Write the electron configurations for the following ions:
2 answers:
Answer:
Co⁺²: 1s²2s²2p⁶3s²3p⁶3d⁷
Sn²⁺: 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰
Zr⁴⁺: 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶
Ag⁺: 1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s¹4d⁹
S²⁻: 1s²2s²2p⁶3s²3p⁶
Explanation:
The electronic configuration is the distribution of the electrons through the orbitals, which are represented by the levels (by numbers) and sublevels (by letters) in the energetic order, which is determined by the Linus Pauling's diagram (which is shown below).
The sublevels maximum number of electrons is:
s = 2, p =6, d= 10, and f = 14.
To do the configuration of ions, we must first do it for the neutral atom (number of electrons = atomic number), and then if it is a cation (positive charge), remove electrons from the valence sublevel (most energetic), and if it's an anion, to added electrons to the most energetic sublevel.
Co⁺²
Neutral atom: Co
Atomic number: 27
Electron configuration of neutral atom:
1s²2s²2p⁶3s²3p⁶4s²3d⁷
In this case, because the atom is a transition metal, the electrons must be removed from the 4s sublevel, and not from the 3d sublevel, because the ion will be more stable if the electrons are removed from the valence shell. So, 2 electrons must be removed (+2).
Ion configuration:
1s²2s²2p⁶3s²3p⁶3d⁷
Sn²⁺
Neutral atom: Sn
Atomic number: 50
The electron configuration of neutral atom:
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰5p²
Two electrons must be removed from the most energetic subshell (5s).
Ion configuration:
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d¹⁰
Zr⁴⁺
Neutral atom: Zr
Atomic number: 40
The electron configuration of neutral atom:
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d²
It must lose 4 electrons. So, it will lose the 2 electrons of 5s (as explained above for Co), and the 2 electrons of 4d, because after that it will be the most energetic sublevel.
Ion configuration:
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶
Ag⁺
Neutral atom: Ag
Atomic number: 47
The electron configuration of neutral atom:
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s²4d⁹
It must lose 1 electron, so, as explained above, it must be removed from 5s.
Ion configuration:
1s²2s²2p⁶3s²3p⁶4s²3d¹⁰4p⁶5s¹4d⁹
S²⁻
Neutral atom: S
Atomic number: 16
The electron configuration of neutral atom:
1s²2s²2p⁶3s²3p⁴
It must gain 2 electrons (2-), which will be added to the most energetic sublevel, 3p.
Ion configuration:
1s²2s²2p⁶3s²3p⁶
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A molecular orbital that decreases the electron density between two nuclei is said to be <u>antibonding.</u>
The bonding orbital, which would be more stable and encourages the bonding of the two H atoms into , is the orbital that is located in a less energetic state than just the electron shells of the separate atoms. The antibonding orbital, which has higher energy but is less stable, resists bonding when it is occupied.
An asterisk (sigma*) is placed next to the corresponding kind of molecular orbital to indicate an antibonding orbital. The antibonding orbital known as * would be connected to sigma orbitals, as well as antibonding pi orbitals are known as * orbitals.
Therefore, molecular orbital that decreases the electron density between two nuclei is said to be <u>antibonding.</u>
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Hence, the correct answer will be option (b)
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To know more about molecular orbital
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