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

Revision Q's. Using the Periodic table to determine the characteristics of elements.

Extracts from this document...


´╗┐PERIODICITY REVIEW ? TOPIC 3 Describe the arrangement of elements in the Periodic Table in order of increasing atomic number. The elements in the Periodic Table are arranged in order of increasing nuclear charge. Distinguish between the term group and period. Group: Column on the periodic table Period: Row on the periodic table Apply the relationship between the electron arrangement of elements and their position in the Periodic Table up to Z = 20 The electron arrangement of phosphorus is 2,8,5. There are 5 outer electrons and there are 3 energy levels on total. The group number tells us about the number of electron shells and the period tells us about the number of electrons in the outer shell. Apply the relationship between the number of electrons in the highest occupied energy level for an element and its position in the ...read more.


As you go down a period, atomic radii decrease. Ionic Radii = the radius ascribed to an atoms ion. As you go down a group, ionic radii increase. As you go down a period, ionic radii increase. First ionization energies = the amount of energy needed to remove one mole of electrons from one mole of gaseous atoms. As you go down a group, first ionization energy decreases. As you go down a period, first ionization energy increases. Electronegativities = the attraction of a covalently bonded atom for a bonding pair of electrons. As you go down a group, electronegativity decreases. As you go down a period, electronegativity increases. Melting points = the temperature at which a givens solid will melt. As you go down group 1, the melting points of the element decrease As you go down group 7, the melting ...read more.


The more reactive halogen displaces the ions of the less reactive halogen. Discuss the changes in nature, from ionic to covalent and from basic to acidic, of the oxides in Period 3. Ionic compounds are generally formed between metal and non-metal elements, so the oxides of elements Na to Al have giant ionic structures Covalent compounds are formed between non-metals, so the oxides of P, S, and Cl have molecular covalent structures. Silicon, which is a metalloid, has a giant covalent structure. The oxides of Na and Mg are basic; the oxides of Al and Si are amphoteric; and the oxides of P, S, and Cl are acidic. A basic oxide reacts with an acid to form salt and water. A non-metallic oxide reacts with water to produce an acidic solution. ...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. A study of trends in period 3

    PCl5(s) + 4H2O(l) ---> H3PO4(aq) + 5HCl(aq) As you go across the period the substances also start to react with water rather than dissolve it. The reactions with water also become more violent. -Going from left to right, each element bonds to an extra chlorine in which it is noticed that the subscript of the Cl increases by one as you move across the period.

  2. IB chemistry revision notes

    Charge Found in atom Proton 1 +1 Nucleus Nucleons Neutron 1 0 Nucleus Electron 1/1840 -1 Shells * Almost all the mass of the atom is concentrated in the nucleus which has a very small radius.

  1. IB questions and answers on Atomic Theory

    15. Write the symbol for the species with 6 protons, 8 neutrons, and 6 electrons. 16. Write the symbol for the species with 3 protons, 3 neutrons, and 2 electrons. 17. Explain why most atomic masses are not whole numbers. Atomic masses from the periodic table represent weighted averages of all of an element's isotopes.

  2. Practical de quimica Structure and Bonding

    Bonding gives the capacity of conductivity for example ionic compounds arepoor conductors as solids because electrons are tied up by ions. However they are good conductors when melted or dissolved because ionic bonds are broken and electrons are free to move around.

  1. Trends across group 2 elements

    Using the pipette and the pH paper, determine the pH value of the mixture and record the data. 6. Record all the data and observations. 7. Repeat steps 1 - 6 for calcium hydroxide and barium hydroxide. 8. Clean out the test tubes.

  2. To determine the molecular mass of an unknown alkali metal carbonate, X2CO3.

    taking the arithmetic mean of the all the three trials for each solution containing 1.5g, 2.0g and 2.5g of substance Z. Sample calculation for finding the average volume of HCl required to completely neutralize 25.0cm3 solution containing 1.5g of substance Z: = = 28.0cm3.

  1. Period 3 Chlorides. Aim: To study the chlorides of period 3 elements and ...

    pH of aqueous solution 8 9 2 Solubility in acetone Poor Good Good Structure bonding Ionic Ionic Ionic Sources: 1) Wikipedia, the free encyclopaedia. Magnesium Chloride. 31 October 2007. 17 November 2007 <http://en.wikipedia.org/wiki/Magnesium_chloride>. 2) Wikipedia, the free online encyclopaedia. Aluminium Chloride.

  2. To determine the standard enthalpy of formation of Magnesium Oxide using Hess Law.

    Whichever point the two lines meet at can safely be assumed to be a good estimate of the maximum temperature reached and how much time had elapsed. Graph 1: Highest temperature reached in Part X, Trial 1. For the best estimation of maximum temperature reached, a magnified view of the intersection of horizontal line and y-axis is useful.

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