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Please help Are alkali metals or alkali earth metal more reactive why?

Please help Are alkali metals or alkali earth metal more reactive why?

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Please help Are alkali metals or alkali earth metal more reactive why? Please use these observations
Part A: CALCIUM - determine how many pieces of calcium you need A. Fill a large test tube with water and invert it into a beaker full of water. Drop a piece of dean calcium into the beaker and hold the inverted test tube immediately above it. When the reaction is over (or when the tube is full of gas), remove it from the beaker but keep it inverted and bring a flaming splint to its mouth. Save the liquid in the beaker and test it with a strip of red litmus paper. i. ii. iii. iv. OBSERVATIONS: gas produced; pop with flaming splint; water turned red litmus paper blue В. Hold a flake of calcium with the crucible tongs and put it into a bunsen flame for 2-3 minutes. Allow the residue to cool. iii. i. i. Wet a piece of red litmus paper and touch the residue. Then drop the residue into a test tube and half fill it with water. Does the residue dissolve? iv. V. OBSERVATIONS: residue did not dissolve very well and turned litmus paper blue C. Very carefully drop a small piece of clean calcium into 5 mL of hydrochloric acid in a small test tube and collect the gas by placing your thumb over the test tube. i. ii. Test the gas with a flaming splint. OBSERVATIONS: vigorous reaction and white solid formed; gas popped in a flaming splint Part B: MAGNESIUM - determine how many pieces of magnesium you need D. Clean two pieces of magnesium ribbon. Drop one piece into a test tube of cold water and the second into a test tube of very hot water. Observe each test tube carefully for signs of a reaction. Drop a piece of red litmus paper into each test tube. Remove the magnesium strips and re-use them for the next experiments. i. ii. ii. iv. V. OBSERVATIONS: cold water showed no reaction; hot water showed vigorous reaction; red litmus did not turn blue Drop a piece of clean magnesium from the cold tube into a test tube containing some dilute hydrochloric acid. Test the gas with a flaming splint. ví. vii. OBSERVATIONS: magnesium reacts producing bubbles: gas popped in a flaming splint E. Burn a strip of magnesium in the air using the crucible tongs and transfer the residue to a test tube of water. Note the solubility of the solid. Drop a piece of red litmus paper into the test tube. Heat the liquid and note all changes. i. i. ii. iv. OBSERVATIONS: bright light produced, solid only slightly soluble: turned litmus paper blue
Transcribed Image Text:Part A: CALCIUM - determine how many pieces of calcium you need A. Fill a large test tube with water and invert it into a beaker full of water. Drop a piece of dean calcium into the beaker and hold the inverted test tube immediately above it. When the reaction is over (or when the tube is full of gas), remove it from the beaker but keep it inverted and bring a flaming splint to its mouth. Save the liquid in the beaker and test it with a strip of red litmus paper. i. ii. iii. iv. OBSERVATIONS: gas produced; pop with flaming splint; water turned red litmus paper blue В. Hold a flake of calcium with the crucible tongs and put it into a bunsen flame for 2-3 minutes. Allow the residue to cool. iii. i. i. Wet a piece of red litmus paper and touch the residue. Then drop the residue into a test tube and half fill it with water. Does the residue dissolve? iv. V. OBSERVATIONS: residue did not dissolve very well and turned litmus paper blue C. Very carefully drop a small piece of clean calcium into 5 mL of hydrochloric acid in a small test tube and collect the gas by placing your thumb over the test tube. i. ii. Test the gas with a flaming splint. OBSERVATIONS: vigorous reaction and white solid formed; gas popped in a flaming splint Part B: MAGNESIUM - determine how many pieces of magnesium you need D. Clean two pieces of magnesium ribbon. Drop one piece into a test tube of cold water and the second into a test tube of very hot water. Observe each test tube carefully for signs of a reaction. Drop