Thus, a magnesium atom will form a cation with two fewer electrons than protons and a charge of 2+. The symbol for the ion is Mg2+, and it is called a magnesium ion.
Sulfur has an electron configuration of 1s²2s²2p⁶3s²3p⁴ (1s2 2s2 2p6 3s2 3p4) meaning it is 2 away from having a noble gas configuration (its charge is − 2 ). So the ion’s configuration is 1s²2s²2p⁶3s²3p⁶ ( 1s2 2s2 2p6 3s2 3p6 ). Alternately, this can be written as [Ne]3s²3p⁶ or [ Ar ].
Cations (positively-charged ions) and anions (negatively-charged ions) are formed when a metal loses electrons, and a nonmetal gains those electrons. The electrostatic attraction between the positives and negatives brings the particles together and creates an ionic compound, such as sodium chloride.
A quick shufti at the Periodic Table tells me that for, we got the element sulfur.
Alkali metals, such as sodium and lithium, have ions with 1+ charge. Alkaline earth metals, which are the second group in the periodic table, form ions with 2+ charge. Halogens, group 17 elements such as fluorine, form ions with 1– charge.
Table of Common Element Charges
The S2- ion, the simplest sulfur anion and also known as sulfide, has an electron configuration of 1s2 2s2 2p6 3s2 3p6. A neutral atom of sulfur has 16 electrons, but the atom then gains an additional two electrons when it forms an ion, taking the total number of electrons to 18.
P3–: From Table 2.2, the electron configuration for an atom of phosphorus is 1s22s22p63s23p3. In order to become an ion with a minus three charge, it must acquire three electrons—in this case another three 3p. Thus, the electron configuration for a P3– ion is 1s22s22p63s23p6.
Explanation: Typically, an atom of O has 8 electrons, so based on the electron configuration system that would be 1s22s22p4, or 2+2+4=8e−.
The inert pair effect in the formation of ionic bonds If the elements in Group 4 form 2 + ions, they lose their p electrons, leaving the s 2 pair unused. For example, to form a lead (II) ion, lead loses its two 6p electrons, but the 6s electrons are left unchanged, an “inert pair”. This is not the case in Group 4.
Ions are formed by the addition of electrons to, or the removal of electrons from, neutral atoms or molecules or other ions; by combination of ions with other particles; or by rupture of a covalent bond between two atoms in such a way that both of the electrons of the bond are left in association with one of the
Consequently, they tend to lose electrons and form cations. Conversely, most nonmetallic atoms attract electrons more strongly than metallic atoms, and so gain electrons to form anions. Cation vs anion chart.
|Examples||Sodium (Na+), Iron (Fe2+), Ammonium (NH4+)||Chloride ( Cl –), Bromide (Br–), Sulfate (SO42–)|
Like the group 14 elements, the lightest member of group 15, nitrogen, is found in nature as the free element, and the heaviest elements have been known for centuries because they are easily isolated from their ores.
Answer and Explanation: There are 27 electrons in the Cu2+ ion.
Because the ion has 16 protons and 18 electrons, its net charge is 2–. Thus, the symbol for the ion is 32S2–.