Periodic Trend - Atomic Size (Radius) Explained!

The video explains atomic size, also known as atomic radius, and its significance in understanding atomic reactivity. It discusses periodic trends, noting that atomic size increases down the periodic table and from right to left. The video explains these trends by examining energy levels and the number of protons, using examples to illustrate how these factors affect atomic size. It emphasizes that energy levels are more significant than nucleus strength when comparing atomic sizes.

What is the general trend for atomic size on the periodic table?

• Atomic size decreases as you move down and from left to right.

• Atomic size increases as you move up and from right to left.

• Atomic size increases as you move down and from right to left.

• Atomic size decreases as you move up and from left to right.

Why do atoms get larger as you move down a group in the periodic table?

• Because the electrons are pulled closer to the nucleus.

• Because the number of protons decreases.

• Because more energy levels are added.

• Because the atomic number decreases.

What happens to the atomic number as you move from right to left across a period?

• It doubles.

• It decreases.

• It remains the same.

• It increases.

Which element is larger, rubidium or iodine, and why?

• Rubidium, because it has more protons.

• Iodine, because it has a weaker nucleus.

• Rubidium, because it has fewer protons.

• Iodine, because it has more energy levels.

When comparing elements with the same number of energy levels, what should be considered next?

• The number of neutrons.

• The atomic mass.

• The number of electrons.

• The strength of the nucleus.