Atomic Structure, Bonding, and Intermolecular Forces

Flashcards based on lecture notes about atomic structure, quantum mechanics, bonding, and intermolecular forces.

Atomism

Small, invisible, and indivisible particles; the idea proposed by Democritus.

Limitations

Modern-day atomic structure has these.

Heisenberg

Proposed the uncertainty principle, stating that you cannot know both the position and speed of a particle with perfect accuracy.

John Dalton

Developed the solid sphere model of the atom.

James Chadwick

Proved the existence of the neutron in 1932.

William Crookes

Discovered cathode rays.

Rutherford

Developed the planetary model of the atom, with electrons orbiting the nucleus.

Principal quantum number

An electron's location in orbitals is specified via this.

Aufbau principle

The principle stating that you should fill low energy orbitals first and then go high.

Hund's rule

This rule dictates that you fill up all empty orbitals first to minimize electron repulsion and achieve stability.

Pauli Exclusion Principle

The principle stating that a maximum of two electrons can occupy each orbital, and they must have opposite spins.

Paramagnetic

Atoms that have unpaired electrons and are attracted to magnets.

Diamagnetic

Atoms where all electrons are paired and are repelled by magnets.

Angular Momentum Quantum Number

Describes the shape of an orbital.

Electron Spin Quantum Number

Specifies the direction an electron is spinning.

Valence connection energy

The energy needed to separate ions.

Covalent bond

This type of bond occurs when atoms share electrons.

Ionic bond

This type of bond is when electrons are transferred.

Covalent bond

A bond with atoms with similar electron attracting ability.

A

Metallic bonding

Valance electrons move freely like the sea.

Electronegativity

A measure of attraction of electrons.

Lewis Dot Structure

A diagram that distributes electrons.

Valance Bond Theory

Atomic orbitals containing unpaired electrons form covalent bonds.

Sigma Bonds

Orbitals are the same as one of lowest overall potential energy and is a stronger bond.

Pi Bond

A weaker bond.

Bond Energy

Energy it takes to break one mole of specific bond.

Melting Point

Factors of this include bond type, surface area, and polarity.

Intramolecular Force

Stronger than intermolecular force.

Amorphous solids

Bonds like rubber or glass with no sharp melting point.

Hydrogen Bonding

A special type of Dipole-Dipole bond that is stronger with high electronegativity and small radius.

London Disperison Force

Uneven electron disperson (very weak).

Surface Tension

More complex molecules with larger chains.

Capillary action

Liquid flowing through material due to attractions between liquid and solid (adhesive and cohesive).

Covalent Coordinate

Electrons donated for sharing purposes to form a bond.