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Periodic Table & Trends Quiz Review

Total questions: 97

Worksheet time: 2hrs 37mins

Name
Class
Date
1.

The ability to attract an electron in a chemical bond

a)

electronegativity

b)

electron affinity

c)

metallic character

d)

ionization energy

2.

The energy it takes to remove an electron from an atom in the gas phase

a)

electron affinity

b)

electronegativity

c)

metallic character

d)

ionization energy

3.

Ionization energy increases

a)

from L to R and from bottom to top

b)

from L to R and from top to bottom

c)

from R to L and from bottom to top

d)

from R to L and from top to bottom

4.

metallic character is greatest

a)

in the top right corner

b)

in the bottom right corner

c)

in the top left corner

d)

in the bottom left corner

5.
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
6.
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
7.
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)
8.

Atomic radius decreases from left to right across a period because from left to right there is

a)

increasing number of valence electrons

b)

increasing shielding

c)

increasing effective nuclear charge

d)

increasing number of protons in the nucleus

9.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
10.

The element with the highest electronegativity is -

a)

At

b)

F

c)

Cl

d)

Br

11.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
12.

Which atom has the smallest metallic character?

a)

O

b)

Ba

c)

Co

d)

K

13.

The ionization energy of Na is larger than Cs because...

a)

Na has a greater effective nuclear charge

b)

Na has fewer energy levels and less shielding

c)

Cs has a greater effective nuclear charge than Na

d)

Cs has more valence electrons than Na

14.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
15.

As you move from top to bottom down a group on the periodic table, the number of valence electrons ___ .

a)

Decreases

b)

Increases

c)

Stays the same

16.

As you move from left to right across a period of the periodic table, the number of valence electrons ___.

a)

Decreases

b)

Increases

c)

Stays the same

17.

As you move from top to bottom down a group on the periodic table, the number of energy levels ___.

a)

Decreases

b)

Increases

c)

Stays the same

18.

As you move from left to right across a period of the periodic table, the number of energy levels ___.

a)

Decreases

b)

Increases

c)

Stays the same

19.

Which of the following elements has the greatest amount of energy levels?

a)

Boron

b)

Gallium

c)

Thallium

d)

They have the same number of energy levels.

20.

As we travel from RIGHT to LEFT on the periodic table, ionization energy ________.

a)

Increases

b)

Decreases

c)

Stays the same

21.

Which of the group 13 elements is the smallest?

a)

B

b)

Ti

c)

Fr

d)

Ga

22.

If an electron is closer to the nucleus, it will be (harder, easier) to remove that electron and its ionization energy will be (high, low )

a)

Easier, High

b)

Easier, Low

c)

Harder, High

d)

Harder, Low

23.
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
24.

Of the following pictured ions and atom, which would have the largest atomic radius

a)
b)
c)

You can't tell from the pictures

d)
25.
Which has the greater EN: 
Cl or Al?
a)
Cl
b)
Al
26.
Which has the greater EN: 
H or F?
a)
H
b)
F
27.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
28.
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
29.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
30.
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
31.
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.
32.
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
33.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
34.

Which statement correctly and completely identifies a trend?

a)

Atomic radius is highest in the lower left part of the periodic table and smallest in the upper right part of the periodic table

b)

Electronegativity lowest in the upper right part of the periodic table and highest in the lower left part of the periodic table

c)

Ionization energy lowest in the upper right part of the periodic table and highest in the lower left part of the periodic table.

d)

Metallic character is lowest in the lower left part of the periodic table and highest in the upper right part of the periodic table

35.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

36.
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
37.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
38.

Electronegativity is...

a)

the ability of an atom to attract/ accept electrons in a compound

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.

39.

A measure of the size of an atom, and is generally defined as the distance from the nucleus to the outermost electron orbit

a)

chemical reactivity

b)

atomic radius

c)

energy levels

d)

orbit

40.
Which element has the greatest electronegativity: Nitrogen (N) or Arsenic (As)?
a)
Nitrogen (N)
b)
Arsenic (As)
41.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
42.

(select 2) Ionization energy increases as you move

a)

Down a Group

b)

Up a Group

c)

Left to Right across a Period

d)

Right to Left across a Period

43.

