Mole Concept
1
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Mole Concept
1
Straight Line Curves
y = mx +c
Slope of
the
curves
Variable
on YAxis
Variable
on XAxis
Intercept
on YAxis
Straight Line Curves
Straight Line Curves
Straight Line Curves
Matter
Matter
Chemical
Classification
Physical
Classification
Solid
(NaCl, Fe etc.)
Liquid
(Br2, H2O etc)
Gas
(O2, air, NH3 etc
Pure
Element
Metal
(Na, Fe, Mg etc.)
Metalloid
(As, Se etc)
Non-metal
(F, Cl, Br, I, P, etc.
Impure
Compound
Covalent
(C6H12O6,
NH2CONH2 etc)
Ionic
(NaCl, CaCl2 etc)
Mixture
Homogen
eous
Heterogen
eous
Matter
Units
Units
Prefixes
Volume Measurements
Volume Measurements
Mass & Weight
Temperature
Element
Element is the purest form of matter. It is made up of only one
type of atoms.
Example: Carbon, Iron, copper, oxygen etc.
Compound
Compound is the substance which is made up of two or more
same elements combined together in a fixed ratio by their weight.
Example: Carbon dioxide.
Mixture
Mixture is the substance which is made up of two or more
substances in any ratio.
Example: Sugar + Water, Sodium Chloride + Water, Sand + Water
Mixture
Homogeneous Mixture
Heterogeneous Mixture
Homogenous Mixture
The mixture which has uniform composition throughout.
Example: sugar solution
Heterogeneous Mixture
The mixture which do not have uniform composition throughout.
Example: Sand in water
Types of Substances
Types of
Substances
Efflorescent
Substances
Hygroscopic
Substances
Deliquescent
Substances
Efflorescent Substances
When some substances are exposed to air, they lose water to the
atmosphere, thereby reducing in weight.
Example: Na2SO4.10H2O, Na2CO3.10H2O, FeSO4.7H2O
Hygroscopy Substances
This is when substances absorb water from air, but not enough to
form solutions.
Example: CaO, NaNO3, Sucrose and CuO.
Deliquescent Substances
This is when certain solid substances, when exposed to air, absorb
water, enough to form solutions.
Example: NaOH, CaCl2, CaCl2.6H2O, P4O10, FeCl3, KOH, MgCl2
Home Work
1. Phosphorus forms two oxides P2O3
and P2O5. Which law can be proved
by the weights of P and O?
A. Constant composition
B.
Multiple Proportions
C. Reciprocal Proportions
D.
Conservation of mass
2. Zinc sulphate contains 22.65% Zn
and 43.9% H2O. If the law of
constant proportions is true, then
the mass of Zinc required to give
40 g crystal will be
A. 90.6 g
B.
9.06 g
C. 0.906 g
D.
906 g
3. Hydrogen combines with Chlorine
to form HCl. It also combines with
sodium to form NaH. If sodium and
chlorine also combine with each
other, they will do so in the ratio
of their masses as
A. 23 : 35.5
B.
35.5 : 23
C. 1 : 1
D.
23 : 1
4. How many significant figures are in
2.345 × 104?
A. 4
B.
3
C. 2
D.
8
Home Work
5. Which of the following number has
3 significant figures?
A. 519.00
B.
2503
C. 0.0500
D.
0.008
6. How many significant figures are
present in 7 × 2.232?
A. 2
B.
3
C. 4
D.
1
7. Which
of
the
following
combinations illustrates the law of
reciprocal proportions?
A. NO2, N2O4, N2O
B.
NaCl, NaBr, NaI
C. PCl3, PH3, PF3
D.
CS2, SO2, CO2
8. 3 g of a hydrocarbon on
combustion with 11.2 g of oxygen
produces 8.8 g CO2 and 5.4 g H2O.
The data illustrates the law of
A. Conservation of mass
B.
Multiple proportions
C. Definite proportions
D.
Reciprocal proportions
Home Work
9. The
scientific
0.00000000068 is?
A. 6.8 × 10–10
B.
68 × 10–11
C. 6.8 × 10–11
D.
68 × 10–10
notation
of
10. Carbon forms two oxides containing
42.9%
and
27.3%
carbons
respectively. Which law of chemical
combination does this illustrate?
A. Law of constant composition
B.
Law of multiple proportions
C. Law of conservation of mass
D.
Law of reciprocal proportions
11. Two oxides of a metal contain
72.4%
and
70%
of
metal
respectively? if formula of 2nd
oxide is M2O3, find that of the first
A. MO
B.
M3O4
C. M3O2
D.
MO2
12. Irrespective to the source, pure
sample of water always yields
11.11% mass of hydrogen and
88.89% mass of oxygen. This is
explained by the law of
A. Conservation of mass
B.
Constant composition
C. Multiple proportions
D.
Constant volume
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