THE MONTH OF JUNE

We were given a worksheet to work on to prepare for our final

PS: if we finish our worksheet then we get 1% higher than our original marks! YAAAAAAY MR.DOKTOR :)

MAY 27

Dear mr. Doktor,

we weren't in class (due to preparing for the sports banquet) but we got a few notes from the other students in our class.

- We needed the following materials: isopropyl alcohol, methanol, salicylic acid, acetic acid, concentrated sulphuric acid, 2 x 200 mL beakers, ice water, eye droppers, and test tubes

- Remember that esterfication is the formation of an Ester from a carboxylic acid and an alcohol

- Esters are responsible for many common smells:
isoamyl acetate-----> banana
isobutyl salicylate-----> raspberry
methyl salicylate----->wintergreen
ethyl butyrate-----> pineapple
benzyl butyrate-----> cherry
ethyl propionate-----> rum
isopropyl acetate-----> perfume
benzyl acetate-----> peach
methyl butyrate----->apple
octyl acetate----->orange
propyl acetate-----> pear
ethyl phenylacetate-----> honey

1) We used a hot plate to heat up about 150 mL of water in a beaker
2) We added one scoop of salicylic acid to a test tube
3) We added 15 drops of methanol to the same test tube
4) We added 2-4 drops of Sulphuric acid (Had to be careful however as sulphuric acid is very corrosive)
5) We placed the test tube in the hot water bath for 15 minutes and placed a 10 ml beaker over the test tube
6) We colled the test tube in the ice water bath for 2 minutes

hope this makes up for it!!

7) We wafted the fumes toward our noses to carefully smell the test tube. Success! Wintergreen!

MAY 25

Today in class we got into groups of 2 or 3 and we were given molecules !!! yaaay and we were given an amount of time to see how many we could built :)

My group and i only got up to 11 but we were having so much fun that we decided to finish it :)

here are the the molecules that we had to build !!!!!!!!!

1) Methyl butanoate
2) dichloroethane
3) 3 enthyl 2 pentanone
4) Acetic acid
5) dimethyl ether
6) ethyl propyl ether
7) 2 bromo 4,4 dimethyl pentanal
8) 2,3 pentadiol
9) ethylamide
11) 2, 2 dimethyl butylamide
12) propyl butanoate
13) Formaldehyde
14) Phenol
15) 3 choloro 3 methyl 2 butanone

MAY 19

AMINES

-contains nitrogen with carbon chains --> primary, secondary, tertiary.

******remember nitrogen can have up to 3 bonds********

- Make up amino acids (amine and carboxyclic acid)
- Naming: Alkyl prefix with -amine ending
- Two ways of naming: Example- Another way of saying methylamine is aminomethane

here is a youtube video where it'll explain it more in depth

http://www.youtube.com/watch?v=R0i74H9-VMs

AMIDES

- General group: Double-bonded oxygen to carbon and NH2
- Naming: Use carbon prefix and -amide suffix
- Building block of proteins
-Nylon/Kevlar/Penicillin/LSD

and here is an example of a guy teaching amides

http://www.youtube.com/watch?v=0JxBxHEoyZI

MAY 17

ALDEHYDES

- Double bonded O, single bonded H at the end of a chain
Naming: change the -e ending to -al

- Found in insect bites
- Building blocks of fats/steroids

- found in flavoring, perfumes, cospectics, fruits, vegetables oil
- They are formed by esterfication of carboxylic acids
- Name the primary chain with -yl ending
- Secondary chain ends in -oate

MAY 13

FUNCTIONAL GROUPS

1. Halides

-group 17 elements

-bromine (bromo), Chlorine (chloro), Flourine (floro)

F- -F

C=C

Br- -Cl

answer: 1 bromo 2 chloro
1,2 floro 1 ethene

2. Alcohols

-have an OH (hydroxyl) functional group

-changing the ending to -- OL

-Cl -OH

CH3 - C - CH - CH3

-Br

answer: 3 bromo 2 butanol

3 chloro

3. Ethers

-there is an oxygen atom in between two carbon chains

-use side chain endings (-YL) for both chains followed by ether

CH3 - CH2 - O - CH2 - CH2 - CH3

answer: ethyl propyl ether

4. Ketone

-double bonded oxygen

-change ending to --ONE

=O -Cl

H3C - C - CH2 - C - CH3

-CH2

-Ch3

answer: 4 methyl 4 chloro

2 hexanone

MAY 5 2010

(this is a continuing of the last class`notes)

B. ALKENES
-all the same rules for naming apply
-use the correct prefix and -ene ending
-identify the location of the double bond using carbon numbers

