Beryllium is a metal. It has 2 valance electrons (in the outer shell), and therefore it tends to lose those electrons in order to achieve a stable electron configuration, which in the case of beryllium is also 2 electrons, but in the inner shell. Nitrogen is a nonmetal, with 5 valence electrons, and it tends to acquire more electrons in order to reach a stable electron configuration of 8. Less energy is need to lose electrons when the result is going to be a stable electron configuration.
both are in the same period which accounts for closeness. they are nonetheless different because there are more protons in the nucleus which means electrons are brought closer to it so there is a higher ionisation energy or potential
yes
Nitrogen has five electrons on the outer level.
Bromine has less valence shells than lead making the distance between its valence electron and its nucleus less than that of lead. This means that there is greater attraction between the nucleus and electron for bromine and it requires a higher ionisation energy to remove its electron.
The rate of effusion for nitrogen is higher.
both are in the same period which accounts for closeness. they are nonetheless different because there are more protons in the nucleus which means electrons are brought closer to it so there is a higher ionisation energy or potential
Calcium: 589,9 kJ/mol. Beryllium: 899,5 kJ/mol.
The ionisation energy depends on the orbital from which the electron is removed and also the distance of the orbital from the nucleus. In the case of Helium, the electron is removed from 1s orbital whereas in the case of argon it is from 3p orbital. As 1s is closer to the nucleus, the force of attraction experience by these electrons is higher and hence helium will have higher 1st ionisation energy.
The ionisation enthalpy of potassium is lower than that of sodium.
yes
1.A small atomic/ionic radius 2.therefore less number of protons 3. more net nuclear attraction between the positively charged nucleus 4. higher energy is needed to break those bonds. 5. therefore an element has high ionisation energy
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.
Nitrogen has five electrons on the outer level.
half filled P orbitals increase the stability resulting in higher ionization energy
Bromine has less valence shells than lead making the distance between its valence electron and its nucleus less than that of lead. This means that there is greater attraction between the nucleus and electron for bromine and it requires a higher ionisation energy to remove its electron.
Higher temperatures mean more heat energy which translates into more kinetic energy of the molecules of nitrogen gas. This greater kinetic energy allows the molecules to diffuse faster than at a lower temperature and lower kinetic energy.
because it lower than Ba as you go down ionization energy increases