Electron gain enthalpy is one of the important periodic property.
Write the oxidation state and covelency of Al in `(Al F_6)^3-`.

Electron gain enthalpy is one of the important periodic property. Define electron gain enthalpy.

Are the oxidation state and covelency of Al in [AlCl (H_2O)_5]^(2+) same ?

Electron gain enthalpy is one of the important periodic property. Explain any two factors affecting electron gain enthalpy.

Electron gain enthalpy is an important periodic property. a) What is meant by electron gain enthalpy? b) What are the factors affecting electron gain enthalpy? c) How electron gain enthalpy varies on moving across a period? Justify.

Atomic size, valency, ionization enthalpy, electron gain enthalpy and electronegativity are the important periodic properties of elements. a) What do you mean by periodicity? b) Periodic properties are directly related to ͟ ͟ ͟͟͟

Ionization enthalpy is an important periodic property. a) What is the unit in which it is expressed? b) What are the factors influencing ionization enthalpy? c) How ionisation enthalpy varies in the periodic table?

Electron gain enthalphy is the amount of energy involved when an isolated gaseous atom accepts an electron to form a monovalent anion the value of the electron gain enthalpy of halogens are given below: F : -328 KJ mol^(-1) Cl - 349 KJ mol^(-1) Br : -325 KJ mol^(-1) I : -295 KJ mol^(-1)Chlorine has more negative electron gain enthalpy than fluorine. why ?

Electron gain enthalphy is the amount of energy involved when an isolated gaseous atom accepts an electron to form a monovalent anion the value of the electron gain enthalpy of halogens are given below: F : -328 KJ mol^(-1) Cl - 349 KJ mol^(-1) Br : -325 KJ mol^(-1) I : -295 KJ mol^(-1) Why the negative electron gain enthalpy decreases from chlorine iodine?

Generally electron gain enthalpy increases along a period and decreases down the group. But electron gain enthalpy of oxygen is -141 kJ//mol while that of sulphur is -200 kJ//mol . Explain.

Justify the placement of '0, S', Se, Te and 'Po' in the same group of the periodic table in terms of electronic configuration, oxidation state and hydride formation.