3.2: Ions
- Page ID
- 83059
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- Define the two types of ions.
- Use Lewis diagrams to illustrate ion formation.
Most atoms do not have eight 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 easily until what remains is a lower shell that contains an octet. Atoms that lose electrons acquire a positive charge as a result because they are left with fewer negatively charged electrons to balance the positive charges of the protons in the nucleus. Positively charged ions are called cations. Most metals become cations when they make ionic compounds.
Some atoms have nearly eight electrons in their valence shell and can gain additional valence electrons until they have an octet. When these atoms gain electrons, they acquire a negative charge because they now possess more electrons than protons. Negatively charged ions are called anions. Most nonmetals become anions when they make ionic compounds.
Note
The names for positive and negative ions are pronounced CAT-eye-ons and ANN-eye-ons, respectively.
Electron Transfer
We can use total electrons or valence electrons to illustrate the electron transfer process between sodium atoms and chlorine atoms. First, we will look at the arrangement of electrons in sodium.
| Sodium Atom, Na (11 p+ in nucleus) | First Shell | Second Shell | Third Shell |
| 11 e- Total Electrons | 2 e- | 8 e- | 1 e- |
As demonstrated in the previous section, sodium is likely to achieve an octet in its outermost shell by losing its one valence electron. Now it has the same number of electrons as the nearest noble gas, neon. The cation produced in this way, Na+, is called the sodium ion to distinguish it from the neutral element. Because the ion has 11 positive protons and 10 negative electrons, there is a net positive charge. That charge is shown as a superscript at the top, right of the symbol.
| Sodium Ion, Na+ (11 p+ in nucleus) | First Shell | Second Shell | Third Shell |
| 10 e- Total Electrons | 2 e- | 8 e- | empty |
The third shell of the ion is empty, so the outermost shell of the sodium ion becomes the second electron shell, which has eight electrons in it. The octet rule has been satisfied. Figure \(\PageIndex{1}\) is a graphical depiction of this process.
Figure \(\PageIndex{1}\): The Formation of a Sodium Ion. On the left, a sodium atom has 11 electrons. On the right, the sodium ion only has 10 electrons and a 1+ charge.
A chlorine atom has the following electron arrangement:
| Chlorine Atom, Cl (17 p+ in nucleus) | First Shell | Second Shell | Third Shell |
| 17 e- Total Electrons | 2 e- | 8 e- | 7 e- |
Only one more electron is needed to achieve an octet in chlorine’s valence shell. (In table salt, NaCl, this electron comes from the sodium atom.) Now the chlorine ion has the same number of electrons as the nearest noble gas, argon. The electron arrangement of the new species that results is as follows:
| Chlorine Ion, Cl- (17 p+ in nucleus) | First Shell | Second Shell | Third Shell |
| 18 e- Total Electrons | 2 e- | 8 e- | 8 e- |
In this case, the ion has the same outermost shell as the original atom (third), but now that shell has eight electrons in it. Once again, the octet rule has been satisfied. By gaining an extra negative electron, the ion now has a net negative charge. The resulting anion, Cl−, is called the chloride ion; note the slight change in the suffix (-ide instead of -ine) to create the name of this anion. Figure \(\PageIndex{2}\) is a graphical depiction of this process.
Figure \(\PageIndex{2}\): The Formation of a Chlorine Ion. On the left, the chlorine atom has 17 electrons. On the right, the chloride ion has 18 electrons and has a 1− charge.
With two oppositely charged ions, there is an electrostatic attraction between them because opposite charges attract. The resulting combination is the compound sodium chloride. Notice that there are no leftover electrons. The number of electrons lost by the sodium atom (one) equals the number of electrons gained by the chlorine atom (one), so the compound is electrically neutral. In macroscopic samples of sodium chloride, there are billions and billions of sodium and chloride ions, although there is always the same number of cations and anions.
In many cases, elements that belong to the same group (vertical column) on the periodic table 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 example, all ions made from alkali metals, the first column on the periodic table, have a 1+ charge. Ions made from alkaline earth metals, the second group on the periodic table, have a 2+ charge. On the other side of the periodic table, the next-to-last column, the halogens, form ions having a 1− charge. Figure \(\PageIndex{3}\) shows how the charge on many ions can be predicted by the location of an element on the periodic table. Note the convention of first writing the number and then the sign on a multiply charged ion. The barium cation is written Ba2+, not Ba+2.
Figure \(\PageIndex{3}\): Predicting Ionic Charges. The charge that an atom acquires when it becomes an ion is related to the structure of the periodic table. Within a group (family) of elements, atoms form ions of a certain charge.
Lewis Diagrams
Chemists use simple diagrams to show an atom’s valence electrons and how they transfer. These diagrams have two advantages over the electron shell diagrams. First, they show only valence electrons. Second, instead of having a circle around the chemical symbol to represent the electron shell, they have up to eight dots around the symbol; each dot represents a valence electron. These dots are arranged to the right and left and above and below the symbol, with no more than two dots on a side. For example, the representation for sodium is as follows:
and the representation for chlorine is as follows:
Note
It does not matter what sides the dots are placed on in Lewis diagrams as long as each side has a maximum of two dots.
These diagrams are called Lewis electron dot diagrams, or simply Lewis diagrams, after Gilbert N. Lewis, the American chemist who introduced them. Figure \(\PageIndex{4}\) shows the electron configurations and Lewis diagrams of the elements lithium through neon, which is the entire second period of the periodic table. For the main group elements, the number of valence electrons is the same as the group number listed at the top of the periodic table.
Figure \(\PageIndex{4}\) Lewis Diagrams of the Elements Lithium through Neon
The transfer of electrons can be illustrated easily with Lewis diagrams:
Above is shown the Lewis diagrams of sodium and chlorine atoms (on the left) exchanging an electrons to become the Lewis diagrams of the ions (in the middle), and with the formula of the compound shown (on the right). In representing the final formula, the dots are omitted (and the individual charges are not shown because they balance to zero).
Example \(\PageIndex{1}\)
Starting with lithium and bromine atoms, use Lewis diagrams to show the formation of the ionic compound LiBr.
SOLUTION
From the periodic table, we see that lithium is in the same column as sodium, so it will have the same valence shell electron configuration. That means that the neutral lithium atom will have the same Lewis diagram that the sodium atom has. Similarly, bromine is in the same column as chlorine, so it will have the same Lewis diagram that chlorine has. Therefore,
Some ionic compounds have different numbers of cations and anions. In those cases, electron transfer occurs between more than one atom. For example, here is the formation of MgBr2:
Most of the elements that make ionic compounds form an ion that has a characteristic charge. For example, sodium makes ionic compounds in which the sodium ion always has a 1+ charge. Chlorine makes ionic compounds in which the chloride ion always has a 1− charge. Some elements, especially transition metals, can form ions of multiple charges. Figure \(\PageIndex{5}\) shows the characteristic charges for some of these ions. As we saw in Figure \(\PageIndex{1}\), there is a pattern to the charges on many of the main group ions, but there is no simple pattern for transition metal ions (or for the larger main group elements).
Figure \(\PageIndex{5}\): Charges of the Monatomic Ions. Note that some atoms commonly form ions of different charges.
Contributors
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