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P. Sci.

P. Sci. Unit 9 Chemical Compounds Chapter 6. Part 2. Compound Names and Formulas. Binary Compounds. Al(ClO 3 ) 3. P 2 O 5. NaCl. Most of the compounds that you will have to name will have only 2 elements (called binary – bi meaning 2) or an element and a polyatomic ion. NaCl.

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P. Sci.

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  1. P. Sci. Unit 9 Chemical Compounds Chapter 6

  2. Part 2 Compound Names and Formulas

  3. Binary Compounds Al(ClO3)3 P2O5 NaCl • Most of the compounds that you will have to name will have only 2 elements (called binary – bi meaning 2) or an element and a polyatomic ion. NaCl CaCl2 P2O5 NaNO3 Al(ClO3)3 CaCl2 NaNO3

  4. Naming Compounds • First you have to identify what type of compound it is : • Ionic – metal and non-metal. • Covalent – two non-metals • Polyatomic - both NaCl N2O4 CaCO3

  5. Ionic Compounds • Write the name of the metal (cations = + ion) Examples: Na = Sodium Ca = Calcium Al = Aluminum

  6. Ionic compounds cont. Write the name of the non-metal (anion = - ion) but change the ending to “ide”. Examples: Chlorine – Chloride Fluorine – Fluoride Oxygen – Oxide Sulfur – Sulfide Phosphorus – Phosphide Iodine - Iodide

  7. Examples • NaCl = Sodium chloride • CaI2 = Calcium iodide • CsBr = Cesium bromide • Al2O3 = Aluminum Oxide For ionic compounds – pay no attention to the subscripts.

  8. Now you try • Name the following ionic compounds. • LiF = • MgO = • SrCl = • K2S = • Ca3N2 =

  9. Answers • LiF = Lithium fluoride • MgO = Magnesium oxide • SrCl = Strontium chloride • K2S = Potassium sulfide • Ca3N2 = Calcium Nitride

  10. Covalent Compounds • First Name • If there is only one atom of this element, just write the name of the element. Example: N = Nitrogen C = Carbon P = Phosphorus

  11. Covalent compounds cont. • First Name cont. • If there is more than one atom of the element, write the name of the element with the pre-fix that tells how many atoms are there.

  12. Pre-fixes 1 – mono 6 – hexa 2 – di 7 – hepta 3 – tri 8 – octa 4 – tetra 9 – nona 5 – penta 10 – deca

  13. Examples: H2 – di-hydrogen C3 – tri-carbon Br4 – tetra-bromine

  14. Covalent compounds cont. • Second Name – Always has a prefix. • Always starts with a prefix that tells how many atoms are there. (even if there is only one)

  15. Covalent compounds cont. • Second Name cont. • ends in “ide” Examples : CO – carbon monoxide CO2 – carbon dioxide CO3 – carbon trioxide

  16. Now you try • Name the following covalent compounds. • NO2 = • PBr3 = • AsCl = • H2O = • H2O2 =

  17. Answers • NO2 = Nitrogen dioxide • PBr3 = Phosphorus tribromide • AsCl = Arsenic monochloride • H2O = Di-hydrogen monoxide • H2O2 = Di-hydrogen dioxide

  18. Polyatomic Ions • Compounds with both ionic and covalent bonds. • Acts the same as any other ion.

  19. Polyatomic ions cont. • Examples: • Ammonium NH4+ • Hydroxide OH- • Sulfate SO4+2 • Carbonate CO3-2

  20. Polyatomic compounds • Follow step one for ionic compounds. (Write the name of the metal) • Write the name of the polyatomic ion (do not change to “ide”) Examples: NaNO3 = Sodium nitrate Al(ClO3)3 = Aluminum chlorate

  21. The End

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