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(Created page with "==Key Stage 4== ===Meaning=== Reactivity is how vigorously a chemical will react. ===About Reactivity=== : Reactivity is determined by how e...")
 
 
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===About Reactivity===
 
===About Reactivity===
 
: [[Reactivity]] is determined by how easily an [[element]] can lose or gain [[electron]]s.
 
: [[Reactivity]] is determined by how easily an [[element]] can lose or gain [[electron]]s.
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: [[Electron]]s are held in [[orbit]] around the [[Atomic Nucleus|nucleus]] because the [[electron]]s are [[Negative Charge|negatively charged]] and are attracted to the [[Atomic Nucleus|nucleus]] which is [[Positive Charge|positively charged]].
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: If an [[element]] loses [[electron]]s easily it is highly '''reactive'''.
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: If an [[element]] gains [[electron]]s readily it is also highly '''reactive'''.
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Three important factors affect [[reactivity]] of [[element]]s.
 
Three important factors affect [[reactivity]] of [[element]]s.
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*The [[charge]] of the [[Atomic Nucleus|nucleus]]
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*The [[Electrical Charge|charge]] of the [[Atomic Nucleus|nucleus]]
 
*The shielding effect of inner [[electron]]s.
 
*The shielding effect of inner [[electron]]s.
 
*Distance between the [[Atomic Nucleus|nucleus]] and the [[Outer Shell|outer shell]].
 
*Distance between the [[Atomic Nucleus|nucleus]] and the [[Outer Shell|outer shell]].
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====Reactivity in Groups 1, 2 and 3====
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{| class="wikitable"
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|-
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|[[File:Group1ElectronShells.png|center|100px]]
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|[[File:Group1ElectronShielding.png|center|100px]]
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| style="height:20px; width:400px; text-align:left;" |In a [[Chemical Reaction|chemical reaction]] the [[electron]] in the [[Outer Shell|outer shell]] is lost.
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The [[reactivity]] increases as you go down the group because:
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*The outer [[electron]] is further away from the [[Atomic Nucleus|nucleus]] with each additional [[Electron Orbital|electron shell]] making the [[force]] of [[attract]]ion weaker. This makes it easier for an [[atom]] to lose it's outer [[electron]].
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*Even though the [[Electrical Charge|charge]] of the [[Atomic Nucleus|nucleus]] increases the outer [[electron]] is shielded from most of the [[Positive Charge|positive charge]] of the [[Atomic Nucleus|nucleus]] by [[electron]]s in the inner shells.
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|}
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====Reactivity in Group 7====
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{| class="wikitable"
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|-
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|[[File:Group7ElectronShells.png|center|100px]]
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|[[File:Group7ElectronShielding.png|center|100px]]
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| style="height:20px; width:400px; text-align:left;" |In a [[Chemical Reaction|chemical reaction]] an extra [[electron]] is added to the [[Outer Shell|outer shell]].
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The [[reactivity]] decreases as you go down the group because:
 +
*The outer [[electron]]s are further away from the [[Atomic Nucleus|nucleus]] with each additional [[Electron Orbital|electron shell]] making the [[force]] of [[attract]]ion weaker. This makes it less able to gain an extra [[electron]].
 +
*Even though the [[Electrical Charge|charge]] of the [[Atomic Nucleus|nucleus]] increases the outer [[electron]]s are shielded from most of the [[Positive Charge|positive charge]] of the [[Atomic Nucleus|nucleus]] by [[electron]]s in the inner shells.
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|}
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====Reactivity along Period 2====
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{| class="wikitable"
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|-
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|[[File:Period2ElectronShells.png|center|600px]]
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|-
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|[[File:Period2ElectronShielding.png|center|600px]]
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|-
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| style="height:20px; width:600px; text-align:left;" |For the first 3 [[element]]s [[Lithium]], [[Beryllium]] and [[Boron]] all lose [[electron]]s in [[Chemical Reaction|chemical reactions]].
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The [[reactivity]] decreases as you go across the [[Period (Chemistry)|period]] because:
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*The outer [[electron]]s are all roughly the same distance away from the [[Atomic Nucleus|nucleus]].
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*The [[Electrical Charge|charge]] on the [[Atomic Nucleus|atomic nucleus]] increases as you move go across the [[period]] but the [[electron]] shielding caused by the two inner [[electron]]s remains the same. This causes the [[electron]]s to experience a greater [[force]] of [[attraction]] as you move along the [[period]], making it harder for the [[atom]]s to lose [[electron]]s and become [[ion]]s.
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[[Nitrogen]], [[Oxygen]] and [[Fluorine]] can all gain [[electron]]s to become [[Negative Charge|negative]] [[ion]]s in certain [[Chemical Reaction|reaction]]s.
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The [[reactivity]] increases as you go across the [[Period (Chemistry)|period]] because:
 +
*The outer [[electron]]s are all roughly the same distance away from the [[Atomic Nucleus|nucleus]].
 +
*The [[Electrical Charge|charge]] on the [[Atomic Nucleus|atomic nucleus]] increases as you move go across the [[period]] but the [[electron]] shielding caused by the two inner [[electron]]s remains the same. This causes the [[electron]]s to experience a greater [[force]] of [[attraction]] as you move along the [[period]], making it easier for an [[atom]]s to gain more [[electron]]s to become [[ion]]s.
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|}
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===References===
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====AQA====
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:[https://www.amazon.co.uk/gp/product/0198359381/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359381&linkCode=as2&tag=nrjc-21&linkId=47c8d1ae58d8b3a5e2094cd447154558 ''Reactivity; alkali metals, pages 26-27, GCSE Chemistry; Third Edition, Oxford University Press, AQA '']
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:[https://www.amazon.co.uk/gp/product/0198359381/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359381&linkCode=as2&tag=nrjc-21&linkId=47c8d1ae58d8b3a5e2094cd447154558 ''Reactivity; metals, pages 26-27, 84-89, 220-221, GCSE Chemistry; Third Edition, Oxford University Press, AQA '']
 +
:[https://www.amazon.co.uk/gp/product/0198359381/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359381&linkCode=as2&tag=nrjc-21&linkId=47c8d1ae58d8b3a5e2094cd447154558 ''Reactivity; periodicity, pages 19, 30-31, GCSE Chemistry; Third Edition, Oxford University Press, AQA '']
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====Edexcel====
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:[https://www.amazon.co.uk/gp/product/1292120215/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=1292120215&linkCode=as2&tag=nrjc-21&linkId=8f96ddb76196848bafdb124354e4cf77 ''Reactivity, pages 86-87, GCSE Chemistry, Pearson, Edexcel '']
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====OCR====
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:[https://www.amazon.co.uk/gp/product/0198359829/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359829&linkCode=as2&tag=nrjc-21&linkId=90e8d7b4f039d53035238fa0320fe00b ''Reactivity; metals, pages 70-71, 125, 133, 141-143, Gateway GCSE Chemistry, Oxford, OCR '']
 +
:[https://www.amazon.co.uk/gp/product/0198359829/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359829&linkCode=as2&tag=nrjc-21&linkId=90e8d7b4f039d53035238fa0320fe00b ''Reactivity; noble gases, page 137, Gateway GCSE Chemistry, Oxford, OCR '']
 +
:[https://www.amazon.co.uk/gp/product/0198359829/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359829&linkCode=as2&tag=nrjc-21&linkId=90e8d7b4f039d53035238fa0320fe00b ''Reactivity; practical activities, pages 264-265, Gateway GCSE Chemistry, Oxford, OCR '']
 +
:[https://www.amazon.co.uk/gp/product/0198359829/ref=as_li_tl?ie=UTF8&camp=1634&creative=6738&creativeASIN=0198359829&linkCode=as2&tag=nrjc-21&linkId=90e8d7b4f039d53035238fa0320fe00b ''Reactivity; trends in Periodic Table, pages 133, 135, 137, 142-143, Gateway GCSE Chemistry, Oxford, OCR '']

