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practice exercise - Needham.K12.ma.us
practice exercise - Needham.K12.ma.us

... Solution Each compound is ionic and is named using the guidelines we have already discussed. In naming ionic compounds, it is important to recognize polyatomic ions and to determine the charge of cations with variable charge. (a) The cation in this compound is K+ and the anion is SO42–. (If you thou ...
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... azimuthal quantum number changes by one unit and only J will remain unchanged. Their occurrence is, therefore, quite in conformity with the correspondence principle. The modification proposed is specially important for explaining the structure of X - ray spectra. These spectra differ from the hydrog ...
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... gas, then collapse back to the ground as the gas is removed. Why do you suppose the tanks are designed to inflate and collapse? One reason is to keep the gas under a constant pressure. The height of each tank varies with the amount of gas inside, so more gas means a greater volume rather than a grea ...
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Lecture 17: Bohr Model of the Atom

... • Niels Bohr uses the emission spectrum of hydrogen to develop a quantum model for H. • Central idea: electron circles the “nucleus” in only certain allowed circular orbitals. • Bohr postulates that there is Coulombic attraction between e- and nucleus. However, classical physics is unable to explain ...
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CHAPTER 1 -Chemistry -Matter -Elements -Atoms

... 3) Which of the following ions has the same number of electrons as Br(a) Ca+2 (b) K+ (c) Sr+2 (d) I(e) Cl4) For which of the following pairs are the atoms most likely to form an ionic compound? (a) Carbon and Oxygen (b) Calcium and Chlorine (c) Chlorine and Oxygen (d) Sodium and Magnesium (e) Chlori ...
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... called stationary states. Each stationary state corresponds to the atom’s electrons occupying fixed, circular orbits around the nucleus. While in one of its stationary states, atoms do not emit energy. An atom changes stationary states by emitting or absorbing a specific quantity of energy that is e ...
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... Nuclear mass and binding energy The mass of a bound system is always less than the mass of its component parts. For example, the mass of the hydrogen atom is 13.5 eV/c2 less than proton mass plus electron mass. When the hydrogen atom is formed, 13.5 eV is released in photons. mH c 2 − m p + me c 2 ...
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... In 1979 the first confined gas of bosons, spinpolarized atomic hydrogen was stabilized, but the conditions for BEC were difficult to achieve. In the 1980s atomic physicists learned how to cool alkali atoms (sodium, rubidium,etc.) to microkelvin temperatures Alkali gases (metastable) were confined i ...
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... influence on the energy. n and m are written numerically, but the spdf ... coding is used for . An example of the configuration for Ca is 1s2 2s2 2p6 3s3d which is frequently abbreviated 3d. In general each configuration leads to several terms which may be split apart by several eV. The above Ca config ...
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... The Heisenberg Uncertainty Principle The Heisenberg uncertainty principle states that it is impossible to know both the velocity and the position of a particle at the same time. • This limitation is critical when dealing with small particles such as electrons. • But it does not matter for ordinary-s ...
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Atomic Structure

< 1 ... 71 72 73 74 75 76 77 78 79 ... 137 >

Atom

An atom is the smallest constituent unit of ordinary matter that has the properties of a chemical element. Every solid, liquid, gas, and plasma is made up of neutral or ionized atoms. Atoms are very small; typical sizes are around 100 pm (a ten-billionth of a meter, in the short scale). However, atoms do not have well defined boundaries, and there are different ways to define their size which give different but close values.Atoms are small enough that classical physics give noticeably incorrect results. Through the development of physics, atomic models have incorporated quantum principles to better explain and predict the behavior.Every atom is composed of a nucleus and one or more electrons bound to the nucleus. The nucleus is made of one or more protons and typically a similar number of neutrons (none in hydrogen-1). Protons and neutrons are called nucleons. Over 99.94% of the atom's mass is in the nucleus. The protons have a positive electric charge, the electrons have a negative electric charge, and the neutrons have no electric charge. If the number of protons and electrons are equal, that atom is electrically neutral. If an atom has more or fewer electrons than protons, then it has an overall negative or positive charge, respectively, and it is called an ion.Electrons of an atom are attracted to the protons in an atomic nucleus by this electromagnetic force. The protons and neutrons in the nucleus are attracted to each other by a different force, the nuclear force, which is usually stronger than the electromagnetic force repelling the positively charged protons from one another. Under certain circumstances the repelling electromagnetic force becomes stronger than the nuclear force, and nucleons can be ejected from the nucleus, leaving behind a different element: nuclear decay resulting in nuclear transmutation.The number of protons in the nucleus defines to what chemical element the atom belongs: for example, all copper atoms contain 29 protons. The number of neutrons defines the isotope of the element. The number of electrons influences the magnetic properties of an atom. Atoms can attach to one or more other atoms by chemical bonds to form chemical compounds such as molecules. The ability of atoms to associate and dissociate is responsible for most of the physical changes observed in nature, and is the subject of the discipline of chemistry.Not all the matter of the universe is composed of atoms. Dark matter comprises more of the Universe than matter, and is composed not of atoms, but of particles of a currently unknown type.
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