The first ionization potential of Na, Mg, Al and Si are in the order: (a) Na>Mg>Al Mg>

The first ionization potential of Na, Mg, Al and Si are in...

The first ionization potential of $\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}$ and $\mathrm{Si}$ are in the order: (a) $\mathrm{Na}>\mathrm{Mg}>\mathrm{Al}<\mathrm{Si}$ (b) $\mathrm{Na}>\mathrm{Mg}>\mathrm{Al}>\mathrm{Si}$ (c) $\mathrm{Na}<\mathrm{Mg}<\mathrm{AKSi}$ (d) $\mathrm{Na}<\mathrm{Mg}>\mathrm{AKSi}$

The first ionization potential of $\mathrm{Na}, \mathrm{Mg}, \mathrm{Al}$ and $\mathrm{Si}$ are in the order:
(a) $\mathrm{Na}>\mathrm{Mg}>\mathrm{Al}<\mathrm{Si}$
(b) $\mathrm{Na}>\mathrm{Mg}>\mathrm{Al}>\mathrm{Si}$
(c) $\mathrm{Na}<\mathrm{Mg}<\mathrm{AKSi}$
(d) $\mathrm{Na}<\mathrm{Mg}>\mathrm{AKSi}$

Key Concepts

First Ionization Energy

This is the energy required to remove the most weakly bound electron from a neutral atom in its ground state. It is a fundamental property that reflects how strongly an atom holds onto its electrons and is influenced by both the effective nuclear charge and the distance of the electron from the nucleus.

Periodic Trends

Across a period in the periodic table, ionization energy generally increases due to increasing effective nuclear charge, which more strongly attracts the electrons, making removal more difficult. However, variations due to the specific electron configurations of the atoms can cause deviations from a simple trend.

Effective Nuclear Charge and Electron Shielding

Effective nuclear charge is the net positive charge experienced by an electron in an atom, taking into account both the actual nuclear charge and the shielding effect of other electrons. Lesser shielding (or penetration effects of orbitals) results in electrons being held more tightly, affecting the ionization energy.

Transcript

00:01 Problem 91 of chapter 3, classification of elements and producity properties in this question, the first ionization potential of sodium, magnesium, aluminum and silicon are in order of what? so ionization energy is the minimum amount of energy that is required to remove most loosely held electron from an isolated gaseous atom.

00:25 And in general, we can represent the equation of ionization energy.

00:34 So how much energy is required to remove more closely held electrons from an isolate cations atom that is known as the ionization energy.

00:43 And in general, if we move from left to right in the product table, then the ionization energy value will increase.

00:50 And if we move from top to bottom in the product table, the ionization energy value will decrease.

00:55 Ionization energy depend on the radius that is inversely proportional to radius.

01:00 Ionization energy is directly proportional to effective nuclear charge.

01:03 And also the ionization energy is directly proportional to the stable configuration.

01:12 So stable electronic configuration of the element.

01:18 So that means for the stable electronic configuration, we required more energy in order to remove the electron.

01:24 So we have sodium magnesium aluminum silicon.

01:28 So right in the order of sodium, magnesium, aluminum, silicon.

01:32 So actually we expected the order of the ionization energy this but this is not a correct order because in case of magnesium as you can see it has the fulfilled electronic configuration in 3s.

01:49 So aluminum has lower ionization energy than magnesium.

01:55 So aluminum has lower ionization energy than that of magnesium...

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