Describe the octet rule in terms of noble-gas configurations and potential energy?

Answer 1

"Noble gas configuration" means that in writing out an electron configuration for an atom, rather than writing out the occupation of each and every orbital specifically, you instead lump all of the core electrons together and designate it with the symbol of the corresponding noble gas on the Periodic Table (in brackets). For example, the noble gas configuration of oxygen is [He]2s22p4

Answer 2

The octet rule is a simple rule of thumb that states that atoms tend to combine in such a way that they each have eight electrons in their valence shells, giving them the same electron configuration as a noble gas. The rule is applicable to the main-group elements. In simple terms, molecules or ions tend to be most stable when the outermost electron shells of their constituent atoms contain eight electrons .

Answer 3

The octet noble gas configuration is an outer electron shell that contains 8 electrons, which is a stable arrangement, that most noble gases have (helium however, has only 2 outer electrons, because it is too small to have a second electron shell, as the other noble gases do). Octet simply means a group of 8.

Answer 4

The octet rule states that atoms tend to gain, lose, or share electrons to achieve a stable electron configuration with a full valence shell of eight electrons, resembling a noble gas configuration. This stability is associated with lower potential energy for the atom, as it becomes more energetically favorable to have a full valence shell.

Answer 5

The valence level is always full. It can not give away an electron or gain an electron. The outer most energy level or sublevel is filled with the maximum number of electrons.