Which of the following has the highest first ionization potential?
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lonization Potential is the amount of energy that is required to remove an electron from the outermost orbit of a gaseous atom.
- Boron
- Nitrogen
- Oxygen
- Carbon
The Correct Option is B
Approach Solution - 1
lonization Potential is the amount of energy that is required to remove an electron from the outermost orbit of a gaseous atom.
Out of Boron, Nitrogen, Oxygen, and Carbon - Nitrogen has a completely half-filled stable configuration.
Nitrogen Electronic Configuration = 1s22s22p3
Due to this stable configuration, it is difficult to remove an electron and hence it requires more energy than others. So, nitrogen has the highest first ionization potential among other elements.
Approach Solution -2
An element's ionization potential depends upon multiple factors. Some important factors are the size of the atom, effective nuclear charge, tendency to form a stable electronic configuration, losing a stable electronic configuration, etc.
Complete step-by-step answer:
- Boron's electronic configuration is 1s22s22p1. Carbon's electronic configuration is 1s22s22p4.
- In these configurations, the removal of an electron generates a stable symmetric configuration.
- Hence, the energy required to remove one electron from the boron requires less energy.
- In the case of nitrogen, its electronic configuration is 1s22s22p3.
- This electronic conjugation has a symmetric distribution which makes it stable.
- Due to this stable electronic configuration, a higher amount of energy is required to remove the electron from its outermost shell.
- Therefore, nitrogen has the highest first ionization potential.
So, the correct answer is option B.
Note: From left to right of a period, the size decreases as the nuclear charge density increases. According to this, the ionization enthalpy of nitrogen should be lower than oxygen. However, in this case, the formation of a stable symmetric electronic configuration overcomes the effect of size.
Approach Solution -3
Ionization potential refers to the amount of energy required to remove an electron from an atom. So, the first ionization potential can be defined as the energy required to remove 1 mole of the most loosely held electron from 1 mole of gaseous atoms to produce 1 mole of gaseous ions with a +1 charge.
Complete step-by-step answer:
- The ionization potential increases as we move across a period from left to right and decreases as we move down the group in a period.
- Ideally, on the basis of the trends of ionization potential, oxygen must possess the highest first ionization potential but this is not the case.
- Nitrogen has the highest ionization potential as the atomic number of nitrogen is 7 and the atomic number of oxygen is 8.
- Therefore, the outermost shell of nitrogen will contain 3 electrons i.e. 2p3 and oxygen will have 4 electrons in its outermost shell i.e. 2p4.
- An atom is highly stable if it has a fully or half-filled orbital.
- In the case of nitrogen, it has a half-filled p−subshell as nitrogen is very stable it will require high energy to remove an electron from its outermost shell and therefore will possess the highest ionization potential among boron, oxygen, and carbon.
So, the correct answer is Option (B).
Among the following element, Nitrogen has the highest first ionization potential.
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Concepts Used:
Trends in Periodic Table
The following trend in periodic properties of elements is observed:
Atomic size Trends:
The distance between the centre of the nucleus and the outermost shell of an atom is known as the atomic radius. In a group the atomic size increases due to the addition of shells as we move from one period to another. Across a period the atomic size decreases as the number of shells remain the same while the nuclear charge increases.
Metallic character Trends:
The elements which lose electrons to form cations are known as metals. Metallic character increases as we move down the group because the atomic size increases which lead to easy loss of electrons. On the other hand, it decreases across a period as we move from left to right.
Non-metallic character Trends:
The elements which have a tendency to gain electrons are known as non-metals. The tendency to gain electrons increases on moving across a period due to an increase in the nuclear charge and decrease in the atomic size. Hence, non-metallic character increases across a period.
Ionization potential Trends:
Ionization potential is defined as the amount of energy required to remove an electron from the outermost shell of a gaseous atom and convert it into a positively charged gaseous ion. The periodic properties in terms of ionization potential increase because the atomic size decreases across a period due to increase in the nuclear charge.
Melting Point Trends:
The melting point of an element is basically the energy required to change the state of an element from its solid state to its liquid state. Which essentially implies breaking a few bonds. Thus, higher the stronger the bond between the atoms, higher will be the melting point.