Slide 1 / 54 1 Put the following elements in order of increasing atomic size: P, Cs, Sn, F, Sr, Tl
Slide 2 / 54 2 Put the following elements in order of increasing atomic size: Ca, Rb, K, O, Al, As
Slide 3 / 54 3 Put the following elements in order of decreasing atomic size: Ga, Fr, Br, Si, Na, N
Slide 4 / 54 4 Put the following elements in order of decreasing atomic size: Po, Sn, Fr, Rb, Cl, Li
Slide 5 / 54 5 Put the following elements in order of increasing atomic size: Ra, F, Al, Ne, H, He,
Slide 6 / 54 6 Put the following elements in order of increasing atomic size: Ar, Ca, Mg, O, N, At
Slide 7 / 54 7 Put the following elements in order of decreasing atomic size: B, P, I, Sb, Be, Pb
Slide 8 / 54 8 Put the following elements in order of decreasing atomic size: N, As, Kr, Fr, S, O
Slide 9 / 54 9 Predict which ions the following elements will produce: A B C D E F G H I Nitrogen Oxygen Flourine Lithium Potassium Barium Chlorine Argon Carbon
Slide 10 / 54 10 Put the following ions in order of increasing ionic size: Si, Si +2, Si +4, Si -4
Slide 11 / 54 11 Put the following ions in order of increasing ionic size: Mn, Mn +2, Mn +3, Mn +4, Mn +7
Slide 12 / 54 12 Put the following ions in order of increasing ionic size: N -3, N, P -3, C -4, O -2
Slide 13 / 54 13 Put the following ions in order of increasing ionic size: Po +2, Sn +2, Fr +, Rb +, Cl -, Li +
Slide 14 / 54 14 Predict which ions the following elements will produce: A B C D E F G H I Beryllium Boron Sulfur Iodine Astatine Sodium Hydrogen Helium Aluminium
Slide 15 / 54 15 Put the following ions in order of increasing ionic size: Sb, Sb +5, Sb +3, Sb -3
Slide 16 / 54 16 Put the following ions in order of increasing ionic size: V, V +2, V +3, V +4, V +5
Slide 17 / 54 17 Put the following ions in order of increasing ionic size: B +3, P -3, I -, Sb -3, Be +2, Pb +4
Slide 18 / 54 18 Put the following ions in order of increasing ionic size: N -3, As -3, Kr, Fr +, S -2, O -2
Slide 19 / 54 19 Put the following elements in order of increasing electronegativity: P, Cs, Sn, F, Sr, Tl
Slide 20 / 54 20 Put the following elements in order of increasing electronegativity: Ca, Rb, K, O, Al, As
Slide 21 / 54 21 Put the following elements in order of decreasing electronegativity: Ga, Fr, Br, Si, Na, N
Slide 22 / 54 22 Put the following elements in order of decreasing electronegativity: Po, Sn, Fr, Rb, Cl, Li
Slide 23 / 54 23 Put the following elements in order of increasing electronegativity: Ra, F, Al, Ne, H, He,
Slide 24 / 54 24 Put the following elements in order of increasing electronegativity: Ar, Ca, Mg, O, N, At
Slide 25 / 54 25 Put the following elements in order of decreasing electronegativity: B, P, I, Sb, Be, Pb
Slide 26 / 54 26 Put the following elements in order of decreasing electronegativity: N, As, Kr, Fr, S, O
Slide 27 / 54 27 Put the following elements in order of increasing first ionization energy: P, Cs, Sn, F, Sr, Tl
Slide 28 / 54 28 Put the following elements in order of increasing first ionization energy: Ca, Rb, K, O, Al, As
Slide 29 / 54 29 Put the following elements in order of increasing first ionization energy: Ga, Fr, Br, Si, Na, N
Slide 30 / 54 30 Put the following elements in order of increasing first ionization energy: Po, Sn, Fr, Rb, Cl, Li
Slide 31 / 54 31 Put the following elements in order of increasing first ionization energy: Ra, F, Al, Ne, H, He,
Slide 32 / 54 32 Put the following elements in order of increasing first ionization energy: Ar, Ca, Mg, O, N, At
Slide 33 / 54 33 Put the following elements in order of increasing first ionization energy: B, P, I, Sb, Be, Pb,
Slide 34 / 54 34 Put the following elements in order of increasing first ionization energy: N, As, Kr, Fr, S, O
Slide 35 / 54 35 Put the following elements in order of increasing metallic character: P, Cs, Sn, F, Sr, Tl
Slide 36 / 54 36 Put the following elements in order of increasing metallic character: Ca, Rb, K, O, Al, As
