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Download 9th Class Chemistry Notes (Unit # 1) for Federal Board (FBISE) Islamabad

Download 9th Class Chemistry Notes (Unit # 1) for Federal Board (FBISE) Islamabad

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Download 9th Class Chemistry Notes (Unit # 1) for Federal Board (FBISE) Islamabad

REVIEW QUESTIONS

[Very Important] Differentiate between anion and a free radical.
Anion: -
·        lon is a charged species formed from an atom by adding or removing electrons.
·        Positively charged ions are called cations.
·        Negatively charged ions are called anions.
·        For example Na forms Na+ by losing one electron and chlorine atom gains one electron and forms CI- ion.
Free radicals:
A free radical is an atom, which has an Un-paired electron and bears no electrical charge. For example:
 
When substances like halogens are exposed to sun light, their molecules split up into free radicals.

[Important] What do you know about corpuscular nature of matter?
Empedocles concept:
An ancient Greek philosopher, Empedocles thought that all materials are made up of four things called elements. i.e. Earth, Air, Water and Fire
Plato concept:
Plato adopted Empedocles theory and evolves the term element to describe these four substances.
Aristotle concept:
Aristotle also adopted the concept of four elements. He introduced the idea that elements can be differentiated on the basis of properties such as hot versus cold and wet versus dry.
The Greek concept of four elements existed for more than 2000 years.

[Important] Differentiate between analytical chemistry and environmental chemistry.
Analytical Chemistry:
The branch of Chemistry that deals with the methods and instruments for determining the composition of matter is called Analytical Chemistry.
Environmental Chemistry:
The branch of Chemistry that deals with the chemicals and toxic substances that pollute the environment and their adverse effects on human beings is called environmental chemistry.

[Very Important] What is mole and Avogadro Number?
·        The amount of matter that contains as many atoms, ions or molecules as the number of atoms in exactly 12g of C-12 is called mole.
·        Mole can also be defined as atomic mass, molecular mass or formula mass expressed in grams.
Mass in grams
Number of moles of a substance    =      ------------------
                                                        Molecular Mass
·        A mole is an amount of a substance that contains 6.02 x 1023 particles of that substance. This experimentally determined number is known as Avogadro number.
·        The symbol of mole is “mol”.

Example:
For example a mole of carbon is 6.02 x 1023 atoms. A mole of sulphur is 6.02 x 1023 atoms. A mole of water is 6.02 x 1O23 molecules

[Very Important] Differentiate between empirical formula and molecular formula.
Empirical Formula:
  • The empirical formula of a compound is the chemical formula that gives the whole number ratio of atoms of each element.
  • It represents the simple whole number ratio of atoms of elements in compound.
  • It is used for both molecular and ionic compounds.
  • CH2O and CH are empirical formulae of glucose and benzene.
Molecular Formula:
  • A molecular formula gives the actual whole number ratio of atoms of each element present in a compound.
  • A formula which represents actual number of atoms of elements in compound.
  • It is used for molecular compounds.
  • C6H12O6 and C6H6 are empirical formulae of glucose and benzene.

Question: What is the number of molecules in 9.0 g of steam?
Mass in grams                    =      9 g

Molar mass of steam (H2O)   =      (2x1) + (1x16)    =      18 g

                                                Mass in Grams
Number of Molecules            =      ----------------- x NA
                                                Molar Mass

                                                9
Number of Molecules            =      --- x 6.022 x 1023
                                                18

Number of Molecules            =      0.5 x 6.022 x 1023

Number of Molecules            =      3.011 x 1023  Molecules

Question: What are the molar masses of uranium-238 and uranium-235?
Molar mass of uranium -238 = Atomic mass of Uranium -238 = 238 g
Molar mass of uranium -235 = Atomic mass of Uranium -235 = 235 g

Question: Why one mole of hydrogen molecules and one mole of H-atoms have different masses?
One-mole quantities of two different substances have different masses for the same reason - the substances have different compositions.
If we put one mole of hydrogen molecules and one mole of H-atoms on separate balances, we would see a difference in mass, just as you do for the eggs and the limes. This occurs because hydrogen molecules differ from H-atoms. Thus, the mass of 6.02 x 1023 hydrogen molecules does not equal to the mass of 6.02 x 1023 H-atoms.

