Question

please give me the correct answer of how to know the electronic configuration of all the elements. the most best answer will be marked as brainliest

Answer 1

1s

2s 2p

3s 3p 3d

4s 4p 4d 4f

5s 5p 5d 5f

6s 6p 6d

7s 7p

The subshells fill diagonally from upper right to lower left in the chart above:

First is 1s, then 2s, then 2p and 3s, then 3p and 4s.

Next comes 3d, 4p, and 5s. Then comes 4d, 5p, and 6s.

After that comes 4f, 5d, 6p, and 7s. Last comes 5f, 6d, and 7p.

 

For an atom with 118 electrons, the electron orbital configuration would be:

1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f145d10 6p6 7s2 5f14 6d10 7p6

Answer 2

1

Find your atom's atomic number. Each atom has a specific number of electrons associated with it. Locate your atom's chemical symbol on the periodic table. The atomic number is a positive integer beginning at 1 (for hydrogen) and increasing by 1 for each subsequent atom. The atom's atomic number is the number of protons of the atom - thus, it is also the number of electrons in an atom with zero charge.

2

Determine the charge of the atom.Uncharged atoms will have exactly the number of electrons as is represented on the periodic table. However, charged atoms (ions) will have a higher or lower number of electrons based on the magnitude of their charge. If you're working with a charged atom, add or subtract electrons accordingly: add one electron for each negative charge and subtract one for each positive charge.

For instance, a sodium atom with a +1 charge would have an electron taken away from its basic atomic number of 11. So, the sodium atom would have 10 electrons in total.

3

Memorize the basic list of orbitals. As an atom gains electrons, they fill different orbitals sets according to a specific order. Each set of orbitals, when full, contains an even number of electrons. The orbital sets are:

The s orbital set (any number in the electron configuration followed by an "s") contains a single orbital, and by Pauli's Exclusion Principle, a single orbital can hold a maximum of 2 electrons, so each s orbital set can hold 2 electrons.

The p orbital set contains 3 orbitals, and thus can hold a total of 6 electrons.

The d orbital set contains 5 orbitals, so it can hold 10 electrons.

The f orbital set contains 7 orbitals, so it can hold 14 electrons.

Remember the order of the letters with this mnemonic:[1]
Sober Physicists Don't Find Giraffes Hiding In Kitchens.

For atoms with even more electrons, the orbitals continue alphabetically past K, skipping letters already used.

4

Understand electron configuration notation. Electron configurations are written so as to clearly display the number of electrons in the atom as well as the number of electrons in each orbital. Each orbital is written in sequence, with the number of electrons in each orbital written in superscript to the right of the orbital name. The final electron configuration is a single string of orbital names and superscripts.

For example, here is a simple electron configuration: 1s2 2s2 2p6. This configuration shows that there are two electrons in the 1s orbital set, two electrons in the 2s orbital set, and six electrons in the 2p orbital set. 2 + 2 + 6 = 10 electrons total. This electron configuration is for an uncharged neon atom (neon's atomic number is 10.)

5

Memorize the order of the orbitals.Note that orbital sets are numbered by electron shell, but ordered in terms of energy. For instance, a filled 4s2 is lower energy (or less potentially volatile) than a partially-filled or filled 3d10, so the 4s shell is listed first. Once you know the order of orbitals, you can simply fill them according to the number of electrons in the atom. The order for filling orbitals is as follows: 1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d, 7p, 8s.

An electron configuration for an atom with every orbital completely filled would be written: 1s2 2s2 2p6 3s2 3p64s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d106p6 7s2 5f14 6d107p6

Note that the above list, if all the shells were filled, would be the electron configuration for Og (Oganesson), 118, the highest-numbered atom on the periodic table - so this electron configuration contains every currently known electron shell for a neutrally charged atom.

6

Fill in the orbitals according to the number of electrons in your atom. For instance, if we want to write an electron configuration for an uncharged calcium atom, we'll begin by finding its atomic number on the periodic table. Its atomic number is 20, so we'll write a configuration for an atom with 20 electrons according to the order above.

Fill up orbitals according to the order above until you reach twenty total electrons. The 1s orbital gets two electrons, the 2s gets two, the 2p gets six, the 3s gets two, the 3p gets 6, and the 4s gets 2 (2 + 2 + 6 +2 +6 + 2 = 20.) Thus, the electron configuration for calcium is: 1s2 2s2 2p6 3s2 3p6 4s2.

Note: Energy level changes as you go up. For example, when you are about to go up to the 4th energy level, it becomes 4s first, then 3d. After the fourth energy level, you'll move onto the 5th where it follows the order once again. This only happens after the 3rd energy level.

7


Specifically, the two leftmost columns represent atoms whose electron configurations end in s orbitals, the right block of the table represents atoms whose configurations end in p orbitals, the middle portion, atoms that end in d orbital, and the bottom portion, atoms that end in the orbit