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CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Science
It is the knowledge that provides understanding of this world and how it works.
Chemistry
The branch of science that deals with the composition, structure, properties and
reactions of matter, is called chemistry.
Importance of chemistry in our daily life
1. We live in the world of chemicals.
2. We use many important chemicals daily such as drugs, detergents, paper,
paints, pigments, insecticides, pesticides and many petrochemical products.
3. Chemistry provides us knowledge and techniques which are used to improve
our health and environment.
4. Chemistry helps us to explore and conserve the natural resources.
5. On the other hand the development of chemical industry has certain
disadvantages also. For example it has generated toxic wastes, contaminated
water and polluted air around us.
HISTORICAL BACKGROUND OF KNOWLEDGE ABOUT MATTER
Greek philosophers
An ancient Greek philosopher, Empedocles thought that all the matter was
made up of only four elements:
1) Earth
2) Air 3) Water
4) Fire
The Greek concept of four elements existed for more than two thousand years.
Dalton’s Atomic Theory
In the beginning of 19th century Dalton proposed an atomic theory. According
to this theory matter is made up of small indivisible particles called atoms. The atoms
of any one element are identical in all respects but different from those of other
elements.
Modern picture of an atom
Modern research has clearly shown that atom is further composed of subatomic particles such as electron, proton and neutron.
Branches of Chemistry
Study of chemistry is divided into the following main branches.
1. Physical Chemistry
It is the study of the Laws and theories that describe the structure and
changes of matter.
CHEMISTRY: 9th
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BY: M. ZIA DOGAR
2. Organic Chemistry
It is the study of covalent compounds of carbon and hydrogen
(hydrocarbons) and their derivatives.
3. Inorganic chemistry
It deals with the study of all element and their compounds except organic
compounds.
4. Biochemistry
It is the study of physical and chemical changes that occur in living
organisms.
5. Industrial Chemistry
The branch of chemistry that deals with the manufacturing of chemical
substances on the commercial scale is called industrial chemistry.
6. Nuclear Chemistry
The study of changes that occur in atomic nuclei is called nuclear
chemistry.
7. Environmental Chemistry
It deals with the chemicals and toxic substances that pollute the
environment and their adverse effect on human beings.
8. Analytical Chemistry
It deals with the methods and instruments that determine the
composition of matter.
Differentiation between branches of Chemistry
Acetic acid chemical formula: CH3 COOH
Source: Vinegar which contain 5% acetic acid.
Smell: Vinegar like smell
Use: Used to flavour food.
Let’s see how various types of studies on this compound can help us to differentiate
between the above mentioned eight branches of chemistry.
1. Since acetic acid is a carbon compound, the study of its methods of
preparation and its chemical properties is a part of organic chemistry.
2. The study of all chemical reactions that acetic acid undergoes in the bodies of
human beings is called biochemistry.
3. The component elements of acetic acid are carbon, hydrogen and oxygen. The
study of this element is included in inorganic chemistry.
4. Use of technology and ways to obtain acetic acid on the large scale is done in
chemical industries, so it is a part of industrial chemistry.
5. Explanation of conversion of acetic acid from solid to liquid and liquid to
gaseous state and vice versa,
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
6. The application of laws and theories to understand its structure.
These two types of studies are a part of physical chemistry.
7. The methods and instruments used to determine its percentage composition
melting and boiling points etc are studies in analytical chemistry.
8. The study of any adverse effects of the compound or the compounds that are
derived from it, on the human is part of environmental chemistry.
9. The study of radioactive radiation or neutron on this compound is a part of
nuclear chemistry.
Identifying examples of different branches of chemistry
i.
ii.
iii.
iv.
v.
vi.
vii.
viii.
Photosynthesis produces glucose and oxygen from carbon dioxide and
water in presence of chlorophyll and sunlight.
Plantation helps in overcoming green house effect.
Haber’s process converts large quantities of hydrogen and nitrogen into
ammonia (NH3).
Ammonia is a colourless gas with pungent irritating odour. It is highly
soluble in water.
A chemist performed an experiment to check the percentage purity of a
sample of glucose (C6H1206).
An analyst determines that N02 is responsible for acid rain.
Chlorofluorocarbon compounds are responsible for the depletion of ozone
layer.
α-particles (He++) when bombard on nitrogen atom, a proton is emitted.
Solution
1. Biochemistry, since photosynthesis is a chemical reaction that occurs in plants
(living organism).
2. Environmental chemistry, since green house effect is an environmental
problem.
3. Industrial chemistry, since large scale production of any substance is the
subject of industrial chemistry.
4. Inorganic chemistry, since it deals with properties of inorganic compounds.
5. Analytical chemistry, since it deals with analysis of a compound, whether
organic or inorganic in nature.
6. Environmental chemistry, since acid rain is an environmental problem.
7. Environmental chemistry, since depletion of ozone layer is environmental
problem.
CHEMISTRY: 9th
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BY: M. ZIA DOGAR
8. Nuclear chemistry, since nuclear change can emit protons.
SELF ASSESSMENT EXERCISE 1.1
Identify the branch of chemistry that is related to the following information:
Hair contains a special class of proteins called keratins, which are present in
i.
nails and wool. .
Answer
Biochemistry
Acetylene is the simplest hydrocarbon that contains carbon - carbon triple
ii.
bond. Hydrocarbons are compounds of carbon and hydrogen.
