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NAMING COMPOUNDS

NAMING COMPOUNDS. TYPES OF COMPOUNDS. Molecular compound (covalent bonds) Compound made of two nonmetals NBr 5 Ionic compound Compound made of a metal and a nonmetal NaCl Acid (ionic bonds) Compound that can donate a hydrogen ion HCl. MOLECULAR COMPOUND (TWO NONMETALS).

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NAMING COMPOUNDS

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  1. NAMING COMPOUNDS

  2. TYPES OF COMPOUNDS • Molecular compound (covalent bonds) • Compound made of two nonmetals • NBr5 • Ionic compound • Compound made of a metal and a nonmetal • NaCl • Acid (ionic bonds) • Compound that can donate a hydrogen ion • HCl

  3. MOLECULAR COMPOUND (TWO NONMETALS) • To name a molecular compound, you have two parts: • The first element in the compound and • The second element in the compound • NBr5 • The first element is called by its normal name: N – nitrogen • The second name is called by its name and ends in –ide: Br – bromine  bromide

  4. PREFIXES • In addition to naming the elements, you have to name how many they are. To do this you need prefixes. • The prefix goes in the front of the name of the element

  5. PREFIXES (CONT) • One – mono • Two – di • Three – tri • Four – tetra • Five - penta • Six – hexa • Seven – hepta • Eight – octa • Nine – nona • Ten - deca

  6. MOLECULAR COMPOUND (CONT) • Therefore if you start with NBr5: • Mononitrogen pentabromide • BUT wait, if you only have one element in the beginning part of the compound, you don’t have to put the prefix: • Nitrogen pentabromide

  7. TRY THESE • SCl6 • N2O4 • P3F5 • CCl4 • XeO • Trinitrogenhexaoxide • Boron pentabromide • Tetrasulfurdecafluoride • Phosphorus octaiodide

  8. ANSWERS • Sulfur hexachloride • Dinitrogentetraoxide • Triphosphoruspentafluoride • Carbon tetrachloride • Xenon monoxide • N3O6 • BBr5 • S4F10 • PI8

  9. SPECIAL CASE • When naming some compounds, it is implied that the compound is a DIATOMIC GAS • There are only 7 diatomic molecules • Hydrogen • Nitrogen • Oxygen • Fluorine • Chlorine • Iodine • Bromine

  10. DIATOMIC MOLECULES • If you ever see any of those molecules, you write them as a compound with two of the atoms • Hydrogen – H2 • Nitrogen – N2 • Oxygen – O2 • Fluorine – F2 • Chlorine – Cl2 • Iodine – I2 • Bromine – Br2

  11. IONIC COMPOUNDS (METAL AND NONMETAL) • The two parts of naming an ionic compound: • The first element is always the metal • The second element is the nonmetal • CaBr2 • The first element is called by its normal name: Ca  Calcium • The second element is named like a molecular compound: Br  bromide • The only difference is that you do not use a prefix ever

  12. IONIC COMPOUNDS • Therefore if you start with CaBr2: • Calcium Bromide • There is no prefix for bromide even though there is a 2

  13. IONIC COMPOUNDS • Before we begin practice naming ionic compounds, look at your ion sheet • Remember: To put ionic compounds together, you need to BALANCE THE CHARGE

  14. EXAMPLE • How would you show the following ionic compound: Strontium iodide • Strontium  Sr (has a +2 charge: alkali earth metal) • Iodide (has a -1 charge: halogen) • Just like before, cancel swap the charges • Sr+2 + 2I - SrI2 • Your ion sheet gives you the names of several ions with the many possible charges of the transition metals

  15. TRY THESE • BaCl2 • K2O • AlF3 • CaO • Magnesium oxide • Potassium sulfide • Sodium chloride • Beryllium iodide

  16. ANSWERS • Barium chloride • Potassium oxide • Aluminum fluoride • Calcium oxide • MgO • K2S • NaCl • BeI2

  17. POLYATOMIC IONS • An ion that is composed of several atoms • FORMAL DEFINITION • Polyatomic ion: an electrically charged group of two or more chemically bonded atoms that function as a SINGLE ION

  18. POLYATOMIC IONS • Since the polyatomic ions are made of more than 1 atom, their names are complicated • Example of some polyatomic ions: • OH - hydroxide • ClO4-  perchlorate • CO3-2  carbonate • NH4+  ammonium

  19. POLYATOMIC IONS • IMPORTANT NOTE: When combining polyatomic ions, you still balance out the NET CHARGE: • Example: If you have sodium hydroxide • Sodium: Na+ • Hydroxide: OH – • Na+ + OH - NaOH

  20. POLYATOMIC ION • What do you do if you have more than 1 polyatomic ion to balance out a charge? • Example: If you have Magnesium acetate • Magnesium: Mg+2 • Acetate: C2H3O2 – • Mg+2 + 2C2H3O2- Mg(C2H3O2)2 • You put the entire polyatomic ion in brackets with the number of ions as a subscript

  21. TRY THESE • Lithium oxalate • Barium bromate • Sodium Phosphate • Aluminum sulfate • K3BO3 • Sr(NO2)2 • Mg3(PO4)2 • CaSO4

  22. ANSWERS • Li2C2O4 • Ba(BrO3)2 • Na3PO4 • Al2(SO4)3 • Potassium borate • Strontium nitrite • Magnesium phosphate • Calcium sulfate

  23. IONIC COMPOUNDS (TRANSITION METALS) • What do you do when you do not know the exact charge of the ion? • In other words, some of the transition metals can have more than 1 ion • Fe+2 • Fe+3 • You distinguish with Roman numerals

