Section 3.1: Atomic Structure of Matter
What is matter?

Section 3.1: Atomic Structure of Matter
Matter is anything that has mass and volume

Section 3.1: Atomic Structure of Matter
• We can classify matter by using the Periodic Table
• 3 Large Groups of elements on the periodic table

Section 3.1: Atomic Structure of Matter
• 1. Metal: shiny, ductile, conducts electricity
• 2. Non-metal: dull, does not conduct electricity
• 3. Metalloid: Shares properties of both metal and non-metal
• Elements are classified according to their place on the Periodic Table .

Periodic Table
6
C
Carbon
12.011

Periodic Table
6
C
Carbon
12.011
Atomic number

Periodic Table
6
C
Carbon
12.011
Atomic number
Element
Symbol

Periodic Table
6
C
Carbon
12.011
Atomic number
Element
Symbol
Element Name

Periodic Table
6
C
Carbon
12.011
Atomic number
Element
Symbol
Element Name
Atomic mass

Section 3.1: Atomic Structure of Matter
Structure of the Atom
• Nucleus: This contains positively charged protons and neutrally charged neutrons.
• Electrons : These surround the nucleus in an electron cloud and are negatively charged.

Section 3.1: Atomic Structure of Matter
Structure of the Atom
• The atomic number, or identity of the atom, is determined by the number of PROTONS !

The Nature of Matter
I. Atom: _____________________________________
A. Subatomic Particles
Particle Charge Relative Mass
Location in
Atom proton 1 neutron negative
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle Charge Relative Mass
Location in
Atom proton 1 neutron negative
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle Charge Relative Mass
Location in
Atom proton positive 1 neutron negative
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle Charge Relative Mass
Location in
Atom proton positive 1 neutron no charge negative
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle Charge Relative Mass
Location in
Atom proton positive 1 neutron no charge electron negative
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle Charge Relative Mass
Location in
Atom proton positive 1 neutron no charge 1 electron negative
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle Charge Relative Mass
Location in
Atom proton positive 1 neutron no charge 1 electron negative ~0
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle proton
Charge positive
Relative Mass
1
Location in
Atom nucleus neutron no charge 1 electron negative ~0
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle proton
Charge positive
Relative Mass
1
Location in
Atom nucleus neutron no charge 1 nucleus electron negative ~0
Most atoms are neutral because they have equal numbers of
________ and _____.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle proton
Charge positive
Relative Mass
1
Location in
Atom nucleus neutron no charge 1 nucleus electron negative ~0 Outside nucleus
Most atoms are neutral because they have equal numbers of
______and _______.
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle proton
Charge positive
Relative Mass
1
Location in
Atom nucleus neutron no charge 1 nucleus electron negative ~0 Outside nucleus
Most atoms are neutral because they have equal numbers of protons and electrons .
Atoms that lose electrons have a ________________ charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle proton
Charge positive
Relative Mass
1
Location in
Atom nucleus neutron no charge 1 nucleus electron negative ~0 Outside nucleus
Most atoms are neutral because they have equal numbers of protons and electrons .
Atoms that lose electrons have a positive charge.
Atoms that gain electrons have a ________________ charge.

The Nature of Matter
I. Atom: smallest unit of matter
A. Subatomic Particles
Particle proton
Charge positive
Relative Mass
1
Location in
Atom nucleus neutron no charge 1 nucleus electron negative ~0 Outside nucleus
Most atoms are neutral because they have equal numbers of protons and electrons .
Atoms that lose electrons have a positive charge.
Atoms that gain electrons have a negative charge.

The Nature of Matter
I. Element: ______________________________________
A. atomic number: _____________________________
B. mass number: _____________________________
C. isotope: __________________________________
______________________________________________
D. radioactive isotope: ________________________
___________________________________________
1. uses: _________________________________
___________________________________________

The Nature of Matter
I. Element: substance made of one type of atom
A. atomic number: _____________________________
B. mass number: _____________________________
C. isotope: __________________________________
______________________________________________
D. radioactive isotope: ________________________
___________________________________________
1. uses: _________________________________
___________________________________________

The Nature of Matter
I. Element: substance made of one type of atom
A. atomic number: #protons – defines an element
B. mass number: _____________________________
C. isotope: __________________________________
______________________________________________
D. radioactive isotope: ________________________
___________________________________________
1. uses: _________________________________
___________________________________________

The Nature of Matter
I. Element: substance made of one type of atom
A. atomic number: #protons – defines an element
B. mass number: sum of protons + neutrons in an atom
C. isotope: __________________________________
______________________________________________
D. radioactive isotope: ________________________
___________________________________________
1. uses: _________________________________
___________________________________________

