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State and explain the general trend in the first ionisation energy across a period.

First, let's check we understand the concept of the first ionisation energy . The term is defined as 'the energy required to remove a mole of electrons from a mole of gaseous atoms'. That is, for each atom i...
BM
Answered by Ben M. • Chemistry tutor
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Giving the electronic configurations for each element, predict the trend in 1st ionisation energies going across period 2 from Lithium to Neon.

First start by giving the definition of first ionisation energy - the energy required to remove one mole of electrons from one mole of gaseous atoms to produce one mole of gaseous ions each with a +1 charge,...
AB
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i)Explain why first ionisation energy shows a general tendency to increase across a period? ii)Using period 3 as an example, which elements show irregularities in this trend and why?

i)As you move across a period the number of protons in the nucleus, and so the overall nuclear charge, increases. All extra electrons are roughly the same energy and distance from the nucleus. This means the...
DM
Answered by David M. • Chemistry tutor
7797 Views

Explain why the first ionisation energy of sulfur is different from that of phosphorus.

The first ionisation energy is defined as, the amount of energy required to remove 1 mole of electrons from 1 mole of gaseous atoms to produce 1 mole of gaseous ions , with a single positive charge. (By dete...
LM
Answered by Lydia M. • Chemistry tutor
87150 Views

Can you give and explain the mechanism for the reaction between aqueous Sodium Hydroxide (NaOH) and Chloroethane at room temperature? What is a competing reaction which may occur and how would you promote this reaction?

Chlorine is highly electronegative and hence electron withdrawing (briefly ask them what electronegativity is to make sure they're completely comfortable with the concept), so the carbon its directly attache...
ND
Answered by Ned D. • Chemistry tutor
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