Safety review. CHAPTER 1 THE SCIENCE OF LIFE Lets play a game… Am I alive? How can you tell?
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Transcript of Safety review. CHAPTER 1 THE SCIENCE OF LIFE Lets play a game… Am I alive? How can you tell?
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Safety review
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CHAPTER 1THE SCIENCE OF LIFE
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Lets play a game…
Am I alive? How can you tell?
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Characteristics of Life?
Organization Response to stimuli Homeostasis metabolism Growth and Development Reproduction Change through time
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Organization
High degree of order between internal and external parts
Interactions with the living world Examples?
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Response to stimuli
Ability to respond to changing environment
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Homeostasis
ability to maintain a stable internal condition.
No matter the changes in environment.
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Metabolism
Use of energy to power life processes
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Growth and Development
Growth? increase in amount of living material Development? process ending in adulhood Ie. Frog
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Reproduction
Production of Offspring Coded information is passed on to the
offspring Like Produces Like
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Change through time
evolution
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Science as a process
Scientific method
Organized approach to learn how the natural world works
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Scientific method
1. Observation / question: 2. Hypothesis: tries to
answer question; proposed explanation
3. Prediction: guesses what will happen
4. Experiment: tests hypothesis
5. Collect and analyze data6. Supports or disputes
hypothesis
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Scientific theory
When a set of confirmed hypotheses is confirmed to be true many times
Examples?
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Tools of the trade
Microscopes1. Compound light microscope Uses light through a specimen Electron microscpes use a stream of
electrons to visualize a specimen2. Scanning (SEM) electron microscope 3-D surface view3. Transmission (TEM) electron microscope 2-D internal view
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Compound Light Microscope
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Scanning Electron Microscope
SEM
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Transmission Electron Microscope
TEM
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Light vs. Electron
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SEM or TEM
SEM TEM
TEM SEM
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SEM or TEM
SEM TEM
TEM SEM
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More SEM
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More SEM
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More SEM
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The Metric System
Common Metric Units
Length (meters) Mass (grams)1 meter (m) = 100 centimeters (cm)1 meter = 1000 millimeters (mm)1000 meters = 1 kilometer
1 kilogram (kg) = 1000 grams (g)1 gram = 1000 milligram (mg)1000 kilograms = 1 metric ton (t)
Volume (liters) Temperature (Celcius)1 liter (L) = 1000 milliliters (mL)1 liter = 1000 cubic centimeters (cm3)
0o Celsius (C) = freezing point of water100o C = boiling point of water
•System of measuremnt in science. •Based on multiples of ten = easy conversion
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Ch 1 Vocab quiz next class
1. Biology2. Compound light
microscope3. Electron
microscope4. Gene 5. Hypothesis
1. Metabolism2. Metric
system3. Organization4. Scientific
method5. Theory
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CH 2CHEMISTRY OF LIFE
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Matter
Everything is made of matter (?) Has mass and occupies space
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Elements and atoms
Element: substances that cannot be broken down into simpler substances
Atoms: smallest particle of an element that retains the properties of that element
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Atomic structure
Nucleus makes up most of mass of an atom
Consists of protons (positive) and neutrons (no charge)
Number of protons = atomic number Number of protons + neutrons = mass number
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Atomic structure
Electrons: negatively charged particles Balance out with positive charge of
protons Very small mass Move around the nucleus in orbitals
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Isotopes
Atoms of same element have equal number of protons but not necessarily neutrons
Isotopes: atoms of the same element that have a different number of neutrons
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Compounds
Made of atoms of two or more elements H2O CO2
CH4
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A Covalent Bond occurs when atoms
share electrons
Covalent Bonds
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Ionic Bonds
Example: Sodium Chloride
Oppositely charged atoms, attracted to each other
Note: they do not share electrons
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Energy and Matter
Energy: ability to do work Many types of energy
Electrical Radiant (light) Thermal (heat) Chemical mechanical
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Chemical reactions
One or more substances change to produce one or more different substances
Reactants: on the left side of the equation
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Chemical reactions
One or more substances change to produce one or more different substances
Products: on the right side of equation
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Activation energy
Energy needed to start a reaction
Catalysts reduce activation energy Example: enzymes
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Water and solutions
Properties of water are necessary for life Many of water’s functions come from it’s
chemical structure Polarity: uneven distribution of charges Water is polar Polar nature allows water to dissolve
polar substances
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Hydrogen bonding
Polar nature allows water to be attracted to one another
+ region of one moleculue attracted to the – region on another
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Cohesion and adhesion
Cohesion: attractive force between molecules of a single substance Water attracted to water
Adhesion: attractive force between molecules of different substances Water attracted to other stuff
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Quick cohesion and adhesion lab HOW MANY DROPS OF WATER CAN I PUT
ON LINCOLN’S HEAD? Get in lab groups. Send one member up to the front to get
a penny and a cup Count the number of drops that you can
put on the head of a penny
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Temperature moderation
Water has a high heat capacity Water can absorb or release large
amounts of energy with only a slight change in temperature
This allows water to absorb heat during the summer to keep air cool w/o increasing the temp.
And at night, water cools and warms the air
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Density
Is ice more or less dense than water?
Discuss with your partner and write your ideas down in your notes
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Solutions
Solution: mixture of two or more substances
Solute: substance that dissolves in a solvent
Solvent: substance in which the solute is dissolved
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Acids and bases
pH scale is used to measure acidity or alkalinity
Scale from 0 14 06.9: acid 7 neutral (water) 7.114: base Buffers: chemical substances that
neutralize small amounts of acids or base added to a solution They keep the pH from changing greatly
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