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CHAPTER 2 THE CHEMISTRY OF LIFE 2.1 Chemical Elements
CHAPTER 2 THE CHEMISTRY OF LIFE 2.1 Chemical Elements

... mass unit (amu) of weight. Electrons are negatively charged particles located in orbitals outside the nucleus. Protons and neutrons in the nucleus determine the mass number of an atom. The atomic number indicates the number of protons and the number of electrons in electrically neutral atoms. Isotop ...
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... The theory of barrier penetration was used by George Gamov in 1928 to explain the enormous variation of the half-lives for α decay of radioactive nuclei. Potential well shown on the diagram for an α particle in a radioactive nucleus approximately describes a strong attractive force when r is less th ...
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... 7.4 The Bohr Model In 1913, Niels Bohr (1885 – 1962) an atomic model that use the quantum concept to explain the spectral pattern of hydrogen. The Bohr’s model for the hydrogen atom is based on the following assumptions: ...
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Chemistry 4.2 notes - Bryant School District

... Atomic Orbitals and Quantum Numbers • Quantum numbers specify the properties of atomic orbitals and the properties of electrons in orbitals. • The principal quantum number, symbolized by n, indicates the main energy level occupied by the electron. 1, 2, 3, etc. as n increases the electron’s energy l ...
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... −1, 0, +1) so is there a preference? Also, Hund only predicts ground states… what about higher energy excited states? Also, are the electrons paired or unpaired? Again, Hund says they should have parallel spins, but to have two electrons in different p orbitals with one being spin “up” and the other ...
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... The spin multiplicity is the same as the # of microstates. Each terms has different energies; they represent three states with different degrees of electron-electron interactions. Which term has the lowest energy. This can be done by using two of Hund’s rules. 1. The ground term (term of lowest ener ...
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< 1 ... 38 39 40 41 42 43 44 45 46 ... 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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