Title: Grade 10 Chemistry
1Grade 10 Chemistry
2What is Chemistry?
- The science that deals with the composition and
properties of substances and various elementary
forms of matter - http//dictionary.reference.com/browse/chemistry
- The study of structure and composition
3What is Chemistry?
- Overlaps with biology and physics
- Examples
- Biochemistry
- Physical Science (What we study)
- Quantum Mechanics
4Branches of Chemistry
- Physical Chemistry (What we study)
- deals with the investigation of the laws and
theories of all branches of chemistry. - primary goal is the investigation of the
structure andtransformation of matter and the
interrelationships of energy and matter. The
subject of matter, the experimental techniques,
and the instruments used are common to
bothchemistry and physics.
5Branches of Chemistry
- Analytical Chemistry
- is concerned with the separation, identification,
and composition of all kinds of matter.
Analytical procedures are used in every branch of
chemistry. -
- Two broad classifications of analytical chemistry
are qualitative analysis and quantitative
analysis. - Qualitative analysis involves the separation and
identification of the individual components of
materials. It answers the question, What is
present? - Quantitative analysis is, in addition, concerned
with how much of each component is present.
6Branches of Chemistry
- Organic Chemistry
- is the study of carbon-containing materials that
are compounds. - The term organic was derived from the original
belief that these types of compounds were found
only in living organisms. - This branch of chemistry now deals with commonly
used synthetic substances such as plastics,
drugs, dyes, explosives, and detergents. - There are many more organic compounds known that
those of all the other kinds combined
7Branches of Chemistry
- Inorganic Chemistry
- covers the chemistry of all of the elements and
their compounds with the exception of carbon and
its compounds. - This area of chemistry comprises the
investigation of those substances which are not
organic such as nonliving matter and minerals
found in the earths crust.
8Branches of Chemistry
- Biochemistry
- branch of chemistry which includes the study of
the materials and processes that occur in living
organisms. - These materials are largely organic
(carbon)compounds.
9Branches of Chemistry
- Nuclear Chemistry
- deals with the changes in the nuclei of atoms and
the uses of these changes, especially in the
study of how substances react. - Radioactive nuclei, both natural and man-made
decompose spontaneously.
10Matter and Properties (Ch. 4)
- Matter anything that has mass and occupies
volume - Ex. Water is matter, oxygen is matter, because
they all have mass and occupy space. Energy
(light, heat) is not matter. - Matter can be classified, from general to
specific.
11Matter and Properties (Ch. 4)
- Physical Properties
- Properties which define a substance using the 5
senses - Ex. Color, lustre, malleability, conductivity,
magnetism, solubility, melting point, freezing
point, density, etc. - Some physical properties can be used to define a
substance. These are called Characteristic
Properties. - Characteristic Properties properties that
define a substance and separate that substance
from all others that look the same. - Boiling Point
- Melting Point
- Density
12Matter and Properties (Ch. 4)
- Chemical Properties
- Properties that define the chemical make up of a
substance and how it will react with other
substances. - Ex. Flammability, reactivity to water, etc.
13Matter and Properties (Ch. 4)
- Make a list of descriptive terms for observations
of physical and chemical properties. - Read pages 63-65. Define
- Mass
- Substance
- Atom
- Element
- Compound
- Molecule
14Matter and Properties (Ch. 4)
- Read pages 74 77
- What happens in a change of phase?
- Differentiate between a physical change and a
chemical change.
15Structure of the Atom and the Periodic Table (Ch.
6)
- The periodic table was classified by Dmitri
Mendeleev in 1869. He classified elements by
mass, color, taste, etc - The Modern Periodic Table is ordered by Atomic
Number. - The reason is the numbers are related to the
structure of the atom. The differing structures
mean different elements react differently, and
can be logically classified this way.
16Structure of the Atom and the Periodic Table (Ch.
6)
17Structure of the Atom and the Periodic Table (Ch.
6)
- Finding protons, neutrons and electrons (p.
109 and p. 131-132) - Proton
- Electron
- Neutron
18Structure of the Atom and the Periodic Table (Ch.