(select 2) Electronegativity energy increases as you move

a)

Down a Group

b)

Up a Group

c)

Left to Right across a Period

d)

Right to Left across a Period

44.

(select 2) Atomic Radius energy increases as you move

a)

Down a Group

b)

Up a Group

c)

Left to Right across a Period

d)

Right to Left across a Period

45.
Atomic Radius is...
a)
the relative size of the atom's nucleus
b)
the relative size of the atom's electron cloud
c)
the energy required to shield the outer electrons from the nucleus
d)
a measure of the ability of an atom to attract electrons
46.
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.
47.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
48.
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)
49.
Which of the following will have a higher ionization energy than arsenic (As)?
a)
Gallium (Ga)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
50.
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. 
51.
What term is used to describe "an atom's tendency to attract electrons to itself when is is chemically combined with another element"
a)
electronation
b)
electron affinity
c)
electronegativity
d)
electrolysis
52.
Electronegativity __________ from left to right within a period and __________ from top to bottom within a group.
a)
decreases, increases 
b)
increases, increases
c)
increases, decreases 
d)
stays the same, increases
53.
Sodium (Na) and potassium (K) are in the same group on the periodic table. Based on their locations, which statement about sodium and potassium is true?
a)
Sodium is less electronegative than potassium. 
b)
Sodium has fewer energy levels than potassium. 
c)
Sodium has a larger ionic radius than potassium. 
d)
Sodium has lower ionization energy than potassium. 
54.

which of the following families is the least electronegative?

a)

noble gases

b)

Halogens

c)

transition metals

d)

alkali metals

55.
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
56.
The picture shows what trend?
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
57.
Which of the following sequences corresponds to a correct trend in ionization energy?
a)
Cl > S > P > Al
b)
Sr > Ca > Mg > Be
c)
Rb > K > Na > Li
d)
Rb > Sr > I > Xe
58.

The name given to vertical (up and down) columns of the periodic table

a)

Group or Famly

b)

Period

59.

The charge of an atom that has an equal number of protons and electrons

a)

Protons

b)

Neutral

c)

Electrons

60.

This tells you the total number of protons plus the neutrons in an atom

a)

Atomic Number

b)

Valence

c)

Atomic Mass

61.

The name given to the horizontal (side to side) rows of the period table

a)

Group or Family

b)

Period

62.

This tells you the number of protons in an atom

a)

Atomic Number

b)

Atomic Mass

c)

AMU

63.

The name of the particles in the furthest shell

a)

Electrons

b)

Neutrons

c)

Protons

d)

Valence Electrons

64.

How many protons does this element have?

a)

7

b)

8

c)

9

65.

How many electrons does this element have?

a)

7

b)

8

c)

9

66.

You have an that has an atomic mass of 23 and an atomic number of 11. How many neutrons does it have?

a)

12

b)

13

c)

14

d)

11

67.

Elements between metals and nonmetals are called

a)

Gasses

b)

Metalloids

c)

Radioactive

68.

What is the name of group number 1?

a)

halogens

b)

noble gases

c)

alkali metals

d)

alkaline earth metals

69.

Which element is found in group 2, period 6?

a)

Oxygen (O)

b)

Barium (Ba)

c)

Selenium (Se)

d)

Carbon (C)

70.

Which halogen is found in period 4?

a)

Krypton (Kr)

b)

Xenon (Xe)

c)

Bromine (Br)

d)

Iodine (I)

71.
Which of the following atomic symbols for bromine is written correctly?
a)
bR
b)
BR
c)
Br
d)
br
72.
Elements which are shiny, conduct electricity and heat are called
a)
metal
b)
nonmetal
c)
metalloid
d)
nonexistent
73.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
74.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
75.

 Using your periodic table, locate the element with the average atomic mass of 101.07  What is the element symbol for this element?

a)

Me (mendelevium)

b)

Os (osium)

c)

Ru (ruthenium)

d)

No (nobelium)

76.

All atoms of a given element contain:

a)

the same number of protons

b)

the same number of neutrons

c)

the same number of electrons

d)

the same number of protons, neutrons, and electrons

e)

none of the subatomic particles will be the same - every atom is different

77.

