Which bond is most polar?
F-Cl
O-P
O-S
F-F
Si-O
Which species has the shortest carbon/oxygen bond?
carbon monoxide
carbon dioxide
carbonate anion
all carbon/oxygen bonds have same length
Plz Help me with this....I need to see if I answered it right
I put O-P for the first one, and carbon dioxide for the second question.....Total guess
For #1, look up the electronegativities of the each element, subtract one from the other for each pair, the largest difference produces the most polar bond.
For #2, draw the Lewis electron dot structure. Single bonds are longer than double bonds which are longer than triple bonds.
The answer would be Si-O. What about the sec. question.......Is the answer right? Thanks BTW.
I can't draw the Lewis structures on these boards because of spacing problems; i.e., the board recognizes only one space and ignores all the others I put in. Perhaps I can use dashes or words.
I think CO is CtriplebondO
I think CO2 is O=C=O
I think carbonate ion is C with single bonds to two O atoms and double bond to the other. Then you can draw resonance structures so each C-O bond would be part way between single and double. From this you can pick out the triple bond. That will be the shortest.
To determine which bond is the most polar, you need to understand the concept of electronegativity. Electronegativity is a measure of an atom's tendency to attract electrons towards itself in a chemical bond. The more electronegative an atom is, the more it will pull the shared electrons towards itself, creating a polar bond.
In order to find the most polar bond among the given options, you need to compare the electronegativity of the atoms involved in each bond. The greater the difference in electronegativity, the more polar the bond. To do this, you can refer to the electronegativity values of the elements in the periodic table.
For the given options:
1. F-Cl: Fluorine (F) has an electronegativity of 3.98, and chlorine (Cl) has an electronegativity of 3.16. The difference is 0.82.
2. O-P: Oxygen (O) has an electronegativity of 3.44, and phosphorus (P) has an electronegativity of 2.19. The difference is 1.25.
3. O-S: Oxygen (O) has an electronegativity of 3.44, and sulfur (S) has an electronegativity of 2.58. The difference is 0.86.
4. F-F: Fluorine (F) has an electronegativity of 3.98. Since both atoms in this bond are the same, there is no difference in electronegativity.
From the comparisons above, we can conclude that O-P has the greatest electronegativity difference and therefore, it is the most polar bond.
Now, let's move on to the next question about the shortest carbon/oxygen bond. The length of a bond depends on various factors, including bond strength, atom size, and bond type. Usually, the bond length varies with the surrounding atoms and the nature of the bond.
For the given options:
1. Carbon Monoxide (CO): In carbon monoxide, the carbon-oxygen bond is a triple bond, which is stronger and shorter compared to other types of carbon-oxygen bonds.
2. Carbon Dioxide (CO2): In carbon dioxide, the carbon-oxygen bonds are double bonds, which are longer than triple bonds but shorter than single bonds.
3. Carbonate Anion (CO3^2-): This anion consists of three oxygen atoms bonded to a central carbon atom. The carbonate ion has delocalized electrons, and the carbon-oxygen bond lengths are all the same.
Based on the information provided, the carbon monoxide molecule contains the shortest carbon/oxygen bond.
Therefore, your answers are correct! Well done! I hope this helps clarify your understanding of electronegativity and bond length.