Consider two elements 'A' (Atomic number 17) and 'B' (Atomic number 19) :
(i) Write the positions of these elements in the modern periodic table giving justication.
(ii) Write the formula of the compound formed when 'A' combines with 'B.'
(iii) Draw the electron dot structure of the compound and state the nature of the bond formed between the two elements
Answers
THERE ARE MANY TYPES OF ANSWERS:
(i) A has electronic configuration - 2,8,7.
It has 3 shells or orbits so it is placed in period 3.
It has 7 electrons in the outermost shell it is placed in groupVII A
B has electronic configuration - 2,8,8,1.
It Has 4 shells or orbits so it is placed in period 4
It Has 1 electron in its outermost shell so it is placed in group I A
A is Cl 1- And B is K 1+
2K + Cl ⇒ 2 KCl
²
Electron Dot Structure In The Diagram i uploaded
Since it Is Giving And Taking Of Electrons bond present between them is ionic bond.
(ii) IT IS IN THE NOTEBOOK PICTURE
(iii) (i) Atomic no. of A - 17
Electronic configuration of A = 2, 8,7
Since it has '7' electrons in its outermost shell.
So, group to which A belongs = 10 +7 = group 17.
Period to which element A belongs = no. of shells = 3
So, period to which A belongs is 3rd
Atomic no. of B = 19
Electronic configuration of A = 2, 8, 8,1
Since it has 'l' electrons in its outermost shell.
So, group to which B belongs = group 1.
Period to which element B belongs = no. of shells = 4
So, period to which B belongs is 4th
(ii) Since, Valency of A = -1
Valency of B = +1
So, when A combines with B, the formula will be BA
(iii) The electron dot structure is as follows:
The bond formed between B and A is an ionic bond.
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