Four: All of its valence electrons. If a silicon atom loses four electrons, it has the stable electron configuration of neon, while if the atom gains four electrons it has the stable electron configuration of argon. A silicon atom can also form a stable compound, as contrasted with a stable electron configuration for a single atom, by sharing four electrons with one or more other atoms.
Sodium needs to lose 1 electron to become stable.
Sr, or Strontium, has an atomic number of 38 and is in Group II. This means it has 2 valence electrons and seeks to lose two of them to be stable.
Well since Sr has 38 protons I think it would also have 38 electrons to balance it out.
Two electrons
Aluminium need five electrons.
They achieve stable configuration by sharing their electrons in their outermost shell.
Oxygen atoms need to share or gain two electrons in order to achieve a stable electron configuration.
silicon's atomic number is 14 so, its electron configuration is 2.8.4, the third shell needs 4 more electrons to make it 8 and to become stable. ---> so the answer is 4.
The expected ground-state electron configuration of copper is ; however, the actual configuration is because a full dsubshell is particularly stable. There are 18 other anomalous elements for which the actual electron configuration is not what would be expected.
Beryllium is a metal. It has 2 valance electrons (in the outer shell), and therefore it tends to lose those electrons in order to achieve a stable electron configuration, which in the case of beryllium is also 2 electrons, but in the inner shell. Nitrogen is a nonmetal, with 5 valence electrons, and it tends to acquire more electrons in order to reach a stable electron configuration of 8. Less energy is need to lose electrons when the result is going to be a stable electron configuration.
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
They achieve stable configuration by sharing their electrons in their outermost shell.
A stable electron configuration.
Elements get stable only when it completes electron octate in its outermost orbit. Elements make compounds with other elements to gain or reduce electrons to get stability. silicon make bonds with oxygen and make silicon dioxide to get stable.
Oxygen atoms need to share or gain two electrons in order to achieve a stable electron configuration.
silicon's atomic number is 14 so, its electron configuration is 2.8.4, the third shell needs 4 more electrons to make it 8 and to become stable. ---> so the answer is 4.
8 valance electron
Only three electrons.
The expected ground-state electron configuration of copper is ; however, the actual configuration is because a full dsubshell is particularly stable. There are 18 other anomalous elements for which the actual electron configuration is not what would be expected.
Beryllium is a metal. It has 2 valance electrons (in the outer shell), and therefore it tends to lose those electrons in order to achieve a stable electron configuration, which in the case of beryllium is also 2 electrons, but in the inner shell. Nitrogen is a nonmetal, with 5 valence electrons, and it tends to acquire more electrons in order to reach a stable electron configuration of 8. Less energy is need to lose electrons when the result is going to be a stable electron configuration.
Tin has 4 valence electrons. Because of this, Tin needs to lose the 4 electrons to make it stable. Thus the answer is SN4+
Because while silicon loses electrons to be stable, it loses an electron shell, whereas phosphorus gains more electrons. Therefore, there is a difference of an entire electron shell.