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Worksheets

Extra Credit/Zero Replacement Quiz

Total questions: 200

Worksheet time: 17hrs 40mins

Name
Class
Date
1.
a)
Periods
b)
Groups
2.
a)
Periods
b)
Groups
3.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
4.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
5.
a)
Same group
b)
Same period
6.
a)
Group 1
b)
Group 17
c)
Group 2
d)
Group 18
7.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
8.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
9.
a)
Metals
b)
Nonmetals
c)
Metalloids
10.
a)
Metals
b)
Nonmetals
c)
Metalloids
11.
a)
Metals
b)
Nonmetals
c)
Metalloids
12.
a)
Metals
b)
Nonmetals
c)
Metalloids
13.
a)
Metals
b)
Nonmetals
c)
Metalloids
14.
a)
Metals
b)
Nonmetals
c)
Metalloids
15.
a)
Metals
b)
Nonmetals
c)
Metalloids
16.

Who invented the Periodic Table?

a)

Mendeleev

b)

Bohr

c)

Lewis

d)

Democritus

17.

What happens to the number of shells as you move down a group?

a)

They decrease by 1

b)

They increase by 1

c)

Nothing

18.

What do all elements in the same period have?

a)

same number of shells

b)

same number of electrons

c)

belong in the same family

19.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
20.
Name group 1A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
noble gases
d)
halogens
21.
Name group 2A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
22.
Name groups 3B - 12B on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
23.
Name group 18 on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
transition metals
d)
noble gases
24.
What does the 6 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
25.
What does 12.011 represent?
a)
atomic mass
b)
atomic number
c)
element name
d)
chemical symbol 
26.
Name group 17 on the periodic table.
a)
transition metals
b)
metalloids
c)
halogens
d)
alkali metals
27.

3 subatomic particles that makeup an atom.

a)

Positive, negative, neutral

b)

Positron, Neutral, Electron

c)

Proton. Neutron, Electron

28.

This subatomic particle has a positive charge.

a)

Proton

b)

Neutron

c)

Electron

29.

The subatomic particle holds the atom together.

a)

Proton

b)

Neutron

c)

Electron

d)

Nucleus

30.

The subatomic particles found in the nucleus.

a)

Electron, Neutron

b)

Proton, Neutron

c)

Electron, Proton

d)

Proton, Neutron, Electron

31.

The subatomic particle that identifies the element.

a)

Proton

b)

Positron

c)

Neutron

d)

Electron

32.

The subatomic particle that determines reactivity.

a)

Electron

b)

Proton

c)

Shell

d)

Neutron

33.

A neutron has a _____ charge.

a)

Positive

b)

Negative

c)

Neutral

d)

1/2 charge

34.

A electron has a ______ charge.

a)

No charge

b)

Positive

c)

Neutral

d)

Negative

35.

The atomic number tells you the number of

a)

Neutrons

b)

Protons

c)

Neutrons plus Protons

36.

The atom model that we will use in this class is called ________ model.

a)

Rutherford

b)

Thompson

c)

Bohr

d)

Karen

37.

An isotope has different number of ______.

a)

Neutrons

b)

Protons

c)

Electrons

d)

Nucleus

38.

The building block of everything.

a)

Atoms

b)

Elements

c)

Positive

d)

Biology

39.

A piece of paper contains_______ of atoms.

a)

Hundreds

b)

Tens

c)

Millions

40.
a)
Bunsen burner
b)
Ring stand
c)
Graduated cylinder
d)
Test tube holder
41.
a)
beaker
b)
cup-with-lines
c)
wash bottle
d)
graduated cylinder
42.
a)
Erlenmeyer flask
b)
beaker
c)
wash bottle
d)
watch glass
43.
a)
graduated cylinder
b)
beaker
c)
Erlenmyer flask
d)
bunsen burner
44.

The following piece of glassware is used to ...

a)

measure a precise volume of a liquid

b)

prepare solutions to an accurate volume

c)

hold and mix chemicals without spilling

45.

Which piece of glassware would you use to measure a precise volume of a liquid?

a)
b)
c)
d)
46.

Which of these would be best to hold large amounts of liquid?

a)

Beaker

b)

Boiling tube

c)

Conical flask

d)

Test tube

47.

Sandals are permitted during laboratory experiments.

a)

True

b)

False

48.

Using chipped glassware is permitted during the labs.

a)

True

b)

False

49.

