1. Chapters 8 and 9 Ionic and Covalent Bonding

2. A chemical bond is a force that holds two atoms together. Chemical bonds may form by the attraction between a positive nucleus and negative electrons OR the attraction between a positive ion and a negative ion.

3. Important fact… REMEMBER!! All atoms want to have eight valence electrons, so some atoms lose or gain electrons to achieve that goal and LOOK like a noble gas. When this happens, it is important to remember that the atom has not changed into a noble gas, its nucleus, which gives it its characteristics, remains unchanged. You can dress up like Madonna, but you are still you. You just look different on the outside.

4. POSITIVE IONS Positive ions form when an atom loses one or more valence electrons in order to attain a noble gas configuration. A positive ion is called a cation.

5. Negative Ions When an atom gains electrons, it becomes a negative ion. A negative ion is also called an anion.

6. Formation of ions Octet Rule – in forming compounds atoms will try to obtain a noble gas electron configuration. To do this metals ________ electrons and nonmetals _________ electrons

7. Metal Examples Na atom = 1s 2 2s 2 2p 6 3s 1 Na Na 1+ = 1s 2 2s 2 2p 6 Na 1+ Note the 3 rd energy level electron was lost to have the same electron configuration as neon Ne = 1s 2 2s 2 2p 6

8. YOU TRY Ca = 1s 2 2s 2 2p 6 3s 2 3p 6 4s 2 :Ca Ca 2+ = 1s 2 2s 2 2p 6 3s 2 3p 6 Ca 2+ What noble gas does Ca 2+ resemble? The oxidation number on the metal ion (cation) is the positive value of how many electrons were lost.

9. Ionic Bonds Ionic bonds occur because of the attraction between oppositely charged ions. Hundreds of compounds contain ionic bonds. Many ionic compounds are binary, they contain only 2 different elements. Binary ionic compounds usually contain a metallic cation and a nonmetallic anion.

10. Example Calcium fluoride CaF 2 Calcium, a group 2A metal with the electron configuration [Ar]3s 2, has 2 valence electrons. Fluorine, a group 7A nonmetal with the electron configuration [He]2s 2 2p 5, must gain one e- to attain the noble gas configuration of neon. Because the number of e- lost must equal the number of e- gained, it will take two fluorine atoms to gain the two e- lost from one calcium atom. The compound formed will contain one calcium ion with a charge of 2+ for every two fluoride ions, each with a charge of 1-.

11. Ca +2 + F -1 CaF 2 Oxidation numbers must equal zero, when added together. Ca +2 + F -1 +F -1

12. Properties of Ionic Compounds Attraction and repulsion between positive and negative ions cause the ions to be packed into a specifically shaped particle called a crystal lattice. In a crystal lattice each positive ion is surrounded by negative ions and each negative ion is surrounded by positive ions.

13. Melting and Boiling Points Because ionic bonds are relatively strong, the crystals that result require a large amount of energy to be broken apart. Therefore, ionic compounds have high melting and boiling points.

14. Conductor of electricity? In the solid state, ionic compounds are nonconductors of electricity because of the fixed positions of the ions. However in a liquid state or when dissolved in water, ionic compounds are electrical conductors because the ions are free to move. An ionic compound whose aqueous solution conducts and electric current is an electrolyte.

15. Lattice Energy The energy required to separate one mole of the ions of an ionic compound is referred to as lattice energy. The more negative the lattice energy, the stronger the force of attraction. Smaller ions have a more negative value for lattice energy because the nucleus is closer to and thus has more attraction for the valence e-.

16. Formulas for Ionic Compounds The simplest ratio of the ions represented in an ionic compound is called a formula unit. A monatomic ion is a one-atom unit (Mg 2+ or S 2- ). The charge of a monatomic ion is its oxidation number. Most transition metals and group 3A and 4A metals have more than one oxidation numbers.

17. The oxidation number of an element in an ionic compound equals the number of electrons transferred from an atom of the element to form the ion.If you add the oxidation number of each ion multiplied by the number of these ions in a formula unit, the total must be zero.

18. Let’s practice Potassium plus sulfur yields _______ Sodium plus oxygen yields _______ Aluminum plus fluoride yields ______ Cesium plus nitrogen yields _______ Magnesium plus chlorine yields ______

19. Polyatomic Ions An ion that is made up of more than one atom is called a polyatomic ion. The charge given to a polyatomic ion applies to the entire group of atoms. The polyatomic ion acts as an individual ion. Because a polyatomic ion exists as a unit, never change subscripts of the atoms within the ion.

20. Oxyanion An oxyanion is a polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms. Go to Nomenclature rules p. 3

21. Metallic Bonds & Properties Metals do not bond ionically, but they form lattices similar to ionic crystal lattices. The electron sea model proposes that all the metal atoms in a metallic solid contribute their valence electrons to form a “sea” of electrons.

22. Delocalized electrons The electrons present in the outer energy levels of the bonding metallic atoms are not held by any specific atom and can move easily from one atom to the next. Because they are free to move, they are often referred to as delocalized electrons. A metallic bond is the attraction of a metallic cation for delocalized electrons.

23. Electron sea model

24. Properties of Metals 1) Moderately high melting points and high boiling points. 2) Malleable and ductile 3) Durable 4) Good conductors of heat and electricity, because the electrons are free to move and can move heat easily

25. Alloys An alloy is a mixture of elements that has metallic properties. Examples of common metal alloys 1. Brass - Cu 67-90%, Zn 10-33% 2. Bronze - Cu 70-95%, Zn 1-25%, Sn 1-18% 3. 10 carat gold – Au 42%, Ag 12-20%, Cu 38-46% 4. Sterling silver – Ag 92.5%, Cu 7.5%