# Electronic configuration of the atom

**The electronic configuration of an atom** is a formula showing the arrangement of electrons in an atom by levels and
sublevels. After studying the article, you will learn where and how electrons are located, get acquainted with quantum numbers and
you will be able to build an electronic configuration of an atom by its number, at the end of the article there is a table of elements.

## Why study the electronic configuration of elements?

Atoms as a constructor: there are a certain number of details, they differ from each other, but two details
the same type are exactly the same. But this constructor is much more interesting than a plastic one and that's why.
The configuration changes depending on who is nearby. For example, oxygen next to hydrogen *can*
it turns into water, next to sodium into gas, and being next to iron turns it into rust at all.
To answer the question of why this happens and to predict the behavior of an atom next to another is necessary
to study the electronic configuration, which will be discussed below.

## How many electrons are there in an atom?

An atom consists of a nucleus and electrons rotating around it, a nucleus consists of protons and neutrons. In neutral in the state of each atom, the number of electrons is equal to the number of protons in its nucleus. Quantity protons are designated by the ordinal number of the element, for example, sulfur has 16 protons - the 16th element of the periodic table the system. Gold has 79 protons - the 79th element of the periodic table. Accordingly, in sulfur in neutral there are 16 electrons in the state, and 79 electrons in gold.

## Where to look for an electron?

Observing the behavior of the electron, certain patterns were deduced, they are described quantum numbers, there are four of them in total:

- The main quantum number
- Orbital quantum number
- Magnetic quantum number
- Spin quantum number

### Orbital

Next, instead of the word orbit, we will use the term "orbital", the orbital is the wave function of an electron, roughly, this is the area where the electron spends 90% of the time.

N - level

L - shell

M_{l}- orbital number

M_{s}- the first or second electron in the orbital

### Orbital quantum number l

As a result of the study of the electron cloud, we found that depending on the energy level, the cloud takes four main forms: a ball, dumbbells and the other two, more complex. In order of increasing energy, these forms are called s-, p-, d- and f-shells. On each of these shells there can be 1 (on s), 3 (on p), 5 (on d) and 7 (on f) orbitals. The orbital quantum number is the shell on which the orbitals. The orbital quantum number for s,p,d and f-orbitals, respectively , takes the values 0,1,2 or 3.

There is one orbital on the s-shell (L=0) - two electrons

There are three orbitals on the p-shell (L=1) - six electrons

There are five orbitals on the d-shell (L=2) - ten electrons

There are seven orbitals on the f-shell (L=3) - fourteen electrons

### Magnetic quantum number m_{l}

There are three orbitals on the p-shell, they are denoted by numbers
from -L to +L, that is, for the p-shell (L=1) there are orbitals "-1", "0" and "1".
The magnetic quantum number is denoted by the letter m_{l}.

It 's easier for electrons inside the shell they are located in different orbitals, so the first electrons fill one for each the orbital, and then each is joined by its pair.

Consider the d-shell:

the d-shell corresponds to the value L=2, that is, five orbitals (-2,-1,0,1 and 2), the first five electrons fill the shell taking the values M_{l}=-2,M_{l}=-1,M_{l}=0, M_{l}=1,M_{l}=2.

### Spin quantum number m_{s}

Spin is the direction of rotation of an electron around its axis, there are two directions, so the spin quantum number
it has two values: +1/2 and -1/2. There can be two electrons on the same energy sublevel only with
opposite backs. The spin quantum number is denoted by m_{s}

### The main quantum number n

The main quantum number is the energy level, at the moment seven energy levels are known, each is denoted by an Arabic numeral: 1,2,3,...7. The number of shells at each level is equal to the level number: on the first level there is one shell, on the second two, etc.

## Electron number

So, any electron can be described by four quantum numbers, the combination of these numbers is unique for each
electron positions, take the first electron, the lowest energy level is N=1, at the first level
there is one shell, the first shell at any level has the shape of a ball (s-shell), i.e. L=0,
a magnetic quantum number can take only one value, M_{l}=0 and the spin will be +1/2.
If we take the fifth electron (in whatever atom it is), then the main quantum numbers for it will be:
N=2, L=1, M= -1, spin 1/2.

Energy levels with sublevels are shown below for clarity, the levels are located from top to bottom and the sublevels are separated by color:

1 | |||||||||||||||||||
---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|---|

2 | |||||||||||||||||||

3 | |||||||||||||||||||

4 | |||||||||||||||||||

5 | |||||||||||||||||||

6 | |||||||||||||||||||

7 | |||||||||||||||||||

8 | |||||||||||||||||||

Table 1. Electron distribution by energy levels |

Here, the energy levels (1-7) are shown from top to bottom, from left to right they are divided into groups. sublevels (s,p,d, f), in each cell there are two electrons in opposite directions. General the principle of electron distribution is such that the energy sublevels are filled in the order of the sum of the main and the orbital quantum numbers, that is: 1S, 2S, 2P, 3S, 3P, 4S, 3D and so on, if the sum is the same, then first , the level with the smaller main quantum number N is filled in.

Some elements have deviations in the formation of the electronic configuration, namely
_{24}Cr,
_{29}Cu,
_{41}Nb,
_{42}Mo,
_{44}Ru,
_{45}Rh,
_{46}Pd,
_{47}Ag,
_{78}Pt,
_{79}Au

## Elements

Check yourself, make an electronic configuration for the elements #5, #12and #19, then check yourself in the table below.

