The electron configuration filling patterns of some elements in group 6b(6) and group 1b(11) reflect the increasing stability of half-filled and completely filled sublevels.
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What is electronic configuration?</h2>
The distribution of electrons in an element's atomic orbitals is described by the element's electron configuration. Atomic subshells that contain electrons are placed in a series, and the number of electrons that each one of them holds is indicated in superscript for all atomic electron configurations. For instance, sodium's electron configuration is 1s22s22p63s1.
Almost all of the elements write their electronic configurations in the same style. When the energies of two subshells differ, an electron from the lower energy subshell occasionally goes to the higher energy subshell.
This is due to two factors:
Symmetrical distribution: As is well known, stability is a result of symmetry. Because of the symmetrical distribution of electrons, orbitals where the sub-shell is exactly half-full or totally filled are more stable.
Energy exchange: The electrons in degenerate orbitals have a parallel spin and are prone to shifting positions. The energy released during this process is simply referred to as exchange energy. The greatest number of exchanges occurs when the orbitals are half- or fully-filled. Its stability is therefore at its highest.
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One way can be forming an ionic bond
Second way can be forming covalent bond
And finally, the third way could be forming Co-ordinate bond
Answer:
Solids have a set shape and can't flow since their particles can only vibrate in a specific direction. They are unable to travel from one location to another.
Explanation:
The element oxidized is the element in which the charge becomes more positive after the reaction, hence the reducing agent. The element that is reduced is the element or compound in which the charge becomes more negative after the reaction. Sn becomes +4 from +2. Hence Sn is the reduced element while Pb becomes +2 from +4 hence Pb is the element oxidized and PbCl4 is the reducing agent.
