Chapter 4 - Review Questions - Page 197: 5

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1. Tetrahedral arrangement of electron pairs: - The central atom in a tetrahedral arrangement of electron pairs requires sp3 hybridization. - In a tetrahedral arrangement, the central atom has four electron pairs, and the hybridization is sp3 to accommodate these four electron pairs. 2. Trigonal planar arrangement of electron pairs: - The central atom in a trigonal planar arrangement of electron pairs requires sp2 hybridization. - In a trigonal planar arrangement, the central atom has three electron pairs, and the hybridization is sp2 to accommodate these three electron pairs. 3. Linear arrangement of electron pairs: - The central atom in a linear arrangement of electron pairs requires sp hybridization. - In a linear arrangement, the central atom has two electron pairs, and the hybridization is sp to accommodate these two electron pairs. 4. Tetrahedral geometry: - When a central atom exhibits tetrahedral geometry, there are 0 unhybridized p atomic orbitals present. - In a tetrahedral arrangement, the four electron pairs are distributed in the sp3 hybrid orbitals, and there are no unhybridized p orbitals. 5. Trigonal planar geometry: - When a central atom exhibits trigonal planar geometry, there is 1 unhybridized p atomic orbital present. - In a trigonal planar arrangement, the three electron pairs are distributed in the sp2 hybrid orbitals, and there is one unhybridized p orbital. 6. Linear geometry: - When a central atom exhibits linear geometry, there are 2 unhybridized p atomic orbitals present. - In a linear arrangement, the two electron pairs are distributed in the sp hybrid orbitals, and there are two unhybridized p orbitals. 7. Bonding in H2S, CH4, H2CO, and HCN: - H2S (Hydrogen Sulfide): - The central sulfur atom exhibits sp3 hybridization, with two bonding pairs and two lone pairs of electrons. - The bonding is described using the localized electron model, where the two hydrogen atoms form covalent bonds with the sulfur atom. - CH4 (Methane): - The central carbon atom exhibits sp3 hybridization, with four bonding pairs of electrons. - The bonding is described using the localized electron model, where the four hydrogen atoms form covalent bonds with the carbon atom. - H2CO (Formaldehyde): - The central carbon atom exhibits sp2 hybridization, with one double bond to the oxygen atom and two single bonds to the hydrogen atoms. - The bonding is described using the localized electron model, where the carbon atom forms a double bond with the oxygen atom and two single bonds with the hydrogen atoms. - HCN (Hydrogen Cyanide): - The central carbon atom exhibits sp hybridization, with a triple bond to the nitrogen atom and a single bond to the hydrogen atom. - The bonding is described using the localized electron model, where the carbon atom forms a triple bond with the nitrogen atom and a single bond with the hydrogen atom.