Problem 101 - A Complete Resource Book in Chemistry for JEE Main

Question

Match the following: List I List II 1\. element with highest (i) \(\mathrm{I}_{2}\) electronegativity 2\. element with highest (ii) \(\mathrm{Br}_{2}\) electron affinity 3\. liquid non metal (iii) \(\mathrm{Cl}_{2}\) 4\. metallic solid (iv) \(\mathrm{F}_{2}\) The correct matching is: (1) (2) (3) (4) (a) (iii) (ii) (i) (iv) (b) (iv) (iii) (i) (ii) (c) (ii) (iii) (iv) (i) (d) (i) (ii) (iii) (iv)

Step-by-Step Solution

Answer

The correct matching is option (d) (i) (ii) (iii) (iv).

Step 1: Matching Highest Electronegativity

Fluorine \((F_2)\) is known to have the highest electronegativity among the elements listed. Thus, we can match element with highest electronegativity to \( (iv) F_2 \).

Step 2: Matching Highest Electron Affinity

Chlorine \( (Cl_2) \) has the highest electron affinity of the elements listed. Therefore, the element with the highest electron affinity corresponds to \( (iii) Cl_2 \).

Step 3: Identifying the Liquid Non-metal

Bromine \( (Br_2) \) is a liquid at room temperature and is a non-metal. Hence, the liquid non-metal matches with \( (ii) Br_2 \).

Step 4: Identifying the Metallic Solid

Iodine \( (I_2) \) is a solid at room temperature and exhibits metallic luster, fitting the description of a metallic solid. Thus, it corresponds to \( (i) I_2 \).

Step 5: Verify Complete Matching

Based on the matches: 1. Element with highest electronegativity: \(iv) F_2 \)2. Element with highest electron affinity: \(iii) Cl_2 \)3. Liquid non-metal: \(ii) Br_2 \)4. Metallic solid: \(i) I_2 \).

Step 6: Determine Correct Answer Choice

Comparing with the options provided:(d) \( (i) (ii) (iii) (iv) \) exactly matches our findings.Therefore, the correct answer is option (d).

Key Concepts

Electronegativity in Elements

Electronegativity is a fundamental concept in chemistry, describing how avidly an atom attracts electrons towards itself in a chemical bond. It plays a crucial role in determining the behavior and properties of molecules. One of the scales used to measure electronegativity is the Pauling scale, where fluorine is at the top with a value of 3.98. This means fluorine is highly effective at attracting electrons, which is why it is recognized as the element with the highest electronegativity. The position of elements in the periodic table influences their electronegativity; it generally increases across a period from left to right and decreases down a group. This trend is attributed to the increasing positive charge of the nucleus which pulls electrons closer. However, the added electron shell as you move down a group acts to weaken the attraction due to electron shielding. Understanding electronegativity helps predict how elements will interact with each other, influencing everything from the bond type to molecular geometry.

Electron Affinity in Elements

Electron affinity refers to the change in energy when an atom gains an electron, and it’s an indication of an atom's ability to accept electrons. A higher electron affinity means that an atom more readily accepts an electron, often releasing energy in the process. Atoms with a high electron affinity are typically non-metals; they tend to have nearly full valence shells and benefit from gaining additional electrons to achieve a stable electronic configuration. Chlorine, for instance, possesses the highest electron affinity among the halogens, and a high negative electron affinity value reflects the substantial amount of energy released when it gains an electron. As with electronegativity, electron affinity generally increases across a period and decreases down a group on the periodic table. This is because additional energy levels added with increasing atomic size cause a reduction in the effective nuclear charge felt by the outer electrons. Understanding electron affinity is critical in comprehending aspects like ionic bond formation and the reactivity of elements.

Properties of Halogens

Halogens are a group of elements found in Group 17 of the periodic table, and they exhibit fascinating properties due to their similar electronic configurations. These elements, including fluorine, chlorine, bromine, and iodine, are highly reactive non-metals with seven electrons in their outermost shell, making them just one electron short of the stable noble gas configuration. They exhibit diverse physical states at room temperature:

• Fluorine and chlorine are gases.
• Bromine is a liquid.
• Iodine is a solid.

Their reactivity is influenced by their high electronegativity and electron affinity, which lead them to readily form negative ions. This reactivity makes them useful in a wide range of applications, from disinfectants and bleaching agents to the production of plastics and pharmaceuticals. Understanding the properties and behavior of halogens not only highlights their individual characteristics but also their pivotal role in chemical reactions and industry applications.

Metallic and Non-metallic Properties

Elements are classified as metals, non-metals, or metalloids based on their physical and chemical properties. Metals are typically characterized by their shiny luster, ability to conduct heat and electricity, and tendency to lose electrons. Non-metals, on the other hand, are generally poor conductors and tend to gain electrons. Iodine, although primarily a non-metal, exhibits a unique metallic luster which can sometimes make it appear to be metallic. It is solid at room temperature, unlike bromine which is a liquid, emphasizing the diversity within non-metals. Metallic and non-metallic properties can vary within a group and across the periodic table. Metals are typically found on the left of the periodic table and non-metals on the right, with metalloids displaying properties of both in the middle. Awareness of these properties aids greatly in understanding periodic trends and predicting an element's behavior in various chemical contexts. Such knowledge is foundational in fields ranging from material science to everyday chemical reactions.