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Why bond angle of H2S is less than H2O?
The bond angle in H2S (92 degrees) is less than in H2O (104.5 degrees) due to the larger size of sulfur compared to oxygen. The larger size of sulfur results in weaker repulsions between the electron pairs, causing the bond angle to be smaller in H2S compared to H2O.
What is Hydrogen sulfide shape is similar to?
Hydrogen sulfide (H2S) has a bent shape similar to water (H2O) due to its two lone pairs of electrons on the sulfur atom. This results in a bond angle of around 92 degrees in H2S, similar to the bond angle in water of approximately 104 degrees.
Why H2S is bent?
H2S is bent because it has a bent molecular geometry due to the lone pairs of electrons on the sulfur atom causing repulsion and pushing the hydrogen atoms closer together. This results in a bond angle of approximately 92 degrees.
Is H2S an ionic bond?
No, H2S (hydrogen sulfide) does not form an ionic bond. It forms a covalent bond where electrons are shared between the hydrogen and sulfur atoms.
Does H2S contain a covalent bond?
Yes, hydrogen sulfide (H2S) contains a covalent bond. In H2S, the hydrogen and sulfur atoms share electrons to form a covalent bond, where they are held together by the sharing of electron pairs.
Why bond angle of H2S is less than H2O?
The bond angle in H2S (92 degrees) is less than in H2O (104.5 degrees) due to the larger size of sulfur compared to oxygen. The larger size of sulfur results in weaker repulsions between the electron pairs, causing the bond angle to be smaller in H2S compared to H2O.
What is Hydrogen sulfide shape is similar to?
Hydrogen sulfide (H2S) has a bent shape similar to water (H2O) due to its two lone pairs of electrons on the sulfur atom. This results in a bond angle of around 92 degrees in H2S, similar to the bond angle in water of approximately 104 degrees.
H2S molecular geometry?
The molecular geometry of H2S is bent, with a bond angle of approximately 92 degrees. This is because of the presence of two lone pairs on the sulfur atom, which push the hydrogen atoms closer together and give the molecule a bent shape.
Why H2S is bent?
H2S is bent because it has a bent molecular geometry due to the lone pairs of electrons on the sulfur atom causing repulsion and pushing the hydrogen atoms closer together. This results in a bond angle of approximately 92 degrees.
Can h2s hydrogen bond?
H2S cannot form Hydrogen bonds.Electro negativity is not enough.
Is H2S an ionic bond?
No, H2S (hydrogen sulfide) does not form an ionic bond. It forms a covalent bond where electrons are shared between the hydrogen and sulfur atoms.
Why is hydrogen sulfide a covalent bond?
h2s
Does H2S contain a covalent bond?
Yes, hydrogen sulfide (H2S) contains a covalent bond. In H2S, the hydrogen and sulfur atoms share electrons to form a covalent bond, where they are held together by the sharing of electron pairs.
Is H2S a covalent bond?
NO!!! It is a compound of hydrogen and sulphur. The bonds between hydrogen and sulphur are covalent. H2S ( hydrogen sulphide) is the sulphur analogue of water. H2S is the bad eggs smell that is given off from rotten eggs.
What is the electron domain for H2S?
The electron domain geometry for H2S is bent or angular, with two electron domains around the sulfur atom. This results in a bond angle of approximately 92 degrees due to the presence of two bonding pairs and two lone pairs of electrons around the sulfur atom.
Why the bond angle of hydrogen sulphide is 92 degrees?
I assume you have come across VSEPR theory. The central sulphur atom has 4 pairs of electrons around it (two pairs in the covalent bonds between S and H and two lone pairs that are sometimes drawn as rabbits ears!) If these four pairs repelled each other equally would form a tetrahedral angle of about 1090 ,this is the angle found in methane wheer the four pairs are identical and repel one another equally. In H2S the two lone pairs repel more strongly and this pushes the hydrogen atoms closer together reducing the bond angle to 920
What is the kind of hydrogen sulphide bonds?
H2S has covalent bond between H and S.
