LewisStructure3. In the Lewis structure of CBr
, the C atom ___ has two double bonds only has four single bonds only has two single bonds, and one double bond only has three single bonds and one lone pair only
The Correct Answer and Explanation is:
In the Lewis structure of CBr₄, the C atom has four single bonds.
Explanation:
When drawing the Lewis structure for CBr₄, the carbon (C) atom is in the center, surrounded by four bromine (Br) atoms. Carbon, being in Group 14 of the periodic table, has four valence electrons, and each bromine atom has seven valence electrons (Group 17). To achieve a stable electron configuration, carbon needs four bonds to complete its octet, and bromine atoms need to gain one electron to complete their octet.
- Carbon shares one electron with each of the four bromine atoms, forming four single bonds. Each bond consists of a pair of electrons, one from carbon and one from bromine.
- The Bromine (Br) atoms each complete their octet by forming a single bond with carbon. Since bromine is in Group 17, each Br atom needs one more electron to achieve a stable octet, and that is provided by bonding with carbon.
In this structure, there are no double bonds between carbon and bromine. There are also no lone pairs on the central carbon atom because it satisfies its octet by bonding with four bromines, and the bromine atoms themselves each have lone pairs to complete their octets.
Thus, the correct answer is that the C atom has four single bonds in CBr₄.
In summary:
- The carbon atom forms four single bonds.
- The structure is tetrahedral because of the four bonds and no lone pairs on carbon.
- There are no double bonds or lone pairs on the central carbon.
