For AsClF42-:
a) Name the hybridization of the orbitals of the central atom.
s
sp
sp2
sp3
sp4
sp3d
sp3d2
b) Estimate the Cl-As-F bond angle.
Slightly less than 90∘
Exactly 90∘
Slightly greater than 90∘
Slightly less than 109.5∘
Exactly 109.5∘
Slightly greater than 109.5∘
Slightly less than 120∘
Exactly 120∘
Slightly greater than 120∘
Slightly less than 180∘
Exactly 180∘
Slightly greater than 180∘
c) Calculate the maximum wavelength, λ, of electromagnetic radiation capable of breaking the weakest bond in AsClF2−4. Express your answer in meters (m).
Bond Bond energies (kJ/mol)
As-As 180
F-F 160
Cl-Cl 240
Sp3 d2
4e-7
a) sp3d2 b)Slightly less than 90∘
4.13346*10^-7
a) The hybridization of the orbitals of the central atom in AsClF42- is sp3d2.
b) The Cl-As-F bond angle is slightly less than 90 degrees.
c) To calculate the maximum wavelength capable of breaking the weakest bond in AsClF2−4, we need to find the bond with the lowest bond energy. In this case, it is the F-F bond with a bond energy of 160 kJ/mol.
To convert the bond energy to energy per mole of photons, we divide it by Avogadro's number (6.022 x 10^23).
160 kJ/mol ÷ (6.022 x 10^23) = 2.655 x 10^-19 J
To calculate the maximum wavelength, we use the equation λ = c/ν, where λ is the wavelength, c is the speed of light (2.998 x 10^8 m/s), and ν is the frequency.
We can find the frequency using the equation E = hν, where E is the energy (2.655 x 10^-19 J) and h is Planck's constant (6.626 x 10^-34 J·s).
ν = E/h = (2.655 x 10^-19 J) / (6.626 x 10^-34 J·s) = 4.011 x 10^14 s^-1
Finally, we can calculate the maximum wavelength:
λ = c/ν = (2.998 x 10^8 m/s) / (4.011 x 10^14 s^-1) = 7.48 x 10^-7 m or 748 nm (rounded to three significant figures).
a) To determine the hybridization of the orbitals of the central atom in AsClF42-, we need to identify the steric number (SN) of the central atom. The steric number is the sum of the number of sigma bonds and lone pair electrons around the central atom. In this case, AsClF42- has one As-F sigma bond, two As-Cl sigma bonds, and four lone pairs on As.
SN = number of sigma bonds + number of lone pairs = 1 + 4 = 5
Now, we can use the steric number to determine the hybridization:
- If SN = 2, the central atom is sp hybridized.
- If SN = 3, the central atom is sp2 hybridized.
- If SN = 4, the central atom is sp3 hybridized.
- If SN = 5, the central atom is sp3d hybridized.
- If SN = 6, the central atom is sp3d2 hybridized.
In the case of AsClF42-, the steric number is 5, which means the hybridization of the orbitals of the central atom is sp3d.
Answer: sp3d
b) The Cl-As-F bond angle in AsClF42- is related to the hybridization of the central atom. In this case, the central atom (As) is sp3d hybridized.
Based on the VSEPR theory, an sp3d hybridized central atom has a trigonal bipyramidal molecular geometry. The Cl atoms and F atoms are located in the equatorial plane of the trigonal bipyramid, while the two lone pairs are in the axial positions.
The bond angle in the equatorial plane (between the Cl-As-F bonds) is slightly less than 120°, whereas the bond angles between the axial positions and the equatorial plane (Cl-As-F angles) are slightly less than 90°.
Therefore, the estimate for the Cl-As-F bond angle in AsClF42- would be **slightly less than 90°**.
Answer: Slightly less than 90°
c) To calculate the maximum wavelength of electromagnetic radiation capable of breaking the weakest bond (As-Cl) in AsClF2-4, we need to use the bond energies provided.
The bond energy is a measure of the energy required to break a bond. Since we are looking for the weakest bond, we need to find the lowest bond energy value for the As-Cl bond, which is 240 kJ/mol.
To calculate the maximum wavelength, we can use the equation:
λ = hc / E
Where:
λ = wavelength of the electromagnetic radiation
h = Planck's constant (6.626 x 10^-34 J s)
c = speed of light (3.00 x 10^8 m/s)
E = energy required to break the bond (in joules)
First, convert the bond energy from kJ/mol to J:
240 kJ/mol * (1 J/1000 kJ) = 0.24 kJ/mol * (1000 J/1 kJ) = 240 J/mol
Next, calculate the energy required to break one mole of As-Cl bonds:
E = (240 J/mol) / (6.022 x 10^23 molecules/mol)
Finally, use the equation to find the maximum wavelength:
λ = (6.626 x 10^-34 J s) * (3.00 x 10^8 m/s) / E
Plug in the value of E to find λ:
λ = (6.626 x 10^-34 J s) * (3.00 x 10^8 m/s) / [(240 J/mol) / (6.022 x 10^23)]
Simplify the equation to find the maximum wavelength.
The resulting value will be the maximum wavelength in meters (m) of electromagnetic radiation capable of breaking the weakest As-Cl bond in AsClF2-4.
Answer: Calculate the maximum wavelength using the provided constants and bond energies.