How does reactivity change as move along a period or fowd a group. Does it depend on whether the element is metal or a non metal?
How does reactivity change as move along a period or fowd a group. Does it depend on whether the element is metal or a non metal?
Reactivity - Reactivity refers to how likely or vigorously an atom is to react with other substances. This is usually determined by how easily electrons can be removed (ionization energy) and how badly they want to take other atom's electrons (electronegativity) because it is the transfer/interaction of electrons that is the basis of chemical reactions.
Metals
Period - reactivity decreases as you go from left to right across a period.
Group - reactivity increases as you go down a group
Why? The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity.
Non-metals
Period - reactivity increases as you go from the left to the right across a period.
Group - reactivity decreases as you go down the group.
Why? The farther right and up you go on the periodic table, the higher the electronegativity, resulting in a more vigorous exchange of electron
Read also:
This is the background info you need to know:
As you go down a group the atomic number increases.
The number of shells of electrons also increases.
The electron shells between the outer electrons and the nucleus have a 'shielding' effect which reduces the attraction of the outer electrons to the nucleus.
The elements on the left side of the table (i.e. group 1 and 2):
These react by losing electrons and reactivity increases as you go down the group.
This is because the increased number of electron shells results in more shielding and a greater distance between the outer electrons and the nucleus, which reduces the attraction of the electrons to the nucleus. This means that less energy is needed to remove the outer electrons, so they are more easily lost.
The elements on the right side of the table (not the noble gases):
These react by gaining electrons and reactivity decreases as you go down the group.
Again, this is because of the increased number of electron shells as you do down means a greater shielding effect and a greater distance between the outer electrons and the nucleus. This time, though the result is that the incoming electrons are less attracted to the nucleus and so are less easily gained
These are the basic trends there is also some specific exceptions
Reactivity - Reactivity refers to how likely or vigorously an atom is to react with other substances. This is usually determined by how easily electrons can be removed (ionization energy) and how badly they want to take other atom's electrons (electronegativity) because it is the transfer/interaction of electrons that is the basis of chemical reactions.
Metals
Period - reactivity decreases as you go from left to right across a period.
Group - reactivity increases as you go down a group
Why? The farther to the left and down the periodic chart you go, the easier it is for electrons to be given or taken away, resulting in higher reactivity.
Non-metals
Period - reactivity increases as you go from the left to the right across a period.
Group - reactivity decreases as you go down the group.
Why? The farther right and up you go on the periodic table, the higher the electronegativity, resulting in a more vigorous exchange of electron
Read also:
This is the background info you need to know:
As you go down a group the atomic number increases.
The number of shells of electrons also increases.
The electron shells between the outer electrons and the nucleus have a 'shielding' effect which reduces the attraction of the outer electrons to the nucleus.
The elements on the left side of the table (i.e. group 1 and 2):
These react by losing electrons and reactivity increases as you go down the group.
This is because the increased number of electron shells results in more shielding and a greater distance between the outer electrons and the nucleus, which reduces the attraction of the electrons to the nucleus. This means that less energy is needed to remove the outer electrons, so they are more easily lost.
The elements on the right side of the table (not the noble gases):
These react by gaining electrons and reactivity decreases as you go down the group.
Again, this is because of the increased number of electron shells as you do down means a greater shielding effect and a greater distance between the outer electrons and the nucleus. This time, though the result is that the incoming electrons are less attracted to the nucleus and so are less easily gained
These are the basic trends there is also some specific exceptions
