Beryllium has greater ionization energy, with 899 kJ/mol versus Germanium's 762 kJ/mol.
The general trend (most prominently displayed in the representative elements) in the Periodic Table is increasing ionization energy across a period, and decreasing ionization energy down a group.
Calcium: 589,9 kJ/mol. Beryllium: 899,5 kJ/mol.
2s
The rise in ionisation energy is not regular. To explain this we must remember that the second shell of electrons is actually subdivided into 2s and 2p. The most easily removed electron in Boron is that in the 2p orbital, higher in energy than the 2s electrons in Beryllium. It therefore needs less energy for total removal than does the 2s electron of Boron. This outweighs the effect of the increased nuclear charge of Boron, which tends to make its outer electron harder to remove.
Alkali metals (group 1 elements) have one valence electron. Hence have one ionization energy Alkaline earth metals (group 2 elements) have two valence electron. Hence have two ionization energy
It is NOT negative (for the first IE). Because Be's configuration is 1s2 2s2, we observe that it has no vacant orbital to accommodate an electron, meaning that to insert an electron, it has to go into a new sub-orbital, the higher-energy 2p. Hence, you need energy to promote this electron to a 2p level to force Be to accept it.
Beryllium will have the highest. Down a group ionization energy decreases.
Barium has more energy levels. So it has lesser ionization energy.
Helium has the highest ionization energy.
937 Kilojoules/mole
Beryllium is the group 3A element with the highest ionization energy.
potassium is greater in the second ionization energy.
Calcium: 589,9 kJ/mol. Beryllium: 899,5 kJ/mol.
The energy level for germanium is 4. You know its 4 because of the period its in for example: beryllium is in row 2 period 2 so the energy level is 2.
fluorine bromine chlorine
Because in Boron there is a complete 2s orbital and the increased shielding of the 2s orbital reduces the ionisation energy compared to that seen in Beryllium.
Ionization energy generally increases across a period as a result of a higher nuclear charge, however there are some exceptions such as Boron which has a lower ionization energy than Beryllium (because it is in a P orbital), and Oxygen which has a lower ionization energy than nitrogen (Because ionization decreases the electron electron repulsion in its orbitals).
It takes more energy to knock off two electrons