Bonding 2008
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The document discusses different types of bonds - metallic, ionic, and covalent - and provides details about each. Metallic bonds form between metal atoms and allow for electron transfer and conductivity. Ionic bonds form between ionic compounds through electrostatic attraction between oppositely charged ions. Covalent bonds form between nonmetal elements through the sharing of electron pairs to achieve stable noble gas configurations. The document also covers Lewis structures, exceptions to the octet rule, and periodic trends in ionization energy, electronegativity, atomic size, and ionic size.
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The document introduces the periodic table and discusses how it is organized. It explains that elements are arranged by atomic number vertically into groups and horizontally into periods. [The document] instructs the reader to draw electron configuration diagrams for the first 20 elements and observe that elements in the same group have the same number of valence electrons. It also notes that elements in the same period have the same number of electron shells. In conclusion, [the document] emphasizes that the number and arrangement of valence electrons determines how an element bonds and reacts chemically.
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Unit 7.1 Intro to Bonding
The document discusses chemical bonding, which occurs when atoms bond together to form more stable arrangements with lower energy than as isolated atoms. Atoms bond by gaining, losing, or sharing valence electrons to achieve stable electron configurations like noble gases, following the octet rule where atoms gain or share electrons to have 8 in their outer shell. The main types of bonds are ionic involving electron transfer, covalent involving electron sharing between nonmetals, and metallic involving delocalized electrons in metals.
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Bonding 2008
- 8. II. Ionic compounds 4. Salts such as NaCl form crystals a. Crystals = solids w/ repeating patterns (“crystal lattice”)held together by electrostatic attractions
- 15. II. Steps for Drawing Lewis Structures D. Some General Guidelines 1. Often the central atom is the first one in the formula 2. Carbon likes to be in the middle with four bonds around it 3. Halogens like to be on ends with only one bond 4. Hydrogen MUST be on an end 5. Oxygen likes two bonds
- 24. Ionization Energy & the Periodic Table Elements with the highest ionization energies occur in the upper right corner (most chemically active nonmetals) Elements with the lowest ionization energies are in the lower left corner of the table (most chemically active metals)
- 27. III. Atomic Size & the P.T. Size is decreasing Size is decreasing