Examples
1. NAME

CH2=CH-CH2-CH3

answer: 1-Butene

2. Draw the structural formula for 2 methyl 1 pentene

H2C=C-CH2-CH2-CH3

3. NAME

H2C=CH-CH=CH-CH3

1,3 PENTADIENE (add a+di,tri,etc to double bonds)

4. NAME
CH3

H2C= CH-C-=CH-CH3

3 methyl 1,3 pentadiene

C. TRIPLE BONDS
-use- YNE ending

5. NAME

ASK FOR EXAMPLES

*your triple and double bonds must be included in your longest chain.
*double and triple cannot be side chains
*it has to be alphabetical when you state your answers

****HOMEWORK***** finish last class`worksheet and do numbers 1,2,3 in your new worksheet!

MAY 3 2010

Today in class we learned something new!!!!

**must remember** CARBONS have to have 4 BONDS!!
ORGANIC CHEMISTRY

-organic chemistry is the study of the carbon atom and its compounds.

-carbon compounds outnumber all other compounds combined!

-->carbon can form many different bonds

-->bonds can have different arrangements

-->carbon can form long chains

HYDROCARBON HIERARCHY

ISOMERS

One molecular formula can represent several different compounds. These are called iomers.

C4H10

CH3-CH2-CH2-CH3

**RULES**

ALKANES

1. Circle the longest carbon chain. Name the chain with the appropriate prefix and the --ANE ending!

2. Locate any side chains by numbering the carbon chain. Use the lowest possible numbers.

3. Name the side chaine with appropriate prefix and --Y ending!

4. If there are more than one of the same chain alkyl side chain add the multiplier in front of the branch name.

EXAMPLES:

ask either on of your group members for the examples because they are honestly way too hard to draw on this blog! (=D)

but here is a link to a few examples

http://butane.chem.uiuc.edu/cyerkes/Chem104A_BFA05/Genchemref/ex_alkanes.GIF

and if you were sick, make sure you go to mr.doktor to ask him for help...

HOMEWORK: worksheet on ORGANIC CHEMISTRY

do not do-----> #3,6,8,10, & 13 h,i,j,k

HELLO MR.DOKTOR

today you told us that we'd be having our chapter test next class.. whoooopeee!
You gave us this class to review. we went over the worksheet. and you handed us a solution chemistry review

* remember to know intermolecular and intramolecular*
inter--> outside
intra-->inside

Today in class we continued learning about polarity and nonpolarity

• MOLECULAR AND INTERMOLECULAR BONDS
Intermolecular means the bonds outside molecules
- Intramolecular means bonds inside molecules

• Polarity is the result of intermolecular bonds
• Most bonds are electrostatic:

1. LONDON DISPURSION FORCE (L.D.F)
- Experienced by all molecules
- Result of electrons pushing on each other
- Weakest of all forces

- As the number of electrons increase L.D.F increases

- Comparison between the atoms Aluminum and Argon
Q:Which molecule will have a longer l.d.f?
A: Argon because it’s got more electrons. Which ever has more electrons experiences a longer LDF
- As the number of electrons increase L.D.F increases.



2. Dipole- Dipole
- Dipoles are partial separation of charges
- L.D.F is a type of temporary dipole
- Why is it a temporary dipole? Because electrons are always moving. Electrons always moving they don’t necessarily have to be in the same place.
- Some molecules have a permanent dipole
- These are polar molecules
- Polarity is determined by electrons affinity (how much an atom wants electrons)
- Electrons affinity is called electronegativity
- Electronegativity is highest on the top right and lowest on the bottom left


- Electronegativity is highest on the top right and lowest on the bottom left.
- A bond between two atoms/molecules with different electronegativities results in a dipole-dipole bond.

• Whats a dipole dipole strength between the two molecules Cl -Cl? None! Because none of them are polar
• Polar= dipole dipole
EXAMPLES: which bonds will result in a dipole-dipole force?

1.H-Clyes
2. O-Hyes
3. F-F No
4. O-Cl yes
5. I-Br yes

Are the following compounds polar or nonpolar?
1. CHCl3polar
2. 2. BI2Brpolar
3. C2H4non polar
4. C2H2Cl2non polar

DIPOLE DIPOLE FORCES ARE WEAK VERSIONS OF IONIC BONDS
COMPOUND Boiling Point Number of electrons
N2 -196 degrees celcius 14
O2 -183 16
NO -152 15
ICL 97 70
Br2 59 70

homework: questions 1 & 2 on worksheet

Today in class we learned about the polar and non polar solvents

Polar and non-polar solvents

• Polar substances have an unequal distribution of changes.
DRAW IMAGE



• Non- polar substance have equal change distribuation
DRAW IMAGE

and we did a lab - the objective was to determine if Glycerin is Polar or non-polar.
after mixing the test tubes, we noticed that the solvents water sugar- after mixing hte two dissolved. also the salt. some of the test tubes changed colors, for ex. iodine and the paint thinner. also after mixing iodine and water: it just changed colors from clear to brown, and it did not dissolve.

