Chem 1-april

60 Questions | Total Attempts: 36

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April Quizzes & Trivia

This is to help me practice for my exam. It took me a long time to type it.


Questions and Answers
  • 1. 
    Which of the following is a physical property?
    • A. 

      Falmmability

    • B. 

      Corrosiveness

    • C. 

      Inertness

    • D. 

      Malleability

    • E. 

      Rust-resistance

  • 2. 
    1-butanethiol, one of the compounds giving skunks their distinctive odor, freezes at -115.7 degree C and boils at 98.5 degrees C.  What is its phase at 200K?
    • A. 

      Gas

    • B. 

      Liquid

    • C. 

      Solid

    • D. 

      A mixture of solid and liquid

    • E. 

      A mixture of liquid and gas

  • 3. 
    Elements in the Periodic Table are arranged according to
    • A. 

      Date of discovery

    • B. 

      Atomic weight

    • C. 

      Atomic number

    • D. 

      Alphabetical order

    • E. 

      Number of neutrons

  • 4. 
    A Chemist is given an unknown gas sample.  Which observation describes a chemical property of the sample?
    • A. 

      It weighs 11.2 grams

    • B. 

      It has a sharp, stinging odor

    • C. 

      Its density is greather than that of air

    • D. 

      It extinguishes a glowing splint

    • E. 

      It is colorless

  • 5. 
    What is teh chemical symbol for chromium?
    • A. 

      Ca

    • B. 

      Cu

    • C. 

      Cl

    • D. 

      Cr

    • E. 

      C

  • 6. 
    What element is represented by the chemical symbol As?
    • A. 

      Gold

    • B. 

      Mercury

    • C. 

      Arsenic

    • D. 

      Silver

    • E. 

      Argon

  • 7. 
    When the prefix micro is used in the metric or SI system, a fundamental unit of measurement is multiplied by what factor?
    • A. 

      10^6

    • B. 

      10^-3

    • C. 

      10^-6

    • D. 

      10^-2

    • E. 

      10^3

  • 8. 
    Which measuremet represents the smallest quantity
    • A. 

      2950 ng

    • B. 

      29.5 mg

    • C. 

      2.95 x 10^-4

    • D. 

      2.95 x 10^3 ug

    • E. 

      2.95 x 10^-6

  • 9. 
    An atom with Z=40 and A=91 contains __________ protons and _______ neutrons.
    • A. 

      91;40

    • B. 

      51;40

    • C. 

      40;131

    • D. 

      40;91

    • E. 

      40;51

  • 10. 
    An atom with Z=35 and A=55 corresponds to the atom
    • A. 

      Cs

    • B. 

      Hg

    • C. 

      Mn

    • D. 

      Mg

    • E. 

      Cr

  • 11. 
    The metric unit for volume is _____ and the SI unit for volume is ______.
    • A. 

      ML; cc

    • B. 

      Cc; L

    • C. 

      M^3; L

    • D. 

      M^3, cm^3

    • E. 

      L, m^3

  • 12. 
    Which of the following measurements has three significant figures?
    • A. 

      0.03750 g

    • B. 

      1,230 g

    • C. 

      4.250 g

    • D. 

      0.0025 g

    • E. 

      0.006 g

  • 13. 
    Dicholoromethane is a liquid that has a specific gravity of 1.33.  It is immiscrible with water, forming a second layer when the two are mixed.  Dicholormethane makes up the ______ layer because it is _______ than water.
    • A. 

      Top, less dense

    • B. 

      Bottom, less dense

    • C. 

      Top, more dense

    • D. 

      Bottom, more dense

    • E. 

      None of the above

  • 14. 
    How many pounds are contained in 17.2 kg?
    • A. 

      0.084 lb

    • B. 

      38.0 lb

    • C. 

      0.038 lb

    • D. 

      185 lb

    • E. 

      380 lb

  • 15. 
    Consider the chemical reaction described as [heating mercury(II) oxide--> mercury + oxygen]. Identify the products in this sample.
    • A. 

      Mercury

    • B. 

      Heat

    • C. 

      Mercury + oxygen

    • D. 

      Mercury (II) oxide

    • E. 

      Oxygen

  • 16. 
    Which of the following are states of matter?
    • A. 

      Solution

    • B. 

      Mixture

    • C. 

      Gas

    • D. 

      Suspension

    • E. 

      All of the above

  • 17. 
    Which of the following is a mixture?
    • A. 

      Steam

    • B. 

