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The document summarizes the quantum model of the atom. It describes how electrons exhibit wave-like properties and have quantized wavelengths. The Heisenberg uncertainty principle states that it is impossible to know both the velocity and position of an electron at the same time. Schrodinger's wave equation defines quantized energy levels and the probability of finding an electron. Electrons occupy orbitals defined by four quantum numbers that specify the electron's unique "address" within the atom.
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2) The Schrodinger equation led to the discovery of quantum numbers that describe electron behavior and allowed for a more accurate model of atomic structure.
3) There are four quantum numbers - the principal quantum number (n) describes the electron shell or energy level, the azimuthal quantum number (l) describes the subshell shape, the magnetic quantum number (m) describes spatial orientation, and the spin quantum number (s) describes electron spin.
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Electrons in atoms are arranged in energy levels (n), sublevels (l), and orbitals (ml). Quantum mechanics treats electrons as waves that can only gain or lose discrete amounts of energy called quanta when changing energy levels. Each energy level corresponds to a row on the periodic table and can contain one or more sublevels representing blocks. Sublevels include s, p, d and f orbitals which electrons fill according to specific rules. The electronic configuration notation specifies the distribution of electrons among the atomic orbitals.
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The document discusses the four quantum numbers that describe electrons in atoms: principal quantum number (n), azimuthal/angular momentum quantum number (l), magnetic quantum number (m), and spin quantum number (s). N determines the shell and average distance from the nucleus. L determines the subshell and shape. M gives orbital orientation. S indicates electron spin direction as clockwise or counterclockwise. Each number has specific allowed values and properties that provide the electron's precise location.
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Electron configurations provide information about the location of electrons in an atom's orbitals. There are three main rules for determining electron configurations: 1) electrons fill orbitals starting with the lowest energy levels and moving upwards, 2) the Pauli exclusion principle states that no two electrons can occupy the same orbital with the same spin, and 3) Hund's rule states that electrons will occupy orbitals singly before pairing up. Writing out electron configurations involves determining the element's number of electrons and following the Aufbau principle of filling orbitals in order of increasing energy.
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The document discusses electron configurations and periodic trends in atomic properties. It describes how electrons fill atomic orbitals according to the building-up principle and Hund's rule. Trends in atomic radius, ionization energy, and electron affinity across the periodic table are also explained, with atomic radius generally decreasing and ionization energy and electron affinity (becoming more negative) generally increasing within a period. Exceptions to trends are seen for some p-block elements.
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The document discusses several key concepts in quantum mechanics:
- Electrons exist in distinct energy levels around the nucleus, originally conceived as orbits but now understood as areas of high probability.
- Light and subatomic particles have both wave and particle properties, described by Planck, De Broglie, and photons.
- Quantum numbers (n, l, m, s) define the distinct energy states of electrons in atoms, analogous to a unique address.
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The modern model of the atom is based on the ideas that electrons behave as both particles and waves and are subject to the Heisenberg uncertainty principle. This quantum mechanical model describes atoms as consisting of energy levels that electrons can occupy, with different orbitals defining the regions where electrons are likely to be located within these levels. The locations and properties of orbitals are determined by quantum numbers, and electron configurations represent the filling of these orbitals according to various principles like Aufbau and Pauli exclusion.
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The document discusses the quantum numbers that describe the electron states in an atom. It explains that each electron is labeled by four quantum numbers: principal (n), angular momentum (l), magnetic (ml), and spin (ms). The Pauli Exclusion Principle states that no two electrons can occupy the same quantum state, which explains the filling order of atomic shells in the periodic table.
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1) The Bohr model of the atom provides accurate predictions of electron energy levels but is not physically realistic, as electrons do not actually orbit the nucleus in defined orbits.
2) Rutherford's nuclear model, based on his gold foil experiment, established that atoms are mostly empty space with a small, dense positively charged nucleus at the center.
3) Bohr's model incorporated Rutherford's nuclear model and quantized electron orbits, predicting discrete energy levels that explained atomic emission spectra. However, a fully correct quantum mechanical model was still needed.
