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168 Cards in this Set
- Front
- Back
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chemical
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any substance with a definite composition
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chemical reaction
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the process by which elements and/or compounds interaxct with one another to form new substances
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exothermic reaction
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a reaction in which heat leaves
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endothermic reaction
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A reaction in which heat is absobed
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product
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a chemical produced as a result of a chemical reaction
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reactant
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a chemical that is present at the beginning of a chemical reaction and that takes part in the reaction
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chemical change (definition and evidence)
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Definition: a change that produces one or more new substances
Evidence: 1. the evolution of a gas 2. the formation of a precipitate 3. The evolution or absorption of heat 4. The emission of light 5. A color change in the reaction system |
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chemical property
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a property of matter that can be observed only when substances interact with one another
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density
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the ratio of mass to volume
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mass
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the quantity of matter in an object
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matter
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anything that has mass and volume
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physical change
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a change that affects only physical properties
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physical property
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any property of matter that can be measured without changing its chemical nature
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quantitative observation
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An observation that has to do with precise measurements. (ie. You are being asked for a number.)
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qualitative observation
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An observation that has to do with characteristics of what is being observed
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quantity
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something that has magnitude or size
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unit
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a standard used when measuring a quantity
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volume
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the amount of space an object occupies
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weight
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the force produced by gravity acting on mass
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allotrope
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one of a number of different molecular or crystalline forms of an element
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atom
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The smallest particle of an element
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ion
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An atom or a group of atoms that carries an electric charge
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element
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smallest form of life
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molecule
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The smallest particle of an element or compound capable of a stable, independent existence
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compound
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A substance of two or more elements in fixed proportions. Compounds can be decomposed into their constituent elements
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mixture
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A sample of matter composed of two or more substances, each of which retains its identity and properties
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heterogeneous mixture
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A mixture that does not have uniform composition and properties throughout
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homogeneous mixture
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A mixture which has uniform composition and properties throughout
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deliquescence
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the process in which a soluble substance picks up water vapor from the air to fom a solution. In order for deliquescence to occur, the vapor pressure of the water in the air must be greater than the vapor pressure of the saturated solution.
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sublimation
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The direct vaporization of a sold by heating without passing through the liquid state
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condensation
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Liquefaction of vapor
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evaporation
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Evaporation is the process whereby atoms or molecules in a liquid state gain sufficient energy to enter the gaseous state.
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boiling
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The temperature at which a liquid changes to a gas
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melting
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The temperature at which a solid changes to a liquid
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freezing
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The temperature at which a liquid changes to a solid
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solution
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Homogeneous mixture of two or more substances
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pure substance
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molecule or atom
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activation energy
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the threshold energy that much be overcome to produce a chemical reaction
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inorganic compound
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any compound that does not contain carbon
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organic compound
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any compound of carbon and another element
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intensive property
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a property that doesnt depends on the amount of material presents
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extensive property
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a property, that depends on the iformation seen or given
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acid
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a class of compounds whose water solutions taste sour, turn blue litmus paper red and react with bases to form salts below 7.0
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base
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a class of compounds that taste bitter, feel slippery in water solution, turn red litmus paper blue and, react with acids to form salts
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pH
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The negative logarithm of the H + ion concentration in a solution
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system international
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the modern form of the metric system and is generally a system devised around the convenience of the number ten. It is the world's most widely used and oldest system of measurement, both in everyday commerce and in science.
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luster
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shininess: the visual property of something that shines with reflected light
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malleability
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the property of being physically malleable; the property of something that can be worked or hammered or shaped without breaking
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ductility
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the property of being bendable
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diatomic (definition)
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consisting of two atoms : having two atoms in the molecule
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diatomic (list)
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The diatomic molecules include hydrogen (H2), nitrogen (N2), oxygen (O2), fluorine (F2), chlorine (Cl2), bromine (Br2), and iodine (I2).
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electrical energy
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energy made available by the flow of electric charge through
a conductor |
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solid
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very little movement, vibrating atoms
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liquid
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atoms are moving faster than solid
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gas
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atoms collide and move the fastest
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plasma
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physical state of matter which exists at extremely high temperatures in which all molecules are dissociated and most atoms are ionized
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precipitate
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An insoluble solid formed by mixing in solution the constituent ions of a slightly soluble solution.
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energy
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The capacity to do work or transfer heat.
