# Complete Electron Configuration for Krypton (Kr)

Krypton is the 36th element in the periodic table and its symbol is ‘Kr’. Krypton is a classified noble gas. In this article, I have discussed in detail how to easily write the complete electron configuration of krypton.

## What is the electron configuration of krypton?

The total number of electrons in krypton is thirty-six. These electrons are arranged according to specific rules in different orbitals.

The arrangement of electrons in krypton in specific rules in different orbits and orbitals is called the electron configuration of krypton.

The electron configuration of krypton is [Ar] 3d^{10} 4s^{2} 4p^{6}, if the electron arrangement is through orbitals. Electron configuration can be done in two ways.

- Electron configuration through orbit (Bohr principle)
- Electron configuration through orbital (Aufbau principle)

Electron configuration through orbitals follows different principles. For example Aufbau principle, Hund’s principle, and Pauli’s exclusion principle.

## Krypton atom electron configuration 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. The complete idea of the orbit is given there.

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

K is the name of the first orbit, 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 |

For example,

- n = 1 for K orbit.

The maximum electron holding capacity in K orbit is 2n^{2}= 2 × 1^{2}= 2. - For L orbit, n = 2.

The maximum electron holding capacity in L orbit is 2n^{2}= 2 × 2^{2}= 8. - n=3 for M orbit.

The maximum electron holding capacity in M orbit is 2n^{2}= 2 × 3^{2 }= 18. - n=4 for N orbit.

The maximum electron holding capacity in N orbit is 2n^{2}= 2 × 4^{2}= 32.

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 krypton is 36. That is, the number of electrons in krypton is thirty-six.

Therefore, the krypton atom will have two electrons in the first shell, eight in the 2nd orbit, eighteen electrons in the 3rd shell, and the remaining eight electrons will be in the fourth shell.

Therefore, the order of the number of electrons in each shell of the krypton atom is 2, 8, 18, 8. Electrons can be arranged correctly through orbits from elements 1 to 18.

The electron configuration of an element with an atomic number greater than 18 cannot be properly determined according to the Bohr atomic model. The electron configuration of all the elements can be done through the orbital diagram.

## Electron configuration of krypton 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 orbital | 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} |

For example,

- 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.

Subshell 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. The method of entering electrons into orbitals through the Aufbau principle is 1s 2s 2p 3s 3p 4s 3d 4p 5s 4d 5p 6s 4f 5d 6p 7s 5f 6d.

The first two electrons of krypton enter the 1s orbital. The s-orbital can have a maximum of two electrons. Therefore, the next two electrons enter the 2s orbital.

The p-orbital can have a maximum of six electrons. So, the next six electrons enter the 2p orbital. The second orbit is now full. So, the remaining electrons will enter the third orbit.

Then two electrons will enter the 3s orbital and the next six electrons will be in the 3p orbital of the third orbit. The 3p orbital is now full. So, the next two electrons will enter the 4s orbital and ten electrons will enter the 3d orbital.

The 3d orbital is now full of electrons. So, the remaining six electrons enter the 4p orbital. Therefore, the krypton complete electron configuration will be 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{10} 4s^{2} 4p^{6}.

Note:The unabbreviated electron configuration of krypton is [Ar] 3d^{10}4s^{2}4p^{6}. When writing an electron configuration, you have to write serially.

## Video for writing the electron configuration for Krypton (Kr)

## Why is krypton inert gas?

Ground state electron configuration of krypton is 1s^{2} 2s^{2} 2p^{6} 3s^{2} 3p^{6} 3d^{10} 4s^{2} 4p^{6}. This electron configuration shows that the last shell of krypton has eight electrons. Therefore, the valence electrons of krypton are eight.

The elements in group-18 of the periodic table are inert gases. The inert gases of Group-18 are helium(He), neon(Ne), argon(Ar), krypton(Kr), xenon(Xe), and radon(Rn).

We know that the element in group-18 is krypton. The electron configuration shows that the orbit at the end of krypton is filled with electrons.

Krypton does not want to exchange or share any electrons because the last orbit is full of electrons and krypton does not form any compounds because it does not share any electrons.

They do not participate in chemical bonding and chemical reactions. For this, they are called inert elements. The inert elements are in the form of gases at normal temperatures. For this inert elements are called inert gases. Again for this same reason, inert gas is called a noble gas.

## FAQs

### What is the symbol for krypton?

**Ans:**The symbol for krypton is ‘Kr’.### How many electrons does krypton have?

**Ans:**36 electrons.### How do you write the full electron configuration for krypton?

**Ans:**The full electron configuration for krypton is 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}.### How many valence electrons does krypton have?

**Ans:**Eight valence electrons.### What is the valency of krypton?

**Ans:**The valency of krypton is 0.### What is the valence electron configuration for the krypton atom?

**Ans:**The valence electron configuration for krypton atom is 4s^{2}4p^{6}.

There are a total of 8 valence electrons in krypton’s outermost energy level, with 2 in the 4s subshell and 6 in the 4p subshell.### How many orbitals does krypton have?

**Ans:**18 orbitals. 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.### What is the complete ground state electron configuration for the krypton atom?

**Ans:**The complete ground state electron configuration for the krypton atom is 1s^{2}2s^{2}2p^{6}3s^{2}3p^{6}3d^{10}4s^{2}4p^{6}.### How many energy levels does krypton have?

**Ans:**Krypton has a total of four energy levels. The order of the number of electrons in each energy level of the krypton atom is 2, 8, 18, 8.### How many energy levels are filled in a krypton atom?

**Ans:**Krypton atoms have a total of four energy levels. Among these, the first three energy levels are filled with electrons. A total of eight electrons occupy the fourth energy level of krypton, i.e. complete the octave.### What is the noble gas configuration for krypton?

**Ans:**The noble gas configuration for krypton is [Ar] 3d^{10}4s^{2}4p^{6}.### How many p-orbitals are occupied by electrons in a krypton atom when in its ground state?

**Ans:**A krypton atom has a total of three p-orbitals. They are 2p, 3p, 4p. The p-orbital can hold a maximum of six electrons. In the ground state of a krypton atom, three p-orbitals are occupied by electrons and all orbitals are filled with electrons.### How many unpaired electrons are present in the ground state kr atom?

**Ans:**All the orbitals of the krypton atom are filled with electrons. That is, there are no unpaired electrons in the krypton atom in the ground state.### How many electrons are there in the outer most level of krypton (kr)?

**Ans:**8 electrons. The order of the number of electrons in each shell of the krypton atom is 2, 8, 18, 8.### How many orbitals are occupied by electrons in the 4p subshell of a krypton atom when in its ground state?

**Ans:**6 electrons. The orbital number of the p-subshell is three and each orbital can have a maximum of two electrons. They are 4p_{x}, 4p_{y}, and 4p_{z}. The sub-shell ‘p’ can hold a maximum of six electrons. All the orbitals of the krypton atom are filled with electrons. All the orbitals of the krypton atom are filled with electrons. That is, in the ground state, all three orbitals of the 4p subshell are filled with a total of six electrons.