The Prison-Industrial Complex

Is prison overcrowding a vexing problem or a tempting opportunity? It depends on whether you see the  nearly 2  million Americans locked in prison cells  as  a  tragic  collection of misspent lives or a  vast self-sustaining supply of cheap labor. To be sure, the growing prison-industrial complex, for better or worse, views the inmate population as the latter. Derived from the  Cold War-era  term â€Å"military-industrial complex,† the term â€Å"prison-industrial complex† (PIC) refers to a combination of private-sector and government interests that profit from  increased  spending on prisons, whether it is truly justified or not. Rather than a covert conspiracy, the PIC is criticized as a convergence of self-serving special interest groups that openly encourage new prison construction, while discouraging the advancement of reforms intended to reduce the inmate population. In general, the prison-industrial complex is made up of: Politicians who play on fear by running on â€Å"get tough on crime† platforms.State and federal  lobbyists  who represent prison industries and the companies that profit from cheap prison labor.Depressed rural areas that depend on prisons for their economic survival.Private  companies that view the  $35 billion spent each year on corrections  as creating a lucrative market, rather than imposing a drain on taxpayers. Influenced by prison industry lobbyists, some members of Congress may be persuaded to press for  harsher federal sentencing laws  that will send more non-violent offenders to prison, while opposing prison reform and inmate rights legislation. Prison Inmate Jobs   As the only Americans not protected from slavery and forced labor by the  Thirteenth Amendment  to the U.S. Constitution, prison inmates have historically been required to perform  routine prison maintenance jobs. Today, however, many inmates take part in work programs that make products and provide services for the private sector and government agencies. Typically paid far below the  federal minimum wage, inmates now build furniture, make clothing, operate telemarketing call centers, raise and harvest crops, and produce  uniforms for the U.S. military. For example, the signature line of jeans and t-shirts Prison  Blues  is produced by inmate-workers at the Eastern Oregon Correctional Institute. Employing more than 14,000 inmates nationwide, one government-managed prison labor agency produces equipment for the U.S. Department of Defense. Wages Paid to Inmate Workers   According to the U.S. Bureau of Labor Statistics (BLS), inmates in prison work programs earn from 95 cents to $4.73 per day. Federal law allows the prisons to deduct up to 80% of their wages for taxes, government programs to assist crime victims, and the costs of incarceration. Prisons also deduct small amounts of money from inmates required to pay child support. In addition, some prisons deduct money for mandatory savings accounts intended to help convicts become re-established in the free community after their release. After deductions, participating inmates netted about $4.1 million of the $10.5 million total wages paid by prison work programs from April to  June  2012, according to the BLS. In privately-run prisons, inmate workers typically make as little as 17 cents per hour for a six-hour day, a total of about $20 per month. As a result, inmate workers in federally-operated prisons find their wages quite generous. Earning an average of $1.25 an hour for an eight-hour day with occasional overtime, federal inmates can net from $200-$300 per month. The Pros and Cons   Proponents of the prison-industrial complex argue that rather than unfairly making the best of a bad situation, prison work programs contribute to the inmates’ rehabilitation by providing job training opportunities. Prison jobs keep inmates busy and out of trouble, and money generated from the sales of prison industries products and services help maintain the prison system, thus easing the burden on taxpayers. Opponents of the prison-industrial complex  contend  that the typically low-skill jobs and minimal training offered by prison work programs simply do not prepare inmates to enter the workforce in the communities to which they will eventually return after their release. In addition, the growing trend toward privately-operated prisons has forced states to pay for the cost of contracts for outsourced incarceration. Money deducted from wages paid to inmates goes to increase the profits of the private prison companies rather than decreasing the cost of incarceration to taxpayers. According to its critics, the effect of the prison-industrial complex can be seen in the stark statistic that while the violent crime rate in the  United States has fallen by about  20% since 1991, the number of inmates in U.S. prisons and jails has grown by 50%. How Businesses View Prison Labor   Private sector businesses that use inmate workers profit from significantly lower labor costs. For example, an Ohio company that supplies parts to Honda pays its prison workers $2 an hour for the same work regular union  auto  workers  are paid $20 to $30 an hour. Konica-Minolta pays its prison workers 50 cents an hour to repair its copiers. In addition, businesses are not required to provide benefits like vacations, health care, and sick leave for inmate workers. Similarly, businesses are free to hire, terminate, and set pay rates for inmate workers without the collective bargaining limitations often imposed by  labor unions. On the downside, small businesses often lose manufacturing contracts to prison industries because they are unable to match the low production costs of a vast pool of low-paid convict workers. Since 2012, several small companies that had historically produced uniforms for the U.S. military have been forced to lay off workers after losing contracts to UNICOR, a government-owned prison labor program. Civil Rights Civil rights groups argue that the practices of the prison-industrial complex  lead to the building, expanding prisons mainly for the purpose of creating employment opportunities utilizing prisoner labor at the expense of the inmates themselves. For example, the American Civil Liberties Union (ACLU) contends that the prison-industrial complex’s drive for profit through privatization of prisons has actually contributed to the continued growth of America’s prison population. In addition, the ACLU argues that the construction of new prisons solely for their profit potential will ultimately  result  in  the often unjust and lengthy imprisonment of  millions  of additional  Americans, with a disproportionately high number of the poor and people of color being jailed.

