The document discusses periodic trends in effective nuclear charge (Zeff) and how it relates to ionization energy. It provides an example calculating the Zeff of the outermost electrons as argon is sequentially ionized from Ar+ to Ar18+. With each additional ionization, an electron is removed and the Zeff of the remaining electrons increases. This leads to higher ionization energies due to the greater attraction felt by the electrons to the increasingly exposed positive nuclear charge.
Physical Chemistry; Exact differentials, state function, Joule Thomson's experiment, derivation of Joule Thomson's coefficient, its significance and applications, inversion temperature.
Partition function indicates the mode of distribution of particles in various energy states. It plays a role similar to the wave function of the quantum mechanics,which contains all the dynamical information about the system.
The document discusses molecular orbital theory (MOT) and ligand field theory (LFT) as applied to transition metal complexes. It provides details on:
1. The construction of molecular orbital diagrams for octahedral complexes using the linear combination of atomic orbitals (LCAO) method, where the metal's d-orbitals combine with ligand orbitals.
2. The splitting of orbitals into bonding, non-bonding and antibonding molecular orbitals, and the filling of electrons according to Aufbau principle.
3. How LFT can explain color, spectra and magnetic properties of complexes based on ligand strength and the energy of the d-orbital splitting.
4. Examples
2018 ELECTRON DIFFRACTION AND APPLICATIONSHarsh Mohan
Low energy electron diffraction (LEED) is a surface-sensitive technique used to determine the structure of crystalline surfaces. LEED works by firing low energy electrons (20-200 eV) at a sample surface and analyzing the diffraction pattern of elastically backscattered electrons on a fluorescent screen. The pattern provides information on the 2D periodic arrangement of atoms in the surface layer. LEED has advantages over x-ray diffraction for studying surfaces and thin films due to its surface sensitivity and ability to operate under vacuum conditions.
1. The document discusses periodic trends in atomic properties such as size, ionization energy, and electron affinity across the periodic table.
2. Key periodic trends described include decreasing atomic size and increasing ionization energy from left to right across a period, and decreasing ionization energy from top to bottom in a group.
3. Exceptions to trends are discussed, such as higher ionization energies for p-block versus s-block elements and for doubly-occupied versus singly-occupied orbitals.
This document discusses theories of heat capacity in solids. It begins by describing Dulong and Petit's 1819 observation that the heat capacity of solids is approximately 3R. Einstein's theory from 1907 treated solids as assemblies of independent oscillators, predicting the heat capacity approaches 3R only at very high temperatures. Debye's 1912 theory improved on this by treating solids as continuous elastic mediums with phonon vibrational waves, removing the restriction of single oscillator frequencies. The document provides equations for calculating heat capacity based on Einstein's and Debye's models, and notes Debye temperature is important in determining when the heat capacity approaches the classical Dulong-Petit limit.
This document discusses transition series elements and their properties. It describes how transition elements have electrons that enter the (n-1)d orbitals, giving them variable oxidation states up to +8. Their atomic radii decrease across periods but increase down groups. Transition metals can conduct heat and electricity well and can be alloyed to improve strength. Some have magnetic properties depending on unpaired electrons. Their colored complexes are due to electron transitions between d orbitals. Common applications include stainless steel, bronze, and uses of copper and nickel in coins, batteries, and turbines.
Physical Chemistry; Exact differentials, state function, Joule Thomson's experiment, derivation of Joule Thomson's coefficient, its significance and applications, inversion temperature.
Partition function indicates the mode of distribution of particles in various energy states. It plays a role similar to the wave function of the quantum mechanics,which contains all the dynamical information about the system.
The document discusses molecular orbital theory (MOT) and ligand field theory (LFT) as applied to transition metal complexes. It provides details on:
1. The construction of molecular orbital diagrams for octahedral complexes using the linear combination of atomic orbitals (LCAO) method, where the metal's d-orbitals combine with ligand orbitals.
2. The splitting of orbitals into bonding, non-bonding and antibonding molecular orbitals, and the filling of electrons according to Aufbau principle.
3. How LFT can explain color, spectra and magnetic properties of complexes based on ligand strength and the energy of the d-orbital splitting.
4. Examples
2018 ELECTRON DIFFRACTION AND APPLICATIONSHarsh Mohan
Low energy electron diffraction (LEED) is a surface-sensitive technique used to determine the structure of crystalline surfaces. LEED works by firing low energy electrons (20-200 eV) at a sample surface and analyzing the diffraction pattern of elastically backscattered electrons on a fluorescent screen. The pattern provides information on the 2D periodic arrangement of atoms in the surface layer. LEED has advantages over x-ray diffraction for studying surfaces and thin films due to its surface sensitivity and ability to operate under vacuum conditions.
1. The document discusses periodic trends in atomic properties such as size, ionization energy, and electron affinity across the periodic table.
2. Key periodic trends described include decreasing atomic size and increasing ionization energy from left to right across a period, and decreasing ionization energy from top to bottom in a group.
3. Exceptions to trends are discussed, such as higher ionization energies for p-block versus s-block elements and for doubly-occupied versus singly-occupied orbitals.
This document discusses theories of heat capacity in solids. It begins by describing Dulong and Petit's 1819 observation that the heat capacity of solids is approximately 3R. Einstein's theory from 1907 treated solids as assemblies of independent oscillators, predicting the heat capacity approaches 3R only at very high temperatures. Debye's 1912 theory improved on this by treating solids as continuous elastic mediums with phonon vibrational waves, removing the restriction of single oscillator frequencies. The document provides equations for calculating heat capacity based on Einstein's and Debye's models, and notes Debye temperature is important in determining when the heat capacity approaches the classical Dulong-Petit limit.
This document discusses transition series elements and their properties. It describes how transition elements have electrons that enter the (n-1)d orbitals, giving them variable oxidation states up to +8. Their atomic radii decrease across periods but increase down groups. Transition metals can conduct heat and electricity well and can be alloyed to improve strength. Some have magnetic properties depending on unpaired electrons. Their colored complexes are due to electron transitions between d orbitals. Common applications include stainless steel, bronze, and uses of copper and nickel in coins, batteries, and turbines.
