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1/27/2017
Marine Science
Chemistry Review 2017
Scientific Method

Scientific Method
–
Six Steps
–
–
1.
2.
3.
4.
5.
6.

Scientific Laws and Theories
After MANY YEARS of retesting and proving the
hypothesis, it can become a Scientific Theory
–
–
–

A Well-Tested Explanation for a set of
observations or experimental results
This is not set in stone!!!
If new Observations/Experiments come along, the
theory can be changed!
Purpose
Research
Hypothesis
Experiment
Analysis
Conclusion
end
Scientific Notation
Steps to writing a number in scientific notation:
•
If the number is BIGGER than 1:
•
1. Find the decimal place
2. Move the decimal place to the LEFT, so that the
number is between 1 and 10
•
**Remember to count the number of places you moved
the decimal!!!!!
•
**Make sure to have 1 number in front and at least 1
number behind the decimal
3. Write the new number
Scientific Law
–
An organized plan for gathering, organizing, and
communicating information
The foundation of ALL modern science
A statement summarizing a pattern found in
nature
4. At the end add: x 10number of places
end
end
Scientific Notation
• If the number is SMALLER than 1
1. Find the decimal place
2. Move the decimal place to the RIGHT, so that
the number is between 1 and 10
• **Remember to count the number of places you
moved the decimal!!!!!
3. Write the new number
• **Make sure to have 1 number in front and 1
number behind the decimal
4. At the end add: x 10-number of places
end
•
•
•
•
•
•
•
•
•
•
•
•
300000000 =
503 =
10600 =
60 =
450 =
7=
0.00086 =
0.1 =
0.00568 =
0.048 =
0.4 =
0.0000000000459 =
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SI Units
• Scientists use a standard
set of units for all
measurements
– The SI Units
• Same as the Metric System
end
1.
2.
3.
4.
5.
6.
What you are
measuring
Unit
Symbol
Length
meter
m
Mass
kilogram
kg
Temperature
kelvin
K
Time
second
s
Volume
liter
L
SI Unit Prefixes
King
Henry Died
Kilo
Hecto Deca
Deci
Centi
Milli
k
h
d
c
m
•
da
By Drinking Chocolate Milk
To convert between prefixes:
– Find the Start and the Finish
– Count the number of places
– Move the decimal in that direction the same number of places
– If there is only 1 letter, then you are at the Base Unit
end
35 mL = ___ L
12 g = ___ mg
25 cm = ___ mm
4 L = ___ daL
4500 mg = ___ g
0.07 m = ___cm
Classifying Matter
• Matter
– Anything that has mass and takes up space
– Can be either a Pure Substance or a Mixture
• Compound
– Can be broken down
– Made of Different Atoms
– Atoms always combine the same way
– Ex: Water (H2O)
• Element
– Cannot be broken down into simpler things
– Made of the Same Atoms
– On the Periodic Table
– Ex: Gold (Au)
end
• Filtration
Separating Mixtures
– Separates based on the size of their particles
– Using a coffee filter
• Desiccation
– Water is completely removed from the
substance/organism
– Sponges: soaked vs dry
• Distillation
– Separates a solution based on boiling points
– Making moonshine
end
Physical Properties
• Physical property
– Something observed/measured that Does NOT
change the material
Examples:
Melting Point
Boiling Point
Density
end
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Density (D)
Physical Properties
– How tightly packed atoms are in a substance
Density
(g/mL or g/cm 3)
m
D
V
mass
(g)
Volume
(mL or cm 3)
– Units are either g/mL or g/cm3
• Remember: 1 mL = 1 cm3 !!!
– Things that are more dense will sink, Things that
are less dense will float
end
Physical Properties
1. A rock has a mass of 12 g. If it has a volume
of 50 mL, what is the rock’s density?
2. A block has a density of 0.15 g/cm3. If the
block has a volume of 75 mL, what is the
block’s mass?
3. A graduated cylinder has 13.4 mL of water.
When a marble, with a density of 6.2 g/mL, is
dropped in the cylinder the water level rises
to 34 mL. What is the marble’s mass?
end
Chemical Properties
Physical vs. Chemical Changes
• Chemical property
• Physical Change
Examples:
Flammability
• Chemical Change
– Something observed/measured that changes the
substance into something else.
– Ability to burn in the presence of oxygen (Make Fire!)
Reactivity
– How quickly a substance combines with another
end
– Some properties change,
• but the substance is still the same
– Ex: Ripping Paper, Ice Melting
– A reaction forms new substances
– Ex: Burning Paper, Making Silly Putty
end
Physical vs. Chemical Changes
• Evidence of a chemical change:
Changes of State (Phase Changes)
Gas
1. Change in color
Ex) Copper roof turns green
2. Production of a gas
Ex) See bubbles or starts to smell
Sublimation
3. Formation of a precipitate
end
Vaporization
Deposition
-Forms a solid
4. Temperature change
5. Production of light
Condensation
Solid
Melting
Freezing
Liquid
end
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Atomic Theories- Modern
Atom

