1. Intro to Chemical Bonding

2. Why do atoms form chemical bonds?
atoms bond to become more stable (lower energy)
energy must be released when a bond is formed (exothermic)
ex) C(s) + O2(g) → CO2(g) kJ
How do they for bonds?
atoms tend to lose, gain, or share electrons in a bond
Elements will react to have a full valence energy level (8 e-)

3. Electron Dot Diagrams (Lewis diagrams)
Method used to analyze the type of bonds formed between atoms
simplified model of the atom
Kernal – consists of the nucleus and the inner e-, represented by the element symbol

4. Li Be B C N How do we write them?
Valence electrons are placed as dots around the element symbol
place one dot on each of the 4 sides of the symbol
after one electron is on each side, double up
Li Be B C N

5. O F Ne
each unpaired electron represents one bonding site

6. Ionic Bonding

7. Formation of Ionic Bonds
Atoms with strong attraction for electrons (nonmetals), remove electrons from atoms with low electronegativity (metals)
Result: electrons are TRANSFERRED from a metal to a nonmetal which form:
Negatively charged ion
Positively charged ion
Ionic bond is the result of the attraction between the oppositely charged ions

8. Electron Dot Diagrams of Ionic compounds
Draw the dot diagrams of the following atoms: Ex) K + Br K Br K + Br K Br

9. DO NOW
Draw electron dot diagrams for the compounds made up of: Strontium and chlorine Potassium and oxygen

10. Electron Dot Diagrams of Ionic compounds
Mg + O Mg O Ca + Cl

11. Electron Dot Diagrams of Ionic compounds
Li + O Al + O

12. Ionic Bond Predictors
The greater the difference in electronegativity values between the elements, the more ionic in nature the bond will be.
Typically the EN difference is 1.7 or greater
(HF is an exception to the rule)

13. Properties of Ionic Compounds
Solids at room temperature
Ions held in fixed positions called crystal lattice
Not composed of molecules, but formula units (ratio of ions in crystal)
High Melting points and boiling points
Brittle, break along planes

14. Properties of Ionic Compounds
Poor conductors of heat and electricity in solid state
Good conductors of electricity when melted or dissolved in water (electrolyte)
Ex) NaCl(l) or NaCl(aq)

15. Formulas of Binary Ionic Compounds
Chemical Formula: combination of symbols and subscripts used to represent the composition of a compound
- Binary means it is made up of 2 different elements
Subscripts represent the simplest ratio of ions that make the compound neutral

16. How do we write formulas for ionic compounds?
Rules:
Write the symbols for the elements that make up the compound.
2. positive ion must be written first
3. sum of charges of ions must equal zero
- criss cross charges if they don’t add up to
zero

17. Examples
Write for formula for: Calcium oxide Potassium sulfide

18. Transition Metals
Can have more than one possible charge, Roman numerals are used to designate the charge of the metal in the compound
Ex) Nickel (II) chloride Iron (III) oxide

19. What’s in a name? Binary compounds always end in –ide
Some compounds end in –ite or –ate
This indicates the presence of a polyatomic ion!!

20. Polyatomic Ions
Polyatomic ions (Table E) are groups of elements that are covalently bonded together and carry a charge.

21. Writing formulas with polyatomic ions.
Ex) sodium phosphate copper (II) sulfate calcium hydroxide magnesium nitrate

22. Naming Ionic Compounds
Name the cation and anion
- use metal name
- change nonmetal name ending to –ide
carbon nitrogen oxygen
carbide nitride oxide
- if there are more than 2 elements, check table E for polyatomic name

23. Naming Ionic Compounds
2. Figure out if you need a Roman numeral in the name. - only when the metal can have more than one charge 3. Figure out what the Roman numeral should be - reverse criss cross

24. Practice Problems
ZnO NaNO3 FeCl3 Pb(NO3)2

25. One more, for good luck
NH4NO3