Charge-Transfer-Spectra. metal to metal, metal to ligandNafeesAli12
The document discusses charge transfer spectra in metal complexes. There are four main types of charge transfer transitions: ligand to metal (LMCT), metal to ligand (MLCT), intermetal or metal to metal (MMCT), and interligand (LLCT). LMCT involves electron transfer from ligand orbitals to metal orbitals, while MLCT is the reverse with electron transfer from metal to ligand orbitals. MMCT occurs between different oxidation states of the same metal. LLCT takes place between different ligands, one acting as an electron donor and the other as an acceptor. Examples are provided of each type of charge transfer and how they influence the color of complexes.
This document provides an overview of metal carbonyls. It discusses how metal carbonyls are formed from transition metals and carbon monoxide, and examples like nickel tetracarbonyl and iron pentacarbonyl. The molecular orbital diagram of carbon monoxide is shown, explaining why it can participate in pi-backbonding. Infrared spectroscopy is described as a useful technique for analyzing metal carbonyls, as it can distinguish terminal from bridging carbonyl ligands based on the infrared absorption frequency. Factors like metal charge and other ligands that affect the carbonyl stretching frequency are also outlined. Finally, some applications of infrared spectra of metal carbonyls are mentioned.
Reference,
https://en.wikipedia.org/wiki/Term_symbol
James E. Huheey, Ellen A. Keiter, Richard L.Keiter and Okhil K. Medhi, Inorganic Chemistry, Principles of Structure and Reactivity. 4th Edn. Pearsons
1. Electromagnetic radiation travels as waves through space at the speed of light and includes radio waves, microwaves, infrared, visible light, ultraviolet, X-rays and gamma rays.
2. Wavelength is the distance between peaks of a wave and frequency is the number of waves passing a point per second.
3. The Bohr model describes atoms with electrons orbiting the nucleus in discrete energy levels, absorbing or emitting energy when changing orbits.
The document discusses the discovery and properties of transuranium elements, which are elements heavier than uranium with atomic numbers 93 and above. It describes how each element was first synthesized, usually through bombardment of lighter elements with particles, as well as their chemical and physical properties such as common oxidation states and half-lives. The heaviest elements currently synthesized are livermorium at atomic number 116, but elements from 113 to 118 still require confirmation and all transuranic elements are very radioactive with short half-lives, limiting opportunities for study and application.
This document summarizes the history and principles of thermoelectricity. It discusses how in the 1820s, Thomas Seebeck discovered that connecting two different metals and maintaining a temperature difference between them produces an electric current, known as the Seebeck effect. Later, Jean Peltier found that applying a current to two metals produces heating or cooling at their junction. In 1851, Lord Kelvin discovered the Thomson effect regarding heat absorption or production based on current direction. The document then explains key concepts in thermoelectric materials like the Seebeck coefficient and figures of merit involving electrical conductivity and thermal conductivity. It also discusses applications of thermoelectric generators and coolers in various technologies.
The document discusses theories related to molecular structure and chemical bonding, including:
- Lewis theory which proposes that atoms bond by sharing valence electrons to achieve stable octet configurations.
- Limitations of the octet rule are discussed, including cases where the central atom has an incomplete or expanded octet.
- Sidgwick–Powell theory predicts molecular geometry based on the number of electron pairs around the central atom.
- VSEPR theory builds on this by accounting for differences in repulsion between bond pairs and lone pairs, allowing for more accurate prediction of molecular geometry. Lone pairs occupy more space and influence the shape.
This document discusses solid state chemistry and provides information on various topics within the subject. It begins by defining the three states of matter and what distinguishes a solid. It then describes the two main types of solids - crystalline and amorphous - and provides details on their structures and properties. Various types of crystal structures are also outlined, including ionic, covalent, molecular and metallic crystals. The document concludes by discussing Bragg's equation and important solid materials like diamond, graphite and fullerenes.
Ligand Field Theory was postulated in the 1950s as a modification of crystal field theory and molecular orbital theory. It can explain the geometry of coordination compounds like octahedral, tetrahedral, and square planar using crystal field theory. However, ligand field theory also considers sigma and pi bonding, which are important for understanding the behavior of neutral ligands like carbon monoxide and the strong field ligands carbon monoxide and cyanide.
The document discusses different types of electrophilic substitution reactions: SE1, SE2, and SEi. SE1 reactions follow first-order kinetics and involve two steps - rate-determining ionization and fast combination. SE2 reactions also follow first-order kinetics, but occur in a single step through a transition state. SE2 reactions can result in retention or inversion of configuration. SEi reactions are concerted mechanisms where the electrophile assists in removing the leaving group, leading to retention of configuration.
This document discusses the Jahn-Teller effect, which states that any non-linear molecule in a degenerate electronic state will distort in order to remove that degeneracy. It provides background on the scientists Hermann Jahn and Edward Teller, who first identified this effect. The document then explains the two types of distortions that can occur - Z-out and Z-in - and provides examples of complexes that exhibit static and dynamic Jahn-Teller distortions. It concludes by stating that the Jahn-Teller effect removes degeneracy in complexes through elongation or compression and that elongation is more energetically favorable, resulting in more stable complexes.
A ppt compiled by Yaseen Aziz Wani pursuing M.Sc Chemistry at University of Kashmir, J&K, India and Naveed Bashir Dar, a student of electrical engg. at NIT Srinagar.
Warm regards to Munnazir Bashir also for providing us with refreshing tea while we were compiling ppt.
Numerical problems on ElectrochemistrySwastika Das
1. The document provides numerical problems and explanations related to electrochemistry concepts like concentration cells, Nernst equation, standard reduction potentials, and calculating cell potentials.
2. Ten sample problems are worked through step-by-step to demonstrate how to calculate cell potentials using concentration, temperature, and standard reduction potential values.
3. The document concludes by providing two sample homework problems for students to practice calculating cell potentials based on given standard electrode potentials and ion concentrations.
This document discusses electronic spectra of metal complexes. It begins by defining quantum numbers related to electron configuration, such as L (total orbital angular momentum) and l (secondary quantum number). It then describes two main types of electronic transitions in coordination compounds: d-d transitions specific to metals, and charge-transfer transitions. The remainder of the document discusses charge-transfer transitions in more detail, defining ligand-to-metal and metal-to-ligand charge transfer, and how solvent polarity affects these transitions.
This document discusses electron configuration and how it is described using quantum numbers. It explains the main concepts like energy shells (n), subshells (s, p, d, f), orbitals and how electrons fill these according to the Aufbau principle and Hund's rule. Examples are provided to show the electron configurations of elements like hydrogen, helium, lithium and how the configurations change as the atomic number increases. Practice problems are included at the end to determine configurations of additional elements.
