1. Matter and Its Properties
Matter is anything that has mass and takes up space.
Mass is a measure of the amount of matter.
Volume is the amount of 3-D space an object occupies.

2. Objectives for this section
Distinguish between the physical and chemical properties of matter
Classify changes of matter as physical or chemical
Explain the gas, liquid, and solid states in terms of particles
Explain how the law of conservation of energy applies to changes of matter
Distinguish between a mixture and a pure substance

3. Basic Building Blocks of Matter
An atom is the smallest unit of an element that maintains the chemical identity of that element.
An element is a pure substance that cannot be broken down into simpler, stable substances and is made one type of atom.
Element types are metals, nonmetals, and metalloids.

4. A compound is a substance made from the atoms of two or more elements that are chemically bonded that can be broken down into simpler stable substances.
Physical and chemical properties are quite different from those of their component elements

5. Think of a molecule as the smallest unit of an element or compound that retains all of the properties of that element or compound.

6. A system is a collection of connected things or parts forming a complex whole within a defined boundary.
A phase is a set of states of a chemical system that have similar bulk structural properties, over a range of conditions, such as pressure or temperature. “Phase” is often used synonymously with “state of matter”.
Phases include solid, liquid, and gaseous states as well as two or more solids or two or more liquids, etc.

7. What properties can be used to describe --
This flower?
This kitten?

8. Properties of Substances
All substances have properties that we can use to identify them. For example we can identify a person by facial features, voice, height, finger prints, DNA etc. The more of these properties that we can identify, the better we know the person.
In a similar way matter has properties - and there are many of them.

9. Properties of Matter
Properties
Extensive
Intensive
There are many ways to classify the properties of matter. Two of the most common are these.
Properties
Physical
Chemical

10. Extensive vs. Intensive
Properties
Extensive
Intensive
Depend on the AMOUNT of substance
Do NOT depend on the amount of substance
Mass
Volume
Energy
Boiling point
Melting point
Density
Electrical conductivity

11. Physical vs. Chemical Properties
Properties that may only be observed by changing the chemical identity of a substance. This property measures the potential for undergoing a chemical change.
Heat of combustion pH
Reactivity to water
Flammability
Physical Properties
Properties that can be observed or measured without changing matter.
Color
Smell
Freezing point
Melting point
Boiling point
Viscosity
Density
Specific heat

12. Physical and Chemical Changes
PHYSICAL CHANGES are concerned with energy and states of matter.
A physical change does not produce a new substance.
Changes in state or phase (melting, freezing, vaporization, condensation, sublimation) are physical changes.
Examples of physical changes include crushing a can, melting an ice cube, and breaking a bottle.
CHEMICAL CHANGES take place on the molecular level.
A chemical change produces a new substance.
Examples of chemical changes include combustion (burning), cooking an egg, rusting of an iron pan, and mixing hydrochloric acid and sodium hydroxide to make salt and water.

13. How to Tell Chemical & Physical Changes Apart
A chemical change makes a substance that wasn't there before. There may be clues that a chemical reaction took place, such as light, heat, color change, gas production, odor, or sound.
The starting and ending materials of a physical change are the same, even though they may look different.

14. States of Matter—Definition
Solid Definite volume (size) and shape
Liquid Indefinite shape (fits shape of container), definite volume
Gas Expands to fill the volume and shape of its container
Plasma Gas of highly ionized particles, carries electric current
Bose-Einstein condensate Close to 0K, stops behaving as independent particles and clumps
Neutron stars, quark-gluon plasma, etc.

15. State of Matter –Visual Depiction
Bose-Einstein condensate

16. Bose-Einstein Condensate
In the 1920s Bose applied the idea of quantum states to photons. His ideas weren’t gaining acceptance until he sent them to Albert Einstein who predicted that, unlike at normal temperatures where atoms would be in many different energy levels, at very low temperatures, a large fraction of the atoms would suddenly go crashing down into the very lowest energy level and for all purposes be identical and coalesce into a single blob. Some people call this a "super atom" for just that reason.

17. SOM—Bonds between particles

18. Phase Transitions Between States
Enthalpy is a measure of the total energy of a thermodynamic system.

19. Energy and Changes in Matter
When physical or chemical changes occur, energy is ALWAYS involved.
For example, heat can provide enough energy for a physical change (such as melting or vaporization) or even for a chemical change (the decomposition of water into hydrogen gas and oxygen gas).
However, chemists don’t always agree whether a change is physical or chemical (dissolving sucrose in water is physical while dissolving table salt is chemical).

20. However
Energy, whether absorbed or released, is merely transformed from one form to another and the total amount of energy remains the same. Physical and chemical changes obey the Law of Conservation of Energy. Energy is neither created nor destroyed.

