(c) Draw the set of five 3d orbitals. Label each orbital and include the set of Cartesian (x, y, z) axes to show the orientation of the orbital. Clearly show the orbital phases.
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- (a) Find the angle u between adjacent nearest-neighbor bonds in the silicon lattice. Recall that each silicon atom is bonded to four of its nearest neighbors.The four neighbors form a regular tetrahedron— a pyramid whose sides and base are equilateral triangles. (b) Find the bond length, given that the atoms at the corners of the tetrahedron are 388 pm apart.3. The number of Bravais lattices are. (a) 7. (b) 14 (c) 104.) Carbon and graphite are allotropes of Carbon. Between graphite and diamond, which one is a good conductor of electricity and which one is not? Support answer with an explanation. (Limit answer to not more than 4 sentences)
- Antibonding molecular orbitals can be used to make bonds to other atoms in a molecule. For example, metal atoms can use appropriate d orbitals to overlap with the T, orbitals of the carbon monoxide molecule. This is called d – T backbonding. (a) Draw a coordinate axis system in which the y -axis is vertical in the plane of the paper and the x -axis horizontal. Write ªM" at the origin to denote a metal atom. (b) Now, on the x -axis to the right of M, draw the Lewis structure of a CO molecule, with the carbon nearest the M. The CO bond axis should be on the x -axis. (c) Draw the CO T, orbital, with phases (see the "Closer Look" box on phases) in the plane of the paper. Two lobes should be pointing toward M. (d) Now draw the dy orbital of M, with phases. Can you see how they will overlap with the T, orbital of CO? (e) What kind of bond is being made with the orbitals between Mand C, o or n?(f) Predict what will happen to the strength of the CO bond in a metal-CO complex compared to CO…Sketch the shape and orientation of the following types oforbitals: (a) s, (b) Pz?7.63 What physical concept forms the premise of VSEPR theory?
- The following figures represent the binary hydrides of the elements of the second period of the p block. A) Identify the different hydrogen atom in each case and write the molecular formula of each hydride. Explain your answer. B) Perform step-by-step hybridization for each one.N2 and CN' are both isoelectronic. (i) Draw the molecular orbital diagram for N2 and CN molecules. (ii) Explain why CN is a toxic substance but N2 isn't. (iii) N2(g) is an inert gas that is suitable for a wide range of application. Would you expect N2" to be a stable diatomic species in the gaseous state? Explain your answer.10. Which of the following does have the lowest polarizability? Z of I = 53, F = 9, Br = 35, I = 53a.Cl-b.I-c.F-d.Br-
- The molecule shown here is difluoromethane (CH2F2), which isused as a refrigerant called R-32. (a) Based on the structure, howmany electron domains surround the C atom in this molecule?(b) Would the molecule have a nonzero dipole moment? (c) Ifthe molecule is polar, which of the following describes the directionof the overall dipole moment vector in the molecule:(i) from the carbon atom toward a fluorine atom, (ii) from thecarbon atom to a point midway between the fluorine atoms,(iii) from the carbon atom to a point midway between the hydrogenatoms, or (iv) from the carbon atom toward a hydrogenatom?Consider the molecule PF4Cl. (a) Draw a Lewis structure forthe molecule, and predict its electron-domain geometry.(b) Which would you expect to take up more space, a P¬Fbond or a P¬Cl bond? Explain. (c) Predict the molecular geometryof PF4Cl. How did your answer for part (b) influenceyour answer here in part (c)? (d) Would you expect the moleculeto distort from its ideal electron-domain geometry? Ifso, how would it distort?QUESTION 5 (31 MARKS) (a) (i) Draw a pz orbital and a d?-y? orbital. (4) (ii) What are the differences between a 5pz orbital and a 4d-y² orbital in the H atom? (6) (b) (i) Draw the Lewis structure of methanol, CH3OH(8). (3) (ii) Show with a simple diagram how methanol dissolves in water. Explain. (2) (c) How does the energy and length of the carbon-oxygen bond in CH3OH(t) compare with the carbon-oxygen distance in carbon monoxide? Explain. (5) (d) Chemical bonds can be classified as polar covalent, according to and (3) (e) Chemical bonds can also be classified as single or number of according to the (2) (f) Draw the Lewis structure(s) for SO3F¯. Explain the structure which you have drawn. (6)