in the end we have conconluded that glycerin is polar because it mixed with water which is also a polar substance.
non polar can only react with non polar.
homework: FINISH THE LAB

April 12, 2010

Electrical conductivity in solutions requires charged ions to be transferred.
Ionic solutions dissociate, or form ions so they always conduct
NaCl(s)- Na(aq) + Cl(aq)
Molecular substances do not (usually) dissociate.
C12 H22 O11 h2o- C12 H22 O11 (aq)
BaCl2 (s) h2oBa(aq)+2 +2Cl- (aq)
CH3COOHCH3COO- +H+
96% 4%

Follow the chart to determine conductivity
Is it a metal if yes it is conductive

Homework:

1) Al (s)
2) H2so4(aq)
3) I2(s)
4) Br2(1)
5) Mg(OH)2(aq)
6) CH4(g)
7) PCL3(1)
8) ZnBr2(s)
9) NH3(aq)
10) Cr(NO3)2
11) H2O2
12) Cu3(PO4)2

In the beginning of class,we marked and went over 5-1 and 6-4.
We reviewed how to do lewis dot diagrams.

Covalent bonds
-electrons shared between non
- To draw lewis dot diagrams
1. Total all valence e- in all atoms
2. Identify the element that can form the most bonds. this will be the central
atom.
3. Draw bonds between atoms as a line. This represents 2 e-.
4. Any e- not part of a bond are lone pairs around the atom
5. Check to make sure each atom has a full octet.exception for hydrogen it has
two.
Mr. Doktor did a demonstration and showed a piece of sodium.It had a shiny finish to it. it has a high melting point. He put the piece of sodium into a glass filled with hydrogen.He tried to accomplish an explosion.
.

March 25

In the beginning of class,we marked and went over 5-1 and 6-4.
We reviewed how to do lewis dot diagrams.

Covalent bonds

• Electrons shared between non-metals


• To draw lewis dot diagrams

1. Total all valence e- in all atoms

Kristina Ravalo
Mr.Doktor
Chemistry 11
Block E
March. 23, 2010

Q: isotopes are used for in medicine? A:they give off radiation

ATOMS & IONS
• Atoms are electrically neutral
• # of protons= # of electrons
• Ions have different number of protons and electrons
• Ions can be either positive (lost e-) or negative (extre e-)
• Metals will be positive and non metals will be negative
• In order for something to be positive, it needs to lose electrons.
• If it’s negative it’s gaining electrons
• Cation= positive ion
• Anion= negative ion

Examples:
Determine how many electrons each of the ions have. What type of ion are they? (cation or anion)?
Ca2+  lose 2e- it is a CATION
Ag+ lose 1e- it is a CATION
F-  gains 1e- it is an ANION
H- gains an e- it is an ANION
H+ loses an e- it is a CATION
N3-  gains 3e- it is an ANION

Examples:
Determine how many protons, neutrons and electrons the following substances have.
Protons: same number as atomic number
Neutrons: atomic mass minus protons
Electrons: atomic number and protons

76AS3- protons: 33
 Neutrons: 43
 Electrons: 36
201 AU+  protons: 79
 Neutrons: 122
 Electrons: 78
56FE 3+ protons: 26
Neutrons: 30
Electrons: 23


BOHR DIAGRAM FOR IONS
• Draw the energy level bohr diagram for the following ions:
-Ca 2+
8e-
8e-
2e-
Ca

-Li+
4-
2-
Li

F-
8-
2-

O2-
8e-
8e-
2e-

P3-
8e-
8e-
2e-

CHEMICAL BONDS
• A bond is an electrostatic attraction between particles
• Bonds occur as elements try to achieve noble gas electron configuration
- Noble gases (usually) do not form compounds or bonds
- In noble gases the outermost energy level have stable octets
• Metals lose electrons (oxidize)
• Non metals gain electrons (reduced)




LEWIS DOT STRUCTURE
• Atoms can be represented by dot diagrams
- - Dots represent electrons
- Only valence level electrons are shown
• Write the atomic symbol for the atom
-This represents the nucleus and filled inner electron levels
• One dot is used to represent outer energy level electrons
-One e- is placed in each orbital before any pairing occurs
- Beginning with the 5th e-, pairing can occur up to a maximum of 8e-