      Gasoline

    • C. 

      Iron

    • D. 

      Antimony

    • E. 

      Sodium hydrogen carbonate

  • 18. 
    In a density  determination, a student measured 114.6mL of a liquid.  How many liters is this?
    • A. 

      1.146 x 10^-3 L

    • B. 

      1.146 L

    • C. 

      0.01146 L

    • D. 

      0.1146L

    • E. 

      11,460 L

  • 19. 
    Which characteristics correctly describe a neutron?
    • A. 

      Approx. mass 1 amu, charge -1 inside nucleus

    • B. 

      Approx. mass 1 amu; charge 0, inside nucleus

    • C. 

      Approx. mass 1 amu; charge +1, inside nucleus

    • D. 

      Approx. mass 5 x 10-4 amu, charge 0; inside nucleus

    • E. 

      Approx. mass 5 x 10-4 amu, charge -1, ouside nucleus

  • 20. 
    How many electrons can occupy the shell have n=2?
    • A. 

      6

    • B. 

      32

    • C. 

      2

    • D. 

      18

    • E. 

      8

  • 21. 
    What is the maximum number of electrons that can occupy the 4p orbitals
    • A. 

      6

    • B. 

      14

    • C. 

      10

    • D. 

      8

    • E. 

      2

  • 22. 
    Main group elements that are metals usually _____ one or more electons to form ______, which have a ______ charge.
    • A. 

      Lose, cations, positive

    • B. 

      Gain, anions, negative

    • C. 

      Lose, cations, negative

    • D. 

      Lose, anions, negative

    • E. 

      Gain, cations, positive

  • 23. 
    The property that describes the ease with which an atom give up an electron to form a positive ion is
    • A. 

      Electronegativity

    • B. 

      Electron affintity

    • C. 

      Ionization energy

  • 24. 
    All of the following are properties typical  of ionic compounds except
    • A. 

      Shatter when crystals are struck

    • B. 

      Exist as crystalline solids at room temperature

    • C. 

      Form distinct moleculres by interactoin of specific particles

    • D. 

      Have very high melting points and boiling points

    • E. 

      Conduct electrical current if dissolved in water

  • 25. 
    What is the most likely charge on an ion formed by an elements with a valence electron configuraton of ns2np4
    • A. 

      +4

    • B. 

      +6

    • C. 

      -1

    • D. 

      -2

    • E. 

      +2

  • 26. 
    Which element will form an ion with the lowest positive charge?
    • A. 

      Mg

    • B. 

      Al

    • C. 

      Sr

    • D. 

      P

    • E. 

      Na

  • 27. 
    Which element is represented by the dot structure shown? X (with 7dots)
    • A. 

      K

    • B. 

      Cr

    • C. 

      Kr

    • D. 

      Pb

    • E. 

      I

  • 28. 
    The name of S2- is
    • A. 

      Sulfur

    • B. 

      Sulfurous ion

    • C. 

      Sulfite ion

    • D. 

      Sulfide ion

    • E. 

      Sulfate ion

  • 29. 
    The name of Cu+ is _______ ion or _________ ion.
    • A. 

      Copper (I); cuprous

    • B. 

      Copper (i); cupric

    • C. 

      Copper; cupric

    • D. 

      Copper (II); cuprous

    • E. 

      Copper (II0; cupric

  • 30. 
    What is the formular of a compound formed by the M+ and X2-?
    • A. 

      MX3

    • B. 

      M2X

    • C. 

      M3X2

    • D. 

      M2X3

    • E. 

      None of the above

  • 31. 
    A formula unit of ionic compound cupric carbonate consists of _______ copper ions and ______ carbonate ions.
    • A. 

      One,two

    • B. 

      One, one

    • C. 

      Two, one

    • D. 

      Two, two

    • E. 

      Some other combination of ions

  • 32. 
    A formula unio of ammonium sulfate consists of __________ ammonium ions and _______ sulfate ions.
    • A. 

      Two, one

    • B. 

      One, two

    • C. 

      Two, three

    • D. 

      Four, four

    • E. 

      Three, two

  • 33. 
    Which of the following formulas represents a compound that is an acid?
    • A. 

      CaSO4

    • B. 

      H2S

    • C. 

      NH4Cl

    • D. 

      LiOH

    • E. 

      None of the above

  • 34. 
    A chemical bond formed when two atoms share two electons is a ____ bond; it is best described as ____________.
    • A. 

      Double, covalent

    • B. 

