Nomenclature

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Nomenclature
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• We can determine the formula of a compound by
  completing Lewis diagrams or via the criss cross
  method
• By knowing the valence of elements you can
  determine the formula of compounds
• E.g. what compound would form from Ca S?
• Step 1 - write valences Ca2S2-
• Step 2 - cross down valences Ca2S2
• Step 3 reduce CaS

a) Al,Br b) K,S c) Zn,O d) Mg,N e) C,Cl f) Cu,O
AlBr3
K2S
ZnO
Mg3N2
CCl4
CuO or Cu2O
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Ionic compounds

• Rules for naming
• Names end in -ide. Example sodium chloride
• Metal (cation) comes 1st (not chlorine sodide)
• Do not capitalize (unless its the start of a
  sentence)
• Give formulae name Ca I, O Mg, Na S
• Ca2I1 CaI2 calcium iodide
• Mg2O2 MgO magnesium oxide
• Na1S2 Na2S sodium sulfide

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Multiple valence Latin naming

• When the metal in an ionic compound is
  multivalent there are 2 methods Latin or IUPAC
• As before, the name ends in -ide metal is first
• The metal is named with its Latin or English
  root and ends in -ic or ous to denote valence
• E.g. Cu1 is cuprous, E.g. Cu2 is cupric
• Lower ous, Higher ic
• Give formulas and Latin names for
• Cu2 Cl- CuCl2 cupric chloride
• copper (II) chloride (IUPAC)
• Cu Cl CuCl cuprous chloride
• copper (I) chloride

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Multiple valence IUPAC naming

• Name ends in -ide, positive/metal comes first
• The valence of the metal is indicated in brackets
  using roman numerals
• E.g. Cu1 is copper(I), Cu2 is copper(II)
• Numbers refer to valences not to s of atoms
• Try
• Cu2Cl, Zn2 Cl, Co2Cl, HgS (do both)
• Cu2Cl Cu2Cl1 CuCl2 copper(II) chloride
• Zn2Cl Zn2Cl1 ZnCl2 zinc chloride
• Co2Cl Co2Cl1 CoCl2 cobalt(II) chloride
• HgS Hg1S2 Hg2S mercury(I) sulfide
• HgS Hg2S2 HgS mercury(II) sulfide

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Compounds containing polyatomic ions

• So far we have given valences to single atoms
• Li O

Li1O2 ? Li2O

• Groups of atoms can also have valences
• Polyatomic ions are groups of atoms that
  interact as a single unit.
• E.g. OH1, (SO4)2. Ba3(PO4)2

barium phosphate

• Naming compounds with polyatomic ions is similar
  to naming other ionic compounds
• You should note that compounds with polyatomic
  ions have names ending in -ate or -ite not -ide
• Note that most are negative, except ammonium
• Name Ca(OH)2, CuSO4, NH4NO3, Co2(CO3)3

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Compounds containing polyatomic ions
- calcium hydroxide - copper(II) sulfate -
ammonium nitrate - cobalt(III) carbonate
Ca(OH)2 CuSO4 NH4NO3 Co2(CO3)3
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Naming covalent compounds

• -ide ending, each element has prefix

1 mono
2 di
3 tri
4 tetra
5 penta
6 hexa
7 hepta
8 octa
9 nona
10 deca

• prefix refers to of atoms - not valence
• N2O4 dinitrogen tetroxide
• Exception drop mono for first element
• CO2 carbon dioxide
• The first vowel is often dropped to avoid the
  combination of ao or oo.
• CO carbon monoxide (monooxide)

P4O10 tetraphosphorus decoxide
SO2 sulfur dioxide (doxide)

• Name CCl4, P2O3, IF7

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Write and name the following covalent compounds
(IUPAC)

• carbon tetrachloride
• diphosporus trioxide
• iodine heptafluoride

CCl4 P2O3 IF7
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Working backwards name to formula

• Its possible to determine a formula from a name
• E.g. What is the formula of sodium oxide?
• To get the answer, first write the valences
• Na1O2 ? Na2O
• What is the formula of copper(II) oxide?
• Cu2O2 ? Cu2O2 ? CuO
• For covalent compounds, simply use the prefixes
  to tell you the number of each element
• What is the formula for dinitrogen trioxide?
• N2O3
• Give formulae for lithium sulfide, dinitrogen
  monoxide, lead(IV) sulfate

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Write and name the following covalent compounds
(IUPAC)
lithium sulfide dinitrogen monoxide lead(IV)
sulfate

