Inorganic Chemistry Flashcards

Vocabulary flashcards for reviewing key concepts in inorganic chemistry.

Principal Quantum Number (n)

The average distance of an orbital from the nucleus.

Values of Principal Quantum Number (n)

n = 1, 2, 3, 4…

Angular Momentum Quantum Number (l)

The shape of an orbital.

Values of Angular Momentum Quantum Number (l)

l = 0, 1, 2, …, (n – 1)

Magnetic Quantum Number (ml)

The orientation of an orbital in space.

Values of Magnetic Quantum Number (ml)

ml = 0, ±1, ±2, …, ±l

Electron Spin Quantum Number (ms)

The spinning motion of an electron in an orbital.

Values of Electron Spin Quantum Number (ms)

ms = ±½

Aufbau Principle

Orbitals of lower energy levels are filled first before those of higher energy levels.

Hund’s Rule

For degenerate orbitals, the most stable arrangement is the one with the greatest number of parallel spins.

Pauli Exclusion Principle

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

Atomic Radius

The distance between the nucleus of an atom and its outermost electron.

First Electron Affinity

The energy change when one mole of electrons is added to one mole of gaseous atom to form one mol of gaseous singly charged anion.

First Ionisation Energy

The energy required to remove one mole of electrons from one mole of gaseous atom to form one mol of gaseous singly charged cation.

Successive Ionisation Energies

Energies required to remove electrons sequentially from an atom or ion in the gaseous state.

Lewis Acid

Electron pair acceptor.

Lewis Base

Electron pair donor.

Sigma Bonds

Result from head-on overlap of orbitals

Pi Bonds

Result from side-on overlap of orbitals.

Uniqueness Principle of Period 2 Elements

Do not have low-lying (or energetically accessible) vacant d orbitals, small size and form cations with a high charge density.

Electronegativity of Central Atom (Oxo-Acids)

The higher the electronegativity of the central atom, the greater the ability to withdraw electrons. This weakens O–H bonds to a greater extent, increasing the ease in which H+ is released. Thus acid strength increases.

Number of Oxo Groups (Oxo-Acids)

The more oxo groups (=O) bonded to the central atom, the greater the ability to withdraw electrons. This weakens O–H bonds to a greater extent, increasing the ease in which H+ is released. Thus acid strength increases.

Molality

The amount of the solute in one kilogram of solvent.

Molarity

The amount of the solute in one litre (or 1 dm3) of solution.

Mole Fraction

The ratio of the amount of the solute to the total amount of all components in the solution.

Vapour pressure

The pressure exerted by its vapour when the liquid and vapour phases are in dynamic equilibrium.

Enthalpy change of vaporisation

The energy required to convert one mole of liquid into gas at constant pressure and temperature.

Volatility

The tendency of a liquid to vaporise under room temperature and pressure.

Boiling point

The temperature at which a liquid’s vapour pressure equals the external atmospheric pressure.

Viscosity

The measure of a liquid's resistance to flow either by shear or tensile stress.

Surface tension

The measure of a liquid’s resistance to increase its surface area by 1 m2.

Wettability

The tendency of a liquid to form spherical droplets or spread out on a surface

Capillary action

The tendency of a liquid to rise up or drawn down a narrow tube.