Atomic Size and Electron Distribution in the Periodic Table

The video explores the concept of atomic size, initially addressing common misconceptions about atomic radius. It explains that electrons are not in fixed orbits but in orbitals, which are probability distributions. The video discusses methods to measure atomic size, such as the Van der Waals and covalent radius. It also examines trends in atomic size across periods and groups in the periodic table, highlighting that atomic size decreases across a period and increases down a group.

What is the main reason electrons do not orbit the nucleus like planets around the sun?

• Electrons are in fixed positions.

• Electrons are too small to orbit.

• Electrons are repelled by the nucleus.

• Electrons exist in probability distributions called orbitals.

Which method involves measuring the closest distance between two non-bonded atoms?

• Covalent radius

• Metallic radius

• Ionic radius

• Van der Waals radius

How does the atomic size change as you move from left to right across a period?

• It fluctuates randomly.

• It remains constant.

• It decreases due to increased nuclear charge.

• It increases due to more electron shells.

Why does krypton have a smaller atomic radius than potassium?

• Krypton is a noble gas.

• Krypton has fewer electron shells.

• Krypton has a higher nuclear charge pulling electrons closer.

• Krypton has more electron shells.

Which element is smaller, helium or hydrogen, and why?

• Hydrogen, because it has fewer protons.

• Helium, because it has more protons attracting the electrons.

• Hydrogen, because it has more electron shells.

• Helium, because it is a noble gas.

Which of the following best describes the atomic size trend across a period?

• Atoms get larger due to electron repulsion.

• Atoms remain the same size.

• Atoms get smaller due to increased nuclear charge.

• Atoms get larger due to more electron shells.

What happens to atomic size as you move down a group in the periodic table?

• It decreases due to electron repulsion.

• It decreases due to increased nuclear charge.

• It increases due to additional electron shells.

• It remains constant.

What is the effect of adding more electron shells as you move down a group?

• It decreases the atomic size.

• It makes the atom more stable.

• It increases the atomic size.

• It has no effect on atomic size.

What is the general trend in atomic size from the bottom left to the top right of the periodic table?

• Atoms get smaller.

• Atoms fluctuate in size.

• Atoms get larger.

• Atoms remain the same size.

Which of the following is true about the atomic size of elements at the bottom left of the periodic table?

• They are the smallest atoms.

• They are the largest atoms.

• They have the same size as those at the top right.

• They are smaller than those at the top right.