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forms of energy
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kinetic and potential energy
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chemical energy
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Energy released in a chemical reaction
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mechanical energy
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energy present in the components of a mechanical system.
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nuclear energy
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energy stored in interactions between the particles in the atomic nucleus
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fission
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the process of using a neutron to split a heavy nucleus into two nuclei with smaller mass numbers
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fusion
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the process of combining two light nuclei to form a heavier, more stable nucleus
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electromagnetic energy
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in the form of electric charges, magnetic fields, and photons;
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sound energy
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vibrational transmission of mechanical energy that propagates through matter as a wave (through fluids as a compression wave, and through solids as both compression and shear waves) that can be audibly perceived by a living organism through its sense of hearing.
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radiant energy
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the energy of electromagnetic waves (sunlight)
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heat
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total kinetic energy in a sample of matter
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chemical bond
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The attractive forces that hold atoms together in elements or compounds.
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kinetic energy
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Energy that matter processes by virtue of its motion
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law of conservation of energy
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Energy cannot be created or destroyed; it may be changed from one form to another
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potential energy
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Energy that matter possesses by virtue of its position, condition or composition.
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temperature
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A measure of the intensity of heat, i.e. the hotness or coldness of a sample. or object
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kelvin scale
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0-373
272 freezing 373 boiling 0- absolute zero |
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Celsius scale
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0-freezing
100-boiling |
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Fahrenheit scale
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32-Freezing
212- Boiling |
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Rankin scale
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491-Freezing
672-Boiling 0-absolute zero |
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absolute zero
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The pint at which there is no molecular movement, lowest possible theoretical point
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conductor
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is a material which contains movable electric charges
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insulator
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To prevent the passage of heat, electricity, or sound into or out of, especially by surrounding with a nonconducting material.
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specific heat
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The amount of heat required to raise the temperature of one gram of substance one degree Celsius
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hypothesis
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A tentative explanation for an observation, phenomenon, or scientific problem that can be tested by further investigation.
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scientific law
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A scientific law is a statement that describes the behavior of some particular thing or set of things within the natural world, with an adequately thorough history of successful scientific replication.
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law of conservation of mass
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the products of a chemical or physical process have the same mass as the reactants
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law of definite proportions
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any sample of a compound always has the same composition
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law of multiple proportions
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the mass ratio for one of the elements that combines with a fixed mass of another element can be expressed in small whole numbers
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theory
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accepted principles and methods of analysis, explanatory statements
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vaariable
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a variable is a quantity whose value may vary over the course of an experiment (including simulations), across samples, or during the operation of a system.
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data
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Factual information, especially information organized for analysis or used to reason or make decisions.
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serendipity
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The faculty of making fortunate discoveries by accident.
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scientific notation
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a way of writing numbers that accommodates values too large or small to be conveniently written in standard decimal notation.
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standard form
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known as scientific notation
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dependent variable
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A dependent variable is the effect of an independent variable occurring in an experiment
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independent variable
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When a variable is manipulated by an experimenter
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accuracy
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the extent to which a measurement approaches the true value if a quantity
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precision
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the extent to which a series of measurements of the same quantity made in the same way agree with one another
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significant figures
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A convention for recording measurements. Measurements are rounded so that they contain only the digits up to and including the first uncertain digit, when the number is written in scientific notation.
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percent error definition and formula
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((observed value)-(true value))
------------------------------------------ * 100 true value Percent error calculations are used to determine how close to the true values, or how accurate, their experimental values really are. |
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Dalton
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* Elements are made of tiny particles called atoms.
* All atoms of a given element are identical. * The atoms of a given element are different from those of any other element; the atoms of different elements can be distinguished from one another by their respective relative weights. * Atoms of one element can combine with atoms of other elements to form chemical compounds; a given compound always has the same relative numbers of types of atoms. * Atoms cannot be created, divided into smaller particles, nor destroyed in the chemical process; a chemical reaction simply changes the way atoms are grouped together. |
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Rutherford
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He discovered that atoms have a small charged nucleus, and thereby pioneered the Rutherford model,
Gold foil experiment |
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Thompson
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discovered the electron
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Bohr
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created the Bohr model
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Schrodinger
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shcrodinger's equatioin
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atomic mass (weight)
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the mass of an atom in atomic mass unit
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atomic theory
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the theory that all matter is composed of indivisible particles called atoms
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Avogadro's number
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the number of particles in one mole
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mole
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the unit for the amount of substance
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atomic number
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the number of protons in the nucleus of an atom
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A number
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mass number
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Z number
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atomic number
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electron
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negative charged particle that moves in shells around protons and electrons
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isotope
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different form of the same element because of neutrons
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mass number
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total number of protons and neutrons
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average isotopic mass
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average occurrence of isotope
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neutron
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a
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nucleus
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a
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proton
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a
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electromagnetic spectrum (radiation)
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radio to gamma
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Lewis Dot
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are diagrams that show the bonding between atoms of a molecule, and the lone pairs of electrons that may exist in the molecule.
