Question

Opbr3 lewis structure

Answer 1

The question appears to reference a compound with a Lewis structure involving a central atom (assumed to be phosphorus) bonded to three bromine atoms and an oxygen atom, possibly implying POBr3. For POBr3, the Lewis structure would show phosphorus at the center with three bromine atoms and a double-bonded oxygen atom, to satisfy the octet rule.

Step-by-step explanation:

The student is asking about constructing a Lewis structure for the compound OPBr3, which seems to be a typographical error but likely refers to a compound containing a central phosphorus atom bonded to three bromine atoms and an oxygen atom, possibly POBr3. The correct Lewis structure of a hypothetical OPBr3 molecule would show the phosphorus atom in the center with three single bonds to bromine atoms and possibly a double bond to oxygen, considering oxygen needs to complete its octet. However, if we are to follow the described structure in the question with a central carbon atom, it conflicts with common valence states of carbon and phosphorus in chemistry. Assuming the molecule is POBr3, and constructing its Lewis structure following valence electron rules, phosphorus would have five valence electrons and each bromine would contribute seven, while oxygen would have six plus one additional electron for the negative charge, leading to a Lewis structure where the central phosphorus atom is bonded to three bromine atoms and one double-bonded oxygen atom, fulfilling the octet rule.

Answer 2

The Lewis dot structure for OPBr3 features a central phosphorus atom with one double bond to oxygen and three single bonds to bromine atoms; oxygen has three lone pairs, bromines have three lone pairs each, and the structure is enclosed in brackets indicating a -2 charge.

Step-by-step explanation:

The Lewis dot structure for OPBr3 starts with a central phosphorus atom bonded to one oxygen and three bromine atoms. The central phosphorus atom has five valence electrons, while oxygen has six and bromine has seven. The oxygen atom is double-bonded to the phosphorus, utilizing four electrons (two pairs), and each bromine is single-bonded to the phosphorus, each utilizing two electrons (one pair).

Since oxygen and bromine atoms need to satisfy the octet rule, each of the bromine atoms will have three lone pairs of electrons, while the oxygen will have three lone pairs after the double bond is formed. The molecule will be drawn inside square brackets with a charge of minus 2, indicating that it is an ion. To show this, each bromine will contribute one extra electron to the central phosphorus to accommodate the two additional electrons required for the charge. No electrons are left for the lone pairs on the central phosphorus atom after this adjustment.

The Lewis structure for OPBr3 will show the central phosphorus with four bonds: one double bond to oxygen and three single bonds to bromines. Oxygen will be illustrated with three lone pairs, and each bromine will have three lone pairs as well. This triangular-shaped molecule with a central phosphorus atom will be enclosed in square brackets indicating it's an ion, with its -2 charge shown outside the brackets.