Electronic Structure Flashcards
What is the name given to the shell and its distance from the nucleus?
Principal quantum number.
What is the principle quantum number of the first shell?
1
What is the principle quantum number of the second shell?
2
What is the principle quantum number of the third shell?
3
What gives a shell a larger principal quantum number?
The further the shell is from the nucleus.
What sub shell does the 1st shell contain?
1s
What sub shells does the 2nd shell contain?
2s and 2p
What sub shells does the 3rd shell contain?
3s, 3p and 3d.
What sub shell does the 4th shell contain?
4s, 4p, 4d and 4f.
What is the number or orbitals and maximum electrons for the s sub-shell?
Number of orbitals- 1
Maximum electrons- 2
What is the number or orbitals and maximum electrons for the p sub-shell?
Number of orbitals- 3
Maximum electrons- 6
What is the number or orbitals and maximum electrons for the d sub-shell?
Number of orbitals- 5
Maximum electrons- 10
What is the number or orbitals and maximum electrons for the f sub-shell?
Number of orbitals- 7
Maximum electrons- 14
What is the s orbital shape?
Spherical
What is the p orbital shape?
Dumbell-shaped.
What 3 ways can you show electron configuration?
Sub shell notation
Arrows in boxes
Energy level diagrams
Which electron shells are filled up first?
Electrons fill orbitals singly before they start sharing, so the two electrons in the 2p sub-shells should be in separate orbitals.
Which one of the first, second or third ionisations of thallium produces an ion with the electron configuration [Xe] 5d10 6s1?
Second
State the general trend in first ionisation energies from carbon to neon.
Deduce the element that deviates from this trend and explain why this element deviates from the trend.
Increase
Oxygen / O
Paired electrons in a (2)p orbital
Write an equation, including state symbols, for the reaction that occurs when the first ionisation energy of carbon is measured.
C(g) → C+(g) + e(-)
Explain why the second ionisation energy of carbon is higher than the first ionisation energy of carbon.
(More energy to) remove an electron from a (more) positive ion.
Deduce the element in Period 2, from lithium to neon, that has the highest second ionisation energy.
Lithium
Explain the trend of increase across Period 2 of ionisation energy.
- Number of protons increases.
- Outermost electrons are in the same shell
- Greater nuclear attraction (on outermost electrons)
The first ionisation energy of oxygen is less than the first ionisation energy of fluorine.
- O has one less proton and so a smaller nuclear charge.
- Atomic radius of O is larger.
- Outer electrons are attracted less strongly (to the nucleus) in O.
When oxygen reacts with metals it forms oxide ions.
Write the electron configurations, in terms of sub-shells, of an oxygen atom and an oxide ion.
Hence, explain why this reaction of oxygen is typical of a non-metal.
1s2 2s2 2p4 and 1s2 2s2 2p6
In the reaction oxygen has formed a negative ion (by gaining two electrons.
Complete the electron configuration of a magnesium atom.
1s2 2s2 2p6 3s2
Write an equation to represent the second ionisation energy of magnesium. Include state symbols.
Mg+(g) -> Mg2+(g) + e–
Explain why there is an increase in first ionisation energy between F and Ne.
Ne has one more proton
Outermost electrons are in the same shell
Greater nuclear attraction on outermost electrons
Explain why there is a decrease in first ionisation energy between Ne and Na.
Na has one more shell
Outermost electron experiences greater shielding
Less nuclear attraction on outermost electrons
Why is the first ionisation energy of strontium larger than the first ionisation energy of rubidium?
Sr has one more proton and therefore greater nuclear charge.
Atomic radius of Sr is smaller.
Sr has greater nuclear attraction on outer electrons / outer shell.
Why is the second ionisation energy of rubidium larger than the second ionisation energy of strontium?
2nd IE of Rb involves removing electron from shell.
Stronger nuclear attraction on outermost electron of Rb.
Explain why xenon has a lower first ionisation energy than neon.
Xe has a bigger atomic radius and more shielding.
What is meant by an orbital?
A region (within an atom) that can hold up to two electrons with opposite spin.
State the total number of electrons occupying the p orbitals in one chlorine atom.
11
How many electrons are there in one ion of Ca2+?
18
Write the equation that represents the third ionisation energy of Al.
Al2+(g) -> Al3+(g) + e–
Define successive ionisation energy
A measure of the energy required to remove each electron in turn.
