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Chapter 3: Stoichiometry
Chapter 3: Stoichiometry

... By difference: 0.1156 g – (0.04467 g C + 0.01862 g H) = 0.5231 g N 0.05231 g x 100 = 45.25 % 0.1156 g compound Determine moles of each element in compound: (could use mass or percent info) C: 38.67 / 12.01 = 3.223 mol C H: 16.11 / 1.00 = 16.11 mol H N: 45.25 / 14.0 = 3.232 mol N Divide by smallest n ...
Chapter 5: Electrons in Atoms 1 Section 5.1: Light and Quantized
Chapter 5: Electrons in Atoms 1 Section 5.1: Light and Quantized

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... energy is added, the electrons are promoted to higher, or excited, energy states. As the electrons lose this energy, light is emitted. The wavelengths of the light emitted enable us to determine the energy levels that the electrons occupied. 2. This emitted light may be measured using a spectroscope ...
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... 2. If an electron moves down an energy level then quantised energy in the form of a photon will be emitted. Similarly if an electron moves to a higher energy level then the atom must absorb some quanta of energy. This explains the existence of spectral lines. 3. Angular momentum = nh/2π, where n is ...
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CCR 19: Spectroscopic Notation

... principal (P term) state, the same limiting term as for the sharp series. Finally, the fundamental emission spectrum was the result of transitions from the higher fundamental (F terms) energy states to the lowest D term state, the limiting term for the fundamental series. In Figure SN-3 the principa ...
General Chemistry I Syllabus
General Chemistry I Syllabus

< 1 ... 76 77 78 79 80 81 82 83 84 ... 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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