well, its quite obvious.
orbital notation is the notaion of orbitals and electron configuration notation is the configuration of electrons?!??!?!
kthanksbye<3(;
3 a magnolia ako
The behavior against polarized light is different.
. Through the transfer of electrons between atoms
The electron microscope is stronger than the optical microscope Electron microscope use electrons not light waves
There are no similarities. Noble gases (group 18 elements) have completely filled orbitals with stable electron configuration and are generally unreactive. Alkali metals (group 1 elements) have one valence electron. They are reactive. When these lose one electron, they form ions which has the electronic configuration of the nearest noble gas.
If alkali metals loses one electron, they achieve the electronic configuration of the nearest noble gases.
Fluorine's electron configuration is 1s2 2s2 2p5, and since fluoride is just fluorine with an extra electron, or F-1, its electron configuration is 1s2 2s2 2p6.
Electron configuration of silicon: [Ne]3s23p2 Electron configuration of germanium: [Ar]3d104s24p2
You can tell the difference between 1s subshell and 3s subshell using quantum numbers and electron configuration.
contrast attachment
The bromide ion, which has a charge of 1-, has one more electron than a neutral bromine atom. Its electron configuration is isoelectric with the noble gas krypton, so it has 36 electrons. Its electron configuration is [Ar]3d10 4s2 4p6. I apologize that the superscripts are not working. I put a space between the different sublevels to make it easier to understand.
Hydrogen is an element, the electron is a subatomic particle.
The behavior against polarized light is different.
These are complete filled electron shells.
It should be read as: [Ar] 4s1 .Meaning: the same electron configuration as Argon(18), expanded with ONE (1) electron in the 4s orbital.So it is one electron, thus also one proton more than Ar(18): this makes it atom number (19), which is named as Potassium:K(19): electron configuration [1s2, 2s2 2p6, 3s2 3p6] 4s1 ,(between squared brackets [...] is the electron configuration of Argon)
An element's electron configuration determines its location (group) in the periodic table. It tells us how many valence electrons (s and p sublevel).
an electron
Let us assume that we have Sodium (Na), it has the ground state electron configuration of: [Ne]3S1. The ANION is negative, and thereby has more electrons, the Na anion(Na.) would have the following electron configuration: [Ne]3S2. The CATION(which is a positive ion) of Na(Na+) would have [Ne] as it electron configuration(as it loses an electron and becomes "equal" to Neon)