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WorksheetsPeriodic Table Review
Total questions: 80
Worksheet time: 52mins
Name
Class
Date
1.
Elements that are poor conductors of heat and electricity. Many are gasses at room temperature
a)
metals
b)
nonmetals
c)
metalloids
d)
transition metals
2.
What is the name of the group that has the MOST reactive METALS in it?
a)
Alkaline earth
b)
Alkali
c)
transition
d)
actinides
3.
Beryllium is in group number______.
a)
Group 2
b)
Group 3
c)
Group 4
d)
Group 7
4.
The period for Bromine is ___________.
a)
3
b)
2
c)
4
5.
What is the name of the group that has the MOST reactive NONMETALS in it?
a)
alkali
b)
alkaline earth
c)
noble gases
d)
halogens
6.
What name is given to the elements in Groups 3 through 12?
a)
Transition Metals
b)
Alkaline Earth Metals
c)
Rare Earth Metals
d)
Alkali Metals
7.
If a metal reacts violently with water, in which group is it likely to be found?
a)
Group 1
b)
Group 2
c)
Group 7
d)
Group 8
8.
Which group of elements reacts violently with elements in Group 1?
a)
Group 15
b)
Group 16
c)
Group 17
d)
Group 18
9.
What kinds of properties do metalloids have elements tend to have?
a)
Metalloids can be shiny or dull, malleable, ductile, brittle, and conduct electricity.
b)
Metalloids have luster, are malleable, ductile and good conductors of heat and electricity.
c)
Metalloids have not luster, are brittle, not ductile, not malleable and poor conductors of electricity.
10.
Locate the box in Group 18 in the fourth period. Predict the state of matter and the chemical reactivity of the element that belongs in that box.
a)
The element is a gas, one of the halogen gases. It does not ordinarily react with other elements to form compounds.
b)
The element is a gas, one of the noble gases. It does ordinarily react with other elements to form compounds.
c)
The element is a gas, one of the noble gases. It does not ordinarily react with other elements to form compounds.
d)
The element is a gas, hydrogen gas. It does ordinarily react with other elements to form compounds.
11.
Group 18 elements are known as the _____ _____ and have full valence shells.
a)
royal gases.
b)
supreme solids.
c)
noble gases.
d)
legit liquids.
12.
Elements in the same ________ are more chemically similar.
a)
group
b)
period
c)
club
d)
table
13.
The alkali metals and alkaline earth metals are very reactive because they _____ their valence electrons easily.
a)
lose
b)
add
c)
gain
d)
spin
14.
__________ , including Silicon and Germanium, are considered "semiconductors" and are used in making electronics.
a)
Rare earth metals
b)
Metalloids
c)
Transition metals
15.
Within a period (row), this is responsible for explaining changes in periodic trends
a)
Shielding effect
b)
Number of core electrons
c)
Effective nuclear charge
d)
The number of valence electrons
16.
The element that will require the least amount of energy to remove an electron is
a)
sodium
b)
magnesium
c)
calcium
d)
potassium
17.
When phosphorus becomes an ion it is most likely that it will
a)
gain 5 electrons
b)
lose 5 electrons
c)
gain 3 electrons
d)
lose 3 electrons
18.
Across a period, left to right, the trend in electronegativity
a)
stays constant
b)
tends to increase
c)
tends to decrease
19.
The group of elements that does not have electronegativity values is
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
noble gases
20.
When magnesium becomes an ion it _____ electrons and gets _____ in size.
a)
gains, smaller
b)
gains, larger
c)
loses, smaller
d)
loses, larger
21.
When oxygen becomes an ion, it _____ electrons and becomes _____ in size.
a)
gains, smaller
b)
gains, larger
c)
loses, smaller
d)
loses, larger
22.
Which of the following is the smallest atom?
a)
boron
b)
carbon
c)
silicon
d)
aluminum
23.
Which of the following is the largest?
a)
potassium
b)
carbon
c)
bromine
d)
cesium
24.
Which of the following elements will attract electrons in a bond most strongly?
a)
gallium
b)
sodium
c)
oxygen
d)
barium
25.
Which of the following will require the least energy to remove an electron?
a)
lithium
b)
beryllium
c)
nitrogen
d)
oxygen
26.
Which of the following elements is the largest when it becomes an ion?
a)
sodium
b)
magnesium
c)
aluminum
d)
phosphorus
27.
Which is smaller, a potassium ion or a chlorine ion?
a)
potassium ion
b)
chlorine ion
c)
they are equal in size
28.
The ability of an atom to attract electrons in a bond is called
a)
atomic radius
b)
electronegativity
c)
ionization energy
d)
anionization
29.
