Naming Compounds Ppt2003
Transcript of Naming Compounds Ppt2003
Chemical nomenclature(Naming compounds)
Chemistry Dept - FAST
Batterjee Medical CollegeObhur, KSA
At the end of these lectures you should be able to:1. Write symbols for elements and ions.
2. Name and write chemical formulae for ionic compounds
3. Name and writes chemical formulae of molecular compounds of two nonmetals.
4. Name a compound, given its chemical formula. Example: N2O4 is dinitrogentetroxide.
5. Write the chemical formula for a compound if you are given the name of that compound.
Example: manganese (IV) oxide is MnO2.
3
Metal Cations• Metals with one possible
Charge (single charge):– metals whose ions can only
have one possible charge• Groups 1 Na+1 & gp 2
Mg+2, gp 3 Al+3, • Transition metals Ag+1,
Zn+2, Sc+3 – cation name = metal name
4
Metal Cations
• Metals with more than one charge:
– Find charge by charge on anion.– cation name = metal name with Roman numbers charge in brackets
5
Naming monatomic nonmetal anion• Find the charge from position on the Periodic
table.• To name anion, change ending on the element
name to –ide
Group 5= -3 Group 6= -2 Group 7 = -1
N3- = nitride O2- = oxide F- = fluoride
P3- = phosphide S2- = sulfide Cl- = chloride
6
Write the formula of a compound made from aluminum ions and oxide ions
1. Write the symbol for the metal cation and its charge
2. Write the symbol for the nonmetal anion and its charge
3. Charge (without sign) becomes subscript for other ion.
4. Reduce subscripts to smallest whole number ratio
5. Check that the total charge of the cations cancels the total charge of the anions.
Al+3 Group 3
O2- Group 6
Al+3 O2-
Al2 O3
Al = (2) (+3) = +6∙O = (3) (-2) = -6∙
7
Learning Check 1
What are the formulas for compounds made from the following ions?
•potassium ion with a nitride ion
•calcium ion with a bromide ion
•aluminum ion with a sulfide ion
8
Solution 1
What are the formulas for compounds made from the following ions?
K+ with N3- K3N
Ca+2 with Br- CaBr2
Al+3 with S2- Al2S3
9
Learning Check 2
What are the formulas for compounds made from the following ions?
1. copper(II) ion with a nitride ion
2. iron(III) ion with a bromide ion
10
Solution 2
What are the formulas for compounds made from the following ions?
1. Cu2+ with N3- Cu3N2
2. Fe+3 with Br- FeBr3
11
Rules for Ionic Compounds• made of cation and anion.• some have one or more nicknames that are
only learned by experience– NaCl = table salt, NaHCO3 = baking soda
• write systematic name by simply naming the ions– If cation is:
• metal with single charge = metal name [eg. Na+ (sodium)]• metal with more than one charge (Transition Metals) = metal
name(charge) [eg.Cu+ Copper (I), Cu2+ Copper(II)]• polyatomic ion = name of polyatomic ion [NH4
+ ammonium] – If anion is:
• nonmetal = part of nonmetal name + ide [eg. Flouride]• polyatomic ion = name of polyatomic ion [eg. Sulphate]
12
Example 1: CsF
1. Identify cation and anionCs = Cs+ because it is Group 1
F = F- because it is Group 72. Name the cation
Cs+ = cesium3. Name the anion
F- = fluoride4. Write the cation name first, then the anion name
cesium fluoride
13
Learning Check 3
Name the following compounds
1. KCl
2. MgBr2
3. Al2S3
14
Solution 3
1. KCl potassium chloride
2. MgBr2 magnesium bromide
3. Al2S3 aluminum sulfide
15
Example 2:CuF2
1. Identify cation and anionF = F- because it is Group 7
Cu = Cu2+ to balance the two (-) charges from 2 F-
2. Name the cationCu2+ = copper(II)
3. Name the anionF- = fluoride
4. Write the cation name first, then the anion namecopper(II) fluoride
16
Learning Check 4
Name the following compounds
1. TiCl4
2. PbBr2
3. Fe2S3
17
Solution 4
1. TiCl4 titanium(IV) chloride
2. PbBr2 lead(II) bromide
3. Fe2S3 iron(III) sulfide
18
Compounds containing polyatomic Ions
• Polyatomic ions are single ions that contain more than one atom.
• Name and charge of polyatomic ion do not change.
• Name any ionic compound by naming cation first and then anion.
