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Ionisation Energy

Some elements just seem to want to react. You expose them to the air, sprinkle them with a tiny drop of water, and wham! They’ve reacted. Take sodium, for example. Sodium is a relatively unassuming Group 1 metal with 11 electrons, yet it must be stored in oil to keep it from reacting with any water vapour in the air. As soon as you drop it in a basin of water, it’ll fizz violently, produce a flame, and turn a green universal indicator solution pink. But neon, which contains just one less electron than sodium, will not react with water at all. An element’s reactivity is all to do with its ability to form ions, and for some elements, this is easier than for others.

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StudySmarter Editorial Team

Team Ionisation Energy Teachers

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    Flashcards in Ionisation Energy 2

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    As the distance between the outer shell electron and the nucleus increases, ionisation energy:


    Decreases

    As the number of inner electron shells increases, ionisation energy:


    Decreases
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    Frequently Asked Questions about Ionisation Energy

    What is ionisation energy?

    Ionisation energy is the energy required to remove one mole of electrons from one mole of gaseous atoms under standard conditions.

    What is the first ionisation energy of an element?

    The first ionisation energy is the energy required to remove one mole of the outermost electrons from one mole of gaseous atoms under standard conditions.

    Why is the second ionisation energy greater than the first?

    The second ionisation energy is greater than the first because an electron is removed from a positive ion, which requires more energy.

    What is the second ionisation energy?

    The second ionisation energy is the energy required to remove one mole of the next outermost electrons from one mole of gaseous cations that have a charge of +1.

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