enthalpy of atomisation help please

https://en.wikipedia.org/wiki/Enthalpy_of_atomization
"Enthalpy of atomization is the amount of enthalpy change when a compound's bonds are broken and the component atoms are reduced to individual atoms.
Enthalpy of atomization is denoted by the symbol ΔHa. The enthalpy change of atomization of gaseous H2O is, for example, the sum of the HO–H and H–O bond dissociation enthalpies.
The enthalpy of atomization of an elemental solid is exactly the same as the enthalpy of sublimation for any elemental solid that becomes a monatomic gas upon evaporation.
When a diatomic element is converted to gaseous atoms, only half a mole of molecules will be needed, as the standard enthalpy change is based purely on the production of one mole of gaseous atoms. When the atoms in the molecule are different isotopes of the same element the calculation becomes non-trivial."

Enthalpy change of atomisation of an element is defined as the enthalpy change which accompanies the formation of one mole of gaseous atoms from its element in its standard state
Enthalpy of atomization of a compound is the amount of enthalpy change when the compound's bonds are broken and the component atoms are reduced to individual atoms.


so
CH4(g) -----> C(g) + 4H(g) yes
H2 (g) ------> 2H (g) no
1/2 H2(g) -> H (g) yes

Thank you, I understand why H2(g) ----> 2H(g) isn't an example of atomisation, but I still don't really understand how CH4 (g) ----> C(g) + 4H(g) is an example of atomisation as 4 moles of H(g) are being produced?

"Enthalpy of atomization is the amount of enthalpy change when a compound's bonds are broken and the component atoms are reduced to individual atoms.
Enthalpy of atomization is denoted by the symbol ΔHa. The enthalpy change of atomization of gaseous H2O is, for example, the sum of the HO–H and H–O bond dissociation enthalpies.
The enthalpy of atomization of an elemental solid is exactly the same as the enthalpy of sublimation for any elemental solid that becomes a monatomic gas upon evaporation.
When a diatomic element is converted to gaseous atoms, only half a mole of molecules will be needed, as the standard enthalpy change is based purely on the production of one mole of gaseous atoms. When the atoms in the molecule are different isotopes of the same element the calculation becomes non-trivial."
Particularly, look at
"Enthalpy of atomization is the amount of enthalpy change when a compound's bonds are broken and the component atoms are reduced to individual atoms.

Enthalpy of atomization is denoted by the symbol ΔHa. The enthalpy change of atomization of gaseous H2O is, for example, the sum of the HO–H and H–O bond dissociation enthalpies."

It is because all bonds in 1 mole of CH4 are broken to form consitituent (individual) atoms

But more than 1 mole of gas is produced

There are different definitions to be considered:
1. The enthalpy change of atomisation for an element is the enthalpy change when 1 mole of gaseous atoms are formed from the element in its standard state, under standard conditions e.g 1/2H2(g) -> H(g)
2. The enthalpy change of atomisation for a compound is the enthalpy change when 1 mole of the compound in its standard state is reduced to its constituent gaseous atoms, under standard conditions. e.g CH4(g) -> C + 4H

The enthalpy change of atomisation for an element is different to that of the enthalpy change of atomisation for a compound.