Theme 2- The electron configuration of atoms and the periodic table Flashcards
what are atomic orbitals and electronic configuration?
Atomic orbitals- regions of space in which electrons orbit
electronic configuration- the orbital arrangements of electrons
what is a quantum?
the discreet amount of energy possessed by each electron.
what is the principle quantum number?
The number (n) assigned to the a specific energy level within an atom , and the maximum number of electrons within this energy level is given by 2n^2
what happens to orbitals as energy levels increase?
the complexity of orbitals increases
what are s orbitals?
The closest energy level to the nucleus (lowest energy). symmetrical round the nucleus and can contain up to TWO electrons
what is different in 2s and 3s etc. energy levels compared to an s energy level?
the orbitals are similar but as they increase in number they get progressively further away from the nucleus, and probability of finding an electron decreases with increasing distance.
what type of orbital appears at the secondary energy level?
P orbitals appear,
what is the difference in shape between p and s orbitals?
P orbitals are shaped like two balloons either side of the nucleus, whereas s orbitals are concentric rings around the nucleus
how many planes do p orbitals exist in? what are these called?
three planes: x,y,z
how many electrons can each orbital contain? what is the spin?
each orbital can only contain TWO electrons, each with opposing directions of spin.
how many electrons are there in a p orbital?
6 (2 in each plane)
how would you denote an s orbital in the first energy level with two electrons?
1s^2
what is aufbans principle?
electrons will fill the lowest energy level available to them.
which energy level fills first: 3d or 4s?
4s as it is a lower energy level than 3d
who designed the first periodic table?
Mendeleev in 1896, basing the table on observed chemical behavior.