The Better Morality Kant and Aristotle on Happiness

Immanuel Kant and Aristotle agree that all rational beings desire happiness and that all rational beings at least should desire moral righteousness. However, their treatments of the relationship between the two are starkly opposed. While Aristotle argues that happiness and morality are nearly synonymous (in the respect that virtue necessarily leads to happiness), Kant claims that not only does happiness have no place in the realm of morality, but that a moral action usually must contradict the actor’s own inclination toward happiness. Because Kant and Aristotle hold practically equal definitions of happiness, the difference must arise from the respective relationships between happiness and each author’s framework of morality. Because Kant†¦show more content†¦Likewise, Kant says that there is no reliable concept of happiness (4:399) and that we can only infer the objects related to happiness through experience, which is inherently misleading as a source of trut h (4:418). Lastly, both philosophers believe that happiness relies on reason. As previously discussed, Aristotle’s conception of the path to happiness depends entirely on our use of reason to conduct virtuous activity. And although Kant says that reason distances us from happiness (4:395), I argue that reason and science have raised our standard of living throughout history. Does he really believe that the cavemen huddling around fires were happier than the healthier, longer-living and more enlightened modern man? Furthermore, reason gives us the tools to pursue wealth and power, whose category he labels as happiness. Lastly, he specifically calls happiness â€Å"Power, riches, honor, even health, and the entire well-being and contentment with one’s condition† (4:393). Self-awareness is a faculty of cognizance, and thus to be â€Å"content with one’s condition† requires some level of reason. Thus, as I have shown, Kant’s and Aristotleâ€℠¢s definitions of happiness are equal: both require fortune, neither is universal, and both require reason. If both philosophers define happiness in equal terms, yet treat it in opposite manners, then the difference must arise in theirShow MoreRelatedComparing Aristotle And John Stuart Mill1130 Words   |  5 PagesEthics 28 April 2015 Essay 2 Comparisons on Pleasure in Morality The role of pleasure in morality has been examined thoroughly throughout the beginning of philosophy and continues to be a questionable issue. With these in-depth examinations, some similar outlooks as well as differing views have been recorded. Many philosophers have dissected this important topic, however I intend to concentrate of the famous works of Aristotle, Immanuel Kant, and John Stuart Mill. 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Physical Properties and Reactions free essay sample

These pages explain the relationship between the physical properties of the oxides of Period 3 elements (sodium to chlorine) and their structures. Argon is obviously omitted because it doesnt form an oxide. A quick summary of the trends The oxides The oxides well be looking at are: |Na2O |MgO |Al2O3 |SiO2 |P4O10 |SO3 |Cl2O7 | | | | | |P4O6 |SO2 |Cl2O | Those oxides in the top row are known as the highest oxides of the various elements. These are the oxides where the Period 3 elements are in their highest oxidation states. In these oxides, all the outer electrons in the Period 3 element are being involved in the bonding from just the one with sodium, to all seven of chlorines outer electrons. The structures The trend in structure is from the metallic oxides containing giant structures of ions on the left of the period via a giant covalent oxide (silicon dioxide) in the middle to molecular oxides on the right. Melting and boiling points The giant structures (the metal oxides and silicon dioxide) will have high melting and boiling points because a lot of energy is needed to break the strong bonds (ionic or covalent) operating in three dimensions. The oxides of phosphorus, sulphur and chlorine consist of individual molecules some small and simple; others polymeric. The attractive forces between these molecules will be van der Waals dispersion and dipole-dipole interactions. These vary in size depending on the size, shape and polarity of the various molecules but will always be much weaker than the ionic or covalent bonds you need to break in a giant structure. These oxides tend to be gases, liquids or low melting point solids. Electrical conductivity None of these oxides has any free or mobile electrons. That means that none of them will conduct electricity when they are solid. The ionic oxides can, however, undergo electrolysis