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153 Cards in this Set
- Front
- Back
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Chemistry
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Anything that has mass and takes us space
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Organic Chemistry
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The study of the composition of matter and the changes that matter undergoes.
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Inorganic Chemistry
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The study of all chemicals containing carbon
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Biochemistry
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The study of chemicals that don’t contain carbon
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Analytical Chemistry
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The study of processes that take place in organisms
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Physical Chemistry
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The study of mechanism, the rate, and the energy transfer that occurs when matter undergoes a change
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Pure Chemistry
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The pursuit of chemical knowledge for its own sake
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Applied Chemistry
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Research that is directed toward a practical goal or application
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Technology
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The means by which a society provides its members with those things needed and desired. It’s a system of applied science.
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Macroscopic World
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The world of objects that is large enough to see with the unaided eye
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Microscopic World
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The world of objects that can be seen only under magnification
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Biotechnology
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Applies science to the production of biological products of processes
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Pollutant
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A material found in air, water, or soil that is harmful to humans and other organisms
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Scientific Method
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A logical, systematic approach to the solution of a scientific problem
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Observation
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Using your senses to obtain information
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Hypothesis
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A proposed explanation for an observation
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Experiment
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A procedure that is used to test a hypothesis
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Manipulated Variable
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Independent variable, one that is changed
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Responding Variable
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Dependent variable, one that is observed
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Theory
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A well tested explanation for a broad set of observations
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Scientific Law
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A concise statement that summarizes the results of many observations
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Mass
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A measure of the amount of matter the object contains
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Volume
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A measure of the space occupied by the object
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Extensive Property
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Property that depends on the amount of matter in a sample
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Intensive Property
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Property that depends on the type of matter in a sample
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Substance
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Matter that has a uniform and definite composition
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Physical Property
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A quality/condition of a substance that can be observed or measured without changing the composition
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Solid
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Form of matter that has definite shape and volume
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Liquid
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Form of matter that has an indefinite shape, flows, yet has a fixed volume
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Gas
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Form of mater that takes the shape and volume of its container
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Physical Change
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Some properties change but the composition doesn’t
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Mixture
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A physical blend of 2 or more compounds
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Heterogeneous Mixture
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Not uniform throughout
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Homogeneous Mixture
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Uniform throughout
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Solutions
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Another name for a homogeneous mixture
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Phase
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Used to describe any part of a sample with uniform composition and properties
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Filtration
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A process that separates a solid from the liquid in a heterogeneous mixture
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Distillation
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A process used to separate dissolved solids from a liquid, which is boiled to produce a vapor that is then condensed into a liquid
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Element
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The simplest form of matter that has unique set of properties
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Compound
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A substance that contains 2 or more elements chemically combined in a fixed proportion
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Chemical Change
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A change that produces matter with a different composition than the original
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Chemical Symbol
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Represents elements by 1-2 letters
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Chemical Property
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The ability of a substance to undergo a specific chemical change
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Chemical Reaction
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When one or more substances change into one or more new substances
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Reactant
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Substance at the start of a reaction
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Product
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A substance produced in the reaction
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Precipitate
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A solid that forms and settles out of a liquid mixture
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Law of Conservation of Mass
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Mass is neither created nor destroyed in a chemical reaction
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Measurement
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A quantity that has both a number and a unit
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Scientific Notation
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A given number that is written as the product of 2 numbers
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Accuracy
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A measure of how close a measurement comes to the actual or true value of whatever is measured
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Precision
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A measure of how close a series of measurements are to one another
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Accepted Value
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The correct value from reliable references
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Experimental Value
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Value measured in the lab
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Error
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The difference between the experimental value and the accepted value
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Percent Error
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Absolute value of the error divided by the accepted value, multiplied by 100%
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Significant Figures
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Include all digits known and last digit that is estimated
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SI (international system of units)
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A revised version of the metric system
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Meter
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The basic unit of length, or linear measure
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Liter
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Unit of volume
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Kilogram
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Unit of mass
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Gram
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The mass at 1 liter of water at 4°c
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Weight
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A force that measures the pull on a given mass by gravity
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Temperature
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A measure of how hot or cold an object is
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Celsius Scale
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Freezing point of water is 0°c; the boiling point is 100°c
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Kelvin Scale
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The freezing point of water is 273.15 Kelvin; the boiling point of water is 373.15 Kelvin
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Absolute Zero
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The zero point on the Kelvin scale, 0 K
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Energy
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Capacity to do work or to produce heat
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Joule
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The SI unit of energy
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Conversion Factor
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A ratio of equivalent measurements
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Dimensional Analysis
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A way to analyze and solve problems using the units of the measurements
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Density
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The ratio of the mass of an object to its volume
D= m/v |
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Atom
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The smallest particle of an element that retains its identity in a chemical reaction
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Dalton's Atomic Theory
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1. All elements are composed of atoms
2. Atoms of the same element are identical. 3. Atoms of different elements can combine to form simple whole-number ratios to form compounds |
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Electrons
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Negatively charged subatomic particles
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Cathode Ray
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Glowing beam
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Protons
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Positively charged subatomic particles
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Neutrons
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Neutrally charged subatomic particles
Mass= mass of a proton |
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Nucleus
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The tiny central core of an atom that is composed of neutrons and protons
