Relative formula mass and empirical
Transcript of Relative formula mass and empirical
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Relative formula mass and empirical
formulaObjectives:
• To know how to write chemical formula.
• To understand the meaning of relative
atomic mass.
• To understand what an empirical formula
is.
• To be able to calculate relative formula
mass.
• To be able to calculate empirical formula.
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SC9a Masses and empirical formulae
Quick Quiz
1 What is the formula of water?
2 What is the formula of sodium chloride?
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SC9a Masses and empirical formulae
Quick Quiz
1 What is the formula of water?
H2O
2 What is the formula of sodium chloride?
NaCl
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SC9a Masses and empirical formulae
Quick Quiz
3 What is the formula of carbon dioxide?
4 The formula of magnesium chloride is MgCl2.
What is the ratio of magnesium ions to chloride
ions?
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SC9a Masses and empirical formulae
Quick Quiz
3 What is the formula of carbon dioxide?
CO2
4 The formula of magnesium chloride is MgCl2.
What is the ratio of magnesium ions to chloride
ions?
1:2
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SC9a Masses and empirical formulae
Quick Quiz
5 The formula of sulfuric acid is H2SO4. How many
atoms of each element are in the formula?
6 The formula of calcium nitrate is Ca(NO3)2. How
many calcium, nitrogen and oxygen atoms are in
the formula?
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SC9a Masses and empirical formulae
Quick Quiz
5 The formula of sulfuric acid is H2SO4. How many
atoms of each element are in the formula?
H = 2, S = 1, O = 4
6 The formula of calcium nitrate is Ca(NO3)2. How
many calcium, nitrogen and oxygen atoms are in
the formula?
Ca = 1, N = 2, O = 6
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SC9a Masses and empirical formulae
Quick Quiz
7 There are two numbers alongside chlorine in the
periodic table, 17 and 35.5. What does the
number 17 represent?
8 What does the number 35.5 represent?
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SC9a Masses and empirical formulae
Quick Quiz
7 There are two numbers alongside chlorine in the
periodic table, 17 and 35.5. What does the
number 17 represent?
atomic number
8 What does the number 35.5 represent?
relative atomic mass (mass number)
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Relative formula mass and empirical
formulaObjectives:
• To know how to write chemical formula.
• To understand the meaning of relative
atomic mass.
• To understand what an empirical formula
is.
• To be able to calculate relative formula
mass.
• To be able to calculate empirical formula.
![Page 13: Relative formula mass and empirical](https://reader030.fdocuments.in/reader030/viewer/2022013001/61ca977d08fcab63004a90d3/html5/thumbnails/13.jpg)
• Why is it called relative atomic mass?
The relative mass of an object is the mass of that
object compared to the mass of another object.
For example, relative
to the girl, the tiger is
four times as heavy.
We say it has a
relative mass of 4.
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Atoms are measured
relative to 1/12th the
mass of a 12C atom.
12C atoms have a relative
mass of 12.
1H atoms are twelve
times lighter so have a
relative mass of 1.
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SC9a Relative formula masses and empirical formulae
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The relative formula mass (Mr) of a substance is the sum
of the relative atomic masses (Ar) of all the atoms or ions in
its formula.
relative atomic mass : Ar (O)
relative formula mass : Mr(HNO3)
Worked example
The formula of nitric acid is HNO3.
This means that it contains 1 hydrogen, 1 nitrogen and
3 oxygens.
Mr of HNO3 = Ar(H) + Ar(N) + 3 × Ar(O)
= 1 + 14 + (3 × 16)
= 63 Notice that
Mrs have
no units
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Relative Formula Mass• How will we calculate this?• To calculate this we simply add together
the atomic masses of all the atoms shown in the formula. (N=14; H=1; Na=23; O=16; Mg=24; Ca=40)
Substance Formula Formula Mass
Ammonia NH3
Sodium oxide Na2O
Magnesium hydroxide Mg(OH)2
Calcium nitrate Ca(NO3)2
14 + (3x1)=17
(2x23) + 16 =62
24+ 2(16+1)=58
40+ 2(14+(3x16))=164
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Calculate the relative formula mass of the
following substances.
a) F2
b) Fe
c) H2SO4
d) Al2O3
e) Al(NO3)3
f) (NH4)2SO4
g) CuCO3
h) AgNO3
i) NH4NO3
RAMs
F=19
Fe=56
H=1
S=32
O=16
Al=27
N=14
Cu=63.5
C=12
Ag=108
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Calculate the relative formula mass of the
following substances.
a) F2
b) Fe
c) H2SO4
d) Al2O3
e) Al(NO3)3
f) (NH4)2SO4
g) CuCO3
h) AgNO3
i) NH4NO3
Answers
a) 38
b) 56
c) 98
d) 102
e) 213
f) 132
g) 123.5
h) 170
i) 80
RAMs
F=19
Fe=56
H=1
S=32
O=16
Al=27
N=14
Cu=63.5
C=12
Ag=108
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Relative formula mass and empirical
formulaObjectives:
• To know how to write chemical formula.
• To understand the meaning of relative
atomic mass.
• To understand what an empirical
formula is.
• To be able to calculate relative formula
mass.
