Problem 39 Why do the elements of the same ... [FREE SOLUTION]

Chapter 3: Problem 39

Why do the elements of the same group show identical property? Explain.

Short Answer

Expert verified

Answer: Elements in the same group of the periodic table have identical properties because they have the same number of valence electrons. This results in similarities in their chemical behavior, as the valence electrons determine how elements form bonds and interact with other elements, which is the basis for their chemical properties. For example, alkali metals (Group 1) all have one valence electron, making them highly reactive, while halogens (Group 17) have seven valence electrons, making them highly reactive non-metals.

Step by step solution

Understand the periodic table structure

The periodic table is organized into groups (columns) and periods (rows), based on their atomic structure and properties. Elements within the same group have the same number of valence electrons, which are the electrons in the outermost energy level.

Valence electrons and chemical properties

Chemical properties of an element predominantly depend on the arrangement of valence electrons that are involved in the formation of chemical bonds. Elements in the same group, thus, have similar chemical properties, because their valence electrons are available for bonding in a similar way.

Example of Group 1 - Alkali Metals

Group 1 of the periodic table consists of the alkali metals: lithium (Li), sodium (Na), potassium (K), rubidium (Rb), cesium (Cs), and francium (Fr). They all have one valence electron, leading to similar chemical properties among them. They are highly reactive and readily lose their single valence electron to form +1 ions with non-metal elements, producing compounds like halides.

Example of Group 17 - Halogens

Group 17 of the periodic table consists of the halogens: fluorine (F), chlorine (Cl), bromine (Br), iodine (I), and astatine (At). They all have seven valence electrons and tend to gain one electron to complete their outer electron shell, forming -1 ions. Consequently, they exhibit similar chemical properties and are highly reactive non-metals. They form ionic compounds with alkali metals, for example, NaCl, and covalent compounds with non-metals, for example, Cl_2.

Conclusion

Elements in the same group of the periodic table show identical properties because they have the same number of valence electrons, leading to similarities in their chemical behavior. These valence electrons determine how elements form bonds and interact with other elements, which is the basis for their chemical properties.

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Key Concepts

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

Periodic Table Groups

The periodic table is an iconic symbol in chemistry, organizing all known elements into a coherent layout based on atomic number and chemical properties. Elements in the same group or column share defining traits. This arrangement helps predict the behavior of these elements in chemical reactions. For example, the similar properties that elements in the same group exhibit are due to sharing the same number of valence electrons. This contributes to patterns in reactivity, ion formation, and bonding preferences which students can use as a basis to predict the chemical behavior of unfamiliar elements.

Valence Electrons

Valence electrons play a star role in the chemical drama. They are the electrons located in the outermost shell of an atom and are pivotal in the atom's ability to bond with others. Since elements in a group have identical numbers of valence electrons, they often share similar chemical characteristics. Understanding their role can significantly boost comprehension when predicting how an element will interact with others. Just as actors follow a script, valence electrons follow rules that influence whether elements will partake in a bond and how stable that bond will be.

Chemical Bonding

Chemical bonds are the glue that holds atoms together in molecules and compounds. At its core, bonding involves the valence electrons of atoms. There are several types of bonds 鈥� iconic, covalent, and metallic being the most common. Ionic bonds typically involve metals donating electrons to nonmetals, leading to the formation of oppositely charged ions that attract. Covalent bonds, on the other hand, involve sharing electron pairs between atoms. Understanding how these bonds form and what characteristics they impart is essential for grasping the fundamentals of chemical reactions.

Alkali Metals

Alkali metals, sitting comfortably in Group 1 of the periodic table, are the social butterflies of elements, always ready to react and mingle, particularly with halogens. These metals have a single valence electron that they readily give up to achieve a more stable configuration. This results in the hallmark reaction profile of these metals: they tend to form +1 ions with exceptional reactivity, especially when mixed with water. Their eagerness to lose that one valence electron also makes them useful in many applications, from batteries to pharmaceuticals.

Halogens

Halogens, occupying Group 17, are the electron seekers, each needing one more electron to complete their outermost shell. Their seven valence electrons make them highly electronegative and reactive, particularly with the alkali metals to form salts like table salt, sodium chloride (NaCl). They can also share electrons with other nonmetals to form covalent bonds, resulting in a variety of organic and inorganic compounds. Halogens are not only chemically interesting but are also of great practical importance, finding uses in disinfection, pharmaceuticals, and as household bleach.

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Why do the elements of the same group show identical property? Explain.

Short Answer

Step by step solution

Understand the periodic table structure

Valence electrons and chemical properties

Example of Group 1 - Alkali Metals

Example of Group 17 - Halogens

Conclusion

Key Concepts

Periodic Table Groups

Valence Electrons

Chemical Bonding

Alkali Metals

Halogens

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