Question
Part 11 Answer the following questions 16 Write Lewis dot symbols for the following atoms and ions :mg , Na, B , N, Br Be, Li^+,Cl^-,O^2-,Mg^2+ and N^3- 17. List four major difference between sigma (sigma ) and pi (pi ) bonds. 18 . Which one is stronger:o-bond or To -bond?? Why? 19 Explain why a BeH_(2) molecule has a zero dipole moment although the Be -H bonds are polar? 20 . How can one non-polar molecule induce a dipole in a nearby non -polar molecule? 21 . Describe the change in hybridization of an aluminum atom lif any)during the reaction: AlCl_(3)+Cl^-arrow AlCl_(4)^- 22 . Apart from tetrahedral geometry,another possible geometry for CH_(4) is square planar with the four H atoms at the corners of the square and C atom at its center. Explain why CH_(4) is not square planar? 23 . Sketch the bond moments and resultant dipole moments in the following molecules: H_(2)O,PCl_(3),NH_(3),NF_(3) 24.Write the resonance structures for SO_(2),NO_(2) and NO_(3)^-.S
Solution
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(230 Votos)
Ximena
Elite · Tutor por 8 anos
Resposta
16. Lewis dot symbols for the given atoms and ions:- Mg: [Mg] with no dots around it.- Na: [Na] with one dot around it.- B: [B] with three dots around it.- N: [N] with five dots around it.- Br: [Br] with seven dots around it.- Be: [Be] with two dots around it.- Li⁺: [Li] with no dots around it.- Cl⁻: [Cl] with eight dots around it.- O²⁻: [O] with eight dots around it.- Mg²⁺: [Mg] with no dots around it.- N³⁻: [N] with eight dots around it.17. Four major differences between sigma (σ) and pi (π) bonds:- Sigma bonds are single covalent bonds, while pi bonds are double or triple covalent bonds.- Sigma bonds are formed by the head-to-head overlap of atomic orbitals, while pi bonds are formed by the side-to-side overlap of atomic orbitals.- Sigma bonds are stronger and shorter than pi bonds.- Sigma bonds allow rotation, while pi bonds do not.18. The sigma (σ) bond is stronger than the pi (π) bond. This is because sigma bonds involve the direct overlap of atomic orbitals, resulting in a stronger bond. Pi bonds, on the other hand, involve the side-to-side overlap of atomic orbitals, which is less effective in creating a strong bond.19. The BeH₂ molecule has a zero dipole moment despite the polar Be-H bonds because the molecule is linear. The two polar Be-H bonds are symmetrically arranged around the Be atom, causing their dipole moments to cancel each other out.20. A non-polar molecule can induce a dipole in a nearby non-polar molecule through temporary fluctuations in electron density, known as London dispersion forces. These temporary dipoles can cause a temporary imbalance in electron distribution in the nearby non-polar molecule, inducing a dipole moment.21. In the reaction AlCl₃ + Cl⁻ → AlCl₄⁻, the aluminum atom undergoes a change in hybridization from sp² to sp³. This is because the addition of the chloride ion (Cl⁻) to the aluminum atom results in the formation of a tetrahedral geometry, requiring the use of sp³ hybrid orbitals.22. CH₄ is not square planar because the carbon atom forms four equivalent sigma bonds with the hydrogen atoms, resulting in a tetrahedral geometry. In a square planar geometry, the bond angles would be 90 degrees, which is not the case in CH₄.23. Bond moments and resultant dipole moments in the given molecules:- H₂O: The oxygen atom is more electronegative than the hydrogen atoms, resulting in a dipole moment pointing towards the oxygen atom.- PCl₃: The chlorine atoms are more electronegative than the phosphorus atom, resulting in dipole moments pointing towards the chlorine atoms.- NH₃: The nitrogen atom is more electronegative than the hydrogen atoms, resulting in a dipole moment pointing towards the nitrogen atom.- NF₃: The nitrogen atom is more electronegative than the fluorine atoms, resulting in a dipole moment pointing towards the nitrogen atom.24. Resonance structures for SO₂, NO₂, and NO₃⁻:- SO₂: Structure 1: S=O-O Structure 2: S-O=O- NO₂: Structure 1: O=N-O Structure 2: O-N=O- NO₃⁻: Structure 1: O-N=O Structure 2: O-N⁺-O⁻ Structure 3: O-N⁺-O⁻