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Chemistry--Unit 10: Chemical Periodicity Test Review Vocab alkali metal alkaline earth metal electronegativity halogen inner transition metal ionization energy noble gas period periodic law representative element transition metal Know s, p, d, and f block and what other names these areas are called (transition, inner transition, representative elements, etc) (also alkali, alkaline earth, halogen, noble gas locations) vertical = groups (families), horizontal = periods, and how these are numbered where electrons are lost from/added to in an atom when ions are formed be able to tell period and group for each element (lots of easy points!) trends in atomic radii, ionization energy, electronegativity and reasons for these trends why electronegativity and ionization follow same trend recall jumps in multiple ionization energies how to determine # of electrons in outermost energy level relationship between size of ions and the atoms from which they form noble gas characteristics be able to read electron configs to I.D. an element review lab questions be able to predict oxidation #’s for representative elements Chemistry--Unit 10: Chemical Periodicity Test Review Answers to attached problems to try I. 1. groups 2. periods 3. atomic number 4. group 5. representative elements 6. noble or inert gases 7. transition metals 8. inner transition metals 9. p 10. partially filled 11. AT 12. NT 13. NT 14. AT 15. b 16. d 17. f 18. c 19. a 20. e 21. 3s1,3s2,3s23p1,3s23p2,3s23p3,3s23p4,3s23p5,3s23p6 22. N nonmetal gas, P nonmetal solid, As and Sb metalloid solid, Bi metal solid II. 1. decrease 2. increases 3. energy levels 4. charge 5. ionization 6. increases 7. electron 8. down a group 9. electronegativity 10. increases 11. AT 12. AT 13. ST 14. NT 15. c 16. e 17. a 18. d 19. b 20. a. Al b. S c. Br d. Na e. O 21. a. Ga b. O c. Cl d. Br Chemistry--Unit 10: Chemical Periodicity Test Review Problems to try I. Classification of the Elements Part A Completion The periodic table organized the elements into vertical __(1)__ and horizontal __(2)__ in order of increasing __(3)__. The table is constructed so that elements that have similar chemical properties are in the same __(4)__. The elements in Groups 1-2 and 13-18 are called the __(5)__. The __(6)__ make up group 18. The elements in Groups 2 and 13 are interrupted in periods 4 and 5 by the __(7)__, and in periods 6 and 7 by the __(8)__. The atoms of the noble gas elements have their outermost s and __(9)__ sublevels filled. The outermost s and p sublevels of the rest of the representative elements are __(10)__. 1. ______________________________ 6. ______________________________ 2. ______________________________ 7. ______________________________ 3. ______________________________ 8. ______________________________ 4. ______________________________ 9. ______________________________ 5. ______________________________ 10. ______________________________ Part B True-False--Use AT (always true), ST (sometimes true) or NT (never true) 11. ____________ The representative elements include the halogens. 12. ____________ Chlorine has the electron configuration 1s22s22p63s23p7. 13. ____________ The element in Group 14, period 3, is gallium. 14. ____________ There is a relationship between the electron configuration of elements and their chemical and physical properties. Part C Matching 15. _______ period a. an element in which the outermost s and p 16. _______ inner transition metal sublevels are filled 17. _______ representative element b. a horizontal row on the periodic table 18. _______ transition metal c. an element whose outermost s and nearby 19. _______ noble gas d sublevel generally contain electrons 20. _______ group d. an element whose outermost s and nearby f sublevel generally contain electrons e. a vertical column on the periodic table f. an element whose outermost s and p sublevels are only partially filled Part D Short Answer 21. List the outer electron configurations for the atoms in period 3 from left to right. 22. List the elements of group 15. Tell whether each is a solid, liquid, or gas, at room temperature; and whether it is a metal, non-metal, or metalloid. Chemistry--Unit 10: Chemical Periodicity Test Review II. Periodic Trends Part A Completion Atomic radii generally __(1)__ as you move from left to right in a period. Atomic size generally __(2)__ within a given group because there are more __(3)__occupied and an increased shielding effect, despite an increase in nuclear __(4)__. The energy required to remove an electron from an atom is known as the __(5)__ energy. This quantity generally __(6)__ as you move left to right across a period. The size of an ion depends on whether the atom from which it formed gained or lost an __(7)__. The ionic radius of anions and cations increases as you move __(8)__. The ability of a bonded atom to attract electrons to itself is known as __(9)__, and this quantity __(10)__ as you move from left to right across a period. 1. ______________________________ 6. ______________________________ 2. ______________________________ 7. ______________________________ 3. ______________________________ 8. ______________________________ 4. ______________________________ 9. ______________________________ 5. ______________________________ 10. ______________________________ Part B True-False--Use AT (always true), ST (sometimes true) or NT (never true) 11. ____________ The radius of an atom cannot be measured directly. 12. ____________ Removing one electron from an atom results in the formation of a positive ion with a +1 charge.. 13. ____________ Electronegativity is measured on the Paulings scale. 14. ____________ Atoms with high electronegativity tend to form positive ions. Part C Matching 15. _______ ionization energy a. negatively charged ion 16. _______ electronegativity b. when elements are arranged in order of 17. _______ anion increasing atomic number, there is a 18. _______ cation periodic pattern in their physical and 19. _______ periodic law chemical properties c. the energy required to overcome the attraction of the nuclear charge and remove an electron from an atom d. positively charged ions e. the tendency for the atoms of an element to attract electrons when they are chemically combined with another element Part D Short Answer 20. For the following pairs of atoms, tell which one of each pair has the largest ionic radius. a. Al, B__________________ d. Na, Al__________________ b. S, O___________________ e. O, F____________________ c. Br, Cl__________________ 21. Indicate which element of the following pairs has the greater electronegativity. a. calcium, gallium_______________ c. chlorine, sulfur_________________ b. lithium, oxygen________________ d. bromine, arsenic_______________