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Chem I

Chem I. Semester 2 Review. 2. All of the following are general characteristics of a substance in the liquid state except a. definite volume. c. not easily compressed. b. able to flow. d. definite shape. d. 2. In the chemical reaction iron plus oxygen →iron oxide,

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Chem I

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  1. Chem I Semester 2 Review

  2. 2 • All of the following are general characteristics of a substance in the liquid state except • a. definite volume. c. not easily compressed. • b. able to flow. d. definite shape. d.

  3. 2 • In the chemical reaction iron plus oxygen →iron oxide, • a. iron oxide is a reactant. c. oxygen is a product. • b. iron is a reactant. d. iron is a product. b.

  4. 2 • Which term does not fit with the others listed? • a. solid c. gas • b. reactant d. liquid b.

  5. 2 • The chemical symbol for sodium is • a. NA. c. SO. • b. Na. d. So. b.

  6. 2 • A basketball has more mass than a golf ball because: • a. the basketball takes up more space. • b. the basketball contains more matter. • c. the golf ball contains a different kind of matter. • d. the golf ball has an indefinite composition. b.

  7. 2 • A gas is a form of matter that • a. has a definite volume. • b. is generally a liquid or solid at room temperature. • c. takes the shape and volume of its container. • d. is difficult to compress. c.

  8. 2 • Homogeneous mixtures • a. are always liquids. • b. consist of two or more phases. • c. have a composition that is fixed. • d. are known as solutions. d.

  9. 2 • A compound • a. is a pure substance. • b. has a composition that varies. • c. can be physically separated into its elements. • d. has properties similar to those of its elements. a.

  10. 2 • Physical properties of a substance include • a. color and odor. c. malleability. • b. melting & boiling points. d. all of the above. d.

  11. 2 • When iron and oxygen combine to form iron oxide, • a. a physical change occurs. • b. a change of state occurs. • c. a change in mass occurs. • d. a chemical change occurs. d.

  12. 3 • How many significant figures are in the measurement 2103.2 g? • a. 2 c. 4 • b. 3 d. 5 d.

  13. 3 • Which of these equalities is not correct? • a. 100 cg= 1 g c. 1 cm3= 1 mL • b. 1000 mm= 1 m d. 10 kg= 1 g d.

  14. 3 • How many of the zeros in the measurement 0.000 040 200 m are significant? • a. 2 c. 7 • b. 3 d. 8 b.

  15. 3 • How many milligrams are in 2.5 kg? • a. 2.5 x 106 mg c. 2.5 x 104 mg • b. 25 mg d. 2.5 x 102 mg a.

  16. 3 • The closeness of a measurement to its true value is a measure of its: • a. usefulness. c. accuracy. • b. precision. d. reproducibility. c.

  17. 3 • Which of these measurements is expressed to three significant figures? • a. 0.070 mm c. 7007 mg • b. 7.30 x 107 km d. 0.007 m b.

  18. 3 • A metric unit of volume is the: • a. L. c. km. • b. mg. d. K. a.

  19. 3 • The number of seconds in a 40-hour work week can be calculated as • follows: c.

  20. 3 • The metric prefix kilo- means: • a. 100 times smaller. c. 1000 times smaller. • b. 1000 times larger. d. 100 times larger. b.

  21. 3 • What is the volume of 60.0 g of ether if the density of ether is 0.70 g/mL? • a. 86 mL c. 2.4 x 102mL • b. 1.2 x 102mL d. 42 mL a.

  22. 3 • The temperature reading of -14C corresponds to a Kelvin reading of: • a. 297.6 K. c. 287 K. • b. -287 K. d. 259 K. d.

  23. 3 • Concentrated hydrochloric acid has a density of 1.19 g/mL. What is the mass, in grams, of 2.00 liters of this acid? • a. 2.38 x 103 g c. 4.20 x 10-4 g • b. 2.38 g d. 4.20 x 104 g a.

  24. 3 • A conversion factor: • a. is equal to 1. • b. is a ratio of equivalent measurements. • c. does not change the value of a measurement. • d. all of the above d.

  25. 3 • Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius? • a. 93C c. -61C • b. 34C d. -34C d.

  26. 3 • A student measures a volume as 25 mL, whereas the correct volume is 23 mL. What is the percent error? • a. 0.087% c. 0.92% • b. 8.7% d. 8.0% b.

