• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

The Polarity of a Compound. We also determined that Water (H2O), is the most polar of all our tested compounds. To explain why it`s polar is simple; it has it`s hydrogen bonds (which cause it to be very polar) and the fact that it is in a isosceles triang

Extracts from this document...


The Polarity of a Compound Conclusion: To start, a non-polar molecule is simply when it is symmetrical (linear, cyclo,etc) in evry way and so, no matter the charge, the molecule can balance it`s charges out at he poles. A polar charge is merely the opposite, where it is unbalanced due to non symmetrical (triganol, etc) have a polar compound is to have a molecule that has an un-even charge therefore a more heavy attraction on one side of the molecule. We also determined that Water (H2O), is the most polar of all our tested compounds. To explain why it`s polar is simple; it has it`s hydrogen bonds (which cause it to be very polar) and the fact that it is in a isosceles triangle formation means that it is not symmetrical thus it is polar because of an uneven distribusuion of elctro-negativity of the hydrogen on either side. Now how to exlain that it is the most polar of the elements tested is because it has the largest uneven distribution of charge. The second most polar of our compounds was propone and thus had the second highest force of attraction towards positive charge of the rod. The only disquishing factor that ould affect this in propone is the fact that it contains double bonds. ...read more.


So, simply put; because maethanol is has smaller gravitational pull et ass than ethanol, it is thus displaced much easier by the polarity of the pole than the latter. Evaluation: To start, our group did most things correctly but merely in a different way. For example when our group measured the degree of deflection caused by the ostivily charged rod, we measured it close to the exit stream of the pepitte for each of the compounds instead of further down on the beaker. This was not nesserally incorrect procedure considering that we had used the same location of measurement for all tested compound, but, it did make it slightly harder for our group to judge what the precise degree of delectation was. This could be simply changed for the next test by recording our results from lower down the stream. One of the largest mistakes our group did though was that we did not retest our degree of deflection tests numerous times. We only would record the degrees once and then leave it alone. We had only one test and one result for each compound tested. Our method could have allowed some very false results to be recorded. To improve the accura cy of our results for next would be to retest each compound`s degree of deflection test 3 to 5 times in order to average it in the end. ...read more.


In regards to the charged ruler, here existed another flaw in the results. The biggest problem with the ruler is that there was no way to tell how charged the ruler was. To charge the ruler we would remove electrons by rubbing the ruler with a woolen cloth. The obvious problem was that we did not have a controlled time set to charge the stick. So when testing the polarity of set substances some tests were using a less polarized rod, which could have if it occurred greatly, changed the results. For next time our group should set a controlled time of 45 seconds so it's enough to fully polarize the rod but, also short enough so that we can repeat the tests for each substance without any time concerns. And yet another flaw occurs when we measured the deflection of the substances with a protractor, which was held at random distances away from the stream. Although it doesn't in any way affect our degree of deflection it did though, make it harder for me the degree reader to read the correct degrees. To add on to this problem we also did not hold our protractor straight and we often recorded the degrees of deflection with a shaky hand. What we could have done is lock the protractor in clamps and put it in a certain location throughout the entirety of the experiment. ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our International Baccalaureate Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related International Baccalaureate Chemistry essays

  1. testing liquis for polarity

    Propanone 2 cm of deflection This molecule shows as very weak polarity because the only way of this molecule being polar is the double bonded Oxygen-Carbon bond. Oxygen is more electronegative than carbon which gives as a result a very weakly charged dipole.

  2. Factors Affecting Angle of Deflection

    Therefore the deflection when the rod is 4cm from the flow will be one quarter of that if the rod is only 2cm away. Dependant, Independent and Controlled Variables: The experiment contains elements of all three variables like all other experiments.

  1. Dissolved Oxygen in water

    Step 1: 2Mn2+ + O2 + 4OH- -->2MnO(OH)2 Step 2: MnO(OH)2 + 2I- + 4H- --> Mn2+ + I2 + 3H2O Step 3: I2 + 2S2O32- --> 2I- + S4O62- Variables: Independent variable: The independent variable in the experiment is the different water samples that we are taking i.e.

  2. liquids polarity

    As shown, the deflection is in big amount. Ethyl acetate 1-2.5 -Polar -Tetrahedral - This molecule shows a small deflection on the stream caused by the position of the Oxygen atoms. One O atom is placed on top of a C atom which will create a dipole moment and a

  1. Atomic Structure Notes

    ratio is also the mass number of each isotope * the height of a peak is the proportional to the relative abundance of the isotope. This information can be used to work out the relative atomic mass, Ar, of the element in the sample.

  2. Aim: To investigate the chemical properties of the halogens and some of their ...

    * Bromine Bromine in sample-tube. (Photo by Greenhorn1) General: Name:Bromine Symbol:Br Type:Halogen Atomic weight:79.904 Density @ 293 K:3.122 g/cm3 Atomic volume:23.5 cm3/mol Discovered:Bromine was discovered by A.J. Balard in 1826 in Montpellier, France. The name comes from the Greek word "bromos" meaning "stench".

  1. The chemistry of atmospheric and water pollution.

    These are some of them: In 1985 a number of governments adopted the Vienna Convention on Protection of Ozone Layer. In 1987, a United Nations Convention established the Montreal Protocol which aimed to restrict and control global emissions of ozone destroying chemicals (such as CFCs and halons)

  2. Testing the Suitability of Pool Water. The expected amount of chlorine which is ...

    This solution was then left for about one day before we began the experiment. 2) On the day of the experiment, we began testing the pool water, by first checking its pH level. This was done by putting a little of it in a test tube and adding a few

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work