Explain why the melting points of ionic compounds and molecular compounds differ?
The melting points of ionic compounds and molecular compounds differ because....
-A tremendous amount of energy (heat transfer) is required to separate the tightly bound ions in solid ionic compounds (better known as melting).
-Since the attractive forces between covalent molecules are relatively weak, they are easy to separate.
I have the answers here, but I would like some help putting this all together, because I don’t get how to start answering from because.
Thanks in advance.
I would use something like this.
http://hyperphysics.phy-astr.gsu.edu/hbase/chemical/bond2.html
When in a solid form, NaCl (salt) is a neutral compound. When dissolved in water the ions dissociate (break apart) to form Na+ and Cl-. How does this explain why salt can conduct electricity when dissolved but not in solid form? _______________________________________________
No problem! Let's break it down step by step.
First, we need to establish the contrast between ionic compounds and molecular compounds. Ionic compounds are formed by the transfer of electrons between a metal and a nonmetal, resulting in the formation of positively charged metal ions and negatively charged nonmetal ions. On the other hand, molecular compounds consist of covalent bonds between nonmetals, where the atoms share electrons to achieve a stable electron configuration.
Now let's tackle the explanation.
1. Start with the statement: "The melting points of ionic compounds and molecular compounds differ."
2. Next, introduce the reason for this difference by saying, "This is because of the unique properties of each type of compound."
3. Then, provide the first reason for the difference: "In the case of ionic compounds, a tremendous amount of energy (heat transfer) is required to separate the tightly bound ions in solid ionic compounds."
4. Explain why this is the case: "Ionic compounds have strong electrostatic forces of attraction between positively and negatively charged ions. Melting an ionic compound requires breaking these bonds, which demands a significant input of energy."
5. Now, shift your focus to molecular compounds: "On the other hand, the attractive forces between covalent molecules in molecular compounds are relatively weak."
6. Elaborate further to explain why: "Covalent bonds involve the sharing of electrons between atoms, resulting in weaker intermolecular forces compared to the strong electrostatic forces in ionic compounds."
7. Wrap up by summarizing: "As a result, molecular compounds have lower melting points compared to ionic compounds since their intermolecular forces are easier to overcome."
To summarize, you can start by stating the difference in melting points between ionic and molecular compounds, then explain how the distinct bonding types and the strength of their intermolecular forces contribute to this difference.