Question

What is the ground state configuration of Cr2+, Cu2+ and Co3+?

Answer 1

Explanation:

Atomic number of chromium is 24 and electronic configuration of $Cr^{2+}$ is as follows.

     $Cr^{2+}$ : $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{0}3d^{4}$

Atomic number of copper is 29 and electronic configuration of $Cu^{2+}$ is as follows.

     $Cu^{2+}$ : $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{0}3d^{9}$  

Atomic number of cobalt is 27 and electronic configuration of $Co^{3+}$ is as follows.

      $Co^{3+}$ : $1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}4s^{0}3d^{6}$  

Answer 2

The ground-state electronic configuration of ${\text{C}}{{\text{r}}^{2 + }}$ is $\boxed{1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^4}}$.

The ground-state electronic configuration of ${\text{C}}{{\text{u}}^{2 + }}$ is $\boxed{1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^9}}$.

The ground-state electronic configuration of ${\text{C}}{{\text{o}}^{3 + }}$ is $\boxed{1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^6}}$.

Further Explanation:

Electronic configuration:

It is the distribution of electrons of an atom in the atomic orbitals. There are two states for an electron: ground as well as the excited state. The configuration of the atom in the lowest possible energy levels is called the ground-state electronic configuration.

The filling of electrons in different energy levels or orbitals is done in accordance with the following three rules.

1. Aufbau principle: It states that the electrons are filled in various orbitals in the increasing order of their energies as follows:

$1s$

2. Hund’s rule: Electron pairing will not start until each orbital is singly occupied.

3. Pauli’s exclusion principle: According to this principle, all the four quantum numbers $\left( {n,\;l,\;{m_l},\;{m_s}} \right)$ for any two electrons can never be the same. In an orbital, the spin of two electrons has to be different. If one electron has the clockwise spin, the other would have the anticlockwise spin and vice-versa.

The atomic number of chromium (Cr) is 24 and its ground-state electronic configuration is $1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^4}$. It loses two 4s electrons to form ${\text{C}}{{\text{r}}^{2+}}$ and its ground-state electronic configuration becomes $1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^4}$.

The atomic number of copper (Cu) is 29 and its ground-state electronic configuration is $1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^1}3{d^{10}}$. It loses one 4s electron and one 3d electron to form ${\text{C}}{{\text{u}}^{2 + }}$ and its ground-state electronic configuration becomes $1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^9}$.

The atomic number of cobalt (Co) is 27 and its ground-state electronic configuration is $1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}4{s^2}3{d^7}$. It loses two 4s electrons and one 3d electron to form ${\text{C}}{{\text{o}}^{3 + }}$ and its ground-state electronic configuration becomes $1{s^2}2{s^2}2{p^6}3{s^2}3{p^6}3{d^6}$.

Learn more:

1. Determine the ion with configuration $\left[ {{\text{Ar}}} \right]\;3{d^2}$: brainly.com/question/7599542

2. Identification of element which has electron configuration $1{s^2}2{s^2}2{p^2}3{s^1}$:brainly.com/question/9616334

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Electronic configuration of the elements

Keywords: ground-state electronic configuration, chromium, copper, cobalt, Cr2+, Cu2+, Co3+, Cr, Cu, Co, atomic number, 24, 29, 27, Aufbau principle, Pauli’s exclusion principle, Hund’s rule.