All of them. There is no problem with elements not having stable electron configurations. The only stability issue concerns the nucleus, not the electrons-- all elements except helium have isotopes with unstable nuclei, some have only unstable nuclei (radioactive elements), and some have only very short-lived unstable nuclei.
In the Periodic Table, the far right hand column is made up of what is called the "inert gases". Inert means unreactive, which is exactly why they're called that. They aren't reactive at all and only naturally occur by themselves, not joined to any other element. As you go along the periodic table, each element has one more electron that the last, and so when you get to the inert gases, the way electrons are configured in shells, each inert gas has a full outer shell and no spare electrons. This is why they're the group that is at a stable energy level and won' react.
no one knows anything anymore why do they do these stupid websites if they dont help
Group VIIIA in the periodic table commonly used in the US. The current naming convention uses the term group 18. These are the noble gasses (e.g. Helium, Neon and Argon)
The noble gases in the far right column.
The Noble gases which is Group 18
helium, xenon, neon
Noble Gases
The electron configurations of LiF will be the same as the electron configurations of atoms in Group 18 (noble gases) because Li will lose its single electron to attain a stable octet similar to the noble gases, while F will gain an electron to achieve a complete valence shell.
The most stable number of valence electrons is 2 for hydrogen and helium, which have only one electron shell in the shell model for atomic electron configurations, and 8 for all other elements.
Stable electron configurations are most likely to contain filled energy levels or filled subshells. These configurations generally follow the octet rule or duet rule, depending on the element. Additionally, stable electron configurations may contain configurations with a full valence shell of electrons.
Inert gas configurations refer to the electron configurations of noble gases, which have a full outer electron shell. These configurations are very stable and unreactive due to their complete outer energy level. Other elements may strive to attain such configurations through chemical bonding to achieve greater stability.
Some elements achieve stable electron configurations through the transfer of electrons, which occurs in ionic bonding. This process involves one element losing electrons (cation) and another element gaining electrons (anion) to reach a stable configuration. Ionic bonding typically occurs between metals and nonmetals with significant differences in electronegativity.
No - they have much more stable configurations than the other elements in the periodic table.
protons
Some elements achieve stable electron configurations through the transfer of electrons, which occurs in ionic bonding. This process involves one element losing electrons (cation) and another element gaining electrons (anion) to reach a stable configuration. Ionic bonding typically occurs between metals and nonmetals with significant differences in electronegativity.
no
any time there are as many electrons and protons and they fill each orbital optimally.
Group 18 as they have completely filled electronic configurations, are stable and hence do not ionize.
The most stable number of valence electrons is 2 for hydrogen and helium, which have only one electron shell in the shell model for atomic electron configurations, and 8 for all other elements.
The atoms of Group 17 elements must gain one electron in order to become stable.
Yes. Helium, Xenon, and Neon have stable electron numbers (octette rule).
6
A stable electron configuration refers to an atom in which the outer electron shell is full. Outermost electron shells hold a maximum of 2, 8, 8, 18,...(etc.) electrons. With an outer shell of 2 electrons, the periodic table shows that helium has a stable electron configuration. The next stable configuration of an element has 10 (2 + 8) electrons. This is neon. Neon is followed by argon, with 18 (2 + 8 + 8) electrons. Krypton, with 36 (2 + 8 + 8 + 18) electrons is next. The remaining stable configurations follow a similar pattern, based on the maximum number of electrons able to fit into the outermost ring. These elements are extremely stable and rarely react with other elements. They are referred to as the noble gases or inert elements. Atoms of other elements may bond with each other or different elements to form molecules having full outermost shells of electrons.
Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.