7. What is the likeliest oxidation number of an element located in Period 3 and Group 16? a. +2 b. +3 c. -3 d The amount of energy required to

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1 1. Which of the following is the most important factor in determining the properties of an element? a. Atomic mass b. Atomic radius c. Periodic table position d. Electron configuration 2. Similar properties for chemical elements recur at certain intervals of atomic number. Therefore, these properties are referred to as a. Intensive b. Periodic c. Extensive d. Intermittent 3. As the principle quantum number increases, the size of the electron cloud 4. As you look across a period from left to right in the periodic table, the size of the atoms 5. In which of the following pairs of particles does the second particle listed have the smaller radius? a. Ni, K b. Na, Cs c. Cl, Cl - d. Li, Li + 6. Which of the following electron configurations represents the particle that is most stable chemically? a. 1s 2 2s 2 2p 6 3s 2 3p 5 b. 1s 2 2s 2 2p 3 c. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 10 4p 6 d. 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 3d 5

2 7. What is the likeliest oxidation number of an element located in Period 3 and Group 16? a. +2 b. +3 c. -3 d The amount of energy required to remove the most loosely held electron from an atom is the a. First ionization energy b. Energy of formation c. Bonding energy d. Activation energy 9. Phosphorus has a first ionization energy of kilojoules per mole. Which of the following elements has a first ionization energy less than that of phosphorus? a. F b. Ga c. N d. Cl 10. Which of the following is not a factor that affects ionization energy? a. Nuclear charge b. Shielding effect c. Electron spin d. Atomic radius

3 11. As you move through a period from metals to nonmetals, the first ionization energy 12. For each subsequent electron removed from an atom, the ionization energy required 13. A measure of the attraction of an atom for additional electrons is referred to as a. Multiple ionization energies b. Electronegativity c. Electron affinity d. Combining capacity 14. In general, as electron affinity increases, ionization energy a. increases b. decreases c. remains constant d. varies at random 15. As you move down through a group, electron affinity 16. If two elements have similar chemical properties, you would expect them to have a. Similar atomic radii b. The same number of energy levels c. The same number of outer electrons d. Similar atomic masses 17. Which of the following has the greatest impact on the atomic radius as you move down through a group? a. Increased principle quantum number b. Increased nuclear charge c. Increased atomic mass d. Decreased electron shielding effect 18. Which of the following describes the size of the elements ions as you move from left to right across the periodic table? d. Decreases, then increases 19. In which of the following pairs of particles does the second particle listed have the larger radius?

4 a. Rb, Y b. Br, F c. S -2, S d. Ga -3, As Elements in the same group or family in the periodic table have which of the following characteristics in common? a. The principle quantum number of the outer energy level b. The number of isotopes that exist c. The atomic radius d. The number of electrons in the outer energy level

5 21. Which of the following occurs when an element in Group 2 attains a stable electron configuration? a. It gains 2 electrons b. It loses 2 electrons c. It gains 6 electrons d. It gains 8 electrons 22. What is the likeliest oxidation number of an element in Period 4 and Group 13? a. +3 b. -3 c. _4 d The first ionization energy of Ca is kilojoules per mole. Which of the following elements has a first ionization energy greater than that of Ca? a. K b. Rb c. Sr d. Mg 24. If an element has a high ionization energy, its electron affinity is a. High b. Low c. Zero d. Completely unpredictable 25. The electron configuration of K + is most similar to that of a. K b. Na + c. Ar d. Ca The radii of the atoms become smaller from sodium to chlorine across period 3. This decrease is primarily a result of a. The shielding effect b. Increased nuclear charge c. Increased number of electrons d. Decreased metallic character

6 Look at a periodic table to answer the following questions: 1. What is the name of group 1? 2. What is the name of group 2? 3. What is the name of group 17? 4. What is the name of group 18? 5. What is the name for the d block? 6. What is the name for the s & p block? 7. What is the name for the 2 periods at the bottom of the periodic table? Answer the following questions with these terms: Noble gases Halogens Alkali metals Transition metals Alkaline-earth metals 8. The have a single electron in the highest energy level? 9. The achieve the electron configurations of noble gases by losing two electrons. 10. The vary in the number of electrons in the highest energy level. 11. The achieve the electron configurations of noble gases by gaining one electron. 12. The have full s and p orbitals in the highest occupied energy levels. 13. The are stable and unreactive. 14. The are highly reactive and readily form salts with metals. 15. The are metals that are more reactive than the transition elements but less reactive than the alkali metals.

7 3 Li Lithium Na Sodium Be Beryllium Mg Magnesium Which element will react more readily with chlorine: sodium or magnesium? Why? 17. Which element is more like lithium in terms of properties: sodium or beryllium? Why? 18. Which element has more electrons in its highest occupied energy level: sodium or magnesium? 19. Which element has a lower melting point: lithium or beryllium? 20. Which element is closer to achieving noble gas configuration: magnesium or lithium? 21. Which element reacts more readily with fluorine: lithium or beryllium? Why?

8 For each choice of words, circle the one that best completes the sentence. 1. The shielding effect increases with increasing atomic number within a (period, group). 2. In any (period, group), the number of electrons between the nucleus and the outer energy level is the same. 3. Within a group, the nucleus has a stronger ability to pull on the outermost electrons in elements of (high, low) atomic number. 4. The more (positive, negative) the value of electron affinity is, the more easily the atom can take on an extra electron. 5. From left to right across a period, electron affinity values become more (positive, negative). 6. The halogens have the (most, least) negative electron affinity values. 7. The (electronegativity, electron affinity) of an atom is the tendency of an atom to attract electrons to itself when it is chemically combined with another element. 8. The (noble gases, halogens) are the most electronegative group. Use the following choices: a. increases b. decreases c. remains constant d. there is no pattern 9. Moving from top to bottom in a group, atomic radius tends to. 10. Moving from top to bottom in a group, shielding effect tends to. 11. Moving from top to bottom in a group, electronegativity tends to. 12. Moving from top to bottom in a group, electron affinity tends to. 13. Moving from top to bottom in a group, ionization energy tends to. 14. Moving from left to right across a period, atomic radius tends to. 15. Moving from left to right across a period, shielding effect tends to. 16. Moving from left to right across a period, electronegativity tends to. 17. Moving from left to right across a period, electron affinity tends to. 18. Moving from left to right across a period, ionization energy tends to. 19. Which atom has the more negative value for electron affinity, sodium or chlorine? 20. Which atom is more electronegative, fluorine or lithium? 21. Which atom has a greater ionization energy, nitrogen or bismuth? 22. Which atom exerts a stronger pull on its outermost electrons: calcium or arsenic? 23. Which atom has a larger atomic radius, fluorine or barium? 24. Which atom has a greater nuclear charge, boron or selenium?