The document discusses the oxidation states of lanthanides. It states that:
1) All lanthanides most commonly exhibit a +3 oxidation state, but some can also be +2, +4, or lower states depending on electronic configuration.
2) The most stable oxidation state is generally +3 due to the strong attraction of the 4f electrons to the nucleus.
3) Elements in other oxidation states act as strong reducing or oxidizing agents as they try to attain the +3 state.
Electronic spectra of metal complexes-1SANTHANAM V
This document discusses electronic spectra of metal complexes. It begins by relating the observed color of complexes to the light absorbed and corresponding wavelength ranges. It then discusses the use of electronic spectra to determine d-d transition energies and the factors that affect d orbital energies. Key terms like states, microstates, and quantum numbers are introduced. Configuration, inter-electronic repulsions described by Racah parameters, nephelauxetic effect, and spin-orbit coupling are explained as factors that determine the splitting of energy levels. Russell-Saunders and j-j coupling are outlined as approaches to describe spin-orbit interactions in light and heavy elements respectively.
Annulenes and Heteroannulenes - Premie FernandesBebeto G
This document discusses annulenes and heteroannulenes. Annulenes are monocyclic conjugated systems represented by the general formula (CH)2m and include benzene and cyclooctatetraene. Heteroannulenes contain one or more heteroatoms in the ring, such as pyridine and thiophene. Aromaticity in these systems is determined by Huckel's rule of (4n+2)π electrons. The document examines various annulene and heteroannulene structures of different ring sizes and whether they obey Huckel's rule and exhibit aromatic, anti-aromatic, or non-aromatic behavior.
This document discusses atomic structure and electron configuration. It begins by explaining Slater's rules for calculating effective nuclear charge. It then provides examples of applying Slater's rules to determine electron shielding and effective nuclear charge. The document also covers electron configurations, term symbols, Hund's rules, and periodic trends in atomic size, ionization energy, and metallic character across periods and groups. It defines concepts like ionization potential, electron affinity, and electronegativity scales. In summary, the document provides an in-depth overview of theoretical atomic structure concepts.
Slater's rules provide a method to calculate the effective nuclear charge (Zeff) experienced by electrons in atoms and ions. The rules account for shielding of the nuclear charge by inner electrons. Zeff is calculated as the nuclear charge (Z) minus the total shielding (S). S is the sum of shielding values assigned based on orbital type and number of electrons. Comparing Zeff values explains trends like orbital filling order and which electrons are lost in cation formation. However, Slater grouped s and p orbitals together, which is incorrect as s orbitals penetrate the nucleus more than p orbitals.
Charge-Transfer-Spectra. metal to metal, metal to ligandNafeesAli12
The document discusses charge transfer spectra in metal complexes. There are four main types of charge transfer transitions: ligand to metal (LMCT), metal to ligand (MLCT), intermetal or metal to metal (MMCT), and interligand (LLCT). LMCT involves electron transfer from ligand orbitals to metal orbitals, while MLCT is the reverse with electron transfer from metal to ligand orbitals. MMCT occurs between different oxidation states of the same metal. LLCT takes place between different ligands, one acting as an electron donor and the other as an acceptor. Examples are provided of each type of charge transfer and how they influence the color of complexes.
This document provides an overview of metal carbonyls. It discusses how metal carbonyls are formed from transition metals and carbon monoxide, and examples like nickel tetracarbonyl and iron pentacarbonyl. The molecular orbital diagram of carbon monoxide is shown, explaining why it can participate in pi-backbonding. Infrared spectroscopy is described as a useful technique for analyzing metal carbonyls, as it can distinguish terminal from bridging carbonyl ligands based on the infrared absorption frequency. Factors like metal charge and other ligands that affect the carbonyl stretching frequency are also outlined. Finally, some applications of infrared spectra of metal carbonyls are mentioned.
Reference,
https://en.wikipedia.org/wiki/Term_symbol
James E. Huheey, Ellen A. Keiter, Richard L.Keiter and Okhil K. Medhi, Inorganic Chemistry, Principles of Structure and Reactivity. 4th Edn. Pearsons
1. Electromagnetic radiation travels as waves through space at the speed of light and includes radio waves, microwaves, infrared, visible light, ultraviolet, X-rays and gamma rays.
2. Wavelength is the distance between peaks of a wave and frequency is the number of waves passing a point per second.
3. The Bohr model describes atoms with electrons orbiting the nucleus in discrete energy levels, absorbing or emitting energy when changing orbits.
The document discusses the discovery and properties of transuranium elements, which are elements heavier than uranium with atomic numbers 93 and above. It describes how each element was first synthesized, usually through bombardment of lighter elements with particles, as well as their chemical and physical properties such as common oxidation states and half-lives. The heaviest elements currently synthesized are livermorium at atomic number 116, but elements from 113 to 118 still require confirmation and all transuranic elements are very radioactive with short half-lives, limiting opportunities for study and application.
This document summarizes the history and principles of thermoelectricity. It discusses how in the 1820s, Thomas Seebeck discovered that connecting two different metals and maintaining a temperature difference between them produces an electric current, known as the Seebeck effect. Later, Jean Peltier found that applying a current to two metals produces heating or cooling at their junction. In 1851, Lord Kelvin discovered the Thomson effect regarding heat absorption or production based on current direction. The document then explains key concepts in thermoelectric materials like the Seebeck coefficient and figures of merit involving electrical conductivity and thermal conductivity. It also discusses applications of thermoelectric generators and coolers in various technologies.
The document discusses theories related to molecular structure and chemical bonding, including:
- Lewis theory which proposes that atoms bond by sharing valence electrons to achieve stable octet configurations.
- Limitations of the octet rule are discussed, including cases where the central atom has an incomplete or expanded octet.
- Sidgwick–Powell theory predicts molecular geometry based on the number of electron pairs around the central atom.
- VSEPR theory builds on this by accounting for differences in repulsion between bond pairs and lone pairs, allowing for more accurate prediction of molecular geometry. Lone pairs occupy more space and influence the shape.
This document discusses solid state chemistry and provides information on various topics within the subject. It begins by defining the three states of matter and what distinguishes a solid. It then describes the two main types of solids - crystalline and amorphous - and provides details on their structures and properties. Various types of crystal structures are also outlined, including ionic, covalent, molecular and metallic crystals. The document concludes by discussing Bragg's equation and important solid materials like diamond, graphite and fullerenes.
