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Nomenclature

Nomenclature. Chemistry Chapter 7. PO 4 3- phosphate ion. HC 2 H 3 O 2 Acetic Acid. C 2 H 3 O 2 - acetate ion. Forms of Chemical Bonds. There are 3 forms bonding atoms: Ionic —complete transfer of 1 or more electrons from one atom to another (one loses, the other gains)

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Nomenclature

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  1. Nomenclature Chemistry Chapter 7 PO43- phosphate ion HC2H3O2 Acetic Acid C2H3O2- acetate ion

  2. Forms of Chemical Bonds • There are 3 forms bonding atoms: • Ionic—complete transfer of 1 or more electrons from one atom to another (one loses, the other gains) • Covalent—some valence electrons shared between atoms • Metallic– holds atoms of a metal together Most bonds are somewhere in between ionic and covalent.

  3. COMPOUNDS FORMED FROM IONS CATION + ANION ---> COMPOUND Na+ + Cl- --> NaCl A neutral compound requires equal number of + and - charges.

  4. Predicting Charges on Monatomic Ions OR USE ION CHART +1 +2 -3 -2 -1 0 Cd+2

  5. Properties of Ionic CompoundsForming NaCl from Na and Cl2 • A metal atom can transfer an electron to a nonmetal. • The resulting cation and anion are attracted to each other by electrostatic forces.

  6. Naming Compounds Binary Ionic Compounds: • 1. Cation first, then anion • 2. Monatomic cation = name of the element • Ca2+ = calciumion • 3. Monatomic anion = root + -ide • Cl- = chloride • 4. MAKE A NEUTRAL COMPOUND with subscripts • CaCl2 = calcium chloride

  7. Naming Ionic Compounds1. Check if ionic: Starts with metal or NH42. Determine the names of the ions from the ion chart3. List the cation, first then the anion • NaF - • LiCl - • MgO -

  8. 0 Naming Ionic Compounds • NaF - sodium fluoride • LiCl - lithium chloride • MgO - magnesium oxide

  9. Naming Binary Ionic Compounds • Examples: NaCl ZnI2 Al2O3 sodium chloride zinc iodide aluminum oxide

  10. Monatomic Ions

  11. Learning Check Complete the names of the following binary compounds: Na3P sodium ________________ KBr potassium ________________ Al2O3 aluminum ________________ MgS _________________________

  12. Writing a Formula Write the formula for the ionic compound for barium chloride It forms between Ba2+ and Cl.

  13. Writing a Formula Write the formula for Ba2+and Cl. Solution: 1. Balance charge with + and – ions 2. Write the positive ion of metal first, and the negative ion Ba2+ClCl 3. Write the number of ions needed as subscriptsBaCl2

  14. Some Ionic Compounds Li+ + N-3 Ca2++ I- ----> Li3N lithium nitride ----> CaI2 calcium iodide

  15. 0 Ionic Compounds Formulas • How do we know how many atoms of each ion we need? • A simple crossing of the charges can answer that question about 90% of the time. • Example: Mg2+ and N3- Mg3N2 Check the charges… 3 x (+2) = +6 2 x (-3) = -6 • When they combined they cancel to yield a neutral compound.

  16. Learning Check Write the correct formula for the compounds containing the following ions: 1. Na+ , S2- a) NaS b) Na2S c) NaS2 2. Al3+, Cl- a) AlCl3 b) AlCl c) Al3Cl 3. Mg2+, N3- a) MgN b) Mg2N3 c) Mg3N2

  17. Solution 1. Na+, S2- b) Na2S 2. Al3+, Cl- a) AlCl3 3. Mg2+, N3- c) Mg3N2

  18. Learning Check Write the correct formula for the compounds : 1. calcium oxide a) CaO b) Ca2O c) CaO2 2. lithium nitride a) LiN3 b) LiN c) Li3N 3. magnesium phosphide a) MgP b) Mg2P3 c) Mg3P2

  19. Learning Check Write the correct formula for the compounds : 1. calcium oxide a) CaO 2. lithium nitride c) Li3N 3. magnesium phosphide c) Mg3P2

  20. Transition Metals POLYVALENT: Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. Look at your ion chart…..do you see some?