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This document discusses electron configuration and the principles that govern how electrons are arranged in atoms. It explains that electrons exhibit wave-like properties and occupy regions of space called atomic orbitals. The distribution of electrons in atoms, known as electron configuration, follows three main principles: the Pauli Exclusion Principle limits orbitals to two electrons of opposite spin; the Aufbau Principle states that orbitals are filled from lowest to highest energy; and Hund's Rule specifies that orbitals are singly occupied with parallel electron spins before double occupation occurs.
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The document contains a test with 7 multiple choice questions covering topics in chemistry and physics including:
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3) Which electron transition in a hydrogen atom would result in the longest wavelength light
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6) The wavelength and absorption/emission of light from a hydrogen electron transition
7) The number of photons emitted from cesium that would produce 1 J of energy
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Hund's rules describe the ground state of multielectron atoms and ions. Rule 1 states that the atomic state with the highest total spin S will have the lowest energy. Rule 2 states that for a given spin multiplicity, the term with the largest orbital angular momentum L has the lowest energy. Rule 3 considers energy shifts due to spin-orbit coupling, where the splitting is determined by the spin-orbit coupling constant λ and the quantum numbers J, L, and S. Examples are provided to illustrate the application of Hund's rules to determine the ground states of silicon and titanium.
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1) Atomic orbitals are mathematical descriptions of where electrons are likely to be found in an atom, obtained by solving the Schrödinger equation. Orbitals have different shapes depending on the electron's energy and angular momentum.
2) Electrons occupy orbitals from lowest to highest energy, with each orbital holding up to two electrons of opposite spin. Orbitals are grouped into shells corresponding to different energy levels.
3) The spatial distribution and probability of finding electrons in an atom can be described as an "electron cloud". Electron configurations contribute greatly to chemical bonding and reactivity patterns.
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The document discusses the four quantum numbers that describe electrons in an atom: principal quantum number (n), azimuthal quantum number (l), magnetic quantum number (m), and spin quantum number (s). It provides details on each number, such as n describing the energy level, l defining the orbital shape, m specifying orbital orientation, and s representing electron spin. Examples are given to calculate the total electrons in different energy levels based on the quantum numbers.
Quantum & e config
The document discusses the quantum model of the atom and electron configurations. It introduces the four quantum numbers - principal, angular momentum, magnetic, and spin - that specify the location of each electron in an atom. The quantum numbers define orbitals that electrons occupy according to various rules, including the Aufbau principle in which electrons fill the lowest energy orbitals first, Hund's rule which places one electron per orbital, and the Pauli exclusion principle which prohibits two electrons from having the same four quantum numbers. Shorthand and longhand electron configurations are written using these principles. Periodic trends in electron configurations are also covered.
Chapter 4.2 : The Quantum Model of the Atom
Louis de Broglie proposed that electrons behave as waves, confined to certain regions around the nucleus at specific energy levels, known as orbitals. The Heisenberg Uncertainty Principle states that it is impossible to know both the position and momentum of an electron simultaneously. Schrodinger's wave equation treats electrons as waves and uses the uncertainty principle to describe the probability of finding electrons in certain orbital regions. Quantum numbers specify the properties of orbitals and electrons, including the principal quantum number for energy level, angular momentum quantum number for orbital shape, and magnetic quantum number for orbital orientation.
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The document discusses orbitals and quantum numbers. It introduces the four quantum numbers - principal (n), azimuthal (l), magnetic (ml), and spin (ms) - that describe an electron's location and properties. The classical view of electrons orbiting the nucleus like planets gave way to the modern atomic model where electrons exist as probabilistic wave functions within orbitals. Orbitals are regions of high probability of finding an electron and come in s, p, d, and f shapes depending on the quantum numbers. Electron configurations use these orbitals to describe the arrangement of electrons in atoms and predict properties.
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The document discusses the electronic structure of atoms based on various atomic models and theories. It describes Bohr's atomic model and theory, which explained the stability of atoms and formation of line spectra in hydrogen atoms. Bohr's model introduced quantized, discrete energy levels for electrons in atoms. The energy of an electron is determined by its principal quantum number. Electrons can absorb or emit photons of specific frequencies when transitioning between energy levels.
