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Chapter 2: Problem 65

Group the following elements in pairs that you would expect to show similar chemical properties: \(\mathrm{K}, \mathrm{F}, \mathrm{P}, \mathrm{Na}, \mathrm{Cl},\) and \(\mathrm{N}\)

Short Answer

Expert verified
The paired elements are \(\mathrm{K}\) and \(\mathrm{Na}\), \(\mathrm{F}\) and \(\mathrm{Cl}\), and \(\mathrm{P}\) and \(\mathrm{N}\).

Step by step solution

01

Understand the Periodic Table

Understand how the periodic table is arranged. Elements in the same vertical column of the periodic table, also known as a group, have similar chemical properties because they have the same number of valence electrons, which are responsible for an element's chemical properties.
02

Identify Elements' Groups

From the provided elements, we know that \(\mathrm{K}\) (Potassium) and \(\mathrm{Na}\) (Sodium) belong to Group 1 (Alkali metals). They each have one valence electron. \(\mathrm{F}\) (Fluorine) and \(\mathrm{Cl}\) (Chlorine) belong to Group 17 (Halogens). They each have seven valence electrons. And, \(\mathrm{P}\) (Phosphorus) and \(\mathrm{N}\) (Nitrogen) belong to the Nitrogen group. Therefore elements in each pair should have similar chemical properties due to the same number of valence electrons.
03

Grouping the Pairs

With the knowledge from step 2, we can now group the elements. Group 1: \(\mathrm{K}\) and \(\mathrm{Na}\) because they are alkali metals. Group 2: \(\mathrm{F}\) and \(\mathrm{Cl}\) because they are Halogens. Group 3: \(\mathrm{P}\) and \(\mathrm{N}\) since both belong to the Nitrogen group. These pairs are expected to show similar chemical properties as they belong to the same group in the periodic table.

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Most popular questions from this chapter

Give two differences between a metal and a nonmetal

Give the number of protons and electrons in each of the following common ions: \(\mathrm{Na}^{+}, \mathrm{Ca}^{2+}, \mathrm{Al}^{3+}, \mathrm{Fe}^{2+}\), \(\mathrm{I}^{-}, \mathrm{F}^{-}, \mathrm{S}^{2-}, \mathrm{O}^{2-}, \mathrm{N}^{3-}\)

Give two examples of each of the following: (a) a diatomic molecule containing atoms of the same element, (b) a diatomic molecule containing atoms of different elements, (c) a polyatomic molecule containing atoms of the same element, (d) a polyatomic molecule containing atoms of different elements.

These phosphorus sulfides are known: \(\mathrm{P}_{4} \mathrm{~S}_{3}, \mathrm{P}_{4} \mathrm{~S}_{7}\) and \(\mathrm{P}_{4} \mathrm{~S}_{10}\). Do these compounds obey the law of multiple proportions?

One isotope of a metallic element has a mass number of 65 and has 35 neutrons in the nucleus. The cation derived from the isotope has 28 electrons. Write the symbol for this cation.
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