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Chapter 6 Review Name _______________________ Period _____ Know the history/development of the periodic table. 1. Who first published the classification of the elements that is the basis of our periodic table today? Mendeleev 2. By what property did Mendeleev arrange the elements? By Atomic Mass 3. By what property did Moseley suggest the periodic table be arranged? By Atomic number 4. What is the periodic law? The Periodic Table is arranged by increasing atomic number, and thus shows mutliple repeating patterns are evident without fail Know the layout/arrangement of the periodic table. 5. What is a period? How many are there in the periodic table? The rows of the Periodic Table, 7 6. What is a group? How many are there in the periodic table? The columns or families of the PT, 18 (8 representative 7. State the number of valence electrons in an atom of: a. Sulfur ____6__ b. Calcium ___2___ c. Chlorine ____7__ d. Arsenic _____5_ 8. Write the name of the element that is found in the following periods and groups: a. Period 2, Group 2A Beryllium__________ b. Period 4, Group 8A ____Krypton_________________ c. Period 6, Group 4A _________Lead____________ 9. Which of the following pairs of elements belong to the same period? a. Na and Cl b. Na and Li c. Na and Cu d. Na and Ne 10. Which of the following pairs of elements belong to the same group? a. H and He b. Li and Be c. C and Pb d. Ga and Ge Chapter 6 Review Name _______________________ Period _____ 11. How does an element’s period number relate to the number of the energy levels of its valence electrons? Representative element – equal to Transition Metals- one more (n-1) 12. Would you expect Strontium to be, chemically, more similar to calcium or rubidium? Why? Calcium 13. What are the Group 1A elements called? Akali metals 14. What are the Group 2A elements called? Akaline earth metals 15. What are the Group 7A elements called? Halogens 16. What are the Group 8A elements called? Noble gases 17. Why do all the members of a group have similar properties? They contain the same number of valence electrons 18. Where, generally, are the metals located on the periodic table? To the left of the staircase 19. Where, generally, are the nonmetals located on the periodic table? To the right of the staircase 20. List some properties of metals. High luster, ductile, malleable, good conductor of heat and electricity 21. List some properties of nonmetals. Poor conductor of heat and electricity, brittle EXCEPT carbon 22. What kinds of properties do metalloids have? Contain properties of both metals and nonmetals depending on the conditions Know the trend for atomic radius. 23. Within a group, what happens to the atomic radius as you go down a group? Why? The atomic radius increases because, as you go down a group the energy level increases 24. Within a period, what happens to the atomic radius? Why? Chapter 6 Review Name _______________________ Period _____ The atomic radius decreases, as you go across a period the valence electrons increase, causing a larger interaction with the nucleus 25. What is the shielding affect? The electrons that are in between the valence shell and the nucleus shield Know the trend for ionic radius. 26. What is the charge of a cation? Increases across the period, same for each group 27. How are neutral atoms made into cations? They lose electrons in their outter shell 28. What is the charge of an anion? Negative, increases across a period and reamin the same going down 29. How are neutral atoms made into anions? They gain electrons to fill their valence shell 30. Metals usually form what type of ions? Cations 31. Nonmetals usually form what type of ions? Anions 32. When an atom becomes an anion, what happens to its radius? Why? With the addition of an electron the repulsion between the electrons increases increasing the size of the ion. 33. When an atom becomes a cation, what happens to its radius? Why? As an atom loses an electron the repulsion decreases 34. For each of the following pairs, circle the atom or ion having the larger radius. a. S or O c. Na+1 or Na e. S-2 or S b. Ca or Ca+2 d. Na or K f. F or F-1 Know the trend for ionization energy. 35. What is ionization energy? The energy required to knock off an electron 36. Which is higher: 1st Ionization energy or 2nd Ionization energy? 37. What is the general trend of ionization energy as you go across a period? Why? Chapter 6 Review Name _______________________ Period _____ Increases, as you go across a period the number of valence electrons increase the more “resistant” the atom is to give up an electron. 38. What is the general trend of ionization energy as you go down a group? Why? Decreases as you go down a group. Shielding is increased the nucleus has less effect on valence electrons Know the trend for electronegativity. 39. What is electronegativity? The affinity for an atom to “pick up” an electron 40. What is the general trend of electronegativity as you go down a group? Decreases 41. What is the general trend of electronegativity as you go across a period? Increases