Far as I am aware a larger atom (They get bigger going down the table) has its electrons orbiting farther from the nucleus so it has a more tenous hold on them, so they can be lost easier. A reaction is just the exchange of electrons. Most metals (or all, not sure) lose electrons in a reaction. Because non metals have to gain them in a reaction, the smaller the atom the better the grip they can get on them. (electric grip)
The number of energy levels increase within a group. Therefor the atomic radius increases. So the atomic volume also increases.The atomic radius also increases in a group.For metals, reactivity increases down the group. For non-metals, reactivity decreases down a group.
The first cloumn in the periodic table has the most reactive elements. The elements decrease in reactivity as you go across the table. in other words alkali metals
reactivity
any metals that are below copper in the reactivity series
Metals which are above Carbon in the reactivity series, eg. Magnesium. These metals need to be extracted by electrolysis.
The chemical reactivity of alkali metals increase when the atomic number increase.
The number of energy levels increase within a group. Therefor the atomic radius increases. So the atomic volume also increases.The atomic radius also increases in a group.For metals, reactivity increases down the group. For non-metals, reactivity decreases down a group.
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The reactivity increase down in the group.
the reactivity in presence of heat or another reactive element increases down the group due to increase in atomic size but in water reactivity decrease down the group due to decrease in charge density ,the smaller ion forms strong bonds with water molecules.
Melting points generally decrease as you go down a group for group I and group II metals. This does not apply to the transition metals. Reactivity of metals increases down a group due to a larger size and less effective charge between the nucleus and valence electrons. Atomic radius increases due to a higher principle number of electrons.
Reactivity in group 1 of elements increases as we go down the group (to francium) because in the alkali metals as we go down the group number of atomic shells increases so the elements with most shells will easily release their electrons in the outer most shell.
Maybe there is no pattern...no it fals
In the alkali metals column (Group 1), atomic radius increases down the group and reactivity increases. There are more shells preventing the attraction between the positive nucleus and negatively charged outer electron. (All Group 1 elements have 1 electron in their outer shell). Also, because they contain more shells down the group, the distance between the nucleus and electrons is increased. Therefore the electrostatic force is lessened between them. Both of these allow the outer electron to be lost easier to other elements, thus increasing reactivity.
Because the atomic radius increases down the group 1 and decreases down the group of halogen
yes, some transition metals like gold(Au) are almost unreactive.
The reactivity of metals is used to transfer electricity without much electrical loss.