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Nomenclature

Nomenclature. Chapter 9. Do Now #1. Which statement is true ? Elements in the same group has the same # of val. e- Elements in the same period has the same # of val. e-. Do Now #2. Write the formula for each of the following compounds. Ammonium sulfate Vanadium (V) fluoride

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Nomenclature

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  1. Nomenclature Chapter 9

  2. Do Now #1 Which statement is true? • Elements in the same group has the same # of val. e- • Elements in the same period has the same # of val. e-

  3. Do Now #2 Write the formula for each of the following compounds. • Ammonium sulfate • Vanadium (V) fluoride • Copper (III) nitrate • Aluminum oxide Answers: • (NH4)2SO4 • VF5 • Cu(NO3)3 • Al2O3

  4. Do Now #3 What is the difference between CuSO4 and CuNO3? Answer: Contain different polyatomic anion CuSO4: copper 2+ CuNO3: copper 1+

  5. Do Now #4 Name the following compounds: • CO • SiO2 • P4O6 Write the formula for the below compounds: • Arsenic tribromide Answer: • Carbon monoxide • Silicon dioxide • Tetraphosphorushexoxide Answer: AsBr3

  6. Types of Chemical Bonds Ionic Compounds: Formed by the opposite attraction between cations & anions. (btwnmetals & non-metals) Salt - scientific name given to many different ionic compounds Transfer of electrons creates ions

  7. Formation of Sodium Chloride

  8. 0 +1 +2 +3 +/-4 -3 -1 -2 Hydrogen can be 1+ or 1-, most common is 1+

  9. Na 1+ CATIONS (alkalai = +1, alkaline earth = +2, aluminum = +3, zinc = +2, silver = +1) sodium ion _______ beryllium ion _______ aluminum ion _____ strontium ion ______ cesium ion _________ silver ion _____ Be 2+ Al 3+ Sr2+ Cs+ Ag+

  10. Cu+ TRANSITION/POST TRANSITION METALS (variable) copper (I) ion _____ copper (II) ion _____ cobalt (II) ion ______ manganese (VII) ion ______ iron (II) ion ______ iron (III) ion _____ Cu2+ Co2+ Mn7+ Fe2+ Fe3+

  11. N3- ANIONS (monoatomic anions all end in –ide) nitride ______ fluoride _______ oxide ______ chloride _____ iodide _______ phosphide ______ F1- O2- Cl1- I1- P3-

  12. BINARY IONIC COMPOUNDS (Salts) Naming rule: Metal name______________ ide (root of non-metal) Ex: AlCl3 = Aluminum Chloride a. Li2O b. MgF2 c. Ca3P2 d. SrI2 Lithium Oxide Magnesium Fluoride Calcium Phosphide Strontium Iodide

  13. Formula writing Al +3 Cl-1 Al1Cl3 = AlCl3 Sodium chloride Calcium chloride Ionic Compound subscripts must be reduced Ti+4O-2Sn+2O-2 Ti2O4 reduces to TiO2Sn2O2 reduces to SnO NaCl CaCl2

  14. Write the FORMULA for: a. lithium fluoride b. calcium bromide LiF CaBr2 c. magnesium phosphide d. barium oxide Mg3P2 BaO e. iron(III) chloride f. lead (II) nitride FeCl3 Pb3N2 g. potassium nitride h. tin(IV) oxide K3N SnO2

  15. Polyatomic ion • Ions made up of 2 or more atoms • Charge is spread across the group of bonded atoms You do not need to memorize them. They will be given to you during the test

  16. Write the FORMULA for: a. lithium sulfate b. calcium hydroxide Li2SO4 Ca(OH)2  c. copper(II) cyanide d. strontium nitrate Cu(CN)2Sr(NO3)2  e. chromium(III) phosphate f. manganese (IV) carbonate CrPO4Mn(CO3)2 g. barium chlorate h. aluminum permanganate Ba(ClO3)2 Al(MnO4)3

  17. NAME the following compounds: a. NH4Cl b. Ca(CN)2 Ammonium Chloride Calcium Cyanide c. Na3PO4 d. Al(OH)3 Sodium Phosphate Aluminum Hydroxide  e. ZnSO4 f. Cs2CO3 Zinc Sulfate Cesium Carbonate g. KClO3 h. Mg3(PO4)2 Potassium Chlorate Magnesium Phosphate

  18. TRANSITION/POST TRANSITION METALS (charge varies) WHAT ABOUT THE METALS THAT HAVE MORE THAN ONE OXIDATION # (CHARGE)? a. Write in the charges for the ions you are sure of (anion) b. Work backwards to find the charge of the metal ion (cation) Which metals DO NOT need Roman Numerals? Column I (alkali) Column II (alkaline earth) Silver (always +1): Ag+ Zinc (always +2): Zn2+ Aluminum (always +3): Al3+

  19. NAME the following compounds(Roman numerals shows the charge of the metal) a. CuS b. FeP  copper (II) sulfide iron (III) phosphide c. FeSO4 d. CuNO3 iron (II) sulfate copper (I) nitrate e. NiI3 f. Cr(MnO4)4 nickel (III) iodide chromium (IV) permanganate g. Pb(NO3)2 h. Pb(SO4)2 lead (II) nitrate lead (IV) sulfate i. Sn(CO3)2 j Sn(NO3)2 tin (IV) carbonatetin (II) nitrate k. Cu3(PO4)2 l. Cu3PO4 copper (II) phosphate copper (I) phosphate

  20. Covalent Compounds • Formed when atoms share one or more pairs of electrons • Bonds between nonmetals

  21. Examples: SO2→ Sulfur dioxide • SO3→ Sulfur trioxide • NO → Nitrogen monoxide NOT Mononitrogenmonooxide • N2O5→ Dinitrogenpentoxide NOT dinitrogenpentaoxide • Some compounds are always referred to by their common names H2O Water NH3Ammonia CH4Methane

  22. C3Cl6 Si2O7 C5F10 PCl5 tricarbonhexachloride Disiliconheptoxide pentacarbondecafluoride phosphorous pentachloride

  23. Writing the formula of molecular/covalent compounds: N2O5 BF3 CO CCl4 N2O NO2 Cl2O CF4 C4Br8 a) dinitrogenpentaoxide b) Boron triflouride c) Carbon monoxide d) Carbon tetrachloride e) dinitrogen monoxide f) nitrogen dioxide g) dichlorine monoxide h) carbon tetrafluoride i) tetracarbonoctabromide

  24. Naming Acids(hint: acids start with “H”) BINARY:Contains exactly two elements. (without oxygen) • prefixhydro-to name the hydrogen part of the acid • add the suffix–ic EXAMPLES: HClHBr hydrochloric acid hydrobromic acid

  25. Naming Acids CONT… Oxyacids: (contain oxygen) (H & polyatomic ion with O) • use the root of the anion • if it is an –ateanion, use the–icending • if it is an –iteanion, use the –ousending H2SO4 HNO3 sulfuricacid nitric acid H2SO3 HNO2 sulfurousacid nitrous acid

  26. Carbonic acid Carbonate Acetate Acetic acid Sulfite Sulfurous acid Phosphide Hydrophosphoric acid Sulfide Hydrosulfuric acid

  27. H3N N3- HNO2 NO2-1 HMnO4 MnO4-1 SO4-2 H2SO4 HF F1- H3PO4 PO4-3 H3P P3-

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