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Chapter 8: Problem 33

Define atomic radius. Does the size of an atom have a precise meaning?

Short Answer

Expert verified
The atomic radius is typically defined as half the distance between the centers of two atoms of the same element that are not bound together. However, the size of an atom isn't precisely defined because the electron cloud surrounding the nucleus doesn't have a defined edge.

Step by step solution

01

Definition of Atomic Radius

The atomic radius, broadly speaking, is half the distance between the centers of two atoms of the same element that are not bound together. It is a measure of the size of an atom's electron cloud or, in simpler terms, the size of an atom.
02

Precision of Atomic Size

In reality, atoms do not have a definitive boundary outside of which electrons cannot be found. The electron cloud surrounding the nucleus doesn't have a defined edge. Consequently, the size of an atom isn't precise and can differ depending on how we choose to measure it.

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Most popular questions from this chapter

The first and second ionization energies of \(\mathrm{K}\) are 419 kJ/mol and \(3052 \mathrm{~kJ} / \mathrm{mol}\), and those of Ca are \(590 \mathrm{~kJ} / \mathrm{mol}\) and \(1145 \mathrm{~kJ} / \mathrm{mol},\) respectively. Compare their values and comment on the differences.

You are given four substances: a fuming red liquid, a dark metallic-looking solid, a pale-yellow gas, and a yellow-green gas that attacks glass. You are told that these substances are the first four members of Group 7A, the halogens. Name each one.

In general, atomic radius and ionization energy have opposite periodic trends. Why?

In halogen displacement reactions a halogen element can be generated by oxidizing its anions with a halogen element that lies above it in the periodic table. This means that there is no way to prepare elemental fluorine, because it is the first member of Group 7A. Indeed, for years the only way to prepare elemental fluorine was to oxidize \(\mathrm{F}\) ions by electrolytic means. Then, in \(1986,\) a chemist reported that by reacting potassium hexafluoromanganate(IV) \(\left(\mathrm{K}_{2} \mathrm{MnF}_{6}\right)\) with antimony pentafluoride \(\left(\mathrm{SbF}_{5}\right)\) at \(150^{\circ} \mathrm{C},\) he had generated elemental fluorine. Balance the following equation representing the reaction: $$ \mathrm{K}_{2} \mathrm{MnF}_{6}+\mathrm{SbF}_{5} \longrightarrow \mathrm{KSbF}_{6}+\mathrm{MnF}_{3}+\mathrm{F}_{2} $$

Sketch the outline of the periodic table and show group and period trends in the first ionization energy of the elements. What types of elements have the highest ionization energies and what types the lowest ionization energies?
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