The energy required to remove an electron from a neutral isolated gaseous atom and convert it into a positively charged gaseous ion is called , Ionisation Potential, The tendency of an atom to attract electrons to itself when combined in a compound, Electronegativity, Ionisation Potential across a period , Increases, Amount of energy released when an atom in the gaseous state accepts an electron to form an anion, Electron affinity, Atomic size down the group , Increases, Electron affinity across a period , Increases, Non-metallic character across a period, Increases, Electronegativity down the group, Decreases, Place the elements F, Be and N in increasing electronegativity, Be, N, F, Identify the group number and period number of element with electronic configuration 2, 8, 3, Group 13, Period 3, Which Element in the given list has highest E.A and Lowest E.A. Li, N, Ne, B, F, Highest F, Least Ne, Which element in the given list can form ions readily? Be, Mg, Ca, Ca, Arrange the given elements in decreasing atomic size. Na, K, Li, K, Na, Li, Which element is metallic out of Cl, F, Br and I, I, Write in increasing order of IP. Na, K, Cl, S, Si, K, Na, Si, S, Cl, Valency of element having electrons number 18, Zero, Electropositive element among Mg, Cl, Na, Na, Most Electronegative element of halogen series, F, Highly reactive element among Na, K, F, S, K, F, A metal present in period 3 with valency 2, Mg.

Periodic Table

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