Periodic Classification of Elements - Class 10th Science

Electronic configuration of copper

(25) Electronic configuration of Mn (Manganese)

The atomic number of Mn (Manganese) = 25

Electronic configuration of Mn (Manganese) = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁵

[∵ 4s orbital has less energy level than 3d orbital, thus electrons will fill 4s before filling the 3d orbital (According to Aufbau's Principle). And in the case of Mn (Manganese) after completely filling the 4s orbital electrons started to fill the 3d orbital.]

Now after rearranging, the electronic configuration of Mn (Manganese) can be written as

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁵ 4s²

[In this rearrangement orbital 3d is written before 4s.]

Or, Electronic configuration of Mn (Manganese) : [Ar] 4s² 3d⁵

Or, Electronic configuration of Mn (Manganese) : [Ar] 3d⁵ 4s²

[Here, Ar (Arsenic) is an inert gas nearest to the Mn (Manganese). Because of this electronic configuration of Mn (Manganese) is written after writing Ar (Arsenic) in the bracket.]

Or, Electronic configuration of Mn (Manganese): 2, 8, 8, 7

Valence electrons of Mn (Manganese) = Number of electrons in the outermost orbit = 7

∵ last electron enters in d–orbital of Mn (Manganese) thus, Mn (Manganese) is a d–block element.

Position of Mn (Manganese) in Periodic Table

Period Number of Mn (Manganese) in the periodic table: 4^th period

[∵ after observing the electronic configuration it becomes clear that there are four orbits in the atom of Mn (Manganese).]

Group number of Mn (Manganese) in the periodic table: 7 B

[Since the valence electron is equal to 7 and the last electron fills the d– orbital]

Block of manganese in the periodic table : d–block.

[∵ the last electron fills the d–orbital.]

(26) Electronic configuration of Fe (Iron)

The atomic number of Fe (Iron) = 26

Electronic configuration of Fe (Iron) = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶

[∵ 4s orbital has less energy level than 3d orbital, thus electrons will fill 4s before filling the 3d orbital (According to Aufbau's Principle). And in the case of Fe (Iron) after completely filling the 4s orbital electrons started to fill the 3d orbital.]

Now after rearranging, the electronic configuration of Fe (Iron) can be written as

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁶ 4s²

[In this rearrangement orbital 3d is written before 4s.]

Or, Electronic configuration of Fe (Iron) : [Ar] 4s² 3d⁶

Or, Electronic configuration of Fe (Iron) : [Ar] 3d⁶ 4s²

Or, Electronic configuration of Fe(Iron) : 2, 8, 8, 6, 2

[Here, Ar (Arsenic) is an inert gas nearest to the Fe (Iron). Because of this electronic configuration of Fe (Iron) is written after writing Ar (Arsenic) in the bracket.]

Calculation of Valence electrons for d–block element

Total number of electrons in outermost orbit + Total number of electrons in penultimate orbit – 8

= 2 + 14 – 8

= 16 – 8

= 8

Thus, valence electrons of Fe (Iron) = 8

[Special rule is followed while calculating the valence electrons of Fe(Iron), Co(cobalt), Ni(Nickel), Cu (Copper) and Zn(Zinc). If number of valence electrons = 8, 9 or 10 then the group number is equal for d–block elements = 8B. And if the valence electrons = 11, then group number is 1^stB. And if the valence electrons = 12, then group number is 2^ndB.]

Position of Fe (Iron) in the Periodic Table

Period Number of Fe (Iron) in the periodic table: 4^th period

[∵ after observing the electronic configuration it becomes clear that there are four orbits in the atom of Fe (Iron).]

Group number of Fe (Iron) in the periodic table: 8 B (8^th column in the Modern Periodic Table)

[∵ valence electron is equal to 8 and the last electron fills the d– orbital, thus group number is 8B.]

Block of Fe (Iron) in periodic table : d–block.

[∵ the last electron fills the d–orbital, thus Fe(Iron) is a d–block element.]

Properties of element [Fe (Iron)]: Transition element (Metallic)

[All d–block elements are transition elements and possess metallic character. Transition elements show multi valency and multi oxidation states. Transition elements have valence electrons between 3 to 12]

(27) Electronic configuration of Co (Cobalt)

Atomic number of Co (Cobalt) = 27

Electronic configuration of Fe (Iron) = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁷

[∵ 4s orbital has less energy level than 3d orbital, thus electrons will fill 4s before filling the 3d orbital (According to Aufbau's Principle). And in the case of Co (Cobalt) after completely filling the 4s orbital electrons started to fill the 3d orbital.]

