1. Bonding, Replacements, Redox
Reactions
Bonding, Replacements, Redox

2. Review - ions Atom – a particle with NO charge (protons = electrons)
Ion – a particle WITH a charge (protons ≠ electrons)
Cation – positive ion
Anion – negative ion
Protons NEVER change (atomic #)
Example: If Na (Sodium) has a +1 charge, that means it lost one electron.
Why: Protons are positive and electrons are negative. So sodium lost one “negative” particle, there is an imbalance.
Atom (p=e) Ion (p≠e)
11 protons = 11 electrons 11 protons = 10 electrons
No Charge +1 charge

3. Practice Did it gain or lose an electron? What is the charge? Cl -1
Gained 1 electron
B -2
Gained 2 electrons
Ga +3
Lost 3 electrons H
Neither, no charge, its an atom
Li +1
Lost 1 electron
What is the charge?
Beryllium: gained 1 electron
-1 charge
Potassium: lost 3 electrons
+3 charge
Lithium atom
No charge!
Boron: lost 2 electrons
+2 charge
Nitrogen: gained 3 electrons
-3 charge

4. Ionic Bonding

6. Sodium lets Chlorine use its valance electron

7. http://www. matsceng. ohio-state

8. http://www. matsceng. ohio-state

9. Ionic Bonds: One big greedy thief dog
Ionic Bonds: One big greedy thief dog! Ionic bonding can be best imagined as one big greedy dog stealing the other dog's bone. If the bone represents the electron that is up for grabs, then when the big dog gains an electron he becomes negatively charged and the little dog who lost the electron becomes positively charged. The two ions (that's where the name ionic comes from) are attracted very strongly to each other as a result of the opposite charges.

10. Surprise!

11. Single & Double Replacement Reactions
Single-replacement reaction: a chemical reaction in which one element is substituted for another element in a compound, making a new element and a new compound as products.
2NaCl(aq) + F2(g) → 2NaF(s) + Cl2(g)
Chlorine is replaced by Fluorine
Example: Formation of rust on
Iron (Fe) in the car's metal body can oxidize forming iron oxide (Fe2O3), or rust. 
Chemically, the iron reacts with water and oxygen to form hydrated iron oxide.  4Fe(s) + 2H2O + 3O2(g)  2Fe2O3 • H2O

12. Single & Double Replacement Reactions
Double-replacement reaction: occurs when parts of two ionic compounds are exchanged, making two new compounds. 
CuCl2(aq) + 2AgNO3(aq) → Cu(NO3)2(aq) + 2AgCl(s)
Chlorine & Nitrate switched
Example: Baking a cake – baking soda (NaHCO3) mixes with acidic substances in the batter
NaHCO3 + HA (acid)  NaA + H(HCO3)
H(HCO3) decomposes into CO2 and Water.
CO2 is responsible for making the cake rise

13. Redox Reactions Oxidized? Reduced? OIL  Oxidation is losing
The loss of electrons
The gain of oxygen
The loss of hydrogen
Reduced?
RIG  Reduction is gaining
The gain of electrons
The loss of oxygen
The gain of hydrogen

14. Reduced? Oxidized? Redox Reactions Burning of methane.
CH4 + 2O2 -> CO2 + 2H2O
Carbon is oxidized (loses all four hydrogen)
Reduced?
Cl2 + H2 → HCl
Hydrogen is added to chlorine to form hydrogen chloride. Thus, chlorine gas is getting reduced to form hydrochloric acid.

15.
Read the 4 slides and take the quiz at the end