Question

Name any two elements of group one and their electronic configurations. What similarity do you observe in their electronic configurations? Write the formula of oxide of any of the aforesaid elements?

Answer 1

Hint: We have to know that in a periodic table there are eighteen groups and seven periods. Group one in alkali metal while group two is alkaline earth metals. Group one and two are s block elements. And p block elements have all three metals, nonmetals and metalloids.

Complete answer:
We need to write two elements of group one. The two elements of group 1 are Sodium (Na) and potassium (K). Their electronic configurations: \[Na = 2,8,1\]; \[K:2,8,8,1\]. Similarity: Both have one valence electron. Atomic size increases down the group, therefore the number of shells also increases due to which effective nuclear charge increases. The similarity in the electronic configuration is that the number of shells is increasing. The valency for both the elements is one. For group one the valency is one. Or we can say that charge is plus one. Oxides of the elements can be sodium oxide and potassium oxide. The formula for the oxides can be written as \[N{a_2}O;{K_2}O\].

Note:
We must have to remember that the alkali metals are all shiny, soft, highly reactive metals at standard temperature and pressure and readily lose their outermost electrons to form cations with charge \[ + 1\]. They can all be cut easily with a knife due to their softness, exposing a shiny surface that tarnishes rapidly in air due to oxidation by atmospheric moisture and oxygen (and in the case of lithium, nitrogen). Because of their high reactivity, they must be stored under oil to prevent reaction with air, and are found naturally only in salts and never as the free elements.