Chapter7 - FSU Chemistry
... (b) How many liters of CO2 (at 25 oC and 1 atm, R = 0.0821 atm.L/mol.K) are formed when 1 kg of octane is burned? How much work is done by the expanding CO2 as 1 kg of octane is burned (again, at 25 oC and 1 atm). (Hint, 1 J = 9.87.10-3 atm.L). What is !E for the reaction? (Hint, the definition of H ...
... (b) How many liters of CO2 (at 25 oC and 1 atm, R = 0.0821 atm.L/mol.K) are formed when 1 kg of octane is burned? How much work is done by the expanding CO2 as 1 kg of octane is burned (again, at 25 oC and 1 atm). (Hint, 1 J = 9.87.10-3 atm.L). What is !E for the reaction? (Hint, the definition of H ...
File
... Heisenberg’s uncertainty principle governs behaviour of electrons impossible to define a point in space where electron certain to be found regions in space where probability of finding an electron high atomic orbitals n defines orbital size l defines shape of orbital MM 2006 AH ...
... Heisenberg’s uncertainty principle governs behaviour of electrons impossible to define a point in space where electron certain to be found regions in space where probability of finding an electron high atomic orbitals n defines orbital size l defines shape of orbital MM 2006 AH ...
Atomic Structure
... Pauli Exclusion Principle = no 2 electrons can have the same set of quantum numbers Example: Sulfur Identify Group, Period, block, total # eWrite orbital notation/orbital diagrams to see specific quantum numbers for atoms/electrons lines/boxes with arrows (2 opposite arrows on each line) (Aufbau Pr ...
... Pauli Exclusion Principle = no 2 electrons can have the same set of quantum numbers Example: Sulfur Identify Group, Period, block, total # eWrite orbital notation/orbital diagrams to see specific quantum numbers for atoms/electrons lines/boxes with arrows (2 opposite arrows on each line) (Aufbau Pr ...
Band Theories
... If the atomic p orbitals lie higher in energy than the s orbitals, the the p band lies higher in energy than the s band and there may be a band gap – a range of energies to which no orbital corresponds. ...
... If the atomic p orbitals lie higher in energy than the s orbitals, the the p band lies higher in energy than the s band and there may be a band gap – a range of energies to which no orbital corresponds. ...
7.4 The Quantum-Mechanical Model of the Atom
... – Assumes the quantization without explanation – Does not take into account Heisenberg’s uncertainty principle – Limited success only for the H atom ...
... – Assumes the quantization without explanation – Does not take into account Heisenberg’s uncertainty principle – Limited success only for the H atom ...
Theories of Covalent Bonding
... • Hybridization – mathematical mixing of two or more valence orbitals on the same atom – Result → hybrid orbitals – The hybrid orbitals have shapes and orientations different than the original orbitals being mixed – The number of hybrid orbitals equals the number of original orbitals – The hybrid or ...
... • Hybridization – mathematical mixing of two or more valence orbitals on the same atom – Result → hybrid orbitals – The hybrid orbitals have shapes and orientations different than the original orbitals being mixed – The number of hybrid orbitals equals the number of original orbitals – The hybrid or ...
Quantum Theory of the Atom
... B. Orbitals – describes the electron’s location 1. 2 electrons per orbital 2. s sublevel has 1 orbital (2 electrons total) 3. p sublevel has 3 orbital (6 electrons total) 4. d sublevel has 5 orbital (10 electrons total ) 5. f sublevel has 7 orbital (14 electrons total) Looking at the periodic table ...
... B. Orbitals – describes the electron’s location 1. 2 electrons per orbital 2. s sublevel has 1 orbital (2 electrons total) 3. p sublevel has 3 orbital (6 electrons total) 4. d sublevel has 5 orbital (10 electrons total ) 5. f sublevel has 7 orbital (14 electrons total) Looking at the periodic table ...
Ch4 notes - Midway ISD
... • l = zero and all positive integers less than or equal to n-1 • l=0, s orbital (spherical) • l=1, p orbital (dumbbell) • l=2, d orbital • l=3, f orbital ...
... • l = zero and all positive integers less than or equal to n-1 • l=0, s orbital (spherical) • l=1, p orbital (dumbbell) • l=2, d orbital • l=3, f orbital ...
Answers to questions on test #2
... [3] (6) Estimate the effective nuclear charge Zef f felt by one of the two electrons in the He atom ground state, configuration 1s2 . You can use Slater’s rules if you know them, or use any other reasonable way to estimate Zef f . Whatever you do, explain how you get your answer. Slater’s rules: Zef ...
... [3] (6) Estimate the effective nuclear charge Zef f felt by one of the two electrons in the He atom ground state, configuration 1s2 . You can use Slater’s rules if you know them, or use any other reasonable way to estimate Zef f . Whatever you do, explain how you get your answer. Slater’s rules: Zef ...
Orbitals and energy levels
... energies an electron can have and how likely it is to find the electron in various locations around the nucleus. This model is based on equations developed by Erwin ...
... energies an electron can have and how likely it is to find the electron in various locations around the nucleus. This model is based on equations developed by Erwin ...
4 colour slides per page
... The most probable distance increases with n but decreases with l. Note also that the radial nodes decrease with l. Notice that the 2s orbital has a small region of electron density in close to the nucleus, while the 2p orbital does not. ...
... The most probable distance increases with n but decreases with l. Note also that the radial nodes decrease with l. Notice that the 2s orbital has a small region of electron density in close to the nucleus, while the 2p orbital does not. ...
Quantum Numbers and Orbitals
... • Now let’s apply this to the p – orbitals. • Recall: There are three p – orbitals and they are the px , py , and pz . • From the slide above we see that the magnetic quantum numbers for the p – orbitals are as ...
... • Now let’s apply this to the p – orbitals. • Recall: There are three p – orbitals and they are the px , py , and pz . • From the slide above we see that the magnetic quantum numbers for the p – orbitals are as ...
4.quantumorbitals
... Quantum Theory The electron is like a cloud of negative energy or a wave. Orbitals are areas in 3D space where the electrons most probably are. The energy of the electron is in its vibrational modes- like notes on a guitar string. Photons are produced when high energy modes change to lower energy mo ...
... Quantum Theory The electron is like a cloud of negative energy or a wave. Orbitals are areas in 3D space where the electrons most probably are. The energy of the electron is in its vibrational modes- like notes on a guitar string. Photons are produced when high energy modes change to lower energy mo ...
Lewis
... n → size, l → shape, m → orientation, s → spin of e; Pauli principle (not all 4 quantum numbers can be equal), Hund‘s rule (spin maximizing). ...
... n → size, l → shape, m → orientation, s → spin of e; Pauli principle (not all 4 quantum numbers can be equal), Hund‘s rule (spin maximizing). ...
Molecular orbital
In chemistry, a molecular orbital (or MO) is a mathematical function describing the wave-like behavior of an electron in a molecule. This function can be used to calculate chemical and physical properties such as the probability of finding an electron in any specific region. The term orbital was introduced by Robert S. Mulliken in 1932 as an abbreviation for one-electron orbital wave function. At an elementary level, it is used to describe the region of space in which the function has a significant amplitude. Molecular orbitals are usually constructed by combining atomic orbitals or hybrid orbitals from each atom of the molecule, or other molecular orbitals from groups of atoms. They can be quantitatively calculated using the Hartree–Fock or self-consistent field (SCF) methods.