1mole of H-atom = 1g, 1 mole of H2 = 1x2 = 2g)

[Important] Define ion, molecular ion, formula unit, free radical, atomic number, mass number, atomic mass unit.
Ion:
·        lon is a charged species formed from an atom by adding or removing electrons.
·        Positively charged ions are called cations.
·        Negatively charged ions are called anions.
·        For example Na forms Na+ by losing one electron and chlorine atom gains one electron and forms CI- ion.
Molecular ion:
·        When a molecule loses or gains electrons, the resulting species is called a molecular ion.
·        For example O2 when loses one electron it forms O2+ ion but when it absorbs an electrons it forms O2- ion. These ions are called molecular ions.
·        These are short lived species and only exist at high temperature. Molecular ions do not form ionic compounds.
Formula unit:
·        Formula unit is the simplest formula of an ionic compound.
·        A formula unit, as the name implies, is one unit, where atom, ion or molecule corresponds to given formula.
·        For example One formula unit of NaCl has one Na+ ion and one Cl- ion. One formula unit of MgBr2 has One Mg+ ion and two Br- ions.
Free radicals:
A free radical is an atom, which has an Un-paired electron and bears no electrical charge. For example:
 
When substances like halogens are exposed to sun light, their molecules split up into free radicals.

Atomic number:
·        The number of protons in the nucleus of an atom is known as its atomic number.
·        For example there is only one proton in the nucleus of H-atom; therefore its atomic number is 1.
Mass number:
·        The total number of protons and neutrons in an atom is known as its mass number.
·        Number of neutrons = mass number - atomic number
Atomic mass unit:
One atomic mass unit (amu) is defined as a mass exactly equal to one-twelfth the mass of one C-12 atom.
[Important] Question: Differentiate between an atom and ion.
·        An ion makes up the electric charge of an atom. It can be a positively charged atom or a negatively charged atom, depending on the number of protons versus electrons.
·        On the other hand, an atom is the smallest part of an element composed of electrons, protons, and the neutrons.

[Important] Question: Differentiate between molecular ion and free radical.
·        Polyatomic and molecular ions are often formed by the combination of elemental ions such as H+ with neutral molecules or by the loss of such elemental ions from neutral molecules. Many of these processes are acid-base reactions.
·        A radical ion is a free radical species that carries a charge. Radical ions are encountered in organic chemistry as reactive intermediates.

Question: Describe how Avogadro number is related to mole of any substance.
One mole of a Substance              =      6.02 x 1023 atoms / molecules.

                                                        Number of molecules of substance
Number of moles of substance      =      ----------------------------------------
                                                                              NA
                                                        Number of molecules of substance
Number of moles of substance      =      ----------------------------------------
                                                                         6.02 x 1023
One mole of hydrogen atoms = 6.02 x 1023 atoms of hydrogen (H) = 1 a.m.u.
One mole of hydrogen molecule = 6.02 x 1023 molecules of hydrogen (H2) = 2 a.m.u
[Very Important] Question: Calculate the number of moles of each substance in samples with the following masses.
2.4 g of He:
Mass of Helium (He)    =      2.4 g
Mollar Mass of Helium  =      4g

                                        Mass in grams            2.4
Number of Moles         =      -----------------    =      ----   =      0.6 moles
                                        Molar Mass                 4

250mg of Carbon:
Mass of Carbon   =      250mg       =      250/1000   =      0.25g
Molar Mass of Carbon                   =      12g

                                        Mass in grams            0.25
Number of Moles         =      -----------------    =      -----  =      0.021 moles
                                        Molar Mass                 12
15g of Sodium Chloride:
Mass of Sodium Chloride (NaCl)     =      15g
Molar Mass of NaCl                      =      23+35.5     =      58.5g

                                        Mass in grams              15
Number of Moles         =      -----------------    =      ------ =      0.256 moles
                                        Molar Mass                 58.5
40g of Sulphur:
Mass of Sulphur          =      40g
Molar Mass of Sulphur  =      32g

