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  • An element X (atomic number 17) reacts with an element Y (atomic number 20) to form a divalent halide. (a) Where in the periodic table are elementsX andY placed (b)Classify X and Y as metal(s)non-metal(s)or metalloid (s)(c)What will be the nature of bondi

An element X (atomic number 17) reacts with an element Y (atomic number 20) to form a divalent halide.
(a) Where in the periodic table are elements X and Y placed?
(b) Classify X and Y as metal (s), non-metal (s) or metalloid (s)
(c) What will be the nature of oxide of element Y? Identify the nature of bonding in the compound formed
(d) Draw the electron dot structure of the divalent halide

Answers (1)

a) Element X has atomic number 17 (Chlorine) and its electronic configuration is 2 8 7
It has 7 valence electrons, so it belongs to group 17 and it has 3 shells which means it belongs to 3rd Period.
Element Y has atomic number 20 (Calcium) and its electronic configuration is 2 8 8 2
It has 2 valence electrons and it belongs to group 2 and it has 4 shells which means it belongs to 4th Period.

b) As element X has 7 electrons in the outer most shell it is short of one
electron for inert gas configuration. So, X will prefer accepting an electron hence it is a Non-Metal. Whereas element Y has 2 electrons in the outermost shell which means this element prefers to lose electrons and reach inert gas configuration. So, element Y is going to be a metal.
c) Since Y is a metal, and all the metallic oxides are basic in nature. Oxygen being a non-metal, the bonding between them is going to be Ionic in nature (Electropositive (Metals) and electronegative (Non-metals) elements will form Ionic Bond).

d) Electronic Configuration of Calcium:   2     8     8      2
  Electronic Configuration of Chlorine:        2      8   7
Electron Dot Structure of Calcium Chloride CaCl2

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