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142 Cards in this Set
- Front
- Back
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Pure Science
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The search for a better understanding of our physical and natural world for its own sake.
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Applied Science/Technology
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Practical Application of Scientific Discoveries
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Data
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Results of experiments, often collections of measurements.
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Chemistry
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The study of matter, its structure, properties, and composition. Five Types: Organic, Biochemistry, Analytical, Physical, Inorganic
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Scientific Method
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The way in which a scientist goes about solving a problem: State a Problem, Observe, Search for Laws, Hypothesize, Theorize, Modify Theories.
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Experiments
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Carefully devised plans and procedures that enable researchers to make observations and gather observations.
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Scientific Law
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States a relationship between observed facts. Often in mathematical form.
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Hypothesis
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An educated guess based on observation.
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Theory
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An explanation for a problem based on observed patterns in facts. CANNOT be proven.
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Controlled Experiment
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An experiment in which variables are changed one at a time and the effect of each variable is noted.
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Quantity
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Term for things that can be measured like length, mass, and time.
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SI Base
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Length:Meter(m)
Time:Second(s) Mass:Kilogram(Kg) Thermodynamic Temperature:Kelvin(K) Amount of Substance:Mole(mol) |
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SI Prefixes
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Prefixes that can be used with SI base units to form new SI units in order to make greater of larger units.
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SI Derived Units
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Quantities measured in terms of other units.
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Precision
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How close a set of measurements for a quantity are to one another.
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Accuracy
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How close a measurement is to the true or correct value for the quantity.
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Significant Figures
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Digits in a measurement having values that are known with certainty plus one digit having an estimated value.
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Observed Value
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Value based on scientists laboratory measurements.
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True Value
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Most probable value based on generally accepted references.
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Absolute Error
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Differnce between the observed value and the true value.
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Percent Error
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Divide the absolute error by the true value and multiply by 100. Smaller value=More accurate measurement.
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Conversion Factors
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Measurements that are used to change, or convert, from one unit to another.
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Factor-Label Method
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Stoichiometry
8wags/1=12zooms/1wag=1bam/3zooms=1000warps/1bam 32000 warps |
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Dimensional Analysis
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The same as the Factor Label Method:Use of conversion factors and unit-labeled numbers.
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Scientific Notation
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A number is expressed as the product of two factors.
5.1x10^3 |
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Matter
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Anything that has mass and occupies space.
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Mass
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A measure of the quantity of matter of an object.
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Substance
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A kind of matter where all samples have the same properties or characteristics.
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Element
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A substance that cannot be broken down into other substances by ordinary chemical change.
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Compound
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A substance made up of two or more elements chemically combined. Can be broken down into simpler substances through chemical change.
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Mixture
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Consists of two or more substances, each of which retains its individual properties.
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Homogenous
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Matter that has uniform characteristics throughout.
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Heterogeneous
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Matter that has parts with different compositions.
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Properties
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The set of characteristics by which a substance is recognized.
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Extensive Properties
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Depend on how much of a particular sample is on hand: weight, volume, mass.
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Intensive Properities
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Do not depend on the size of the sample: melting point, density.
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Physical Properties
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Characteristics that can be observed without the production of new substances: color,odor,density,melting point.
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Chemical Properties
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Characteristics that describe how the substance interacts with other substances to produce new substances.
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Physical Change
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One or more physical properties of a substance are changed without any change in their chemical properties or composition and no new substances are produced.
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Chemical Change
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Change that results in the production of one or more substances that differ in chemical properties and composition from the original substance.
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Free State/Elemental State
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Elements exist alone, uncombined with other elements.
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Combined State
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Elements combined with other elements as part of a compound.
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Law of Conservation of Mass
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Matter cannot be created or destroyed in a chemical change.
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Chemical Symbols
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Abbreviation for the name of an element.
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Energy
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The ability to do work.
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Work
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Done on an object in response to a force (push or pull) moves some distance while the force is being applied to it. Work=Force x Distance
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Kinetic Energy
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Energy of Motion
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Joule
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Unit of Energy (J)
Newton x Meter (Kilogram x Meter)^2/second^2 |
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Law of Conservation of Energy
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No energy can be created or destroyed as a result of changes.
