chemistry
In their reactions, calcium and strontium each lose electrons to form ions with a 2 charge.
The first and second ionisation energies of calcium and strontium are shown below.
1st ionisation energy / kJ mol–1 2nd ionisation energy / kJ mol–1
calcium 590 1145
strontium 550 1064
Why are the second ionisation energies of calcium and strontium greater than their first ionisation energies?
The first and second ionisation energies of calcium and strontium are shown below.
1st ionisation energy / kJ mol–1 2nd ionisation energy / kJ mol–1
calcium 590 1145
strontium 550 1064
Why are the second ionisation energies of calcium and strontium greater than their first ionisation energies?
is this bond energy??
Original post by Mokhions
In their reactions, calcium and strontium each lose electrons to form ions with a 2 charge.
The first and second ionisation energies of calcium and strontium are shown below.
1st ionisation energy / kJ mol–1 2nd ionisation energy / kJ mol–1
calcium 590 1145
strontium 550 1064
Why are the second ionisation energies of calcium and strontium greater than their first ionisation energies?
The first and second ionisation energies of calcium and strontium are shown below.
1st ionisation energy / kJ mol–1 2nd ionisation energy / kJ mol–1
calcium 590 1145
strontium 550 1064
Why are the second ionisation energies of calcium and strontium greater than their first ionisation energies?
It requires more energy as the electrons are being removed from a positive ion.
The positive nuclear charge stays the same but the number of electrons is reduced. So each individual electron is more effected by the nuclear charge.
The positive nuclear charge stays the same but the number of electrons is reduced. So each individual electron is more effected by the nuclear charge.
(edited 3 years ago)
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