Chemistry Week Two

Electron Configuration

The arrangement of electrons in orbitals of an atom

How many electrons can an s subshell hold?

2

How many electrons can a p subshell hold?

6

How many electrons can a d subshell hold?

10

How many electrons can f orbitals have

14

Pauli Exclusion Principle

No two electrons can share the same four quantum numbers. These means orbitals can only hold two electrons spinning in different directions.

Hund’s rule

Electrons will only share an orbital if all other orbitals of the same energy level have electrons in them.

Diamagnetic

Atoms with all electrons paired. They are repelled by magnetic fields.

Paramagnetic

Atoms with unpaired electrons. They are attracted to magnetic fields.

Noble gas core

The completed shell configuration of a noble gas. They are used to abbreviate the electron configuration of other atoms.

Transition metals

Elements that readily gain or lose electrons in their d shells.

Effective nuclear charge

The magnitude of positive force felt by electrons. Increases from left to right on the period table.

Shielding

When the effective nuclear charge felt by an electron decreases due to repulsion by other electrons

Atomic radius

The distance between the nucleus of an atom and its valence shell. Decreases from left to right and increases from top to bottom on the periodic table.

Ionization energy

The energy necessary to remove an electron from its nucleus. Generally increases from left to right on the periodic table, and after multiple ions have been removed or separating ions from complete shells.

Cation

An ion with a positive charge

Ion

An atom that has lost or gained electrons so that it is no longer neutrally charged

Electron affinity

Energy released when an atom accepts an electron. Increases from left to right on the periodic table.

Anion

An ion with a negative charge

Metallic Character

A property quantifying the metallic properties of an element. Decreases from left to right and increases from top to bottom on the periodic table.

Diagonal relationships

Elements that are diagonal to each other on the periodic table usually share similar properties.

Isoelectronic

Ions and atoms with the same number of electrons

Ionic radius

The distance between an ion’s nucleus and valence electrons. Increases when an ion gains electrons and decreases when an ion loses electrons.