The smallest particle of an element that retains
the properties of the element


Structure of the Atom
Atoms are made up of 3 particles


Protons, Electrons, and Neutrons
Called subatomic particles
end




Isotopes
Isotopes

Atoms of the same element
With different numbers of neutrons

end
Which means different mass numbers
All elements have isotopes
Elements occur naturally as a mixture of isotopes
Chemical Bonding

Chemical Bond

3 types

1.
2.
3.
end


Ionic Bonding
Ionic Bonding
Holds cations and anions together
 metal and a nonmetal (or polyatomic ion)
 Electrons are transferred

Ionic Compounds form a structure called a Crystal
Lattice

The cations and anions alternate to form a cube
end
holds atoms or ions together
Ionic--Metal and Nonmetal (& Polyatomic Ions)
Covalent--Nonmetal and Nonmetal
Metallic--Metal and Metal
end
Naming Ionic Compound
• Naming Ionic Compounds is easy.
• There are 3 steps
1. Name the metal
2. Name the nonmetal
3. Change the Ending to –ide
end
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Naming Ionic Compounds
Covalent Bonding
• Name the following:
1.
2.
3.
4.
5.
6.
7.

BaS
MgF2
Ca3N2

KOH
NaC2H3O2
Covalent Bond

nonmetal and a nonmetal
SHARE electrons

These are called the Diatomics (H, N, O, F, Cl, Br, I)

There are 7 nonmetals that never exist by
themselves.
Na2SO4


BrIN-Cl-HOF
Look for the 7 on the P.T.
Sr3(PO4)2
end
end
Naming Covalent Molecules

When naming Covalent
Molecules:
1.
2.
3.
4.
Use a prefix for first element
If it is 1, do NOT use a MONO
Name the first element
Use a prefix for second element
Always!!!
change the ending to –ide
end
Organic Chemistry
Number
Prefix
1
Mono-
3
Tri-
2
4
Di-
Tetra-
5
Penta-
7
Hepta-
9
Nona-
6
8
10
Hexa-
Naming Covalent Molecules

Practice:
1.
2.
3.
4.
As2O3
N2H4
CCl4
SO
Octa-
Deca-
• Organic chemistry is the study of carbon and
the study of the chemistry of life
• Main focus is on Carbon which is essential to
all life on earth
• Hydrogen, Nitrogen, Sulfur, and Oxygen are
also involved
end
Naming Organic Compounds
Prefixes for organic carbon chains:
Number of C
Prefix
1
meth
2
eth
3
prop
4
but
5
pent
6
hex
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• Name the following
1. CH4
2. C2H6
3. C4H10
4. C6H14
Acids and Bases
• Acid
– A compound that produces the hydronium ion
(H3O+) when dissolved in water
H2O + HCl  H3O+ + Cl– Chemical formulas start with an “H”
• HCl, H2SO4, H3PO4
– Remember: H+ = H3O+
end
Acids and Bases
• 3 general properties of acids:
– Sour Taste
• Like vinegar or spoiled milk
• Base
– A compound that produces the hydroxide ion
(OH-)
NaOH  Na+ + OH– Chemical formulas end with an “OH”
– Reactive with Metals
• Mixed with metals they will produce hydrogen gas
– Color change in indicators
• NaOH, Mg(OH)2, Al(OH)3
• 0-6 on pH scale
• Phenolphthalein turns colorless
• Litmus paper turns red
end
end
Acids and Bases
• 3 general properties of bases:
– Bitter Taste
Chemical Reaction
• Neutralization
– Reaction between an acid and a base
– This is a Double-Replacement Reaction
– Produces a salt and water
HCl + NaOH  H2O + NaCl
• Like dark chocolate and Cough syrups
– Slippery Feeling
• The base is dissolving your skin cells
– Color change in indicators
• 8-14 on the pH scale
• Phenolphthalein turns pink/red
• Litmus paper turns blue
end
Acids and Bases
Acid
Base
Water
Salt- an Ionic Compound
H2SO4 + Mg(OH)2  2H2O + MgSO4
end
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Strength of Acids and Bases
• pH scale
– A measure of the hydronium ion (H3O+)
concentration
– More H3O+ = More Acidic = Lower pH
Acidic
Neutral
Physics and Bio Review
Marine Science
2017
Basic
end

