Please post 2 or more peer responses
In the response posts, remember to demonstrate you have read and understood the student’s post by taking their discussion to the next level through your responses to the following:
· Identify the poster’s two additional molecules as ionic or covalent and then name them according to IUPAC rules.
· Discuss how you identified each as ionic or covalent and how you named each.
· Provide the common name for each molecule, if possible.
· Explain each molecule, how it can be used, or where it is found.
Please be sure to validate your opinions and ideas with citations and references in APA format.
Estimated time to complete: 2 hours
Response posts are worth
50% of your grade for this discussion.
Please review the initial post/response instructions
and
the rubric for this discussion to ensure that your response meets the criteria.
Ionic and Covalent bonding
· When it comes to ionic and covalent bonding, they differ in more ways then they are similar. For instance, their similarities are as follows:
-They both are types of bonding
-They both are relatively strong bonds, in comparison to London Dispersion
-They both go by the Octet Rule, as in they both strive to form an octet, have 8 valence electrons, and be like noble gases.
·
Covalent Bond Characteristics
-They do not always share electrons equally
-Covalent bonds can be polar and non polar
-The electronegativity difference for polar bonds is: <0.4
-The electronegativity difference for non polar bonds is between 0.4 and 2.0.
-Lewis structures are used to indicate the formation of covalent bons
-They are stronger bonds than ionic
-Shared between two non metals
-They used these bonds to fill their valence shells to gain stability
-They can form one to six covalent bonds
-Due to this stability that they gain from filling their valence shells, they tend to have lower melting and boiling points, and be gases.
-They do not conduct electricity
-The electrons that they share, are the valence electrons of each element.
-Example 1 of a covalent bond:
Formula: HCl
IUPAC Name: Hydrogen Chloride
Common Name: Hydrochloric Acid
·
Ionic Bond Characteristics
-Formed between a metal and a non metal
-These bonds occur between ions
-There is a larger difference in electronegativity when compared to covalent bonds, for instance, >2.0 Electronegativity difference denotes ionic bonding.
-When naming Ionic bonds, you remove the ending of the second element and replace it with “-ide.”
-Not as strong of a bond as covalent
-Example of an ionic bond:
Formula: KI
IUPAC Name: Potassium Iodide
· Additional Formulas without denoting their Bonds:
SO2 and
CaF2
References
Dillon, S. R. (n.d.).
Ionic and Covalent Bonding. Ionic and covalent bonding.
to an external site.
Realizeit Learning Content (n.d.).
Covalent and Ionic Bonding.
to an external site.
Ionic and covalent bonds are two different types of chemical bonds. The similarities of the two differing bonds are that they both: use valence electrons to form the bonds, give elements stability, and use electronegativity but differently for compounds (Helmenstein, 2020). There are more differences in the two bonds than similarities. In most circumstances, they appear to be opposite of one another.
Ionic bonds are formed between metals and nonmetals that have opposite charges that are attracted to one another. The ionic bond always donates an electron to the nonmetal element. Ionic bonds have a high melting point, polarity, and boiling point, and dissolve in water (Diffen, n.d.). Covalent bonds are formed between two nonmetals and share electrons to meet the need for stability. There are different types of covalent bonds. The bonds can be single, double, or triple in formation. The covalent bond has a lower melting point, lower polarity, and boiling point, and varies whether it dissolves in water (Diffen, n.d). An example of an ionic bond is NaCl, Sodium chloride. An example of a covalent bond is CH4, Methane.
Formulas: Ca3P2 & CO
References
Diffen. (n.d.). Covalent bonds vs. ionic bonds.
Helmenstein, A. (2020). Ionic and covalent bonds: understand the difference.
