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Title and
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Topic:
EQ:
NOTES: • Write out the notes from my website.
Use different types of note-taking methods to
help you recall info (different color
pens/highlighters, bullets, etc)
• When I lecture we will add more info, so
leave spaces in your notes
• DRAW ANY PICTURES, FIGURES, AND
WRITE OUT ANY PRACTICE
PROBLEMS/QUESTIONS.
• WE WILL ANSWER THEM TOGETHER.
So…LEAVE SPACES SO WE CAN
ANSWER QUES.
Summary (end of notes) :
1-2 Sentences of what you learned
Reflect
Question:
Reflect on
the
material by
asking a
question
(its not
suppose to
be
answered
from
notes)
Chemistry & Matter
Chemistry is the study of matter and the changes that it undergoes.
- Central Science!!!
Matter is anything that has mass and takes up space.
Almost everything is MATTER…..so what isn’t matter?
• Matter is composed of atoms, submicroscopic particles that are the fundamental building blocks of matter.
• Atoms are bonded together to form molecules, two or more atoms joined to one another.
States of Matter
• All matter that exists on Earth can be classified as one of these physical forms (s, l, g) called states of matter.
• States of matter – Physical property
Solids
• Examples: Wood, paper, iron, and sugar.
• The particles of a solid:
– Very tightly packed
– When heated, a solid expands
– Definite shape and volume – does not change to the shape of the container
– Incompressible - cannot be pressed into a smaller volume.
Liquids
• Examples: Water, blood, soda, and mercury
• The particles in a liquid:
– Not held in place
– Less closely packed than solids
– Able to move past each other = FLOWS
– Takes the shape of the container
– The volume is constant no matter what container it is in
– Liquids are incompressible
Gases
• Example: Neon, methane, carbon dioxide, and air
• flows to conform to the shape of its container
• fills the entire volume of its container
• Far apart
• Easily compressed – What does this mean??
Gases are compressible. Since the atoms or molecules that compose gases are not in contact with one another, gases can be compressed. Example – pushing on a balloon!! Bring gas particles closer together
Vapor vs. Gas • Gas and vapor are similar, but not the same
• Water is called a ______ when it is in the gaseous form?
• Carbon dioxide is called a _____ , not vapor.
• What’s the difference?
vapor
gas
A gas is something that is gaseous at room temperature while a vapor is something that was either a solid or liquid when at room temperature.
• Solid
• Liquid
• Gas
SHAPE
• definite shape
• of container
• indefinite shape
VOLUME
• definite volume
• definite volume
• indefinite volume
COMPRESSIBLE
• NO
• NO
• YES
Summary of States of Matter Chart
Pure Substance: Elements or Compounds
• Pure Substance - Matter that has a uniform and unchanging composition.
– 2 types: Elements and Compounds (and molecules)
element
compound
Elements vs. Compounds
• An element cannot be ___________ down or _____________ into
simpler substances by chemical means.
• Elements are the _________ forms of matter that can exists.
Examples: _______, Helium, __________
• A compound is made up of ____ or ________ elements
______________ bonded together.
• Compounds can only be broken down into simpler substances by
____________ ____________.
Examples: _______, Sand, _______________
broken changed
simplest
Mercury Gold
2 more chemically
chemical changes
Water NaCl (table salt)
Mixtures
• A mixture is composed of two or more different types of atoms or molecules combined in variable proportions.
onot chemically united, but simply mixed together.
o2 types: Homogeneous and Heterogeneous
Mixtures
Mixtures are a physical blend of two or more substances
mixed together.” Can be separated by _________ means.
Chicken Noodle Soup Whole Blood Salt Water
Homogeneous mixture (always called SOLUTIONS) – uniform composition.
Heterogeneous mixture – NOT uniform composition.
4 Separation methods: physically!! (distillation, filtration, crystalization, chromatography)
physical
Heterogeneous Mixtures
1. 2 categories of Matter – Pure Substances (Element/Compounds) and Mixtures (Homo/Heter)
2. All elements are made of atoms
3. All compounds are made from elements (chemically bound in a fixed ratio)
4. All Mixtures are made from combinations of elements and/or compounds (not chemically bound)
C12H22O11
NaHCO3
So, In conclusion….
Part 2 Topic: Physical vs
Chemical
EQ: What is the
difference between a
property and a change?
Title:Chem Review 1
Observing properties of matter
• Every substance has its own physical and chemical properties.
• Chemical and physical properties depend on temperature and pressure. – At room temp. water is a liquid with a density of
1.00 g/mL
Make this chart
**The next 3 slides of notes put in the chart**
Physical Properties
Chemical Properties
Physical Properties (add to chart) • physical property – a characteristic that can be
observed or measured without changing the identity of the substance. Examples are….. (write example words)
melting point state of matter
mass color
Boiling point density
odor taste
hardness
Chemical Properties (add to chart) • chemical property – a characteristic that can
be observed or measured with a change in the identity of the substanceExamples are….. (write example words)
flammability
reacts with oxygen
reacts with an acid
rust
Physical and Chemical Changes (Make chart – next 9 slides of
notes put in the chart) Physical Changes Chemical Changes
Physical Changes (add to chart)
• In a physical change, matter changes its appearance but not its composition.
