True,
Okay to be honest, I'm not entirely sure, but I think its false because the larger the positive or negative charge of the ion, the greater lattice energy it has.According to the answers of similar questions, I think it's true.
A high hydration energy gives an increased solubility.
since ca2+ has a larger atomic radii compared to Mg2+ (and the same for F and CL2), the electrons are dispersed over a wider surface area and so have a lesser strength than that of magnesium. Hence, with a smaller atomic radii, Magnesium has stronger attractive forces with require more energy to be broken and therefore making it more exothermic than calcium.
5396kJ/mol
lattice energy.
Okay to be honest, I'm not entirely sure, but I think its false because the larger the positive or negative charge of the ion, the greater lattice energy it has.According to the answers of similar questions, I think it's true.
Lattice energy is directly related to the size of the ions bonded. Smaller ions generally have a more negative value for lattice energy because the nucleus is closer to and thus has more attraction for the valence electrons.
Ionic Charge and Ionic Radius - the smaller the radius the greater the lattice energy
Ionic Charge and Ionic Radius - the smaller the radius the greater the lattice energy
ionic charge and ionic radius; the smaller the ionic radius the greater the lattice energy
Ions release some amount of energy when they get together to form a lattice. If it is needed to be seperated into ions again, the same energy should be absorbed. The energy to break 1 mole of a lattice at the standard temperature and pressure is defined as the standard lattice energy. Using formulae, the lattice energy at any conditions can be found as the standard values are tabulated.
Ionic Charge and Ionic Radius - the smaller the radius the greater the lattice energy. The charge of the ions is what affects the lattice energy.
A high hydration energy gives an increased solubility.
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
Lattice energy increases with greater charge and smaller size. Since the charges are the same for both compounds, you have to look at the sizes of the atoms, K and Na, and since both have Cl, you don't have to compare that with anything. K is larger than Na, so since NaCl has a smaller size and the same charge, it has higher lattice energy.
The lattice energy of potassium bromide is more exothermic than the lattice energy of rubidium iodide because lattice energy is inversely proportional to atomic radius.
it releases lattice energy