Free Printable Practice--Periodic Table and Shorthand Electron Configuration

1.

What is the shorthand electron configuration for chlorine (Cl)?

a)

[Ne] $3s^2 3p^5$

b)

[Ar] $4s^2 3d^{10} 4p^5$

c)

[He] $2s^2 2p^5$

d)

[Ar] $3s^2 3p^5$

2.

How many valence electrons does sulfur (S) have?

a)

16

b)

6

c)

2

d)

8

3.

Which orbital notation correctly represents the valence electrons of oxygen?

a)

$2s^2 2p^4$

b)

$2s^2 2p^6$

c)

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

d)

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

4.

Identify the valence electron configuration for magnesium (Mg).

a)

$3s^2$

b)

$2s^2 2p^6$

c)

$3s^1$

d)

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

5.

What is the total number of electrons in the $p$ orbitals of chlorine's valence shell?

a)

5

b)

6

c)

7

d)

8

6.

Using shorthand notation, write the electron configuration for potassium (K).

a)

[Ne] $4s^1$

b)

[Ar] $4s^1$

c)

[He] $3s^1$

d)

[Ne] $3s^2 3p^6 4s^1$

7.

Calculate the number of valence electrons in phosphorus (P).

a)

3

b)

5

c)

15

d)

2

8.

Which of the following represents the orbital notation for the valence electrons of nitrogen?

a)

$2s^2 2p^3$

b)

$2s^2 2p^5$

c)

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

d)

$1s^2 2s^2 2p^5$

9.

Determine the shorthand electron configuration for copper (Cu).

a)

[Ar] $4s^1 3d^{10}$

b)

[Ne] $3s^2 3p^6 3d^9 4s^2$

c)

[Ar] $3d^9 4s^2$

d)

[Kr] $4d^{10} 5s^1$

10.

How many valence electrons are present in an atom of aluminum (Al)?

a)

13

b)

3

c)

5

d)

2

11.

Explain why the valence electron configuration of calcium (Ca) is $4s^2$ .

a)

Calcium is in the second group and loses two electrons to achieve a noble gas configuration.

b)

Calcium has a total of 20 electrons, and the last two are in the $4s$ orbital.

c)

The $4s$ orbital is the highest energy level filled in calcium.

d)

All of the above are correct.

12.

Using orbital notation, show the arrangement of valence electrons for silicon (Si).

a)

$3s^2 3p^2$

b)

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

c)

$2s^2 2p^2$

d)

$3s^2 3p^6$

13.

Predict the shorthand electron configuration for bromine (Br), and explain the reasoning.

a)

[Ar] $4s^2 3d^{10} 4p^5$ ; Bromine follows argon in the periodic table, filling the $4s$ , $3d$ , and $4p$ orbitals.

b)

[Kr] $5s^2 4d^{10} 5p^5$ ; Bromine is in the same group as chlorine and follows a similar electron configuration pattern.

c)

[Ne] $3s^2 3p^5$ ; Bromine needs to gain one electron to achieve a noble gas configuration.

d)

[Ar] $3d^{10} 4s^2 4p^5$ ; Bromine is one electron short of krypton, making this configuration correct.

14.

What is the significance of valence electrons in chemical bonding?

a)

They determine the atom's core structure.

b)

They are involved in forming chemical bonds.

c)

They are only present in metals.

d)

They have no significant role in chemistry.

15.

Design a process to determine the number of valence electrons in an unknown element using its position in the periodic table.

a)

Count the total electrons and subtract the number of core electrons based on the nearest noble gas.

b)

Identify the group number for main-group elements; this often equals the number of valence electrons.

c)

Use X-ray spectroscopy to directly observe the electron configuration.

d)

Calculate the atomic mass and divide by the atomic number.

16.

Before Mendeleev's table, how were elements arranged in order to classify them?

a)

In order of atomic mass

b)

In order of atomic weight

c)

By physical and chemical properties

d)

They weren't

17.

What were some problems with the early versions of the periodic table?

a)

Some elements had not been discovered so the tables were not complete.

b)

The elements did not follow a regular pattern.

c)

The weight of some elements had been calculated incorrectly.

d)

Elements were placed in order of atomic weight, so some ended up in the wrong group.

18.

How did Mendeleev overcome some of the problems in his version of the periodic table?

a)

He made up new elements to fill in gaps.

b)

He left gaps for undiscovered elements.

c)

He ordered the elements in terms of atomic mass.

d)

He placed elements in groups according to similar properties.

19.

In the periodic table, the (a) number tells us the number of electron shells in an atom.

20.

In the periodic table, the (a) number tells us the number of electrons in the outer shell of an atom.

21.

The order of elements in the periodic table is based on

a)

the number of protons in the nucleus.

b)

the electric charge of the nucleus.

c)

the number of neutrons in the nucleus.

d)

atomic mass.

22.

Atoms of elements that are in the same group have the same number of

a)

protons.

b)

neutrons.

c)

valence electrons.

d)

protons and neutrons.

23.

In Mendeleev's periodic table, elements in each column had similar

a)

atomic masses.

b)

properties.

c)

atomic numbers.

d)

symbols.

24.

Mendeleev left gaps in his periodic table because

a)

the table was too small.

b)

protons belonged there.

c)

the table was too full.

d)

no known elements fit there.

25.

Each column of the periodic table is

a)

an element.

b)

a group.

c)

an isotope.

d)

a period.

26.

The order of elements in the modern periodic table is based on an element's

a)

atomic number.

b)

name.

c)

chemical symbol.

d)

atomic mass.

27.

In which period is an element that has the electron configuration 1s²2s²2p⁶3s²3p⁶3d¹⁰4s²4p¹ when it is in its ground state?

a)

Period 1

b)

Period 2

c)

Period 3

d)

Period 4

28.

What law states that when elements are organized in order of increasing atomic number their chemical and physical properties will repeat?

a)

Periodic Law

b)

Periodicity Law

c)

Law of Property Repetition

d)

None of these

29.

If the f block contains 14 columns, then it would make sense that an f orbital can hold up to _____ electrons.

a)

2

b)

5

c)

7

d)

14

30.

Look at a periodic table. Count how many columns on the periodic table are in the "p" block. How many columns did you find?

a)

2

b)

6

c)

10

d)

14

Practice--Periodic Table and Shorthand Electron Configuration

Total questions: 30

Worksheet time: 18mins

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