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. 2. Fill out the Ionic Compound column of the graphic organizer.
Do Now
1. Write down one goal you have for yourself in this class for Marking Period 2.
2. Fill out the Ionic Compound column of the graphic organizer.
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3. Magnesium and Fluorine Calcium and Sulfur Potassium and Nitrogen
Do Now
Write the formula of the ionic compound formed when the following elements combine:
Sodium and Chlorine
Lithium and Oxygen
Magnesium and Fluorine
Calcium and Sulfur
Potassium and Nitrogen
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4. Late assignments will result in a grade reduction of 10 pts per day.
Homework Policy
Late assignments will result in a grade reduction of 10 pts per day.
2 missed assignments will result in parental notification.
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5. Molecules and Molecular Compounds
In nature, only the noble gas elements exist as uncombined atoms.
They are monatomic; that is, they consist of single atoms.
Helium, which is less dense
than air, is often used to
inflate balloons.
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6. Molecules and Molecular Compounds
There are two ways elements can be like the nearest noble gas.
Transfer electrons to form an ionic compound.
Share electrons to form covalent compounds.
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7. 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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8. Molecules and Molecular Compounds
Covalent bond: a bond in which atoms are held together through the sharing of electrons
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9. Electronegativity – ability of an atom to attract electrons when it is in a compound.
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10. Molecules and Molecular Compounds
The electronegativity difference between two atoms tells you what kind of bond is likely to form.
>2.0 tends to form an ionic bond
<2 tends to form a covalent bond
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11. Molecules and Molecular Compounds
Molecule: a neutral group of atoms joined together by covalent bonds
Examples: F2
H2O
CH4
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12. Molecules and Molecular Compounds
Diatomic molecule—a molecule that contains two atoms.
Other elements found in nature in the form of diatomic molecules include hydrogen, nitrogen, oxygen, and the halogens.
HOFBrINCl
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13. Molecules and Molecular Compounds
Draw the electron dot structures for the following molecules.
Chlorine, Cl2
Bromine, Br2
Iodine, I2
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14. Molecules and Molecular Compounds
Molecules can also be made of atoms of different elements.
- Examples: H2O (water), CO2 (carbon dioxide), and N2O (nitrous oxide)
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15. Molecules and Molecular Compounds
Molecular formula - chemical formula of a molecular compound.
shows how many atoms of each element a substance contains
H2O – 2 Hydrogen, 1 Oxygen
C4H10 – 4 Carbon, 10 Hydrogen
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16. Molecules and Molecular Compounds
Identify the number and kinds of atoms present in a molecule of each compound.
C6H8O6 – ascorbic acid (vitamin C)
C12H22O11 – sucrose (table sugar)
C7H5N3O6 – trinitrotoluene (TNT)
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17. Comparing Molecular and Ionic Compounds
Properties of Molecular Compounds
Lower melting and boiling points than ionic compounds
Solids, liquids or gases at room temperature
Composed of atoms of two or more nonmetals
Do not conduct electricity
Do not dissolve in water as well as ionic compounds
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18. Comparing Molecular and Ionic Compounds
Water, which is a molecular compound, and sodium chloride, which is an ionic compound, are compared here.
Array of
sodium ions and
chloride ions
Collection of
water molecules
Formula unit of
sodium chloride
Molecule of
water
Chemical formula
H2O
NaCl
Chemical formula
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19. 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
High or low melting point? Conduct electricity?
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20. END OF 8.1
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