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The Periodic Table Unit 4 Review

Total questions: 40

Worksheet time: 28mins

Name
Class
Date
1.
Which of the following will have a larger radius than Zinc?
a)
Gallium
b)
Aluminum
c)
Magnesium
d)
Strontium
2.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
3.
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)
4.
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
5.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
6.
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
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.
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
9.
The atom with the largest atomic radius in Group 18 is - 
a)
Ar
b)
He
c)
Kr
d)
Rn
10.
Which statement correctly and completely identifies a trend?
a)
Atomic radius decreases across a period and increases down a group.
b)
Electronegativity decreases across a period and decreases down a group.
c)
Ionization energy increases across a period and increases down a group.
d)
Ionic radius increases across a period and increases down a group.
11.
The element with the largest electronegativity in the halogens is - 
a)
At
b)
F
c)
Cl
d)
Br
12.

The element with the lowest electronegativity in Period 3 is -

a)

Na

b)

Cl

c)

Ar

d)

Mg

13.
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 
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 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
16.
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
17.
What is the name of family I
a)
Alkaline Earth Metals
b)
Boron Family
c)
Alkali Metals
d)
Halogen Family
18.
Group B is known as the:
a)
Inner Metals
b)
Transition Metals
c)
Weirdos
d)
Changelings 
19.
Families all have similar 
a)
Names
b)
atomic numbers
c)
atomic masses
d)
properties
20.
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
21.
What is an ion?
a)
A Charged Atom
b)
A Large Atom
c)
A Small Atom
d)
A Cute Atom
22.

What is the charge of a sodium ion?

a)

+2

b)

+1

c)

-1

d)

-2

23.
Group 17 always has ions with a charge of 
a)
+1
b)
+2
c)
-1
d)
-2
24.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
25.
Which of the following has a -3 charge?
a)
Boron
b)
Fluorine
c)
Nitrogen
d)
Neon
26.
Elements on the LEFT side of the periodic table will most likely form:
a)
Positive ions
b)
Negative ions
c)
Neutral Ions
d)
None of these
27.
Cations are...
a)
Positive
b)
Negative
c)
Neutral
d)
Purring
28.
Anions are...
a)
Positive
b)
Negative
c)
Neutral
d)
Crying
29.
An atom becomes _______ when it loses electrons.
a)
Positive
b)
Negative
c)
Neutral
d)
Invinsible
30.

The electron configuration below is for which element?

1s22s22p63s23p64s23d10

a)

Zinc

b)

Copper

c)

Nickel

d)

Germanium

31.

Which electron configuration belongs to chlorine (Cl)?

a)

1s2 2s2 2p6 3s2 3p5

b)

1s2 2s2 2p6 3s2 3p6

c)

1s2 2s2 2p6 3s2 3p7

32.

The electron configuration below is for which element?1s22s22p63s2

a)

Neon

b)

Magnesium

c)

Aluminum

d)

Potassium

33.

Which of the following is the electron configuration for iron?

a)

1s22s22p63s23p64s23d6

b)

1s22s22p63s23p63d8

c)

1s22p63s23p64s23d6

d)

1s22s22p63s23p64s13d6

34.

What is meant by isolectronic?

a)

Group of atoms or ions that have the same electronic configuration

b)

Group of atoms or ions that have the same protonic configuration

c)

Group of atoms or ions that have the same electrical properties

d)

Group of atoms or ions that have the same electron charge

35.

What is the example of species that are isolectronic?

a)

Na+ and Si4+

b)

Na+ and Cl-

c)

Mg2+ and Al +

d)

S2- and O2-

36.

Which species is larger?

a)

Ne

b)

F-

37.

Which species is smaller?

a)

P3-

b)

Cl-

38.

Arrange these species in decreasing order of size.

F- , Na+ , Mg2+ , O2- , Al3+ , Ne

a)

Al3+ > Mg2+ > Na+ > Ne > F- > O2-

b)

O2- > F- > Ne > Na+ > Mg2+ > Al3+

c)

Al3+ < Mg2+ < Na+ < Ne < F- < O2-

d)

O2- < F- < Ne < Na+ < Mg2+ < Al3+

39.

Arrange these species in increasing order of size.

Cl- , Ca2+ , S2- , Ar , K+

a)

Ca2+ > K+ > Ar > Cl- > S2-

b)

S2- > Cl- > Ar > K+ > Ca2+

c)

Ca2+ < K+ < Ar < Cl- < S2-

d)

S2- < Cl- < Ar < K+ < Ca2+

40.

Which of the following statements is true regarding the ion for aluminum.

a)

The aluminum atom loses 3 electrons forming an ion with a charge of -3

b)

The aluminum atom loses 1 electron forming an ion with a charge of -1

c)

The aluminum atom loses 1 electron forming an ion with a charge of +1

d)

The aluminum atom loses electrons forming an ion with a charge of +3

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