Chemistry (CP) Study Guide
Second Trimester Exam March 15
The first trimester exam will ask 120 questions from chapters 6 thru 9. Questions will be based on this study guide.
Matching
Match each item with the correct statement below.
a. / electronegativity / f. / periodic lawb. / ionization energy / g. / cation
c. / atomic radius / h. / period
d. / metal / i. / group
e. / transition metal / j. / electrons
____ 1. horizontal row in the periodic table
____ 2. vertical column in the periodic table
____ 3. A repetition of properties occurs when elements are arranged in order of increasing atomic number.
____ 4. type of element that is a good conductor of heat and electric current
____ 5. type of element characterized by the presence of electrons in the d orbital
____ 6. one-half the distance between the nuclei of two atoms when the atoms are joined
____ 7. type of ion formed by Group 2A elements
____ 8. subatomic particles that are transferred to form positive and negative ions
____ 9. ability of an atom to attract electrons when the atom is in a compound
____ 10. energy required to remove an electron from an atom
Match each item with the correct statement below.
a. / halide ion / e. / valence electronb. / octet rule / f. / coordination number
c. / ionic bond / g. / metallic bond
d. / electron dot structure
____ 11. an electron in the highest occupied energy level of an atom
____ 12. Atoms react so as to acquire the stable electron structure of a noble gas.
____ 13. a depiction of valence electrons around the symbol of an element
____ 14. the force of attraction binding oppositely charged ions together
____ 15. the attraction of valence electrons for metal ions
____ 16. the number of ions of opposite charge surrounding each ion in a crystal
Match each item with the correct statement below.
a. / coordinate covalent bond / d. / single covalent bondb. / double covalent bond / e. / polar bond
c. / structural formula / f. / hydrogen bond
____ 17. a depiction of the arrangement of atoms in molecules and polyatomic ions
____ 18. a covalent bond in which two pairs of electrons are shared
____ 19. a covalent bond in which the shared electron pair comes from only one of the atoms
____ 20. a covalent bond between two atoms of significantly different electronegativities
____ 21. a type of bond that is very important in determining the properties of water and of important biological molecules such as proteins and DNA
Match each item with the correct statement below.
a. / network solid / e. / tetrahedral angleb. / bonding orbital / f. / VSEPR theory
c. / dipole interaction / g. / sigma bond
d. / bond dissociation energy
____ 22. energy needed to break a single bond between two covalently bonded atoms
____ 23. symmetrical bond along the axis between the two nuclei
____ 24. molecular orbital that can be occupied by two electrons of a covalent bond
____ 25. 109.5
____ 26. shapes adjust so valence-electron pairs are as far apart as possible
____ 27. attraction between polar molecules
____ 28. crystal in which all the atoms are covalently bonded to each other
Match each item with the correct statement below.
a. / monatomic ion / f. / cationb. / acid / g. / binary compound
c. / base / h. / anion
d. / law of definite proportions / i. / polyatomic ion
e. / law of multiple proportions
____ 29. atom or group of atoms having a positive charge
____ 30. tightly-bound group of atoms that behaves as a unit and carries a net charge
____ 31. compound composed of two different elements
____ 32. produces a hydrogen ion when dissolved in water
____ 33. produces a hydroxide ion when dissolved in water
____ 34. In any chemical compound, the masses of elements are always in the same proportion by mass.
____ 35. when two elements form more than one compound, the masses of one element that combine with the same mass of the other element are in the ratio of small, whole numbers
Multiple Choice
Identify the choice that best completes the statement or answers the question.
____ 36. What is another name for the representative elements?
a. / Group A elements / c. / Group C elementsb. / Group B elements / d. / transition elements
____ 37. What is another name for the transition metals?
a. / noble gases / c. / Group B elementsb. / Group A elements / d. / Group C elements
____ 38. Which of the following elements is in the same period as phosphorus?
a. / carbon / c. / nitrogenb. / magnesium / d. / oxygen
____ 39. Who arranged the elements according to atomic mass and used the arrangement to predict the properties of missing elements?
a. / Henry Moseley / c. / John Daltonb. / Antoine Lavoisier / d. / Dmitri Mendeleev
____ 40. Which of the following categories includes the majority of the elements?
a. / metalloids / c. / metalsb. / liquids / d. / nonmetals
____ 41. Of the elements Pt, V, Li, and Kr, which is a nonmetal?
a. / Pt / c. / Lib. / V / d. / Kr
____ 42. 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
____ 43. 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
____ 44. What element has the electron configuration 1s2s2p3s3p?
a. / nitrogen / c. / siliconb. / selenium / d. / silver
____ 45. Which of the following is true about the electron configurations of the noble gases?
a. / The highest occupied s and p sublevels are completely filled.b. / The highest occupied s and p sublevels are partially filled.
c. / The electrons with the highest energy are in a d sublevel.
d. / The electrons with the highest energy are in an f sublevel.
