around the nucleus called __________________________
a)
Energy Levels
b)
Electron Lanes
c)
Electron Places
d)
Atomic Mass
44.
Which model is this?
a)
Thomson Model
b)
Rutherford Model
c)
Cloud Model
d)
Bohr Model
45.
Which of these particles was discovered first?
a)
Protons
b)
Electrons
c)
Neutrons
d)
Quarks
46.
Which model of the atom proposed that atoms were positive spheres with negative electrons in them?
a)
Heliocentric Model
b)
Solid Sphere Model
c)
Plum Pudding Model
d)
Planetary Model
47.

Who was the Greek philosopher who called the smallest particle of matter as "atom"?

a)

Democritus

b)

Aristotle

c)

J.J Thompson

d)

Einstein

48.
Who is the scientist who proposed the "solar system" model of an atom where the electrons revolve around the nucleus?
a)
Dalton
b)
Niels Bohr
c)
Ernest Rutherford
d)
Democritus
49.
What did James Chadwick discover?
a)
neutrons
b)
electrons
c)
the atomic theory
d)
protons
50.
This number gives the number of protons in each atom of an element.
a)
mass number
b)
atomic number 
c)
atomic mass
51.

Which of the following is/are conclusions based on Rutherford’s gold foil experiment?

a)

Atom is mostly empty space

b)

The nucleus is positively charged

c)

The atom has a small dense nucleus

d)

All answers are correct

52.
all matter is made of what 
a)
energy 
b)
atoms 
c)
electrons 
d)
compounds 
53.
Where are electrons of an atom found?
a)
Nucleus
b)
Electron Cloud
c)
Some are in the nucleus and some in the electron cloud.
d)
They are moving everywhere.
54.
If an element has 6 protons, 7 neutrons, and 6 electrons, what type of charge does the element have?
a)
positive
b)
negative
c)
neutral
d)
imaginary
55.
If an atom has 24 protons and 24 electrons, what is the atomic number of this element?
a)
24
b)
48
c)
0
d)
42
56.
How many protons does this element have?
a)
40
b)
21
c)
20
d)
41
57.
Elements in the same ________ are more chemically similar.
a)
group
b)
period
c)
club
d)
table
58.
Rows on the periodic table are called _____ while columns are called _____.
a)
groups, families
b)
groups, periods
c)
periods, groups
d)
families, groups
59.
What does the H stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
60.
What does the 1 stand for?
a)
Hydrogen
b)
atomic number
c)
atomic mass
d)
atomic explosion
61.
An element with a mass number of 11 and an atomic number of 5 has how many neutrons?
a)
11
b)
5
c)
6
d)
16
62.
How did Mendeleev arrange the elements?
a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
63.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
64.
Which group of the periodic table is composed of inert (not reactive)  gases?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
65.
This class of elements are sometimes called "semiconductors."
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Groups
66.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
67.
The family in the periodic table that contains the most reactive metals is the_______
a)
Alkaline Earth Metals
b)
Transition Metals 
c)
Alkali Metals
d)
Other Metals
68.

Most noble gases have _______ valence electrons.

a)

1

b)

2

c)

7

d)

8

69.
All elements found on the left side of the Periodic Table of the Elements have what properties in common?
a)
They conduct heat and electricity 
b)
They are all gases 
c)
They are brittle and dull
d)
They are radioactive
70.

Why do all bonds form?

a)

To fill up the outer shell and become more stable.

b)

To look cool.

c)

To become less stable.

d)

So they don't have to be alone.

71.

What two types of atoms make a covalent bond?

a)

metal atom and metal atom

b)

metal atom and non metal non atom

c)

non metal atom and non metal atom

72.

When an atom loses an electron, it becomes a _________.

a)

noble gas

b)

anion

c)

cation

73.

Atoms are most stable when their outer shell is full or complete.

a)

True

b)

False

74.

What part of an atom is involved in chemical bonding?

a)

proton

b)

neutron

c)

electron

75.

How many bonds can Hydrogen make?

a)

1

b)

2

c)

3

d)

4

76.

Where are the non-metals located on the periodic table?

a)

all over

b)

On the left side of the "staircase"

c)

On the right side of the "staircase"

77.

Predict the bond that form between Be and F

a)

Covalent

b)

Ionic

78.

What kind of bond form when atoms share electrons?

a)

Covalent

b)

Ionic

c)

Metallic

d)

Non metallic

79.

Atoms gain or lose electrons to become stable by satisfying this rule.

a)

Ionic law

b)

Lewis structure rule

c)

Periodic law

d)

octet rule

80.

