Electronegativity increases across a period as atomic charge increases and the atomic radius decreases, thus the pull on the electrons in greater and the ability to attract electrons in a covalent bond increases.
As we go down a group, shielding increases, lessening the attraction of the politively charged nucleus and negatively charged electrons. This means electrons are more easily lost and therefore these elements can be described as having low electronegativity or can be described as electropositive.