      Double, ionic

    • C. 

      Single, covalent

    • D. 

      Triple; covalent

    • E. 

      Single; ionic

  • 35. 
    Which element is most likely to form four covalent bonds?
    • A. 

      As

    • B. 

      P

    • C. 

      Se

    • D. 

      S

    • E. 

      Ge

  • 36. 
    In forming covalent bonds where the octet rule is obeyed, nitrogen usually forms ___________ bonds and oxygen forms ______ bonds.
    • A. 

      Five; two

    • B. 

      Two;three

    • C. 

      Three; six

    • D. 

      Five; six

    • E. 

      Three; two

  • 37. 
    Which formula is least likely to represent the molecular compound that really exists?
    • A. 

      SF6

    • B. 

      PCl5

    • C. 

      SF4

    • D. 

      Br3Cl5

    • E. 

      C2H6

  • 38. 
    The water moleculre has a ____ geometry because its central atoms has ____ bonds and ____ lone pairs of electrons..
    • A. 

      Tetrahedral; four;zero

    • B. 

      Linear; two, two

    • C. 

      Planar triangular; three; one

    • D. 

      Bent; two; two

    • E. 

      Pyramidal; three;one

  • 39. 
    If the elements W,X,Y,Z have electronegativity values of 1.0, 2.0, 2.5, and 3.5, respectively, which bond is least polar?
    • A. 

      YZ

    • B. 

      WZ

    • C. 

      XZ

    • D. 

      WX

    • E. 

      XY

  • 40. 
    The ammonia molecule is phyramidal.  The electronegativities of N and H are 3.0 and 2.1, respectively.  Based on these values and on consideration of molecular geometry, the C-O bond is ______ and the molecule is___________.
    • A. 

      Non-polar; non-polar

    • B. 

      Non-polar, polar

    • C. 

      Polar; non-polar

    • D. 

      Polar;polar

    • E. 

      None of the above

  • 41. 
    The molevule SO2 has a _______ shape.
    • A. 

      Pyramidal

    • B. 

      Tetrahedral

    • C. 

      Bent

    • D. 

      Linear

    • E. 

      Planar

  • 42. 
    The molecule HC(Triplebonds)N has a _______ shape.
    • A. 

      Pyramidal

    • B. 

      Tetrahedral

    • C. 

      Bent

    • D. 

      Linear

    • E. 

      Planar

  • 43. 
    The element least like to obey the octet rule in forming chemical bonds is
    • A. 

      Nitrogen

    • B. 

      Neon

    • C. 

      Oxygen

    • D. 

      Fluorine

    • E. 

      Carbon

  • 44. 
    Which description best fits a solid?
    • A. 

      Volume and shape of container, no intermolecular attractions

    • B. 

      Volume and shape of container, stronger intermolecular forces

    • C. 

      Definite volume and shape of container, moderate intermolecular attractions

    • D. 

      Definite volume; shape of container, no intermolecular attractions

    • E. 

      Definite shape and volume, strong intermolecular attractions

  • 45. 
    Which of the assumptions of the kinetic-molecular theory best explains the observatoin that a ballon collapses when exposed to liquid nitrogen(which is much colder than a cold winter day!!)?
    • A. 

      The velocity of gas moleculres is proportional to their kevin temperature

    • B. 

      In collisions with the walls of teh container or with other moleculres, energy is conserved

    • C. 

      The amount of space occupied by a gas is much greater than the spaced occupied by teh actual gas molecules

    • D. 

      Collisions with the walls of the container or with other molecules are elastic

    • E. 

      Gas molecules move at random with no attractive forces between them

  • 46. 
    What would the new pressure if a 400mL gas smaple at 380 mm Hg is expanded to 800 mL with no change in temperature?
    • A. 

      380 mm Hg

    • B. 

      760 mm Hg

    • C. 

      950 mm Hg

    • D. 

      570 mm Hg

    • E. 

      190 mm Hg

  • 47. 
    All of the statements are true for spontaneous reactions except
    • A. 

      If the enthalpy change is unfavorable, they occur at high temperature

    • B. 

      They are said to be exergonic

    • C. 

      The value of delta G is unaffected by a catalyst

    • D. 

      The value of delta G is less than zero

    • E. 

      The reaction rate is determined by the value of delta G

  • 48. 
    As a pure element the oxidation number of zinc is ________, but in compounds such as ZnCO3 its oxidation number is__.
    • A. 

      0, +2

    • B. 

