Free Printable Exam Review Practice

1.

Which group in the periodic table contains the alkali metals?

a)

Group 2

b)

Group 1

c)

Group 17

d)

Group 18

2.

How many valence electrons do the noble gases (except Helium) have?

a)

2

b)

6

c)

8

d)

7

3.

What is the common oxidation number (ion charge) for halogens?

a)

$+1$

b)

$-2$

c)

$-1$

d)

$+2$

4.

Which of the following elements is an alkaline earth metal?

a)

Sodium

b)

Magnesium

c)

Chlorine

d)

Neon

5.

Which group is known as the chalcogens?

a)

Group 1

b)

Group 2

c)

Group 16

d)

Group 18

6.

What is the full electron configuration for phosphorus ( $Z=15$ )?

a)

$1s^2 2s^2 2p^6 3s^2 3p^3$

b)

$1s^2 2s^2 2p^6 3s^2 3p^5$

c)

$1s^2 2s^2 2p^6 3s^2 3p^6$

d)

$1s^2 2s^2 2p^6 3s^2 3p^1$

7.

Which of the following is a transition element?

a)

Calcium

b)

Iron

c)

Sodium

d)

Argon

8.

What is the noble gas configuration for sodium ( $Z=11$ )?

a)

[Ne] $3s^1$

b)

[He] $2s^2 2p^6 3s^1$

c)

[Ar] $4s^1$

d)

[He] $2s^2 2p^6$

9.

Which element in Period 2 has a full valence shell?

a)

Neon

b)

Oxygen

c)

Fluorine

d)

Nitrogen

10.

Which of the following is an inner transition element?

a)

Lanthanum

b)

Potassium

c)

Sulfur

d)

Zinc

11.

Which property is characteristic of alkali metals?

a)

High melting points

b)

React vigorously with water

c)

Form $-2$ ions

d)

Are gases at room temperature

12.

What is the valence electron configuration for magnesium ( $Z=12$ )?

a)

$3s^2$

b)

$2p^6$

c)

$3p^2$

d)

$2s^2$

13.

Which of the following elements would most likely form a $+2$ ion?

a)

Sodium

b)

Calcium

c)

Chlorine

d)

Argon

14.

Which group contains elements that are all diatomic in their natural state?

a)

Alkali metals

b)

Halogens

c)

Noble gases

d)

Alkaline earth metals

15.

Which of the following ions has the same electron configuration as neon?

a)

$Na^+$

b)

$Mg^{2+}$

c)

$F^-$

d)

All of the above

16.

Which element in the third period has the highest first ionization energy?

a)

Sodium

b)

Magnesium

c)

Phosphorus

d)

Argon

17.

Which of the following best explains why halogens are highly reactive?

a)

They have a full valence shell

b)

They need one more electron to achieve a full valence shell

c)

They have low electronegativity

d)

They are metals

18.

Given the electron configuration $1s^2 2s^2 2p^6 3s^2 3p^4$ , what is the element and its most common ion?

a)

Sulfur, $S^{2-}$

b)

Phosphorus, $P^{3-}$

c)

Chlorine, $Cl^-$

d)

Oxygen, $O^{2-}$

19.

A student is given the following electron configuration: $[Ne] 3s^2 3p^5$ . Which element is this, and what is its likely ion charge?

a)

Chlorine, $-1$

b)

Argon, $0$

c)

Sulfur, $-2$

d)

Sodium, $+1$

20.

Which of the following statements best describes the difference between transition and inner transition elements?

a)

Transition elements are found in the s-block, inner transition elements are in the p-block

b)

Transition elements are in groups 3-12, inner transition elements are the lanthanides and actinides

c)

Transition elements are nonmetals, inner transition elements are metals

d)

Transition elements have full d-subshells, inner transition elements have full f-subshells

21.

Which of the following would create an ion with a +2 charge?

a)

Lithium

b)

Nitrogen

c)

Chlorine

d)

Calcium

22.

Which of the following would create an ion with a -3 charge?

a)

Nitrogen

b)

Aluminum

c)

Sulfur

d)

Potassium

23.

What is the charge of tin in Tin (IV) Oxide?

a)

+4

b)

-4

c)

+2

d)

-2

24.

What is the charge of Iron in the following compound?

FeCl₃

a)

+1

b)

-1

c)

+3

d)

-3

25.

What Periodic Table family is represented by the Lewis dot diagram?

a)

Halogens

b)

Alkali Metals

c)

Transition Metals

d)

Noble Gases

26.

What is the total number of electrons found in the valence shell of a halogen in the ground state?

a)

1

b)

7

c)

2

d)

8

27.

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

28.

What two types of atoms make a covalent bond?

a)

metal atom and metal atom

b)

metal atom and non metal non atom

c)

non metal atom and non metal atom

29.

Atoms are most stable when their outer shell is full or complete.

a)

True

b)

False

30.

Atoms involved in a covalent bond are not charged, while atoms involved in an ionic bond are charged (negative or positive)

a)

True

b)

False

31.

Which of the pair of elements form an ionic bond?

a)

Magnesium and Oxygen

b)

Magnesium and Sodium

c)

Iron and Zinc

d)

Nitrogen and Hydrogen

32.

If an atom gains two electrons what charge will it have?

a)

-2

b)

-1

c)

+1

d)

+2

33.

What is the noble gas shorthand electron for Sulfur atom?

a)

[Ar] 3p⁴

b)

[He] 3s²3p⁴

c)

[Ne] 3s²3p⁴

d)

[Na] 3s²3p⁴

34.

What atom matches this electron configuration?
[Xe] 6s²4f¹⁴5d⁹

a)

Mercury

b)

Gold

c)

Platinum

d)

Thallium

Exam Review Practice

Total questions: 34

Worksheet time: 17mins

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