pri chem

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a fixed amount: quantum
all orbitals filled unpaired first: Hund's rule
atomic size across a group, atomic size down a period: decreases and increases
atoms emit or absorb energy in quanta; energy of light is quantized as photons: quantum theory
bond found in metals: metallic bond
class of hydrocarbons with a triple bond: alkynes
class of hydrocarbons, contains all single bonds: alkanes
class of hydrocarbons, contains double bond: alkenes
constant value that the mass action expression gives you: equilibrium constant- Keq
Define: Calorimetry: The measurement of heat flow.
Define: Enthalpy: Heat flow in chemical reactions occuring at constant pressure when no forms of work are performed other than P-V work.
Define: Enthalpy of Reaction: The enthalpy change of a reaction. (delta)H=H(products)-H(reactants)
Define: Heat Capacity: The amount of energy required to raisre it's temperature 1 degree C.
Define: Molar heat capacity: The heat capacity of one mol of substance.
Define: Specific Heat Capacity: The heat capacity of 1g of substance.
Define: Standard enthalpy: the enthalpy change when all reactants and products are in their standard state.
Define: The enthalpy of formation: The enthalpy change associated wth the formation of a compund from it's constitutional elements.
Define: Thermochemical Equation: An balanced chemical equation the shows the associated enthalpy change.
Define: Thermochemistry: The relationship between chemical reactions and energy changes involving heat.
Define: Thermodynamics: The study of energy and it's transformations.
effective collisions: collisions must be effective in order for there to be a reaction
Electrons are emitted by metal only if light has freq greater than certain min. value, not matter how intense the light: photoelectric effect
electrostatic force between ions of opposite charge: ionic bond
emission of electrons from metal surfaces on which light shines: photoelectric effect
emission of light from electronically excited gas atoms: emission spectra
emission of light from hot objects: black body effect
energy needed to remove an electron: ionization energy
energy of a photon is what number?: planck's constant 6.606e-34 j s
enthalpy: the change in the amount of heat during a reaction
entropy: S- easure of disorder/measure of randomness
equal sharing of electrons: nonpolar bond
equilibrium: is reached when the rate of the forward reaction equals the rate of the reverse reaction
factors affecting rate of reaction: 1. temp (for every 10 degree incrase,it doubles the rate of reaction
2. concentration-adding particles increases it
3. particle size -larger surface area=faster
4. catalyst- helps orient the molecules5. inhibitor- slows down rate
.: .
force holding atom or ions together: chemical bond
Functional Groups:: Carbon-Carbon Single Bond
: 4. change in temp- an increase in temperature favors teh ENDOthermic reaction
What are Alkanes?: Ex. 2-methylpentane
G: free energy- energy available to do work
gibbs free energy equation: deltaG= deltaH - TdeltaS
If (delta)H is negative, what does that indicate?: The reaction was exothermic.
Inorganic Chemistry: Chemistry of compounds not containing carbon.
is cation or anion smaller?: cation because has same charge but less e, so each e pulled closer
is heat of reaction negative or positive in exothermic: negative
it is inherently impossible for us to know simultaneously both the exact momentum of the e and its exact location in space: uncertainty principle
it takes extra energy to remove an electron when?: when subshell filled or half filled
Keq: equilibrium constant- how far a reversible reaction goes forward
L values correspond to these subshells: 0 s 1 p 2 d 3 f
largest wavelength: radio
Le Chateliers principle: explains how a system at equilibrium responds to relieve any stress on the system
light emitted by excited atoms: line spectra
limitation of the bohr model: can only explain line spectrum for H atom
mass action expression: [C] x [D]
more than one lewis structure for fixed nuclear arrangement: resonance
negative and positive entropy: increasing- +
no two e in an atom can have the same set of four quantum numbers: pauli exclusion principle
organization of periodic table determined by: electron configurations
principal quantum number: n
quantum number, measures orientation: ml
quantum number, measures shape: l
quantum number, measures size: n
quantum number, measures spin: ms
quantum??: a fixed amount
rate determining step: the one that happens the slowest (only as fast as the slowest part)
region of space with size, shape, characteristic energy: orbitals
rutherford experiment: shot particles at gold foil, discovered the nucleus
said energy can only be released or absorbed by atoms only in discrete chunks of some minimum size: planck
shape of d orbital number 5: 5 shapes
shape of p orbital number 3: dumbbell
shape of s orbital number 1: spherical
sharing of electrons between two bonded atoms: covalent bond
smallest wavelength: gamma rays
stress: any change in temp, concentration, or pressure on an equilibrium system
tendency of an atom to attract electrons to itself in a bond: electronegativity
these control the chemistry of the elements: valence electrons
these electrons are more easily removed, outer or inner: outer
this is the purest covalent bond: between two identical atoms
unequal sharing of electrons: polar bond
what 2 things make collisions effective: 1. adequate rate
What are Alcohols?: Carbon-Oxygen Hydrogen Bond
What are Aldehydes?: A double bonded Oxygen bonded to just one carbon, on one side. (Hydrogen may be on other side)
What are Alkenes?: (Olefins)
What are Alkynes?: Carbon---Carbon Triple bond
What are Amides?: A double bonded Oxygen bonded to just one carbon, on one side, a nitrogen on the other side bonded to two carbons. (carbon could be a hydrogen)
What are Amines?: A Nitrgoen being bonded to Carbon or hydrogen
What are Aromatics?: (Arenes)
What are Carboxylic Acids?: A double bonded Oxygen bonded to just one carbon, on one side and an OH group on the other side.