• When ice melts, it looks different but its composition is the same. Solid ice and liquid water are both composed of water molecules, so melting is a physical change.
Physical Changes (in chart) • physical change – a change in a substance that
does NOT involve a change in the identity of the substance. Examples are….. (write example words)
cutting breaking
tearing dissolving
boiling
Chemical Changes (in chart)
• chemical change – a change in a substance that DOES involve a change in the identity of the substance. Examples are….. (write example words)
color change
…four good indications of a chemical change.
(HINT: Homework & Test Question!!)
gas released (often with an
odor)
energy change (light,
heat, …)
precipitate formed
Chemical changes ( in chart)
• Examples: explode, rust, oxidize, corrode, tarnish, ferment, burn, rot, dissolving metal in acid, spoilage of food.
• Rusting is a chemical change.
(it turns from iron to iron oxide)
1) ________ is produced: (________)
2) ________ is produced: (_____________ bugs/_____________)
3) ______________ is produced:
(______________)
Indications of Chemical Reactions
lightning fireflies
matches Heat
Light
Electricity
batteries
(HINT: Homework & Test Question!!)
Indications of Chemical Reactions 4) ___________________ forms: (_______ ________)
5) gas/smoke/odor/bubbles produced:
(_____________ ______)
Two liquids chemically
react to form a solid.
soap scum Precipitate (solid)
baking soda and vinegar
Physical and Chemical Changes
• So……..The difference between chemical and physical changes are
A physical change results in a different form of the same substance. A chemical change results in a completely new substance.
Separating Mixtures (4 types)
• Mixtures are physically combined & separated using the difference in physical properties of the substances.
Filtration (Lab)
Separates heterogeneous
mixtures composed
of solids and liquids.
Distillation (draw with notes) • Distillation is a separation technique that is based on differences in
the boiling points.
Step 1: _________ the solution.
Step 2: ________________ the vapor as is escapes and collect it.
www.edumedia-sciences.com/a438_l2-distillation.html
Boil
Condense
Crystallization
• Crystallization is a separation technique that results in the formation of pure solid particles from a solution containing the dissolved substance.
• Rock candy, pop rocks, suckers
Chromatography
• Chromatography separates the components of a mixture on the basis of how they travel or drawn across the surface of another material.
• The separation occurs because the various components of the ink spread through the paper at different rates.
Part 3 Topic: Law of
Conservation Mass and
Energy
EQ: How can a reaction
not lose or gain
mass/energy during a
chem rxn?
Title:Chem Review 1
How Matter Changes: Chemical Reactions
• Matter undergoes a chemical change when it undergoes a chemical reaction.
• In a chemical reaction, the substances present before the chemical change are called reactants.
• The substances present after the change are called products.
Law of Conservation of Mass:
There Is No New Matter
• Matter is neither created nor destroyed in a
chemical reaction.
• The total mass involved in the reaction remained constant.
• The law of conservation of mass states that mass is neither created nor destroyed during a chemical reaction—it is rearranged. (Also called the “Law of Conservation of Matter”)
Energy
• Energy is a major component of our
universe.
• Energy is the capacity to do work.
• Work is defined as a force acting on a
distance.
• The behavior of matter is driven by energy.
• Like matter, energy is conserved.
• The law of conservation of energy states that energy is neither created nor destroyed….The total amount of energy is constant.
• Energy can be changed and transferred from one object to another.
• Energy cannot be created out of nothing, and it does not vanish into nothing.
Endothermic and Exothermic
Reactions • Systems that absorb energy from
their surroundings – endothermic reactions
–Example: cold pack.
• Systems that release energy to their surroundings – exothermic reactions
–Example: holding a cup of coffee.
• Energy Diagrams – show how the energy changes between the reactants and products.
Temperature: Random Motion of
Molecules and Atoms
• The atoms and molecules that compose
matter are in constant random motion—
they contain thermal energy.
• The temperature of a substance is a
measure of its thermal energy.
• The hotter an object, the greater the
random motion of the atoms and the
higher its temperature.
We must be careful to not confuse
temperature with heat. Heat - is the transfer or exchange of
thermal energy caused by a
temperature difference.
Temperature - is a measure of how hot or cold an object is.
• indicates that heat ALWAYS flows from HOT objects to COLDER objects.
• measured using a thermometer.
3 Temperature scales:
• Fahrenheit (°F) scale, used mostly for weather (uses thermometer to measure heat in air).
• Celsius (°C) scale – uses thermometer
– water freezes at 0 °C
– boils at 100 °C.
– Room temperature is ~ 25 °C.
3 Temperature scales:
• The Kelvin (K) scale – no thermometer!!
– It’s a calculation to avoid negative temperatures.
• Absolute zero
• 0 K is the coldest temperature possible
• is the temperature at which molecular motion virtually stops.