  21. Transition Metals Elements that can have more than one possible charge MUST have a Roman Numeral to indicate the charge on the individual ion. 1+ or 2+ 2+ or 3+ Cu+,Cu2+ Fe2+, Fe3+ copper(I) ion iron(II) ion copper (II) ion iron(III) ion

  22. Transition Metals The ROMAN NUMERAL is the charge on the metal. If it’s NOT on the ion chart, you can still do the work! tin (IV) = Sn4+ chromium (VI) = Cr6+

  23. Names of Variable Ions These compounds REQUIRE Roman Numerals because they have metals that can have more than one possible charge: FeCl3(Fe3+) iron (III) chloride CuCl (Cu+ ) copper (I) chloride SnF4 (Sn4+) tin (IV) fluoride PbCl2 (Pb2+) lead (II) chloride Fe2S3 (Fe3+) iron (III) sulfide

  24. Names of Variable Ions How can you tell which one it is? FeCl3Is it iron (II) or iron(III) (Fe2+) iron (II) chloride (Fe3+) iron (III) chloride Work backwards from anion. Figure out both choices and match OR Inverse criss-cross (only works sometimes)

  25. Examples of Older Names of Cations formed from Transition Metals(you do not have to memorize these)

  26. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 iron (_____) bromide CuCl copper (_____) chloride SnO2 ___(_____ ) ______________ Fe2O3 ________________________ Hg2S ________________________

  27. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 iron ( II ) bromide CuCl copper (_____) chloride SnO2 ___(_____ ) ______________ Fe2O3 ________________________ Hg2S ________________________

  28. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 iron ( II ) bromide CuCl copper ( I ) chloride SnO2 ___(_____ ) ______________ Fe2O3 ________________________ Hg2S ________________________

  29. Learning Check Complete the names of the following binary compounds with variable metal ions: FeBr2 iron ( II ) bromide CuCl copper ( I ) chloride SnO2tin (IV) oxide exception to inverse criss-cross Fe2O3 ________________________ Hg2S ________________________

  30. Polyatomic Ions NO3- nitrate ion NO2- nitrite ion

  31. NH4+ Cl- Ionic Compounds with Polyatomic Ions More than one element in the ion! Only one element. ammonium chloride, NH4Cl

  32. NH4+ Cl- Ionic Compounds with Polyatomic Ions More than one element in the ion! ammonium chloride, NH4Cl Only one element. SPECIAL NAME for POLYATOMIC IONS: Can you see them on your ion chart?

  33. Ternary Ionic Nomenclature Writing Formulas SAME: • Write each ion, cation first. • Don’t show charges in the final formula. • Overall charge must equal zero. • If charges cancel, just write symbols. • If not equal to zero, use subscripts to balance charges.

  34. Ternary Ionic Nomenclature Writing Formulas • Write each ion, cation first. • Don’t show charges in the final formula. • Overall charge must equal zero. • If charges cancel, just write symbols. • EXACTLY as appear on ion chart. • POLYATOMIC may have subscripts. • If not equal to zero, use subscripts to balance charges. • Use parentheses to show more than one of a particular polyatomic ion.

  35. Ternary Ionic Nomenclature Writing Formulas magnesium phosphate • Write each ion, cation first. • Overall charge must equal zero. • If charges cancel, just write symbols. • EXACTLY as appear on ion chart for polyatomic. • POLYATOMIC may have subscripts. • If not equal to zero: Use parentheses to show more than one of a particular polyatomic ion anduse subscripts to balance charges.

