a) K+ is common is all, the only difference is
anions, all are same group anions and down the group, size
increases, the order of the size of anions will be: F-
< Cl- < Br- < I-
hence, overall size order will be: KF < KCl < KBr < KI
(increasing order of size)
b) Lattice energy depends on the inter-ionic distance between
cations and anions, smaller the distance between them, stronger
will be the force of attraction, hence higher will be lattice
energy of the compound.
as F is smallest while I is largest,
therefore, the distance between cation and anion will be smallest
in KF and largest in KI,
thus, increasing order of lattice energy will be: KI < KBr <
KCl < KF
In an ionic compound, the size of the ions affects the internuclear distance (the distance between...
In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, arrange these compounds by their expected lattice energy. Note that many sources define lattice energies as negative values. Please arrange by magnitude and ignore the sign. attice energyl absolute value of the lattice energy Greatest lattice energy (strongest bonds) Least lattice...
In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, rank these compounds of their expected lattice energy.. Note: Many sources define lattice energies as negative values. Please rank by magnitude and ignore the sign. |Lattice energy| = absolute value of the lattice energy. RbCl ,RbBr ,Rbl ,RbF
In an ionic compound, the size of the ions affects the internuclear distance (the distance between the centers of adjacent ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, arrange these compounds by their expected lattice energy. Note that many sources define lattice energies as negative values. Please arrange by magnitude and ignore the sign. ∣∣lattice energy∣∣=absolute value of the lattice energy RbCl, RbI, RbBr, RbF
ILLIU, DUE VULLS LLLLLLL ions), which affects lattice energy (a measure of the attractive force holding those ions together). Based on ion sizes, arrange these compounds by their expected lattice energy Note that many sources define lattice energies as negative values. Please arrange by magnitude and ignore the sign. lattice energy = absolute value of the lattice energy Greatest lattice energy (strongest bonds) Least lattice energy (weakest bonds) Answer Bank Oci KC RC LICI Naci bo ply m e contact...
The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic attraction holding that compound together. Based on ion charges and relative ion sizes, arrange these ionic compounds by their expected melting points. Highest melting point MgF2 NaF Mgo KBr Lowest melting point Answer Bank
The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic attraction holding that compound together. Based on ion charges and relative ion sizes, arrange these ionic compounds by their expected melting points. Highest melting point KF CaF, RbBr Cao Arrange the compounds from highest melting point to lowest melting point. Highest melting point CH,CH, SiO2 RbI CH, OH Naci Lowest melting point
The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic interaction between the ions and thus the strength of the lattice energy of the ionic compound. Arrange the compounds according to the magnitudes of their lattice energies based on the relative ion charges and sizes. Highest lattice energy MgO MgF, NaF КСІ Lowest lattice energy
The charges and sizes of the ions in an ionic compound affect the strength of the electrostatic interaction between the ions and thus the strength of the lattice energy of the ionic compound. Arrange the compounds according to the magnitudes of their lattice energies based on the relative ion charges and sizes. Highest lattice energy RbF Csi SrF2 Sro Lowest lattice energy
7. Salts-ionic compounds-also exist in solid form, and ionic charges hold them together. (That should trigger some Coulomb's Law flashbacks...) Based on this, rank the melting points—1 for the lowest melting point to 5 for the highest melting point-for the substances below. Remember to consider both the magnitude and the distance separating (i.e., size of) the ions. NaCl RbBr NaBr KI KBr Propose a chloride salt with chemical formula XCl that has a higher melting point than any of these....
1.2. Consider a hypothetical ionic compound AB (comprised of At and B ions). Given the following enthalpy data and using a Born-Haber cycle calculation, predict AHlattice in kJ mol1. AB (s) A,H = -422 kJ mol-1 A (s) B (s) A (g) AH = 105 kJ mol1 A (s) B (g) A,H = 109 kJ mol-1 B (s) First ionization energy of A (gas phase) = 530 kJ mol1 -379 kJ mol-1 Electron affinity of B (taking into account it's...