The activity of any element depends on the number of electrons it has in its outer energy level, called valence electrons. Atoms in group one, metals have only one electron in their outer energy level, instead of two so they have incomplete outer energy levels; they are always looking to lose or share their electron with another atom to complete their outer energy level and become more stable. In contrast, the noble gases have complete outer energy levels so they do not interact with other elements. Thus, knowing the electron configuration enables you to determine the valence electrons and predict the reactivity of an element.
Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
An activity series is used to predict whether metals will displace hydrogen gas from water and acid solutions. It is also used to predict whether metals will displace other metals.
color, magnetism, conductivity to name a few.
Alkali metals are more reactive as they are in group 1 and therefore has only one valence electron. With only one valence electron, its easy for them to achieve inert configuration/ noble gas configuration, which makes them so reactive.
There are no similarities. Noble gases (group 18 elements) have completely filled orbitals with stable electron configuration and are generally unreactive. Alkali metals (group 1 elements) have one valence electron. They are reactive. When these lose one electron, they form ions which has the electronic configuration of the nearest noble gas.
Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
An activity series is used to predict whether metals will displace hydrogen gas from water and acid solutions. It is also used to predict whether metals will displace other metals.
The transition metals
Alkali metals are more reactive as they are in group 1 and therefore has only one valence electron. With only one valence electron, its easy for them to achieve inert configuration/ noble gas configuration, which makes them so reactive.
color, magnetism, conductivity to name a few.
2 electrons in the outermost shell.
The electron configuration of hydrogen is similar with that of alkali metals.
By using the activity series (sometimes called reactivity series) which orders metals by their reactivity with other metals, one can determine the reactivity of a metal
No. Hydrogen is a nonmetal. It is only put in the alkali metal column because it has a similar electron configuration.
There are no similarities. Noble gases (group 18 elements) have completely filled orbitals with stable electron configuration and are generally unreactive. Alkali metals (group 1 elements) have one valence electron. They are reactive. When these lose one electron, they form ions which has the electronic configuration of the nearest noble gas.
The Alkali Metals loose one electron in order to achieve a nobel gas configuration.
The valance electron configuration is the same in each at ns1 where n = the period number.