november 26, 2014
Types of Chemical Reactions
Synthesis (Combination) Reaction
A reaction in which two or more substances react to produce a single product.
A + B ----> AB
decomposition reaction
A reaction in which a single compound breaks down into two or more elements or compounds.
AB ------> A + B
Single-Replacement Reactions
A reaction in which the atoms of one element replace the atoms of another element in a compound
A + BX ------> AX + B
or
A + XB -------> XA + B
A metal or halogen will only replace another metal or halogen if it is more reactive than that metal or halogen. You must refer to the activity series of metals or halogens.
Double Replacement Reactions
A reaction that involves the exchange of ions between two compounds
AB + CD -----> AD + CB
Combustion Reactions
A reaction in which oxygen combines with a substance.
A + O2 -------->
In a balanced chemical equation the mass is conserved.
Each side of the equation has the same number of atoms of each element.
Chemical reaction
The changing of substances into different substances by the breaking of old bonds and the formation of new bonds
Chemical equation
An expression representing a chemical reaction. (a recipe)
The formulas of the reactants(on the left) are connected by an arrow with the formulas of the
products on the
right.
Reactant
A starting substance in
a chemical reaction
Product
A substance formed in a chemical reaction
Coefficient
A small whole number
that appears in front of a formula that indicated the number of molecules, atoms or formula units, of that substance
Subscript
a number that appears smaller than the normal type and slightly below to indicate the number
of that element in the
compound
In a balanced chemical equation the mass is conserved.
Each side of the equation has the same number of atoms of each element.
November 21
Blocks 1A,2A,5A
atom
single unit of an element (except for the diatomics)
molecule
single unit of a compound or
diatomic element
formula unit
single unit of an ionic
compound
mole
the amount of a substance that contains 6.02 x 10 exp23 representative particle of that substance. The mass is equal to its' atomic mass in grams of the substance.
Representative particle
the particle that a substance commonly exists in.
Example:
atoms, molecules,
ions
Avogadro's number
6.02 x 10 exp 23
the number of representative particles contained in one mole of a substance.
molar mass
the mass of one mole of a substance . Equal to the atomic mass ( or sum of atomic
masses)of the substance in
grams.
November 13
Block 1A
Review for quarterly
Scientific method
an approach to the solution of scientific problems
Observation
look at something and state
the problem
Hypothesis
a proposed reason for
what is observed
Experiment
means of testing a
hypothesis
Theory
a thoroughly tested explanation
of why an experiment gives certain results
Blocks 2A, 5A
Review for quarterly
Half Life
Time required for one
half of a sample of a radioisotope to decay.
November 6
Block 1A
Review for quarterly
Percent Composition
(Percent by mass)
mass of the part divided by the mass of the whole, multiplied by
100.
part
whole X 100
Blocks 2A,5A
Review for quarterly
Scientific method
an approach to the solution of scientific problems
Observation
look at something and state
the problem
Hypothesis
a proposed reason for what is
observed
Experiment
means of testing a
hypothesis
Theory
a thoroughly tested explanation
of why an experiment gives certain
results
Chromatography
A method of separation
of mixtures that relies on the difference in the attraction of the
components of the mixture to the chromatagraph medium.
November 1
Block 1A
Naming and writing formulas of ionic compounds that contain transition metals
Blocks 2A,5A
Nuclear chemistry
deals with the changes in the nucleus of the atom
radioisotope
isotopes that have unstable nuclei and undergo radioactive decay
radioactive decay
process in which an unstable nucleus emits radiation
radioactivity
the process in which a nucleus gives off alpha, beta or gamma radiation
radiation
the giving off of energy
alpha emission(radiation)
emission of an alpha particle (helium nuclus) from the nucleus of an atom.
Beta emission(radiation)
emission of a high speed electron, formed when a neutron decomposes into a proton, from the nucleus of an atom.
gamma emission(radiation)
emission of high energy electromagnetic radition from the nucleus of the atom.
Block 5B
November 30, 2012
Do Now: write the electron configuration and the orbital notation for an atom of argon
Students worked on more electron configurations.
