Covalent Bonding Chap. 9. I.Why does it form? A.Octet rule An atom will gain, lose, or share electrons in order to get a full set

Covalent BondingCovalent Bonding

Chap. 9Chap. 9Chap. 9Chap. 9

I.I. Why does it form?Why does it form?


A.A. Octet rule Octet rule

An atom will gain, lose, or An atom will gain, lose, or shareshare electrons in order to get a full setelectrons in order to get a full set


A.A. Octet ruleOctet rule

B.B. Stability/Minimum energyStability/Minimum energy


II.II. What is a molecule?What is a molecule?

Molecule = covalent compoundMolecule = covalent compound


II.II. What is a molecule?What is a molecule?A.A. Non-metal with a non-metalNon-metal with a non-metal



B.B. Some molecules are diatomicSome molecules are diatomic

Molecules made of two of the Molecules made of two of the same atomsame atom



B.B. Some molecules are diatomicSome molecules are diatomic

C.C. PropertiesProperties

1.1. Often are gases or liquidsOften are gases or liquids

Properties of Covalent CompoundsProperties of Covalent Compounds


2.2. Tend to have lower M.P.Tend to have lower M.P.




3.3. Often are softOften are soft




3.3. Often are softOften are soft

4.4. Many are non-electrolytesMany are non-electrolytes


III.III. Representing MoleculesRepresenting Molecules

Lewis structure uses dots and dashes Lewis structure uses dots and dashes to represent electrons and bondsto represent electrons and bonds


IV.IV. Covalent Bond typesCovalent Bond types


IV.IV. Covalent Bond typesCovalent Bond typesA.A. Single bondSingle bond

Bond made of one Bond made of one pairpair of of shared electronsshared electrons



B.B. Double bondDouble bond

Bond made of two Bond made of two pairspairs of of shared electronsshared electrons




C.C. Triple bondTriple bond

Bond made of three Bond made of three pairspairs of of shared electronsshared electrons




C.C. Triple bondTriple bond

D.D. Quadruple bond?Quadruple bond?



V.V. Bond strengthBond strength

Bond energy measures the bond Bond energy measures the bond strength.strength.



V.V. Bond strengthBond strengthA.A. The longer the bond the The longer the bond the

______ the bond energy______ the bond energy



V.V. Bond strengthBond strengthA.A. The longer the bond the The longer the bond the

______ the bond energy______ the bond energy

B.B. Double bonds require Double bonds require _____ energy to break _____ energy to break than single bonds.than single bonds.

Bond energy exampleBond energy example

HH22 + Cl + Cl22 2HCl 2HCl

H-H 436 kJ

Cl-Cl 242 kJ

HCl 431 kJ

What is the energy change for What is the energy change for this reaction? Is it exothermic?this reaction? Is it exothermic?

