Which feature was missing from John Dalton’s, J.J. Thomson’s, and Ernest Rutherford’s models of the atom, and why was this missing feature a disadvantage?
The charge of electrons was not included in these models. This was a disadvantage because the results from experiments involving cathode-tube rays could not be explained.
The behavior of electrons was not included in these models. This was a disadvantage because properties of bulk materials, such as metals, could not be explained.
The location of protons was not included in these models. This was a disadvantage because experimental results from the gold foil experiment could not be explained.
The location of electrons was not included in these models. This was a disadvantage because experimental results involving light and blackbody radiation could not be explained.
Well, it's like they say, "Electrons be like... who needs 'em!" But in all seriousness, the missing feature in John Dalton's, J.J. Thomson's, and Ernest Rutherford's models of the atom was the location of electrons. And oh boy, was that a disadvantage! Without knowing where those sneaky little electrons were hangin' out, scientists couldn't explain experimental results involving light and blackbody radiation. It's like trying to find your keys in the dark... good luck with that! So, you see, not including the location of electrons in those models was a real downside. They were left in the dark, just like my sense of fashion!
The correct answer is:
The charge of electrons was not included in these models. This was a disadvantage because the results from experiments involving cathode-tube rays could not be explained.
The correct answer is: The charge of electrons was not included in these models. This was a disadvantage because the results from experiments involving cathode-tube rays could not be explained.
To understand why this missing feature was a disadvantage, we need to look at the historical context. During the late 19th and early 20th centuries, scientists were trying to understand the nature of the atom. John Dalton proposed the first modern atomic theory, which stated that atoms were indivisible and that all atoms of the same element were identical. However, this theory couldn't explain the behavior of cathode rays.
J.J. Thomson then discovered that cathode rays were made up of negatively charged particles, which he called electrons. He proposed the "plum pudding" model, where electrons were embedded within a positively charged jelly-like substance. While this model explained the existence of electrons, it didn't account for the charge of the electrons or how they were distributed within the atom.
Later, Ernest Rutherford conducted the famous gold foil experiment, in which he found that most of the mass of an atom was concentrated in a tiny, positively charged nucleus. However, in Rutherford's model, the location of protons was not included.
The missing feature from all three models was the charge of the electrons. By not considering the charge, these models couldn't explain the behavior of cathode-tube rays, which were known to be negatively charged. It wasn't until the development of the atomic model by Niels Bohr that the idea of electrons in well-defined energy levels around the nucleus with specific charges was introduced.
So, in summary, the missing feature of the charge of electrons in the models by Dalton, Thomson, and Rutherford was a disadvantage because it prevented these models from explaining crucial experimental results involving cathode-tube rays.