Electron Gain Enthalpy NEET Questions

Inorganic Chemistry - Classification of Elements and Periodicity in Properties

Electron Gain Enthalpy MCQ Questions


13.
Despite positive overall electron gain enthalpy, O²⁻ ions exist in oxides because:
A.
Atmospheric O₂ favors O²⁻
B.
Second electron release is favorable
C.
O²⁻ is more stable than O⁻ in gas phase
D.
Lattice energy of the ionic solid compensates for the unfavorable electron addition
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ANSWER :
D. Lattice energy of the ionic solid compensates for the unfavorable electron addition
14.
Electron gain enthalpy generally becomes more negative as we move across a period from left to right because:
A.
Effective nuclear charge increases and atomic size decreases, making the atom more attractive to incoming electrons
B.
Atomic mass increases
C.
Number of valence electrons decreases
D.
Energy levels of orbitals decrease
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ANSWER :
A. Effective nuclear charge increases and atomic size decreases, making the atom more attractive to incoming electrons
15.
Across the second period (Li to F), electron gain enthalpy becomes:
A.
Constant across the period
B.
Decreases then increases
C.
More positive across the period
D.
Generally more negative (with some irregularities like Be and N)
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ANSWER :
D. Generally more negative (with some irregularities like Be and N)
16.
Among the period 2 elements, the most negative electron gain enthalpy is for:
A.
Lithium (Li)
B.
Oxygen (O)
C.
Fluorine (F)
D.
Carbon (C)
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ANSWER :
C. Fluorine (F)
17.
Halogens (Group 17) have very negative electron gain enthalpies because:
A.
They are metals
B.
They have low ionization energy
C.
They achieve stable noble gas configuration (ns²np⁶) by adding one electron
D.
They have large atomic size
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ANSWER :
C. They achieve stable noble gas configuration (ns²np⁶) by adding one electron
18.
Noble gases (Group 18) have positive electron gain enthalpies because:
A.
They have very small atomic size
B.
They are non-reactive
C.
Their ns²np⁶ valence shell is completely filled; adding an electron forces it into the next higher shell
D.
They have low ionization energy
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ANSWER :
C. Their ns²np⁶ valence shell is completely filled; adding an electron forces it into the next higher shell