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Periodic Table & Trends

Total questions: 122

Worksheet time: 6hrs 12mins

Name
Class
Date
1.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

2.

The vertical (up and down) columns in the Periodic Table are called

a)

groups

b)

towers

c)

periods

d)

atomic numbers

3.
The Modern Periodic Table of Elements is arranged by
a)
atomic mass
b)
atomic number
c)
valence electrons
d)
number of isotopes
4.
The atoms along the staircase are called 
a)
metals
b)
nonmetals
c)
metalloids
d)
noble gases
5.
Which is a halogen?
a)
Helium
b)
Chlorine
c)
Oxygen
d)
Neptune
6.
Which is an alkali metal?
a)
Magnesium
b)
Iron
c)
Sodium
d)
Europium
7.
Elements in a ..................have similar chemical properties.  
a)
period
b)
group
c)
row
8.
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
9.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
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.
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
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.
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
14.
a)
2
b)
3
c)
5
15.
How many valence electrons are in an atom of K?
a)
3
b)
8
c)
4
d)
1
16.
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
17.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
18.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
19.
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
20.
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
21.
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.
22.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
23.
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
24.
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 
25.
Vertical columns of elements (families) on the periodic table with similar  properties
a)
groups
b)
periods
c)
quadrants
d)
rows
26.
Which element could be lustrous and brittle?
a)
A
b)
B
c)
G
d)
L
27.

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

28.

Which element has 3 valence electrons?

a)

A

b)

B

c)

E

d)

C

29.
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. 
30.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
31.
Which of these elements has an electron structure most similar to that of element X?
a)
1
b)
2
c)
3
d)
4
32.
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)
33.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
34.

What happens to the atomic numbers as you move from left to right on the periodic table?

a)

Increase

b)

Decrease

c)

Stay the same

d)

Nothing

35.

Which of the following elements is most likely to have similar properties to those of sodium (Na)?

a)

Magnesium (Mg)

b)

Sulfur (S)

c)

Francium (Fr)

d)

Titanium (Ti)

36.

Two elements that have similar physical and chemical properties are most likely in the same...

a)

period

b)

row

c)

group

37.

Which element is located in period 4 and group 5?

a)

Vanadium (V)

b)

Zirconium (Zr)

c)

Niobium (Nb)

d)

Titanium (Ti)

38.

In which group would an element that is a gas most likely be located?

a)

1

b)

3

c)

12

d)

18

39.
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
40.
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. 
41.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
42.

As you move down a group on the periodic table, the number of valence electrons....

a)

Increases

b)

Decreases

c)

Remains the same

43.

As you move from left to right on the periodic table, the number of valence electrons.......

a)

Increases

b)

Decreases

c)

Remains the same

44.

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

a)

+1

b)

+7

c)

-7

d)

-1

e)

17

45.

Which of the following is true of atomic radius?

a)

The radius is mainly due to how large an atom's nucleus is.

b)

The radius is mainly due to the size of the electron cloud.

c)

The atomic radius is a way we measure the mass of an atom.

d)

Neutrons account for the majority of an atom's radius.

46.
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
47.
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 
48.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
49.

As you move from left to right on the periodic table, the number of valence electrons.......

a)

Increases

b)

Decreases

c)

Remains the same

50.

As you move down a group on the periodic table, the number of valence electrons....

a)

Increases

b)

Decreases

c)

Remains the same

51.

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

a)

+1

b)

+7

c)

-7

d)

-1

e)

17

52.

Which of the following is true of atomic radius?

a)

The radius is mainly due to how large an atom's nucleus is.

b)

The radius is mainly due to the size of the electron cloud.

c)

The atomic radius is a way we measure the mass of an atom.

d)

Neutrons account for the majority of an atom's radius.

53.

Why are elements at the bottom of the PT larger than those at the top?

a)

They have more orbitals

b)

They have more valence electrons

c)

They have more charge

d)

They have a weaker attraction

54.

Why are elements at the top of the PT have higher electronegativity than those at the bottom?

a)

They have fewer orbitals, this makes them smaller and since electrons are closer to the nucleus there will be a stronger ability to attract electrons

b)

They have fewer valence electrons

c)

They have more orbitals, this makes them larger and since electrons are further from the nucleus there will be a stronger ability to attract electrons

55.

Why are elements at the top of the PT have higher ionization energy than those at the bottom?

a)

They have fewer orbitals, this makes them smaller and since electrons are closer to the nucleus the attraction is stronger which makes it more difficult to remove

b)

They have fewer valence electrons

c)

They have more orbitals, this makes them larger and since electrons are further from the nucleus the attraction is weaker which make it easier to remove

56.

