Question

Diagonal relationships in the periodic table exist as well as the vertical relationships. For example, Be and Al are similar in some of their properties as are \(\mathrm{B}\) and \(\mathrm{Si}\). Rationalize why these diagonal relationships hold for properties such as size, ionization energy, and electron affinity.

Short answer

Diagonal relationships in the periodic table, such as those between Be and Al or B and Si, can be rationalized due to the trends in atomic size, ionization energy, and electron affinity. As diagonally related elements have comparable sizes and only slight differences in nuclear charge and shielding effect, their properties tend to show similarities despite not being in the same group or period. This is due to the combination of the increasing nuclear charge and shielding effect as we move across and down the periodic table.

Step-by-step solution

Understanding Diagonal Relationships

Diagonal relationships occur between certain pairs of elements that are not in the same group or period of the periodic table, but still show similarities in their properties. Some examples of such pairs include Be and Al, as well as B and Si. To understand why these relationships exist, we need to look at the trends in the periodic table regarding size, ionization energy, and electron affinity.

Periodic Trends: Atomic Size

Atomic size generally increases as we move down a group and decreases as we move from left to right along a period in the periodic table. This is due to the 'shielding effect' of inner electrons and the increasing positive charge in the nucleus. When we compare Be and Al, or B and Si, both elements in a pair are located one step down and one step right from each other in the periodic table. This means their atomic sizes do not change drastically, causing their properties to be similar.

Periodic Trends: Ionization Energy

Ionization energy is the energy required to remove an electron from an atom. It generally increases as we move from left to right across a period and decreases as we move down a group due to the increasing nuclear charge and the shielding effect of inner electrons. In diagonal relationships, like Be and Al, or B and Si, the increasing nuclear charge is somewhat compensated by the increasing shielding effect, resulting in similar ionization energies.

Periodic Trends: Electron Affinity

Electron affinity is the energy released when an electron is added to an atom. It generally increases as we move from left to right across a period and decreases as we move down a group. The trend in electron affinity is relatively similar to ionization energy. For diagonally related elements like Be and Al, or B and Si, the combination of the increasing nuclear charge and shielding effect results in these elements having similar electron affinities. To sum up, the diagonal relationships among elements in the periodic table, such as those between Be and Al or B and Si, can be rationalized due to the trends in atomic size, ionization energy, and electron affinity. As these diagonally related elements have comparable sizes and only slight differences in nuclear charge and shielding effect, their properties tend to show similarities despite not being in the same group or period.