1.3.6 and 1.3.7 - Ionization Energies Flashcards
What is the first ionization energy of an element?
the energy needed to remove one mole of electrons from the ground state of one mole of the gaseous atom
What energy level is an electron considered to be in once removed from an atom?
n= infinity
How can we calculate the ionization energy for one mole?
find the frequency at which convergence occurs (change in frequency = 0), then use E=hf to find the ionization energy for one atom, then multiply by avogadro’s number to find the ionization energy for one mole
Why is it more difficult to remove electrons as electrons are removed?
it gets closer to the nucleus where there is a stronger attraction for the electrons
How do successive ionization energies provide evidence of sublevels and that the s sublevel can hold 2 electrons and the p sublevel can hold 6?
When zooming in on ionization energy, for the second energy level, there is a slight jump after the first 6 electrons are removed, indicating that the second energy level is divided into two sublevels
Why would an electron leave more easily when paired in an orbital with another compared to being single in an orbital?
because the two electrons in the same orbital repel each other
Why is the increase in successive energies more stable between the 3d and 4s orbitals compared to when an electron is removed from the 3p orbital?
because the 3d and 4s orbitals are close in energy
Why do ionization energies generally increase from left to right across a period?
because the nuclear charge increases so even the the electrons are being removed from the same energy level, there is an increase in the force of electrostatic attraction between the nucleus and outer electrons
Why does ionization energies decrease down a group?
because a new energy level is being occupied which is further from the nucleus, therefore less energy is required to remove the outer electrons
How can the metals on the left side of the periodic table be characterized in general?
as having low ionization levels and form stable positive ions
How can non-metals on the right side of the periodic table be characterized in general?
as having high ionization energies and do not lose electrons readily and form negative ions
Why is there a decrease in ionization energies between group 2 and group 13 elements?
becauseit transitions from an s orbital to a p orbital which is at a higher energy and further away from the nucleus
Why is there a decrease in ionization energy between group 15 and group 16 elements?
because they transition from half filled p orbitals to double filled p orbitals and the two electrons in these orbitals repel each other