when they are molten. They can conduct electricity because of the movement of the ions towards the electrodes and the discharge of the ions when they get there. The metallic oxides The structures Sodium, magnesium and aluminum oxides consist of giant structures containing metal ions and oxide ions. Melting and boiling points There are strong attractions between the ions in each of these oxides and these attractions need a lot of heat energy to break. These oxides therefore have high melting and boiling points. Electrical conductivity None of these conducts electricity in the solid state, but electrolysis is possible if they are molten. They conduct electricity because of the movement and discharge of the ions present. The only important example of this is in the electrolysis of aluminum oxide in the manufacture of aluminum. Whether you can electrolyze molten sodium oxide depends, of course, on whether it actually melts instead of subliming or decomposing under ordinary circumstances. If it sublimes, you wont get any liquid to electrolyze! Magnesium and aluminum oxides have melting points far too high to be able to electrolyze them in a simple lab. Silicon dioxide (silicon(IV) oxide) The structure The electronegativity of the elements increases as you go across the period, and by the time you get to silicon, there isnt enough electronegativity difference between the silicon and the oxygen to form an ionic bond. Silicon dioxide is a giant covalent structure. There are three different crystal forms of silicon dioxide. The easiest one to remember and draw is based on the diamond structure. Melting and boiling points Silicon dioxide has a high melting point varying depending on what the particular structure is (remember that the structure given is only one of three possible structures), but they are all around 1700 °C. Very strong silicon-oxygen covalent bonds have to be broken throughout the structure before melting occurs. Silicon dioxide boils at 2230 °C. Because you are talking about a different form of bonding, it doesnt make sense to try to compare these values directly with the metallic oxides. What you can safely say is that because the metallic oxides and silicon dioxide have giant structures, the melting and boiling points are all high. Electrical conductivity Silicon dioxide doesnt have any mobile electrons or ions so it doesnt conduct electricity either as a solid or a liquid. The molecular oxides Phosphorus, sulphur and chlorine all form oxides which consist of molecules. Some of these molecules are fairly simple others are polymeric. We are just going to look at some of the simple ones. Melting and boiling points of these oxides will be much lower than those of the metal oxides or silicon dioxide. The intermolecular forces holding one molecule to its neighbors’ will be van der Waals dispersion forces or dipole-dipole interactions. The strength of these will vary depending on the size of the molecules. None of these oxides conducts electricity either as solids or as liquids. None of them contains ions or free electrons. The phosphorus oxides Phosphorus has two common oxides, phosphorus (III) oxide, P4O6, and phosphorus (V) oxide, P4O10. Phosphorus (III) oxide (tetraphosphorus hexoxide) Phosphorus (III) oxide is a white solid, melting at 24 °C and boiling at 173 °C. The phosphorus is using only three of its outer electrons (the 3 unpaired p electrons) to form bonds with the oxygens. Phosphorus (V) oxide (tetraphosphorus decoxide) Phosphorus (V) oxide is also a white solid, subliming (turning straight from solid to vapour) at 300 °C. In this case, the phosphorus uses all five of its outer electrons in the bonding. Solid phosphorus(V) oxide exists in several different forms some of them polymeric. We are going to concentrate on a simple molecular form, and this is also present in the vapour. This is most easily drawn starting from P4O6. The other four oxygens are attached to the four phosphorus atoms via double bonds. [pic] The sulphur oxides Sulphur has two common oxides, sulphur dioxide (sulphur (IV) oxide), SO2, and sulphur trioxide (sulphur (VI) oxide), SO3. Sulphur dioxide Sulphur dioxide is a colourless gas at room temperature with an easily recognized choking smell. It consists of simple SO2 molecules. [pic] The sulphur uses 4 of its outer electrons to form the double bonds with the oxygen, leaving the other two as a lone pair on the sulphur. The bent shape of SO2 is due to this lone pair. Sulphur trioxide Pure sulphur trioxide is a white solid with a low melting and boiling point. It reacts very rapidly with water vapour in the air to form sulphuric acid. That means that if you make some in the lab, you tend to