Chemistry G10 &G11 Name:
Chapter 5 and 6 Test Choose the Correct Answer 1. Mende endelleev eev pred prediicted cted that that the the gaps aps in his his peri period odiic table represented a. isotopes. b. rad radioac ioacttive ele elemen ments. ts. c. permanent gaps. d. undisco iscov vered red ele element ents. 2.The
person whose work led to a periodic table based on increasing atomic number was a. Moseley. b. Mendeleev. c. Rutherford. d. Cannizzaro. 3.The
periodic law states that the physical and chemical properties of elements of elements are periodic functions of their atomic a. masses. b. numbers. c. radii. d. structures. 4. Refer to a periodic table. In which period is calcium? a. Period 2 b. Period 4 c. Period 6 d. Period 8 5. Refer to a periodic table. In which group is calcium? a. Group 1 b. Group 2 c. Group 17 d. Group 18 element that has the electron configuration 1s2 2s2 2p6 3s2 3p5 is in which period? a. Period 2 b. Period 3 c. Period 5 d. Period 7 2 2 7.An element that has the electron configuration 1s 2s 2p6 3s2 3p5 is in which group? a. Group 2 6.An
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b. c. d.
8. table a. b. c. d. 9. a. b. c. d.
Group 5 Group 7 Group 17 Elements in the s- or p-blocks of the periodic are called alloys. main-group elements. metals. transition metals.
Elements in Group 18 have very low reactivity. good conductivity. very high reactivity. metallic character.
Nonmetallic elements in Group 17 that react with metals to form salts are a. alkali-metals. b. halogens. c. lanthanides. d. noble gases. 10.
11. The outer shell electron configuration of an alkaline-earth metal has a. one electron in the s orbital. b. two electrons in the s orbital. c. one electron in the p orbital. d. two electrons in the p orbital. 12. The alkali metals are found on Earth only in compounds because they a. have small atoms. b. are very reactive elements. c. are rare elements. d. are metallic elements. 13.
a. b. c. d.
14. a. b. c. d. 15.
table a. b. c.
To which group does hydrogen belong? Group 1 Group 2 Group 18 None of the above A metal is expected to be a(n) nonconductor. insulator. conductor. fluid at room temperature. An element found in Groups 3–12 of the periodic is classified as a(n) alkali metal. alloy. transition metal.
2
d.
actinide.
An element that has an outer shell electron configuration consisting of two electrons in the d orbital and one electron in the s orbital is in which group? a. Group 1 b. Group 2 Group 3 c. d. Group 5 16.
17. Lanthanide elements are found in the –block of the periodic table. a. s b. p c. d d. F Ionization energy is the energy required to remove from an atom of an element. a. the electron cloud b. all electrons c. one electron d. an ion 18.
19. Across a period in the periodic table, ionization energy generally a. decreases. b. decreases and then increases. c. increases. d. remains constant. 20. due to a. b. c. d.
The change in ionization energy down a group is increased electron shielding. decreased charge of the nucleus. increased neutrons in the nucleus. Both (a) and (b)
When determining the size of an atom by measuring the bond radius, the radius of an atom is a. equal to the distance between nuclei. b. one-half the distance between nuclei. c. twice the distance between nuclei. d. one-fourth the distance between nuclei. 21.
22. Across a period in the periodic table, atomic radii generally a. decrease. b. decrease, then increase. 3
c. d.
increase. increase, then decrease.
23. Down a group in the periodic table, atomic radii generally a. decrease. b. remain constant. c. increase. d. vary unpredictably An element with the lowest electro negativity would be found in of the periodic table. a. Group 1, Period 7 b. Group 3, Period 4 c. Group 5, Period 3 d. Group 17, Period 2 25. Refer to a periodic table and determine which element has the lowest electron affinity. a. Cl b. Se c. Cs d. Te 24.
As the atomic number of the metals of Group 1 increases, the ionic radius a. increases. b. decreases. c. remains the same. d. cannot be determined. 26.
27.
ionic) a. b. c. d.
An element with the smallest anionic (negativeradius would be found in of the periodic table. Group 1, Period 7 Group 3, Period 4 Group 5, Period 3 Group 17, Period 2
28. What is another name for the representative elements? a. Group A elements Group C elements b. c. Group B elements d. transition elements 29. Which of the following elements is in the same period as phosphorus? Carbon a. Nitrogen b. Magnesium c. Oxygen d. 30. ____.
