Periodic Table and Alkaline Earth Metals
Laboratory# 26 Group 2: The Alkaline Earth Metals
Period E Bautista, Angel
Table D Comer, Tyler
3/22/12 Sullivan, Brittany Truong, Phuoc
Conclusions and Questions
1. Step 1: Ca(s) +H2O->Ca (OH)2(aq)+H2(g) Step 4: Mg(s) +H2O->Mg (OH)2(aq)+H2(g) Step 10: CaSO4 + H2O-> Ca(OH)2 + H2SO4 MgSO4 + H2O ->Mg (OH)2 + H2SO4 Barium Sulfate: No reaction Step 13: MgCl2 + Na2CO3 -> MgCO3 + 2NaCl CaCl2 + Na2CO3 -> CaCO3 + 2NaCl BaCl2 + Na2CO3 -> BaCO3 + 2NaCl
2. The reactivity of the metal increases with each period it goes down. Magnesium is the least reactive and is in the third period with an atomic number of 12. Calcium is slightly more reactive being in the fourth period and having an atomic number of 20. Barium is the most reactive because it is in the sixth period and it has an atomic number of 56. So the farther down in the group they go the more reactive they are.
3. Alkali metals (group 1) have 1 electron in their outermost energy level, the s sublevel, and they want to lose that electron, that is why alkali metals react vigorously with nonmetals, especially halogens, because halogens need 1 electron to be stable. All alkali metals react with water to produce hydrogen gas and substances called alkalis. Alkaline earth metals (group 2) are less reactive than alkali metals because alkaline earth metals have 2 electrons in the s sublevel. Because the main energy level is filled, they are less likely to lose or gain an electron.
4. Alkaline earth metals are elements of group 2 in the periodic table, so they have 2 electrons in outermost energy level. So to become stable they will try to lose 2 electrons to have a stable electron configuration. So they all have +2 oxidation states.
5. The metallic character of alkaline earth metals increases as you go down the group because the further down the group you go, the less ionization energy there is. The less ionization energy there
Period E Bautista, Angel
Table D Comer, Tyler
3/22/12 Sullivan, Brittany Truong, Phuoc
Conclusions and Questions
1. Step 1: Ca(s) +H2O->Ca (OH)2(aq)+H2(g) Step 4: Mg(s) +H2O->Mg (OH)2(aq)+H2(g) Step 10: CaSO4 + H2O-> Ca(OH)2 + H2SO4 MgSO4 + H2O ->Mg (OH)2 + H2SO4 Barium Sulfate: No reaction Step 13: MgCl2 + Na2CO3 -> MgCO3 + 2NaCl CaCl2 + Na2CO3 -> CaCO3 + 2NaCl BaCl2 + Na2CO3 -> BaCO3 + 2NaCl
2. The reactivity of the metal increases with each period it goes down. Magnesium is the least reactive and is in the third period with an atomic number of 12. Calcium is slightly more reactive being in the fourth period and having an atomic number of 20. Barium is the most reactive because it is in the sixth period and it has an atomic number of 56. So the farther down in the group they go the more reactive they are.
3. Alkali metals (group 1) have 1 electron in their outermost energy level, the s sublevel, and they want to lose that electron, that is why alkali metals react vigorously with nonmetals, especially halogens, because halogens need 1 electron to be stable. All alkali metals react with water to produce hydrogen gas and substances called alkalis. Alkaline earth metals (group 2) are less reactive than alkali metals because alkaline earth metals have 2 electrons in the s sublevel. Because the main energy level is filled, they are less likely to lose or gain an electron.
4. Alkaline earth metals are elements of group 2 in the periodic table, so they have 2 electrons in outermost energy level. So to become stable they will try to lose 2 electrons to have a stable electron configuration. So they all have +2 oxidation states.
5. The metallic character of alkaline earth metals increases as you go down the group because the further down the group you go, the less ionization energy there is. The less ionization energy there