see it as a white sludge which fumes dramatically in moist air (forming a fog of sulphuric acid droplets). Gaseous sulphur trioxide consists of simple SO3 molecules in which all six of the sulphurs outer electrons are involved in the bonding. [pic] There are various forms of solid sulphur trioxide. The simplest one is a trimer, S3O9, where three SO3 molecules are joined up and arranged in a ring. The fact that the simple molecules join up in this way to make bigger structures is what makes the sulphur trioxide a solid rather than a gas. The chlorine oxides Chlorine forms several oxides. Here we are just looking at two of them – chlorine (I) oxide (dichlorine monoxide), Cl2O, and chlorine (VII) oxide (dichlorine heptoxide), Cl2O7. Chlorine (I) oxide (dichlorine monoxide) Chlorine (I) oxide is a yellowish-red gas at room temperature. It consists of simple small molecules. [pic] Theres nothing in the least surprising about this molecule and its physical properties are just what you would expect for a molecule this size. Chlorine (VII) oxide (dichlorine heptoxide) In chlorine (VII) oxide, the chlorine uses all of its seven outer electrons in bonds with oxygen. This produces a much bigger molecule, and so you would expect its melting point and boiling point to be higher than chlorine (I) oxide. Chlorine (VII) oxide is a colourless oily liquid at room temperature. The diagram has been drawn as a standard structural formula for simplicity. In fact, the shape is tetrahedral around both chlorines, and V-shaped around the central oxygen. [pic] PROPERTIES OF THE PERIOD 3 CHLORIDES This page looks at the structures of the chlorides of the Period 3 elements (sodium to sulphur*), their physical properties and their reactions with water. Chlorine and argon are omitted chlorine because it is meaningless to talk about chlorine chloride, and argon because it doesnt form a chloride. A quick summary of the trends The chlorides The chlorides well be looking at are: |NaCl |MgCl2 |AlCl3 |SiCl4 |PCl5 |S2Cl2 | | | | | |PCl3 | | As you will see later, aluminum chloride exists in some circumstances as a dimer, Al2Cl6. The structures Sodium chloride and magnesium chloride are ionic and consist of giant ionic lattices at room temperature Aluminum chloride and phosphorus (V) chloride are tricky! They change their structure from ionic to covalent when the solid turns to a liquid or vapour. There is much more about this later on this page. The others are simple covalent molecules. Melting and boiling points Sodium and magnesium chlorides are solids with high melting and boiling points because of the large amount of heat (energy) which is needed to break the strong ionic attractions. The rest are liquids or low melting point solids. Leaving aside the aluminum chloride and phosphorus (V) chloride cases where the situation is quite complicated, the attractions in the others will be much weaker intermolecular forces such as van der Waals dispersion forces. These vary depending on the size and shape of the molecule, but will always be far weaker than ionic bonds. Electrical conductivity Sodium and magnesium chlorides are ionic and so will undergo electrolysis when they are molten. Electricity is carried by the movement of the ions and their discharge at the electrodes. In the aluminum chloride and phosphorus (V) chloride cases, the solid doesnt conduct electricity because the ions arent free to move. In the liquid (where it exists both of these sublime at ordinary pressures), they have converted into a covalent form, and so dont conduct either. The rest of the chlorides dont conduct electricity either solid or molten because they dont have any ions or any mobile electrons. Reactions with water As an approximation, the simple ionic chlorides (sodium and magnesium chloride) just dissolve in water. The other chlorides all react with water in a variety of ways described below for each individual chloride. The reaction with water is known as hydrolysis. The Individual Chlorides Sodium chloride, NaCl Sodium chloride is a simple ionic compound consisting of a giant array of sodium and chloride ions. A small representative bit of a sodium chloride lattice looks like this: [pic] This is normally drawn in an exploded form as: [pic] The strong attractions between the positive and negative ions need a lot of heat energy to break, and so sodium chloride has high melting and boiling points. It doesnt conduct electricity in the solid state because it hasnt any mobile electrons and the ions arent free to move. However, when it melts it undergoes electrolysis. Sodium chloride simply dissolves in water to give a neutral solution. Magnesium chloride, MgCl2 Magnesium chloride is also