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Periodic Trends Review

Total questions: 41

Worksheet time: 40mins

Name
Class
Date
1.
Which of the following will have a higher electronegativity than arsenic (As)?
a)
Carbon (C)
b)
Neon (Ne)
c)
Antimony (Sb)
d)
Germanium (Ge)
2.
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
3.
Which atom has the largest atomic radius?
a)
potassium
b)
rubidium 
c)
francium
d)
cesium
4.
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
5.
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.
6.
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.
7.
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. 
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.
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
10.
The element with the smallest ionization energy in Period 6 is - 
a)
Rn
b)
Cs
c)
Os
d)
Tm
11.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

12.

What is a positively-charged ion which forms when an atom loses electrons?

a)

atom

b)

ion

c)

cation

d)

anion

13.

What is a negatively-charged ion which forms when an atom gains electrons?

a)

cation

b)

anion

c)

electron

d)

ion

14.

An element has similar chemical properties as oxygen and selenium. It has an atomic number greater than krypton but less than iodine. Use the periodic table to identify the element

a)

selenium

b)

polonium

c)

tellurium

d)

sulfur

15.

Which atom is more electronegative?

a)

K

b)

Rb

c)

Cl

d)

B

16.

How many valence electrons does a neutral atom of nitrogen have?

a)

2

b)

4

c)

5

d)

6

17.

Which has a lower ionization energy: Lithium or Potassium?

a)

Lithium

b)

Potassium

18.

Which of the following has a larger radius than Zinc

a)

Gallium

b)

Magnesium

c)

Strontium

d)

Aluminum

19.

If a potassium atom lost one electron, it becomes an ion. What would be the symbol for that ion?

a)

b)

c)

d)

20.

Which of the following elements is the most electronegative?

a)

Hydrogen, H

b)

Aluminum, Al

c)

Oxygen, O

d)

Cesium, Cs

21.

What is the ion formed from Sulfur? If it has 6 valence electrons.

a)

S+2

b)

S-2

c)

S+6

d)

S-6

22.

How many electrons would a Calcium ion gain/lose? If it has 2 valence electrons.

a)

lose 1

b)

gain 1

c)

lose 2

d)

gain 2

23.

How many valence electrons does an atom of silicon have?

a)

3

b)

4

c)

5

d)

6

24.

Be, Mg, and Ca have ___ valence electrons.

a)

1

b)

2

c)

3

d)

4

25.

Atoms will gain or lose electrons in order to have a full outer energy level this is called the _____ rule.

a)

valence

b)

cation

c)

octet

d)

anion

26.
What charge will an Oxygen ion have? 
a)
+1
b)
-1
c)
+2
d)
-2
27.
How many valence electrons does Carbon have?
a)
4
b)
12
c)
6
d)
14
28.

What will be the charge of this atom after it has been ionized?

a)

-2

b)

-1

c)

+1

d)

+2

29.

Which atom has the HIGHEST ionization energy (energy to remove 1 electron)

a)
b)
c)
30.

This atom will form a

a)

Cation

b)

Anion

31.

Anion are made by _______ electrons from an atom.

a)

removing

b)

adding

32.

What is the name of the family that is highlighted?

a)

Alkali Metal Family

b)

Halogen Family

c)

Alkaline Earth Metals

d)

Transition Metal Family

33.
Which of the following is a transition metal? 
a)
Iron
b)
Oxygen
c)
Neon
d)
Barium
34.
Which of the following is a Halogen? 
a)
Bromine
b)
Rubidium
c)
Argon
d)
Beryllium
35.
Which of the following is a Noble Gas? 
a)
Krypton
b)
Chlorine
c)
Radium
d)
Gallium
36.
Which of the following is an Alkali Metal? 
a)
Magnesium
b)
Chromium
c)
Sodium
d)
Fluorine 
37.

Which ion has the smaller radius?

a)

P-3

b)

Cl-1

c)

S-2

d)

all are anions in the same period so they are the same size

38.

Which is larger:

P or P-3 ?

a)

P because it is the neutral atom.

b)

P-3 because it lost 3 electrons.

c)

P-3 because it gained 3 electrons.

d)

They are the same size since they are both P.

39.

Which is the smaller atom: Mg or Mg+2?

a)

Mg because it gains an energy level since it gains 2 electrons.

b)

Mg due to extra electron repulsion created by gaining 2 electrons.

c)

Mg+2 because of extra electron repulsion created by gaining 2 electrons.

d)

Mg+2 because it loses an energy level since it loses 2 electrons.

40.

Arrange the following by decreasing ionic radius: Ag+1, In+3, Cd+2, Sn+4?

a)

Ag+1, In+3, Cd+2, Sn+4

b)

Ag+1, Cd+2, In+3, Sn+4

c)

Sn+4, In+3, Cd+2, Ag+1

d)

Sn+4, Cd+2, In+3, Ag+1

41.

  • Which of the following in this isoelectric series would be the smallest?

  • Kr, Se2-, Sr2+, Br-

a)

Kr

b)

Se2-

c)

Sr2+

d)

Br-

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