Question

In the long form of periodic table, the non-metals are placed in (a) \(s\)-block (b) \(p\)-block (c) \(d\)-block (d) \(f\)-block.

Short answer

Non-metals are placed in the p-block.

Step-by-step solution

Understand the Periodic Table structure

The long form of the periodic table is divided into blocks based on the subshell in which the 'last electron' enters. The blocks are named as s, p, d, and f.

Identify Non-Metal Blocks

Non-metals are elements that generally gain electrons to form anions, have high ionization energies, and are poor conductors of heat and electricity. In the periodic table, non-metals mainly reside in the p-block, although some are also in the s-block.

Choose Correct Option

Among the given options, non-metals are primarily placed in the p-block. Therefore, option (b) is the correct answer.

Key concepts

Periodic Table Blocks

The periodic table is a comprehensive grid that represents the chemical elements in an ordered form, reflecting trends in their properties. These elements are sorted into different blocks known as 's', 'p', 'd', and 'f' blocks, categorizations which relate back to the atomic orbitals or subshells into which the last electron of an element is theoretically added according to its electronic configuration.

Specifically, the s-block comprises the first two groups of the table, including the alkali metals and alkaline earth metals, where the last electron fills the 's' orbital. The p-block contains the last six groups, featuring a mix of metals, metalloids, and non-metals, many of which are essential for life. Next, the d-block consists of transition metals where the 'd' orbitals are being filled, and finally, the f-block, located below the main table, is home to the lanthanides and actinides where the 'f' orbitals are at play.

Those tasked with memorizing sections of the table might benefit from mnemonic devices or visual aids that group elements by their block, enhancing recall through patterns and associations.

Non-Metal Characteristics

Non-metals possess distinct features that contrast them from their metallic counterparts. A fundamental understanding of these characteristics assists in predicting non-metal behavior in various states and reactions.

Common traits of non-metals include their tendency to gain electrons due to their high electronegativity, leading to the formation of anions. They also display high ionization energies, as they are more inclined to accept electrons than to give them up. Additionally, non-metals are often poor conductors of heat and electricity and exhibit higher volatility, low elasticity, and a lack of metallic luster in their natural state. They can be found in all three states of matter at room temperature: solids (e.g., carbon), liquids (e.g., bromine), and gases (e.g., oxygen).

Moreover, non-metals serve various roles in both inorganic and organic chemistry, including the formation of life-essential molecules like DNA. Students should pay attention to these properties, as they can often deduce the behavior of unknown non-metals through an understanding of their characteristics.

Electronic Configuration

Understanding the electronic configuration of elements is pivotal for grasping fundamental chemistry concepts. Electronic configuration refers to the distribution of electrons in an atom's orbitals, which are distinct energy levels around the nucleus. Primary configuration involves electrons filling the orbitals in ascension of their energy levels, following the Aufbau principle, Pauli exclusion principle, and Hund's rule.

A simplified representation of this is '1s² 2s² 2p⁶...' — indicating how electrons fill the 's', 'p', 'd', and 'f' orbitals. In the context of non-metals, their electronic configurations end in the 'p' orbital, as they seek the most stable, noble-gas electron configuration by gaining the requisite number of electrons to fill their outermost p-orbitals.

Students learning chemistry must familiarize themselves with the fundamental rules governing the electronic configuration to predict the chemical behavior of elements, from forming bonds to their reactivity. Simplification techniques or mnemonics such as the 'periodic table block' method can be beneficial in mastering this complex concept.