Arrange the following order of the property indicated:
(a). F, Cl, Br and I (negative electron gain enthalpy)
(b). Mg, Al, Si and Na (ionization enthalpy)
(c). C, N, O and F (second ionization enthalpy)
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In which of the following arrangements the order is NOT according to the property indicated against it?
(b) : As we move from left to right across a period, ionisation enthalpy increases with increasing atomic number. So the order of increasing ionisation enthalpy should be B <...
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Electron gain enthalpy with negative sign of fluorine is less than
(c) The electron gain enthalpy order for halogens is Cl > F > Br > I Due to small size of fluorine the extra electron to be added feels more...
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Which of the following noble gases has the highest positive electron gain enthalpy value? (a) Helium
(d) Electron gain enthalpy for noble gases is positive and it becomes less positive with increase in size of atom. Value of electron gain enthalpy He – 48 kJ mol–1, Ne –...
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Assertion : N2 is less reactive than P4. Reason : Nitrogen has more electron gain enthalpy than phosphorus
(c) Assertion is correct, reason is incorrect
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Which of the following order is/are incorrect regarding the property indicated against it?
(a) Metal halides with higher oxidation state are more covalent than the one in lower oxidation state.
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How would you account for the following: (i) The electron gain enthalpy with negative sign is less for oxygen than that for sulphur.
(i) This is due to smaller size of oxygen the electron cloud is distributed over a small region of space, making electron density high which repels the incoming electrons. (ii) Because...
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Would you expect the second electron gain enthalpy of O as positive, more negative or less negative than the first? Justify your answer
Second electron affinity of O is largely +ve because of repulsion between negatively charged ions and second electron to be added. Energy required to overcome repulsion is more than the...
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Explain why Halogens have very high negative electron gain enthalpy?
The electron gain enthalpy for halogens is highly negative because they can acquire the nearest stable noble gas configuration by accepting an extra electron.
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From the elements: Cl, Br, F, O, Al, C, Li, Cs and Xe; choose the following: (a) The element with highest negative electron gain enthalpy.
(a). The element chlorine (Cl) has the highest negative electron gain enthalpy. (b). The element cesium (Cs) has lowest ionization enthalpy. (c). The element fluorine F has lowest atomic radius. (d). The element...
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ASSERTION (A): Electron gain enthalpy becomes less negative as we go down a group.
(d) electron gain enthalpy becomes more negative as we go down a group.
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