Energy orbital fill differently after the third period.
The d orbitals of the previous energy level (3) fill before the p orbitals of the same energy level (4)
Students worked on the worksheet below
electron_configuration_worksheet.pdf | |
File Size: | 85 kb |
File Type: |
Valence electrons:
The electrons in an atoms outermost orbitals. Valence electrons determine the elements chemical properties.
Block 1B
November 30, 2012
Do now: What caused the colors we produced in the lab from the flame tests?
Erwin Schrodinger
Derived an equation to deteremine the electrons energy and position. It is called the "Quantum Mechanical Model of the Atom".
Atomic Orbital
area around the nucleus where the electron is likely to be
found.
Probability
Principal Quantum Number (n) denotes the Principal Energy Level and describes the size and energy of the atomic orbital.
Energy Sublevels
Principal quantum numbers indicate
the number of
sublevels.
s,p,d,f
Orbitals
per
sublevel
s=1
p=3
d=5
f=7
An
atomic orbital can hold 2 electrons with opposite
spins
Electron Configuration
The arrangement of electrons in
the atom
Rules for Electron Configuration
1) Aufbau Principle: electrons will always occupy the lowest energy orbitals available first.
2) Pauli Exclusion Principle: a
maximum of 2 electrons (with opposite spins) can occupy an orbital.
3) Hund's Rule: for equal energy orbitals, electrons will occupy each orbital before pairing up
Block 1A,2A and 5A
November 29,2012
Do Now: How can we calculate the energy given off when we placed the atoms in the bunsen burner in wednesdays lab?
Neils Bohr
The Bohr atom contained orbits around the nucleus in which the electron could be found.
An electron in an orbit needs to have the specific energy of that orbit. Therefore the electrons in the Bohr atom had energy
Click below to see animation of the Bohr atom
Bohr atom animation
Erwin Schrodinger
Derived an equation to deteremine the electrons energy and position. It is called the "Quantum Mechanical Model of the Atom".
Atomic Orbital
area around the nucleus where the electron is likely to be found. Probability
Principal Quantum Number (n) denotes the
Principal Energy Level and describes the size and energy of the atomic orbital.
Energy Sublevels
Principal quantum numbers indicate the number of sublevels.
s,p,d,f
Orbitals per sublevel
s=1
p=3
d=5
f=7
An atomic orbital can hold 2 electrons with opposite spins
Electron Configuration
The arrangement of electrons in the atom
Rules for Electron Configuration
1) Aufbau Principle: electrons will always occupy the lowest energy orbitals available.
2) Pauli Exclusion Principle: a maximum of 2 electrons (with opposite spins) can occupy an orbital.
3) Hund's Rule: for equal energy orbitals, electrons will occupy each orbital before pairing up
Block 1B
November 28, 2012
Do now:
What does the Bohr atom have that the Rutherford atom did not have?
Student performed the flame test lab. Click below to download the lab
flame_tests_lab.pdf | |
File Size: | 140 kb |
File Type: |
Erwin Schrodinger
Derived an equation to deteremine the electrons energy and position. It is called the
"Quantum Mechanical Model of the Atom".
Atomic Orbital
area around the nucleus where the electron is likely to be found. Probability
Principal Quantum Number (n) denotes the
Principal Energy Level and describes the size and
energy of the atomic orbital.
Energy Sublevels
Principal quantum numbers indicate the number of sublevels.
s,p,d,f
Orbitals per sublevel
s=1
p=3
d=5
f=7
An atomic orbital can hold
2 electrons with
opposite spins
Block 5B November 28, 2012
Erwin Schrodinger
Derived an equation to deteremine the electrons energy and position. It is called the "Quantum Mechanical Model of the Atom".
Atomic Orbital
area around the nucleus where the electron is likely to be found. Probability
Principal Quantum Number (n) denotes the
Principal Energy Level and describes the size and energy of the atomic orbital.
Energy Sublevels
Principal quantum numbers indicate the number of sublevels.
s,p,d,f
Orbitals per sublevel
s=1
p=3
d=5
f=7
An atomic orbital can hold 2 electrons with opposite spins
Electron Configuration
The arrangement of electrons in the atom
Rules for Electron Configuration
1) Aufbau Principle: electrons will always occupy the lowest energy orbitals available.
