Questions
The stability of an ionic compound is mostly due to:
- ionization energy
- electron affinity
- lattice energy
- electronegativity
Decreasing order of lattice energy of $FeO, Fe _2O _3, NaCl$ is:
- $NaCl>FeO>Fe _2O _3$
- $Fe _2O _3>FeO>NaCl$
- $NaCl>FeO=Fe _2O _3$
- $Fe _2O _3>NaCl>FeO$
The magnitude of the lattice energy of a soild increases if:
- the ions are large
- the ions are small
- the ions are of equal size
- charges on the ions are small
The higher lattice energy corresponds to
- ${\rm{MgO}}$
- ${\rm{CaO}}$
- $4{\rm{SrO}}$
- ${\rm{BaO}}$
Maximum lattice enthalpy is present in
- $K _{2}O$
- $CaO$
- $Al _{2}O _{3}$
- $KCl$
The melting point of a material with low binding energy is:
- high
- low
- infinity
- negative
Which pair is not correct order of lattice energy?
- $KCI > MgO$
- $AlN > MgO$
- $BeCO _3 > MgCO _3$
- $KCI < MgO$
The relation between the magnitudes of lattice energy of crystal and its formation energy is:
- lattice energy > formation energy
- lattice energy $=$ formation energy
- lattice energy < formation energy
- none of the above
If $Na^+$ ion is larger than $Mg^{2+}$ ion, and $S ^{2-}$ion is larger than $Cl^{-}$ ion, which of the following will be less soluble in water?
- $NaCl$
- $Na _{2}S$
- $MgCl _{2}$
- $MgS$
When sodium and chlorine react, energy is:
- released and ionic bond is formed.
- released and covalent bond is formed.
- absorbed and covalent bond is formed.
- absorbed and ionic bond is formed.
Lattice energy of an ionic compound depends upon:
- charge on the ion and size of the ion
- packing of ions only
- size of the ion only
- charge on the ion only
Which of the following has higher lattice energy -$Al _2O _3$ or $Al _2Se _3$?
- $Al _2O _3$ > $Al _2Se _3$
- $Al _2O _3$ < $Al _2Se _3$
- $Al _2O _3$ = $Al _2Se _3$
- None of these
Which has larger lattice energy among $ZnO$ and $NaCl$?
- $ZnO$ > $NaCl$
- $ZnO$ < $NaCl$
- $ZnO$ = $NaCl$
- None of these
The addition of energy in the form of heat causes molecules or crystals of the substance to break up into ions.
- True
- False
Which shows the highest lattice energy?
- $RbF$
- $CsF$
- $NaF$
- $KF$
Based on lattice energy and other considerations which one of the following alkali metal chloride has the highest melting point ?
- $KCl$
- $RhCl$
- $LiCl$
- $NaCl$
Which compound processes the greatest lattice energy?
- $LiBr$
- $LiCl$
- $LiI$
- $LiF$
Select the correct order of lattice energy.
- $LiF\, <\, LiBr\, <\, LiI$
- $LiCl\, >\, LiBr\, >\, LiI$
- $LiCl\, >\, NaCl\, >\, KCl$
- $BeCO _3\, <\, MgCO _3\, <\, SrCO _3\, <\, BaCO _3$
Lattice energy of ionic compounds depend upon:
- packing of ions only
- charge and size of ions
- charge on ion only
- size of ions only
Which of the following compounds will have the largest lattice energy?
- $AlBr _3$
- $CaO$
- $LiBr$
- $MgBr _2$
The lattice energies of the oxidies of $Mg,Ca,Sr ;$ and $;Ba$ follow the order:
- $BaO\;>\;SrO\;>\;CaO\;>MgO$
- $CaO\;>\;BaO\;>\;SrO\;>\;MgO$
- $MgO\;>\;SrO\;>\;CaO\;>\;BaO$
- $MgO\;>\;CaO\;>\;SrO\;>\;BaO$
The order of increasing lattice energy of the following compounds is :
- $NaCl\;<\;CaO\;<\;NaBr\;<\;BaO$
- $NaBr\;<\;NaCl\;<\;BaO\;<\;CaO$
- $NaCl\;<\;NaBr\;<\;BaO\;<\;CaO$
- $NaBr\;<\;NaCl\;<\;CaO\;<\;BaO$
From the following sequence calculate the lattice energy of AB(s):
$A(s)\rightarrow A(g)+e$; $610;kJ;mol^{-1}$
$B(g)+e\rightarrow B(g);$ $-260;kJ;mol^{-1}$
$A(s)+B(g)\rightarrow AB(s);$ $-569;kJ;mol^{-1}$
- $-219$
- $-919$
- $+1539$
- $+301$
The lattice energies of $KF,KCl,KBr ;$ and $;KI$ follows the order:
- $KF>KCl>KBr>KI$
- $KI>KBr>KCL>KF$
- $KF>KCl>KI>Br$
- $KI>KBr>KF>KCl$
Strength of ionic bond depends on lattice energy.
- True
- False
Identify the correct order of lattice energies.
- $CsCl < RbCl < KCl < NaCl$
- $KCl > CaCl _2 > AlCl _3$
- $NaCl < LiCl < MgCl _2 < AlCl _3$
- $LiCl > NaCl < MgCl _2 < AlCl _3$
The lattice energy of four ionic compounds $W, X, Y,$ and $Z$ are measured. The energies are found to be $-922\ kJ/mol, -769\ kJ/mol, -718\ kJ/ mol,$ and $-688\ kJ/mol$ respectively.
The four ionic, compounds are $NaCl, NaF, KBr$, and $KCl$.
Which of these ionic compounds could be identified as compound X based on the lattice energy?
- $NaCl$
- $NaF$
- $KBr$
- $KCl$
Boiling point of a substance is based on the intermolecular and intramolecular forces which in turn determine the lattice energy of a substance.
Which of the following substance would have the highest boiling point?
- $NaCl$
- $Hg$
- $AlF _{3}$
- $H _{2}O$
We have all heard the phrase "opposites attract but like repels." This is especially true for ionic compounds.
Which one of the following has the largest lattice energy as a result of this attraction?
- $LiCl$
- $NaCl$
- $K _{2}O$
- $MgCl _{2}$
Considering only lattice enthalpy, arrange them in the increasing order of their stability:
$NaCl$ , $MgCl _{2}$ , $MgO$
- $NaCl$ , $MgO$, $MgCl _{2}$
- $NaCl$ , $MgCl _{2}$ , $MgO$
- $MgCl$, $MgO$, $MgCl _{2}$
- none of these
The correct order of the lattice energies of the following ionic compound is :
- $NaCl > MgBr _2 > CaO > Al _2O3$
- $NaCl > CaO > MgBr _2 > Al _2O _3
$ - $Al _2O _3 > MgBr _2 > CaO > NaCl$
- $Al _2O _3 > CaO > MgBr _2 > NaCl$
$MgO$ has a high melting point because due to the highly charged ions, ionic force is strong and lattice energy is........
- High
- Low
- Both are
- None of these