Classification of Elements and Periodicity in Properties Test

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Classification of Elements and Periodicity in Properties Test - 54

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Weekly Quiz Competition

Question 1
1 / -0

Which statements about Group I and Group VII elements are correct?
1. In Group I, lithium is more reactive than potassium.
2. In Group VII, chlorine is more reactive than fluorine.

A
Statement $$1 - \checkmark$$, statement $$2 - \checkmark$$

B
Statement $$1 - \checkmark$$, statement $$2 - X$$

C
Statement $$1 - X$$, statement $$2 - \checkmark$$

D
Statement $$1 - X$$, statement $$2 - X$$
Solution
- Potassium has more tendency to lose electron, hence potassium is more reactive than lithium.
- Chlorine is less reactive than fluorine because it is less electronegative than fluorine.
Question 2
1 / -0

In the modern periodic table, elements are arranged in order of increasing atomic number which is related to the electronic configuration. Depending upon the type of orbitals receiving the last electron, the elements in the periodic table have been divided into four blocks, viz s, p, d and f. The modern periodic table consists of 7 periods and 18 groups. Each period begins with the filling of a new energy shell. In accordance with the Aufbau principle filling of a new energy shell. In accordance with the Aufbau principle, the seven period (1 to 7) have 2,8,8,18,18,32 and 32 elements respectively. The seventh period is still incomplete. To avoid the periodic table being too long, the two series of f - block elements, called lanthanoids and actinoids are placed at the bottom of the main body of the periodic table..
The electronic configuration of the elements which is just above the elements with atomic number 43 in the same group is ____

A
$$1s^22s^22p^63s^23p^63d^54s^2$$

B
$$1s^22s^22p^63s^23p^63d^54s^24p^6$$

C
$$1s^22s^22p^63s^23p^63d^64s^2$$

D
$$1s^22s^22p^63s^23p^63d^74s^2$$

Solution
Question 3
1 / -0

Statement I: In $$ClF_{3}$$, chlorine has the oxidation number - 1.

Statement II: Electron affinity of chorine is greater than that of fluorine.

A
If both statements are CORRECT, and Statement II is the CORRECT explanation of Statement I.

B
If both statements are CORRECT, and Statement II is NOT the CORRECT explanation of Statement I.

C
If Statement I is CORRECT, but Statement II is INCORRECT.

D
If Statement I is INCORRECT, but Statement II is CORRECT.

Solution

$$ ClF_{3}$$ as $$ F$$ has O.N = -1

$$ \therefore Cl $$ has =$$ +3$$

statement I incorrect.

Election affinity of $$Cl$$ is greater than $${F}$$
because $$Cl$$ has "d" orbital take up $$ e^{\circleddash }$$
while F has smaller size.

$$ \therefore $$ Statement II is correct.
Question 4
1 / -0

The electronic structure of zinc $$(Z=30)$$ is $$2,8,18,2.$$ The electronic structure of gallium $$(Z=31)$$ will be

A
$$2,8,18,2,1$$

B
$$2,8,19,2$$

C
$$2,8,18,3$$

D
$$2,8,19,3$$

Solution

The maximum number of electrons in K,L and M orbits are 2, 8 and 18 respectively. Hence, the extra electron in the case of Gallium (Z=31) will be in Nth orbit and electronic structure will be 2, 8, 18, 3.
Question 5
1 / -0

Correct option for electron affinity of :

A
carbon is higher than oxygen

B
sulphur is lesser than oxygen

C
iodine is higher than bromine

D
chlorine is higher than fluorine

Solution

Fluorine has low electron affinity than chlorine. This is because due to smaller size of fluorine and electrons are more closely bound together so that incoming electron feels repulsion so additional energy is required to hold the incoming electron. That's why fluorine has smaller electron affinity.
Question 6
1 / -0

Which of the following electronic configuration represents most electropositive element?

