Today in Class we learned how to draw out Bohr models and Energy levels, we went over a few diagrams.

Bohr Model

- Atoms are electrically neutral= it is equal
- Two different models can be used to describe electron configuration
- 1)Energy level 2) Bohr Model
- Electrons occupy shells which are divided into orbitals.( 2, 8, 8 )
- 2 e- in the first orbital
- 8 e- in the second orbital-octet
- 8 e- in the third orbitaloctet

ARGON
Energy level Model

40
18Ar

2e-
8e-
8e-

(draw image)^

CHLORINE

Energy level mdoel

7e-
8e-
2e-

35
17Cl

Atomic mass – the # of protons= neutrons
(draw image)^
Orbital shapes
- Atomic orbitals each have specific name and shape
- 1s


Hybridized orbitals
- The first of the bohr levels is the 1st orbital and it holds 2e-
- The second level contains the 2s, 2px, 2pv, 2pz orbitals. They combine (hybridize) to form on 2sp3 orbital
Draw img.

Other hybridized orbitals
- There are many different types of hybrized orbitals

FOR HOMEWORK: we are to complete the page in the package titled " ELECTRON ENERGY LEVEL DIAGRAMS FOR ATOMS"
( Pictures coming soon!!)

in the beginning of class, mr.Doktor told us we were gonna go through a review of grade 9 chemistry, going through isotopes-->(different number of neutrons) etc. and he showed us a review of atomic theory.

ATOMIC THEORY

Early atomic theory
Greeks – in 300 BC Democritus said atoms were indivisible particles
(that matter can be divided up into a certain point until you wouldn’t be able to cut down any further)
-Democritus was the first person to mention atoms. – other than that everything else he said was wrong.
-Not testable- no predictions and no information to test whether it was right or wrong.
- cannot be used to explain a chemical reactions.

LAVOISIER(late 1700s) came up with 2 things:
law of conversation of mass & law of definite proportions
- wasn't a true atomic theory b/c it didn't discuss what atoms were or how they were arranged.

PROUST(1799)
-if a compound is broken down into its constituents, the products exist in the same ratio as in the compound.
- experimentally proved Lavoisier laws.

DALTON(early 1800s) 1803-1805
-atoms are solid, indestructible spheres (like billiard balls)
-provides for different elements( these would be diff spheres)
- does not mention subatomic particles
- cannot explain isotopes
-no mention of the nucleus

the grade 12's had to leave for the honors assembly and that is as far as we got. we were given handouts to work on for homework though, 3-1 EXPLORE

JANUARY 29

(Kristina)

JANUARY 27

(alanna)

January 25,2010

Today in class, Mr. Doktor went over any questions from the last homework.
MASS TO MASS & OTHER CONVERSIONS
Example.
Lead(IV) nitrate reacts w/5.0 g of potassium iodide. How many grams of lead(IV) nitrate are required for a complete reaction.
Pb(NO3)4 + 4KI -> PbI4 + 4KNO3

5.0g x 1 mole/ 166g x 1 mole/4 KI x 4 55.29/1 mole Pb(NO3)4 = 35g

2)How many grams of O2 are produced from the decomposition of 3.0g of potassium chlorate?
2KClO3 -> 2KCl + 3O2

3.0g x 1mole/122.6g x 3 mol O2/ 2 mole KClO3 x 33g/ 1 mole O2 = 1.2 g

3) If a 100mL solution of 2.0M(mol/L) H2SO4 is neutralized by solution hydroxide. What mass water is produced.
H2S04 + 2NaOH -> 2HoH + Na2SO4

0.100L x 2.0 mole/ L = .200 mole

.200mole H2SO4 x 2 mole HOH/ 1 mole H2SO4 x 18.0g/1mole = 7.2 g

% yield

• Theorteical yield of a reaction is the quanitity of producits expected
• The amount produced in an experiement is teh actual yield

The percent yield is:
% yield = actual/theoretical x 100

Example
The production of urea CO(NH2)2 is given by
NH3 + CO2 -> CO(NH2)2 + H20

47.7 g of urea are produced, determine
a)Theoretical yield if 1 mol of CO2 reacts
1.0 mole CO2 x 1 CO(NH2)2/1 CO2 x 60.1g/1mole = 60.1g
b) actual yield
47.7g
c)percent yield
47.7g/60.1g x 100 =

HOMEWORK

Gravimetric stoichiometry # 15-20 & extra stoichiometry problems worksheet

JANUARY 19

(Kristina)

JANUARY 13

In the beginning of class we corrected our homework from last days class (ask mr. Doktor for the answer key)

here are the notes mr. Doktor wrote on the board.

EXAMPLE #1

EXAMPLE #2

See mr. Doktor for our homework (worksheet) :

Enthalpy and Heat of Combustion

also be prepared to do a lab next class!