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Ionic bonding binds oppositely charged ions through attraction governed by electrostatics. In ordinary solid sodium chloride, each cation interacts with many anions, and also with other cations: attraction and repulsion together contribute to the binding of an extended ionic crystal. The chemical formula $\mathrm{NaCl}$ specifies equal numbers of the two kinds of ions; it does not divide the solid into isolated two-atom molecules.^[ref]

This distinction explains a striking combination of properties: ordinary dry sodium chloride conducts electric current poorly, while its molten form or a sufficiently concentrated chemical solution in water conducts well. The ions already exist in the solid; their ability to move through the sample changes. A conductivity experiment on salt solutions tests this transport picture, rather than simply asserting that charged constituents must make every material conductive.

Ordinary solid sodium chloride has the rock salt structure. Choose a conventional cube of side $a$ with chlorine anions at the corners and face centers, and sodium cations at the edge centers and cube center. Corner sites are shared by eight cubes, face sites by two and edge sites by four. The unit cell counts are thereforeThere are four formula units per conventional unit cell, rather than four separate NaCl molecules.^[ref]

The Bravais lattice is a face-centered cubic lattice. One choice of primitive lattice translation vectors and atomic basis isThe determinant gives a primitive unit cell volume of $a^3/4$; that cell represents one cation and one anion. Four such volumes make the conventional cube. The union of all ion positions resembles a primitive cubic lattice of step $a/2$ only if the chemical labels are discarded: translation by $a(1,0,0)/2$ exchanges unlike ions and fails to preserve the chemical structure.

Each ion has six nearest unlike neighbors at distance $a/2$, along the positive and negative directions of the three cube axes. Thus the coordination number is six. Within either same-species face-centered cubic lattice, the nearest same-ion neighbors instead number twelve: their displacements are permutations of $(\pm a/2,\pm a/2,0)$, all of length $a/\sqrt{2}$. Since $a/\sqrt{2}>a/2$, those twelve are a more distant shell in the complete sodium chloride structure. The number twelve describes the same-ion FCC lattice neighborhood; six describes the nearest unlike-ion neighborhood.

Use an oxygen-mediated superexchange path between two magnetic metal orbitals. A minimal one-active-orbital three-site charge-transfer superexchange Hamiltonian is clearest in a hole representation:Here $d_i$ describes a metal hole, $p$ a ligand hole, and $\Delta >0$ is the energy needed to create the virtual ligand hole. The low-energy configuration has one hole on each metal orbital and no ligand hole, corresponding to a filled bridging ligand orbital in the electron picture. $U_d$ and $U_p$ penalize double hole occupancy on the corresponding sites.

Virtual metal–ligand hopping transfers charge through oxygen without producing a real mobile carrier. Eliminating the ligand gives an effective metal–metal hopping $t_{dd}^{\mathrm{eff}}\sim t_{pd}^2/\Delta$. Combining it with the large metal repulsion givesA ligand double-occupancy channel adds a contribution of the same sign for the simple half-filled straight-bond model, often organized as $J\sim (4t_{pd}^4/{\Delta }^2)[1/U_d+2/(2\Delta +U_p)]$. The precise coefficients depend on the orbitals and hopping conventions; the essential mechanism is virtual charge transfer plus spin-selective access to intermediate states. The effective spin interaction favors antiparallel alignment while the material can remain insulating.

For MnO's rock salt structure, the strong approximately $180^{\circ }$ Mn–O–Mn path joins next-nearest Mn sites. It is not the nearest fcc Mn–Mn separation used in the direct-overlap estimate of part e. The oxygen-mediated path avoids relying on the tiny direct overlap of the two distant 3d tails. A realistic model includes several Mn 3d orbitals, Hund coupling and the high-spin Mn ion; the single-orbital Hamiltonian above isolates the antiferromagnetic exchange channel. Approximately $90^{\circ }$ paths and different orbital occupancies need not have the same sign.