Ligand Field Theory was postulated in the 1950s as a modification of crystal field theory and molecular orbital theory. It can explain the geometry of coordination compounds like octahedral, tetrahedral, and square planar using crystal field theory. However, ligand field theory also considers sigma and pi bonding, which are important for understanding the behavior of neutral ligands like carbon monoxide and the strong field ligands carbon monoxide and cyanide.
The document discusses different types of electrophilic substitution reactions: SE1, SE2, and SEi. SE1 reactions follow first-order kinetics and involve two steps - rate-determining ionization and fast combination. SE2 reactions also follow first-order kinetics, but occur in a single step through a transition state. SE2 reactions can result in retention or inversion of configuration. SEi reactions are concerted mechanisms where the electrophile assists in removing the leaving group, leading to retention of configuration.
This document discusses the Jahn-Teller effect, which states that any non-linear molecule in a degenerate electronic state will distort in order to remove that degeneracy. It provides background on the scientists Hermann Jahn and Edward Teller, who first identified this effect. The document then explains the two types of distortions that can occur - Z-out and Z-in - and provides examples of complexes that exhibit static and dynamic Jahn-Teller distortions. It concludes by stating that the Jahn-Teller effect removes degeneracy in complexes through elongation or compression and that elongation is more energetically favorable, resulting in more stable complexes.
A ppt compiled by Yaseen Aziz Wani pursuing M.Sc Chemistry at University of Kashmir, J&K, India and Naveed Bashir Dar, a student of electrical engg. at NIT Srinagar.
Warm regards to Munnazir Bashir also for providing us with refreshing tea while we were compiling ppt.
Numerical problems on ElectrochemistrySwastika Das
1. The document provides numerical problems and explanations related to electrochemistry concepts like concentration cells, Nernst equation, standard reduction potentials, and calculating cell potentials.
2. Ten sample problems are worked through step-by-step to demonstrate how to calculate cell potentials using concentration, temperature, and standard reduction potential values.
3. The document concludes by providing two sample homework problems for students to practice calculating cell potentials based on given standard electrode potentials and ion concentrations.
This document discusses electronic spectra of metal complexes. It begins by defining quantum numbers related to electron configuration, such as L (total orbital angular momentum) and l (secondary quantum number). It then describes two main types of electronic transitions in coordination compounds: d-d transitions specific to metals, and charge-transfer transitions. The remainder of the document discusses charge-transfer transitions in more detail, defining ligand-to-metal and metal-to-ligand charge transfer, and how solvent polarity affects these transitions.
This document discusses electron configuration and how it is described using quantum numbers. It explains the main concepts like energy shells (n), subshells (s, p, d, f), orbitals and how electrons fill these according to the Aufbau principle and Hund's rule. Examples are provided to show the electron configurations of elements like hydrogen, helium, lithium and how the configurations change as the atomic number increases. Practice problems are included at the end to determine configurations of additional elements.
The document discusses the oxidation states of lanthanides. It states that:
1) All lanthanides most commonly exhibit a +3 oxidation state, but some can also be +2, +4, or lower states depending on electronic configuration.
2) The most stable oxidation state is generally +3 due to the strong attraction of the 4f electrons to the nucleus.
3) Elements in other oxidation states act as strong reducing or oxidizing agents as they try to attain the +3 state.
Electronic spectra of metal complexes-1SANTHANAM V
This document discusses electronic spectra of metal complexes. It begins by relating the observed color of complexes to the light absorbed and corresponding wavelength ranges. It then discusses the use of electronic spectra to determine d-d transition energies and the factors that affect d orbital energies. Key terms like states, microstates, and quantum numbers are introduced. Configuration, inter-electronic repulsions described by Racah parameters, nephelauxetic effect, and spin-orbit coupling are explained as factors that determine the splitting of energy levels. Russell-Saunders and j-j coupling are outlined as approaches to describe spin-orbit interactions in light and heavy elements respectively.
Annulenes and Heteroannulenes - Premie FernandesBebeto G
This document discusses annulenes and heteroannulenes. Annulenes are monocyclic conjugated systems represented by the general formula (CH)2m and include benzene and cyclooctatetraene. Heteroannulenes contain one or more heteroatoms in the ring, such as pyridine and thiophene. Aromaticity in these systems is determined by Huckel's rule of (4n+2)π electrons. The document examines various annulene and heteroannulene structures of different ring sizes and whether they obey Huckel's rule and exhibit aromatic, anti-aromatic, or non-aromatic behavior.
This document discusses atomic structure and electron configuration. It begins by explaining Slater's rules for calculating effective nuclear charge. It then provides examples of applying Slater's rules to determine electron shielding and effective nuclear charge. The document also covers electron configurations, term symbols, Hund's rules, and periodic trends in atomic size, ionization energy, and metallic character across periods and groups. It defines concepts like ionization potential, electron affinity, and electronegativity scales. In summary, the document provides an in-depth overview of theoretical atomic structure concepts.
Slater's rules provide a method to calculate the effective nuclear charge (Zeff) experienced by electrons in atoms and ions. The rules account for shielding of the nuclear charge by inner electrons. Zeff is calculated as the nuclear charge (Z) minus the total shielding (S). S is the sum of shielding values assigned based on orbital type and number of electrons. Comparing Zeff values explains trends like orbital filling order and which electrons are lost in cation formation. However, Slater grouped s and p orbitals together, which is incorrect as s orbitals penetrate the nucleus more than p orbitals.
The document discusses electron shielding and how to calculate the effective nuclear charge (Zeff) experienced by an electron. Electrons closer to the nucleus provide more shielding from the nuclear charge than outer electrons. Rules are provided to calculate the shielding constant (S) based on the electronic configuration and determine Zeff by subtracting S from the atomic number (Z). Examples demonstrate applying the rules to calculate Zeff for valence and inner electrons of various elements.
1) Slater proposed rules to calculate the effective nuclear charge (Zeff) felt by outer electrons by accounting for shielding effects.
2) Zeff is calculated as Z - S, where Z is the nuclear charge and S is the Slater screening constant.
