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1 Put the following elements in order of increasing atomic...
Transcript of 1 Put the following elements in order of increasing atomic...
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4 Put the following elements in order of decreasing atomic size: Po, Sn, Fr, Rb, Cl, Li
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9 Predict which ions the following elements will produce:
A Nitrogen
B Oxygen
C Flourine
D Lithium
E Potassium
F Barium
G Chlorine
H Argon
I Carbon
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11 Put the following ions in order of increasing ionic size: Mn, Mn+2, Mn+3, Mn+4, Mn+7
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13 Put the following ions in order of increasing ionic size: Po+2, Sn+2, Fr+, Rb+, Cl-, Li+
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14 Predict which ions the following elements will produce:
A BerylliumB Boron
C Sulfur
D Iodine
E Astatine
F Sodium
G Hydrogen
H HeliumI Aluminium
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17 Put the following ions in order of increasing ionic size: B+3, P-3, I-, Sb-3, Be+2, Pb+4
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18 Put the following ions in order of increasing ionic size: N-3, As-3, Kr, Fr+, S-2, O-2
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19 Put the following elements in order of increasing electronegativity: P, Cs, Sn, F, Sr, Tl
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20 Put the following elements in order of increasing electronegativity: Ca, Rb, K, O, Al, As
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21 Put the following elements in order of decreasing electronegativity: Ga, Fr, Br, Si, Na, N
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22 Put the following elements in order of decreasing electronegativity: Po, Sn, Fr, Rb, Cl, Li
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23 Put the following elements in order of increasing electronegativity: Ra, F, Al, Ne, H, He,
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24 Put the following elements in order of increasing electronegativity: Ar, Ca, Mg, O, N, At
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25 Put the following elements in order of decreasing electronegativity: B, P, I, Sb, Be, Pb
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26 Put the following elements in order of decreasing electronegativity: N, As, Kr, Fr, S, O
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27 Put the following elements in order of increasing first ionization energy: P, Cs, Sn, F, Sr, Tl
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28 Put the following elements in order of increasing first ionization energy: Ca, Rb, K, O, Al, As
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29 Put the following elements in order of increasing first ionization energy: Ga, Fr, Br, Si, Na, N
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30 Put the following elements in order of increasing first ionization energy: Po, Sn, Fr, Rb, Cl, Li
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31 Put the following elements in order of increasing first ionization energy: Ra, F, Al, Ne, H, He,
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32 Put the following elements in order of increasing first ionization energy: Ar, Ca, Mg, O, N, At
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33 Put the following elements in order of increasing first ionization energy: B, P, I, Sb, Be, Pb,
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34 Put the following elements in order of increasing first ionization energy: N, As, Kr, Fr, S, O
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35 Put the following elements in order of increasing metallic character: P, Cs, Sn, F, Sr, Tl
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36 Put the following elements in order of increasing metallic character: Ca, Rb, K, O, Al, As
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37 Put the following elements in order of decreasing metallic character: Ga, Fr, Br, Si, Na, N
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38 Put the following elements in order of decreasing metallic character: Po, Sn, Fr, Rb, Cl, Li
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39 Put the following elements in order of increasing metallic character: Ra, F, Al, Ne, H, He
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40 Put the following elements in order of increasing metallic character: Ar, Ca, Mg, O, N, At
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41 Put the following elements in order of decreasing metallic character: B, P, I, Sb, Be, Pb
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42 Put the following elements in order of decreasing metallic character: N, As, Kr, Fr, S, O
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43 Consider the element Cesium.
A What is the most common ion that Cesium forms?
BWhich is larger neutral Cesium or the ion named in part 1? Why?
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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. [*]
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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. [*]
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46 Compare Cesium and Barium
A Which element has the larger atomic radius?
BCesium 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?
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47 Compare Rubidium and Barium
A Which element has the larger atomic radius?
BRubidium 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?
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48 Compare Cesium and Rubidium
A Which element has the larger atomic radius?
BCesium 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?
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49 Consider Nitrogen
A What is the most common ion that Nitrogen forms?
BWhich is larger, neutral Nitrogen or the ion named in part 1? Why?
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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. [*]
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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. [*]
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52 Compare Nitrogen and Phosphorus
A Which element has the larger atomic radius?
BNitrogen 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?
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53 Compare Nitrogen and Carbon
A Which element has the larger atomic radius?
BNitrogen 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?
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54 Compare Phosphorus and Carbon
A Which element has the larger atomic radius?
BPhosphorus 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?