Read the two passages.
Silicon is an element that is directly below carbon on the periodic table. Silicon can form bonds similar to carbon.
Silicon-silicon single bonds require 222 kJ/mol of energy to break.
Based on the statements, how much energy would it take to break a carbon-carbon single bond?
more than 222 kJ/mol
exactly 444 kJ/mol
exactly 222 kJ/mol
less than 222 kJ/mol
To answer the question, we need to understand the relationship between silicon and carbon on the periodic table and how they form bonds.
The first passage states that silicon is directly below carbon on the periodic table. In a simplified view, elements in the same column on the periodic table tend to have similar chemical properties. Therefore, silicon and carbon have some similarities in their bonding behavior.
The second passage mentions that silicon-silicon single bonds require 222 kJ/mol of energy to break. This information provides a specific value for the energy required to break silicon-silicon single bonds.
Now, let's apply this information to carbon-carbon single bonds. Since silicon and carbon are similar, it is reasonable to assume that carbon-carbon single bonds would have a similar energy requirement to break.
Therefore, based on the given information, the energy required to break a carbon-carbon single bond would also be approximately 222 kJ/mol. Hence, the correct answer is "exactly 222 kJ/mol."