**Introduction:**
The Rutherford model, proposed by Ernest Rutherford in 1911, describes the structure of an atom as a small, positively charged nucleus at the center, surrounded by negatively charged electrons in orbits. In this model, alpha particles are emitted from the radioactive source and directed towards a thin gold foil.

**Explanation:**

**1. Alpha Particles:**
Alpha particles are positively charged particles consisting of two protons and two neutrons, which are emitted during the process of radioactive decay. They have a relatively high energy and a large mass compared to electrons.

**2. Gold Foil Experiment:**
Rutherford conducted the gold foil experiment, where alpha particles were directed towards a thin gold foil. Based on the prevailing Thomson's model, it was expected that the alpha particles would pass straight through the foil with only slight deflection.

**3. Observation:**
However, the experimental results were surprising. While most of the alpha particles passed through the foil, some were deflected at large angles, and a few even bounced back. This observation led to the rejection of the Thomson model and the development of the Rutherford model.

**4. Explanation of Alpha Particle Deflection:**
According to the Rutherford model, the positive charge in an atom is concentrated in a small, dense nucleus at the center. The electrons orbit around the nucleus at a considerable distance.

When an alpha particle approaches the gold foil, it interacts with the positive charge of the nucleus. The positive charge of the alpha particle and the positive charge of the gold nucleus repel each other due to their like charges. This repulsion causes the alpha particle to experience deflection or even bounce back.

**5. Electron and Alpha Particle Interaction:**
In the Rutherford model, electrons are considered to be relatively light particles compared to alpha particles. They have a negligible mass compared to the mass of the alpha particle. Additionally, electrons reside in the outer orbits of the atom, far away from the nucleus.

The distance between the nucleus and the electrons is significant enough that the attractive force between the positive charge of the alpha particle and the negative charge of the electron is relatively weak. This weak force is not sufficient to cause significant attraction or deflection of the electrons towards the alpha particle.

Hence, the alpha particles do not attract electrons in the Rutherford model due to the small size and negligible mass of the electrons, as well as the significant distance between the electrons and the alpha particle.

In conclusion, according to the Rutherford model, the alpha particles do not attract electrons due to the weak attractive force between their positive charge and the negative charge of the electrons, as well as the significant distance between them.

The alpha rays have a charge of +2 only and this charge isn't enough to eject an electron from energy shell of gold. Moreover alpha rays travel at high speeds too, hence had no significant effect on the electrons in gold foil.