Latest revision as of 17:46, 18 December 2019

Contents

Key Stage 4

Meaning

Reactivity is how vigorously a chemical will react.

About Reactivity

Reactivity is determined by how easily an element can lose or gain electrons.
Electrons are held in orbit around the nucleus because the electrons are negatively charged and are attracted to the nucleus which is positively charged.
If an element loses electrons easily it is highly reactive.
If an element gains electrons readily it is also highly reactive.

Three important factors affect reactivity of elements.

Reactivity in Groups 1, 2 and 3

 
 
 In a chemical reaction the electron in the outer shell is lost.

The reactivity increases as you go down the group because:

Reactivity in Group 7

 
 
 In a chemical reaction an extra electron is added to the outer shell.

The reactivity decreases as you go down the group because:

Reactivity along Period 2

 
 
For the first 3 elements Lithium, Beryllium and Boron all lose electrons in chemical reactions.

The reactivity decreases as you go across the period because:

Nitrogen, Oxygen and Fluorine can all gain electrons to become negative ions in certain reactions.

The reactivity increases as you go across the period because:


References

AQA

Reactivity; alkali metals, pages 26-27, GCSE Chemistry; Third Edition, Oxford University Press, AQA
Reactivity; metals, pages 26-27, 84-89, 220-221, GCSE Chemistry; Third Edition, Oxford University Press, AQA
Reactivity; periodicity, pages 19, 30-31, GCSE Chemistry; Third Edition, Oxford University Press, AQA

Edexcel

Reactivity, pages 86-87, GCSE Chemistry, Pearson, Edexcel

OCR

Reactivity; metals, pages 70-71, 125, 133, 141-143, Gateway GCSE Chemistry, Oxford, OCR
Reactivity; noble gases, page 137, Gateway GCSE Chemistry, Oxford, OCR
Reactivity; practical activities, pages 264-265, Gateway GCSE Chemistry, Oxford, OCR
Reactivity; trends in Periodic Table, pages 133, 135, 137, 142-143, Gateway GCSE Chemistry, Oxford, OCR
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