spm chemistry chapter 3
DESCRIPTION
SPM CHEMISTRY CHAPTER 3: CHEMICAL FORMULAE AND EQUATIONSTRANSCRIPT
SPM CHEMISTRY
Chapter 3: Chemical Formulae & Equations
Prepared by: Ms. Brintha Ganapathy BSc. MSc.
3.1 Relative atomic mass and Relative molecular mass
1. Relative atomic mass, Ar is the __________________________ of an atom
when compared to a __________________________.
2. Standard atom:
a. Hydrogen scale: hydrogen is the lightest atom of all and the mass
of one hydrogen atom was assigned 1 unit.
Weakness of Hydrogen scale:
not too many elements can react readily with hydrogen,
hydrogen exists as a gas at room temperature and
has a number of isotopes with different masses.
b. Helium scale: the second lightest atom of all and the mass of one
helium atom were assigned 1 unit.
Weakness of Helium scale:
helium exists as a gas at room temperature and
helium is an inert gas.
c. Oxygen scale: chose as the standard atom to compare the masses
of atoms
Weakness of Oxygen scale:
the existence of three isotopes of oxygen were discovered
natural oxygen (containing all the three isotopes) as the
standard
used the isotopes oxygen-16 as the standard
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d. Carbon scale: standard atom of comparison internationally.
a carbon-12 atom is __________________________than an atom of
hydrogen
exists as a solid at room temperature
most abundant carbon isotope, happening about 98.89%
3. Relative atomic mass, Ar of an atom is
4. Relative molecular mass, Mr of a substance is
5. Example:
Relative atomic mass, Ar of helium = 4
Relative molecular mass, Mr of H O ₂
Relative formula mass, Na2CO3·10H2O
=
2
Practice 3.1
Calculate the RMM of the following substances.
[RMM: H, 1; C, 12; O, 16; Cl, 35.5, Na, 23; Mg, 24; Al, 27; S, 32; Ca, 40]
a. Ethanol, C H OH₂ ₅ b. Oxygen gas, O₂ c. Carbon dioxide,
CO₂
d. Water molecule,
H O₂e. Tetrachloromethane,
CCl₄f. Sodium chloride,
NaCl
g. Carbon monoxide,
CO
h. Aluminium
carbonate, Al (CO )₂ ₃ ₃i. Magnesium
chloride, MgCl₂
j. Calcium carbonate,
CaCO₃k. Calcium sulphate,
CaSO₄l. Hydrochloric acid,
HCl
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3.2, 3.3, 3.4 Relationship between the number of moles and the
number of particles, mass and volume of gas
1. Avogadro constant / Avogadro’s number is 6.02 x 1023
2. Room temperature and pressure (r.t.p.) = 24 dm3 mol-1
(25°C and 1 atm)
3. Standard temperature and pressure (s.t.p) = 22.4 dm3 mol-1
Mass (g) = Number of moles x Molar mass
Number of particles = Number of moles x Avogadro constant
Volume (dm3) = Number of moles x Molar volume
Question!
State three formulae to find number of moles
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3.5 Empirical and Molecular Formulae
1. Empirical formulae definition
Simplest ratio of atoms of each element that present in the compound
2. Molecular formulae definition
Actual number of atoms of each element that is present in one
molecule of the compound
3. Molecular formula = (empirical formula)n,
Calculation of Empirical Formula
Example 1 Example 2
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List of cations = positively-charged ions
Charge Cations Formula
+ 1 Ammonium ion NH4+
+ 1 Copper(I) ion Cu+
+ 1 Hydrogen ion H+
+ 1 Lithium ion Li+
+ 1 Nickel(I) ion Ni+
+ 1 Potassium ion K+
+ 1 Silver ion Ag+
+ 1 Sodium ion Na+
+ 2 Barium ion Ba2+
+ 2 Calcium ion Ca2+
+ 2 Copper(II) ion Cu2+
+ 2 Iron(II) ion Fe2+
+ 2 Lead(II) ion Pb2+
+ 2 Magnesium ion Mg2+
+ 2 Manganese(II) ion Mn2+
+ 2 Nickel(II) ion Ni2+
+ 2 Tin(II) ion Sn2+
+ 2 Zinc ion Zn2+
+ 3 Aluminium ion Al3+
+ 3 Chromium(III) ion Cr3+
+ 3 Iron(III) ion Fe3+
+ 4 Lead(IV) ion Pb4+
+ 4 Tin(IV) ion Sn4+
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PLEASE MEMORISE!
