Electronegativity is a chemical property that describes the tendency of an atom to attract a shared pair of electrons (or electron density) towards itself in a chemical bond. The Pauling scale is the most commonly used scale to measure electronegativity. According to this scale:

• The electronegativity of Fluorine (F) is the highest among the elements at around 3.98.
• Oxygen (O) follows next with an electronegativity of about 3.44.
• Nitrogen (N) has an electronegativity of approximately 3.04.
• Carbon (C) has an electronegativity value close to 2.55.
• Silicon (Si), being further down the group in the periodic table than Carbon, has a lower electronegativity of about 1.90.

Based on these values, we can arrange the elements in order of increasing electronegativity as follows:

$$ \text{Si} < \text{C} < \text{N} < \text{O} < \text{F} $$

Thus, considering the options provided:

Option A: Si < C < N < O < F is the correct answer since it correctly ranks the elements from the lowest to the highest electronegativity.