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Matter And Energy

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Compounds can be formed in more than one way between two or more elements. Elements can combine in different proportions with whole number ratios when this happens. ... – PowerPoint PPT presentation

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Title: Matter And Energy


1
Matter And Energy
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Chemistry I Chapter 2a Chemistry I Honors
Chapter 2 ICP Chapter 15 16a
2
The Nature of Matter
Gold
Mercury
  • Chemists are interested in the nature of matter
    and how this is related to its atoms and
    molecules.

3
Chemistry Matter
  • We can explore the MACROSCOPIC world what we
    can see
  • to understand the PARTICULATE worlds we cannot
    see.
  • We write SYMBOLS to describe these worlds.

4
A Chemists View of Water
Macroscopic
H2O (gas, liquid, solid)
Symbolic
Particulate
5
A Chemists View
Macroscopic
2 H2(g) O2 (g) --gt 2 H2O(g)
Particulate
Symbolic
6
Kinetic Nature of Matter
  • Matter consists of atoms and molecules in _____.

7
STATES OF MATTER
  • _______ have rigid shape, fixed volume.
    External shape can reflect the atomic and
    molecular arrangement.
  • Reasonably well understood.
  • _______ have no fixed shape and may not fill a
    container completely.
  • Not well understood.
  • _______ expand to fill their container.
  • Good theoretical understanding.

8
OTHER STATES OF MATTER
  • PLASMA an electrically charged gas Example
    the sun or any other star
  • BOSE-EINSTEIN CONDENSATE a condensate that
    forms near absolute zero that has superconductive
    properties Example supercooled Rb gas

9
Physical Properties
  • What are some physical properties?
  • color
  • melting and boiling point
  • Odor
  • Anything you can touch, see, hear, taste

10
Extensive vs. intensive property
  • Extensive properties are dependent upon the
    amount of substance present. Ex- mass, length
  • Intensive property is independent of the amount
    of substance present. Ex- density, temperature

11
  • Graphite layer structure of carbon atoms
    reflects physical properties.

12
Physical Changes
  • can be observed without changing the identity of
    the substance
  • Some physical changes would be
  • boiling of a liquid
  • melting of a solid
  • dissolving a solid in a liquid to give a
    homogeneous mixture a SOLUTION.

13
Chemical Properties and Chemical Change
  • Chemical properties cannot be seen- reactivity,
    flammability, corrosiveness.
  • Burning hydrogen (H2) in oxygen (O2) gives H2O.

14
Chemical Properties and Chemical Change
  • Burning hydrogen (H2) in oxygen (O2) gives H2O.
  • Chemical change or chemical reaction
    transformation of one or more atoms or molecules
    into one or more different molecules.

15
Sure Signs of a Chemical Change
  • Heat
  • Light
  • Gas Produced (not from boiling!)
  • Precipitate a solid formed by mixing two
    liquids together
  • Law of conservation of mass- Matter is neither
    created nor destroyed during a chemical reaction.
  • Practice problems p78- Q5-9. P79 q13.

16
Physical vs. Chemical
  • physical
  • chemical
  • physical
  • physical
  • chemical
  • Examples
  • melting point
  • flammable
  • density
  • magnetic
  • tarnishes in air

17
Physical vs. Chemical
  • Examples
  • rusting iron
  • dissolving in water
  • burning a log
  • melting ice
  • grinding spices

18
Matter Flowchart
MATTER
yes
no
Can it be physically separated?
Homogeneous Mixture (solution)
Heterogeneous Mixture
Compound
Element
19
Types of Mixtures
  • Variable combination of 2 or more pure substances.

Heterogeneous visibly separate phases
Homogeneous Same throughout
20
Methods of separation
  • Filtration- use filter paper to separate based on
    particle size
  • Distillation- boil off liquids at different
    temperatures
  • Crystallization- separate based on formation of
    crystals
  • Sublimation- solids going directly to
    gases.opposite- deposition.
  • Chromatography- liquids rise up in a column based
    on affinity
  • Do Chromatography lab

21
Elements and compounds
  • Elements- simplest form of matter
  • Compounds formed by combining elements in a fixed
    ratio.
  • Periodic table- organizes elements into groups
    (families) and periods.
  • Groups are vertical and periods are horizontal
  • Law of definite proportions- Any compound is
    always composed of same elements in same
    proportion.
  • Ex- CuF2 1 Cu 2F
  • Percent by massmass of element/ mass of compound
    x100.
  • P88 Practice problems- q19-22

22
Law of multiple proportions
  • Compounds can be formed in more than one way
    between two or more elements.
  • Elements can combine in different proportions
    with whole number ratios when this happens.
  • Ex- H2O and H2O2
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