Section 1
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Atomic Mass
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Cards (154)
Section 1
(50 cards)
Atomic Mass
Average of all naturally occurring isotopes
Condensation
Phase change from a gas to a liquid
Insoluble
Does not dissolve in water
Freezing
Phase change from a liquid to a solid
Exothermic
Energy is released by the system
Anion
Negatively charge ion
Ionization Energy
Energy required to remove the outer electron from a gaseous atom
Direct Relationship
Relationship between two variables where when one changes, the other changes in the same manner
Conversion Factor
Allows for the conversion from one unit of measure to another
Boiling
Phase change from a liquid to a gas
Electrolytic Cell
Redox reaction that is not spontaneous
Atom
Smallest constituent unit of ordinary matter that has the properties of a chemical element
Formula Unit
Ionically bonded atoms
Intermediate
Species produced in one step and consumed in another step
Double Bond
Two shared pairs of electrons
Calorimetry
Means of measuring the heat gained/ lost by a system during a chemical reaction
Deposition
Phase change from a gas to a solid
Dissociate
To break into ions
Empirical Formula
Lowest whole number ratio of atoms in a compound
Dissolve
To break into smaller pieces
Chemical Equilibrium
Rate of the forward reaction equals the rate of the reverse reaction
Distillation
Process of separating liquids based on differences in boiling temperatures
Bronsted-Lowry Acid
Donates a proton, H+
Alpha Particle
He2+ 2 protons, mass number = 4, 2+ charge Highly ionizing particle; Low energy
Dipole-Dipole
Permanent IMF present in polar molecules
Halogen
Elements in group 17. Form halides as ions
Arrhenius Acid
Donates a H+ ion
Electron Affinity
Energy released when an atom gains an electron
Filtration
Process of separating a precipitate from its aqueous solution
Filtrate
Liquid that passes through the filter paper
Cation
Positively charged ion
Gamma Ray
0 protons, mass number = 0, Low ionizing ability, high energy
Ion
Charge particle
Beta Particle
-1 proton, mass number =0; medium ionizing ability, medium energy
Covalent Bond
Bond formed by the sharing of electrons between atoms.
Electronegativity
The ability of an atom to attract electrons from another atom
Electron
Negatively charged particle. Charge = -1, Mass ~0amu. Located in the orbitals surrounding the nucleus
Electrolyte
Dissociates into charge particles which are capable of conducting electricity
Bronsted-Lowry Base
Accepts a proton, H+
Galvanic / Voltaic Cell
Redox reaction that is spontaneous
Activation Energy
Minimum energy needs to be added to a system in order for the chemical reaction to occur
Kinetic Energy
Energy of motion, temperature is a measure of KE
Atomic Number
Number of protons; defines the atom
Intermolecular Forces, IMF
Attractive forces between molecules
Absorbance
Light that does not pass through a solution A = abc
Arrhenius Base
Donates a OH- ion
Hydrogen Bonding
Strong dipole that results when H is bonded to F, O, or N
Ionic Bond
Bond formed by the transfer of 1 or more electrons from the least electronegative atom to the more electronegative atom
Indirect relationship
Relationship between two variables where when one changes, the other changes in the opposite manner
Catalyst
Lowers the activation energy. Not a reactant. Not a product
Section 2
(50 cards)
JJ Thomson
Discovered the e-
Rutherford
Theorized the nuclear model of the atom
Strong Acid
Dissociates 100% to produce H+
Hvap
Energy required to change 1 mol (l) to (g)
Oxidation
Process of losing electrons which increases the oxidation number
Soluble
Dissolves in water
Molecular Formula
actual number of moles of each atom in a compound
Goldstein
Discovered the P
Enthalpy
Delta H - (endo/exo)
Mass Number
Mass of all protons and neutrons
Reduction
Process of gaining electrons which reduces the oxidation number
Ideal Gas Law
PV=nRT
Percent Yield
(Quantity produced / Theoretical Amount) x 100%
Surroundings
This refers to everything outside of the system
Gibbs Free Energy
Energy available to do work
Molar Mass
grams per 1 mol
Strong Base
Dissociates 100% to produce OH-
Triple Bond
Three shared pairs of electrons
Oxidation Number
A charge assigned to an atom that represents that charge it would have if it contained and ionic bond. Are written as charge value, +4, -6, +2
Weak Acid or Base
Dissociates very little. Remains mostly in its molecular form
Principle Energy Level
n= 1 means first energy level. They contain sublevels
Significant Figures
Those digits that carry meaning contributing to its precision
Entropy
Delta S - (disorder/order)
