Problem Set 1 (Due January 30th by 7:00 PM) Answers to the
... 16. Calculate the threshold energy (in Joules) of a metal surface if an electron is ejected travelling at 7.308 x 105 m/s upon irradiation with a wavelength of: a. 400 nm b. 580 nm 17. For each of the following sets of atoms, determine which has the smallest radius. a. P, As, S, or Se? b. O, Cl, Xe, ...
... 16. Calculate the threshold energy (in Joules) of a metal surface if an electron is ejected travelling at 7.308 x 105 m/s upon irradiation with a wavelength of: a. 400 nm b. 580 nm 17. For each of the following sets of atoms, determine which has the smallest radius. a. P, As, S, or Se? b. O, Cl, Xe, ...
Basic Atomic Theory
... forces • Strength of Coulomb forces much larger than gravitational • +ve and –ve charges cause attractive and repulsive interactions. ...
... forces • Strength of Coulomb forces much larger than gravitational • +ve and –ve charges cause attractive and repulsive interactions. ...
Molecular Geometry and Chemical Bonding Theory
... The Valence -Shell Electron -Pair Repulsion (VSEPR) Model predicts the shapes of the molecules and ions by assuming that the valence shell electron pairs are arranged as far from one another as possible. To predict the relative position of the atoms around a given central atom using the VESPR model ...
... The Valence -Shell Electron -Pair Repulsion (VSEPR) Model predicts the shapes of the molecules and ions by assuming that the valence shell electron pairs are arranged as far from one another as possible. To predict the relative position of the atoms around a given central atom using the VESPR model ...
CHAPTER 5
... electrons in the same atom can have the same set of quantum #’s • 3. Hund’s Rule- orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second electron • all electrons in single occupied orbitals must have the same spin ...
... electrons in the same atom can have the same set of quantum #’s • 3. Hund’s Rule- orbitals of equal energy are each occupied by 1 electron before any orbital is occupied by a second electron • all electrons in single occupied orbitals must have the same spin ...
Chapter 9: Chemical Quantities
... Properties of Light - wavelength, frequency and energy of light - electromagnetic spectrum and energy of light - spectrum and energy of visible light ...
... Properties of Light - wavelength, frequency and energy of light - electromagnetic spectrum and energy of light - spectrum and energy of visible light ...
CHEMISTRY – UNITS 3 and 4 REVIEW PACKET Name Date
... Formula for calculating half-life and/or total time elapsed: ...
... Formula for calculating half-life and/or total time elapsed: ...
Ch. 2: The Chemical Context of Life AP Reading Guide
... Concept 2.1 Matter consists of chemical elements in pure form and in combinations called compounds 1. Define and give an example of the following terms: matter, element, compound. 2. What four elements make up 96% of all living matter? 3. What is the difference between an essential element and a tra ...
... Concept 2.1 Matter consists of chemical elements in pure form and in combinations called compounds 1. Define and give an example of the following terms: matter, element, compound. 2. What four elements make up 96% of all living matter? 3. What is the difference between an essential element and a tra ...
Quantum Theory of the Atom
... particle and a wave, we can start to understand the emission spectra of atoms. One in particular, hydrogen (shown below) The theory of Planck and Einstein states that there are only certain allowable energy levels or states. The lowest allowable state is called the ground state. ...
... particle and a wave, we can start to understand the emission spectra of atoms. One in particular, hydrogen (shown below) The theory of Planck and Einstein states that there are only certain allowable energy levels or states. The lowest allowable state is called the ground state. ...
Review for Exam 1
... orbitals in the same shell have the same _______________ and similar ___________. n = 1, 2, 3, ... ......K, L, M, N, ...... 2) All atomic orbitals with the same value of n, but different l values are said to be in different _____________ or _____________ of a given shell. l = 0, 1, 2, 3, 4, ........ ...
... orbitals in the same shell have the same _______________ and similar ___________. n = 1, 2, 3, ... ......K, L, M, N, ...... 2) All atomic orbitals with the same value of n, but different l values are said to be in different _____________ or _____________ of a given shell. l = 0, 1, 2, 3, 4, ........ ...
amu (atomic mass unit): a unit used to express very small masses
... Niels Bohr's ideas of electron distribution within the atom are useful concepts and laid the foundation for much of the later progress in understanding atomic structure. But, as is the case with many theories, Bohr's assumptions have had to be modified. Difficulty arose in applying the theory to at ...
... Niels Bohr's ideas of electron distribution within the atom are useful concepts and laid the foundation for much of the later progress in understanding atomic structure. But, as is the case with many theories, Bohr's assumptions have had to be modified. Difficulty arose in applying the theory to at ...
Chapter 40
... Sodium: The atom has 11 electrons. Ten of them form a closed neon-like core, and has zero angular momentum. The remaining electron is largely outside this inert core, in the 3s subshell. This is the valence electron of the atom, and the atom’s angular momentum and magnetic dipole moment must be due ...
... Sodium: The atom has 11 electrons. Ten of them form a closed neon-like core, and has zero angular momentum. The remaining electron is largely outside this inert core, in the 3s subshell. This is the valence electron of the atom, and the atom’s angular momentum and magnetic dipole moment must be due ...
1.3.4 Atoms and molecules Name Symbol Definition SI unit Notes
... The concept of electronegativity was intoduced by L. Pauling as the power of an atom in a molecule to attract electrons to itself. There are several ways of defining this quantity. The one given in the table has a clear physical meaning of energy and is due to R.S. Mulliken. The most frequently used ...
... The concept of electronegativity was intoduced by L. Pauling as the power of an atom in a molecule to attract electrons to itself. There are several ways of defining this quantity. The one given in the table has a clear physical meaning of energy and is due to R.S. Mulliken. The most frequently used ...
Atomic Structure
... to study the behavior of small particles going at high speeds. Classical mechanics studies large particles going at relatively slow speeds. Since electrons are small particles going at high speeds the electron (and thus chemistry) can only be understood through the use of quantum mechanics. ...
... to study the behavior of small particles going at high speeds. Classical mechanics studies large particles going at relatively slow speeds. Since electrons are small particles going at high speeds the electron (and thus chemistry) can only be understood through the use of quantum mechanics. ...
Chapter 8 - Bakersfield College
... B. A spectroscope is an instrument that disperses the light emitted by an excited gas into the different frequencies the light contains. C. An emission spectrum consists of the various frequencies of light given off by an excited substance. D. A continuous spectrum consists of all frequencies of lig ...
... B. A spectroscope is an instrument that disperses the light emitted by an excited gas into the different frequencies the light contains. C. An emission spectrum consists of the various frequencies of light given off by an excited substance. D. A continuous spectrum consists of all frequencies of lig ...
Frank-Hertz Experiment with Argon
... Prize in Physics in 1925 for this work. In the early 20th century, experiments by Ernest Rutherford established that atoms consisted of a diffuse cloud of negatively charged electrons surrounding a small, dense, positively charged nucleus. Given this experimental data, Rutherford naturally considere ...
... Prize in Physics in 1925 for this work. In the early 20th century, experiments by Ernest Rutherford established that atoms consisted of a diffuse cloud of negatively charged electrons surrounding a small, dense, positively charged nucleus. Given this experimental data, Rutherford naturally considere ...
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.