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TT0
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If there was a bond in the 2p vs 3p subshell, which would be stronger? Taking into consideration that they are in the same group
Thanks
Thanks
Quite the opposite really, moving down a group the general trend is 1st ionisation values tend to decrease; this is explained by the increase in the number of occupied energy levels causing an increase in atomic radius, therefore electrostatic attraction between valence electrons and the nucleus is weaker. Hence, 1st I.E values decrease moving down a group as the atom requires less energy to be ionised and overcome the electrostatic attraction.TT0 said:I see, thanks. But then when you move down a group, doesn't the ionisation energy increase? Or am I mixing two different things?
Higher energy levels refer to the shells or orbitals in an atom that have a greater amount of energy compared to lower energy levels. These shells are labeled with the letters s, p, d, and f, with s being the lowest energy level and f being the highest.
Bonds are formed when atoms share or transfer electrons to achieve a more stable electron configuration. In higher energy levels, electrons have more energy and are therefore more likely to participate in bonding with other atoms.
Yes, bonds formed in higher energy levels are generally weaker compared to those formed in lower energy levels. This is because electrons in higher energy levels are farther from the nucleus and are less strongly attracted to it, resulting in weaker bonding forces.
Yes, bonds formed in higher energy levels can be broken more easily compared to those formed in lower energy levels. This is due to the weaker bonding forces and the fact that these electrons are more likely to be involved in chemical reactions.
The weaker bonds formed in higher energy levels have implications in various chemical processes such as reactions and molecule stability. They can also affect the physical properties of substances, such as melting and boiling points, as these are influenced by the strength of the bonds between atoms.