Friday, March 27, 2020

How to Win in Monopoly an Example by

How to Win in Monopoly The complexity of the economy of the real world makes even the most expert economist scratch their heads. That is just one reason why the board game Monopoly is such a popular game among any age group. As the title of the game suggests, it also feeds one of the darkest of human intentions, which is to monopolize everything. In the context the game, there is nothing more satisfying than seeing your playmates cling unto their last dollar and worship you for your economic dominance-the sad part is it is only a game. But the question that should be asked is: how does a player get the majority of the property cards and have large amounts of cash that even the baker would envy? Need essay sample on "How to Win in Monopoly" topic? We will write a custom essay sample specifically for you Proceed The first step would be familiarizing oneself to the rules of the game. Monopoly is a brutal and an unforgiving board game. Those who are already familiar with the game are like sharks that can smell blood. They can sense whether a player is just a novice. And if a player had joined the game without being familiar with the rules-that player must prepare oneself to be bullied...in a board-game context. Read the rulebook first and know the nature of the game, from there you could strategize. University Students Frequently Tell EssayLab support:Who wants to write essay for me?Specialists recommend: If You Think About Someone To Write Your Paper - Essaylab The Right Place!Help Write Essay Services Get Paid To Write Papers How to Make Assignment College Essay Writing Service It would be very helpful if a player would not get upset in the entire course of the game. The player should remember that Monopoly is a game that is based on luck-perhaps the two size-sided dice and the "chance cards" would remind us of that fact. Do not get frustrated if you do not land on Park Lane even if you wished it on a falling star. No one can tell the roll of the dice unless a player is a mutant or something. Moreover, being frustrated would only distract you from your strategy. And of course, approaching the game with a little dose of intellect would not hurt. It would always pay to smart in any game, even in life. You really tell whether a person have difficulty in handling money when he or she is always going bankrupt in Monopoly. A proven effective way of playing smart Monopoly is spending the money wisely. Smarting spending in Monopoly would mean constant purchasing of available properties. Again, do not wait until you land on expensive properties such as Park Lane. I would reiterate that Monopoly is a game of luck, the company that had published the game even states that in the manual. There would be two main reasons why a player should buy properties when they have the chance. First is that purchasing one could lead a player to purchasing all the properties of the same color. Your opponents would kneel down to you if you have purchased all of the same color group as you can charge them double rent. Second is that it simply prevents the other players from having the chance to charge you with double rent-simple. May I just add that the money in Monopoly is not real after all. Do not be afraid to spend fake money, but still spend it wisely or else you would be subject to oppression from other players, but only during the duration of the game. To boost your chances of winning the game, you could learn probabilities-but the technical stuff strips the game of the fun. It is already a logically-winning-inclined situation if a player would play the game wisely. So if you would soon play Monopoly, you must remember to know the rules, know the nature of the game, and be wise, do not talk to the dice, just monopolize. Reference Hasbro.com. Monopoly. Retrieved 13 May 2008 http://www.hasbro.com/games/kid- games/monopoly/default.cfm?page=StrategyGuide/Rules/rules_payingrent