Answer
Organic chemistry
White lead is a pigment used by artists for centuries, the metal Pb in the
iii.
compound is extracted from its ore, galena (PbS).
Answer
Inorganic chemistry
iv.
Sulphuric acid (H2SO4) is weaker than hydrochloric acid.
Answer
Inorganic chemistry
Gases can be compressed by applying pressure.
v.
Answer
Physical chemistry
Some examples of complete protein food are meat, milk and eggs.
vi.
Answer
Biochemistry
vii.
Element radium decays by emitting a-particles and is converted into another
element radon.
Answer
Nuclear Chemistry
8) Calorimeter is a device that measures the amount of heat, a substance absorbs on
heating or emits on cooling.
Answer
Physical chemistry
BASIC DEFINITIONS
Matter
Anything that has mass and occupies space is called matter.
Examples
Water, wood, air, paper, gold etc.
Classification of Matter
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
All materials are either a substance or a mixture. The following figure shows simple
classification of the matter into different forms.
Classification of Matter
Substance
It is a matter that has a particular set of characteristics which differ from the
character of any other kind of matter.
Examples
Oxygen, water, urea, glucose and common salt are different substances.
Element
The substance that cannot be converted into other simpler substances is called
an element.
Oxygen, hydrogen, Iron, copper and gold are few examples of elements.
Modern definition of Element
It is a substance made up of same type of atoms, having same atomic number.
Compound
A compound is a pure substance that is made up of two or more elements held
together in fixed ratios by natural forces called chemical bonds.
The properties of compounds are different from the properties of the elements from
which they are formed. Elements and compounds have uniformed composition
throughout.
Examples
Water, carbon dioxide, copper sulphate, sodium chloride etc. are compounds.
Mixture
An impure substance that contains two or more pure substances which retain
their individual chemical characteristics is called a mixture.
The entire world is made up of mixture of element and compound. A mixture can be
converted into two or more pure substances by a physical method.
Examples
Air, water containing dissolved oxygen, table salt dissolved in water, salt and
etc.. Types of Mixture
a) Homogenous Mixture
A mixture that consists of only one phase is called homogenous mixture.
Examples
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Salt or sugar dissolved in water, air etc Homogenous mixtures have uniformed
composition throughout.
b) Heterogeneous Mixture
A mixture that consists of two or more visibly different components is called
heterogeneous mixture.
Examples
Sand + Salt, oil floating on water, a class room etc.
DIFFERENCES BETWEEN A COMPOUND AND MIXTURE
The following are important differences between a compound and a mixture
Table Difference between a Compound and a Mixture
Compound
i.
ii.
iii.
iv.
' V.
vi.
vii.
Mixture
It is formed by a chemical
Mixture is formed by the simple mixing
combination of atoms of the
up of the substances.
The constituents lose their identity Mixture shows the properties of the
and from a new substance having constituents.
entirely different properties from
Mixtures do not have fixed composition.
Compounds always have fixed
composition by mass.
The components cannot be
The components can be separated by
separated by physical means.
simple physical methods.
Every compound is represented by a It consists of two or more components
chemical formula.
and does not have any chemical
Compounds have homogeneous
They may be homogeneous or
composition.
heterogeneous in composition
Compounds have sharp and fixed Mixture does not have sharp and fixed
melting points,
melting points.
Atomic Number
The number of protons in the nucleus of an atom is known as its atomic
number.
It is represented by symbol “Z”. As all atoms of an element have same
number of protons in their nucleus, they have same atomic number.
Examples
All hydrogen atoms have 1 proton, their atomic number is 1. Similarly all
atoms in carbon have 6 protons, their atomic number is 6.
Mass Number
The total number of protons and neutrons is an atom in known as its
mass number. It is represented by symbol ‘A’.
Examples
Hydrogen atom has one proton and no neutron in its nucleus hence its
mass number is 1. Carbon atom has 6 protons and 6 neutrons; hence its
mass number is 12.
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
The difference between the mass number and the atomic number is equal to the
number of neutrons in the nucleus
No of neutron = Mass number - Atomic number = A - Z
Example 1.2
Determining the number of protons and neutrons in an atom.
Atomic number of an element is 17 and mass number is 35. How many protons and
neutrons are in the nucleus of an atom of this element?
Solution
Number of protons = atomic number = 17
Number of neutrons = mass number - atomic number
= 35-17 = 18
Relative atomic mass
An atom is extremely small particle, therefore we cannot determine the mass of a
single atom. However it is possible to determine the mass of one atom of an element
relative to another experimentally. The light isotope of carbon (C-12) has been
chosen as a standard, with reference to which atomic masses of all other elements
can be determined
Thus
“The mass of an atom of an element relative to the mass of an atom of C-12 is called
relative atomic mass”
a. Atomic Mass Unit (amu)
One atomic mass unit is one-twelfth the mass of one atom of carbon-12
Mass of one C-12 atom =12 amu
1 amu =
Examples
An atom of Hydrogen is 8.4% as massive as C-12. Therefore relative atomic mass of
.
12
= 1.008 amu
Similarly, relative atomic masses of oxygen and sodium are 15.9994 amu and
22.9898 amu respectively.
Chemical Formula
Compounds are represented by chemical formulas. A chemical formula tells us:
 Which elements are present in a compound?
 The whole number ratio of their atoms thus a chemical formula shows the type
and the number of each atom in a compound.
