3.3 orbital notation
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Orbital notation represents the electron configuration of an element by showing the placement of each electron through arrows. It illustrates the Pauli exclusion principle, which states that no two electrons in the same atom can have the same quantum numbers, requiring opposite spin directions. The homework involves writing out electron configurations using orbital notation diagrams for various elements like sodium, boron, and titanium.
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Orbital Notation
The document discusses orbital notation, which visually represents electron configuration by showing the placement and spin of each electron in an atom. It defines key terms like Pauli exclusion principle, Aufbau principle, and Hund's rule that govern how electrons fill atomic orbitals. Examples are given of writing the electron configurations of sodium, boron, titanium, and calcium using orbital notation with half arrows to symbolize individual electrons.
Chapter 4.3 : Electron Configuration
The document outlines objectives for learning about electron configuration including listing the number of electrons in each main energy level, stating the Aufbau principle, Pauli exclusion principle, and Hund's rule, and describing electron configurations using orbital, electron-configuration, and noble-gas notations. It then defines electron configuration and the ground state and provides rules for electron configuration including the Aufbau principle, Pauli exclusion principle, and Hund's rule.
Electron configuration
Electron configuration represents the arrangement of electrons in an atom's orbital shells and subshells. There are three main rules that determine electron configuration: the Aufbau principle, which states that orbitals are filled in order of increasing energy; the Pauli exclusion principle, where no two electrons can have the same quantum numbers; and Hund's rule, where orbitals in a subshell are singly occupied with parallel spins before pairing. Electron configuration can be written out or represented through orbital diagrams, the periodic table, or Möller diagrams.
Applied Chapter 3.3 : Electron Configuration
The document discusses electron configuration and the quantum models of the atom. It compares the Rutherford, Bohr, and quantum models. It explains the four quantum numbers - principal, angular momentum, magnetic, and spin quantum numbers. It describes how light emission spectra provide information about an atom's energy levels. Rules for writing electron configurations are given, including the Aufbau principle, Pauli exclusion principle, and Hund's rule. Orbital notation, electron configuration notation, and noble gas notation are defined. Examples are provided of writing the electron configuration for atoms with specific atomic numbers.
Ch. 7 electron configuration
- Electron configuration describes the arrangement of electrons in an atom's orbitals and energy levels according to 4 quantum numbers.
- The Pauli Exclusion Principle states that no two electrons can have the same set of 4 quantum numbers.
- Elements are arranged on the periodic table based on their electron configurations, with groups reflecting which orbitals are being filled.
- A noble gas configuration can be used to abbreviate long electron configurations by writing the nearest noble gas followed by the remaining electrons.
Electron configuration
This document discusses electron configuration and the rules that define how electrons are arranged in an atom's orbitals. It explains:
1) There are three main rules that define electron configuration: the Aufbau principle, Pauli exclusion principle, and Hund's rule.
2) Higher energy levels can hold more electrons than lower energy levels because they are associated with larger volumes that can contain more orbitals.
3) Electron configuration can be represented using orbital diagrams with arrows or electron configuration notation using symbols and superscripts.
Electronic configuration
The document discusses electronic configuration, which is the arrangement of electrons in an atom's orbitals. It is described using symbols that indicate the principal shell, subshell, and number of electrons. The Aufbau principle states that electrons fill the lowest available energy levels. Pauli's exclusion principle limits each orbital to two electrons with different quantum numbers. Hund's rule states that orbitals in a subshell will each have one electron before any are doubly filled, with parallel electron spins. Partial configurations, orbital diagrams, and number of inner electrons are provided for potassium, molybdenum, and lead as examples. Key terms like isoelectronic, valence electrons, and magnetic properties are also defined.
3.3 electron configuration
The document discusses electron configuration and energy levels. It introduces the historical models of the atom including Rutherford's plum pudding model and Bohr's model introducing energy levels. Modern models use orbitals that show the probability of finding electrons. Light can be described as both a wave and particle. Electrons absorb energy to move to excited states then emit light returning to ground states. Elements' electron configurations follow the aufbau principle filling lower energy orbitals first up to the periodic table.
