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Explain why the theoretical lattice energies become less exothermic from AgF to AgI?
The decrease in exothermicity in theoretical lattice energies from AgF to AgI is mainly due to the decrease in the charge density of the anions as you move from fluoride to iodide. The larger iodide ions are less able to polarize in response to the cation, resulting in weaker electrostatic interactions and a less exothermic lattice energy.
Is the side centered cube a bravais lattice?
Hi, No the side centered lattice is not a Bravais Lattice as the lattice doesn't look the same from an atom on the corner of the cube and an atom in the middle of a vertical edge of the cube (they don't even have the same number of neighbors). In fact, the side centered lattice is a simple cubic lattice with a basis of two atoms.
What is the difference between adhesive and cohesive forces in materials?
Adhesive forces are the attraction between different substances, while cohesive forces are the attraction between molecules of the same substance.
What are the properties of a hexagonal lattice and how does it differ from other types of lattice structures?
A hexagonal lattice is a type of lattice structure that has six-fold rotational symmetry and consists of repeating hexagonal units. This lattice has properties such as high packing efficiency and isotropy, meaning that it looks the same in all directions. One key difference between a hexagonal lattice and other types of lattice structures, such as square or cubic lattices, is the arrangement of atoms or particles. In a hexagonal lattice, the units are arranged in a hexagonal pattern, while in other lattices, the units are arranged in square or cubic patterns. This difference in arrangement affects the overall symmetry and properties of the lattice structure.
How does lattice energy change with a change in the size of an ion?
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
How do the lattice energies of different ionic compounds compare in terms of their stability and bonding strength?
The lattice energies of different ionic compounds vary in terms of their stability and bonding strength. Compounds with higher lattice energies are more stable and have stronger bonding compared to compounds with lower lattice energies.
What is cohesive energy in case of NaCl?
If you think to lattice energy the value is 789 kJ/mol.
Born haber cycle n its applications?
it is used for calculating lattice energies of different ions.
What type of bonding is Copper metal lattice?
Copper metal lattice is held together by metallic bonding. In metallic bonding, electrons are delocalized and free to move throughout the lattice, creating a structure with strong cohesive forces.
How lattice energy affect solubility?
Lattice energy is the energy required to separate ions in a solid state, which influences the solubility of a compound in a solvent. Compounds with higher lattice energies tend to be less soluble in a solvent because it requires more energy to break the ionic bonds and dissolve the compound. Conversely, compounds with lower lattice energies are typically more soluble in a solvent as it is easier to overcome the forces holding the compound together.
What are the lattice energies of barium sulphate and calcium carbonate and how do they relate to dissolution in acids?
don't know xd
How can one determine the highest lattice energy in a compound?
The highest lattice energy in a compound can be determined by considering the charges of the ions involved and their sizes. Generally, compounds with ions that have higher charges and smaller sizes will have higher lattice energies.
Explain why the theoretical lattice energies become less exothermic from AgF to AgI?
The decrease in exothermicity in theoretical lattice energies from AgF to AgI is mainly due to the decrease in the charge density of the anions as you move from fluoride to iodide. The larger iodide ions are less able to polarize in response to the cation, resulting in weaker electrostatic interactions and a less exothermic lattice energy.
How would you compare the crystal lattice energy compared to the energies of the neutral atoms forming the ionic compound?
The crystal lattice energy is the energy released when ions come together to form a crystal lattice structure. It is typically much larger in magnitude compared to the energies required to separate the neutral atoms into individual ions. This is because the crystal lattice energy includes both the ionization energy and electron affinity of the atoms involved.
If the lattice energy of compound A is greater than compound B is A an ionic compound?
Not necessarily. Lattice energy is a measure of the strength of the forces holding ions together in a solid crystalline structure. While ionic compounds generally have higher lattice energies due to strong electrostatic forces between ions, there are covalent compounds with high lattice energies as well. It's important to consider other factors like electronegativity and bond type to determine if a compound is ionic.
How can one determine lattice energy using information from the periodic table?
Lattice energy can be determined using information from the periodic table by looking at the charges of the ions involved in the ionic compound. The higher the charges of the ions, the greater the lattice energy. Additionally, the size of the ions also plays a role, with smaller ions having higher lattice energies.
Determining lattice energy from Born-Haber cycle data requires the use of?
various thermodynamic data including enthalpies of formation, ionization energies, electron affinities, and dissociation energies. These data are used to calculate the overall energy change associated with the formation of an ionic compound from its elements. The lattice energy is the energy required to separate ions in a solid crystal structure into infinitely separated gaseous ions.
