Chem 31 - Exam #3
... questions. For questions involving calculations, show all of your work -- HOW you arrived at a particular answer is MORE important than the answer itself! Circle your final answer to numerical questions. The entire exam is worth a total of 150 points. Attached are a periodic table and a formula shee ...
... questions. For questions involving calculations, show all of your work -- HOW you arrived at a particular answer is MORE important than the answer itself! Circle your final answer to numerical questions. The entire exam is worth a total of 150 points. Attached are a periodic table and a formula shee ...
1) - Kurt Niedenzu
... Final EOC Review - Sheet 2 32) The increase in atomic radius of each successive element within a group is primarily due to an increase in the number of a) neutrons in the nucleus b) electrons in the outermost shell c) unpaired electrons d) occupied principal energy levels 33) Elements that have pro ...
... Final EOC Review - Sheet 2 32) The increase in atomic radius of each successive element within a group is primarily due to an increase in the number of a) neutrons in the nucleus b) electrons in the outermost shell c) unpaired electrons d) occupied principal energy levels 33) Elements that have pro ...
Atomic Structure
... Daltons Atomic Theory • 1. All elements are composed of tiny indivisible particles called atoms. • 2. Atoms of the same element are identical. The atoms of one element are different from the atoms of another element. • 3. Atoms of different elements can physically mix together or can chemically com ...
... Daltons Atomic Theory • 1. All elements are composed of tiny indivisible particles called atoms. • 2. Atoms of the same element are identical. The atoms of one element are different from the atoms of another element. • 3. Atoms of different elements can physically mix together or can chemically com ...
Fall Semester Review Packet
... variable and a control. Describe how these variables relate to one another during an experiment. 12. Explain the difference between accuracy and precision when describing scientific measurements. 13. Explain how atoms of the same element may differ. Include all of the following terms in your explana ...
... variable and a control. Describe how these variables relate to one another during an experiment. 12. Explain the difference between accuracy and precision when describing scientific measurements. 13. Explain how atoms of the same element may differ. Include all of the following terms in your explana ...
Chapter 5: Electrons in Atoms
... sublevels and orbitals of electrons in an atom. 2. Determine how to write electron configuration and orbital notation for atoms and ions. ...
... sublevels and orbitals of electrons in an atom. 2. Determine how to write electron configuration and orbital notation for atoms and ions. ...
Ch 2 Atomic History
... Results: Most of the α particles went straight through the foil without deflection. Some α-particles were deflected at high angles. ...
... Results: Most of the α particles went straight through the foil without deflection. Some α-particles were deflected at high angles. ...
physical chemistry ii chem 3354
... De Broglie proposed that any moving particle (with a linear momentum r) should a wavelength – These “fictitious waves” are called mater waves. – The de Broglie relation can be derived from Eistein’s relativity theory and the Planck-Einstein relation. – The de Broglie relation can also be derived by ...
... De Broglie proposed that any moving particle (with a linear momentum r) should a wavelength – These “fictitious waves” are called mater waves. – The de Broglie relation can be derived from Eistein’s relativity theory and the Planck-Einstein relation. – The de Broglie relation can also be derived by ...
Simple Models for Classical Electron Radius and Spin
... current physical theories support such a thing. If one eliminates results with vr /c > 1, we left with results at the order 10−13 m. These are really big radius values for electron. From these results, one can say that in this format these models are away from the experimental measurements. ...
... current physical theories support such a thing. If one eliminates results with vr /c > 1, we left with results at the order 10−13 m. These are really big radius values for electron. From these results, one can say that in this format these models are away from the experimental measurements. ...
Simple harmonic motion= motion that repeats itself in an identical
... Atoms can only interact/release very precise quantities of energy. Energy in atoms is generally by electrons, and it determines the location of the electron. Why would an electron in an atom have energy? Electron energy is a combination of kinetic and electrical potential energy. The energy of an el ...
