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Periodic Table Review

Periodic Table Review . Place each of the following groups of elements in order of DECREASING atomic radius. Li, Rb , K, Na . Rb , K, Na, Li. Place each of the following groups of elements in order of DECREASING atomic radius. Mg, Cl , Na, P. Na, Mg, P, Cl.

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Periodic Table Review

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  1. Periodic Table Review

  2. Place each of the following groups of elements in order of DECREASING atomic radius.Li, Rb, K, Na • Rb, K, Na, Li

  3. Place each of the following groups of elements in order of DECREASING atomic radius.Mg, Cl, Na, P • Na, Mg, P, Cl

  4. Place each of the following groups of elements in order of DECREASING atomic radius.Li, O, C, F, N • Li, C, N, O, F

  5. Define “first ionization energy”. • Energy required to remove an electron from an atom

  6. State the period trend (moving left to right across the periods) for first ionization energy. • INCREASES

  7. State the group trend (moving top to bottom down the groups) for first ionization energy. • DECREASES

  8. Arrange the following elements in order of decreasingfirst ionization energy: Li, O, C, K, Ne, F • Ne, F, O, C, Li, K

  9. Arrange the following elements in order of decreasingfirst ionization energy: Li, B, Rb, F, C • F, C, B, Li, Rb

  10. Arrange the following elements in order of decreasingfirst ionization energy: Mg, Ba, Be • Be, Mg, Ba

  11. Define “electronegativity”. • Measure of the ability of an atom in a chemical compound to attract electrons

  12. State the period trend (moving left to right across the periods) for electronegativity. • INCREASES

  13. State the group trend (moving top to bottom down the groups) for electronegativity. • DECREASES

  14. Place each of the following groups of elements in order of DECREASING electronegativity.Po, Se, O • O, Se, Po

  15. Place each of the following groups of elements in order of DECREASING electronegativity.Ga, Br, Ra, Ca • Br, Ga, Ca, Ra

  16. How did HenryMoseley arrange elements on the Periodic Table? • Increasing atomic NUMBER

  17. What is the ending of all monatomic anions? • ide

  18. State the period trend (moving left to right across the periods) for atomic radius. • DECREASES

  19. where you would find elements with similar properties? Group or Period • GROUP

  20. List 4 properties of metals. • Luster • Good conductors of electricity • Ductile • Malleable • High Melting points • Solid, except Hg is a liquid • Lose electrons

  21. What is the atomic number of nickel? • 28

  22. What is the difference between a group and a period? List the number of groups and period. • Group = columns (#1-18) • Periods = rows (#1-7)

  23. What element is in group 2 and period 2? • Be

  24. what group of elements are considered the most stable? • Noble Gases

  25. How are the elements arranged on the Periodic Table today? • Increasing atomic NUMBER

  26. What is the atomic mass of lithium? • 6.941amu

  27. What element is in group 7 and period 4? • Mn

  28. What is the atomic number of bromine? • 35

  29. Group 17 elements are called? • Halogens

  30. Define “atomic radius”. • Half the distance between the nuclei of identical atoms joined in a molecule

  31. State the group trend (moving top to bottom down the groups) for atomic radius. • INCREASES

  32. What is a metalloid? • Element that has properties of BOTH metals and nonmetals

  33. As you go from left to right across the periodic table, the elements go from (metals / nonmetals) to (metals / nonmetals). • Metals; nonmetals

  34. The most active element in Group 17 is? • Fluorine (F)

  35. What is the difference between anions and cations? Explain. • Anion = negative ion b/c electron(s) were GAINED • Cation= positive ion b/c electron(s) were LOST

  36. Group 18 elements are called? Why? • Noble Gases; b/c the contain 8 electrons in their outer energy level which gives them a stable electron configuration

  37. A positive ion is (larger / smaller) than its parent atom. Why? • SMALLER; b/c the atom LOST electron(s)

  38. The majority of elements in the periodic table are (metals / nonmetals). • Metals

  39. List 4 properties of nonmetals. • No Luster • Not good conductors of electricity • Not Ductile • Not Malleable • Low Melting points • Gain electrons

  40. Suppose magnesiumformed an ion. How many electrons and protons does a calcium ion have? • Mg+2 (lost 2 e-) • 12protons & 10electrons

  41. What is the difference between a monatomic ion and a polyatomic ion? • Monatomic = ion formed from a single atom • Polyatomic = a group of bonded atoms with a charge

  42. A negative ion is (larger / smaller) than its parent atom. Why? • LARGER; b/c the atom GAINED electron(s)

  43. An element with both metallic and nonmetallic properties is called a __________ • Metalloid

  44. Suppose nitrogenformed an ion. -3 10 • What is the charge of the N ion? _________ • How many electrons does an Nion have?________ • How many protons does an N ion have?_________ • Write the name for the N ion.__________ 7 Nitride

  45. Place the ionic charges for the following groups on the Periodic Table: group 1, group 2, group 3-12, group 13, group 14, group 15, group 16, group 17 and group 18 +1 0 +2 +3 +4 -3 -2 Mostly+2 -1

  46. Compounds that contain elements from group 17 are commonly called? • Salts

  47. Elements of Group 3-12 are called? • Transition Metals

  48. The noble gases contain _______ electrons in their outer energy level. • 8

  49. Metals are usually solids under ordinary conditions. List one exception. • Hg (mercury) is a liquid

  50. Elements in the periodic table are arranged according to their ___________ • Increasing atomic number

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