      0,0

    • C. 

      0, +1

    • D. 

      +1,0

    • E. 

      None of the above

  • 49. 
    A 250 mL sample of gas at 1.00 atm and 20 degrees C has the temperature increase to 40 degress C and the volume increased to 500 mL.  What is the new pressure?
    • A. 

      0.468 atm

    • B. 

      1.87 atm

    • C. 

      2.14 atm

    • D. 

      0.534 atm

    • E. 

      0.374 atm

  • 50. 
    Consider the reation shown: N2 + O2 --> 2NO  Delta H=+43.2 kcal.  When 50.0 g of N2 react, _____ kcal will be _________.
    • A. 

      77.1, produced

    • B. 

      2160; consumed

    • C. 

      77.1; consumed

    • D. 

      2160 produced

    • E. 

      43.2 produced

  • 51. 
    How much Ca(NO3)2 should be weighed out to have 0.650 mol?
    • A. 

      133g

    • B. 

      66.4 g

    • C. 

      165g

    • D. 

      97.6 g

    • E. 

      107g

  • 52. 
    105g of MgCl2 contains __________ mol MgCl2.
    • A. 

      1.10

    • B. 

      1.76

    • C. 

      6.62 x 10^23

    • D. 

      105

    • E. 

      1.06 x 10^24

  • 53. 
    The molecular weight of PCl3 is ________amu.
    • A. 

      136.00

    • B. 

      199.26

    • C. 

      139.00

    • D. 

      66.42

    • E. 

      137.33

  • 54. 
    The position of the equilibrium for a system where K= 4.6 x 10^-15 can be described as being favored to _____; the concentration of products is relatively____________.
    • A. 

      The right; small

    • B. 

      The left, large

    • C. 

      The left; small

    • D. 

      The right; large

    • E. 

      Neither direction;large

  • 55. 
    Which change to this reaction system would cause the equilibrium to shift to the right? N2 (g) + 3 H2 --> 2 NH3 (g) + heat
    • A. 

      Removal of H2 (g)

    • B. 

      Heating the system

    • C. 

      Addition of a catalyst

    • D. 

      Lowering the temperature

    • E. 

      Addition of Nh3

  • 56. 
    For the following reation, increasing the pressure will cause the equilibrium _____2 SO2+ O2 -->  2 SO3 + Heat
    • A. 

      Shift to the right, toward ths products

    • B. 

      Pressure has no effect on equilibrium

    • C. 

      Remain undchanged, but the mixxture will get warmer

    • D. 

      Remain unchanged, but the mixture will get colder

    • E. 

      Shfit to the left, towards reactants

  • 57. 
    For the reaction given below, what quantity of heat will be produced if 90 g of C3H8 are consumed in the reaction? C3H8 + 5 O2 ---> 2 CO2 + 4H2O +488 kca
    • A. 

      488 kcal

    • B. 

      332 kcal

    • C. 

      996 kcal

    • D. 

      976 kcal

    • E. 

      239 kcal

  • 58. 
    Which statement based on the mole concept is not correct?
    • A. 

      The number of atoms in one moele of platinum is the smae as the number of atoms in one mole of uranium.

    • B. 

      One mole of sodium chloride, NaCl, contains the same number of ions as one mole of calcium sulfate, CaSO4.

    • C. 

      One mole of methane, CH4, contains the same number of atoms as one mole of carbond dioxide, Co2.

    • D. 

      One mole of bromine, Br2, contains the same number of molecules as one mole of propane, C3H8.

    • E. 

      The molar mass of a diatomic element is its atomic weight times two.

  • 59. 
    Which process is endothermic?
    • A. 

      Gasoline spilled on the ground evaporates very quickly

    • B. 

      The melted waz harden after a candle is extinguished.

    • C. 

      Water condenses on the outside of a cold soda can.

    • D. 

      Water vapor forms ice crystals in the upper atmosphere.

    • E. 

      None of these

  • 60. 
    S + O2 --> SO2 +70.8 kcal based on teh reation shown, which statement is true?
    • A. 

      70.8 kcal are consumed when 32.1 g of sulfur reacts

    • B. 

      70.8 kcal are produced when 1 g of sulfure reacts

    • C. 

      70.8 kcal are consumed when 1 g of sulfur reacts

    • D. 

      70.8 kcal are produced when 32.1 g of sulfur reacts

    • E. 

      70.8 kcal are procued when 1 g of sulfur dioxide is produced