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Name: ___________________________ Per: _____ Date: ____________ Unit 5 Redemption Packet: The Periodic Table Use the information in your notes and text book, pages 174 - 194 to answer the following questions. If you missed any notes, you will find them at www.starkchemistry.weebly.com. 1. Mendeleev arranged the elements in his periodic table by increasing _______________ ________________. 2. Why did Mendeleev leave spaces in his periodic table? _________________________________________________________________________ 3. The modern periodic table is arranged by increasing ________________ _________________. 4. Elements become more / less metallic as you go across a period on the periodic table. 5. Elements in the same group / period have similar chemical properties. 6. Which element listed below should have chemical properties similar to fluorine (F)? A. Li C. Br B. Si D. Ne 7. Identify each property below as more characteristic of a metal or a nonmetal. a) A gas at room temperature ________________ b) Brittle ________________ c) Malleable ________________ d) Poor conductor of heat ________________ e) Shiny ________________ 8. Identify each element as a metal, metalloid, or nonmetal. a) Fluorine ___________________ b) Germanium ___________________ c) Zinc ___________________ d) Phosphorus ___________________ e) Lithium ___________________ 9. Which of the following is NOT a transition metal? a) Magnesium b) Titanium c) Chromium d) Mercury 1 10. Elements can be divided into metals, nonmetals, and metalloids. Distinguish between them. Metals: ________________________________________________________________ Nonmetals: _______________________________________________________________ Metalloids: ________________________________________________________________ 11. The following families are located in which group(s) on the periodic table? a) Alkali metals _____________ b) Alkaline Earth metals _____________ c) Halogens _____________ d) Noble gases _____________ e) Transition Metals _____________ 12. Label as alkali metal, alkaline earth metal, halogen, noble gas, or transition metal. a) Ca ________________________________ b) Cu ________________________________ c) Br ________________________________ d) Na ________________________________ e) He ________________________________ f) ________________________________ Fe 13. How many valence electrons do the following elements contain? a) K ________ b) Cl ________ c) Ar ________ d) Si ________ e) Ga ________ f) ________ Cr 14. Name the element that matches the following description. a) Has 5 electrons in the 3rd energy level. _____________________ 2 5 b) Has an electron configuration that ends with 4s 4p _____________________ c) Group 6A element in period 4. _____________________ d) Alkaline earth metal in period 5 _____________________ 2 15. Which noble gas does not have 8 valence electrons? _______________ 16. How is the atomic radius of an atom determined? _________________________________ ________________________________________________________________________ 17. a) How does atomic radius change across a period? ________________________ b) How does atomic radius change down a group? _______________________ 18. Circle the element in each pair that has atoms with a larger atomic radius. a) Sodium, lithium b) Strontium, magnesium c) Carbon, germanium d) Selenium, oxygen 19. Order the elements S, Cl, and F in terms of increasing atomic radii. ______________ 20. Define ionization energy. _____________________________________________________ _________________________________________________________________________ 21. a) How does IE change across a period? _____________________ b) How does IE change down a group? _____________________ 22. Circle the element in each pair that has the greater ionization energy. a) Lithium, boron b) Magnesium, strontium c) Cesium, aluminum 23. Arrange the following groups of elements in order of increasing ionization energy. a) Be, Mg, Sr ______________________ b) Bi, Cs, Ba ______________________ c) Na, Al, S ______________________ 24. Metal atoms tend to lose / gain electrons and form positive / negative ions. (circle) 25. Nonmetal atoms tend to lose / gain electrons to form positive / negative ions. 26. What is a cation? ____________________________________ 27. What is an anion? ____________________________________ 28. Circle the particle that has the larger radius in each atom / ion pair. a) Na, Na+ c) I, I b) S, S2 d) Al, Al3+ 29. What is electronegativity? ____________________________________________________ _________________________________________________________________________ 3 30. How does EN change across a period? __________________________________ 31. How does EN change down a group? _________________________________ 32. Circle the element in each pair that has a higher electronegativity value. a) Cl, F c) Mg, Ne b) C, N d) As, Ca 33. When the elements in each pair are chemically combined, which element in each pair has a greater attraction for electrons? a) Ca or O c) H or O b) O or F d) K or S 34. For which of these properties does lithium have a larger value than potassium? A. First ionization energy B. Atomic radius C. Electronegativity D. Ionic radius 35. Which of the following properties generally increases as we go from the lower left to the upper right of the periodic table? A. Atomic number B. Number of electron shells C. Atomic size D. Ionization energy E. None of the above 36. a) The overall reactivity of metals increases / decreases down a group. b) The most reactive metal is ___________________. 37. a) The overall reactivity of nonmetals increases / decreases down a group. b) The most reactive nonmetal is __________________. 4