Elements in group two become more stable as they all have complete electron shell.They do not have valence electrons and hence they are less reactive.Some of the elements of group 2 are Barium,Magnesium and Calcium
The elements in Group 7A (halogens) on the periodic table would need only 1 electron to achieve a stable electron configuration by filling their outermost shell with 8 electrons. For example, elements like fluorine, chlorine, and bromine each need only 1 more electron to reach stability.
Halogens have the highest electron affinity among all elements. This is because halogens have a strong tendency to gain an electron to achieve a full outer energy level and become stable.
Elements in group 1 (alkali metals) have 1 valence electron. This single electron is in the outermost energy level of the atom, making these elements very reactive and likely to lose this electron to achieve a stable electron configuration.
Elements in group 17 (Halogens) such as fluorine, chlorine, bromine, iodine, and astatine will become more stable by gaining one electron to achieve a full outer electron shell and form a negatively charged ion.
Group 1 elements (alkali metals) prefer to combine with Group 17 elements (halogens) because alkali metals have one electron in their outer shell, which they can easily donate to achieve a stable electron configuration. Halogens, on the other hand, have seven electrons in their outer shell and can easily accept an electron to achieve a stable electron configuration. This electron transfer results in the formation of ionic compounds between alkali metals and halogens.
The group of elements that have a stable electron configuration are the noble gases.
i guess you mean that the group 1 elements usually lose a electron in order to become stable because the outermost of the group 1 elements have only one valence electron and it is easy to lose one than to gain seven.
It is in Group 17 that you will find the most reactive elements. These elements all lack only one electron from having that "magic" electron configuration of the inert gases. That makes these elements very "hungry" to get that "last electron" so their electron structures become more stable.
The elements in Group 7A (halogens) on the periodic table would need only 1 electron to achieve a stable electron configuration by filling their outermost shell with 8 electrons. For example, elements like fluorine, chlorine, and bromine each need only 1 more electron to reach stability.
Halogens have the highest electron affinity among all elements. This is because halogens have a strong tendency to gain an electron to achieve a full outer energy level and become stable.
Group 1 metals, such as sodium and potassium, readily combine with group 17 elements (halogens) to form salts. These metals have one electron in their outermost shell, which they can easily lose to achieve a stable electron configuration, while halogens are one electron short of a stable configuration and readily accept an electron to form a stable ion.
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.
Elements in group 1 (alkali metals) have 1 valence electron. This single electron is in the outermost energy level of the atom, making these elements very reactive and likely to lose this electron to achieve a stable electron configuration.
Elements in group 17 (Halogens) such as fluorine, chlorine, bromine, iodine, and astatine will become more stable by gaining one electron to achieve a full outer electron shell and form a negatively charged ion.
Group 1 elements (alkali metals) prefer to combine with Group 17 elements (halogens) because alkali metals have one electron in their outer shell, which they can easily donate to achieve a stable electron configuration. Halogens, on the other hand, have seven electrons in their outer shell and can easily accept an electron to achieve a stable electron configuration. This electron transfer results in the formation of ionic compounds between alkali metals and halogens.
Group 17 elements, also known as halogens, typically gain one electron to achieve a full outer electron shell. Group 1 elements, known as alkali metals, often lose one electron to achieve a stable electron configuration.
Metals typically become cations by losing electrons to attain a stable electron configuration. Transition metals and main group metals are common examples of elements that form cations.