argon
The electron configuration of fermium is [Rn]5f12.7s2.
The electron configuration of oxygen (atomic number 8) is 1s2 2s2 2p4The noble gas form is [He] 2s22p41s2 2s2 2p4
The Noble gas notation for Krypton can be written as [Kr] because it is a Noble gas or [Ar]4s2 3d10 4p6.
Sulfur atoms will gain two electrons in order to achieve a noble gas electron configuration. A sulfide ion has the formula S2-.
The electron configuration of einsteinium is [Rn]5f11.7s2.
The noble gas electron configuration of Phosphorus is [Ne] 3s2 3p3
Selenium: [Ar]3d104s24p4 Phosphorus: [Ne]3s23p3
Fluorine attains the electron configuration of neon (the nearest noble gas).
Phosphorus has to gain a total of 3 electrons to achieve a noble gas configuration. You can find this for any non-metal because the last digit of its group number is the number of valence electrons it has. For example Phosphorus has 5 and Sulfur has 6. In order to achieve a noble gas electron configuration, you must have 8 valence electrons, so phosphorus must gain 3.
P3- ion or phosphide ion as the same electron configuration as the noble gas, argon
Yes it will as P-3 ion will have the same electron configuration of the noble gas, argon.
The "Noble gas electron configuration," or the condensed electron configuration, for F is [He] 2s2 3p5.
P3- or phosphide ion is formed. it has the same number of electrons as the noble gas, argon
"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 phosphorus will be [Ne]3s23p3
The noble gas electron configuration of radon is [Xe]4f145d106s26p6.
Losing an electron cesium has a noble gas configuration.
The electron configuration of boron is: [He]2s2.2p1.