Atomic Structure
... Electrons existed in “states” (i.e. constant energy) with circular paths called orbits. Energy is absorbed when an electron jumps to a higher orbit and lost upon a drop to a lower energy orbit. These transitions (jumps) will occur when an energy change occurs which exactly matches the difference in ...
... Electrons existed in “states” (i.e. constant energy) with circular paths called orbits. Energy is absorbed when an electron jumps to a higher orbit and lost upon a drop to a lower energy orbit. These transitions (jumps) will occur when an energy change occurs which exactly matches the difference in ...
Atoms
... the beginning of the 20th century established that atoms consist of a positively charged nucleus and negatively charged electrons. In a neutral atom, the positive charge on the nucleus exactly balances the total negative charge of the electrons. All experiments up to the present time indicate that t ...
... the beginning of the 20th century established that atoms consist of a positively charged nucleus and negatively charged electrons. In a neutral atom, the positive charge on the nucleus exactly balances the total negative charge of the electrons. All experiments up to the present time indicate that t ...
Problem set 6
... 1. Consider a free non-relativistic particle of mass m. In the lecture we assumed the time evolution of each Fourier component of a matter wave ψ(x, t) was given by ei(kx−ω(k)t) corresponding to a right moving wave if k, ω(k) were of the same sign. We could equally well have considered the time evol ...
... 1. Consider a free non-relativistic particle of mass m. In the lecture we assumed the time evolution of each Fourier component of a matter wave ψ(x, t) was given by ei(kx−ω(k)t) corresponding to a right moving wave if k, ω(k) were of the same sign. We could equally well have considered the time evol ...
Document
... distinct from one another. In quantum theory, mass and energy are not distinguished. Matter (electrons, neutrons, atoms, molecules,…) behaves like a wave and energy (= radiation: light, x-rays, g,...) behaves like a particle. Quantum theory does not give us an intuitive picture of the fundamental na ...
... distinct from one another. In quantum theory, mass and energy are not distinguished. Matter (electrons, neutrons, atoms, molecules,…) behaves like a wave and energy (= radiation: light, x-rays, g,...) behaves like a particle. Quantum theory does not give us an intuitive picture of the fundamental na ...
Using mass to calculate molecular formula
... Benzene consists of 7.69% H and 92.31%C. Converting this to a formula gives CH. This is the simplest integer ratio. In fact a molecule of benzene has the formula C6H6. Empirical formula CH – simplest whole number ratio. Molecular formula C6H6 – actual number of atoms in the molecule. Percentages of ...
... Benzene consists of 7.69% H and 92.31%C. Converting this to a formula gives CH. This is the simplest integer ratio. In fact a molecule of benzene has the formula C6H6. Empirical formula CH – simplest whole number ratio. Molecular formula C6H6 – actual number of atoms in the molecule. Percentages of ...
Can nature be q-deformed?
... on which the metric determinations of space are based … lose their validity in the infinitely small; one ought to assume this as soon as it permits a simpler way of explaining phenomena …“ (Bernhard Riemann) „I … believe firmly the solution to the present troubles (with divergences) will not be reac ...
... on which the metric determinations of space are based … lose their validity in the infinitely small; one ought to assume this as soon as it permits a simpler way of explaining phenomena …“ (Bernhard Riemann) „I … believe firmly the solution to the present troubles (with divergences) will not be reac ...
Presentation
... 10. Starting with the idea that an electron is a wave, prove that En =n2h2/8mL2 for an electron trapped as a standing wave in a one-dimensional box. Assume the length of the box is L and that m is the mass of the electron (hint: use de Broglie’s equation and find momentum in terms of kinetic energy) ...
... 10. Starting with the idea that an electron is a wave, prove that En =n2h2/8mL2 for an electron trapped as a standing wave in a one-dimensional box. Assume the length of the box is L and that m is the mass of the electron (hint: use de Broglie’s equation and find momentum in terms of kinetic energy) ...
Electron Deep Orbits of the Hydrogen Atom1
... The deep orbits are obtained only if the radial quantum number N = 0. We recall further the general conditions for deep orbits. With N = 0, the sub-expression Δ = N + ½ - (¼ - α2)1/2 can be reduced to α2 and then E0 ~ mc2α. So, if α −> 0, we have the total energy E0 −> 0, and this implies that the a ...
... The deep orbits are obtained only if the radial quantum number N = 0. We recall further the general conditions for deep orbits. With N = 0, the sub-expression Δ = N + ½ - (¼ - α2)1/2 can be reduced to α2 and then E0 ~ mc2α. So, if α −> 0, we have the total energy E0 −> 0, and this implies that the a ...
Periodic Table, Bonding, Reactions, and Moles
... 6. Explain, in terms of electrons, why the ionic radius of a Group 2 element is smaller than its atomic radius. 7. What is the total number of electron pairs shared between the carbon atom and one of the oxygen atoms in a carbon dioxide molecule? 8. Explain, in terms of valence electrons, why the bo ...
... 6. Explain, in terms of electrons, why the ionic radius of a Group 2 element is smaller than its atomic radius. 7. What is the total number of electron pairs shared between the carbon atom and one of the oxygen atoms in a carbon dioxide molecule? 8. Explain, in terms of valence electrons, why the bo ...
Calculation of the Zeeman-Fine Energies and the Spectrum with
... Received April 18, 2011; revised May 27, 2011; accepted June 12, 2011 ...
... Received April 18, 2011; revised May 27, 2011; accepted June 12, 2011 ...
Quantum Chemistry
... near a hydrogen nucleus. His model postulated a set of circular orbits for electrons with specific, discrete radii and energies and that electrons could move in each orbit without radiating energy (even though this violated classical ideas). Bohr’s theory failed to (i) explain multi-electron atoms ( ...
... near a hydrogen nucleus. His model postulated a set of circular orbits for electrons with specific, discrete radii and energies and that electrons could move in each orbit without radiating energy (even though this violated classical ideas). Bohr’s theory failed to (i) explain multi-electron atoms ( ...
Quantum Numbers
... • Aufbau principle – electrons fill energy levels and sublevels in order of increasing energy • Pauli Exclusion principle – no two electrons can have the same set of four quantum numbers (which means no two electrons can be in the same place at the same time) • Hund’s rule – when adding electrons to ...
... • Aufbau principle – electrons fill energy levels and sublevels in order of increasing energy • Pauli Exclusion principle – no two electrons can have the same set of four quantum numbers (which means no two electrons can be in the same place at the same time) • Hund’s rule – when adding electrons to ...
Hydrogen atom
A hydrogen atom is an atom of the chemical element hydrogen. The electrically neutral atom contains a single positively charged proton and a single negatively charged electron bound to the nucleus by the Coulomb force. Atomic hydrogen constitutes about 75% of the elemental (baryonic) mass of the universe.In everyday life on Earth, isolated hydrogen atoms (usually called ""atomic hydrogen"" or, more precisely, ""monatomic hydrogen"") are extremely rare. Instead, hydrogen tends to combine with other atoms in compounds, or with itself to form ordinary (diatomic) hydrogen gas, H2. ""Atomic hydrogen"" and ""hydrogen atom"" in ordinary English use have overlapping, yet distinct, meanings. For example, a water molecule contains two hydrogen atoms, but does not contain atomic hydrogen (which would refer to isolated hydrogen atoms).