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Ionisation Energy
Some help with these questions would be great:
1. Which element out of Oxygen, Fluorine, Neon, Sodium, Magnesium and Aluminium has the highest second ionisation energy?
2. Why is the ionisation energy of sodium less than that of magnesium?
Why is the second ionisation energy of sodium more than the second ionisation energy of magnesium?
3. Why do neon and sodium have such very different first ionisation energies?
4. Place in asending order the ionisation energies of,
a) F+, F, F-
b) Cl, Br, I
c) Fr, Ra, Rn
5. Why is Na+ smaller than Na?
Why is F- larger than F?
Why is Mg2+ smaller than Na+, despite the fact that they both have the same electronic configuration?
Which is larger out of N3- and O2, and why?
1. Which element out of Oxygen, Fluorine, Neon, Sodium, Magnesium and Aluminium has the highest second ionisation energy?
2. Why is the ionisation energy of sodium less than that of magnesium?
Why is the second ionisation energy of sodium more than the second ionisation energy of magnesium?
3. Why do neon and sodium have such very different first ionisation energies?
4. Place in asending order the ionisation energies of,
a) F+, F, F-
b) Cl, Br, I
c) Fr, Ra, Rn
5. Why is Na+ smaller than Na?
Why is F- larger than F?
Why is Mg2+ smaller than Na+, despite the fact that they both have the same electronic configuration?
Which is larger out of N3- and O2, and why?
indigogirl
Some help with these questions would be great:
1. Which element out of Oxygen, Fluorine, Neon, Sodium, Magnesium and Aluminium has the highest second ionisation energy?
2. Why is the ionisation energy of sodium less than that of magnesium?
Why is the second ionisation energy of sodium more than the second ionisation energy of magnesium?
3. Why do neon and sodium have such very different first ionisation energies?
4. Place in asending order the ionisation energies of,
a) F+, F, F-
b) Cl, Br, I
c) Fr, Ra, Rn
5. Why is Na+ smaller than Na?
Why is F- larger than F?
Why is Mg2+ smaller than Na+, despite the fact that they both have the same electronic configuration?
Which is larger out of N3- and O2, and why?
1. Which element out of Oxygen, Fluorine, Neon, Sodium, Magnesium and Aluminium has the highest second ionisation energy?
2. Why is the ionisation energy of sodium less than that of magnesium?
Why is the second ionisation energy of sodium more than the second ionisation energy of magnesium?
3. Why do neon and sodium have such very different first ionisation energies?
4. Place in asending order the ionisation energies of,
a) F+, F, F-
b) Cl, Br, I
c) Fr, Ra, Rn
5. Why is Na+ smaller than Na?
Why is F- larger than F?
Why is Mg2+ smaller than Na+, despite the fact that they both have the same electronic configuration?
Which is larger out of N3- and O2, and why?
1. Sodium. Out of all the elements there, only Sodium has a stable 1+ ion. Stable usually means energetically stable, which means a large amount of energy is required to move it from that state (in either direction).
2. First question: Na has one less proton thus has a weaker electric attraction to its outter electron than Mg.
Second question: refer to last question. Mg+ is not stable as Na+ as Na+ only has full shells.
3.
Reply 2
all particle sizes are governed by three factors:
1. The number of energy shells - more shells = bigger particles
2. The attraction between the positive nucleus and the outer electrons - more positive charge = greater attractive force on the outer shell electrons (and the others, but we're not concerned with them) = smaller size
3. More electrons for the same number of protons = bigger particle due to inter-electron repulsions.
Apply these three ideas in order of importance 1, 2, 3 and you won't go far wrong.
For example:
only apply (2) IF number of shells is the same
only apply (3) IF number of shells is the same AND the number of protons is the same
1. The number of energy shells - more shells = bigger particles
2. The attraction between the positive nucleus and the outer electrons - more positive charge = greater attractive force on the outer shell electrons (and the others, but we're not concerned with them) = smaller size
3. More electrons for the same number of protons = bigger particle due to inter-electron repulsions.
Apply these three ideas in order of importance 1, 2, 3 and you won't go far wrong.
For example:
only apply (2) IF number of shells is the same
only apply (3) IF number of shells is the same AND the number of protons is the same
yep charco is right..
for example on question 2, the ionisation energy of sodium is less than that of magnesium because magnesium has a higher nuclear charge (greater proton number) and so there is a greater attraction between the outer electrons and the nucleus. the atomic radius doesn't really play a big factor here because across a period electrons are added to the same shell...which also means that they experience the same amount of sheilding.
remember also.....
key factor for ionisation energy across a period is nuclear charge.
key factor for ionisation energy down a group is atomic radius and electron sheilding.
umm il skip to question 5 as im not quite sure on 3 n 4 at the moment! Na+ is smaller than Na because its given away an electron and as it only had one electron in its outer shell...that shell no longer remains when the electron is removed. Na will have 3 shells whereas Na+ has 2....so the atomic radius will be smaller.
umm im not sure here but i think the N3- is larger than the O2 because of the same reason above ^
Mg2+ is smaller than Na+ as remember...atoms get smaller across a period. the proton number (nuclear charge) increases as the outer electrons are added to the same shell so the attraction between the nucleus and outer electrons increases...making the atom smaller!
hope thats helped!
for example on question 2, the ionisation energy of sodium is less than that of magnesium because magnesium has a higher nuclear charge (greater proton number) and so there is a greater attraction between the outer electrons and the nucleus. the atomic radius doesn't really play a big factor here because across a period electrons are added to the same shell...which also means that they experience the same amount of sheilding.
remember also.....
key factor for ionisation energy across a period is nuclear charge.
key factor for ionisation energy down a group is atomic radius and electron sheilding.
umm il skip to question 5 as im not quite sure on 3 n 4 at the moment! Na+ is smaller than Na because its given away an electron and as it only had one electron in its outer shell...that shell no longer remains when the electron is removed. Na will have 3 shells whereas Na+ has 2....so the atomic radius will be smaller.
umm im not sure here but i think the N3- is larger than the O2 because of the same reason above ^
Mg2+ is smaller than Na+ as remember...atoms get smaller across a period. the proton number (nuclear charge) increases as the outer electrons are added to the same shell so the attraction between the nucleus and outer electrons increases...making the atom smaller!
hope thats helped!
Reply 4
Q3.
Sodium's outer electron is in a 3s orbital
Neon's is in a 2p orbital, which is lower in energy / closer to the nucleus.
So it takes more energy to remove the 2pelectron in Ne than the 3s electon in Na.
(The relative energies of the orbitals outweigh the fact that the sodium has a greater nuclear charge)
Q4a) count the # of protons and electrons in each particle.
b) look at atomic radius / the orbital the outermost electron is in
c) look at atomic radius and nuclear charge.
Sodium's outer electron is in a 3s orbital
Neon's is in a 2p orbital, which is lower in energy / closer to the nucleus.
So it takes more energy to remove the 2pelectron in Ne than the 3s electon in Na.
(The relative energies of the orbitals outweigh the fact that the sodium has a greater nuclear charge)
Q4a) count the # of protons and electrons in each particle.
b) look at atomic radius / the orbital the outermost electron is in
c) look at atomic radius and nuclear charge.
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