Shielding

The video tutorial explores the reactivity of alkali metals with water, emphasizing the concept of shielding and its impact on atomic structure and reactivity trends. It explains how atomic radius and electron shells influence the ease of losing electrons, using a magnet analogy to illustrate the shielding effect. The tutorial also covers ionization energy and its decrease down a group in the periodic table, and discusses the reactivity of halogens and their electron affinity.

What happens to the reactivity of alkali metals with water as you move down the group?

• It fluctuates randomly.

• It remains the same.

• It increases.

• It decreases.

Which factor contributes to the decreased attraction between the nucleus and the outermost electron in alkali metals?

• Decreased number of electron shells

• Increased shielding

• Decreased atomic radius

• Increased nuclear charge

How does increased shielding affect ionization energy?

• It has no effect on ionization energy.

• It increases ionization energy.

• It makes ionization energy fluctuate.

• It decreases ionization energy.

What is the term used to describe the energy released when an electron is added to a neutral atom?

• Ionization energy

• Electron affinity

• Electronegativity

• Atomic radius

What trend is observed in the reactivity of halogens as you move down the group?

• Reactivity increases.

• Reactivity remains constant.

• Reactivity decreases.

• Reactivity fluctuates.