![]() ![]() (The new compound formed is sodium chloride). Chlorine gained one electron, so it gained an extra negative charge, making it a negative (-1) Chlorine ion. Since sodium lost a negatively charged particle, it’s overall charge becomes positive, making it a positive (+1) sodium ion. Both have full outer shells and so have become stable. Now the configuration of Sodium will be 2,8 and the configuration of Chlorine will be 2,8,8. So sodium will have to lose it’s outer electron to chlorine. In order to make them both stable, sodium needs to lose 1 electron and Chlorine needs to gain 1 electron. Let’s take the electronic configurations of metal ‘Na’ Sodium and the non-metal ‘Cl’ Chlorine.īoth elements are not stable. The elements in group 1 and 2 are metals and the elements in group 7 are non-metals. The block of elements in the yellow colour above are not considered part of any groups here). (Note that the columns in the periodic table are called groups. Describe the formation of ionic bonds between metals and non-metals as exemplified by elements from Groups I and VII.You’ll understand this with the example below. They can do this by gaining or losing electrons from and to the other element’s atoms respectively. The other elements in the periodic table don’t have a full outer shells and so reacts with other elements- they can gain or lose electrons.Īfter any reaction, the atoms of an element has to have full outer shells- that is, they must become stable. We saw that elements in the last group (column) of the periodic table – the noble gases- have full electron shells- they are stable. It will be positively charged if it loses electrons (because there are more protons than electrons now) and negatively charged when it gains more electrons (more electrons than protons present now). An ion is an atom that is electrically charged. When it loses or gains electrons the charge balance is tipped. We know that atoms are neutrally charged (no. In the last topic, I mentioned that elements gain or lose or share electrons when undergoing reactions with other elements. ![]() Describe the formation of ions by electron loss or gain.We apologise for the inconvenience, but hope that the new images will provide you with an even better learning experience. The greater the distance, the less the attraction and so the less energy is released as electron affinity.Disclaimer: Due to unforeseen difficulties, we have had to take down the images on this notes page. The over-riding factor is therefore the increased distance that the incoming electron finds itself from the nucleus as you go down the group. This will be approximately the same in both these cases and so does not affect the argument in any way (apart from complicating it!). There is also a small amount of screening by the 2s electrons in fluorine and by the 3s electrons in chlorine. But again the incoming electron feels a net attraction from the nucleus of 7+ (17 protons less the 10 screening electrons in the first and second levels). In contrast, chlorine has the electronic structure 1s 22s 22p 63s 23p x 23p y 23p z 1 with 17 protons in the nucleus. It therefore feels a net attraction from the nucleus of 7+ (9 protons less the 2 screening electrons). It has 9 protons in the nucleus.The incoming electron enters the 2-level, and is screened from the nucleus by the two 1s 2 electrons. ChlorineĪ fluorine atom has an electronic structure of 1s 22s 22px 22py 22pz 1. ![]()
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