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87 Cards in this Set
- Front
- Back
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Signs of a chemical reaction...
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-Color Change
- Solid forms - Bubbles are produced -A flame occurs - Change in heat: either produced or absorbed |
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Chemical Reaction
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The rearranging of the atoms in grouping
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Chemical Equation
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A representation of a chemical reaction showing through a reorganization of the atoms
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Reactants
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- a starting substance in a chemical reaction
-A reactant is shown to the left of the arrow in a chemical equation |
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Products
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A substance resulting from a chemical reaction
-A product is shown to the right of the arrow in a chemical equation |
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Balancing the chemical equation
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Making sure that there is the same number of each type of atom on the product side and the reactant side.
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Physical states and their symbol
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-Solid- s
-Liquid- l -Gas- g -Dissolved in water (aqueous solution)- aq |
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Coefficients
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The smallest integers (whole numbers) put in front of elements in a chemical equation to balance it
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Different reactions
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-Bubbles (gas given off)
-Changes in color -Heat -Becomes a solid |
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Driving forces
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-formation of a solid
-formation of water -transfer of electrons -formation of a gas |
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precipitation
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the formation of a solid
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precipitate
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the solid that forms
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precipitation reaction
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the reaction itself
- in virtually every case when a solid containing ions dissolves in water, the ions separate and move independently -ions of the solid dissociate when the solid dissolves in water |
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strong electrolyte
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a material that, when dissolved in water, dissociates (ionizes) completely and gives a solution that conducts an electric current very efficiently
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Soluble solid
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a solid that readily dissolves in water
-The solid “disappears” as the ions are dispersed in the water |
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Insoluble solid
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a solid where such a tiny amount dissolves in water that it is undetectable with the naked eye
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Slightly soluble solid
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a solid where such a tiny amount dissolves in water that it is undetectable with the naked eye
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molecular equation
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shows the complete formulas of all reactants and products
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Complete ionic equation
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better represents all forms of the reactants and products in solution.
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Spectator ions
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ions that do not participate directly in a reaction in solution
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Net ionic equation
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shows only those components that are directly involved in the reaction
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acid
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a substance that produces H+ ions (protons) when it is dissolved in water
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strong acids
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an acid that completely dissociates (ionizes) to produce H+ ion and the conjugate base
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base
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a substance that produces hydroxide ions in water
-NaOH (sodium hydroxide) is the most commonly used |
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Strong base
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- a metal hydroxide compound that completely dissociates into its ions in water
-KOH (potassium hydroxide is common |
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Oxidation-reduction reaction
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a reaction that involves a transfer of electrons
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Double-displacement reaction
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AB + CD -> AD + CB
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Acid-base reactions
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You can recognize an acid- base reaction because it involves an H+ ion that ends up in the product water
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Single- replacement reaction
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A + BC -> B +AC
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Precipitation Reaction
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a formation of a solid when two solutions are mixed
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Acid-Base Reaction
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-when a strong acid and a strong base are mixed and water is formed
-Examples of strong Acids: HCl (aq) and HNO3 (aq) -Examples of strong bases: NaOH (aq) and KOH (aq) |
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Combustion Reaction
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reactions that involve oxygen that produces energy so fast that make flames
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Synthesis (Combination) reaction
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when a given compound is formed from simpler materials
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Decomposition Reactions
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When a compound is broken down into simpler materials
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1 mol = ...
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6.022 x 1023
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Mole ratio
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a fraction relating the number of moles
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Grams -> moles
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divide by the molar mass
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Moles -> grams:
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multiply by the molar mass
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Percent Yield:
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% yield = actual yield/theoretical yeild x 100
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Wavelength
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The distance from one crest to another
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Frequency
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how freguently the crests pass by a certain point
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Electromagnetic Radiation
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Light exists as waves
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Photon
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Tiny packet of energy
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Ground State
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State a which a wave length has the least amount of energy
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Excited State
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State at which a wave length has an excess amount of energy
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Quantized
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a. Only certain levels of energy are allowed
b. Unable to stop in the middle |
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Pauli Exclusion Principle
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There can only be 2 electrons occupying one orbital because 2 electrons with the same spin cannot be together
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Electrons Spin...
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-Clockwise or counterclockwise
-Electrons that spin in the same direction will repel each other |
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What are the principle energy levels?
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1, 2, 3, 4…
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What are the sublevels?
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s, p, d, and f
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How many orbitals does the s orbital have?
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1
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How many orbitals does the p have?
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3
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How many orbitals does the d orbital have?
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5
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how many orbitals does the f have?
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7
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Lanthanides occupy what orbital...
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6f
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Actinides occupy what orbital?
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7f
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Valence electrons
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electrons in the outermost principle energy level
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Core electrons
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all electrons that are not valence
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atomic size
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the size of an atom
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Ionization Energy
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is the energy needed to remove an electron from an atom
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Bond
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force that holds atoms together
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Bond Energy
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energy needed to break a bond
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Ionic Bond
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bond between ions in which an electron is transferred
-Metal and nonmetal |
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Covalent Bond
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electrons sharing
-Nonmetal and nonmetal |
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If it is above 2.0 difference it is ...
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an ionic bond/compound
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.4 < d < 2.0
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Polar Covalent
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< .4
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Non polar Covalent
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Dipole moment
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compound has a center of positive charge and center of negative charge (you must have a polar covalent bond, but not every polar covalent bond has a dipole moment)
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Metal Ions
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have electron configurations similar to noble gas BEFORE them
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Nonmetal Ions
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have electron configurations similar to noble gas AFTER them
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Lewis structure
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a drawing that shows how valence electrons and atoms are arranged in the molecule.
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Duet rule
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Hydrogen & Helium
forms bonds to have 2 electrons |
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Octet rule
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all other atoms need 8 electrons to be stable
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Ione pairs
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unshared pairs of electrons
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double bond
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4 electrons shared
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triple bond
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6 electrons shared
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Resonance structure
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more than 1 Lewis Structure for a molecule
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Polyatomic Sharing
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to show that it is a polyatomic, you must put brackets around it, and show the charge.
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Boyle’s Gas Law
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P1 V1 = P2 V2
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Charles Gas Law
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V1/T1 = V2/T2
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Avogadro’s Law
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V1/n1= V2/n2
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Ideal Gas Law
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PV = nRT
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Combined Gas Law
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P1 V1 = n1R1T1
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Dalton’s Gas Law
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Ptotal = ntotal ( RT)
V |
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universal gas constant...
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R=.08206
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transition metals have how many valence electrons?
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2
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All Transition Metals have what sublevel?
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d
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