The standard state of phosphorus at 25∘C is P4. This molecule has four equivalent P atoms, no double or triple bonds, and no exp
anded octets. Draw its Lewis structure. Draw the molecule by placing atoms on the grid and connecting them with bonds. Include all non-bonding electrons.
1 answer:
Explanation:
<em>Lewis-dot structure</em> : It shows the bonding between the atoms of a molecule and it also shows the unpaired electrons present in the molecule.
In the Lewis-dot structure the valance electrons are shown by 'dot'.
Phosphorus in its standard from exist as molecule.the
hybridized phosphorus atom lies in the corner of the regular tetrahedron. Each phosphorus atom is connected to three other phosphorus atoms.
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Answer:
2.83 g
Explanation:
At constant temperature and pressure, Using Avogadro's law
Given ,
V₁ = 2.12 L
V₂ = 3.12 L
n₁ = 0.120 moles
n₂ = ?
Using above equation as:
n₂ = 0.17660 moles
Molar mass of methane gas = 16.05 g/mol
So, Mass = Moles*Molar mass = 0.17660 * 16.05 g = 2.83 g
<u>2.83 g are in the piston.</u>
Answer:
The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.
Explanation:
It takes 839 kJ/mol to break a carbon-carbon triple bond.
Energy required to break 1 mole of carbon-carbon triple bond = E = 839 kJ
E = 839 kJ/mol = 839,000 J/mol
Energy required to break 1 carbon-carbon triple bond = E'
The energy require to single carbon-carbon triple bond will corresponds to wavelength which is required to break the bond.
(Using planks equation)
The maximum wavelength of light for which a carbon-carbon triple bond could be broken by absorbing a single photon is 143 nm.