Free Practice Quiz Question List

02/14 Atomic Structure and the Periodic Table Quiz Online Quiz Questions

Use this free practice quiz with 20 questions to review 02/14 Atomic Structure and the Periodic Table, test your knowledge, and prepare for your next test or exam.

20 questions

Choose one

1 point

How many protons and electrons are present in a $\mathrm{Mg^{2+}}$ ion?

A
12 protons and 12 electrons
B
12 protons and 10 electrons
C
10 protons and 12 electrons
D
10 protons and 10 electrons

True or false

1 point

True or false: An atomic orbital can contain three electrons if all three have parallel spins.

A
True
B
False

Written response

1 point

How many neutrons are in a neutral chlorine-35 atom? Enter the number of neutrons as a whole number.

Choose all

1 point

Select all statements that correctly describe isotopes.

A
They have the same number of protons.
B
They always have the same number of neutrons.
C
They have different mass numbers.
D
They are atoms of the same element.
E
They must have different numbers of electrons.

Fill in the blank

1 point

A sulfide ion, S²⁻, has electrons in its outermost principal energy level.

Choose one

1 point

Why does first ionization energy generally increase from left to right across a period?

A
The effective nuclear charge generally increases.
B
The number of occupied principal energy levels increases substantially.
C
The valence electrons become farther from the nucleus.
D
The nucleus contains fewer protons.

True or false

1 point

True or false: The electron configuration of Fe²⁺ is [Ar]3d⁶ because iron loses its two 4s electrons before removing 3d electrons.

A
True
B
False

Written response

1 point

Which principle explains why two electrons in the same orbital must have opposite spins? Enter the principle's full name.

Choose all

1 point

Select all statements that correctly describe the maximum capacities of subshells.

A
An s subshell can hold 2 electrons.
B
A p subshell can hold 8 electrons.
C
A d subshell can hold 10 electrons.
D
An f subshell can hold 14 electrons.
E
A d subshell contains 6 orbitals.

Open ended

1 point

An element has two isotopes: one has a mass of 10.0129 u and an abundance of 19.9%, and the other has a mass of 11.0093 u and an abundance of 80.1%. Calculate the average atomic mass and explain why it is closer to one isotope's mass than the other's.

Choose one

1 point

Which species has the smallest ionic or atomic radius in the isoelectronic series O²⁻, F⁻, Ne, Na⁺, and Mg²⁺?

A
O²⁻ has the smallest radius because it has the fewest protons.
B
Ne has the smallest radius because it is neutral.
C
Mg²⁺ has the smallest radius because it has the most protons.
D
Na⁺ has the smallest radius because it has a positive charge.

True or false

1 point

True or false: In an ordinary chemical reaction, an atom’s number of protons remains unchanged.

A
True
B
False

Choose one

1 point

How many electrons are in a Mg²⁺ ion?

A
8 electrons
B
10 electrons
C
12 electrons
D
14 electrons

Choose one

1 point

What is the maximum number of electrons that the third principal energy level, n = 3, can hold?

A
6
B
9
C
18
D
32

Written response

1 point

A chlorine isotope is written as chlorine-35 and has atomic number 17. How many neutrons does it contain? Enter the number of neutrons as a whole number.

Written response

1 point

What is the maximum number of electrons that a d subshell can contain? Enter the number as a whole number.

Choose one

1 point

An element has two isotopes: one with mass 10.0129 u and abundance 19.9%, and one with mass 11.0093 u and abundance 80.1%. What is its average atomic mass?

A
10.0129 u
B
10.5000 u
C
10.811 u
D
11.0093 u

Choose one

1 point

Which comparison of atomic radius is generally correct for sodium and chlorine, which are both in period 3?

A
Sodium has the smaller radius because it has fewer electrons.
B
Chlorine has the smaller radius because it has the greater effective nuclear charge.
C
They have equal radii because they are in the same period.
D
Chlorine has the smaller radius because it has more occupied principal energy levels.

Choose one

1 point

Which order lists the following isoelectronic species from largest to smallest ionic or atomic radius: O²⁻, F⁻, Ne, Na⁺, and Mg²⁺?

A
O²⁻ > F⁻ > Ne > Na⁺ > Mg²⁺
B
Mg²⁺ > Na⁺ > Ne > F⁻ > O²⁻
C
F⁻ > O²⁻ > Na⁺ > Ne > Mg²⁺
D
Ne > O²⁻ > F⁻ > Mg²⁺ > Na⁺

Fill in the blank

1 point

Phosphorus has atomic number 15. Its abbreviated ground-state electron configuration is $\mathrm{P}: [\mathrm{Ne}]3s^2$ . Enter the final subshell and its electron count.