Explain Methods of writing electronic configuration.
Answers
Hund's rule:- It states that the pairing of the electrons does not takes place in the orbitals of a particular sub shells (s,p,d) untill all the orbitals of sub shells first singly occupied. Moreover the singly occupied orbitals must contain the electrons with the opposite spins.
Electronic configuration varies from element to element
For example the electronic configuration of aluminum is 3s23p1.
Answer:
This may seem very long but is very useful...
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 0 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 1 electron for each negative charge and subtract 1 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.
A sodium atom with a -1 charge would have 1 electron added to its basic atomic number of 11. The sodium atom would then have a total of 12 electrons.
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.
The g, h, i and k orbital sets are theoretical. No known atoms have electrons in any of these orbitals. The g set has 9 orbitals, so it could theoretically contain 18 electrons. The h set would have 11 orbitals and a maximum of 22 electrons, the i set would have 13 orbitals and a maximum of 26 electrons, and the k set would have 15 orbitals and a maximum of 30 electrons.
Remember the order of the letters with this mnemonic:[1]Sober Physicists Don't Find Giraffes Hiding In Kitchens.
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 2 electrons in the 1s orbital set, 2 electrons in the 2s orbital set, and 6 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 3p6 4s2 3d10 4p6 5s2 4d10 5p6 6s2 4f14 5d10 6p6 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.
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