S M BAQIR LECTURES
Chp-3, Periodic table and periodicity of properties
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Objective Part
Choose the right option. 10×1=10
A
B
C
D
1
Transition elements are:
All gases
All metals
All non-metals
All metalloids
2
Mendeleev periodic table was based upon the:
Electronic configuration
Atomic mass
Atomic number
Completion of subshells
3
Unit of ionization energy are:
KJ/mol
KJmol
KJ
J/mol
4
The d-block elements lie between the______ blocks.
s-p
d-f
p-s
f-d
5
Sixth and seventh periods are called:
Short period
Normal period
Long period
Very long period
6
Along the period, which one of the following decreases
Atomic radius
Ionization energy
Electron affinity
Electro negativity
7
The half of the distance between the nuclei of two bonded atom is referred as:
Atomic size
Atomic radii
Ionic radii
Common size
8
Which scientist had given the idea of octaves in periodic table?
Mendeleev
Al-Razi
Newland
Dobereiner
9
In __________ H. Moseley discovered a new property of the elements i.e. atomic number
1913
1914
1915
1916
10
The amount energy given out when an electron is added to an atom is called :
Lattice energy
Ionization energy
Electro negativity
Electron affinity
Subjective
Answer the short questions. 10×2=20
1. What do you mean by groups and periods in a periodic table?
2. Give the trend of ionization energy in a periodic table?
3. Why noble gases are not reactive?
4. State Mendeleev’s periodic law.
5. From which element lanthanide series starts?
6. Define ionization energy.
7. How can you define atomic radius?
8. Why the trend of electron affinity and electronegativity is same in a period?
9. What is shielding effect?
10. What is the reason of arranging elements in a group?
Long Questions 5×1=5
1. (a) Write down the salient features of long form of periodic table. 3
(b) Describe the trends of electronegativity in a period and in a group. 2