Types of chemical formulas.
There are several types of chemical formulas but two important types are:
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
1. Empirical Formula
2. Molecular Formula
Empirical Formula
It gives the simplest whole number ratio of atoms present in a compound
Examples
The covalent compound hydrogen peroxide has simplest ratio of 1:1 of hydrogen to
oxygen. Therefore, its empirical formula is HO. Similarly the simplest ratio between C,
H and O atoms in glucose is 1:2:1. Hence its empirical formula is CH2O
Molecular Formula
It gives the actual whole number ratio of atoms of each element present in a
molecule of that compound.
Examples
The actual ratio of hydrogen to oxygen atoms in a molecule of hydrogen peroxide is
2:2. Hence its molecular formula is H2O2
The actual ratio between C, H and O atoms in a glucose molecule is 6:12:6, so its
molecular formula is C6H12O6
What is the relationship between empirical and molecular formula
We know that molecular formula of a compound may be some as its
empirical formula e.g. H2O CO2, HCl, CH4, CCI4, NH3, HBr, PCl3, H2S04 etc.
Molecular formula may be obtained by multiplying empirical formula with number ‘n’
Molecular Formula = n x Empirical formula = (Empirical formula)n
Where n is 1, 2, 3 and so on.
For example, molecular formula of benzene is C6H6 which is derived from the
empirical formula CH where the value of n is 6. The following Table shows some
compounds with their empirical and molecular formulas.
The Empirical Formulae of Some of the Compounds
No. Molecular formula
Empirical formula
Ethene(C2H6)
1.
2. Ethene (C2H4)
CH3
3. Diborane (B2H6)
BH3
4. Nitrogen tetraoxide (N2O4)
NO2
5. Water (H20)
6. Sodium carbonate
(Na2CO3)
7. Hydrogen Peroxide H2O2
SELF ASSESSMENT EXERCISE 1.2
CH2
H2O
Na2CO3
HO
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Write the empirical formulas for the compound containing carbon to hydrogen in the
following ratios.
a)
1:4
b) 2:6
c) 2:2
d) 6:6
Answer
a) CH4
b) CH3
c) CH
d) CH
For many compounds, empirical and molecular formulas are same. For example
water (H2O), carbon dioxide (CO2), ammonia (NH3), methane (CH4), sulphur dioxide
(SO2) etc. Can you show it why?
Answer
The molecules of these compounds contain atoms in their simplest ratios.
SELF ASSESSMENT EXERCISE 1.3
1. Aspirin is used as a mild pain killer. There are nine carbon atoms, eight
hydrogen atoms and four oxygen atoms, in this compound. Write its
empirical and molecular formulas.
Answer
The empirical and molecular formula is same i.e. C9 H8 O4
2. Vinegar is 5% acetic acid. This contains 2 carbon atoms, 4 hydrogen atoms
and 2 oxygen atoms. Write its empirical and molecular formulas.
Answer
Molecular formula: C2 H4 O2
Empirical Formula: CH2O
3. Caffeine (C8H5N402) is found in tea And coffee. Write the empirical formula
for caffeine.
Answer
Empirical formula: C4H5N2O
What do you understand by the terms Molecular Mass and Formula mass? How
these masses can be determined?
Molecular Mass
It is the sum of atomic masses of all the atoms present in the molecule.
Example
Molecular mass of water (H2O) =
= 2 (atomic mass of H) + atomic mass
oxygen
= 2(1) + 16= 18 amu
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
PROBLEMS:
1. Determine the molecular mass of glucose, C6H206, which is also known as blood
sugar.
2. Determine the molecular mass of naphthalene C10H8, which is used in
mothballs.
Solution
Molecular mass of C6H12O6 =
= 6(12.00) + 12(1.008) + 6(16.00)
= 180.096 amu
Molecular mass of CI0H8 =
=1 2 x 1 0 + 1 x 8
= 120 + 8 = 128 amu
2) Formula Mass
The term formula mass is used for ionic substances. Ionic compounds consist
of oppositely charged ions rather than separate molecules. So we represent an ionic
compound by its formula unit.
Formula Unit
It indicates the simplest ratio between cations and anions in an ionic
compound. Example
The common salt consists of Na+ and Cl¯ ions. It has one Na+ ion for every Cl¯
ion. So formula unit for common salt is NaCl.
Formula Mass
The sum of the atomic masses of all the atoms in the formula unit of a
substance is called formula mass.
Examples
Formula mass of sodium chloride is 58.5 amu and that of CaC03 is 100 amu.
How to determine the formula mass?
Example 1.4
Determining formula mass
 Sodium Chloride, also called table salt is used to flavour food, preserve meat,
and in the preparation of large number of compounds. Determine its formula
mass.
 Milk of magnesia which contains Mg (OH) 2 is used to treat acidity. Determine
its formula mass.
Problem solving strategy
Add the atomic masses of all the atoms in the formula unit.
Solution
Formula mass of NaCl = 1 x Atomic mass of Na +1 x Atomic mass of Cl
= 1 x 23 + 1 x 35.5 = 58.5 amu
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Formula mass of Mg (OH) 2 = 2 4 + 1 6x 2 + 1 x 2
= 2 4 + 3 2 + 2 = 5 8 a mu
1. SELF ASSESSMENT EXERCISE 1.4
2. Potassium Chlorate (KCIO3) is used commonly for the laboratory preparation
of 0 gas. Calculate its formula mass.
