20 Mrs. Leinweber. Chemistry 20 Introduction What is science? What is chemistry?

20

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

Electrolysis of Water

Classifying Matter

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 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