  24. IONIC COMPOUNDS (TRANSITION METALS) • Solution: The name of the compound tells you the charge. • If you have a compound of iron and oxygen, an example would be: • Iron (III) oxide • This means that iron has a +3 charge • 2Fe+3 + 3O-2 Fe2O3

  25. IONIC COMPOUNDS (TRANSITION METALS) • This means that if you’re given the formula, you have to figure out the charge of the metal ion: • Example: MnO2 • What you know: O has a -2 charge • Therefore the total negative is -4 • This means that you need a +4 to balance • You get Manganese (IV) oxide

  26. TRY THESE • Nickel (III) iodate • Lead (II) chloride • Gold (I) Sulfate • Vanadium (III) chlorate • W(PO4)2 • AuBO3 • Tl3PO4 • Sn(NO3)4

  27. ANSWERS • Ni(IO3)3 • PbCl2 • Au2SO4 • V(ClO3)3 • Tungsten (VI) phosphate • Gold (III) borate • Thallium (I) phosphate • Tin (IV) nitrite

  28. ACIDS • What is an acid? • For now: An acid is a compound that will donate a proton (H+) • How do you recognize an acid • Any compound that begins with H+ • There are two basic types of acids for naming • Binary acid • Polyatomic acid

  29. BINARY ACID • A binary acid has a hydrogen ion and a single halide • Examples: HCl, HF, HBr, HI • Naming these acids takes the following format: • Hydro-(root of the name of the halide)-ic acid • Therefore HCl becomes Hydrochloric acid

  30. BINARY ACID • What would be the names of the following: • HF • HBr • HI

  31. ANSWERS • Hydrofluoric acid • Hydrobromic acid • Hydroiodic acid

  32. POLYATOMIC ACIDS • Similar convention to binary acids • (Base name of the polyatomic ion)-ic acid • HC2H3O3 • This is an H+ with a C2H3O3- • The name of the polyatomic ion is acetate • The name is Acetic acid

  33. POLYATOMIC ACIDS • The differences • What if you have H2SO4 and H2SO3 • What’s the difference in these two names?: • only one can be sulfuric acid

  34. POLYATOMIC ACIDS • If the ion ends in the name “-ate” • Sulfate, nitrate, chlorate • The name of the acid is (root of ion)-ic acid • Sufuric acid, nitric acid, chloric acid • If the ion ends in the name “-ite” • Sulfite, nitrite, chlorite • The name of the acid is (root of ion)-ous acid • Sulfurous acid, nitrous acid, chlorous acid

  35. TRY THESE • H2CO3 • HNO2 • HIO3 • H3PO4 • Oxalic acid • Sulfurous acid • Sulfuric acid • Bromic acid

  36. ANSWERS • Carbonic acid • Nitrous acid • Iodic acid • Phosphoric acid • H2C2O4 • H2SO3 • H2SO4 • HBrO3

  37. SUMMARY • Before you start naming, determine the type of compound • Molecular, ionic or acid • Naming molecular compounds (nonmetal and nonmetal) • Name of the first element • Base name of the second element + ide • Make sure you use the prefix indicating number of atoms

  38. SUMMARY (CONT) • Naming ionic compounds (metal and nonmetal) • Name of the first element • Name of the second element + ide or • Name of the second polyatomic ion • Make sure you balance the charges of each ion • If the metal has more than 1 possible charge, indicate the charge with a Roman numeral

  39. SUMMARY (CONT) • Acids (the compound has a hydrogen ion H+) • Binary acids • Hydro (base name of the halogen)-ic acid • Polyatomic acids • (Base name of the polyatomic ion w/ “-ate”) – ic acid • (Base name of the polyatomic ion w/ “-ite”) – ous acid

  40. WRITE THE SYMBOL OR NAME • Calcium chloride • Lead (IV) sulfate • Carbon tetrachloride • Hydroiodic acid • Sulfuric acid • Dinitrogen hexachloride • HBr • NH4NO3 • S3Br8 • NO • HNO2 • Mn(C2H3O2)3 • Pb(SO3)2

  41. ANWERS • CaCl2 • Pb(SO4)2 • CCl4 • HI • H2SO4 • N2Cl6 • Hydrobromic acid • Ammonium nitrate • Trisulfur octabromide • Nitrogen monoxide • Nitrous acid • Manganese (III) acetate • Lead (IV) sulfite

  42. PUTTING THIS IN A CHEMICAL REACTION • General Format: • Reactants  Products • Steps • Translate the chemical into its symbol and then put the state of matter AFTER the chemical symbol • Put a “+” between each set of reactants and products

  43. STATES OF MATTER • Symbols for states of matter: • Solid (s) • Liquid (l) • Gas (g) • Aqueous (aq)

  44. EXAMPLE • Solid sodium is mixed with chlorine gas to form aqueous sodium chloride • Solid sodium = ? • is mixed with = ? • chlorine gas = ? • to form = ? • aqueous sodium chloride = ?

  45. FINAL ANSWER • Na(s) + Cl2(g) NaCl(aq)

  46. TRY THESE • Solid iron is combined with oxygen gas to produce solid iron(III) oxide. • Aqueous magnesium nitrate is combined with solid zinc to form aqueous zinc nitrate and solid magnesium.

  47. ANSWERS • Fe(s) +O2(g) Fe2O3(s) • Mg(NO3)2(aq) + Zn(s)  Zn(NO3)2(aq) + Mg(s)

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