1. Ions Unit 7 Chapter 6

2. Getting Started When the difference in electronegativity of two atoms is greater than 1.6, electrons are transferred from one atom to the other. Since electrons are negatively charged, when an atom loses an electron, it becomes positively charged.

3. Q is the Loneliest Number… When an atom gains an electron, it becomes negatively charged. You can calculate the charge, Q, by subtracting the number of electrons from the number of protons: Q = p + – e - Aluminum has 13 protons. If it loses 3 electrons, Q = 13 – 10 = +3

4. Positively Shocking A cation is a positively charged ion. They form when atoms lose electrons There are more protons than electrons. All metals form cations. Cations have no special name: Na + is the sodium ion.

5. Don’t Be So Negative! An anion is a negatively charged ion. They form when atoms gain electrons There are more electrons than protons. Most nonmetals will form anions.

6. The “-ides” of Chemistry Anions are named by dropping the final syllable(s) of the element and adding “-ide”. Chlorine becomes chloride, Cl - Oxygen becomes oxide, O -2

7. Mono-a-Mono Monatomic ions are ions made up of single atoms. For example, magnesium forms the Mg +2 cation as one single positively charged atom. Bromine forms the Br -1 anion as one single negatively charged atom.

8. Poly Wanna Covalent Ion!?! Polyatomic ions are ions made up of more than one atom. In polyatomic ions, covalent bonds form between atoms within the ion. The covalent bonds do not dissociate in water. Electrons have been gained or lost during formation.

9. The Cyanide Ion (CN - ) Carbon has 4 valence electrons and N has 5. A covalent bond forms between C and N sharing 3 electrons each. Carbon steals an extra electron The whole molecule acquires a negative charge. C N

10. Polyelectric…is that like GE? Polyatomic ions form ionic bonds with other ions. These ionic bonds will dissociate, and because of this, polyatomic ions can conduct electricity just like monatomic ions.

11. Making ‘em Big! The sulfate ion is SO 4 -2. It is made up of one sulfur atom covalently bonded to four oxygen atoms. When the sulfate ion was formed, it consumed two extra electrons (probably from some metal).

12. A Little of this… The magnesium ion, Mg +2, can combine with the sulfate ion, SO 4 -2, to form magnesium sulfate, MgSO 4 also known as Epsom Salts.

13. It’s ‘Cause They’re So Cool When we talked about the Noble Gases, we learned that they are nonreactive because they have full s and p orbitals (d & f, too). When the outer s and p orbitals are full, the atom is very stable. Ions form when atoms attempt to fill their outer s and p orbitals to be Isoelectronic with the Noble Gases.

14. The Yin & Yang of Stabilization Orbitals are stabilized when they are completely full, completely empty, or half-full (d and f orbitals only). Since an s-orbital can hold 2 electrons and a p-orbital can hold 6, atoms are stable when they have 8 electrons in their valence shell (we usually ignore d’s and f’s).

15. Eight is Enough The Octet Rule: Atoms will attempt to gain or lose electrons to have 8 electrons in their outer s & p orbitals.

16. Hangin’ on the p-Block s- & p-block elements almost always obey this rule, but d- & f-block elements do not always. d and f-block elements have lots of orbitals with nearly overlapping energies. Because of this, many elements in the d and f-blocks can form ions with more than one charge.

17. Predicting Charges We can look at the electron configuration of a neutral atom to predict the charge of its ion. Na = [Ne]3s 1  [Ne]3s 0 = Na +1 S = [Ne]3s 2 3p 4  [Ne]3s 2 3p 6 = S -2 Be = [He]2s 2  [He]2s 0 = Be +2 N = [He]2s 2 2p 3  [He]2s 2 2p 6 = N -3

18. Ions N -3 Na +1 NO 3 -1 CN -1 B +3 Al +3 ClO 4 -1 ClO 2 -1 Br -1 Sr +2 CO 3 -2 NH 4 +1 O -2 C -4 PO 4 -3 PO 3 -3