Formula Mass of KCIO3 = 39 + 35.5 + 3 (16)
= 122.5 amu
3. When baking soda, NaHCO3 is heated it releases carbon dioxide, which is
responsible for the rising of cookies and bread. Determine the formula
masses of baking soda and carbon dioxide.
Answer
Formula Mass of NaHCO3 = 23 + 1 + 12 + 3(16)
= 84 amu
Formula Mass of CO2
= 12 + 2(16)
= 44 amu
4. Following compounds are used as fertilizers. Determine their formula
masses.
Urea, (NH2)2CO, Ammonium nitrate, NH4NO3
Answer
Formula Mass of Urea = 2(14) + 4(1) + 12 + 16
= 60 amu
Formula Mass of NH4NO3 = 14 + 4+ 14 + 3 (16)
= 80 amu
Chemical species
Matter is composed of chemical species. These species are atoms, ions, free
radicals, molecules and formula units.
Atom
Atom is the smallest particle of an element that cannot exist in Free State it is
electrically neutral.
Ion
Ion is an atom or group of atoms having a charge on it.
Types of ions
There are two types of ions.
1) Cations 2) Anions
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
1) Cations
An atom or group of atoms having positive charge on it is called cation. Metal atoms
generally lose one or more electrons and form cations.
Examples
Na form Na+ by losing one electron, Ca forms Ca2+ by losing two electrons.
2) Anions
An atom or group of atoms having negative charge on it is called anion. Non-metals
usually gain one are more electrons and form anions.
Examples
Chlorine atom gains one electron and forms Cl¯ ion, O atom gains two electrons and
form O2- ion.
why an ion acquires a net positive or negative charge.
Anion acquires a net positive or negative charge due to difference in number of
protons and electrons in it.
For example chlorine atom gains one electron and forms Cl¯ ion, O-atom gains two
electrons and forms O2- ion.
Let us understand why an ion acquires a net positive or negative charge. Consider the
formation of Na+ ion.
Note that sodium has a nucleus of 11 protons and 12 neutrons. Thus its nucleus has a
total charge of+11. Around the nucleus, in the ion are 10 electrons, with a total
charge of-10. The charge on the ion is + 11 + (-10) = +1
SELF ASSESSMENT EXERCISE 1.5
Explain Why?
1. An oxide ion has -2 charge.
Answer
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
An oxide ion has a nucleus of 8 protons and 8 neutrons. Around the nucleus, there
are 10 electrons in oxide ion.
8 protons has charge = +8
10 electrons has charge = -10
Net charge on the ion = -2
2. Magnesium ion, Mg+2 has +2 charge.
Answer
12 protons has charge =
+12
10 electron
=
-10
Net charge on the ion =
+2
-2
3. Sulphide ion, S has -2 charge.
Answer
16 protons has charge = +16
18 electron has charge = -18
Net charge on the ion = -2
MOLECULAR IONS
When a molecule loses or gains electrons, the resulting species is called a molecular
ion.
These ions are short lived species and only exist at high temperature. Molecular ions
do not form ionic compounds.
Examples
 When O2 loses an electron it forms O⁺2 ion, but when it absorbs an electron it
forms O2¯ ion. These ions are called molecular ions.
 Similarly N2¯and N2⁺ are examples of molecular ions of N2 gas.
Difference between Molecule and Molecular Ion
No.
Molecule
Molecular Ion
i)
It is the smallest particle of an
element or compound which can
ii)
It is always neutral.
It is formed by gain or loss of
electron by a molecule.
It can have negative or positive
charge.
iii)
*
It is formed by the combination of
atoms.
It is formed by the ionization of
molecule.
iv)
It is a stable unit.
It is reactive specie.
FREE RADICALS
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Free radicals are atoms or group of atoms having odd number of (unpaired)
electron. Free radicals are electrically neutral species.
Some substances like halogens when exposed to sun light, their molecules split up
into free radicals. They are represented by putting a dot over the symbol of an
element.
Examples
Cl°, H°, H3C° are examples of free radicals.
Differences between Ion and free radicals
No.
i)
ii)
iii)
Ion
Free Radical
An atom or group of atoms having An atom or group of atoms having
charge
unpaired electrons
They exist in solution or in crystal They exist in solution as well as in
air.
lattice.
Ion cannot be produced with the
Light may produce free radicals.
help of light.
SELF ASSESSMENT EXERCISE 1.6
Identify ions, molecular ions and free radicals from the following species.
CN‾,CN,He+2, Ӧ, N
Answer
1. Ions: N-3
2. Molecular ions: He+2 , CN‾
3. Free radicals: N, O , CN
Representative particles of an element or compound
The representative particles of a substance are atoms, molecules or formula units.
The following example helps us to identify the particles of elements and compounds.
Molecule
Smallest particle of a covalent compound or an element which can exist
independently is called molecule.
Types of Molecules Molecules can be classified as:
i) Monoatomic
ii) Polyatomic
Monatomic
A molecule that contains only one atom is called monoatomic molecule.
Examples
Inert gases consist of monoatomic molecules such as He, Ne, Ar, Kr and Rn.
Polyatomic Molecules
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
A molecule that contains two or more similar or different atoms called polyatomic is
molecule.
Examples
 H2, O2, N2, CI2, S8 etc are polyatomic molecules of different elements.
