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