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Unit 3 Periodic Trends Practice Problems

Unit 3 Periodic Trends Practice Problems. Station 1 Atomic Size: Put the following elements in order of INCREASING atomic size :. 1. P, Cs, Sn , F, Sr , Tl 2. Ca , Rb , K, O, Al, As *3. Ga, Fr, Br, Si, Na, N *4. Po , Sn, Fr, Rb, Cl, Li **5 . Ra , F, Al, Ne, H, He,

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Unit 3 Periodic Trends Practice Problems

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  1. Unit 3 Periodic TrendsPractice Problems

  2. Station 1Atomic Size: Put the following elements in order of INCREASING atomic size: 1. P, Cs, Sn, F, Sr, Tl 2.Ca, Rb, K, O, Al, As *3. Ga, Fr, Br, Si, Na, N *4. Po, Sn, Fr, Rb, Cl, Li **5. Ra, F, Al, Ne, H, He, **6. Ar, Ca, Mg, O, N, At

  3. Station 2Atomic Size: Put the following elements in order of DECREASINGatomic size: 7. Po, Sn, Fr, Rb, Cl, Li 8. Ra, F, Al, Ne, H, He, *9. Ar, Ca, Mg, O, N, At *10. B, P, I, Sb, Be, Pb

  4. Station 3Ions: Predict which ions the following elements will produce: • Nitrogen • Oxygen • Fluorine • Lithium • Potassium • Barium • Chlorine • Argon • Carbon • Sulfur

  5. Station 4*Ions: Predict which ions the following elements will produce: • Beryllium • Boron • Sulfur • Iodine • Astatine • Sodium • Hydrogen • Helium • Aluminium • Phosphorus

  6. Station 5Ionic Size: Put the following ions in order of INCREASINGionic size: • 10. Si, Si+2, Si+4, Si-4 • Mn, Mn+2, Mn+3, Mn+4, Mn+7 • N-3, N, P-3, C-4, O-2 • Po+2, Sn+2, Fr+, Rb+, Cl-, Li+

  7. Station 6 *Ionic Size: Put the following ions in order of INCREASINGionic size: • Sb, Sb+5, Sb+3, Sb-3 • V, V+2, V+3, V+4, V+5 • B+3, P-3, I-, Sb-3, Be+2, Pb+4 • N-3, As-3, Kr, Fr+, S-2, O-2

  8. Station 7Electronegativity: Put the following elements in order of INCREASINGelectronegativity: • P, Cs, Sn, F, Sr, Tl • Ca, Rb, K, O, Al, As • *Ra, F, Al, Ne, H, He • *Ar, Ca, Mg, O, N, At

  9. Station 8Electronegativity:Put the following elements in order of DECREASINGelectronegativity • Ga, Fr, Br, Si, Na, N • Po, Sn, Fr, Rb, Cl, Li • *B, P, I, Sb, Be, Pb • *N, As, Kr, Fr, S, O

  10. Station 9Ionization Energy: Put the following elements in order of INCREASINGfirst ionization energy: • P, Cs, Sn, F, Sr, Tl • Ca, Rb, K, O, Al, As • *Ga, Fr, Br, Si, Na, N • *Po, Sn, Fr, Rb, Cl, Li

  11. Station 10*Ionization Energy: Put the following elements in order of INCREASINGfirst ionization energy: • Ra, F, Al, Ne, H, He • Ar, Ca, Mg, O, N, At • B, P, I, Sb, Be, Pb • N, As, Kr, Fr, S, O

  12. Station 11Metallic Character: Put the following elements in order of INCREASINGmetallic character: • P, Cs, Sn, F, Sr, Tl • Ca, Rb, K, O, Al, As • *Ga, Fr, Br, Si, Na, N • *Po, Sn, Fr, Rb, Cl, Li

  13. Station 11*Metallic Character: Put the following elements in order of INCREASINGmetallic character: • Ra, F, Al, Ne, H, He • Ar, Ca, Mg, O, N, At • B, P, I, Sb, Be, Pb • N, As, Kr, Fr, S, O

  14. Station 12Free Response Questions  Type 1 1. Consider the element Cesium. • What is the most common ion that Cesium forms? • Which is larger neutral Cesium or the Cesium Ion? Why? Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Describe Cesium’s electronegativity. • Describe Cesium’s metallic character.

  15. Station 12Free Response Questions Type 1 2. Consider the element Barium. • Describe Barium’s atomic radius. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. •  Describe Barium’s’s first ionization energy. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. •  Describe Barium’s’s electronegativity. •  Describe Barium’s’s metallic character.

  16. Station 13*Free Response Questions Type 1 Both Partners Work Together! Consider the element Rubidium. • Describe Rubidium’s atomic radius. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Describe Rubidium’s first ionization energy. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Describe Rubidium’s electronegativity. • Describe Rubidium’s metallic character.

