1. Minerals
and
CHEMISTRY

2. Minerals All minerals must have the following characteristics:
Naturally occurring by Earth’s processes.
Solid orderly crystalline structure
Definite Chemical Composition
Inorganic (salt IS a mineral, sugar is NOT because it is organic)

3. Minerals
A mineral is a naturally occurring, inorganic solid with an orderly crystalline structure and a definite chemical composition.

4. Minerals Why are the following materials NOT minerals?
Chunk of Concrete
Brass Ring
Natural Gas

5. Matter Everything in the universe is made of matter.
Matter is found usually in three states:
Solid
Liquid
Gas
The building blocks of matter are elements.

6. Atoms
An atom is the smallest particle of matter that contains the characteristics of an element.
Atoms contain subatomic particles:
Protons: Positively charged, found in the nucleus
Electrons: Negatively charged, found outside of the nucleus.
Neutrons: No charge, found in the nucleus.
Atomic number: The number of protons in the nucleus of an atom.
In a neutral atom, number of protons = number of electrons.

8. Elements
An element is a substance that cannot be broken down into simpler substances by physical or chemical means.
There are currently more than 112 known elements.
92 occur naturally, others are created in laboratories
These elements are organized on the periodic table of elements.

11. Mixture
A mixture is a substance made by combining two or more different materials without a chemical reaction occurring (the objects do not bond together).

12. The Periodic Table (Pages 142-143 of your book)
Atomic Number H
Element
Symbol
Element
Name
Hydrogen
Mass
Number or
Atomic
1.0079

13. Using the periodic table:
You will need:
Graph paper, and a pen/pencil
Using the periodic table:
Make a line graph with atomic number on the vertical axis and mass number on the horizontal axis. Go from elements 1-30.
Answer the following:
What does the graph show about the general relationship between atomic number and atomic mass?
Are there any points on the graph that do not follow the pattern?
Does it make sense to organize the periodic table by atomic mass or atomic number?

14. Atoms
An atom is the smallest particle of matter that contains the characteristics of an element.
Atoms contain subatomic particles:
Protons: Positively charged, found in the nucleus
Electrons: Negatively charged, found in the outside the nucleus.
Neutrons: No charge, found in the nucleus.
Atomic number: The number of protons in the nucleus of an atom.
In a neutral atom, number of protons = number of electrons.

15. Isotopes
Atoms of the same element always have the same number of protons; but the number of neutrons can vary.
Atoms with the same number of protons but different numbers of neutrons are isotopes of an element.
(remember: Atomic Mass: Number of protons + neutrons)
Example: Carbon-12 (99% of all carbon) has 6 protons and 6 neutrons.
Carbon-13 has 6 protons and 7 neutrons
Carbon-14 has __ protons and __ neutrons 6 8

16. Charge (ions)
Remember that in a neutral atom the number of protons = number of electrons.
If there are more electrons than protons, the overall charge of the atom is negative.
If there are more protons than electrons, the overall charge of the atom is positive. 11
Atomic Number:
Atomic Mass/Mass Number:
Charge:
Number of Protons:
Number of Neutrons:
Number of Electrons: Na +1 23 +1 11 12 10

17. Bonds
A compound is a substance that consists of two or more elements that are chemically combined.
When atoms combine to form compounds, electrons are gained, lost, or shared.
Ionic bonds form between positive and negative ions. Electrons are transferred.
Covalent bonds form when electrons are shared.
Metallic bonds form when electrons are shared by metal ions.