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elements in the halogen family react easily with other elements whose atoms can give up electrons.alkali metals lose one electron they are left with 0 valence electrons and they become more chemically stable
The atomic radii of members of the Group 1A (Alkali metals), increases down the group. Therefore Francium has the largest atomic radius of the Alkali metals. However Fr has no stable isotopes, thus is not naturally occurring. So Cs-133 is the largest you can find.
Alkali metals, such as sodium and potassium, are highly reactive and tend to combine quickly with other elements in nature to form compounds. This is because they have only one valence electron, which they easily lose to achieve a stable electron configuration. Therefore, it is rare to find pure alkali metals in their elemental form in nature.
Alkali Metals are group One elements and have one electron in their outer electron shell. In order to become stable they tend to lose an electron by reacting with something that needs an electron to become stable such as a group seven halogen. The Alkali Metal then become positive ions.This is because they only have on valance electron. This makes it easier to react with other elements and more often also.
Alkali metals, have only one valence electron so they will "want" to lose it to achieve a stable electron arrangement.
transition elements are not as reactive as alkali metals or alkaline earth metals.. this is so because of the valence electronic configurations. alkali metals have ns1 configurations which have easy chances of loosing electrons so as to gain the stable state. Attaining a stable state is the law of nature. hence to attain it they have to redily donate electron. this is not so easily possible for the transition elements..
The most stable elements are found in the Noble Gases, in group 8 or group 0. The most UNstable elements are found in the alkali metals.
Highly active metals are the most easily oxidized because they react with oxygen easily.
elements in the halogen family react easily with other elements whose atoms can give up electrons.alkali metals lose one electron they are left with 0 valence electrons and they become more chemically stable
The atomic radii of members of the Group 1A (Alkali metals), increases down the group. Therefore Francium has the largest atomic radius of the Alkali metals. However Fr has no stable isotopes, thus is not naturally occurring. So Cs-133 is the largest you can find.
Alkali metals, such as sodium and potassium, are highly reactive and tend to combine quickly with other elements in nature to form compounds. This is because they have only one valence electron, which they easily lose to achieve a stable electron configuration. Therefore, it is rare to find pure alkali metals in their elemental form in nature.
Alkali metals, like sodium and potassium, typically form ionic bonds. These metals have one valence electron that is easily transferred to another element to achieve a stable electron configuration. As a result, they form positive ions and bond with elements that readily accept electrons, such as halogens or nonmetals.
There are 7 elements in group 1: hydrogen, lithium, sodium, potassium, rubidium, cesium, and francium. All of these (except hydrogen) are considered alkali metals. They react very easily with other elements.
Alkali Metals are group One elements and have one electron in their outer electron shell. In order to become stable they tend to lose an electron by reacting with something that needs an electron to become stable such as a group seven halogen. The Alkali Metal then become positive ions.This is because they only have on valance electron. This makes it easier to react with other elements and more often also.
Alkali metals have increasing reactivity going down the group. Francium may not be considered as it is not a stable atom: it is radioactive. The next four are Cesium, Rubidium, Potassium and Sodium in decreasing reactivity order.
Alkali metals, have only one valence electron so they will "want" to lose it to achieve a stable electron arrangement.
Noble gases are most stable due to the presence of octet of electrons