a group of elements in the periodic table are given below ( boron is the first member of the group and thallium is the last). boron,aluminum, gallium, indium,thallium Answer the following question in relations to the above groups of elements: (a) which element has the most metallic character? (b) which element would be expected to have the highest electro negativity ? ( c) if the electronic configuration of aluminum is2,8,3,how many electron are there in the outer shell of thallium? (d) the atomic number of boron is5 .write the chemical formula of the compound formed when boron reacts with chlorine. (e) will the elements in the group to the right of this boron group be more metallic or less metallic in character? justify your answer
Answers
Answer:
(i) thallium
(ii)boron
(iii)3 electron present in the outermost shell
(iv)BCl3
(v)less metallic becoz on moving from left to right in a periodic table metallic character decreases....
Explanation:
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Answer:
(a) On moving down the group, the electropositive or metallic character of the elements of group 13 increases because of the ionization energy decreases. Therefore, boron is non metal and the rest of the elements are typical metals. The thallium element has the most metallic character.
(b) On moving down the group, the electronegativity decreases as the atomic size increases. Therefore Boron would be expected to have the highest electronegativity.
(c) The atomic number of aluminium is 13 and its electronic configuration is (2, 8, 3). The number of electrons in the outermost shell of every element of group 13 are three. So electrons in the outermost shell of thallium are 3.
(d) Boron combine with chlorine gas at high temperature and forms BCl₃.
2B + 3Cl₂ 2BCl₃
(d) The group 14 is present to the right of the boron group. As we know that on moving left to right electronegativity increases and electropositive character decreases. Therefore, group 14 (carbon family) is less metallic than the group 13 (boron group),