INTERMOLECULAR CHEMICAL BONDING

INTERMOLECULAR CHEMICAL BONDING

Covalent Disulfide Bond

Non-Covalent

Polar

Ion-Dipole

Dipole-Dipole

H-Bonding

Non-Polar

Vander Waals

Pi-Pi Complex

Hydrophobic

Force of attraction between molecules.

Covalent:Disulfide Bond

Covalent: Disulfide Bond

Attraction between cysteine residue.Linkage is also called an SS-bond or

disulfide bridge.Overall connectivity is therefore R-S-

S-R.

Covalent: Disulfide Bond

Formal Depiction of Disulfide Bond Formation as an Oxidation.

Covalent: Disulfide Bond

Cystine, which is Composed of Two Cysteines Linked by a Disulfide Bond.

Non-Covalent:Polar:Ion-Dipole

Non-Covalent: Polar:Ion-Dipole

Attraction between ionic compound and dipole molecule.

Cations are attracted to the negative end of a dipole .

Anions are attracted to the positive end of a dipole.

Ex. a salt in aqueous solvent

Non-Covalent: Polar:Ion-Dipole

An Ion-Dipole Force Exist Between a Charged Ion and a Polar

Molecule.

Non-Covalent:Polar:Dipole-Dipole

Non-Covalent: Polar:Dipole-Dipole

Attraction between opposite charges of polar molecule.

Polar molecules attract one another when the partial positive charge on one molecule is near the partial negative charge on the other molecule

The polar molecules must be in close proximity for the dipole-dipole forces to be significant.

Dipole-dipole forces are weaker than ion-dipole forces.

Non-Covalent: Polar:Dipole-Dipole

A Dipole-dipole Force Exists Between Neutral Polar Molecules.

Non-Covalent: Polar:Dipole-Dipole

HCL, With a Dipole-Dipole Force

Non-Covalent:Polar:Hydrogen Bond

Non-Covalent: Polar:Hydrogen Bond

Force of attraction between H and more electronegative atom of another molecule:√ Hydrogen – 2.1 √ Nitrogen – 3.0√ Oxygen – 3.5 √ Fluorine – 4.0

considered to be dipole-dipole type interactions, but are stronger than dipole-dipole forces.

Non-Covalent: Polar:Hydrogen Bond

The hydrogen atom has no inner core of electrons, so the side of the atom facing away from the bond represents a virtually naked nucleus.

This positive charge is attracted to the negative charge of an electronegative atom in a nearby molecule.

Because the hydrogen atom in a polar bond is electron-deficient on one side, this side of the hydrogen atom can get quite close to a neighboring electronegative atom.

Non-Covalent: Polar:Hydrogen Bond

Water, Forming an Extensive Hydrogen Bonding Network

Non-Covalent:Non-Polar:Vander Waals

Non-Covalent: Non-Polar:Vander Waals

Attraction between the proton and valence electron of another non-polar molecule.

Strength of VDW:SOLID>LIQUID>GAS

Non-Covalent:Non-Polar:Pi-Pi Complex

Non-Covalent: Non-Polar:Pi-Pi Complex

Interaction between aromatic molecules.

Also called pi-pi interaction or plot stocking.

Ex. Attraction between benzene and phenol.

Non-Covalent:Non-Polar:Hydrophobic

Non-Covalent: Non-Polar:Hydrophobic

HYDROPHOBIC MOLECULES

Are repelled by water (literally, hydrophobe means fear of water).

Includes alkanes, oils, fats, and other greasy substances.

Tend to be electrically neutral and non-polar and work better with neutral and non-polar solvents.

Often cluster together when dropped in water.

Non-Covalent: Non-Polar:Hydrophobic

Interaction between Hydrocarbons or other non-polar molecules.

In a hydrophobic interaction, water is rejecting the hydrophobic molecules in favor of bonding to itself (intermolecular H-bond).

Water bonds easily with polar molecules (likes dissolve likes).Since water itself is polar, it will prefer

water molecules (polar) rather than oil molecules (non-polar).

Hydrophobic molecules cluster together though they're not attracted to each other, because large numbers of like molecules are energetically more favorable than smaller numbers (thermodynamics).

Non-Covalent: Non-Polar:Hydrophobic

Intermolecular Chemical Bonding Group

Algaba, BealeCorpuz, Blessy JaneDamian, SharmaineManlulu, Ivan Joseph

Soriano, Euniqa DancilleTiu, Lorraine

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