Metals like sodium,potassium get noble gas configuration by losing electrons. Elements like nitrogen,oxygen get noble gas configuration by gaining electrons. Halogens get noble gas configuration by sharing electrons.
Stable electronic configuration is when the valence shell of an element is completely filled (8 electrons) whereas unstable electronic configuration is when the valence shell of an element is not completely filled
Calcium's electron configuration is [Ar] 4s2. To attain a noble gas configuration, calcium must lose 2 electrons to have the same electron configuration as argon, 4s2 3d10.
Chlorine is expected to form a chloride ion with a charge of -1 by gaining one electron to achieve a full valence shell and attain a stable electronic configuration.
Bromine (Br) forms anions in potassium bromide (KBr). It gains one electron to attain a full outer electron shell and achieve a stable electronic configuration.
an element is chemically active till it does not attain an inert gas configuration.
Metals , generally, have electronic configuration: with outermost electron having 1,2 or 3. Since, they can easily attain noble gas configuration to attain stability; they readily loose electron.
Stable electronic configuration is when the valence shell of an element is completely filled (8 electrons) whereas unstable electronic configuration is when the valence shell of an element is not completely filled
There are three different ways for this. Elements can either gain electrons or lose electrons or share electrons and attain a stable noble gas electronic configuration.
since not all atoms have same no.of electronic configuration they try to attain an octet sharing electrons each other
A species (element, cation or anion) should have eight valence electrons to have a noble gas electronic configuration. However element upto atomic number 4 may have 2 valence electrons and attain the electronic configuration of helium noble gas.
elements combine to attain more stability, generally by attaining the electronic configuration of the nearest noble gases. they do so by donating electrons, accepting electrons or by sharing electrons
All the elements in their normal state are reactive and unstable. In order to attain stability i.e. a state of minimum energy, they tend to form ions by loosing or gaining electrons. By doing so, they achieve stable electronic configuration or noble gas configuration. However, some elements do not form ions. Instead of that, two such atoms share electrons with each other and achieve this noble gas configuration. At the end, the main reason for attaining a noble gas configuration is to attain max. stability and min. energy.
They are formed to attain a balance octet configuration
group 18 has completely filled electronic configuration and hence are stable. group 1 and group 2 have 1 and 2 electrons respectively in their valence shells and needs to lose these to attain completely filled electronic configuration. hence they are reactive.
Phosphorus should gain 3 electrons and form P3- ion to attain a noble gas configuration
Sulfur gains two electrons to attain a noble gas configuration, which is the electron configuration of argon. This allows sulfur to have a stable octet of electrons in its outer shell and achieve a more stable electron configuration.
Atoms lose or gain or share electrons and tend to attain noble gas configuration