Single Choice

Which sequence of ionization potential is correct?

A$$B < Be$$
Correct Answer
B$$Be < B$$
C$$Be = B$$
DNone of the above

Solution

The atomic number of $$Be$$ is 4 and therefore, has a stable fully filled configuration : $$1s^{2}2s^{2}$$.
The atomic number of $$B$$ is 5 and has an unstable configuration $$1s^{2}2s^{2}2p^{1}$$.
Therefore, a large amount of energy is required to remove an electron from the stable configuration of Be and hence, ionization potential of $$Be > B$$.

SIMILAR QUESTIONS

Periodic Classification of Elements

Which ionisation potential (IP) in the following equations involves the greatest ammount of energy?

Periodic Classification of Elements

Ionisation energy in the alkali metals group :

Periodic Classification of Elements

As nuclear charge increases and atomic radii increases, ionisation potential :

Periodic Classification of Elements

B has a smaller first ionization enthalpy than Be. Consider the following statements: (I) it is easier to remove $$2p$$ electron than $$2s$$ electron (II) $$2p$$ electron of B is more shielded from the nucleus by the inner core of electrons than the $$2s$$ electrons of Be (III) $$2s$$ electron has some penetration power than $$2p$$ electron (IV) atomic radius of B is more than Be (atomic number $$B=5, Be=4$$) The correct statements are:

Periodic Classification of Elements

In comparison to boron, berylium has:

Periodic Classification of Elements

The electronic configuration with the highest ionization enthalpy is:

Periodic Classification of Elements

Which of the following atoms has the highest first ionization energy?

Periodic Classification of Elements

The decreasing order of the ionization potential of the following elements is:

Periodic Classification of Elements

Arrange the elements $$Se, Cl$$ and $$S$$ in the increasing order of ionisation energy.

Periodic Classification of Elements

Which of the following has maximum ionisation potential?

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