How does an element in group 2 attain a stable electron configuration?
It loses 2 electrons and becomes a +2 ion.
It is because Sodium has to lose one electron to gain the nearest octet configuration of Neon and Chlorine has to gain one electron to attain stable electronic configuration of the nearest inert gas which is Argon. Thus there is complete transference of an electron from Sodium to Chlorine and thus the ionic bonding If the first element is a metal it is ionic, that's why sodium chloride is ionic. It the first element is…
The atomic number of potassium is 19. The outer shell of potassium contains one electron. It can attain a stable configuration by loosing this electron. This is the reason that potassium forms k+ ions. Similarly, calcium contains two electrons in its outer shell and attain stable configuration by loosing the 2 electrons. Thus, it forms Ca2+ ions.
Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration. Although the formation of an octet is the most stable electron configuration, other electron configurations provide stability. These relatively stable electron arrangements are referred to a pseudo-noble gas configuration.
Metals useually have few valence electrons and they loose electrons from their outermost shell thus, forming an ion with positive charge (cations). This is because it is easy for metals to loose electron and attain stable or octet configuration similar to rare gases. Hence to attain stability metals lose valence electrons. E.g. sodium (At no. =11 ; electronic configu-1s2, 2s2, 2p6, 3s1) metal has one valence electron and it is easy for it to loose…
Fluorine is the most electronegative element in the periodic table. It needs just one electron to attain the stable noble gas configuration. A fluorine atom will thus gain an electron, thereby incurring a single negative charge, to form the fluoride ion, F-. This is an anion as it is a negatively charged ion.
How many electrons does a nitrogen atom need to gain in order to attain a noble gas electron configuration?
What symbol would represent a chlorine ion that has ionized to have a stable electron configuration?
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.
Well it depends upon which element you are talking about Eg flourine atom has 9 protons and electrons normally configuration will be 2,8,1 But if u r talking about a stable fluorine electron, configuration will be 2,8 This happens since the outermost octate of fluorine is not filled completely so it is not stable in it's structure so it loses the 1 extra electron in it's last octate and becomes stable gaining a negative charge…
Generally, atoms would want to fulfill the octet rule: 8 electrons in the valence shell. This gives the atom a noble gas configuration and is seen as stable. Since the Chlorine atom is in group 7 of the periodic table, it "prefers" to gain one electron instead of losing 7 to attain the stable octet configuration.
A subshell is particularly stable if it is half full or full, the atom would "choose" the more stable one. to attain a more stable configuration, the electron from s orbital jumps to the previous d orbital.Chromium has a configuration of [Ar]4s13d5, although you would expect to see four d electrons instead of five.Cu: [Ar]4s23d9, to gain stability stability, one electron from the s shell jumps into the d shell: [Ar]4s13d10.