naming acids-bases chemicals

Naming CompoundsNaming Compounds

Day 2Day 2

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

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

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

1. Give the valence of a) Fe in FeO, b) Mn in MnO2

3. Write formulas for: a) sodium oxide, b) potassium iodide, c) lead(IV) sulfide, d) mercury(I) oxide, e) Iron(II) 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

Complete exercises on handout

Steps:

1. Determine if its ionic or covalent

2. If ionic, determine if its metal has one or more valence

3. Name according to appropriate rules

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

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

• 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

• 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 hydr(o)iodic acidhydrogen sulfidehydrosulfuric acid

• 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

• 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

- nitrous acid - HClO

- phosphoric acid - H2CO3

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) hydrogen sulphatei) sulfuric acidj) chlorous acidk) hydrofluoric acid

• Some compounds contain H2O in their struc-ture. 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

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