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This document discusses quantum theory and the electronic structure of atoms. It introduces quantum numbers like principal, angular momentum, and electron spin quantum numbers used to describe atomic orbitals. Atomic orbitals like s, p, and d orbitals are described along with their shapes and orientations. Electron configurations follow rules like the Aufbau principle, Pauli exclusion principle, and Hund's rule. The document shows how electrons fill atomic orbitals in order of increasing energy to write electron configurations of elements, which are represented using noble gas cores. Exceptions to electron filling order are noted for some transition metals.
Lecture 7
1) The document discusses the electronic configuration of atoms, including the development of wave mechanics and quantum theory to explain the structure of atoms. It introduces concepts like the de Broglie wavelength, quantum numbers, atomic orbitals and shapes, Pauli's exclusion principle, and Hund's rule for electron configuration.
2) Key scientists discussed include de Broglie, Heisenberg, Schrodinger, Pauli, and their contributions to developing models of the atom and allowing prediction of electron configurations.
3) The document provides examples of writing out electron configurations for elements and explaining the rules for filling atomic orbitals in the Aufbau principle.
Chemistry-Presentation.pptx
The document discusses the quantum numbers used to describe electrons in atoms. There are four quantum numbers: principal (n), angular momentum (l), magnetic (ml), and electron spin (ms). The principal quantum number defines the electron's energy level and average distance from the nucleus. The angular momentum number describes the orbital shape as s, p, d, or f. The magnetic number defines the orbital orientation. Orbitals are regions where electrons are likely to be found and have different shapes depending on the angular momentum number.
Quantum no.ppt
The Electron Cloud Model describes an atom as consisting of a dense nucleus surrounded by electrons that exist in different probability clouds or regions at various energy levels, as developed by Erwin Schrodinger and Werner Heisenburg. The Heisenberg Uncertainty Principle states that it is impossible to know both the momentum and position of a particle like an electron at the same time. To measure an electron's position requires striking it with a photon, which affects its motion and makes its momentum uncertain. Quantum numbers describe an electron's unique state and include the principal, angular, magnetic, and spin quantum numbers.
QUANTUM MECHANICAL MODEL.pptx
The document discusses the quantum mechanical model of the atom. It describes how Bohr's model improved on Rutherford's model by considering electrons as particles orbiting the nucleus in specific circular paths. Later, de Broglie proposed that electrons could be considered as both particles and waves. Schrodinger and Heisenberg further developed these ideas into mathematical models using quantum numbers to describe electron location and energy levels. The quantum numbers are n (principal), l (angular momentum), ml (magnetic), and ms (electron spin). Electron configuration notes how electrons fill these energy levels and orbitals according to Aufbau principle, Hund's rule, and Pauli exclusion principle.
Structure of atom Practice Exercise
Node is defined as a region where the probability of finding an electron is zero. According to Bohr's theory of the atomic model, electron orbits only certain allowed orbits where its angular momentum is an integral multiple of h/2π. The wavelength of a spectral line is inversely related to the difference in energy levels involved in an electronic transition between orbits.
Quantum numbers
The document discusses quantum numbers which describe the properties of an electron in an atom. There are three main quantum numbers - the principal quantum number n, which indicates the main energy level; the azimuthal quantum number l, which defines the orbital shape; and the magnetic quantum number ml, which describes the orientation of the orbital. Together these quantum numbers uniquely specify each atomic orbital an electron can occupy. The document provides examples of the quantum numbers for different atomic orbitals and energy levels.
chemistry. pptx.pptx
The document discusses the four quantum numbers used to describe electrons in atoms:
1. The principal quantum number (n) designates the principal electron shell. n is a positive integer.
2. The azimuthal quantum number (l) describes the orbital shape and ranges from 0 to n-1.
3. The magnetic quantum number (ml) determines the number and orientation of orbitals in a subshell.
4. The electron spin quantum number (ms) gives the direction of electron spin.
Together, the four quantum numbers uniquely describe each electron in an atom. Electrons fill atomic orbitals according to the Aufbau principle, occupying lower energy orbitals first.
