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Slide 1
Slide 1

Lecture 15
Lecture 15

Examination
Examination

... the instructions from the proctor for completing the student information on your answer sheet. Record your answers to the Part A and Part B–1 multiple-choice questions on this separate answer sheet. Record your answers for the questions in Part B–2 and Part C in your separate answer booklet. Be sure ...
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"Applications of nuclear physics"()

... protons and neutrons within nuclei lie in orbits much as electrons in atoms, but on the other hand nuclei behave in many ways as if they were made of incompressible fluid. All nuclei except the very lightest have the same density, much as water droplets all have the same density. If the nucleons are ...
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3.1 Atomic Mass - Pace University Webspace

... • In nature, most elements have more than one isotope, meaning that the same element with a different number of neutrons exists. • The average atomic mass that is seen on the periodic table is the average mass of the different isotopes of an element that occur naturally. • To figure out the average ...
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... causes a torque on the dipole     B but no net force. A Stern-Gerlach experiment sends atoms through a nonuniform magnetic field which can exert a net force on a magnetic dipole. ...
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110 EXAM Review MATERIALTro

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... 39. The requirements for the airbag that you developed in the first lab were that it could be deployed at a given time and that it inflates to the largest possible volume. The constraints on the airbag design were that it could not weigh more than 3.5 g and you could only use the materials available ...
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... In 1897, J. J. Thomson demonstrated in an experiment that cathode rays were deflected by an electric field. This suggested that cathode rays were composed of negatively charged particles found in all atoms. Thomson concluded that the atom was a positively charged sphere of almost uniform density in ...
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Chemistry Final Test 1999-2000 - Nashoba Valley Technical High
Chemistry Final Test 1999-2000 - Nashoba Valley Technical High

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Laser Cooling of Atom

< 1 ... 46 47 48 49 50 51 52 53 54 ... 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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