D. S-2
Electron configuration has to do with the number of electrons, so using a Periodic Table, it is easy to find this answer.
Remember 'minus' means more electrons so for electron configurations you move forward on the Periodic table for ions with negative charge and backwards if the ion is positive.
Coordination number of an ion is the number of oppositely charged ions present around that ion as the neighbour ions , in that ionic crystal.
Na+ and Cl- are spectator ions.
The negative ions are chloride, bicarbonate, and phosphate
calcium ions that has lost electrons. It will give away electrons.
The arrangement of atoms or ions in a crystal.
yes
Alkali metals and alkaline earth metals will form ions (by losing 1 and 2 electrons respectively) with noble gas electron configuration.
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.
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
Chemical properties depend on electron configuration. By either gaining or losing electrons, an atom changes its electron configuration and therefore its chemical properties also change.The atoms of an element will react to achieve a noble-gas configuration. The atoms will either gain or lose electrons to achieve such a configuration.
Be3+ has only 2 valence electron and not 8.
A noble gas electronic configuration has an outer shell of ns2, np6. Examles of ions with this configuration are O2- [He], 2s2 2p6 (the neon configuartion) Cl- [Ne] 3s2 3p6 (the argon configuration)
metals lose electrons to form ions so as to obtain noble gas configuration. for e.g. sodium(Na) has 11 electrons i.e. 1 electron in its valent (last) shell, to attain noble gas configuration sodium loses 1 electron which may be gained by a non-metal to stabilize itself.
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.