Question

Which of the following represents Plumbous ions?
(A) $P{{b}^{+2}}$
(B) $P{{b}^{+4}}$
(C) $P{{b}^{+1}}$
(D) $P{{b}^{+3}}$

Answer 1

Pb is a chemical element with atomic number 82 and the symbol Pb. It's a type of heavy metal that's denser than most other metals. Lead is both soft and pliable, as well as having a low melting point. Lead is silvery with a tinge of blue when freshly cut; when exposed to air, it tarnishes to a drab grey tint. Lead has the greatest atomic number of any stable element, and three of its isotopes are nuclear decay endpoints for heavier elements.

Complete Step By Step Answer:
The oxidation states of lead are +4 and +2. For the carbon group, the tetravalent state is frequent. For carbon and silicon, the divalent state is rare; for germanium, it is minor; for tin, it is important; and for lead, it is the more important of the two oxidation states. This is due to relativistic effects, especially the inert pair effect, which occurs when the electronegativity of lead and oxide, halide, or nitride anions differs significantly, resulting in a substantial partial positive charge on lead. The upshot is that the lead 6s orbital contracts more than the 6p orbital, rendering it relatively inert in ionic compounds.
When lead makes covalent bonds with elements with comparable electronegativity, such as carbon in organolead compounds, the inert pair effect is less effective. The 6s and 6p orbitals are identical in size in these, and $s{{p}^{3}}$ hybridization is still energetically advantageous. In such compounds, lead, like carbon, is mostly tetravalent. Lead(II) has an electronegativity of 1.87, whereas lead(IV) has an electronegativity of 2.33. By comparison, tin has values of 1.80 in the +2 oxidation state and 1.96 in the +4 state, reversing the pattern of increased stability of the +4 oxidation state as one moves down the carbon group.
When lead is combined with another element, it loses two electrons.
Plumbous ion is denoted by the symbol $P{{b}^{+2}}$ .
Hence option A is correct.

Note:
Lead is a post-transition metal that is largely unreactive. Its amphoteric nature exemplifies its weak metallic character; lead and lead oxides react with acids and bases and prefer to form covalent bonds. Lead compounds are generally found in the +2 oxidation state, rather than the +4 oxidation state seen in lighter carbon group members. Organolead compounds are the most common exception. Lead, like the lighter members of the family, has a proclivity for bonding with itself, forming chains and polyhedral structures.