Electronic structure and the periodic table Flashcards
What are the four quantum numbers?
Principle (n)
Angular momentum (/)
Magnetic (m/)
Spin (ms)
Define the principle quantum numbers.
The atomic shells K (n=1), L (n=2), M (n=3)
Define the angular momentum quantum numbers.
The shape of the atomic orbital
Define the magnetic quantum numbers.
The orientation of the orbital around the nucleus
Define the spin quantum numbers.
+1/2 (spin up) or -1/2 (spin down) for the electron
How do you interpret angular momentum quantum numbers?
For a shape defined by n, / takes all integer values between 0 and n-1
/ = 0 is s
/ = 1 is p
/ = 2 is d
/ = 3 is f
How do you interpret magnetic quantum numbers?
For a given value of /, the m/ can take any of the 2/ + 1 integer values between -/ and +/
when / = 0, m/ = 0 (sphere)
when / = 1, m/ = 3 (with x, y and z axis)
What does pauli’s exclusion principle state?
if two electrons in an atom share the same n, / and m/, their ms have to be opposite sides.
List the three orbital filling rules
for a given n: maximum number of electrons allowed is 2n²
for a given /: (s, p, d, f), this number is 4/ + 2
for a given m/: max number of 2 electrons is allowed
What is the order orbitals are filled in?
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p.
What does box diagrams show?
the orbitals with the same / grouped together
From the periodic table, how do you find valence (outermost) electrons?
the row/period number
What makes up the S block?
the first two columns of the periodic table
What makes up the P block?
groups 3A to 8A
What is the first ionisation energy?
the energy required to remove one outermost electron from an atom in the gaseous state
What are the trends down the periodic table?
increasing IE/IP
decreasing electronegativity
increasing atomic radius
What are the trends across the periodic table?
increase in IE
increasing electronegativity
decreasing atomic radius
