Bonding and Nomenclature UnitAbout 3 weeksWill discuss the bonds that elements form

and how to name the compounds formedThere are many rules and procedures that

simply must be memorized and practicedTherefore, there will be small amounts of

homework regularly and several quizzes

Ionic Bonding

Covalent Bonding

Transfer of Electrons (e-)

Sharing Electrons (e-)Between (b/w)

cations & anions

B/w metals & nonmetals

B/w two nonmetals

Stronger than covalent bonding

Weaker than Ionic bonding

Soluble: ability to be dissolved

Can be soluble or insoluble depending on polarity

Therefore, higher melting point (mp), boiling point (bp) and hardness

Therefore, lower melting point (mp), boiling point (bp) and hardness

Sometimes referred to as a molecular compound (cmpd)Example: Na+

Cl- NaClSodium Chloride

Example: CO Carbon Monoxide

Cmpds shown as a

formula with chemical

symbols and numbers

Both follow Octet Rule: Cmpds form so that each atom

has an octet of ve-. Can lose,

gain or share to reach 8. Except H

which is full with 2.

Chemical bond: mutual electrical attraction between the nuclei and valance electrons of atoms which binds the atoms together.

Covalent BondingCan be either polar or non-polar

Polar: uneven distribution of charge caused by two different nonmetals bonding together. If there is a large enough difference, they can be soluble. Ex: C-O

Nonpolar: An even distribution of charge caused by the same non-metal bonded to one another. These are insoluble. Ex: Cl-Cl

Homework tonight! Define the key terms: Chapter 6, Sections 1, 2,

and 3 (page 208—21 words)

Tomorrow we will be drawing compounds as Lewis Dot Diagrams. You do not need your

book.