____ 46. Which of the following electron configurations is most likely to result in an element that is relatively inactive?
a. / a half-filled energy sublevelb. / a filled energy sublevel
c. / one empty and one filled energy sublevel
d. / a filled highest occupied principal energy level
____ 47. Which subatomic particle plays the greatest part in determining the properties of an element?
a. / proton / c. / neutronb. / electron / d. / none of the above
____ 48. Which of the following elements is a transition metal?
a. / cesium / c. / telluriumb. / copper / d. / tin
____ 49. Which of the following groupings contains only representative elements?
a. / Cu, Co, Cd / c. / Al, Mg, Lib. / Ni, Fe, Zn / d. / Hg, Cr, Ag
____ 50. Which of the following is true about the electron configurations of the representative elements?
a. / The highest occupied s and p sublevels are completely filled.b. / The highest occupied s and p sublevels are partially filled.
c. / The electrons with the highest energy are in a d sublevel.
d. / The electrons with the highest energy are in an f sublevel.
____ 51. What are the Group 1A and Group 7A elements examples of?
a. / representative elements / c. / noble gasesb. / transition elements / d. / nonmetallic elements
____ 52. Of the elements Fe, Hg, U, and Te, which is a representative element?
a. / Fe / c. / Ub. / Hg / d. / Te
____ 53. How does atomic radius change from top to bottom in a group in the periodic table?
a. / It tends to decrease. / c. / It first increases, then decreases.b. / It tends to increase. / d. / It first decreases, then increases.
____ 54. How does atomic radius change from left to right across a period in the periodic table?
a. / It tends to decrease. / c. / It first increases, then decreases.b. / It tends to increase. / d. / It first decreases, then increases.
____ 55. What causes the shielding effect to remain constant across a period?
a. / Electrons are added to the same principal energy level.b. / Electrons are added to different principal energy levels.
c. / The charge on the nucleus is constant.
d. / The atomic radius increases.
____ 56. Atomic size generally ____.
a. / increases as you move from left to right across a periodb. / decreases as you move from top to bottom within a group
c. / remains constant within a period
d. / decreases as you move from left to right across a period
____ 57. What element in the second period has the largest atomic radius?
a. / carbon / c. / potassiumb. / lithium / d. / neon
____ 58. Which of the following factors contributes to the increase in atomic size within a group in the periodic table as the atomic number increases?
a. / more shielding of the electrons by the highest occupied energy levelb. / an increase in size of the nucleus
c. / an increase in number of protons
d. / fewer electrons in the highest occupied energy level
____ 59. Which of the following elements has the smallest atomic radius?
a. / sulfur / c. / seleniumb. / chlorine / d. / bromine
____ 60. What is the charge of a cation?
a. / a positive chargeb. / no charge
c. / a negative charge
d. / The charge depends on the size of the nucleus.
____ 61. Which of the following statements is true about ions?
a. / Cations form when an atom gains electrons.b. / Cations form when an atom loses electrons.
c. / Anions form when an atom gains protons.
d. / Anions form when an atom loses protons.
____ 62. The metals in Groups 1A, 2A, and 3A ____.
a. / gain electrons when they form ions / c. / all have ions with a 1 chargeb. / all form ions with a negative charge / d. / lose electrons when they form ions
____ 63. Which of the following statements is NOT true about ions?
a. / Cations are positively charged ions.b. / Anions are common among nonmetals.
c. / Charges for ions are written as numbers followed by a plus or minus sign.
d. / When a cation forms, more electrons are transferred to it.
____ 64. Why is the second ionization energy greater than the first ionization energy?
a. / It is more difficult to remove a second electron from an atom.b. / The size of atoms increases down a group.
c. / The size of anions decreases across a period.
d. / The nuclear attraction from protons in the nucleus decreases.
____ 65. In which of the following sets are the charges given correctly for all the ions?
a. / Na, Mg, Al / c. / Rb, Ba, Pb. / K, Sr, O / d. / N, O, F
____ 66. In which of the following groups of ions are the charges all shown correctly?
a. / Li, O, S / c. / K, F, Mgb. / Ca, Al, Br / d. / Na, I, Rb
____ 67. What is the element with the lowest electronegativity value?
a. / cesium / c. / calciumb. / helium / d. / fluorine
____ 68. What is the element with the highest electronegativity value?
a. / cesium / c. / calciumb. / helium / d. / fluorine
____ 69. Which of the following elements has the smallest ionic radius?
a. / Li / c. / Ob. / K / d. / S
____ 70. What is the energy required to remove an electron from an atom in the gaseous state called?
a. / nuclear energy / c. / shielding energyb. / ionization energy / d. / electronegative energy
____ 71. For Group 2A metals, which electron is the most difficult to remove?
a. / the firstb. / the second
c. / the third
d. / All the electrons are equally difficult to remove.
____ 72. Which of the following factors contributes to the decrease in ionization energy within a group in the periodic table as the atomic number increases?
a. / increase in atomic sizeb. / increase in size of the nucleus
c. / increase in number of protons
d. / fewer electrons in the highest occupied energy level
____ 73. Which of the following elements has the smallest first ionization energy?
a. / sodium / c. / potassiumb. / calcium / d. / magnesium
____ 74. Which of the following elements has the lowest electronegativity?
a. / lithium / c. / bromineb. / carbon / d. / fluorine
____ 75. Which statement is true about electronegativity?
a. / Electronegativity is the ability of an anion to attract another anion.b. / Electronegativity generally increases as you move from top to bottom within a group.
c. / Electronegativity generally is higher for metals than for nonmetals.
d. / Electronegativity generally increases from left to right across a period.
____ 76. Which of the following decreases with increasing atomic number in Group 2A?
a. / shielding effect / c. / ionization energyb. / ionic size / d. / number of electrons
____ 77. Which of the following statements correctly compares the relative size of an ion to its neutral atom?