• To be able to calculate empirical
formula.
![Page 20: Relative formula mass and empirical](https://reader030.fdocuments.in/reader030/viewer/2022013001/61ca977d08fcab63004a90d3/html5/thumbnails/20.jpg)
Empirical formula
• The simplest whole number ratio of atoms
in a compound
eg. H2O2 empirical formula is
C3H6 empirical formula is
H O
CH2
Molecular formula
(true formula of compound)
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SC9a Relative formula masses and empirical formulae
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Worked example
Aluminium bromide is formed from 0.51 g of aluminium and
4.49 g of bromine. Calculate the empirical formula of
aluminium bromide.
Relative atomic masses:
Al = 27 Br = 80
Set your working out in columns and explain each step.
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SC9a Relative formula masses and empirical formulae
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Al Br
Mass (g) 0.51 4.49
You can round
numbers that
are close to a
whole number,
but if it is .5,
double both
numbers
Don’t forget
to write the
formula from
the ratio
÷ by RAM
÷ by smallest number
Simplest whole
number ratio
Empirical formula
= 0.0189 = 0.0561
= 1 = 2.97
1 3
AlBr3
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SC9a Relative formula masses and empirical formulae
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Question
A sample of sodium phosphate contains 3.45 g of sodium,
1.55 g of phosphorus and 3.20 g of oxygen. Calculate the
empirical formula of sodium phosphate.
Relative atomic masses:
O = 16 Na = 23 P = 31
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SC9a Relative formula masses and empirical formulae
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Na P O
Mass (g) 3.45 1.55 3.20
Answer
= 0.15 = 0.05 = 0.20
= 3 = 1 = 4
Na3PO4
÷ RAM
÷ 0.05
Empirical formula
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SC9a Relative formula masses and empirical formulae
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Question
An oxide of phosphorus contains 3.49 g of phosphorus and
4.51 g of oxygen. Calculate the empirical formula of this
phosphorus oxide.
Relative atomic masses:
O = 16 P = 31
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SC9a Relative formula masses and empirical formulae
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P O
Answer
Divide the mass of
each element by the Ar
Divide the answers by
the smallest number…
…to find the
simplest ratio
Simplest whole
number ratio
Empirical formula
= 0.113 = 0.282
= 1 = 2.5
2 5
P2O5
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SC9a Relative formula masses and empirical formulae
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Question
Calculate the relative formula mass of:
a zinc sulfate, ZnSO4
b iron(III) oxide, Fe2O3
c aluminium carbonate, Al2(CO3)3.
Relative atomic masses:
C = 12 S = 32
O = 16 Fe = 56
Al = 27 Zn = 65
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SC9a Relative formula masses and empirical formulae
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a Mr of ZnSO4 = Ar(Zn) + Ar(S) + 4 × Ar(O)
= 65 + 32 + (4 × 16)
= 161
b Mr of Fe2O3 = 2 × Ar(Fe) + 3 × Ar(O)
= (2 × 56) + (3 × 16)
= 160
c Mr of Al2(CO3)3 = 2 × Ar(Al) + 3 × Ar(C) + 9 × Ar(O)
= (2 × 27) + (3 × 12) + (9 × 16)
= 234
When part of a
formula is in a
bracket,
multiply
everything
inside the
bracket by the
number outside
Answer
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SC9a Masses and empirical formulae
Quick Quiz
9 Sodium chloride has the formula NaCl. The
relative atomic mass of sodium is 23 and that of
chlorine is 35.5. What is the relative formula
mass of NaCl?
58.5
10 A water molecule has the formula H2O. The
relative atomic mass of hydrogen is 1 and that of
oxygen is 16. What is the relative formula mass
of a molecule of water?
18
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• We calculate the empirical formula of a
compound by looking at the masses of
elements that react together to form the
compound.
• Analysis of 20.1g of iron bromide showed
that it contained 3.8g of iron and 16.3g of
bromine. What is its empirical formula?
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Fe : Br
Mass (g) 3.8 : 16.3
÷RAM 3.8 : 16.3
56 80
= 0.068 : 0.204
÷smaller 0.068 : 0.204
0.068 0.068
= 1 : 3
Empirical formula: FeBr3
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•
1 Calculate the empirical formula of the following
substances:
a water, if a sample contains 0.6 g of hydrogen
and 4.8 g of oxygen (H=1, O=16)
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H : O
Mass (g) 0.6 : 4.8
÷RAM 0.6 : 4.8
1 16
= 0.6 : 0.3
÷smaller 0.6 : 0.3
0.3 0.3
= 2 : 1
Empirical formula: H2O
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•
1 Calculate the empirical formula of the following
substances:
b lithium carbonate, if a sample contains 2.8 g of
lithium, 2.4 g of carbon and 9.6 g of oxygen
(Li=7,C=12, O=16)
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Li : C : O
Mass (g) 2.8 : 2.4 : 9.6
÷RAM 2.8 : 2.4 : 9.6
7 12 16
= 0.4 : 0.2 : 0.6
÷smaller 0.4 : 0.2 : 0.6
0.2 0.2 0.2
= 2 : 1 : 3
Empirical formula: Li2CO3