Intermolecular Forces

Flashcards covering key concepts about intermolecular forces, including types of bonds, properties of water, and the principles of solubility.

Intermolecular Forces

Forces between molecules that affect their physical properties.

Intramolecular Forces

Forces within a molecule, primarily covalent bonds.

Covalent Bonds

Bonds formed by sharing outer electrons between two atoms.

Single Bond

A covalent bond where one pair of electrons is shared.

Double Bond

A covalent bond where two pairs of electrons are shared.

Triple Bond

A covalent bond where three pairs of electrons are shared.

Coordinate Bond

A covalent bond formed when one atom donates both electrons to be shared.

Induced Dipole-Dipole Forces

Weak forces resulting from the temporary dipoles in nonpolar molecules.

London Dispersion Forces

Another name for induced dipole-dipole forces.

Permanent Dipole-Dipole Forces

Attractive forces between neighboring molecules that have permanent dipoles.

Hydrogen Bonding

A strong type of dipole-dipole interaction that occurs when hydrogen is bonded to O, N, or F.

Strength of Intermolecular Forces

Intramolecular forces are stronger than intermolecular forces.

Temporary Dipole

A temporary polarization of electron density in a molecule.

Polar Molecule

A molecule that has a permanent dipole moment due to its shape and the electronegativity of its atoms.

Nonpolar Molecule

A molecule that has no permanent dipole moment, typically symmetrical.

Boiling Point

The temperature at which a substance changes from liquid to gas.

Melting Point

The temperature at which a solid becomes a liquid.

Surface Tension

The ability of a liquid's surface to resist external forces.

Density

Mass per unit volume of a substance.

Hydrogen Bonding in Water

Causes water's anomalous properties like high boiling point and surface tension.

Open Lattice Structure of Ice

Causes ice to be less dense than liquid water.

Bond Angle

The angle formed between three atoms in a molecule.

Solvent Choice Principle

'Like dissolves like' - polar substances dissolve in polar solvents.

Dipole-Dipole Interaction

Attraction between positive and negative ends of polar molecules.

Hydrogen Bond in Alcohols

Forms between the hydrogen of one alcohol molecule and oxygen of another.

Hydrogen Halides

Compounds formed from hydrogen and halogens, with varying boiling points.

Intermolecular Bonding

The bonding between molecules, different from intramolecular bonds.

Hydration Shell

The layer of solvent molecules that surrounds a solute particle.

Ionic Lattice

A three-dimensional structure of ions held together by ionic bonds.

Electrostatic Forces

Attractive forces between charged particles or ions.

Enthalpy of Vaporization

The energy required to evaporate a substance.

Anomalous Properties of Water

Unique properties of water arising from hydrogen bonding.

Boiling Points of Noble Gases

Increase with molecular size due to stronger dispersion forces.

Surface Area Effect on Intermolecular Forces

Larger surface area typically increases the strength of dispersion forces.

Alcohols

Organic compounds containing hydroxyl groups (-OH) capable of hydrogen bonding.

Ammonia

A polar molecule (NH3) that can form hydrogen bonds.

Amines

Functionally similar to ammonia and capable of hydrogen bonding.

Carboxylic Acids

Organic acids containing -COOH groups that can form hydrogen bonds.

Hydrogen Fluoride

Polar molecule (HF) that forms strong hydrogen bonds.

Proteins

Biomolecules that can form hydrogen bonds due to their amino or carboxy groups.

Hydrogen Bonding Strength

Stronger than most other types of intermolecular forces.

Breaking Strong Intermolecular Bonds

Requires significant energy input, such as heat.

Higher Density of Water

Water is denser as a liquid than as a solid due to molecular structure.

Polar Covalent Substance

Molecules where electrons are shared unequally, creating partial charges.

Covalent Lattice Structure

A strong structure formed by covalently bonded atoms, resistant to dissolving.

Hexanol

An alcohol that is less soluble in water compared to ethanol due to larger non-polar part.

Solubility of Ionic Compounds

Depends on the ability of water to disrupt ionic lattices.

Sodium Chloride Solubility

Dissolves readily in water due to strong dipole interactions.

Calcium Chloride Solubility

Less soluble in water than sodium chloride due to its higher ionic charge.

Electronegativity

A measure of an atom's ability to attract shared electrons.

C-X Bond Polarity

Refers to the polar covalent bond formed between carbon and halogens.

Hydrophobic Effect

The tendency of non-polar substances to aggregate in aqueous solutions.

Thermodynamic Stability

Related to how well substances resist changes in their state.