one electron in the 5s orbital
A filled valence shell often has 8 electrons, which is called an octet. This configuration is considered stable because it mimics the electron configuration of noble gases, which have full valence shells.
The valence shell is the outermost shell of the atom. For example, hydrogen (which is located on Period 1) has only one shell and it is its valence shell. Another example, bromine (which is located on Period 4) has four electron shells, and its fourth shell (counting away from the nucleus) is its valence shell containing seven electrons.
the noble gas configuration of silver would be [Kr]4d105s1, because the s orbital is the valence shell, whereas the d orbital is a lower energy level. Thus, it would not be [Kr]4d95s2.
No, the valence shell of sodium (Na) is not full. Sodium has an atomic number of 11, which means it has 11 electrons, with 1 electron in its outermost shell (the third shell). This single valence electron makes sodium highly reactive, as it tends to lose that electron to achieve a full outer shell, resembling the electron configuration of the nearest noble gas, neon.
The group attains electron configuration of noble gases by gaining one electron is the halogens. They have seven valence electrons and need one more electron to complete their outer shell, resulting in a full valence shell like the noble gases.
Valence electron configuration in group 1A: ns1 in which n=1, 2, 3, 4, 5, ... etc. Starting with Hydrogen, H, electron configuration: 1s1 followed by Lithium, Li, electron configuration: (1s2), 2s1 (non valence electrons in () brackets)
Se and Te will have the same valence-shell electron configuration as they are both in the same group (group 16) and have 6 valence electrons. Sr and Cs will have different valence-shell electron configurations as Sr is in group 2 with 2 valence electrons and Cs is in group 1 with 1 valence electron. N and O will have different valence-shell electron configurations as N has 5 valence electrons while O has 6. H and He will have different valence-shell electron configurations as H has 1 valence electron and He has 2.
It can reveal the number of valence electrons in the last shell.
Magnesium will lose 2 electrons to have the same electron configuration as Neon. Neon has a full valence shell with 8 electrons, and Magnesium has 2 valence electrons. By losing 2 electrons, Magnesium can achieve a full valence shell and the same electron configuration as Neon.
Valence electron configuration in group 7A (halogens): ns2, np5 in which n=2, 3, 4, 5, ... etc. Starting with fluorine, F, electron configuration: (1s2), 2s2 2p5 (non valence electrons in () brackets)
It needs only 1 more electron since it already has 7 valence electrons.
A filled valence shell often has 8 electrons, which is called an octet. This configuration is considered stable because it mimics the electron configuration of noble gases, which have full valence shells.
Boron exists in period 2, group 13 (IIIA) of the periodic table, with valence of 3 electrons in the outer shell. The electron configuration of boron is 1s22s22p1
Chlorine atoms have 7 outermost electrons and need to gain an electron to achieve the stability of a full valence shell.
The outer electron configuration for germanium is 4s^2 4p^2. Germanium has 4 valence electrons in the outermost shell.
Argon, being one of the noble gases, has a completely filled outer electron shell and thus has zero valency.
The valence electron configuration of europium (atomic number 63) is [Xe] 4f7 6s2. This means that europium has 2 valence electrons in its outermost shell.