Atomic Structure Flashcards
What is the overall mass of an electron?
1/1840
What is the definition of relative atomic mass?
The average mass of an atom/isotope of an element compared to 1/12 the mass of a C12 atom.
How are electrons arranged?
In energy levels which have sub-levels and orbitals.
How many electrons can each orbital hold?
2
How many orbitals does sub-level s have and how many electrons can it hold?
1 orbital, 2 electrons
How many orbitals does sub-level p have and how many electrons can it hold?
3 orbitals, 6 electrons
How many orbitals does sub-level d have and how many electrons can it hold?
5 orbitals, 10 electrons
How is electronic structure written?
(how far down the row)(s/p/d)*(how far across the period)
What is ionisation energy?
The energy required to remove one electron from each atom in a mole of gaseous atoms to form one mole of gaseous ions.
What is the equation for first ionisation energy?
X(g)->X+(g) + e-
What are the three factors affecting ionisation energy?
Nuclear charge, distance from nucleus, shielding
How does nuclear charge affect ionisation energy?
more protons is stronger attraction between outer electron and nucleus so stronger nuclear charge, increases I.E
How does the distance from nucleus affect ionisation energy?
the further the outer electron from nucleus, the weaker the attraction so I.E decreases
How does atomic shielding affect ionisation energy?
the more shielded the outer electron is, the weaker the attraction so I.E decreases
What is the general trend in I.E across a period and why?
Generally increases due to more protons so a stronger attraction between nucleus and outer electron.
