Chemical Nomenclature Review of Atomic Structure from Physical Science.
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Transcript of Chemical Nomenclature Review of Atomic Structure from Physical Science.
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Chemical Nomenclature
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Review of Atomic
Structure from
Physical Science
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Two major parts of an atom
Nucleus (not to scale)
Electron Cloud
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Three Major Sub-Atomic Particles
• Protons• Neutrons• Electrons
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a single, relatively large particle with a
positive charge that isfound in the nucleus
PROTON (p+)
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THE PROTON
p+
• Fat (heavy)
• Positive (charge)
• Doesn’t move (lazy)
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a single, relatively large particle with a
neutral charge that isfound in the nucleus
NEUTRON (N°)
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THE NEUTRON
N°
• Fat (heavy)
• Neutral (charge)
• Doesn’t move (lazy)
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a single, very small particle with a
negative charge that isfound in a “cloud” around the nucleus
ELECTRON (e-)
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THE ELECTRON• Skinny (very light)
• Negative (charge)
• Moves a lot (runs around)
e-
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Review: Subatomic Particles
e-
N°
p+
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ELEMENTSa type of matter that
can not be broken down by ordinary chemical means
(everything on the PT)
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Elements are the simplest form of
matter. They can’t be broken down
anymore. They are the building blocks
of all matter!
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If it’s on the PT, its an Element!
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Atoms of the same element that differ in
charge.(They have the same # of p+, but different # of e-)
ION
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LiBr Al2O3 Na2O BI3
CaBr2 K2Se AlF3
MgCl2 NaF B2S3
KCl CaI2 NaAt
Group the above compounds by similarities. Make as many groups as you want. Put your results on “Charges” sheet.
• Based on your patterns, write rules concerning the ratio of elements in a compound.
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Positive Ions(cations)
Negative Ions(anions)
• Na+ (lost 1 e-)
• Ca2+ (lost 2 e-)
• Al3+ (lost 3 e-)
• Pb4+ (lost 4 e-)
• H+ (lost 1 e-)
• Cl- (gain 1 e-)
• O2- (gain 2 e-)
• P3- (gain 3 e-)
• S2- (gain 2 e-)
• OH- (gain 1 e-)
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If an atom GAINS electrons, its overall charge
becomes more negative.If it LOSES electrons, its
charge becomes more positive
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An ion comprised of a single atom
(Na+, O2-)
Monatomic Ion
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An ion made up of two or more atoms(i.e. O2
2- or SO42-)
Polyatomic Ion
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The charge on a monatomic ion
( O2- )
OXIDATION #
Oxidation #
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Compound made up of only two types of
elements(NaCl; Fe2O3)
Binary Compound
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Compound made up of more than two
elementsNaClO3; (Hg2)3 (PO4)2
Tertiary Compound
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How to Write Ionic Formulas
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When writing ionic formulas the sum of the charges
must equal zero
GOAL
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To balance the charges you need
2Al and 3O
Al3+ with O2-
Al2O3
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Parentheses must be used when
adding subscripts to polyatomic ions
HINT
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To balance the charges you need
2Al and 3 Sulfates
Al3+ with SO4
2-
Al2(SO4)3
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Kris Kross Method!
Ca3As2
Ca2+As3-
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Just kris kross the positive and the negative chargesNa1+Cl1- NaClBa2+O2- BaO
Pb4+NO31- Pb(NO3)4
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How to Name Ionic Formulas
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An ion with a POSITIVE
charge
CATION
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An ion with a NEGATIVE
charge
ANION
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1) Write the name of the cation
Naming Binary Formulas
2) Write the name of the anion, drop the ending, and add -ide
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Don’t forget to include the Roman Numeral when you
are naming atoms with multiple oxidation states
CAUTION
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Name: Fe2O3
Naming Roman Numerals
Iron (III) Oxide
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Old way of Naming Roman Numerals
Fe2+ = FerrousFe3+
= Ferric
Use endings –ous (smaller) or –ic (bigger) on the root of the Latin
name to represent charges
Cu+ = CuprousCu2+
= Cupric
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1) Write the name of the cation
Naming Other Ionic Compounds
2) Write the name of the anion (if it’s a polyatomic)
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HINTS ON NAMING
-ites are oxyanions with less oxygen than -ates
Sulfate = SO42- Sulfite = SO3
2-
Nitrate = NO31- Nitrite = NO2
1-
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HINTS ON NAMINGHypo- (less O) and Per- (more O) are
used to indicate relative Oxygen Hypochlorite = ClO1-
Chlorite = ClO21-
Chlorate = ClO31-
Perchlorate = ClO41-
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A compound with 3 different atoms
TERTINARY COMPOUND
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Oxidation #s of Ternary Compounds
*** Must get all the charges to equal 0 ***
In Na2SO4 what is the oxidation number on S?
Na = (1+) * (2) = 2+ O = (2-) * (4) = 8-
Without Sulfur, the charge is 6-. Thus, to get to an overall charge of
0, Sulfur must be a 6+!
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Oxidation #s of Polyatomic Ions
*** Must get all the charges to equal charge on polyatomic ion ***
In NO31- what is the oxidation number on N?
O = (2-) * (3) = 6-
Without Nitrogen, the charge is 6-. Thus, to get to an overall charge of 1-, Nitrogen
must be a 5+!
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Working with Hydrocarbons
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1) Count the # of C and pick the correct stem.
Naming Hydrocarbons
2) Add the suffix –ane3) If ring, add prefix–cyclo
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1) Linear = (2 x (# of C)) + 2
Finding the Formula for Hydrocarbons
2) Ring = 2 x (# of C)
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The formula for a substance as it exists in its molecular state
MOLECULAR FORMULA
Benzene: C6H6
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The simplest formula for a substance
EMPIRICAL FORMULA
Benzene: C6H6 CH
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Molecular FormulaC6H12O6
Molecular/Ionic Formula vs. Empirical Formula
Empirical FormulaCH2O
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The coefficient before a compound that
represents the amount of substance present
FORMULA UNIT
7 C6H6