23. Explain the following.
i) PbO, acts as oxidising agent.
ii) Halogens are strong oxidizing agent.
निम्नलिखित की व्याख्या कीजिए :
1) Pbo, ऑक्सीकारक की तरह कार्य करता है.
ii) हैलोजन प्रबलतम् ऑक्सीकारक होते हैं।
Answers
Answer:
i)PbO, acts as oxidising agent.
has a higher tendency to be reduced, which means to gain electrons. A substance is reduced when it oxidizes or takes electrons from another substance.
Lead has an atomic number of 82 that is it's electronic configuration is [Xe] 4f14 5d10 6s2 6p2. The 6s2 electron has a tendency to participate in the formation of a chemical bonding . That is why lead exists in two oxidation states 2+ and 4+ . The 4+ state is very unstable because there is a huge energy difference between the 6s and 6p electrons . So it is not an easy process to promote the 6s electrons to the 6p sub shell for the formation of +4 oxidation state by lead removing it's 4 electrons because this requires a lot of energy . This is known as inert electron pair effect .
ii)Halogens are strong oxidizing agents because they have high electronegativity and high electron affinity which makes them to take electrons very much readily takes electrons from other elements and oxidise other elements.
Decreasing order of Oxidising strength among halogens is : F > Cl > Br > I
Thus, halogens need only one more electron to complete their octet and to attain the stable noble gas configuration. Also, halogens are highly electronegative with low dissociation energies and high negative electron gain enthalpies. Therefore, they have a high tendency to gain an electron. Hence, they act as strong oxidizing agents
Explanation:
Explanation:
i)PbO, acts as oxidising agent.
has a higher tendency to be reduced, which means to gain electrons. A substance is reduced when it oxidizes or takes electrons from another substance.
Lead has an atomic number of 82 that is it's electronic configuration is [Xe] 4f14 5d10 6s2 6p2. The 6s2 electron has a tendency to participate in the formation of a chemical bonding . That is why lead exists in two oxidation states 2+ and 4+ . The 4+ state is very unstable because there is a huge energy difference between the 6s and 6p electrons . So it is not an easy process to promote the 6s electrons to the 6p sub shell for the formation of +4 oxidation state by lead removing it's 4 electrons because this requires a lot of energy . This is known as inert electron pair effect .
ii)Halogens are strong oxidizing agents because they have high electronegativity and high electron affinity which makes them to take electrons very much readily takes electrons from other elements and oxidise other elements.
Decreasing order of Oxidising strength among halogens is : F > Cl > Br > I
Thus, halogens need only one more electron to complete their octet and to attain the stable noble gas configuration. Also, halogens are highly electronegative with low dissociation energies and high negative electron gain enthalpies. Therefore, they have a high tendency to gain an electron. Hence, they act as strong oxidizing agents