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Chapter 9: Problem 11

Explain why the radii of atoms do not simply increase uniformly with increasing atomic number.

Short Answer

Expert verified
The size of atoms does not increase uniformly with increasing atomic number because the atomic number increases nuclear charge which pulls the electrons closer, hence decreasing the radius. At the same time, the addition of new energy levels and electron-electron repulsion in these levels tend to increase the atomic radius. Both these factors together, make the atomic size vary non-uniformly with atomic number.

Step by step solution

01

Understanding Atomic Structure

An atom consists of a nucleus (containing protons and neutrons) with surrounding energy levels in which electrons move. The number of protons is the atomic number of the atom. When an electron is added, it will occupy an energy level. The more levels an atom has, the larger the atom is.
02

Explain the role of Atomic Number

The atomic number increases as we move from left to right and top to bottom in the periodic table. As the atomic number increases, the number of protons in the nucleus increases. This increases the nuclear charge, pulling the electrons closer to the nucleus and, thus, decreasing the atomic radius.
03

Role of Electron Shielding

However, every time we move to a new period in the periodic table, a new energy level is added. This increases the size of the atom regardless of the number of protons. Additionally, the electron-electron repulsion in these new energy levels also causes the electrons to spread out more, thereby increasing the size of the atom.
04

Consideration of Both Factors

Both the increasing atomic number, which tends to decrease atomic radius, and the addition of new energy levels and electron-electron repulsion, which tend to increase atomic radius, play a role. Therefore, the radii of atoms do not simply increase uniformly with increasing atomic number.

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Most popular questions from this chapter

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