  27. 4 • Which of the following is not a part of Dalton’s atomic theory? • a. All elements are composed of atoms. • b. Atoms of the same element are alike. • c. Atoms are always in motion. • d. Atoms that combine do so in simple whole-number ratios. c.

  28. 4 • The nucleus of an atom is • a. negatively charged and has a low density. • b. negatively charged and has a high density. • c. positively charged and has a low density. • d. positively charged and has a high density. d.

  29. 4 • Dalton theorized that atoms are indivisible and that all atoms of an element are identical. Scientists now know that • a. Dalton’s theories are completely correct. • b. atoms of an element can have different numbers of protons. • c. atoms are all divisible. • d. all atoms of an element are not identical but they all have the same mass. c.

  30. 4 • The number of neutrons in the nucleus of an atom can be calculated by • a. adding together the numbers of electrons and protons. • b. subtracting the number of protons from the number of electrons. • c. subtracting the number of protons from the mass number. • d. adding the mass number to the number of protons. c.

  31. 4 • The sum of the protons and neutrons in an atom equals the • a. atomic number. c. atomic mass. • b. number of electrons. d. mass number. d.

  32. 4 • All atoms of the same element have the same: • a. number of protons. c. mass number. • b. number of neutrons. d. mass. a.

  33. 4 • Which of these statements is false? • a. Electrons have a negative charge. • b. Electrons have a mass of 1 amu. • c. The nucleus of an atom is positively charged. • d. The neutron is found in the nucleus of an atom. b.

  34. 4 • An atom of an element with atomic number 48 and mass number 120 contains • a. 48 protons, 48 electrons, and 72 neutrons. • b. 72 protons, 48 electrons, and 48 neutrons. • c. 120 protons, 48 electrons, and 72 neutrons. • d. 72 protons, 72 electrons, and 48 neutrons. a.

  35. 4 • The number 80 in the name bromine-80 represents • a. the atomic number. • b. the mass number. • c. the sum of protons and electrons. • d. none of the above b.

  36. 4 • Which of these statements is not true? • a. Atoms of the same elements can have different masses. • b. The nucleus of an atom has a positive charge. • c. Atoms of isotopes of an element have different numbers of protons. • d. Atoms are mostly empty space. c.

  37. 4 • Relative atomic masses are measured in • a. nanograms. c. angstroms. • b. grams. d. amus. d.

  38. 4 • If E is the symbol for an element, which two of the following symbols represent isotopes of the same element? c.

  39. 5 • The fourth principal energy level has • a. 4 orbitals. c. 32 orbitals. • b. 16 orbitals. d. 9 orbitals. b.

  40. 5 • If the electron configuration of an element is 1s22s22p63s23p5, the element is • a. iron. c. chlorine. • b. bromine. d. phosphorus. c.

  41. 5 • The electron configuration of calcium is • a. 1s22s22p23s23p34s2. • b. 1s22s22p103s23p4. • c. 1s22s23s23p6 3d8. • d. 1s22s22p63s23p64s2. d.

  42. 5 • The maximum number of electrons that can occupy the third principal energy level is • a. 18. c. 2. • b. 32. d. 8. a.

  43. 5 • As the frequency of light increases, the wavelength • a. increases. • b. remains the same. • c. decreases. • d. approaches the speed of light. c.

  44. 5 • In order to occupy the same orbital, two electrons must have • a. the same direction of spin. • b. low energy. • c. opposite charge. • d. opposite spin. d.

  45. 5 • Stable electron configurations are likely to contain • a. high-energy electrons. • b. unfilled s orbitals. • c. fewer electrons than unstable configurations. • d. filled energy sublevels. d.

  46. 5 • According to Hund’s rule, when electrons occupy orbitals of equal energy, one electron enters each orbit until • a. all the orbitals contain one electron, with spins parallel. • b. all the orbitals contain one electron, with opposite spins. • c. there are two electrons in each orbital. • d. electron velocities become constant. a.

  47. 6 • In the periodic table, there is a periodic pattern in the physical and chemical properties of elements when they are arranged in order of • a. increasing atomic mass. • b. increasing electronegativity. • c. increasing atomic radius. • d. increasing atomic number. d.

  48. 6 • Which sublevel corresponds to the transition metals in the periodic table? • a. s c. d • b. p d. f c.

  49. 6 • Which of the following elements is a metalloid? • a. As c. Br • b. Se d. Kr a.

  50. 6 • The element iodine, I, is a • a. period 5 alkali metal. • b. period 4 halogen. • c. period 5 halogen. • d. period 5 transition metal. c.

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