Synthesis of the tetrachloroaluminate(III) anion
Note that the first reaction would require substantial amount of heat to assure the designated product $\ce{NaAlO2}$ is formed (nowhere near STP):

$$\ce{2 Al(s) + 2 NaOH(l) + 2 H2O(g) -&gt;[\pu{\approx 450 °C}] 2 NaAlO2(s) + 3 H2(g)}$$

In aqueous solution the product would be tetrahydroxoaluminate $\ce{[Al(OH)4]-}:$

$$\ce{2 Al(s) + 2 NaOH(aq, conc) + 6 H2O (l) -&gt;[Δ] 2 Na[Al(OH)4](aq) + 3 H2(g)}$$

Synthetic procedure from "common laboratory reagents" is described in Brauer's Handbook of Preparative Inorganic Chemistry [1, p. 816]:


  Sodium Tetrachloroaluminate
  
  $\ce{NaAlCl4}$
  
  $$\ce{\underset{58.4}{NaCl} + \underset{133.4}{AlCl3} = \underset{191.8}{NaAlCl4}}$$
  
  The reaction is carried out in a Pyrex vessel (Fig. 245), which should be as compact as possible.
  The stoichiometric amounts of C.P. $\ce{NaCl}$ and freshly sublimed $\ce{AlCl3}$ are introduced into the pear-shaped part of the reaction vessel.
  
  
  Fig. 245. Preparation of sodium tetrachloroaluminate.
  
  The filling is done under nitrogen and the vessel should be very clean and dry.
  A melting point capillary is then affixed underneath the ground joint; the apparatus is evacuated to a high vacuum and torch-sealed.
  It is then immersed as deeply as possible in an oil bath at 200–240 °C.
  The $\ce{AlCl3},$ which tends to sublime onto the cool parts of the wall, is driven back by passing a luminous flame over the condensate spots.
  When the flask contents have become a nearly clear melt, they are poured hot into the side flask of the vessel.
  The product solidifies on cooling.


References


Handbook of Preparative Inorganic Chemistry, 2nd ed.; Brauer, G., Ed.; Academic Press: New York; London, 1963; Vol. 1.