Sodium And Potassium Reaction Lab
Results and discussion:
I.
a. How would you compare that relative reactivity of Na and k
-Sodium and potassium react somewhat similar when reacting with water however they are slightly different. Sodium moves because of the hydrogen coming off of it and has a low melting point while potassium’s reaction is faster and enough heat is produced to set light to the hydrogen coming off of it. Each leaves a pink color hue in the water.
Discuss the similarities and differences in the behavior of the metals tested with water relative to their positions in the periodic table. Compare behavior within a family and in the same period.
- The similarities and differences between the metals tested with water that are relative to their position in the periodic …show more content…
table is that those that reacted, calcium, magnesium and sodium due to the fact that most of them are group one elements and thus making it easier for them to react producing more heat and reacting with the water. While non-metallic elements has more of a tendency to oxidize quickly rather then react so vigorously.
What would you predict to be the relative reactivity’s of cesium and lithium with water?
- Cesium metal reacts rapidly with water to form a colorless solution. The resulting solution is basic because of the dissolved hydroxide. The reaction is very exothermic. The reaction is so fast that if the reaction is carried out in a glass vessel, the glass container will shatter.
Compare the reactivates of group IIA and IIIA with dilute acids
II.
a) What color is the gas
-The gas is a bright orange color that is being emitted.
b) What color are the iodine crystals?
-The iodine crystals are a deep purple color.
What relationship can you draw between the molecular weight of the halogens and their physical state relate your answer to the principles developed in lecture concerning intermolecular forces of attraction.
-As the molecular weight of the halogens increases the intermolecular attraction amongst the molecules increases and the physical state changes from gas to solid.
A) Summarize your results by comparing the reactivity’s of the free halogen elements in relation to their positions in the periodic table
- Halogens are those of nature to oxidize very quickly and the oxidizing strength of the halogens increases in the same order from astatine to fluorine and since they have seven valance electrons it renders them as strong oxidizers considering they can still accept one electron in-group 17 to become stable like the noble gasses.
B) Which halogen is most likely to gain electrons and why
-Cl would be the most reactive due to the fact that it is all the way at the top of the group therefore it can gain electrons easier than those all the way at the bottom and it is the second most electronegative after fluorine.
C) Which halogens are least likely to gain electrons why?
-KI or I would be the least reactive due to the fact that the element is less reactive as you go down the group the electronegativity is decreasing and world not be as say to grab an electron like fluorine.
III.
What general conclusions can you draw concerning the acidity or basicity of the hydroxides of the elements of the third period?
- The main factor in determining the strength of the acid is how stable the anion is once the hydrogen has been removed.
This in turn depends on how much the negative charge can be spread around the rest of the ion.
Discuss general trends in metallic and non- metallic properties as shown by the experiment.
- Metal ions and elements tend to form positive ions and like charges repel therefore they can migrate and the fluid mosaic allows them to move around the atomic radius is half the distance between the two adjacent nuclei of atoms in a metal lattice. Metallic properties also are very exothermic and vigorously when heated.
Conclusion:
The elements are arranges due to their atomic weight, exhibiting an evident stepwise variation of properties. Chemically analogous elements have similar atomic weights or increase by equal increments. Within the period each elemtens reacts differently with a solution that it could be put in. This is due to either what group or period it is in and periodic trends also affect this. Whether the element is metallic or non metallic the elements differ. Metallic elements have higher atomic weight and radius while non-metallic have high electronegativity and ionization trends. With each being so different we tested each element given and saw what happened when dropped into a certain solution to determine how periodic trends related to this
experiment.
I.
a. How would you compare that relative reactivity of Na and k
-Sodium and potassium react somewhat similar when reacting with water however they are slightly different. Sodium moves because of the hydrogen coming off of it and has a low melting point while potassium’s reaction is faster and enough heat is produced to set light to the hydrogen coming off of it. Each leaves a pink color hue in the water.
Discuss the similarities and differences in the behavior of the metals tested with water relative to their positions in the periodic table. Compare behavior within a family and in the same period.
- The similarities and differences between the metals tested with water that are relative to their position in the periodic …show more content…
table is that those that reacted, calcium, magnesium and sodium due to the fact that most of them are group one elements and thus making it easier for them to react producing more heat and reacting with the water. While non-metallic elements has more of a tendency to oxidize quickly rather then react so vigorously.
What would you predict to be the relative reactivity’s of cesium and lithium with water?
- Cesium metal reacts rapidly with water to form a colorless solution. The resulting solution is basic because of the dissolved hydroxide. The reaction is very exothermic. The reaction is so fast that if the reaction is carried out in a glass vessel, the glass container will shatter.
Compare the reactivates of group IIA and IIIA with dilute acids
II.
a) What color is the gas
-The gas is a bright orange color that is being emitted.
b) What color are the iodine crystals?
-The iodine crystals are a deep purple color.
What relationship can you draw between the molecular weight of the halogens and their physical state relate your answer to the principles developed in lecture concerning intermolecular forces of attraction.
-As the molecular weight of the halogens increases the intermolecular attraction amongst the molecules increases and the physical state changes from gas to solid.
A) Summarize your results by comparing the reactivity’s of the free halogen elements in relation to their positions in the periodic table
- Halogens are those of nature to oxidize very quickly and the oxidizing strength of the halogens increases in the same order from astatine to fluorine and since they have seven valance electrons it renders them as strong oxidizers considering they can still accept one electron in-group 17 to become stable like the noble gasses.
B) Which halogen is most likely to gain electrons and why
-Cl would be the most reactive due to the fact that it is all the way at the top of the group therefore it can gain electrons easier than those all the way at the bottom and it is the second most electronegative after fluorine.
C) Which halogens are least likely to gain electrons why?
-KI or I would be the least reactive due to the fact that the element is less reactive as you go down the group the electronegativity is decreasing and world not be as say to grab an electron like fluorine.
III.
What general conclusions can you draw concerning the acidity or basicity of the hydroxides of the elements of the third period?
- The main factor in determining the strength of the acid is how stable the anion is once the hydrogen has been removed.
This in turn depends on how much the negative charge can be spread around the rest of the ion.
Discuss general trends in metallic and non- metallic properties as shown by the experiment.
- Metal ions and elements tend to form positive ions and like charges repel therefore they can migrate and the fluid mosaic allows them to move around the atomic radius is half the distance between the two adjacent nuclei of atoms in a metal lattice. Metallic properties also are very exothermic and vigorously when heated.
Conclusion:
The elements are arranges due to their atomic weight, exhibiting an evident stepwise variation of properties. Chemically analogous elements have similar atomic weights or increase by equal increments. Within the period each elemtens reacts differently with a solution that it could be put in. This is due to either what group or period it is in and periodic trends also affect this. Whether the element is metallic or non metallic the elements differ. Metallic elements have higher atomic weight and radius while non-metallic have high electronegativity and ionization trends. With each being so different we tested each element given and saw what happened when dropped into a certain solution to determine how periodic trends related to this
experiment.