Periodic Trends and Ion Properties

This video covers periodic trends including atomic and ionic radius, electronegativity, ionization energy, electron affinity, and metallic character. It explains how these properties change across the periodic table and the factors influencing them, such as nuclear charge and electron shielding. The video also discusses exceptions to these trends and provides examples to illustrate the concepts.

Which of the following statements best describes the trend in atomic size across a period in the periodic table?

• Atomic size decreases from left to right.

• Atomic size increases from left to right.

• Atomic size first increases and then decreases.

• Atomic size remains constant across a period.

What is the primary reason that a lithium ion is smaller than a lithium atom?

• The lithium ion has a larger nuclear charge.

• The lithium ion has more electrons.

• The lithium ion has fewer electron shells.

• The lithium ion has more protons.

How does the size of an anion compare to its parent atom?

• An anion has no definite size compared to its parent atom.

• An anion is smaller than its parent atom.

• An anion is the same size as its parent atom.

• An anion is larger than its parent atom.

Which element is the most electronegative in the periodic table?

• Nitrogen

• Fluorine

• Chlorine

• Oxygen

In which direction does metallic character increase on the periodic table?

• Down and to the right

• Up and to the right

• Up and to the left

• Down and to the left

Which element is expected to have the highest metallic character?

• Sulfur

• Sodium

• Chlorine

• Silicon

What happens to ionization energy as you move from left to right across a period?

• It decreases

• It fluctuates randomly

• It increases

• It remains constant

Why is it easier to remove an electron from sodium than from lithium?

• Sodium's valence electron is further from the nucleus

• Sodium is smaller in size

• Sodium has fewer electron shells

• Sodium has a higher nuclear charge

Which group in the periodic table is most exothermic in terms of electron affinity?

• Group 7

• Group 4

• Group 8

• Group 1

What is the relationship between electron affinity and the stability of the ion formed?

• Electron affinity is inversely proportional to ion stability

• Higher electron affinity means more stable ion

• Higher electron affinity means less stable ion

• Electron affinity does not affect ion stability