Short Answer TypeWhich of the following elements has more negative electron gain enthalpy?
(i) [Ne] 3s2sp3
(ii) [Ne] 3s23p4
(iii) [Ne] 3s2 3p5
Long Answer TypeWhich of the following pairs of elements would have a more negative electron gain enthalpy?
(i) O or F (ii) F or Cl
What is the significance of the terms - "isolated gaseous atom' and 'ground state' while defining the ionization enthalpy and electron gain enthalpy?
(a) The significance of term ‘isolated gaseous atom:’ When an atom is isolated in the gaseous state, its electron releasing tendency and electron accepting tendency are both absolute in nature. It means that their values of ionization enthalpy and of electron gain enthalpy are not influenced by the presence of the other atoms. It is not possible to express these when the atoms are in the liquid or solid state.
(b) The significance of ground state: As we know that both ionization enthalpy and electron gain enthalpy are related to the force binding the electrons with the nucleus of the atom, therefore these are related to the energy states of the atoms whether ground states or excited states.
Short Answer TypeExplain, which of the following pairs of elements would have a more negative electron gain enthalpy:
(i) N or O (ii) O or S
Using the periodic table predicts the formulae of compounds which might be formed by the following pairs of elements:
(a) Silicon and bromine.
(b) Aluminium and sulphur.
The electron gain enthalpy of chlorine is 3.7 eV per atom. How much enthalpy in kJ is released when 1g of chlorine is converted completely of Cl- ion in the gaseous state?
Long Answer TypeShort Answer TypeWrite the electronic configuration of the elements with Z = 9, 11 and 36. Predict the following from the configuration:
(i) Which of them has the large negative value of electron gain enthalpy?
(ii) Which of them has the lowest ionisation enthalpy?
(iii) Which has positive electron gain enthalpy?
Long Answer TypeUse the periodic table to answer the following questions:
(a) Identify an element with five electrons in the outer subshell.
(b) Identify an element that would tend to lose two electrons.
(c) Identify an element that would tend to gain two electrons.
(d) Identify the group having metal, non-metal, liquid as well as gas at the room temperature.
The increasing order of reactivity among group 1 elements is Li < Na < K < Rb is F > CI > Br > I. Explain.
Switch
