Define electropositive and electronegative elements and how can you explain the reactive nature of elements based on electropositive and electronegative nature in groups or periods
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Electropositivity can be defined as the tendency of an atom to donate electrons and form positively charged cations. This property is primarily exhibited by metallic elements, especially the alkali metals and the alkaline earth metals. It is important to note that electropositivity is the opposite of electronegativity, which is a measure of the tendency of an atom to gain electrons and form negatively charged anions. Therefore, highly electropositive elements have very low electronegativities and highly electronegative elements have very low electropositivity (electronegative elements typically do not have the tendency to lose electrons to form cations and electropositive elements generally do not to gain electrons to form anions).
Electropositive elements often form ionic salts with electronegative elements. For example, sodium is a highly electropositive element which readily gives up an electron in order to obtain a stable electronic configuration. Chlorine, on the other hand, is a highly electronegative element which readily accepts an electron to achieve a stable octet. Thus, sodium and chlorine can form an ionic bond with each other to yield sodium chloride (an ionic salt with the chemical formula NaCl).
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