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Exothermic
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Reactants have more potential energy than the products. Gives off energy.
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Endothermic
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Products contain more energy than the reactants. Take in energy.
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Activation Energy
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The energy required to start a reaction.
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Celsius Scale
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Freezing Point of Water = 0.
Boiling Point of Water = 100. |
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Absolute Zero
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0 degrees on the Kelvin Scale
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Kelvin Scale
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Celsius Scale Plus 273
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Calorie
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Commonly used to measure heat. The amount of heat it takes to raise 1g of water 1 degree Celsius.
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Calorimetry
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The amount of heat released or absorbed during a chemical reaction.
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Calorimeter
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A reaction chamber surrounded by a known mass of water. The reaction takes place in the chamber and raises the temperature of the water.
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Specific Heat
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The amount of heat energy required to raise the temperature of 1 unit of mass of a substance by 1 unit of temperature.
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Electrostatic Force
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Force of attraction or repulsion between two charged bodies.
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Electric Current
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Flow of charge between two conductors.
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Electrical Conductors
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Substances between which electric charge flows.
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Chapter Six
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Shoma Shoma Shoma
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Atoms
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Fundamental building blocks that make up all matter.
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Nucleus
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Positive. Made of Protons and Neutrons. In the center of the atom.
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Subatomic Particles
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Electons, Neutrons, and Protons
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Electron
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Negative, Reside in Orbitals, 2000x smaller than protons and neutrons.
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Proton
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Positive, Reside in the Nucleus, 2000x bigger than electron, same size as neutron
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Neutron
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Neutral, Reside in the Nucleus, 2000x bigger than electron, same size as proton
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Discontinuous Theory of Matter
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Matter is made up of particles so small and indestructible that they cannot be divided into anything smaller.
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Continuous Theory of Matter
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A solid body can be divided into smaller and smaller pieces without limit.
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Law of Definite Proportions
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Proportion by mass of all elements in a given compound is always the same.
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Chapter One
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Shoma Shoma Shoma
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Chapter Two
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Shoma Shoma Shoma
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Chapter Three
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Shoma Shoma Shoma
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Chapter Four
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Shoma Shoma Shoma
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Chapter Five
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Shoma Shoma Shoma
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Law of Multiple Proportions
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Pairs of elements can form more than one compound.
ex: H and O can form water and hydrogen peroxide. |
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Cathode-Ray Particles
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What we now call electrons.
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Quantum Theory
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The idea that light come in discrete packets (quanta).
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Charge to Mass Ratio
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The ratio of charge on an electron to its mass.
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Alpha Particles
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One of the types of particles realeased when uranium and some other radioactive elements disintegrate.
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Energy Levels
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Electron orbits.
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Ground State
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All electrons are in the lowest energy levels available. Energetically stable.
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Excited State
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Electrons move from a lower energy level to a higher level.
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Charge-Cloud Model
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Nucleus is a dense positively charged core at the center of the atom, made of p+ and n. Electrons exist in orbitals outside the nucleus. e- form a cloud and show where they probably are.
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Orbital Model
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Nucleus is a dense positively charged core at the center of the atom, made of p+ and n. Electrons exist in orbitals outside the nucleus. e- form a cloud and show where they probably are.
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Quantum-Mechanical Model
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Nucleus is a dense positively charged core at the center of the atom, made of p+ and n. Electrons exist in orbitals outside the nucleus. e- form a cloud and show where they probably are.
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Orbitals
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Regions in space between sublevels.
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Scientific Model
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A mental picture that helps us understand something we cannot see or experience directly.
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Quanta
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Plural of quantum (bundle of energy).
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Quantum
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Bundle of energy.