2) Pauli Exclusion Principle: a maximum of 2 electrons (with opposite spins) can occupy an orbital.
3) Hund's Rule: for equal energy orbitals, electrons will occupy each orbital before pairing up
Block 1A,2A,4A
November 27, 2012
Do Now:
What is the wavelength of light that has a frequency of 2.7 x 1015 Hz?
electromagnetic waves (electromagnetic radiation)
waves that can travel without a medium and
travel at the speed of light in a vacuum.
click below to see a video on the electromagnetic spectrum
electromagnetic
spectrum
includes all forms of electromagnetic
waves
The atomic emission spectrum of an element is the specific set of frequencies emitted by atoms of that element.
Max Planck
Energy can only be absorbed or released in specific amounts called quanta.
Quantum
The minimum amount of energy that can be gained or lost by an atom
He calculated the relationship between the energy of a photon and the frequency of the emitted waves.
Photon
a quantum of light energy
E=hv
h= plancks constant
Students performed the flame test lab in todays class.
Click below to download the lab
flame_tests_lab.pdf | |
File Size: | 140 kb |
File Type: |
Block 5B
November 26, 2012
Do Now:
What does the Bohr atom have that Rutherfords atom did not have?
Max Planck calculated the relationship between the energy of a photon and the frequency of the emitted waves.
E=hv
h= plancks constant
Students performed the flame test lab in todays class.
Click below to download the lab
Erwin Schrodinger
Derived an equation that treated the electron as a wave. It is called the
"Quantum Mechanical Model of the Atom".
Atomic Orbital
area around the nucleus where the electron is likely to be found. Probability
Principal Quantum Number (n) denotes the
Principal Energy Level and
describes the size and energy of the atomic orbital.
Energy Sublevels
Principal quantum numbers indicate the number of sublevels.
s,p,d,
Orbitals per sublevel
s=1
p=3
d=5
f=7
An atomic orbital can hold 2 electrons with opposite spins
Electron Configuration
The arrangement of electrons in the atom
Rules for Electron Configuration
1) Aufbau Principle: electrons will always occupy the lowest energy orbitals available.
2) Pauli Exclusion Principle: a maximum of 2 electrons (with opposite spins) can occupy an orbital.
3) Hund's Rule: for equal energy orbitals, electrons will occupy each orbital before pairing up
flame_tests_lab.pdf | |
File Size: | 140 kb |
File Type: |
November 26,2012
Block 1A
Do Now:
What is the wavelength of light that has a frequency of 2.7 x 1015 Hz
electromagnetic waves (electromagnetic radiation)
waves that can travel without a medium and
travel at the speed of light in a vacuum.
click below to see a video on the electromagnetic spectrum
electromagnetic
spectrum
includes all forms of electromagnetic
waves
Max Planck
Matter can only
gain or lose energy in small specific amounts called quanta
Quantum
The minimum amount of
energy that can be gained or lost by an
atom
Niels
Bohr The Bohr Atom
a) electrons move around the nucleus in
concentric circles called orbits
b) electrons contain the specific amount of
energy of that orbit.
c) The orbits closest to the nucleus contain less
energy than the orbits further from
the nucleus.
Ground State
the lowest
energy state of an
electron
n=quantum number
(energy level) of the orbit
Click the link below to see the Bohr
Atom
Bohr
Atom
CP Chemistry
November 19,2012
November 20, 2012
November 21, 2012
Light
Energy that travels in waves
Wave
A disturbance that carries energy
Characteristics of a wave:
wavelength
the shortest distance between equivalent points of two adjacent waves
frequency
number of waves that pass a given point per second
electromagnetic waves (electromagnetic radiation)
waves that can travel without a medium and travel at the speed of light in a vacuum.
electromagnetic spectrum
includes all forms of electromagnetic waves
waves_worksheet_wavelength_frequency.pdf | |
File Size: | 96 kb |
File Type: |