Step 1: Ionization Energy Trend.
Ionization energy generally increases across a period from left to right owing to increasing nuclear charge. Exceptions exist due to electron configuration, notably in nitrogen (N) and oxygen (O), where half-filled or filled orbitals offer greater stability.
Step 2: Comparison of the Given Elements.
- (C) Carbon exhibits the lowest first ionization energy as it is in the 2nd period and possesses fewer protons than the other elements, facilitating electron removal.- (N) Nitrogen displays a higher ionization energy than carbon, attributed to its stable half-filled configuration.- (O) Oxygen's ionization energy is higher than carbon's but lower than nitrogen's.- (F) Fluorine possesses the highest ionization energy due to its strong electronegativity and diminutive size.
Step 3: Conclusion.
Consequently, Carbon (C) is the element with the lowest first ionization energy, correlating to option (1).
Given below are two statements:
Statement (I): According to the Law of Octaves, the elements were arranged in the increasing order of their atomic number.
Statement (II): Meyer observed a periodically repeated pattern upon plotting physical properties of certain elements against their respective atomic numbers.
In the light of the above statements, Choose the correct answer from the options given below:
The correct orders among the following are:
[A.] Atomic radius : \(B<Al<Ga<In<Tl\)
[B.] Electronegativity : \(Al<Ga<In<Tl<B\)
[C.] Density : \(Tl<In<Ga<Al<B\)
[D.] 1st Ionisation Energy :
In\(<Al<Ga<Tl<B\)
Choose the correct answer from the options given below :