Why chlorine participates in resonance even though it is a electron withdrawing group in case of phenyl chloride

Background

A fundamental concept imparted at the beginning of organic chemistry is electronegativity. $$\ce{N, O, F}$$ and $$\ce{Cl}$$ are particularly electronegative and are capable of shifting the electron cloud of bonded atoms towards themselves in resonance, which I have read recently.

While reading about haloarenes, I encountered this statement "In aryl halides, a $$\ce{C-X}$$ bond acquires partial double bond character due to resonance, and subsequently the halogen atom acquires partial positive charge"

Question

How is the above statement true? Isn't chlorine more electronegative? How does it acquire positive charge? Isn't inductive effect stronger than resonance effect?

• That's formal charge in those structures. Also there's noting strange in opposite effects. – Mithoron Dec 9 '18 at 23:33