Covalent Bonding Diagrams Chapter 16 Notes, Part I Covalent Bonding Diagrams

An Addendum to Lewis Structures Carbon and silicon are exceptions to the pattern of how to place electrons in a Lewis Dot Structure. This is because they have hybrid orbitals (where the s and p sublevels blend together and have four equal energy orbitals.)

Covalent Bonding A covalent bond occurs between two non-metals Electrostatic bonding does not occur—in other words, there is no “give and take” of electrons

It ends up being a “tug of war” of electrons Where the electrons end up somewhere in the middle.

Single Bonds A single bond occurs when one pair of electrons is shared by two atoms. This pair of bonded electrons is called a shared pair.

Double and Triple Bonds Double bonds occur when two atoms have two shared pair of electrons Triple bonds occur when two atoms share three pair of electrons

Ionic compounds bonded together don’t really exist, but molecular compounds do!

Covalent Bonding Diagrams Like the ionic bonding diagrams, first draw the dot diagram for each element Now, however, the electrons are not being given away or taken, but shared; so signify a pair being shared by circling both electrons. Every element should have eight electrons (count each shared pair as two).

Covalent Bonding Diagrams If there is more than one of each element in the compound, you have to have a central atom. It will be the one with the most spots to bond to.

Hydrogen Since hydrogen is in the first energy level, it will not need 8 valence electrons to be stable—it will only need 2.

H2

H2O

Cl2

O2

N2

CCl4

CO2

HCN

PCl3

H2O2

C2H4

CSF2

SiS2

Covalent Bonding and Polyatomic ions A polyatomic ion is just a charged molecule that bonds covalently. The charge signifies how many electrons are given/taken away.

OH1-

NO21-

CO32-

PO33-