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Orbital Notation
The document discusses orbital notation, which visually represents electron configuration by showing the placement and spin of each electron in an atom. It defines key terms like Pauli exclusion principle, Aufbau principle, and Hund's rule that govern how electrons fill atomic orbitals. Examples are given of writing the electron configurations of sodium, boron, titanium, and calcium using orbital notation with half arrows to symbolize individual electrons.
Chapter 4.3 : Electron Configuration
The document outlines objectives for learning about electron configuration including listing the number of electrons in each main energy level, stating the Aufbau principle, Pauli exclusion principle, and Hund's rule, and describing electron configurations using orbital, electron-configuration, and noble-gas notations. It then defines electron configuration and the ground state and provides rules for electron configuration including the Aufbau principle, Pauli exclusion principle, and Hund's rule.
Electron configuration
Electron configuration represents the arrangement of electrons in an atom's orbital shells and subshells. There are three main rules that determine electron configuration: the Aufbau principle, which states that orbitals are filled in order of increasing energy; the Pauli exclusion principle, where no two electrons can have the same quantum numbers; and Hund's rule, where orbitals in a subshell are singly occupied with parallel spins before pairing. Electron configuration can be written out or represented through orbital diagrams, the periodic table, or Möller diagrams.
Applied Chapter 3.3 : Electron Configuration
The document discusses electron configuration and the quantum models of the atom. It compares the Rutherford, Bohr, and quantum models. It explains the four quantum numbers - principal, angular momentum, magnetic, and spin quantum numbers. It describes how light emission spectra provide information about an atom's energy levels. Rules for writing electron configurations are given, including the Aufbau principle, Pauli exclusion principle, and Hund's rule. Orbital notation, electron configuration notation, and noble gas notation are defined. Examples are provided of writing the electron configuration for atoms with specific atomic numbers.
Ch. 7 electron configuration
- Electron configuration describes the arrangement of electrons in an atom's orbitals and energy levels according to 4 quantum numbers.
- The Pauli Exclusion Principle states that no two electrons can have the same set of 4 quantum numbers.
- Elements are arranged on the periodic table based on their electron configurations, with groups reflecting which orbitals are being filled.
- A noble gas configuration can be used to abbreviate long electron configurations by writing the nearest noble gas followed by the remaining electrons.
Electron configuration
This document discusses electron configuration and the rules that define how electrons are arranged in an atom's orbitals. It explains:
1) There are three main rules that define electron configuration: the Aufbau principle, Pauli exclusion principle, and Hund's rule.
2) Higher energy levels can hold more electrons than lower energy levels because they are associated with larger volumes that can contain more orbitals.
3) Electron configuration can be represented using orbital diagrams with arrows or electron configuration notation using symbols and superscripts.
Electronic configuration
The document discusses electronic configuration, which is the arrangement of electrons in an atom's orbitals. It is described using symbols that indicate the principal shell, subshell, and number of electrons. The Aufbau principle states that electrons fill the lowest available energy levels. Pauli's exclusion principle limits each orbital to two electrons with different quantum numbers. Hund's rule states that orbitals in a subshell will each have one electron before any are doubly filled, with parallel electron spins. Partial configurations, orbital diagrams, and number of inner electrons are provided for potassium, molybdenum, and lead as examples. Key terms like isoelectronic, valence electrons, and magnetic properties are also defined.
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The document discusses electron configuration and energy levels. It introduces the historical models of the atom including Rutherford's plum pudding model and Bohr's model introducing energy levels. Modern models use orbitals that show the probability of finding electrons. Light can be described as both a wave and particle. Electrons absorb energy to move to excited states then emit light returning to ground states. Elements' electron configurations follow the aufbau principle filling lower energy orbitals first up to the periodic table.
