Without looking at data in the text, sketch a qualitative...

Key Concepts

Electron Configuration and Subshell Stability

Electron configurations determine the stability of electrons in an atom. When electrons occupy a complete or half-complete subshell, they are usually more stable. For period 3 elements, the removal of electrons from valence orbitals (such as the 3s or 3p orbitals) typically requires less energy compared to removing an electron from a noble-gas core configuration. The qualitative graph of the third ionization energy versus atomic number reflects these differences; elements that yield a noble gas configuration before the third removal show a sudden jump, while others show a smoother trend.

Effective Nuclear Charge and Electron Shielding

Effective nuclear charge is the net positive charge experienced by an electron after accounting for the shielding effect of inner electrons. As atomic number increases across a period, effective nuclear charge generally increases, making electrons more tightly bound. In the context of successive ionizations, removing an electron that is shielded less (or is from an inner shell) requires significantly more energy, and this effect contributes to distinct jumps in the qualitative graph.

Periodic Trends in Ionization Energy

Across a period, ionization energies generally increase because of rising effective nuclear charge. However, when analyzing successive ionization energies, especially for elements with different electron configurations, one can observe dips and sharp jumps. For period 3 elements, variations in the third ionization energy are influenced by whether the electron being removed is from a relatively weakly bound valence shell or a much more stable, noble-gas core configuration.

Ionization Energy and Successive Ionization Energies

Ionization energy is the amount of energy needed to remove an electron from a gaseous atom or ion. Successive ionization energies refer to the energy required to remove each additional electron after the first. In problems like this, the third ionization energy is key because it often involves removing an electron from a configuration that may be much more stable than the previous, leading to discontinuities in the trend.

Transcript

00:01 All right, guys, the new problem 182, chapter 7.

00:03 So if i'm looking at data and text, get you a quality of graph with third ionization energy versus atomic number of sodium through argon, and explain your graph.

00:11 So we're in the third energy level.

00:14 So we have 3s and 3p or plus.

00:19 So with sodium, we have 1 3s electron.

00:23 So if we're in the third ionization energy, we're taking out that valence electron, and then we have to take out two core shell electrons.

00:30 And taking out the core shell electrons, that takes more energy and taking out the balance electrons.

00:42 Because these core electrons, these are closer nucleus, and because they're closer nucleus, they're as they're more strongly attracted to it.

00:51 So it's going to be hard to take those off.

00:54 So sodium is going to be the one of the highest electron.

00:57 So sodium is going to be the one with the highest third ionization energy.

01:01 With magnesium, that's going to be second highest.

01:04 Because magnesium you're going to see you're going to take out these two balanced electrons but you're only going to take out one core electron for that third ionization energy.

01:15 So it's going to be, so although it's going to be high energy, it's not going to be as high as sodium.

01:22 Next, this is aluminum.

01:24 So of aluminum, you're going to take out these three balanced electrons, but you're not going to take out anything.

01:32 But you're not going to take out anything else...

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