Difference between revisions of "Reactivity"
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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]]. | | 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]]. | ||
| − | The [[reactivity]] decreases as you go across the [[Period (Chemistry)|period]]: | + | The [[reactivity]] decreases 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 outer [[electron]]s are all roughly the same distance away from the [[Atomic Nucleus|nucleus]]. |
*The [[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. | *The [[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. | ||
| − | + | [[Nitrogen]], [[Oxygen]] and [[Fluorine]] can all gain [[electron]]s to become [[Negative Charge|negative]] [[ion]]s in certain [[reaction]]s. | |
| + | The [[reactivity]] increases as you go across the [[Period (Chemistry)|period]]: | ||
| + | *The outer [[electron]]s are all roughly the same distance away from the [[Atomic Nucleus|nucleus]]. | ||
| + | *The [[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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Revision as of 19:49, 5 December 2018
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.
- The charge of the nucleus
- The shielding effect of inner electrons.
- Distance between the nucleus and the outer shell.
Reactivity in Groups 1, 2 and 3
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In a chemical reaction the electron in the outer shell is lost.
The reactivity increases as you go down the group because:
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Reactivity in Group 7
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In a chemical reaction an extra electron is added to the outer shell.
The reactivity decreases as you go down the group because:
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Reactivity along Period 2
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| 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:
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