Question

What is the correct order of first ionization enthalpy for second period elements?

• A. $\mathrm{Li}<\mathrm{Be}<\mathrm{B}<\mathrm{C}<\mathrm{N}<\mathrm{O}<\mathrm{F}<\mathrm{Ne}$
• B. $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}<\mathrm{O}<\mathrm{N}<\mathrm{F}<\mathrm{Ne}$
• C. $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}<\mathrm{N}<\mathrm{O}<\mathrm{F}<\mathrm{Ne}$
• D. $\mathrm{Li}<\mathrm{Be}<\mathrm{C}<\mathrm{O}<\mathrm{N}<\mathrm{F}<\mathrm{Ne}$

Answer 1

The correct option is B

$\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}<\mathrm{O}<\mathrm{N}<\mathrm{F}<\mathrm{Ne}$

The explanation for the correct option:

Option (B) $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}<\mathrm{O}<\mathrm{N}<\mathrm{F}<\mathrm{Ne}$

1. The order of increasing atomic number and periodic features of the elements determine how the elements are organized in the contemporary periodic table. Ionization energy, electron affinity, atomic radius, electronegativity, and ionic radius are the periodic properties.
2. Ionization energy, also known as ionization enthalpy, is the minimal amount of energy needed to remove one electron from a neutral gaseous atom in its ground state in order to generate a gaseous ion.
3. $\mathrm{X}\left(\mathrm{g}\right)\to {\mathrm{X}}^{+}\left(\mathrm{g}\right)+{\mathrm{e}}^{-}$
4. First ionization potential is the term for the energy needed to remove one electron, and smaller ionization enthalpy makes it simpler to ionize an atom into its positive ion.
5. The amount of energy required to remove one electron from an isolated gaseous atom in its gaseous form is known as the ionization enthalpy of an element.
6. Moving from left to right in a period, the ionization energy increases.
7. The first ionization enthalpy is the enthalpy change associated with the loss of the first electron from an isolated gaseous atom in its ground state.

Therefore, Option (B) is the correct option, i.e. $\mathrm{Li}<\mathrm{B}<\mathrm{Be}<\mathrm{C}<\mathrm{O}<\mathrm{N}<\mathrm{F}<\mathrm{Ne}$.