1. Matter and Change
Chapter 1

2. Theoretical Chemistry
Branches of Chemistry
Organic Chemistry
Inorganic Chemistry
Physical Chemistry
Analytical Chemistry
Biochemistry
Theoretical Chemistry
….and many more!

3. anything that has mass and takes up space
Matter
anything that has mass and takes up space
pure substances – compounds and elements
mixtures – two or more pure substances mixed in the same container…not bonded

4. Pure Substances
Element – A pure substance made of only one kind of atom Atom – An atom is the smallest unit of an element that maintains the properties of that element

5. Pure Substances
Compound – A substance that is made from the atoms of two or more elements that are chemically bonded.
Molecule – the smallest unit of an element or compound that retains all of the properties of that element or compound

6. How can a molecule describe an element?
Huh?
How can a molecule describe an element?

7. H2, Br2,O2, F2, I2, N2, Cl2, Diatomic Elements Uncle Henry BrOFINCl
These elements are found as a pair, chemically bonded to one another. They are not always in pairs in a compound but are in pairs when they are found as the pure element. Ex: H2O (only 1 oxygen)

8. Compounds and Elements

9. space filling model
molecular model
chemical formula
structural formula

10. SHAPE
definite shape
indefinite shape
VOLUME
definite volume
indefinite volume
Solid
Liquid
Gas

11. States of Matter
The particles of a solid are packed together in relatively fixed positions.
The particles have strong attractive forces and low energy.
(s)

12. States of Matter
The particles of a liquid are close together but can most past one another.
These particles have more energy than those of a solid, and this energy is what allows a liquid to flow.
Pure liquid = (l)
A liquid solution = (aq)

13. States of Matter
The particles of a gas move rapidly past one another, and are at a great distance apart from one another compared to their size.
These particles have very high energy.
(g)

14. States of Matter - Plasma
A plasma is a very high temperature physical state of matter in which atoms lose their electrons.
Plasma is found in fluorescent light bulbs and plasma Televisions.

15. Solid, Liquid, or Gas?

19. What two phase changes are occurring at the same time?

20. Physical Properties
physical property – a characteristic that can be observed or measured without changing the identity of the substance
state of matter
melting point
mass
color

21. Physical Changes
physical change – a change in a substance that does not involve a change in the identity of the substance
breaking
cutting
dissolving
boiling
tearing

22. All phase changes are physical changes.

23. Chemical Properties
chemical property – a characteristic that can be observed or measured with a change in the identity of the substance
flammability
reacts with an acid
reacts with oxygen

24. Chemical Changes
chemical change – a change in a substance that does involve a change in the identity of the substance
color change
gas released (often with an odor)
energy change (light, heat, …)
precipitate formed
…four good indications of a chemical change.

25. Precipitate aqueous – dissolved in water
precipitate – a solid formed from two aqueous solutions during a chemical reaction

26. Extensive vs. Intensive Properties
extensive – DOES depend on the amount of matter present
Example: mass, volume, amount of energy within a substance
intensive – does NOT depend on the amount of matter present
Examples: color, melting point, density, luster
If mass and volume are extensive properties, why is density an intensive property?

27. Classification of Matter

28. Decomposition of Water
water ® hydrogen + oxygen
2H2O(l) ® 2H2(g) + O2(g) +
reactants
yield
products

29. Hoffman Apparatus
The Hoffman Apparatus is used to decompose water into its pure elements. This is a chemical change. The new substances (hydrogen gas and oxygen gas) did not retain the properties of the original substance (water).

30. Heterogeneous Mixtures
Homogeneous Mixtures
the same throughout…each sample contains the same ratio of ingredients
(Also called solutions)
Heterogeneous Mixtures
different throughout…each sample contains a different ratio of ingredients

31. Separation of Mixtures
density
PHYSICAL changes only
magnetism
by hand
evaporation
filtration
chromatography

32. Separation of elemental Fe
magnetism
This doesn’t work with iron that is bound into a compound, only with elemental Fe.

33. Distillation Apparatus

34. Mixture or Pure Substance?

35. Homogeneous Mixture, Heterogeneous Mixture or Pure Substance?