3) Slater's rules provide a method to calculate S by considering the shielding contributions of core and other valence electrons.
how to write electronic configuration of an atom
rules of filling electrons in energy levels
aufbau principle. hund's rule, Pauli's Exclusion principle
This document discusses atomic structure and properties related to electrons and subatomic particles. It begins by defining the atom and its main components: protons, neutrons, and electrons. It then discusses isotopes and the behavior of subatomic particles in electric fields. The document goes on to explain electronic configuration, ionization energy, and factors that influence ionization energy such as atomic radius, nuclear charge, and shielding effects. Trends in ionization energy across periods and down groups in the periodic table are also summarized.
Interatomic potentials are needed to model interactions between atoms and molecules in simulations. The most common approaches are semi-empirical potentials which make an educated guess about the potential energy surface and adjust parameters to experimental data. Common potentials include Lennard-Jones for non-bonded interactions and Morse for bonded interactions. However, pair potentials have limitations and fail to capture properties of metals where electrons are delocalized. Embedded-atom models provide a better description of metallic bonding. Specialized potentials are also developed for materials with directional bonding like silicon.
Hunds rule, Crystal field splitting and spectroscopic splitting factor.pptxAnnieNeema
This document discusses three topics related to magnetic properties of solids:
1) Hund's rules, which describe how electrons fill atomic orbitals to give the ground state with maximum spin and orbital angular momentum.
2) Crystal field splitting, which occurs when an ion's d or f orbitals interact with the electric field of surrounding ions, splitting orbital degeneracies.
3) The spectroscopic splitting factor g, which relates the energy separation of spin states in an applied magnetic field to the field strength and describes spin-orbit and crystal field interactions.
This document provides information about electrochemical cells. It begins by defining an electrochemical cell as consisting of two electrodes in contact with an electrolyte, with each electrode and electrolyte comprising an electrode compartment. It describes the two main types of electrochemical cells - electrolytic cells, where an external current causes non-spontaneous oxidation and reduction, and galvanic cells, where a spontaneous chemical reaction produces electricity. It then discusses standard reduction potentials, cell potentials, the Nernst equation, types of electrodes, and methods for determining standard electrode potentials, free energy changes, and equilibrium constants from cell potentials.
Slater's rules provide a method to estimate the shielding of electrons and the effective nuclear charge experienced by electrons in an atom. The rules involve writing the electron configuration, ignoring higher energy level electrons, and applying shielding constants of 0.35 for electrons in the same subshell and 0.85 for electrons in the previous subshell. As an example, the rules are used to calculate that the effective nuclear charge experienced by the valence electrons of nitrogen is 3.9 instead of the actual nuclear charge of 7.
The document discusses periodic properties of elements including atomic radii, ionization energy, electron affinity, ionic radii, and electronegativity. It provides information on trends in these properties across the periodic table and examples demonstrating how to order elements based on each property. Atomic radii decrease and ionization energy increases moving from left to right within a period due to increased nuclear charge. Electron affinity and ionic radii values become more negative in the same trend.
This document discusses periodic trends in atomic and ionic properties, including:
- Atomic and ionic radii decrease across a period as effective nuclear charge increases. Radii increase down a group as principal quantum number increases.
- Ionization energies generally increase across a period as it becomes more difficult to remove electrons. Exceptions include group 2A and 5A having higher energies than 3A and 6A respectively within periods.
- Cations have smaller radii than their parent atoms as electrons are removed. Anions have larger radii as more electrons are gained. Isotectronic ions with more protons have smaller radii.
I am Ben R. I am a Physical Chemistry Exam Helper at liveexamhelper.com. I hold a Masters' Degree in Physical Chemistry, from the University of Denver, USA. I have been helping students with their exams for the past 8 years. You can hire me to take your exam in Chemistry. Visit liveexamhelper.com or email info@liveexamhelper.com. You can also call on +1 678 648 4277 for any assistance with the Physical Chemistry Exam.
Electron Configurations in Science Education and Chemistry .pptClaudineRepil
You might have heard of the wise saying that
'experience is the best teacher". Each
year in your life ushers in a lot of experiences for you
to reflect on. You may not like everything
that happens to you in school or in the community,
especially those that bring you discomfort,
dificulty or detriment, but you have to bear with these
occurrences with a positive disposition.
You have to remember that you cannot prevent
circumstances from happening
especially those that might challenge your patience
determination and drive as a young
learner. lt's good to remember that experiences
whether in school or in the community, will
open opportunities for you to gain lessons which you
can utilize to help and inspire yourself
and others. Your negative or positive personal
experiences coupled with your coping skills can
serve as your stepping stones to academic successYou might have heard of the wise saying that
'experience is the best teacher". Each
year in your life ushers in a lot of experiences for you
to reflect on. You may not like everything
that happens to you in school or in the community,
especially those that bring you discomfort,
dificulty or detriment, but you have to bear with these
occurrences with a positive disposition.
You have to remember that you cannot prevent
circumstances from happening
especially those that might challenge your patience
determination and drive as a young
learner. lt's good to remember that experiences
whether in school or in the community, will
open opportunities for you to gain lessons which you
can utilize to help and inspire yourself
and others. Your negative or positive personal
experiences coupled with your coping skills can
serve as your stepping stones to academic success You might have heard of the wise saying that
'experience is the best teacher". Each
year in your life ushers in a lot of experiences for you
to reflect on. You may not like everything
that happens to you in school or in the community,
especially those that bring you discomfort,
dificulty or detriment, but you have to bear with these
occurrences with a positive disposition.
You have to remember that you cannot prevent
circumstances from happening
especially those that might challenge your patience
determination and drive as a young
learner. lt's good to remember that experiences
whether in school or in the community, will
open opportunities for you to gain lessons which you
can utilize to help and inspire yourself
and others. Your negative or positive personal
experiences coupled with your coping skills can
serve as your stepping stones to academic successYou might have heard of the wise saying that
'experience is the best teacher". Each
year in your life ushers in a lot of experiences for you
to reflect on. You may not like everything
that happens to you in school or in the community,
especially those that bring you discomfort,
dificulty or detriment, but you have to bear with these
occurrences with a positive disposition.
You have to remember h
Oxidation and Reduction (Uses of Redox potential data) By Latish Barve.pdfLatishBarve
Electrode potential is a measure of the tendency of an electrode to gain or lose electrons in a half-cell reaction. Standard electrode potentials (E°) are measured under standard conditions. E° values are used to determine the feasibility of redox reactions, calculate free energy change, and understand the oxidizing or reducing properties of substances. The electrochemical series arranges E° values from strongest reducing agent to strongest oxidizing agent. E° data can also be used to calculate non-standard electrode potentials and cell potentials using Nernst equations.
