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Discipline, Knowledge & Results
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1) Symbols of proton, electron and neutrons are
2) Electrons are discovered by ………………………………………………………………………………………………………….
3) Protons are discovered by ……………………………………………………………………………………………………………
4) Neutrons are discovered by …………………………………………………………………………………………………………
5) The mass of an electron is ……………………………………………………………………………………………………………
6) The mass of a proton is ………………………………………………………………………………………………………………..
7) The mass of a proton is …………….….times the mass of an electron
8) The plum pudding model was proposed by ………………………………………………………………………………….
9) Protons and neutrons found in the nucleus are called ………………………………………………………………….
10) The planetary model was proposed by …………………………………………………………………………………………
11) Max. No. of electrons in the 3rd (M) and 4th (N) energy levels are respectively ……………………………
12) Max. No. of electrons in the last energy levels of a free atom ………………………………………………………
13) Substances or matter occupy space and have ………………………………………………………………………………
14) Molecules are made up of ……………………………………………………………………………………………………………
15) Compounds are made up of …………………………………………………………………………………………………………
16) The mass of a protons is nearly equal to the mass of a ………………………………………………………….......
17) The number of protons of an atom is called …………………………………………………………………………………
18) The charge of an atom is ………………………………………………………………………………………………………………
19) Some atoms donate (remove) electrons and become………………………………………………………………….
20) Some atoms accept (gain) electrons and become…………………………………………………………………………
21) In anions, electrons……………..protons. Hence the charge of an anion is………………………………………..
22) In cations, electrons…………….protons. Hence the charge of a cations is ……………………………………….
23) In atoms, protons ………………. Electrons. Hence the charge of an atom is …………………………………….
24) The sum of protons and neutrons in an atom is called …………………………………………………………………
25) ……….. = Mass No
26)
39
19
–
Number of neutron
Atomic Number : ………………………………… Mass Number :…………………………….
K
p : ……………………. e: ……………………. n: ………………………
electronic configuration. ………………………. Group :………………… Period……………
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Mass No
Atomic No
p
e
n
e-configuration
Group
Period
31
15
27)
28)
29)
30)
31)
32)
34)
35)
36)
37)
38)
39)
40)
41)
44)
45)
46)
47)
49)
50)
51)
33)
18
6
18
42)
2, 8, 7
43)
VI
2
12
48)
I
3
8
52)
53)
54)
55) Atoms having same number of p but different number of n are called …………………………….......
56) Atoms having same atomic number but different mass number are called …………………………...
Element
Mass number
Atomic Number
P
35
14
Q
37
17
R
35
17
S
37
18
57) The isotopes among the above elements are……………………………………………………………………………
Element
Mass number
neutrons
K
14
8
L
14
7
M
12
6
N
13
7
58) The isotopes among the above elements are…………………………………………………………………………….
59) Write the symbols of Protium, Deuterium and Tritirium
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60) Write the symbol of the most abundant isotope of chlorine..……………………………………………………….
61) Write the formulae of the following
a) Aluminium oxide …………………………..….
b) Sodium oxide……………….………………………………
c) Magnesium oxide …………………………….
d) Calcium phosphate …………………………………….
e) Ammonium sulphate……………………….
f) Calcium bicarbonate……………………………………..
g) Ferric oxide ……………………..………………
h) Cuprous oxide………………………………………………
i)
Ferric sulphate…………………………………
j) Magnesium nitrite…………………………………………
k) Calcium Sulfide ………………………………..
l) Ammonium sulfite ……………………………………….
m) Cupric nitrate …………………………………..
n) Zinc bisulfate ………………………………………………
o) Sulfuric acid ……………………………………..
p) Nitric acid …………………………………………………..
q) Hydrochloric acid………………………………
r) Potassium manganate …………………………………
s) Zinc chloride …………………………………….
t) Silver sulphate ……………………………………………..
(62 ) Name the following according to the International Union Pure and Applied Chemistry –
IUPAC. The valencies should be written in parenthesis () when writing elements having variable
valencies.
a) FeCl3………………………………………………………. b) FeCl2…………………………………………………………….
c) Pb(NO2)2………………………………………………..
d) Pb(NO2)4 ……………………………………………………..
e) CuOH………………………………………………………
f) Cu(OH)2…………………………………………………………
g) PbO…………………………………………………………
h) PbO2 …………………………………………………………….
i)
FeO…………………………………………………………. J) Fe2O3……………………………………………………….
(63) The formular of oxide formed my element X is X2O3. Write the formular of Sulphate formed
by M………………………………………………………………….
64) The formular of Sulphate formed by Y element is YSO4. Write the formular of the phosphate
formed by Y………………………………………………………
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65) The formular of Manganate formed by element Z is Z2(MnO4)3. Write the formular of the of
the phosphate formed by Z…………………………………………………………………………………………………………
63) The mass of C atom is 1.99 x 10-23g. The mass of N is 2.32 x 10-23g. Find the relative atomic
mass of N.
……………………………………………………………………………………………………………………………………………………..
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(64) The mass of C atom is 1.99 x 10-23g. The relative atomic mass of Ca is 40. Find the relative
molecular mass of Ca.
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H= 1 C=12
Fe=56
N=14 O=16
Mn=55
Na=23 Mg=24
Cu=63.5
Al=27 S=32
Cl=35.5
K=39
65) Find the mass of 3 moles of ferric sulphate
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66) Find the mass of 0.25 moles of potassium permanganate
……………………………………………………………………………………………………………………………………………………..
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67) Find the number of ammonium sulphate moles in 27g of ammonium sulphate
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68) Find the number of H atoms in 12g of urea CO(NH2)2
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69) Find the number of Oxygen atoms in 49.9g of hydrous cupper sulphate
……………………………………………………………………………………………………………………………………………………..
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70) Show how 27Al and 8O atoms form aluminum oxide molecule
71) Show how 12Mg and 16S atoms form Magnesium oxide molecule
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72) Show how 1H and 17Cl atoms form HCl molecule
73) Show how 7N and 1H atoms form NH3 molecule
74) Underline the molecules having covalent bonds and circle the molecules having ionic bonds
HCl
NH4OH
AgNO3
Mg(OH)2
SO2
75) Write 5 features of ionic compounds
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76) A soid compound PQ soluble in water is formed when the element P combines with the
element Q. It has become necessary to determine experimentally whether the bonds of the
compound PQ are ionic bonds or covalent bonds. For this purpose an electric bulb, battery, 2
rods or carbon, connecting wires a beaker and water are supplied, along with the compound PQ.
Draw a labeled diagram of a set-up using the materials and equipments supplied to determine
the nature of the bonding and state the observation made through the set-up if the bonds in the
compound PQ are ionic bonds.
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