Investigate the reactions of group 2 elements

Show answers Print Version with answers Introduction You are to investigate some of the reactions of the Group 7 elements, and try to identify any patterns in the reactivity. You will then try to explain these patterns in terms of the electronic structures of the elements. The displacement of iodide by chlorine The displacement of iodide by chlorine Open Yenka file Model 1.

Investigate the reactions of group 2 elements

Reactivity trend All Group 2 elements need to lose two electrons to react. The easier it is to lose the electrons the faster the element will be able to react. It's easier to lose electrons that are only weakly held by the nucleus.

As usual there are three factors to consider: The second and third factors outweigh the first - say something like this in your answers. So as we go down the group the electrons are more weakly held and more easily lost and so the reactivity increases.

We can put numbers to this by looking a first and second Ionisation Energies.

Investigate the reactions of group 2 elements

The lower the combined Ionisation Energies the easier it is to lose electrons. You can be asked to define the first ionisation energy but not any of the others. You can be asked to write an equation for any ionisation energy - so you need to recall that you are always losing one electron, and that everything is gaseous.

You don't really need to know that Barium gives a green flame and Strontium a Crimson one. It would be difficult to observe much difference in the speed of burning but we can assume that the lower in the group the faster all reactions are for the reasons set out above.

AS Chemistry - Redox Reactions and Group 2 Elements | Owlcation

So no one is likely to ask you much about an element that doesn't fit with the trend. Reaction with Water All Group 2 metals except Be react with water up to a point - Magnesium only reacts with very hot water when its has been freshly ground into a very fine powder.

As you go down the group they react faster, as expected. You may even have to explain the tising and falling of the Calcium - it rises when Hydrogen bubbles form round it and sinks again due to its density when they escape at the surface. The white solid will be Calcium Hydroxide - its not very soluble, which is why there are always bits in bottles of Limewater Calcium Hydroxide solution You should not say: Hydrogen is seen - you can't see that it is Hydrogen.

This time the trend is observable from almost no reaction for Mg, to quite a vigorous reaction with Ca to very vigorous reactions at the bottom of the group.

Investigate the reactions of group 2 elements

You should probably also know how to make Magnesium react with water in the form of steam. Heating the Magnesium until it almost burns them passing steam over it causes a jet of flammable Hydrogen to be made.

The Magnesium reacts fiercely enough to melt into the glass. You'll have done this with Magnesium and Calcium - you can assume that the reactions with Ba and Sr will be more vigorous.

Welcome to the Sixth Form Reactions with Halogens Hopefully you'd expect reactive metals to react with reactive non-metals by now. It's not mentioned on the syllabus but you know how examiners are: I mean, I'm telling you that this is a picture of Magnesium Chloride but it could be anything, couldn't it.

When Calcium and Barium are added separately to water, similar reactions occur.Apr 06,  · 1) A salt is formed (MI2) - it's an acid base reaction so a salt is formed and group 2 elements have a 2+ charge so salt would be (MI2) as I has a charge of 1- so the salt needs to consist of 2 iodines to balance the charge Open.

reactions of the group 2 elements with water This page looks at the reactions of the Group 2 elements - beryllium, magnesium, calcium, strontium and barium - with water (or steam).

It uses these reactions to explore the trend in reactivity in Group 2. Metals in group 2 of the periodic table are less reactive than those in group 1.

This experiment indicates the relative reactivity of elements within the group. Halogens as oxidising agents: 1/2Cl 2(g) + e- Cl-(g) These elements gain 1 electron when they react. This means that what ever they react with must lose electrons. Losing electrons is an oxidation reaction: Oxidation Is Loss of electrons Reduction Is Gain of electrons As the Group 7 elements cause the oxidation of other compounds or elements we say it is a.

Group IA, Group IIA, Group III A etc. except Sn and Pb which shows Pb 2+, Pb 4+, Sn 2+, and Sn 4+ more than one charge.

Transition elements have more . Density refers to the mass contained within a unit volume under specified conditions. Data given here refer to the solid. Density is temperature dependent and different allotopes of one element possess different densities.

The Chemistry of the Halogens