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 each quantum state can contain only one electron, which explains the filling order and structure of the periodic table.
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.
1) Neil Bohr proposed the Bohr model of the atom to explain the hydrogen spectrum. In this model, electrons revolve around the nucleus in definite orbits called energy levels without radiating energy.
2) When an electron jumps from a higher to a lower energy level, a photon is emitted with a frequency corresponding to the energy difference between the levels. The radius, energy, and angular momentum of an orbit depends on the quantum number n.
3) Applications of the Bohr model include the derivation of the radius, energy, and frequency of radiation emitted when an electron changes orbits for the hydrogen atom based on Planck's constant and other fundamental constants.
1) Atomic radius generally increases down a group and decreases across a period due to shielding effects of additional electron shells and increasing nuclear charge, respectively.
2) Ionization energy generally increases down a group and across a period as it becomes increasingly difficult to remove an electron due to greater nuclear attraction from less shielding and more protons. Exceptions occur when removing an electron would destabilize a full shell.
3) Electronegativity generally increases across a period as the effective nuclear charge felt by valence electrons increases with fewer shielding shells and more protons.
This document provides information on wave quantum mechanics and electron configurations. It discusses:
- Erwin Schrodinger's contributions to developing quantum mechanics and proposing the wave-like nature of electrons.
- How electrons occupy distinct energy levels and orbitals around the nucleus, rather than defined circular orbits. Electrons have wave-like properties.
- The shapes of s, p, d and f orbitals and how electrons fill these orbitals according to various principles like Aufbau and Hund's rule.
- Exceptions to the Aufbau principle seen in some elements.
- How to represent electron configurations using both energy level diagrams and shorthand notation.
- Gases have negligible volume and molecules are far apart with mostly empty space between them. Gas molecules move randomly in straight lines and collide elastically.
- The kinetic molecular theory describes gas properties including high translational energy of gas molecules that move randomly in all directions.
- Pressure, volume, temperature of gases are directly or inversely related as described by Boyle's, Charles', and Gay-Lussac's laws and the combined gas law.
- Elements in the same group have similar properties due to having the same number of valence electrons. Atoms get smaller from left to right in a period as protons are added, and larger from top to bottom in a group as energy levels are added.
- Electronegativity, ionization energy, and electron affinity all generally increase from left to right across a period as the effective nuclear charge increases. Electronegativity also increases up a group as the distance from valence electrons to the nucleus decreases.
- Ionization energy increases from top to bottom within a group as it is easier to remove an electron from an atom with fewer energy levels. Electron affinity generally increases from left to right across a period and decreases
This document discusses acids and bases. It defines their key properties including reacting with metals, carbonates, conducting electricity, turning litmus paper colors, and neutralizing each other. It explains the theories of Arrhenius, Brønsted-Lowry, and Lewis on acids and bases. It also covers acid-base reactions, indicators, pH, titrations, strong/weak acids and bases, and acid-base stoichiometry.
Gases are composed of molecules that are far apart from each other and occupy the entire volume of their container. Gas molecules move randomly in straight lines and collide elastically with each other and the container walls. The kinetic molecular theory describes gases as having negligible intermolecular forces and volume. Pressure, volume, temperature of a gas are related by the combined gas law and ideal gas law. Gas calculations involve using stoichiometry, the ideal gas law, and gas laws like Boyle's, Charles', and Gay-Lussac's to determine volume, pressure, amount, or temperature changes.
The document discusses the key properties and reactions of acids and bases. It defines acids as substances that produce hydrogen ions (H+) in water and bases as substances that produce hydroxide ions (OH-). Acids react with metals, carbonates, conduct electricity, turn litmus paper red, and neutralize bases. Bases conduct electricity, turn litmus paper blue, and neutralize acids. Theories of acids and bases including Arrhenius, Brønsted-Lowry, and Lewis are explained. Strong and weak acids/bases, monoprotic/diprotic/triprotic acids, pH, titrations, and acid-base indicators are also covered.
This document provides an overview of solution stoichiometry and includes 3 sample problems demonstrating how to use a balanced chemical equation to solve for unknown quantities. The general steps are: 1) Write the balanced equation, 2) Convert given amounts to moles, 3) Use the mole ratio to calculate moles of the unknown, 4) Convert moles to the required unit. Sample Problem 1 calculates molar concentration of sulfuric acid. Sample Problem 2 determines the minimum volume of sodium carbonate needed. Sample Problem 3 calculates the mass of silver chromate precipitate formed.
This document discusses water treatment processes including water softening. Water softening is a treatment process that uses chemicals to remove minerals like calcium and magnesium from hard water to make it softer. Acceptable concentrations of chemicals used in water treatment processes are also mentioned.
- Concentration can be expressed in several ways including mass/volume percent, mass/mass percent, volume/volume percent, parts per million (ppm), and molar concentration (mol/L).
- Mass/volume percent is the mass of solute divided by the volume of solution. Volume/volume percent is the volume of solute divided by the volume of solution.
- Mass/mass percent is the mass of solute divided by the mass of solution. Parts per million (ppm) and parts per billion (ppb) express very small concentrations.
- Molar concentration expresses the number of moles of solute per liter of solution and is the standard unit for expressing concentration in chemistry
This document discusses acids and bases according to several theories. It begins by describing the properties of acids, including reacting with metals and carbonates, conducting electricity, turning litmus paper colors, and neutralizing bases. It then discusses the properties of bases. The Arrhenius theory defines acids as substances that produce H+ ions in water and bases as those that produce OH- ions. However, this theory has limitations and does not account for all acids and bases. The Brønsted-Lowry theory broadens the definition to any substance that can donate or accept protons. Strong acids fully dissociate in water while weak acids only partially dissociate. The pH scale measures the concentration of H+ ions on a
The document discusses key concepts about solutions including:
- The components of a solution are a solvent and one or more solutes. Common solvents include water and gases.
- Factors that affect solubility and the rate of dissolving include temperature, agitation, and surface area of the solute. Increasing these factors generally increases solubility.
- Solutions can be classified as saturated, unsaturated, or supersaturated depending on the amount of solute dissolved compared to the maximum amount possible at a given temperature.
- Solubility is also affected by properties of the solute molecules like polarity, charge, and size - more polar or charged molecules or smaller ions tend to be more soluble.
