Unit 1 key terms

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Across
  1. 3. When a polar molecule causes a skew in the electron cloud of a non-polar molecule it is called an ________________ dipole and will create Debye forces.
  2. 4. The saying “like dissolves like” will help to determine the _______________________ of one substance in another.
  3. 9. Regions around a central atom where electrons are found.
  4. 10. Used to see if the most stable Lewis Structure has been drawn.(two words)
  5. 13. The alternating arrangement of ions in an ionic compound.
  6. 18. When solids have strong forces of attraction between the particles, the _____________________ point of the substance tends to be high.
  7. 20. The shape of molecules is determined by ______________________ between the bonding and non-bonding domains
  8. 22. A shortened version of a full electron configuration
  9. 23. A charge separation across a bond or molecule.
  10. 24. Electrical conductivity is only possible when there are ___________________ particles that can move freely.
  11. 25. A packet of energy.
  12. 26. A giant covalent compound with a very high melting point because it has no intermolecular forces
  13. 28. This type of spectrum includes colored lines on a black background.
  14. 29. London dispersion forces are created when a ________________________ dipole forms in one atom or molecule and attracts to a neighboring atom or molecule.
  15. 31. In order to have dipole-dipole attractions and hydrogen bonding, a molecule must be ____________
  16. 33. a metal will be ___________________ when it has unpaired electrons in its orbitals
  17. 36. An indication of how hard an atom pulls on shared electrons in a compound.
  18. 37. 120॰ 109.5॰ or 90॰ (two words)
Down
  1. 1. Copper and Chromium have electron configurations that are _____________________ to the rule.
  2. 2. The longer they are, the less energy they have.
  3. 5. The shape of an AX2E2 molecule
  4. 6. This principle says that electrons must fill lower energy orbitals before filling higher energy orbitals
  5. 7. A three-dimensional space where we can find electrons.
  6. 8. A way of explaining observations that changes as new evidence becomes available
  7. 9. When one atom provides both electrons for a covalent bond it forms this type of bond.
  8. 11. When a double bond can be in various positions in a Lewis structure.
  9. 12. The outermost electrons that can participate in bonding.
  10. 14. Forces of attraction between neighbouring molecules.
  11. 15. when an electron changes from one energy level to another
  12. 16. Beryllium and Boron will typically form molecules with an _____________________ octet.
  13. 17. Provides an indication of the strength of a covalent bond. Can be a whole number or fractional (two words)
  14. 19. Sulfur and Phosphorus will typically form molecules with an _____________________ octet.
  15. 21. The process of blending orbitals to create new ones with intermediate properties
  16. 27. An electron in its lowest energy state is said to be in this state.
  17. 30. the type of bond formed by the side to side overlap of orbitals
  18. 32. Layers of sp2 hybridized carbon atoms held together by weak intermolecular forces.
  19. 34. When an electron is not stuck in one position.
  20. 35. The type of bond formed by the end-to-end overlap of orbitals