Passage
Sulfur is the 10th most abundant element on Earth and is an essential element in biological systems. Sulfur can form a variety of chemical compounds and will react with nearly every element except Au, Pt, Ir, Te, and the noble gases. A list of several common inorganic compounds of sulfur is given in Table 1.Table 1 Selected Common Inorganic Sulfur Compounds
Reduction of elemental sulfur by bacteria during anaerobic digestion produces the toxic, foul-smelling gas H₂S. Oxidation of elemental sulfur via combustion or volcanic processes yields gases of SO₂ and SO₃. When dissolved in water, both SO₂ and SO₃ produce acidic solutions, and SO₃ reacts with water to form the acid H₂SO₄. Neutralization of H₂SO₄ can provide a variety of salts, including Na₂SO₄.Elemental sulfur can also react with halogen gases to form sulfur halides such as the industrially important insulator gas SF₆ and the synthetic reagent S₂Cl₂. S₂Cl₂ facilitates the formation of other sulfur compounds. For example, reacting S₂Cl₂ with NH₃ produces the sulfur pnictide S₄N₄.
-What is the molecular geometry of hydrogen sulfide?

Question

Passage
Sulfur is the 10th most abundant element on Earth and is an essential element in biological systems. Sulfur can form a variety of chemical compounds and will react with nearly every element except Au, Pt, Ir, Te, and the noble gases. A list of several common inorganic compounds of sulfur is given in Table 1.Table 1 Selected Common Inorganic Sulfur Compounds

Reduction of elemental sulfur by bacteria during anaerobic digestion produces the toxic, foul-smelling gas H₂S. Oxidation of elemental sulfur via combustion or volcanic processes yields gases of SO₂ and SO₃. When dissolved in water, both SO₂ and SO₃ produce acidic solutions, and SO₃ reacts with water to form the acid H₂SO₄. Neutralization of H₂SO₄ can provide a variety of salts, including Na₂SO₄.Elemental sulfur can also react with halogen gases to form sulfur halides such as the industrially important insulator gas SF₆ and the synthetic reagent S₂Cl₂. S₂Cl₂ facilitates the formation of other sulfur compounds. For example, reacting S₂Cl₂ with NH₃ produces the sulfur pnictide S₄N₄.
-What is the molecular geometry of hydrogen sulfide?

Quizplus · Accepted Answer

11ecba2d_1233_4fed_a3bf_4301ae4b51b9_MD0008_00 Hybridization is the process by which two or more atomic orbitals (s, p, d, f) combine to form new hybrid orbitals that have different shapes and spatial orientations than the atomic orbitals that produce them. Conservation of orbitals dictates that the number of hybrid orbitals formed must equal the number of atomic orbitals that hybridize. For example, in sp³ hybridization, 4 atomic orbitals hybridize, so 4 hybrid orbitals are formed. When hybrid orbitals are formed, the orbitals will adopt a spatial orientation that maximizes separation between the orbitals to minimize the repulsion between the electron-dense regions. This action forms an electron geometry for the electron-dense regions that acts as a frame on which bonding may occur. However, the specific molecular geometry (shape) of a compound depends on the number and orientation of the bonds around the central atom. As a result, two compounds with the same electron geometry may have different molecular geometries depending on the number of pairs of nonbonding electrons present in each. The Lewis structure of hydrogen sulfide (H₂S) shows that the central sulfur atom has two pairs of nonbonding electrons and two bonds (a total of four electron-dense areas). The four electron-dense areas of the S atoms give H₂S a tetrahedral electron geometry, but because two of the four electron-dense regions are nonbonding electrons, the molecular geometry (the shape made by the bonded atoms) is bent. (Choice B) A trigonal planar molecular geometry results from a trigonal planar electron geometry without any nonbonding electrons. H₂S has a tetrahedral electron geometry. (Choice C) A tetrahedral molecular geometry results from a tetrahedral electron geometry that lacks any nonbonding electrons. H₂S has two pairs of nonbonding electrons. (Choice D) A trigonal pyramidal molecular geometry results from a tetrahedral electron geometry with only one pair of nonbonding electrons. Educational objective: Atomic orbitals can combine into hybrid orbitals, which adopt an electron geometry that maximizes the separation and minimizes the repulsion between the electron-dense orbital regions. The molecular geometry (shape) of a molecule depends on the electron geometry and number of nonbonding electron pairs of the central atom.

Passage Sulfur Is the 10th Most Abundant Element on Earth and and Is