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Chapter 8: Problem 19

Without referring to a periodic table, write the electron configurations of elements with these atomic numbers: (a) \(9,\) (b) \(20,\) (c) \(26,\) (d) 33. Classify the elements.

Short Answer

Expert verified
For atomic number 9: 1s² 2s² 2p⁵ (p block), atomic number 20: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² (s block), atomic number 26: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d⁶ (d block), and atomic number 33: 1s² 2s² 2p⁶ 3s² 3p⁶ 4s² 3d¹⁰ 4p³ (p block).

Step by step solution

01

Understanding the Aufbau principle

The Aufbau principle states that an electron occupies the lowest-energy orbital that can receive it, which is represented as: 1s < 2s < 2p < 3s < 3p < 4s < 3d < 4p < 5s < 4d < 5p < 6s. This diagram will guide the electron configurations for each atom number.
02

Configure Electrons for atomic number 9

The atomic number 9 corresponds to 9 electrons. Following the Aufbau principle this gives: 1s2 2s2 2p5. So, it belongs to the p block.
03

Configure Electrons for atomic number 20

For atomic number 20, we have 20 electrons. Following the pattern: 1s2 2s2 2p6 3s2 3p6 4s2. So, it falls in the s block.
04

Configure Electrons for atomic number 26

For atomic number 26, there are 26 electrons, giving: 1s2 2s2 2p6 3s2 3p6 4s2 3d6. It's a d block element.
05

Configure Electrons for atomic number 33

For atomic number 33, the electron configuration becomes: 1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p3. Therefore, it's a p block element.

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Most popular questions from this chapter

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