Chapter 4 Study Guide
True/False
Indicate whether the statement is true or false.
____ 1. The modern periodic table is arranged by increasing atomic mass of the elements.
____ 2. Aristotle named atoms atoms.
____ 3. A cathode ray tube consists of a stream of protons.
____ 4. In a neutral atom, the number of protons is equal to the number of neutrons.
____ 5. Gamma decay emits energy but no particles.
____ 6. An alpha particle is the equivalent of a Helium-4 nucleus.
____ 7. Nuclear decay can change one element into another one.
____ 8. Isotopes are forms of an element that have the same number of protons but a different number of electrons.
____ 9. An input of energy is required in order for nuclear decay to happen in an atom.
____ 10. Gamma decay is a form of nuclear radiation that consists entirely of energy, not matter.
____ 11.
The stability of a nucleus is determined by the ratio of electrons to protons.
____ 12. The mass of a neutron is approximately equal to the mass of a proton.
____ 13. The modern periodic table is arranged from right to left in order of increasing atomic mass.
____ 14. Greek philosophers thought that matter was composed of four elements: air, earth, fire, and water.
____ 15. In the notation , 107 represents the atomic number and 47 represents the atomic mass of silver.
____ 16. Radon is a radioactive substance that undergoes spontaneous emission of radiation due to its unstable nuclei.
____ 17. Atoms of a radioactive element can change into atoms of another element by emitting radiation.
____ 18. A proton is a subatomic particle carrying a charge equal to but opposite that of an electron.
____ 19. Cathode rays are deflected toward a negatively charged plate in an electric field.
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 20. The box for an element from the periodic table is shown. Which is the atomic mass?
a. / A / c. / Cb. / B / d. / D
____ 21. The box for an element from the periodic table is shown. Which is the atomic number?
a. / A / c. / Cb. / B / d. / D
____ 22. Which scientist described a positively charged core (“nucleus”) in the middle of a lot of empty space?
a. / Chadwick / c. / Rutherfordb. / Thomson / d. / Bohr
____ 23. Which scientist described an atom made of a solid positively charged substance with electrons dispersed throughout it?
