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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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V.Chemical Bonding A.Octet Rule –1.Definition –2.Noble Gases
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V.Chemical Bonding B.Ionic Bonding –1.Example 11 Na 17 Cl
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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 20 Ca and 17 Cl combine by ionic bonding? 1.Ca 2 Cl 2.CaCl 3.CaCl 2 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
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