rpatel said:
compare nuclear charge and shielding effect. guess i can't tell you too much since you didnt even try the qn As semc indicated, the point of learning is to understand the subject, not simply to answer test questions! semc also points you in the right direction. What determines the binding energy of an atomic electron?rpatel said:
Ionisation energy is the amount of energy required to remove an electron from an atom or molecule, resulting in the formation of an ion.
Ionisation energy is important because it helps us understand the chemical reactivity and stability of atoms and molecules. It also plays a crucial role in the formation of chemical bonds and the behavior of elements in different chemical reactions.
Ionisation energy is measured in units of energy such as joules (J) or electron volts (eV). It can be measured experimentally by using various techniques, such as spectroscopy, mass spectrometry, and electron impact ionisation.
The main factors that affect ionisation energy include the atomic or molecular structure, the number of protons in the nucleus, and the distance between the outermost electron and the nucleus. Other factors such as shielding effect, electron configurations, and nuclear charge can also influence the ionisation energy of an atom or molecule.
Ionisation energy generally increases as you move from left to right across a period in the periodic table. This is because the number of protons and the nuclear charge increases, making it more difficult to remove an electron. It also decreases as you move down a group due to the shielding effect and the increasing distance between the outermost electron and the nucleus.