The nitrogen atoms in N2 participate in multiple bonding whereas those in hydrazine, N2H4, do not. a.) Draw Lewis structures for
both molecules. b.) What is the hybridization of the nitrogen atoms in each molecule? c.) Which molecule has a stronger N-N bond?
1 answer:
Answer:
a) Attached images.
b) N₂: sp; N₂H₄: sp³
c) N₂
Explanation:
a) In the attached images are the Lewis structures.
<em>N₂:</em> there is a triple covalent bond between the N atoms.
<em>N₂H₄:</em> there is a single covalent bond between the N atoms.
b)
<em>N₂:</em> N has 2 electron domains. The corresponding hybridization is sp. 1 sp orbital form 1 sigma bonds whereas 2 p orbitals from 2 pi bonds.
<em>N₂H₄:</em> N has 4 electron domains. The corresponding hybridization is sp³. The 3 sp³ orbitals form 3 sigma bonds.
c) The triple bond is stronger than the single bond. Then, the bond in N₂ is stronger than the bond in N₂H₄.
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Answer:
N-Cl
Explanation:
Look at the chart below. Since N-Cl bond has a electronegativity difference of (3.0-3.0) zero, they are non-polar.
Answer: The volume of 0.640 grams of gas at Standard Temperature and Pressure (STP) is 0.449 L.
Explanation:
Given: Mass of gas = 0.640 g
Pressure = 1.0 atm
Temperature = 273 K
As number of moles is the mass of substance divided by its molar mass.
So, moles of (molar mass = 32.0 g/mol) is as follows.
Now, ideal gas equation is used to calculate the volume as follows.
PV = nRT
where,
P = pressure
V = volume
n = no. of moles
R = gas constant = 0.0821 L atm/mol K
T = temperature
Substitute the values into above formula as follows.
Thus, we can conclude that the volume of 0.640 grams of gas at Standard Temperature and Pressure (STP) is 0.449 L.