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Wave Length
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The distance between two neighboring peaks or troughs.
wavelength=velocity/frequency λ=vf |
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Frequency
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The number of peaks that pass a given point each second.
frequency=velocity/wavelength f=v/λ |
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Hertz
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Measure of Frequency
Cycles per Second Abbreviated Hz |
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Velocity
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The distance a peak moves in a unit of time.
velocity=frequency x wavlength v=f x λ |
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Electomagnetic Spectrum
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Formed by all types of radiation.
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Continuous Spectrum
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The band of colors visible when light passes through a prism.
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Brightline Spectrum
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The set of lines visible when an element is burned and the light passes though a prism. Each element has its own set.
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Planck's Constant
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Energy is directly proportional to the frequency of the radiation. Represented by h.
E=hf E=energy (J) of a photon of radiation of frequency f. h=6.6x10^-34J/Hz |
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Nucleons
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The particles that make up the nucleus of an atom. Protons and neutrons.
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Atomic Number
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Number of protons in the nucleus of an atom.
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Isotopes
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Atoms of the same element that have different number of neutrons in their nuclei and therefore have different masses.
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Mass Number
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The sum of the protons and neutrons in the nucleus of an atom.
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Atomic Mass
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The average value of the masses of the isotopes in a natural sample of an element.
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Atomic Mass Unit
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One twelfth of a mass of an atom of the carbon-12 isotope; a unit used for stating atomic and formula weights.
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Chapter 13 and 14
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Shoma Shoma Shoma
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Neils Bohr
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Proposed that a seperate set of Laws of Physics existed for atoms and atomic sized particles. Quantum model of atom.
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Ernest Rutherford
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Proposed a new model of the atom which included a small, very dense, positive nucleus surrounded by mostly empty space where electrons existed. Gold foil experiment.
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James Chadwick
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Described the work of Iren Joliet-Curie as neutron emission rather than a new radioactive particle.
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J.J. Thompson
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Cathode Ray Tubes. Discovered electrons. Stated they came from the supposedly indestructible atom. Plum-Pudding Model.
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Robert Milikan
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Oil Drop Experiment. Determine the charge of an electron.
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John Dalton
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Made discoveries that became the basis of modern atomic theory. Developed the first unified atomic theory.
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Joseph Proust
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Law of Definite Proportions: The proportion by mass of the elements in a given compound is always the same. Basis for Dalton.
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Ancient Greek Model
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"atomos"-small, indivisible; all atoms made of same kind of matter; sized and shape determines element.
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Thompson (Plum Pudding Model)
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Mass of positive matter embedded with negative electrons.
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Bohr Model
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Positively charged nucleus with electrons in set orbits in distinct energy levels.
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Cloud Charge Model
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Positively charged center made of protons and neutrons with electrons in orbitals around it. They form a cloud and show where they most likely are.
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Ionization Energy
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The energy required to remove the most loosely held electron from the outer energy level of an atom in the gas phase.
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Electonegativity
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The measure of the ability of an atom that is chemically combined with another element to attract electrons to itself.
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Ionic Radius
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The effective distance from the nucleus of an atom to its valence shell.
Lose electrons: IR<AR Gain electrons: IR>AR |
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Atomic Radius
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Size of an atom
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Heisenberg Uncertainty Principle
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Cannot know the location and velocity of subatomic particle at the same time. No longer have the Bohr Model.
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Pauli Exclusion Principle
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In order for two electrons to occupy the same orbital they must have opposite spin.
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Aufbau Principle
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Electrons will first fill in areas that require low energy and then higher energy.
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Hund's Rule
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Electrons will spread out as much as possible within the orbitals amongst the suborbitals before filling in the suborbitals completely.
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Period
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horizontal row ordered by increasing atomic number.
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Group/Family
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vertical column; similar chemical properties.
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Chapter 7
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Shoma Shoma Shoma
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Alkali Metals
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s
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Alkaline Earth Metals
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h
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Metalloids
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h
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Nitrogen Family
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h
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Halogens
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h
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Noble Gases
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Group 18. Unreactant. Full outer shell.
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Triads
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hh
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Kernel
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h
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Qualitative Analysis
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g
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Quantitative Analysis
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g
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Molecule
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g
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Monatomic
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g
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Diatomic
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g
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