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The document provides an overview of electron configuration, which is the arrangement of electrons in an atom. It explains the key concepts of principal quantum number (n), sublevels (s, p, d, f), orbitals, the Aufbau principle, Pauli exclusion principle, Hund's rule, and how to write out the electron configuration for different elements. Examples are given for elements such as hydrogen, helium, lithium, carbon, nitrogen, fluorine, aluminum, argon, iron, and lanthanum.
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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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This document provides information about electron configuration, which describes the arrangement of electrons in an atom. It discusses three main principles for determining electron configuration:
1. The Aufbau principle states that electrons occupy the lowest available energy orbitals. Energy levels are filled in order of increasing energy, with s orbitals having the lowest energy followed by p, d, and f orbitals.
2. Hund's rule states that electrons occupy different orbitals within the same energy level with parallel spin before pairing electrons with opposite spin in the same orbital.
3. The Pauli exclusion principle allows no more than two electrons to occupy the same orbital, and these electrons must have opposite spins.
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The document discusses electronic configurations of atoms. It explains that the electron configuration represents the arrangement of electrons in an atom's orbital shells and subshells in its ground state, and can also represent ionized atoms. Many physical and chemical properties correlate to unique electron configurations, especially the valence electrons in the outermost shell. Electrons fill orbitals according to increasing energy levels and subshells in a set order. Orbital diagrams, spdf notation, and noble gas notation are used to represent electron configurations.
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This document provides information about electron configuration. It begins by defining electron configuration as the arrangement of electrons in an atom's orbitals, which is described using quantum numbers. It then discusses the three main rules for writing electron configurations: 1) Aufbau principle, which states that electrons fill the lowest available energy levels first, 2) Pauli exclusion principle, which limits each orbital to two electrons of opposite spin, and 3) Hund's rule, which states that degenerate orbitals will fill with one electron each before pairing. The document provides examples of writing full and condensed electron configurations and drawing orbital diagrams for various elements. It includes an activity for students to practice these skills.
Electron configuration
The document discusses electron configurations and how to write them. It explains that electron configurations describe how electrons are arranged in an atom's shells and subshells. It provides examples of writing configurations for different elements like oxygen, bromine, sulfur, rubidium, and barium. The document also introduces noble gas configurations, which provide a shorthand version of electron configurations by writing the closest noble gas in brackets followed by the remaining electrons.
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Periodic table n electron config
1. Electrons in atoms are arranged in shells, subshells, and orbitals according to their quantum numbers. Each orbital can contain a maximum of two electrons with opposing spins.
2. Atoms experience an effective nuclear charge that increases across a period, leading to higher ionization energies and smaller atomic and ionic sizes as more protons are exposed.
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Chm151 exam 4 slides sp10
This document covers electron energy levels, sublevels and orbitals. It discusses writing Lewis structures and determining molecular shape using VSEPR theory. Key points include:
- Electrons occupy discrete energy levels labeled by the principal quantum number n. Each level contains sublevels (s, p, d, f) that further divide electrons.
- Lewis structures show valence electron bonding using dots. Molecular shape is predicted by VSEPR to minimize electron pair repulsions based on the steric number.
- Resonance structures average to best depict molecules like HNO3 that resonate between structures. Formal charges help identify the most stable Lewis structure.
Quantum Mechanics
This document provides an overview of quantum mechanics concepts related to light and atomic structure. It discusses how light behaves as both a wave and particle, and introduces the electromagnetic spectrum. It then covers atomic structure concepts like electron configurations, energy levels, quantum numbers, and orbital shapes and filling diagrams. The document aims to explain how electrons are arranged in atoms and the underlying quantum mechanical principles.
Quantum Mechanic Model
The four quantum numbers specify the location of electrons in an atom. The principal quantum number (n) determines the electron's energy level and orbital size. Higher n means a larger orbital farther from the nucleus, increasing the atom's energy. The angular momentum quantum number (l) corresponds to an orbital's subshell type (s, p, d, f). The third and fourth quantum numbers further specify an electron's orientation. Electrons fill atomic orbitals according to Aufbau principle, Pauli exclusion principle, and Hund's rule to achieve the lowest energy configuration.