  36. 0 Ionic Compounds Formulas • How do we know how many atoms of each ion we need? • A simple crossing of the charges can answer that question about 90% of the time. • Example: Mg2+ and PO43- Mg3(PO4)2 Check the charges… 3 x (+2) = +6 2 x (-3) = -6 • When they combined they cancel to yield a neutral compound.

  37. 0 Ionic Compounds Formulas • The crossing technique does not work if the magnitude of the charges is the same • Example: Mg2+ and CO32- Mg2(CO3)2 This is incorrect since we want the lowest ratio possible which is 1:1 to yield MgCO3

  38. Ternary Ionic Nomenclature Sodium Sulfate Na+ and SO4-2 Na2SO4 Iron (III) hydroxide Fe+3 and OH- Fe(OH)3 Ammonium carbonate NH4+ and CO3–2 (NH4)2CO3

  39. Cd(OH)2 cadmium hydroxide Ca(ClO2)2 calcium chlorite AgCN silver cyanide Na2SO4 sodium sulfate Na2SO3 sodium sulfite KClO3 potassium chlorate 0 More Practice

  40. Learning Check 1. aluminum nitrate a) AlNO3 b) Al(NO)3 c) Al(NO3)3 2. copper(II) nitrate a) CuNO3 b) Cu(NO3)2 c) Cu2(NO3) 3. Iron (III) hydroxide a) FeOH b) Fe3OH c) Fe(OH)3 4. Tin(IV) hydroxide a) Sn(OH)4 b) Sn(OH)2 c) Sn4(OH)

  41. Naming Ternary Compounds • Contains at least 3 elements • There MUST be at least one polyatomic ion (it helps to circle the ions) • Examples: NaNO3 sodium nitrate K2SO4potassium sulfate Al(HCO3)3aluminumbicarbonate or aluminumhydrogen carbonate

  42. Learning Check Match each set with the correct name: 1.Na2CO3a) magnesium sulfite MgSO3b) magnesium sulfate MgSO4c) sodium carbonate 2 . Ca(HCO3)2a) calcium carbonate CaCO3b) calcium phosphate Ca3(PO4)2 c) calcium bicarbonate

  43. Mixed Practice! Name the following: • Na2O • CaCO3 • PbS2 • Sn3N2 • Cu3PO4 • HgF2

  44. Mixed Up… The Other Way Write the formula: • copper (II) chlorate • calcium nitride • aluminum carbonate • potassium bromide • barium fluoride • cesium hydroxide

  45. Naming Molecular Compounds All are formed from two or more nonmetals. CO2 Carbon dioxide Ionic compounds generally involve a metal and nonmetal (NaCl) BCl3boron trichloride CH4 methane

  46. 0 Naming Covalent Compounds • A covalent compoundis formed by sharing electrons between 2 nonmetals or metalloids. • These compounds are usually molecular and are named using a prefix system. • When naming these compounds name the element further to the left (in the periodic table) first, then the one on the right.

  47. Naming Covalent Compounds • You name the first element using the exact element name. • Name the second element by writing the root of the element’s name and add the suffix “–ide.” • If there is more than one atom of any given element, you add the Greek prefix denoting how many atoms of that element are present. Use list of Greek prefixes. • If only one atom of the second element is present it gets the prefix “mono”, but not for the first element.

  48. Molecular Nomenclature Prefixes PREFIX mono- di- tri- tetra- penta- hexa- hepta- octa- nona- deca- NUMBER 1 2 3 4 5 6 7 8 9 10

  49. Naming Covalent Compounds • Here are some examples of prefix names for binary molecular compounds. • PF5 phosphorus pentafluoride • SO2 sulfur dioxide • SF6 sulfur hexafluoride • N2O4 dinitrogentetroxide • CO carbon monoxide

  50. Molecular (Covalent) Nomenclaturefor two nonmetals • Prefix System (binary molecular compounds) • Add prefixes to indicate # of atoms. • Omit mono- prefix on the FIRST element. Mono- must be used on the SECOND element . • Change the ending of the second element to -ide. Do the reverse for writing formulas!

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