Friday, March 6, 2020

Chem 17 Reviewer (1st Exam) Essays

Chem 17 Reviewer (1st Exam) Essays Chem 17 Reviewer (1st Exam) Essay Chem 17 Reviewer (1st Exam) Essay CHEMISTRY 17 1ST LONG EXAM REVIEWER I. ELECTRONIC STRUCTURE OF ATOMS -arrangement of atoms’ electrons -the number of electrons in an atom -distribution of electrons around the nucleus and their energies ATOMS *Billiard Ball Model (JOHN DALTON) *Plum Pudding Model (JOSEPH J. THOMPSON) *RUTHERFORD’s Model of Atom -atoms are tiny, hard, indivisible spheres -electrons (negative charge) occupy the atom Atom is mostly empty space with a dense nucleus PROBLEMS with Rutherford’s Model According to laws of physics, Rutherford’s atom should collapse *The model CANNOT explain differences in properties of elements *The model CANNOT explain the colors emitted by elements when heated A. THE QUANTUM MODELS (WAVE) -formed through studies about light DESCRIBING ELECTROMAGNETIC WAVE *Wavelength (? †lambda†) -distance between two adjacent peaks or troughs (m) *Frequency (? †nu†) number of cycles(complete wavelengths) that pass a given point each sec ond (Hz or /s) **Wavelength is inversely proportional to frequency. Where: c= 3. 00 x 10? m/s B. QUANTIZED ENERGY AND PHOTONS Blackbody Radiation oPerfect absorber and emitter of light oAt high temperature, solids emit radiation oRadiation depends on the temperature not in the element the solid is made from. oPREDICTION: â€Å"As temperature increases, the frequency of light emitted also increases. † oOBSERVATION: There was a peak. Photoelectric Effect and Photons oWhen a beam of light shines on a certain surface (e. g. some metals), electrons are ejected. oThe effect is instantaneous. PREDICTION: †It will take time for effect to be observed†; â€Å"and light will produce the effect, given enough time† oOBSERVATION: Effect is instantaneous. There is a minimum frequency of light needed to produce the effect. o**†If frequency of light is below a certain value called the threshold frequency, the number of electrons will be ejected. † o**†If i ntensity of light is increased, flow of current also increases. † QUANTUM THEORY (Max Planck *1858-1947*) oQuantum (fixed amount) – smallest quality oEach particle corresponds to certain energy. Planck proposed that the minimum amount of radiant energy that can gain or lose is related to the frequency of radiation. o†Radiation consists of packets/quantum of energy (PHOTONS *name given by G. N. Lewis*). † oQuantum Theory: â€Å"Energy is quantized. It can only have certain allowed values. † oEnergy of radiation is proportional to the frequency of radiation. Higher frequency ? More energy; Lower wavelength ? More energy oMonochromatic light consists of photons with the same frequency or same energy. oIntensity of the light depends on the number of photons emitted per second. Einstein’s Explanation on the Photoelectric Effect Light consisting of energy packets hit the metal and their energy is absorbed by the electrons. oOne packet of energy (phot on) hits the metal surface, one electron is emitted. oIf energy of a bundle is not enough, it will not be able to dislodge electron from the attraction of the atomic nuclei. No photoelectric effect. oIf energy of a bundle is enough (equal to the threshold energy). It will dislodge an electron from the attraction of the atomic nuclei. oEnergy in excess of energy to dislodge electron (in excess of the threshold energy) becomes kinetic energy of the electron. Higher energy/ frequency of light ? more excess energy ? Higher kinetic energy of electron C. LINE SPECTRA AND THE BOHR MODEL Line Spectra oMonochromatic radiation is composed of single wavelength. oSpectrum is produced when radiation from light is separated into different wavelength components. oContinuous spectrum ?ROYGBIV, containing light of all wavelength oLine spectrum ?Spectrum containing radiation of only specific wavelengths Bohr’s Model (Spectra of Hydrogen Atom) oAssumed that electron move in circular orbits arou nd the nucleus oPOSTULATES: Only orbits of certain radii, corresponding to certain definite energies, are permitted for the electron in a hydrogen atom. ?An electron in a permitted orbit has a specific energy and is in an allowed energy state. An electron in an allowed energy state will not spiral into the nucleus. ?Energy is transmitted or absorbed by the electron only as the electron changes from one allowed energy state to another. This energy is emitted or absorbed as a photon, E= h?. For electron to move farther from the nucleus, it needs more potential energy. oDistance