Clicker Questions

1
Clicker Questions

• Review

2
As atoms bond with each other, they

• increase their potential energy, thus creating
  less-stable arrangements of matter.
• decrease their potential energy, thus creating
  less-stable arrangements of matter.
• increase their potential energy, thus creating
  more-stable arrangements of matter.
• decrease their potential energy, thus creating
  more-stable arrangements of matter.

3
A compound that conducts electricity and is a
solid at room temperature is usually

1. Ionic
2. Covalent

4
As light strikes the surface of a metal, the
electrons in the electron sea

1. a. allow the light to pass through.
2. b. become attached to particular positive ions.
3. c. fall to lower energy levels.
4. d. absorb and re-emit the light.

5
Most chemical bonds are

1. purely ionic.
2. purely covalent.
3. partly ionic and partly covalent.
4. metallic.

6
Dinitrogen pentoxide contains how many oxygens?

• 5
• 0.0

7
In the compound Fe2O3, the charge of iron is

• 3
• 0.0

8
If you were to bond Tin (IV) with oxygen (-2
charge), what is the subscript behind oxygen?
(Sn_O?)

• 2
• 0.0

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An ionic bond is between

1. Two or more metals
2. A metal and a non-metal
3. Two or more non-metals
4. All of the above

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A covalent bond is between

1. Two or more metals
2. A metal and a non-metal
3. Two or more non-metals
4. All of the above

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II. Molecular Compounds

• Chemical Bonding

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A. Energy of Bond Formation

• Potential Energy
• based on position of an object
• low PE high stability

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A. Energy of Bond Formation

• Potential Energy Diagram

attraction vs. repulsion
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A. Energy of Bond Formation

• Potential Energy Diagram

attraction vs. repulsion
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A. Energy of Bond Formation

• Bond Energy
• Energy required to break a bond

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A. Energy of Bond Formation

• Bond Energy
• Short bond high bond energy

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B. Lewis Structures

• Electron Dot Diagrams
• show valence e- as dots
• distribute dots like arrows in an orbital
  diagram
• 4 sides 1 s-orbital, 3 p-orbitals
• EX oxygen

O
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B. Lewis Structures

• Octet Rule
• Most atoms form bonds in order to obtain 8
  valence e-
• Full energy level stability Noble Gases

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B. Lewis Structures

• Nonpolar Covalent - no charges
• Polar Covalent - partial charges

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C. Molecular Nomenclature Review!

• Prefix System (binary compounds)
• 1. Less e-neg atom comes first.
• 2. Add prefixes to indicate of atoms. Omit
  mono- prefix on first element.
• 3. Change the ending of the second element to
  -ide.

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C. Molecular Nomenclature

• PREFIX
• mono-
• di-
• tri-
• tetra-
• penta-
• hexa-
• hepta-
• octa-
• nona-
• deca-

• NUMBER
• 1
• 2
• 3
• 4
• 5
• 6
• 7
• 8
• 9
• 10

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C. Molecular Nomenclature

• CCl4
• N2O
• SF6

• carbon tetrachloride

• dinitrogen monoxide

• sulfur hexafluoride

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C. Molecular Nomenclature

• arsenic trichloride
• dinitrogen pentoxide
• tetraphosphorus decoxide

• AsCl3

• N2O5

• P4O10

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C. Molecular Nomenclature

• The Seven Diatomic Elements
• Br2 I2 N2 Cl2 H2 O2 F2

H
N
O
F
Cl
Br
I
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III. Ionic Compounds

• Chemical Bonding

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A. Energy of Bond Formation

• Lattice Energy
• Energy released when one mole of an ionic
  crystalline compound is formed from gaseous ions

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B. Lewis Structures

• Covalent show sharing of e-
• Ionic show transfer of e-

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B. Lewis Structures

• Covalent show sharing of e-
• Ionic show transfer of e-