- Solub
The document discusses percentage yield and percentage purity calculations for chemical reactions. It provides an example calculation for percentage yield where 1.72g of ammonia is obtained from a reaction using 7.5g of nitrogen. The percentage yield is calculated to be 18.9%. An example is also given for calculating percentage purity of an impure iron pyrite sample where the purity is found to be 86.3%. Formulae for percentage yield and percentage purity are defined. Key steps like using stoichiometry and unit conversions are highlighted.
The document discusses the mole concept in chemistry. It defines the mole as 6.022x10^23 particles, which is known as Avogadro's number. The mole can refer to individual atoms, molecules, ions or other particles. The document provides examples of how to calculate the number of particles or moles of a substance using the formula N=n×NA. It also discusses molar mass and how to calculate the mass of a substance using the formula m=n×M.
This document discusses the rules for determining significant digits in measurements and calculations. It defines four main rules:
1. All non-zero digits are significant, as are zeros between non-zero digits.
2. Leading zeros are not significant.
3. Trailing zeros may or may not be significant, depending on whether a decimal is present.
4. In calculations, the answer should match the least number of significant digits in the input values.
It provides examples like 0.08006 having 4 significant digits, and 1000mL having 1 significant digit. The document also covers rounding rules and calculating volumes and perimeters based on measurements to the correct number of significant digits.
This document discusses isotopes and nuclear reactions. It defines isotopes as atoms of the same element with different numbers of neutrons. It also describes how atomic mass is calculated based on isotope abundances. The document then discusses four types of nuclear reactions: fusion, fission, alpha decay, and beta decay. It provides examples of writing balanced nuclear equations and calculating half-life. Artificial transmutation and uses of nuclear technology like reactors and weapons are also summarized.
Isotopes are atoms of the same element that have different numbers of neutrons. Atoms of the same element can have different mass numbers depending on their number of neutrons. The atomic mass listed on the periodic table is an average that takes into account the relative abundances of each isotope of that element. Atomic mass calculations involve multiplying the mass and abundance percentage of each isotope and adding them together.
This document defines and provides examples of different types of chemical reactions including synthesis, decomposition, single displacement, double displacement, neutralization, and combustion reactions. Key aspects that determine the reaction type are whether reactants are elements, compounds, or if oxygen is involved. The position of elements in the periodic table also provides clues about reactivity in displacement reactions.
2. PERIODIC TRENDS AND Zeff
The effective Nuclear Charge (Zeff) that acts on an
electron is related its ionization energy.
2p
2s Dramatic changes in
ionization energy
1s occur between
energy levels and
subshells
nucleus
3. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar (1s2) (2s22p6) (3s23p6)
7 other 3s 3p electrons = 7 x 0.35 = 2.45
8 2s 2p electrons = 8 x 0.85 =6.80
2 1s electrons = 2 x 1.00 = 2
S = 2.45 + 6.80 + 2 = 11.25
Zeff = Z – S
= 18 – 11.25
= 6.75
4. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar1+ (1s2) (2s22p6) (3s23p5)
6 other 3s 3p electrons = 6 x 0.35 = 2.1
8 2s 2p electrons = 8 x 0.85 =6.80
2 1s electrons = 2 x 1.00 = 2
S = 2.1 + 6.80 + 2 = 10.9
Zeff = Z – S
= 18 – 10.9
= 7.1
5. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar2+ (1s2) (2s22p6) (3s23p4)
5 other 3s 3p electrons = 5 x 0.35 = 1.75
8 2s 2p electrons = 8 x 0.85 =6.80
2 1s electrons = 2 x 1.00 = 2
S = 1.75 + 6.80 + 2 = 10.55
Zeff = Z – S
= 18 – 10.55
= 7.45
6. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar3+ (1s2) (2s22p6) (3s23p3)
4 other 3s 3p electrons = 4 x 0.35 = 1.4
8 2s 2p electrons = 8 x 0.85 =6.80
2 1s electrons = 2 x 1.00 = 2
S = 1.4 + 6.80 + 2 = 10.2
Zeff = Z – S
= 18 – 10.2
= 7.8
7. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar4+ (1s2) (2s22p6) (3s23p2)
3 other 3s 3p electrons = 3 x 0.35 = 1.05
8 2s 2p electrons = 8 x 0.85 =6.80
2 1s electrons = 2 x 1.00 = 2
S = 1.05 + 6.80 + 2 = 9.85
Zeff = Z – S
= 18 – 9.85
= 8.15
8. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar5+ (1s2) (2s22p6) (3s23p1)
2 other 3s electrons = 2 x 0.35 = 0.7
8 2s 2p electrons = 8 x 0.85 =6.80
2 1s electrons = 2 x 1.00 = 2
S = 0.7 + 6.80 + 2 = 9.5
Zeff = Z – S
= 18 – 9.5
= 8.5
9. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar6+ (1s2) (2s22p6) (3s2)
1 other 3s electron = 1 x 0.35 = 0.35
8 2s 2p electrons = 8 x 0.85 =6.80
2 1s electrons = 2 x 1.00 = 2
S = 0.35 + 6.80 + 2 = 9.15
Zeff = Z – S
= 18 – 9.15
= 8.85
10. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar7+ (1s2) (2s22p6) (3s1)
0 other 3s electrons = 0 x 0.35 = 0
8 2s 2p electrons = 8 x 0.85 =6.80
2 1s electrons = 2 x 1.00 = 2
S = 0 + 6.80 + 2 = 8.80
