BIOKMOR

IONIC

Results from the transfer of electrons from one element to another

Covalent

Result from the sharing of electrons between atoms

\+1

Formal charge of C when it has three bonds

0

Formal charge of C when it has 4 bonds

\-1

Formal charge of C when it has three bonds and one lone pair

\+1

Formal charge of N when it has 4 bonds

0

Formal charge of N where it has three bonds

\-1

Formal charge of N where it has two bonds and two lone pairs

\+1

Formal charge of O when it has three bonds

0

Formal charge of O when it has two bonds and two lone pairs

\-1

Formal charge of O when it has one bond and three lone pairs

Linear

Molecular shape of AX (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Linear

Molecular shape of AX (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Linear

Molecular shape of AXE (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Trigonal planar

Molecular shape of AX3 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Bent

Molecular shape of AX2E (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Linear

Molecular shape of AXE2 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Tetrahedral

Molecular shape of AX4 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Trigonal pyramid

Molecular shape of AX3E (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Linear

Molecular shape of AXE3 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Linear

Electron Geometry of AX (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Linear

Electron Geometry of AX (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Linear

Electron Geometry of AX (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Trigonal planar

Electron Geometry of AX3 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Trigonal planar

Electron Geometry of AXE2 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Tetrahedral

Electron Geometry of AX4 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Trigonal pyramid

Electron Geometry of AX3E (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Tetrahedral

Electron Geometry of AX2E2 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

Tetrahedral

Electron Geometry of AXE3 (A= central atom, X= an atom bonded to A, E= a lone pair on A)

s

Hybridization of AX

sp

Hybridization of AX2 and AXE

sp2

Hybridization of AX3, AX2E, AXE2

sp3

Hybridization of AX4, AX3E, AX2E2, AXE3

180

Bond angle of linear

120

Bond angle of trigonal planar

109\.5

Bond angle of tetrahedral

107

Bond angle of trigonal pyramid

105

Bond angle of Bent

Linear

Electron Geometry of H2

Linear

G

Trigonal planar

Electron Geometry of AlBr3

Trigonal planar

Electron Geometry of SnCl2

Trigonal planar

Electron Geometry of O2

Tetrahedral

Electron Geometry of SlCl4

Tetrahedral

Electron Geometry of PH2

Bent

Electron Geometry of SeBr2

Tetrahedral

Electron Geometry of Cl2

Solid line

bond in the plane

Wedge line

Bond in front of the plane

Dashed line

Bond behind the plane

Nonpolar

When electrons are equally shared, the bond is __________

Nonpolar

Whenever two different atoms having similar electronegativities are bonded together, the bond is _________

Polar covalent bond

Bonding between atoms with different electronegativities yields a ______________

Polar molecules

Has either one polar bond, or two or more bond dipoles that reinforce each other.

Nonpolar molecules

A nonpolar molecule has either no polar bonds, or two or more bond dipoles that cancel

Intermolecular forces

Attractive forces between molecules

Intramolecular forces

Hold atoms together in a molecule

Dipole-dipole forces

Attractive forces between polar molecules

London Dispersion Forces

Attractive forces that arise as a result of temporary dipoles induced in atoms or molecules

Ion-dipole forces

Attractive forces between an ion and a polar molecule

Ion-induced dipole interaction

Has a temporary separation of charge and temporarily creates a partial negative region and a partial positive region

Hydrogen bond

Special dipole-dipole interaction between the hydrogen atom in a polar N-H, O-H, or F-H bond and an electronegative O, N, or F atom.

Ion-dipole

Metal to non metal

Hydrogen bond

Dipole-dipole where H bonds with N, F, O

Dipole-dipole

Polar nonmetal bonds

LDF or VDW

All molecules; more electrons = strongest force

Higher

The larger the surface area, the ________ the boiling point

Higher

The more polarizable the atoms, the ______ the boiling point

Higher

The more symmetrical the compound, the ______ the melting point.

Ionic compounds

Ionic compounds soluble in water, but insoluble in organic solvents

Organic molecules

Water soluble only if it contains one polar functional group capable of hydrogen bonding with the solvent for every five C atoms it contains.

Butane and Acetone

They are both organic compounds so they are soluble in organic solvent CCl4

Water

Size of an organic molecule with a polar functional group determines it s water solubility

Hydrophobic

Nonpolar part of a molecule that is not attracted to H2O

Hydrophilic

Polar part of a molecule that can hydrogen bond to H2O

S orbital

Has a sphere of electron density and is lower in energy than the other orbitals of the same shell

p orbital

Has a dumbbell shape and contains a node (no electron density) at the nucleus and it is higher in energy than an s orbital

Linear

\

Trigonal planar

\

Bent

\

Tetrahedral

\

Bent

\

Trigonal bipyramidal

\

See-saw

\

T-shaped

\

Linear

\

Octahedral

\

Square pyramidal

\

Alkane

\

Alkene

\

Alkyne

Aromatic compound

Alkyl halide

Alcohol

Ether

Amine

Thiol

Sulfide

Aldehyde