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Chemistry - Chp 5 - Electrons In Atoms - Powerpoint
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Martensen 3.1
This document discusses atomic theory and the key discoveries of Dalton. It explains that atoms are the fundamental building blocks of all matter, though they cannot be seen. Dalton proposed that elements are made of unique atom types, and compounds are made of two or more atom types combined in fixed ratios. The document reviews Dalton's five principles of atomic theory, including that atoms combine in whole number ratios. It provides examples of elemental and compound formulas showing atomic ratios.
2012 newsletter
This document provides information for students taking Chemistry class with Mr. Martensen in the fall of 2012. It outlines classroom rules, grading policies, and requirements for a scientific calculator. Students must have their own scientific calculator, as they will not be provided. The class builds skills incrementally through units, so it is important not to fall behind. Mr. Martensen offers help sessions and maintains a class website to support students.
Ch3 test prep
The document contains a series of questions and answers about chemistry concepts like electron configurations, noble gas configurations, and atom to element ratios. It reviews elements like chlorine, sodium, iron, bromine, barium, neptunium, cobalt, silver, tellurium, radium, and ruthenium. It also addresses common errors in writing electron configurations and calculates atom to element ratios for compounds like H2O, H2SO4, C6H12O6, and KClO3.
Ch3 test prep forslideshare
The document contains examples of chemistry problems involving elements, electron configurations, and ratios of atoms to elements in compounds. It provides the answers to questions about protons, neutrons, and electrons in chlorine. It also gives electron configurations for various elements as well as which elements have specific noble gas configurations. Finally, it lists the atom to element ratios for common compounds like H2O, H2SO4, C6H12O6, and KClO3.
13.3 solubility
When ionic compounds dissolve in water, they break down into their constituent ions. Water is able to dissolve ionic compounds because it is a polar solvent. The solubility of a substance depends on temperature - solids generally become more soluble as temperature increases while gases become less soluble. A saturated solution contains as much solute as can dissolve at a given temperature, while an unsaturated solution contains less and a supersaturated solution contains more.
13.2 molarity
Molarity describes the concentration of a solution in terms of moles of solute per liter of solution. To calculate molarity, you need the moles of solute and the total volume of solution. The moles of solute can be determined by converting any given mass of solute to moles using the molar mass. The total volume must include both the solute and solvent volumes, as adding solute increases the total volume of the solution. Proper unit conversion and labeling of final answers is important when calculating molarity.
13.1 solutions
A solution is a homogeneous mixture of two or more substances uniformly dispersed throughout a single phase. A suspension is a heterogeneous mixture where particles remain mixed while being stirred but later settle to the bottom. A colloid is a middle-sized mixture that is stable and homogeneous like a solution but contains particles that can be seen with a light microscope.
12.3
The document discusses key concepts relating to gases:
1) The ideal gas law (PV=nRT) relates pressure, volume, amount of gas, temperature using the gas constant R.
2) Gases diffuse from areas of higher to lower concentration until uniformly mixed.
3) Dalton's law of partial pressures states that in a gas mixture, each gas exerts pressure as if alone, and total pressure equals sums of partial pressures.
4) Ratios of gas volumes correspond to mole ratios in chemical equations based on Avogadro's law.
12.1
Gases have low density due to the long distances between particles that are in constant, rapid motion. Gases are fluids that can flow and be compressed into a smaller volume by increasing pressure from particle collisions. The kinetic-molecular theory describes gases as consisting of particles that are far apart and in constant, rapid motion, allowing gases to be fluids that fill their container and can be compressed.
