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Naming Compounds

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E.g. What is the formula of sodium oxide? To get the answer, first write ... 3. Write formulas for: a) sodium oxide, b) potassium iodide, c) plumbic sulfide, ... – PowerPoint PPT presentation

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Title: Naming Compounds


1
Naming Compounds
Day 2
2
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

3
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

4
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

5
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

6
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
7
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

8
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
9
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
hydr(o)iodic acid
hydrogen sulfide
hydrosulfuric acid
10
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
11
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
12
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
13
Hydrates
For more lessons, visit www.chalkbored.com
  • 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. 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
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