1. Matter, Energy & Change W/ Concept Mapping
Chapter 1
Matter, Energy & Change
W/ Concept Mapping

2. Chapter Objectives
TSW be able to apply the skill of concept mapping as a means of organizing the classification of matter system.
TSW have a solid understanding of how our universe is composed of different arrangements & combinations of the known 113 elements.
TSW be able to differentiate between physical and chemical properties and physical and chemical changes
TSW be able to distinguish between intensive and extensive properties
TSW be able to identify changes as endothermic or exothermic and display an understanding that energy is involved in all changes of matter.

3. Matter is…
By definition matter is anything that has mass and volume (or takes up space)
Since everything has mass and takes up space…everything we see and touch is composed of matter.
The “Building Blocks” of matter are atoms.

4. Mass vs. Weight
We use these terms interchangeably, however, they do have different meanings when used correctly.
Mass is defined as a measure of the amount of matter in a sample.
Weight is defined as a measure of the pull of gravity on a sample of matter.
Mass would remain constant anywhere in the universe, however, the weight would change.

5. Atoms
An atom is the smallest portion of an element that retains the unique properties of that element.
We will learn more about atoms in the next chapter.

6. Pure Substances
Are any materials with a fixed composition having definite set of physical and chemical properties
There two types of pure substances
Elements – unique arrangements of electrons, protons and neutrons that specific properties.
Compounds – two or more element chemically connected with definite composition and arrangements.

7. Examples Elements: Compounds: Na – sodium O2 – oxygen
MgCl2 – Magnesium Chloride
H2O – Water
H2O2 – Hydrogen Peroxide

8. Mixtures
Are materials with two or more pure substances mixed together but not chemically connected to one another.
There are two types of mixtures
Homogeneous – one phase with uniform distribution of particles
Heterogeneous – clusters of atoms with two or more phases and a non-uniform distribution of particles.

9. Properties of Matter
Every pure substance has a definite set of physical and chemical properties that exist even in the smallest sized sample.
We can use these properties to identify a pure substance.

10. Chemical Property
A Chemical Property is one that can only be observed during the course of a chemical change.
There are four tell tale signs that a chemical change is occurring…
A release of a gas
A change of color
A release or absorption of heat and/or light
Formation of a precipitate

11. A Precipitate?
A precipitate is a solid that is produced from two liquid reactants.
Example: Pb(NO3)2 + KI  Yellow Precipitate

12. Examples of Chemical Properties
Flammability
Reactivity
Stability

13. Chemical Changes
A Change that results in a new substance that has a different arrangement of atoms with a set of chemical and physical properties different from the substance we started with.

14. Physical Properties
A physical property is one which can be observed in the absence of a chemical change.
Mass
Density
MP/BP
Conductivity
Color
Malleability
Physical State
Every element, compound or molecule has a unique combination of these properties that allow us to use them in separating them from a mixture.

15. Intensive & Extensive
Some properties depend on the amount of the substance present and others do not…
An Intensive property is one that does not depend on the amount of substance present.
An Extensive property is one that is dependant on the amount of the substance present.

16. Density…
Density is one of the most useful intensive physical properties.
We can observe that each substance has its own unique value…thus we can determine the density of any unknown and use it to determine the substances identity.
The formula for density is
D = mass / volume

17. Physical States of Matter
Solid – Sample of matter that has a definite volume and shape.
Liquid – Sample of matter that has a definite volume, but it adopts the shape of any container.
Gas – Sample of matter that has neither a definite shape nor definite volume.
Plasma – Sample of matter at high temperature where individual atoms lose their electrons.

18. Physical Changes
These are changes in the appearance of a substance, not in the identity of a sample of matter.
One example of this would be a change in the physical state that a sample of matter exists in.
Example: Ice (solid water) melting into liquid water.

19. Changes in State
You will see throughout the course that energy is involved in all changes, both chemical and physical changes
That means that changes in state are also displays of changes in energy.

20. More About Change
When a change occurs and energy is lost it is called exothermic…think of it this way:
Exo  Exiting the system
When a change occurs and energy is absorbed it is called endothermic…think of it this way:
Endo  Entering the system

22. Law of Conservation of Matter
States:
The amount of matter in the universe is constant
Matter cannot be created or destroyed only change form.