NEET Practice Questions (MCQs) with Answers & Solutions

$ Cl_2 + 2KBr \rightarrow 2KCl + Br_2 $ A more electronegative halogen can displace less acid because of lowest bond dissociation Energy.

$ 2NaOH(dil) + Cl_2 \rightarrow [] { { Cold} } NaCl + NaClO + H_2O. Sod. Hypochlorite. $ $ 6NaOH(conc) + 3Cl_2 \rightarrow [] { { Heat} } 5NaCl + NaClO_3 + 3H_2O Sodium chlorate $

$Br_2$ gas turns starch iodide paper blue. This happens because bromine ($Br_2$) oxidizes iodide ions ($I^-$) present in the starch iodide paper to iodine ($I_2$). The iodine then reacts with starch to form a blue-colored complex.

HF is weakest acid. Since it is on able to give H + ions which are trapped in H - Bonding

Deacon’s process is used in the manufacture of chlorine ($Cl_2$). In this process, hydrogen chloride ($HCl$) gas is oxidized by atmospheric oxygen in the presence of a copper chloride ($CuCl_2$) catalyst, producing chlorine gas and water.

Iodine is indeed a solid at room temperature. This is because iodine has a relatively high molecular mass and stronger intermolecular forces compared to other halogens like chlorine and bromine, which are gases or liquids at room temperature.

Fluorine ($F_2$) is the most reactive halogen. This is due to its high electronegativity and small atomic size, which allow it to attract electrons more readily compared to other halogens like chlorine ($Cl_2$), bromine ($Br_2$), and iodine ($I_2$).

Iodine (I) has the largest atomic size and the lowest electronegativity among the halogens, making it the most electropositive. Electronegativity decreases down the group in the periodic table, and electropositivity increases. Hence, Iodine shows clear electropositive properties.

The outermost electronic configuration of halogens is $ S^2 P^5 $. Halogens have seven valence electrons, which is represented by this configuration. This configuration makes them highly reactive as they seek to gain one electron to achieve a stable noble gas configuration.