 H2O, HBr, HCI, NH3, H2SO4 etc are polyatomic molecules of different
compounds.
AVOGADRO’S NUMBER AND MOLE
Avogardro’s Number
The number of atoms, ions or molecules present in one mole of a substance is called
Avogadro’s number. It is denoted by NA and is equal to 6.02 x 1023.
Relation between mole and Avogadro’s number.
1 mole of any substance = Avogadro’s number = 6.02 x 1023
Examples
 6.02 x 1023 atoms of carbon are equivalent to one mole of carbon.
 6.02 x 1023 molecules of water are equivalent to one mole of water.
 6.02 x 1023 formula units of NaCl are equivalent to one mole of sodium
chloride.
Thus 6.02 x 1023 atoms of an element or 6.02 x 10 molecules of a molecular
compound or 6.02 x 1023 formula units of an ionic compound are equivalent to one
mole.
Molar Mass
The mass of one mole of a substance is called its molar mass.
Mole
The atomic mass, molecular mass or formula mass expressed in grams is called mole.
Gram Atomic Mass
Atomic mass of an element expressed in grams is called gram atomic mass. It is also
called a mole or a gram atom.
Examples
1 g-atom of hydrogen = 1.00 g = 1 mol of hydrogen.
i)
1 g-atom of carbon = 12g = 1 mol of carbon.
ii)
It shows that 1-gram atom of different elements has different masses.
Gram Molecular Mass
Molecular mass of an element or a compound expressed in grams is called gram
molecular mass. It is also called a mole or a gram molecule.
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Examples
i)
1 g-molecule of H2 = 2g = 1 mol of hydrogen
ii)
1 g-molecule of H2O - 18 g = 1 mol of water.
iii)
1 g - molecule of C6H1206 = 180 g = 1 mol of glucose.
Gram Formula Mass
Formula mass of an ionic compound expressed in grams is called gram molecular
mass or gram molecule. It is also called a mole.
Examples
i.
1 g - formula NaCl - 58.5 g= 1 mol of NaCl.
ii.
1 g - formula of KC1 = 74.5 amu = 1 mol of KC1.
iii.
Differences between the terms gram atomic mass, gram molecular mass and gram
formula mass.
Gram atomic mass represents one mole of atom of an element, gram
molecular mass represents one mole of molecules of a compound or an
element that exists'in molecular state whereas gram formula mass represents
one mole of an ionic compound.
Gram atomic mass contains 6.022 x 1023 atoms, gram molecular mass contains
6.022 x 102j molecules whereas gram formula mass contain 6.022 x 1023
formula units.
 All of these quantities represent molar mass. Mass of one mole of a substance
expressed in gram is called molar mass,
“Therefore, mole can be defined as atomic mass, molecular mass or formula
mass expressed in grams
CHEMICAL CALCULATIONS
In chemical calculations we apply the concept of mole and Avogadro’s number. We
can study these calculations under the following headings.
1) Mole - Mass calculations
2) Mole- particles calculations
Let us learn about these two types of calculations with the help of few examples.
Mole - Mass Calculations
Example 1.5
Calculating mass of one mole of a substance
Calculate the molar masses of (a) Na (b) Nitrogen (c) Surcose C12H22O11.
Problem solving strategy
If an element is a metal then its molar mass is its atomic mass expressed in grams
(gram atomic mass). If an element exists as molecule, its molar mass is its molecular
mass expressed in grams (gram molecular mass).
1)
l mole of Na = 23g
Nitrogen occurs as diatomic molecules.
2)
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Molecular mass of N2 = 1 4 x 2 =28amu
Therefore, mass of 1 mole of N2 = 28 g
c) Its molecular mass expressed in grams.
Molecular mass of C12H22O11 = 1 2 x 1 2 + 1 x 2 2 + 1 6 x 1 1
= 144 + 22+ 176
=342 g
Therefore, mass of 1 mole of sucrose = 342g
SELF ASSESSMENT EXERCISE 1.8
Calculate the mass of one mole of (a) Copper (b) Iodine (c) Potassium (d) Oxygen.
Answer
a. mole of Cu = 63.5 g
b. Iodine exist as diatomic molecule
(mole of I-atom = 127 g)
1 mo le o f l 2 = 2 x 1 2 7
= 254 g
c. 1 mole of k = 39 g
d. oxygen exist as diatomic molecule
16)
1 mo le o f O2 = 2 x 1 6
= 32g
(1 mole of O-atom =
EXAMPLE 15 (a)Calculating the mass of a given number of moles of a substance
Oxygen is converted to ozone (03) during thunder storms. Calculate the mass of
ozone if 9.05 moles of ozone is formed in a storm?
Problem solving strategy
Ozone is a molecular substance. Determine its molar mass and use it to convert
moles to mass in grams.
9.05 moles of 03
g of 03
Solution
1 mole of O3 = 16 x 3 = 48 g
1 mole of O3 = 48 g
So,
9.05 moles of O3 = 48 g x 9.05 = 434.4g of 03
Example 1.6
When natural gas burns CO2 is formed. If 0.25 moles of CO2 is formed, what mass of
CO2 g is produced?
Problem solving strategy
Carbon dioxide is a molecular substance. Determine its molar mass and use it to
convert moles to mass in grams.
