Basic concepts of Chemistry and chemical calculations

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31 Terms

1

Atomic mass unit

One twelfth of the mass of a Carbon-12 atom in its ground state.

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2

Relative atomic mass (RAM)

Ratio of the average atomic mass to the unified atomic mass unit.

Ar = average mass of the atom/unified atomic mass

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3

Molecular mass

Ratio of mass of a molecule to the unified atomic mass unit.

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4

Mole

  • One mole is the amount of substance of a system, which contains as many elementary particles as there are atoms in 12 g of Carbon-12 isotope.

  • The elementary particles can be molecules, atoms, ions, electrons or any other specified particles.

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5

Avogadro Number

The total number of entities present in one mole of any substance is equal to 6.022 × 10²³.

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6

Molar mass

  • Mass of one mole of a substance

  • Molar mass of a compound is equal to the sum of its relative atomic masses of its constituents

  • Unit : g mol-¹

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7

Molar volume

Volume occupied by one mole of a substance in the gaseous state at a given temperature and pressure.

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8

Gram equivalent mass

  • Mass of an element (compound or ion) that combines or displaces 1.008 g hydrogen, 8 g oxygen or 35.5 g chlorine

  • equivalent mass = Molar mass (g mol-¹) / equivalence factor ( eq mol-¹)

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9

Equivalent mass of acids

E = Molar mass of the acid / basicity of the acid

Basicity - No. of replaceable H+ ions

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10

Equivalent mass of Bases

E = Molar mass of the the base / Acidity of the base

Acidity - no. of replaceable OH- ions

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11

Equivalent mass of Oxidising agent or reducing agent

E = Molar mass of the oxidising (or) reducing agent/ No. of moles of electrons gained or lost by one mole of the oxidising or reducing agent

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12

Stoichiometry

It gives the numerical relationship between chemical quantities in a balanced chemical equation

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13

Limiting reagent

  • When a reaction is carried out using non-stoichiometric quantities of the reactants, the product yield will be determined by the reactants that is completely consumed

  • It limits the further reaction from taking place and is called as the limiting reagent.

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14

Excess reagents

Other reagents which are in excess

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15

Cyanide poisoning

  • Oxygen binds to haemoglobin

  • Cyanide binds irreversibly to haemoglobin and blocks oxygen binding

  • Transport of oxygen from lungs to tissues is stopped

  • Leads to quick death of the person

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16

Oxidation number

  • Imaginary charge left on the atom when all the other atoms of the compound have been removed in their usual oxidation states

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17

Oxidation number of elements in ground state

0

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18

Oxidation number of Na+

+1

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19

Oxidation number of Cl-

-1

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20

Oxidation number of Hydrogen

+1 except metallic hydrides (-1)

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21

Oxidation number of Fluorine

-1

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22

Oxidation number of alkali metals (1st group)

Li, Na, K, Rb, Cs

+1

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23

Oxidation number of alkaline earth metals (2nd group elements)

Mg, Ca, Sr

+2

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24

Sum of the oxidation numbers of elements in a compound

0

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25

Sum of the oxidation numbers of elements in a polyatomic ion

Charge carried by the ion

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26

Oxidation reaction

  • Addition of Oxygen

  • Removal of Hydrogen

  • Loss of electrons

  • Oxidation number in increases

  • Eg : C + O2 → CO2

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27

Reduction reaction

  • Addition of Hydrogen

  • Removal of Oxygen

  • Gain of electrons

  • Oxidation number decreases

  • Eg : H2 + Cl2 → 2 HCl

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28

Combination reactions

It is a reaction in which two substances combine to form a single compound

C + O2 → CO2

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29

Decomposition reaction

It is a reaction in which a compound breaks down into two or more components

2 KClO3 → 2 KCl + 3 O2

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30

Disproportionation reaction (Auto redox reaction)

It is a reaction in which same compound undergoes both oxidation and reduction

2 H2O2 → 2 H2O + O2

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31

Displacement reaction

It is a reaction in which an ion or atom in a compound is replaced by an ion or atom of another element.

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