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Will electron lattice electron interaction lower the energy of electrons?
Yes, electron-lattice interactions can lower the energy of electrons in a material. When electrons interact with the lattice of atoms in a solid, they can transfer energy through processes like phonon emission or absorption, which can result in a net lowering of the electron energy. This interaction is a key factor in phenomena such as electron-induced superconductivity or electron-phonon coupling in materials.
Which compound should have the largest lattice energy?
The compound that should have the largest lattice energy is the one with the highest charge and smallest ionic radius.
What periodic trends are inversely proportional to effective nuclear charge?
Atomic radius and ionization energy are inversely proportional to effective nuclear charge. As the effective nuclear charge increases, the attraction between the nucleus and the electrons increases, causing the atomic radius to decrease. In contrast, the ionization energy increases because it becomes harder to remove an electron from the atom due to the stronger attraction.
What is the correlation of ionization energies to atomic radii for the elements?
There is an inverse relationship between ionization energy and atomic radius: as atomic radius increases, ionization energy decreases. This is because as the distance between the nucleus and valence electrons increases, the attraction between them weakens, making it easier to remove an electron.
Why does the melting point of group 2 oxides decrease down the group?
The melting point of group 2 oxides decreases down the group because the atomic size of the cations (Group 2 metals) increases, leading to weaker metallic bonding with the oxide ions. This results in lower energy required to overcome these weaker bonds, hence lowering the melting point.
