Lab Aids Chemistry Semester 2 Final Exam

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Across
  1. 8. The smallest possible quantity (or quanta) of light. Light exists in discrete bundles of energy called photons.
  2. 11. The distance (separation) between any two successive peaks (or valleys) of a wave.
  3. 12. Any 1 of the 7 horizontal rows of the periodic table.
  4. 16. Principle that states that 2 electrons in the same atom may NEVER be in the same quantum state.
  5. 19. The exact number and type of atoms in a molecule (covalent).
  6. 20. A process by which the nucleus of an atom spontaneously changes itself by emitting particles or energy, a property of some element to break up and release energy.
  7. 22. A diagram showing 1 dot for each valence electron an atom has. The dots surround the element symbol for the atom.
  8. 25. Family of moderately reactive metals located in Group 2A of the periodic table.
  9. 27. A family of virtually inert (unreative) gases located in group 18A(8)of the periodic table.
  10. 28. Repeating at regular intervals. The periodic table is named for this because the rows are organized by repeating patterns found in both atomic structure and the properties of the elements.
  11. 29. Rule that states that the atoms of most elements (except H through B)strive to have a total of 8 electrons in their outermost orbital (by sharing, gaining, or losing electrons.)
  12. 30. The number of protons plus neutrons in the nucleus.
  13. 31. A shape formed when a central atom has 2 unshared pairs of electrons and is bonded to 2 other atoms; water has this shape.
  14. 33. The attractive forces that occur between the + part of one polar molecule and the - part of another polar molecule; found between all polar molecules.
  15. 38. A shape (molecular geometry) formed when a central atom has 2 regions of electron density and zero lone pairs; 180 degree bond angle.
  16. 39. A value between 0 and 4 that describes the relative “pull” of an element for electrons from other atoms. High numbers mean stronger attraction for electrons; the ability for an atom to attract another atom’s electrons when bonded to that other atom; tends to increase from left to right and up to fluorine.
  17. 41. A group of quantum states that have similar spatial shapes. The orbitals are labeled s, p, d, and f.
  18. 42. The tiny core of an atom that contains all the protons and neutrons. It is extraordinarily small- about 1/10,000 the diameter of the atom.
  19. 43. A description of which orbitals contain electrons for a particular atom.
Down
  1. 1. A shape formed when a central atom is bonded to 4 other atoms.
  2. 2. The distance from the center of an atom to its “outer edge;” on the periodic table this property tends to increase as you go down a group and decrease from left to right across a period.
  3. 3. Electrons in the highest/outermost unfilled energy level. These are the electrons involved in making chemical bonds.
  4. 4. A trigonal shape (molecular geometry) formed when a central atom has 3 bonded pairs and 1 lone pair of electrons.
  5. 5. A small molecule (with 2 or more atoms) with an overall positive or negative charge (usually).
  6. 6. A type of covalent bond formed between two nonmetal atoms in which the electrons are shared equally or almost equally between the 2 atoms.
  7. 7. A theory that states the shapes of molecules are dictated, in part, by the repulsion of the shared electrons and the unshared (lone) pairs of electrons.
  8. 9. A large family of less reactive metals located in Groups 3-12 of the periodic table; many known for their ability to lose different numbers of electrons.
  9. 10. Family of extremely reactive metals located in Group 1A of the periodic table.
  10. 12. A type of covalent bond formed between two nonmetal atoms in which the electrons ARE NOT shared equally.
  11. 13. The energy required to completely remove an electron; increases from left to right and up to helium.
  12. 14. the "dispersion" attractive forces that occurs between nonpolar molecules due to temporary, slight polarizations that occur when the normally equal distributions of electrons is shifted.
  13. 15. A representation that analyzes a sample of light into its component energies or colors, can be a picture, graph, table of data.
  14. 17. Atoms or elements that have the same number of protons in the nucleus, but different numbers of neutrons.
  15. 18. A type of chemical bond that often involves a metal, which loses 1 or more electrons to a more electronegative nonmetal.
  16. 21. The family consisting of the most reactive nonmetals of the periodic table located in group 17A (7).
  17. 23. the set of quantum states that have approximately the same energy.
  18. 24. when a chemical formula could represent > 1 molecule, the same number/type of atoms bonded into different ways.
  19. 26. Any 1 of the 8(18) vertical columns of the periodic table.
  20. 32. An atom or small molecule with an overall + or - charge due to an imbalance of protons and electrons.
  21. 34. A trigonal shape (molecular geometry) formed when a central atom has 3 bonded pairs and 0 lone pair of electrons.
  22. 35. The attractions that occur between molecules.
  23. 36. (Z) The number of protons in the nucleus, unique to each element.
  24. 37. A theory of chemistry and physics that accurately describes the universe on very small scales, such as the inside of an atom.
  25. 40. Formula with the simplest ratio of atoms in a substance.