1. What is matter? 2. What are the 3 states of matter? 3. Give one example each of an element, a compound, and a mixture. Actual SISS iron 21.05% sawdust 3.70% Values (write these down) sand: 56.76% salt: 18.49% http://www.youtube.com/watch?v=OTEX38bQ-2w Next lecture: bring some gum to chew (it must have sugar in it!)
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1. What is matter? 2. What are the 3 states of matter? 3. Give one example each of an element, a compound, and a mixture. Actual SISS iron21.05% sawdust3.70%
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1. What is matter?2. What are the 3 states of matter?3. Give one example each of an element,
a compound, and a mixture.
Actual SISSiron
21.05%sawdust
3.70%
Values (write these down)
sand: 56.76%salt: 18.49%
http://www.youtube.com/watch?v=OTEX38bQ-2w
Next lecture: bring some gum to chew (it must have sugar in it!)
is anything with mass and volume that takes up spaceand is made of ATOMS
If I go over something in lecture REALLY fast, it’s probably not THAT important. If we spend time on something….then it IS important (AND covered on the test
Matter can be found as:ELEMENT a pure
substance made of ONE kind of atom.
COMPOUND substance made from 2 or more atoms that are stuck together (bonded).
MIXTURE combination of 2 or more substances
Pure substancesMixturesWhether they are homogenous or heterogeneous depends on their phase
Classify each example. If it is a substance, write ELEMENT or COMPOUND . If it is a mixture, write
HETEROGENEOUS or HOMOGENEOUS in the mixture column.
homogenous
homogeneous
heterogeneous
homogenous
element
element
heterogeneous
element
compound
homogenous
SOLID LIQUID GAS
Keeps its shape. Does NOT keep its shape (takes shape of container).
Does NOT keep its shape (takes shape of container).
Can NOT be compressed (keeps same volume)
Can NOT be compressed (keeps the same volume)
Can be compressed to fit a smaller volume.
Particles are relatively fixed.
Particles are close but can flow past each other.
Particles have a ton of energy and fly apart.
Session 4 – Matter and EnergyTNTP Chemistry Content Seminar
Many materials are naturally available in pure form. Mixtures can be separated physically, but it requires energy.
Evaporation – separates substances by their volatility. Allowing a volatile component of a mixture to evaporate off leaves the other component behind.
Session 4 – Matter and EnergyTNTP Chemistry Content Seminar
Chromatography –separates substances by the speed that they pass through a stationary phase
Centrifuge – separates solids by density through use of gravitational and inertial forces. More dense solids end up at the bottom of a centrifuge tube as the centrifuge spins.
Session 4 – Matter and EnergyTNTP Chemistry Content Seminar
Extraction – separates solutes by their differences in solubility in polar and non-polar solvents
Recrystallization –separates a solute by its solubility in a solvent. A super-saturated mixture is made and then the solubility is reduced (by cooling or adding another solvent) and the solute “crashes-out” of solution in crystal form. (ex. making rock candy).
Session 4 – Matter and EnergyTNTP Chemistry Content Seminar
Filtering – separates a solute by its phase. Filtering solids through filter paper and allowing the liquid filtrate to pass into a collection flask.
Decanting – separates a solute by its phase and density. Simply pour the liquid off of a solid-liquid mixture.
Is this statement true? “Fog is air saturated with water, and as the air cools the water molecules get bigger and bigger until they become visible.”
No! Water molecules do not change in size. They can cluster and form liquid (fog!) or separate and form a vapor.
Distillation – uses difference in boiling points. Liquids are boiled and the vapors are condensed a different temperatures
http://www.youtube.com/watch?v=OTEX38bQ-2wPhysical vs Chemical Changes:
Evaporation vs. Electrolysis of H2Oevaporation: H2O(l) H2O(g)What bonds are disrupted? How do we know?Just ‘intermolecular forces’. The product is still water
(vapor) which is NOT. flammable
electrolysis: H2O(g) H2(g) + O2(g)What bonds are disrupted? How do we know?Covalent bonds break, products are flammable
BTW: We think of oxygen as a flammable gas, but oxygen is not a flammable gas-it does not burn…it supports the burning of other substances. By using the chemical properties of flammability and supporting burning, you can distinguish between the two gases hydrogen and oxygen.