Effective Nuclear Charge and Atomic Radius

Front

What is Effective Nuclear Charge (Z_eff)?

Back

The net positive charge experienced by valence electrons in an atom, accounting for shielding by inner electrons.

Front

How does Effective Nuclear Charge change across a period in the periodic table?

Back

Effective nuclear charge increases across a period due to the increase in protons without a significant increase in shielding.

Front

What is the trend of atomic radius as you move across a period?

Back

Atomic radius decreases as you move across a period due to increased effective nuclear charge pulling electrons closer to the nucleus.

Front

What is the trend of atomic radius as you move down a group in the periodic table?

Back

Atomic radius increases down a group due to the addition of electron shells.

Front

Which element has the largest atomic radius: Lithium, Boron, Neon, or Nitrogen?

Back

Lithium has the largest atomic radius among these elements.

Front

What role do core electrons play in determining Effective Nuclear Charge?

Back

Core electrons shield valence electrons from the full charge of the nucleus, reducing the effective nuclear charge felt by valence electrons.

Front

Why do atoms get smaller as you move from left to right across a period?

Back

Atoms get smaller because the effective nuclear charge increases, pulling the electrons closer to the nucleus.

Front

What is the relationship between atomic radius and ionization energy?

Back

Generally, as atomic radius decreases, ionization energy increases because electrons are held more tightly by the nucleus.

Front

What is the definition of shielding effect?

Back

The reduction in effective nuclear charge on the electron cloud, due to the presence of other electrons, particularly core electrons.

Front

How does the effective nuclear charge affect the chemical reactivity of an element?

Back

Higher effective nuclear charge typically leads to lower reactivity in metals and higher reactivity in nonmetals.