CHEMISTRY
... Most atoms team up with or overtake other atoms in an attempt to get the “right” number of electrons. This is how molecules are formed. Only the NOBLE GASSES can exist on their own. ATOMS will switch partners when provoked. This is what chemical reactions are all about. Don’t mess with an atom’s nuc ...
... Most atoms team up with or overtake other atoms in an attempt to get the “right” number of electrons. This is how molecules are formed. Only the NOBLE GASSES can exist on their own. ATOMS will switch partners when provoked. This is what chemical reactions are all about. Don’t mess with an atom’s nuc ...
Periodic Table Puzzle
... Periodic Table Puzzle The code letters A to Z have been assigned to represent the first 26 representative elements in the Periodic Table. The letters do not relate to the actual chemical symbols for these elements. Your challenge is to put the code letters in the correct boxes in the Periodic Table, ...
... Periodic Table Puzzle The code letters A to Z have been assigned to represent the first 26 representative elements in the Periodic Table. The letters do not relate to the actual chemical symbols for these elements. Your challenge is to put the code letters in the correct boxes in the Periodic Table, ...
Arrangement of the Electrons Chapter 4
... 1.) The electron travels in orbits (energy levels) around the nucleus. 2.) The orbits closest to the nucleus are lowest in energy, those further out are higher in energy. 3.) When energy is absorbed by the atom, the electron moves into a higher energy orbit. This energy is released when the elec ...
... 1.) The electron travels in orbits (energy levels) around the nucleus. 2.) The orbits closest to the nucleus are lowest in energy, those further out are higher in energy. 3.) When energy is absorbed by the atom, the electron moves into a higher energy orbit. This energy is released when the elec ...
Lecture 24: Quantum mechanics
... Question then arose how do we prove the wave nature of electrons. In a brilliant experiment, Stern and Gerlach proved this. They exploited Huygen’s principle that was used to prove light is wave. The primary effect of wave nature is the observation of diffraction or interference phenomena. Using sin ...
... Question then arose how do we prove the wave nature of electrons. In a brilliant experiment, Stern and Gerlach proved this. They exploited Huygen’s principle that was used to prove light is wave. The primary effect of wave nature is the observation of diffraction or interference phenomena. Using sin ...
Study Guide Matter: Building Blocks of the Universe
... You should be prepared to answer questions on these topics. * Know the key people in the history of the atom and their contribution to our understanding of the atom. These should be in your lab book conclusion for shoe box atoms. * Know the atomic particles: electron, neutron, and proton. where are ...
... You should be prepared to answer questions on these topics. * Know the key people in the history of the atom and their contribution to our understanding of the atom. These should be in your lab book conclusion for shoe box atoms. * Know the atomic particles: electron, neutron, and proton. where are ...
m ι
... • Wavelength (l, lambda): a measure of the distance covered by the wave. • Frequency (n, nu): the number of waves that pass a point in a given period of time. Unit = cycles/s or s–1 (Hz, hertz). ...
... • Wavelength (l, lambda): a measure of the distance covered by the wave. • Frequency (n, nu): the number of waves that pass a point in a given period of time. Unit = cycles/s or s–1 (Hz, hertz). ...
Electronic Structure of Atoms
... – Indicate whether the wavelength calculated in the previous part is longer or shorter than the wavelength assoicated with an electron moving from n=5 to n=2. Explain (there are no calculations involved) ...
... – Indicate whether the wavelength calculated in the previous part is longer or shorter than the wavelength assoicated with an electron moving from n=5 to n=2. Explain (there are no calculations involved) ...
Electron Configuration (You will have to read this more than once to
... This is where our buddies Schrodinger and Heisenberg come in. They took the idea that the energies that electrons could hold are quantized and they ran with it. Heisenberg went off and studied the nature of light and the nature of electrons. As it turns out light is made up of really tiny particles ...
... This is where our buddies Schrodinger and Heisenberg come in. They took the idea that the energies that electrons could hold are quantized and they ran with it. Heisenberg went off and studied the nature of light and the nature of electrons. As it turns out light is made up of really tiny particles ...
Chapter 7
... • The energy of a photon given off can be calculated by subtracting the lower energy level from the higher energy level (energy of a photon is positive) ...
... • The energy of a photon given off can be calculated by subtracting the lower energy level from the higher energy level (energy of a photon is positive) ...
Chapter 12 Worksheet
... 3. According to Heisenberg uncertainty principle; a. the momentum of a particle cannot be measured precisely b. neither the position nor the momentum can be measured precisely c. the position and the momentum of a particle can be measured precisely, but not at the same time d. the positon of a parti ...
... 3. According to Heisenberg uncertainty principle; a. the momentum of a particle cannot be measured precisely b. neither the position nor the momentum can be measured precisely c. the position and the momentum of a particle can be measured precisely, but not at the same time d. the positon of a parti ...
Slide 1
... waves can behave as particles and particles can behave as waves. This is called wave– particle duality. m = mass in kg p = momentum (mc) or (mv) h h For Light : = ...
... waves can behave as particles and particles can behave as waves. This is called wave– particle duality. m = mass in kg p = momentum (mc) or (mv) h h For Light : = ...
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.