1. Anything that has mass and volume
Matter:
Anything that has mass and volume
Mass – the amount of material in an object (the amount of inertia an object contains.)
Volume – the amount of space an object occupies.

3. Matter Classifications …
Pure Substance – type of matter with fixed composition that does NOT vary from sample to sample
Element – substance that cannot be broken down
Compound – substance made up of atoms of two or more elements, with the different kinds of atoms combined in fixed proportions

4. Each element is assigned a unique chemical symbol
Elements are substances that cannot be decomposed by chemical means into simpler substances
Each element is assigned a unique chemical symbol
Most are one or two letters
First letter is always capitalized
All remaining letters are lowercase
Names and chemical symbols of the elements are listed on the inside front cover of the book

5. Compounds are substances formed from two or more different elements combined in a fixed proportion by mass
The physical and chemical properties of a compound are, in general, different than the physical and chemical properties of the elements of which it is comprised.
Elements and compounds are examples of pure substances whose composition is the same, regardless of source

7. A mixture consists of varying amounts of two or more elements or compounds
Heterogeneous mixtures consist
of two or more phases
Homogeneous mixtures or solutions have the same properties throughout the sample

8. At the molecular level:

9. Solutions
A solution is a homogeneous mixture in which the two or more components mix freely
The solvent is taken as the component present in the largest amount
A solute is any substance dissolved in the solvent

10. Solute = the discontiguous phase of a solution Solvent = the contiguous phase of a solutions

11. Solutions have variable composition.
The solute-to-solvent ratio is called the concentration.
Formation of a solution of iodine molecules in ethyl alcohol. Ethyl alcohol is the solvent and iodine the solute.
Solutions are transparent homogeneous mixtures

12. Concentration is an intensive, physical property.
There is usually a limit to the amount of solute that can dissolve in a given amount of solvent
For example, 36.0 g NaCl is able to dissolve in 100 g of water at 20°C
A solution is said to be saturated when no more solute can be dissolved at the current temperature
Concentration is an intensive, physical property.

14. Special Types of Heterogeneous Mixtures
Colloids – small particles that remain dispersed in the mixture (medium).
Examples – milk, smoke, paints, aerosols, emulsions
Suspensions – larger particles that can be acted upon by gravity. Maintain uniformity through shaking.
Examples – “bubble gum” medicine, salad dressings

15. Pure Substances and Mixtures

16. Separation techniques for Homogeneous Mixtures
Crystallization – the solvent is allowed to partially evaporate and the solute forms crystals.
Chromatography – separation of the solution components by differences in their attraction (adsorption) on a medium.
Distillation – takes advantage of differences in boiling points of two liquids.
- if solute is a solid, the liquid boils away and is collected while the solids are left behind.
Filtration separates heterogeneous mixtures
of liquids and solids.

17. This is important because…
Characteristics or properties of materials distinguish one type of substance from another.
This is important because…
Matter is often classified by properties
Properties may also be used to separate one substance from another.

18. Properties of Matter
Physical property: characteristic displayed by a sample of matter without undergoing any change in its composition (nothing new is produced.)
ex. Color, physical state
EOS
Physical properties can be observed without changing the chemical makeup of the substance

19. ex. Reactivity, flammability
Properties of Matter
Chemical property: characteristics displayed as a result of change in composition
ex. Reactivity, flammability
Chemical properties
involve a chemical change and result in different substances.
Indicate something could happen (not that it did…)
EOS

20. EOS

21. Properties can also be described as intensive or extensive
Intensive properties are independent of sample size
Examples: sample color and melting point
Extensive properties depend on sample size
Examples: sample volume and mass
In general, intensive properties are more useful in identifying a substance

22. Temperature is an intensive, physical property.

23. The three common physical states of matter have different properties:
Solids have a fixed shape and volume
Particles are close together and have restricted motion
Liquids have indefinite shape but fixed volume
Particles are close together but are able to flow
Gases have indefinite shape and volume
Particles are separated by lots of empty space

24. Physical state is an intensive, physical property.

25. Density is an intensive physical property.

27. Energy – Not a property of matter but related to changes in matter.
Literally means “work within,” however no object contains work
Work (w) is motion against an opposing force that is, to move or displace matter

28. – Kinetic (moving objects doing work)
EOS
3 basic types of energy:
– Potential (possibility of doing work because of composition or position)
– Kinetic (moving objects doing work)
– Radiant (energy transferred by electromagnetic waves)

29. KE can be converted into PE and vice versa
When the child is at points (a) and (c) they have only PE; at point (b) only KE. Total energy is conserved (PE + KE = constant).
When fully compressed or extended only PE; at natural length only KE. Total energy is conserved.

30. Heat (q)
Heat is energy transfer resulting from thermal differences between the system and surroundings
“flows” spontaneously from higher T  lower T
EOS
“flow” ceases at thermal equilibrium

31. The energy that is transferred as heat comes from the object’s internal energy
The energy associated with the motion of the object’s molecules is referred to as its molecular kinetic energy
The temperature of an object is related to the average kinetic energy of its atoms and molecules

32. Heat is a transfer of energy due to a temperature difference
Isolated warm (left) and cold (right) objects
Thermal contact is made: thermal energy is transferred from left to right
Thermal equilibrium: the same average KE for molecules in both objects

33. The temperature of an object is related to the average kinetic energy of its atoms and molecules
The temperature for curve (1) is lower than for curve (2) because the average kinetic energy is lower.

34. Temperature Scales
Figure: 01-18

35. Physical and Chemical Changes
Physical Change: changes in appearance but not in composition
e.g., sublimation of ice in the winter
EOS
Chemical Change: changes resulting in altered composition and/or molecular structure
e.g., spoilage of foods

36. Indications of Physical Change
The substance HAS NOT CHANGED its identity.
Its physical properties may change.
Changes of State are physical changes

38. Molecules on the move.

39. Indications of Chemical Change
Results in a new substance being formed!
Changes in physical properties:
Color change
Formation of a gas
Formation of a precipitate
Production or loss of heat
Production of other types of energy

42. The Law of Conservation of Mass or Matter
In any chemical reaction, matter (or mass) is neither created nor destroyed.