Bohr's Atomic Model and Quantum Concepts

Dalton's Atomic Model

Atoms are indivisible and identical for each element.

Bohr's Atomic Model

Electrons orbit the nucleus like planets around the sun.

Ground State

Lowest energy state of an electron.

Excited State

Electrons absorb energy and move to higher orbits.

Energy Release

Electrons emit radiation returning to ground state.

Planetary Model

Electrons occupy specific orbits, n=1 closest to nucleus.

Electromagnetic Radiation

Includes all wavelengths of electromagnetic waves.

Visible Light

Wavelengths between 400-700 nm.

Wavelength (λ)

Distance between consecutive wave crests.

Frequency (v)

Number of waves passing a point per second.

Inverse Relationship

Longer wavelength equals lower frequency.

Electromagnetic Spectrum

Includes all types of electromagnetic waves.

Wave-Particle Duality

Light behaves as both wave and particle.

Speed of Light

Constant at 3.00 x 10^8 m/s.

Planck's Constant

Value is 6.626 x 10^-34 J·s.

De Broglie Hypothesis

Electrons exhibit wave-like properties.

Electron Cloud Model

Electrons exist in probable regions called orbitals.

Orbital Shapes

Includes s, p, d, and f shapes.

Aufbau Principle

Electrons fill lowest energy orbitals first.

Hund's Rule

Each orbital gets one electron before pairing.

Pauli Exclusion Principle

No two electrons can have identical quantum numbers.

Coulombic Attraction

Force between oppositely charged particles.

Electron Shielding

Inner electrons block nucleus' pull on outer electrons.

Atomic Radius

Increases down a group, decreases across a period.

Ionization Energy (IE)

Increases up a group and across a period.

Electronegativity

Increases up a group and across a period.

Reactivity of Metals

More reactive down a group, less across a period.

Reactivity of Non-metals

More reactive up a group and across a period.