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82 Cards in this Set
- Front
- Back
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CHEMISTRY
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THE STUDY OF MATTER
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CHEMICAL
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ANY SUBSTANCE THAT HAS A DEFINED COMPOSITION
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CHEMICAL REACTION
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The process by which one or more substances change to produce one or more different substances.
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States of Matter
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The physical forms of matter: Solid, Liquid, Gas, and Plasma
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Solid
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Fixed volume and shape, particles held in a rigid structure, vibrate only slightly
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Liquid
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Fixed volume, not shape. Particles flow past each other, take on the shape of the container.
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Gas
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Neither fixed volume nor shape. Molecules weakly attracted
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Physical changes
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Changes in which the identity of a substance doesn't change; changes of state
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Chemical Changes
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Identities of substances change and new substances form
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Reactant
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A substance or molecule that participates in a chemical reaction
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Product
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A substance that forms in a chemical reaction
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Evidence of a chemical change
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Evolution of gas
Formation of precipitate Release or absorption of energy: light or temperature Change in color, odor, or taste |
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Defined composition
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Always the same "stuff", no matter the origin
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Chemical reactions ->
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Chemical changes
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Matter
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Anything that has mass and takes up space
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Volume
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A measure of the size of a body or region in three-dimensional space
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Mass (definition)
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A measure of the amount of matter in an object; a fundamental property of an object that is not affected by the forces that act on the object
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Weight
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A measure of the gravitational force exerted on an object
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Conversion Factor
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A ratio that is derived from the equality of two different units and that can be used to convert form one to the other
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Physical property
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A characteristic that doesn't involve a chemical change, such as density, color, or hardness
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Chemical Property
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A property of matter that describes a substances ability to participate in chemical reactions
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Length (SI)
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meter
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Mass (SI)
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kilogram
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Time (SI)
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second
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Thermodynamic Temperature
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Kelvin
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Amount of substance (SI)
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Mole
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Electric Current (SI)
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Ampere
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Luminous Intensity
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Candella
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Quantity
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A property that can be measured
-time -length -mass -temperature |
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Unit
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The size of the pieces the object is measured in
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Atom
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the smallest unit of an element that maintains the properties of that element
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Pure substance
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A sample of matter, either a single element or a single compound, that has definite physical and chemical properties
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Element
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the smallest unit of a substance that keeps all of the physical and chemical properties of that substance. It can consist of one atom or two or more atoms bonded together
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Molecule
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The smallest unit of a substance that keeps all of the physical and chemical properties of that substance. It can consist of one atom or two or more atoms bonded together
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Compound
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A substance made up of atoms of two or more different elements joined by chemical bonds
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Mixture
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A combination of two or more substances not chemically combined
-In a mixture, proportions of ingredients may vary |
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Homogeneous
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Describes something that has a uniform structure or composition throughout
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Heterogeneous
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Composed of dissimilar materials
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monoatomic
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With one atom existing individually
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Diatomic elements
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-gens and -ines
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Energy
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The capacity to do work
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Evaporation
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The change of a substance from liquid to gas
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Endothermic
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Describes the process in which heat is absorbed from the environment
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Exothermic
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Describes the process in which heat is released to the environment
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Law of Conservation of Energy
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Law that states that energy cannot be created or destroyed but can be changed from one form to another through physical or chemical means
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Heat
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The energy transferred between objects of different temperatures
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Kinetic engergy
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Energy of motion
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Temperature
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A measure of the average kinetic energy of particles in an object
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Specific heat
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The amount of heat needed to raise the temperature of one gram of a homogeneous material by one degree C
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Work
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Force applied through distance
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Energy Units
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Joules
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Kinetic Energy
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KE=1/2mv^2
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Boiling
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Only occurs at one temperature
Occurs throughout the liquid |
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Evaporation (Under what conditions?)
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Occurs at any liquid temperature
Occurs only at the surface |
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Sublimation (Under what conditions?)
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Occurs at any solid temperature
Occurs only at the surface |
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Scientific Method
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A series of steps followed to solve problems
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Hypothesis
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A theory or explanation that is based on observations that can be tested
Mimier Definition: An Educated Prediction |
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Theory
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An explanation for some phenomenon that is based on observations, experimentation, and reasoning
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Law
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A summary of many observations and experimental results
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Law of Conservation of matter
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Law that states that matter cannot be created or destroyed in ordinary chemical and physical changes
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2 Main Steps to Scientific Method
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Hypothesis
Controlled Experiment |
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Controlled Experiment
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Changes only 1 independent variable (x) and measures the effect on "y"
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Laws
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Specific rules that explain <i>how</i> nature works
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Theories
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General explanations of <i>why</i> nature behaves the way it does
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Model
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A way to visualize something that is too big, too small, or too complicated to deal with.
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Precisou
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Exactness or detail of a measurement
-or- How well a group of measurements agree with one another |
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Accuracy
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How well the measurements agree with the accepted value
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Law of Definite Proportions
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The law that states that a chemical compound always contains the same elements in exactly the same proportions in weight or mass
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Law of Multiple Proportions
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When two elements combine to form two or more compounds, the mass of one element that combines with a given mass of the other is in the ratio of small whole numbers
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Dalton's Principles
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-All matter is composed of extremely small particles, which cannot be subdivided, created, or destroyed
-Atoms of a given element are identical in their physical and chemical properties -Atoms of different elements differ in their physical and chemical properties -Atoms of different elements combine in simple, whole-number ratios to form compounds -In chemical reactions, chemicals are combined, separated, or rearranged, but never created, destroyed, or changed. |
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Democritus
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400 BC: came up with idea of atoms. Shot down by Aristotle
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John Dalton
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1800: Law of definite proportions
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Electron
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A subatomic particle with a negative charge
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Nucleus
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An atom's central region, which is made up of protons and neutrons
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Proton
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A subatomic particle that has a positive charge, found in the nucleus
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Atomic number determined by...
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Number of protons
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Thomson
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1897: discovers electrons coming out of every using cathode rays. Disagrees w/ Dalton, makes "plum pudding" model
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Rutherford
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1909: Gold Foil experiment.
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Rutherford's conclusions
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-Something in the atom is very hard, dense, small, positively charged, and massive = nucleus
-99.99% empty space, makes up most of the volume of the atom -Electrons on the outside Solar System Model |
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Chadwick
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1931: neutrons
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Atomic Number (symbol and definition)
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Z, number of protons
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Mass number (symbol and definition)
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A: number of protons+number of neutrons
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