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Chapter 8: Problem 2

What is Moseley's contribution to the modern periodic table?

Short Answer

Expert verified
Moseley's contribution to the modern periodic table was his discovery and application of the atomic number, which allowed elements to be arranged more accurately than by atomic mass.

Step by step solution

01

Understanding The Periodic Table

The periodic table is a way of organizing chemical elements by their atomic number, electron configuration, and recurring chemical properties. Elements are listed in order of increasing atomic number, which corresponds to the number of protons in an element's atomic nucleus.
02

Henry Moseley's research

Henry Moseley was a British physicist. His major contribution was to experimentally determine the charges on the nuclei of most elements. He did this by bombarding each element with high-speed electrons and measuring the wavelength of the X-rays they gave off. He found that each element number, which he called the atomic number, was equal to the charge of the nucleus.
03

Henry Moseley's Contribution to the Periodic Table

Before Moseley, the elements in the periodic table were organized by atomic mass, which resulted in a few inconsistencies. Moseley's research into atomic numbers established the concept that each element has one more proton than the preceding one. This allowed for the reorganization of the periodic table based on atomic numbers rather than atomic mass. This corrected the previously inconsistent position of some elements and has since been the basis for the organization of the Periodic table.

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Most popular questions from this chapter

When magnesium metal is burned in air, it forms two products \(A\) and \(B\). A reacts with water to form a basic solution. B reacts with water to form a similar solution as that of A plus a gas with a pungent odor. Identify \(A\) and \(B\) and write equations for the reactions.

Explain which of these ions is larger, and why: \(\mathrm{Cu}^{+}\) or \(\mathrm{Cu}^{2+}\).

How does atomic radius change as we move (a) from left to right across the period and (b) from top to bottom in a group?

Why are the Group \(1 \mathrm{~B}\) elements more stable than the Group IA elements even though they seem to have the same outer electron configuration \(n s^{1}\) in which \(n\) is the principal quantum number of the outermost shell?

Arrange the elements in each of these groups in order of increasing electron affinity: (a) \(\mathrm{Li}, \mathrm{Na}, \mathrm{K}\) (b) \(\mathrm{F}, \mathrm{Cl}, \mathrm{Br}, \mathrm{I}\)
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