Slide 37 / 54 37 Put the following elements in order of decreasing metallic character: Ga, Fr, Br, Si, Na, N
Slide 38 / 54 38 Put the following elements in order of decreasing metallic character: Po, Sn, Fr, Rb, Cl, Li
Slide 39 / 54 39 Put the following elements in order of increasing metallic character: Ra, F, Al, Ne, H, He
Slide 40 / 54 40 Put the following elements in order of increasing metallic character: Ar, Ca, Mg, O, N, At
Slide 41 / 54 41 Put the following elements in order of decreasing metallic character: B, P, I, Sb, Be, Pb
Slide 42 / 54 42 Put the following elements in order of decreasing metallic character: N, As, Kr, Fr, S, O
Slide 43 / 54 43 Consider the element Cesium. A B What is the most common ion that Cesium forms? Which is larger neutral Cesium or the ion named in part 1? Why?
Slide 44 / 54 44 Consider the element Barium. A 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. B 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. C Describe Barium s s electronegativity. D Describe Barium s s metallic character. [*]
Slide 45 / 54 45 Consider the element Rubidium. A 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. B 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. C Describe Rubidium s electronegativity. D Describe cesium s metallic character. [*]
Slide 46 / 54 46 Compare Cesium and Barium A B Which element has the larger atomic radius? Cesium and Barium both commonly form Cations. Which Cation will be smaller? C 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. D How does Cesium s first ionization energy compare to Bariums? How might this difference affect your answer in part c?
Slide 47 / 54 47 Compare Rubidium and Barium A B Which element has the larger atomic radius? Rubidium and Barium both commonly form Cations. Which Cation will be smaller? C 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. D How does Rubidium s first ionization energy compare to Bariums? How might this difference affect your answer in part c?
Slide 48 / 54 48 Compare Cesium and Rubidium A B Which element has the larger atomic radius? Cesium and Rubidium both commonly form Cations. Which Cation will be smaller? C 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. D How does Cesium s first ionization energy compare to Rubidium? How might this difference affect your answer in part c?
Slide 49 / 54 49 Consider Nitrogen A B What is the most common ion that Nitrogen forms? Which is larger, neutral Nitrogen or the ion named in part 1? Why?
Slide 50 / 54 50 Consider Phosphorus. A 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. B * 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. C Describe Phosphorus s electronegativity. D Describe Phosphorus s metallic character. [*]
Slide 51 / 54 51 Consider Carbon. A 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. B 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. C Describe Carbon s electronegativity. D Describe Carbon s metallic character. [*]
Slide 52 / 54 52 Compare Nitrogen and Phosphorus A B Which element has the larger atomic radius? Nitrogen and Phosphorus both commonly form Anions. Which Anion will be smaller? C 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. D How does Nitrogen s first ionization energy compare to Phosphorus? How might this difference affect your answer in part c?
Slide 53 / 54 53 Compare Nitrogen and Carbon A B Which element has the larger atomic radius? Nitrogen and Carbon both commonly form Anions. Which Anion will be smaller? C 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. D How does Nitrogen s first ionization energy compare to Carbon s? How might this difference affect your answer in part c?
Slide 54 / 54 54 Compare Phosphorus and Carbon A B Which element has the larger atomic radius? Phosphorus and Carbon both commonly form Anions. Which Anion will be smaller? C 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. D How does Phosphorus s first ionization energy compare to Carbon s? How might this difference affect your answer in part c?