Chemistry 1050 final study guide

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Chemistry 1050 final study guide
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2011-12-13 00:13:51
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Study for chemistry 1050 final
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  1. What is the name of CoS?
    Cobalt(II) sulfide
  2. What is the formula for an ionic compound made of magnesium and sulfer?
    MgS
  3. Which of the following was discovered by rutherford (gold foil)
    Atoms are mostly empty space
  4. which of the following items is a chemical property?
    The odor of spearmint gum
  5. What is the name of HClO3?
    Chloric acid
  6. A good definition of chemistry is
    the science that seeks to understand what matter does by studying what atoms and molecules do.
  7. The empirical formula of a compound
    indicates the simplest ratio of atoms in the compound.
  8. The pressure of a gas is due to
    collisions of gas molecules
  9. Charles law
    T1V1=T2V2
  10. The principle quantum numer (n)
    specifies the subshell of the orbital
  11. The wavelength of light is inversely related to its...
    energy
  12. Avogadro's law is expressed as
    V=1/n
  13. Chlorine and bromine have very similar chemical properties. This is best expliained by the fact that both elements
    have the same number of valence electrons.
  14. When neon light is passed through a prism, what is observed?
    bright colored lines
  15. "When filling orbitals of equal energy, electrons fill them singly first with parallel spins." This is known as:
    Hunds rule
  16. Electromagnetic spectrum from shortest to longest wavelenght.
    Gamme rays--> X-rays -->Ultraviolent radiation-->visible light--> infrared radiation-->microwaves-->radio waves
  17. Properties of bases
    • žBitter taste, slippery feeling (NaOH)
    • žTurn red litmus blue
    • žDissociate to give OH- ions
    • žAqueous solutions: pH > 7
  18. Properties of acids
    • žSour taste
    • žTurn blue litmus red
    • žDissociate to give H+
    • (or H3O+) ions
    • žAqueous solutions: pH < 7
  19. Liquids thta have high vapor pressure and low boiling poins are called
    violatile liquids
  20. Density=
    mass/volume
  21. Pure substance-
    one type of atom or molecule that is bonded together
  22. Mixture
    • two or more different atoms or molecules that
    • are not bonded together
  23. Element-
    • two or more like atoms bonded together (gold,
    • lead oxygen)
  24. Compound-
    • two or more different atoms bonded together
    • salt, sugar, distilled water)
  25. Physical properties
    Doesan't change properties, ex odor, color, taste, appearance, melting, boiling, freezing, weight, density
  26. Chemical properties-
    • Combustion, oxidation, reduction, acid/base
    • reaction
  27. calorie-joules
    1 calorie (cal)= 4.184 joules (J)
  28. kilowatt-hour (kWh)-joules (J)
    1 Kwh = 3.60 *10^6 (J)
  29. T(in K) = T (in C)
    T (in oC) + 273.15
  30. T (in oF) = C
    1.8T (in oC) + 32
  31. Be able to calculate the specific heat of a reaction (heat capacity). Formula?
    q = m x Cs x AT

    (Its not really an A)
  32. q = m x Cs x AT
    • q=heat absorbed or released
    • m=mass
    • Cs=specificheat
    • AT=temperature
    • change
  33. the specific heat of water
    4.186 joule/gram
  34. Democritus
    Atoms are the smallest complete unit of matter which cannot be broken down or changed into another form by chemical or physical means
  35. Thompson
    Cathrode ray (materials contain electrons), plub pudding model (electrons held in sphere of protons)
  36. Rutherford
    Gold foil experiment = nucleus
  37. Dalton
    atomic theory (you may want to look at more)
  38. Atomic mass
    (% abundance)n * (mass)n
  39. Diatomic elements
    H, N, O, F, Cl, Br, I
  40. Molecular compound
    • with usually two like nonmetal atoms bond
    • together as their basic unit
  41. Molecular compound
    • with usually two like nonmetal atoms bond
    • together as their basic unit
  42. Ionic
    • Exist in nature when one metal atom bonds with
    • one or more nonmetal atoms
  43. binary ionic type 1
    • formed between metal and non metal name:(cation
    • + anion + ide)
  44. binary ionic type 2
    • formed between transition metal and non metal
    • name:(cation + roman numeral + anion + ide)
  45. ionic compounds containing polyatomic ions name
    :(cation + anion using polyatomic names)
  46. molecular compounds
    • formed between two non metals name:(prefix +
    • element most like metal + prefix + next metal like atom)
  47. name acids without oxygen name:
    :(hydro + anion + ic + acid)
  48. acids with oxygen with ending ate name
    :(anion + ic + acid)
  49. acids with oxygen with ending ite name
    :(anion + ous + acid)
  50. Avogadro’s number for molecules/atoms
    6.022x1023
  51. Precipitation reaction
    Forms solid
  52. acid-base
    salt and water form
  53. gas evolution
    gas forms
  54. oxidation-reduction
    electron transfer
  55. combustion-substance reacts with oxygen
    • -substance reacts with oxygen
    • -also a type of oxidation-reduction reaction
  56. Pauli Exclusion Principle
    • orbitals may hold no more than two electrons
    • with opposing spins.
  57. Aufbau principle.
    • We place electrons in the energy shells and
    • subshells in order of energy, from low energy to high energy.
  58. Hund’s rule:
    When filling orbitals of equal energy, electrons fill them singly first, with parallel spins
  59. 1 atmosphere (atm) = (mmHg)
    1 atmosphere (atm) = 760 millimeters of mercury (mmHg)
  60. 1 atm = (psi)
    1 atm = 14.7 pounds per square inch (psi)
  61. 1mmHg = Torr
    1mmHg = 1 Torr
  62. 1 atm = (in. Hg)
    1 atm = 29.92inches of mercury (in. Hg)
  63. Charles law
    V1/T1=V2/T2
  64. Boyle law
    P1V1 =P2V2
  65. Avogadros law
    Avogadros-V1/n1 =V2/n2 (n= number of moles)
  66. ideal gas law
    PV=nRT
  67. PV=nRT (R =
    PV=nRT (R is constant = 0.0821 L*atm/mol*K)
  68. STP
    temp
    pressure
    volume
    Temp=273 KPressure=1 atmVolume= 22.4 L
  69. Dalton’s law
    Ptotal = Pa + Pb + Pc + ……

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