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Which of the molecules, CO2, NH3 and BCl3 will be polar?
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- What is the hybridization of the central atom in the hypophosphite (PO3-2) ion?What is the hybridization state of the Beryllium in BeClBr? And is this a polar or nonpolar molecule?The dipole moment of gaseous Ag – Cl is ? = 6.08 D, and the bond distance is r(Ag − Cl) = 228. 1 pm. Calculate the percent ionic character for this bond in the gas phase. In solid form it is however, found the following values for the two silver halides Ag − CL and Ag − F: See image Explain why solid silver chloride is sparingly soluble in water, while solid silver fluoride is moderately soluble B) Explain why solid silver chloride is sparingly soluble in water, while solid silver fluoride is moderately soluble Given extra information: Formal charge: ?? = ??? – (??? + ???); where ??? = valence electrons in free atom, ???= free-pair electrons, ??? = number of bonds to the atom. The elementary charge: ? = 1.6022 × 10−19 C.1 Debye (?)= 3.3356 × 10−30 C × m. The dipole moment has definition: ? = ? × ?, where ? is partialcharge in Coulomb (?), ? is the bond distance (?). Picometer: 1 ?? = 1 × 10−12
- Use VSEPR theory to judge whether PCI5 is polar.What is the hybridization of the central phosphorus atom of PO43− ?Consider the SCl2 molecule. (a) What is the electron configuration of an isolated S atom? (b) What is the electron configuration of an isolated Cl atom? (c) What hybrid orbitals should be constructed on the S atom to make the S-Cl bonds in SCl2 ? (d) What valence orbitals if any, remain unhybridized on the S atom in SCL2 ?
- The ionization potential of sodium is 5.14 eV, the electron affinity of fluorine is 3.40 eV, and the equilibrium separation of sodium fluoride (NaF) is 0.193 nm. 1)The dissociation energy of NaF is 4.99 eV. What is the energy due to repulsion of the ions at the equilibrium separationWhat is the electron geometry and molecular geometry of C2H2Br2?4. (a) Draw the shape of the atomic valence orbitals formed by the overlaping of two fluoride 2p atomic orbitals. (b) Draw the molecular orbital diagrams for F2 and F2*. Identify their bond order and magnetic properties. (c) An unstable nucleus exhibit radioactivity. (i) Explain how the number of protons and neutrons in a radioactive nucleus can be used to predict its probable mode decay. (ii) Illustrate your answer in (i) with a schematic graph.