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Nomenclature

Nomenclature. Chapter 7 Sec 3. Nomenclature. Study of naming compounds or writing chemical formulas Use different set of rules based on the types of compounds a) Binary Ionic Compounds – “A” metals b) Binary Ionic Compounds – “B” metals c) Polyatomic compounds

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Nomenclature

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  1. Nomenclature Chapter 7 Sec 3

  2. Nomenclature • Study of naming compounds or writing chemical formulas • Use different set of rules based on the types of compounds a) Binary Ionic Compounds – “A” metals b) Binary Ionic Compounds – “B” metals c) Polyatomic compounds d) Binary Covalent Compounds

  3. Nomenclature Flow Chart

  4. Name Binary Ionic Compounds (“A” metals) *Made of one metal element and one nonmetal element • Name the metal. Ignore the subscript! • Name the nonmetal with the modified “-ide” ending. Ignore the subscript! * hydrogen  hydride * nitrogen  nitride * oxygen  oxide * silicon  silicide * phosphorus  phosphide * bromine  bromide * fluorine  fluoride *iodine  iodide

  5. Examples • Na2O – sodium oxide • Ca3N2 – calcium nitride • AlF3 – aluminum fluoride

  6. Name Binary Ionic Compounds (“B” metals) *Made of a transition metal element and a nonmetal element • Name the transition metal. • Write the charge of one transition metal atom with a Roman numeral in a parenthesis. * I = 1; II = 2; III = 3; IV=4; V=5; VI=6; VII=7; VIII=8; IX=9; X=10 * The charge of one transition metal atom must be determined from the anions. 3. Name the nonmetal with the “-ide” ending.

  7. Examples • CrO – chromium (II) oxide • Cr2O – chromium (I) oxide • FeCl3 – iron (III) chloride • Ni2S3 – nickel (III) sulfide **Ag+ and Zn2+ are transition metals but their charge numbers don’t change, so don’t write the Roman numerals. **Sn and Pb are not transition metals, they act like they are. Write the Roman numerals.

  8. Polyatomic compounds • Composed of at least three different elements. • Composed of either polyatomic cation or anion – Refer to the handout. • Name the metal. Use a Roman if the metal is a “B” metal. Name NH4 as “ammonium”. 2) Name the polyatomic anion. Use the handout. If the anion is not a polyatomic ion, end with the “-ide” ending. *Do not read the subscripts *If more than one unit of polyatomic ion are needed, put a parenthesis around the polyatomic ion and write the subscript outside the parenthesis

  9. Examples • (NH4)2S – ammonium sulfide • Na2SO4 – sodium sulfate • Pb(C2H3O2)2 – lead (II) acetate • AgOH – silver hydroxide • Ni(CO3)2 – nickel (IV) carbonate

  10. Writing Formulas for Ionic Compounds 1) Use the jigsaw puzzle pieces until all teeth are matched up. The numbers of cation pieces or anion pieces used are the subscripts 2) Determine the subscripts from the LCM (least common multiple). (Ex) calcium phosphate (made of Ca2+ & PO43-)  LCM of 2 and 3 = 6 For Ca2+, 6 ÷ 2 = 3, the subscript for Ca For PO43-, 6 ÷ 3 = 2, the subscript for PO4 Putting it together, Ca3(PO4)2

  11. Binary Covalent Compounds • Made up of two different nonmetal elements • Names include Greek prefixes for subscripts * 1 – mono 2 – di 3 – tri 4 – tetra 5 – penta 6 – hexa 7 – hepta 8 – octa 9 – nona 10 – deca

  12. Naming Binary Covalent Compounds • Use the Greek prefix for the subscript of the first nonmetal element. Exception: Don’t use “mono” on the first element. • Name the first nonmetal element. • Use the Greek prefix for the subscript of the second nonmetal element. • Name the second nonmetal element with the “-ide” ending

  13. Examples • PCl3 – phosphorus trichloride • N2O5 – dinitrogen pentoxide • CO – carbon monoxide • P4O10 – tetraphosphorus decoxide

  14. Writing Formulas for Covalent Compounds 1) Write the element symbol. 2) The Greek prefix is the subscript, which is written after the element. (Ex) disiliconpentahydride – Si2H5

  15. Practices Write the formulas. • Antimony tribromide • Hexaboronmonosilicide • Chlorine dioxide • Hydrogen monoiodide • Nitrogen trihydride • Phosphorus pentachloride Write the names. 7. P4S5 8. H2O 9. SeF6 10. B2Si 11. CH4 12. NO

  16. Nomenclature Flow Chart

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