Classification of Elements and Periodicity in Properties Test

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Classification of Elements and Periodicity in Properties Test - 51

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Weekly Quiz Competition

Question 1
1 / -0

Which of the following statements are correct?

A
The second ionization enthalpy of oxygen element is greater than that of the fluorine element.

B
The first ionization enthalpy of phosphorus is greater than that of aluminium .

C
The first ionization enthalpy of aluminum is slightly greater than that of gallium.

D
The first ionization enthalpy of B is less than that of Be.

Solution

The electronic configuration of

1. Oxygen-$$1s^22s^22P^4$$

2. Fluorine $$1s^22s^22p^6$$
3. Phosphorous $$[Ne]3s^23p^3$$
4. Aluminium $$[Ne]3s^23p^1$$
5. Gallium: $$[Ar]3d^{10}4s^24p^1$$
6. Boron $$1s^22s^22p^1$$
7. Berylium $$1s^22s^2$$
* Second ionization enthalpy is very high compared to fluorine due to the half-filled configuration of $$O^+$$
* The first ionization enthalpy of phosphorous is very high due to the half-filled configuration of $$3p-$$ orbitals.
* Electrons easy to remove in galium because they are far from nucleus compared to aluminum.
* The first ionisation enthalpy at berylium is low because it attains stable full-filled configuration of $$2s^2$$
Question 2
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The smog is essentially caused by the presence of:

A
$$O_2$$ and $$O_3$$

B
$$O_2$$ and $$N_2$$

C
$$O_3$$ and $$N_2$$

D
Oxides of sulphur and Nitrogen

Solution

The smog is essentiallly caused by presence of oxides of sulphur and nitrogen, i.e NO, NO2 , SO3 and SO2 are mainly responsible for smog
Question 3
1 / -0

Which of the following order is incorrect.

A
IE of $$F> Cl$$

B
$$IE \ of \ F^{-}> Cl^{-}$$

C
E.A of $$F< Cl$$

D
E.A of $$F^{+}> Cl^{+}$$

Solution

In a group, the ionization energy decreases from top to bottom.
The size of the anion is greater than the size of the neutral atom. Due to this, the attraction of the nucleus for the valence electrons is larger in case of neutral atom. Hence, the ionization energy of the neutral atom is larger than that of anion. In case of halogens, the addition of an electron leads to breaking of the noble gas configuration. The ionization energy of fluoride ion is lowest due to electron electron repulsion.
Hence I.E of $$F^-<Cl^-$$
Option B Is incorrect.
Hence option B is correct answer.
Question 4
1 / -0

The elements with atomic number 117 and 120 are yet to be discovered. In which group would you place these elements when discovered?

A
17, 2

B
16, 4

C
15, 3

D
18, 2

Solution
Question 5
1 / -0

Consider 2 electronic configuration of potassium
$$K=1s^2,2s^2,2p^6,3s^2,3p^6, 4s^1$$
$$K=1s^2,2s^2,2p^6, 3s^2,3p^6,3d^1$$
find the effective nuclear charge experienced by last electron in (I) and (ii)

A
2.20 and 7.40

B
2.20 and 1.00

C
2.20 and 2.20

D
2.20 and 6.30

Solution
Question 6
1 / -0

In long form of periodic table, the total number of periods is:

A
5

B
7

C
8

D
9

Solution

1.There are seven periods in the periodic table, with each one beginning at the far left.
2. A new period begins when a new principal energy level begins filling with electrons.
Question 7
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The electronic configuration of an element is $$1s^22s^22p^63s^23p^63d^{10}4s^1$$. What is the atomic number of the next element of the same group?

A
$$20$$

B
$$119$$

C
$$30$$

D
$$47$$

Solution
Question 8
1 / -0

Which of the following option is incorrect?

A
$$Au > Ag\left( {I.{E_1}.} \right)$$

B
$$Cl > N\left( {E.{A_1}.} \right)$$

C
$$T{l^{ + 1}} > T{l^{ + 3}}\left( {stability} \right)$$

D
$$L{i^ + }\left( {aq.} \right) > B{e^{ + 2}}\left( {aq.} \right)\left( {atomic\ radius} \right)$$
Question 9
1 / -0

Which of the following processes involves absorption of energy?

A
Cl (g) + e$$^{-}$$ $$\rightarrow $$Cl$$^{-}$$(g)

B
O$$^{-}$$ + $$e^{-}$$ $$\rightarrow $$ O$$^{2-}$$ (g)

C
O (g) + e$$^{-}$$$$\rightarrow$$ O$$^{-}$$(g)

D
S (g) + e$$^{-}$$$$\rightarrow$$ S$$^{-}$$ (g)
Solution
- $$O^-$$ to $$O^{2-}$$ because of interelectronic repulsion, it will require energy to add an electron to its outermost shell.
- Hence option B is correct answer.
Question 10
1 / -0

Nuclides have:

A
specific atomic number

B
same numbers of proton

C
same numbers of neutrons

D
specific atomic number and mass number
Solution
- A nuclide is a species of an atom with a specific number of protons and neutrons in the nucleus leads a specific mass number.
- The nuclide concept (referring to individual nuclear species) emphasizes nuclear properties over chemical properties.
- for example, $$carbon-13$$ with $$6$$ protons and $$7$$ neutrons.

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Classification of Elements and Periodicity in Properties Test - 51

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Classification of Elements and Periodicity in Properties Test - 51

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Question 1

The second ionization enthalpy of oxygen element is greater than that of the fluorine element.

The first ionization enthalpy of phosphorus is greater than that of aluminium .

The first ionization enthalpy of aluminum is slightly greater than that of gallium.

The first ionization enthalpy of B is less than that of Be.

Solution

Question 2

$$O_2$$ and $$O_3$$

$$O_2$$ and $$N_2$$

$$O_3$$ and $$N_2$$

Oxides of sulphur and Nitrogen

Solution

Question 3

IE of $$F> Cl$$

$$IE \ of \ F^{-}> Cl^{-}$$

E.A of $$F< Cl$$

E.A of $$F^{+}> Cl^{+}$$

Solution

Question 4

17, 2

16, 4

15, 3

18, 2

Solution

Question 5

2.20 and 7.40

2.20 and 1.00

2.20 and 2.20

2.20 and 6.30

Solution

Question 6

5

7

8

9

Solution

Question 7

$$20$$

$$119$$

$$30$$

$$47$$

Solution

Question 8

$$Au > Ag\left( {I.{E_1}.} \right)$$

$$Cl > N\left( {E.{A_1}.} \right)$$

$$T{l^{ + 1}} > T{l^{ + 3}}\left( {stability} \right)$$

$$L{i^ + }\left( {aq.} \right) > B{e^{ + 2}}\left( {aq.} \right)\left( {atomic\ radius} \right)$$

Question 9

Cl (g) + e$$^{-}$$ $$\rightarrow $$Cl$$^{-}$$(g)

O$$^{-}$$ + $$e^{-}$$ $$\rightarrow $$ O$$^{2-}$$ (g)

O (g) + e$$^{-}$$$$\rightarrow$$ O$$^{-}$$(g)

S (g) + e$$^{-}$$$$\rightarrow$$ S$$^{-}$$ (g)

Solution

Question 10

specific atomic number

same numbers of proton

same numbers of neutrons

specific atomic number and mass number

Solution

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