1. Chapter 3: Matter-Properties and Changes

2. 3.1 Properties of Matter

3. Substances Matter is anything that has mass and takes up space.
Matter with a uniform and unchanging composition is called a substance.
Also known as a pure substance

4. States of Matter
All matter that exists naturally on Earth can be classified as one of the states of matter
The three common states of matter are solids, liquids, and gases

5. Solids
A solid is a form of matter that has its own definite shape and volume.
The particles of matter in a solid are very tightly packed
When heated, expands only slightly
Incompressible – cannot be pressed into a smaller volume

6. Liquids
A liquid is a form of matter that flows, has constant volume, and takes the shape of its container.
The particles in a liquid are not rigidly held in place and are less closely packed than the particles in a solid.
Liquid particles are able to move past each other
Allows a liquid to flow and take the shape of its container
Virtually incompressible
Tend to expand when heated

7. Gases
A gas is a form of matter that not only flows to conform to the shape of its container but also fills the entire volume of its container.
Because of the significant amount of space between particles, gases are easily compressed.
“Gas” refers to a substance that is naturally in the gaseous state at room temperature; “vapor” refers to the gaseous state of a substance that is a solid or liquid at room temperature.

8. Physical Properties of Matter
A physical property is a characteristic that can be observed or measured without changing the sample’s composition.
Density, color, odor, hardness, melting point, and boiling point are common physical properties that scientists record as identifying characteristics of a substance.

9. Extensive and intensive properties
Extensive properties are dependent on the amount of substance present
Ex: mass, length, or volume
Intensive properties are independent of the amount of substance present.
Ex: density
A substance can often be identified by its intensive properties

10. Chemical Properties of Matter
The ability or inability of a substance to combine with or change into one or more other substances is called a chemical property

11. Observing Properties of Matter
Every substance has its own unique set of physical and chemical properties
The particular form, or state, of a substance is a physical property, changing the state introduces or adds another physical property to its characteristics.
Important to state the specific conditions under which observations are made

12. 3.2 Changes in Matter

13. Physical Changes
A change which alters a substance without changing its composition is a physical change.
As temperature and pressure change, most substances undergo a change from one state (or phase) to another
A phase change is a transition of matter from one state to another
The temperature and pressure at which a substance undergoes a phase change are important physical properties – melting and boiling points.

14. Chemical Changes
A process that involves one or more substances changing into new substances is called a chemical change.
Commonly referred to as a chemical reaction
The new substances formed in the reaction have different compositions and different properties from the substances present before the reaction occurred.
In chemical reactions, the starting substances are called reactants, and the new substances that are formed are called products
A chemical reaction always produces a change in properties

15. Conservation of Mass
By carefully measuring mass before and after many chemical reactions, it was observed that, although chemical changes occurred, the total mass involved in the reaction remained constant.
The law of conservation of mass states that mass is neither created nor destroyed during a chemical reaction – it is conserved.
Mass reactants = Mass products

16. 3.3 Mixtures of Matter

17. Mixtures
A mixture is a combination of two or more pure substances in which each pure substance retains its individual chemical properties.
The composition of mixtures is variable, and the number of mixtures that can be created by combining substances is infinite.
Substances tend to mix naturally; it is difficult to keep any substance pure

18. Types of mixtures
A heterogeneous mixture is a mixture that does not blend smoothly throughout and in which the individual substances remain distinct.
Composition is not uniform
A homogeneous mixture is a mixture that has constant composition throughout; it always has a single phase.
Also referred to as solutions
Can include solids, liquids, and/or gases (Table 3)

19. Separating Mixtures
It is important to be able to separate mixtures into their component substances
The processes used to separate a mixture are physical processes that are based on the differences in the physical properties of the substances.
Heterogeneous mixtures composed of solids and liquids are easily separated by filtration.
Filtration is a technique that uses a porous barrier to separate a solid from a liquid.

20. Most homogeneous mixtures can be separated by distillation.
Distillation is a separation technique that is based on differences in the boiling points of the substances involved.
A mixture is heated until the substance with the lowest boiling point boils to a vapor that can then be condensed into a liquid and collected.

21. Crystallization is a separation technique that results in the formation of pure solid particles of a substance from a solution containing the dissolved substance.
Sublimation is the process during which a solid changes to vapor without melting
Can be used to separate two solids present in a mixture
Chromatography is a technique that separates the components of a mixture dissolved in either a gas or a liquid based on the ability of each component to travel or to be drawn across the surface of a fixed substrate

22. 3.4 Elements and Compounds

23. Elements
All matter can be broken down into a relatively small number of basic building blocks called elements.
An element is a pure substance that cannot be separated into simpler substances by physical or chemical means.
On Earth, over 90 elements occur naturally

24. Each element has a unique chemical name and symbol
The chemical symbol consists of one, two, or three letters
The first letter is always capitalized, and the remaining letter(s) are always lowercase
As many new elements were being discovered in the early nineteenth century, chemists began to observe and study patterns of similarities in the chemical and physical properties of particular sets of elements.

25. In 1869, the Russian chemist Dmitri Mendeleev devised a chart which organized all of the elements that were known at the time based on the similarities and masses of the elements.
Mendeleev’s table was the first version of the periodic table of elements.
The periodic table organizes the elements into a grid of horizontal rows called periods and vertical columns called groups or families.
Elements in the same group have similar chemical and physical properties

26. Compounds
A compound is made up of two or more different elements that are combined chemically
The chemical symbols of the periodic table make it easy to write the formulas for chemical compounds
Compounds can be broken down into simpler substances by chemical means

27. In general, compounds that occur naturally are more stable than the individual component elements
Separating a compound into its elements often requires external energy
The properties of a compound are different from those of its component elements.

28. Law of Definite Proportions
The law of definite proportions states that a compound is always composed of the same elements in the same proportion by mass, no matter how large or small the sample.
Percent by mass is the ratio of the mass of each element to the total mass of the compound expressed as a percentage
Percent by mass (%) = (mass of element/mass of compound) x 100

29. Law of Multiple Proportions
The law of multiple proportions states that when different compounds are formed by a combination of the same elements, different masses of one element combine with the same fixed mass of the other element in a ratio of small whole number.
Ex: water (H2O) and hydrogen peroxide (H2O2)