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Atomic Number
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The number of protons in the nucleus of an element
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Mass Number
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The total number of protons and neutrons in the nucleus of an atom
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Isotope
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Atoms that have to same number of protons but different number of neutrons
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Atomic Mass Unit (amu)
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1/12 of the mass of a carbon-12 atom
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Atomic Mass
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A weighted average mass of the atoms in a naturally occurring sample of an element
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Periodic Table
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An arrangement of elements in which the elements are set up according to a set of repeating properties
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Period
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Horizontal row of the periodic table
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Group
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Vertical column of the periodic table
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Energy Levels
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The fixed energies an electron can have
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Quantum
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The amount of energy required to move an electron from one energy to another
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Quantum Mechanic Model
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The modern description of the electrons in atoms
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Atomic Orbital
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Region of space where there is a high probability of finding and electron
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Electron Configurations
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The ways in which electrons are arranged in various orbitals around the nuclei of atoms
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Aufbau Principle
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Electrons occupy the orbital of the lowest energy first
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Pauli Exclusion Principle
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An atomic orbital may describe at most 2 electrons
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Hund's Rule
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Electrons occupy orbitals of the same energy in a way that makes the number of electrons with the same spin direction as large as possible
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Amplitude
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A wave’s height from 0 to the crest
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Wavelength
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Distance between the crests
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Frequency
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The number of wave cycles to pass a given point per unit of time
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Hertz
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SI unit of cycles per second
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Electromagnetic Radiation
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Energy waves that travel in a vacuum speed of 2.998 × 10^8 m/s
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Spectrum
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Wavelengths of visible light that are separated when a beam of light passes through a prism; range of wavelengths of electromagnetic radiation
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Atomic Emission Spectrum
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The pattern formed when light passes through a prism or diffraction grating to separate it into the different frequencies of light it contains
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Ground State
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The lowest possible energy of an electron described by quantum mechanics
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Photons
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A quantum of light
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Heisenberg Uncertainty Principle
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It is impossible to know exactly both the velocity and the position of a particle at the same time
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Periodic Law
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When elements are arranged in order of increasing atomic number, there is a periodic repetition of their physical and chemical properties
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Metals
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Good conductors of heat and electric current; have a high luster, or sheen; all metals are solids at room temperature except Mercury (Hg)
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Non Metals
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Poor conductors of heat and electric current; carbon is the exception
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Metalloid
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Generally has properties similar to both metals and nonmetals
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Alkali Metals
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Group 1A
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Alkaline Earth Metals
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Group 2A
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Halogens
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Group 7A
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Noble Gases
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Elements in group 8A
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Representative Elements
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Groups 1A-7A; they display a wide range of physical and chemical properties
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Transition Metals
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One of the Group B elements in which the highest occupied s sublevel and a nearby f sublevel generally contain electrons
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Inner Transition Metals
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An element in the Lanthanide or Actinide series; the highest occupied s sublevel and nearby f sublevel of its atoms generally contain electrons
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Atomic Radius
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½ the distance between the nuclei of 2 atoms of the same element when the atoms are joined
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Ion
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An atom or group of atoms that has a negative of positive charge
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Cation
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Any atom or group of atoms with a positive charge
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Anion
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Any atom or group of atoms with a negative charge
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Alkaline Earth Metals
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Group 2A
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Halogens
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Group 7A
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Noble Gases
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Elements in group 8A
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Representative Elements
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Groups 1A-7A; they display a wide range of physical and chemical properties
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Transition Metals
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One of the Group B elements in which the highest occupied s sublevel and a nearby f sublevel generally contain electrons
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Inner Transition Metals
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An element in the Lanthanide or Actinide series; the highest occupied s sublevel and nearby f sublevel of its atoms generally contain electrons
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Atomic Radius
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½ the distance between the nuclei of 2 atoms of the same element when the atoms are joined
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Ion
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An atom or group of atoms that has a negative of positive charge
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Cation
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Any atom or group of atoms with a positive charge
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Anion
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Any atom or group of atoms with a negative charge
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Ionization Energy
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The energy required to move an electron from an atom in its gaseous state
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Electronegativity
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The ability of an atom to attract electrons when the atom is in a compound
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Valence Electrons
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An electron in the highest occupied energy level of an atom
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Electron Dot Structures
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A notation that depicts valence electrons as dots around the atomic symbol of the element
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Octet Rule
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Atoms react by gaining or losing electrons as to acquire the stable electron structure of a noble gas, usually 8 valence electrons
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Halide ions
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A negative ion formed when a halogen atoms gains an electron
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Ionic Compounds
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A compound composed of positive and negative ions
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Ionic Bonds
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The electrostatic attraction that binds oppositely charged ions together
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Ionization Energy
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The energy required to move an electron from an atom in its gaseous state
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Electronegativity
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The ability of an atom to attract electrons when the atom is in a compound
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Chemical Formula
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An expression representing a chemical reaction
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Valence Electrons
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An electron in the highest occupied energy level of an atom
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Formula Unit
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The lowest whole-number ratio of ions in an ionic compound
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Electron Dot Structures
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A notation that depicts valence electrons as dots around the atomic symbol of the element
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Octet Rule
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Atoms react by gaining or losing electrons as to acquire the stable electron structure of a noble gas, usually 8 valence electrons
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Halide ions
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A negative ion formed when a halogen atoms gains an electron
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Ionic Compounds
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A compound composed of positive and negative ions
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Ionic Bonds
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The electrostatic attraction that binds oppositely charged ions together
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Chemical Formula
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An expression representing a chemical reaction
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Formula Unit
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The lowest whole-number ratio of ions in an ionic compound
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Coordinate Number
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The number of ions of opposite charge that surround each ion in a crystal
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Metallic Bonds
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The force of attraction that holds metals together
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Alloys
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A mixture composed of 2 or more elements, at least one is a metal
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