Free Printable Unit 2/3 Test Electrons & Periodic Table

1.

What is the electron configuration of a neutral carbon atom?

a)

$1s^2 2s^2 2p^2$

b)

$1s^2 2s^2 2p^4$

c)

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

d)

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

2.

Which of the following elements has the smallest atomic radius?

a)

Lithium (Li)

b)

Beryllium (Be)

c)

Boron (B)

d)

Carbon (C)

3.

Describe the trend in atomic radius as you move down a group in the periodic table.

a)

It decreases

b)

It increases

c)

It remains constant

d)

It fluctuates

4.

Which of the following elements is most electronegative?

a)

Hydrogen (H)

b)

Carbon (C)

c)

Nitrogen (N)

d)

Oxygen (O)

5.

Explain why ionization energy generally increases across a period from left to right.

a)

Increased nuclear charge attracts electrons more strongly

b)

Decreased nuclear charge allows electrons to spread out

c)

Additional electron shells are added

d)

Electrons are lost, reducing size

6.

Predict the electron configuration of a chlorine atom

a)

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

b)

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

c)

$1s^2 2s^2 2p^6 3s^2 3p^4$

d)

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

7.

Which of the following statements best explains why electronegativity decreases down a group?

a)

Electrons are added to the same energy level

b)

Electrons are added to higher energy levels, increasing distance from the nucleus

c)

Nuclear charge decreases

d)

Electrons are removed from the outer shell

8.

What is the general trend of ionization energy as you move down a group in the periodic table?

a)

It increases

b)

It decreases

c)

It remains constant

d)

It fluctuates

9.

Identify the element with the electron configuration $[Ar] 4s^2 3d^{10} 4p^5$ .

a)

Bromine (Br)

b)

Krypton (Kr)

c)

Selenium (Se)

d)

Arsenic (As)

10.

How does the electron configuration of noble gases differ from that of other elements?

a)

Noble gases have completely filled valence shells

b)

Noble gases have partially filled d subshells

c)

Noble gases have no s subshells

d)

Noble gases have filled f subshells

11.

Which of the following elements would you expect to have the highest first ionization energy?

a)

Lithium (Li)

b)

Beryllium (Be)

c)

Boron (B)

d)

Carbon (C)

12.

Which of the following elements has the largest atomic radius?

a)

Helium (He)

b)

Neon (Ne)

c)

Argon (Ar)

d)

Xenon (Xe)

13.

Explain why alkali metals have low ionization energies.

a)

They have a single electron in their outer shell, which is easily removed

b)

They have high nuclear charge

c)

They have small atomic radii

d)

They have high electronegativity

14.

Which of the following best describes the trend in electronegativity as you move across a period from left to right?

a)

It decreases

b)

It increases

c)

It remains constant

d)

It fluctuates

15.

Which of the following elements is expected to have the highest electronegativity?

a)

Fluorine (F)

b)

Chlorine (Cl)

c)

Bromine (Br)

d)

Iodine (I)

16.

Of the halogens, which has the smallest radius?

a)

F

b)

Br

c)

He

d)

At

17.

Which of the following elements is a noble gas?

a)

Oxygen (O)

b)

Neon (Ne)

c)

Nitrogen (N)

d)

Hydrogen (H)

18.

Which of the following elements has the highest first ionization energy?

a)

Sodium (Na)

b)

Magnesium (Mg)

c)

Aluminum (Al)

d)

Phosphorus (P)

19.

What happens to Group 1 metals when they are put into water?

a)

Group 1 metals dissolve in water without any reaction.

b)

Group 1 metals explode upon contact with water.

c)

They do not react because they are noble gases.

d)

They melt and become liquid.

20.

What is the following electron configuration written in shorthand form?

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p4

a)

[Ar] 4s2 3d10 4p2

b)

[Ar] 4s2 3d10 4p6

c)

[Ar] 4s2 3d10 4p4

d)

[Ar] 4s2 3d6 4p4

21.

Which of the following is the correct electron configuration for a neutral sulfur atom?

a)

$1s^2 2s^2 2p^6 3s^2 3p^4$

b)

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

c)

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

d)

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

22.

This orbital diagram represents:

a)

C

b)

B

c)

N

d)

O

23.

Which element is pictured?

a)

neon

b)

fluorine

c)

magnesium

d)

argon

24.

What is the correct noble-gas notation for the electron configuration of an atom of chlorine?

a)

a. [Ar]3s² 3p⁵

b)

b. [Ne]3s² 3p⁴

c)

c. [Ar]3s² 3p⁴

d)

d. [Ne]3s² 3p⁵

25.

Who is the father of the periodic table?

a)

Dmitri Mendeleev

b)

Niels Bohr

c)

Isaac Newton

d)

Albert Einstein

26.

The electromagnetic waves with the highest frequencies and the shortest wavelength are called

a)

radio waves

b)

gamma rays

c)

x-rays

d)

visible light

27.

What color has the highest energy?

a)

red

b)

violet

c)

green

d)

orange

28.

This could be the dot diagram of

a)

Si

b)

Br

c)

B

d)

S

29.

How would you draw a Lewis dot diagram for Magnesium?

a)

b)

c)

d)

30.

On the periodic table the group number gives you the

a)

number of valence electrons in the outer shell

b)

number of total electrons

c)

number of energy levels

d)

atomic number of the element

31.

On the periodic table the period number give you the

a)

The number of valence electrons

b)

The number of protons in the nucleus.

c)

The highest energy level of electrons in the elements.

d)

The number of total electrons

32.

The symbols W, X, Y, and Z represent four elements shown on the outline of a periodic table.
Which element has the highest atomic size?

a)

W

b)

X

c)

Y

d)

Z

Unit 2/3 Test Electrons & Periodic Table

Total questions: 32

Worksheet time: 37mins

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