true ;)
Yes
Lattice Energy
Bond enthalpy is the energy required to break a chemical bond whereas lattice energy is the enthalpy of formation of one mole of an ionic compound from gaseus ions under standard conditions.
The bonds in compound A are stronger than the bonds in compound B.
Bromine is a molecular compound Br2 and the intermolecular forces are london dispersion forces. Potassium chloride is an ionic compound forming a lattice with strong electrostatic forces holding the lattice together. Less thermal energy is required to shake solid Br2 apart than that required for KCl
The crystal lattice that is formed has a lower potential energy than the reactants. This is because energy is expended to create the ionic compound.
Lattice Energy
Lattice energy is energy required to separate ions to infinite distance with no more interaction. Cohesive energy is energy required to separate atoms to infinite distance with no more interaction.
what role does lattice energy play in forming an ionic compound?
Definitions of lattice energy: * The energy released when one mole of a crystal is formed from gaseous ions.misterguch.brinkster.net/vocabulary.html * The energy for the reaction of the infinitely separated ions to give the solid. It measures the electrostatic interaction between the ions.www.everyscience.com/Chemistry/Glossary/L.php * The energy given off when oppositely charged ions in the gas phase come together to form a solid. For example, the energy given off in the following reaction: Na + (g) + Cl - (g) NaCl(s).xenon.che.ilstu.edu/genchemhelphomepage/glossary/l.html * Lattice energy deals primarily with metals. The lattice energy, or lattice enthalpy, of an ionic solid is a measure of the strength of bonds in that ionic compound. It is given the symbol U and is equivalent to the amount of energy required to separate a solid ionic compound into gaseous ions. ...en.wikipedia.org/wiki/Lattice energy the lattice energy of an ionic solid is a measure of the strength of bods in that ionic compound. it is usually defined as the enthalpy of formation of ionic compound from the gaseous ions and as such is invariably exothermic
Bond enthalpy is the energy required to break a chemical bond whereas lattice energy is the enthalpy of formation of one mole of an ionic compound from gaseus ions under standard conditions.
Because the electrostatic force of attraction between opposite charges increases as the distance between the charges decreases, smaller ions produce stronger inter ionic attractions and greater lattice energies. When attraction between ions increases and the charge of the ion increases , the lattice energy increases. Down the groups in periods the lattice energy decreases
When a salt, such as NaCl dissolves in water, the crystals disappear on the macroscopic scale. On the atomic scale, the Na+ and Cl- ions in the crystal are released into solution.NaCl(s) H2O Na+(aq) + Cl-(aq)The lattice energy of a salt therefore gives a rough indication of the solubility of the salt in water because it reflects the energy needed to separate the positive and negative ions in a salt.It also tells how stronger the ion is.
The bonds in compound A are stronger than the bonds in compound B.
An estimate of the strength of the bonds in an ionic compound can be obtained by measuring the lattice energy of the compound, which is the energy given off when oppositely charged ions in the gas phase come together to form a solid.
The crystal lattice that is formed has a lower potential energy than the reactants. This is because energy is expended to create the ionic compound.
Bromine is a molecular compound Br2 and the intermolecular forces are london dispersion forces. Potassium chloride is an ionic compound forming a lattice with strong electrostatic forces holding the lattice together. Less thermal energy is required to shake solid Br2 apart than that required for KCl
The lattice energy of an ionic solid is a measure of the strength of bonds in that ionic compound. It is usually defined as the enthalpy of formation of the ionic compound from gaseous ions and as such is invariably exothermic. The concept of lattice energy has initially been developed for rocksalt-structured and sphalerite-structured compounds like NaCl and ZnS, where the ions occupy high-symmetry crystal lattice sites. In case of NaCl, the lattice energy is the energy released by the reaction