As one travels down through a family of elements, the size of the atoms of those elements

Increases in size as you go down due to the addition of new layers of electrons.

Decreases as you go down due to the addition of new layers of electrons

Increases as you go down due to the changes in orientation of electrons along the various axes.

Increases in size due to advanced electronic transmutations.

As one travels across a series or period of elements, the size of the atoms are those elements

Decreases due to increased attraction between the positively charged nucleus and the negatively charged electrons.

Increases due to the addition of layers of electrons as you move across the series.

Increases due to the addition of neutrons, electrons, and protons

Decreases due to the removal of layers of electrons.

Lesson 10 Test - Atomic Size And The Periodic Table | Attempts: 1610

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1/10 Questions

As one travels down through a family of elements, the size of the atoms of those elements
- Decreases as you go down due to the addition of new layers of electrons
- Increases as you go down due to the changes in orientation of electrons along the various axes.
- Increases in size as you go down due to the addition of new layers of electrons.
- Increases in size due to advanced electronic transmutations.

About This Quiz

Atoms, atomic number and size are factors that define an element and depending on the atomic size or number, an element can be placed as a solid, gas or liquid in a periodic table. This is a good challenge for you if you just studied the periodic table. Give it a shot!

Lesson 10 Test - Atomic Size And The Periodic Table - Quiz

2.

As one travels across a series or period of elements, the size of the atoms are those elements
- Decreases due to increased attraction between the positively charged nucleus and the negatively charged electrons.
- Increases due to the addition of layers of electrons as you move across the series.
- Increases due to the addition of neutrons, electrons, and protons
- Decreases due to the removal of layers of electrons.
Correct Answer

A. Decreases due to increased attraction between the positively charged nucleus and the negatively charged electrons.

Explanation

As one travels across a series or period of elements, the size of the atoms decreases due to increased attraction between the positively charged nucleus and the negatively charged electrons. This is because as you move across the series, the number of protons in the nucleus increases, which strengthens the positive charge of the nucleus. At the same time, the number of electrons also increases, but they are added to the same energy level or shell. This means that the attractive force between the nucleus and the electrons becomes stronger, pulling the electrons closer to the nucleus and thus reducing the size of the atom.

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1
3.

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?
- Sodium
- Cesium
Correct Answer

A. Cesium

Explanation

Cesium has a larger atomic radius compared to Sodium. This is because atomic radius generally increases as you move down a group on the periodic table. Cesium is located below Sodium in the same group (Group 1), indicating that it has more energy levels and a larger atomic radius. Therefore, Cesium has a larger atomic radius than Sodium.

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1
4.

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?
- Calcium
- Nickel
Correct Answer

A. Calcium

Explanation

Calcium has a larger atomic radius compared to Nickel based on their relative positions on the periodic table. Atomic radius generally decreases across a period from left to right due to increasing nuclear charge, which attracts the electrons closer to the nucleus. Calcium is located to the left of Nickel in the periodic table, indicating that it has more energy levels and a larger atomic radius. Therefore, Calcium has a larger atomic radius than Nickel.

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5.

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?
- Oxygen
- Selenium
Correct Answer

A. Selenium

Explanation

Selenium has a larger atomic radius compared to oxygen based on their relative positions on the periodic table. Atomic radius generally decreases from left to right across a period, and increases from top to bottom within a group. Oxygen is located to the right of selenium on the periodic table, indicating that it has a smaller atomic radius. Therefore, selenium has a larger atomic radius than oxygen.

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2
6.

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?
- Titanium
- Potassium
Correct Answer

A. Potassium

Explanation

Potassium has a larger atomic radius compared to Titanium. The atomic radius generally increases as you move down a group in the periodic table. Since Potassium is located below Titanium in the same group (Group 1), it has more energy levels and therefore a larger atomic radius.

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5
7.

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?
- Zinc
- Mercury
Correct Answer

A. Mercury

Explanation

Mercury has a larger atomic radius compared to Zinc. This is because, as you move down a group in the periodic table, the atomic radius generally increases due to the addition of more energy levels or shells. Since Mercury is located below Zinc in the periodic table, it has more energy levels and therefore a larger atomic radius.

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8.

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?
- Chlorine
- Iodine
Correct Answer

A. Iodine

Explanation

Iodine has a larger atomic radius compared to Chlorine because atomic radius generally increases as you move down a group in the periodic table. Iodine is located below Chlorine in the same group, so it has more energy levels and a larger atomic radius.

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9.

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?
- Zirconium
- Silver
Correct Answer

A. Zirconium

Explanation

Zirconium has a larger atomic radius compared to silver based on their relative positions on the periodic table. Atomic radius generally decreases across a period from left to right due to increasing nuclear charge and the attraction between the electrons and the nucleus. Zirconium is located to the left of silver on the periodic table, indicating that it has more energy levels and electrons shielding the nucleus, which results in a larger atomic radius.

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10.

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?
- Iron
- Arsenic
Correct Answer

A. Iron

Explanation

Iron has a larger atomic radius compared to Arsenic because atomic radius generally decreases across a period from left to right on the periodic table. Iron is located to the left of Arsenic, so it has more electron shells and a larger atomic radius.

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Quiz Edited by
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Jul 31, 2013

Quiz Created by
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Lesson 10 Test - Atomic Size And The Periodic Table

As one travels down through a family of elements, the size of the atoms of those elements

Quiz Preview

As one travels across a series or period of elements, the size of the atoms are those elements

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?

Which of the elements has the larger atomic radius based upon their relative positions on the periodic table?