pri chem
Terms
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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