File
... Early 20th century: -De Broglie: believed electrons have dual waveparticle properties -Scientists demonstrated that electrons could be bent or diffracted -Diffraction: bending of a wave as it passes by the edge of an object ...
... Early 20th century: -De Broglie: believed electrons have dual waveparticle properties -Scientists demonstrated that electrons could be bent or diffracted -Diffraction: bending of a wave as it passes by the edge of an object ...
Electron Configuration
... 1. Split up into groups of 3. 2. Draw one wave with wavelength 4 cm 3. Draw second wave with wavelength twice of the first wave. 4. Draw a third wave with 3 times the wavelength the first wave. 5. Draw 3 more waves with the same wavelengths as the first set but with an amplitude of 6 cm. ...
... 1. Split up into groups of 3. 2. Draw one wave with wavelength 4 cm 3. Draw second wave with wavelength twice of the first wave. 4. Draw a third wave with 3 times the wavelength the first wave. 5. Draw 3 more waves with the same wavelengths as the first set but with an amplitude of 6 cm. ...
chapter 3
... and then came the physicists, Faraday 1833, electrolysis, if 96 485 C is passed through molten NaCl, 23 g of Na deposit on the cathode and (½) 35.5 g of Cl(2) bubble off why precisely that amount of charge? we know today it’s 1 mol of electrons = Avogadro’s number, 6.0221 1023 mol-1, times electron ...
... and then came the physicists, Faraday 1833, electrolysis, if 96 485 C is passed through molten NaCl, 23 g of Na deposit on the cathode and (½) 35.5 g of Cl(2) bubble off why precisely that amount of charge? we know today it’s 1 mol of electrons = Avogadro’s number, 6.0221 1023 mol-1, times electron ...
Chemical Bonding
... » Covalent Bonding – Non-metal with non-metal Weak Bonds » Dipole-dipole » Hydrogen bonding » Dispersion forces ...
... » Covalent Bonding – Non-metal with non-metal Weak Bonds » Dipole-dipole » Hydrogen bonding » Dispersion forces ...
In 1913 Bohr proposed his quantized shell model of the atom to
... Radiation can occur only when the electron jumps from one orbit to another. The atom will be completely stable in the state with the smallest orbit, since there is no orbit of lower energy into which the electron can jump. Bohr's starting point was to realize that classical mechanics by itself could ...
... Radiation can occur only when the electron jumps from one orbit to another. The atom will be completely stable in the state with the smallest orbit, since there is no orbit of lower energy into which the electron can jump. Bohr's starting point was to realize that classical mechanics by itself could ...
ATOMIC STRUCTURE, ELECTRONS, AND PERIODICITY All matter
... Shells in an atom reflect quantization. Each electron has a unique set of 4 quantum numbers. ...
... Shells in an atom reflect quantization. Each electron has a unique set of 4 quantum numbers. ...
2.4 Revision 1: There were two atoms. One got hit by an extremely
... d. Conducts electricity when dissolved or melted but not as a solid? e. Forces that hold non-polar molecular solids together. f. Can conduct heat and electrical charge. g. Which of the following solids have hydrogen bonds between molecules; hydrogen chloride, calcium, sodium chloride, ammonia, graph ...
... d. Conducts electricity when dissolved or melted but not as a solid? e. Forces that hold non-polar molecular solids together. f. Can conduct heat and electrical charge. g. Which of the following solids have hydrogen bonds between molecules; hydrogen chloride, calcium, sodium chloride, ammonia, graph ...
Which frequency of light has the most energy
... In what way do atomic spectra support the Bohr model of the atom? A. The spectra indicate that electrons have practically no mass. B. The spectra make it possible to calculate the charge on the electron. C. The spectra indicate that the nucleus is very small compared to the atom. D. The spectra cont ...
... In what way do atomic spectra support the Bohr model of the atom? A. The spectra indicate that electrons have practically no mass. B. The spectra make it possible to calculate the charge on the electron. C. The spectra indicate that the nucleus is very small compared to the atom. D. The spectra cont ...
Chapter 9: Atoms
... It does not allow for any radial motion of the electron If we perform a fully quantum mechanical treatment of hydrogen we find that electrons are not in circular orbits and can spread out in the radial direction. The hydrogen atom is clearly a 3-dimensional problem. z Let’s break it down into sp ...
... It does not allow for any radial motion of the electron If we perform a fully quantum mechanical treatment of hydrogen we find that electrons are not in circular orbits and can spread out in the radial direction. The hydrogen atom is clearly a 3-dimensional problem. z Let’s break it down into sp ...
