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(Solved) Ali 1 Muhammad Ali Mr. Tyler SCH4U0 Monday, March 27, 2017 Ionic and Covalent Properties: Lab Purpose: The purpose of this experiment is to observe...


Hi there! I need guidance in how to improve my lab report for Ionic and Covalent Properties. I've gotten feedback from teacher and he gave me a few suggestions on how to improve it. This is the feedback I have received:

Good job overall, just looking for a little more detail in a few areas:

  • :you want to explain the trends you observed in melting point and conductivity in solution the same way you did for solubility in water
  • :you also want to explain why sucrose dissolved in water while the other covalent compounds did not

In general, you want to remember that we're looking for your ability to connect theory to observations in these labs. Always provide explanations/conclusions in terms of what you've learned from the course material.

---I have attached my lab so you can see whats it about. Thanks.

Ali 1
Muhammad Ali
Mr. Tyler
SCH4U0
Monday, March 27, 2017
Ionic and Covalent Properties: Lab
Purpose:
The purpose of this experiment is to observe properties of various compounds and identify those
properties as either primarily ionic or primarily covalent.
Data Table: Questions:
1. Determine whether each of the compounds is ionic or covalent.
o Benzoic Acid (6H5COOH): Covalent
o Magnesium Chloride (MgCl2): Ionic
o Paradichloro benzene (C6H4Cl2): Covalent Ali 2
o Potassium chloride (KCl): Ionic
o Sucrose (C12H22O11): Covalent
o Magnesium nitrate Mg (NO3)2: Ionic
2. Look at the results carefully. Are there any patterns that you have observed in the
property of solubility? Explain.
One of the patterns that I have observed in the property of solubility was that all covalent
compounds are not soluble in water and that all ionic compounds are soluble in water. By
saying that all ionic compounds are soluble in water, what I mean is that all ionic compounds
are soluble in water to a certain extent and that the degree of solubility varies. This is due to
the polarity of the water (because water is polar). The positive hydrogen atoms of the water
molecule attract to the anion on the surface of the solid ionic compounds while the negative
oxygen atoms are attracted towards the cation; forming bonds with anion and cation. This
allows the anion and cation to attract one another and dissolve and become soluble in water.
3. Similarly, look at the other properties. What can you say about each of the other
properties: melting point and electrical conductivity in relation to the ionic or
covalent character of the compounds? Melting Point
Solubility Ionic
High melting point
Soluble: Dissolves in water Electrical conductivity Conducts electricity Covalent
Low melting point
Non-soluble: Does not dissolve
in water
Does not conduct electricity 4. Predict the following:
a. Solubility of sodium iodide in water
NaL is an iconic compound since its composed of a metal and non-metal. As a result,
it would dissolve very well in water since iconic compound have good water solubility.
b. Melting point of sodium iodide
The melting point of Sodium Iodide depends on the amount of NaL we have knowing
that it won’t melt until the temperate reaches a high point. Since we already know that
Ionic Solids have a high melting point, its melting point would be close to 661 Celsius.
c. Electrical conductivity of a glucose solution
Glucose would not conduct electricity since it is a covalent compound: It would not
dissociate into ions when dissolved in water resulting in glucose being considered as
a nonelectrolyte without any electrical conductivity. Ali 3
FEEDBACK: Hi Muhammad:
Good job overall, just looking for a little more detail in a few areas: you want to explain the trends you observed in melting
point and conductivity in solution the same way you did for
solubility in water you also want to explain why sucrose dissolved in water
while the other covalent compounds did not
In general, you want to remember that we're looking for your
ability to connect theory to observations in these labs. Always
provide explanations/conclusions in terms of what you've
learned from the course material.

 


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