Chemistry Final Semester 1

Card Set Information

Author:
Anonymous
ID:
130712
Filename:
Chemistry Final Semester 1
Updated:
2012-01-26 02:49:37
Tags:
Chemistry Final Semester
Folders:

Description:
Chemistry Final Semester 1
Show Answers:

Home > Flashcards > Print Preview

The flashcards below were created by user Anonymous on FreezingBlue Flashcards. What would you like to do?


  1. How do you solve for density?
  2. How do you find mass?
  3. How do you find volume?
  4. HCl
    hydoro-chloric acid
  5. Phospheric acid
  6. Hydro-chloric acid
  7. Phospheric acid
  8. Nitric acid
    HNO3
  9. HNO3
    Nitric acid
  10. Sulfuric acid
    H2SO4
  11. H2SO4
    Sulfuric acid
  12. Acetic acid
    CH3COOH
  13. CH3COOH
    Acetic acid
  14. Carbonic acid
    H2Co3
  15. H2CO3
    Carbonic acid
  16. Water freezes at?
    0o C
  17. Water boils at?
    100oC
  18. Oxidation numbers
    • Find two elements oxidation numbers, add them up, then find the last one. Ex. Mg(No3)2
    • O: 3x2=6 so (6)(-2)=-12
    • Mg:(1)(2)=2
    • -12+2=-10
    • N:(2)(5)=10
    • -10+10=0
  19. Isotopes
    • Number of protons and nutrons. (They are the same number)
    • Ex. C- 6+6=12amu's
    • Electrons have no mass. Don't add them. Look at atomic mass and top number.
  20. Vertical columns of teh periodic table are called?
    Groups or families
  21. The horizontal rows of elements in the periodic table are called?
    Periods
  22. Mass
    • Symbol: m
    • Unit name: kilogram
    • Unit abbreviation: kg
  23. Length
    • Symbol: l
    • Unit name: meter
    • Unit abbreviation: kg
  24. Volume
    • Symbol: V
    • Solve: Length x width x height
  25. Kilo
    • Abbreviation: k
    • Exponential factor: 103
    • Meaning:1,000
    • Example: 1 kilometer(km)=1,000m
  26. centi
    • Abbreviation: c
    • Exponential Factor:10-2
    • Meaning: 1/100
    • Example: 1 centimeter (cm) = o.o1 m
  27. mili
    • Abbreviation: m
    • Exponential factor: 10-3
    • Meaning: 1/1,000
    • Example: 1millimeter (mm) = 0.001 m
  28. deci
    • Symbol: d
    • Exponential factor: 10-1
    • Meaning: 1/10
    • Example: 1 decimeter (dm)=0.1m
  29. Convert C o to Fo
    Multiply by 9, then divide by 5, then add 32
  30. Convert from Fo to Co
    Deduct 32, then multiply by 5, then divide by 9
  31. Energy levels
    • n=1 (s)
    • n=2 (s,p)
    • n=3 (s,p,d)
    • n=4 (s,p,d,f)
    • n=5
    • n=6
  32. Number of electrons in the blocks
    • s=2
    • p=6
    • d=10
    • f=14
  33. Number of orbitals per block
    • s=1
    • p=3
    • d=5
    • f=7
  34. Development of the periodic table
    Johann Dobereiner began to group elements with similar properties into groups. A.E. Beguyer de Chancourtois was the first person to make use of atomic weights to reveal that te elements were arranged according to their atomic weights with similar elements occurring at regular intervals. Medeleev and Meyer produced it.
  35. Nucleus
    Composed of protons, electrons, and neutrons. Protons are positive, electrons are negative, and neutrons are neutral.
  36. Significant digits
    • 1.All digits are significant except zeros at the beginning of the number, and possibly terminal zeros.
    • 2.Terminal zeros ending at the right of the decimal point are significant.
    • 3.Terminal zeros in a number without an explicit decimal point may or may not be significant.
    • Ex. 0.0025 = 2 Significant Figures
    • 252 = 3 Significant Figures
    • 250 =2 or 3 Significant Figures
  37. Scientific notation
    • Just the digits (with the decimal point placed after the first digit), followed by× 10 to a power that puts the decimal point where it should be (i.e. it shows how many places to move the decimal point).
  38. Avogardro's constant
    mole=6.02x1023
  39. Empirical Formula Determination
    • 1.treat % as mass, and convert grams to moles.
    • 2.divide each value of moles by the smallest of the values.
    • 3.multiply each number by an integer to obtain all whole numbers.
  40. Finding Molecular Formula
    • 1.find the formula mass of C3H5O2
    • 2.divide the molecular mass by the mass given by the empirical formula.
    • 3.multiply the empirical formula by this number to get the molecular formula.

What would you like to do?

Home > Flashcards > Print Preview