Fe is most likely to form a 3⁺ ionFurther explanation
In an atom, there are levels of energy in the shell and subshell
This energy level is expressed in the form of electron configurations.
Writing electron configurations starts from the lowest to the highest sub-shell energy level.
Charging electrons in the subshell uses the following sequence:
1s², 2s², 2p⁶, 3s², 3p⁶, 4s², 3d¹⁰, 4p⁶, 5s², 4d¹⁰, 5p⁶, 6s², etc.
Atoms release or bind electrons to get stable electron configuration from noble gases
The metal element usually releases electrons to stabilize it like a noble gas element
While non-metallic elements will bind electrons to be stable like the noble gas element
Let see the electron configuration of each element1. Li
Lithium is an alkali metal located in group 1
Electron configuration: [He] 2s¹
So to achieve stability like He will release 1 electron to form the Li⁺ cation2. Fe
Iron is a metal that is located in group 8 and is a transition metal
Electron configuration: [Ar] 3d⁶ 4s²
For transition metals the exact charge cannot be determined based on the group, but if we look at Fe, as a metal it will tend to release electrons, which are electrons that fill 4s² orbitals (valence electrons) of 2 electrons to form Fe²⁺ or release 3 electrons so that they have 3d orbitals which stable (with 5 electrons) so that the configuration becomes [Ar] 3d⁵ and forms the Fe³⁺ cation3. P
Phosphorus is a non-metallic element in group 15
Electron configuration: [Ne] 3s² 3p³
So to achieve stability such as Ar it will bind 3 electrons to form P³⁻ anions4. S
Sulfur is a non-metallic element in group 16
Electron configuration: [Ne] 3s² 3p⁴
So to achieve stability such as Ar it will bind 2 electrons to form S²⁻ anionsLearn more
electron configurations using the Aufbau rule
the reactivity of element
non metals element
N and N
N and H
O and Na
H and H
Nonmetals are poor electrical conductors but they are considered as good insulators. Among the given statement, the most likely reason that nonmetals are electrical insulators is that since valence shells in nonmetal atoms are almost full, the atoms attract electrons and hold them tightly to fill their valence shells. In this manner the atoms of the nonmetals cannot give their electrons making them poor conductor of electricity.
On the other hand since metals, have a valence shells that are mostly empty, the atom attract and hold any electrons they can in order to fill their valence shells. Lastly the elements known as noble gases that has a complete valence electron are unreactive.
Other questions related to this are as follows:
sulfur, a nonmetal with 6 valence electrons
The weight of an atom comes mostly from its
Sub Particles Atomic