20
Mrs. Leinweber
Chemistry 20
Introduction
What is
science?
What is
chemistry?
Scientific Process
Chemical Changes
Physical changes produce no new substances.
Chemical changes produce new substances.
Observations & Interpretations
Qualitative observations involve descriptions.
Quantitative observations involve measurements.
What would be some examples of qualitative and
quantitative observation when vinegar is added to
baking soda?
Observations & Interpretations
Interpretations (Inferences) is an indirect form of knowledge that builds on a concept or
an experience to further describe or explain an observation.
What would be a qualitative observation when observing the
light bulb?
What would be a quantitative observations when observing the
light bulb?
What would be an interpretation when observing the light bulb?
Classifying Knowledge
Empirical knowledge is observable.
Theoretical knowledge is not observable, it
explains and describes
observations in terms of ideas.
Electrons occupy energy levels.
Metals are shiny.
Classifying Matter
Classifying Matter
Electrolysis of Water
Review what you just learned
Check your Knowledge
1. Questions pg 11 #1-5, 7, 8
2. Questions pg 13 #1-5
The Periodic Table
Elements Song
How It Is Put Together
What are the parts ?
What are the parts ?
How To Use It
Atomic Theories
Electron Energy Levels
Atomic Theories
Atoms and Ions
Metals lose electrons to become cations (sodium ion)
Nonmetals gain electrons to become anions (chloride ion)
Carbon, boron, silicon and noble gas generally do not form ions.
Atoms and Ions
PRACTICE :)
Energy Diagrams
Review what you just learned
Check your Knowledge
Read pg 14-17
Questions pg 16 #1-6,8,9
Ionic Compounds
Ionic Compounds
Ionic compounds are formed when metals lose electrons to non-metals and
then are attracted to each other, forming an ionic bond.
Example: Magnesium and oxygen.
12p+
Magnesium
Electrons
8p+
Oxide
Oxygen
Ionic Compounds
All ionic compounds are solids at SATP
and form conducting solutions.
Practice Writing Names & formulas
Magnesium and fluorine
Potassium and sulfur
Magnesium and oxygen
Potassium and nitrogen
Magnesium and nitrogen
Calcium and phosphorus
Potassium and bromine
Sodium and chlorine
Multivalent Ionic Compounds
Many metals can form more than one ion, iron for
example can form Fe2+ and Fe3+ ions.
Naming Multivalent Ionic Compounds
Example #1
FeO(s)
Example #4
Chromium(III) sulfide
Fe2O3(s)
Example #2
SnF4(s)
SnF2(s)
Example #3
BiP(s)
Bi3P5(s)
Example #5
Technetium(VII) nitride
Example #6
Copper (II) Sulfate
Polyatomic Ionic Compounds
Polyatomic ions are composed of two or more elements covalently bonded with an
overall negative or positive charge.
Predicting Polyatomic Ionic Compounds
Example #1sodium hydroxide
Example #2potassium sulfate
Example #3calcium nitrate
Example #4iron(III) dichromate
Example #5cupric phosphate
Predicting Polyatomic Ionic Compounds
Example #6NH4Cl(s)
Example #7Co(IO3)3(s)
Example #8RuPO4(s)
Ionic Hydrates
Some ionic compounds exist as hydrates; have water molecules attached.
Example:
CuSO4*5H2O
Ionic Hydrates
Review what you just learned
Check your Knowledge
Questions pg 32 Q 3,4,5,15,16
Molecular Compounds and Elements
Molecular Elements and Compounds
Molecular molecules are formed between two nonmetals
due to a sharing of electrons.
+
P
hydrogen atom
+
P
hydrogen atom
Both hydrogen atoms need an extra electron to complete
their outer energy levels. Since neither is strong enough
to steal an electron away they share valence electrons.
Forming a covalent bond.
Molecular Elements
Many nonmetals are diatomic, others come
in groups of three, four, or eight
Binary Molecular Compounds
For hydrogen compounds such as
hydrogen sulfide, H2S(g), common practice
is not to use the prefix system.
Memorize the following table:
Acids and Bases
Acids are molecular hydrogen compounds whose solutions
conduct electricity.
Ionic bases contain the hydroxide ion.
Nomenclature Notes and Examples
Review what you just learned
Check your Knowledge
Questions pg 32 Q 3,4,5,15,16
Check your Knowledge
Questions pg 36 Q 1-3
Balancing Equations
Balancing Equations
Balancing Equations
Balancing Equations
Classifying Reactions
Combustion
Formation
Decomposition
Classifying Reactions
Assignment
1. Section 2.5 pg 59-60 Q 1 - 6
Classifying Reactions
Single Replacement
Double Replacement
Classifying Reactions
Classifying Reactions
SOLUBILITY
A SOLUTION is a homogeneous mixture of a SOLUTE (substance dissolved) and a
SOLVENT (substance dissolving, usually a liquid).
SOLUBILITY is the maximum amount of a substance that can be dissolved at a specific
temperature.
Assignment
1. Section 2.6 pg 64 Q 1 - 5
Chemical Amount
Chemical Amount
1. Molar Mass (M) molar mass, Me the mass of one mole of a substance in units of grams per mole
(g/mol)
2. Mass (m) -
A measure of the amount of matter in an object. Mass is usually measured in grams or kilograms.
3. Moles (n) -
mole t the SI base unit for the chemical amount or amount of a substance, where
one mole is the number of entities corresponding to Avogadro’s constant; unit
symbol, mol
molecular
Chemical Amount
Determine the molar mass of:
a. H2O
b.
CuSO4.5H2O
c.
Ca(NO3)2
d.
Iron(III) sulfate
Chemical Amount
Determine the chemical amount for:
a. 1500g of CaCO3
b. 50.0g of sucrose
Chemical Amount
Determine the mass for the following:
a. 2.50 mol of K2CrO4
b. 3.45 mmol of sodium sulfate
Assignment
1. Pg 53-54 Q1-5
2. Pg 57 Q1-3 & 5 & 6