1.2 - 1-4 Flashcards
What are he factors that affect ionisation energies?
Atomic radius (distance from the nucleus it the outer shell electrons) - the greater the atomic radius, the smaller the attraction experienced by the outer electrons.
Nuclear charge - the greater the nuclear charge, the greater the attractive force on the outer electrons.
Electron shielding or screening - inner shells repel the outer-shell electrons. This is called electron shielding or screening. The more inner shells, the larger the shielding effect and the smaller the nuclear attraction experienced by the outer electrons.
What is the first ionisation energy of an element?
It’s the energy required to remove on electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.
Wha is electron screening?
The repulsion between electrons in different inner shells, this reduces the net attractive force from the positive nucleus on the outer shell electrons.
How do you represent ionisation energies?
Li (g) → Li+ (g) + e- (1st ionisation energy)
Li+ (g) → Li²+ (g) + e- (2nd ionisation energy)
What causes a big increase in successive ionisation energies?
Moving to the a different shell, closer to the nucleus.
What is an atomic orbital?
A region within an atom that can hold up to two electrons, with opposite spins.
What does the principal quantum number represent?
The shell that the electrons occupy.
What is a shell?
A group of atomic orbitals with the same principal quantum number.
What shape is an s-orbital?
Spherical.
How many electrons can one s-orbital hold?
2 (1 pair)
What shape is a p-orbital?
It has a 3-D dumb bell shape.
How many electrons can a p-orbital hold?
6 (3 pairs)
How many electrons can a d-orbital hold?
10 (5 pairs)
How many electrons can a f-orbital hold?
14 (7 pairs)
What is a sub shell?
A group of the same type of atomic orbitals (s, p, d or f) within a shell.