Use the total scattering angle $\psi =2\theta$. For a cubic unit cell, Bragg's law and the Miller indices giveThe four measured values of ${\sin }^2\theta$, normalized to the first, are $1,1.330,2.655,3.649$. Multiplying by three gives approximately $3,4,8,11$, the initial allowed sequence for a face-centered cubic lattice:The FCC lattice factor is $1+(-1{)}^{h+k}+(-1{)}^{h+l}+(-1{)}^{k+l}$; it vanishes unless all three indices have the same parity. Thus the initial ratios differ from those of a primitive or body-centered cubic lattice. This is the conventional minimal cubic indexing; arbitrarily hiding additional weak reflections could make a short list alone ambiguous.

The low-pressure rock salt structure has an FCC Bravais lattice with one NaCl formula unit per primitive unit cell, or four per conventional cube. A possible atomic basis of a crystal is Na at zero and Cl at $(1/2,0,0)$ in conventional fractional coordinates. The two species have unequal atomic scattering factors, so both the odd and even FCC families can occur.

The four independent lattice constant estimates areTheir small scatter reflects the rounded angular data. The appropriate reported result is

Use mass density $\rho =ZM/(N_A{a}^3)$, with $M=74.55\mathrm{g}\mathrm{mo}{\mathrm{l}}^{-1}$. The rock salt structure has $Z=4$ formula units per conventional cell; the CsCl structure has $Z=1$. In pressure order the densities are approximatelyThe increase across the transition is approximately $14.5\%$, much greater than the smooth compression within either branch. Comparing $a^3$ directly without correcting the different $Z$ would create a fictitious volume discontinuity.

Within each cubic phase, increasing pressure decreases $a$, so $d_{hkl}=a/\sqrt{h^2+k^2+l^2}$ decreases and Bragg's law moves a given reflection to higher $2\theta$. Near $2.55\mathrm{GPa}$, peaks of the rock salt structure disappear as those of the CsCl structure appear, potentially with a coexistence interval. The former has an FCC translation selection rule, with $h,k,l$ all even or all odd; mixed-parity reflections vanish kinematically. The latter has primitive-cubic translations and basis factor $f_K+(-1{)}^{h+k+l}{f}_{Cl}$, so it has no FCC extinction rule. Odd-sum reflections may nevertheless be weak because the two ionic scattering factors are similar. Peak spacings, relative intensities and the cell volume per formula unit change discontinuously. A simple uniform shift of the entire original pattern cannot describe the structural transition.

The coordination number rises from six in the rock salt structure to eight in the CsCl structure. In the elementary hard-sphere ionic bonding model, accommodating eight opposite neighbours favours a larger cation/anion radius ratio: the geometrical limiting ratios are $\sqrt{2}-1$ for sixfold and $\sqrt{3}-1$ for eightfold coordination. The high-pressure change is therefore consistent with $r_K/r_{Cl}$ increasing under compression. Sincethe chloride ion is inferred to be more compressible than the potassium ion in this radius-ratio interpretation. This is a qualitative structural argument; real ionic radii depend on coordination and electronic structure, and the transition does not uniquely determine separate microscopic compressibilities.

The rock salt structure of ordinary sodium chloride has a coordination number of six for each kind of ion: six nearest neighbours of the opposite sign surround each ion along three perpendicular directions. Its conventional cubic unit cell contains four formula units; sharing corner, face, and edge sites between adjacent cells must be included in that count. Sixfold local coordination is compatible with $1:1$ overall stoichiometry.^[ref]

The checkerboard plane in the diagram is a slice through this three-dimensional arrangement. It leaves out the two nearest neighbours above and below the plane. Repeating a complete even-by-even patch gives equal numbers of signs; the displayed odd-by-odd crop has a boundary imbalance and is not a complete neutral ionic crystal or a unit cell. Other salts need not have the rock salt structure or the same coordination number.