Answer:
CO HAS A TRIPLE BOND WHILE C-O BOND IN CO2 IS A DOUBLE BOND
CO HAS A LONE PAIR ON CARBON WHILE CO2 DOES NOT
Explanation:
Bond dissociation bond enthalpy or energy is the energy needed to break 1 mole of a divalent molecule into separate atoms mostly in the gaseous state.
The carbon and oxygen in carbon monoxide form a triple bond as carbon monoxide has 10 electrons in their outermost shell which results into six shared electrons in 3 bonding orbitals as against the double bond formed by other carbon compounds. Four electrons come from oxygen and the remaining two from carbon and due to this, two electrons from oxygen will occupy one orbital and this forms a dative bond. Also because of the triple bond, carbon monoxide is often regarded as a more stable compound than carbon dioxide with a double bond. This gives it its higher bond dissociation enthalpy value and more energy is needed to break it into its separate atoms. This is in conjunction with a larger bond length similar to the bong length in a triple bond. This makes it more stronger than the bond dissociation enthalpy of carbon dioxide having a double bond.
In chemistry, a valence electron is an outer shell electron that is associated with an atom, and that can participate in the formation of a chemical bond if the outer shell is not closed; in a single covalent bond, both atoms in the bond contribute one valence electron in order to form a shared pair.
It forms magnesium nitride
Answer:
4.2 mol NH3
Explanation:
First, balance your reaction.
N2 + 3H2 --> 2NH3
Multiply 6.3 mol H2 by the mole ratio of 2 mol NH3 for every 3 mol H2 to get moles of NH3 produced.
6.3 mol H2 • (2 mol NH3 / 3 mol H2) = 4.2 mol NH3
Answer:
Being a covalent compound, the intermolecular forces between the Cl2O molecules are weak and easily overcome. Therefore little heat energy, in terms of low boiling point is involved.