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List of Anions = negatively-charged ions
Charge Anions Formula
- 1 Bromide ion Br-
- 1 Chloride ion Cl-
- 1 Chlorate(V) ion ClO3-
- 1 Ethanoate ion CH3COO-
- 1 Fluoride ion F-
- 1 Hydride ion H-
- 1 Hydroxide ion OH-
- 1 Iodide ion I-
- 1 Manganate(VII) ion MnO4-
- 1 Nitrate ion NO3-
- 1 Nitrite ion NO2-
- 2 Oxide ion O2-
- 2 Carbonate ion CO32-
- 2 Chromate(VI) ion CrO42-
- 2 Dichromate(VI) ion Cr2O72-
- 2 Sulphide ion S2-
- 2 Sulphate ion SO42-
- 2 Sulphite ion SO32-
- 2 Thiosulphate ion S2O32-
- 3 Nitride ion N3-
- 3 Phosphate ion PO43-
- 3 Phosphite ion PO33-
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PLEASE MEMORISE!
Chemical formulae for ionic compounds
Name Chemical
formula
Number of
cation
Number of
anion
Zinc chloride ZnCl2
Copper(II)
sulphate
CuSO4
Aluminium
sulphate
Al2(SO4)3
Prefixes
Prefix Meaning
Mono- 1
Di- 2
Tri- 3
Tetra- 4
Penta- 5
Hexa- 6
Hepta- 7
Octa- 8
Nona- 9
Deca- 10
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Chemical Equation
nA + nB nC + nD
Example 1:
Word equation:
Sodium hydroxide + sulphuric acid sodium sulphate + water
Chemical equation: NaOH + H2SO4 Na2SO4 + H2O
Balancing equation: 2NaOH + H2SO4 Na2SO4 + 2H2O
Complete chemical equation: 2NaOH + H2SO4 Na2SO4 + 2H2O
Example 2:
Word equation:
Aluminium + copper(II) oxide aluminium(III) oxide + copper
Chemical equation: Al + CuO Al2O3 + Cu
Balancing equation: __________________________________________________________
Complete chemical equation: _______________________________________________
Example 3:
Word equation: Nitrogen + hydrogen ammonia
Chemical equation: N2 + H2 NH3
Balancing equation: __________________________________________________________
Complete chemical equation: _______________________________________________
Information obtainable from chemical equations
i) mass of reactants
ii) volume of reacting gas
iii) mass of products formed
iv) volume of gas produced
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Balancing Chemical Equations
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TIPS!Always balance the chemical equations
starting from the gases
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Example:
2 cm3 of lead (II) nitrate solution is added to excess of potassium iodide
solution. How many molecules of potassium nitrate will be formed?
[Relative atomic mass: N, 14; O, 16; K, 39; I, 127; Pb, 207; Avogadro's constant:
6.02 x 1023 mol-1]
Step 1: Write a complete chemical equation.
Pb(NO3)2(aq) + 2KI(aq) –> PbI2(s) + 2KNO3(aq)
From the equation, 1 mole of Pb(NO3)2 reacts with 2 moles of KI formed
1 mole PbI2 of and 2 moles of KNO3.
Step 2: Convert to moles.
No. of moles of Pb(NO3)2
= Mass of Pb(NO3)2 / Relative molecular mass
= 2 / [207 + 2(14 + 3 x 16)]
= 6.04 x 10-3 mol
Step 3: Ratio of moles.
Number of moles of KNO3/ Number of moles of Pb(NO3)2
= 2/1
Number of moles of KNO3
= (2 x 6.04 x 10-3) / 1
= 12.08 x 10-3 mol
Step 4: Convert to the number of molecules of potassium nitrate.
Number of molecules of KNO3
= 12.08 x 10-3 x 6.02 x 1023
= 7.27 x 1021
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This part of the chapter is the most challenging, but
once you hit the technique it will be easy forever.