Name:___________________________
Period:__________________________
Chemistry Unit 6 – Covalent Compounds and Covalent Bonding
Chemistry Daily Journal
Today’s
Date
What do I need to accomplish today?
What do I need to finish up at home?
Objective
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Learning Opportunities
6.1 Write Names and Formulas
for Covalent Compounds
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Podcast 5.5 Bonding Basics
Read p. 268-270; Questions 20-24 p. 270
Naming Molecular Compounds
Writing Formulas From Names
Naming Covalent Compounds Quiz (12/2)
Podcast 5.6 Molecular Structures
Molecular Structural Formulas
Electronegativity and Polarity POGIL 12/2
Unit 6 Review 12/4
Unit 6 Molecular Geometry Quiz 12/5
6.2 Sketch Molecular Structures
for Covalent Compounds
6.3 Determine if a Compound is
Nonpolar Covalent, Polar
Covalent, or Ionic
Suggested
Due Date
12/01/14
Date
Completed
12/04/14
12/05/14
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Podcast 5.5: Naming Covalent Compounds
What is a covalent bond?
 Atoms ______________________ one or more electrons with each other to form the bond.

Each atom is left with a ______________________ outer shell.

A covalent bond forms between two ______________________.
Example C1: Hydrogen + Hydrogen
Example C2: 2 Hydrogen + Oxygen
Example C3: Chlorine + Chlorine
Example C4: Oxygen + Oxygen
Example C5: Carbon + 2 Oxygen
Example C6: Carbon + 4 Hydrogen
Challenge: What are some other ionic or covalent bonds that can be formed by the elements you see? Write the chemical formula for the
compound and its name on a separate piece of paper and attach to this page.
-ide ending, each element has “prefix”
 prefix refers to _________________ of __________ – NOT CHARGE
N2O4 =
 Exception: drop mono- for ________element
CO2 =
 The first vowel is often dropped to avoid the combination of “___” or “___”.
1
2
3
4
5
6
7
8
9
10
mono
di
tri
tetra
penta
hexa
hepta
octo
nono
deca
CO =
P4O10 =
SO2 =
Example: Name the following covalent compounds.
a) CCl4
b) P2O3
c) IF7
Writing Formulas from Names
1. Identify the ____________________ involved
2. Use the ______________to write the formula
Examples:
a) Nitrogen dioxide
c) Tetraphosphorous decoxide
b) Dinitrogen trioxide
d) Xenon tetrafluoride
WARNING!!! **Decide whether the compound is ionic or covalent BEFORE trying to name it or write it’s formula!
Example: Fe2O3 is called ____________________ or iron (III) oxide, NOT di-iron trioxide
MEMORIZE THIS ONE:
NH3 is called ___________. Nitrogen trihydride is OK, but it already has a name
2
Naming Molecular Compounds
A. Name the following molecular compounds.
1. CO2
_______________________________
11. PCl3 ____________________________
2. CO
_______________________________
12. PCl5 ____________________________
3. SO2
_______________________________
13. NH3 ____________________________
4. SO3
_______________________________
14. SCl6 ____________________________
5. N2O
_______________________________
15. P2O5 ____________________________
6. NO
_______________________________
16. CCl4 ____________________________
7. N2O3 _______________________________
17. SiO2 ____________________________
8. NO2
_______________________________
18. CS2
____________________________
9. N2O4 _______________________________
19. OF2
____________________________
10. N2O5 _______________________________
20. PBr3 _____________________________
B. Write formulas for the following molecular compounds.
1. Carbon monoxide
___________________
2. Diphosphorus pentaoxide
___________________
3. Sulfur dioxide
___________________
4. Phosphorus tribromide
___________________
5. Dinitrogen tetraoxide
___________________
6. Sulfur hexachloride
___________________
7. Oxygen difluoride
___________________
8. Carbon disulfide
___________________
9. Iodine heptafluoride
___________________
10. Chlorine trifluoride
___________________
11. Phosphorus pentabromide
___________________
12.
Dichlorine heptoxide
___________________
13. Trisilicon Tetranitride
___________________
14. Phosphorus pentabromide
___________________
15. Dicarbon octabromide
___________________
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Naming Molecular Compounds
1. CO2
_______________________________
6. Chlorine trifluoride
____________
2. PCl3
_______________________________
7. Phosphorus tribromide
____________
3. SO3
_______________________________
8. Dichlorine heptoxide
____________
4. SCl6
_______________________________
9. Phosphorus pentabromide ____________
5. N2O5 _______________________________
10. Carbon monoxide
____________
Naming ALL Compounds
For this section you will be naming ionic compound, molecular compounds. You will need to determine
what type of compound it is and them name it correctly. Give the stock name when appropriate.
Formula
Type of Compound
Name
1. SF6
2. PbCl2
3. ZnSO4
4. Al(OH)3
5. Al2O3
6. N2O3
For this section you will be given the name of a compound. You will need to determine what type of
compound it is (ionic, molecular, acid, or base) and write the correct formula.
Name
Type of Compound
Chemical Formula
7. Lead (II) sulfide
8. Zinc hydroxide
9. Ammonium carbonate
10. Chromium (III) sulfite
11. Sulfur trioxide
12. Tetraphosphorus decoxide
13. Plumbic carbonate
14. Sodium hydroxide
15. Barium sulfite
16. Carbon tetrachloride
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Podcast 5.6: Molecular Structures
Molecular Compounds
• Molecule
– A ______________ group of atoms joined together by covalent bonds
• Covalent Bond
– Sharing of electrons between two or more ____________________
Molecular Formulas
• Represents how many atoms of each element are in the compound
– Cannot be determined by the
__________ - ___________ Method
– Can be determined by creating a structural (Lewis dot) formula
• Octet Rule
– Atoms still tend to attain the electron configuration for a __________ ________ by sharing electrons
Structural Formula
 Shows the arrangement of covalently bonded atoms using ______________ as bonds (shared electrons) and
_____________ as unshared electrons
 Example – Hydrogen