If you do not understand a direction or part of a lab procedure, you should

a)

figure it out as you do the lab

b)

try several methods until something works

c)

ask the instructor before proceeding

d)

skip it and go on to the next part

50.

Ionic bonding occurs between a _________ and a __________.

a)

metal, metal

b)

metal, nonmetal

c)

nonmetal, nonmetal

d)

metallic, sea of electrons

51.

In an ionic bonds electrons are ____________.

a)

transferred

b)

shared

c)

transferred and shared

d)

arrange like a sea of electrons

52.

A covalent bond occurs between a __________ and a __________.

a)

nonmetal, nonmetal

b)

metal. metal

c)

metal, nonmetal

d)

sea of electrons, metallic

53.

In a covalent bond electrons are _____________.

a)

transferred

b)

shared

c)

depends on ionization energy

d)

connect through a sea of electrons

54.

Valence electrons are the electrons in ______________.

a)

the inner shell

b)

the outermost shell

c)

includes all electrons

d)

depends on atom

55.

Valence electrons determine___________.

a)

the reactivity of the atom

b)

the identity of the atom/element

c)

the atomic number of the atom

d)

the charge of the atom in a neutral sphere

56.

In an ionic bond metals will have a _______________ charge.

a)

positive

b)

negative

c)

neutral

d)

protonic

57.

According to the octet rule most elements need _______ valence electrons.

a)

2

b)

8

c)

6

d)

18

58.

Why do all bonds form?

a)

so the number of protons equals the number of electrons

b)

so an atom can become unstable

c)

to fill the outermost energy level

59.
 Which of the following is the correct formula for these two ions:
Al+3 +  S-2
a)
AlS3
b)
Al2S3
c)
Al3S2
d)
Al3S
60.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
61.
How do the following two elements bond together?
Cr3+  O2-         
a)
CrO
b)
Cr3O2
c)
Cr2O3
d)
CrO3
62.
In chemical compounds, covalent bonds form when
a)
the electronegativity difference between two atoms is very large.
b)
electrons are completely transferred between two metals.
c)
pairs of electrons are shared between two nonmetal atoms.
d)
two nonmetal atoms are attracted to each other by opposite charges.
63.
What region of the periodic table contains atoms that form covalent bonds?
a)
the left side
b)
the middle
c)
the right side
d)
top left
64.
phosphorus trichloride
a)
KCl3
b)
PCl3
c)
K3Cl
d)
P3Cl
65.
silicon dioxide
a)
SO2
b)
NaO2
c)
SiO2
d)
SiO
66.

dinitrogen pentoxide

a)

N2O5

b)

NO5

c)

N5O2

d)

N2O6

67.

What is an ion?

a)

An atom that gains or loses electrons

b)

Pieces of the atom that are atoms of the same element

c)

An atom that is the sum of the number of protons and neutrons in an element.

68.

The isotope is the change in what number of the nucleus?

a)

Protons

b)

Neutrons

c)

Electrons

d)

Protons and Neutrons

69.
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. 
70.

Water melting, freezing, or evaporating is an example of a

a)

physical change

b)

chemical change

c)

physical property

d)

chemical propery

71.

When polyatomic ions bond with other ions the net charge of the ionic compound will be

a)

zero

b)

positive

c)

negative

d)

depends on the bond

72.

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

a)

true

b)

false

73.
Combining substances to form a new substance
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
74.
Breaking down a substance into simpler substances
a)
Displacement
b)
Synthesis
c)
Decomposition
d)
Oxidation
75.
How many Hydrogen are in 4H2O?
a)
6
b)
8
c)
2
d)
4
76.
How many Oxygen are in H2O?
a)
1
b)
2
c)
0
d)
4
77.
2H2 + O2 ----> 2H2O What is the product?
a)
------>
b)
2H2O
c)
2H2+ O2
78.
2H2 + O2 --------> 2H2O What  are the reactants?
a)
----->
b)
2H2O
c)
2H2 +O2
79.
How many atoms are there TOTAL in:
H2SO4
a)
6
b)
5
c)
7
d)
3
80.
How many elements are in C6H12O6?
a)
1
b)
2
c)
3
d)
4
81.

What is the charge/oxidation number in group 1?

a)

+1

b)

-1

c)

varies due to valence electrons

d)

depends on element

82.

What is the oxidation number/charge for transition metals?

a)

varies

b)

3-12

c)

+3

83.