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This document provides details about the chapter structure of the atom in a 10th standard chemistry textbook. It lists 100 multiple choice questions from the chapter, ranging from 1 to 4 marks. It covers topics like atomic theory, subatomic particles, cathode rays, atomic models (Thomson, Rutherford, Bohr), quantum numbers, electron configuration and orbitals. The chapter aims to teach students about the internal structure of atoms through experiments and quantum mechanical models.
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The document summarizes the development of atomic models from Rutherford to the current quantum mechanical model. It discusses inadequacies in Rutherford's model that could not explain atomic properties and emissions. Bohr proposed electrons orbit in distinct energy levels, but this failed to explain multi-electron atoms. The quantum mechanical model treats electrons as waves using Schrodinger's equation, describing electrons as probability distributions rather than particles. It introduces quantum numbers to characterize electron states and explains how orbitals are filled according to various rules.
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This document summarizes key concepts in atomic structure:
1. It outlines the early theories of Dalton, Thomson, Rutherford, and Bohr, which proposed that atoms are made of fundamental particles and have small, dense nuclei surrounded by orbiting electrons.
2. It describes experiments that discovered the electron and properties of cathode rays. Rutherford's gold foil experiment provided evidence for a small, dense nucleus.
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This document discusses the electronic structure of atoms and the periodic table. It covers:
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Quantum Numbers and Atomic Orbitals By solving t.pdf
Quantum Numbers and Atomic Orbitals By solving the Schrödinger equation (Hy
= Ey), we obtain a set of mathematical equations, called wave functions (y), which describe the
probability of finding electrons at certain energy levels within an atom. A wave function for an
electron in an atom is called an atomic orbital; this atomic orbital describes a region of space in
which there is a high probability of finding the electron. Energy changes within an atom are the
result of an electron changing from a wave pattern with one energy to a wave pattern with a
different energy (usually accompanied by the absorption or emission of a photon of light). Each
electron in an atom is described by four different quantum numbers. The first three (n, l, ml)
specify the particular orbital of interest, and the fourth (ms) specifies how many electrons can
occupy that orbital. Principal Quantum Number (n): n = 1, 2, 3, …, 8 Specifies the energy of
an electron and the size of the orbital (the distance from the nucleus of the peak in a radial
probability distribution plot). All orbitals that have the same value of n are said to be in the same
shell (level). For a hydrogen atom with n=1, the electron is in its ground state; if the electron is in
the n=2 orbital, it is in an excited state. The total number of orbitals for a given n value is n2.
Angular Momentum (Secondary, Azimunthal) Quantum Number (l): l = 0, ..., n-1. Specifies the
shape of an orbital with a particular principal quantum number. The secondary quantum number
divides the shells into smaller groups of orbitals called subshells (sublevels). Usually, a letter
code is used to identify l to avoid confusion with n: l 0 1 2 3 4 5 ... Letter s p d f g h ... The
subshell with n=2 and l=1 is the 2p subshell; if n=3 and l=0, it is the 3s subshell, and so on. The
value of l also has a slight effect on the energy of the subshell; the energy of the subshell
increases with l (s < p < d < f). Magnetic Quantum Number (ml): ml = -l, ..., 0, ..., +l. Specifies
the orientation in space of an orbital of a given energy (n) and shape (l). This number divides the
subshell into individual orbitals which hold the electrons; there are 2l+1 orbitals in each subshell.
Thus the s subshell has only one orbital, the p subshell has three orbitals, and so on. Spin
Quantum Number (ms): ms = +½ or -½. Specifies the orientation of the spin axis of an electron.
An electron can spin in only one of two directions (sometimes called up and down). The Pauli
exclusion principle (Wolfgang Pauli, Nobel Prize 1945) states that no two electrons in the same
atom can have identical values for all four of their quantum numbers. What this means is that no
more than two electrons can occupy the same orbital, and that two electrons in the same orbital
must have opposite spins. Because an electron spins, it creates a magnetic field, which can be
oriented in one of two directions. For two electrons in the same orbital, the spins must be
opposite to each oth.
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みなさんこんにちはこれ何文字まで入るの？40文字以下不可とか本当に意味わからないけどこれ限界文字数書いてないからマジでやばい文字数いけるんじゃないの？えこ...
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