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11th Chemistry Monthly Test - 1 ( Periodic Classification Of Elements )

MABS Institution

11th Chemistry Monthly Test - 1 ( Periodic Classification Of Elements )-Aug 2020

Time : 2.30 Hours

Part - A

Multiple Choice Question - Answer All Question

The general electronic configuration of d-block element is _____

ns²np⁶
(n-1) d^1-10 ns^0-2
(n-1) d¹ ns^0-2
(n-1) d^0-10 ns²

Choose the correct order of ionization energy.

N>O>F
F>O>N
N>O<F
O>F>N

Which of the following have the highest value of electronegativity?

Halogens
Alkali metals
Alkaline earth metals
Transition metals

Which of the following processes involves absorption of energy?

Cl_(g) +e^- ⟶ Cl^-
O^-_(g) +e^- ⟶ O^2-
O_(g) +e^- ⟶ O_(g)^-
S_(g)+e^- ⟶ S^-_(g)

Considering the elements B, C, N, F and Si, the correct order of their non-metallic character is ________.

B > C > Si > N > F
Si > C > B > N > F
F > N > C > B > Si
F > N > C > Si > B

Which one among the following exhibits a valency greater than 4?

Na
P
H
Ar

With respect to chlorine, hydrogen will be

Electropositive
Electronegative
Neutral
None of these

Which period contain 32 elements?

Period 1
Period 4
Period 5
Period 6

Electronegativity of the following elements increases in the order

C, N, Si, P
N, Si, C, P
Si, P, C, N
P,Si, N, C

What would be the formula of the compound formed by A and B, where A has the valence 3 and B has the valence 3?

AB
AB₃
A₃B
3AB₃

Part - B

Generic 2 - Answer All Question

How does the basic and acidic nature of oxides vary along a period and in group?.

Electron affinity of oxygen is less negative than sulphur. Justify this statement.

Explain why covalent radius is always shorter than actual atomic radius

Anionic radius is higher than the corresponding neutral atom.Give reason.
Explain the influence of shielding effect as the ionisation energy of elements

What are semi-metals? Give example.

What do you understand by the term 'variable oxidation state? Which elements in a group or period exhibit variable oxidation state?

How do atomic radius vary in a period and in a group? How do you explain the variation.

Explain the term valence or oxidation state. How does it vary in a period and in group?

Explain about the period variation of electronegativity along a group.

Part - C

Generic 3 - Answer All Question

How is screening effect of inner electrons affect ionization energy?

Predict the periods and blocks to which each of the following elements belongs?
(i) ₁₃Al
(ii) ₂₄Cr
(iii) ₂₉Cu
(iv) ₁₁Na

State the findings of modern periodic law.

How does the shielding effect caused by inner electrons affect the ionisation energy?

Write a note about metallic radius.
Define metallic radius.

Explain classification of elements based on Newland's law of Octaves.

Out of Na and Mg, which has higher second ionisation energy?

Arrange the following elements in the increasing order of non-metallic character. B, C, Si, N, F

Explain how electronegativity values are used to predict the nature of the bond between two atoms between A and B

Part - D

Generic 5 - Answer All Question

Why the first ionisation enthalpy of sodium is lower than that of magnesium while its second ionisation enthalpy is higher than that of magnesium.

Calculate the ionic Radii of Na⁺ and F^- ion in NaF crystal whose interionic distance is equal to 231 pm

By using paulings method calculate the ionic radii of K⁺ and CI^- ions in the potassium chloride crystal. Given that d_k⁺-Cl^-=3.14 Å.

Prove that the atomic radii is a periodic property.

How do you classify of elements into blocks? Give their electronic configuration.

Given the bona lengths of H₂, Cl₂, C - C bond in diamond, Si - C bond in carborundum and C - CI bond in CCl₄ are 0.74, 1.9, 1.54, 1.93 and 1.76A respectively, find the covalent radius of hydrogen, chlorine, carbon in diamond, silicon and carbon in CCI₄.

(a) State Mendeleev's periodic law.
(b) Describe about the merits of Mendeleev's periodic table.
Explain the classification of elements based on chemical behaviour and on physical properties.

Explain the periodic trend of ionisation potential.

Explain the following, give appropriate reasons.
(i) Ionisation potential of N is greater than that of O.
(ii) First ionisation potential of C-atom is greater than that of B atom, where as the reverse is true is for second ionisation potential.
(iii) The electron affinity values of Be, Mg and noble gases are zero and those of N (0.02 eV) and P (0.80 eV) are very low.
(iv) The formation of F-(g) from F(g) is exothermic while that of O^2-(g) from O (g) is endothermic.

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