Each period in the periodic table corresponds to
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a.
b. c.
d.
a principal energy level an orbital an energy sublevel a suborbital
31. Which of the following categories includes the majority of the elements? a. Metalloids b. Metals c. Liquids Nonmetals d.
32. Of the elements Pt, V, Li, and Kr, which is a nonmetal? a. Pt b. Li c. V Kr d. 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 b. Cs, 55 protons, 132.9 electrons c. Zn, 30 protons, 60 electrons d. F, 19 protons, 19 electrons 33.
34. The atomic number of an element is the total number of which particles in the nucleus? Neutrons a. Electrons b. Protons c. d. protons and electrons What element has the electron configuration 1s2 2s2 2p6 3s2 3p2? Nitrogen a. Silicon b. Selenium c. Silver d. 35.
Which of the following is true about the electron configurations of the noble gases? The highest occupied s and p sublevels are completely a. filled. b. The highest occupied s and p sublevels are partially filled. The electrons with the highest energy are in a d c. sublevel. d. The electrons with the highest energy are in an f sublevel. 36.
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Elements that are characterized by the filling of p orbitals are classified as ….. a. groups 3A through 8A b. inner transition metals c. transition metals d. groups 1A and 2A 37.
Which subatomic particle plays the greatest part in determining the properties of an element? a. proton b. neutron c. electron none of the above d. 38.
39. Which of the following elements is a transition metal? a. Cesium b. Tellurium c. Copper Tin d. 40. Which of the following groupings contains only representative elements? a. Cu, Co, Cd b. Al, Mg, Li Ni, Fe, Zn c. d. Hg, Cr, Ag 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. 41.
42. What are the Group 1A and Group 7A elements examples of? a. representative elements b. noble gases transition elements c. d. nonmetallic elements 43. From which of the following is it easiest to remove an electron? a. Mg b. Na c. Al d. S
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44. a. b. c. d.
Which of the following elements is least metallic? oxygen fluorine sulfur chlorine
45. a. b. c. d.
Low ionization energy is characteristic of: metals non-metals metalloids liquids
Complete the Following Statements The chemical properties of atoms, ions, and molecules 46. are related to the arrangement of the___________________________within them. J.J. Thomson’s model is referred to as 47. the______________________ model. The ways in which electrons are arranged around the 48. nuclei of atoms are called_____________________________ To occupy the same orbital, two electrons must 49. have___________________ spins. Hund’s rule states that the electrons pair up only after 50. each orbital in a sublevel is occupied by_____________________ The region in which an electron is most likely to be 51. found is called a(an)______________________ An atom in which an electron has moved to a higher 52. energy level is in a(an) __________________________state.
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A neutron has approximately the same mass as 53. a___________________ In the quantum mechanical model the regions where 54. electrons are likely to be found are called ____________________ In general, the higher the electron is on the energy ladder, the __________ it is from the nucleus. 55.
Short Answer Questions Rank the following elements by increasing atomic 56. radius: sulfur, oxygen, neon, aluminum
10. Rank the following elements from high to low electro negativity: carbon, aluminum, oxygen, potassium. 57.
11. Why does Chlorine have higher ionization energy than Sulfur? 58.
59.
Why do the noble gases lack electro negativity values?
Which of the elements of the fourth period has the 60. smallest atomic radius? Name two elements that have properties similar to 61. those of the element potassium. What is the common characteristic of the electron 62. configurations of the elements Ne and Ar? In which group would you find them? Predict the size of the astatine (At) atom compared to 63. that of tellurium (Te). Explain your prediction
3. Would you expect a Cl -1 ion to be larger or smaller than an Mg+2 ion? Explain. 64.
Use the following diagram to solve questions 65 - 72
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65.
66. 67. 68.
Which of the atoms has the highest Ionization energy? Which of the atoms has the smallest radius? The outer shell is the first energy level Which of the atoms has the easiest electron to be
removed?
69.
There is only one electron in the outer shell and it is
being held by only 3 protons.
70. 71.
Which of the atoms is the largest? Assuming the atoms are neutral, write the element
names above the diagram.
72.
Rank the diagrams from lowest to highest electro
negativity.
Write the electron configurations of the following elements: (2 marks each) 73.
chromium
74.
iodine
75.
potassium
76.
bismuth
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