KS3+Patterns+of+reactivity

The **reactivity** **series** is a list of metals with the __ most __ reactive at the top and the __ least __ reactive at the bottom. media type="custom" key="28985829" Explain how metals and non-metals react with oxygen, water and acid __ Products __: The __new substances produced__ in a chemical reaction and shown on the right of a word equation. __ Reactants __: The starting __substances used__ in a chemical reaction and shown on the left of a word equation. Word equation: A summary of a chemical reaction in words. __ Chemical __ reaction: A change in which new substances are made and which cannot easily be reversed. __ Catalyst __: A substance that can help the reactants in a chemical reaction react with each other faster and that is **not** actually become part of the products of the reaction. In a chemical rection, the substances thaat undergo a chemical change are called the__ reactants __. The substances that result from the change are called the __ products __.
 * Reactivity Series **
 * Keywords**:

Reaction of metals with water
Metals react with water to produce __ hydroxides __, giving alkaline solutions. Universal indicator turns green to blue when adding to water as indication of the production of an alkaline solution. Some metals require steam to react since their reaction with water is __ slow __.

1. What happens when pieces of lithium are dropped into a bowl of water? What safety measures should be taken when carrying out this type of experiment? Bubbles of gas were given off quite quickly. Water becomes alkaline when tests with universal indicator. 2. What happens when pieces of sodium are dropped into a bowl of water? What colour flame appears when the sodium reacts with the water? The sodium dissolved and skimmed over the surface. Sometimes a yellow-orange flame appeared. 3. What happens when pieces of potassium are dropped into a bowl of water? What colour flame appears when the potassium reacts with the water? Potassium immediately produced a lilac flame as it skimmed around the surface making a fizzing noise.

1. Calcium sinks in cold water and bubbles of hydrogen form on its surface, slowly at first then increase in number quickly. calcium + water >> calcium hydroxide + hydrogen gas 2. Copper sinks in cold water and does not react with it. It also does not react with steam. 3. Sodium floats on the surface of the water and a fizzing sound is heard as bubbles of hydrogen are quickly produced around it. A clear solution of sodium hydroxide forms. sodium + water >> sodium hydroxide + hydrogen gas 4. Iron sinks in water and no bubbles of hydrogen form. When the metal is heated in steam, hydrogen is produced slowly. Iron + water(steam) >> Iron hydroxide + hydrogen gas 5. Magnesium sinks in water. Bubbles of hydrogen are produced only very slowly and a solution of magnesium hydroxide is formed. When the metal is heated in steam hydrogen is produced quickly. magnesium + water >> magnesium hydroxide + hydrogen gas 6. Potassium floats on water and burst into flames immediately. Hydrogen bubbles are rapidly produced around the metal. A clear solution of potassium hydroxide forms. potassium + water >> potassium hydroxide + hydrogen gas
 * Describe the reactions between water and metals of calcium, copper, sodium, iron, magnesium and potassium.**

Reaction of metals with oxygen
Some metals react very vigorously with oxygen, while others barely react at all. 1. A piece of magnesium is heated in a Bunsen burner flame. The magnesium is then placed in a jar of oxygen. How reactive is the magnesium with oxygen? Describe your observation. Magnesium burns vigorously with glowing light. The ribbon burned with a dazzling white flame giving grey white smoke and ash. 2. A piece of iron wool is heated in the Bunsen burner flame. The iron wool is then placed in a jar of oxygen. How reactive is the iron wool? Compare the reactivity with oxygen to your observation in 1. Iron oxide, which is reddish brown or orange brown, forms slowly without glowing. The iron wool glowed red and sparkled leaving a brown black solid. 3. Finally, a piece of copper is heated in the Bunsen burner flame. The copper is then placed in a jar of oxygen. How reactive is the copper with oxygen? Describe the changes on the surface of copper strip. Coper turns grey then develops a covering of a black powder without glowing or bursting into flame. The copper turnings went through reds and oranges and then slowly got a permanent coating of black.

Reaction of metals with acids
[|When metals meet acids] from intel.co.uk Acids + Metal → Salts + Hydrogen gas 1. hydrochloric acid + magnesium → magnesium chloride + hydrogen 2HCl(aq) + Mg(s) → MgCl 2 (aq) + H 2 (g) 2. hydrochloric acid + zinc → zinc chloride + hydrogen 2HCl(aq) + Zn(s) → H 2 (g) + ZnCl 2 (aq) 3. magnesium + //sulphuric acid// → //magnesium// sulphate + hydrogen. //Mg// + H 2 SO 4 → MgSO 4 + H 2 4. Sulphuric acid + Zinc → Zinc sulphate + Hydrogen Zn + H 2 SO 4 → ZnSO 4 + H 2

Construct a reactivity series for metals. The reactivity series is a list of metals, listed in order of __reactivity__. Find answers to the questions 1,2,3 below. 1. Will an electron feel a greater force of attraction when it is close to the nucleus, or when it is further away?

2. Here is some data for Group 1 of the Periodic Table. i) Plot a graph of atomic radius (vertical axis) against number of electrons in the atom (horizontal axis).
 * = Order of reactivity ||= Name of metal ||= Number of electrons ||= Atomic radius (nm) ||
 * = 5 ||= Lithium ||= 3 ||= 0.157 ||
 * = 4 ||= Sodium ||= 11 ||= 0.191 ||
 * = 3 ||= Potassium ||= 19 ||= 0.235 ||
 * = 2 ||= rubidium ||= 37 ||= 0.250 ||
 * = 1 ||= caesium ||= 55 ||= 0.272 ||

ii) Describe the relationship between the number of electrons and atomic radius.

iii) Describe the relationship between reactivity and atomic radius.

