Matter and States of Matter Student Notes PDF

Matter? What is matter? What matters matter?  Mass is a measure of the amount of matter in an object. Does not change regardless of location or gravity. Remains the same – earth, moon , space  An element is a pure substance that cannot be broken down into simpler substances by c...

Matter? What is matter? What matters matter?  Mass is a measure of the amount of matter in an object. Does not change regardless of location or gravity. Remains the same – earth, moon , space  An element is a pure substance that cannot be broken down into simpler substances by chemical means. It consists of only one type of atom. Examples: Unique atom number Oxygen (O) mono atom? Gold (Au) Periodic table Carbon (C)  A compound is a pure substance formed when two or more different elements chemically bond together in fixed proportions. Examples: Water (H₂O), which consists of hydrogen and oxygen. Sodium chloride (NaCl), which consists of sodium and chlorine. Glucose (C₆H₁₂O₆), which consists of carbon, hydrogen, and oxygen. Property change Break down Chem formula  A homogeneous mixture is a mixture that has a uniform composition and appearance throughout. The individual components are not distinguishable and are evenly distributed. Examples: Saltwater Uniformity Air Phases separation Vinegar Alloys (like brass)  A heterogeneous mixture is a mixture that does not have a uniform composition and where the individual components are distinguishable. Examples: Salad Uniformity Sand and salt mixture Phases Oil and water separation Concrete What are the differences? Are they made up of pure matter? Is the composition of elements/constituents fixed or not? Retention of original properties? Chemical bonding of elements or constituents? Separation method? Can elements be broken down into smaller matter? YES.  STATES OF MATTER The Four States of Matter Solid Liquid Gas Plasma  Properties Density Shape Characteristic property of pure substances Solids have well defined shapes and require Solids and liquids are much more dense than no container to hold them. gases. Liquids flow and take on the shape of their The solid and liquid states of a particular pure container substance have very similar densities. Gases , like liquids, flow and take on the The solid is usually slightly more dense than shape of their container - expands the liquid. Water is an exception, which is why ice floats. Compressibility Thermal expansion The ability to reduce the volume of a The increase in volume that occurs when a substance by applying pressure substance is heated. Gases are highly compressible Gases display moderately high thermal Liquids and solids both have very low expansion compressibility. Liquids and Solids expand very little when heated.  PHASE CHANGES Description of Term for Phase Heat Movement During Phase Change Change Phase Change Vaporization, Liquid to which includes Heat goes into the gas boiling and liquid as it vaporizes. evaporation Heat leaves the gas Gas to liquid Condensation as it condenses. Heat goes into the Solid to gas Sublimation solid as it sublimates.  KINETIC THEORY Kinetic Theory states that the tiny particles in all forms of matter are in constant motion. 3 Principles of Kinetic Theory – All matter is made of tiny particles (atoms) – These particles are in constant motion – When particles collide with each other or the container, the collisions are perfectly elastic (no energy is lost)  STATES OF MATTER Kinetic & potential energy Disruptive vs cohesive SOLID LIQUID GAS PLASMA Tightly packed, in a Close together with Well separated with Has no definite regular pattern no regular no regular volume or shape Vibrate, but do not arrangement. arrangement. and is composed of move from place to Vibrate, move Vibrate and move electrical charged place about, and slide freely at high particles past each other speeds  ATOMS A unit of matter Smallest unit of a chemical element Consists of a central nucleus surrounded by one or more electrons Is it the smallest thing in the Universe?  ATOMOS = INDIVISIBLE Democritos 460 - 370 B.C IF YOU CUT IN TREE IN PIECES, AND CONTINUE TO CUT IT, THERE WILL COME A POINT WHERE YOU CANNOT CUT IT INTO SMALLER PIECES  John Dalton 1800 -Dalton proposed a modern atomic model based on experimentation not on pure reason. All matter is made of atoms and are indivisible. Atoms of an element are identical in mass and properties. Each element has different atoms. Atoms of different elements combine in constant ratios to form compounds. Atoms are rearranged in reactions. His ideas account for the law of conservation of mass (atoms are neither created nor destroyed) and the law of constant composition (elements combine in fixed ratios).  Ernest Rutherford (movie: 10 min.) Rutherford shot alpha () particles at gold foil. Zinc sulfide screen Thin gold foil Lead block Radioactive substance path of invisible -particles Most particles passed through. So, atoms are mostly empty. Some positive -particles deflected or bounced back! Thus, a “nucleus” is positive & holds most of an atom’s mass.  Bohr’s model Electrons orbit the nucleus in “shells” Electrons can be bumped up to a higher shell if hit by an electron or a photon of light. What is the smallest particle we know?  I AM SURE ALL OF YOU KNOW WHAT AN ATOM NUMBER AND ATOMIC MASS IS. ISOTOPES Radioisotopes - Naturally occurring vs synthetically made Read up on this on your own and because I will probably test you on this. Valence electrons & valence shells?  Octet Rule Atoms will gain or lose electrons to have a full outer shell ( 4 valence e = gain; less than 4 valence e – lose ) Full shell = stability Chemical bonds  Bonding capacity – atom’s valence Electronegativity – atom’s attraction to the shared electron Polar vs non-polar covalent bond results in equal/non equal sharing ------ partial positive /negative charges  Hydrogen bond Hydrogen atom covalently attached to an electronegative atom is also attracted to another electronegative atom. O, N Electronegativity is an atom's tendency to attract electrons to itself in a chemical bond.  Van der waals If electrons are distributed asymmetrically in molecules or atoms, they can result in “hot spots” of positive or negative charge Van der Waals interactions are attractions between molecules that are close together as a result of these charges  WHY DO ATTEND ONLINE CLASS? A. JUST FOR THE ATTENDANCE B. TO AVOID HOUSE CHORES C. NOTES ( seniors told me notes may/may not be the same every year) D. I have NOTHING better to do in life E. Pursuit of knowledge….yeah right?! ONLINE LEARNING IS STILL LEARNING PAY ATTENTION MANAGE TIME FIRST YEAR IS THE EASIEST TO SCORE, DON’T WASTE IT COMMUNICATE WITH YOUR LECTURERS THIS IS ANDROGOGY , NOT PEDAGOGY!