• 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. IB chemistry revision notes

    --> Z is the Atomic Number, X the symbol. Mass Numbers * It is the sum of the number of protons plus the number of neutrons in an atom or ion. --> A is the Atomic Mass, X the symbol.

  2. IB questions and answers on Atomic Theory

    This number is usually a decimal 18. In the context of electromagnetic radiation, what is wavelength? How does wavelength relate to energy? wavelength is the distance between two successive crests on a wave (or any two repeating points). The longer the wavelength, the lower the energy in the wave 19.

  1. 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) Test the solubility of Iodine: 1. A very small amount of iodine was put into water, cyclohexane and KI(aq) respectively 2. The color changes of the solutions and the solubility in each solvent were recorded 2) Test iodine reacts with starch: 1.

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

    Uncertainty for the value of average volume of HCl required for complete neutralization is ±0.10cm3 since averaging values do not lead to change in uncertainties.

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

    Using the burette, 15cm3 of 2M HCl was withdrawn into the calorimeter and was allowed to sit for a minute or two so that its temperature reaches the ambient temperature. In the duration of these few minutes, Magnesium was prepared for reaction using the following two steps.

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

    Source: John Green and Sadru Damji. "Chemistry, International Baccalaureate Diploma Programme." 2nd Edition. Victoria: IBID Press, 2001. Variables: * Independent variable: There was no independent variable present. * Dependent variable: The dependent variables of this experiment were the measurements of temperature and pH level. * Controlled variable: The controlled variable of this experiment was the volume of distilled water used in each experiment.

  2. Chemistry Revision - ATOMIC STRUCTURE REVIEW TOPIC 2

    The positive ions are deflected by a magnetic field. The ions are detected by producing a current. Calculate average atomic mass from isotopes and relative abundance. For elements, which have more than one isotope (the majority), the measured relative atomic mass of a sample will be the average mass of all the isotopes in the sample.

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