6)
- To find electrons, it is the atomic number (Z).
Since atoms are neutral (same number of positive
and negative charges), the number of protons for
a neutral atom is the same as the electrons. - Since neutrons are found in the nucleus, and make
up the atomic mass, the number of neutrons is the
atomic mass (A) (rounded to the nearest whole
number) subtracting the atomic number. (Z)
19Structure of the Atom and the Periodic Table (Ch.
6)
- Why does the atomic mass have a decimal?
- It is the average atomic mass. It is made up of
all the known isotopes for that element. - Isotope
- atoms of an element that are identical in terms
of their chemical properties (numbers of p and
e-) (Z) but differ by number of neutrons, and the
Atomic Number (A) differs - Mass Spectrometry (Read handout)
20Structure of the Atom and the Periodic Table (Ch.
6)
- Finding Average Atomic Mass (p. 138 139)
- The atomic mass of the elements have decimal
points. This is due to the calculating of the
average atomic mass, using the percentages of the
abundance found of each isotope. - Ex.
-
- What is the average atomic mass of the element
oxygen, if the naturally occurring abundance of
each is 16O (99.759), 17O (0.037) and 18O
(0.204)?
21Structure of the Atom and the Periodic Table (Ch.
6)
- History of the Atom and Atomic Theory
- Using your electronic device and textbook,
research the following scientists discoveries and
theories. Pay special attention to how the
theory changes over time. - Keep in mind the difference between a hypothesis,
theory and a law.
22Structure of the Atom and the Periodic Table (Ch.
6)
- Democritis
- Antoine Lavoisier
- Law of Conservation of Mass
- Law of Definite Proportions
- Law of Multiple Proportions
- John Dalton and Atomic Theory
- JJ Thomson
- Ernest Rutherford
- Robert Millikan
- Neils Bohr
23Structure of the Atom and the Periodic Table (Ch.
6)
- p.121 What were the short comings of
Rutherfords Model? - Bohrs Model explained some of the short comings
of the planetary model and also, how the
electrons are arranged.
24New Approach to the Atom (Ch. 6 p. 122 - 131)
- Electromagnetic Spectrum
- Line spectra
- Wave vs. Particle
- Bohr Model
- Quantum Mechanical Model
25New Approach to the Atom (Ch. 6 p. 122 - 131)
- Electromagnetic Spectrum
- Entry Level Knowledge
- Grade 8 Electromagnetic Radiation
- How do we see different colors?
26New Approach to the Atom (Ch. 6 p. 122 - 131)
- See light based upon the wavelengths of light
travelling to our eye. - How we see color, is our eyes detect the
wavelength of light that corresponds to that
color - Example If we see green all colors are
absorbed, and green light wavelength is reflected
back to our eye
27New Approach to the Atom (Ch. 6 p. 122 - 131)
28New Approach to the Atom (Ch. 6 p. 122 - 131)
- Electromagnetic Spectrum
- Wavelength is made of three parts
- Frequency
- Number of wave cycles to pass a given point per
unit of time (cycles per second or Hertz (Hz)) - Wavelength
- The distance between crests or troughs of a wave
- Amplitude
- The waves height from 0 to crest
29New Approach to the Atom (Ch. 6 p. 122 - 131)
30New Approach to the Atom (Ch. 6 p. 122 - 131)
- There is an inverse relationship between
wavelength and frequency - All light moves at the speed of light
- c 3.00 x 10 8 m/s
- Energy is a product of the frequency and the
speed of light - Therefore, the greater the frequency, the smaller
the wavelength and the more energy produced
31New Approach to the Atom (Ch. 6 p. 122 - 131)
- Neils Bohr
- Found when an atom was excited light was given
off - Electron gains E, moves from its ground state, to
a higher E level, and then drops back to its
ground state, losing E in the form of light - Light corresponded to the energy given
- Greater the energy, greater the jump, smaller the
wavelength - 7 different colors of light, 7 energy levels
32New Approach to the Atom (Ch. 6 p. 122 - 131)
33New Approach to the Atom (Ch. 6 p. 122 - 131)
34Applications of Line Spectrum
- Research one of the following
- Aurora borealis
- Fireworks
- Neon Lights
35Applications of Line Spectrum
36Energy (Ch. 5)
- The essence of chemical reactions is the making
of a new substance, through a chemical process. - This means that new bonds are formed by the
rearranging of old bonds to make a new substance - All chemical reactions are based upon energy. If
there is enough energy, the reaction goes if
not, the reaction does not occur.
