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49 Cards in this Set
- Front
- Back
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Bonus Question: The scientists at Crayola discovered a new method to determine the energy content of their new crayons. They called the new device a _________.
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colorimeter
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The chemist could not get chemical terminology out of his brain. When he was asked to determine the concentration of small mountains in the region, he decided to call it _______.
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hillarity
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What is the definition of energy?
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The ability to do work or transfer heat.
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______ is when energy is used to cause an object that has mass to move.
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Work
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What is the definition of heat?
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Energy used to cause the temperature of an object to rise.
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Define: P.E.
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Energy an object possesses by virtue of its position or chemical composition.
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Define: K.E.
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Energy an object possesses by virtue of its motion.
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The formula for K.E. is _______.
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KE= V(sub 2)mv(superscript 2)
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The SI unit of energy is the ______ (word not symbol).
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Joules
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One J is equal to _______.
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1 Kgm(superscript 2) / sec (superscript 2)
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An older non-SI unit still used is the ________, which is equal to ________J.
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calorie (cal); 4.184 J
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The formula for work is _______. (explain each symbol)
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w= f x d
(w= work, f= force, d= distance) |
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In chemistry, the most common way to measure energy is by measuring the change in ________.
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temperature
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What is the first law of Thermodynamics?
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Energy is neither created nor destroyed.
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The _______ _______ of a system is the sum of all kinetic and potential energies of all components of the system. Its symbol is _____.
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internal energy; E
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ΔE is equal to ________ (equation).
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E(subscript final) - E(subscript initial)
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ΔE can also be expressed as _______ (equation).
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q + w
(heat + work) |
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When heat is _______ by the system from the surroundings the process is endothermic.
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absorbed
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When heat is _______ by the system to the surroundings the process is exothermic.
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released
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The internal energy of a system is a state function because it is ________ of the path by which the system achieved that state.
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independent
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The thing that students hate to do is called work. It can be expressed in terms of pressure and volume by the equation ________.
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W= - PΔV
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______ (word and symbol) is the internal energy plus the product of pressure and volume.
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Enthalpy (H)
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When the system changes at constant pressure, the change is known as _______ and can be written as _______ (equation).
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ΔH; ΔH= Δ(E + PV)
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If ΔH is negative, then the reaction is _______.
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exothermic
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If ΔH is positive, then the reaction is _______.
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endothermic
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Calorimetry is the experimental science for measuring the _______ ______ _______.
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flow of heat
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The amount of energy required to raise the temperature of a substance by 1K (1 degree C) is its _______ _______.
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heat capacity
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Specific heat is equal to the ______ ______ over the ______ times _______ ______.
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heat transferred; mass; temperature change.
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Hess' law states that if a reaction is carried out in a series of steps, ΔH for the overall reaction will be equal to the sum of the ______ ______ for the individual steps.
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enthalpy changes
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Standard enthalpies of formation ΔH(degree sign)(subscript f) are measured under standard conditions which are ______ degrees and ______ pressure.
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25(degrees) C; 1 atm
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Two important properties of waves are their ______ and ______ (words and symbols).
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wavelengths (λ); frequency (f)
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______ concluded that energy is proportional to ______ the equation is defined by E=hv.
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Einstein; frequency
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h is equal to _______'s constant which numerically is _______.
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Planck; 6.63 x 10 (superscript -34) J/s
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de Broglie demonstrated that the relationship between mass and wavelength was _______(equation).
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λ=h/mv
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(Δx)(Δmv) is greater than or equal to h/4π is known as _______ _______ _______.
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Heisenberg's Uncertainty Principle.
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Erwin Schrodinger developed a mathematical treatment that took into account both the wave and particle nature of matter which became known as _______ _______.
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quantum mechanics.
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An orbital is described by a set of quantum numbers which are:
the _______ quantum number, abbreviated ______. the _______ quantum number, abbreviated ______. the _______ quantum number, abbreviated ______; and finally the the _______ quantum number, abbreviated ______. |
-Principle, n
-Azimuthal, l -Magnetic, m (subscript l) -Spin, m (subscript s) |
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The word "degenerate" when referring to energy means that the orbitals have the ______ ______.
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same energy.
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No two electrons in the same atom can have exactly the same energy; this is known as the ______ ______ ______.
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Pauli Exclusion Principle.
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Given: 5d (superscript 7)
Question: 5 stands for the ______ ______. d stands for the ______ and 7 stands for the ______ ______ ______. |
energy level; orbital; number of electrons.
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For electron box diagrams, each box represents ______ ______, half-arrows represent ______ and the direction of the arrow represents the ______ of the electron.
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one orbital; electrons; spin
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For degenerative orbitals, the lowest energy is attained when the number of electrons with the same spin is ______. This is known as ______ _____.
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maximized; Hund's Rule.
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In a chemical reaction, if there is more of one reactant than necessary, that reactant is said to be ______ ______. The other reactant is known as the ______ ______ and is used in all molar calculations.
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in excess; limiting reagent
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Solutions are ______ mixtures of two or more pure substances.
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homogeneous
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The dissolving medium is called the ______ while the chemical dissolved is known as the ______.
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solvent; solute.
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______ occurs when an ionic substance dissolves in water.
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Dissociation
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Give six examples of strong acids.
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- HCl
- HBr - HI - H(subscript 3)PO(subscript 4) - H(subscript 3)SO(subscript 4) - H(subscript 2)SO(subscript 4) |
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Give five examples of strong bases.
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- LiOH
- NaOH - KOH - Ca(OH)(subscript 2) - Ba(OH)(subscript 2) |
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If sulfuric acid reacted with lithium hydroxide, specifically what kind of reaction would take place?
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neutralization reaction
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