Chapter 6: Electronic Structure of Atoms

Electronic Structure

Electronic Structure

The arrangement and energy of electrons.

Wavelength (\lambda)

The distance between corresponding points on adjacent waves.

Frequency (v)

The number of waves passing a given point per unit of time.

Speed of Light (c)

The speed at which all electromagnetic radiation travels, approximately 3.00\cdot 10^{8}m/s

Photoelectric Effect

The phenomenon where electrons are ejected from a metal when it absorbs energy that is proportional to frequency.

Plank’s Constant ($h$)

A constant valued at 6.626\cdot 10^{-34}J\cdot s used in the photoelectric effect equation (E=hv).

Quantum Mechanics

The branch of physics that describes the movement and behavior of electrons.

Principal Quantum Number (n)

Describes the energy level of an orbital and is an integer greater than or equal to 1.

Angular Momentum Quantum Number (l)

Defines the shape of the orbital, with allowed values ranging from 0 to n-1.

Magnetic Quantum Number (m_l)

Describes the three-dimensional orientation of the orbital with allowed values from -l to l.

Hund’s Rule

For orbitals in the same sublevel, each must contain one electron before any pairing occurs.

Pauli Exclusion Principle

States that no two electrons in the same atom can have the same set of four quantum numbers.

Electron Configuration

The distribution of electrons in an atom, specified by energy level, orbital type, and number of electrons.

Ground State

The lowest possible energy configuration of an atom's electrons.

Condensed Electron Configuration

A shorthand notation for electron showing valence electrons and using noble gas symbols.

s Orbitals

Spherical-shaped orbitals with a value of l equal to 0.

p Orbitals

Orbital shape with two lobes and one nodal plane, with a value of l equal to 1.

d Orbitals

Orbitals with more complex shapes, where the value of l is 2.

f Orbitals

Highly complex-shape orbitals with a value of l equal to 3.