• 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. 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".

  2. IB questions and answers on Atomic Theory

    5.9% 6Li and 94.1% 7Li -1x = -0.059 x = 0.059 or 5.9% 6Li 13. State the name and the mass number of the isotope relative to which all atomic masses are measured. 12C 14. Write the symbol for the species with 17 protons, 19 neutrons, and 18 electrons. 15.

  1. IB chemistry revision notes

    n=x Continuum- e- shells merge- ionisation energy n=5 Pfund lines n=4 (N shell) Brackett lines n=3 (M shell) Transitions causing Paschen lines. Infrared region. n=2 (L shell) Transitions causing Balmer lines. Visible light region. n=1 (K shell) Transitions causing Lymen lines.

  2. 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.

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

    - - Solution began bubbling, heat was released c) Physical and chemical properties for the given chlorides: Property NaCl MgCl2 AlCl3 Melting point (� C) 801 714 190 Boiling point (� C) 1465 1412 178 Physical state at r.t.p White crystals (solid) Colourless, hygroscopic solid Pale yellow solid Conductivity of liquid Good Good Poor Action of water Dissolves Dissolves Hydrolysis (vigorous reaction)

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

    Molarity of HCl No. of moles of HCl per unit volume should remain constant so that no, of moles of HCl remains constant. All trials, the HCl was withdrawn from the same 2.0M stock solution prepared. Table 1: Controlled Variables APPRATUS AND CHEMICALS: Quantity × Item Purpose 2 × Polystyrene cup To be used for making the calorimeter.

  1. 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.

  2. Using Silicon - microchips and semiconductors

    Modern microchip contain thousands upon thousands of tiny transistor packed closely together, they work by having the transistor oscillate between on and off which in terms can be translated to binary language, off equals 0 and on equals 1.(Chandler, 2001)

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