Atomic structure explained

What are the principal differences in physical and chemical properties between any one metal from Group I and any one metal from Group IV and any one transition metal How far can you explain these differences in terms of their different atomic structures ... 

The development of the structural theory of the atom was the result of advances made by physics. In the 1920s, the physical chemist Langmuir (Nobel Prize in chemistry 1932) wrote, The problem of the structure of atoms has been attacked mainly by physicists who have given little consideration to the chemical properties which must be explained by a theory of atomic structure. The vast store of knowledge of chemical properties and relationship, such as summarized by the Periodic Table, should serve as a better foundation for a theory of atomic structure than the relativity meager experimental data along purely physical lines. ... 

Lewis s interest in chemical bonding and structure dated from 1902. In attempting to explain "valence" to a class at Harvard, he devised an atomic model to rationalize the octet rule. His model was deficient in many respects for one thing, Lewis visualized cubic atoms with electrons located at the corners. Perhaps this explains why his ideas of atomic structure were not published until 1916. In that year, Lewis conceived of the... 

To understand how the electron has been applied to explanations of the periodic table we must start with the discovery of the periodic system itself. The Russian chemist Dimitri Mendeleev announced in 1869 that the properties of elements arranged in order of increasing atomic weight appeared to repeat after certain definite intervals. Yet even as this discovery became increasingly well established, Mendeleev remained strongly opposed to any attempt to reduce or explain the periodicity in terms of atomic structure. He resisted the notion of any form of primary matter, which was actively discussed by his contemporaries, and opposed... 

To explain his observations, Rutherford proposed a new h /pothesis for atomic structure. He suggested that every atom has a tiny central core, called the nucleus, within which all the positive charge and most of the mass is concentrated. Electrons surround this central core, as shown schematically in Figure 2-16. Electrons occupy a volume that is huge compared with the size of the nucleus, but each electron has such a small mass that alpha particles are not deflected by the electrons. Consequently, an alpha particle is deflected only when it passes very near a nucleus, and it bounces back only when it collides head-on with a nucleus. Because most of the volume of an atom contains only electrons, most projectiles pass through the foil without being affected. 

Ernest Rutherfords proposed atomic structure added to the problems posed to nineteenth century physics by the ultraviolet catastrophe and the photoelectric effect. Rutherfords atom had a negatively charged electron circling a positively charged nucleus. The physics of the day predicted that the atom would emit radiation, causing the electron to lose energy and spiral down into the nucleus. Theory predicted that Rutherfords atom could not exist. Clearly, science needed new ideas to explain these three anomalies. 

These speculations about the ionic, polar, or electronic nature of chemical bonding, which arose largely from solution theory, resulted mostly in static models of the chemical bond or atom structure. In contrast is another tradition, which is more closely identified with ether theory and electrodynamics. This tradition, too, may be associated with Helmholtz, especially by way of his contributions to nineteenth-century theories of a "vortex atom" that would explain chemical affinities as well as the origin of electromagnetism, radiation, and spectral lines. 

What is the quantum mechanical model of the atom, and how does a understanding of atomic structure enable chemists to explain the properties of substances and their chemical bonding ... 

Chemical reactions take place when the reacting atoms, molecules or ions collide with each other. Therefore the outer electrons are Involved when different substances react together and we need to understand the electronic structure of atoms to explain the chemical properties of the elements. Much of the information about the electronic structure of atoms and molecules is obtained using spectroscopic techniques based on different types of electromagnetic radiation. 

In 1920 Bohr turned his attention to the problem of atomic structure. Matters had become somewhat more complicated than they were in Mendeleev s day. By 1920, 14 elements had been discovered that did not seem to follow Mendeleev s periodic law. Called the rare earths, they had similar properties and followed one another in the table of elements they were elements 58 through 71. When Mendeleev formulated his law only two had been discovered, so they didn t seem to present any great problem. But now they presented an anomaly that no one had been able to clear up. A workable theory of atomic structure would have to explain not only why periodicities were seen in the larger part of the table of the elements but also why they disappeared when one came to the rare earths. 

The existence of surface states is a consequence of the atomic structure of solids. In an infinite and uniform periodic potential, Bloch functions exist, which explains the band structures of different solids (Kittel, 1986). On solid surfaces, surface states exist at energy levels in the gap of the energy band (Tamm, 1932 Shockley, 1939 Heine, 1963). 

The presence of atoms or groups of atoms, called modulators, close to the reactional group as described above, in the molecular structure explains the variation of the intensity of the reactional expression. 

Up to about 1930, it was believed that the nucleus of an atom with atomic number Z and mass number A consisted of A protons and A — Z electrons. Which of the first 13 nuclear spins in the Appendix Table A.6 are incompatible with this hypothesis of nuclear structure Explain your answer. 

As explained in the entry on Chemical Elements Atomic Structure of... 

As pointed out by Stephens and Goldman (State University of New York at Stony Brook). Quasicrystals are neither uniformly ordered like crystals nor amorphous like glasses. Many features of quasicrystals cun be explained, but their atomic structure remains to be described fully. See also Aluminum Alloys and Engineered Materials... 

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