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WorksheetsPeriodic Trends
Total questions: 84
Worksheet time: 3hrs 4mins
Name
Class
Date
1.
As you move down a group, atomic radius increases because -
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
2.
The atom with the largest atomic radius in Group 18 is -
a)
Ar
b)
He
c)
Kr
d)
Rn
3.
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
4.
The atom with the largest atomic radius in Period 4 (row 4) is -
a)
K
b)
Kr
c)
Fe
d)
Fe
5.
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
6.
The element with the smallest ionization energy in Period 6 is -
a)
Rn
b)
Cs
c)
Os
d)
Tm
7.
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.
8.
The energy required to remove electrons is the definition of:
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
9.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
10.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings
11.
Families all have similar
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
12.
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.
13.
Which has the greater Electronegativity:
N or C?
N or C?
a)
C
b)
N
14.
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
15.
As you move down a group, atomic radius increases because -
a)
you add more and more neutrons
b)
you add more and more protons
c)
you add more and more shells (energy levels)
d)
you add more atomic mass
16.
The atom with the largest atomic radius in Group 18 is -
a)
Ar
b)
He
c)
Kr
d)
Rn
17.
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
18.
The atom with the largest atomic radius in Period 4 (row 4) is -
a)
K
b)
Kr
c)
Fe
d)
Fe
19.
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
20.
The element with the smallest ionization energy in Period 6 is -
a)
Rn
b)
Cs
c)
Os
d)
Tm
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.
The energy required to remove electrons is the definition of:
a)
Electronegativity
b)
Atomic Number
c)
Atomic Radius
d)
Ionization
23.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
24.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings
25.
Families all have similar
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
26.
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.
27.
Which has the greater Electronegativity:
N or C?
N or C?
a)
C
b)
N
28.
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
29.
Which element has the greater ionization energy?
a)
Magnesium
b)
Phosphorus
30.
Put the following in order of increasing ionization energy:Strontium, Aluminum, Indium
a)
Strontium, Indium, Aluminum
b)
Strontium, Aluminum, Indium
c)
Indium, Aluminum, Strontium
d)
Aluminum, Indium, Strontium
31.
Put the following in order of increasing ionization energy:Cobalt, Tungsten, Ruthenium
a)
Tungsten, Ruthenium, Cobalt
b)
Cobalt, Tungsten, Ruthenium
c)
Ruthenium, Cobalt, Tungsten
d)
Cobalt, Ruthenium, Tungsten
32.
Put these in increasing order of atomic radii:
F, N, B
F, N, B
a)
B < N < F
b)
B < F < N
c)
N < F < B
d)
F < N < B
33.
The element with the lowest electronegativity in Period 3 is -
a)
Na
b)
Cl
c)
Ar
d)
Mg
34.
Which of the following elements has the smallest atomic radius: Li, O, C, F?
a)
Li
b)
O
c)
C
d)
F
35.
Of the elements Ca, Be, Ba, and Sr, which has the largest atomic radius?
a)
Be
b)
Ba
c)
Ca
d)
Sr
36.
Rank the following elements by increasing atomic radius:
carbon, aluminum, oxygen, phosphorus.
Not sure? check out page 151 in your textbook
carbon, aluminum, oxygen, phosphorus.
Not sure? check out page 151 in your textbook
a)
O, C, P, Al
b)
Al, P, C, O
c)
O,P, C, Al
d)
O, P, Al, C
37.
The general trend of metal ion size is that they decrease in size as you move from ______ to ______ on the PT.
a)
Right to left
b)
Left to right
c)
Diagonally
d)
Top to bottom
38.
The general trend of non-metal ion size is that they increase in size as you move from ______ to ______ on the PT.
a)
Left to right
b)
Bottom to top
c)
Top to bottom
39.
What element is the MOST reactive metal on the PT?
a)
Cu
b)
Mn
c)
F
d)
Fr
40.
Which element is a metalloid?
a)
S
b)
Br
c)
As
d)
Au
41.
Alkali metals are characterized by their...
a)
Formation of +2 charges
b)
High levels of reactivity
c)
Low melting points
d)
valence electrons in the "p" block
42.
Noble gases are characterized by...
a)
High reactivity
b)
Being solid at room temperature
c)
Low ionization energy
d)
Full valence shell of electrons
43.
Calcium belongs to which orbital block? (s, p, d, or f)
a)
s
b)
p
c)
d
d)
f
44.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
45.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
46.
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)
47.
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
48.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium
c)
francium
d)
cesium
49.
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
50.
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.
51.
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.
52.
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.
53.
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
54.
Metals have the largest -
a)
atomic radius and electronegativity
b)
electronegativity and ionization energy
c)
atomic radius only
d)
ionization energy and atomic radius
55.
The element with the largest electronegativity in the halogens is -
a)
At
b)
F
c)
Cl
d)
Br
56.
The element with the lowest electronegativity in Period 3 is -
a)
Na
b)
Cl
c)
Ar
d)
Mg
57.
The electronegativity of Cl is the highest in Period 3. Why?
a)
Cl is the largest and has the greatest effective nuclear charge
b)
Cl is the smallest and has the lowest effective nuclear charge
c)
Cl is the largest and has the lowest effective nuclear charge
d)
Cl is the smallest and has the greatest effective nuclear charge
58.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
59.
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
60.
The core of an atom where most of the mass of an atom exists; contains protons and neutrons
a)
nucleus
b)
electron shell
c)
proton
d)
electron
61.
The minimum energy required to remove an electron from the ground state of an atom
a)
electron configuration
b)
energy levels
c)
ionization energy
d)
ionic bond
62.
A negatively charged subatomic particle that exists in various energy levels outside the nucleus of an atom
a)
neutron
b)
electron
c)
proton
d)
subatomic particle
63.
The chart scientists use to organize and classify all the known elements
a)
elements chart
b)
the chart
c)
Periodic Table of the Elements
d)
Period table
64.
The tendency of an atom to attract electrons and acquire a negative charge
a)
electronegativity
b)
charge
c)
bonding ability
d)
electron configuration
65.
The energies of electrons as they orbit the nucleus of an atom
a)
energy levels
b)
orbits
c)
shells
d)
electron area
66.
An electron that resides in the outermost shell, or principal quantum level, of an atom
a)
periodic trend
b)
electron shell
c)
ionic radius
d)
valence electron
67.
In which of the following atoms is the 2s orbital closest to the nucleus? (Bonus question, worth 2 marks.)
a)
S
b)
Cl
c)
P
d)
Si
e)
They are the same distance in all of these atoms.
68.
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
69.
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
70.
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.
71.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium
c)
francium
d)
cesium
72.
The atom with the largest atomic radius in Group 18 is -
a)
Ar
b)
He
c)
Kr
d)
Rn
73.
Which periodic group has the smallest atomic radius?
a)
Alkali metals
b)
Halogens
c)
Noble Gases
d)
Transition metals
74.
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
75.
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)
76.
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)
77.
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.
78.
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.
79.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
80.
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
81.
The electronegativity of Cl is the highest in Period 2. Why?
a)
Cl is the largest and has the greatest effective nuclear charge
b)
Cl is the smallest and has the lowest effective nuclear charge
c)
Cl is the largest and has the lowest effective nuclear charge
d)
Cl is the smallest and has the greatest effective nuclear charge
82.
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
83.
What term is used to describe "The energy required to remove an electron from gaseous atoms"
a)
excitation energy
b)
ionization energy
c)
polarization energy
d)
electrolytic energy
84.
What term is used to describe "A measure of the size of an atom"
a)
chemical reactivity
b)
atomic radius
c)
energy levels
d)
orbit
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