Endothermic
Energy is gained by the system
Chadwick
Discovered the N
Coulombic Attraction
Force of attraction as protons pull electrons inward
Noble Gas
Group 18 on the PT. Each has 8 valence electrons. Nonreactive
Specific Heat
Energy required to raise 1 gram of a substance 1C
System
This refers to the reaction
Melting
Phase change from a solid to a liquid
Limiting Reactant
Reactant to runs out first thus limiting the amount of product that can be formed
Neutron
Neutral particle. No charge. Mass = 1amu, Located in the nucleus
Molality
kg solute / Liter of Solvent
Solvent
The species that does the dissolving to form a solution
Orbital
Regions of probability where electrons are located. Each orbital can contain up to 2 electrons
Solute
The species that gets dissolved to form a solution
Single Bond
One shared pair of electrons
Percent Error
Absolute value (Theoretical - Experimental) / Theoretical) x 100%
Precipitate
Solid matter that forms from the reaction of two aqueous solutions
Proton
Positively charged particle. Charge = +1, Mass = 1amu, Located in the nucleus
Molarity
moles of solute per liter of solution
Sublevel
s, p, d, and f. defines the shape
Hfus
energy required to change 1 mol (s) to (l)
Solution
Solute and solvent
Sublimation
Phase change from a solid to a gas
Transmittance
Light that passes through a solution
Lone Pair
Unbonded electrons
Molecule
Covalently bonded atoms
Valence electrons
Outer electrons which are available for bonding
London Dispersion Forces
Temporary IMF caused by the movement of electrons
Section 3
(50 cards)
Mass Action Expression, Equilibrium Expression
[Products]^coeff / [React]^coeff
Pi Bond
Shared pair of e- above & below the molecule (second and third bond)
Conjugate Acid
What the base becomes after accepting a H+
Alkali
Group I
Immiscible
Solvent and Solute do NOT dissolve completely (oil and water)
Diamagnetic
Not attracted to a magnet (all e- paired)
Dalton's Law of Partial Pressure
P total = P1 + P2 + P3+....
Ka
Acid Equilibrium constant
Granametric Analysis
analytical technique which involves measuring mass
Critical Point
Temp above which the gas cannot be converted back to a liquid
1/2 Equivalence Point
1/2 Acid (or base) has been converted to its conjugate
Molality
Mol solute / kg solvent
Salt
Strong Electrolyte (see vocab)
Triple Point
Point in a Phase Diagram where all three phases are in equilibrium
Graham's Law of Effusion
rate is inversly proportional to the SQRT MM
Sigma Bond
Shared pair of e- between 2 nucei (single and first of double and triple bond)
Ductile
Can be drawn into a wire
Phase Daigram
Conditions of T and P in which a solid, loquid and gas can exist
Equivalence Point
Mol Acid = Mol Base
Quanta
A discreet amount of energy
Metallic Bond
Sea of electrons (delocalized)
Formal Charge
FC= Val e- - [lone pair e- + 1/2 bonded e-]
Kb
Base Equilibrium constant
Lattice Energy
Q1Q2/ r^2
Conjugate Base
What the acid becomes after losing a H+
LeChatelier's Principle
Whan a system at equilibrium is stressed, the rxn will shift to achieve a new equilibrium position
Reaction Mechanism
Series of elementary steps which when added together equals the overall reaction
Vapor Pressure
Pressure that must be achieved by a liquid in a closed container to achieve equilibrium between the liquid and gas phases
Malleable
Can be hammered flat (Mashable)
Enthalpy of Formation, Delta Hf
Energy required to form ONE mole of a substance
Kw
Autoionization of water; Ka x Kb = Kw (1 x 10^-14)
Percent Ionization
Change / originial concentration X 100%
Nonvolatile
Does not have a measurable vapor pressure
Idea Gas
Behaves according to KMT
Molar Solubility , s
mole of ppt that dissolve / liter of solution
Solubility Product, Ksp
Equilibrium constant for the solubility of a solid
Alkaline Earth Metals
Group II
Raoult's Law
Ptotal = XP (A and P are in terms of the solvent)
Amphoteric
Substance that can act as either and acid or a base
Ground State
Aufbau's Law - most stable configuration for electrons
Excited State
Electron(s) can jump to higher energy levels
Rate
Change in Molarity / Change in Time
Rate Determining Step
Slow step in a mechanism - has the same rate law as the overall reaction
Equilibrium Constant, K
[Products]^coeff / [React]^coeff
Van Hoff't Factor (i)
Number of moles of IONS that a compound will dissociated into
Molecularity
Number of moles reacting in an elemenary step
Kinetic Molecular Theory
Gas particles act independently - 4 postulates
Bond Energy
Measure of the strength of a covalent bond
Miscible
Solvent and Solute dissolve completely (water and ethanol)
Paramagnetic
Attracted to a magnet (e- not paired)
Section 4
(4 cards)