Chapter 4: Problem 49

Consider two main-group elements, \(\mathrm{A}\) and B. Element A has an ionization energy of 419 \(\mathrm{kJ} / \mathrm{mol} .\) Element \(\mathrm{B}\) has an ionization energy of 1000 \(\mathrm{kJ} / \mathrm{mol} .\) Which element is more likely to form a cation?

Short Answer

Expert verified

The element more likely to form a cation is Element A due to its lower ionization energy.

Step by step solution

Understand the Concept of Ionization Energy and Cation Formation

Ionization energy is the energy required to remove an electron from an atom. A cation is formed when an atom loses an electron. The element with a lower ionization energy would more easily lose an electron, and thus, is more likely to form a cation.

Compare the Ionization Energies of the Given Elements

As per the exercise, Element A has an ionization energy of 419 \( \mathrm{kJ} / \mathrm{mol} \) and Element B has an ionization energy of 1000 \( \mathrm{kJ} / \mathrm{mol} \). Comparing these values, Element A has a lower ionization energy than Element B.

Determine Which Element is More Likely to Form a Cation

Since Element A has the lower ionization energy compared to Element B, it requires less energy to remove its electron(s). Therefore, Element A is more likely to form a cation.

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Consider two main-group elements, \(\mathrm{A}\) and B. Element A has an ionization energy of 419 \(\mathrm{kJ} / \mathrm{mol} .\) Element \(\mathrm{B}\) has an ionization energy of 1000 \(\mathrm{kJ} / \mathrm{mol} .\) Which element is more likely to form a cation?

Short Answer

Step by step solution

Understand the Concept of Ionization Energy and Cation Formation

Compare the Ionization Energies of the Given Elements

Determine Which Element is More Likely to Form a Cation

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