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Electronic configuration of atom & reason for stability of half and fully filled orbitals.

Day 1
4.5.20
6 th  period

 Good Morning Boys,
Today we will do the the topic of electronic configurations of atom and Reason for stability of half and fully filled orbitals .

Learning Outcomes :
Students will be able to
  1.  Write electronic configuration of  various elements.
  2.  understand the  reason for stability of half and fully filled orbitals.
  3. Apply rules and formula. 
note : periodical table given at the end of the blog is only for refering to electronic 
Electronic configuration of Atoms :


In this figure, the element symbol H is followed by the electron configuration is 1 s superscript 1. An orbital diagram is provided that consists of a single square. The square is labeled below as, “1 s.” It contains a single upward pointing half arrow.
In this figure, the element symbol H e is followed by the electron configuration, “1 s superscript 2.” An orbital diagram is provided that consists of a single square. The square is labeled below as “1 s.” It contains a pair of half arrows: one pointing up and the other down.
In this figure, the element symbol L i is followed by the electron configuration, “1 s superscript 2 2 s superscript 1.” An orbital diagram is provided that consists of two individual squares. The first square is labeled below as, “1 s.” The second square is similarly labeled, “2 s.” The first square contains a pair of half arrows: one pointing up and the other down. The second square contains a single upward pointing arrow.
In this figure, the element symbol B e is followed by the electron configuration, “1 s superscript 2 2 s superscript 2.” An orbital diagram is provided that consists of two individual squares. The first square is labeled below as, “1 s.” The second square is similarly labeled, “2 s.” Both squares contain a pair of half arrows: one pointing up and the other down.
In this figure, the element symbol B is followed by the electron configuration, “1 s superscript 2 2 s superscript 2 2 p superscript 1.” The orbital diagram consists of two individual squares followed by 3 connected squares in a single row. The first square is labeled below as, “1 s.” The second is similarly labeled, “2 s.” The connected squares are labeled below as, “2 p.” All squares not connected contain a pair of half arrows: one pointing up and the other down. The first square in the group of 3 contains a single upward pointing arrow.
  • In this figure, the element symbol C is followed by the electron configuration, “1 s superscript 2 2 s superscript 2 2 p superscript 2.” The orbital diagram consists of two individual squares followed by 3 connected squares in a single row. The first blue square is labeled below as, “1 s.” The second is similarly labeled, “2 s.” The connected squares are labeled below as, “2 p.” All squares not connected to each other contain a pair of half arrows: one pointing up and the other down. The first two squares in the group of 3 each contain a single upward pointing arrow.
  • This figure includes electron configurations and orbital diagrams for four elements, N, O, F, and N e. Each diagram consists of two individual squares followed by 3 connected squares in a single row. The first square is labeled below as, “1 s.” The second is similarly labeled, “2 s.” The connected squares are labeled below as, “2 p.” All squares not connected to each other contain a pair of half arrows: one pointing up and the other down. For the element N, the electron configuration is 1 s superscript 2 2 s superscript 2 2 p superscript 3. Each of the squares in the group of 3 contains a single upward pointing arrow for this element. For the element O, the electron configuration is 1 s superscript 2 2 s superscript 2 2 p superscript 4. The first square in the group of 3 contains a pair of arrows and the last two squares contain single upward pointing arrows. For the element F, the electron configuration is 1 s superscript 2 2 s superscript 2 2 p superscript 5. The first two squares in the group of 3 each contain a pair of arrows and the last square contains a single upward pointing arrow. For the element N e, the electron configuration is 1 s superscript 2 2 s superscript 2 2 p superscript 6. The squares in the group of 3 each contains a pair of arrows.
  • Na
Class_11_Chemistry_Structure_Of_Atom_Filling_Of_Orbitals_In_Sodium