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Hund's Rule
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Empty Bus Seat: every orbital in a subshell is singly occupied with one electron before any one orbital is doubly occupied, and all electrons in singly occupied orbitals have the same spin.
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Heisenberg Uncertainty Principle
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states that the values of certain pairs of conjugate variables (position and momentum, for instance) cannot both be known with arbitrary precision.
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Aufbau Principle
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A description of the building up of the elements in which the structure of each in sequence is obtained by simultaneously adding one positive charge (proton) to the nucleus of the atom and one negative charge (electron) to an atomic orbital.
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Pauli's Exclusion Priniciple
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no two electrons in the same atom can have the same set of four quantum numbers.
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Excited state
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is any quantum state of the system that has a higher energy than the ground state (that is, more energy than the absolute minimum).
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ground state
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energy than the absolute minimum
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Bright Line spectrum
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Opposite of Absorption spectrum, only has minor colors seen
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Absorption spectrum
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Includes most of bright line spectrum but leaves out some colors
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Continuous Spectrum
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All of the Rainbow due to diffraction grating
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white light
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lack of color in a spectrum
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orbital
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a region of an atom in which there is a high probability of finding one or more electrons
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sub-level
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the levels of electrons
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energy level
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the shells of electrons starting with 2 and then 8 continously
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quantum theory
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principles are both a dual wave-like and particle-like behavior of matter and radiation
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electron cloud
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The region of negative charge surrounding an atomic nucleus that is associated with an atomic orbital.
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frequency
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the number of occurrences of a repeating event per unit time.
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speed of light
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the rate at which light travels
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Mendeleev
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He is credited as being the creator of the first version of the periodic table of elements. Using the table, he predicted the properties of elements yet to be discovered.
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Mosley
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established a physical basis for the periodic table and found that atomic mass and atomic number have trends in the periodic talbe
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Seaborg
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contributed to the discovery and isolation of ten elements, developed the actinoids concept and was the first to propose the actinoids series which led to the current arrangement of the Periodic Table of the Elements.
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wavelength
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the distance between repeating units of a propagating wave of a given frequency.
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Alkali metals
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Group 1
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valence electrons
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outermost electron shell
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main group (representative elements)
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Groups 1,2 and 13-18
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rare earth elements
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lanthanoids and actinoids
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Bohr diagram
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The original diagram displaying the atom
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salt
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mix between group 2 metals and group 17
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transition metal
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group 3 to 12 that are in the D level
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periodic law(periodicity)
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is the quality of occurring at regular intervals or periods (frequency)
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Anion
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negatively charged ions
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Binary ionic compound
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An ionic compound that has two atoms
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polyatomic ionic compound
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An ionic compound that has three or more atoms
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cation
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positively charged ions
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electroneutrality
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Having same number of pos and neg electrons
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coulombic force
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The fundamental law of electrostatics stating that the force between two charged particles is directly proportional to the product of their charges and inversely proportional to the square of the distance between them.
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ion
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charged particle
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ionic compound
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a compound in which one atom has the desired electron nearly all the time
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isoelectronic
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having the same electron configuration as another atom
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octet
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the tendency of atoms of elements to gain or lose electrons so that their outer s and p orbitals are full with eight electrons
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Subscript
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number of atoms you have in that bond, molecule etc
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superscript
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charge of atom
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crystal lattice
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repetition of points for atoms, ions, or molecules to form a crystal structure
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halide
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salt formed from the halogen group
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ionic bond
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the coulombic force of attraction between ions of opposite charge
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monatomic ion
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single ion
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polyayomic ion
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two or more ions
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oxidation number
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the number assigned to an atom in a polyatomic based on the assumption of electrons transferred
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oxyion
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a positive polyatiomic ion containing oxygen
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stock system
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using the knowledge known to find the charge, number of electrons or etc
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