Download IB1 Introduction to Ch

IB Chemistry
A Watson/
Scheffler
South Pointe High
School
IB Chemistry
Instructor : Mrs. Allyson Watson
Email : [email protected]
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Class Information/
Expectations Form
Your Name
Address
Telephone Number
Email
Hobbies:
Goals:
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IB Chemistry Agenda
Periods
• Information forms
• Safety contracts
• Class Policies
• Cornell Notes
• Brief overview of the course
• Chemical Hazards/Lab Safety
• Scientific Methods
• Assignments
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IB Chemistry JUNIORS
Assignments
• NEXT CLASS: Return signed the Safety
Agreement and read thoroughly the chemical
hazards/Lab Safety handout
• OTHER CLASS: Finish reading topic 1 in textbook
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Expectations
See expectation handouts for
details
• Attendance
• Make Up
• Behavior
• Grading
• Cornell notes
Cornell Notes
• Divide the paper
• Documentation
• Record notes
• Review and Clarify
• Summarize
• Study
Introduction to Chemistry
Chemistry
The study of matter and its relationships
The study of materials and how they
interact
The Central Science
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Chemistry Topics Include
Atomic Theory
Periodic Table
Bonding
Formulas and
Stoichiometry
States of matter
Calorimetry /
Thermodynamics
Solutions
Kinetics
Equilibrium
Acids and Bases
Oxidation
Reduction
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Is Chemistry Hard??
Maybe! --- but you will
develop skills that are
valuable for the rest of
your life!
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Is Chemistry Hard??
Well maybe but you will develop skills
that are valuable for the rest of your life
These include:
Abstract Thinking
Critical Thinking
Analysis
Logic
Math Skills
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Is Chemistry Hard??
Well maybe but you will develop skills
that are valuable for the rest of your life
These include:
Abstract Thinking
Critical Thinking
Analysis
Logic
Math Skills
Problem Solving
Communication
Time Management
Hazards Management
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Is Chemistry Dangerous??
Well maybe. sort of…..
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Chemical Hazards
Hazard Criteria
 A Threshhold Limit value of less than 500
ppm
 A Lethal dose (LD50) less than 500 mg per kg
 Readily polymerizable
 Flashpoint less than 140oF
 A strong oxidizer or reducing agent
 Highly corrosive
 Carcinogen, mutagen,or teratogen.
 Radioactive
 See the handout for more definitions and
criteria for chemical hazards
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Scientific Methods
• Always based on observation and
experimentation
• Observable and reproducible evidence
are required to support conclusions
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Scientific Method
Investigation process
- Preliminary observations
-
Formulation of a hypothesis
Design experiments to test the hypothesis
Evaluate and interpret data
Draw appropriate conclusions
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Hypothesis, Theory and Law
A Hypothesis is a tentative explanation or
expected result based on past evidence
and experience
A Theory is an explanation of a phenomona
based on the results of scientific
experimentation.
A Law is a principle that can be observed
repeatedly in the world over a long period
of time
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Scientific Methods
The scientific method is not necessarily
a chronological order that scientists
always follow.
But remember ………..
Scientific information is always based
on evidence. The emphasis is always
on information that we can gain from
observations and experiments
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Matter
• Has both volume and mass
• Exists in various states:




Solid
Liquid
Gas
Plasma
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Forms of Matter
• Element
• Compound
• Mixture
 Homogeneous
 Heterogeneous
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Elemental Composition
of the Earth
Properties of Matter
• Physical -
• Chemical • Extensive • Intensive -
Color
Density
Melting point
How the substance reacts with
other substances
Depend on the amount of
material
Independent of the amount of
material
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Density
• Definition
Ratio of mass to volume
• Formula
D = Mass/ volume
Density is an intensive property. It
is constant for most solids and
liquids, but it depends on the
pressure and temperature for a
gas
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Physical and Chemical Changes
• Physical -
• Chemical -
A change in state or shape.
Affects the physical properties
but retains the properties of the
substance
Undergoes a chemical reaction.
A new substance is formed with
new physical and chemical
properties
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Measurement
Measurements in the laboratory will
normally be made using the metric
system and SI units where feasible
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Temperature Scales
Kelvin Celsius Fahrenheit
Boiling point
of water.
373 K
100 oC
212 oF
Freezing point
of water.
273 K
100 oC
32 oF
0K
-273 oC
-460 oF
Absolute Zero.
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Temperature Conversions
Fahrenheit to Celsius
oC
= 5/9 ( oF - 32)
Celsius to Fahrenheit
o
F = 9/5 oC + 32
Celsius to Kelvin
K = oC +273
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Problem Solving Density
Formulas
Density = Mass/volume
D = m/V
M = DV
V = m/D
If you solve the formula
correctly the units will
match
D = m/V = g/cm3
M = DV = (g/cm3) /(cm3) = g
V = m/D =(g)/(g/cm3) = cm3
Units
Density = g/cm3
Mass = grams or g
Volume = cubic centimeters or
cm3
Measurement Issues
Uncertainty
Accuracy
Precision
Error
Significant Figures
Scientific Notation
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