Ionisation energies Flashcards

1
Q

What does it mean when an electrons have been removed from an atom or molecule?

A

It has been ionised.

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2
Q

What is the energy you need to remove the first electron called?

A

The first ionisation energy.

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3
Q

What is the first ionisation energy?

A

The first ionisation energy is the energy needed to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous 1+ ions.

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4
Q

How do you write equations for ionisations, e.g. the first ionisation of oxygen?

A

image

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5
Q

What symbol must you use in ionisation equations?

A

The gas state symbol, because ionisation energies are measured for gaseous atoms.

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6
Q

What should you always refer to rather than a single atom?

A

1 mole of atoms.

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7
Q

What does the lower the ionisation energy mean?

A

The easier it is to form a positive ion by removing electrons.

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8
Q

What does a high ionisation energy mean?

A

There is a high attraction between the electron and the nucleus, so more energy is needed to remove the electron.

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9
Q

What are the three factors which affect ionisation energies?

A
  • Nuclear charge
  • Distance from nucleus
  • Shielding
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10
Q

How does the nuclear charge affect ionisation energies?

A

The more protons there are in the nucleus means the more positively charged the nucleus is, causing a stronger attraction for the electrons to the nucleus.

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11
Q

How does distance from the nucleus affect ionisation energies?

A

Attraction to the nucleus falls very rapidly with distance, so an electron close to the nucleus will be much more strongly attracted than one further away.

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12
Q

How does shielding affect ionisation energies?

A

As the number of electrons increases, the outer electrons are shielded by the inner electrons (blocked by the electrons) this causes less attraction from the outer electrons to the nucleus

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13
Q

h

A

h

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14
Q

h

A

h

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15
Q

h

A

h

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