Difference between revisions of "Reactivity"

Revision as of 10:43, 6 April 2019

Reactivity is how vigorously a chemical will react.

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.

		In a chemical reaction the electron in the outer shell is lost. The reactivity increases as you go down the group because: The outer electron is further away from the nucleus with each additional electron shell making the force of attraction weaker. This makes it easier for an atom to lose it's outer electron. Even though the charge of the nucleus increases the outer electron is shielded from most of the positive charge of the nucleus by electrons in the inner shells.

		In a chemical reaction an extra electron is added to the outer shell. The reactivity decreases as you go down the group because: The outer electrons are further away from the nucleus with each additional electron shell making the force of attraction weaker. This makes it less able to gain an extra electron. Even though the charge of the nucleus increases the outer electrons are shielded from most of the positive charge of the nucleus by electrons in the inner shells.



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: The outer electrons are all roughly the same distance away from the nucleus. The charge on the atomic nucleus increases as you move go across the period but the electron shielding caused by the two inner electrons remains the same. This causes the electrons to experience a greater force of attraction as you move along the period, making it harder for the atoms to lose electrons and become ions. 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: The outer electrons are all roughly the same distance away from the nucleus. The charge on the atomic nucleus increases as you move go across the period but the electron shielding caused by the two inner electrons remains the same. This causes the electrons to experience a greater force of attraction as you move along the period, making it easier for an atoms to gain more electrons to become ions.

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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 Shell|inner shells]].
+*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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