CHEMISTRY: 9th
CHAPTER:01
0.25 moles of CO2
BY: M. ZIA DOGAR
? g of C02
Solution
So,
Molar mass of CO2 = 12 + 2x 1 6 = 44g
1 mole of CO2 = 44g of C O2
0.25 moles of CO2 = 44 x 0.25 = 1 1 g o f C O 2
Example 1.7
Converting grams to moles
How many moles of each of the following substance are present?
a)
A balloon filled with 5g of hydrogen.
b)
A block of ice that weighs 100g.
Problem solving strategy
Hydrogen and ice both are molecular substances. Determine their molar masses. Use
the molar mass of each to convert masses in grams to moles.
mass
?moles
Solution
a)
Mass of H2
Molar mass of H2
1 mole of H2
2.016 g of H2
Number of moles
=
=
=
=
=
=
=
5g
1.008 x 2 = 2.016g
2.016g
1 mole of H2
.
2.48 moles of H2
b)
Mass of H2O
=
Molar mass of H2O =
=
=
Number of moles =
=
=
SELF ASSESSMENT EXERCISE 1.9
100 g
2 x 1.008+ 16
2.016+ 16
18.016 g
.
5.55 moles of H2O
1) The molecular formula of a compound used for bleaching hair is H2O2. Calculate
a) Mass of this compound that would contain 2.5 moles, (b) No. of moles of this
compound that would exactly weigh 30 g.
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Answer
a)
Molar mass of H2O2 = 2 + 2(16)
= 34g /mol
1 mole of H2O2
= 34 g
Mass of H2O2
= molar mass of H2O2 x No. of moles
Mass of H2O2
= 34 x 2.5 = 85g
b)
mass of H2O2
=
molar mass of H2O2 =
Number of moles =
30 g
34 g/ mol
2
2
2
2
=
= 0.88 mol
2)
A spoon of table salt, NaCl contains 12.5 grams of this salt. Calculate the
number of moles it contains.
Answer
Mass of NaCl
=
12.5 g
Molar mass of NaCl = 23 + 35.5 =58.5 g
molar mass of H2O2 =
34 g/ mol
Number of moles =
=
=
viii.
.
.
0.21 mol
Before the digestive systems X-rayed, people are required to swallow
suspensions of barium sulphate (BaSO4). Calculate mass of one mole of BaSO4.
Answer
Molar mass of BaSO4 = 137 + 32 + 4(16) = 233g
Mole - Particles calculations
Example 1.8
Calculating number of atoms in given moles
1) Zn is a silvery metal that is used to galvanize steel to prevent corrosion. How
many atoms are there in 1.25 moles of Zn?
3)
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
2) A thin foil of Aluminum (Al) is used as wrapper in food industries. How many
atoms are present in a foil that contains 0.2 moles of Aluminium?
Problem solving strategy
Remember that symbols Zn and Al stand for one mole of Zn and Al atoms
respectively.
Solution
1)
1 mole of Zn contains 6.022 x 1023 atoms
Number of atoms = No. of moles x Avogadro number
= 1.25 x 6.022 x 1023
= 7.53 x 1023 Zn atoms
2)
1 mole of Al contains 6.022 x 1023 atoms
Number of atoms = No. of moles x Avogadro number
= 6.022 x 1023 x 0.2
= 1.2044 x 1023 atoms.
Example 1.9
Calculating number of molecules in given moles of a substance
1) Methane (CH4) is the major component of natural gas. How many molecules are
present in 0.5 moles of a pure sample of methane?
2) At high temperature hydrogen sulphide (H2S) given off by a volcano is oxidized by
air to sulphur dioxide (SO2). Sulphur dioxide reacts with water to form acid rain. How
many molecules are there in 0.25 moles of SO2?
Solution
1.
1 mole of CH4 contains = 6.022 x 1023 molecules
Number of moles
=
0.5 moles
Number of molecules
=
?
Number of molecules
= Avogadro number x No. of molecules
= 6.022 x JO23 x 0.5
= 3.011 x 1023 molecules
2.
1 mole of SO2 contains = 6.022 x 1023 molecules
Number of moles
=
0.25 moles
Number of molecules
=
?
Number of molecules
= Avogadro number x No. of molecules
= 6.022 x 1023 x 0.25
= 1. 5055 x 1023 molecules
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
Example 1.10
Calculating number of moles in the given number of atoms
Titanium is corrosion resistant metal that is used in rockets, aircrafts and jet engines.
Calculate the number of moles of this metal in a sample containing 3.011 x 1023 Tiatoms.
Remember
1 mole of an element contains 6.022 x 1023 atoms.
Number of atoms =3.011 x 1023
Number of moles =?
No. of moles
=
.
23
.
23
=
23
.
= 0.5 moles of Ti
Calculating number of moles in the given number of molecules
Formaldehyde is used to preserve dead animals. Its molecular formula is CH2O.
Calculate the number of moles that would contain 3.011 x 1022 molecules of this
compound.
 Remember that 1 mole of any compound contains 6.022 x 1023 molecules.
Number of HCHO molecules =3.011 x 1023
Number of moles =?
No. of moles
=
23
.
.
22
=
23
.
= 0.05 moles of HCHO(formaldehyde)
SELF ASSESSMENT EXERCISE 1.10
1. Aspirin is a compound that contains carbon, hydrogen and oxygen. It is used
as a pain killer. An aspirin tablet contains 1.25 x 1030 molecules. How many
moles of this compound are present in the tablet?