Why is group 18 unreactive?

a)

the outer shell is full

b)

it has 7 valence electrons

c)

the inner shell contains 2 electrons

d)

they are gases

84.

The largest atom on the periodic table is _____

a)

F

b)

Fr

c)

Og

d)

H

85.

The most electronegative atom on the periodic table______

a)

Fr

b)

F

c)

He

d)

Og

86.

Ionization energy is the energy needed to...

a)

remove an electron

b)

remove a proton

c)

gain an electron

d)

gain a proton

87.

Ionization energy down a group will...

a)

increase because you are not adding energy levels

b)

decrease because you are adding energy levels

c)

stays the same

88.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
89.

A chemical change occurs when a piece of wood

a)

splits

b)

cut

c)

chopped

d)

burns

90.

Which of the following is a heterogeneous mixture?

a)

milk

b)

gatorade

c)

hot tea

d)

sand

91.

An element has an atomic number of 76. The number of protons and electrons in a neutral atom of the element are ____.

a)

76

b)

undetermined

c)

38 each

d)

152

92.

From left to right across a period of the periodic table, atomic radius tends to -

a)

increase

b)

decrease

c)

stay the same

d)

depends on acetate

93.

The law of conservation of mass states that_______.

a)

matter can be created into a new substance from random stuff.

b)

matter can not be created nor destroyed only rearranged.

c)

matter will become water that evaporates into the atmosphere.

d)

matter smells like acetate.

94.

Who is buried in Grant's tomb?

a)

Grant

b)

Reid

c)

Lincoln

95.

What school do you take Chemistry?

a)

Tascosa

b)

Harvard

c)

Yale

d)

Princeton

96.

An atom with atomic number 6 would have how many protons

a)

6

b)

12

c)

3

d)

cannot be determined

97.

Which elements have the most similar chemical properties?

a)

boron and carbon

b)

oxygen and sulfur

c)

aluminum and bromine

d)

argon and silicon

98.

This is a correct dot diagram for carbon (C)

a)

true

b)

false

99.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons in the second shell
100.

Ionic compounds are formed between ________ and _________.

a)

metals and metals

b)

nonmetals and nonmetals

c)

metals and nonmetals

101.

In ionic compounds electrons are

a)

transferred

b)

shared

c)

lost

d)

no clue

102.
Elements in the same column of the periodic table always have the same # of _______ as one another.
a)
Protons
b)
Neutrons
c)
Electrons
d)
Valence Electrons
103.
Valence electrons are the...
a)
Innermost electrons
b)
Middle electrons
c)
Outermost electrons
d)
Any electrons
104.
When an ionic compound is formed, its charge is 
a)
negative
b)
neutral (no charge)
c)
positive
105.

In ionic compounds electrons are

a)

transferred

b)

shared

c)

lost

d)

both shared and exchanged

106.
A charged particle that has gained or lost electrons is called a _____.
a)
molecule
b)
ion
c)
isotope
d)
element
107.

What happens when two negatively charged ions are pushed together?

a)

they will repel (move apart)

b)

they will be attracted to each other (move together)

108.

What happens when two oppositely charged ions are pushed together?

a)

they will repel (move apart)

b)

they will be attracted to each other (move together)

109.
If I gain electrons I become
a)
Positive because I've added to my atom
b)
negative because I've added electrons
c)
same because i'm balanced
d)
equal because now I have electrons
110.
Metals tend to 
a)
gain electrons
b)
lose electrons
111.
Nonmetals tend to 
a)
gain electrons
b)
lose electrons
112.
When an ionic compound is formed, its charge is 
a)
negative
b)
neutral (no charge)
c)
positive
113.
Valence electrons are: 
a)
Electrons farthest away from the nucleus
b)
Electrons closest to the nucleus
c)
Electrons that just come and go - they don't stay with the atom
d)
Electrons in the second shell
114.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Noble Gas Family

d)

Transition Metal Family

115.
Which element has a full valence shell?
a)
F
b)
D
c)
C
d)
E
116.

Which element has 3 valence electrons?

a)

A

b)

B

c)

E

d)

C

117.
Which elements have the same number of valence electrons?
a)
A & C
b)
E & C
c)
F & A
d)
F & B
118.
Which elements are in the same period?
a)
A & F
b)
F, B & D
c)
E & D
d)
F & B
119.
How many valence electrons does an atom of oxygen have?
a)
2
b)
5
c)
6
d)
16
120.
List the two most reactive families on the periodic table.
a)
Alkali metals & Transition Metals
b)
Noble gases & Oxygen Family
c)
Halogens & Alkali metals
d)
Halogens & Noble gases
121.

