d and f BLOCK ELEMENTS MCQ Quiz: GKFix - Bridge of Knowledge

Question 1636

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Why are ns electrons lost before (n-1)d electrons when d-block elements form ions?

The ns orbitals are lower in energy than the (n-1)d orbitals
The ns orbitals are higher in energy than the (n-1)d orbitals in the ground state of transition metal atoms
The ns electrons are closer to the nucleus
The (n-1)d electrons are more stable

Question 1637

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Which configuration of an ion formed by a 3d transition element is considered particularly stable and can influence ionisation enthalpy trends?

d0 configuration
d5 configuration
d10 configuration
s2 configuration

Question 1638

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What happens to the relative energies of 4s and 3d orbitals when an electron is removed from a 3d transition element?

The 4s orbital always becomes lower in energy
The 3d orbital always becomes lower in energy
The removal of an electron can alter the relative energies of 4s and 3d orbitals
The energy difference between them remains constant

Question 1639

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Why is the increase in successive ionisation enthalpies (second, third, etc.) not as steep for transition elements as for non-transition elements?

The d-orbitals are higher in energy
One d-electron does not shield another d-electron effectively from the nuclear charge
The nuclear charge decreases with each ionisation
The atomic radius increases significantly

Question 1640

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What is the main reason for the variation in ionisation enthalpy along a transition series being much less than that along a period of non-transition elements?

The transition elements have fewer electrons
The increased nuclear charge is effectively shielded by the filling of inner d orbitals
The transition elements have lower atomic masses
The transition elements form only cations

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