VI. Naming Covalent VI. Naming Covalent CompoundsCompounds


A.A. Binary Inorganic Binary Inorganic MoleculesMolecules

Rules for Naming Rules for Naming Covalent CompoundsCovalent Compounds


1. Name the first. . .1. Name the first. . .


1. Name the first. . .

2. Name the second with. . .






3. Use prefixes to tell. . .








4. Never begin name with . . .




4. Never begin name with . . .

Prefixes for Prefixes for Numbers of AtomsNumbers of Atoms


1. mono-1. mono-


1. mono-

2. di-

1. mono-

2. di-


1. mono-

2. di-

3. tri-

1. mono-

2. di-

3. tri-


1. mono-

2. di-

3. tri-

4. tetra-

1. mono-

2. di-

3. tri-

4. tetra-


1. mono-

2. di-

3. tri-

4. tetra-

5. penta-

1. mono-

2. di-

3. tri-

4. tetra-

5. penta-


1. mono- 6. hexa-

2. di-

3. tri-

4. tetra-

5. penta-

1. mono- 6. hexa-

2. di-

3. tri-

4. tetra-

5. penta-


1. mono- 6. hexa-

2. di- 7. hepta-

3. tri-

4. tetra-

5. penta-

1. mono- 6. hexa-

2. di- 7. hepta-

3. tri-

4. tetra-

5. penta-


1. mono- 6. hexa-

2. di- 7. hepta-

3. tri- 8. octa-

4. tetra-

5. penta-

1. mono- 6. hexa-

2. di- 7. hepta-

3. tri- 8. octa-

4. tetra-

5. penta-


1. mono- 6. hexa-

2. di- 7. hepta-

3. tri- 8. octa-

4. tetra- 9. nona-

5. penta-

1. mono- 6. hexa-

2. di- 7. hepta-

3. tri- 8. octa-

4. tetra- 9. nona-

5. penta-


1. mono- 6. hexa-

2. di- 7. hepta-

3. tri- 8. octa-

4. tetra- 9. nona-

5. penta- 10. deca-

1. mono- 6. hexa-

2. di- 7. hepta-

3. tri- 8. octa-

4. tetra- 9. nona-

5. penta- 10. deca-





4. Never begin name with. . .




4. Never begin name with. . .



B.B. Common NamesCommon Names

Covalent compounds with carbon



B.B. Common NamesCommon Names

C.C. Organic MoleculesOrganic Molecules

Names for organic Names for organic hydrocarbonshydrocarbons


CH4 methaneCH4 methane


CH4 methane

C2H6 ethane

CH4 methane

C2H6 ethane


CH4 methane

C2H6 ethane

C3H8 propane

CH4 methane

C2H6 ethane

C3H8 propane


CH4 methane

C2H6 ethane

C3H8 propane

C4H10 butane

CH4 methane

C2H6 ethane

C3H8 propane

C4H10 butane


CH4 methane

C2H6 ethane

C3H8 propane

C4H10 butane

C5H12 pentane

CH4 methane

C2H6 ethane

C3H8 propane

C4H10 butane

C5H12 pentane


C6H14

C7H16

C8H18

C9H20

C10H22

C6H14

C7H16

C8H18

C9H20

C10H22


C6H14 hexane

C7H16

C8H18

C9H20

C10H22

C6H14 hexane

C7H16

C8H18

C9H20

C10H22


C6H14 hexane

C7H16 heptane

C8H18

C9H20

C10H22

C6H14 hexane

C7H16 heptane

C8H18

C9H20

C10H22


C6H14 hexane

C7H16 heptane

C8H18 octane

C9H20

C10H22

C6H14 hexane

C7H16 heptane

C8H18 octane

C9H20

C10H22


C6H14 hexane

C7H16 heptane

C8H18 octane

C9H20 nonane

C10H22

C6H14 hexane

C7H16 heptane

C8H18 octane

C9H20 nonane

C10H22


C6H14 hexane

C7H16 heptane

C8H18 octane

C9H20 nonane

C10H22 decane

C6H14 hexane

C7H16 heptane

C8H18 octane

C9H20 nonane

C10H22 decane

Self Check 1Self Check 1

PFPF33 SFSF66

CSCS22 SiHSiH44

Write the names for these compoundsWrite the names for these compounds


Carbon tetrachlorideCarbon tetrachloride

Diphosphorus decachlorideDiphosphorus decachloride

Write the formulas for these compoundsWrite the formulas for these compounds

Acids are hydrogen-donating compounds


D.D. Naming acidsNaming acids

Acids composed of H+ ion and a monatomic anion.



1.1. Binary AcidsBinary Acids

Rules for Naming AcidsRules for Naming AcidsAnion NameAnion Name Acid NameAcid Name

chloridechloride Hydrochloric acidHydrochloric acid

FormulaFormula


chloride

fluoride

chloride

fluoride

Hydrochloric acid

Hydrofluoric acid

Hydrochloric acid

Hydrofluoric acid

FormulaFormula


chloride

fluoride

bromide

chloride

fluoride

bromide

Hydrochloric acid

Hydrofluoric acid

??

Hydrochloric acid

Hydrofluoric acid

??

FormulaFormula


chloride

fluoride

bromide

chloride

fluoride

bromide

Hydrochloric acid

Hydrofluoric acid

Hydrobromic acid

Hydrochloric acid

Hydrofluoric acid

Hydrobromic acid

FormulaFormula


chloride

fluoride

bromide

____-ide

chloride

fluoride

bromide

____-ide

Hydrochloric acid

Hydrofluoric acid

Hydrobromic acid

Hydro____ic acid

Hydrochloric acid

Hydrofluoric acid

Hydrobromic acid

Hydro____ic acid

FormulaFormula



1.1. Binary AcidsBinary Acids

2.2. OxyacidsOxyacids

Acids composed of H+ ion and a polyatomic anion containing oxygen.

Rules for Naming OxyacidsRules for Naming OxyacidsAnion NameAnion Name Acid NameAcid Name

chloratechlorate Chloric acidChloric acid

FormulaFormula


chlorate

nitrate

chlorate

nitrate

Chloric acid

Nitric acid

Chloric acid

Nitric acid

FormulaFormula


chlorate

nitrate

sulfate

chlorate

nitrate

sulfate

Chloric acid

Nitric acid

??

Chloric acid

Nitric acid

??

FormulaFormula


chlorate

nitrate

Sulfate

chlorate

nitrate

Sulfate

Chloric acid

Nitric acid

Sulfuric acid

Chloric acid

Nitric acid

Sulfuric acid

FormulaFormula


chlorate

nitrate

Sulfate

______ate

chlorate

nitrate

Sulfate

______ate

Chloric acid

Nitric acid

Sulfuric acid

______ic acid

Chloric acid

Nitric acid

Sulfuric acid

______ic acid

FormulaFormula


chloritechlorite Chlorous acidChlorous acid

FormulaFormula


chlorite

nitrite

chlorite

nitrite

Chlorous acid

Nitrous acid

Chlorous acid

Nitrous acid

FormulaFormula


chlorite

nitrite

sulfite

chlorite

nitrite

sulfite

Chlorous acid

Nitrous acid

??