The Nature of Matter
I. Element: substance made of one type of atom
A. atomic number: #protons – defines an element
B. mass number: sum of protons + neutrons in an atom
C. isotope: atoms of the same element with different numbers of neutrons
D. radioactive isotope: ________________________
___________________________________________
1. uses: _________________________________
___________________________________________

The Nature of Matter
I. Element: substance made of one type of atom
A. atomic number: #protons – defines an element
B. mass number: sum of protons + neutrons in an atom
C. isotope: atoms of the same element with different numbers of neutrons
D. radioactive isotope: isotope with an unstable nucleus that breaks down over time (emits radiation)
1. uses:
_________________________________
________________________________________
___

The Nature of Matter
I. Element: substance made of one type of atom
A. atomic number: #protons – defines an element
B. mass number: sum of protons + neutrons in an atom
C. isotope: atoms of the same element with different numbers of neutrons
D. radioactive isotope: isotope with an unstable nucleus that breaks down over time (emits radiation)
1. uses: dating fossils, diagnosing and treating diseases, killing bacteria in food/ on surgical equipment

The Nature of Matter
Nonradioactive carbon-12 Nonradioactive carbon-13 Radioactive carbon-14
6 electrons
6 protons
6 neutrons
6 electrons
6 protons
7 neutrons
6 electrons
6 protons
8 neutrons

Section 3.1: Atomic Structure of Matter
Structure of the Atom
• Isotopes are atoms with usually more neutrons than protons.
• The mass number equals the sum of protons plus neutrons.

Section 3.2: Composition of Minerals
Structure of the Atom
• A compound is a substance with two or more elements.
• Example is table salt or Sodium
Chloride (NaCl)

The Nature of Matter
III. Compound: _________________________________
______________________________________________
IV. Chemical Bonds
A. valence electrons: _________________________ ion: ______________________________
B. ionic bond: ___________________________________
____________________
C. covalent bond: _______________________________
___________ molecule: ___________________________________

The Nature of Matter
III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions
IV. Chemical Bonds
A. valence electrons: _________________________ ion: ______________________________
B. ionic bond: ___________________________________
____________________
C. covalent bond: _______________________________
___________ molecule: ___________________________________

The Nature of Matter
III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions
IV. Chemical Bonds
A. valence electrons: outermost electrons in an atom ion: ______________________________
B. ionic bond: ___________________________________
____________________
C. covalent bond: _______________________________
___________ molecule: ___________________________________

The Nature of Matter
III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions
IV. Chemical Bonds
A. valence electrons: outermost electrons in an atom ion: atom that has gained or lost electrons
B. ionic bond: ___________________________________
____________________
C. covalent bond: _______________________________
___________ molecule: ___________________________________

The Nature of Matter
III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions
IV. Chemical Bonds
A. valence electrons: outermost electrons in an atom ion: atom that has gained or lost electrons
B. ionic bond: bond formed by the transfer of electrons from one atom to another
C. covalent bond: _______________________________
___________ molecule: ___________________________________

The Nature of Matter
III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions
IV. Chemical Bonds
A. valence electrons: outermost electrons in an atom ion: atom that has gained or lost electrons
B. ionic bond: bond formed by the transfer of electrons from one atom to another
C. covalent bond: bond formed when atoms share electrons molecule: ___________________________________

The Nature of Matter
III. Compound: substance formed by the chemical combination of ≥ 2 elements in definite proportions
IV. Chemical Bonds
A. valence electrons: outermost electrons in an atom ion: atom that has gained or lost electrons
B. ionic bond: bond formed by the transfer of electrons from one atom to another
C. covalent bond: bond formed when atoms share electrons molecule: group of atoms covalently bonded together

The Nature of Matter
Sodium atom (Na) Chlorine atom (Cl)
Protons +11
Electrons -11
Charge 0
Transfer of electron
Protons +17
Electrons -17
Charge 0

The Nature of Matter
Sodium atom (Na) Chlorine atom (Cl) Sodium ion (Na + ) Chloride ion (Cl )
Protons +11
Electrons -11
Charge 0
Transfer of electron
Protons +17
Electrons -17
Charge 0
Protons +11
Electrons -10
Charge +1
Protons +17
Electrons -18
Charge -1

Section 3.2: Composition of Minerals
Bonding of Atoms
• Ions are formed when the number of electrons is either more or less than the number of protons .

Section 3.2: Composition of Minerals
Bonding of Atoms
• A covalent bond is when two atoms share electrons.
• A molecule is formed by covalent bonding of two or more atoms.

Section 3.2: Composition of Minerals
Bonding of Atoms
• An ionic bond is when atoms are held together by electrical attraction.

Section 3.2: Composition of Minerals

Section 3.2: Composition of Minerals
1.
2.
3.
4.
5.

