![]() ![]() For example, Caesium has a large atomic radius, whereas Flourine has a very small one. This results in some atoms having a larger atomic radius than others. The more electrons there are (and the more shells that exist between the nucleus and valence shell), the harder it is for this goal to be accomplished. The protons in the nucleus of an atom are positively charged, and want to draw in the electrons surrounding it. Thus, in the d-block you don't have a clear periodic trend for electronegativity as you do in the s and p blocks.Īs in, an atom wanting more to hog electrons? (I'm assuming this because this comment is on the electronegativity video) In the d-block, you have many competing factors such as then need to have a full s and p, to energetic nuances due to the d subshell being partially full, and all these affect the electronegativity. That is why electronegativity goes down as you go down a Group of the periodic table in the s and p blocks (the d block is different). The more electrons the element has, the less advantage there is to gaining an electron compared to other members of the same Group. ![]() One has to do with how many electrons (not valence electrons, all of the electrons) the element has. However, there are also competing factors. This need for being in an energetically favorable state gives rise to electronegativity. Thus, the closer an element is to completing both its outermost p and s subshells, the more energetically favorable it is to gain an electron to help that process along. I can give you some overly simplified basics though.Ītoms are particularly energetically stable if the s and p subshells of their outermost electron shell are both completely full. Elements towards the left have lesser valence electrons so they give away electrons easily.That is a complex issue and a bit of an advanced topic.This tendency is shown by elements like sodium or magnesium which are placed towards the left in the table. Metals have freely available electrons that can be easily lost to attain a stable electronic configuration.Metals tend to give away electrons because they have low ionisation energy.The energy required to remove electrons from the atom is called Ionisation energy.Metallic character of elements decreases from left to right in the period.There is a difference in the valency of elements belonging to the same period.All these elements show the valency one because they accept one electron from the other elements. From fluorine to iodine, there are the same number of valence electrons in their outermost orbital, As we move down the group, the valency of elements remains the same because the number of valence electrons is the same throughout the group.įor example, halogens belonging to the 17th column have the same valency.In any particular group, elements have the same valency.The valency of both will be one because the first atom can donate one electron and the second one can accept 1 electron.ġ electron → Donate 1 electron 7 electrons → Accept 1 electron The atom, having 7 electrons in the outermost orbit, tends to accept or gain an electron from outside. The atom, having one electron in its outermost shell, wants to donate or lose that electron.The capacity of the atom to give or take electrons during bond formation is called. ![]()
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