1. Solid, Liquid and Gas Classification of Matter Separation Techniques
Chapter 3
Solid, Liquid and Gas
Classification of Matter
Separation Techniques

2. Solid, Liquid, Gas
(a) Particles in solid (b) Particles in liquid (c) Particles in gas

3. Solid
H2O(s) Ice
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 31

4. Liquid In a liquid H2O(l) Water molecules are in constant motion
there are appreciable
intermolecular forces
molecules are close
together
Liquids are almost
incompressible
Liquids do not fill the
container
some writing from Kotz (PowerPoints online)
H2O(l) Water
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 31

5. Gas
H2O(g) Steam
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 31

6. Gas, Liquid, and Solid Gas Liquid Solid
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 441

7. Some Properties of Solids, Liquids, and Gases
Property Solid Liquid Gas
Shape Has definite shape Takes the shape of Takes the shape
the container of its container
Volume Has a definite volume Has a definite volume Fills the volume of
the container
Arrangement of Fixed, very close Random, close Random, far apart
Particles (compressible)
Interactions between Very strong Strong Essentially none
particles

8. MATTER yes no MIXTURE PURE SUBSTANCE yes no yes no Homogeneous Mixture
Can it be physically separated?
MIXTURE
PURE SUBSTANCE
yes
Is the composition uniform? no
yes
Can it be chemically decomposed? no
Homogeneous Mixture
(solution)
Heterogeneous Mixture
Compound
Element
Courtesy Christy Johannesson

9. Pure Substances Element composed of identical atoms
EX: copper wire, aluminum foil
Courtesy Christy Johannesson

10. Pure Substances Compound
composed of 2 or more elements in a fixed ratio
properties differ from those of individual elements
EX: table salt (NaCl)
Courtesy Christy Johannesson

11. Mixtures Variable combination of 2 or more pure substances.
Heterogeneous
Homogeneous
Courtesy Christy Johannesson

12. Pure Substances Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different ratios to form different compounds.
Courtesy Christy Johannesson

13. Two different compounds, each has a definite composition.
Pure Substances
For example…
Carbon, C Oxygen, O Carbon monoxide, CO
Carbon, C Oxygen, O Oxygen, O Carbon dioxide, CO2
Two different compounds, each has a definite composition.
Courtesy Christy Johannesson

14. Mixtures Solution homogeneous very small particles
Tyndall Effect
Solution
homogeneous
very small particles
particles don’t settle
EX: rubbing alcohol
Courtesy Christy Johannesson

15. Air is a Solution Air Nitrogen Helium Oxygen Neon Water vapor Carbon
dioxide
Argon
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 34

16. An alloy is a mixture of metals.
Brass = Copper + Zinc
Solid brass
homogeneous mixture
Solid Brass
Consumer Tip
Pay attention to labels when purchasing brass. Brass is sold with the label ‘Brass’ or ‘Solid Brass’.
‘Brass’ means brass coated – the object is not ‘solid brass’. It is likely inexpensive, cheap zinc in the center and has only a thin coating of brass on the outside.
Toilet bowl seat screws are often sold as ‘brass’ ($1.29) or ‘solid brass’ ($1.99).
Pay more, the ‘brass’ screw may snap off as zinc is a brittle metal under stress.
‘Solid brass’ is stronger and the better value.
Copper
Zinc

17. Classification of Matter
(gas. Liquid,
solid, plasma)
Separated by
PURE
SUBSTANCES
MIXTURES
physical means into
Separated by
COMPOUNDS
ELEMENTS
HOMOGENEOUS
MIXTURES
HETEROGENEOUS
MIXTURE
chemical
means into
Kotz & Treichel, Chemistry & Chemical Reactivity, 3rd Edition , 1996, page 31

18. Elements, Compounds, and Mixtures
oxygen atoms
hydrogen
atoms
hydrogen
atoms
“Elements, Compounds, and Mixtures”
Description: This slide shows the molecular composition of an element, a compound, and two mixtures.
Basic Concepts
All samples of a substance have the same molecular composition and intensive properties and are homogeneous.
Elements and compounds are substances; mixtures are not.
The elements making up a compound combine in fixed ratios.
Mixtures can be separated by physical methods.
Mixtures that have a uniform composition throughout are homogeneous; those that have parts with different compositions are heterogeneous.
Teaching Suggestions
Use this transparency to help students visualize the molecular composition of elements, compounds, and mixtures and to review the definitions of these terms. Make sure students understand the difference between the terms matter and substance. Remind students that elements and compounds are always homogeneous, while mixtures can be either homogeneous or heterogeneous.
Questions:
Which of the bottles pictured above contain(s) matter? Which contain(s) a single substance? Explain your answers.
How many elements are present in each molecule of water shown in bottle (b)? What is the relative number of atoms of each element in a water molecule?
As you know, ice is frozen water. In other words, ice and water are the same substance, in different phases. What would you expect the ratio of hydrogen atoms to oxygen atoms to be in a molecule of ice? Explain your reasoning.
Bottle (c) and bottle (d) both contain mixtures. How are these mixtures similar? How are they different?
Suppose you find an unlabeled bottle containing a clear liquid. Can you tell by looking at it whether the material is a compound or a mixture? Explain your answer.
How can you prove that a sample of sea water is a mixture?
Classify the following items as elements, compounds or mixtures; rice pudding, copper, carbon dioxide, air, milk, magnesium chloride, granite, mercury, and maple syrup.
A chocolate-chip cookie with more chips in one part of the cookie than another can be used to demonstrate a heterogeneous mixture. Name two other materials that can be classified as heterogeneous mixtures. Explain your reasoning.
(a)
an element
(hydrogen)
(b)
a compound
(water)
(c)
a mixture
(hydrogen
and oxygen)
(d)
a mixture
(hydrogen
and oxygen)
Dorin, Demmin, Gabel, Chemistry The Study of Matter , 3rd Edition, 1990, page 68

19. Classify the following as element, compound, solution, or heterogeneous mixture
Copper
H2O
Salt in water
Air
Sand in water
Sulfur

20. Separation of Mixtures
Filtration
Distillation
Crystallization
Chromatography

21. Filtration
Filter paper placed in a funnel is used to separate a solid from a liquid. The solid will stay on the filter paper and the liquid flows through the paper to a collection beaker below.

22. The solution is boiled and steam is driven off.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 39

23. Separation of a sand-saltwater mixture.
Zumdahl, Zumdahl, DeCoste, World of Chemistry 2002, page 40

24. Crystallization
Formation of a pure solid from a solution. An example of this is rock candy.

25. Paper Chromatography
Separates the parts of a mixture as it travels across the surface of another material.

26. Conservation of Mass
Mass cannot be created or destroyed.

28. Mass of Reactants=Mass of Products
(reactants) (products)
Magnesium + Oxygen  Magnesium Oxide
10.0 g ??  g
How much oxygen reacts with the magnesium to form the magnesium oxide?

29. Pure Substances Law of Definite Composition
A given compound always contains the same, fixed ratio of elements.
Law of Multiple Proportions
Elements can combine in different ratios to form different compounds.
Courtesy Christy Johannesson

30. Two different compounds, each has a definite composition.
Pure Substances
For example…
Carbon, C Oxygen, O Carbon monoxide, CO
Carbon, C Oxygen, O Oxygen, O Carbon dioxide, CO2
Two different compounds, each has a definite composition.
Courtesy Christy Johannesson

31. Sucrose The formula is C6H12O6
Every sample of sucrose contains 42.1% carbon, 6.48% hydrogen and 51.4% oxygen.