  17. Station 14Free Response Questions Type 1 3. Consider Nitrogen • What is the most common ion that Nitrogen forms? • Which is larger, neutral Nitrogen or the ion named in part 1? Why? Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Describe Nitrogen’s electronegativity. • Describe Nitrogen’s metallic character.

  18. Station 14Free Response Questions Type 1 4. Consider Phosphorus • Describe Phosphorus’s atomic radius. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Describe Phosphorus’s first ionization energy. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Describe Phosphorus’s electronegativity. • Describe Phosphorus’s metallic character.

  19. Station 15*Free Response Questions Type 1 Both Partners Work Together! Consider Carbon. • Describe Carbon’s atomic radius. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Describe Carbon’s first ionization energy. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Describe Carbon’s electronegativity. • Describe Carbon’s metallic character.

  20. Station 16Free Response Questions Type 2 1. Compare Cesium and Barium • Which element has the larger atomic radius? • Cesium and Barium both commonly form Cations. Which Cation will be smaller? • Samples of Cesium and Barium are both put in beakers of water and left to react. Based on electronegativity, which will react more readily? Explain your answer. • How does Cesium’s first ionization energy compare to Bariums? How might this difference affect your answer in part c?

  21. Station 16Free Response Questions Type 2 2. Compare Rubidium and Barium • Which element has the larger atomic radius? • Rubidium and Barium both commonly form Cations. Which Cation will be smaller? • Samples of Rubidium and Barium are both put in beakers of water and left to react. Based on electronegativity, which will react more readily? Explain your answer. • How does Rubidium’s first ionization energy compare to Bariums? How might this difference affect your answer in part c?

  22. Station 17*Free Response Questions Type 2 Both Partners Work Together! Compare Cesium and Rubidium • Which element has the larger atomic radius? • Cesium and Rubidium both commonly form Cations. Which Cation will be smaller? • Samples of Cesium and Rubidium are both put in beakers of water and left to react. Based on electronegativity, which will react more readily? Explain your answer. • How does Cesium’s first ionization energy compare to Rubidium? How might this difference affect your answer in part c?

  23. Station 18Free Response Questions Type 2 3. Compare Nitrogen and Phosphorus • Which element has the larger atomic radius?  • Nitrogen and Phosphorus both commonly form Anions. Which Anion will be smaller? • Samples of Nitrogen and Phosphorus are both put in beakers of water and left to react. Based on electronegativity, which will react more readily? Explain your answer. • How does Nitrogen’s first ionization energy compare to Phosphorus’? How might this difference affect your answer in part c?

  24. Station 18Free Response Questions Type 2 4. Compare Nitrogen and Carbon • Which element has the larger atomic radius? • Nitrogen and Carbon both commonly form Anions. Which Anion will be smaller? • Samples of Nitrogen and Carbon are both put in beakers of water and left to react. Based on electronegativity, which will react more readily? Explain your answer. • How does Nitrogen’s first ionization energy compare to Carbon’s? How might this difference affect your answer in part c?

  25. Station 19*Free Response Questions Type 2 Both Partners Work Together! Compare Phosphorus and Carbon • Which element has the larger atomic radius? • Phosphorus and Carbon both commonly form Anions. Which Anion will be smaller? • Samples of Phosphorus and Carbon are both put in beakers of water and left to react. Based on electronegativity, which will react more readily? Explain your answer. • How does Phosphorus’s first ionization energy compare to Carbon’s? How might this difference affect your answer in part c?

  26. Station 20Free Response Questions Type 3 In one or two well-written sentences, explain each of the following observations using principles of atomic structure and/or bonding. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Potassium has a lower first-ionization energy than Sodium. • The ionic radius of P3 ̄ is larger than that of S2 ̄ . • A Scandium atom is larger than a Nickel atom. • An atom of Fluorine is more electronegative than an atom of Nitrogen.

  27. Station 21*Free Response Questions Type 3 In one or two well-written sentences, explain each of the following observations using principles of atomic structure and/or bonding. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Calcium has a lower first-ionization energy than Magnesium. • The ionic radius of Al 3+ is smaller than that of Mg2+ . • A Titanium atom is larger than a Germanium atom. • An atom of Arsenic has lower metallic character than an atom of Gallium

  28. Free Response Questions Type 4 The above table shows the first three ionization energies for atoms of four elements from the SECOND PERIOD of the periodic table. The elements are numbered randomly. Use the information in the table to answer the following questions in one or two well-written sentences. Justify your response using one or more of these terms: effective nuclear charge, shielding, Coulomb’s law, atomic size, principle quantum number and/or energy level. • Which element is most METALLIC in character? • Identify element 3. • Write the complete electron configuration for an atom of element 3. • What is the expected charge for the most common ion of element 2? • What is the chemical symbol for element 2? • A neutral atom of which of the four elements has the SMALLEST radius?

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