21. Reactants and Products
The substances that react in a chemical change are called the REACTANTS.
The substance(s) that are formed by the chemical change are called the PRODUCT(S).
When charcoal is burned in air, carbon and oxygen are the reactants in a combustion (burning) reaction which produces carbon dioxide.
Carbon plus oxygen yields carbon dioxide
C O CO2

22. More Ways to Classify: Mixtures
Another classification scheme for matter is whether or not it can be separated.
If “yes,” it is a MIXTURE. Heterogeneous mixtures include suspensions and colloids, while homogeneous mixtures include solutions.
If “no,” it is a PURE SUBSTANCE. It can be an element or a compound.
We will also discuss methods for separating mixtures.

23. Classification of Matter
Leave room in your boxes to write definitions and examples!!
Suspension
Colloid
Solution
Tyndall Effect--

24. This means that NO chemical bonds have been broken.
Mixtures
When two or more substances combine, and yet the substances keep their individual properties, the result is a MIXTURE.
This means that NO chemical bonds have been broken.

25. Heterogeneous Mixture
If the composition of the mixture is NOT the same, or uniform, throughout, this is a HETEROGENEOUS mixture.

26. Heterogeneous Mixture
The components are readily distinguishable.
Heterogeneous mixtures may have 2 or more phases present (stew has liquid and solid).

27. Homogeneous Mixtures
A mixture that is uniform throughout is called a homogeneous mixture. It can exist as a solid, liquid or gas (any phase).
Particles far smaller than colloidal particles also may be present in a mixture. There is no Tyndall effect and you can’t see separate particles even at high magnification.

28. Heterogeneous Mixtures
A SUSPENSION is a heterogeneous mixture that has solid or liquid particles suspended in a liquid. These particles can be filtered or will settle out.

29. If the particles are too small to settle out, this type of mixture is called a COLLOID.
Sometimes you can’t see small suspended particles unless you shine a light through the liquid. This is called the Tyndall effect.

30. Colloidal Dispersions
Besides milk (solids particles in liquid), examples are smoke (solid particles in a gas), mayonnaise (liquid in liquid), fog (liquid particles in a gas), and jello (liquid particles in a solid).

31. Solutions
All SOLUTIONS are homogeneous mixtures.

32. Solutions
Solutions are composed of a SOLVENT and at least one SOLUTE. For salt water, salt is the solute and water is the solvent.
SOLUTION of salt water (ocean)
SOLVENT = substance into which the solute dissolves
SOLUTE = substance that dissolves

33. Pure Substances A pure substance has
a definite and constant composition (its properties are constant throughout the whole sample and its composition is homogeneous)
cannot be decomposed by ordinary chemical, physical or mechanical means (sifting, filtering, crystallization, distillation, etc.)
properties that do not depend on how it is prepared or purified
remains either an element or a compound (e.g., water or CO2)
sharply defined melting point and boiling point
Gold remains gold even if hammered thinly.

34. Type of mixture
Example
Gas in gas
Atmosphere is a mixture of mostly nitrogen and oxygen
Liquid in liquid
Wine is mostly a mixture of ethanol and water
Solid in solid
Alloys such as brass are a mixture of metals
Gas in liquid
Carbonated soft drinks, CO2 in sugar water
Solid in liquid
Seawater, dissolved salt in water
Solid in gas
Smoke, tiny solid particles in atmospheric gases

35. Decanting
Filtering
Centrifuging
Sifting or sieving
Crystallization
Distillation
Evaporation
Chromatography
Magnetic attraction

36. Separation Techniques
Property used for separation
Examples
Sifting (sieving)
Particle size, density
Alluvial gold sifted from finer soil and sand by panning
Visual sorting
Color, shape, or size
Gold nuggets from crushed rock
Magnetic attraction
Magnetism
Iron can be separated from non-magnetic sulfur

37. More Separation Techniques
Property used for separation
Examples
Decanting
Density or solubility
Liquid water poured off from settled sand; lighter oil from water
Filtration
Solubility
Insoluble CaCO3 from soluble NaCl in solution

38. More Separation Techniques
Property used for separation
Examples
Evaporation
Solubility and boiling point
Soluble NaCl can be separated from water
Crystallization
Solubility
Slightly soluble CuCl2 can be separated from water

39. More Separation Techniques
Property used for separation
Examples
Distillation
Boiling point
Ethanol can be separated from water because it has a lower BP than water
Centrifuge
Density, viscosity
Blood constituents can by separated
Chromatography
(capillary action)
Polarity, size, solubility
Metal ions by differential solubility

40. Grades of Chemical Purity
Some Grades of Chemical Purity
ACS
American Chemical Society reagents
USP
US Pharmacopoeia standards CP
Chemically pure NF
National Formulary
FCC
Food Chemical Code specs
Technical
Industrial standards
Increasing Purity