How many valence electrons do the atoms of elements in group 13 have (the Boron Group)?

a)

3

b)

5

c)

8

d)

13

122.
a)
Periods
b)
Groups
123.
a)
Periods
b)
Groups
124.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
125.
a)
energy levels
b)
valence electrons
c)
protons
d)
neutrons
126.
a)
Same group
b)
Same period
127.
a)
Group 1
b)
Group 17
c)
Group 2
d)
Group 18
128.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
129.
a)
Group 1
b)
Group 17
c)
Group 18
d)
Group 2
130.
a)
Metals
b)
Nonmetals
c)
Metalloids
131.
a)
Metals
b)
Nonmetals
c)
Metalloids
132.
a)
Metals
b)
Nonmetals
c)
Metalloids
133.
a)
Metals
b)
Nonmetals
c)
Metalloids
134.
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. 
135.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
136.
What is ionization energy?
a)
Energy needed to destroy an atom
b)
Energy required to remove an electron
c)
Energy needed to split an electron
d)
Energy required to add an electron
137.
a)
metric ruler
b)
Celsius thermometer
c)
graduated cylinders
d)
pan balances
138.

What is used to swirl, mix, or store chemicals?

a)

Beaker

b)

Flask

c)

Test Tube

d)

Graduated Cylinder

139.
This item is used to simply hold or approximately measure a liquid.
a)
beaker
b)
flask
c)
graduated cylinder
d)
test tube
140.

All matter is made of what

a)

energy

b)

atoms

c)

electrons

d)

compounds

141.

The positive particles of an atom are

a)

electrons

b)

positrons

c)

neutrons

d)

protons

142.

The central region of an atom where its neutrons and protons are is its

a)

nucleus

b)

electron cloud

c)

core

d)

center

143.

An atom with atomic number 6 would have how many protons

a)

6

b)

12

c)

3

d)

cannot be determined

144.

Particles in an atom that are neutral and have no charge are

a)

negatrons

b)

electrons

c)

neutrons

d)

protons

145.

A particle that moves around the nucleus is a(n)...

a)

Proton

b)

Neutron

c)

Electron

d)

Quark

146.

In the modern periodic table, elements are arranged by:

a)

atomic mass

b)

atomic number

c)

valence electrons

d)

number of isotopes

147.

What particle uniquely identifies an element?

a)

Number of Valence Electrons

b)

Number of Protons

c)

Number of Electrons

d)

Atomic Mass

148.

Electrons are___________

a)

Extremely small even in comparison to protons.

b)

part of the nuclues.

c)

Super Positive, like cheerleaders!

d)

very large

149.
electrons have this type of charge?
a)
negative
b)
positive
c)
neutral
150.
An atom's mass number equals the number of...
a)
protons plus the number of electrons
b)
protons plus the number of neutrons
c)
protons
d)
neutrons
151.

Which group is referred to as Alkali Metals?

a)

3

b)

1

c)

7

d)

17

152.
The majority of elements on the periodic table are
a)
man made.
b)
nonmetals.
c)
metals.
d)
gases.
153.

Name group 1A on the periodic table.

a)

alkali metals

b)

alkaline earth metals

c)

noble gases

noble gases

d)

halogens

154.
Name group 2A on the periodic table.
a)
alkali metals
b)
alkaline earth metals
c)
noble gases
d)
transition metals
155.

Name group 18 on the periodic table.

a)

alkali metals

b)

alkaline earth metals

c)

transition metals

d)

noble gases

156.
Name groups 3B - 12B on the periodic table.
a)
noble gases
b)
halogens
c)
metalloids
d)
transition metals
157.

Name group 17 on the periodic table.

a)

transition metals

b)

metalloids

c)

halogens

d)

alkali metals

158.

What are the vertical columns on the periodic called?

a)

groups

b)

periods

c)

nonmetals

d)

metals

e)

metalloids

159.
How many electrons does Oxygen need to fill its outer shell?
a)
3
b)
4
c)
1
d)
2
160.
How many valence electrons are found in atoms of group 1?
a)
7
b)
6
c)
4
d)
1
161.

What is the charge (oxidation number) of Magnesium (Mg)?

a)

+2

b)

-2

c)

+4

d)

-4

162.

