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Naming

Naming. Binary Covalent & Acids. Molecules. ________– two or more atoms covalently bound together ____________________– two of the same atom bound together. Diatomic Molecules. Br I N Cl H O F or the Magnificent 7 These atoms never exist alone. They always come in pairs For example:

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Naming

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  1. Naming Binary Covalent & Acids

  2. Molecules • ________– two or more atoms covalently bound together • ____________________– two of the same atom bound together

  3. Diatomic Molecules • Br I N Cl H O F or the Magnificent 7 • These atoms never exist alone. • They always come in pairs • For example: • Br  Br2 • I  I2 • N  N2 • Cl  Cl2 • H  H2 • O  O2 • F  F2

  4. Binary Molecular Compounds • Binary Compounds consist of 2 ___________________ • Before you can name binary covalent compounds, you MUST know the prefixes!

  5. Mono Di Tri Tetra Penta Hexa Hepta Octa Nona Deca 1 2 3 4 5 6 7 8 9 10 Prefixes

  6. Rules for naming Binary Covalent Compounds • Name the __________ for the number of atoms of the first element • Then name the first __________ • Name the __________ for the number of atoms of the second element • Than name the __________ of the second element with the ending - __________

  7. Note… • No charges are used in Binary Covalent Compounds • If the 1st prefix is mono…. __________ ! • When the prefix ends in an o or a, and the name of the element begins with a vowel, the o or a is often dropped

  8. Examples • What is the name of N2O4?

  9. More examples • Name SO2

  10. More examples • Write the formula for dichlorine monoxide

  11. More examples • Write the formula for disulfur dichloride

  12. Acids • Acids can be recognized because the start with __________ • Examples • HCl • H2SO4 • HI

  13. Acids • Acids are in __________ solution (aq) • For the purposes of this class, we will assume that if it begins with H, we will name it according to the rules of naming acids • If the HX were to be in a gas form, it would be named hydrogen x-ide

  14. Rule #1 - naming acids • If the anion ends in –ide, the acid will be named… • Hydro (root) – ic acid • This is usually for H plus one element

  15. For example • HCl • HI • H2S

  16. Rule #2 – naming acids • If you have an H plus an anion ending in –ate, the acid will be named… • (root) – ic acid

  17. Examples • H2SO4 • HNO3 • H3PO4

  18. Rule # 3 – naming acids • If you have an H plus an anion ending in –ite, the acid will be named… • (root) – ous acid

  19. Examples • H2SO3 • HNO2 • H3PO3

  20. Remember… ate  ic ite - ous

  21. Writing formulas for acids • When writing formulas for acids you MUST look at the charges and bring them down!

  22. Examples • HBr • HClO3

  23. H2SO3 H2CO3 HF Nitrous acid Perchloric acid Iodic acid Phosphorous acid More examples

  24. KClO2 CO2 H2SO4 NH4Br CuCO3 Fe2O3 HClO Mixed examples(remember to figure out what type of compound it is 1st!)

  25. Carbon tetrachloride Phosphorous pentachloride Aluminum oxide Copper (II) nitrate Chlorous acid Hydrophosphoric acid Iron (III) hydroxide More Mixed Examples

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