Suggest why the ionization energy of magnesium is greater than the ionization energies of sodium

step 1 Okay, now we do question 100. And when we do question 100, you have to write down the electron c

Suggest why the ionization energy of magnesium is greater...

Key Concepts

Effective Nuclear Charge

Effective nuclear charge refers to the net positive charge experienced by electrons after accounting for the shielding effect of inner electrons. A higher effective nuclear charge means that the valence electrons are pulled closer to the nucleus, which increases the ionization energy as more energy is required to remove an electron.

Electron Configuration

The specific arrangement of electrons in an atom’s orbitals influences its stability. Magnesium’s configuration, which involves a fully filled valence subshell, contributes to a more stable state compared to configurations with partially filled or more diffuse orbitals, and thus a higher ionization energy.

Orbital Penetration and Shielding

Electrons in s-orbitals tend to penetrate closer to the nucleus and experience less shielding from inner electrons, resulting in a stronger nuclear attraction. This contrasts with electrons in p-orbitals or higher-energy orbitals, which are more shielded and less tightly held, leading to lower ionization energies.

Periodic Trends in Ionization Energy

Ionization energy generally increases across a period due to increasing effective nuclear charge and decreases down a group due to increased electron shielding and orbital size. Magnesium's position in the period gives it a greater effective nuclear pull on its valence electrons than that found in elements with extra electron shells or less optimal orbital configurations.

Transcript

00:01 Okay, now we do question 100.

00:05 And when we do question 100, you have to write down the electron configuration.

00:13 So we do you understand more.

00:15 We have sodium.

00:17 Sodium, we have neon and 3s1.

00:21 And they are the same periods here.

00:24 Manusium, neon, and 3s2.

00:28 And aluminum.

00:29 Neon and 3 .82, 3b1.

00:35 So down below the magnesium is calcium.

00:39 Of course, when the same root calcium has lower ionization than magnesium, right? so argon, 4x2.

00:51 And now we compare.

01:41 Okay, first one.

01:43 So now you have to see the periods and you see like before i stand the shielding in this question, i thought, i think maybe he just asked about the first ionization energy because sodium got only one electron.

01:59 So for the first ionization energy, of course, magnesium had to get greater, the greater energy than sodium because magnesium is more non -metal than sodium, right? and for aluminum, we have, we have three electrons.

02:17 So the first ionization energy, it should be removed.

02:22 It should remove electrons from the orbital.

02:26 And the orbital, they get electrons...

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