37Energy (Ch. 5)
- 95 of all reactions will go to completion
(REACTANTS to PRODUCTS) - These reactions are considered SPONTANEOUS
REACTIONS - Where does the energy come from?
- Internal
- Bonds between reactants
- When bonds break, E is given off
- If there is enough E, the reaction takes place
- External
- Outside source, like a burner, sun (uv light),
etc.
38Energy (Ch. 5)
- In a change of state
- When a substance melts, E is ____________.
- When a substance condenses, E is
- _________.
- Animation
Added
Removed
39Energy (Ch. 5)
The ability to do work
Done on an object, in response to a force, moves
some distance
40Energy (Ch. 5)
- Forms of Energy (unit Joule (J))
- Potential Energy
- Stored energy, that is available for doing work
- Kinetic Energy
- The energy moving particles or objects have
- Examples
41Energy (Ch. 5)
- Read p. 90 in your textbook
- How is energy converted from one form to another?
- How is energy converted to do work?
- What is the law of conservation of Energy?
42Energy and Chemical Reactions (Ch. 5)
- How can we tell a chemical reaction has taken
place?
Precipitate forms
Gas is given off
Color Change
An odour appears
A change in temperature
43Energy and Chemical Reactions (Ch. 5)
- In reactions, a temperature change is a measure
of energy being lost or gained for the reaction
to occur - When energy is lost to the environment, the
energy of the reactants is greater than the
products. The surroundings will be warmer. - This is called an exothermic reaction.
- (Exo out)
44Energy and Chemical Reactions (Ch. 5)
- When energy is gained from the environment, the
energy of the reactants is less than the
products. The surroundings will be cooler. - This is called an endothermic reaction.
- (Endo in)
45Energy and Chemical Reactions (Ch. 5)
- The minimum starting energy to get a reaction
going is called the Activation Energy. - It is like going over a fence. You have the
energy to get over, but need a little extra to
get over. Once you are on the top, you simple go
to the other side. - On the graphs, it is represented by the
transition from reactants to products.
46Heat Energy, Temperature, and Calorimetry (p. 92
99)
- Temperature is a measure of heat energy
- We use two scales
- Celsius
- Freezing Point of Water 0oC
- Boiling Point of Water 100oC
- Kelvin
- Absolute Zero 0 K (all movement of particles
stops) - Freezing Point of Water 273 K
47Heat Energy, Temperature, and Calorimetry (p. 92
99)
- Heat
- Energy transferred from one medium to another in
a thermal interaction - Temperature is the measure of heat
- Calorie was used as a unit, but a joule is used
- What is a calorie we find on the food we buy?
48Heat Energy, Temperature, and Calorimetry (p. 92
99)
- Calorimetry
- The measurement of the amount of heat released or
absorbed in a chemical reaction - Explain how calorimeter works in your own words.
49Heat Energy, Temperature, and Calorimetry (p. 92
99)
- Calorimetry is a combination of the mass of the
water, the change in the temperature and a
constant for the substance called the specific
heat. - Specific Heat
- Amount of heat energy needed to raise the
temperature of 1 unit of mass of the substance,
by 1 unit of temperature.
50Heat Energy, Temperature, and Calorimetry (p. 92
99)
Substance Specific Heat Capacity at 25oC in J/goC
H2 gas 14.267
He gas 5.300
H2O(l) 4.184
lithium 3.56
ethyl alcohol 2.460
ethylene glycol 2.200
ice _at_ 0oC 2.010
steam _at_ 100oC 2.010
vegetable oil 2.000
sodium 1.23
air 1.020
magnesium 1.020
aluminum 0.900