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Chapter 3: Problem 17

What do you mean by representative elements? Give example.

Short Answer

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Answer: Representative elements, also known as main group elements, are located in groups 1, 2, and 13-18 of the Periodic Table and have their outermost electrons in s or p orbitals. Their chemical properties typically represent the properties of their respective groups. Examples include alkali metals such as lithium (Li) and sodium (Na); alkaline earth metals like beryllium (Be) and magnesium (Mg); and p-block elements such as boron (B), carbon (C), nitrogen (N), oxygen (O), fluorine (F), and helium (He).

Step by step solution

01

Definition of Representative Elements

Representative elements, also known as main group elements, are located in groups 1, 2, and 13-18 of the Periodic Table. They include the alkali metals, alkaline earth metals, and elements within the p-block (groups 13-18). These elements are referred to as representative elements because their chemical properties typically represent the properties of their respective groups, and they have a wide range of properties. These elements have their outermost electrons in s or p orbitals, which determine their chemical and physical properties.
02

Examples of Representative Elements

To illustrate the concept of representative elements, we can provide examples from the Periodic Table: 1. Alkali Metals (Group 1): These elements have one electron in their outermost (s) orbital, making them highly reactive. Examples include lithium (Li), sodium (Na), and potassium (K). 2. Alkaline Earth Metals (Group 2): These elements have two electrons in their outermost (s) orbital, making them slightly less reactive than alkali metals but still very reactive. Examples include beryllium (Be), magnesium (Mg), and calcium (Ca). 3. P-block elements (Groups 13-18): These elements have varying numbers of electrons in their outermost (p) orbitals, which impacts their reactivity and properties. Examples include boron (B) from Group 13, carbon (C) from Group 14, nitrogen (N) from Group 15, oxygen (O) from Group 16, fluorine (F) from Group 17, and helium (He) from Group 18. In summary, representative elements are main group elements with a wide range of properties. They are significant because they help us understand the trends and chemical properties of groups within the Periodic Table.

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Key Concepts

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

Periodic Table
The Periodic Table is a comprehensive chart that organizes all known chemical elements in an informative way. It's structured in rows and columns based on atomic number, electron configuration, and recurring chemical properties. The Periodic Table is exceptionally useful for scientists because it visually displays relationships among elements. Each element is positioned to highlight predictability in atomic structure and properties.

The table is divided into blocks based on the subshells being filled with electrons: s-block, p-block, d-block, and f-block. Representative elements, located in groups 1, 2, and 13-18, primarily encompass the s-block and p-block elements. This layout supports the depiction of trends in element behavior, such as reactivity and ionization energy, making the Periodic Table a vital tool for understanding chemical interactions.
Alkali Metals
Alkali metals are found in Group 1 of the Periodic Table. These are some of the most reactive metals, owing to their single electron in the outermost s-orbital. This lone electron is easily lost, making these elements highly reactive, particularly with water, to form alkaline hydroxides and hydrogen gas.

Key characteristics of alkali metals include:
  • Soft texture which can often be cut with a knife.
  • Low melting and boiling points relative to most other metals.
  • High electrical conductivity.
  • Forming +1 ions by losing their valence electron.
  • Strongly react with halogens to form ionic salts.
Examples of alkali metals include:
  • Lithium (Li)
  • Sodium (Na)
  • Potassium (K)
These properties collectively make alkali metals an essential area of study in chemistry, particularly when learning about basic metallic chemistry and reactivity.
Alkaline Earth Metals
Alkaline earth metals are located in Group 2 of the Periodic Table, directly adjacent to the alkali metals. They possess two electrons in their outermost s-orbital, resulting in less reactivity compared to alkali metals, but they are still relatively reactive compared to most elements. Their two valence electrons can be lost to form +2 ions, enabling them to engage easily in chemical reactions.

Distinct properties of alkaline earth metals include:
  • Higher melting points compared to alkali metals.
  • Greater hardness, often not as soft as alkali metals.
  • Effective conductors of electricity.
  • Commonly forming oxide and carbonate compounds.
  • Less soluble in water compared to alkali metal compounds.
Common examples include:
  • Beryllium (Be)
  • Magnesium (Mg)
  • Calcium (Ca)
Their balanced properties and relative stability make them crucial in various fields, from materials science to biological systems.
P-block Elements
The p-block is a significant portion of the Periodic Table, containing the final six groups (13-18). These elements have their outermost electrons in p orbitals, resulting in a wide range of chemical properties. Because these groups span metals, metalloids, and non-metals, the p-block displays exceptional diversity in chemical behavior.

Key features of p-block elements include:
  • Variable valency, often displaying more than one oxidation state.
  • Non-metallic elements tend to form covalent bonds.
  • Typical of forming strong acids and bases.
  • Presence of several elements essential for life (such as carbon and nitrogen).
  • The ability to form complex compounds.
Examples of p-block elements across different groups include:
  • Boron (B) from Group 13
  • Carbon (C) from Group 14
  • Nitrogen (N) from Group 15
  • Oxygen (O) from Group 16
  • Fluorine (F) from Group 17
  • Helium (He) from Group 18
This group of elements is central to many aspects of chemistry, driving both industrial processes and academic research.

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Most popular questions from this chapter

What are the merits and limitations of the long form of periodic table?

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Why is the modern periodic table also referred as Bohr's table?

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