Answer:
268 nm
Explanation:
First' let's calculate the average bond energy:
(276 + 615)/2 = 445.5 kJ/mol
By Avogadro's number 1 mol = 6.02x10²³ molecule, then the energy necessary to break the amide bond in 1 molecule is:
E = 445.5/6.02x10²³ = 7.4x10⁻²² kJ = 7.4x10⁻¹⁹ J
So, the wavelength of light (λ) can be calculated by:
E= h*c/λ
Where h is the Planck's constant (6.626x10⁻³⁴ J.s), and c is the light speed (3.0x10⁸ m/s).
7.4x10⁻¹⁹ = 6.626x10⁻³⁴ * 3.0x10⁸/λ
λ = 2.68x10⁻⁷ m
λ = 268 nm
<span>Xenon has 8 valence electrons, each hydrogen atom has 1, therefore you have 8+4=12 valence electrons. 8 electrons are used to make 4 bonds between the Xe atom and the 4 hydrogen atoms. That leaves 12-8=4 left over electrons, which will occur in two lone pairs of electrons on the center xenon atom. There are 4 bonding pairs and two lone pairs of electrons and they will be arranged in an octahedral arrangement around the center atom, with the lone pairs across the molecule (180 degrees from each other). The resulting molecular structure will be square planar.</span><span>
8+4=12 valence electrons. 8 electrons are used to make 4 bonds between the Xe atom and the 4 hydrogen atoms. That leaves 12-8=4 left over electrons, which will occur in two lone pairs of electrons on the center xenon atom. There are 4 bonding pairs and two lone pairs of electrons and they will be arranged in an octahedral arrangement around the center atom, with the lone pairs across the molecule . The resulting structure is square planar.</span>
Your answer is d hope I helped