Midterm Review.ppt - Chemistry R: 4(AE)
... mass of water in a sample of BaCl2 * 2H2O. The accepted value is 14.8%. What was the ...
... mass of water in a sample of BaCl2 * 2H2O. The accepted value is 14.8%. What was the ...
photon may be totally absorbed by electron, but not have enough
... momentum of a particle. He proposed that only those orbits where the wave would be a circular standing wave will occur. This yields the same relation that Bohr had proposed. In addition, it makes more reasonable the fact that the electrons do not radiate, as one would otherwise expect from an accele ...
... momentum of a particle. He proposed that only those orbits where the wave would be a circular standing wave will occur. This yields the same relation that Bohr had proposed. In addition, it makes more reasonable the fact that the electrons do not radiate, as one would otherwise expect from an accele ...
Chemistry for Bio 11
... • There are 92 naturally occurring elements • Many others have been synthesized Atomic number: # protons Atomic mass: protons Isotopes- different atoms of same element, with different # neutrons Atomic weight: Naturally occurring average of isotopes of a substance ...
... • There are 92 naturally occurring elements • Many others have been synthesized Atomic number: # protons Atomic mass: protons Isotopes- different atoms of same element, with different # neutrons Atomic weight: Naturally occurring average of isotopes of a substance ...
Topic 7: Atomic and nuclear physics 7.1 The atom
... The electrons in Rutherford’s model should, therefore lose energy and spiral into the nucleus in a matter of nanoseconds. Rutherford’s model, then, cannot explain why stable atoms exist. 2. Rutherford’s model did not explain the observed emission spectra ...
... The electrons in Rutherford’s model should, therefore lose energy and spiral into the nucleus in a matter of nanoseconds. Rutherford’s model, then, cannot explain why stable atoms exist. 2. Rutherford’s model did not explain the observed emission spectra ...
Slide 1
... mass of water in a sample of BaCl2 * 2H2O. The accepted value is 14.8%. What was the student's ...
... mass of water in a sample of BaCl2 * 2H2O. The accepted value is 14.8%. What was the student's ...
Spectra of Atoms
... emitted by atoms of a given element is absolutely the same for every atom of that element, no matter how hot or cold it is. Mystery #4. What is the dynamics that causes line spectra? ...
... emitted by atoms of a given element is absolutely the same for every atom of that element, no matter how hot or cold it is. Mystery #4. What is the dynamics that causes line spectra? ...
Chapter 4 - SchoolRack
... Octet – the outer energy level is considered filled when the s and p sublevels are completely filled with 8 electrons A filled outer energy level (8 electrons) is a very stable electron configuration. The noble gases have filled outer energy levels. This is why they are unreactive. ...
... Octet – the outer energy level is considered filled when the s and p sublevels are completely filled with 8 electrons A filled outer energy level (8 electrons) is a very stable electron configuration. The noble gases have filled outer energy levels. This is why they are unreactive. ...
Atomic orbital
An atomic orbital is a mathematical function that describes the wave-like behavior of either one electron or a pair of electrons in an atom. This function can be used to calculate the probability of finding any electron of an atom in any specific region around the atom's nucleus. The term may also refer to the physical region or space where the electron can be calculated to be present, as defined by the particular mathematical form of the orbital.Each orbital in an atom is characterized by a unique set of values of the three quantum numbers n, ℓ, and m, which respectively correspond to the electron's energy, angular momentum, and an angular momentum vector component (the magnetic quantum number). Any orbital can be occupied by a maximum of two electrons, each with its own spin quantum number. The simple names s orbital, p orbital, d orbital and f orbital refer to orbitals with angular momentum quantum number ℓ = 0, 1, 2 and 3 respectively. These names, together with the value of n, are used to describe the electron configurations of atoms. They are derived from the description by early spectroscopists of certain series of alkali metal spectroscopic lines as sharp, principal, diffuse, and fundamental. Orbitals for ℓ > 3 continue alphabetically, omitting j (g, h, i, k, …).Atomic orbitals are the basic building blocks of the atomic orbital model (alternatively known as the electron cloud or wave mechanics model), a modern framework for visualizing the submicroscopic behavior of electrons in matter. In this model the electron cloud of a multi-electron atom may be seen as being built up (in approximation) in an electron configuration that is a product of simpler hydrogen-like atomic orbitals. The repeating periodicity of the blocks of 2, 6, 10, and 14 elements within sections of the periodic table arises naturally from the total number of electrons that occupy a complete set of s, p, d and f atomic orbitals, respectively.