# Number Of E- Probably Lost Or Gained

## four.vii: Ions - Losing and Gaining Electrons

##### Learning Objectives
• Ascertain the two types of ions.

Most atoms practise not have 8 electrons in their valence electron shell. Some atoms have only a few electrons in their outer shell, while some atoms lack only one or two electrons to have an octet. In cases where an atom has three or fewer valence electrons, the atom may lose those valence electrons quite hands until what remains is a lower beat that contains an octet. Atoms that lose electrons acquire a positive charge as a result considering they are left with fewer negatively charged electrons to rest the positive charges of the protons in the nucleus. Positively charged ions are called
cations. Most metals become cations when they make ionic compounds.

## Cations

A neutral sodium atom is likely to attain an octet in its outermost shell by losing its one valence electron.

$\ce{Na \rightarrow Na^{+} + e^{-}} \nonumber$

The cation produced in this way, Na+, is called the sodium ion to distinguish it from the element. The outermost shell of the sodium ion is the 2d electron shell, which has viii electrons in it. The octet rule has been satisfied. Figure $$\PageIndex{i}$$ is a graphical delineation of this procedure.

## Anions

Some atoms have nigh 8 electrons in their valence shell and can gain additional valence electrons until they take an octet. When these atoms gain electrons, they acquire a negative accuse because they now possess more electrons than protons. Negatively charged ions are called
anions. Most nonmetals get anions when they make ionic compounds.

A neutral chlorine atom has vii electrons in its outermost shell. Only one more electron is needed to attain an octet in chlorine’s valence shell. (In table salt, this electron comes from the sodium atom.)

$\ce{e^{-} +Cl -> Cl^{-}} \nonumber$

In this case, the ion has the same outermost shell as the original cantlet, simply now that crush has viii electrons in it. One time over again, the octet dominion has been satisfied. The resulting anion, Cl, is called the chloride ion; note the slight modify in the suffix (-ide
instead of -ine) to create the name of this anion. Figure $$\PageIndex{two}$$ is a graphical depiction of this process.

The names for positive and negative ions are pronounced CAT-middle-ons and ANN-middle-ons, respectively.

In many cases, elements that belong to the same group (vertical column) on the periodic tabular array form ions with the same charge because they have the same number of valence electrons. Thus, the periodic table becomes a tool for remembering the charges on many ions. For case, all ions fabricated from brine metals, the start column on the periodic table, take a 1+ charge. Ions fabricated from element of group i world metals, the second group on the periodic tabular array, accept a two+ accuse. On the other side of the periodic table, the next-to-last column, the halogens, class ions having a 1− charge. Figure $$\PageIndex{three}$$ shows how the accuse on many ions can exist predicted by the location of an chemical element on the periodic table. Notation the convention of beginning writing the number and then the sign on a ion with multiple charges. The barium cation is written Baii
+, non Ba+ii.

Source: https://chem.libretexts.org/Bookshelves/Introductory_Chemistry/Map%3A_Introductory_Chemistry_(Tro)/04%3A_Atoms_and_Elements/4.07%3A_Ions_-_Losing_and_Gaining_Electrons

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