1. Chapter 1 Basic Concepts of Chemistry

2. States of Matter
The three common states of Matter:
Solid
Liquid
Gas

3. Solid State – matter in the solid state has definite volume and shape.
The particles that make up the solid are packed close together in relatively fixed positions.
The particles are held close together by strong attractive forces.

4. Liquid State – matter in the liquid state has definite volume but an indefinite shape.
A liquid assumes the shape of its container. The particles that make up the liquid are packed close together but can move past one another.
The rapidly moving particles cause them to temporarily overcome the attractive forces between them, allowing the liquid to flow.

5. Gas State – matter in the gas state has no definite volume nor shape.
Gases have this characteristic because they are composed of particles that move very rapidly and are at great distances from one another.
A gas will expand to fill any size container and take the shape of that container.

6. Condense
Freeze
Melt
Evaporate
Solid
Liquid
Gas

7. Types of Matter
All matter can be classified into one of two groups: pure substances or mixtures.
Pure Substance – can be an element or compound. The composition of a pure substance is the same throughout and does not vary from sample to sample.
Examples include: water, sugar, gold and aluminum.

8. Mixture – contains more than one substance.
They can vary in composition and properties from sample to sample.
Examples include: sugar dissolved into water, granite, brass (copper and zinc), chocolate chip cookie and air.

9. Mixtures
Homogeneous- same composition throughout. Homogenous mixtures are also called solutions.
Example: salt water solution and air
Heterogeneous- mixture is not the same throughout the sample.
Example: sand and water. The heavier sand settles to the bottom.

10. Solutions Homogeneous mixture Can occur between any state of matter.
Solid in liquid- Kool-aid
Liquid in liquid- antifreeze in a car radiator
Gas in gas- air (oxygen, nitrogen and argon)
Solid in solid – brass (copper and zinc)

11. Separating Mixtures

12. Summary

13. Building Blocks of Matter
The fundamental building blocks of matter are atoms.
Element – a pure substance made of only one kind of atom.
Atoms – the smallest unit of an element that maintains the properties of the element.

14. Elements The elements are recorded on the PERIODIC TABLE
There are 117 recorded elements at this time.
The Periodic table will be discussed further in chapter 2.

15. Compound – a substance that is made from the atoms of two or more elements that are chemically bonded.
Compound Examples – water (made of hydrogen and oxygen), methane (made of carbon and hydrogen) and sugar (made from carbon, hydrogen and oxygen).
H2O, CH4 and CxHxOx

16. Chemical compounds are composed of two or more atoms.

17. Chemical Compounds Molecule: Ionic Compound Ammonia (NH3)
Iron pyrite (FeS2)

18. Chemical Compounds All Compounds are made up of molecules or ions.
A molecule is a compound consisting of two nonmetals and held together by covalent bonds.
Ionic compounds are between a metal and nonmetal
Optional slide

19. Molecular Formula H2O C8H10N4O2 - caffeine
See Chapter 1 Video Presentation Slide 4

20. Physical Properties Some physical properties: Color
State (s, g or liq)
Melting and Boiling point
Density (mass/unit volume)
Extensive properties (mass) depend upon the amount of substance.
Intensive properties (density) do not.

21. Physical Properties Mixtures may be separated by physical properties:
Physical Property
Means of Separation
Density
Decantation, centrifugation
Boiling point
Distillation
State of Matter
Filtration
Intermolecular Forces
Chromatography
Vapor pressure
Evaporation
Magnetism
Magnets
Solubility

22. Chemical Properties Chemical properties are really chemical changes.
See Chapter 1 Video Presentation Slide 5
Chemical properties are really chemical changes.
The chemical properties of elements and compounds are related to periodic trends and molecular structure.

23. Chemical Properties
A chemical property indicates whether and sometimes how readily a material undergoes a chemical change with another material.
For example, a chemical property of hydrogen gas is that it reacts vigorously with oxygen gas.
Optional Slide

24. Qualitative Observations
No numbers involved
Color, appearance, statements like “large” or “small:
Stating that something is hot or cold without specifying a temperature.
Identifying something by smell
No measurements

25. Qualitative Observations
A quantity or attribute that is measureable is specified.
Numbers with units are expressed from measurements.
Dimensions are given such as mass, time, distance, volume, density, temperature, color specified as a wavelength etc...

26. Energy: Some Basic Principles
Energy can be classified as Kinetic or Potential.
Kinetic energy is energy associated with motion such as:
• The motion at the particulate level (thermal energy).
• The motion of macroscopic objects like a thrown baseball, falling water.
The movement of electrons in a conductor (electrical energy).
Wave motion, transverse (water) and compression (acoustic).
Matter consists of atoms and molecules in motion.
See Chapter 1 Video Presentation Slide 9

27. Energy: Some Basic Principles
Potential energy results from an object’s position:
Gravitational: An object held at a height, waterfalls.
Energy stored in an extended spring.
Energy stored in molecules (chemical energy, food)
The energy associated with charged or partially charged particles (electrostatic energy)
Nuclear energy (fission, fusion).