Using your periodic table, locate the element with the atomic number  of 35.  What is the element name for this element?

a)

B (boron)

b)

He (helium)

c)

Cl (chlorine)

d)

Br (bromine)

78.

What do elements in the same group on the periodic table have in common?

a)

They have the same number of protons.

b)

They have the same atomic number.

c)

They have similar chemical symbols.

d)

They have the same number of valence electrons.

e)

They have the same average atomic mass.

79.

 Elements on the periodic table are classified into which three major categories (classes)?

a)

atomic number, chemical symbol, element name

b)

solid, liquid, gas

c)

metals, nonmetals, metalloids

d)

period, row, columns

80.

. The periodic table has a lot of information in the form of letters and number.  The information is organized into boxes, which are placed into rows and columns. Which of the following does each box represent?

a)

a group

b)

a period

c)

an element

d)

an atom

81.

What is true about the position of all metals in the periodic table?

a)

They are in the group 3.

b)

They are in period 1.

c)

They are to the right of the zigzag line created by the metalloids.

d)

They are to the left of the zigzag line created by the metalloids.

e)

They are the touching the zigzag line created by the metalloids.

82.

What is true about the position of all nonmetals in the periodic table?

a)

They are in group 13.

b)

They are in period 3.

c)

They are to the right of the zigzag line created by the metalloids.

d)

They are to the left of the zigzag line created by the metalloids.

e)

They are the touching the zigzag line created by the metalloids.

83.

Which describe how elements are arranged in the periodic table?

a)

by decreasing atomic number

b)

alphabetical order by element symbol

c)

by increasing atomic mass

d)

by increasing atomic number

e)

by decreasing atomic mass

84.

. ______________ are elements that have some properties of metals and some properties of nonmetals.

a)

metals

b)

nonmetals

c)

metalloids

d)

gasses

85.

______________ are elements that are good conductors of heat and electricity.  They are usually shiny and malleable.

a)

metals

b)

nonmetals

c)

metalloids

d)

gasses

86.

______________ are elements that are poor conductors of heat and electricity.  They are usually dull and brittle.

a)

metals

b)

nonmetals

c)

metalloids

d)

gasses

87.

______________ is credited with creating the periodic table.

a)

Sir Isaac Newton

b)

Albert Einstein

c)

Marie Curie

d)

Dmitri Mendeleev

88.

 The periodic table ______________.

a)

has never changed since the time of Aristotle.

b)

changes whenever someone makes a claim that it should whether or not there is evidence.

c)

always has been the same and will never change.

d)

changes as scientist have new data about new elements.

89.

If scientists discover a new element, what would happen to the current periodic table?

a)

It has never changed since the time of Aristotle so the element wouldn’t be added.

b)

Nothing would happen. 

c)

It would change to include the new element as long there was enough evidence to prove that it really existed.

d)

It would be added to the new periodic table in 2100 as new elements can only be added every 100 years.

90.

Elements in the same column have the same number of 

valence electrons which results in them having similar 

___________.

a)

atomic mass

b)

color

c)

physical properties

d)

chemical properties

91.

_________ is an element with an atomic number of 19 that can 

be found in the periodic table.

a)

calcium

b)

potassium

c)

chlorine

d)

flourine

92.

______ is the element with the fewest protons that can 

be found in the periodic table.

a)

hydrogen

b)

helium

c)

oganesson

d)

lawrencium

93.
Most of the elements on the periodic table are classified as _____.
a)
Metals
b)
Nonmetals
c)
Metalloids
d)
Periods
94.

The first orbital can hold ______ electrons.

a)

2

b)

8

c)

18

d)

0

95.

the positively charged subatomic particle contained in the nucleus of an atom

a)

proton

b)

neutron

c)

electron

d)

matter

96.

a subatomic particle, contained in the nucleus of an atom, having the same mass as a proton but no electrical charge

a)

proton

b)

neutron

c)

electron

d)

matter

97.

a negatively charged subatomic particle that orbits the nucleus of an atom

a)

proton

b)

neutron

c)

electron

d)

matter

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