№ |
| |||
---|---|---|---|---|

1 | H | 1s ^{1} |
1 | |

2 | He | 1s ^{2} |
1 | |

3 | Li | 1s ^{2}2s ^{1} |
2 | |

4 | Be | berillii | 1s ^{2}2s ^{2} |
2 |

5 | B | 1s ^{2}2s ^{2}2p ^{1} |
2 | |

6 | C | 1s ^{2}2s ^{2}2p ^{2} |
2 | |

7 | N | 1s ^{2}2s ^{2}2p ^{3} |
2 | |

8 | O | 1s ^{2}2s ^{2}2p ^{4} |
2 | |

9 | F | 1s ^{2}2s ^{2}2p ^{5} |
2 | |

10 | Ne | nothe | 1s ^{2}2s ^{2}2p ^{6} |
2 |

11 | Na | 1s ^{2}2s ^{2}2p ^{6}3s ^{1} |
3 | |

12 | Mg | 1s ^{2}2s ^{2}2p ^{6}3s ^{2} |
3 | |

13 | Al | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{1} |
3 | |

14 | Si | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{2} |
3 | |

15 | P | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{3} |
3 | |

16 | S | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{4} |
3 | |

17 | Cl | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{5} |
3 | |

18 | Ar | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6} |
3 | |

19 | K | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{1} |
4 | |

20 | Ca | kalbcii | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2} |
4 |

21 | Sc | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{1} |
4 | |

22 | Ti | titAn | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{2} |
4 |

23 | V | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{3} |
4 | |

24 | Cr | hrom | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{1}3d^{5} |
4 |

25 | Mn | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{5} |
4 | |

26 | Fe | wateezoh | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{6} |
4 |

27 | Co | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{7} |
4 | |

28 | Ni | hikateb | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{8} |
4 |

29 | Cu | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{1}3d^{10} |
4 | |

30 | Zn | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10} |
4 | |

31 | Ga | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{1} |
4 | |

32 | Ge | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{2} |
4 | |

33 | As | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{3} |
4 | |

34 | Se | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{4} |
4 | |

35 | Br | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{5} |
4 | |

36 | Kr | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6} |
4 | |

37 | Rb | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{1} |
5 | |

38 | Sr | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2} |
5 | |

39 | Y | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{1} |
5 | |

40 | Zr | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{2} |
5 | |

41 | Nb | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{1}4d^{4} |
5 | |

42 | Mo | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{1}4d^{5} |
5 | |

43 | Tc | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{5} |
5 | |

44 | Ru | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{1}4d^{7} |
5 | |

45 | Rh | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{1}4d^{8} |
5 | |

46 | Pd | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}4d^{10} |
5 | |

47 | Ag | cerfuckro | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{1}4d^{10} |
5 |

48 | Cd | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10} |
5 | |

49 | In | andndii | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{1} |
5 |

50 | Sn | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{2} |
5 | |

51 | Sb | surma | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{3} |
5 |

52 | Te | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{4} |
5 | |

53 | I | yod | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{5} |
5 |

54 | Xe | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6} |
5 | |

55 | Cs | tsezeeth | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{1} |
6 |

56 | Ba | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2} |
6 | |

57 | La | lAnthatn | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}5d^{1} |
6 |

58 | Ce | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{2} |
6 | |

59 | Pr | nRazeodthem | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{3} |
6 |

60 | Nd | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{4} |
6 | |

61 | Pm | nrometith | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{5} |
6 |

62 | Sm | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{6} |
6 | |

63 | Eu | ebpopii | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{7} |
6 |

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

65 | Tb | terbith | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{9} |
6 |

66 | Dy | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{10} |
6 | |

67 | Ho | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{11} |
6 | |

68 | Er | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{12} |
6 | |

68 | Tm | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{13} |
6 | |

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

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

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

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

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

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

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

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

78 | Pt | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{1}4f^{14}5d^{9} |
6 | |

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

80 | Hg | rtutb | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10} |
6 |

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

82 | Pb | cveenotc | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{2} |
6 |

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

84 | Po | byloneitherth | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{4} |
6 |

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

86 | Rn | phellhe | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{1}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6} |
6 |

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

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

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

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

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

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

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

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

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

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

97 | Bk | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{8}6d^{1} |
7 | |

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

99 | Es | eynpcherneitherth | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{11} |
7 |

100 | Fm | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{12} |
7 | |

101 | Md | mendateherveeth | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{13} |
7 |

102 | No | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{14} |
7 | |

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

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

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

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

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

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

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

110 | Ds | darmstadt | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{14}6d^{8} |
7 |

111 | Rg | x-ray | 1s ^{2}2s ^{2}2p ^{6}3s ^{2}3p^{6}4s ^{2}3d^{10}4p^{6}5s^{2}4d^{10}5p^{6}6s^{2}4f^{14}5d^{10}6p^{6}7s^{2}5f^{14}6d^{9} |
7 |

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

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

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

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

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

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

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

Table 2. Electronic configuration of atoms |

If you want to learn how to make an electronic configuration, refer to the article «how to write an electronic configuration»

Quantum numbers of electrons in atoms