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Chapter 12: Problem 97

Which ionization potential in the following equations involves the greatest amount of energy? (a) \(\mathrm{Na} \longrightarrow \mathrm{Na}^{+}+\mathrm{e}\) (b) \(\mathrm{K} \longrightarrow \mathrm{K}^{+} \mathrm{e}^{-}\) (c) \(\mathrm{Cs}^{2+} \longrightarrow \mathrm{Cs}^{3+}+\mathrm{e}^{-}\) (d) \(\mathrm{Ca}^{+} \longrightarrow \mathrm{Ca}^{2+}+\mathrm{e}^{-}\)

Short Answer

Expert verified
(c) Cs虏鈦� to Cs鲁鈦� involves the greatest energy.

Step by step solution

01

Understanding Ionization Potential

Ionization potential refers to the energy required to remove an electron from an atom or ion in its gaseous state. It typically increases as electrons are removed from closer energy levels or higher positive charged species.
02

Equation Analysis - First Ionization

In options (a) and (b), first ionization is occurring where a neutral atom loses one electron to form a singly charged ion: - (a) Na to Na鈦� - (b) K to K鈦� The ionization potentials for first ionizations are usually lower than for higher ionizations because they involve removal from less strongly attracted outer electrons.
03

Equation Analysis - Subsequent Ionizations

In options (c) and (d), an electron is removed from ions with existing positive charge: - (c) Cs虏鈦� to Cs鲁鈦� - (d) Ca鈦� to Ca虏鈦� These involve greater amounts of energy because it's harder to remove electrons from positively charged ions due to greater attractive forces on the electrons.
04

Comparison of Higher Ionizations

Comparing (c) and (d), removing an electron from a doubly charged cation like Cs虏鈦� (c) to form a triply charged ion involves the greatest energy because each additional positive charge significantly increases the electron's attraction to the nucleus. This is more intense than the energy needed to remove an electron from Ca鈦� to form Ca虏鈦� in (d).
05

Conclusion

The transfer from Cs虏鈦� to Cs鲁鈦� (c) requires the most energy due to increased positive charge and smaller atomic radius, leading to a stronger attraction of the electron to the nucleus.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

First Ionization Energy
The first ionization energy is the energy needed to remove the first electron from a neutral atom. In simple terms, it's like peeling off the first layer of an onion鈥攖he outer electrons are removed first. These outer electrons tend to be less tightly bound than those closer to the atom's center because they are shielded by inner electrons from the full attraction of the nucleus.

For elements such as sodium (Na) and potassium (K) in our example, this involves transforming:
  • Sodium (Na) to Sodium ion (Na鈦�)
  • Potassium (K) to Potassium ion (K鈦�)
First ionization energies are generally lower compared to second or third ionizations because breaking the "first bond" is always the easiest. It generally requires less energy to remove the first electron from the outermost shell.
Subsequent Ionization
As we remove more electrons, the process is referred to as subsequent ionization. Each electron removal beyond the first is called a subsequent ionization.
  • In our given equations, looking at Cs虏鈦� to Cs鲁鈦� and Ca鈦� to Ca虏鈦� showcases second and third ionizations.
This process requires much more energy than removing the first electron because, with each removal, the remaining electrons are held more tightly by the nucleus. The increase in positive charge after each electron is removed increases the attraction between the electrons and the nucleus, requiring more significant energy input for subsequent ionizations.
Energy Levels
Every electron in an atom is located in an energy level or shell. These levels are like rungs on a ladder, where moving up the ladder requires energy.
  • Electrons closer to the nucleus are at lower energy levels and are held more tightly.
  • Outer electrons, at higher energy levels, are easier to remove.
In the context of ionization, the energy level tells us how much energy is required to remove an electron. The lower the energy level (closer to the nucleus), the more challenging it is to remove the electron, thus requiring a higher ionization energy.
Charge and Electron Removal
When ionizing an atom or ion, electron removal becomes increasingly challenging as the positive charge of the ion increases.
  • More positively charged ions attract electrons more strongly.
  • Consequently, subsequent ionizations become more energy-consuming.
Considering our step by step problem solution, removing an electron from Cs虏鈦� to form Cs鲁鈦� entails a significant amount of energy due to the increased nuclear charge. In simpler terms, as you remove more electrons, the remaining ones cling more closely to the positively charged nucleus, making each subsequent removal require an even greater amount of energy.

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Most popular questions from this chapter

Pick out the statement(s) which is are not true about the diagonal relationship of \(\mathrm{Li}\) and \(\mathrm{Mg}\). (1) Polarizing powers of \(\mathrm{Li}^{+}\)and \(\mathrm{Mg}^{2+}\) are almost same. (2) Like Li, Mg decomposes water very fast. (3) \(\mathrm{LiCl}\) and \(\mathrm{MgCl}_{2}\) are deliquescent. (4) Like Li, Mg readily reacts with liquid bromine at ordinary temperature. (a) (1) and (4) (b) (2) and (4) (c) only (2) (d) only(l)

Which one of the following sets of ions represents a collection of isoelectronic species? [2006] (a) \(\mathrm{K}^{+}, \mathrm{Cl}^{-}, \mathrm{Ca}^{2+}, \mathrm{Sc}^{3+}\) (b) \(\mathrm{Ba}^{2+}, \mathrm{Sr}^{2+}, \mathrm{K}^{+}, \mathrm{Ca}^{2+}\) (c) \(\mathrm{N}^{3}, \mathrm{O}^{2-}, \mathrm{F}^{-}, \mathrm{S}^{2-}\) (d) \(\mathrm{Li}^{+}, \mathrm{Na}^{+}, \mathrm{Mg}^{2+}, \mathrm{Ca}^{2+}\)

An element with atomic number 34 belongs to which period?

Match the following: List I element with highest electronegativity 2- element with highest electron affinity 3\. liquid non metal 4\. metallic solid List II (i) \(\mathrm{I}_{2}\) (ii) \(\mathrm{Br}_{2}\) (iii) \(\mathrm{Cl}_{2}\) (iv) \(\mathrm{F}_{2}\) The correct matching is: $$ \begin{array}{|c|c|c|c|c|} \hline & 1 & 2 & 3 & 4 \\ \hline \mathrm{a} & \text { (iii) } & \text { (ii) } & \text { (i) } & \text { (iv) } \\ \hline \mathrm{b} & \text { (iv) } & \text { (iii) } & \text { (i) } & \text { (ii) } \\ \hline \mathrm{c} & \text { (ii) } & \text { (iii) } & \text { (iv) } & \text { (i) } \\ \hline \mathrm{d} & \text { (i) } & \text { (ii) } & \text { (iii) } & \text { (iv) } \\ \hline \end{array} $$

The correct statement among the following is (a) the first ionization potential of \(\mathrm{Al}\) is less than the first ionization potential of \(\mathrm{Mg}\). (b) the second ionization potential of \(\mathrm{Mg}\) is greater than the second ionization potential of \(\mathrm{Na}\). (c) the first ionization potential of \(\mathrm{Na}\) is less than the first ioniation potential of \(\mathrm{Mg}\). (d) the third ionization potential of \(\mathrm{Mg}\) is greater than the third ionization potential of Al.
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