Table of Contents
- 1 How is SO2 stable?
- 2 Why is SO2 unstable?
- 3 How stable is SO3?
- 4 Which is more stable CO2 or SO2?
- 5 Why does sulfur form sulfur dioxide?
- 6 Under which conditions is SO3 most stable?
- 7 Which is more acidic SO3 or P2O5?
- 8 What is the difference between SO2 and SO3?
- 9 Why is (£CE{SO3}$) stable?
- 10 Is SO3 a strong or weak acid?
How is SO2 stable?
Since sulfur has access to its 3d-orbitals, it’s perfectly capable of expanding its octet to accomodate 10 electrons instead of 8. So, in theory, this structure would be more stable than the previous two based on the fact that it has more covalent bonds and no formal charges an any of the atoms.
Why is SO2 unstable?
Sulfur dioxide is a colorless gas with a pungent odor. It is a liquid when under pressure, and it dissolves in water very easily. Sulfur dioxide in the air comes mainly from activities such as the burning of coal and oil at power plants or from copper smelting.
Is SO3 unstable?
Statement 2: SO3 is very unstable and resonates between these possible structures.
How stable is SO3?
As to why SO3 is stable… Sulfur forms an expanded octet. That means that it doesn’t really obey the octet rule, allowing it to take on extra electrons. Sulfur is a 3rd-period element; hence it can use its 3d orbitals to make more than 4 bonds.
Which is more stable CO2 or SO2?
The CO2:SO2 heterodimer exists in two stable structures, both bound by about 2 kcal/mol. Due to the stronger interaction between pairs of SO2 as compared to CO2 molecules, the (SO2)2:CO2 trimers are more strongly bound than (CO2)2:SO2.
Is SO2 or SO3 more acidic?
SO3 is much more acidic than SO2 is illustrated by the much greater ionization constants (smaller pKa’s) and the fact that it reacts with it self to form a cyclic trimer, which can be crystallized.
Why does sulfur form sulfur dioxide?
Combustion routes Sulfur dioxide is the product of the burning of sulfur or of burning materials that contain sulfur: S + O2 → SO2, ΔH = −297 kJ/mol. To aid combustion, liquified sulfur (140–150 °C, 284-302 °F) is sprayed through an atomizing nozzle to generate fine drops of sulfur with a large surface area.
Under which conditions is SO3 most stable?
Sulfur trioxide is a colourless compound that exists at room temperature either as a volatile liquid or in any of three allotropic solid forms. The liquid boils at 44.6° C (112° F) and solidifies at 16.83° C (62° F); the most stable of the solid forms melts at 62° C (144° F).
Which out of CO2 SO2 CH4 H2 shows maximum adsorption and why?
(a) CO2 (b) S02 (c) CH4 (d) H2. Answer: (d) Lesser the value of critical temperature of gases lesser will be the extent of adsorption. Hence, hydrogen gas shows least adsorption on a definite amount of charcoal.
Which is more acidic SO3 or P2O5?
Higher the oxidation state of centeral atom, more is the acidic strength of that compound. thus P2O5 has higher oxidation state than P2O3, so P205 is more acidic than P2O3.
What is the difference between SO2 and SO3?
SO3 Because it has a higher oxidative state than SO 2. SO2 is formed naturally by volcanic activity. It can also be formed by the combustion of coal or petroleum or other minerals containing sulfur, along with smelting metals and other industrial processes.
Why is sulphur trioxide more stable than sulphur dioxide?
The formation of sulphur trioxide from sulphur dioxide is exothermic and spontaneous at room temperature and pressure. That makes sulphur trioxide more stable in the standard definition of the word stability. Please note that sulphur trioxide is more reactive than sulphur dioxide, violently forming sulphuric acid on reaction with water.
Why is (£CE{SO3}$) stable?
As to why $\\ce{SO3}$ is stable… Sulfur forms an expanded octet. That means that it doesn’t really obey the octet rule, allowing it to take on extra electrons. Sulfur is a 3rd-period element; hence it can use its 3d orbitals to make more than 4 bonds. Wikipedia has a page on hypervalency, and from an answer here:
Is SO3 a strong or weak acid?
Strong acids are those that completely ionize in a solvent solution. Strong acids are the following: But those acids are bronsted acids, so they easily donate protons. Now SO3 acts as a strong Lewis acid, so it will readily accept an electron pair.