Week 5 Flashcards

1
Q

Ionisation Energy

A

the minimum energy required to remove an electron from a gaseous ground state atom or ion

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2
Q

Which electrons take less energy to remove?

A

Less energy to remove the first electron from the ground state atom
More energy to to remove the remaining electrons from the resulting ions
1st IE < 2nd IE

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3
Q

Less energy to remove the first electron

A

The electron-electron repulsion or electron shielding results in a weaker attraction of the nucleus for each electron

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4
Q

More energy to remove remaining electrons

A

When the first electron is removed, in the resulting cation there are fewer electrons present so there is less shielding and the electrons feel larger effect of the nuclear charge.

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5
Q

Periodic table trends for IE

A

Across a period- first IE increases

Down a group- first IE decreases

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6
Q

Type of element with highest first IE

A

Noble gases

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7
Q

Type of element with lowest first IE

A

Group one (alkali metals)

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8
Q

Size of atoms and cations

A

Cations are smaller than neutral atoms because cation’s valence shell is pulled towards the nucleus with greater effective nuclear charge

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9
Q

Size of atoms and anions

A

Anion is bigger than neutral atoms because anion’s valence shell is pulled towards nucleus with less effective nuclear charge

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10
Q

Reactivity of elements

A

Elements lose or gain electrons to complete the octet rule.

Noble gases- totally inert chemically. All have filled valence sub-shells, a condition that represents great stability.

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11
Q

Metals across the period

A

Across the period, IE increases due to greater core charge. As it increases, metals become less reactive as they lose electrons in chemical reactions

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12
Q

Metals down the group

A

Down the group, IE decreases and the metals become more reactive due to greater shielding effect

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13
Q

Non-metals across the period

A

Across the period, non-metals become more reactive because of increasing trend in electronegativity due to greater core charge

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14
Q

Non-metals down the group

A

Down the group, electronegativity decreases, due to greater shielding effect and non-metals become less reactive.

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15
Q

nth IE

A

removal of nth electron from gaseous ground +(n-1) cation

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