Why are elements at the left of the PT larger than those at right?

a)

They have fewer orbitals

b)

They have more valence electrons

c)

Their electrons have a stronger attraction because there's more charge

d)

Their electrons have a weaker attraction because there's less charge

57.

Why are elements at the right of the PT have more electronegativity than those at left?

a)

They have fewer orbitals

b)

They have more charge which gives them a stronger attraction for electrons. (Non-metals form anions)

c)

The have less valence electrons

d)

They have less charge which gives them a stronger attraction. (Metals form cations)

58.

Why are elements at the right of the PT have higher ionization energy than those at left?

a)

They have more orbitals

b)

Since they are much larger its difficult to find their valence electrons

c)

They have more charge and are closer to completing the octet rule which is difficult to remove electrons

d)

They have less charge and its very easy to remove electrons from metals

59.

What is the difference between ionization energy and electronegativity?

a)

Ionization energy is the ability to attract a valence electron while, electronegativity is the energy needed to remove a valence electron.

b)

Ionization energy is the energy needed to remove a valence electron while, electronegativity is the ability to attract a valence electron.

c)

Ionization energy is the level of attraction between electrons and the nucleus while, electronegativity is the sharing of pairs of electrons.

60.

What is the difference between electronegativity and atomic radius?

a)

electronegativity is the level of attraction between electrons and the nucleus while, atomic radius is the energy needed to remove electrons.

b)

electronegativity is the energy needed to remove electrons while, atomic radius is the level of attraction between electrons and the nucleus.

c)

electronegativity is the level of attraction between electrons and the nucleus while, atomic radius is the size of the atom

61.

Beryllium (Be) has an atomic number of 4 & Magnesium (Mg) has an atomic number of 12. They have very similar chemical properties and will behave the same in a chemical reaction. How should they be placed on the periodic table?

a)

They should be placed in the same group with Mg on the top and Be below.

b)

They should be placed in the same group with Be on the top and Mg below.

c)

They should be placed in the same period with Mg on the left and Be on the right.

d)

They should be placed in the same period with Be on the left and Mg right.

62.

Which are 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

63.

What is it about group 1 and group 17 elements that make them so reactive?

a)

They have more orbitals than the rest of the elements

b)

They have less charge than the rest of the elements

c)

They are the two families that are closest to completing the octet rule

d)

They have more charge than the rest of the elements

64.
In which group does this atom belong?
a)
1
b)
3
c)
13
d)
11
65.

As you move down a group, atomic radius increases because...

a)

you add more and more valence electrons

b)

you add more and more protons

c)

you add more and more orbitals

d)

you add more and more charge

66.

Which element has a full valence shell and completed the octet rule?

a)

F

b)

D

c)

C

d)

E

67.

Which element has 3 valence electrons?

a)

A

b)

B

c)

E

d)

C

68.
Which elements are in the same period?
a)
A & F
b)
F, B & D
c)
E & D
d)
F & B
69.

Use your periodic table to rank the following elements according to their atomic radius (Smallest to Largest):


Nickel, Silver, Sulfur, Francium & Calcium.

a)

S < Ni < Ag < Ca < Fr

b)

S < Ag < Ni < Ca < Fr

c)

S < Ca < Ag < Ni < Fr

d)

Ni < Ag < S < Fr < Ca

70.

Use your periodic table to rank the following elements according to their Ionization Energy (Lowest to highest):


Carbon, Cobalt, Cesium, Helium & Krypton

a)

Cs < Co < C < Kr < He

b)

Cs < C < Co < Kr < He

c)

Cs < Kr < Co < C < He

d)

Co < C < Kr < Cs < He

71.

Use your periodic table to rank the following elements according to their Electronegativity (Lowest to highest):


Lithium, Titanium, Silicon, Fluorine & Nitrogen

a)

Li < Ti < Si < N < F

b)

Li < Si < N < Ti < F

c)

Li < N < Si < Ti < F

d)

Ti < Si < Li < F < N

72.