Why does group number 18 have the least reactive elements?
a)
They all have an odd number of protons.
b)
They all have an even number of protons.
c)
They have the largest masses.
d)
Their electron shells are the most filled and do not need to be very reactive.
30.
Which group contains: chlorine, fluorine, bromine, iodine, astatine?
a)
Group 18-Noble Gases
b)
Group 16-Oxygen Family
c)
Group 17-Halogen Family
d)
Group 15-Nitrogen Family
31.
What period and group is Silver (Ag)?
a)
Period 2, Group 1
b)
Period 3, Group 16
c)
Period 5, Group 11
d)
Period 2, 14
32.
What period and group is Fluorine on the periodic table?
a)
Period 7, Group 3
b)
Period 5, Group 4
c)
Period 2, Group 17
d)
Period 8, Group 2
33.
Which of the following elements has the highest ionization energy?
a)
sodium
b)
aluminum
c)
calcium
d)
phosphorus
34.
Which elements have the most similar chemical properties?
a)
K and Na
b)
K and Ca
c)
K and Cl
d)
K and S
35.
Which element in period four is a metalloid?
a)
Silicon
b)
Gallium
c)
Arsenic
d)
Titanium
36.
Which group of elements tends to make ions with a charge of +2?
a)
alkali metals
b)
alkaline earth metals
c)
halogens
d)
the nitrogen group
37.
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
38.
The atomic radius of main-group elements generally increases down a group because ________.
a)
effective nuclear charge increases down a group
b)
effective nuclear charge decreases down a group
c)
effective nuclear charge zigzags down a group
d)
the principal quantum number of the valence orbitals increases
39.
Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)?
a)
F < K < Ge < Br < Rb
b)
F < Ge < Br < K < Rb
c)
F < K < Br < Ge < Rb
d)
F < Br < Ge < K < Rb
40.
Which of the following correctly lists the five atoms in order of increasing size (smallest to largest)?
a)
O < F < S < Mg < Ba
b)
F < O < S < Mg < Ba
c)
F < O < S < Ba < Mg
d)
O < F < S < Ba < Mg
41.
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
42.
In general, as you go across a period in the periodic table from left to right: (1) the atomic radius __________; (2) the electronegativity __________; and (3) the first ionization energy __________.
a)
decreases, decreases, increases
b)
increases, increases, decreases
c)
increases, increases, increases
d)
decreases, increases, increases
43.
The first ionization energies of the elements __________ as you go from left to right across a period of the periodic table, and __________ as you go from the bottom to the top of a group in the table.
a)
increase, increase
b)
increase, decrease
c)
decrease, increase
d)
decrease, decrease
44.
Of the choices below, which gives the order for first ionization energies?
a)
Cl > S > Al > Ar > Si
b)
Ar > Cl > S > Si > Al
c)
Al > Si > S > Cl > Ar
d)
Cl > S > Al > Si > Ar
45.
Of the following atoms, which has the largest first ionization energy?
a)
Br
b)
O
c)
C
d)
P
46.
__________ have the lowest first ionization energies of the groups listed.
a)
Alkali metals
b)
Transition metals
c)
Halogens
d)
Alkaline Earth metals
47.
The list that correctly indicates the order of metallic character is __________.
a)
B > N > C
b)
F > Cl > S
c)
Si > P > S
d)
P > S > Se
48.
Which of the following sets of elements are ranked in order of INCREASING ionization energy?
a)
B, C, N, O
b)
F, Cl, Br, I
c)
Cr, V, Ti, Sc
d)
Zn, Ag, Pt, Mt
49.
Which of the following sets of elements are ranked in order of INCREASING atomic radius?
a)
Rb, Sr, Y, Zr
b)
Kr, Br, Cl, S
c)
Sr, Ca, Mg, Be
d)
He, H, Be, Li
50.
Which of the following electron configurations is most likely to form an anion?
a)
1s22s2
b)
1s22s22p1
c)
1s22s22p6
d)
1s22s22p4
51.
Put the following elements in order of increasing atomic radius:
Rb, Na, K, Fr.
Rb, Na, K, Fr.
a)
Rb, Na, K, Fr
b)
K, Rb, Fr, Na
c)
Fr, K, Na, Rb
d)
Na, K, Rb, Fr
52.
Based on electronegativity trends in the periodic table, which of the following is the most likely value for the electronegativity of silicon?
a)
2.44
b)
1.23
c)
2.22
d)
2.03
53.
What is this element?
1s22s22p63s23p64s23d10
1s22s22p63s23p64s23d10
a)
Zinc
b)
Copper
c)
Nickel
d)
Germanium
54.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
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.
