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Title: Grade 10 Chemistry


1
Grade 10 Chemistry
2
What 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

3
What is Chemistry?
  • Overlaps with biology and physics
  • Examples
  • Biochemistry
  • Physical Science (What we study)
  • Quantum Mechanics

4
Branches 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.

5
Branches 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.

6
Branches 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

7
Branches 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.

8
Branches 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.

9
Branches 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.

10
Matter 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.

11
Matter 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

12
Matter 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.

13
Matter 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

14
Matter and Properties (Ch. 4)
  • Read pages 74 77
  • What happens in a change of phase?
  • Differentiate between a physical change and a
    chemical change.

15
Structure 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.

16
Structure of the Atom and the Periodic Table (Ch.
6)
17
Structure of the Atom and the Periodic Table (Ch.
6)
  • Finding protons, neutrons and electrons (p.
    109 and p. 131-132)
  • Proton
  • Electron
  • Neutron

18
Structure 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)

19
Structure 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)

20
Structure 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)?

21
Structure 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.

22
Structure 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

23
Structure 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.

24
New Approach to the Atom (Ch. 6 p. 122 - 131)
  • Electromagnetic Spectrum
  • Line spectra
  • Wave vs. Particle
  • Bohr Model
  • Quantum Mechanical Model

25
New Approach to the Atom (Ch. 6 p. 122 - 131)
  • Electromagnetic Spectrum
  • Entry Level Knowledge
  • Grade 8 Electromagnetic Radiation
  • How do we see different colors?

26
New 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

27
New Approach to the Atom (Ch. 6 p. 122 - 131)
  • Emission Spectrum
  • Absorption Spectrum

28
New 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

29
New Approach to the Atom (Ch. 6 p. 122 - 131)
30
New 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

31
New 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

32
New Approach to the Atom (Ch. 6 p. 122 - 131)
33
New Approach to the Atom (Ch. 6 p. 122 - 131)
34
Applications of Line Spectrum
  • Research one of the following
  • Aurora borealis
  • Fireworks
  • Neon Lights

35
Applications of Line Spectrum
36
Energy (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.

37
Energy (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.

38
Energy (Ch. 5)
  • In a change of state
  • When a substance melts, E is ____________.
  • When a substance condenses, E is
  • _________.
  • Animation

Added
Removed
39
Energy (Ch. 5)
  • Definitions
  • Energy
  • Work

The ability to do work
Done on an object, in response to a force, moves
some distance
40
Energy (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

41
Energy (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?

42
Energy 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
43
Energy 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)

44
Energy 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)

45
Energy 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.

46
Heat 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

47
Heat 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?

48
Heat 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.

49
Heat 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.

50
Heat 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
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