# How to Write the Electron Configuration for Titanium (Ti)

Titanium is the 22th element in the periodic table and the symbol is ‘Ti’. Titanium has an atomic number of 22, which means that its atom has 22 electrons around its nucleus.

**To write the electron configuration for titanium, the first two electrons enter the 1s orbital. Since the 1s orbital can hold only two electrons the next two will enter the 2s orbital. The next six electrons enter the 2p subshell. The p subshell can hold a maximum of six electrons. So first we put six electrons in the 2p subshell and then the next two electrons in the 3s orbital.**

**Since the 3s is now full, the electrons will move to the 3p subshell, where the next six electrons will enter. The 3p subshell is now full. Consequently, the following two electrons will enter the 4s orbital. Since the 4s orbital is now full, the remaining two electrons will move into the 3d subshell. Hence, the electron configuration of titanium will be 1s ^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{2}.**

The electron configuration of titanium refers to the arrangement of electrons in the titanium atom’s orbitals. It describes how electrons are distributed among the various atomic orbitals and energy levels, and provides a detailed map of where each electron is likely to be found.

To understand the mechanism of titanium electron configuration, you need to understand two basic things. These are orbits and orbitals. Also, you can arrange electrons in those two ways. In this article, I have discussed all the necessary points to understand the mechanism of titanium electron configuration. I hope this will be helpful in your study.

## Electron arrangement of Titanium through orbit

Scientist Niels Bohr was the first to give an idea of the atom’s orbit. He provided a model of the atom in 1913 and provided a complete idea of orbit in that model.

The electrons of the atom revolve around the nucleus in a certain circular path. These circular paths are called orbits (shells or energy levels). These orbits are expressed by n. [n = 1,2,3,4 . . . The serial number of the orbit]

The name of the first orbit is K, L is the second, M is the third, and N is the name of the fourth orbit. The electron holding capacity of each orbit is 2n^{2}.

Shell Number (n) | Shell Name | Electrons Holding Capacity (2n^{2}) |

1 | K | 2 |

2 | L | 8 |

3 | M | 18 |

4 | N | 32 |

### Explanation:

- Let, n = 1 for K orbit. So, the maximum electron holding capacity in the K orbit is 2n
^{2}= 2 × 1^{2}= 2 electrons. - n = 2, for L orbit. The maximum electron holding capacity in the L orbit is 2n
^{2}= 2 × 2^{2}= 8 electrons. - n=3 for M orbit. The maximum electron holding capacity in the M orbit is 2n
^{2}= 2 × 3^{2 }= 18 electrons. - n=4 for N orbit. The maximum electron holding capacity in N orbit is 2n
^{2}= 2 × 4^{2}= 32 electrons.

Therefore, the maximum electron holding capacity in the first shell is two, the second shell is eight and the 3rd shell can have a maximum of eighteen electrons.

The atomic number is the number of electrons in that element. The atomic number of titanium is 22. That is, the number of electrons in titanium is twenty-two. Therefore, the titanium atom will have two electrons in the first shell, and eight in the 2nd shell.

According to Bohr’s formula, the third orbit will have twelve electrons but the third orbit of titanium will have ten electrons and the remaining two electrons will be in the fourth orbit. Therefore, the order of the number of electrons in each shell of the titanium atom is 2, 8, 10, 2.

The Bohr atomic model has many limitations. In the Bohr atomic model, the electrons can only be arranged in different shells but the exact position, orbital shape, and spin of the electron cannot be determined.

Also, electrons can be arranged correctly from 1 to 18 elements. The electron arrangement of any element with atomic number greater than 18 cannot be accurately determined by the Bohr atomic model following the 2n^{2} formula. We can overcome all limitations of the Bohr model following the electron configuration through orbital.

## Electron configuration of Titanium through orbital

Atomic energy shells are subdivided into sub-energy levels. These sub-energy levels are also called orbital. The most probable region of electron rotation around the nucleus is called the orbital.

The sub-energy levels depend on the azimuthal quantum number. It is expressed by ‘l’. The value of ‘l’ is from 0 to (n – 1). The sub-energy levels are known as s, p, d, and f.

Orbit Number | Value of ‘l’ | Number of subshells | Number of orbitals | Subshell name | Electrons holding capacity | Electron configuration |

1 | 0 | 1 | 1 | 1s | 2 | 1s^{2} |

2 | 0 1 | 2 | 1 3 | 2s 2p | 2 6 | 2s^{2} 2p^{6} |

3 | 0 1 2 | 3 | 1 3 5 | 3s 3p 3d | 2 6 10 | 3s^{2} 3p^{6} 3d^{10} |

4 | 0 1 2 3 | 4 | 1 3 5 7 | 4s 4p 4d 4f | 2 6 10 14 | 4s^{2} 4p^{6} 4d^{10} 4f^{14} |

### Explanation:

- If n = 1,

(n – 1) = (1–1) = 0

Therefore, the value of ‘l’ is 0. So, the sub-energy level is 1s. - If n = 2,

(n – 1) = (2–1) = 1.

Therefore, the value of ‘l’ is 0, 1. So, the sub-energy levels are 2s, and 2p. - If n = 3,

(n – 1) = (3–1) = 2.

Therefore, the value of ‘l’ is 0, 1, 2. So, the sub-energy levels are 3s, 3p, and 3d. - If n = 4,

(n – 1) = (4–1) = 3

Therefore, the value of ‘l’ is 0, 1, 2, 3. So, the sub-energy levels are 4s, 4p, 4d, and 4f. - If n = 5,

(n – 1) = (n – 5) = 4.

