An element A has an atomic number of 6. Another element B has 17 electrons in its one neutral atom.
(a) In which groups of the periodic table would you expect to find these elements?
(b) what type of bond is formed between A and B?
(c) Suggest a formula of the compound formed between A and B.
(a) Element A has an atomic number of 6, so its electronic configuration is 2,4. Therefore, the group number for element A = valence shell + 10
= 4+10 =14.
Hence, Element A belongs to group 14.
Element B has an atomic number of 17, hence its electronic configuration is 2,8,7. Therefore, the group number of element B = valence shell + 10
= 7 + 10 = 17.
Hence, Element B belongs to group 17.
(b) As the group 14 elements and group 17 elements are all non-metallic in nature, hence, they form a covalent bond.
(c) As the element A has a valency of 4 and element B has a valency of 1, therefore the formula of the compound formed by them is AB4.
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