Section 3.2: Composition of Minerals

Section 3.2: Composition of Minerals
1. By the Crystallization of Magma as it cools . Crystals form over long periods of slow cooling of magma.
2. By the pressure process as minerals are converted to other minerals by great amounts of heat and pressure.
3. By the evaporation of mineral-rich water. This is how geodes and the Cavern of Crystal Giants formed.

Section 3.3: Structure of Minerals
Why should we care about minerals? What do we use them for and what is our impact on the planet by using them?

Section 3.3: Structure of Minerals
What is the basic chemistry of the Earth’s Crust?
Other, 1.5% Common Elements of Earth's Crust
Mg, 2.1%
K, 2.6%
Na, 2.8%
Ca, 3.6%
Fe, 5.0%
Al, 8.1%
O, 46.6%
O
Si
Al
Fe
Ca
Na
K
Mg
Other
Si, 27.7%

Section 3.3: Structure of Minerals
Silicate Structures and Animations : The
Silica Tetrahedron
Four Oxygen atoms combine with one Silicon by covalent bonding of atoms

Structure of Graphite vs. Diamond
Diamond
Graphite
Both graphite and diamond are made of pure carbon, but diamond is much harder due to its tetrahedral structure. Graphite forms in carbon sheet structures. This allows it to be soft and flaky. This is good for use in pencils and lubrication for lock cores. Diamond is used in industrial purposes for saw blades and abrasives. It is also used as bling bling for jewelry!

Structure of Graphite vs. Diamond
Diamond Graphite
Both graphite and diamond are made of pure carbon, but diamond is much harder due to its tetrahedral structure. Graphite forms in carbon sheet structures. This allows it to be soft and flaky. This is good for use in pencils and lubrication for lock cores. Diamond is used in industrial purposes for saw blades and abrasives. It is also used as bling bling for jewelry!

Identifying Minerals

7
8
9
10
4
5
2
3
6
1
Rating
Mohs Scale of Hardness
Reference Mineral
Talc
(easily scratched by fingernail)
Reference Tool
Gypsum
(scratched by fingernail)
Fingernail (2.5)
Calcite
(barely scratched by penny)
Copper Penny (3.5)
Fluorite
(scratched by glass)
Apatite
(scratched by glass)
Potassium Feldspar
(scratches glass, but not steel nail)
Quartz
(scratches glass and steel)
Glass Plate (5.5)
Steel File (6.5)
Topaz
(scratches quartz)
Corundum
(scratches topaz)
Diamond
(scratches everything)

Mineral Groups
Silicates
• 90% of the Minerals in
Earth’s crust are silicates.
• A silicate is a compound of Silicon,
Oxygen, and one or more metallic elements.
Quartz (SiO
2
)
Orthoclase Feldspar (KAlSi
3
O
8
)

Mineral Groups
Carbonates
• Positive metal ion combined with a negative Carbonate
(CO
3
2) ion.
• Fizzes with
Hydrochloric Acid
Calcite (CaCO
3
)
Malachite (CaCO
3
)
Dolomite CaMg(CO
3
)
2

Mineral Groups
Halides
• Group of minerals that contains one of the halogen elements (F, Cl, Br,
I) as a building block
Fluorite (CaF
2
)
Halite (NaCl)

Mineral Groups
Native Elements
• Elements that are by themselves on
Gold (Au) the Periodic
Table
Diamond (C)
Sulfur (S)

Mineral Groups
Oxides
• Metal element combined with oxygen
• Valuable for their economic and industrial importance
Hematite (Fe
2
O
3
)
Magnetite (Fe
3
O
4
)

Mineral Groups
Sulfates
• Compounds containing the sulfate group (SO
4
2)
• Gypsum valuable for its industrial importance in construction (wallboard)
• Barite useful as main ore of Barium (used for barium contrast for Xray machines)
Gypsum
(CaSO
4
*2H
2
O)
Barite (BaSO
4
)

Mineral Groups
Sulfides
• Metal element combined with sulfur.
• When Hydrochloric
Acid is poured on
Galena, hydrogen sulfide gas (used to make stink bombs) is produced! Yuck!
Pyrite (FeS
2
)
Galena (PbS)

Mineral Groups
Phosphates
• Minerals that have phosphate (PO
4
) 3in their chemical formula
• Turquoise used for centuries by Egyptians and
Native Americans for jewelry
• Apatite is the main source of the phosphorous nutrient for plants. Your bones and teeth are made of the same substance as apatite!

Turquoise
(CuAl
6
(PO
4
)
4
(OH)
8
*5(H2O))
Apatite (Ca
5
(PO
4
)
3
(F,Cl,OH) )