Matter: It’s what the world’s made of.
Dec 30, 2015
Chemistry Studies Matter- Branches of Chemistry
Organic Study of most carbon-containing compounds Basis for most life processes as well as plastics, drugs,
petrochemicals, food, etc.
Inorganic Study of non-organic substances
Physical Study of properties and changes of matter and their relation to
energy
Analytical- identification of the components and composition of materials
Biochemistry- study of substances and processes occurring in living things
Theoretical- use of math and computers to provide theories that explain chemical observations; predict properties of new compounds
Chemistry Studies Properties Extensive properties
depend on amount of matter present volume, mass, and amount of energy
present Intensive properties
independent of the amount present boiling point, melting point, density,
conducting electricity and energy, phase change energy and others
States of Matter Solid – Definite shape and volume Liquid – Definite volume but variable
shape Assumes the shape of its container
Gas – Neither definite shape or volume Expands to fill any size container Takes the shape of the container
Plasma – Extremely high energy state where electrons have been ejected
Changes of State Melting Freezing Vaporizing
Boiling- change from liquid to vapor within the liquid as well as at the surface
Evaporation- change from liquid to gas at the surface of the liquid; occurs at much lower temperatures than boiling
Condensing Sublimation- example: dry ice (CO2)
Deposition- example: frost forming on a cold surface
What is Matter made of?
ElementsCompoundsMixturesSee classification scheme for matter
on p.11 of the text
What is Matter made of? Elements-cannot be broken down
Atomic-most elements can exist as individual atoms(smallest particle of any element). Examples: Fe, Au, Ag, Al
Molecular-some elements are… Diatomic H2, O2, N2, F2, Cl2, Br2, I2
Triatomic O3
Tetratomic P4
Octatomic S8
Elements are found on Periodic Table
What is Matter made of? Compounds-Two or more elements
chemically bonded together These can be broken down into smaller
compounds or elemental parts Examples: CaCO3(chalk), Fe2O3(rust)
Smallest particle is a Molecule
Pure Substances Always have a fixed composition Can be elements or compounds Always have the same properties Always have the same composition
Pure water is always 11.2% Hydrogen and 88.8% Oxygen by mass
What is Matter made of?
Mixtures-These are made of two or more chemicals that are not chemically bonded together. Examples: Sand, Salt/Pepper, Milk, Blood, Muddy water
Homogeneous – uniform throughout Heterogeneous – differences are found Mixtures can often be separated easily by
physical means such as filtration, distillation or chromatography.
Filtration: Separates solid substances from liquids and solutions.
Coffee FiltersSome water filtersPool filters using
sand or DE- diatomaceous earth (spongy skeleton)
Distillation: SeparatesHomogeneousmixtures using the differences inboiling points.BPH20 = 100˚C
BPNaCl = 808˚C
Water vapor rises first and condenses in the tube.
Physical Properties
Observed without changing the identity of a substance
Volume, mass, size, color, shape, smell, hardness, density, texture, melting & boiling points, temperature…
Physical Changes Change that alters appearance or
form of material but does not change the identity of the substance
Examples: tearing paper, breaking pencil, ice melting
Phase changes are ALWAYS Physical Changes
Chemical Properties What are the chemical activities of
the material Does it react with Oxygen Does it react with Water Does it react with Chlorine Does it react with Fluorine Does it react with …
Chemical Changes A chemical reaction occurs that
produces NEW substances Old chemicals bonds(Reactants) must
be broken and new ones(Products) formed usually with energy exchanging
Example: burning fuel, digesting food, Photosynthesis, rusting iron, plant decay
2 Kinds of Chemical Reactions
Exothermic Releases heat into surroundings Might feel warm or hot to the touch Reactants have higher energy in their bonds Examples:
Mixing acid with bases Burning of a fuel Digestion
2 Kinds of Chemical Reactions
Endothermic Absorbs heat from the surroundings Could feel cool to the touch Products have more energy than reactants Examples:
Cooking an egg Dissolving Baking Soda Photosynthesis Cooking coffee beans
Chemical Equations 2 H2(g) +O2(g) 2 H2O(l) + Energy
Coefficients “yields” (s), (g), (l) Energy is always involved-Heat or Light
Exothermic Endothermic
Balancing will follow later Matter CANNOT be created or destroyed
but it can be changed in reactions
Measuring Matter Using Le Système International (SI)
(Metric System only)(see pg 34) Volume -- V=LxWxH V=r2h
V=4/3r3
Mass -- gram, Kilogram- not affected by gravity, based on quantity of matter
Weight -- Pounds, Ounces- caused by the pull of gravity which can change
Volume – Gallons, Liters- space that a substance takes up
Density = mass/volume
Measurements are wrong! Measurements are not pure
numbers Measurements are made by man
using instruments made by man and subject to error
UNCERTAINTY FACTORS 345±2ml Every measuring device has an UF Usually ½ of the smallest readable
graduation
Uncertainty in Derived Quantities
For Addition and Subtraction Round all numbers to accuracy of the
least Do the desired math operation (A) Add all Uncertainty Factors of each
measurement used above (B) Write as A±B
Uncertainty in Derived Quantities
Multiplication and DivisionA. Round all numbers to accuracy of the least
accurate number involvedB. Do the desired math operation C. Divide each uncertainty by its measurement.
Pick the largest uncertainty from previous stepD. Multiply the Answer (C) times the value of B
B X C = new UF Combine B ± D (Derived answer w/ new UF)