In period 3? It has to be Boron although technically it is not a gas. The electron configuration is either 2, 3 or 1s^2, 2s^2, 2p^1 depending on what level of chemistry you are working at. If the latter looks like a different language you to, go with the first!
that is actually wrong above^^, the real answer is argon so its electron configuration is 1s2, 2s2, 2p6, 3s2, 3p6
Bit of a trick question in some ways. It's Helium. But helium doesn't appear in period 2 on the Periodic Table, it's above the noble gasses. That's just for convenience since it has similar properties.
But Helium has 2 valance electrons and by all rights, belongs to the second period.
That would be Argon (Ar).
argon
silicon
The noble gas electron configuration indium is[Kr]4d10.5s2.5p1.
Because each of them can form a cation with the electron configuration of a noble gas by donating one electron to another element.
The inert gas had no effect on the experiment. The bomb was inert and failed to explode.
Nitrogen is an inert gas; it is non-reactive in chemical situations.
In Periodic table , Group 18 corresponds to Nobel gas group. They are six elements in this group. Helium , Neon , Argon , Krypton , Xenon , Radon constitute these group. They are chemically inert elements and having stable configuration.
The inert gas in Period 2 is the element Neon(Ne). Its electron configuration is 2-8.
having 8 electron in the outermost shell or in valence shell....
Noble gases have a stable electron configuration. So they are less reactive.
The "Noble gas electron configuration," or the condensed electron configuration, for F is [He] 2s2 3p5.
Fr is in the 1st period. It removes an electron to get noble gas configuration. Fr+ does not have valence electrons.Francium has 1 electron in its outermost energy level. It donates its outermost electron to stabilize its electron configuration. Francium(I) has no valence electrons.
Neon is in the 2d period so the 2s and 2p are filled- it is anoble gas so it is the last one in the period. 1s2; 2s2, 2p6
An atom of silicon needs to gain 4 electrons in its 3p sublevel to attain the noble gas electron configuration of argon, the noble gas in period 3 of the periodic table.
A full outer electron shell, the so-called valence shell, creates an inert gas in those elements (the inert or noble gases). In other elements, what is called "inert gas configuration" will apear in the Halogens (the Group 17 elements) and some Group 16 elements. When they "borrow" an electron or electrons in an ionic bond, they do so to achieve "inert gas configuration" by "filling" their valence shell with the borrowed electrons.
an element with 2 valence electrons can obtain a stable electron configuration by "kicking out" two electrons to have the same electron config as the noble gas in the previous period
Losing an electron cesium has a noble gas configuration.
The electron configuration of ununoctium is: [Ra] 5f14 6d10 7s2.
The electron configuration of boron is: [He]2s2.2p1.