Write three dimensional structure of CHCINH2 (C is the central atom; the hydrogen atom and the fluorine atom are in the plane, Cl is out of the plane and NH is behind the plane)
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- 7.84 Which of the following molecules is least likely to actually exist OF4,SF4,SeF4 , or TeF4 ? Why?Consider the element silicon, Si. (a) Write its electron configuration.(b) How many valence electrons does a siliconatom have? (c) Which subshells hold the valenceelectrons?Mixing SbCl3 and GaCl3 in a 1;1 molar ratio (usingliquid sulfur dioxide as a solvent) gives a solid ioniccompound of empirical formula GaSbCl6. A controversyarises over whether this compound is ( ) SbCl2 + ( ) GaCl 4 - or( ) GaCl+ 2 ( ) SbCl 4 -(a) Predict the molecular structures of the two anions.(b) It is learned that the cation in the compound has abent structure. Based on this fact, which formulationis more likely to be correct?
- Of the elements Li, K, N, P, and Ne, which (a) is the most electronegative, (b) has the greatest metallic character, (c) can bond tomore than four atoms in a molecule, and (d) forms π bonds most readily?Consider the A2X4 molecule depicted here, where A and Xare elements. The A¬A bond length in this molecule is d1,and the four A¬X bond lengths are each d2. (a) In terms ofd1 and d2, how could you define the bonding atomic radii ofatoms A and X? (b) In terms of d1 and d2, what would you predictfor the X¬X bond length of an X2 molecule?Consider the A2X4 molecule depicted here, where A and Xare elements. The A¬A bond length in this molecule is d1,and the four A¬X bond lengths are each d2. (a) In terms ofd1 and d2, how could you define the bonding atomic radii ofatoms A and X? (b) In terms of d1 and d2, what would you predictfor the X¬X bond length of an X2 molecule? [Section 7.3]
- Which member of each pair is less metallic?(a) I or O(b) Be or Ba(c) Se or GeBy using photons of specific wavelengths, chemists can dissociate gaseous HI to produce H atoms with accurately known speeds. When HI dissociates, the H atoms move away rapidly, whereas the relatively heavy I atoms move little. Use Table 9.2 in your textbook to answer the following questions: (a) What is the longest wavelength (in nm) that can dissociate a molecule of HI? 4.0 nm (b) If a photon of 227 nm is used, what is the excess energy (in J) over that needed for the dissociation? 4.0 (c) If all of this excess energy is carried away by the H atom as kinetic energy, what is its speed (in m/s)? 4.0 m/s Average Bond Energies (kJ/mol) Bond Energy Bond Energy Bond Energy Bond Energy Single Bonds H-H 432 N-H 391 Si-H 323 S-H 347 H-F 565 N-N 160 Si-Si 226 S-S 266 H-CI 427 N-P 209 Si-O 368 S-F 327 Н-Br 363 N-O 201 Si-S 226 S-CI 271 H-I 295 N-F 272 Si-F 565 S-Br 218 N-CI 200 Si-CI 381 S-I ~170 310 234 C-H 413 N-Br 243 Si-Br C-C 347 N-I 159 Si- F-F 159 C-Si 301 F-CI 193 305 0-H 467 P-H 320…For many years after they were discovered, it was believed that the noble gases could not form compounds. Now we know that belief to be incorrect. A mixture of xenon and fluorine gases, confined in a quartz bulb and placed on a windowsill, is found to slowly produce a white solid. Analysis of the compound indicates that it contains 77.55% Xe and 22.45% F by mass.(a) What is the formula of the compound?(b) Write a Lewis structure for the compound.(c) Predict the shape of the molecules of the compound.(d) What hybridization is consistent with the shape you predicted?
- Predict the best choice in each of the following. You may wish to review the chapter on electronic structure for relevant examples.(a) the most metallic of the elements Al, Be, and Ba(b) the most covalent of the compounds NaCl, CaCl2, and BeCl2(c) the lowest first ionization energy among the elements Rb, K, and Li(d) the smallest among Al, Al+, and Al3+(e) the largest among Cs+, Ba2+, and Xe(b) List some properties of Group 1 elements which indicate they are all metals. (c) What valence do all Group 1 elements exhibit in their compounds? (a) Write the names and symbols of the elements of Group 2.5. (a) Draw and name the molecular shape for SeCla molecule. [2] (b) Explain the polarity of selenium tetrachloride, SeCla. [3]
