1. Matter and Change

2. Chemistry is…
…the study of the composition, structure, and properties of matter and the changes it undergoes

3. Anything that has mass and occupies space
Matter
Anything that has mass and
occupies space
Mass
A measure of the amount of matter
Weight
The measure of the force of gravity
acting on an object

4. Atom
The smallest unit of an element that maintains
the properties of that element

5. By asking questions scientists can classify matter into:
Mixtures – two or more substances that are not chemically combined with each other
and can be separated by physical means. The substances in a mixture retain their individual properties.
Solutions – a special kind of mixture where one substance dissolves in another.
Elements – simplest form of pure substance. They cannot be broken into anything else by physical or chemical means.
Compounds – pure substances that are the unions of two or more elements. They can be broken into simpler substances by chemical means.

6. Types of Chemical Formulas • An empirical formula gives the relative number of atoms of each element in a compound; i.e., the smallest whole number ratio that is possible. • A molecular formula gives the actual number of atoms of each element in a molecule of a compound Molecular Empirical Hydrogen peroxide H2O HO Water H2O H2O Glucose C6H12O CH2O • A structural formula uses lines to represent covalent bonds, and shows how the atoms in a molecule are joined together: H—O—O—H H—O—H O=C=O

7. Homogeneous – a substance that is the same throughout
Homogeneous – a substance that is the same throughout. Heterogeneous – a substance that is different throughout.

8. Separation of a Compound The Electrolysis of water
Compounds must be separated by chemical means.
With the application of electricity, water can be
separated into
its elements
Reactant  Products
Water  Hydrogen + Oxygen
H2O  H O2

10. Separation of a Mixture
Distillation

11. Properties of Matter
depend on the amount of matter that is present.
Extensive properties
Volume
Mass
Intensive properties
do not depend on the amount of matter present.
Melting point
Boiling point
Density

12. Physical Change
A change in a substance that does not involve a change in the identity of the substance.
Example:
A change in
size, shape
color etc.
Phase Changes

13. Phase Differences
Solid – definite volume and shape; particles packed in fixed positions.
Liquid – definite volume but indefinite shape; particles close together but not in fixed positions

14. Gas – neither definite volume nor definite shape; particles are at great distances from one another Plasma – high temperature, ionized phase of matter as found on the sun.

15. Phase changes occur when a substance changes state from…
A solid to liquid…melting
A liquid to solid…freezing
A liquid to gas…boiling
A gas to liquid…condensing
A solid to gas…subliming
A gas to a solid…deposition

17. The heat that is being added to a given state that does not result in a temperature increase is being used to overcome the intermolecular forces between the particles.
The heat added to a solid to convert it to a liquid is called the heat of fusion. (fusion means melting)
You add heat to get a solid to melt. When you condense a liquid back to a solid, you get that heat back!
Melting and freezing are only different in which way heat flows in or out of a substance.

18. The same occurs at the boiling/condensation point
The same occurs at the boiling/condensation point. The heat put in to a liquid to convert it to a gas is called the heat of vaporization.
When a gas is condensed to a liquid, then that heat is again released.
Boiling and condensation are only different in the direction of heat flow in or out of a substance.

19. Copper Phases - Solid

20. Copper Phases - Liquid

21. Copper Phases – Vapor (gas)

22. Chemical Change
A change in which one or more substances are converted into different substances. Something new is created.
Heat and light are often evidence of a chemical change.

23. Catalyst – a substance that increases the rate of a chemical reaction without itself being permanently changed. Entropy – the measure of disorder in a substance.

24. Physical properties shape. size texture. hardness odor. mass color
Physical properties shape size texture hardness odor mass color state freezing point magnetism melting point

25. More physical properties
More physical properties
conductivity (conducts electricity) malleability (can be hammered into sheets) ductility (can be drawn into wires) solubility (will dissolve in another substance) density (mass / volume)

26. Chemical properties
Flammibilty
Reactivity
Combustibility
Acidic or basic

27. Properties of Metals
Metals are good conductors of heat and electricity
Metals are malleable
Metals are ductile
Metals have high tensile strength
Metals have luster

28. Examples of Metals
Potassium, K reacts with water and must be stored in kerosene
Mercury, Hg, is the only metal that exists as a liquid at room temperature

29. Properties of Nonmetals
Carbon, the graphite in “pencil lead” is a great example of a nonmetallic element.
Nonmetals are poor conductors of heat and
electricity
Nonmetals tend to be brittle
Many nonmetals are gases at room temperature

30. Examples of Nonmetals
Sulfur, S, was once known as “brimstone”
Graphite is not the only pure form of carbon, C. Diamond is also carbon; the color comes from impurities caught within the crystal structure

31. Properties of Metalloids
Metalloids straddle the stairstep.
They have properties of both metals and nonmetals.
Metalloids are more brittle than metals, less brittle than most nonmetallic solids
Metalloids are semiconductors of electricity
Some metalloids possess metallic luster

32. Silicon, Si – A Metalloid
Silicon has metallic luster
Silicon is brittle like a nonmetal
Silicon is a semiconductor of electricity

33. Number of naturally occuring elements is 90
Sir ramsey discovered the Noble gases, octets, group 8, helium family
Accuracy – nearness of a measurement to its accepted value
Precision – agreement between numerical values of a set of measurements.