FUNCHEM 3 - ELECTRONIC CONFIGURATIONS OF ATOMS AND IONS

Electronic Configurations of Atoms and Ions of Physiological Importance

Bohr

* Electron moves in circular orbits around the nucleus
* Orbits have specific energies - energy levels

Thomson

* Discovered the first subatomic particle (the electron).
* Plum pudding - nuclear model

Rutherford

Protons in the nucleus.

Einstein

Light, although a wave, could have particle properties.

De Broglie

* Matter, like light, can have wave properties
* Electrons can have particle properties
* Wave-particle duality

Heisenberg

Can know momentum or position of particle but can’t know both at the same time with certainty.

Schrodinger wave equation

Used to calculate the probability of finding an electron within a particular position within an atom.

Atomic orbital

A region in space within an atom and around the nucleus where the probability of finding an electron is high.

Atomic orbitals and shapes

1. S orbital: Spherical.
2. P orbital: Dumbbell with 3 different orientations.
3. D orbital: 5 different shapes, 4 of which are similar.

Energy sublevel

A group of atomic orbitals within an atom, all of which have the same energy.

What are the number of orbitals and maximum number of electrons in each sublevel?

1. Sublevel s - Number of orbital: 1, Max number of electrons in each orbital: 2
2. Sublevel p - Number of orbital: 3, Max number of electrons in each orbital: 6
3. Sublevel d - Number of orbital: 5, Max number of electrons in each orbital: 10

Pauli’s Exclusion Principle

* No more than 2 electrons can occupy an orbital
* Electrons must have opposite spin

Aufbau Principle

Electrons fill the lowest available energy level first.

Hund’s Rule

Electrons fill orbitals singly before filling in pairs.

* Think of passengers in a bus.

Valence electrons

Outermost electrons.

What dictates a stable atom?

Stability is achieved if the outermost orbital are hall-filled or completely filled.

Cation

Positively charged ion.

Anion

Negatively charged ion.