Covalent Bonding

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Types of Bonds Review

Metallic

Ionic

Covalent

Transfer

Electrons

Delocalized

Electrons

(sea of e-)

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Electrons

Molecule

UnitCell

Electronegativity and bond types• Another way to usually tell whether a bond is

ionic or covalent is with electronegativities

• Electronegativity (Page 194)– the tendency of an atom to gain electrons in a chemical bond.

• If the difference between the electronegativities is large, the bond tends to be ionic. If it is small, it tends to be covalent.

• Compounds can have both, but usually show one type more than the other chemically, usually ionic).

Naming Covalent Compound

Types of Covalent Compounds• Diatomic molecules (twins):

________________________________

________________________________

• NEVER FOUND AS SINGLE

ATOMS if “alone”

• Their names are just the name of the element

H2, N2, O2, F2, Cl2, Br2, I2

There are seven diatomic molecules

Binary Molecular Compounds ___________________________(no metals or

ions) i.e. Does not start with an H.

• Steps to name compoundsa. _________ _________ - use entire nameb. _________ _________ - change ending to –idec. Prefixes used to indicate _________ of atoms of

each p. 832• Only time that no prefix is used is if the first is

a one• Examples:

CCl4 –As2O3 –

Non-metals with no H+

Name firstName second

number

triditetrachloridecarbon

arsenic oxide

The PrefixesMono- monocle Tri- tricycle

Penta- pentagon Octa- octopusTetra- Tetris

Di-Dialogue

Acids

• Always begin with ______

• Two Types: _________ and ___________

H+

oxyacidbinary

Remember: The number of hydrogen atoms in the acid

equals the charge of the anion

Binary Acids

• Binary Acids - ______ but no _______

• Steps to name compoundsa. Use prefix - _________

b. Root of second element plus suffix - _________ followed by the word acid

• Example:

HCl -

H+ O

hydro

-ic

hydrochloric acid

Oxyacids

• – has a ________________, so most have ___

Steps to name compounds• Identify polyatomic ion p. 178

a. Use root of anion, change suffix ending and word acida. Suffix rules: ends in ate change to _________

b. ends in ite change to _________

Example:

HNO3 -

polyatomic ion

-ic

-ous

nitric acid

O

Hydrocarbons• a compound containing carbon and hydrogen

• Named using prefixes that correspond to the number of carbons in the compound.

• 1 – meth

• 2 – eth

• 3 – prop

• 4 – but

• After this it used the “normal” prefixes

Hydrocarbons• Ending refers to the type of functional group

found in the compound. • -ane – alkane - simplest hydrocarbon - only

has single bonded carbons with hydrogens (2(Carbon atoms)+2).

• -ene – alkene - has a double bonded carbon in the formula

• -yne – alkyne - has a triple bonded carbon in the formula

More functional groupsClass Attached Functional

GroupEffect on Name

Alcohol

Changes end to -ol

Aldehyde Changes end to -al

Amine Changes end to -amine (or starts with amino-)

Carboxylic acid Changes end to -oic acid

Ester Divides compound in two parts, side without O is named as functional group, side with O will end with -oate

Ether Divides compound in two parts, name both halves as a functional group and add ether to the end

Ketone Changes end to -one

Practice

Formula Type of Covalent Bond Name

PCl5

HI

N2

C2H6

H3PO4

HClO2

N2H4Dinitrogen

tetrahydride

Phosphic acid

Nitrogen

Hydroiodic acid

Binary Molecular

Diatomic

Binary Acid

Phosphorous pentachlorideBinary Molecular

Oxyacid

Oxyacid Chlorous acid

Hydrocarbon ethane