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Chem Exam 3
Chapters 4-5
Question | Answer |
---|---|
Thermochemistry | Quantitative study of chem reactions involving the transfer of heat |
2 Types of chem reactions | Exothermic and Endothermic |
2 Types of energy | Potential and Kinetic |
Potential | Energy due to position ( stored) |
Kinetic | Energy due to motion |
Chemistry Potential Energy | breaking and making of chemical bonds |
1st Law of thermodynamics | total energy of universe remains constant (Energy can not be created or destroyed but transferred from one form to another) |
7 forms of energy | Mechanical, Radiant/Solar, Sound, Chemical, Heat, Electrical, Nuclear |
Universe equation | System + Surroundings |
Exothermic | Heat(q) exits or Work (w) done by the system |
Endothermic | Heat(q) enters or Work (w) is done on the system |
3 types of systems | Open, Closed, Isolated |
State Functions | properties that are determined by the state o the system, regardless of how the condition was achieved |
4 examples of state function | Energy, Pressure, Volume, Temperature |
What is Temperature | Measure of Hotness |
Absolute Zero | 0K Lowest Possible Temp |
Change of 1 degree Celsius equals | 1 K change |
Heat always moves from | hot (more energetic) to cold (less energetic) |
Thermal Energy | Joules or Cal energy associated with motion of particles |
Heat | Transfer of thermal energy from one place to another collision of particles |
Thermal Energy depends on | how much material you have |
temp depends on | average Kinetic Energy of the particles |
Heat Capacity | amount of heat required to raise the temp by one degree |
Heat capacity is sample size dependent | True |
Specific Heat Capacity | independents sample size |
Calorimetry | the experimental determination of heat flow |
Specific heat with large volume | takes longer to change heat |
Q=m*c*^T | M= mass in grams, c=Specific heat (J/K*G), ^T=change in temp (final- initial) |
Thermochemical Equations | where we deal with 1 mole of product ( reactant fractions) |
^H | change in enthalpy for the reaction that forms 1 mole of a substance from its elements in there standard states |
Hess's Law | if a reaction is carried out in a series of steps, ^H for the reaction equals sum of enthalpy changes |
4 types of Physics | Electricity, Magnetism, Radioactivity, Light |
Frequency (v) | number of waves per second |
higher frequency equals | higher energy |
Visible light | consists of electromagnetic waves |
Electromagnetic Radiation | the emission and transmission of energy in the form of electromagnetic waves |
Electromagnetic Spectrum | Gamma, X-ray, UV, Visible, Infrared, Microwaves, Radar, TV/Radio |
Gamma rays (left) are | Short and Fast with high energy |
TV/Radio Waves are | Long and Slow with Low energy |
Visible Spectrum | ROYGBIV backwards |
Wavelength and frequency of radiant energy | Inversely Related |
Radiational Energy | Proportional to frequency directly |
Light | Both a wave and a particle, result of an excited electron returning to a lower energy level |
Heisenberg Uncertainty Principle | define the energy of an electron exactly but accept limitation that we do not know the exact positions |
Schrodinger's Wave Equation | Describes energy of a given electron, probability of finding an electron in volume of space |
n | energy levels |
l | shape of orbital, volume of space that e- occupies |
ml | orientation off the orbital in space |
l equals | n-1 |
ml numbers | plus or minus l and everything in-between |
2 electrons in the same orbital | they have sake n, l, ml, but deferent ms |
Pauli Exclusion Principle | no 2 electrons in an atom can have the same 4 quantum numbers |
4 Quantum numbers | n, l, ml, ms |
d4 exception | Cr, s level doesnt fill |
d9 exception | doesnt fill s level, Cu |
Zn | completely filled and nonmagnetic |
the more unpaired | the more magnetic |
4 periodic trends | Atomic Size, Ionic Size, Ionization Energy, Electron Affinity |
where is the nucleus | Center of XYZ coordinate |
X-Ray Spectrosapy | indirect measurement, diffraction pattern |
Atomic Radius decreases | left to right where left the biggest |
Z*= | Z-(number of core electrons) |
Atomic Radius Increasing in size | Top to Bottom where bottom the biggest |
Cations | Loose electrons and are smaller than neutral |
Anions | Gain electrons and are bigger than neutral |
Ionization Energy | minimum energy required to remove an electron from a gaseous atom in its grand state |
ionization Energy formula | I1 + X(g)=X+(g)+e- |
what takes more energy | takes more energy to move additional electrons |
Electron Affinity | reflects ability's of an atom to accept one or more electrons, energy charge that occurs when an electron is added to gaseous atom |
Large negative electron affinity | negatives ion is more stable |
11 Gases | H, N, O, F, He, Cl, Ar, Kr, Xe, Rn |
2 liquids | Hg, Br |