• Li1S2 ? Li2S
• N2O
• Pb4(SO4)2 ? Pb2(SO4)4 ? Pb(SO4)2

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Assignment

• Name each according to IUPAC rules a)
  ZnS, b) FeCl3, c) CaCO3, d) P2O5, e) NaCN, f)
  N2F2, g) MgHPO4, h) Cu(BrO3)2, i) K2O, j) BF3
• Give the valence of a) Fe in FeO, b) Mn in MnO2
• 3. Write formulas for a) sodium oxide,
  b) potassium iodide, c) plumbic sulfide,
  d) mercury(I) oxide, e) ferrous oxide,
  f) iron(II) phosphate, g) copper(II)
  fluoride, h)
  dichlorine monoxide, i) silver sulfide,
  j) magnesium nitride, k) aluminum hypochlorite,
  l) iodine pentafluoride, m) calcium chromate,
  n) diphosphorus pentasulfide

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Answers 1, 2

1. zinc sulfide
2. iron(III) chloride
3. calcium carbonate
4. diphosporus pentoxide
5. sodium cyanide
6. dinitrogen difluoride
7. magnesium hydrogen phosphate
8. copper(II) bromate
9. potassium oxide
10. boron trifluoride

2 a) 2 b) 4
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Answers 3

1. Na2O
2. KI
3. PbS2
4. Hg2O
5. FeO
6. Fe3(PO4)2
7. CuF2

1. Cl2O
2. Ag2S
3. Mg3N2
4. Al(ClO)3
5. IF5
6. CaCrO4
7. P2S5

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Naming Bases

• Bases contain an OH group
• C6H12O6 does not have an OH group
• If an OH group is present it will be clearly
  indicated e.g. NaOH, Ca(OH)2
• Also notice that bases have a metal (or positive
  ion such as NH4 at their beginning)
• Bases are named like other ionic compounds
• ve is named first, followed by the polyatomic ion

- calcium hydroxide - copper(I)
hydroxide - Al(OH)3 - NH4OH
Ca(OH)2 CuOH aluminum hydroxide ammoni
um hydroxide
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Naming Acids Binary acids

• All acids start with H (e.g. HCl, H2SO4)
• 2 acids types exist binary acids and oxyacids
• Binary H non-metal. E.g. HCl
• Oxy H polyatomic ion. E.g. H2SO4
• Each have different naming rules.
• Binary acids naming depends on state of acid
• If its not aqueous hydrogen non-metal
• HCl(g) hydrogen chloride
• If it is aqueous hydro non-metal ic acid
• HCl(aq) hydrochloric acid (aqueous hydrogen
  chloride)

HBr(s) HI(aq) H2S(aq)
H2S(g)
hydrogen bromide
hydroiodic acid
hydrogen sulfide
hydrosulfuric acid
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Naming Acids Oxyacids

• Naming does not depend on the state (aq)
• 1) name the polyatomic ion
• 2) replace ate with ic, ite with ous
• 3) change non-metal root for pronunciation
• 4) add acid to the name
• E.g. H2SO3

1) sulphite,
2) sulphous,
3) sulphurous,
4) sulphurous acid
HNO2 hypochlorous acid H3PO4(aq)
carbonic acid
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Naming Acids Oxyacids
HNO2 hypochlorous acid H3PO4(aq)
carbonic acid
- nitrous acid
- HClO
- phosphoric acid
- H2CO3
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Assignment give formula or name

• a) chloric acid
• b) hydrosulfuric acid
• c) hydrobromic acid
• d) phosphorous acid
• e) iodic acid
• f) HCl(g)
• g) HCl(aq)
• h) H2SO4(s)
• i) H2SO4(aq)
• j) HClO2
• k) HF(aq)

a) HClO3 b) H2S(aq) c) HBr(aq) d) H3PO3 e)
HIO3 f) hydrogen chloride g) hydrochloric acid h)
sulfuric acid i) sulfuric acid j) chlorous
acid k) hydrofluoric acid
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Hydrates

• Some compounds contain H2O in their structure.
  These compounds are called hydrates.
• This is different from (aq) because the H2O is
  part of the molecule (not just surrounding it).
• The H2O can usually be removed if heated.
• A dot separates water e.g. CuSO45H2O is
  copper(II) sulfate pentahydrate.
• A greek prefix indicates the of H2O groups.

sodium sulfate decahydrate nickel(II) sulfate
hexahydrate Na2CO3H2O BaCl22H2O
Na2SO410H2O NiSO46H2O sodium carbonate
monohydrate barium chloride dihydrate