The stable ions of all the elements except the Transition metals, Actinide, and Lanthanide series (that is the d and f block elements) form stable ions that are isoelectronic to a nobel gas by gaining or losing electrons in order to achieve an s2 p6 stable octet. For example, sodium will lose one electron to have the same electron configuration as neon, while nitrogen will gain three electrons to become isoelectronic to neon.
All atoms "want" to have a noble gas electron configuration through the sharing or transferring of electrons. Therefore, any atom can achieve the electron configuration of a noble gas.
Not necessarily. Ions of groups 1, 2, 17, 16, 15 will generally have the electron configuration of noble gases.Ions of transition metals may not have the electron configuration of noble gases.
Halide ions
There are no similarities. Noble gases (group 18 elements) have completely filled orbitals with stable electron configuration and are generally unreactive. Alkali metals (group 1 elements) have one valence electron. They are reactive. When these lose one electron, they form ions which has the electronic configuration of the nearest noble gas.
Potassium and chlorine are the only two that can.
Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
Electronegativity affects the amount of ions in an element thus affecting the formation of an ionic compound. The more electronegativity, the more ions, the greater ability to react.
Cl- and Ca2+ has the electronic configuration of the noble gas, Ar, with 18 electrons.
yes
There are no similarities. Noble gases (group 18 elements) have completely filled orbitals with stable electron configuration and are generally unreactive. Alkali metals (group 1 elements) have one valence electron. They are reactive. When these lose one electron, they form ions which has the electronic configuration of the nearest noble gas.
Potassium and chlorine are the only two that can.
Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
Generally (but not always) stable ions will have the same the electronic configuration as that of noble gases (completely filled valence shells / orbitals)
Electronegativity affects the amount of ions in an element thus affecting the formation of an ionic compound. The more electronegativity, the more ions, the greater ability to react.
Cl- and Ca2+ has the electronic configuration of the noble gas, Ar, with 18 electrons.
In NaF, there exists Na+ and F- ions and with the electron configuration of [He]2s22p6 (for Na+) and [He]2s22p6 (for F-)
In NaCl, there exists Na+ and Cl- ions and with the electron configuration of [He]2s22p6 (for Na+) and [Ne]3s23p6 (for Cl-)
Noble Gas
socks answer should be D
The Noble Gases (Group VIIIA or Group 8A) do not exchange electrons or become ionized into ions since they already have a full electron configuration.