456 cards
A/an supercritical fluid is one in which ____.
____ combines enthalpy and entropy into a single value and is used to determine the spontaneity of a reaction.
Gibbs Free Energy combines ____ into a single value and is used to determine the spontaneity of a reaction.
Gibbs Free Energy combines enthalpy and entropy into a single value and is used to determine ____.
If a reaction has a positive ∆H and positive ∆S , then it will be ____ temperatures.
If a reaction has a ____ ∆S , then it will be spontaneous at high temperatures.
If a reaction has a positive ∆H and negative ∆S , then it will be ____ temperatures.
If a reaction has a ____ ∆S , then it will be non-spontaneous at all temperatures.
If a reaction has a negative ∆H and positive ∆S , then it will be ____ temperatures
If a reaction has a ____ ∆S , then it will be spontaneous at all temperatures
If a reaction has a negative ∆H and negative ∆S , then it will be ____ temperatures
If a reaction has a ____ ∆S , then it will be spontaneous at low temperatures
Room temperature is approximately ____
____ temperature is approximately 25°C aka 75°F
Body temperature is approximately ____
____ temperature is approximately 37°C aka 98.6°F
____ is a measure of the potential energy of a system found in intermolecular attractions and chemical bonds .
Enthalpy (H) is a measure of ____ found in intermolecular attractions and chemical bonds .
Enthalpy (H) is a measure of the potential energy of a system found in ____ .
Phase changes from solid → liquid → gas are ____.
Phase changes from ____ are endothermic.
Phase changes from gas → liquid → solid are ____
Phase changes from ____ are exothermic
Give the formula for ∆H when using heat of formations
Give the formula for ∆H when using bond dissociation energies ____
____ is a measure of how much energy has spread out or how spread out energy has become.
Give the formula for the standard entropy of reaction____
Give the Gibbs Free Energy equation that uses the equilibrium constant K eq ____
Give the Gibbs Free Energy equations that use the reaction quotient Q
If ∆G < O, the reaction will be ____.
If ∆G ____ O, the reaction will be spontaneous.
If ∆G = O, the reaction will be ____
If ∆G ____ O, the reaction will be at equilibrium
If ∆G > O, the reaction will be ____
If ∆G ____ O, the reaction will be non-spontaneous
Orbits that are farther the nucleus have ____ energy.
Orbits that are ____ the nucleus have increased energy.
If an electron moves to a farther orbital, a photon is ____.
If an electron moves to a ____ orbital, a photon is absorbed.
If an electron moves to a closer orbital, a photon is ____
If an electron moves to a ____ orbital, a photon is emitted
Ionic bonds have a △EN that is ____.
____ bonds have a △EN that is greater than 1.7.
The orbital hybridization of an atom with 2 electron groups is ____.
The orbital hybridization of an atom with ____ electron groups is sp.
The electronic geometry of an atom with 2 electron groups is ____.
The electronic geometry of an atom with ____ electron groups is linear.
The orbital hybridization of an atom with 3 electron groups is ____.
The orbital hybridization of an atom with ____ electron groups is sp 2 .
The electronic geometry of an atom with 3 electron groups is ____
The electronic geometry of an atom with ____ electron groups is trigonal planar
The orbital hybridization of an atom with 4 electron groups is ____.
The orbital hybridization of an atom with ____ electron groups is sp 3 .
The electronic geometry of an atom with 4 electron groups is ____.
The electronic geometry of an atom with ____ electron groups is tetrahedral.
The orbital hybridization of an atom with 5 electron groups is ____.
The orbital hybridization of an atom with ____ electron groups is sp 3 d.
The electronic geometry of an atom with 5 electron groups is ____.
The electronic geometry of an atom with ____ electron groups is trigonal bipyramidal.
The orbital hybridization of an atom with 6 electron groups is ____.