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Hello students hope you are doing great.
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Let us understand the strengths in periodic table.
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First let's study about the atomic radius.
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As we move down from as we move down the periodic table, principal quantum number which is represented by n increases.
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As a principal quantum number increases, number of shell increases due to which the distance between nucleus and electron increases.
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As the distance between nucleus and electron increases, it means that the atomic radius increases.
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From this it is clear that as we move down the periodic table, atomic radius increases.
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Now let us see how the ionization enthalpy changes.
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Ionization enthalpy.
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So as we move from left to right in the periodic table, effective nuclear charge increases.
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Effective nuclear charge increases.
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As the effective nuclear charge increases, the attraction between nucleus and electron increases.
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The attraction between nucleus and electron increases because of which more energy is required, more energy needed to remove outermost electron.
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So from this we understand that as we move from left to right in periodic table, ionization enthalpy increases.
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Here we have carbon, boron, oxygen, nitrogen and fluorine.
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Boron is having the least ionization energy, then carbon, then nitrogen, then oxygen and then fluorine is having the highest ionization enthalpy.
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Let us see how electron negativity changes.
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Now as we move from left to right in periodic table, the effective nuclear charge increases...