a. / Chadwick / c. / Rutherfordb. / Thomson / d. / Bohr
____ 24. Which scientist developed the model of the atom shown?
a. / Chadwick / c. / Rutherfordb. / Thomson / d. / Bohr
____ 25. Which scientist developed the model of the atom shown?
a. / Chadwick / c. / Rutherfordb. / Thomson / d. / Bohr
____ 26. Which scientist described the existence of the neutron?
a. / Chadwick / c. / Rutherfordb. / Thomson / d. / Bohr
____ 27. Which one is comprised of the other three?
a. / proton / c. / electronb. / atom / d. / neutron
____ 28. Which has a charge of +1?
a. / proton / c. / electronb. / atom / d. / neutron
____ 29. Which one(s) have a mass of 1 amu?
a. / electron / c. / proton and neutronb. / proton / d. / electron and proton
Atoms
Atom / Protons / Neutrons / Electrons
1 / 8 / 10 / 8
2 / 10 / 9 / 10
3 / 9 / 9 / 9
4 / 8 / 11 / 8
____ 30. Which two are isotopes of one another?
a. / Atoms 1 & 2 / c. / Atoms 1 & 3b. / Atoms 2 & 3 / d. / Atoms 1 & 4
____ 31. Which two have the same mass?
a. / Atoms 1 & 2 / c. / Atoms 1 & 4b. / Atoms 2 & 4 / d. / Atoms 2 & 3
____ 32. Which is the smallest part of an element that retains all the properties of the element?
a. / proton / c. / electronb. / neutron / d. / atom
____ 33. Which type of nuclear decay releases the type of particle shown?
a. / alpha / c. / gammab. / beta / d. / proton
Atoms
Atom / Protons / Neutrons / Electrons / Mass Number
Sodium / 12 / 23
Chlorine / 17 / 17 / 35
____ 34. How many neutrons are in an atom of chlorine?
a. / 17 / c. / 34b. / 18 / d. / 35
____ 35. How many electrons are in an neutral atom of sodium?
a. / 22 / c. / 12b. / 11 / d. / 23
____ 36. What is the mass number of the atom shown?
a. / 11 / c. / 19b. / 18 / d. / 20
____ 37. Which element does this atom represent?
a. / potassium / c. / fluorineb. / neon / d. / sodium
____ 38. Which is the correct symbol for this atom?
a. / / c. /b. / / d. /
____ 39. Which is the correct symbol for the atom with 42 protons and 49 neutrons?
a. / / c. /b. / / d. /
____ 40. Which is the number of protons in ?
a. / 26 / c. / 56b. / 30 / d. / 82
____ 41. Which is the number of neutrons in ?
a. / 35 / c. / 80b. / 45 / d. / 115
____ 42. Which element has 14 protons?
a. / Nitrogen / c. / Aluminumb. / Silicon / d. / Sulfur
____ 43. Which scientist measured the charge on an electron as 1.602 x 10-19 Coulombs?
a. / Democritus / c. / Rutherfordb. / Millikan / d. / Bohr
____ 44. According to the modern concept of the atom, which are located in the nucleus of an atom?
a. / electrons and protons / c. / neutrons and electronsb. / protons only / d. / protons and neutrons
____ 45. An atom has 23 protons and 29 neutrons. Which is the correct chemical symbol for this atom?
a. / / c. /b. / / d. /
____ 46. An industrially important element contains 26 electrons and rusts in the presence of air and moisture. Identify the element.
a. / Aluminum / c. / Potassiumb. / Iron / d. / Sodium
____ 47. In the nuclear equation given below, calculate the mass number of the alpha particle.
a. / 0 / c. / 234b. / 4 / d. / 238
____ 48. Who was the man who lived from 460B.C.–370B.C. and was among the first to suggest the idea of atoms?
a. / Atomos / c. / Democritusb. / Dalton / d. / Thomson
____ 49. Which of the following was NOT among Democritus’s ideas?
a. / Matter consists of tiny particles called atoms.b. / Atoms are indivisible.
c. / Atoms retain their identity in a chemical reaction.
d. / Atoms are indestructible.
____ 50. Dalton's atomic theory included which idea?
a. / All atoms of all elements are the same size.b. / Atoms of different elements always combine in one-to-one ratios.
c. / Atoms of the same element are always identical.
d. / Individual atoms can be seen with a microscope.
____ 51. Which of the following is NOT a part of Dalton's atomic theory?
a. / All elements are composed of atoms.b. / Atoms are always in motion.
c. / Atoms of the same element are identical.
d. / Atoms that combine do so in simple whole-number ratios.
____ 52. Which of the following was originally a tenet of Dalton's atomic theory, but had to be revised about a century ago?
a. / Atoms are tiny indivisible particles.b. / Atoms of the same element are identical.
c. / Compounds are made by combining atoms.
d. / Atoms of different elements can combine with one another in simple whole number ratios.
____ 53. The comparison of the number of atoms in a copper coin the size of a penny with the number of people on Earth is made to illustrate which of the following?
a. / that atoms are indivisibleb. / that atoms are very small
c. / that atoms are very large
d. / that in a copper penny, there is one atom for every person on Earth
____ 54. The range in size of most atomic radii is approximately ____.
a. / 2 to 5 cm / c. / 5 10 m to 2 10 mb. / 2 to 5 nm / d. / 5 10 m to 2 10 m
____ 55. Dalton hypothesized that atoms are indivisible and that all atoms of an element are identical. It is now known that ____.
a. / all of Dalton's hypotheses are correctb. / atoms of an element can have different numbers of protons
c. / atoms are divisible
d. / all atoms of an element are not identical but they must all have the same mass
____ 56. Why did J. J. Thomson reason that electrons must be a part of the atoms of all elements?
a. / Cathode rays are negatively-charged particles.b. / Cathode rays can be deflected by magnets.
c. / An electron is 2000 times lighter than a hydrogen atom.
d. / Charge-to-mass ratio of electrons was the same, regardless of the gas used.