12.2
This document summarizes four gas laws: Boyle's Law, Charles' Law, Gay-Lussac's Law, and Avogadro's Law. Boyle's Law states that gas pressure and volume are inversely related. Charles' Law describes the direct relationship between gas temperature and volume. Gay-Lussac's Law explains that gas pressure and temperature are directly related. Finally, Avogadro's Law says gas volume is directly proportional to the number of moles of gas at constant temperature and pressure. Homework problems are assigned from pages 425, 428, and 431 of the book to practice applying these gas laws.
12.2
This document summarizes three gas laws: Boyle's Law which relates pressure and volume, stating that as pressure increases, volume decreases; Charles's Law which relates temperature and volume, such that increasing temperature increases volume; and Gay-Lussac's Law which relates pressure and temperature, with increasing temperature also increasing pressure. It also introduces Avogadro's Law relating the volume and number of moles of gas at constant temperature and pressure conditions.
12.1
Gases have low density due to the long distances between their particles. Gases are compressible as gas particles can be moved closer together with increased pressure, decreasing the volume. Gases will completely fill any container as their particles are constantly moving and do not attract each other. Gas pressure is caused by collisions between gas molecules, and atmospheric pressure results from the weight of air above. Standard temperature and pressure was established to compare gases between experiments.
Stoichiometry
The document provides instructions on stoichiometry calculations using the decomposition of hydrogen peroxide as an example. It explains how to write and balance chemical equations, determine the mole ratios from coefficients, and use mole ratios to convert between amounts of reactants and products in moles, grams, and liters. Sample calculations are shown for determining moles, liters, and grams of reactants or products given amounts of other substances.
Classification of Reactions
The document classifies different types of chemical reactions:
1) Synthesis reactions involve combining two or more reactants to form one product.
2) Decomposition reactions involve breaking down one reactant into two or more products.
3) Single displacement reactions involve one compound exchanging ions with another.
4) Double displacement reactions involve two compounds exchanging ions to form two new compounds.
Balancing equations
The document discusses balancing chemical equations according to the law of conservation of matter. It states that chemical equations must have the same number and type of atoms on both sides. It provides examples of balancing sample equations by adding coefficients to the reactants and products so the number of each atom is equal. Diatomic elements like hydrogen, oxygen, nitrogen, chlorine are always written with a subscript of 2 when alone. The document demonstrates how to balance several example chemical equations.
8.1 the secret language of chemical equations
The document provides instructions on writing chemical formulas and equations. It defines the components of a formula, such as lithium carbonate (Li2CO3), and states that diatomic elements like hydrogen (H2) exist as discrete units. The text then explains the components of a chemical equation, including reactants, products, and states of matter (s, l, g, aq). Sample equations are given that show hydrogen gas and oxygen gas reacting to form liquid water, and sodium metal with water forming sodium hydroxide and hydrogen gas.
%Composition
This document discusses how to calculate the percentage composition of compounds from their chemical formulas. It explains that the chemical formula tells the number of moles of each element in one mole of the compound. It then provides steps to calculate percentage composition: write the chemical formula, find the molar mass of the compound and each element, divide the molar mass of each element by the total molar mass and multiply by 100. Examples are given for potassium chlorate and ammonium phosphate.
Empirical formulas
This document discusses empirical formulas and how to determine them from percentage composition or experimental data. It provides examples of calculating empirical formulas from the mass percentages of elements in a compound or the grams of elements in a sample. It also explains how to determine the molecular formula of a compound from the empirical formula and experimental molar mass. Key steps include converting percentages to grams of elements, calculating moles of each element, and dividing by the smallest ratio of elements to give whole number ratios in the empirical formula. The molecular formula is found by dividing the experimental molar mass by the molar mass of the empirical formula.
Mole calculations
The document discusses mole conversions between number of atoms/molecules, moles, and grams. It provides shortcuts for common conversions between these units and works through sample problems converting between atoms, molecules, moles, and grams of various substances using their molar masses.
