Covalent Bonding and Nomenclature

Unit 2 Notes

Ionic vs. Covalent Bonding (INTRAmolecular forces)

● Ionic Bonding - the TRANSFER of electrons from a metal to a nonmetal, creating cations and anions that attract one another

● Covalent Bonding - SHARING of electrons between two nonmetals so that both atoms have 8 valence electrons

Ionic vs. Covalent Bonding (INTRAmolecular forces)

● Ionic Bonding - the TRANSFER of electrons from a metal to a nonmetal, creating cations and anions that attract one another

● Covalent Bonding - SHARING of electrons between two nonmetals so that both atoms have 8 valence electrons

● BOTH: the goal of both is to make all atoms involved have a full valence electrons (most stable!), whether through the transfer or sharing of electrons

Ionic vs. Covalent Bonding (INTRAmolecular forces)

● Ionic Bonding - the TRANSFER of electrons from a metal to a nonmetal, creating cations and anions that attract one another

● Covalent Bonding - SHARING of electrons between two nonmetals so that both atoms have 8 valence electrons

Covalent Bonding (INTRAmolecular forces)

● Covalent Bonding - SHARING of electrons between two nonmetals so that both atoms have 8 valence electrons

Covalent Bonding (INTRAmolecular forces)

● Covalent Bonding - SHARING of electrons between two nonmetals so that both atoms have 8 valence electrons

Covalent Bonding (INTRAmolecular forces)

● Covalent Bonding - SHARING of electrons between two nonmetals so that both atoms have 8 valence electrons

Covalent Bonding (INTRAmolecular forces)

● Nonpolar Covalent Bond: ✓ Equal sharing of electrons✓ Difference in electronegativity < 0.5

● Polar Covalent Bond: ✓ Unequal sharing of electrons,

creating a dipole moment✓ Difference in electronegativity > 0.5

POLARITYPolar Molecules - Uneven distribution of electrons throughout molecule

Intermolecular Forces:Dipole-dipole and LDFHydrogen Bonding if hydrogen attached to FON and lone pair are present

Intramolecular Forces:Polar covalent bonds

POLARITYNonpolar Molecules - Even distribution of electrons throughout molecule

Intermolecular Forces:LDF ONLY

Intramolecular Forces:Nonpolar covalent bondsAND/OR polar covalent bonds if polar covalent bonds cancel

ઠ-

ઠ-

ઠ-

ઠ-

ઠ+

ALL POLAR BONDS CANCEL

ALL POLAR BONDS CANCEL

ALL NONPOLAR

BONDS

DIATOMIC MOLECULES

● Seven different elements on the periodic table exist in a diatomic form (nonpolar!)

Di = two

Atomic = atom

● Need to memorize these!

Naming Covalent Compounds

1. Use the element name to name the first element in the formula.

2. The second element is named as though it were an anion: root + ide

3. Prefixes are used to denote the numbers of atoms present.

* The prefix “mono-” is NEVER used for naming the first element!

NO2

Nitrogen dioxide

N2O5

Dinitrogen pentoxide

CCl4

Carbon tetrachloride

Metallic Bonding

● Metallic Bonding- like covalent bonding, but instead of two nonmetals sharing electrons, many metal atoms share many electrons (sea of delocalized electrons)○ Makes metals good conductors (allow electrons to flow!)