Therefore, l = 0,1,2,3,4. The number of sub-shells will be 5 but 4s, 4p, 4d, and 4f in these four subshells it is possible to arrange the electrons of all the elements of the periodic table.

Sub-shell name | Name source | Value of ‘l’ | Value of ‘m’(0 to ± l) | Number of orbital (2l+1) | Electrons holding capacity2(2l+1) |

s | Sharp | 0 | 0 | 1 | 2 |

p | Principal | 1 | −1, 0, +1 | 3 | 6 |

d | Diffuse | 2 | −2, −1, 0, +1, +2 | 5 | 10 |

f | Fundamental | 3 | −3, −2, −1, 0, +1, +2, +3 | 7 | 14 |

The orbital number of the s-subshell is one, three in the p-subshell, five in the d-subshell, and seven in the f-subshell. Each orbital can have a maximum of two electrons.

The sub-energy level ‘s’ can hold a maximum of two electrons, ‘p’ can hold a maximum of six electrons, ‘d’ can hold a maximum of ten electrons, and ‘f’ can hold a maximum of fourteen electrons.

Aufbau is a German word, which means building up. The main proponents of this principle are scientists Niels Bohr and Pauli. The Aufbau method is to do electron configuration through the sub-energy level.

The Aufbau principle is that the electrons present in the atom will first complete the lowest energy orbital and then gradually continue to complete the higher energy orbital.

The energy of an orbital is calculated from the value of the principal quantum number ‘n’ and the azimuthal quantum number ‘l’. The orbital for which the value of (n + l) is lower is the low energy orbital and the electron will enter that orbital first.

Orbital | Orbit (n) | Azimuthal quantum number (l) | Orbital energy (n + l) |

3d | 3 | 2 | 5 |

4s | 4 | 0 | 4 |

Here, the energy of 4s orbital is less than that of 3d. So, the electron will enter the 4s orbital first and enter the 3d orbital when the 4s orbital is full.

Following the Aufbau principle, the sequence of entry of electrons into orbitals is 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d 7p.

Therefore, the complete electron configuration for titanium should be written as 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 4s^{2} 3d^{2}.

Note:The abbreviated electron configuration of titanium is [Ar] 3d^{2}4s^{2}. When writing an electron configuration, you have to write serially.

## The excited state electron configuration of Titanium

Atoms can jump from one orbital to another orbital in an excited state. This is called quantum jump. The ground state electron configuration of titanium is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{2} 4s^{2}. We already know that the p-subshell has three orbitals. The orbitals are p_{x}, p_{y}, and p_{z} and each orbital can have a maximum of two electrons.

In the titanium ground-state electron configuration, the two electrons of the 3d orbital are located in the d_{xy} and d_{yz} orbitals. We already know that the d-orbital has five orbitals. The orbitals are d_{xy}, d_{yz}, d_{zx}, d_{x2-y2} and d_{z2} and each orbital can have a maximum of two electrons.

Then the correct electron configuration of titanium in the ground state will be 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d_{xy}^{1} 3d_{yz}^{1} 4s^{2}. This electron configuration shows that the titanium atom has two unpaired electrons(3d_{xy}^{1} 3d_{yz}^{1}). So the valency of titanium is 2.

When a titanium atom is excited, then the titanium atom absorbs energy. As a result, an electron in the 4s orbital jumps to the 4p_{x} orbital. Therefore, the electron configuration of titanium(Ti*) in an excited state will be 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d_{xy}^{1} 3d_{yz}^{1} 4s^{1} 4p_{x}^{1}. The valency of the element is determined by electron configuration in the excited state.

Here, titanium has four unpaired electrons. Therefore, the valency of titanium is 4. From the above information, we can say that titanium exhibits variable valency. Therefore, the valency of titanium is 2, 4. Due to this, the oxidation states of titanium are +2, and +4.

## Titanium ion(Ti^{2+}, Ti^{3+}, Ti^{4+}) electron configuration

The electron configuration of titanium shows that the last shell of titanium has two electrons and the d-orbital has a total of two electrons. Therefore, the valence electrons of titanium are four.

Titanium has three oxidation states. These are 2+, 3+, 4+. That is, the titanium atom can have three ions. The titanium atom donates two electrons from the last shell to form the titanium ion(Ti^{2+}).

Ti – 2e^{–} → Ti^{2+}

The electron configuration of this titanium ion(Ti^{2+}) is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{2}. The titanium atom donates two electrons in 4s orbital and an electron in 3d orbital to convert to titanium ion(Ti^{3+}).

Ti – 3e^{–} → Ti^{3+}

The electron configuration of this titanium ion(Ti^{3+}) is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{1}. The titanium atom donates two electrons in 4s orbital and two electrons in 3d orbital to convert to titanium ion(Ti^{4+}).

Ti – 4e^{–} → Ti^{4+}

The electron configuration of this titanium ion(Ti^{4+}) is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6}. This electron configuration shows that the titanium ion(Ti^{4+}) has acquired the electron configuration of argon and it achieves an octave full stable electron configuration.

## Compound formation of titanium

Titanium participates in the formation of bonds through its valence electrons. This valence electron participates in the formation of bonds with atoms of other elements.

Titanium atoms form bonds by sharing electrons with oxygen atoms. The electron configuration of oxygen shows that oxygen has six valence electrons.

Two oxygen atoms and one titanium atom make titanium dioxide(TiO_{2}) compounds by sharing electrons. As a result, the oxygen atom completes its octave and acquires the electron configuration of neon.

On the other hand, titanium acquires the electron configuration of argon. Therefore, one titanium atom shares electrons with two oxygen atoms to form the titanium dioxide(TiO_{2}) compound through covalent bonding.