Excess florine, F2(g) reacts at 150 degrees celius with bromine, Br2(g) to give the compound BrF(n). If 423 mL of Br2 at 150 Degrees and 748mmHg produced $.20 g BrF(n), what is it? describe the bonding in the molecule, using valence bond theory.
To find out what compound BrF(n) is, we need to calculate the number of moles of BrF(n) produced in the reaction.
First, let's use the Ideal Gas Law to find the number of moles of Br2(g) used in the reaction at 150 degrees Celsius and 748 mmHg pressure. The Ideal Gas Law equation is:
PV = nRT,
where P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature in Kelvin.
First, we need to convert the volume from mL to L:
423 mL = 423/1000 = 0.423 L
Next, we need to convert the pressure from mmHg to atm:
748 mmHg = 748/760 = 0.9838 atm
The ideal gas constant R is 0.0821 L·atm/(mol·K).
Now we can rearrange the Ideal Gas Law equation to solve for the number of moles (n):
n = PV / RT
Substituting the values into the equation:
n = (0.9838 atm) * (0.423 L) / [(0.0821 L·atm/(mol·K)) * (150 + 273 K)]
n ≈ 0.01084 mol
Now we know that 0.01084 mol of Br2 reacted to produce 0.20 g of BrF(n).
To find the molar mass of BrF(n), we need to know the mass of one mole of the compound. Since the mass given is for 0.20 g, we can divide it by the number of moles to find the molar mass:
molar mass = mass / moles
molar mass = 0.20 g / 0.01084 mol
molar mass ≈ 18.42 g/mol
The molar mass of BrF(n) is approximately 18.42 g/mol.
Now let's move on to describing the bonding in the molecule BrF(n) using valence bond theory.
In BrF(n), Bromine (Br) and Fluorine (F) atoms are bonded together. According to valence bond theory, the bond between them is formed by the overlapping of half-filled atomic orbitals of each atom, resulting in the formation of molecular orbitals.
Both Bromine and Fluorine have one unpaired electron in their outermost shell. During the reaction, these unpaired electrons in the atomic orbitals participate in overlapping. The interaction between the unpaired electrons leads to the formation of a covalent bond between Br and F.
The molecular orbital formed due to this overlap is a sigma bond (σ bond), which is a strong and stable bond. It is formed by the end-to-end overlap of the atomic orbitals along the internuclear axis.
Overall, in BrF(n), the bonding is achieved through the formation of sigma bonds between Bromine and Fluorine atoms, resulting in a stable and covalent molecule.