Force



Forces
A push or pull that acts on an object
Causes an object to accelerate
Friction
 Force that opposes an object’s
motion
 Keeps it still or slows it down
Types of Friction
1. Static Friction
a) A book resting on a table… it’s not going anywhere!!
2. Sliding Friction
a) A box being pushed on the floor… it’s sliding!
3. Rolling Friction
a) A ball rolling across the floor… it’s rolling!
4. Fluid Friction
a) A boat moving through a river (Fluid is the river)
b) An object in free-fall (fluid is the air)
end
Motion and Forces

Isaac Newton

In 1687 Newton created the
“Three Laws of Motion”
 Newton’s
 An
1st Law of Motion
object at rest will stay at rest, unless acted upon
object in motion will stay in motion, unless
acted upon
 An
 Also
 Inertia
called the “Law of Inertia”
 Objects
end
Motion and Forces
do NOT want to change their motion
end
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
Motion and Forces
Newton’s

2nd
Law of Motion
An object will accelerate when a force is applied
Motion and Forces

Newton’s 3rd Law of Motion

Example: Fish swimming
How?: In the ocean, fish move with the current
of the water as objects having force exerted on
them. Fish can use their fins to move in the
ocean over and above how the currents take
them. The force of the water combined with
the force of the fish in motion enable it to
move.
Example: Tides
How?:
• Newton mathematically explained how
forces in nature are affected by the
gravitational pull from the moon and sun.
• He explained that the pull of the sun and
moon on Earth’s oceans causes the
movement of tides.
• Earth's gravitational and rotational motion
forces the ocean waters to move.
end
For every action there is an equal and opposite
reaction
end
Layers of the Earth
• The earth is layered like an onion.
• There are 4 main parts:
1. Crust
2. Mantle
a) Lithosphere
b) Asthenosphere
c) Mesosphere
3. Outer Core
4. Inner Core
Plate Tectonics
• Plates are found in the lithosphere within the mantle and
part of the crust
• There are 10 major plates:
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
Pacific plate
North American plate
Cocos plate
Nazca plate
South American plate
African plate
Eurasian plate
Indian plate
Australian plate
Antarctic plate
Movement of Plates
Convergent: Plates come together
creates mountains and volcanoes
Divergent: Plates move apart
forms “rifts”—where new crust is
formed
ex) Mid Atlantic Ridge
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• 2 Types:
Cell Structure
– Prokaryotic:
• Bacteria and Archaea
• Lack membranes around organelles
• DNA located in nucleoid
– Eukaryotic:
• Plants and Animals
• Organelles have membranes
• DNA located in nucleus
Basic Cell Anatomy
• Nucleus: “brain” of the cell that holds DNA
• Ribosomes: protein synthesis using RNA and amino
acids
• Endoplasmic reticulum:
– Rough : has ribosomes, makes proteins
– Smooth: no ribosomes, makes lipids, transports
proteins
• Cell Membrane: surrounds animal cells, protects
from environment
• Cell wall: surrounds plant cells
• Cytoplasm: semi-fluid substance inside cell,
protects/cushions organelles
• Golgi Apparatus: moves proteins and lipids from
the ER and ribosomes to the rest of the cell
• 2 types:
Basic Cell Anatomy Continued
Chloroplasts: only in plant cells. Site of photosynthesis
Mitochondria: Site of cellular respiration (energy)
Lysosomes: digestive sacs that breakdown waste
Vacuole: Storage organelle, holds food, water, and
waste
• Nucleolus: Where DNA is held, ribosome get
information to make proteins
• Nuclear Membrane: double layered membrane,
separates the inside of the nucleus from the outside
• Centriole: organizes cell reproduction (division)
•
•
•
•
Eukaryotic Cells
– Plant Cells
•
•
•
•
Cell Wall
Chloroplasts
Central vacuole
No lysosomes
•
•
•
•
No cell wall
No chloroplasts
Smaller cauoles
lysosomes
– Animal Cells
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