CHEM1111 Test 1

  1. What symbol depicts Tera-
    What symbol depicts  Giga-
    • T: 1e^12
    • G: 1e^9
  2. What symbol depicts -Mega?
    What symbol depicts -Kilo?
    • M: 1e^6
    • K: 1e^3
  3. What symbol depicts -Deci?
    What symbol depicts -Centi?
    • d: 1e^-1
    • c: 1e^-2
  4. What symbol depicts mili-?
    What symbol depicts micro-?
    • m: 1e^-3
    • μ:  1e^-6
  5. What symbol depicts nano-?
    What symbol depicts pico-?
    • n: 1e^-9
    • p: 1e^-12
  6. What is the study of matter and the changes that matter undergoes?
    Chemistry
  7. What is anything that has mass and occupies space; everything you see around you?
    Matter
  8. Define chemistry
    The study of matter and the changes that matter undergoes
  9. Define Matter.
    Anything that has mass and occupies space; everything you see around you.
  10. What are the two types of mixtures?
    What are the two types of pure substance?
    • Homogeneous and Heterogenous 
    • Compound and Element
  11. How does a mixture change into pure substances?
    Separation by physical methods
  12. What are the 3 physical classification of matter?
    • Solid
    • Liquid 
    • Gas
  13. Describe the 3 physical classifications of matter.
    • Solid: Particles held together, does not take the shape of the container
    • Liquid: Particles not held rigidly, conform to the shape of the container
    • Gas: Particles have freedom to move around, assume the volume and shape of the container
  14. Equation for Celcius to Kelvin
    K=C+273.15
  15. Kelvin (SI unit) is represented by ___; no ____ sign. The ____ scale.
    • K
    • Degree
    • Absolute
  16. Volume (derived unit): meter cubed (m3)
    The unit liter (L) is more commonly used in the laboratory setting.
    1L = 1 dm3 or 1000cm3.
    1dm x 1dm x 1dm = 1 dm3 = 1 L1dm = 0.1m = 10cm 10 cm x 10 cm x 10 cm = 1000 cm3 = 1000 mL (1cm3 = 1mL) = 1 L
  17. What density and its formula?
    • Ratio of mass to volume
    • Formula:

    d=m/v

    • d = density (g/mL)
    • m = mass (g)
    • V = volume (mL or cm3)
  18. The density of a piece of copper wire is
    8.96 g/cm3. Calculate the volume in cm3
    of a piece of copper with a mass of 4.28 g.
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  19. Scientific Notations: N x 10n

    The N is a number between __ and __
    n is a ___ or ___ integer
    • 1
    • 10
    • Positive 
    • Negative
  20. Scientific Equations Add or Subtract

    1) Write each quantity with the same ___
    2)Combine N1 and N2
    3)The exponent, n, . . . .
    • exponent n
    • remains the same


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  21. (4.0 x 10^-5) x (7.0 x 10^3) =
    • (4.0 x 7.0) x (10^-5+3) =
    • 28 x 10^-2 =
    • 2.8 x 10^-1
  22. 8.5 x 10^4 ÷ 5.0 x 10^9 =
    • (8.5 ÷ 5.0) x 10^4-9 =
    • 1.7 x 10^-5
  23. Scientific Notation; Multiplication

    1)_____ N1 and N2
    2)_____exponents n1 and n2
    • Multipy 
    • Add
  24. Scientific Notation; Division 

    1)_____ N1 and N2
    2)_____ exponents n1 and n2
    • Divide
    • Subtract
  25. What is how close a measurement is to the true or accepted value?
    Accuracy
  26. What is how closely measurements of the same thing are to one another?
    Precision
  27. Define Accuracy.
    how close a measurement is to the true or accepted value
  28. Define Precision.
    how closely measurements of the same thing are to one another
  29. Difference between exact numbers and inexact numbers
    • Inexact number are obtained by any other method  other than counting
    • e.g. weighing, measuring by ruler, thermometer, etc.
  30. An inexact number must be reported so as to indicate its uncertainty

    Significant figures are the meaningful digits in a reported number.

    The last digit in a measured number is referred to as the ____ digit.
    uncertain
  31. Read the level with the correct number of significant figures.

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    E)
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    E)
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    E)
  34. Leading zeros (place holder) are ____ significant .0023
    Leading zeros (place holder) are not significant .0023
  35. Zeros to the right of the last non-zero digit are ______ significant if decimal is not present. 230
    not
  36. Trailing zeros are ___ significant only if decimal is present 2.30
    Trailing zeros are significant only if decimal is present 2.30
  37. Zeros to the left of the first non-zero digit are ____ significant 02304
    Zeros to the left of the first non-zero digit are not significant 02304
  38. Captive zeros are ___ significant 2304
    Captive zeros are always significant 2304
  39. Determine the number of significant figures in
    each of the following.

