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.
.
Thursday, March 25, 2010
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
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
Tuesday, March 23, 2010
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
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
Monday, March 8, 2010
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)
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)
Thursday, March 4, 2010
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 orbitaloctet
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!!)
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 orbitaloctet
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!!)
Tuesday, March 2, 2010
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
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
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