molecular geometry

linear

where atoms are arranged in a straight line, typically with bond angles of 180 degrees. This shape occurs in diatomic molecules and certain polyatomic molecules with no lone pairs. XY2

Trigonal planar

a molecular geometry where three atoms are arranged around a central atom in a plane, with bond angles of 120 degrees. This shape occurs in molecules with three bonding pairs and no lone pairs. XY3

Tetrahedral

where four atoms are arranged around a central atom in three-dimensional space, with bond angles of approximately 109.5 degrees. This shape occurs in molecules with four bonding pairs and no lone pairs. XY4

Trigonal pyramid

where three atoms are bonded to a central atom, with one lone pair of electrons, leading to bond angles of less than 109.5 degrees. This shape occurs in molecules like ammonia (NH3). XY3E

Bent

where two atoms are bonded to a central atom, with one or more lone pairs of electrons, leading to bond angles that are typically less than 120 degrees due to the repulsion of the lone pairs. This shape occurs in molecules like water (H2O) XY2E or XY2E2

trigonal bipyramidal

here five atoms are arranged around a central atom, with two atoms in axial positions (180-degree bond angles) and three atoms in equatorial positions (120-degree bond angles). This shape occurs in molecules with five bonding pairs and no lone pairs. XY5

Octahedral

where six atoms are arranged around a central atom, with bond angles of 90 degrees. This shape occurs in molecules with six bonding pairs and no lone pairs. XY6.

dipole

intramoleculer equal but opposite charge separated by a short distance

London dispersion force

temporary dipole, found in all molecules, but it is the only force in nonpolar molecules

hydrogen bonding

strong dipole, the intermolecular attraction between hyrogen atom covalent, bonded to either a Fluorine, Oxygen, Nitrogen atom with an unshared pair of electrons on the atom

Ionic Bonds

metal and non-metal atoms transfer electrons to form compounds

Metallic Bonds

metal and metal atoms (electron sea model)

covalent bonds

nonmetal and nonmetal sharing electrons (polar and non polar stuff)

nonpolar covalent bonds

equal amounts of electron sharing between atoms, resulting in no charge separation, all sides of bond has equal charge

polar covalent bonds

electrons are shared unequally due to a significant difference in electronegativity between the bonded atoms, leading to positive and negative charges.

how to figure out electronegativity based on number

en <= 0.3 means non polar

en <= 1.7 polar

en.> 1.7 ionic bond

(anything lower than 0.3 nonpolar, 0.4-1.7 polar, greater than 1.7 ionic bond)

diatomic molecule (contains z atoms)

Br, I, N, Cl, H, O, F (only for covalent)