Use your periodic table to determine which of the following elements are larger than Sulfur (S):

(Select all that apply)

a)

Phosphorus (P)

b)

Arsenic (As)

c)

Chlorine (Cl)

d)

Nitrogen (N)

e)

Fluorine (F)

73.
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. 
74.
Which of these elements has the greatest atomic radius? 
a)
H
b)
N
c)
Cl
d)
Cs
75.
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.
76.
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
77.
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 
78.
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 
79.
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
80.
Which of these elements has an electron structure most similar to that of element X?
a)
1
b)
2
c)
3
d)
4
81.
Based on their locations in the periodic table, which element has chemical properties most similar to those of calcium, Ca?
a)
beryllium, Be
b)
potassium, K
c)
titanium, Ti
d)
yttrium, Y
82.
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)
83.
According to the Periodic Table of the Elements, which set of elements has similar properties?
a)
H, C, I
b)
He, H, Al
c)
He, Ne, Ar
d)
Na, Ca, Al
84.
What is the family name of this group of elements? 
a)
Alkali metals 
b)
Halogens 
c)
Noble Gases 
d)
Alkali Earth Metals 
85.
Which element has 2 valence electrons? 
a)
cesium (Cs) 
b)
magnesium (Mg)
c)
boron (B)
d)
argon (Ar) 
86.
How many Valance electrons does Iodine Have?
a)
6
b)
16
c)
7
d)
17
87.
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)
88.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
89.
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. 
90.
Metals have the largest - 
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
91.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
92.
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
93.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
94.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
95.
The element with the lowest electronegativity in Period 3 is - 
a)
Na
b)
Cl
c)
Ar
d)
Mg
96.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
97.
Which has the greater EN: 
N or C?
a)
C
b)
N
98.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
99.

Which of the alkaline-earth metals has the smallest electronegativity

a)

Be

b)

Sc

c)

Ra

d)

Sr

100.

Which alkali metal is the least reactive?

a)

Li

b)

Na

c)

H

d)

Fr

101.

Of the halogens, which has the smallest electronegativity?

a)

F

b)

Cl

c)

At

d)

Ne

102.

Which elements have 1 valence electron?

a)

period 1

b)

group 1

c)

group 4

103.

which elements have 4 valence electrons?

a)

group 3

b)

group 4

c)

group 14

104.

Which element is located in Group 11 & Period 4?

a)

Vanadium

b)

Cadmium

c)

Copper

d)

Rhodium

105.

What element is located in Group 18 & Period 5?

a)

Xenon

b)

Krypton

c)

Radon

d)

Helium

106.

Which element is located in Group 3 & Period 5?

a)

Yttrium

b)

Scandium

c)

Lanthanum

d)

Magnesium

107.

Which element is located in Group 5 & Period 4?

a)

Nitrogen

b)

Phosphorus

c)

Antimony

d)

Vandium

108.

Which element is located in Group 1 & Period 2?

a)

Hydrogen

b)

Beryllium

c)

Lithium

d)

Sodium

109.

Which of these has the smallest ionization energy?

a)

N

b)

P

c)

As

d)

Ne

110.

Which of these is a metal?

a)

Li

b)

Si

c)

S

d)

Ne

111.

Which of these has the largest atomic mass?

a)

K

b)

Ca

c)

Sc

112.
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)
113.

The element with the highest electronegativity is -

a)

At

b)

F

c)

Cl

d)

Br

114.

Which atom has the smallest metallic character?

a)

O

b)

Ba

c)

Co

d)

K

115.

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

116.

For groups 13 through 18, the number of valence electrons is equal to the group number

a)

plus 1

b)

plus the period number

c)

minus the period number

d)

minus 10

117.

Using just the valence electrons on each atom determine which 2 atoms should be in the same group.

a)

atom 1 and 2

b)

atom 3 and 4

c)

atom 1 and 4

d)

atom 2 and 3

118.
The atom with the largest atomic radius in Period 4 (row 4) is - 
a)
K
b)
Kr
c)
Fe
d)
Fe
119.
Which has the greater Electronegativity: 
N or C?
a)
C
b)
N
120.
Place the following elements in order of decreasing atomic radius: Cl, Mg, Al, Ca
a)
Ca, Mg, Al, Cl
b)
Mg, Al, Cl, Ca
c)
Ca, Al, Cl, Ca
d)
Cl, Al, Mg, Ca
121.

Where would you expect to find the smallest atoms?

a)

upper left

b)

upper right

c)

lower left

d)

lower right lower right

122.

Why are the ionic radii generally larger for group 15 than for group 17?

a)

Atoms in group 15 are larger than atoms in group 17.

b)

Atoms in group 15 have more protons than atoms in group 17

c)

Ions forming from group 15 atoms have a greater negative charge than ions forming from group 17 atoms.

d)

Atoms in group 15 are less likely to lose electrons than atoms in group 17.

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Billings Unit 1 Test Review

quiz

Worksheet

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9th - 12th Grade