(Lewis Dot Structure)
Creates an electron configuration of _____________ (noble gas) for both hydrogens by sharing the electrons
(Structural Formula)
Shared electrons represented by a dash
Drawing Structural Formulas – Steps
1) Count the _____________________________________________________ for the compound
ex. CH4 (methane)
2) Arrange the __________________
– _________________ is NEVER in the middle
– Elements with only one atom are typically in the middle and usually written _____________ in the formula
3) Fill in electrons, starting around the ___________ atom(s) until all your valence electrons are used.
4) Draw ________________ (dashes) for any _______________electron pairs and leave all unshared electrons where they
are.
Drawing Structural Formulas – Now Try These
– H2O
–
F2
–
NH3
Bond Order
• Single Bond
– Two atoms held together by sharing ______ electrons (1 pair)
• Double Bond
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•
•
•
•
– Two atoms held together by sharing ______ electrons (2 pairs)
Triple Bond
– Two atoms held together by sharing ______ electrons (3 pairs)
Double and triple bonds NEVER form with ________________ or the ___________________!!
Examples
Double and triple bonds are needed sometimes to satisfy the ________________ rule for all the atoms in the
compound.
Exceptions to Octet Rule (Page 228)
– For small atoms, like Boron
• BF3
– For some atoms in the 3p-block that have access to d-orbitals and can be _________-____________
• PCl5 or SF6
Molecular Shape
• Compounds are ______________-DIMENSIONAL
• ____________
– Valence-Shell Electron-Pair Repulsion Theory
– The negative charge on electrons _________ each other creating molecular shapes where the electrons are
as far away from each other as possible.
Common Shapes
• Tetrahedral (Angle – 109.5⁰)
•
Trigonal Pyramidal
•
Bent
•
Linear
•
Trigonal Planar
•
There are others – page 233
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Name: _______________________
Molecular Formulas
Lewis Dot, Structural Formulas, and Shape
For each of the compounds below, create the Lewis dot structure, structural formula, and a 3-D model. Be sure to show your work for calculating the number of valence
electrons and give the shape of the molecule.
Molecular
Formula
Valence Electron
Calculations
Lewis Dot Structure
Structural Formula
Shape
Polar
Bonds?
Yes/No
Polar
Molecule?
Yes/No
1. H2O
2. CH4
3. HCl
4. C2H6
5. NH3
6. CO2
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Molecular
Formula
Valence Electron
Calculations
Lewis Dot Structure
Structural Formula
Shape
Polar
Bonds?
Yes/No
Polar
Molecule?
Yes/No
7. H2O2
8. H2CO
(Try building this
before drawing it)
9. H2S
10. C3H8
11. PCl3
12. CCl4
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Molecular
Formula
Valence Electron
Calculations
Lewis Dot Structure
Structural Formula
Shape
Polar
Bonds?
Yes/No
Polar
Molecule?
Yes/No
13. NO2
14. NO2-1
15. CO3 2-
16. HCN
Use the table bellow to answer determine the shape of each molecule (more shapes can be found on p. 233 in your textbook):
Bonding Pairs
4
3
2
1
Non-Bonding Pairs
0
1
2
3
Molecular Shape
Tetrahedral
Pyramidal
Bent
Linear
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Molecular Compounds Review
1. Describe the difference between an ionic , a metallic, and a covalent bond.
2. How many ELECTRONS do two atoms in a triple bond share?
3. How many VALENCE ELECTRONS are in a molecule of Cl2O?
4. How many VALENCE ELECTRONS are in a molecule of CuC2H3O2?
Use the table bellow to answer the following three questions:
Bonding Pairs
Non-Bonding Pairs
4
0
3
1
2
2
1
3
Molecular Shape
Tetrahedral
Pyramidal
Bent
Linear
5. Draw the structural formula (with the dashes) of I2 and give the shape of the molecule. Describe whether the
BONDS on the central atom are polar or nonpolar. Then tell whether the overall molecule is polar or
nonpolar.
6. Draw the structural formula (with the dashes) of PF3 and give the shape of the molecule. Describe whether
the BONDS on the central atom are polar or nonpolar. Then tell whether the overall molecule is polar or
nonpolar.
7. Draw the structural formula (with the dashes) of SCl2 and give the shape of the molecule. Describe whether
the BONDS on the central atom are polar or nonpolar. Then tell whether the overall molecule is polar or
nonpolar.
8. Determine if the following substances are ionic compounds, molecular compounds, then name the substance
or give its chemical formula (not just the charges).
Type of compound
a.
Name/Formula
PI3
____________________
__________________________________
b. K2CO3
____________________
__________________________________
c. KI
____________________
__________________________________
d. Nitrogen dioxide
____________________
__________________________________
e. Tin (IV) cyanide
____________________
__________________________________
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