Chlorine is more electronegative than sulfur due to
a)
The number of valence electrons
b)
Shielding effect
c)
Effective nuclear charge
d)
Number of core electrons
57.
Which of the following would have a larger ionic radius than atomic radius?
a)
Aluminum
b)
Calcium
c)
Zinc
d)
Oxygen
58.
The tendency of an atom to attract electrons is called...
a)
ionization energy
b)
electronegativity
c)
atomic radius
d)
ionic radius
59.
Ionization energy is the amount of energy required to remove the electron that is closest to the nucleus.
a)
True
b)
False
60.
An atom with more electrons than protons is called...
a)
cation
b)
anion
c)
neutral
d)
shielded
61.
Why is this statement untrue? A cation has a positive charge because it has gained electrons.
a)
Cations are negative.
b)
This would describe anions.
c)
A cation's positive charge is due to lost electrons.
d)
The statement is actually true.
62.
Which of the following elements would be smaller as an ion than as a neutral atom?
a)
Fluorine
b)
Phosphorus
c)
Iodine
d)
Aluminum
63.
Which of the following would have a larger ionic radius than atomic radius?
a)
Aluminum
b)
Calcium
c)
Zinc
d)
Oxygen
64.
Which of the following elements are in order from lowest electronegativity to highest?
a)
F, N, B, Li
b)
Ga, Si, O, He
c)
K, Al, C, F
d)
Mg, V, Mo, Os
65.
Which of the following trends would be higher for noble gases than for alkali metals?
a)
atomic radius
b)
electronegativity
c)
ionization energy
d)
ionic radius
66.
Which of the following would be higher for alkali metals than for halogens?
a)
atomic radius
b)
ionic radius
c)
electronegativity
d)
ionization energy
67.
Helium has the highest...
a)
electronegativity
b)
ionization energy
c)
atomic radius
d)
valence electrons
68.
Which of the following is NOT true about a phosphorus ion?
a)
It is a cation.
b)
It has a -3 charge to meet the octet rule.
c)
It is larger than a neutral phosphorus atom.
d)
It has more electrons than a neutral chlorine atom.
69.
Which of these has the largest atomic radius?
a)
Fluorine
b)
Arsenic
c)
Calcium
d)
Rubidium
70.
Which of these has the highest electronegativity?
a)
Sulfur
b)
Germanium
c)
Scandium
d)
Cesium
71.
Which is not true of atomic radius?
a)
Larger going down due to added energy levels expanding the size of the atom.
b)
Larger going across from left to right due to increasing nuclear charge.
c)
Noble gases have the smallest atomic radius due to highest number of protons in each period.
d)
Strontium atoms are larger than iodine atoms because iodine has more protons.
72.
Why does fluorine have a higher ionization energy than iodine?
a)
The outer electrons are farther away from the nucleus in an iodine atom, so the attraction is lower.
b)
There are more electrons in the inner shells of a fluorine atom, so the outer electrons are shielded from the nuclear charge.
c)
Actually, iodine has a higher ionization energy than fluorine because it has a higher atomic number.
d)
Iodine has more valence electrons than fluorine.
73.
The transition metal with the highest ionization energy is...
a)
Mercury (Hg)
b)
Zinc (Zn)
c)
Scandium (Sc)
d)
Lawrencium (Lr)
74.
List the following atoms in order of increasing electronegativity: O, Al, Ca
a)
O, Al, Ca
b)
Ca, Al, O
c)
Al, Ca, O
d)
O, Ca, Al
75.
Elements that tend to gain electrons for stability have the largest _____.
a)
atomic radius only
b)
ionization energy only
c)
ionization energy and electronegativity
d)
atomic radius and electronegativity
76.
Rn has the lowest first ionization energy in Group 18. Why?
a)
The shielding effect in Rn is the greatest, so Rn's nucleus feels low attraction for valence electrons
b)
The shielding effect in Rn is the lowest, so Rn's nucleus feels high attraction for valence electrons
c)
Rn has the most protons in Group 18, so Rn's nucleus feels high attraction for valence electrons
d)
Rn has the most electrons in Group 18, so Rn has the lowest amount of electron repulsion
77.
Why is the electronegativity of noble gases always zero?
a)
Noble gases have the lowest effective nuclear charge in their period
b)
Noble gases have the highest first ionization energies in their period
c)
Noble gases are chemically stable and have a full stable valence energy level
d)
Noble gases are the smallest atoms in their period
78.
Which has the LARGEST atomic radius?
a)
N
b)
N-3
c)
N-2
d)
N+5
79.
How does ionization energy change as you go down a family?
a)
It doesn't
b)
It increases
c)
It decreases
80.
How does ionization energy change as you go across a period ?
a)
It doesn't
b)
It increases
c)
It decreases
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