∆H (enthalpy change) should be positive because you would need energy to break the oxygen- oxygen bond to generate 2 molecules of Oxygen .
<h3>What is enthalpy change ?</h3>
It is type of energy or the measurement of energy . The quantity of enthalpy equals to the total content of heat of a system .
It can be defined as the sum of total internal energy and the product of volume and pressure .
It describes the system is endothermic or exothermic .
<h3>What is exothermic reaction? </h3>
It is a reaction in which energy is released from the system in the form of heat and light.
in this loss of energy occurs. energy liberated from system to surrounding. the enthalpy change i.e. ∆H<0.
<h3>
What is endothermic reaction? </h3>
It is a reaction in which energy is absorbed from the surrounding to the system. in this gain of energy occurs. the enthalpy change i.e ∆H>0.
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I don't not know I did not learn this yet
Answer:
B) The molecular orbital formed is lower in energy than a hydrogen 1s atomic orbital.
Explanation:
When two atoms of hydrogen come close to each other , there is formation of molecular orbital . Due to overlap of 1 s orbital of one and 1 s orbital of another atom , two molecular orbitals are formed . One of these molecular orbital has energy less than 1 s atomic orbital . It is called 1 s sigma bonding molecular orbital . The other molecular orbital has energy more than 1 s atomic orbital . It is called antibonding molecular orbital . Two electrons occupy bonding sigma molecular orbital .
So , the statement that "the molecular orbital formed is lower in energy than a hydrogen 1s atomic orbital " is wrong .