Answer
Molar mass of Aspirin (C9H8O4) = 9(12) +8 + 4(16)
= 180 g
No. of moles
=
.
=
23
.
.
30
23
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
=0.2 x 107
=
2 x 106mol
2)
A method used to prevent rusting in ships and underground pipelines
involves connecting the iron to a block of a more active metal such as magnesium.
This method is called cathodic protection. How many moles of magnesium are
present in 1 billion (1 x 109) atoms of magnesium?
Answer
Number of atoms = 109
No. of moles
=
.
23
9
= .
23
= 1.66x 10-15 mol
EXERCISE
i.
vi.
d
b
ii.
vii.
d
a
iii.
viii.
c
b
iv
ix.
d
d
v.
x.
b
b
Q 2.
ii.
What do you know about Corpuscular nature of matter?
Answer
According to this concept matter is supposed to be composed of minute particles. An
ancient Greek philosopher, Empedocles thought that all materials were made up of
four things called elements:
1) Earth
2) Air 3) Water
4) Fire
Many successors of Empedocles like Plato and Aristotle adopted this concept of four
elements. This concept of four elements existed for more than two thousand years.
vi.
What is the number of molecules in 9.0g of steam?
Answer
Molar mass of H2O = 1 x 2 + I 6 = 1 8 g
Mass of H2O =
9.0 g
Number of molecules= ?
Number of molecules=
6.022 x 1023
CHEMISTRY: 9th
CHAPTER:01
=
.
BY: M. ZIA DOGAR
6.022 x 1023
=3.01x1023 molecules
vii) What are the molar masses of Uranium 238 and Uranium - 235?
Answer
Atomic mass of U-238 = 328 amu
molar mass of U-238 = 238 g
Atomic mass of U-235 = 235amu
molar mass of U-23 5 = 235g
viii) Why one mole of hydrogen molecules and one mole of H-atoms have different
masses?
Answer
 Atomic mass of H = 1amu
1 mole of H = lg
 Molecular mass of H2 = lx2 = 2amu
1 mole of H2 = 2g
Because molecular mass of H2 is twice to atomic mass of H, therefore the molar mass
of H2 is two times to the molar mass of hydrogen atom.
Q.4: a) What are the differences between Atom and Ion?
Answer
a) Differences between Atom and Ion
No
Atom
No
Ion
i)
The smallest particle of an
element is atom.
It may or may not have
independent existence
0
The smallest unit of an ionic substance
is ion.
It cannot exist independently and is
surrounded by oppositely charged ions.
It has either positive or negative charge
on it.
ii)
ii)
iii)
Atom is a neutral particle.
iii)
No
Molecular ion
No
Free Radical
i)
It is an atom or group of atoms having
an unpaired electron.
ii)
It is electrically neutral.
iii)
These have great tendency to
complete their octets by gaining or
losing electrons.
b)
i)
ii)
iii)
When a molecule loses or
gains electron, molecular ion
is formed.
It has a positive or negative
charge on it.
Molecular ions do not form
ionic compounds.
CHEMISTRY: 9th
iv)
CHAPTER:01
Examples
CH 4 + , He +
iv)
BY: M. ZIA DOGAR
Examples H°, Cl°, H3C° etc.
Q.6: Calculate the number of moles of each substance in samples with the following
masses?
a. 2.4 g of He
mass of He =
2.4 g
Molar mass of He = 4g
4g of He = 1mol
Number of moles of He= 2.4/4
= 0.6 mol
b. 250 mg of Carbon
Molar mass of carbon = 12 g
Mass of carbon
= 250 mg = 250/1000 = 0.25 g
Number of moles =0.25/12 m= 0.02 mol
c. 15g of Sodium Chloride
Molar mass of Sodium Chloride =
23 + 35.5
=
58.5g
Mass of NaCl
=
15/58.5
=
0.25 mol
d. 40 g Sulphur
Mass of sulphur
=
40 g
Molar mass of S
=
32 g
Number of moles =
=
40/32
=
1.25 mol
e. 1.5 Kg of MgO
Mass of MgO
= 1.5 Kg
=1.5x1000 = 1500 g
Molar mass of MgO
=
40 g
Number of moles
=
1500/40
=
3.5 mol
Q.7: Calculate the mass in grams of the following samples?
a. 1.2 moles of K
Molar mass of K = 39g
Number of moles= 1.2 mol
Mass of K = 39x 1.2 = 46.8g
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
b. 75 moles of H2
Molar mass of H2 = 2g
Moles of H2
= 75 mol
Mass of H2 = 2x75 = 150g
c. 0.25 moles of Steam
Molar mass of Steam(H20) = 2 + 16 = 18g
mol of steam = 0.25 mol
mass of steam
= 0.25x 18
=4.5g
d. 1.05 moles of CuSO4.5H2O
Molar mass of CuSO4.5H2O=
= 64 + 32 + 4(16)+ 5 (18)
= 64 + 32 + 64 + 90 - 250.g
Moles of CuSO4.5H2O
= 1.05 mol
Mass of CuSO4.5H2O
=250 x 1.05 = 262.5g
e. 0.15 moles of H2S04
Molar mass of H2SO4 = 2 + 32 + 64
=
98g
Number of moles of H2SO4
=
0.15 mol
Mass of H2SO4
= 98x0.15= 14.7g
Q.8: Calculate the number of molecules present in each of the following samples?