ionic, but with a more complicated arrangement of the ions to allow for having twice as many chloride ions as magnesium ions. Again, lots of heat energy is needed to overcome the attractions between the ions, and so the melting and boiling points are again high. Solid magnesium chloride is a non-conductor of electricity because the ions arent free to move. However, it undergoes electrolysis when the ions become free on melting. Magnesium chloride dissolves in water to give a faintly acidic solution (pH = approximately 6). When magnesium ions are broken off the solid lattice and go into solution, there is enough attraction between the 2+ ions and the water molecules to get co-ordinate (dative covalent) bonds formed between the magnesium ions and lone pairs on surrounding water molecules. Hexaaquamagnesium ions are formed, [Mg(H2O)6]2+. [pic][pic] Ions of this sort are acidic the degree of acidity depending on how much the electrons in the water molecules are pulled towards the metal at the centre of the ion. The hydrogens are made more positive than they would otherwise be, and more easily pulled off by a base. In the magnesium case, the amount of distortion is quite small, and only a small proportion of the hydrogen atoms are removed by a base in this case, by water molecules in the solution. [pic][pic] The presence of the hydronium ions in the solution causes it to be acidic. The fact that there arent many of them formed (the position of equilibrium lies well to the left), means that the solution is only weakly acidic. You may also find the last equation in a simplified form: [pic][pic] Hydrogen ions in solution are hydronium ions. If you use this form, it is essential to include the state symbols. Aluminum chloride, AlCl3 Electronegativity increases as you go across the period and, by the time you get to aluminum; there isnt enough electronegativity difference between aluminum and chlorine for there to be a simple ionic bond. Aluminum chloride is complicated by the way its structure changes as temperature increases. At room temperature, the aluminum in aluminum chloride is 6-coordinated. That means that each aluminum is surrounded by 6 chlorines. The structure is an ionic lattice although with a lot of covalent character. At ordinary atmospheric pressure, aluminum chloride sublimes (turns straight from solid to vapour) at about 180 °C. If the pressure is raised to just over 2 atmospheres, it melts instead at a temperature of 192 °C. Both of these temperatures, of course, are completely wrong for an ionic compound they are much too low. They suggest comparatively weak attractions between molecules not strong attractions between ions. The coordination of the aluminum changes at these temperatures. It becomes 4-coordinated each aluminum now being surrounded by 4 chlorines rather than 6. What happens is that the original lattice has converted into Al2Cl6 molecules. [pic] This conversion means, of course, that you have completely lost any ionic character which is why the aluminum chloride vaporizes or melts (depending on the pressure). There is an equilibrium between these dimers and simple AlCl3 molecules. As the temperature increases further, the position of equilibrium shifts more and more to the right. [pic][pic] Summary †¢ At room temperature, solid aluminum chloride has an ionic lattice with a lot of covalent character. At temperatures around 180 190 °C (depending on the pressure), aluminum chloride coverts to a molecular form, Al2Cl6. This causes it to melt or vaporize because there are now only comparatively weak intermolecular attractions. †¢ As the temperature increases a bit more, it increasingly breaks up into simple AlCl3 molecules. Solid aluminum chloride doesnt conduct electricity at room temperature because the ions arent free to move. Mo lten aluminum chloride (only possible at increased pressures) doesnt conduct electricity because there arent any ions any more. The aluminum chloride reacts with the water rather than just dissolving in it. In the first instance, hexaaquaaluminum ions are formed together with chloride ions. [pic][pic] You will see that this is very similar to the magnesium chloride equation given above the only real difference is the charge on the ion. That extra charge pulls electrons from the water molecules quite strongly towards the aluminum. That makes the hydrogens more positive and so easier to remove from the ion. In other words, this ion is much more acidic than in the corresponding magnesium case. These equilibria (whichever you choose to write) lie further to the right, and so the solution formed is more acidic there are more hydroxonium ions in it. [pic][pic] or, more simply: [pic][pic] Silicon