![]() ![]() Describe the lattice structure of ionic compounds as a regular arrangement of alternating positive and negative ions, exemplified by the sodium chloride structure.Magnesium lost two electrons, so has a +2 charge and oxygen gained two electrons so has -2 charge. Now the configuration of magnesium is 2,8 and that of oxygen is 2,8. The quicker reaction is magnesium giving out the two electrons to oxygen. Oxygen needs to gain two electrons or give out 6 electrons. In order to be stable magnesium either needs to lose the 2 electrons or get 6 electrons. Magnesium has configuration 2,8,2 and oxygen has configuration 2,6. In the chemical bond created between metals and non-metals are always ionic because the metal (Sodium) becomes a positive ion and the non-metal (Chlorine) becomes a negative ion.Īnother example of ionic bonding bonding is the one between the metal Magnesium and the non-metal Oxygen. The above is an example of an ionic bond, where, oppositely charged ions are attracted. Explain the formation of ionic bonds between metallic and non-metallic elements. ![]() (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.
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