Chapter 2 The Quantum-Mechanical Model of the Atom

Wavelength (λ)

Distance between corresponding points on waves.

Frequency (ν)

Number of waves passing a point per second.

Speed of light (c)

3.00 × 10^8 m/s.

Light equation

c = λν.

Frequency formula

ν = c/λ.

Wavelength formula

λ = c/ν.

Photon

Packet of light energy.

Planck's equation

E = hν.

Planck's constant (h)

6.626 × 10^-34 J·s.

Energy using wavelength formula

E = hc/λ.

Photoelectric effect

Light can cause a metal to release electrons if the light has enough energy.

Inverse relationship

As wavelength (λ) increases, frequency (ν) decreases.

Bohr model

Electrons can occupy only specific allowed energy levels.

Line spectrum

Specific/discrete wavelengths emitted by an atom.

Electron transition

Movement of an electron between energy levels.

de Broglie equation

λ = h/mv.

Heisenberg Uncertainty Principle

You cannot precisely know both an electron's position and momentum simultaneously.

Schrödinger's model

Models electrons using both wave and particle behavior.

Orbital

Spatial distribution/probable region of an electron.

Quantum numbers

Set of numbers used to describe the properties of electrons.

n

Energy level/shell.

ℓ

Orbital shape/type.

mₗ

Orbital orientation.

mₛ

Electron spin.

s orbital shape

Sphere.

p orbital shape

Dumbbell/two lobes.

d orbital shape

Mostly four lobes.

Number of s orbitals

1.

Number of p orbitals

3.

Number of d orbitals

5.

Number of f orbitals

7.