Question

A 0.08425 g sample of gas occupies 10.0-mL at 292.5 K and 1.10 atm. Upon further analysis, the compound is found to be 13.068% C and 86.932% Br. What is the molecular formula of the compound?

Identify the geometry around each carbon atom. a)trigonal pyramidal b)bent c)tetrahedral d)linear e)trigonal planar Is the compound polar or nonpolar?

Answer 1

The empirical formula of the compound is CBr6. The geometry around each carbon atom is octahedral. The compound is polar due to its polar covalent bonds.

Step-by-step explanation:

To determine the molecular formula of the compound, we need to start by finding the empirical formula. Given that the compound is 13.068% C and 86.932% Br, we can assume 100 g of the compound and convert the percentage of each element into grams. Next, we determine the number of moles of carbon and bromine in the 100-g sample of the compound. Dividing by the smallest number of moles relates the number of moles of carbon to the number of moles of bromine. The smallest whole number ratio gives us the empirical formula, which is CBr6.

The geometry around each carbon atom can be determined based on the number of regions of electron density. In this case, each carbon atom is bonded to six bromine atoms, so the geometry is octahedral.

Since the compound contains polar covalent bonds, it is a polar compound.

Answer 2

The compound is found to be 13.068% C and 86.932% Br so the molecular formula is CBr. The geometry around the carbon atom is just linear. And the compound formed is polar due to the electronegativity of the bromine atom attached to the carbon atom.