1. Chapter 6
Chemical Bonds

2. 6.1 Ionic Bonding Stable Electron Configurations
When the highest occupied energy level of an atom is filled with electrons, the atom is stable and will NOT react.
Ex: Noble Gases (8 valence electrons) and Helium (2 v.e.)

3. Electron Dot Diagrams
Electron Dot Diagrams (Lewis Structures) is a model of an atom in which each dot represents a valence electron

4. Ionic Bonds
Elements that do not have complete sets of valence electrons will be reactive. By reacting, they can achieve complete sets.
Some elements achieve stable electron configurations through the transfer of electrons between atoms.

5. Formation of Ions
When an atom gains or loses an electron, the protons do not equal the electrons. The atom is no longer neutral.
Ion- Atom that has a net positive or negative charge.
Anion- Ion with a negative charge.
To name an anion, you change the suffix to –ide and add ion.
Ex: Chloride ion
Cation- Ion with a positive charge.
To name a cation, you add ion to the end.
Ex: Sodium ion

6. Formation of Ionic Bonds
Chemical Bond- force that holds atoms or ions together.
Ionic Bond- force that holds anions and cations together.
An ionic bond forms when electrons are transferred from one atom to another
Ionization Energy- the amount of energy needed to remove an electron.
The lower the ionization energy, the easier it is to remove an electron.
It’s easier to
remove an
electron from
a metal than
from a
nonmetal

7. Ionic Compounds
A chemical formula is a notation that shows what elements a compound contains and the ratio of the atoms or ions of these elements in the compound.
Ex: MgCl2

8. Ionic Compound Diagrams to try:
K and Cl Li and S
Sr and Cl Al and N
*Ga and S

9. Crystal Lattices Remember that orderly, 3-D structure of solids?
In NaCl, each chloride ion is surrounded by 6 sodium ions and each sodium ion is surrounded by 6 chloride ions.
The opposite charges keep ions in their fixed positions in a rigid framework, or lattice.
Crystals- Solids whose particles are arranged in a lattice structure.

10. Properties of Ionic Compounds
The properties of an ionic compound can be explained by the strong attractions among ions.
high melting point
poor conductor of electricity when solid, good conductor when melted.
shatter when struck by a hammer

11. 6.2 Covalent Bonds Sharing Electrons
H has 1 electron. If it had two electrons, it would be happy. (It would have a full outer energy level.)
Two H atoms can share their electrons 
Covalent Bond- chemical bond in which 2 atoms share a pair of valence electrons.
When two atoms share 1 pair of electrons, the bond is a single bond.

12. Molecules of Elements
Two hydrogen atoms bonded together form a unit called a molecule
Molecule- neutral group of atoms that are joined together by one or more covalent bonds
The attractions between the shared electrons and the protons in each nucleus hold the atoms together in a covalent bond.

13. Diatomic Molecules & Multiple Covalent Bonds
Diatomic Molecules- occurs in many nonmetals. It’s two atoms of the same element.
Ex: Halogen Group
HONClBrIF
Multiple Covalent Bonds
Nitrogen has 5 valence electrons. It needs to share 3 pairs of electrons in order to be happy.

14. Unequal Sharing of Electrons
In general, elements on the right of the periodic table have a greater attraction for electrons.
Fluorine has the strongest attraction. 
Polar Covalent Bonds
Electrons are not shared equally. Ex: H-Cl
Electrons will hang out by Cl, giving it a slight negative charge. The other atom will have a slight positive charge.
Shared electrons in a hydrogen chloride molecule spend less time near the hydrogen atom than near the chlorine atom.

15. Nonpolar Covalent Bonds
Electrons are shared equally.
Polar molecules have stronger attractions to each other.

16. 6.3 Naming Compounds and Writing Formulas
Naming Ionic Compounds
Binary Ionic Compounds – Made from only 2 elements – 1 metal and 1 nonmetal
Cation first followed by anion.
Change the ending of the anion to -ide

17. 6.3 Naming Compounds and Writing Formulas
Writing Formulas for Ionic Compounds
Place the symbol of the cation first, followed by the symbol for the anion.
Use subscripts to show the ratio of the ions in the compound (all compounds must be neutral)
Use criss-cross method

18. 6.3 Naming Compounds and Writing Formulas
Naming Molecular Compounds
The more metallic element appears first.
The name of the second element changes its ending to –ide.
Ex: carbon dioxide
Use the Greek prefixes to reflect the number of atoms of each element.
Ex: dinitrogen tetraoxide N2O4
If mono appears in the first element, the prefix is dropped.
Ex: NO2 mononitrogen dioxide becomes nitrogen dioxide.

19. 6.3 Naming Compounds and Writing Formulas
Writing Molecular Formulas
Write the symbols for the elements in the order the elements appear in the name
Prefixes indicate the number of atoms of each element – they become subscripts
If there is no prefix, there is only 1 atom
Ex: Diphosphorus tetrafluoride
P2F4

20. 6.4 The Structure of Metals
Remember, metals like to lose electrons.
What happens if no nonmetals are present to accept the extra electrons?
In a metal, valence electrons are free to move along the atoms.
Metal atoms become cations surrounded by a “sea of electrons”
Metallic Bond- the attraction between a metal cation and the shared electrons that surround it.
The cations in a metal form a lattice that is held in place by the strong metallic bonds between cations and the surrounding valence electrons.
Overall, a metal is neutral because the total number of electrons does not change.

21. The sea of valence electrons can explain the various properties of metals
1. Alkali metals are very soft. The bonds between the cations and the electrons are very weak because each metal only contributes 1 valence electron.
2. An electric current is a flow of charged particles. Metals have a built-in flow of charged particles.
3. Metals are malleable. When metal is struck with a hammer, the metal ions shift their position and the shape changes
In a metal, cations are surrounded by shared valence electrons. If a metal is struck, the ions move to new positions, but the ions are still surrounded by electrons.

22. Alloys
Gold is a soft metal. It becomes harder when mixed with Ag, Cu, Ni, or Zn
Alloy – A mixture of two or more elements, at least one of which is a metal.
Alloys have the characteristic properties of metals.
EX:
Gold that is 100 percent pure is labeled 24-karat gold.
Gold jewelry that has a 12-karat label is only 50 percent gold.
Jewelry that has an 18-karat label is 75 percent gold.