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Naming Rules for Ionic and Covalent Compounds

Understand the rules for naming ionic compounds involving metals and non-metals, the role of cations and anions, formulas based on electron ratios, use of Roman numerals, and handling polyatomic ions. Also learn about naming covalent compounds with non-metals, including the use of prefixes.

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Naming Rules for Ionic and Covalent Compounds

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  1. Naming Rules Review

  2. Ionic Compounds • A combination between: • A metal and a non-metal • Metals are on the left side of the “staircase” starting at Boron • Electrons are donated and accepted

  3. Ionic Compounds • Which ion goes first? • Cation comes first • Metal • Electron donor • Positive ion forms • Anion • Non-metal • Electron acceptor • Negative ion forms • E.g. Ca +2 (cation) and Br-1 (anion) makes CaBr2

  4. Ionic Compounds • How to figure out their formulas or What ratios elements will combine in? • Valence shell electrons • Stable octet desires • Lose or gain electrons • Overall neutral charge required • Ca +2 (loses 2 electrons) and Br-1 (gains 1 electron EACH) makes CaBr2 • Ionic charge reflects electron:proton ratio

  5. Ionic Compounds • How to write their names: • Use Periodic Table to find out names from symbols • Drop the usual ending from the anion and add “-ide” • E.g. NaBr is sodium bromide (not bromine)

  6. Ionic Compounds • When to use Roman numerals: • For cations (metals) that have multiple combining capacities • E.g. Iron can donate two or three electrons, so we name them: • Iron (II) • Iron (III)

  7. Ionic Compounds • Where do Roman numerals go in the name? • AFTER the cation (metal) • E.g. Iron (II) phosphide

  8. Ionic Compounds • What is a polyatomic ion? • A group of atoms that behave as an anion or cation unit • E.g. OH-

  9. Ionic Compounds • How do polyatomic ions change naming rules? • The ending may not be “-ide”, but will be the name of the ACTUAL polyatomic ion • E.g. beryllium nitrite is Be(NO2)2

  10. Ionic Compounds • The only polyatomic ion to end in “ide”: • Hydroxide, OH- • E.g. beryllium hydroxide is Be(OH)2

  11. Covalent Compounds • A combination between: • A non-metal and a non-metal • Electron sharing

  12. Covalent Compounds • How are the naming rules different than ionic compounds? • Names use prefixes to indicate the formula subscripts • Mono- (1) • Di- (2) • Tri- (3) • Tetra- (4) • Penta- (5) • Hexa -(6) • Etc.

  13. Covalent Compounds • E.g. Carbon tetraflourideis CF4 • The prefix “mono-” not always used (see above example), but can be useful for differentiating between two compounds. • E.g. Carbon monoxide and carbon dioxide

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