Explaining differences in rate of propagation based on monomer structure
The argument presented by your instructor is based on one factor: the stability of the radical terminus of the polymer. But for bimolecular polymerization reactions we need to consider 4 things:


Stability of the radical
Stability of the monomer
Stability of the transition state
The probability of the radical and the monomers being correctly oriented


The first three items affect the activation energy ($E_\mathrm{a}$), while the final item affects the frequency factor ($A$), or pre-exponential factor in the Arrhenius equation:

$$ k = A \exp{\left(\frac{-E_\mathrm{a}}{RT}\right)} $$

For styrene, vinyl acetate (a vinyl ester), and ethylene, I have found the following values for radical polymerization processes.[1,2] These have been calculated to provide an apples-to-apples comparison: 

$$\begin{array}{cc}
\hline
\text{Monomer} &amp; E_\mathrm{a}~/~\mathrm{kJ~mol^{-1}} &amp; A~/~\mathrm{L~mol^{-1}~s^{-1}} &amp; T~/~^\circ\mathrm{C} &amp; k_\mathrm{p}~/~\mathrm{L ~mol^{-1}~s^{-1}} \\ \hline
\text{Styrene} &amp; 32.5 &amp; 4.3 \times 10^7 &amp; 60 &amp; 341  \\
\text{Vinyl acetate} &amp; 20.4 &amp; 1.5 \times 10^7 &amp; 60 &amp; 9460 \\ 
\text{Ethylene} &amp; 27.7\mathrm{-}32.8 &amp; 2.0 \times 10^3 \mathrm{-} 3.0 \times 10^4 &amp; 60 &amp; 0.1\mathrm{-}0.2 \\ \hline
\end{array}$$

Note: 


  "the propagation rate coefficient for most monomers is strongly pressure-dependent with large negative activation volumes; thus an increase in pressure leads to an increased $k_\mathrm{p}$ value."[1]


This is particularly relevant for the ethylene example, which is done at $100\ \mathrm{bar}$. At $60\ ^\circ\mathrm{C}$, this should be about $0.15\ \mathrm{g~mL^{-1}}$,[3] which is a factor of 7 less dense than the styrene and vinyl acetate systems. 

With those caveats noted, the argument of the vinyl ester having a lower activation energy ($E_\mathrm{a}$) due to the reactants being less stable relative to the transition state seems valid. However, the data for ethylene shows that the pre-exponential factor ($A$) is likely responsible for the lesser rate of propagation displayed by ethylene. 

Sources: 


Krzysztof Matyjaszewski &amp; Thomas P. Davis, Handbook of Radical Polymerization, 2003, p 199. 
Etienne Grau, Jean-Pierre Broyer, Christophe Boisson, Roger Spitz, and Vincent Monteil, Macromolecules 2009, 42, 7279–7281. DOI: 10.1021/ma901622u
Thomas, W. &amp; Zander, M. Int J Thermophys (1980) 1: 383. DOI: 10.1007/BF00516565