crays said:Hi, may i know why is the first row of the d orbitals (starting from scandium to zinc) should such a weird graph of ionization energy against number of protons? Here the proton number 22 element (titanium) has a higher ionization energy than the proton number 23 element (Vanadium). It is not half filled or fully filled. What's the reason?
GCT said:Probably has something to do with the additional shielding of the valence electrons with the extra electron in the d shell thus causing the IE to become slightly more negative ... Not certain about this.
chemisttree said:Correct!
D orbitals refer to the set of five orbitals (dxy, dyz, dzx, dx^2-y^2, and dz^2) that are present in the second energy level of an atom. First ionisation energy is the energy required to remove one electron from an atom in its ground state. D orbitals play a crucial role in determining the first ionisation energy of an atom, as the electrons in these orbitals have higher energy and are more easily removed compared to those in other orbitals.
As you move from left to right across the periodic table, the first ionisation energy generally increases. This is because the number of protons and electrons increases, leading to a stronger attraction between the positively charged nucleus and the negatively charged electrons. As a result, more energy is required to remove an electron from an atom in its ground state.
The first ionisation energy of an atom can be affected by several factors, including the number of protons in the nucleus, the distance between the nucleus and the outermost electrons, and the shielding effect of inner electrons. Additionally, the type of orbital that the outermost electron is in can also play a role, as D orbitals are generally easier to remove an electron from compared to other orbitals.
As you move down a group in the periodic table, the first ionisation energy generally decreases. This is because the outermost electrons are further away from the nucleus, making them easier to remove. Additionally, the shielding effect of inner electrons also increases with the addition of more energy levels, further decreasing the first ionisation energy.
The first ionisation energy of transition metals is generally lower due to their partially filled D orbitals. These orbitals have higher energy and are more easily removed compared to the S and P orbitals found in other elements. Additionally, the presence of multiple energy levels and the shielding effect of inner electrons also contribute to the lower first ionisation energy of transition metals.