Chapter 9: Problem 4
Explain, in terms of absorbed and reflected light, why a blue object appears blue.
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These are the key concepts you need to understand to accurately answer the question.
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Chapter 9: Problem 4
Explain, in terms of absorbed and reflected light, why a blue object appears blue.
These are the key concepts you need to understand to accurately answer the question.
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Explain the difference between valence electrons and core electrons.
What is the difference between the ground state of an atom and an excited state of an atom?
Arrange these elements in order of increasing atomic size: \(\mathrm{Cs}, \mathrm{Sb}, \mathrm{S}, \mathrm{Pb}, \mathrm{Se}\).
You learned in this chapter that ionization generally increases as you move from left to right across the periodic table. However, consider the following data, which shows the ionization energies of the period 2 and 3 elements: $$ \begin{array}{ccccc} \text { Group } & \begin{array}{c} \text { Period 2 } \\ \text { Elements } \end{array} & \begin{array}{c} \text { lonization } \\ \text { Energy } \\ \text { (kJ/mol) } \end{array} & \begin{array}{c} \text { Period 3 } \\ \text { Elements } \end{array} & \begin{array}{c} \text { Ionization } \\ \text { Energy } \\ \text { (kJ/mol) } \end{array} \\ \text { 1A } & \text { Li } & 520 & \text { Na } & 496 \\ \text { 2A } & \text { Be } & 899 & \text { Mg } & 738 \\ \text { 3A } & \text { B } & 801 & \text { Al } & 578 \\ \text { 4A } & \text { C } & 1086 & \text { Si } & 786 \\ \text { 5A } & \text { N } & 1402 & \text { P } & 1012 \\ \text { 6A } & \text { 0 } & 1314 & \text { S } & 1000 \\ \text { 7A } & \text { F } & 1681 & \text { Cl } & 1251 \\ \text { 8A } & \text { Ne } & 2081 & \text { Ar } & 1521 \\ \hline \end{array} $$ Notice that the increase is not uniform. In fact, ionization energy actually decreases a bit in going from elements in group \(2 \mathrm{~A}\) to \(3 \mathrm{~A}\) and then again from \(5 \mathrm{~A}\) to \(6 \mathrm{~A}\). Use what you know about electron configurations to explain why these dips in ionization energy exist.
Arrange these elements in order of increasing atomic size: \(\mathrm{Ca}, \mathrm{Rb}, \mathrm{S}, \mathrm{Si}, \mathrm{Ge}, \mathrm{F}\).
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