1s2 2s2 2p6 3s2 3p6
The rule you are referring to is the octet rule. It states that representative elements tend to form chemical bonds in a way that they achieve a stable electron configuration with eight electrons in their outermost shell. This provides the atoms with greater stability and is commonly observed in elements that are not in the transition metals group.
The maximum number of electrons that a representative element can possess is 8. This is because the outermost electron shell of these elements can hold a maximum of 8 electrons in order to achieve a stable electron configuration.
Elements tend not to undergo chemical reactions that decrease stability. Chemical reactions typically result in products that are more stable than the reactants involved. Elements tend to form compounds to achieve a more stable electron configuration.
Because emission spectrum are the result of the electron configuration of the element and no two elements have exactly the same electron configuration.
Electron configurations are only made for pure elements. The electron configuration for Hydrogen is 1s1. The electron configuration for Oxygen is 1s2 2s2 2p4
Groups 1, 2, and 13-18.
Every elements have the electrons of an atom distribution or a molecule in molecular orbitals and it is called electron configuration. The element that can be grouped in the family with above electron configuration is called antimony.
Electron configuration is a term applied to chemical elements not to compounds.
The outermost s sublevel of the representative elements is filled first, followed by the p sublevel. This results in the outermost electron configuration being in the s and p sublevels.
The rule you are referring to is the octet rule. It states that representative elements tend to form chemical bonds in a way that they achieve a stable electron configuration with eight electrons in their outermost shell. This provides the atoms with greater stability and is commonly observed in elements that are not in the transition metals group.
The group of elements that have a stable electron configuration are the noble gases.
The maximum number of electrons that a representative element can possess is 8. This is because the outermost electron shell of these elements can hold a maximum of 8 electrons in order to achieve a stable electron configuration.
The outer electron configuration for all group 1 elements is ns1, where n represents the energy level of the outermost electron. This means that group 1 elements have one electron in their outermost shell.
Elements tend not to undergo chemical reactions that decrease stability. Chemical reactions typically result in products that are more stable than the reactants involved. Elements tend to form compounds to achieve a more stable electron configuration.
Because emission spectrum are the result of the electron configuration of the element and no two elements have exactly the same electron configuration.
Electron configurations are only made for pure elements. The electron configuration for Hydrogen is 1s1. The electron configuration for Oxygen is 1s2 2s2 2p4
Elements in family 1 are very reactive because they have one electron in their outermost shell, making them highly likely to lose that electron to achieve a stable electron configuration. This results in the formation of positive ions, which allows these elements to readily bond with other elements to achieve stability.