Now after rearranging, the electronic configuration of Co (Cobalt) can be written as

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁷ 4s²

[In this rearrangement orbital 3d is written before 4s.]

Or, Electronic configuration of Co (Cobalt) : [Ar] 4s² 3d⁷

Or, Electronic configuration of Co (Cobalt) : [Ar] 3d⁷ 4s²

Or, Electronic configuration of Co(Cobalt) : 2, 8, 8, 7, 2

[Here, Ar (Arsenic) is an inert gas nearest to the Co (Cobalt). Because of this electronic configuration of Co (Cobalt) is written after writing Ar (Arsenic) in the bracket.]

Calculation of Valence electrons for d–block element

Total number of electrons in outermost orbit + Total number of electrons in penultimate orbit – 8

= 2 + 15 – 8

= 17 – 8

= 9

Thus, valence electrons of Co (Cobalt) = 9

[Special rule is followed while calculating the valence electrons of Fe(Iron), Co(cobalt), Ni(Nickel), Cu (Copper), and Zn(Zinc). If number of valence electrons = 8, 9 or 10 then the group number is equal for d–block elements = 8B. And if the valence electrons = 11, then group number is 1^stB. And if the valence electrons = 12, then the group number is 2^ndB.]

Position of Co (Cobalt) in the Periodic Table

Period Number of Co (Cobalt) in the periodic table: 4^th period

[∵ after observing the electronic configuration it becomes clear that there are four orbits in the atom of Co (Cobalt).]

Group number of Co (Cobalt) in periodic table: 8 B (9^th column in Modern Periodic Table)

[∵ valence electron is equal to 8 and the last electron fills the d– orbital, thus group number is 8B.]

Block of Co (Cobalt) in periodic table : d–block.

[∵ the last electron fills the d–orbital, thus Co (Cobalt) is a d–block element.]

Properties of element [Co (Cobalt)] : Transition element (Metallic)

[All d–block elements are transition elements and possess metallic character. Transition elements show multi-valency and multi-oxidation states. Transition elements have valence electrons between 3 to 12]

(28) Electronic configuration of Ni (Nickel)

The atomic number of Ni (Nickel) = 28

Electronic configuration of Ni (Nickel) = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁸

[∵ 4s orbital has less energy level than 3d orbital, thus electrons will fill 4s before filling the 3d orbital (According to Aufbau's Principle). And in the case of Ni (Nickel) after completely filling the 4s orbital electrons started to fill the 3d orbital.]

Now after rearranging, the electronic configuration of Ni (Nickel) can be written as

1s² 2s² 2p⁶ 3s² 3p⁶ 3d⁸ 4s²

[In this rearrangement orbital 3d is written before 4s.]

Or, Electronic configuration of Ni (Nickel) : [Ar] 4s² 3d⁸

Or, Electronic configuration of Ni (Nickel) : [Ar] 3d⁸ 4s²

Or, Electronic configuration of Ni(Nickel) : 2, 8, 8, 8, 2

[Here, Ar (Arsenic) is an inert gas nearest to the Ni (Nickel). Because of this electronic configuration of Ni (Nickel) is written after writing Ar (Arsenic) in the bracket.]

Calculation of Valence electrons for d–block element

Total number of electrons in outermost orbit + Total number of electrons in penultimate orbit – 8

= 2 + 16 – 8

= 18 – 8

= 10

Thus, valence electrons of Ni (Nickel) = 10

Position of Ni (Nickel) in the Periodic Table

Period Number of Ni (Nickel) in the periodic table: 4^th period

[∵ after observing the electronic configuration it becomes clear that there are four orbits in the atom of Ni (Nickel).]

Group number of Ni (Nickel) in the periodic table : 8 B (10^th column in the Modern Periodic Table)

[∵ valence electron is equal to 8 and the last electron fills the d– orbital, thus group number is 8B.]

Block of Ni (Nickel) in periodic table : d–block.

[∵ the last electron fills the d–orbital, thus Ni (Nickel) is a d–block element.]

