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LogicalAcid
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Because, if a higher electronegativity means a higher attraction to electrons an atom has, wouldn't that mean that a greater energy would have to be put into ionise an atom with a higher electronegativity?
The ionisation energy generally increases with electronegativity. This is because as the electronegativity of an atom increases, it becomes more difficult to remove an electron from its outer energy level. Therefore, more energy is required to remove an electron, resulting in a higher ionisation energy.
Yes, there is a direct relationship between ionisation energy and electronegativity. As the electronegativity of an atom increases, its ionisation energy also increases. This is because electronegativity is a measure of an atom's ability to attract electrons, and a higher electronegativity indicates a stronger attraction for electrons.
The size of an atom has an inverse relationship with its ionisation energy and electronegativity. As the size of an atom increases, its ionisation energy decreases because the electrons are further from the nucleus and are therefore easier to remove. Similarly, electronegativity decreases with increasing atomic size because the larger size of the atom reduces its ability to attract electrons.
Yes, ionisation energy and electronegativity can be used to predict chemical reactivity. Elements with low ionisation energy and high electronegativity tend to be more reactive because they readily lose electrons and attract electrons from other elements to form chemical bonds.
The periodic trend of ionisation energy follows a similar pattern to electronegativity. Both increase from left to right across a period and decrease from top to bottom in a group. This is because as you move from left to right across a period, the number of protons and the nuclear charge increase, making it more difficult to remove an electron. As you move down a group, the atomic size increases, resulting in a weaker attraction for electrons.