Lab 1 reactivity of metals
Safety: Wear goggles and aprons at all times. Abraham, M.
Reactivity of metals experiment
Graph of expected results rise in temperature : The rise in temperature for each of the metal powders to be used is shown after a period of 2 minutes for each reaction. Do NOT burn the calcium. This happens because the compound on the reactants side is quite unstable and thus breaks up easily and so much energy is not used up. Consider a group of nonmetals. Element 1st 2nd 3rd 4th 5th 6th 7th 8th Na 4, 5, 5, 6, 7, 7, 8, Mg 1, 7, 8, 9, 10, 11, 11, Al 1, 2, 11, 12, 12, 14, 14, X 1, 3, 4, 5, 8, 9, 27, 28, a. Sodium, Magnesium, and Aluminum are in Period 3. Dependant variable: o Temperature change when each of the metals reacts with copper sulphate in a given period of time. The rise in temperature will become lesser in the order of reactivity and therefore the reaction between rion and copper sulphate will be the least reactive and will take the longest time for the reaction to complete. Which samples reacted with water? Materials: 3 petri dishes top and bottom , labeling paper, wash bottle, lab burner, striker, forceps, watch glass, magnesium, calcium, aluminum, sand paper Procedure: Part 1: Observing Effects of Exposure of Al and Mg period 3 metals to Heat and Oxygen 1. Write the electron configuration, list number valence electrons, and draw the electron dot diagram for Sodium, Potassium, Magnesium, Calcium, and Aluminum.
This reaction if it occurs will also produce hydrogen gas, and would be an exothermic reaction. Kieffer, W.
Mg, Al, Zn and Fe. Consider a group of nonmetals. Rate the three samples based on reactivity with oxygen.
Do NOT burn the calcium. These metals will form bases IF they react with the water. What type of evidence of reaction should be present if the metals react with oxygen?
Why does it ALWAYS take more energy to remove the 2nd electron than the 1st or more energy to remove the 3rd electron than the 2nd, and so on?
Reaction of metals with acids experiment
For this experiment, the four metal powders given are magnesium, zinc, aluminium and iron. This reaction is carried out using the metal powder given and a weak compound such as copper sulphate in which the metal ion is lower than the metal powder in the reactivity series. Dependant variable: o Temperature change when each of the metals reacts with copper sulphate in a given period of time. Where are the significant leaps? A small amount of heat and flammable gas will be produced in parts 2 and 3—follow directions in order to prevent exposure. Press enter to begin your search Reactivity of Metals: Lab Report No Comments Reactivity of Metals Experiment Aim: To investigate and see the reaction of four metals- magnesium, zinc, aluminium and iron with copper sulphate to find out which one is the most reactive and which one the least reactive. Learning Objectives 1. When a displacement reaction occurs, heat energy is given out which means that the reaction is exothermic. Observe for three minutes over the white paper, then record observations in data table 2. Metals tend to be lusterous, but areas exposed to oxygen will form a dull coating.
The activity series of metals. Graph of expected results rise in temperature : The rise in temperature for each of the metal powders to be used is shown after a period of 2 minutes for each reaction.
In theory, when a more reactive metal takes part in a displacement reaction, the reaction is more vigorous and exothermic.
based on 51 review