Life in Suburbia essays

Life in Suburbia essays After World War II the concept of life in America began a new. The process of suburbanization began in cities all across the nation. Today the cities of yesteryear are gone and life as we knew it ended. However, people do not want it to end. They still want the American Dream; the house in the suburbs, the good job, the wife, car and 2.4 kids playing in the yard. These people have been the driving force in the division of socioeconomic status, and the division of race in the suburbs. They accomplish this through local governments and the decisions made through them. Though what has been created, by all of this over the years, isn't necessarily bad, but it has hurt the country in ways that we did not expect. When soldiers returned from the war they were greeted with open arms and a new booming economy. It was this booming economy, of service-oriented jobs, that allowed the middle class of people the opportunity to move away from their jobs and separate their work from their home. Also during that time we were still, as a country, practicing racial segregation, which is part of the reason for the racial inequalities in the suburbs today. These new communities, of mostly white nuclear families, were now in need of a council to make the decisions that needed to be made for their area. They didn't want the city to make these decisions for them since they were so far away. Also since most people worked in the city, they wanted to continue with the dream of keeping home and work separate. Therefore they banded together as neighborhoods and communities to make the decisions that affected that area on a daily basis. The benefit of this was that now they had almost total autonomy from the poor and the lower class they so quickly left behind in the city. This is where the socioeconomic division began. The people of the suburbs loved their lives. They lived around the people of the same socioeconomic status and w ...

Learn About Molecular and Empirical Formulas

Learn About Molecular and Empirical Formulas The molecular formula is an expression of the number and type of atoms that are present in a single molecule of a substance. It represents the actual formula of a molecule. Subscripts after element symbols represent the number of atoms. If there is no subscript, it means one atom is present in the compound. The empirical formula is also known as the simplest formula. The empirical formula is the ratio of elements present in the compound. The subscripts in the formula are the numbers of atoms, leading to a whole number ratio between them. Examples of Molecular and Empirical Formulas The molecular formula of glucose is  C6H12O6. One molecule of glucose contains 6 atoms of carbon, 12 atoms of hydrogen and 6 atoms of oxygen. If you can divide all of the numbers in a  molecular formula by some value to simplify them further, then the empirical or simple formula will be different from the molecular formula. The empirical formula for glucose is CH2O. Glucose has 2 moles of hydrogen for every mole of carbon and oxygen. The formulas for water and hydrogen peroxide are: Water Molecular Formula: H2OWater Empirical Formula: H2OHydrogen Peroxide Molecular Formula: H2O2Hydrogen Peroxide Empirical Formula: HO In the case of water, the molecular formula and empirical formula are the same. Finding Empirical and Molecular Formula from Percent Composition Percent (%) composition (element mass/compound mass) X 100 If you are given the percent  composition of a compound, here are the steps for finding the empirical formula: Assume you have a 100 grams  sample. This makes the calculation simple because the percentages will be the same as the number of grams. For example, if 40% of the mass of a compound is oxygen then you calculate you have 40 grams of oxygen.Convert grams to moles. Empirical formula is a comparison of the number of moles of a compound so you need your values in moles. Using the oxygen example again, there are 16.0 grams per mole of oxygen so 40 grams of oxygen would be 40/16 2.5 moles of oxygen.Compare the number of moles of each element to the smallest number of moles you got and divide by the smallest number.Round your ratio of moles to the nearest whole number as long as it is close to a whole number. In other words, you can round 1.992 up to 2, but you cant round 1.33 to 1. Youll need to recognize common ratios, such as 1.333 being 4/3. For some compounds, the lowest number of atoms of an element might not be 1! If the lowest number of moles is four-thirds, you will need to multi ply all ratios by 3 to get rid of the fraction. Write the empirical formula of the compound. The ratio numbers are subscripts for the elements. Finding the molecular formula is only possible if you are given the molar mass of the compound. When you have the molar mass you can find the ratio of the actual mass of the compound to the empirical mass. If the ratio is one (as with water, H2O), then the empirical formula and molecular formula are the same. If the ratio is 2 (as with hydrogen peroxide, H2O2), then multiply the subscripts of the empirical formula by 2 to get the correct molecular formula. two.