3. concentric circles (one smaller circle inside another). as

scientists attempt to understand the structure of the atom, why

was "bohr's planetary design" widely accepted? what do the

principles of gravity illustrate about keeping electrons close to

the nucleus of the atom?

Bohr's "planetary project" was widely accepted because he was able to explain a factor that Ruthford failed to achieve. Bohr was able to explain how electrons and energy worked in a simple atom, such as hydrogen, which consists of an electron orbiting a single proton.

In addition, he was able to explain, using the principles of gravity, how electrons do not fall on top of the proton but rather orbit around the proton.

Explanation:

Danish physicist Niels Bohr proposed an atomic model for the hydrogen atom which was later extended to other elements. Its model is based on the Solar System, in which the planets rotate around the sun. For Bohr, electrons rotate in orbit around the atomic nucleus grouped into energy levels.

Until 1913, there was no satisfactory model that explained even the simplest of atoms - hydrogen, which consists of an electron orbiting a single proton.

By assigning the concept of energy levels, Bohr was able to create a version of the hydrogen atom that was possibly stable and satisfying spectral observations. Until then, all theoretical predictions suggested that it should not exist for more than a split second - a failure that bothered physicists a great deal. It was therefore a monumental advance.

Bohr was also able to explain why electrons do not fall on protons using concepts of gravity. In Bohr's atomic model, electrons rotate around the nucleus like planets around the sun. According to Bohr, an electron does not fall into the nucleus because it cannot: its orbits are like steps in a ladder. We may be in one or the other but not in two. Imagine the atom as a kind of tiny football stadium.

The core is in the center of the lawn. Electrons can run around the steps of the stands. From time to time, they jump from step to step. If they go up they use energy, down they release energy.

However, electrons can never leave the stands to invade the field. Bohr did not explain why the ban.

first, consult an activity series chart to determine if al is more reactive than fe. it is, so it will replace the fe. now, one can continue with the problem.

next, make sure you have a correctly balanced equation.

3feo + 2al ==> 3fe + al2o3

now, determine which reactant (feo or al) is in limiting supply.

moles feo present = 125 g x 1 mole/71.8 g = 1.74 moles

moles al present = 25.0 g x 1 mole/26.98 g = 0.927 moles

since from the balanced equation, it take 3 mol feo for every 2 mol al, al will be limiting.

you can determine this simply by dividing moles of each by their coefficient in the balanced equation. for example: 1.74/3 = 0.58 and 0.927/2 = 0.464. al is less, so it is limiting.

finally, using the stoichiometry in the balanced eq. determine mass of fe that can be produced from 0.927 moles of al.

0.927 moles al x 3 moles fe/2 moles al x 55.8 g/mole = 77.6 g