1. Matter States, Properties and Changes

2. Matter and States of Matter
What is Matter?
Matter
anything that occupies space and has mass
3 states of matter (technically 4)
Solid
Liquid
Gas
Plasma 2

3. Matter and States of Matter
Solid
a form of matter that has its own definite shape and volume
Liquid
flows, has its own volume, but takes shape of container
Gas
flows to conform to the shape of its container AND fills the entire volume of its container
Plasma
an ionized gas (a gas where ions and electrons coexist)
the sun, like most stars, is a great big ball of plasma. 3

4. 3 Classes of Matter
Mixtures
Compounds
Matter
Elements

5. Classification of Matter
Pure Substances
Mixtures
Elements
Compounds
Heterogeneous
Homogeneous
Elements:
The simplest forms of matter that can exist under normal laboratory conditions.
Elements are represented with a one or two letter chemical symbol.
Example: Na, S, K, Ag, etc.
Compounds:
Substances that can be separated into simpler substances only by chemical means.
Example: NaCl, H2O 5

6. Classification of Matter
Elements:
The simplest forms of matter that can exist under normal laboratory conditions.
Elements are represented with a one or two letter chemical symbol.
Example: Na, S, K, Ag, etc.
Compounds:
Substances that can be separated into simpler substances only by chemical means.
Example: NaCl, H2O 6

7. Mixtures Mixture: A physical blend of two or more substances.
Examples: dinner salad and salt water(solution)
A MIXTURE can be separated by physical methods whereas a COMPOUND can not
Heterogeneous mixture:
A mixture that is not uniform in composition.
Example: chef salad
Homogeneous mixture:
A mixture that is completely uniform composition.
Example: salt water 7

8. Heterogeneous Mixtures
A mixture with an uneven texture and the components of the mixture can be detected with the eyes.

9. Homogeneous Mixtures
A uniform mixture at the particulate level that consists of two or more substances in the same phase.
Homogeneous mixture are often referred to as solutions.
Solid phase homogeneous mixture are referred to as alloys. (e.g. brass, 14K gold, etc.)

10. Examples of Homogeneous Mixtures
Also:
Salt Water, Sugar Water and most clean air

11. SUSPENSION a heterogenous mixture that settles to the bottom of the container

12. Representation of Pure Substances and Mixtures
Mixture of elements
and compounds
Compound
Mixture
Element
Compound
Mixture of compounds 12

13. Separation of mixtures
Separation Techniques - Physical Methods
Magnetic removal: If there is iron,nickel, cobalt
Filtration: A solid which has not dissolved
in a liquid can be separated by filtration
Hand sorting particles:
Decanting: Pouring off the less dense liquid
Crystallisation: The solution is warmed in an open container,
allowing the solvent to evaporate, leaving a saturated solution
Distillation: A liquid can be separated from a mixture
of liquids in a solution by fractional distillation
Chromatography: a technique that separates the
components of a mixture (called the mobile phase)
on the basis of the tendency of each to travel or be
drawn across the surface of another material
(called the stationary phase) 13

14. Distillation

15. Decide if the substances is Element, Compound, or Mixture?
Water
Table Salt
Oxygen
Dirt
Air
Copper
Soda
Steel
Rain
Ice-cream
Compound
Element
Mixture 15

16. In which state of matter do the particles spread out in all directions, filling their container?
Solid
Liquid
Gas

17. What is any material made up of only ONE kind of matter called?
Compound
Element
Substance
State

18. What are the characteristics of a material that can only be seen when the material changes and a NEW material is formed?
A. Metric properties
B. Physical properties
C. Chemical properties
D. International properties

19. A mixture in which particles of different substances are mixed evenly throughout:
Compound
Solution
State
Formula

20. Liquid water freezing to become ice is a:
Physical Change
Chemical Change

21. When iron rusts, this is a:
Physical Change
Chemical Change

22. Odor, shape, color and temperature are:
Chemical properties
Physical properties
Compounds
Elements

23. Properties of Matter HCl is soluble in water
Distinguish between physical and chemical properties
Physical Property – a characteristic that can be observed or measured without changing the sample’s composition (e.g. color, density, buoyancy, viscosity, and freezing point) Chemical Property – the ability of a substance to combine with or change into one or more other substances
HCl is soluble in water
physical property
HCl is corrosive to metals
chemical property
HCl burns skin 24

24. Extensive and Intensive Properties
Physical properties of matter are categorized as
Intensive or Extensive:
Intensive - Properties that do not depend on the amount of the
matter present.
Color
Odor
Conductivity
Hardness
Melting/Freezing Point
Boiling Point
Density
Extensive - Properties that do depend on the amount of matter
present.
Mass
Weight
Volume
Length

25. Physical Properties of Matter
Density
shows how tightly the matter within the object is packed together.
equal to 1 g/mL

26. Anything with a density of GREATER than 1g/mL will sink in water
Anything with a density LESS than 1g/mL will float in water.

27. Physical Properties of Matter
Buoyancy
The ability of a liquid or gas to push up on an object placed in it
For example, you in a swimming pool
Ships are built to be less dense than water. The curved shape of a ship displaces the water around it, or moves it out of the way.

28. If the buoyant force is greater than the weight, then object FLOATS!
If not…it sinks.

29. Archimedes’ Principle
States that the buoyant force on an object is equal to the weight of the fluid displaced.
If the buoyant force is greater or equal to the boats weight, the boat floats.
If the buoyant force is not greater than the boat, it sinks!

30. Physical Properties of Matter
Viscosity
A measure of a material’s resistance to flow
Which substance here has a higher viscosity?
How can it be measured?
Viscosity is a property of fluids, along with density and buoyancy. Viscosity is the measure of a material’s resistance to flow. In this example, catsup has a higher viscosity, since it resists flow much more than water. This is something that many people have actually experienced. It may be fun to ask people to try and give examples of materials that they see everyday that have high viscosity. Some may include molasses, honey, certain kinds of glue, nacho cheese dip, some kinds of paint, and many other materials. If we could measure how fast the liquid actually moves, we could get a better idea of a material’s viscosity. However, this could get messy and the equipment we need to use like the photogates and the timer don’t get along too well with liquids. What we need to do is keep the liquids contained and keep our work area and equipment free from sticky substances. Luckily, there is an easy, safe and fun solution to this problem. The Viscometer.

32. Define physical change and list several common physical changes.
a change which alters a substance without changing its composition
Examples:
Cutting
Bending
Melting
Freezing
Condensing
Vaporizing
Boiling

33. Chemical Changes Chemical change Evidence of chemical change:
involves a change in a substance’s composition
Evidence of chemical change:
- gas bubbles evolved
- precipitate (ppt) or solid formed
- heat released/absorbed
- light released
- change in color
Exothermic Reaction: Release heat, feel warm to the touch
Endothermic Reaction: Absorb heat, feel cool.

34. Law of Conservation of Mass
Chemical Reaction:
1 or more substances are changed into new substances
Products: Substances formed
Reactants: Starting substances
Apply the law of conservation of mass to chemical reactions.
Mass is neither created nor destroyed during a chemical reaction
Mass is conserved!
Massreactants = Massproducts