An Introduction to Chemistry

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An Introduction to Chemistry

• Important biological elements
• Carbon
• Oxygen
• Nitrogen
• Hydrogen
• Sulfur
• Na
• K

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II. Atomic Structure

• A. Definition
• B. Analogy of structure
• C. Subatomic particles
• 1. Protons
• 2. Neutrons
• 3. Electrons

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III. Electron orbitals

• A. Location
• B. Maximum number of electrons in an orbital
• C. Orbital filling
• D. Examples
• 1. H
• 2. C
• 3. Na
• 4. Si

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III. Electron orbitals

• E. Valence electrons
• 1. Definition
• 2. Involved in chemical bond formation
• 3. Determines chemical properties of the atom
• 4. Elements with the same number of valence
  electrons have similar chemical properties

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III. Electron orbitals

• E. Valence electrons
• 5. gaining and losing energy

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IV. Periodic table
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An atom with an atomic number of 13 and a mass of
22 possesses ____ electrons.

1. 13
2. 22
3. 9
4. 3
5. The answer cannot be determined

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An atom with an atomic number of 13 and a mass of
22 possesses ____ valence electrons.

1. 2
2. 3
3. 8
4. 13

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Chemical Bonding

• A. Octet Rule
• 1. Definition
• 2. Noble Gases

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V. Chemical Bonding

• B. Ionic Bonding
• 1. Example
• 11Na
• 17Cl

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V. Chemical Bonding

• B. Ionic Bonding
• 2. Definition

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Ionic bonding
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What is the equation of the compound formed when
20Ca and 17Cl combine by ionic bonding?

1. Ca2Cl
2. CaCl
3. CaCl2
4. The answer cannot be determined

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V. Chemical Bonding

• C. Covalent bonding
• 1. Definition
• 2. Example of nonpolar covalent
• 3. Example of polar covalent bonding

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Nonpolar Covalent
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Polar Covalent Bond