tetrachloride, SiCl4 Silicon tetrachloride is a simple no-messing-about covalent chloride. There isnt enough electronegativity difference between the silicon and the chlorine for the two to form ionic bonds. Silicon tetrachloride is a colourless liquid at room temperature which fumes in moist air. The only attractions between the molecules are van der Waals dispersion forces. It doesnt conduct electricity because of the lack of ions or mobile electrons. It fumes in moist air because it reacts with water in the air to produce hydrogen chloride. If you add water to silicon tetrachloride, there is a violent reaction to produce silicon dioxide and fumes of hydrogen chloride. In a large excess of water, the hydrogen chloride will, of course, dissolve to give a strongly acidic solution containing hydrochloric acid. [pic] The phosphorus chlorides There are two phosphorus chlorides – phosphorus (III) chloride, PCl3, and phosphorus (V) chloride, PCl5. Phosphorus (III) chloride (phosphorus trichloride), PCl3 This is another simple covalent chloride again a fuming liquid at room temperature. It is a liquid because there are only van der Waals dispersion forces and dipole-dipole attractions between the molecules. It doesnt conduct electricity because of the lack of ions or mobile electrons. Phosphorus (III) chloride reacts violently with water. You get phosphorous acid, H3PO3, and fumes of hydrogen chloride (or a solution containing hydrochloric acid if lots of water is used). [pic][pic] Phosphorus (V) chloride (phosphorus pentachloride), PCl5 Unfortunately, phosphorus (V) chloride is structurally more complicated. Phosphorus (V) chloride is a white solid which sublimes at 163 °C. The higher the temperature goes above that, the more the phosphorus (V) chloride dissociates (splits up reversibly) to give phosphorus (III) chloride and chlorine. [pic][pic] Solid phosphorus (V) chloride contains ions which is why it is a solid at room temperature. The formation of the ions involves two molecules of PCl5. A chloride ion transfers from one of the original molecules to the other, leaving a positive ion, [PCl4]+, and a negative ion, [PCl6]-. At 163 °C, the phosphorus (V) chloride converts to a simple molecular form containing PCl5 molecules. Because there are only van der Waals dispersion forces between these, it then vaporizes. Solid phosphorus (V) chloride doesnt conduct electricity because the ions arent free to move. Phosphorus (V) chloride has a violent reaction with water producing fumes of hydrogen chloride. As with the other covalent chlorides, if there is enough water present, these will dissolve to give a solution containing hydrochloric acid. The overall equation in boiling water is: pic] *Disulphur dichloride, S2Cl2* Disulphur dichloride is a simple covalent liquid orange and smelly! The shape is surprisingly difficult to draw convincingly! The atoms are all joined up in a line but twisted: [pic] The reason for drawing the shape is to give a hint about what sort of intermolecular attractions are possible. There is no plane of symmetry in the molecule and that means that it will have an overall permanent d ipole. The liquid will have van der Waals dispersion forces and dipole-dipole attractions. There are no ions in disulphur dichloride and no mobile electrons so it never conducts electricity. Disulphur dichloride reacts slowly with water to produce a complex mixture of things including hydrochloric acid, sulphur, hydrogen sulphide and various sulphur-containing acids and anions (negative ions). There is no way that you can write a single equation for this and one would never be expected in an exam. Summary 1. Physical properties of oxides: The physical properties of these oxides depend on the type of bonding. Na2O, Al2O3 and MgO are ionic oxides and hence have a high melting point. MgO and Al2O3 have a higher melting point than Na2O since the charges are higher, resulting in a stronger attraction between the ions. SiO2 has a giant covalent structure and hence a high melting point. There are strong covalent bonds between all the atoms and thus lots of energy is required to break them. P4O10 and SO3 are molecular covalent and so only intermolecular forces exist between the molecules. The melting points are thus much lower. P4O10 is a much bigger molecule than SO3 and so has a much higher melting point, as the van der Waal’s forces are stronger. Element |Na |Mg |Al |Si |P |S | |Formulae of oxide |Na2O |MgO |Al2O3 |SiO2 |P4O10 |SO3 | |Structure of oxide |Ionic |Ionic |Mostly ionic |Giant covalent |Molecular covalent|Molecular covalent | |Melting point of oxide / °C |1275 |2852 |2072 |1703 |300 |-10 | 2. Acid-base character of oxides.

