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Chapter 6: Problem 13

What are three characteristics of an atom (or ion) which must be considered in determining its relative radius?

Short Answer

Expert verified
The three characteristics of an atom or ion to be considered when determining its relative radius are the atomic number, the ionic charge, and the electron configuration.

Step by step solution

01

Identifying the Atomic Number

The first characteristic to consider is the atomic number. The atomic number of an atom or ion gives the number of protons in the nucleus, which correlates with the number of electrons (in a neutral atom). An atom with a greater atomic number will have more electron shells, making it larger in size.
02

Considering the Ionic Charge

The second characteristic to consider is the ionic charge. Ions are atoms that have gained or lost electrons. When an atom loses an electron and becomes a positive ion (cation), it decreases in size. This is because the number of protons now exceeds the number of electrons, and the electrons are pulled in closer to the nucleus due to the stronger net positive charge. On the other hand, when an atom gains an electron becoming a negative ion (anion), the ion increases in size. This is because the number of electrons now exceeds the number of protons, causing the electrons to spread out more due to repulsion.
03

Contemplating the Electron Configuration

The last characteristic to consider is the electron configuration, especially whether the highest energy electron falls in an s or p block on the periodic table. Atoms with a high energy electron in a p block in general have larger radii than those with an electron in the s block. This is due to the fact that the farther an electron orbital from the nucleus, the less tightly it is held by the protons in the nucleus and hence, these electrons are more likely to be found further from the nucleus, giving the atom a larger atomic radius.

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Most popular questions from this chapter

Why does the core charge increase as one moves from left to right across a period in the periodic table - for example, from boron to carbon to oxygen?

What trend in atomic radius is observed as one moves down a group in the periodic table? Explain why this trend exists.

Predict which is larger: the \(\mathrm{O}^{2-}\) ion or the \(\mathrm{F}^{-}\) ion. Explain your reasoning.

Provide a shell model diagram for \(\mathrm{K}^{+}\) showing all electrons explicitly and then show how the core charge for \(\mathrm{K}^{+}\) was calculated.

What trend in atomic radius is observed as one moves from left to right across a period? Explain why this trend exists.
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