Yes, a stronger bond requires more energy to break, and also releases more energy when it is made. In a chemical reaction, if you are breaking strong bonds, and only making weak ones, the reaction will require a lot of energy (endothermic). If instead you are breaking weak bonds and making very strong ones in the products, the reaction will release energy (exothermic).
Greater the bond strength, greater is the bond dissociation energy. (So they are proportional to each other).
They are the same
Bond energy is a defined quantity, the amount of energy to convert 1 mole of compound into its constituent atoms, bond strength is not a strictly defined entity, it is sometimes used as a synonym for bond energy. Spectroscopists talk of bond strength and relate this to the resonant frequency of functional groups in say the IR/Raman spectra.Bond energy is the energy that is needed to break down one mole. Bond strength is the degree that is in a atom.
The strength of the bond increases as the bond dissociation energy increases.
Polarity is related to bond strength because the bigger the difference in electronegativity, the higher the bond energy will be. This will then give rise to a much stronger bond.
Bond energies are the measure of strength of a chemical bond. The larger the bond energy, the stronger the bond.
Lattice Energy :)
It is measured the energy in kJ/mol.
Enthalpy is the measurement of total energy change of a reaction. The energy of bond formation and bond breaking can be used to calculate the bond enthalpy of the reaction. Bond enthalpy is the enthalphy change when 1 mol of bond is broken. Therefore the general equation to calculate the enthalpy change is energy of bond broken subtract by energy of bond formation.
The strength of a chemical bond is equivalent to the energy that is released when that bond is formed, and that is called the heat of formation. It is measured in calories per mole.
That this bond is strong and needs a higher influx of energy to have disassociation happen.
The energy needed to break one mole of bonds. A large bond dissociation energy corresponds to Strong covalent bond. They are unreactive partly because this dissociation energy for each of these bonds is high
Metallic bond strength refers to the amount of energy as heat required to vaporize the metal. The enthalpy of vaporization is defined as the amount of energy absorbed as heat when a specified amount of substance vaporizes at constant pressure. Metallic bond strength increases as the enthalpy increases.
two factors that effect bond energy are polarity of molecule or compound and size of molecule
potential energy decreases when bond is made, increases when broken
Bond energy is a measure of the strength of a chemical bond, that is the amount of energy required to break a bond. The larger the bond energy, the stronger the bond. For covalent bonds, bond energies and bondlengths depend on many factors: electron afinities, sizes of atoms involved in the bond, differences in their electronegativity, and the overall structure of the molecule. There is a general trend in that the shorter the bondlength, the higher the bond energy and the stronger the bond.
Molar bond enthalpy shows the change in a bond association. For example, if one mole of bond is broken, the energy change that results is DHd (degree).
The energy of each o the bonded atoms decreases when such a bond is formed.
Bond dissociation enthalpy (BDE) is a measure of how much energy is required for a bond to break in a molecule or compound. This can be quite low, e. a C-H bond, or extremely high, like a N-N triple bond, which needs almost 1000 kJ mol-1 of energy to break the bond.
Order of bond strength from lowest to highest:Van der Waals
they release energy!
yes. greater the bond order, greater the strength of the bond between the two atoms.