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Understanding Chemical Bonds: Solubility and Valence Concepts

Discover the fascinating world of solubility with "likes dissolve likes" principle. Dive into valence, covalence, and electrovalence, exploring how elements form bonds by gaining, losing, or sharing electrons. Learn about the Octet Rule, where atoms aim to fill their outer shell with 8 electrons for stability.

sigourney-buckley
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Understanding Chemical Bonds: Solubility and Valence Concepts

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  1. Chapter 3: Solubility, valence, covalence, electrovalence, the octet rule

  2. SOLUBILITY • “Likes dissolve likes” • Non-polar solvents (eg. TTE) dissolve non-polar solutes (eg. Iodine) • Polar solvents (eg. Water) dissolve polar and ionic solutes (eg. Anything with full or partial charges such as salts, alcohol, etc) • Opposite charges still attract. Something with charges dissolves something else with charges and non-polar dissolves non-polar

  3. Valence, Covalence, Electrovalence • Valence shell: outer shell • Valence: How many bonds it forms (by losing, gaining, or sharing electrons). • Covalence: (Non-metals) How many electrons the element must share to fill its outer shell (how many shared pairs) • Electrovalence: (Metal and non-metal) The charge on the ions in the compound Eg. The charge in an ionic compound from losing or gaining electrons to empty or fill its outer shell

  4. Recall: Metals LOSE electrons. Non-metals gain (ionic) or share (covalent) electrons

  5. IONIC AND COVALENT BONDING: THE OCTET RULE • Group VIIIA (18) is chemically stable (“inert”: little or no ability to react). The rest of the elements in the periodic table seem to copy this stability by losing (metals) or gaining/sharing (non-metals) electrons until their outer shell is full. This usually means 8 electrons in the outer shell 8 8 8 8

  6. ISOELECTRONIC: See Overhead

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