![]() ![]() ![]() As a result, the likelihood of reactants to be able to react together can be determined from the Periodic Table of Elements. In all these metals there is only one free electron and these ball-shaped orbitals are denoted by 1 s, 2 s, 3 s, etc., all with an increasing average radius from the nucleus.įor all the subsequent groups, characterizations can be formulated based upon similarities in reactivity-the way they react, how many electrons can be shared, etc. The one free electron in the outer valence shell is in a so-called ns- orbital. Because these electrons are all at a greater distance from the nucleus, the energy gained from removing one electron diminishes according to the proportionality of n −2. As the mass of the nucleus increases with each neutron and proton, so also does the number of electrons (to balance the electric charge). This lowered reactivity is related to the atomic weight. Going down from Li, Na, K to Fr the reactivity decreases, but these metals react easily – for example, with water, in a very exothermic way. They are characterized by having a single electron in their outer valence orbital. On the extreme left there is a group of metals, called the alkali metals. (See the article atomic orbital for a more detailed explanation of the building up of the electronic shells.) Because they have an outer shell of electrons that is completely filled, they are inert in behavior. For instance, the right column is occupied by the noble gases. The number of electrons in the outer shells of the electron orbitals is the same within a group, only the principal quantum number n describing the orbitals increases. Elements by periodic table group (vertical column) See Atomic electron configuration for the orbital occupancies of ground state atoms.Įlements in any one group behave in a similar way and show the same overall general properties. ![]()
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