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Mrs. Leinweber
Chemistry 20Introduction
What isscience?
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?
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 quantitative observations when observing the light bulb?
What would be a qualitative observation when observing the light bulb?
What would be an interpretation when observing the light bulb?
Observations & Interpretations
Classifying Knowledge
Empirical knowledge is observable.
Theoretical knowledge is not observable, it explains and describes observations in terms of ideas.
Metals are shiny.Electrons occupy energy levels.
Classifying Matter
Review what you just learned
Check your Knowledge
1. Questions pg 11 #1-5, 7, 8
2. Questions pg 13 #1-5
How It Is Put Together
What are the parts ?
What are the parts ?
How To Use It
Atomic TheoriesElectron Energy Levels
Atomic Theories
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
Atoms and Ions
PRACTICE :)
Energy Diagrams
Review what you just learned
Check your KnowledgeRead pg 14-17Questions pg 16 #1-6,8,9
Ionic Compounds
OxideOxygen
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+ 8p+
Magnesium
Electrons
Ionic Compounds
Ionic Compounds
All ionic compounds are solids at SATP and form conducting solutions.
Practice Writing Names & formulas
Magnesium and fluorine
Magnesium and oxygen
Magnesium and nitrogen
Potassium and bromine
Potassium and sulfur
Potassium and nitrogen
Calcium and phosphorus
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 #1FeO(s)
Fe2O3(s)
Example #2SnF4(s)
SnF2(s)
Example #3BiP(s)
Bi3P5(s)
Example #4Chromium(III) sulfide
Example #5Technetium(VII) nitride
Example #6Copper (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 #1 sodium hydroxide
Example #2 potassium sulfate
Example #3 calcium nitrate
Example #4 iron(III) dichromate
Example #5 cupric phosphate
Predicting Polyatomic Ionic Compounds
Example #6 NH4Cl(s)
Example #7 Co(IO3)3(s)
Example #8 RuPO4(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+ P+
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.
hydrogen atom hydrogen atom
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 36 Q 1-3
Check your Knowledge
Questions pg 32 Q 3,4,5,15,16
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
1. Molar Mass (M) -
2. Mass (m) -
3. Moles (n) -
A measure of the amount of matter in an object. Mass is usually measured in grams or kilograms.
molar mass, Me the mass of one mole of a substance in units of grams per mole(g/mol)
mole t the SI base unit for the chemical amount or amount of a substance, whereone mole is the number of entities corresponding to Avogadro’s constant; unitsymbol, molmolecular
Chemical Amount
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