3. Give two possible explanations for the reactions of metals. i) Metals react when some of their outer electrons are given away to other non-metal atoms. ii) Metals react when they take in extra electrons from non-metal atoms.

Reactivity series (A list of metals, recorded in order of __ reactivity __ )
The most reactive metals, like __ potassium __ and __ sodium __, are at the top of the list. These metals react vigorously with __w ater __, __ acids __ and __ oxygen __. The least reactive metals, like __ copper __, __silver and gold__, react very slowly or not at all. These unreactive metals can be used for making __saucepans__, __water pipes__ and __j ewellery __. Aluminium is high in the reactivity series, but because it is coated with a layer of aluminium __ oxide __, it can be used for applications that normally require an unreactive metal. media type="youtube" key="-R2eNZRzg7Q" width="560" height="315" [|Making Predictions Using Reactivity Series] | Chemistry for All | The Fuse School [|FuseSchool - Global Education] Published on 7 Dec 2015
 * Metal || Reaction with oxygen || Reaction with water || Reaction with acid ||
 * 1. Potassium ||  ||   ||   ||
 * 2. Sodium ||  ||   ||   ||
 * 3. Calcium ||  ||   ||   ||
 * 4. Magnesium ||  ||   ||   ||
 * 5. Aluminium ||  ||   ||   ||
 * 6. Zinc ||  ||   ||   ||
 * 7. Iron ||  ||   ||   ||
 * 8. Tin ||  ||   ||   ||
 * 9. Copper ||  ||   ||   ||
 * 10. Silver ||  ||   ||   ||
 * 11. Gold ||  ||   ||   ||

Know the methods of extraction of some metals and some non-metals. Give examples of displacement reactions.

Displacement reaction
Sample [|displacement animation], [|Displacement reaction].

When metals react with acids, they displace hydrogen from the acid form a salt solution. A more reactive metal can displace a less reactive metal from a salt solution of the metal. =Metals and the reactivitiy series= Click the link below and conduct the experiment by following the instructions given in each step. Record your results of Activity 1 to 4 in a Word document and upload them on MB before the end of this lesson. =[|Activity Series of Metals Computer Simulation] from University of Oregon = strips of zinc foil, strips of magnesium ribbon, strips of copper foil, strips of lead foil (10mm x 5mm) chemical solutions(either nitrate of sulphate solutions such as zinc sulphate solution, magnesium sulphate solution, copper sulphate solution and Iron sulphat), spotting tile, pipette, label 1. Clean each of the metal strips with sand paper. 2. Using a pipette, put some of the solution of a metal compound in four of the holes in the spotting tile. - Label the row with the name of each solution. 3. Do this for all metal solutions. 4. Put a piece of each metal in each of the solution. 5. Put a tick or a cross in your table to show if they have reacted.
 * [[image:sciencelanguagegallery/Copper wire coils in silver sulfate solution. Silver formed on the wire..png]] || [[image:Iron nail left in copper sulfate solution. Copper formed on the nail..png width="361" height="299"]] ||
 * Copper wire coils in silver sulfate solution. Silver formed on the wire. || Iron nail left in copper sulfate solution. Copper formed on the nail. ||
 * Aim:** To investigate displacement reactions between metals and salts solutions
 * Hypothesis: Research the reason of your expectation and include the explanation.**
 * Apparatus:**
 * Diagram:**
 * Method:**
 * To prevent contamination and confusion, it is a good idea for you to put the solutions onto the spotting tiles sequentially and label each row.

Which metal reacts with what solution(s)? Which metal is the most/ the least reactive? Can you arrange the metals in order of their reactivity? Do your results support your hypothesis?
 * Results** table: Use a tick (//V//) to show reactivity and and cross (//X)// to show no reaction.
 * Solution / Metal || Magnesium sulfate || Zinc sulfate || Iron sulfate || Copper sulfate ||
 * Magnesium ||  ||   ||   ||   ||
 * Zinc ||  ||   ||   ||   ||
 * Iron ||  ||   ||   ||   ||
 * Copper ||  ||   ||   ||   ||
 * Conclusion:**

[|Dsiplacement reaction simulation] from group.chem.iastate.edu

Make predictions about displacement reactions =Displacement in action= //Displacement reactions can be used to put a thin coating of one metal on another. You are going to see how this works.// Wear goggles, Wash copper sulfate solution off your skin immediately. 1. Fill a boiling tube about half full with copper sulphate solution. 2. Stand a zinc strip in the tube. 3. Look at the strip after a few minutes. 4. Work as a group of three to think about what you see (There should be a girl and a couple of boys in your group). 5. Work as the same group to answer the questions in the boxes below. Why do we use this method and explain your reasoning. ||
 * Safety**
 * Observation**
 * Make a large simply shaded diagram of our observations.
 * Write explanations in bubbles around your diagram to explain the changes.
 * Include a word equation, ideas about reactivity of metals and ideas about displacement.
 * **Q1. Galvanised iron to make barriers and fences.** || **Q2. Silver plated jewellery by putting a thin plating of silver on another metal, such as iron.** ||
 * Can iron be plated with silver by dipping iron into a solution of a silver salt? Explain your reasoning. || Can iron be plated with zinc by dipping iron into zinc sulphate solution?

explain why the historical order of the discovery of metals is related to their reactivity [|Reactivities and Reactions of metals] from springfield.co.uk