Electron Configuration
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Strengths and weaknesses of the gcse planetary mode of the atom ?
Strengths *the number of shells *number of electrons *number of outer shell Weakness *2d not 3d *does not account for subshells
Filling up the shells with ?
1s2 2s2 2p6 3s2 3p6 4s2 3d10 4p6
What is an orbital ?
A region in space within an atom which can hold up to 2 electrons
Difference between the s orbital and p orbital?
S orbital *(sphere shape) P orbital *(like a dumbbell) *same equal energy everywhere
Definition of a s/d/pblock Element?
An element with it’s outermost electron in a s/d/p orbital
Describe the relative energies of the 2s orbital and each of the three 2p orbitals in a nitrogen atom?
*p orbital have greater energy than s orbital *p orbitals have equal energy
Explain the maximum number of electrons that can occupy each shell and sub shell ?
*1st shell - (total number is 2) SUBSHELL s- 2 *2nd shell - (total number is 8) SUBSHELL s-2 and p-6 *3rd shell - (total number is 18) SUBSHELL s-2 and p-6 and d-10
What is an orbital maximum ?
2 electrons
Define First ionisation ?
Energy required to remove 1 electron from each atom from 1 mole of gaseous atoms
What are the ionisation keywords?
*nuclear charge - positive charge on nucleus *atomic radius - distance from the outer most electron to the nucleus in a neutral atom *ionic radius - distance from outermost electron to the nucleus in a charged species *electron sheilding- repulsion caused between an inner shell of electrons and the outermost electron *nuclear attraction- the strength of attraction between nucleus and it’s outermost electron
What happens as you go down a group 1 ?
• as you go down a group 1 the nuclear charge increases -number of electrons shells increases -electron shielding increases so it weakens the nuclear attraction -atomic radius would increase and this weakens nuclear attraction • so overall nuclear attraction to outermost electron decreases
As you go across a period what happens?
• as you go across a period the nuclear charge increases which strengthens attraction -electron shells stays the same -electron shielding stays the same -atomic radius decreases which strengthens the nuclear attraction to the outermost electron • so overall nuclear attraction to outermost electron increase so the ionisation energy needed increases
Why is there such a large drop in first ionisation energy between periods ?
• changing period • higher period has an extra shell • greater atomic radius and more electron sheilding • significant decrease in nuclear attraction to outermost electron
Explain the anomaly drop between beryllium and boron?
-group 2 outershell has a (any number ) s subshell - where the group 3 has a (any number) p subshell - the p subshell is at a higher energy than the s subshell - so it takes less energy to remove it( lower first ionisation energy)
Explain the anomaly drop between group 5 and 6?
• group 4 electron configuration is ….. whilst group 6 is ….. • in group 6 the _p electron begin to be pair which causes extra repulsion so the 2p electron are at higher energy (less stable) • and takes less energy to remove (lower first ionisation energy)
Define second and third ionisation energy between?
Energy required to remove 1 electron from each +1/+2 ion of 1 mole of gaseous +1/+2 ions
Model answer to explain increase in ionisation of energy from graph or table?
A large increase in ionisation energy between _ and _ electrons indicates _ electron is being removed from an inner shell
First second and third equation with state symbols showing the ionisation energy of oxygen?
O(g) ——>O+(g) + e- (first) O+(g) —->O2+(g) + e- (second) O2+(g) —-> O3+(g) + e-(third)
What is the ionisation energy equation?
Xn+ (g) ———-> X(n+1)+ (g) + e-