3. run the simulation using hydrogen for a few seconds. then switch to sodium.\na. what do you notice about…

3. run the simulation using hydrogen for a few seconds. then switch to sodium.\na. what do you notice about the spacing of the electron levels of these two elements?\nhydrogen has more evenly spaced electron levels compared to sodium more complex and irregular spacing\nb. as the sodium simulation runs, what do you notice about the number of transitions in the uv, visible and far ir portions of the spectrum? explain your observations, referring to your answer to 3a and comparing its spectrum to that of hydrogen.\nanalysis questions:\n1. how did the electrons in the elements you observed become “excited”?\ngases - absorb energy heat,electrical and discharge\nsolids -heat,light, or electric field\n2. when do electrons emit light energy?when returning form excited to lower energy state

3. run the simulation using hydrogen for a few seconds. then switch to sodium.\na. what do you notice about the spacing of the electron levels of these two elements?\nhydrogen has more evenly spaced electron levels compared to sodium more complex and irregular spacing\nb. as the sodium simulation runs, what do you notice about the number of transitions in the uv, visible and far ir portions of the spectrum? explain your observations, referring to your answer to 3a and comparing its spectrum to that of hydrogen.\nanalysis questions:\n1. how did the electrons in the elements you observed become “excited”?\ngases - absorb energy heat,electrical and discharge\nsolids -heat,light, or electric field\n2. when do electrons emit light energy?when returning form excited to lower energy state

Answer

Brief Explanations:

a. Hydrogen has a single - electron system, resulting in more evenly - spaced electron levels. Sodium, with multiple electrons and electron - electron interactions, has more complex and irregularly spaced levels. b. Sodium has more complex electron - level spacing. This leads to a greater number of possible transitions across the UV, visible, and far - IR spectrum compared to hydrogen. Hydrogen's simple electron structure limits the number of transitions. For analysis question 1, electrons become excited by absorbing energy in the form of heat, electricity, or light depending on the state (gas or solid). For analysis question 2, electrons emit light energy when they return from an excited state to a lower energy state.

Answer:

a. Hydrogen has more evenly spaced electron levels compared to sodium's more complex and irregular spacing. b. Sodium has more transitions across the UV, visible, and far - IR spectrum due to its complex electron - level structure compared to hydrogen.

  1. Gases: absorb energy (heat, electrical, and discharge). Solids: heat, light, or electric field.
  2. When returning from excited to lower energy state.