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
For metals, reactivity decreases as you go from left to right in a period.
This is the tendency of the atoms of an element to undergo a chemical
reaction with other elements.
In metals, the more the valence electron, the less reactive the
element.Metals which have less valence electrons have higher reactivity.
In the periodic table, the valence electron of the elements increases
across the period which translates to a decrease in reactivity.
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