Introduction to Criminal Justice free essay sample

This definition of a crime comes from (Merriam-Webster On-line Dictionary) and reads; â€Å"Crime: an act or the commission of an act that is forbidden or the omission of a duty that is commanded by a public law and that makes the offender liable to punishment by that law; especially: a gross violation of the law†. There are several definitions of crime, but there all consistent for the most part. People who commit crimes are held to answer for the crimes they are accused of.For this, we must have a judicial system in place that is fair and balanced. Although the person accused of committing the crime is sometimes judged before he’s even gone to court, he must be allowed certain rights and due process. Those rights must not be violated prior to a trial. It’s this system that makes American what we are. Sometimes there are cases that make us feel that the person being tried should just be executed or sent to jail, because the media has basically tried and convicted the person prior to trial. We will write a custom essay sample on Introduction to Criminal Justice or any similar topic specifically for you Do Not WasteYour Time HIRE WRITER Only 13.90 / page This was evident in the â€Å"Casey Anthony† murder trial. Most Americans and the media had convicted her prior to trial. She was found not guilty earlier today by twelve jurors. Is the system fair? Who knows, but this is the reason, lots of people believe there should be professional jurors for high profile cases like this. On the other hand our judicial system has been around for a long time and delivers in most cases a fair system of government that protects the innocent, the victims and the accused. Of course all parties involved don’t feel this way based on where you’re at during the judicial process, but it’s a system that’s fair to all parties. The system is overseen by federal systems that try to keep order and balance throughout the country. Without any of this we would be a country with no law and order. Vigilantes’ would run the streets creating their own laws and chaos would prevail. The three components of the criminal justice system are The Police, The Criminal Courts and The Correctional Institutions.Each one of these components has a very specific function and go hand in hand with one another. For example; if a person is arrested by a police officer for a residential burglary, there is a series of events that happen on the law enforcement side, before the suspect goes to court and before he becomes a part of the correctional institutions. . Once an officer confirms a crime has been committed, he must place the person under arrest and show there was probable cause to arrest the person.This information goes into a â€Å"Probable Cause statement that’s submitted during the booking process. If the suspect is questioned he must be advised of his Miranda rights by the law enforcement officer. Evidence must be collected to prove the crime was committed and the person being charged committed the crime. The suspect is then transported to the county jail for booking. The officer must then document the incident in a police report and be able to articulate the elements of the crime have been fulfilled. The evidence must be booked and the police report must then be submitted to the District Attorney’s office within a 48 hour time frame before the suspect is arraigned in court. If any of this fails’ to happen the courts could release the suspect under Penal Code 825. The case can still be submitted to the District Attorney’s office, but it will be filled out of custody. If this process has been completed correctly the criminal courts takes over their function. Once the suspect goes to court for his first appearance he is advised of his charges and the probable cause is confirmed by the courts.During this phase the report and evidence collected are examined by the defense counsel to see if the suspect has a chance of winning the case. If the defense attorney feels that his client may lose the case based off of the evidence presented he may be allowed to plea bargain in which the suspect could plead to a lesser crime or admit guilt to the crime he is accused of. There are several things that determine if this allowed to happen, to include the suspects past criminal history and the seriousness of the crime.If the courts feel there is enough probable cause and the suspect’s rights have not been violated, the suspect will be held to answer to the charges brought against him. Otherwise the suspect could be let free based on the lack of probable cause, lack of physical evidence or the suspect’s rights being violated during the arrest or questioning process. If the suspect is held to answer he will then go to an arraignment. Once there he will plead either not guilty, guilty, or no contest. If a person pleads â€Å"not guilty† he is set for pre-trial at which time his case is handled by the person’s lawyer.If need be the case goes to trial where he is judged by twelve of his peers or the person pleads to a lesser charge and the case is closed prior to the trial. If a trial takes place and the person is found guilty he will be sentenced by the judge based on the crimes committed. This can be immediately or shortly after the trial. If the suspect is sentenced to prison he then becomes a part of the correctional institution. After sentencing he is usually turned over immediately to the custody of the sheriff’s department while awaiting transportation to prison.