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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

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