A
$$ [He] 2s^1 $$

B
$$ [He] 2s^2 $$

C
$$ [Xe] 6s^1 $$

D
$$ [Xe] 6s^2 $$

Solution

Group one elements with ns1 configuration are more electropositive than group 2 elements.

Electropositive character increases down the group

Option C is correct.
Question 7
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Which of the following statements is incorrect?

A
Among all the elements, fluorine has the highest electron gain enthalpy.

B
Among all the elements, helium has the highest ionisation enthalpy.

C
Elements of groups 1, 2, 13, 14, 15, 16 and 17 are called representative elements.

D
All the d-block elements are metallic in nature.

Solution

Answer A
The statement is wrong among all elements chlorine has the highest electron gain enthalpy due to the size difference between fluorine and chlorine
Question 8
1 / -0

The most predominantly electrovalent compounds will be obtained from the combination of elements belonging to:

A
I and VII groups

B
II and VI groups

C
III and V groups

D
None of these

Solution

We know that increase in electronegativity difference increases the ionic character and decreases the covalent character.

As the electronegativity difference between VIIA group and IA group elements is higher than the remaining set of groups, it has the most predominantly electrovalent compounds.
Question 9
1 / -0

Which of the following elements has the maximum electron gain enthalpy?

A
oxygen

B
chlorine

C
fluorine

D
nitrogen

Solution

Answer: B
Chlorine has the maximum electron gain enthalpy. Halogens have the highest electron gain enthalpy (electron affinity). Normally electron affinity decreases as we move down the group. However, fluorine has a lower value than chlorine which is due to its small size.
Question 10
1 / -0

Diagonal relationship in periodic table is shown by elements of _____ and _____ periods:

A
I and II

B
II and III

C
III and IV

D
I and III

Solution

Answer B
The diagonal relationship is shown by 2nd and 3rd-period elements of the periodic table as they have similar properties. The diagonal relationship is due to similar sizes of atoms or ions and electronegativities of the participating elements and the same polarising power. Eg: Li and Mg.

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Classification of Elements and Periodicity in Properties Test - 54

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Classification of Elements and Periodicity in Properties Test - 54

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Question 1

Statement $$1 - \checkmark$$, statement $$2 - \checkmark$$

Statement $$1 - \checkmark$$, statement $$2 - X$$

Statement $$1 - X$$, statement $$2 - \checkmark$$

Statement $$1 - X$$, statement $$2 - X$$

Solution

Question 2

$$1s^22s^22p^63s^23p^63d^54s^2$$

$$1s^22s^22p^63s^23p^63d^54s^24p^6$$

$$1s^22s^22p^63s^23p^63d^64s^2$$

$$1s^22s^22p^63s^23p^63d^74s^2$$

Solution

Question 3

If both statements are CORRECT, and Statement II is the CORRECT explanation of Statement I.

If both statements are CORRECT, and Statement II is NOT the CORRECT explanation of Statement I.

If Statement I is CORRECT, but Statement II is INCORRECT.

If Statement I is INCORRECT, but Statement II is CORRECT.

Solution

Question 4

$$2,8,18,2,1$$

$$2,8,19,2$$

$$2,8,18,3$$

$$2,8,19,3$$

Solution

Question 5

carbon is higher than oxygen

sulphur is lesser than oxygen

iodine is higher than bromine

chlorine is higher than fluorine

Solution

Question 6

$$ [He] 2s^1 $$

$$ [He] 2s^2 $$

$$ [Xe] 6s^1 $$

$$ [Xe] 6s^2 $$

Solution

Question 7

Among all the elements, fluorine has the highest electron gain enthalpy.

Among all the elements, helium has the highest ionisation enthalpy.

Elements of groups 1, 2, 13, 14, 15, 16 and 17 are called representative elements.

All the d-block elements are metallic in nature.

Solution

Question 8

I and VII groups

II and VI groups

III and V groups

None of these

Solution

Question 9

oxygen

chlorine

fluorine

nitrogen

Solution

Question 10

I and II

II and III

III and IV

I and III

Solution

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