1. Facts of Matter
By Ms. Renfro

2. The two categories of matter
Pure Substances
Are chemically the same throughout
Mixtures
Substances that are not chemically combined

3. Pure substances
Pure substances include:
Atoms-the smallest part of all matter made of protons, neutrons, and electrons
Elements- substances made up of only 1 type of atom
MOLECULES ARE PURE SUBSTANCES THAT are formed from 2 or more Atoms Chemically combining
Compounds- Elements that chemically combine to form a new substance
dyjams/jams/science/matter/elements -and-compounds.htm

4. https://www.youtub e.com/watch?v=FofP jj7v414
Elements
Pure substances made from only one type of atom
Example: carbon only has carbon atoms, nitrogen only has nitrogen atoms
Cannot be broken down into simpler substances…they are pure!
Can be chemically combined to form compounds
e.com/watch?v=FofP jj7v414

5. What is the difference between atoms and elements?
Atoms are the smallest bits of ordinary matter.
Atoms are made from tiny particles called protons (positive), neutrons (no charge) and electrons (negative).
The protons and neutrons cluster together in the central part of the atom, called the nucleus
the electrons 'orbit' the nucleus.
A particular atom will have the same number of protons and electrons and most atoms have at least as many neutrons as protons.
An element is a substance that is made entirely from one type of atom.
For example, the element hydrogen is made from atoms containing just one proton and one electron.
Or the element gold, is made from atoms containing 79 protons and 79 electrons.

6. What is the difference between a compound and a molecule?
A molecule is formed when two or more atoms join together chemically.
A compound is a molecule that contains at least two different elements.
All compounds are molecules but not all molecules are compounds.
Molecular hydrogen (H2),  oxygen (O2) and nitrogen (N2) are not compounds because each is composed of a single element.
Water (H2O), carbon dioxide (CO2) and methane (CH4) are compounds because each is made from more than one element.
The smallest bit of each of these substances would be referred to as a molecule. For example, a single molecule of molecular hydrogen is made from two atoms of hydrogen while a single molecule of water is made from two atoms of hydrogen and one atom of oxygen.

7. Elements: pure substance
There are over 120 elements and most (92) are found in nature.
Fun Facts!
Approximately 95% of your body is made of the elements
Hydrogen __________
Carbon____________
Nitrogen______
Oxygen___________
Phosphorous_________
Calcium_____________

8. The Periodic table

9. Reading the periodic table
Provides a wealth of information about elements
Each element has a chemical symbol
Atomic number- tells the number of protons in the nucleus
Atomic mass-tells the mass of the protons and neutrons in the nucleus
The number of protons= the number of electrons

10. How the periodic table is organized
The basics
The periodic table is arranged in order of increasing atomic number.
The 2 main groups of elements on the periodic table are metals and non-metals.
The metals are on the left side of the table moving to the non- metals on the right.
The elements in the center are called transition metals.
Metalloids are found along either side of the staircase.

11. How the periodic table is organized
Groups/Families and Periods
The vertical columns are called groups/Families
The families have similar properties.
They also have the same number of electrons on the outer shell, which are called valence electrons.
Valence electrons are what determines an elements properties and reactivity.
The most reactive elements are on the far left and the least reactive elements are on the far right of the periodic table.
The horizontal rows are called periods.
Each element in the same period have the same number of atomic orbitals, or electron shells (the path that electrons follow around the nucleus)

12. Metals, nonmetals Non-Metals Metals Shiny 'metallic' appearance
Solids at room temperature (except mercury)
Very reactive
High melting points
High densities
Low electronegativities
Usually, high deformation (can bend without breaking)
Malleable
Ductile
Thermal conductors
Electrical conductors
High ionization energies
High electronegativities
Poor thermal conductors
Poor electrical conductors
Brittle solids
Little or no metallic luster
Gain electrons easily

13. Physical Properties of Metalloids Chemical Properties of Metalloids
The Metalloids, or semi-metals, are elements with properties that share properties of metals and non-metals.
Physical Properties of Metalloids
State of Matter
Solid
Luster
Metallic luster
Elasticity
Brittle
Conductivity
Semi-conductive. Average transmission of heat.
Chemical Properties of Metalloids
Oxidation
Readily form glasses
Alloys
Form alloys with metals
*Allotropic
Several metallic and non-metallic allotropic forms
Melting
Some metalloids contract on melting
Compounds
Reacts with the halogens to form compounds

14. What is a physical property?
A feature of matter that can be observed with your senses and measured without changing its identity.

15. Physical property examples
States of matter
If it’s a solid, liquid, gas, or plasma is a phys. Prop!
Texture
Color
Density
Luster
Melting, boiling, freezing point
Streak Odor Mass Volume Hardness

16. What is a Physical change?
A change that causes a physical property to change but it doesn’t change the identity of the substance.

17. Examples of physical changes
Matter changing states
Freezing, melting, boiling
Cutting, crushing, dissolving
Losing or gaining mass
***What does the arrow represent in this picture?
Solid
liquid
Gas
plasma

18. What is a chemical property?
The ability of matter to interact with something and change into a new substance with different properties.
It requires a chemical reaction!

19. Examples of chemical properties
Reactivity with oxygen
When 2 or more substances combine to form a new substance.
Example:
water+oxygen +Iron Rust

20. Examples of chemical properties
2. Flammability- The ability of a substance to burn What cannot burn??

21. 3. How fast a substance can catch on fire or burst into flames!
Combustibility
3. How fast a substance can catch on fire or burst into flames!

22. Chemical changes
Happens when 1 or more substances are changed into new substances with new properties.
Once there is a chemical change, it cannot change back!

23. Examples of chemical changes
Souring milk- smells bad due to bacteria forming
Bubbling when acid reacts with baking soda
3. rusting 4. Burning ** Chemical changes have chemical formulas because they are entirely new substances Example: H2O