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Chapter 2: Problem 24

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

Short Answer

Expert verified
The pairs of elements that are expected to show similar chemical properties are: (K, Na), (F, Cl) and (P, N).

Step by step solution

01

Identify Groups

The first step is to identify the group of each element in the periodic table. Here are their groups: Potassium (K) and Sodium (Na) are in Group 1 (alkali metals), Fluorine (F) and Chlorine (Cl) are in Group 17 (halogens), Phosphorus (P) and Nitrogen (N) are in Group 15 (pnictogens).
02

Form Pairs

Now form pairs of elements that are in the same group which are expected to show similar properties. The pairs that can be formed are: (K, Na), because both are alkaline metals; (F, Cl), because both are halogens; and (P, N), because both are pnictogens.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Understanding Periodic Table Groups
The periodic table is a systematic arrangement of elements based on their atomic number, electron configurations, and recurring chemical properties. Elements in the same column, known as a 'group', tend to share similar chemical properties due to having the same number of valence electrons. These valence electrons determine how the element reacts with other substances.

For instance, in a classroom setting, students sitting at the same table often have similar interests or classes. Similarly, elements in the same group of the periodic table have comparable characteristics. Recognizing these groups is crucial when predicting the behavior of elements in chemical reactions.
The Reactivity of Alkali Metals
Alkali metals, found in Group 1 of the periodic table, are known for their high reactivity, especially with water. This group includes elements like lithium, sodium, potassium, rubidium, cesium, and francium.

Imagine them as the social butterflies of the periodic table who eagerly interact with others. Their single valence electron makes them keen to bond with other elements. The similarities in properties among alkali metals, like softness and low density, can be attributed to their similar electron configuration.
The Highly Reactive Halogens
The halogens make up Group 17 of the periodic table and are composed of the elements fluorine, chlorine, bromine, iodine, and astatine. These nonmetals are known for their high reactivity, particularly with alkali and alkaline earth metals to form salts.

Consider them as the 'clean-up crew', eagerly interacting with metals to create stable compounds. Halogens are unique, as they need only one more electron to reach a full valence shell, leading to their eagerness to react and form negative ions called halides.
Pnictogens: The Versatile Group 15
Take Group 15, where the pnictogens reside; this group includes nitrogen, phosphorus, arsenic, antimony, and bismuth. These elements are quite the all-rounders, able to form a variety of compounds thanks to their five valence electrons.

They tend to form three covalent bonds as they seek to fill or share their three remaining electrons to complete an octet. This ability to form multiple bonds makes pnictogens essential in a wide array of biological and industrial processes.

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Most popular questions from this chapter

(a) Describe Rutherford's experiment and how it led to the structure of the atom. How was he able to estimate the number of protons in a nucleus from the scattering of the \(\alpha\) particles? (b) Consider the \({ }^{23} \mathrm{Na}\) atom. Given that the radius and mass of the nucleus are \(3.04 \times 10^{-15} \mathrm{~m}\) and \(3.82 \times 10^{-23} \mathrm{~g},\) respectively, calculate the density of the nucleus in \(\mathrm{g} / \mathrm{cm}^{3}\). The radius of a \({ }^{23}\) Na atom is \(186 \mathrm{pm}\). Calculate the density of the space occupied by the electrons in the sodium atom. Do your results support Rutherford's model of an atom? [The volume of a sphere is \((4 / 3) \pi r^{3},\) where \(r\) is the radius. \(]\)

Compare the properties of: \(\alpha\) particles, cathode rays, protons, neutrons, and electrons. What is meant by the term "fundamental particle"?

Elements whose names end with "-ium" are usually metals; sodium is one example. Identify a nonmetal whose name also ends with "-ium."

Give two differences between a metal and a nonmetal

Why do all atoms of an element have the same atomic number, although they may have different mass numbers? What do we call atoms of the same element with different mass numbers? Explain the meaning of each term in the symbol \({ }_{Z}^{A} \mathrm{X}\).
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