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?
Exactly 222 kJ/mol
Exactly 444 kJ/mol
More than 222 kJ/mol
Less than 222 kJ/mol
I chose "More than 222 kJ/mol", is this correct?
I agree. Do you have a reason for your answer? It's important to know why.
Yes, you are correct. Silicon and carbon are both in Group 14 of the periodic table, which means they have similar electronic configurations and can form similar types of chemical bonds. However, the energy required to break a bond can depend on various factors such as bond length and strength.
Since silicon-silicon single bonds require 222 kJ/mol of energy to break, it is reasonable to assume that carbon-carbon single bonds would require more energy to break. Carbon-carbon single bonds are typically stronger than silicon-silicon single bonds due to carbon's smaller atomic size and higher electronegativity. Therefore, it would take more than 222 kJ/mol of energy to break a carbon-carbon single bond.
Hence, your choice of "More than 222 kJ/mol" is correct.