Ex. Draw the lewis dot diagram for the following atoms:
- Nitrogen
- Fluorine
- Oxygen
- Calcium
- Lithium
- Hydrogen



LEWIS DOT STRUCTURE
• Atoms can be represented by dot diagrams
- - Dots represent electrons
- Only valence level electrons are shown
• Write the atomic symbol for the atom
-This represents the nucleus and filled inner electron levels
• One dot is used to represent outer energy level electrons
-One e- is placed in each orbital before any pairing occurs
- Beginning with the 5th e-, pairing can occur up to a maximum of 8e-

Ex. Draw the lewis dot diagram for the following atoms:
- Nitrogen
- Fluorine
- Oxygen
- Calcium
- Lithium
- Hydrogen

IONIC BONDS
• Electrons are transferred from metal to nonmetal
- No dots are shown on metal
• ‘charged’ species is written in brackets
• Example: sodium chloride
Na Cl

EX: DRAW THE LEWIS DOT DIAGRAM FOR
- LITHIUM FLUORIDE
- CALCIUM CHLORIDE

Thompson experimented with ELECTRONS.

8e-
8e-
2e-
Nucleus

Increase in voltage = increase in energy

High voltage power source
1. Hydrogen – spectrum lines are very simple
2. Different elements on periodic table have different colors
3. Colors help determine what elements are in a star for example

Emission Spectra

• Each element gives off a specific colour of light
• These are known as emission spectra
-unique to each element
• If electrons absorb energy they can be bumped to a higher level
• When they fall to a lower level they release energy as light
• Each element has its OWN combination of colours

Atomic Structure

• Atoms are made up of parts called SUBATOMIC particles
• Protons (positive)
• Neutrons (neutral)
• Electrons (negative)
• Electrons have to exist in energy levels

PARTICLE MASS
(multiples of proton) CHARGE
(elementary charges) LOCATION
PROTON 1 +1 Nucleus
NEUTRON 1 0 Nucleus
ELECTRON 1/1837 -1 Outside




Atomic Number

• Atomic Number: number of protons
• Diagram of the element Titanium (Labels: atomic number, symbol, atomic mass, and ion charges)

Isotopes

• The number of protons determine the type of element
• Changing the number of neutrons changes the ISOTOPE of the element
• All isotopes have the same chemical properties
• The nuclei of the three isotopes of hydrogen
Protium Deuterium Tritium
*1 proton *1 proton *1 proton
*1 neutron *2 neutrons

Mass Number

• Mass number is total of protons and neutrons
• Symbol give is A
• Different isotopes have different masses (ex. Helium)
• Mass Number = Atomic Number + Number of Neutrons
A = Z+N
• Examples:
How many protons and neutrons are in each of the elements?
Lithium Titanium Silver
Protons = 3 Protons = 22 Protons = 47
Neutrons = 4 Neutrons = 26 Neutrons = 61

Complete the table
ISOTOPE MASS # ATOMIC # # OF PROTONS # OF NEUTRONS
OS
Osmium 190 76 76 115
Zn
Zinc 65 30 30 35
C
Carbon 14 6 6 8
H
Hydrogen 2 1 1 1

HOMEWORK: 1Periodic Table Assignment & 2Atomic Theory: Isotopes (in the booklet)

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!

January 11

To start class off we corrected the classifying chemical equations and another worksheet. Mr. doktor did a demonstration on burning steel wool and magnesium. When Mr.doktor burnt the steel wool, the part that was in the fire was darker then the rest because the burnt wool was ion oxidized and it does not burn. When he burnt the magnesium, it looked like fireworks, it was very bright. He also passed around ammonia nitrate, he told the class that this was the stuff that is in the heat packs.

Heat in Chemical RxNs

• Reactions that release heat are exothermic
• Reactions that absorb heat heat are edothermic

Heat is a form of energy. All chemicals have stored energy called enthalpy

Enthalpy of water < align="left">

January 7

January 5

Today in class we learned about the different types of reactions.
SYNTHESIS
A + B = AB
ex. Al + F2 -> AlF3

DECOMPOSITION
AB -> A + B
ex. H3PO4 -> H2 + P4 + O2

SINGLE REPLACEMENT
A + BC -> B + AC
ex. Ca + KCl -> K + CaCl2

DOUBLE REPLACEMENT
AB + CD -> AD + CB
ex. MgCl2 + K2SO4 -> MgSO4 + ClK

NEUTRALIZATION
Acid + base -> Water + Ionic salt
ex. H2S04 + KOH -> HOH + K2SO4

COMMBUSTION
* reaction with oxygen
ex. C8H18 + 02 -> Co2 + H2O