Chem 11 Test 1

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  1. Scientific Method
    • Define the problem or question
    • Perform experiments
    • Interpretation of Results (hypothesis)
    • Extensive testing leads to formation of a law
    • Eventually leads to a theory
    • Theory is tested and discarded/modified as necessary
  2. Def: Qualitative
    Observations like color and shape
  3. Def: Quantitative
    Taking measurements with precision
  4. Def: Weight
    Refers to the force that gravity exerts on an object
  5. Def: Mass
    Always the same, the weight of the object
  6. mL to cm conversion
    1mL = 1cm^3
  7. Inches to cm conversion
    1in = 2.54cm
  8. Volume Formula
    • V=distance^3
    • Distance could be in:
    • cm^3/mL (conversion)
    • m^3 (SI unit for volume)
  9. SI Unit for Volume
  10. Density Formula
  11. Temperature conversions
    • K = °C+273.15
    • °F = 1.8*°C+32
    • °C = (°F-32)/1.8
  12. Yard to Feet Conversion
    1yd = 3ft
  13. Miles to Feet Conversion
    1mi = 5280ft
  14. Yard to Inches Conversion
    1yd = 36in
  15. Matter
    Anything that occupies space and has mass
  16. Substances
    A form of matter that has a definite composition and distinct properties
  17. Mixture
    Combination of two or more substances in which the substances retain their distinct identities
  18. Homogeneous Mixture
    The composition of the mixture is the same throughout
  19. Heterogeneous Mixture
    The composition of the mixture is not uniform
  20. Element
    Substance that cannot be separated into simpler substances by chemical means
  21. Compound
    A substance composed of atoms of two or more elements chemically united in fixed proportions
  22. Physical Properties
    Properties that can be measured and observed without changing the composition or identity of a substance
  23. Chemical properties
    Properties that can only be observed by carrying out a chemical change
  24. Extensive Properties
    • Depend on how much matter is being considered.
    • Like mass, length, volume
  25. Intensive Properties
    • Independent on how much matter is being considered.
    • Like Temperature, density, color
  26. Law of Conservation of Mass
    No measurable change in mass occurs during a chemical reaction
  27. Law of Definite Proportions
    All sample of the same compound always contain the same proportions by mass of the component elements
  28. Law of Multiple Proportions
    When two elements combine to form more than one compound, the ratios of the masses of the second element combining with 1 gram of the first element can always be reduced to simple whole number ratios
  29. Dalton's Atomic Theory
    • All matter is composed of exceedingly small, indivisible particles called atoms
    • All atoms of the givem element are identical both in mass and chemical properties
    • Atoms are not created or destroyed in chemical reactions
    • Atoms combine in simple. fixed, whole-number ratios to form compounds
  30. Cathode
    Negatively charged plate
  31. Anode
    Positively charged plate
  32. Radioactivity
    Spontaneous emission of particles/radiation
  33. Alpha Particles
    • Positively charged and very heavy
    • Bend toward negative charge plate
  34. Beta Particles
    • Negatively charged and much lighter
    • Bend toward positive charge plate
  35. Gamma Particles
    • No charge
    • Electrically neutral
  36. How to read an element: AZX
    • A = Mass Number (Protons + Neutrons)
    • Z = Atomic Number (Number of protons)
    • X = Element
  37. Ions
    An atom or group of atoms that has a net positive or negative charge
  38. Cations
    Positively charged ions resulting from the loss of one or more electrons
  39. Anions
    Negatively charged ions resulting from the addition of one or more electrons
  40. 7 Diatomic Elements
    • H - Hydrogen
    • N - Nitrogen
    • O - Oxygen
    • F - Flourine
    • Cl - Chlorine
    • Br - Bromine
    • I - Iodine
Card Set:
Chem 11 Test 1
2016-01-10 04:03:20
Chem 11 Test

Chem 11 Test 1
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