Ionic bonding factors affecting formation and lattice enthalpy - One Line Questions
1.
The 'n' value in the Born-Lande equation is typically between: —
5 and 12
2.
Which of the following contributes negatively to the Born-Haber cycle calculation of lattice enthalpy? —
Electron affinity
3.
The Born-Lande equation for lattice enthalpy (U) is U = - (N_A * M * z^+ * z^- * e^2) / (4 * pi * epsilon_0 * r_0) * (1 - 1/n). What does 'n' represent? —
Born exponent
4.
The Born-Landé equation is an approximation. The Born-Mayer equation is another model used to calculate lattice enthalpy. What is a key difference in their approach? —
Born-Landé uses empirical 'n' values, while Born-Mayer uses quantum mechanical calculations for repulsion.
5.
Which ionic compound is expected to have the LEAST stable lattice? —
BaCl2
6.
Which of the following oxides has the highest lattice energy? —
MgO
7.
Which of the following factors does NOT directly influence the magnitude of lattice enthalpy according to Coulomb's Law? —
Number of moles of ions
8.
If the electronegativity difference between two elements is large, it favors the formation of: —
Ionic bonds
9.
For a given period in the periodic table, as the nuclear charge increases, the ionization energy generally: —
Increases
10.
The process of forming gaseous ions from a solid ionic compound requires energy and is related to: —
Lattice enthalpy
11.
Which of the following contributes positively to the Born-Haber cycle for NaCl formation? —
Enthalpy of atomization of Na
12.
Lattice enthalpy is generally negative because: —
Energy is released when ions attract each other
13.
The enthalpy of sublimation of a metal is a measure of: —
Energy required to convert a solid metal into gaseous atoms
14.
The Born-Haber cycle is a thermodynamic cycle that relates the lattice energy of an ionic compound to various other enthalpy changes. Which of the following enthalpy changes is NOT typically included in the Born-Haber cycle? —
Enthalpy of fusion
15.
Which of the following contributes negatively to the Born-Haber cycle for the formation of an ionic compound? —
Lattice enthalpy
16.
The energy released when gaseous ions form a solid ionic lattice is defined as: —
Lattice enthalpy
17.
The energy released when gaseous atoms form gaseous ions is the sum of ionization energy and: —
Electron affinity
18.
Which of the following has the highest electron affinity? —
Cl
19.
Which factor is MOST crucial for the formation of a stable ionic bond? —
High lattice energy of the ionic compound
20.
The formation of an ionic bond is favored by: —
High lattice energy and low ionization energy
21.
A higher ionization energy for a metal generally leads to: —
Lower lattice enthalpy
22.
If the distance between the ions in an ionic compound increases, the lattice enthalpy will: —
Decrease
23.
In general, for alkali metal halides, lattice enthalpy decreases down a group due to: —
Increase in anion size
24.
Which of the following factors DECREASES lattice enthalpy? —
Increase in inter-ionic distance
25.
Which of the following factors would DECREASE the electronegativity difference between two elements, making ionic bond formation less likely? —
Increasing the atomic radius of both elements
26.
Electron affinity of the non-metal contributes to ionic bond formation by: —
Increasing the energy released during ion formation
27.
Which of the following statements about ionic bonding is FALSE? —
Ionic compounds are good conductors of electricity in the solid state.
28.
The Born-Haber cycle is used to calculate: —
Lattice enthalpy
29.
The energy released when one mole of gaseous anions is formed from gaseous atoms by the addition of electrons is called: —
Electron affinity
30.
In the Born-Haber cycle, the enthalpy of formation of an ionic compound is equal to the sum of: —
Sublimation, atomization, ionization, electron affinity, and lattice enthalpy
31.
The energy change associated with the conversion of one mole of a metal from solid to gaseous state is called: —
Enthalpy of sublimation
32.
Which statement about lattice enthalpy is INCORRECT? —
It decreases with increasing charges on the ions.
33.
Which of the following ionic compounds has the highest melting point, indicating a very strong ionic lattice? —
KF
34.
Which ionic compound would have the smallest lattice enthalpy? —
KI
35.
Which of the following factors would lead to a higher electron affinity for the non-metal? —
Higher effective nuclear charge
36.
Which of the following has the lowest ionization energy? —
Rb
37.
Which of the following factors is MOST responsible for the high stability of AlN lattice? —
High charges and small size of Al3+ and N3- ions
38.
Which pair of ions would result in a LESS stable ionic lattice compared to Ca2+ and O2-? —
K+ and F-
39.
Which of the following has the largest ionic radius? —
F-
40.
Which of the following ionic compounds would have the highest lattice enthalpy (most negative)? —
AlN
41.
For which pair of compounds is the lattice enthalpy difference expected to be the largest? —
MgO and CaO
42.
Lattice enthalpy of an ionic compound is defined as the energy change when: —
43.
The ionic radius of the ions is inversely related to lattice enthalpy because: —
Smaller ions can approach each other more closely
44.
The lattice enthalpy of an ionic compound is MOST directly related to its: —
Melting point
45.
Which of the following steps in the Born-Haber cycle for MgCl2 formation from Mg(s) and Cl2(g) would have a positive enthalpy change? —
Ionization of Mg
46.
Which factor is MOST important in determining the stability of an ionic compound? —
The energy released during lattice formation
47.
Which of the following factors is LEAST likely to affect lattice enthalpy? —
The number of electrons in the valence shell
48.
According to Born-Lande equation, lattice enthalpy is directly proportional to: —
The product of the charges of the ions
49.
The Madelung constant in the calculation of lattice energy accounts for: —
The geometry of the crystal lattice
50.
The high melting point of ionic compounds is a direct consequence of: —
Strong electrostatic forces between ions in the lattice