                                        Mass in grams              40
Number of Moles         =      -----------------    =      ------ =      1.25 moles
                                        Molar Mass                   32
1.5Kg of MgO:
Mass of MgO               =      1.5Kg                =      1500g
Molar Mass of MgO      =      24+16       =      40g

                                        Mass in grams            1500
Number of Moles         =      -----------------    =      ------         =      37.5 moles
                                        Molar Mass                   40

[Very Important] Question: Calculate the mass in grams of each of the following samples
1.2 moles of K:
Number of moles of potassium (K) =      1.2 moles
Molar mass of potassium (K)                 =      39 g
Mass in gram                              =      Number of moles x Molar mass
=      1.2 x 39 = 46.8 g
75 moles of H2
Number of moles of hydrogen (H2) =      75 moles
Molar mass of hydrogen (H2)                 =      2 x 1= 2g
Mass in gram                              =      Number of moles x Molar mass
                                                =      75 x 2 = 150g
0.25 moles of steam:
Number of moles of hydrogen (H2O)       =      75 moles
Molar mass of hydrogen (H2O)               =      2 x 1 + 16 = 18g
Mass in gram                                      =      Number of moles x Molar mass
                                                        =      0.25 x 18 = 4.5g
1.05 moles of CuSO4.5H2O
Number of moles of CuSO4.5H2O    =      1.05 moles
Molar mass of CuSO4.5H2O           =      63.5 + 32 + 4x16 + 5(2x1+16)
=      63.5 + 32 + 64 + 5(18)
=      249.5g
Mass in gram                              =      Number of moles x Molar mass
=      1.05 x 249.5 = 261.96 g
0.15 moles of H2SO4
Number of moles of H2SO4            =      0.15 moles
Molar mass of H2SO4                   =      2x1 + 32 + 4x16
=      2 + 32 + 64 = 98 g

Mass in gram                              =      Number of moles x Molar mass
=      0.15 x 98= 14.7 g

[Very Important] Question: Calculate the number of molecules present in each of the following samples.

2.5 moles of carbon dioxide:
Number of moles                 =      2.5 moles
Avogadro's number      =      NA = 6.022 x 1023
Number of molecules   =      Number of moles x NA
        =      2.5 x 6.022 x 1023
        =      15.055 x 1023
        =      1.505 x 1024 Molecules
3.4 moles of ammonia (NH3):
Number of moles                 =      3.4 moles
Avogadro's number      =      NA = 6.022 x 1023
Number of molecules   =      Number of moles x NA
        =      3.4 x 6.022 x 1023
        =      20.5 x 1023
        =      2.05 x 1024 Molecules
1.09 moles of benzene, (C6H6):
Number of moles                 =      1.09 moles
Avogadro's number      =      NA = 6.022 x 1023
Number of molecules   =      Number of moles x NA
        =      1.09 x 6.022 x 1023
        =      6.56 x 1023 Molecules
0.01 moles of acetic acid (CH3COOH):
Number of moles                 =      0.01 moles
Avogadro's number      =      NA = 6.022 x 1023
Number of molecules   =      Number of moles x NA
        =      0.01 x 6.022 x 1023
        =      0.062 x 1023
        =      6.02 x 1021 Molecules
Question: Decide whether or not each of the following is an example of empirical formula:
Al2Cl6:
No, since, 2 : 6 is not the simplest whole number ratio therefore Al2Cl6 is not empirical formula. Hence, Al2Cl6 is a molecular formula.
Hg2Cl2:
No, since, 2 : 2 is not the simplest whole number ratio, therefore Hg2Cl2 is not empirical formula. Hence, Hg2Cl2 is a molecular formula.
NaCl:
Yes, since, 1 : 1 is the simplest whole number ratio therefore NaCl is empirical formula.
C2H6O:
Yes, since, 2 : 6 : 1 is the simplest whole number ratio therefore C2H6O is empirical formula,

Question: 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.
C7H6N5O6

Question: 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        =      P4O10
Empirical formula        =      P2O5
Molar mass of P4O10       =      4 x 31 +10 x 16 = 124 + 160 = 284 g