Properties of element [Ni (Nickel)]: Transition element (Metallic)

(29) Electronic configuration of Cu (Copper)

The atomic number of Cu (Copper) = 29

Electronic configuration of Cu (Copper) = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s¹ 3d¹⁰

[∵ 4s orbital has less energy level than 3d orbital, thus electrons will fill 4s before filling the 3d orbital (According to Aufbau's Principle). And in the case of Cu (Copper) after completely filling the 4s orbital electrons started to fill the 3d orbital.]

According to Hund's Rule, Completely half-filled orbitals are more stable than less than completely half-filled orbitals.

Thus, in the case of Cu (Copper) in order to make the atom stable, one electron from 4s goes to 3d, and the number of electrons in 3d becomes 10 instead of 9. In this way, there is only 1 (one) electron left in 4s instead of 2.

Thus, electronic configuration of Cu (Copper) becomes [Ar] 4s¹ 3d¹⁰

Now after rearranging, the electronic configuration of Cu (Copper) can be written as

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s¹

[In this rearrangement orbital 3d is written before 4s.]

Or, Electronic configuration of Cu (Copper) : [Ar] 4s¹ 3d¹⁰

Or, Electronic configuration of Cu (Copper) : [Ar] 3d¹⁰ 4s¹

Or, Electronic configuration of Cu (Copper) : 2, 8, 8, 10, 1

[Here, Ar (Arsenic) is an inert gas nearest to Cu (Copper). Because of this electronic configuration of Cu (Copper) is written after writing Ar (Arsenic) in the bracket.]

Calculation of Valence electrons for d–block element

Total number of electrons in outermost orbit + Total number of electrons in penultimate orbit – 8

= 2 + 17 – 8

= 19 – 8

= 11

Thus, valence electrons of Cu (Copper) = 11

Position of Cu (Copper) in the Periodic Table

Period Number of Cu (Copper) in the periodic table: 4^th period

[∵ after observing the electronic configuration it becomes clear that there are four orbits in the atom of Cu (Copper).]

Group number of Cu (Copper) in the periodic table: 1 B (11^th column in Modern Periodic Table)

[∵ valence electron is equal to 11 and the last electron fills the d– orbital, thus group number is 1B or 11B.]

Block of Cu (Copper) in periodic table : d–block.

[∵ last electron fills the d–orbital, thus Cu (Copper) is a d–block element.]

Properties of element [Cu (Copper)] : Transition element (Metallic)

(30) Electronic configuration of Zn (Zinc)

The atomic number of Zn (Zinc) = 28

Electronic configuration of Zn (Zinc) = 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰

[∵ 4s orbital has less energy level than 3d orbital, thus electrons will fill 4s before filling the 3d orbital (According to Aufbau's Principle). And in the case of Zn (Zinc) after completely filling the 4s orbital electrons started to fill the 3d orbital.]

Now after rearranging, the electronic configuration of Zn (Zinc) can be written as

1s² 2s² 2p⁶ 3s² 3p⁶ 3d¹⁰ 4s²

[In this rearrangement orbital 3d is written before 4s.]

Or, Electronic configuration of Zn (Zinc) : [Ar] 4s² 3d¹⁰

Or, Electronic configuration of Zn (Zinc) : [Ar] 3d¹⁰ 4s²

Or, Electronic configuration of Zn (Zinc) : 2, 8, 8, 10, 2

[Here, Ar (Arsenic) is an inert gas nearest to the Zn (Zinc). Because of this electronic configuration of Zn (Zinc) is written after writing Ar (Arsenic) in the bracket.]

Calculation of Valence electrons for d–block element

Total number of electrons in outermost orbit + Total number of electrons in penultimate orbit – 8

= 2 + 18 – 8

= 20 – 8

= 12

Thus, valence electrons of Zn (Zinc) = 12

Position of Zn (Zinc) in the Periodic Table

Period Number of Zn (Zinc) in the periodic table: 4^th period

[∵ after observing the electronic configuration it becomes clear that there are four orbits in the atom of Zn (Zinc).]

Group number of Zn (Zinc) in the periodic table: II B (2_ndB) (12^th column in Modern Periodic Table)

[∵ valence electron is equal to 8 and the last electron fills the d– orbital, thus group number is 8B.]

Block of Zn (Zinc) in periodic table : d–block.

[∵ the last electron fills the d–orbital, thus Zn (Zinc) is a d–block element.]

Properties of element [Zn (Zinc)]: Transition element (Metallic)

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