What is the charge of ( oxidation number) for Flourine (F)?

a)

+1

b)

-1

c)

17

d)

7

163.

All matter is made of what

a)

energy

b)

atoms

c)

electrons

d)

compounds

164.
What is mass?
a)
How much MATTER makes up an object.
b)
How much GRAVITY is pulling an object.
165.
The force of gravity acting on an object is the object's ______.
a)
mass
b)
matter
c)
weight 
d)
friction 
166.

This subatomic particle holds the atom together

a)

proton

b)

electron

c)

neutron

d)

plasma

167.

Who is buried in Grant's tomb?

a)

Grant

b)

Coach Reid

168.

What class does Coach Reid teach?

a)

Orchestra

b)

Chemistry

c)

Band

169.

When was the war of 1812?

a)

1812

b)

1999

170.
The energy of waves _______ as the wavelength gets shorter.
a)
increases
b)
decreases
c)
stays the same
171.

The energy of waves _______ as the wavelength gets shorter, making the waves closer together.

a)

increases

b)

decreases

c)

doesn't change

172.

What charge does an atom have when it GAINS electrons?

a)

Positive

b)

Negative

c)

Neutral

173.

What is a representation of an ion?

a)

Li

b)

Na-22

c)

O-2

174.

What does it change in an ion?

a)

The number of electrons

b)

The number of protons

c)

The number of neutrons

175.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
176.
Balance the following reaction :
 
CaC₂(s)   +   H₂O(l)   -->   C₂H₂(g)   +   Ca(OH)₂(aq)
a)
1,2,2,2
b)
1,2,1,1
c)
2,1,1,1
d)
2,1,2,1
177.

The abbreviation STP stands for______________.

a)

Stoichiometry Temperature Probability

b)

Solid Temperature Practice

c)

Standard Temperature Pressure

178.

Temperature at STP is

a)

0 celsius

b)

100 celsius

c)

0 Kelvin

d)

212 F

179.

Pressure at STP is

a)

1 atmosphere

b)

1 Torr

c)

100 atmosphere

d)

6.02 hexallion

180.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

181.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more nuetrons
182.
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.
183.
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 
184.

An atom with atomic number 6 would have how many protons

a)

6

b)

12

c)

3

d)

cannot be determined

185.

In the modern periodic table, elements are arranged by:

a)

atomic mass

b)

atomic number

c)

valence electrons

d)

number of isotopes

186.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
187.
What is the molar mass of NaOH?
a)
40 g/mol
b)
38.989 g/mol
c)
23.998 g/mol
d)
57.004 g/mol
188.
As atoms of elements in group 16 are considered in order from top to bottom, the electronegativity of each successive element....
a)
decreases
b)
increases
c)
remains the same
d)
none of the above
189.
As you move down the periodic table atoms get bigger.  This is because ____________.
a)
The atoms have more mass.
b)
The atoms have more protons.
c)
The atoms have more energy levels
d)
The atoms have more neutrons
190.
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. 
191.
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
192.
Which end of the water molecule has a slightly positive charge?
a)
the oxygen end
b)
the hydrogen end
c)
both ends are slightly positive
d)
neither end is positive
193.

Used to describe a molecule that has an unequal distribution of charges (positive and negative)

a)

non polar

b)

element

c)

polar

d)

chemicals

194.

A weak bond formed by the attraction of more positively charged H on one molecule and the more negatively charged O (or N or F) on a different molecule.

a)

ionic

b)

covalent

c)

hydrogen

195.

Refer to the picture of water sticking to a leaf; this is occurring because of:

a)

Adhesion

b)

Cohesion

196.

Describe COHESION.

a)

Water molecules attracted to other substances.

b)

Water molecules climbing upwards against the force of gravity.

c)

Water molecules dissolving many substances because of its polarity.

d)

Water molecules attracted to other water molecules.

197.
What is adhesion?
a)
Water's ability to stick to itself
b)
Water's ability to stick to other substances
c)
The strength of the cohesion of all the water molecules combined
d)
Tape, glue and other adhesives
198.

The amount of heat needed to increase the temperature of a substance by 1 degree Celcius.

a)

surface tension

b)

specific heat

c)

universal solvent

d)

capillary action

199.

The water stays cool when the weather is hot due to the property of:

a)

cohesionn

b)

specific heat

c)

surface tension

d)

adhesion

200.

Which atom has the largest atomic radius?

a)

potassium

b)

rubidium

c)

francium

d)

cesium

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