Question

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

Short answer

The correct match is: (b) (4), (3), (2).

Step-by-step solution

Identify Properties for Items in List I

To solve the matching task, start by identifying the property each element in List I represents: 1. Element with highest electronegativity. 2. Element with highest electron affinity. 3. Liquid non-metal. 4. Metallic solid.

Recognize Properties of Elements in List II

Now, relate the elements in List II to their features:- \(\mathrm{I}_2\) ": Iodine is relatively electronegative but not the highest.- \(\mathrm{Br}_2\) ": Bromine is a liquid at room temperature.- \(\mathrm{Cl}_2\) ": Chlorine has one of the highest electron affinities.- \(\mathrm{F}_2\) ": Fluorine is the most electronegative element.

Match the Items Based on Properties

Based on the identified properties, match the elements:1. \(\mathrm{F}_2\) has the highest electronegativity, so it matches with List I's point 1.2. \(\mathrm{Cl}_2\) has the highest electron affinity, so it matches with List I's point 2.3. \(\mathrm{Br}_2\) as a liquid non-metal matches with List I's point 3.4. None of the given options in List II corresponds to a metallic solid. Therefore, point 4 cannot be matched with any option from List II.

Conclusion from Matches

The matched pairs are: 1. (4) for highest electronegativity \(\mathrm{F}_2\).2. (3) for highest electron affinity \(\mathrm{Cl}_2\).3. (2) for liquid non-metal \(\mathrm{Br}_2\). Since there's no match for a metallic solid, choose option (b) as it correctly identifies the available matches.

Key concepts

Electronegativity

Electronegativity is a measure of an atom's ability to attract and hold onto electrons within a chemical bond. It is a fundamental concept in chemistry that helps explain how atoms interact with one another. The higher the electronegativity, the more an atom attracts electrons.

Fluorine ( F_2) is known as the most electronegative element in the periodic table. It has an electronegativity value of 3.98 on the Pauling scale. This means that it strongly attracts electrons when forming chemical bonds. Understanding electronegativity can help predict how chemical compounds will form and behave.

Here are some key points about electronegativity:

• Electronegativity values increase across a period (left to right) in the periodic table.
• Values tend to decrease as you move down a group (top to bottom).
• The difference in electronegativity between two atoms determines the bond type (ionic, polar covalent, or nonpolar covalent).

Electron Affinity

Electron affinity measures the energy change that occurs when an electron is added to a neutral atom in the gaseous state, forming a negative ion. It indicates how much an atom wants to gain an electron, which can directly affect its reactivity and stability.

Chlorine ( Cl_2) has one of the highest electron affinities, meaning it readily gains electrons to become stable. This is due to the high energy released when it gains an electron, making it a highly reactive element that often forms negative ions in compounds such as NaCl (table salt).

Key aspects of electron affinity include:

• Elements with more negative values release more energy when gaining electrons, indicating higher affinity.
• Electron affinity generally increases across a period and can vary significantly among non-metals.
• Understanding electron affinity can help explain the formation of anions in chemical reactions.

Non-Metal Properties

Non-metals are a group of elements that have distinct properties differentiating them from metals. They are typically poor conductors of heat and electricity and have high ionization energies and electronegativities. Non-metals tend to gain electrons during chemical reactions.

One fascinating aspect of non-metals is the variety in their physical states at room temperature. For example, bromine ( Br_2) is unique among non-metals as it exists as a liquid at room temperature. This contrasting state to the more common gases or solids provides insight into how diverse non-metallic elements can be.

Some essential properties of non-metals include:

• Brittleness in solid form, meaning they shatter rather than bend when struck.
• High ionization energies, making them less likely to lose electrons.
• High electronegativities, often leading to formation of negative ions.
• Exist in a variety of physical states: gases ( O_2, N_2), solids ( C, P), and liquids ( Br_2).

Chemical Properties of Halogens

Halogens are a group of elements found in Group 17 of the periodic table. They are known for their reactivity and are all one electron short of a full outer shell, making them highly eager to gain an electron to achieve stability.

The chemistry of halogens is dominated by their high electronegativity and strong tendency to form negative ions. Each halogen has unique properties, but they share several chemical behaviors. For instance, fluorine ( F_2) is the most reactive and electronegative, capable of forming compounds with almost all other elements. Meanwhile, iodine ( I_2) is less reactive but still enough to form compounds in conditions where fluorine might react explosively.

Key chemical aspects of halogens include:

• Reactivity decreases from fluorine (most reactive) to iodine (least reactive).
• Halogens can form salts, providing the origin of their name from the Greek words "hals" (salt) and "genes" (forming).
• Tend toward diatomic molecules, forming bonds with themselves (e.g., Cl_2, Br_2).
• They exhibit high electron affinities and because of this, often participate in redox reactions.