Slide 1 / Put the following elements in order of increasing atomic size: P, Cs, Sn, F, Sr, Tl

Transcription

1 Slide 1 / 54 1 Put the following elements in order of increasing atomic size: P, Cs, Sn, F, Sr, Tl

2 Slide 2 / 54 2 Put the following elements in order of increasing atomic size: Ca, Rb, K, O, Al, As

3 Slide 3 / 54 3 Put the following elements in order of decreasing atomic size: Ga, Fr, Br, Si, Na, N

4 Slide 4 / 54 4 Put the following elements in order of decreasing atomic size: Po, Sn, Fr, Rb, Cl, Li

5 Slide 5 / 54 5 Put the following elements in order of increasing atomic size: Ra, F, Al, Ne, H, He,

6 Slide 6 / 54 6 Put the following elements in order of increasing atomic size: Ar, Ca, Mg, O, N, At

7 Slide 7 / 54 7 Put the following elements in order of decreasing atomic size: B, P, I, Sb, Be, Pb

8 Slide 8 / 54 8 Put the following elements in order of decreasing atomic size: N, As, Kr, Fr, S, O

9 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

10 Slide 10 / Put the following ions in order of increasing ionic size: Si, Si +2, Si +4, Si -4

11 Slide 11 / Put the following ions in order of increasing ionic size: Mn, Mn +2, Mn +3, Mn +4, Mn +7

12 Slide 12 / Put the following ions in order of increasing ionic size: N -3, N, P -3, C -4, O -2

13 Slide 13 / Put the following ions in order of increasing ionic size: Po +2, Sn +2, Fr +, Rb +, Cl -, Li +

14 Slide 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

15 Slide 15 / Put the following ions in order of increasing ionic size: Sb, Sb +5, Sb +3, Sb -3

16 Slide 16 / Put the following ions in order of increasing ionic size: V, V +2, V +3, V +4, V +5

17 Slide 17 / Put the following ions in order of increasing ionic size: B +3, P -3, I -, Sb -3, Be +2, Pb +4

18 Slide 18 / Put the following ions in order of increasing ionic size: N -3, As -3, Kr, Fr +, S -2, O -2

19 Slide 19 / Put the following elements in order of increasing electronegativity: P, Cs, Sn, F, Sr, Tl

20 Slide 20 / Put the following elements in order of increasing electronegativity: Ca, Rb, K, O, Al, As

21 Slide 21 / Put the following elements in order of decreasing electronegativity: Ga, Fr, Br, Si, Na, N

22 Slide 22 / Put the following elements in order of decreasing electronegativity: Po, Sn, Fr, Rb, Cl, Li

23 Slide 23 / Put the following elements in order of increasing electronegativity: Ra, F, Al, Ne, H, He,

24 Slide 24 / Put the following elements in order of increasing electronegativity: Ar, Ca, Mg, O, N, At

25 Slide 25 / Put the following elements in order of decreasing electronegativity: B, P, I, Sb, Be, Pb

26 Slide 26 / Put the following elements in order of decreasing electronegativity: N, As, Kr, Fr, S, O

27 Slide 27 / Put the following elements in order of increasing first ionization energy: P, Cs, Sn, F, Sr, Tl

28 Slide 28 / Put the following elements in order of increasing first ionization energy: Ca, Rb, K, O, Al, As

29 Slide 29 / Put the following elements in order of increasing first ionization energy: Ga, Fr, Br, Si, Na, N

30 Slide 30 / Put the following elements in order of increasing first ionization energy: Po, Sn, Fr, Rb, Cl, Li

31 Slide 31 / Put the following elements in order of increasing first ionization energy: Ra, F, Al, Ne, H, He,

32 Slide 32 / Put the following elements in order of increasing first ionization energy: Ar, Ca, Mg, O, N, At

33 Slide 33 / Put the following elements in order of increasing first ionization energy: B, P, I, Sb, Be, Pb,

34 Slide 34 / Put the following elements in order of increasing first ionization energy: N, As, Kr, Fr, S, O

35 Slide 35 / Put the following elements in order of increasing metallic character: P, Cs, Sn, F, Sr, Tl

36 Slide 36 / Put the following elements in order of increasing metallic character: Ca, Rb, K, O, Al, As

37 Slide 37 / Put the following elements in order of decreasing metallic character: Ga, Fr, Br, Si, Na, N

38 Slide 38 / Put the following elements in order of decreasing metallic character: Po, Sn, Fr, Rb, Cl, Li

39 Slide 39 / Put the following elements in order of increasing metallic character: Ra, F, Al, Ne, H, He

40 Slide 40 / Put the following elements in order of increasing metallic character: Ar, Ca, Mg, O, N, At

41 Slide 41 / Put the following elements in order of decreasing metallic character: B, P, I, Sb, Be, Pb

42 Slide 42 / Put the following elements in order of decreasing metallic character: N, As, Kr, Fr, S, O

43 Slide 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?

44 Slide 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. [*]

45 Slide 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. [*]

46 Slide 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?

47 Slide 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?

48 Slide 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?

49 Slide 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?

50 Slide 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. [*]

51 Slide 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. [*]

52 Slide 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?

53 Slide 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?

54 Slide 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?