Chemistry
Arrange as per the instruction :
(i) He, Ar, Ne (Increasing order of the number of electron shells)
(ii) Na, Li, K (Increasing Ionization Energy)
(iii) F, Cl, Br (Increasing electronegativity)
(iv) Na, K, Li (Increasing atomic size).
Periodic Table
ICSE 2017
86 Likes
Answer
(i) He < Ne < Ar
Reason — Number of electron shells increases as we move down the group.
(ii) K < Na < Li
Reason — Ionization Potential decreases as we move down the group.
(iii) Br < Cl < F
Reason — Electronegativity decreases as we move down the group.
(iv) Li < Na < K
Reason — Atomic Size increases as we move down the group.
Answered By
45 Likes
Related Questions
Select the correct answer — The energy required to remove an electron from a neutral isolated gaseous atom and convert it into a positively charged gaseous ion is called ………. (electron affinity, ionization potential, electronegativity)
Match the atomic number 2, 4, 8, 15 and 19 with each of the following:
(i) A solid non-metal belonging to the third period.
(ii) A metal of valency 1.
(iii) A gaseous element with valency 2.
(iv) An element belonging to Group 2.
(v) A rare gas.
Give one word or a phrase for the following statement: The energy released when an electron is added to a neutral gaseous isolated atom to form a negatively charged ion.
Give reasons :
(i) Inert gases do not form ions.
(ii) Ionization potential increases across a period — left to right.