Mole intro and molar mass
This document provides instructions and information about chemistry semester 2. It outlines rules like no food, drink, or phones, and requirements like having a scientific calculator. Several examples are given to illustrate the size of one mole of different substances like pennies, paperclips, and M&Ms. The mole is defined as 6.02x10^23 items. Formulas are given for determining molar mass of elements and compounds from the periodic table. Homework problems are assigned from page 239.
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3.3 orbital notation
- 1. Orbital NotationOrbital Notation Props to Mr. Smyk for giving this to me.
- 2. What is Orbital NotationWhat is Orbital Notation Orbital notation is a visual transformationOrbital notation is a visual transformation of the electron configuration.of the electron configuration. Orbital notation shows you where eachOrbital notation shows you where each specific electron is placed (in order) andspecific electron is placed (in order) and what it’s “spin” is.what it’s “spin” is.
- 3. Vocabulary List CheckVocabulary List Check Pauli Exclusion Principle:Pauli Exclusion Principle: No two electrons in the same atom can have the same spin quantum number. If one electron has the value of +½ then the other electron must have the value of −½. In Orbital notation this means the arrows representing the electrons must face opposite direction (+ is up, - is down).
- 4. Vocabulary List CheckVocabulary List Check Aufbau principle: (you already knowAufbau principle: (you already know the concept)the concept) Aufbau is the German word for “building up.” The principle states that electrons fill orbitals that have the lowest energy first. You fill electrons in a certain order. 11ss < 2< 2ss < 2< 2pp < 3< 3ss < 3< 3p < 4s < 3d < 4p < 5s <p < 4s < 3d < 4p < 5s < 4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d <4d < 5p < 6s < 4f < 5d < 6p < 7s < 5f < 6d < 7p7p
- 5. Vocabulary List CheckVocabulary List Check Hund’s Rule:Hund’s Rule: The rule that states that for an atom in the ground state, the number of unpaired electrons is the maximum possible and these unpaired electrons have the same spin. What? You must share your electrons. “Everybody gets one before anyone gets two.”
- 6. What’s next?What’s next? The orbital notationThe orbital notation reference sheet.reference sheet. This shows eachThis shows each orbital split apart intoorbital split apart into its 3 dimensionalits 3 dimensional axes.axes. Relax, this is easy.Relax, this is easy.
- 7. Write out the electron configurationWrite out the electron configuration for Sodiumfor Sodium Na, 11eNa, 11e-- 1s1s22 2s2s22 2p2p66 3s3s11 We are now going toWe are now going to represent each electronrepresent each electron as a ‘half arrow”.as a ‘half arrow”. We must fill in (buildWe must fill in (build up) the electrons as weup) the electrons as we did previously but showdid previously but show them using arrows onthem using arrows on the orbital notationthe orbital notation diagram.diagram. First one in an orbital isFirst one in an orbital is placed up (+placed up (+½½ spin)spin)
- 8. Write out the electron configurationWrite out the electron configuration for Boronfor Boron B, 5eB, 5e-- 1s1s22 2s2s22 2p2p11 We are now going toWe are now going to represent each electronrepresent each electron as a ‘half arrow”.as a ‘half arrow”. We must fill in (buildWe must fill in (build up) the electrons as weup) the electrons as we did previously but showdid previously but show them using arrows onthem using arrows on the orbital notationthe orbital notation diagram.diagram. First one in an orbital isFirst one in an orbital is placed up (+placed up (+½½ spin)spin)
- 9. Write out the electron configurationWrite out the electron configuration for Titaniumfor Titanium Ti, 22eTi, 22e-- 1s1s22 2s2s22 2p2p66 3s3s22 3p3p66 3d3d22 4s4s22
- 10. On your own. CalciumOn your own. Calcium Ca, 20eCa, 20e-- 1s1s22 2s2s22 2p2p66 3s3s22 3p3p66 4s4s22
- 11. HomeworkHomework Complete the Electron ConfigurationComplete the Electron Configuration Homework WKST.Homework WKST.