    345.5 cm
    0.0058 g
    1205m
    250 mL
    250.00 mL
    • 4
    • 2
    • 4
    • 5
  40. Adding and Subtracting 

    The answer cannot have more digits to the right of the decimal point than any of the original numbers.

    Least number of digits to the right of decimal

    102.50 ← two digits after the decimal point
    + 0.231 ← three digits after the decimal point

    102.731 ← round to 102.73
  41. 105.5 L + 10.65 L =
    • Calculator answer: 116.15 L
    • Round to: 116.2 L Answer to the tenth position
  42. 1.0267 cm x 2.508 cm x 12.599 cm =
    • Calculator answer: 32.4419664 cm3
    • Round to: 32.44 cm3 round to the smallest number of significant figures
  43. Q: How many significant figures should you report as the sum of
    8.3801 + 2.57?

    A) 3, B) 5, C) 4, D) 6, E) 2
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  44. How many mL are in 1.63 L?
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  45. What is the wavelength, in meters, of orange light of wavelength 615 nm?
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  46. Area of an object is = 48.5cm2
    Express it in inch2 ?
    Given 1inch = 2.54cm
    Ans: 7.52 inch2
  47. How many millimeters are present in 20.0 inches?
    Ans: 508mm
  48. 2. The volume of a wooden block is 6.30 in3. This is equivalent to how many cubic centimeters?
    Ans: 103 cm3
  49. Density of Aluminum=2.70 g/cm3
    What is its density in kg/m3 ?
    • 2.70g x 1kg/1000g = 2.70 x 10-3 kg
    • 1cm3 = 10-6 m3 (1 m/100cm)
    • Density = 2.70 x 103 kg/m3
  50. Atoms have a nucleus which contains ____ and _____.
    Atoms have a nucleus which contains protons and neutrons
  51. The nucleus is surrounded by a cloud of electrons containing ____ charge.
    The nucleus is surrounded by a cloud of electrons containing negative charge.
  52. Protons – ____charge ____ in magnitude to the electron’s negative charge.
    Protons – positive charge equal in magnitude to the electron’s negative charge.
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    • Atomic number (Z) = number of protons in nucleus = number of electrons since atoms are neutral
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  54. ___ are atoms of the same element (X) with different numbers of neutrons in their nuclei

    Same atomic number but different mass number
    Isotopes
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    • 197 is the mass number and refers to the total number of protons and neutrons.
    • 79 is the atomic number and refers to the number of protons. Hence this atom has 79 electrons and 197-79 = 118 neutrons
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    B
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  58. The chlorine has two stable isotopes: 35Cl, with a mass of 34.97 amu and 75.77% abundance; and 37Cl, with a mass of 36.95 amu and 24.23%
    abundance.

    What is the atomic weight of chlorine?
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  59. _____ formula - shows exact number of atoms of each element in a molecule
    Subscripts indicate number of atoms of each element present in the formula.

    Example: H2O, C12H22O11
    Molecular
  60. Prefix meanings

    Mono-
    Di-
    Hexa-
    Hepta-
    • 1
    • 2
    • 6
    • 7
  61. Prefix meanings

    Tri-
    Tetra-
    Octa-
    Nona-
    • 3
    • 4
    • 8
    • 9
  62. Prefix meanings

    Penta-
    Deca-
    • 5
    • 10
  63. Write formulas for the following:

    Diphosphorus pentoxide
    Sulfur hexafluoride
    • P2O5
    • SF6
  64. Write formulas for the following:

    NO2
    N2O4
    • nitrogen dioxide
    • dinitrogen tetraoxide
  65. An ___ is formed when an atom, or group of atoms, has a net positive or negative charge


    If a neutral atom looses one or more electrons, it carries a positive charge and is known as a ____


    If a neutral atom gains one or more electrons, it carries a negative charge and is known as a ___
    • Ion
    • Cation
    • Anion
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    • 13 protons 10 electron
    • 16 protons 18 electrons
  67. Monatomic Ions

    1+
    • Li
    • Na
    • K
    • Rb
    • Cs
    • Ag
  68. Monatomic Ions

    2+
    • Mg
    • Ca
    • Sr
    • Ba
    • Cd
    • Zn
    • Hg
  69. Monatomic Ions

    1-
    • F
    • Cl
    • Br
    • I
  70. Monatomic Ions

    2-
    • O
    • S
    • Se
    • Te
  71. Monatomic Ions

    3-
    • N
    • P
  72. Monatomic Ions

    4-
    • C
    • Pb
  73. Monatomic Ions

    Either 2+ or 3+
    • Cr
    • Mn
    • Fe
    • Co
    • Ni
  74. Monatomic Ions

    Charges for 

    Cu
    Hg or Hg2
    Pb
    SN
    • + or 2+
    • 2+
    • 2 or 4+
    • 2 or 4+
  75. NH4
    Ammonium
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Author
fjn900
ID
334405
Card Set
CHEM1111 Test 1
Description
UTRGV
Updated