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Chem I

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Chem I

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  1. Chem I Semester 2 Review

  2. 1 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.

  3. 1 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.

  4. 1 • Which term does not fit with the others listed? • a. solid c. gas • b. reactant d. liquid

  5. 1 The chemical symbol for sodium is a. NA. c. SO. b. Na. d. So.

  6. 1 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.

  7. 1 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.

  8. 1 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.

  9. 1 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.

  10. 1 Physical properties of a substance include a. color and odor. c. malleability. b. melting & boiling points. d. all of the above.

  11. 1 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.

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

  13. 2 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

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

  15. 2 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

  16. 2 The closeness of a measurement to its true value is a measure of its: a. usefulness. c. accuracy. b. precision. d. reproducibility.

  17. 2 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

  18. 2 A metric unit of volume is the: a. L. c. km. b. mg. d. K.

  19. 2 The number of seconds in a 40-hour work week can be calculated as follows:

  20. 2 The metric prefix kilo- means: a. 100 times smaller. c. 1000 times smaller. b. 1000 times larger. d. 100 times larger.

  21. 2 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

  22. 2 The temperature reading of -14C corresponds to a Kelvin reading of: a. 297.6 K. c. 287 K. b. -287 K. d. 259 K.

  23. 2 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

  24. 2 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

  25. 2 Chlorine boils at 239 K. What is the boiling point of chlorine expressed in degrees Celsius? a. 93C c. -61C b. 34C d. -34C

  26. 2 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%

  27. 3 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.

  28. 3 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.

  29. 3 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.

  30. 3 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.

  31. 3 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.

  32. 3 • All atoms of the same element have the same: • a. number of protons. c. mass number. • b. number of neutrons. d. mass.

  33. 3 • 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.

  34. 3 • 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.

  35. 3 • 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

  36. 3 • 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.

  37. 3 • Relative atomic masses are measured in • a. nanograms. c. angstroms. • b. grams. d. amus.

  38. 3 • If E is the symbol for an element, which two of the following symbols represent isotopes of the same element?

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

  40. 4 • If the electron configuration of an element is 1s22s22p63s23p5, the element is • a. iron. c. chlorine. • b. bromine. d. phosphorus.

  41. 4 • The electron configuration of calcium is • a. 1s22s22p23s23p34s2. • b. 1s22s22p103s23p4. • c. 1s22s23s23p6 3d8. • d. 1s22s22p63s23p64s2.

  42. 4 • The maximum number of electrons that can occupy the third principal energy level is • a. 18. c. 2. • b. 32. d. 8.

  43. 4 • As the frequency of light increases, the wavelength • a. increases. • b. remains the same. • c. decreases. • d. approaches the speed of light.

  44. 4 • 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.

  45. 4 • 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.

  46. 4 • 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.

  47. 5 • 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.

  48. 5 • Which sublevel corresponds to the transition metals in the periodic table? • a. s c. d • b. p d. f

  49. 5 • Which of the following elements is a metalloid? • a. As c. Br • b. Se d. Kr

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