Answer: +35
explanation: 30+35£~£
Answer:
The energy need to break this 0=0 bond is 495 kJ/mol
Explanation:
Step 1: Data given
oxygen molecule = O2
In an O2 molecule, the 2 O-atoms are held together by a double bond with a bond energy of 495 kJ/mol.
To break this chemical bound, it requires energy
2O(g) → O2(g)
The bound energy of a double oxygen bound = 495 kJ/mol
Since we have 1 molecule (consisting in 2 O atoms)
The energy need to break this 0=0 bond is 495 kJ/mol
Answer:
Potassium < lithium < Selenium < Oxygen
Explanation:
Oxygen has the highest electronegativity value from the given choices.
Electronegativity of an element is a property that combines the ability of its atom to lose and gain electrons.
It is a measure of the relative tendency with which atoms of the element attracts valence electrons in a chemical bond.
- Down a group, electronegativity reduces and across the period from left to right, it increases
Potassium and lithium are in group 1 , selenium and oxygen are group 7;
So group 1 elements will have lower electronegativity value.
Potassium is below lithium in group 1 and its electronegativity value will be lower.
Selenium is below oxygen and also, its electronegativity value is lesser.
Answer:
A: Antibonding molecular orbitals are higher in energy than all of the bonding molecular orbitals.
Explanation:
Molecular orbital theory describes <u>covalent bonds in terms of molecular orbitals</u>, which result from interaction of the atomic orbitals of the bonding atoms and are associated with the entire molecule.
A bonding molecular orbital has lower energy and greater stability than the atomic orbitals from which it was formed. An antibonding molecular orbital has higher energy and lower stability than the atomic orbitals from which it was formed.
Electrons in the antibonding molecular orbital have higher energy (and less stability) than they would have in the isolated atoms. On the other hand, electrons in the bonding molecular orbital have less energy (and hence greater stability) than they would have in the isolated atoms.