[Important] Question: 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 Indigo (C16H10N2O2) =      16x12 + 10x1 + 2x14 + 2x16
=      192 + 10 + 28 + 32
=      262 g
Empirical formula of Indigo (C16H10N2O2)         =      C8H5ON

Molar mass of Indoxyl (C8H7ON)    =      8x12 + 7x1 + 16 +14
=      96 + 7 + 16 +14
=      133 g
Empirical formula of Indoxyl (C8H7ON)            =      C8H7ON

Question: Identify the substance that has formula mass of 133.5 amu.
Formula mass of MgCl2         = 24 + 2 x 35.5          = 24 + 71 = 95 amu
Formula mass of S2Cl2          = 2 X 32 + 2 x 35.5     = 64 +71 = 135 amu
Formula mass of BCI3                     = 11 + 3 x 35.5          = 11 + 106.5 = 117.5 amu
Formula mass of AlCl3          = 27 + 3 x 35.5          = 27 + 106.5 = 133.5 amu
Hence Formula mass of AlCl3 is 133.5
[Very Important] Question: Calculate the number of atoms in each of the following samples.
3.4 moles of nitrogen atoms:
Number of moles                         =      3.4 moles
Avogadro's number      =      NA     =      6.022 x 1023
Number of atoms                        =      Number of moles x NA
                                                =      3.4 x 6.022 x 1023
                        =      20.5 x 1023
=      2.05 x 1024 atoms
23g of Na:
Mass in gram                              =      23 g
Molar mass of sodium (Na)           =      23 g
Avogadro's number      =      NA     =      6.022 x 1023
                                                Mass in grams
Number of atoms                =      ----------------- x NA
                                                Molar Mass
                                                23
Number of atoms                =      --- x 6.022 x 1023                        = 6.022 x 1023 atoms
                                                23
5g of H atoms:
Mass in gram                              =      5 g
Molar mass of hydrogen (H)          =      1 g
Avogadro's number      =      NA     =      6.022 x 1023
                                                Mass in grams
Number of atoms                =      ----------------- x NA
                                                Molar Mass
                                                5
Number of atoms                =      -- x 6.022 x 1023              = 30.1 x 1023 atoms
                                                1
Number of atoms                =      3.01 x 1024 atoms
[Very Important] Question: Calculate the mass of following.
3.24 x 1018 atoms of iron:
Number of atoms                        =      3.24 x 1018 atoms
Molar mass of iron (Fe)                =      56 g
Avogadro's number      =      NA     =      6.022 x 1023
                                                        Number of atoms x Molar Mass
Mass in grams                    =              ---------------------------------
                                                        NA
                                                        3.24 x 1018 x 56
Mass in grams                    =              ------------------
                                                        6.022 x 1023
                                                        181.44 x1018
Mass in grams                    =              ------------------   =      30.1 x 1018-23
                                                        6.022 x 1023

Mass in gram                      =              30.1 x 10-5 g       =      3.01 x 10-4 g
2 x 1019 molecules of nitrogen gas:
Number of molecules                   =      2 x 1019 atoms
Molar mass of nitrogen gas (N2)    =      2 x 14 = 28 g
Avogadro's number                      = NA = 6.022 x 1023

Number of molecules x Molar mass
Mass in grams            =              ------------------------------------
NA

2 x 1019 x 28              56 x 1019
Mass in grams            =              ---------------       =      -------------------
6.022 x 1023                       6.022 x 1023

Mass in grams            =              9.3 x 1019-23       =      9.3 x 10-4

1 x 1025 molecules of water:
Number of molecules                   =      1 x 1025 molecules
Molar mass of Water (H2O)           =      2 x 1 + 16 = 18 g
Avogadro's number                      = NA = 6.022 x 1023

Number of molecules x Molar mass
Mass in grams            =              ------------------------------------
NA

1 x 1025 x 18              18 x 1025
Mass in grams            =              ---------------       =      -------------------
6.022 x 1023                       6.022 x 1023

Mass in grams            =              2.99 x 1025-23      =      2.9 x 102


3 x 106 atoms of Al:
Number of atoms                        =      3 x 106 atoms
Molar mass of Aluminium              =      27 g
Avogadro's number                      = NA = 6.022 x 1023