Ionic bonding is when a metal donates one or more ___________ to a non-metal atom.

a)

electrons

b)

protons

c)

atoms

d)

neutron

81.

Anion is ....

a)

negatively charged

b)

positively charged

c)

neutral

d)

a vegetable

82.

Sodium has ________ electron to donate.

a)

1

b)

2

c)

3

d)

4

83.

Looking at the Whiteboard, Match the element with the number of bonds it can make.

a)

Hydrogen

1.

1

b)

oxygen

2.

2

c)

Nitrogen

3.

3

d)

Carbon

4.

4

84.

Mendeleev was the first person to arrange the elements into a table. How did he arrange the rows?

a)
alphabetical 
b)
density
c)
melting point
d)
atomic mass
85.

Which of the following will have similar properties?

a)

O, S, Se

b)

O, F, Ne

c)

N, Ne, Na

d)

H, K, P

86.

Moseley arranged what we know as the "modern periodic table". How did he arrange it?

a)

atomic mass

b)

atomic number

c)

valence electrons

d)

number of isotopes

87.
Each column in the periodic table is called a _________ .
a)
period
b)
group
c)
cluster
d)
unit
88.
Periods on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
89.
Groups on the periodic table are __________.
a)
Horizontal Rows
b)
Vertical Columns
90.

How many periods are on the periodic table?

a)

5

b)

6

c)

7

d)

8

91.

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

92.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
93.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
94.

Name this group: These metals contain familiar metals such as gold, iron, and copper.

a)
b)
c)
d)
95.

Find an element with similar chemical properties to Barium (Ba).

a)

Ca an Ra, because they are in the same group and have similar chemical properties.

b)

Cs and La, b/c they are in the same period number.

c)

Ca and Y, b/c they are 90 degree angle and have similiar properties.

96.
a)
Same group
b)
Same period
97.

The blue elements (left side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
98.

The yellow elements (right side) are called 

a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
99.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
100.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
101.

What do the periods (rows) represent?

a)

an additional energy level

b)

an additional proton

c)

an additional group

d)

an additional electron

102.

Put the groups of the periodic table in order from group 1A to group 8A (18).

a)

alkali metals

b)

alkaline earth metals

c)

halogens

d)

noble gases

1)
2)
3)
4)
103.

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

104.

Match the following

a)

lithium

1.

2 energy levels

b)

helium

2.

1 energy level

c)

aluminum

3.

3 energy levels

d)

bromine

4.

4 energy levels

e)

strontium

5.

5 energy levels

105.

Mendeleev & Moseley both organized the columns (groups) by...

a)

mass

b)

number

c)

symbol

d)

properties

106.

Element symbols have _____ capital letter(s).

a)

1

b)

2

c)

3

d)

4

107.

Compound formulas have ____ capital letter(s).

a)

1

b)

2

c)

3

d)

more than 1

108.

Carbon

a)

CA

b)

C

c)

Ca

d)

Cn

109.

Sn

a)

tin

b)

sulfur

c)

iron

d)

sodium

110.

Zinc

a)

Z

b)

Zi

c)

ZN

d)

Zn

111.

Sulfur

a)

Sf

b)

Su

c)

Sr

d)

S

112.

Neon

a)

N

b)

No

c)

Ne

d)

Nn

113.

Calcium

a)

Cl

b)

Ca

c)

C

d)

Cm

114.

Copper

a)

CU

b)

Cp

c)

Cu

d)

Cr

115.

Helium

a)

He

b)

Hl

c)

HE

d)

Hm

116.

Hydrogen

a)

Hy

b)

H

c)

Hr

d)

Hn

117.

N

a)

Sodium

b)

Nitrogon

c)

Nonium

d)

Nitrogen

118.

Gold

a)

Go

b)

Gl

c)

AU

d)

Au

119.

Pb

a)

Gold

b)

Lead

c)

peanut butter

d)

Paribium

120.

Iron

a)

Ir

b)

In

c)

Fe

d)

FE

121.

Nickel

a)

Ni

b)

N

c)

Nl

d)

Nc

122.

Mercury

a)

Me

b)

Hg

c)

HG

d)

ME

123.

Iodine

a)

Ie

b)

I

c)

Id

d)

Io

124.

Potassium

a)

P

b)

K

c)

Pt

d)

k

125.

Aluminum

a)

A

b)

Al

c)

Am

d)

Au

126.

Mg

a)

Manganese

b)

Mangium

c)

Magnesium

d)

Manzanium

127.

Xenon

a)

Xe

b)

X

c)

Xn

d)

Xo

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