Electronic Structure of Atoms (copy)

What is electromagnetic radiation characterized by?

Wavelength, frequency, and energy.

What equation relates energy (E), frequency (f), and wavelength (λ) in electromagnetic radiation?

E = hf = hc/λ where h is Planck's constant and c is the speed of light.

List the types of waves included in the electromagnetic spectrum.

Gamma rays, X-rays, ultraviolet, visible light, infrared, microwaves, and radio waves.

What is the formula to calculate wavelength from frequency?

λ = c/f where c is the speed of light.

State Heisenberg's Uncertainty Principle.

It is impossible to simultaneously know both the exact position and momentum of a particle.

What does Quantum Theory explain?

The behavior of matter and energy on atomic and subatomic scales.

What does the Photoelectric Effect demonstrate about light?

Light can eject electrons from a material, indicating that light has particle-like properties (photons).

What is de Broglie's Hypothesis?

Particles exhibit wave-like characteristics, and the wavelength associated with a particle is inversely proportional to its momentum.

What are the four quantum numbers that define an electron's state?

Principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (ml), and spin quantum number (ms).

What is the Pauli Exclusion Principle?

No two electrons in an atom can have the same set of quantum numbers.

Describe the Aufbau Principle.

Electrons fill orbitals starting from the lowest energy level to higher levels.

What is Hund's Rule?

For degenerate orbitals, one electron enters each orbital before pairing occurs to minimize repulsion.

What is Effective Nuclear Charge (Z_eff)?

The net positive charge experienced by an electron in a multi-electron atom, influencing attraction between the nucleus and electrons.

How do atomic radii change across a period and down a group?

Decrease across a period and increase down a group.

Why do cations have smaller radii than their parent atoms?

Cations are smaller due to loss of an electron and decreased electron-electron repulsion.

How does ionization energy change across a period and down a group?

Increases across a period and decreases down a group.

What is the trend for electron affinity across a period?

Generally increases across a period.

How does reactivity relate to position on the periodic table?

Position influences ionization energy, electron affinity, and atomic radii; elements with high electronegativity tend to be more reactive.