Bond dissociation energy is inversely proportional to Bond length.
The longer the bond is, lesser the energy it requires to break the bond.
Therefore, it is easier to break single bond.
Single bond>double bond>triple bond -------(Bond length)
Answer:
2.65 atm.
Explanation:
- We can use the general law of ideal gas: <em>PV = nRT.</em>
where, P is the pressure of the gas in atm.
V is the volume of the gas in L.
n is the no. of moles of the gas in mol.
R is the general gas constant,
T is the temperature of the gas in K.
- If n and V are constant, and have different values of P and T:
<em>(P₁T₂) = (P₂T₁).</em>
P₁ = 3.0 atm, T₁ = 30°C + 273 = 303 K,
P₂ = ??? atm, T₂ = -5°C + 273 = 268 K.
∴ P₂ = (P₁T₂)/(T₁) = (3.0 atm)(268 K)/(303 K) = 2.65 atm.
Answer:
Correct answer is (C) Silicon has the ability to form a partial double bond with a halogen through the overlap of its d-orbital with a p-orbital of the halogen
You question did not complete as the options are missing. See the options below;
A) The larger silicon atoms permit better overlap of its atomic orbitals with those of the halogens than the smaller carbons atoms do.
B) The large electronegativity difference between silicon and the halogens makes their bonds stronger than those of carbon.
C) Silicon has the ability to form a partial double bond with a halogen through the overlap of its d-orbital with a p-orbital of the halogen.
D) Silicon has a larger effective nuclear charge than carbon which allows it to bond more strongly to the more negative halogens than carbon.
E) Carbon-halogen bonds are unusually weak
Explanation:
Silicon reacts vigorously with halogens to form siliconhalides. The d subshell has 5 orbitals and halogen carries seven valence electronics with 5 in its p-orbital. When they react, they form stronger bonding than carbonhalide
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