Question

The ________ ion is represented by the electron configuration [ar]3d2.

Answer 1

The Ti 2+ ions is  represented  by  electron  configuration  (Ar)3d2. Titanium is in  atomic  number  22  and  its  electronic  configuration  is  (Ar)3d2 4s2.  Titanium loss two  electron that  is  4s2 electrons  hence the  electronic  configuration ( Ar)3d2.  4s2 is  the  valence electron  hence  it   the  one   which  is  lost  to  form  Ti2+

Answer 2

The ion which represent by the electronic configuration $\left[ {{\text{Ar}}} \right]3{d^2}$ is $\boxed{{\text{T}}{{\text{i}}^{2 + }}}$

Further Explanation:

The electronic configuration 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. When an electron jumps from the stable ground state to some higher level, that state is called the excited state and the electronic configuration corresponding to this state is known as the excited-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: The principle states that the electrons are filled in various orbitals in the increasing order of their energies as follows:

$1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d < 7p$

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 general expression for full electron configuration contains all the symbols of occupied. It is given as follows:

$n{\left( {{\text{symbol for }}l} \right)^{{\text{ number of electrons in orbital}}}}$

For example, Boron has atomic number 5. Therefore, filling of electrons for boron takes place as follows:

Full Electronic configuration: $1{s^2}2{s^2}3{s^1}$

The condensed electronic configuration is a way to write the electronic configuration where the inner shell configurations are compressed to the nearest noble gas configuration and represent in a square bracket and only the valence shell configuration is written in the expanded form.

Condensed electronic configuration for boron is as follows:

$\left[ {{\text{He}}} \right]2{s^2}3{s^1}$

Given electronic $\left[ {{\text{Ar}}} \right]3{d^2}$ configuration is a condensed electronic configuration in which Ar is a atomic symbol of argon noble gas. Noble gas argon has an atomic number 18, therefore, electrons present in argon are 18. Also, there are 2 electrons present in the 3d orbital. Therefore, total number of electron present in the given element is 20.

According to the Aufbau principle, the given electronic configuration can be represented as $\left[ {{\text{Ar}}} \right]4{s^0}3{d^2}$. Since two electrons are removed from the 4s orbital thus ion contains 22 initially. According to the periodic table, the element with the 22 atomic number is titanium (Ti) and after the loss 2 electrons it becomes ${\text{T}}{{\text{i}}^{2 + }}$.

Learn more:

1. What happens to the reducing agent during redox reaction?: brainly.com/question/2890416

2. Identification of element which has electron configuration  :brainly.com/question/9616334

Answer details:

Grade: High School

Subject: Chemistry

Chapter: Electronic configuration of the elements

Keywords: neutral element, electronic configuration, element, electronic, titanium, 22, 20, electrons, Ar, 3d2, Ti2+.