Why does the first ionisation energy of atoms generally increase across a period?
The first ionisation energy is defined as the energy required to remove one mole of electrons from each atom of a mole of gaseous atoms. As we go along a period in the periodic table, the atomic number increases. As the atomic number increases, the number of protons in the nucleus increases. This causes the electrostatic attraction between the nucleus and the outermost electron to generally become stronger across a period.
Related Chemistry A Level answers
All answers ▸The ionic product of water, Kw = 2.93 × 10−15 mol dm−6 at 10 °C. Calculate the pH of a 0.0131 mol dm−3 solution of calcium hydroxide at 10 °C Give your answer to two decimal places.
How do you calculate the equilibrium constant, Kc, of a reaction?
Explain why the first ionisation energy of strontium is less than the first ionisation energy of calcium
Give and explain 2 of the anomalous properties of ice caused by hydrogen bonding