from the nucleus of an allowed orbit, n. Energy of the electron in the allowed orbit, n. oApplications ?Fireworks ?Use of emission spectroscopy to analyse for the presence of elements. Success of Bohr Model oIt successfully predicted the frequencies of the lines in the hydrogen spectrum oIt introduced the concept of discrete energy levels of electron in atoms and the first quantum number, n. oThe model failed to predict energy levels for atoms with more than 1 electron. (if 2/more electrons are present, the electrons repel) D. THE WAVE BEHAVIOR OF MATTER Louis de Broglie (1892-1987) â€Å"Depending on the experimental circumstances, radiation appears to have either a wavelike or a particle-like (photon) character. † o**As the electron moves about the nucleus, it is associated with a particular wavelength. The characteristic wavelength of the electron, or of any particle, depends on its mass, m, and moving at speed, v. oThe quantity mv for any object is its momentum. oMatter waves, wave characteristic of material particles. oThis hypothesis is found to be applicable to all matter; any object of mass and velocity would give rise to a characteristic matter wave. Uncertainty Principle -There is an inherent uncertainty in the precision with which we can simultaneously specify the position and momentum of a particle. This uncertainty is significant only for particles of extremely small mass, such as electrons. oWerner Heisenberg (1901-1976) ?â€Å"The dual nature of matter places a fundamental limitation on how precisely we can know both the location and the momentum of any object. The limitation becomes important only when we deal with matter at the subatomic level (that is with masses as small as that of an electron). † E. QUANTUM MECHANICS AND ATOMIC ORBITALS Erwin Schr? dinger (1887-1961) oQuantum physics opened a new treatment of atoms, electrons, ions and molecules: by describing it mathematically oUsed Broglie’s hypothesis that electrons can be described as a wave. oSolutions to the equation are called wave functions (energy state of an atom). ?WAVE FUNCTIONS: ?Only certain wave functions are allowed. An electron can only have certain energy states: the energy of the electron is quantized. ?They are called orbitals. ?Its square (? ) is called either probability density or the electron density. Mathematical description of a region in space where an electron has some probability of being found. ?Each wave function (or each energy state/orbital) is characterized by a set of 3 quantum numbers: n, l, ml oSchr? dinger’s theory chose to define the energy of the electron precisely. Therefore, according to the uncertainty principle, this would result in a large uncertainty finding the locatio n of the electron. oWhen the Schr? dinger’s equation for the H-atom is solved, the resulting wave functions contain 3 integral numbers called quantum numbers. Orbitals and Quantum Numbers oWhat for? ?Solutions to wave equations given ?Energy of electron ?Probable location of electron ?Identify an orbital oTo identify an orbital, we use THREE quantum numbers. oTo describe an electron, we use FOUR quantum numbers. Principal Quantum Number (n) a. n defines a main energy level or a principal shell b. the size of orbital and energy of orbital depends mainly on n c. As n increases, there will be higher energy of electrons and the farther is the distance of the electron from the nucleus. Azimuthal Quantum Number (l) a. Each value of l defines a type of sublevel or subshell, or an orbital type. b. Thus, we speak of op sublevel/ p orbitals od sublevel/ d orbitals c. Allowed values: positive integer values (from O ? (n-1)) d. Orbitals and sublevels are designated by letters. e. Determines the shape of the orbital. Value of l012345 Letter designatedspdfgh Magnetic Quantum Number (ml) a. Describe the 3D orientation of the orbital b. Gives the number of orbitals in a given substance c. Orbitals in some sublevel have same energy but differ in orientation in space called degenerate orbitals. . Value depends on l. e. Allowed values from –l to +l. Spin Quantum Number (ms) a. Pauli Exclusion Principle oNo 2 electrons in the same atom can have exactly same energy. b. Energies of orbital for H-atom. oFor 1 electron H-atom, orbitals on the same energy level have same energy. They are degenerate. oEnergy of the orbitals of H-atom depends only on the principal quantum number, n. oEnergies of Orbitals As num ber of electron increase, so do the repulsion interactions among them. oSubshells in a Principal Shell have different energies: s