Chemistry I

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  1. Alkali Metals
    H, Li, Na, K, Rb, Cs, Fr
  2. Alkali Earth Metals
    Be, Mg, Ca, Sr, Ba, Ra
  3. Halogens
    F, Cl, Br, I, At
  4. Noble Gases
    He, Ne, Ar, Kr, Xe, Rn
  5. Diatomic Molecule
    Contains two atoms.

    Ex: H2, N2, O2, HCl, CO
  6. Diatomic Elements
    H2, N2, O2, F2, Cl2, Br2, I2
  7. Common Ions
    NH4-, OH-, NO3-, ClO3-, CH2COO-, SO42-, CO32-, PO43-
  8. NH4+
  9. OH-
  10. NO3-
  11. ClO3-
  12. CH3COO-
  13. SO42-
  14. CO32-
  15. PO43-
  16. Molecular Formula
    Shows the exact number of atoms of each element in the smallest unit of a substance.
  17. Empirical Formulas
    Shows the simplest whole-number ratio of the atoms in a substance.
  18. Ionic Compounds
    Consist of metal and non-metal. Cation with Anion
  19. Molecular Compounds
    Consist of non-metals.
  20. Allotrope
    Different forms of an element in the same physical state.

    Ex: O2, O3
  21. Common single charge ions.
    1A, 2A, Ag+, Zn2+, Cd2+, Al3+
  22. Common two charge ions.
    Fe2+, Fe3+, Co2+, Co3+, Ni2+, Ni3+, Cu+, Cu2+, Hg22+, Hg2+, Sn2+, Sn4+, Pb2+, Pb4+
  23. Naming ions
    Lower charge metal ion -ous ending.

    Higher charge metal ion -ic ending.
  24. H2CO3
    Carbonic Acid
  25. HClO3
    Chloric Acid
  26. HNO3
    Nitric Acid
  27. H3PO4
    Phosphoric Acid
  28. H2SO4
    Sulfuric Acid
  29. English metric conversion
    1lb = 454g, 1in = 2.52cm, 1L = 1.06qt
  30. Fo to Co
    (F-32) x 5/9
  31. Co to Fo
    (C x 1.8) + 32
  32. Co to K
    C + 273o
  33. Matter
    Anything that takes up space and has mass.
  34. "Pure" Substance
    Form of matter that has a definite (constant) composition and distinct properties.
  35. Mixture
    Combination of two or more substances in which the substances retain their distinct identities.
  36. Compound
    A substance composed of atoms of two or more elements chemically united in fixed proportions.
  37. Solid
    Molecules are held close together in an orderly fashion with little freedom of motion.
  38. Liquid
    Molecules are held together but are not held rigidly in position.
  39. Gas
    Molecules are separated by distances that are large compared with the size of the molecules.
  40. Extensive property
    Depends on how much matter is being considered.

    Ex: Mass, Volume, Lenth
  41. Intensive property
    Does not depend on how much matter is being considered.

    Ex: Density, Temperature, Color
  42. Isotopes
    Atoms of the same element having a different number of neutrons.
  43. Law of definite proportions
    States that different samples of the same compound always contain its constituent elements in the same proportion by mass.
  44. Law of multiple proportions
    If two elements can combine to form more than one compound, the masses of one element that combine with a fixed mass of the other elements are in ratios of small whole numbers.
  45. Law of conservation of mass
    Matter can neither be created nor destroyed.
  46. Greek prefix 1-
  47. Greek prefix 2-
  48. Greek prefix 3-
  49. Greek prefix 4-
  50. Greek prefix 5-
  51. Greek prefix 6-
  52. Greek prefix 7-
  53. Greek prefix 8-
  54. Greek prefix 9-
  55. Greek prefix 10-
  56. Giga
    G 109, 1 gigameter= 1X109 meter
  57. mega
    M 106, 1 megameter= 1X10meter
  58. deci
    d 10-1, 1 decimeter= 0.1meter
  59. centi
    c 10-2, 1 centimeter= 0.01 meter
  60. milli
    m 10-3 1 millimeter= 0.001 meter
  61. micro
    u 10-6 1 micrometer = 1 X 10-6 meter
  62. nano
    n 10-9, 1 nanometer = 1 X 10-9 meter
  63. pico
    • p 10-12, 1 picometer = 1 X 10-12 meter
Card Set:
Chemistry I
2013-01-28 01:01:43

atoms, compounds, acids, bases, naming
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