• Essential objectives:
• Describe the difference between ions and
isotopes.
• Compare the major types of chemical bonds
and how do they differ.
UNIT 2 MINERALS
Minerals form raw materials manufactured
products.
Aluminum, graphite, copper, talc, silver, gold,
gemstones, and silicon.
Malachite: Ore of copper and a gemstone.
Quartz: Source of silicon used
in making computer chips
Galena: Ore of lead
Gemstones!
1. States of Matter.
a. Solids- atoms/molecules organized fixed
structures/defined shape. Atoms limited
vibration.
b. Liquids fluid mixtures atoms/molecules existing
charged atoms/molecules form ions. Form loose
associations through brief electronic bonds.
Liquid no fixed structures.
c. Gases fluid atoms/molecules rapid motion,
freely moving no fixed structure. Gases expand
to fill available space.
•Elements: Different types atoms that, in pure
form, cannot be divided into smaller units without
changing their properties.
•Atom: Smallest division of element, that still
possesses chemical properties unique to element.
•Compounds: 2 or more atoms bonded together.
Composed of atoms of same element, or combinations
of several different elements.
Nucleus contains:
Protons
= Particles mass of 1.0
positive electrical charge.
Neutrons = mass of1.0
neutral electrical charge.
electrons
A single
atom
protons
Orbiting the
nucleus are
electrons having
essentially no
mass and a
negative charge.
Number of protons in
nucleus of element
atomic number.
Model of
one atom
nucleus
Elements are distinguished from
each other by their atomic
number.
Examples: All Helium atoms have 2 protons
“ Carbon “
“ Uranium “
“ 6 “
“ 92 “
2. Atomic mass # protons plus # neutrons.
Most elements have different versions differ slightly
in mass because they have different # neutrons in
nucleus, isotopes.
Many isotopes are unstable, disintegrate through
radioactive decay – particles and/or energy are
emitted from the nucleus.
Ex. Carbon 14
Carbon example:
# protons determines type of atom
6 protons = carbon
# neutrons in atoms can vary.
# neutrons + # protons = atomic “mass”.
Here are the three isotopes of Carbon:
6 protons & 6 neutrons: mass number = 12
6 protons & 7 neutrons: mass number = 13 How we write it
6 protons & 8 neutrons: mass number = 14
12C
13C
14C
equals # of protons
3. When atoms gain or lose electrons they take on
an electrical charge- an ion.
Atoms with + charge are cations.
Atoms with - charge are anions.
4. Compounds are made /combining different
elements.
• 5. Minerals- naturally occurring compounds
classification by their chemical composition
/internal (atomic) structure.
• Characteristic – naturally occurring, inorganic,
solid, possess an orderly internal structure, and
have a defined chemical composition.
Example: Quartz
Quartz contains:
silicon (Si) and
oxygen (O)
element
name
Chemical formula for quartz is: SiO2
symbol
 Atomic Bonding
Bonding between atoms!
3 main ways:
“Ionic bonding” - loaning electrons
“Covalent bonding” - sharing electrons
“Metallic bonding” - electrons free to move about from atom to atom
Sharing Electrons: Covalent Bonding
Nucleus
Shared electrons
Example: Table Salt: Sodium (Na) and Chlorine (Cl)
Sodium gives up an
electron becoming
a positively-charged
charged cation.
Chlorine picks up the electron
from Sodium taking becoming
a negatively charged anion.
Example: Sodium (Na) and Chlorine (Cl)
Atoms arrange in orderly fashion: w/ alternating sodium and chlorine
atoms, so each negative ion is surrounded by positive ions, and visa versa.