1. Chapter 8 Covalent Bonding 8.1 Molecular Compounds
8.2 The Nature of Covalent Bonding
8.3 Bonding Theories
8.4 Polar Bonds and Molecules
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2. Do Now
Identify each property as that of an ionic or covalent compound.
High melting point
Low difference in electronegativity of atoms
Conducts electricity when dissolved in water or melted
Identify each compound as ionic or covalent
CaCl2
NI3
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3. Molecules and Molecular Compounds
Use the element cards and chips to model the bonding of 2 fluorine atoms.
Each chip is one valence electron.
How can they share electrons to achieve the electron configurations of a noble gas?
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4. Molecules and Molecular Compounds
Covalent bond: a bond in which atoms are held together through the sharing of electrons
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5. Molecules and Molecular Compounds
Molecule: neutral group of atoms joined together by covalent bonds
Examples: F2
H2O
CH4
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6. Molecules and Molecular Compounds
Molecular formula - shows how many atoms of each element a molecule contains
H2O - water
C4H10 - butane
C7H5N3O6 – trinitrotoluene (TNT)
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7. Molecules and Molecular Compounds
Diatomic molecule - molecule that contains two atoms.
HOFBrINCl
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8. Atoms of nonmetals can combine in more than one way.
C O O = C = O
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9. Binary Molecular Compounds
Does NOT occur naturally in the atmosphere
Occurs naturally in the atmosphere
Result of oxygen starved combustion in improperly ventilated fuel-burned equipment
Natural by product of respiration, fermentation, chemical reactions, and combustion fossil fuels/woods
Common type of fatal poisoning
Poisoning is rare
Flammable gas
Non-flammable gas
Symptoms: confusion, nausea, lassitude, syncope, cyanosis, chest pain, abdominal pain
Symptoms: sweating, increased heart rate, frostbite, convulsion, panic, memory problems
Target organ: lungs, blood, central nervous system
Target organ: respiratory system
OSHA permissible exposure limit: 50 ppm
OSHA permissible exposure limit: 5,000 ppm
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10. Naming Molecular Compounds
Look at the list of covalent compounds. See if you can find any patterns in how they are named.
FORMULA
NAME
NO2
Nitrogen Dioxide
N2O3
Dinitrogen Trioxide
CCl4
Carbon Tetrachloride
Cl2O
Dichlorine Monoxide
S2Cl2
Disulfur Dichloride
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11. Binary Molecular Compounds
Prefixes Used in Naming Binary Molecular Compounds
Prefix
Number
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8
nona- 9
deca- 10
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12. Binary Molecular Compounds
Naming binary molecular compounds
Write names of elements in the order listed in formula.
Use prefixes to indicate number of each kind of atom.
- Mono is not used on the first element.
- Vowel at end of prefix is sometimes dropped
End the name of the second element with the suffix -ide.
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13. Naming Binary Molecular Compounds
Sample Problem 9.6
Naming Binary Molecular Compounds
Name the following binary molecular compounds.
N2O
PCl3
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14. Naming Binary Molecular Compounds
Sample Problem 9.6
Naming Binary Molecular Compounds
Name the following binary molecular compounds.
N2O - dinitrogen monoxide
PCl3 - phosphorus trichloride
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15. Writing Formulas for Binary Molecular Compounds
Sample Problem 9.7
Writing Formulas for Binary Molecular Compounds
Write formulas for the following binary molecular compounds.
nitrogen trifluoride
disulfur dichloride
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16. Writing Formulas for Binary Molecular Compounds
Sample Problem 9.7
Writing Formulas for Binary Molecular Compounds
Write formulas for the following binary molecular compounds.
nitrogen trifluoride -
disulfur dichloride -
NF3
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17. Comparing Molecular and Ionic Compounds
Properties of Molecular Compounds
Composed of two or more nonmetals
Lower melting and boiling points
Solids, liquids or gases at room temp.
Do not conduct electricity
Do not dissolve in water as well as ionic compounds
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18. Molecules and Molecular Compounds
Classify compounds into groups according to their chemical bonding (ionic or covalent).
Sodium Chloride, NaCl
Methane, CH4
Oxygen, O2
Ammonia, NH3
Magnesium Oxide, MgO
Barium Iodide, BaI2
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19. Comparing Molecular and Ionic Compounds
Water
Molecular Compound
Sodium Chloride
Ionic Compound
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20. END OF 8.1
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