Diagonal relationships in the periodic table exist as well as the vertical relationships. For ex

step 1 All right, guys. You're doing problem 36 of chapter 7. So diagonal relation to periodic table ex

Diagonal relationships in the periodic table exist as well...

Key Concepts

Periodic Trends

Periodic trends describe the patterns in behavior of elements’ properties such as atomic size, ionization energy, and electron affinity as one moves across the periodic table. These trends arise from the underlying atomic structure, including the number of protons, electrons, and the nature of electron shells, and they help in predicting and rationalizing the properties of elements relative to one another.

Effective Nuclear Charge and Electron Shielding

Effective nuclear charge is the net positive charge experienced by an electron in an atom, after accounting for the repulsive effects of other electrons. Electron shielding reduces the full impact of the nuclear charge on outer electrons, thereby influencing atomic size and energy levels. Together, these factors determine the strength of attraction between the nucleus and electrons, which in turn affects properties like ionization energy and electron affinity.

Diagonal Relationships

Diagonal relationships occur when certain elements in different groups but in diagonal positions across the periodic table exhibit similar chemical and physical properties. This phenomenon is attributed to a balance between increasing nuclear charge and enhanced electron shielding across periods and groups, which causes elements like beryllium and aluminum or boron and silicon to have comparable sizes, ionization energies, and electron affinities despite belonging to different groups.

Transcript

00:01 All right, guys.

00:01 You're doing problem 36 of chapter 7.

00:04 So diagonal relation to periodic table exists as well as vertical relationships.

00:08 For example, beryllium and aluminum are similar in some of their properties and b and b and b and b and b and s and b and sillac and silicon.

00:15 Rationalize why these diagonal relationships hold for properties such as size ionization energy and and electron affinity.

00:27 So as you go so we know that atomic radius increases towards the bottom right the period table.

00:32 Well, going down, it's pretty simple.

00:34 As you increase, as you go down to peer -eyed table, you're increasing the, you're going to increasing energy levels.

00:41 So you're adding more and more layers, more and more layers of electrons.

00:46 And that's causing your atomic radius increase.

00:49 But if you're going to the, and if you're going to the left of your period table, you're decreasing your effective nuclear charge.

00:56 So remember what nuclear charge, effective nuclear charge is.

00:59 Your nucleus is positively charged due to the protons, and so the core electrons in your nucleus will actually screen out some of that positive charge so that you can, will actually screen out some of the positive charge.

01:13 So your valence electrons are only feeling a fraction of your nuclear, of the actual nuclear charge.

01:21 So when you go from right to left on the periodic table, your number of core electrons say the same, but you're decreasing number of protons in your nucleus.

01:31 So that's causing your effective nuclear charge to decrease.

01:34 So your valance electrons won't be held as strongly by your atom.

01:38 So that's going to cause your atom to expand.

01:42 So that's why your atomic radius decreases as you go further, as you goes to the, of course, the bottom left.

01:52 When you go down, your atom increased in size due to increased number of electron shells.

01:57 And to the left, your decreased effective nuclear charge causes your valence electrons not to be held as tightly and cause your atom to expand.

02:06 Now for ionization energy...

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