Number of molecules x Molar mass
Mass in grams            =              ------------------------------------
NA

3 x 106 x 27                81 x 106
Mass in grams            =              ---------------       =      -------------------
6.022 x 1023                       6.022 x 1023

Mass in grams            =              13.46 x 106-23     =      13.46 x 10-16

[Very Important] Question: Identify branch of chemistry that deals the following examples
A cornstalk grows from a seed.
Biochemistry
Dynamite (C3H5N3O9) explodes to form a mixture of gases.
Inorganic chemistry
Purple iodine vapour appears when solid iodine is warmed.
Analytical chemistry
Gasoline (a mixture of hydrocarbons) fumes are ignited in an auto mobile engine.
Organic chemistry.
A silver article tarnishes in air.
Environmental chemistry.
Ice floats on water.
Physical chemistry.
Sulphur dioxide is the major source of acid rain.
Environmental chemistry, since acid rain is an environmental problem.
Many other light chlorinated hydrocarbons in drinking water are carcinogens.
Environmental chemistry.
In Pakistan most of the factories use wet process for the production of cement.
Industrial chemistry.
Carbon-14 is continuously produced in the .atmosphere when high energy neutrons from space collide with nitrogen-14.
Nuclear chemistry.

Question: What mass of sodium metal contains the same number of atoms as 12.00g of carbon.
Avogadro's number      =      NA     = 6.022 x 1023
1 mole of sodium atom        =      1 mole of carbon-12     =      6.022 x 1023 atoms.
Therefore 23g of sodium metal contains the same number of atoms as 12.00g of carbon.
Question: What mass of oxygen contains the same number of molecules as 42g of nitrogen.
1 mole of N        =      14 g
3 mole of N                =      3x14          =      42g
1 mole of O        =      16 g
3 mole of O                =      3x16          =      48g
Question: Calculate the mass of one hydrogen atom in grams.
                                                Atomic mass of hydrogen
Mass of 1 hydrogen atom     =      ----------------------------
    Avogadro's number
                                                    1.008
Mass of 1 hydrogen atom     =      --------------        =      0.1674x10-23
6.022 x 1023
=      1.674 x 10-24 g
Question: Calculate the number of H-atoms present in 18g H2O.
Known mass of H2O = 18g = 1 mole of H2O = 6.022 x 1023 atoms.
Since one molecule of water has two atoms of hydrogen, therefore,
Number of hydrogen atoms in 18g of H2O = 2 x 6.022 x 1023 = 1.204 x 1024 atoms.

Question: Calculate the total number of atoms present in 18g H2O.
Known mass of H2O = 18 g = 1 mole of H2O = 6.02 x 1023 atoms.
Since one molecule of water has two atoms of-hydrogen; and one atom of oxygen.
Therefore, one molecule of water has total number of atoms = 2 + 1 = 3 atoms.
Total number of atoms in 18g of water = 3 x 6.02 x 1023 = 1.806 x 1024 atoms.

THEORY

Question: How do chemistry led to rapid progress in 19th century?
As 19th century began, John Dalton proposed an atomic theory. This theory led to rapid progress in chemistry.

Question: Define Chemistry.
Chemistry, is the branch of science, which deals with the composition, properties, chemical changes in matter and the laws and principles, which govern these changes.
Background:
The word Chemistry is derived from Kheem which is the ancient name of Egypt and the word Kheem was probably given to chemistry due to the black colour of the soil of Egypt. The The Arabs named it Al-Kimya in their own language and in the English, it became Alchemy.

[Very Important] Question: Define the branches of Chemistry.
Physical Chemistry: -
It is the study of physical properties of material things.
Inorganic Chemistry: -
It is the study of all compounds except of carbon.
Organic Chemistry: -
It is the study of compounds of carbon.
Analytical Chemistry: -
It is the study of analytical methods for getting information about chemical compounds.
Bio Chemistry: -
It is the study of chemical compounds and their reactions occurring in living things.
Industrial Chemistry: -
It is the study of chemical knowledge in technology and preparation of industrial products.

