Oh, dude, the orbital of noble gases is like the VIP section of the Periodic Table. They have full outer electron shells, making them super stable and unreactive. It's like they're the cool kids at the chemistry party, just chilling while everyone else is causing drama.
This is the family of noble gases (group 18).
No. Helium is the only noble gas to have an empty p-orbital, and has one full s-orbital. The rest all have at least one of each orbital full.
All group 18 noble gases have a completely filled outer electron shell, which gives them stability and inertness. Their electron configurations end in s2p6, meaning they have a full s orbital and a full p orbital in their outermost shell.
"Noble gases" is the usual name given. The noble gases are inert due to closed electron systems and strong typically antibonding character in their molecular orbital systems.
s orbital for helium and p orbitals for other noble gases.
The valence electrons are filled in the p orbitals for noble gases (s orbital for helium)
This is the family of noble gases (group 18).
No. Helium is the only noble gas to have an empty p-orbital, and has one full s-orbital. The rest all have at least one of each orbital full.
they are very unreactive
All group 18 noble gases have a completely filled outer electron shell, which gives them stability and inertness. Their electron configurations end in s2p6, meaning they have a full s orbital and a full p orbital in their outermost shell.
"Noble gases" is the usual name given. The noble gases are inert due to closed electron systems and strong typically antibonding character in their molecular orbital systems.
Noble gases do not naturally form chemical bonds because their valence orbital is full of electrons. Helium has 2 electrons, and the other noble gases have 8 electrons in their full valence orbital. This full shell makes them unreactive (they have high ionization energy and almost zero electron affinity). However, under special conditions in the lab, scientists can artificially synthesize noble gas compounds such as XeF6.
s orbital for helium and p orbitals for other noble gases.
Number of electrons, but more importantly the number of electrons in the outermost orbital. This determines the reactivity of the atom (noble gases have a fully filled outer orbital, so they dont need any more or any less electrons to make them "happy". Therefore, noble gases are very stable. There's plenty of other factors that determine their chemical properties such as electronegativity (which is affected by the number of electrons, the nuclear charge, the atomic radius etc..)
any time there are as many electrons and protons and they fill each orbital optimally.
Noble gases are chemically inert.
it's not