Chlorous acid

Nitrous acid

??

FormulaFormula


chlorite

nitrite

sulfite

chlorite

nitrite

sulfite

Chlorous acid

Nitrous acid

Sulfurous acid

Chlorous acid

Nitrous acid

Sulfurous acid

FormulaFormula


chlorite

nitrite

sulfite

____ite

chlorite

nitrite

sulfite

____ite

Chlorous acid

Nitrous acid

Sulfurous acid

______ous acid

Chlorous acid

Nitrous acid

Sulfurous acid

______ous acid

FormulaFormula


Carbonic acidCarbonic acid

Phosphoric acidPhosphoric acid

Acetic acidAcetic acid

Write the formulas for these compoundsWrite the formulas for these compounds

VII. Structural FormulasVII. Structural Formulas

A Lewis structure shows which atoms are bonded to which.

Valence electrons = outermost electrons.

VII. Structural FormulasVII. Structural FormulasA.A. Valence electrons importantValence electrons important

Pair of electrons shared between two elements.


1.1. Bonding ElectronsBonding Electrons

Pair of electrons not being shared.


1.1. Bonding ElectronsBonding Electrons

2.2. Lone pairsLone pairs


B.B. Drawing a Lewis structureDrawing a Lewis structure



1.1. for moleculesfor molecules

Rules for Lewis StructuresRules for Lewis Structures

1. Determine the total . . .1. Determine the total . . .



2. Join all elements with . . .2. Join all elements with . . .



2. Join all elements with . . .2. Join all elements with . . .

3. Arrange remaining . . . 3. Arrange remaining . . .




2.2. for molecules with multiple bondsfor molecules with multiple bonds





3.3. for ionsfor ions


CHCH33ClCl

CSCS22

Phosphorus trifluoridePhosphorus trifluoride

Dichlorine monoxideDichlorine monoxide

Draw a Lewis structure for: Draw a Lewis structure for:





3.3. for ionsfor ions

4.4. resonance structuresresonance structures

Concept that a molecule is Concept that a molecule is described by more than one described by more than one structurestructure

ResonanceResonance



C.C. ExceptionsExceptions



C.C. ExceptionsExceptions1.1. odd number of electronsodd number of electrons




2.2. less than an octetless than an octet




2.2. less than an octetless than an octet

3.3. more than an octetmore than an octet

VIII. Molecular ShapeVIII. Molecular Shape

VIII. Molecular ShapeVIII. Molecular ShapeA.A. VSEPR TheoryVSEPR Theory

Valence shell electron pair repulsion theory: electrons are placed at maximum distances from other electrons


B.B. Molecular ShapesMolecular Shapes


B.B. Molecular ShapesMolecular Shapes1.1. Linear (BeClLinear (BeCl22))



2.2. Trigonal planar (BFTrigonal planar (BF33))




3.3. Tetrahedral (CHTetrahedral (CH44))




3.3. Tetrahedral (CHTetrahedral (CH44))a.a. trigonal pyramidal (NHtrigonal pyramidal (NH33))




3.3. Tetrahedral (CHTetrahedral (CH44))a.a. trigonal pyramidaltrigonal pyramidal

b.b. bentbent





4.4. Trigonal bipyramidalTrigonal bipyramidal





4.4. Trigonal bipyramidalTrigonal bipyramidal

5.5. OctahedralOctahedral

IX. PolarityIX. Polarity

IX. PolarityIX. PolarityA.A. When is a bond polar?When is a bond polar?

Polar bonds occur when electrons are shared unequally.

Bond typesBond typesElectronegativityElectronegativity BondBondDifferenceDifference TypeType


0.0 – 0.40.0 – 0.4 non-polar non-polar covalentcovalent



0.5 – 1.90.5 – 1.9 polar polar covalentcovalent



0.5 – 1.90.5 – 1.9 polar polar covalentcovalent

1.9 -1.9 - ionicionic

“CO

VA

LE

NT

”

Electronegativity Difference

0.5 1.0 1.5 2.0 2.5 3.0 3.5

Bond typesBond types

IX. PolarityIX. PolarityA.A. When is a bond polar?When is a bond polar?

B.B. When is a molecule polar?When is a molecule polar?

Polar molecules contain polar bonds and are NOT symmetrical.


Are the bonds in ammonia (NHAre the bonds in ammonia (NH33) )

polar? polar?

Is the molecule polar?Is the molecule polar?

The EndThe End

Documents

Covalent Bonding Chap. 9. I.Why does it form? A.Octet rule An atom will gain, lose, or share electrons in order to get a full set