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Chapter 8: Problem 41

Why is the radius of the lithium atom considerably larger than the radius of the hydrogen atom?

Short Answer

Expert verified
The atomic radius of Lithium atom is larger than that of hydrogen because lithium has more energy levels (electron shells). While hydrogen has only 1 energy level, lithium has 2.

Step by step solution

01

Understanding Atomic Structure

Atomic structure is key to answering this question. The smallest component of an element is its atom. An atom is made up of a nucleus, which contains protons and neutrons, and electrons which orbit the nucleus in energy levels also known as electron shells.
02

Understanding Hydrogen and Lithium Atoms

Hydrogen has 1 proton and 1 electron that orbits around the nucleus in a single energy level or electron shell. On the other hand, Lithium has 3 protons, 4 neutrons and 3 electrons, with two electrons in the first energy level and one in the second energy level. More energy levels (or electron shells) mean a greater distance from the nucleus to the outermost electron, increasing the atomic radius.
03

The Role of Electron Shells in Determining Atomic Radius

The more electron shells an atom has, the larger its atomic radius. The size of the atom is determined by the size of the area which the electrons occupy (known as the electron cloud). Each electron shell can only hold a certain number of electrons. Hydrogen has 1 electron in its 1st and only shell, whereas lithium has 2 electrons in its 1st shell and 1 electron in its 2nd shell. Hence, lithium has a larger atomic radius because it has more electron shells than hydrogen.

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Most popular questions from this chapter

List these ions in order of increasing ionic radius: \(\mathrm{N}^{3-}, \mathrm{Na}^{+}, \mathrm{F}^{-}, \mathrm{Mg}^{2+}, .\mathrm{O}^{2-}\)

What factors account for the unique nature of hydrogen?

Arrange the following isoelectronic species in order of (a) increasing ionic radius and (b) increasing ionization energy: \(\mathrm{O}^{2-}, \mathrm{F}^{-}, \mathrm{Na}^{+}, \mathrm{Mg}^{2+}\).

Name the ions with +3 charges that have these electron configurations: (a) \([\mathrm{Ar}] 3 d^{3},(\mathrm{~b})[\mathrm{Ar}],\) (c) \([\mathrm{Kr}] 4 d^{6}\) (d) \([\mathrm{Xe}] 4 f^{14} 5 d^{6}\)

What is a representative element? Give names and symbols of four representative elements.
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