Q.Write the cell notation (cell representation) for the Daniell cell consisting of a zinc electrode in $1\ \text{M}\ \text{ZnSO}_4$ and a copper electrode in $1\ \text{M}\ \text{CuSO}_4$, connected by a salt bridge.

[!TLDR] By convention, cell notation lists anode | anode-solution || cathode-solution | cathode. [!ANSWER] $\text{Zn}(s)\ |\ \text{Zn}^{2+}(1\ \text{M})\ ||\ \text{Cu}^{2+}(1\ \text{M})\ |\ \text{Cu}(s)$.

Cell notation (cell representation) is a shorthand that records, from left to right, the anode material, the anode's solution (with its concentration), a double vertical line for the salt bridge, the cathode's solution, and finally the cathode material. Single vertical lines mark a phase boundary (solid–solution interface). For the Daniell cell, zinc is the anode (it is oxidized, as established by comparing $E^{\circ}(\text{Zn}^{2+}/\text{Zn}) = -0.76\ \text{V}$ against $E^{\circ}(\text{Cu}^{2+}/\text{Cu}) = +0.34\ \text{V}$) and copper is the cathode (it is reduced). Writing left to right — anode metal, its ion in solution, salt bridge, cathode's ion in solution, cathode metal — gives $\text{Zn}(s)\ |\ \text{Zn}^{2+}(1\ \text{M})\ ||\ \text{Cu}^{2+}(1\ \text{M})\ |\ \text{Cu}(s)$. This single line fully specifies the cell: which reaction occurs where, and at what concentration, without needing a separate diagram. [!ANSWER] $\text{Zn}(s)\ |\ \text{Zn}^{2+}(1\ \text{M})\ ||\ \text{Cu}^{2+}(1\ \text{M})\ |\ \text{Cu}(s)$.

Identify anode and cathode from the reduction potentials, then write anode | anode-ion(conc) || cathode-ion(conc) | cathode.

Writing the cell backwards (cathode first); using a single line where a double line (salt bridge) is required, or vice versa.