  • This figure includes the element symbol N a, followed by the electron configuration for the element. The first part of the electron configuration, 1 s superscript 2 2 s superscript 2 2 p superscript 6, is shaded in purple and is labeled, “core electrons.” The last portion, 3 s superscript 1, is shaded orange and is labeled, “valence electron.” To the right of this configuration is the word “Abbreviation” followed by [ N e ] 3 s superscript 1.
 Another way to represent sodium  : [Ne]3s1.  
 the symbol [Ne] represents core electrons, (1s22s22p6) 
  • This figure provides the electron configuration 1 s superscript 2 2 s superscript 2 2 p superscript 6 3 s superscript 2 3 p superscript 3. It includes a diagram with two individual squares followed by 3 connected squares, a single square, and another connected group of 3 squares all in a single row. The first square is labeled below as, “1 s.” The second is similarly labeled, “2 s.” The first group of connected squares is labeled below as, “2 p.” The square that follows is labeled, “3 s,” and the final group of three squares is labeled, “3 p.” All squares except the last group of three squares has a pair of half arrows: one pointing up and the other down. Each of the squares in the last group of 3 contains a single upward pointing arrow.
  • For Potassium(k) :Atomic number =19
Electronic configuration = 1s2,2s2,2p6,3s2,3p6,4s1
  Electronic configuration of  ions :
(a) Na+        =  (  10 electrons )

1s2,2s2,2p6
(b) P3–        = (18 electrons )
[Ne] 3s² 3p⁶   or     1s22s22p63s23p6  
(c) Al3+        =  (10 electrons)
1s2,2s2,2p6
EXCEPTIONAL ELECTRONIC CONFIGURATION OF CHROMIUM AND COPPER
 Copper (Cu)
Atomic number 29   = [Ar],4s23d9
 actual configuration  is : [Ar]4s13d10
Chromium (Cr) 
Atomic number 24 = 1s22s22p63s23p64s23d4.
But in actual it is:=[Ar]4s13d5
Reason  for exceptional configuration :
  1. Half-filled and fully filled orbital are more stable
Note :

 Reasons for Stability of completely filled and half filled subshells:

a.  Symmetrical distribution of electrons- the completely filled or half filled sub-shells have symmetrical distribution of electrons in them and are more stable.

b.  Exchange energy-The two or more electrons with the same spin present in the degenerate orbitals of a sub-shell can exchange their position and the energy released due to this exchange is called exchange energy. The number of exchanges is maximum when the subshell is either half filled or completely filled. As a result the exchange energy is maximum and so is the stability.
more is the exchange energy -more is the stability.


If configuration was 4s23d4 the exchange energy is:
 Class_11_Chemistry_Structure_Of_Atom_Exchange_Of_Energy
Total number of exchanges = 3 + 2 + 1 = 6
 If configuration is 4s13d5the exchange energy is:
 Class_11_Chemistry_Structure_Of_Atom_Exchange_Of_Energy_1
Total number of exchanges = 4 + 3 + 2 + 1 = 10





A periodic table, entitled, “Electron Configuration Table” is shown. The table includes the outer electron configuration information, atomic numbers, and element symbols for all elements. A square for the element hydrogen is pulled out beneath the table to provide detail. The blue shaded square includes the atomic number in the upper left corner, which is 1, the element symbol, H in the upper right corner, and the outer electron configuration in the lower, central portion of the square. For H, this is 1 s superscript 1.

Thats all for the day
Take Care
Stay Safe
Mark your attendance on the form and the comment section of the blog.




Comments

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  7. AnonymousMay 3, 2020 at 10:43 PM

    ma'am you are giving a lot of work to write how we are supposed to learn at hme most of the time goes in doing your work douring your period we also have a lot of work to do in the zero period . now we have learn three chapters which are very long can you pls minimize some of the written work

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    Symmetrical distribution of electrons- the completely filled or half filled sub-shells have symmetrical distribution of electrons in them and are more stable...... Ma'am why so ?? Why does stability prefers symmetry?

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