____ 57. Which of the following is true about subatomic particles?
a. / Electrons are negatively charged and are the heaviest subatomic particle.b. / Protons are positively charged and the lightest subatomic particle.
c. / Neutrons have no charge and are the lightest subatomic particle.
d. / The mass of a neutron nearly equals the mass of a proton.
____ 58. Who conducted experiments to determine the quantity of charge carried by an electron?
a. / Rutherford / c. / Daltonb. / Millikan / d. / Thomson
____ 59. What is the relative mass of an electron?
a. / 1/1840 the mass of a hydrogen atom / c. / 1/1840 the mass of a C-12 atomb. / 1/1840 the mass of a neutron + proton / d. / 1/1840 the mass of an alpha particle
____ 60. Which hypothesis led to the discovery of the proton?
a. / When a neutral hydrogen atom loses an electron, a positively-charged particle should remain.b. / A proton should be 1840 times heavier than an electron.
c. / Cathode rays should be attracted to a positively-charged plate.
d. / The nucleus of an atom should contain neutrons.
____ 61. Which of the following is correct concerning subatomic particles?
a. / The electron was discovered by Goldstein in 1886.b. / The neutron was discovered by Chadwick in 1932.
c. / The proton was discovered by Thomson in 1880.
d. / Cathode rays were found to be made of protons.
____ 62. All atoms are ____.
a. / positively charged, with the number of protons exceeding the number of electronsb. / negatively charged, with the number of electrons exceeding the number of protons
c. / neutral, with the number of protons equaling the number of electrons
d. / neutral, with the number of protons equaling the number of electrons, which is equal to the number of neutrons
____ 63. As a consequence of the discovery of the nucleus by Rutherford, which model of the atom is thought to be true?
a. / Protons, electrons, and neutrons are evenly distributed throughout the volume of the atom.b. / The nucleus is made of protons, electrons, and neutrons.
c. / Electrons are distributed around the nucleus and occupy almost all the volume of the atom.
d. / The nucleus is made of electrons and protons.
____ 64. The nucleus of an atom is ____.
a. / the central core and is composed of protons and neutronsb. / positively charged and has more protons than neutrons
c. / negatively charged and has a high density
d. / negatively charged and has a low density
____ 65. The atomic number of an element is the total number of which particles in the nucleus?
a. / neutrons / c. / electronsb. / protons / d. / protons and electrons
____ 66. What does the number 84 in the name krypton-84 represent?
a. / the atomic number / c. / the sum of the protons and electronsb. / the mass number / d. / twice the number of protons
____ 67. Isotopes of the same element have different ____.
a. / numbers of neutrons / c. / numbers of electronsb. / numbers of protons / d. / atomic numbers
____ 68. Isotopes of the same element have different ____.
a. / positions on the periodic table / c. / atomic numbersb. / chemical behavior / d. / mass numbers
____ 69. In which of the following sets is the symbol of the element, the number of protons, and the number of electrons given correctly?
a. / In, 49 protons, 49 electrons / c. / Cs, 55 protons, 132.9 electronsb. / Zn, 30 protons, 60 electrons / d. / F, 19 protons, 19 electrons
____ 70. Using the periodic table, determine the number of neutrons in O.
a. / 4 / c. / 16b. / 8 / d. / 24
____ 71. How many protons, electrons, and neutrons does an atom with atomic number 50 and mass number 125 contain?
a. / 50 protons, 50 electrons, 75 neutrons / c. / 120 neutrons, 50 protons, 75 electronsb. / 75 electrons, 50 protons, 50 neutrons / d. / 70 neutrons, 75 protons, 50 electrons
____ 72. Which of the following statements is NOT true?
a. / Atoms of the same element can have different masses.b. / Atoms of isotopes of an element have different numbers of protons.
c. / The nucleus of an atom has a positive charge.
d. / Atoms are mostly empty space.
____ 73. If E is the symbol for an element, which two of the following symbols represent isotopes of the same element?