[Very Important] Question: Give main postulates of Dalton's atomic theory?
Main postulates of Dolton atomic theory are as under:
i)            All elements are composed of tiny indivisible particles called atoms.
ii)           Atoms of a particular element are identical. They have same mass and same volume.
iii)         During chemical reaction atoms combine or separate or re-arrange. They combine in simple ratios.
iv)         Atoms can neither be created nor destroyed.
[Very Important] Question: What are the defects of Dalton's atomic theory?
Series of experiment that were performed in 1850's and beginning of 20th century clearly demonstrated that atom is divisible and consists of subatomic particles, electrons, protons and neutrons. Also the atoms of an element may differ in masses (such atoms are called isotopes). Thus some of the postulates of Dalton's atomic theory were found defective and were changed.

Question: Photosynthesis produces glucose and oxygen from carbon dioxide and water in presence of chlorophyll and sunlight. Identify the branch of chemistry in this case.
Biochemistry, since photosynthesis is a chemical reaction that occurs in plants (living organism).
Question: Plantation helps in overcoming green house effect. Identify the branch, of chemistry in this case.
Environmental chemistry, since green house effect is an environmental problem.
Haber's process converts large quantities of hydrogen and nitrogen into ammonia (NH3). Identify the branch of chemistry in this case.
Industrial chemistry, since large scale production of any substance is the subject of industrial chemistry.
Question: Ammonia is a colourless gas with pungent irritating odour. It is highly soluble in water. Identify the branch of chemistry during this process.
Inorganic chemistry, since it deals with properties of inorganic compounds.
Question: A chemist performed an experiment to check the percentage purity of a sample of glucose (C6H12O6). Identify branch of chemistry in this case.
Analytical chemistry, since it deals with analysis of a compound, whether organic or inorganic in nature.
Question: An analyst determines that NO2 is responsible for acid rain. Identify the branch of chemistry in this case.
Environmental chemistry, since acid rain is an environmental problem.
Question: Chlorofluorocarbon compounds are responsible for the depletion of ozone layer. Identify the branch of chemistry in this case.
Environmental chemistry, since depletion of ozone layer is environmental problem.
Question: alpha-particles (He) when bombard on nitrogen atom, a proton is emitted. Identify the branch of chemistry in this case.
Nuclear chemistry, since nuclear change can emit protons.

Question: Define the followings:
Matter:
Anything that occupies space and has mass is called matter.
Mass:
Quantity of matter in a body, is called its mass.
Substance:
Matter that has a particular set of characteristics that differ from the characteristics of another kind of matter is called a substance.
Element:
An element is a substance whose all the atoms have the same atomic number.
Compound:
A compound consists of two or more elements held together in fixed proportions by chemical bonds.
Mixture:
An impure substance that contains two or more pure substances that retain their individual chemical characteristics is called a mixture. It has two types:
  • Heterogeneous mixture consists of two or more visibly, different components
  • Homogeneous mixture consists of only one phase.

[Very Important] Question: Write the two main advantages of garlic.
  • Bad breath may be-good for you. The chemistry of garlic is not simple.
  • Garlic contains more than 200 compounds.
  • People who eat a lot of garlic have a lower chance of getting stomach cancer, suffering from heart disease.

[Very Important] Question: Describe the classification of molecules?
Monoatomic molecules:
A molecule that contains only one atom is called monoatomic.
Polyatomic molecules:
Molecules that contain two or more similar or different atoms are palled polyatomic molecules.

[Very Important] Question: Write the formation of Na+ ion?
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

[Very Important] Question: Write the Empirical and Molecular Formulas of Aspirin and Vinegar.
Empirical formula of Aspirin is C9H8O4.
Molecular formula of Aspirin is also C9H8O4.
Empirical formula of Vinegar is C2H4O2.
Molecular formula of Vinegar is CH2O.

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Download Class Notes: Download 9th Class Chemistry Notes (Unit # 1) for Federal Board (FBISE) Islamabad
Download 9th Class Chemistry Notes (Unit # 1) for Federal Board (FBISE) Islamabad
Download 9th Class Chemistry Notes (Unit # 1) for Federal Board (FBISE) Islamabad
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