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Naming Compounds. Day 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: Na 1 O 2  Na 2 O What is the formula of copper(II) oxide? Cu 2 O 2  Cu 2 O 2  CuO

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working backwards name to formula
Working backwards: name to formula
  • It’spossibletodetermineaformulafromaname
  • 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
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

slide4

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
  • Givethevalenceofa)FeinFeO,b)MninMnO2
  • 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)magnesiumnitride, k)aluminumhypochlorite, l) iodine pentafluoride, m) calcium chromate, n) diphosphorus pentasulfide
complete exercises on handout

Complete exercises on handout

  • Steps:
  • Determine if its ionic or covalent
  • If ionic, determine if its metal has one or more valence
  • Name according to appropriate rules
answers 1 2
Answers – 1, 2
  • zinc sulfide
  • iron(III) chloride
  • calcium carbonate
  • diphosporus pentoxide
  • sodium cyanide
  • dinitrogen difluoride
  • magnesium hydrogen phosphate
  • copper(II) bromate
  • potassium oxide
  • boron trifluoride

2 a) 2 b) 4

answers 3
Answers – 3
  • Cl2O
  • Ag2S
  • Mg3N2
  • Al(ClO)3
  • IF5
  • CaCrO4
  • P2S5
  • Na2O
  • KI
  • PbS2
  • Hg2O
  • FeO
  • Fe3(PO4)2
  • CuF2
naming bases
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:
  • +veisnamedfirst,followedbythepolyatomicion

- calcium hydroxide

- copper(I) hydroxide

- Al(OH)3

- NH4OH

Ca(OH)2

CuOH

aluminum hydroxide

ammonium hydroxide

naming acids binary acids
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 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)

HBr(s) HI(aq)

H2S(aq) H2S(g)

hydrogen bromide

hydr(o)iodic acid

hydrosulfuric acid

hydrogen sulfide

naming acids oxyacids
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

naming acids oxyacids11
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

- nitrous acid

- HClO

- phosphoric acid

- H2CO3

assignment give formula or name
Assignment: give formula or name

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

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)

hydrates

For more lessons, visit www.chalkbored.com

Hydrates
  • 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.

sodium sulfate decahydrate

nickel(II) sulfate hexahydrate

Na2CO3•H2O

BaCl2•2H2O

Na2SO4•10H2O

NiSO4•6H2O

sodium carbonate monohydrate

barium chloride dihydrate