1. Atomic Structure
... The orbital with the lowest (n + l) value is filled first. When two or more orbitals have the same (n + l) value, the one with the lowest ‘n’ value is preferred in filling. Consider two orbitals 3d and 4s. The n + l value of 3d = 3 + 2 = 5 and of 4s = 4 + 0 = 4. Since 4s has lowest (n + l) value, it ...
... The orbital with the lowest (n + l) value is filled first. When two or more orbitals have the same (n + l) value, the one with the lowest ‘n’ value is preferred in filling. Consider two orbitals 3d and 4s. The n + l value of 3d = 3 + 2 = 5 and of 4s = 4 + 0 = 4. Since 4s has lowest (n + l) value, it ...
Atomic Structure and Periodicity
... Section 7.7 Orbital Shapes • Areas of high probability are separate by areas of low probability. (NODES) • Degenerate orbitals have different orientation or shape but the same ENERGY. • Lowest available energy level for an electron = ground state • Higher energy levels than expected = excited state ...
... Section 7.7 Orbital Shapes • Areas of high probability are separate by areas of low probability. (NODES) • Degenerate orbitals have different orientation or shape but the same ENERGY. • Lowest available energy level for an electron = ground state • Higher energy levels than expected = excited state ...
Final Exam Review
... D. 5.96 g KOH E. 937 g Ca( C2H3O2)2 F. 0.800 g Ca 111. classify each of the following as a physical change or a chemical change: A. an aspirin tablet is crushed to a powder B. a red rose turns brown C. grape juice turns to wine D. fingernail polish remover evaporates E. a bean seed sprouts F. a piec ...
... D. 5.96 g KOH E. 937 g Ca( C2H3O2)2 F. 0.800 g Ca 111. classify each of the following as a physical change or a chemical change: A. an aspirin tablet is crushed to a powder B. a red rose turns brown C. grape juice turns to wine D. fingernail polish remover evaporates E. a bean seed sprouts F. a piec ...
5. The Hydrogenoid Atom
... We have derived the same quantized energy expression as that of the BOHR classical model of the Hydrogenic atom, but this time it was derived rigorously from Quantum Mechanics. The quantization once again results from imposing boundary conditions on the wavefunction. ...
... We have derived the same quantized energy expression as that of the BOHR classical model of the Hydrogenic atom, but this time it was derived rigorously from Quantum Mechanics. The quantization once again results from imposing boundary conditions on the wavefunction. ...
Activity 17 Follow-up
... very reactive. When the sodium reacts with the water it takes the place of one of the hydrogen atoms. This happens because sodium is more reactive than the hydrogen it is replacing. Reactivity is largely due to the atomic radius of an element and the valence. Larger metals lose their outer electrons ...
... very reactive. When the sodium reacts with the water it takes the place of one of the hydrogen atoms. This happens because sodium is more reactive than the hydrogen it is replacing. Reactivity is largely due to the atomic radius of an element and the valence. Larger metals lose their outer electrons ...
Ch 5 Electrons in Atoms
... a. Describe how isotopes of the same element differ from one another b. Do isotopes of the same element have the same chemical properties? c. Explain how the number of neutrons affect the mass of an atom 8. Chemical properties of an atom are mostly determined by overall charge and total number of po ...
... a. Describe how isotopes of the same element differ from one another b. Do isotopes of the same element have the same chemical properties? c. Explain how the number of neutrons affect the mass of an atom 8. Chemical properties of an atom are mostly determined by overall charge and total number of po ...
Chapter 3 Study Guide
... i. Tells you the order in which electrons fill up an atom. b. Rules to obey when determining electron configurations: i. Pauli Exclusion Principle: no two electrons in the same orbital can have the same 4 quantum numbers. ii. aufbau principle: electrons fill up the lowest available energy levels fir ...
... i. Tells you the order in which electrons fill up an atom. b. Rules to obey when determining electron configurations: i. Pauli Exclusion Principle: no two electrons in the same orbital can have the same 4 quantum numbers. ii. aufbau principle: electrons fill up the lowest available energy levels fir ...
Notes on the Electronic Structure of Atoms
... though, so does the repulsion between them. h • Therefore, in many‐ electron atoms orbitals electron atoms, orbitals on the same energy level are no longer degenerate. • Orbitals in the same subshell are degenerate subshell are degenerate ...
... though, so does the repulsion between them. h • Therefore, in many‐ electron atoms orbitals electron atoms, orbitals on the same energy level are no longer degenerate. • Orbitals in the same subshell are degenerate subshell are degenerate ...
Chapter 5
... circling around a nucleus and concluded that electrons have specific energy levels. • Erwin Schrödinger (1887–1961): Proposed quantum mechanical model of atom, which focuses on wavelike properties of electrons. ...
... circling around a nucleus and concluded that electrons have specific energy levels. • Erwin Schrödinger (1887–1961): Proposed quantum mechanical model of atom, which focuses on wavelike properties of electrons. ...
lecture notes, page 2
... • Unlike s orbitals, p-orbitals have θ, φ dependence. P-orbitals _____________ spherically symmetrical. • p orbitals consist of two lobes (of opposite sign) separated by a _____________ plane on which Ψ = 0 (and Ψ2 = 0). • There is zero probability of finding a p-electron in a nodal plane. Thus, ...
... • Unlike s orbitals, p-orbitals have θ, φ dependence. P-orbitals _____________ spherically symmetrical. • p orbitals consist of two lobes (of opposite sign) separated by a _____________ plane on which Ψ = 0 (and Ψ2 = 0). • There is zero probability of finding a p-electron in a nodal plane. Thus, ...
2.4. Quantum Mechanical description of hydrogen atom
... Radial electron density: probability of finding the electron at distance r from the nuclei (i.e. in a shell of the spere). ...
... Radial electron density: probability of finding the electron at distance r from the nuclei (i.e. in a shell of the spere). ...
The Atom and Its Properties
... • See how frequency of light emitted by an atom is unique to that atom • Compare and contrast the Bohr and quantum mechanical models of the atom • Express the arrangements of electrons in atoms through orbital notations, electron configurations, and electron dot structures ...
... • See how frequency of light emitted by an atom is unique to that atom • Compare and contrast the Bohr and quantum mechanical models of the atom • Express the arrangements of electrons in atoms through orbital notations, electron configurations, and electron dot structures ...
Chapter 7 Atomic Structure and Periodicity Study Guide
... no more than a mathematical function describing the standing wave that gives the probability of the electron manifesting itself at any given location in space. More commonly (and loosely) we use the word to describe the region of space in which an electron is likely to be found. Each kind of orbital ...
... no more than a mathematical function describing the standing wave that gives the probability of the electron manifesting itself at any given location in space. More commonly (and loosely) we use the word to describe the region of space in which an electron is likely to be found. Each kind of orbital ...
Chemistry - chem.uwec.edu
... Inner electrons shield outer electrons more effectively than do electrons in the same sublevel. ...
... Inner electrons shield outer electrons more effectively than do electrons in the same sublevel. ...
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.