Inv 2 Exp 2 - Periodic Table and Atomic Structure - Day 2

Front

What is the effective nuclear charge (Z_eff)?

Back

The effective nuclear charge (Z_eff) is the net positive charge experienced by valence electrons in an atom, accounting for the shielding effect of inner electrons.

Front

How does atomic radius change across a period in the periodic table?

Back

Atomic radius decreases across a period from left to right due to increasing nuclear charge, which pulls electrons closer to the nucleus.

Front

How does atomic radius change down a group in the periodic table?

Back

Atomic radius increases down a group due to the addition of electron shells, which outweighs the increase in nuclear charge.

Front

What is the trend of ionization energy across a period?

Back

Ionization energy generally increases across a period due to increased nuclear charge and decreased atomic radius.

Front

What is the trend of ionization energy down a group?

Back

Ionization energy generally decreases down a group because the outer electrons are further from the nucleus and experience more shielding.

Front

What is the significance of the octet rule in chemistry?

Back

The octet rule states that atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons, leading to greater stability.

Front

What is the difference between a cation and an anion?

Back

A cation is a positively charged ion formed by losing electrons, while an anion is a negatively charged ion formed by gaining electrons.

Front

What is the role of valence electrons in chemical bonding?

Back

Valence electrons are the outermost electrons of an atom and are involved in forming chemical bonds with other atoms.

Front

What is the shielding effect?

Back

The shielding effect is the phenomenon where inner electrons reduce the effective nuclear charge felt by outer electrons, affecting their energy levels.

Front

How do you determine the order of elements based on atomic radius?

Back

To determine the order of elements based on atomic radius, compare their positions in the periodic table, considering trends of increasing or decreasing radius.