a. 2.5 moles of Carbon dioxide
1 mole of CO2 = 6.02 x 1023 molecules
2.5 moles of C02 = 6.02x 1023x2.5
= 1.5x1024 molecules
b. 3.4 moles of ammonia, NH3
1 mole of NH3 = 6.02 x 1023 molecules
3.4 moles ofNH3 = 6.02x 1023x 3.4 = 2 x 1024
c. 1.09 moles of benzene, C6H6
=
6.02 x 1023 molecules
=
6.02 x 1023x 1.09
=
6.56 x 1023 molecules
d. 0.01 moles of acetic acid, CH3COOH
1 mol ofC6H6
1.09 mol of C6H6
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
1 molofCH3COOH = 6.02 x 1023 molecules
0.01 molofCH3COOH = 6.02 x 1023x 0.01
= 6.0 x 1021 molecules
Q.9: Decide whether or not each of the following is an example of empirical
formula:
a) Al2CI6b) Hg2Cl2 c) NaCl d) C2H6O
a. A12CI6
It is a molecular formula. Its empirical formula is AICI3.
b. Hg2Cl2
It is molecular formula & Empirical Formula = HgCl
c. NaCl
Yes. It is example of an empirical formula.
d. C6H6O
Yes. It is example of an empirical formula.
Q.10: TNT or trinitrotoluene is an explosive compound used in bombs. It contains 7
C-atoms, 6 H-atoms, 5 N-atoms and 6 O-atoms. Write its empirical formula?
Molecular formula of TNT = C7H6N5O6
Empirical formula of TNT = C7H6N506
Q.11: A molecule contains four phosphorus atoms and ten oxygen atoms. Write the
empirical formula of this compound. Also determine the molar mass of this
molecule?
Molecular formula of the compound = P4O10
Empirical formula of the compound = P2O5
Molar Mass of P4O10 = 4(31) + 10(16) = 284
Q.12: Indigo (C16H10N2O2), the dye used to colour blue jeans is derived from a
compound known as indoxyl (C8H7ON). Calculate the molar masses of these
compounds. Also write their empirical formulas?
Molar mass of C16H10N2O2= 16(12) + 10 +2 (14) + 2 (16)
= 262g
Empirical formula of indigo= C8H5NO
Molar mass of indoxyl C8H7ON = 8(12) + 7 + 1 6 + 1 4
= 133g
Empirical formula of indoxyl = G8H7ON
Q.13: Identify the substance that has formula mass of 133.5amu?
a) MgCl2 b) S2CI2 c) BCI3 d) AlCl3
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
AICI3 is the substance having formula mass of 133.5 amu.
Formula mass of A1C13 = 27+3 (35.5) = 133.5 amu
Q.14: Calculate the number of atoms in each of the following samples?
a. 3.4 moles of nitrogen atoms
1 mole of Nitrogen atoms = 6.02 x 1023
3.4 mole of Nitrogen atoms = 6.02 x 1023x 3.4
= 2xl024 atoms
b. 23g of Na
23g of Na = 1 mole
1 mole of Na contain = 6.02x 1023 atoms
c. 5g of H atoms
Mass of H atoms = 5 g
Molar mass of H = 1 g
Number of H-atoms =
6.02 x 1023
=
6.02 x 1023
=
=
5x6.02xl023
3 x 1024 atoms
Q.15: Calculate the mass of the following
a. 3.24 x 1018 atoms of iron
Number of atoms = 3.24 x 1018
Molar mass of iron= 56 g
Mass of iron =
.
23
56 x 3.24 x 1018
b. 2x1010
=
23
.
= 30 x 10l8 - 23 = 3x 10-4g
molecules of nitrogen gas
Number of molecules = 2x1010
Molar mass of nitrogen gas = 28 g
Mass of nitrogen =
=
28 x 2x1010
6.02 x 1023
=9.3 x 10 -3 g
.
23
CHEMISTRY: 9th
CHAPTER:01
BY: M. ZIA DOGAR
c. 1 x 1025 molecules of water
Molecules of water = 1 x 1025
Molar mass of water = 18 g/mol
Mass of water =
.
23
1025
=
23
.
2
= 3 x 10 g
d. 3 x 106 atoms of Al
Molecules of Al= 3 x 106
Molar mass of Al= 27 g/mol
Mass of Al =
27x 3 x 106
.
23
=
23
.
= 1.34x 1016g
Q.16: Identify the branch of chemistry that deals with the following examples:
1) A cornstalk grows from a seed.
2) Dynamite (C3H5N3O9) explodes to form a mixture of gases.
3) Purple iodine vapour appears when solid iodine is warmed.
4) Gasoline (a mixture of hydrocarbons) fumes are ignited in an auto mobile
engine.
5) A silver article tarnishes in air.
6) Ice floats on water.
7) Sulphur dioxide is the major source of acid rain.
8) Many other light chlorinated hydrocarbons in drinking water are carcinogens.
9) In Pakistan most of the factories use wet process for the production of cement.
10)
Carbon-14 is continuously produced in the atmosphere when high
energy neutrons from space collide with nitrogen-14.
Answers
1. Biochemistry
2. Analytical chemistry
3. Environmental chemistry
4. Environmental chemistry
5. Industrial chemistry
6. Inorganic chemistry
7. Organic chemistry
8. Physical chemistry
9. Environmental chemistry
10.Nuclear chemistry