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Chapter 2: Problem 5

Describe the contributions of the following scientists to our knowledge of atomic structure: J. J. Thomson, R. A. Millikan, Ernest Rutherford, James Chadwick.

Short Answer

Expert verified
J.J. Thomson discovered the electron, thereby introducing the idea of subatomic particles. R.A. Millikan determined the charge of an electron through his oil-drop experiment. Ernest Rutherford introduced the concept of a small, dense, positively-charged nucleus within an atom surrounded by electrons. James Chadwick discovered the neutron, explaining the additional atomic mass not accounted for by protons and electrons.

Step by step solution

01

J.J. Thomson's Contribution

J.J. Thomson is best known for discovering the electron in 1897 through his cathode ray experiments. He proposed the existence of these tiny, negatively-charged particles, thereby introducing the concept of subatomic particles. This was a significant departure from the previously accepted 'plum pudding' model of the atom.
02

R.A. Millikan's Contribution

Robert Andrew Millikan is famous for his oil-drop experiment conducted in 1909. From his experiment, Millikan was able to calculate the charge of an electron. His results marked a big stride in quantifying properties of subatomic particles.
03

Ernest Rutherford's Contribution

Ernest Rutherford, often called the father of nuclear physics, performed the gold foil experiment in 1911. He demonstrated that the atom consists of a small, dense, positively charged nucleus surrounded by a large volume of space occupied by electrons. Hence, he established the nuclear model of an atom.
04

James Chadwick's Contribution

James Chadwick in 1932 discovered the neutron, a neutral particle that resides in the nucleus of an atom. His discovery advanced atomic theory by explaining the presence of atomic mass that couldn't be accounted for by protons and electrons alone.

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Most popular questions from this chapter

What are the empirical formulas of the following compounds? (a) \(\mathrm{Al}_{2} \mathrm{Br}_{6}\) (b) \(\mathrm{Na}_{2} \mathrm{~S}_{2} \mathrm{O}_{4}\) (c) \(\mathrm{N}_{2} \mathrm{O}_{5}\) (d) \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\)

The following table gives numbers of electrons, protons, and neutrons in atoms or ions of a number of elements. Answer the following: (a) Which of the species are neutral? (b) Which are negatively charged? (c) Which are positively charged? (d) What are the conventional symbols for all the species? $$ \begin{array}{lccccccc} \begin{array}{l} \text { Atom or Ion } \\ \text { of Element } \end{array} & \mathbf{A} & \mathbf{B} & \mathbf{C} & \mathbf{D} & \mathbf{E} & \mathbf{F} & \mathbf{G} \\ \hline \text { Number of electrons } & 5 & 10 & 18 & 28 & 36 & 5 & 9 \\ \text { Number of protons } & 5 & 7 & 19 & 30 & 35 & 5 & 9 \\ \text { Number of neutrons } & 5 & 7 & 20 & 36 & 46 & 6 & 10 \\ \hline \end{array} $$

Explain why anions are always larger than the atoms from which they are derived, whereas cations are always smaller than the atoms from which they are derived. (Hint: Consider the electrostatic attraction between protons and electrons.)

Name these compounds: (a) \(\mathrm{KClO}\) (b) \(\mathrm{Ag}_{2} \mathrm{CO}_{3}\) (c) \(\mathrm{FeCl}_{2}\), (d) \(\mathrm{KMnO}_{4}\), (e) \(\mathrm{CsClO}_{3}\), (f) \(\mathrm{HIO},(\mathrm{g}) \mathrm{FeO}\), (h) \(\mathrm{Fe}_{2} \mathrm{O}_{3}\) (i) \(\mathrm{TiCl}_{4},(\mathrm{j}) \mathrm{NaH},(\mathrm{k}) \mathrm{Li}_{3} \mathrm{~N},\) (1) \(\mathrm{Na}_{2} \mathrm{O}\) (m) \(\mathrm{Na}_{2} \mathrm{O}_{2},\) (n) \(\mathrm{FeCl}_{3} \cdot 6 \mathrm{H}_{2} \mathrm{O}\).

Define molecular formula and empirical formula. What are the similarities and differences between the empirical formula and molecular formula of a compound?
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