State whether each of these statements is true or false. (a) The longer the bond, the stronger the bond. (c) A typical double bond length is in the 500–1000 pm range.

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welcome back everyone were asked is the carbon carbon bond stronger between Athene or ethane And we have to explain why. So we're going to begin by recalling that when it comes to a greater average bond order that will correspond to a greater or stronger we can say bond strength and also corresponds to a shorter bond length. So we're going to need to draw out the structures of ethane and methane. So beginning with a thin C two H four, we wanna in order to draw its lewis structure, calculate total valence electrons. We would recognize that on our periodic table. Carbon is located in Group four a corresponding to four valence electrons. And we see that in the formula we have two atoms of carbon. So that would give us a total of eight electrons from carbon. And now we would find hydrogen on our periodic tables in group one a corresponding to one valence electron multiplied by our four atoms of hydrogen which would give us again four electrons. And adding to this, we have a total of 14 valence electrons. Or sorry, we have a total of 12 valence electrons here. So we're going to use this to draw our structure according to our formula, we have two carbon atoms in the center surrounded by four hydrogen atoms. We're going to begin by making the base connections between our atoms. So we would have a bond between carbons which we would recall a bond uses of two electrons and then connecting our hydrogen atoms to the carbons. We have 2468, 10 of our 12 electrons that we've used up. So we would say -10. And that leaves us with two more electrons left and right now we can count a total of three bonds on each of our carbon atoms. However, we want to recall that carbon has a bonding preference. So let's note this down. The bonding preference of carbon Is going to have a carbon with four bonds so that it has a full octet. And so we would go ahead and place a double bond between our two carbon atoms to use up our last two electrons. And so this would be our structure for 18. And we want to see that because we have a carbon carbon double bond, this corresponds to a bond order. That is equal to a value of two. So now we want to compare this to the bond order of our bond in our ethane structure. So let's go ahead and draw that out below. We'll use a different color now. So for ethane we have C two H six as our formula, meaning that for total valence electrons we would just add two more From our previous count for Athene which was 12. And so this would give us a total of 14 valence electrons. So, drawing out our structure for ethane, we have C two surrounded by six hydrogen. So we have one there, a second here, the third here of fourth here and then our last 5th and 6th hydrogen atoms here. Let's begin by making our base connections. Where we would use 2468, 10, 12, 14 Of all of our 14 valence electrons. And so this structure only has a carbon carbon single bond. And we would recall that from our notes that a carbon carbon, carbon single bond has a bond order of just one. And so we would say that the bond order of our ethane C two H six is less than the bond order of our Athene C two H four. And so therefore we would say that our carbon carbon bond in death in C two H four, it's stronger then in Ethane C2 Age six because it has a higher bond order, Which we calculated to be two. And so this entire statement is going to be our final answer. To complete this example. I hope that everything I reviewed was clear. If you have any questions, leave them down below and I'll see everyone in the next practice video

State whether each of these statements is true or false. (a) The longer the bond, the stronger the bond. (c) A typical double bond length is in the 500–1000 pm range.

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Key Concepts

Bond Length and Strength

Types of Chemical Bonds

Bond Length Measurements