Unit1 TSNF

Front

What is ionization energy?

Back

The energy required to remove an electron from an atom in its gaseous state.

Front

How does the energy level of an electron affect its ionization energy?

Back

Electrons in lower energy levels have higher ionization energy because they are closer to the nucleus and experience a stronger attraction.

Front

What happens to atomic size as you move across a period in the periodic table?

Back

Atoms get smaller due to an increase in the number of protons, which increases the positive charge and pulls electrons closer to the nucleus.

Front

What is the relationship between binding energy and electron proximity to the nucleus in PES graphs?

Back

A larger binding energy indicates that the electrons are closer to the nucleus.

Front

Why are anions larger than their neutral atoms?

Back

Anions have more electrons than protons, leading to increased electron-electron repulsion and more shielding, which makes them larger.

Front

What does mass spectroscopy measure?

Back

Mass spectroscopy measures the mass of isotopes in a sample.

Front

Define effective nuclear charge (Z_eff).

Back

The net positive charge experienced by an electron in a multi-electron atom, accounting for shielding from other electrons.

Front

What is the trend of atomic radius in the periodic table?

Back

Atomic radius decreases across a period and increases down a group.

Front

Explain the concept of shielding in atomic structure.

Back

Shielding occurs when inner electrons repel outer electrons, reducing the effective nuclear charge felt by the outer electrons.

Front

What is the significance of the photoelectron spectroscopy (PES) graph?

Back

PES graphs provide information about the energy levels of electrons in an atom and their binding energies.