Molecular structure and Polarity

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Across
  1. 1. a partial positive charge on A, turn on the electric field
  2. 3. to solve for the energy of one mole of bonds.
  3. 7. Why is the H–N–H angle in NH3 smaller than the H–C–H bond angle in CH4
  4. 9. the shape of a molecule with the formula AB3
  5. 15. A useful solvent present in paint strippers that will dissolve salts as well as organic compounds is this compound
  6. 16. the shape that describes each hybrid orbital set sp
  7. 17. one example structures with lone pairs that are exceptions to Mxn molecule rule. What is one example
  8. 18. theory assumes that electron pairs in the valence shell of a central atom will adopt an arrangement that minimizes repulsions between these electron pairs by maximizing the distance between them.
  9. 19. example of molecule that contains polar bond and dipole moment
  10. 20. why the concept of hybridization required in valence bond theory
  11. 22. why bonds occur at specific average bond distances instead of the atoms approaching each other infinitely close.
  12. 23. formed by overlapping of 2px, 2py and 2pz
  13. 25. Bond distances measurement
  14. 26. molecular structure of the stable form of FNO2? (N is the central atom.)
  15. 30. the hybridization of each type of CH₃ carbon atom.
  16. 31. the hybridization of the central atom in each of PO43−
  17. 33. predict the geometry about the CH₃ carbon atom
  18. 35. the hybridization of the central atom in each of SF6
  19. 37. geometry considers the placement of all electrons
  20. 40. the shape that describes each hybrid orbital set sp3d
  21. 42. refers only to the placement of atoms in a molecule and not the electrons, is equivalent to electron-pair geometry only when there are no lone electron pairs around the central atom
  22. 43. the molecular structure when Two of the electron regions are lone pairs
  23. 45. explains why HOH bent
  24. 46. strongest bond between covalent sigma and pi bonds
  25. 47. includes an axial and an equatorial position
  26. 48. type of bond present in this molecule in the bonding in F2, HF, and ClBr
Down
  1. 2. the shape that describes each hybrid orbital set:sp2
  2. 4. how a molecule that contains polar bonds can be nonpolar
  3. 5. has only two regions of electron density (all bonds with no lone pairs); the shape is linear
  4. 6. molecules interact with electric fields, whereas nonpolar molecules do not.
  5. 8. Why is the H–N–H angle in NH4+ identical to the H–C–H bond angle in CH4
  6. 10. Explain how σ and π bonds are similar
  7. 11. Phosporus molecule has a dipole moment.
  8. 12. to calculate the energy for one single HCl bond (Hint: How many bonds are in a mole?)
  9. 13. repulsion reduced when the various regions of high electron density assume positions as far from each other as possible
  10. 14. the electron-pair geometry and molecular structure of a polyatomic ion
  11. 21. the shape that describes each hybrid orbital set sp3d2
  12. 22. feature of a Lewis structure can be used to tell if a molecule's (or ion's) electron-pair geometry and molecular structure will be identical
  13. 24. why a carbon atom cannot form five bonds using sp3d hybrid orbitals.
  14. 27. difference between electron-pair geometry and molecular structure
  15. 28. the angle between any two bonds that include a common atom, usually measured in degrees
  16. 29. molecule must to use valence bond theory to O2
  17. 32. bonds lie in a plane with 120° angles between them and has a trigonal planar molecular structure
  18. 34. number of σ and π bonds are present in the molecule HCN
  19. 36. molecule with dipole moment
  20. 38. direction of planes of hydrogen atoms after the hybridization of each carbon atom for the molecule allene, H2C = C = CH2
  21. 39. the hybridization of the central atom in each of BeH2
  22. 41. the resulting molecular bonds take less energy to form with hybridized than with non-hybridized atomic orbitals
  23. 44. arrangement of six regions of high electron density around the xenon atom with two lone pairs and four bonds