chem molecule thing

intramolecular forces

exist inside a molecule, influence chemical properties

intermolecular forces

exist between molecules, influence physical properties

Hydrogen Bonding

An H bonded w/ a F O N - strong bond & polar

Dipole-Dipole

Two polar covalent(non mental) compounds - strong bond

London Dispersion

two non polar covalent compounds - weak bond & present in all types of compounds - unequal sharing of electrons

Ionic Bond

metal + non metal

Covalent bond

nonmetal + nonmetal

physical properties and intermolecular forces

stronger intermolecular force, greater physical property - boiling point, melting point, viscosity, surface tension

cation

lose electrons to become positive

anions

gain electrons to become negative

octet rule

Atoms tend to gain, lose, or share electrons to achieve a full outer shell of eight electrons, leading to greater stability.

duet rule

A guideline stating that atoms, particularly hydrogen and helium, are stable when they have two electrons in their outer shell.

valence electrons

group of element

what goes in the center of a lewis dot structure

least electronegative element (usually first one) and never hydrogen

resonance structure

A way of representing a molecule where the structure can be depicted as two or more valid Lewis structures. These structures demonstrate the delocalization of electrons in a molecule.

Linear

2 electron groups, 180 degrees, non polar molecular geometry with no lone pairs

Trigonal Planar

3 electron groups, 120 degrees, non polar molecular geometry with no lone pairs.

Trigonal Bent

4 electron groups, 110 degrees, polar molecular geometry with one lone pair.

Tetrahedral

4 electron groups, 109.5 degrees, non polar molecular geometry with no lone pairs.

Trigonal Pyramid

4 electron groups, 107 degrees, polar molecular geometry with one lone pair.

Tetrahedral Bent

4 electron groups, 105 degrees, polar molecular geometry with two lone pairs

electronegativity

a measure of an atom's ability to attract and hold onto electrons in a chemical bond, influencing bond polarity and molecular structure.