a piece of red litmus paper into each test tube. Remove the magnesium strips and re-use them for the next experiments. i. ii. ii. iv. V. OBSERVATIONS: cold water showed no reaction; hot water showed vigorous reaction; red litmus did not turn blue Drop a piece of clean magnesium from the cold tube into a test tube containing some dilute hydrochloric acid. Test the gas with a flaming splint. ví. vii. OBSERVATIONS: magnesium reacts producing bubbles: gas popped in a flaming splint E. Burn a strip of magnesium in the air using the crucible tongs and transfer the residue to a test tube of water. Note the solubility of the solid. Drop a piece of red litmus paper into the test tube. Heat the liquid and note all changes. i. i. ii. iv. OBSERVATIONS: bright light produced, solid only slightly soluble: turned litmus paper blue
SCH3U0 Name: Eanouel Omotoso BEHAVIOUR OF GROUP I METALS PURPOSE: The purpose of this experiment is to observe patterns in the reactivity of lithium, sodium, and potassium, all of which are Group I metals. Also, some chemical properties of Li and Na will be explored. MATERIALS: Part 1: Part 2: Clean 500 mL beaker Bunsen burner and flint Tap Water Deflagrating spoon Forceps Red litmus paper paper towel Phenolphthalein Wire gauze 500 mL beaker Tap water Pea size chunk of Na Pea size chunk of Na МЕТНOD: Part 1: Lua'er 1. Fill beaker with 250 mL of water. 5. Record all observations in bullet form. 2. Add 2 drops of phenolphthalein to water. 3. Record the physical properties of the piece of sodium you have been given. 4. Add the sodium to the water using the forceps • The Jodiumi piece is very Idullaus • Lualer turned pink Light praduced • The procuct was a base from thes chemical hat cas 1 presend in th and immediately cover the beaker with the wire gauze. reaction The worer vs also releasing smoke Part 2: 300 4. Heat the sodium until it catches fire and burns. 1. Prepare a beaker with 100 mL of tap water. 2. Light the Bunsen burner until an intense blue flame is achieved. You may need to adjust the air intake to get this colour. 3. Put the sodium into the deflagrating spoon using 5. Record all observations in bullet form. the forceps. Cool the residue and then put into the beaker. Add a few drops of phenolphthalein to the beaker and cover with wire gauze. • The flame abere the solution Jurns eraig t • Tae selutIon inside tns white aimost ke table salt • As s0on as we pur the cleflahng speon inside the beaker and tirred , turns pink
Transcribed Image Text:SCH3U0 Name: Eanouel Omotoso BEHAVIOUR OF GROUP I METALS PURPOSE: The purpose of this experiment is to observe patterns in the reactivity of lithium, sodium, and potassium, all of which are Group I metals. Also, some chemical properties of Li and Na will be explored. MATERIALS: Part 1: Part 2: Clean 500 mL beaker Bunsen burner and flint Tap Water Deflagrating spoon Forceps Red litmus paper paper towel Phenolphthalein Wire gauze 500 mL beaker Tap water Pea size chunk of Na Pea size chunk of Na МЕТНOD: Part 1: Lua'er 1. Fill beaker with 250 mL of water. 5. Record all observations in bullet form. 2. Add 2 drops of phenolphthalein to water. 3. Record the physical properties of the piece of sodium you have been given. 4. Add the sodium to the water using the forceps • The Jodiumi piece is very Idullaus • Lualer turned pink Light praduced • The procuct was a base from thes chemical hat cas 1 presend in th and immediately cover the beaker with the wire gauze. reaction The worer vs also releasing smoke Part 2: 300 4. Heat the sodium until it catches fire and burns. 1. Prepare a beaker with 100 mL of tap water. 2. Light the Bunsen burner until an intense blue flame is achieved. You may need to adjust the air intake to get this colour. 3. Put the sodium into the deflagrating spoon using 5. Record all observations in bullet form. the forceps. Cool the residue and then put into the beaker. Add a few drops of phenolphthalein to the beaker and cover with wire gauze. • The flame abere the solution Jurns eraig t • Tae selutIon inside tns white aimost ke table salt • As s0on as we pur the cleflahng speon inside the beaker and tirred , turns pink
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