... Atoms can only interact/release very precise quantities of energy. Energy in atoms is generally by electrons, and it determines the location of the electron. Why would an electron in an atom have energy? Electron energy is a combination of kinetic and electrical potential energy. The energy of an el ...
THE CHEMICAL BASIS OF LIFE
... a. more H than OH _______________________ b. water loving _______________________ c. water hating _______________________ d. unit of an element _______________________ e. more OH than H _______________________ f. negatively charged subatomic particle _______________________ g. positively cha ...
... a. more H than OH _______________________ b. water loving _______________________ c. water hating _______________________ d. unit of an element _______________________ e. more OH than H _______________________ f. negatively charged subatomic particle _______________________ g. positively cha ...
Chapter 27 - Planet Holloway
... measurements from various materials The wavelength of the electrons calculated from the diffraction data agreed with the expected de Broglie wavelength This confirmed the wave nature of electrons Other experimenters have confirmed the wave nature of other particles ...
... measurements from various materials The wavelength of the electrons calculated from the diffraction data agreed with the expected de Broglie wavelength This confirmed the wave nature of electrons Other experimenters have confirmed the wave nature of other particles ...
chapter27
... Each photon can give all its energy to an electron in the metal The maximum kinetic energy of the liberated photoelectron is KEmax = hƒ – Φ Φ is called the work function of the metal ...
... Each photon can give all its energy to an electron in the metal The maximum kinetic energy of the liberated photoelectron is KEmax = hƒ – Φ Φ is called the work function of the metal ...
Document
... experiment, the electrons must have the same wavelength To have the same wavelength, the electrons must have the same momentum or equivalently, energy ...
... experiment, the electrons must have the same wavelength To have the same wavelength, the electrons must have the same momentum or equivalently, energy ...
Bonding in Solids, Structural and Chemical Properties
... molecular. Unfortunately, this division conceals the more interesting fact that a pure bonding type is very unusual. In fact, simple covalency only occurs between isolated homonuclear pairs, such as in the diamond allotrope of carbon. Conversely, the graphite allotrope of carbon exhibits both distin ...
... molecular. Unfortunately, this division conceals the more interesting fact that a pure bonding type is very unusual. In fact, simple covalency only occurs between isolated homonuclear pairs, such as in the diamond allotrope of carbon. Conversely, the graphite allotrope of carbon exhibits both distin ...
Bohr model
In atomic physics, the Rutherford–Bohr model or Bohr model, introduced by Niels Bohr in 1913, depicts the atom as a small, positively charged nucleus surrounded by electrons that travel in circular orbits around the nucleus—similar in structure to the solar system, but with attraction provided by electrostatic forces rather than gravity. After the cubic model (1902), the plum-pudding model (1904), the Saturnian model (1904), and the Rutherford model (1911) came the Rutherford–Bohr model or just Bohr model for short (1913). The improvement to the Rutherford model is mostly a quantum physical interpretation of it. The Bohr model has been superseded, but the quantum theory remains sound.The model's key success lay in explaining the Rydberg formula for the spectral emission lines of atomic hydrogen. While the Rydberg formula had been known experimentally, it did not gain a theoretical underpinning until the Bohr model was introduced. Not only did the Bohr model explain the reason for the structure of the Rydberg formula, it also provided a justification for its empirical results in terms of fundamental physical constants.The Bohr model is a relatively primitive model of the hydrogen atom, compared to the valence shell atom. As a theory, it can be derived as a first-order approximation of the hydrogen atom using the broader and much more accurate quantum mechanics and thus may be considered to be an obsolete scientific theory. However, because of its simplicity, and its correct results for selected systems (see below for application), the Bohr model is still commonly taught to introduce students to quantum mechanics or energy level diagrams before moving on to the more accurate, but more complex, valence shell atom. A related model was originally proposed by Arthur Erich Haas in 1910, but was rejected. The quantum theory of the period between Planck's discovery of the quantum (1900) and the advent of a full-blown quantum mechanics (1925) is often referred to as the old quantum theory.