Nomenclature We can determine the formula of a compound by completing Lewis diagrams or via the...
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Transcript of Nomenclature We can determine the formula of a compound by completing Lewis diagrams or via the...
![Page 1: Nomenclature We can determine the formula of a compound by completing Lewis diagrams or via the criss cross method By knowing the valence of elements.](https://reader030.fdocuments.in/reader030/viewer/2022032703/56649d175503460f949ecf61/html5/thumbnails/1.jpg)
NomenclatureNomenclature
![Page 2: Nomenclature We can determine the formula of a compound by completing Lewis diagrams or via the criss cross method By knowing the valence of elements.](https://reader030.fdocuments.in/reader030/viewer/2022032703/56649d175503460f949ecf61/html5/thumbnails/2.jpg)
• 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: Ca2+S2-
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 compoundsRules for naming
• Names end in -ide. Example: sodium chloride• Metal (cation) comes 1st (not chlorine sodide)• Do not capitalize (unless it’s 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 it’s 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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Element(valence)
Englishname
Latin Name Highervalence
Lowervalence
Metals that have and use latin namesCu (1,2) Copper Cuprum Cupric CuprousFe (2,3) Iron Ferrum Ferric FerrousPb (2,4) Lead Plumbum Plumbic PlumbousSn (2,4) Tin Stannum Stannic Stannous
Metals that do not have latin namesCo (2,3) Cobalt - Cobaltic CobaltousCr (2,3) Chromium - Chromic ChromousMn (2,3) Manganese - Manganic Manganous
Metals that have latin names but use english rootHg (1,2) Mercury Hydrargyrum Mercuric Mercurous
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• 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: • Cu2+Cl, Zn2 + Cl, Co2+Cl, Hg+S (do both)
Cu2+Cl = Cu2Cl1 = CuCl2 = copper(II) chloride
Zn2+Cl = Zn2Cl1 = ZnCl2 = zinc chloride
Co2+Cl = Co2Cl1 = CoCl2 = cobalt(II) chloride
Hg+S = Hg1S2 = Hg2S = mercury(I) sulfide
Hg+S = Hg2S2 = HgS = mercury(II) sulfide
Multiple valence: IUPAC naming
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• 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 =
Compounds containing polyatomic ions• So far we have given valences to single atoms
Li + O Li1O2 Li2O
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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- calcium hydroxide
- copper(II) sulfate
- ammonium nitrate
- cobalt(III) carbonate
Ca(OH)2
CuSO4
NH4NO3
Co2(CO3)3
Compounds containing polyatomic ions
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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 valenceN2O4 = dinitrogen tetroxide
• Exception: drop mono for first elementCO2 = carbon dioxide
• The first vowel is often dropped to avoid the combination of “ao” or “oo”.
CO = carbon monoxide (monooxide)
SO2= sulfur dioxide (doxide)
• Name: CCl4, P2O3, IF7
P4O10= tetraphosphorus decoxide
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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• It’s 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)
Li1S2 Li2S
N2O
Pb4(SO4)2 Pb2(SO4)4 Pb(SO4)2
lithium sulfide
dinitrogen monoxide
lead(IV) sulfate
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1. 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
2. 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
Assignment
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Answers – 1, 2a) zinc sulfide b) iron(III) chloridec) calcium carbonated) diphosporus pentoxidee) sodium cyanidef) dinitrogen difluorideg) magnesium hydrogen phosphateh) copper(II) bromatei) potassium oxidej) boron trifluoride
2 a) 2 b) 4
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Answers – 3
a) Na2O
b) KI
c) PbS2
d) Hg2O
e) FeO
f) Fe3(PO4)2
g) CuF2
h) Cl2O
i) Ag2S
j) Mg3N2
k) Al(ClO)3
l) IF5
m) CaCrO4
n) P2S5
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• 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
Naming Bases
- calcium hydroxide - copper(I) hydroxide
- Al(OH)3
- NH4OH
Ca(OH)2
CuOHaluminum hydroxide
ammonium hydroxide
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• All acids start with H (e.g. HCl, H2SO4)• 2 acids types exist: binary acids and oxyacids
Binary: H + non-metal. E.g. HClOxy: H + polyatomic ion. E.g. H2SO4
• Each have different naming rules.Binary acids: naming depends on state of acid• If it’s 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)
Naming Acids: Binary acids
HBr(s) HI(aq)H2S(aq) H2S(g)
hydrogen bromide hydroiodic acidhydrogen sulfidehydrosulfuric acid
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• Naming does not depend on the state (aq)• 1) name the polyatomic ion
2) replace ate with ic, ite with ous3) change non-metal root for pronunciation4) add “acid” to the name
E.g. H2SO3
Naming Acids: Oxyacids
HNO2 hypochlorous acid
H3PO4(aq) carbonic acid
1) sulphite, 2) sulphous,
3) sulphurous, 4) sulphurous 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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a) chloric acidb) hydrosulfuric acidc) hydrobromic acidd) phosphorous acide) iodic acidf) HCl(g)g) HCl(aq)h) H2SO4(s)
i) H2SO4(aq)
j) HClO2
k) HF(aq)
Assignment: give formula or namea) HClO3
b) H2S(aq)
c) HBr(aq)d) H3PO3
e) HIO3
f) hydrogen chlorideg) hydrochloric acidh) sulfuric acidi) sulfuric acidj) chlorous acidk) hydrofluoric acid
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• 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. CuSO4•5H2O is
copper(II) sulfate pentahydrate.• A greek prefix indicates the # of H2O groups.
Hydrates
sodium sulfate decahydrate nickel(II) sulfate hexahydrate
Na2CO3•H2O BaCl2•2H2O
Na2SO4•10H2O NiSO4•6H2O sodium carbonate monohydratebarium chloride dihydrate