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An Introduction to Chemistry • Important biological elements – Carbon – Oxygen – Nitrogen – Hydrogen – Sulfur – Na –K II. Atomic Structure • A. Definition • B. Analogy of structure • C. Subatomic particles – 1. – 2. – 3. Protons Neutrons Electrons III. Electron orbitals • A. Location • B. Maximum number of electrons in an orbital • C. Orbital filling • D. Examples – – – – 1. 2. 3. 4. H C Na Si III. Electron orbitals • E. Valence electrons – 1. – 2. – 3. – 4. Definition Involved in chemical bond formation Determines chemical properties of the atom Elements with the same number of valence electrons have similar chemical properties III. Electron orbitals • E. Valence electrons – 5. gaining and losing energy IV. Periodic table An atom with an atomic number of 13 and a mass of 22 possesses ____ electrons. 79% 21% Th e an sw er ca nn o tb ... 3 0% 0% 9 0% 22 13 22 9 3 The answer cannot be determined 13 1. 2. 3. 4. 5. An atom with an atomic number of 13 and a mass of 22 possesses ____ valence electrons. 68% 2 3 8 13 16% 11% 13 8 3 5% 2 1. 2. 3. 4. V. Chemical Bonding • A. Octet Rule – 1. – 2. Definition Noble Gases V. Chemical Bonding • B. Ionic Bonding – 1. Example • 11Na • 17Cl V. Chemical Bonding • B. Ionic Bonding – 2. Definition Ionic bonding What is the equation of the compound formed when 20Ca and 17Cl combine by ionic bonding? Ca2Cl CaCl CaCl2 The answer cannot be determined 63% 19% 19% Th e an sw er ca nn o C tb ... aC l2 aC l C a2 Cl 0% C 1. 2. 3. 4. V. Chemical Bonding • C. Covalent bonding – 1. – 2. – 3. Definition Example of nonpolar covalent Example of polar covalent bonding Nonpolar Covalent Polar Covalent Bond