Electron structure
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Define orbital
A region around the nucleus (of an atom) that can hold up to two electrons with opposite spins
What is the trend in ionisation energy from Li to Ne? i) Explain why
The IE increases i) The charge of the nucleus increases, the atomic radius gets smaller so more energy to required as there is a greater attraction between the electrons and nucleus. Shielding stays the same
Name the 4 shapes of orbitals For two describe what you would draw in order to represent them
s, p, d, and f (NOTE- the letters must be lowercase) s- spherical p- dumb-bell shape
Up to how many electrons can an orbital tolerate?
2
What condition is needed for 2 electrons to be held in an orbital?
The electrons must have opposite spins
How do electrons fill orbitals?
From the lowest energy level up
How many electrons are there in: i) a full p subshell ii) a half full s subshell iii) a full 3rd electron shell
i) 6 ii) 1 iii) 18
How many orbitals are there in: i) a d sub-shell ii) a f sub-shell ii) a p sub-shell
i) 5 ii) 7 iii) 3
Write the spdf notation of Na
1s1 2s2 2p6 3s1
What does the term degenerate mean when applied to orbitals?
Having identical energy
Which type of subshells contain several degenerate orbitals?
p, d, and f
What order are subshells filled?
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 5d, 4p, 4f
Define subshell
A group of orbitals of the same type within a shell
Define electronic configuration
A shorthand representation that shows how electrons occupy subshells in an atom