What are Esters?: A double bonded Oxygen bonded to just one carbon, on one side and an oxygen bonded to a carbon on the other side.
What are Ethers?: Carbon-Oxygen-Carbon bond
What are Haloalkanes?: Alkyl halides,
What are Ionic Bonds?: Formed by the transfer of one or more electrons from one atom to another to create ions (ionic bonds are formed between metal and a non-metal).
What are Ketones?: A double bonded Oxygen bonded to just two carbons, one on each sides.
What are oxidation numbers?: They are assigned to atoms in order to keep track of the redistribution of electrons during a chemical reaction
What are the 4 quantum numbers?: n(principle quantum #): 0 to infinity
what different kinds of stress can you put on equilibrium and what are the affects: 1. change in pressure- if you increase the pressure, it will shift towards the side with less moles
What does a salt bridge do?: A salt bridge allows the charge gradient to be dissipated, which permits the exchange of cations and anions
What does a salt bridge usually contain?: It usually contains an inert electrolyte, usually KCL or NH4NO3, whose ions will not react with the electrodes or with the ions in solution
What does Hess's Law State?: If a reaction is carried out in a series of steps, (delta)H for te reaction will equal the sum of the enthalpy changes for the individual steps.
What does the law of conservation of charge say?: It says that an electrical charge can be neither created nor destroyed
What does this law imply about oxidation and reduction?: An isolated loss or gain of electrons cannot occur, but they must occur simultaneously, resulting in an electron transfer called a redox reaction
what happens to energy as bonds are formed?: energy is released
What is a covalent bond?: A bond that is formed when the two atoms share electrons (covalent bonds are formed between non-metals).
What is a reducing agent?: It causes the other atom to be reduced, and is it oxidized
What is an orbital?: A region of space where the probabilty of finding an electron is large.
What is an oxidizing agent?: It causes another atom in a redox reaction to under oxidation, and is itself reduced
What is Aufbau Principle?: Orbitals are filled up so that those of lowest energy are filled first.
What is Hund's Rule?: When we come to orbitals of equal energy (degenrate orbital) such as the three "p" orbital, we add one electron to each with their spins unpaired until each degenerate orbital contains one electron, then, we begin adding a second electron to each degenerate orbital so that the spins are paired.
What is Organic Chemistry?: Chemistry of compounds containing carbon.
What is oxidation?: The loss of electrons
What is reduction?: The gain of electrons
What is the Heinsenburg Uncertainty principle?: We CANNOT know simultaneously the position and momentum of an electron. That is, we cannot pin down the electrons as precisely as our explanation suggests.
What is the Octet Rule?: Bonded atoms tend to possess or share a total of eight valence-shell electrons.
what is the only thing that can change the value of Keq: temp
What is the Pauli Exclusion Principle?: No two electrons can have the same four quantum #'s!!
What is the simplest organic compound?: Methane: CH4
What is the symbol for enthalpy?: H
what Keq FAVORS the products: when it is GREATER THAN 1
what keq favors the reactants: when it is LESS THAN 1
when do pressure changes not have an effect on the rate of reaction: when only solids and liquids are involveed
when is G equilibrium: when delta G is zero
when is G improbable: when delta G is prositive
when is G spontaneous: when delta G is negative
Which direction do electrons flow?: They flow from the anode through the wire and the voltmeter toward the cathode

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