19
Some Common Polyatomic IonsName Formulaacetate C2H3O2
–
carbonate CO32–
hydrogen carbonate( bicarbonate)
HCO3–
hydroxide OH–
nitrate NO3–
nitrite NO2–
chromate CrO42–
dichromate Cr2O72–
ammonium NH4+
Name Formulahypochlorite ClO–
chlorite ClO2–
chlorate ClO3–
perchlorate ClO4–
sulfate SO42–
sulfite SO32–
hydrogen sulfate(aka bisulfate)
HSO4–
hydrogen sulfite(aka bisulfite)
HSO3–
20
1. Identify the ionsNa = Na+ because in Group 1SO4 = SO4
2- a polyatomic ion2. Name the cation
Na+ = sodium, metal with single charge3. Name the anion
SO42- = sulfate
4. Write the name of the cation followed by the name of the anion
sodium sulfate
Example 3:Na2SO4
21
Example 4: Fe(NO3)3
1. Identify the ionsNO3 = NO3
- a polyatomic ionFe = Fe+3 to balance the charge of the 3 NO3
-1
2. Name the cationFe+3 = iron(III)
3. Name the anionNO3
- = nitrate4. Write the name of the cation followed by the
name of the anioniron(III) nitrate
22
Learning Check 5
Name the following
1. NH4Cl
2. Ca(C2H3O2)2
3. Cu(NO3)2
23
Solution 5
1. NH4Cl ammonium chloride
2. Ca(C2H3O2)2 calcium acetate
3. Cu(NO3)2 copper(II) nitrate
24
Learning Check 6
What are the formulas for compounds made from the following ions?
1. aluminum ion with a sulfate ion
2. chromium(II) with hydrogen carbonate
25
Solution 6
What are the formulas for compounds made from the following ions?
1. Al+3 with SO42- Al2(SO4)3
2. Cr+2 with HCO3─ Cr(HCO3)2
26
Hydrates• hydrates are ionic compounds
containing a specific number of waters for each formula unit.
• water of hydration often “driven off” by heating.
• in formula, attached waters follow ∙– CoCl2∙6H2O
• -add hydrate after name of ionic compound– CoCl2 6H∙ 2O = cobalt(II) chloride hexa hydrate– CaSO4∙½H2O = calcium sulfate hemi hydrate
Prefix No. of Waters
hemi ½
mono 1
di 2
tri 3
tetra 4
penta 5
hexa 6
hepta 7
octa 8
Hydrate
CoCl2∙6H2O
AnhydrousCoCl2
27
Learning Check 7
1. What is the formula of magnesium sulfate heptahydrate?
2. What is the name of NiCl2•6H2O?
28
Solution 7
1. What is the formula of magnesium sulfate heptahydrate? MgSO47H2O
2. What is the name of NiCl2•6H2O? nickel(II) chloride hexahydrate
Naming of covalent compounds
30
Writing names of binary molecular compounds of 2 nonmetals
1. Write name of first element in formula– element furthest left and down on the Periodic Table– use the full name of the element
2. Write name of the second element in the formula with an -ide suffix
– as if it were an anion, however, remember these compounds do not contain ions!
3. Use a prefix in front of each name to indicate the number of atoms
_ never use the prefix mono- on the first element
31
Subscript - prefixes
• 1 = mono- – not used on first
nonmetal• 2 = di-• 3 = tri-• 4 = tetra-• 5 = penta-
• 6 = hexa-• 7 = hepta-• 8 = octa-• 9 = nona-• 10 = deca-
• drop last “a” if name begins with vowel
32
Example 5: BF3
1. Name the first elementboron
2. Name the second element with an –idefluorine fluoride
3. Add a prefix to each name to indicate the subscript
monoboron, trifluoride4. Write the first element with prefix, then the
second element with prefix– Drop prefix mono from first element
boron trifluoride
33
Learning Check 8
Name the following1. NO2
2. PCl5
3. I2F7
34
Solution 8
1. NO2 nitrogen dioxide
2. PCl5 phosphorus pentachloride
3. I2F7 diiodine heptafluoride
35
Example 6:dinitrogen pentoxide
• Identify the symbols of the elements
nitrogen = N
oxide = oxygen = O• Write the formula using prefix number for
subscript
di = 2, penta = 5
N2O5
36
Learning Check 9
Write formulas for the following
1. dinitrogen tetroxide
2. sulfur hexafluoride
3. diarsenic trisulfide
37
Solution 9
1. dinitrogen tetroxide N2O4
2. sulfur hexafluoride SF6
3. diarsenic trisulfide As2S3
covalent formulae Ionic formulae
H2O
CO2
NH3
H2
O2
N2
SO2
Water
Carbon dioxide
Ammonia
Hydrogen
Oxygen
Nitrogen
Sulphur dioxide
NaCl
CaCl2
MgO
HCl(aq)
H2SO4(aq)
HNO3(aq)
NaOH
Ca(OH)2
CaCO3
Al2O3
Fe2O3
Sodium chloride
Calcium chloride
Magnesium oxide
Hydrochloric acid
Sulphuric acid
Nitric acid
Sodium hydroxide
Calcium hydroxide
Calcium carbonate
Aluminium oxide
Iron (III)oxide