Zeff = Z – S
= 18 – 8.80
= 9.2
11. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar8+ (1s2) (2s22p6)
7 other 2s 2p electrons = 7 x 0.35 = 2.45
2 1 s electrons = 2 x 0.85 = 1.7
S = 2.45 + 1.7 = 4.15
Zeff = Z – S
= 18 – 4.15
= 13.85
12. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar9+ (1s2) (2s22p5)
6 other 2s 2p electrons = 6 x 0.35 = 2.1
2 1 s electrons = 2 x 0.85 = 1.7
S = 2.1 + 1.7 = 3.8
Zeff = Z – S
= 18 – 3.8
= 14.2
13. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar10+ (1s2) (2s22p4)
5 other 2s 2p electrons = 5 x 0.35 = 1.75
2 1 s electrons = 2 x 0.85 = 1.7
S = 1.75 + 1.7 = 3.45
Zeff = Z – S
= 18 – 3.45
= 14.55
14. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar11+ (1s2) (2s22p3)
4 other 2s 2p electrons = 4 x 0.35 = 1.4
2 1 s electrons = 2 x 0.85 = 1.7
S = 1.4 + 1.7 = 3.1
Zeff = Z – S
= 18 – 3.1
= 14.9
15. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar12+ (1s2) (2s22p2)
3 other 2s 2p electrons = 3 x 0.35 = 1.05
2 1 s electrons = 2 x 0.85 = 1.7
S = 1.05 + 1.7 = 2.75
Zeff = Z – S
= 18 – 2.75
= 15.25
16. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar13+ (1s2) (2s22p1)
2 other 2s 2p electrons = 2 x 0.35 = 0.7
2 1 s electrons = 2 x 0.85 = 1.7
S = 0.7 + 1.7 = 2.4
Zeff = Z – S
= 18 – 2.4
= 15.6
17. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar14+ (1s2) (2s2)
1 other 2s 2p electron = 1 x 0.35 = 0.35
2 1 s electrons = 2 x 0.85 = 1.7
S = 0.35 + 1.7 = 2.4
Zeff = Z – S
= 18 – 2.05
= 15.95
18. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar15+ (1s2) (2s1)
0 other 2s 2p electrons = 0 x 0.35 = 0
2 1 s electrons = 2 x 0.85 = 1.7
S = 0 + 1.7 = 1.7
Zeff = Z – S
= 18 – 1.7
= 16.3
19. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar16+ (1s2)
1 other 1s electron = 1 x 0.35 = 0.35
S = 0.35
Zeff = Z – S
= 18 – 0.35
= 17.65
20. PERIODIC TRENDS AND Zeff
Example #1 - Calculate the effective nuclear charge of the
outermost electron in the following:
The electron configuration of argon is 1s2 2s2 2p6 3s2 3p6
Ar17+ (1s1)
0 other 1s electrons = 0 x 0.35 = 0
S=0
Zeff = Z – S
= 18 – 0
= 18
21. PERIODIC TRENDS AND Zeff
Zeff Vs . Ioniz ation E nerg y of the 18 E lec trons in Arg on
450000 20
The jump from the
second energy level to
400000 18
the first energy level
16
350000
14
300000
Ioniz ation E nerg y (eV )
12
250000
I.E .
Z eff
10
(eV )
200000 Zeff
8
150000
6
100000
4
50000 The jump2 from the
third energy level to
0 the second energy
0
0 2 4 6 8 10 12 14 16 level
18 20
Oute rm ost e le c tron to inne rm ost e le c tron
22. PERIODIC TRENDS AND Zeff
Zeff Vs . Ioniz ation E nerg y of the 18 E lec trons in Arg on
TREND: As the effective nuclear
450000 20
charge on an electron increases, so
18
does its ionization energy
400000
16
350000
14
300000
Ioniz ation E nerg y (eV )
12
250000
I.E .
Z eff
10
(eV )
200000 Zeff
8
150000
6
100000
4
50000 2
0 0
0 2 4 6 8 10 12 14 16 18 20
Oute rm ost e le c tron to inne rm ost e le c tron
23. PERIODIC TRENDS AND Zeff
TREND: As the effective nuclear
charge on an electron increases, so
does its ionization energy
Lower Zeff.
Attraction by
2p nucleus weaker.
Higher Zeff.
Attraction by 2s
nucleus stronger. .: less energy
1s required to
.: more energy remove this
required to O electron
remove this
electron
24. PERIODIC TRENDS AND Zeff
Example #2 - Calculate the effective nuclear charge of the
outermost electron in the first 36 elements
H (1s1)
0 other 1s electrons = 0 x 0.35 = 0
S=0
Zeff = Z – S
=1–0
=1
25. PERIODIC TRENDS AND Zeff
Example #2 - Calculate the effective nuclear charge of the
outermost electron in the first 36 elements
He (1s2)
1 other 1s electrons = 1 x 0.35 = 0.35
S = 0.35
Zeff = Z – S
= 2 – 0.35
= 1.65
26. PERIODIC TRENDS AND Zeff
Example #2 - Calculate the effective nuclear charge of the
outermost electron in the first 36 elements
Li (1s2) (2s1)
2 1s electrons = 2 x 0.85 = 1.7
S = 1.7
Zeff = Z – S
= 3 – 1.7
= 1.3
27. PERIODIC TRENDS AND Zeff
Example #2 - Calculate the effective nuclear charge of the
outermost electron in the first 36 elements
Be (1s2) (2s2)
1 2s electron = 1 x 0.35 = 0.35
2 1s electrons = 2 x 0.85 = 1.7
S = 0.35 + 1.7
Zeff = Z – S
= 4 – 2.05
= 1.95
28. PERIODIC TRENDS AND Zeff
Example #2 - ANSWERS
Atomic Element
Number Symbol Zeff
1 H 1 19 K 2.2
2 He 1.65 20 Ca 2.85
3 Li 1.3 21 Sc 3
4 Be 1.95 22 Ti 3.15
5 B 2.6 23 V 3.3
6 C 3.25 24 Cr 2.95
7 N 3.9 25 Mn 3.6
8 O 4.55 26 Fe 3.75
9 F 5.2 27 Co 3.9
10 Ne 5.85 28 Ni 4.05
11 Na 2.2 29 Cu 3.7
12 Mg 2.85 30 Zn 2.85
13 Al 3.5 31 Ga 5
14 Si 4.15 32 Ge 5.65
15 P 4.8 33 As 6.3
16 S 5.45 34 Se 6.95
17 Cl 6.1 35 Br 7.6
18 Ar 6.75 36 Kr 8.95
29. PERIODIC TRENDS AND Zeff
Zeff vs 1st I.E Elements 1-36
10 30
9
25
8
7
20
6
1st I.E (eV)
Zeff v1
Zeff
5 15
1st ionization energy (eV)
4
10
3
2 This shows that it is
5
difficult to remove
1
the last electron of
0
an0 energy level (it
will destabilize it)
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
Atomic Number
30. PERIODIC TRENDS AND Zeff
It requires much more energy to remove the
outermost electron of helium than lithium
2s
1s 1s
He Li
This will destabilize a This will not destabilize
full orbital a full orbital
.: greater ionization .: less ionization energy
energy is required is required
32. PERIODIC TRENDS AND Zeff
Zeff vs 1st I.E Elements 1-36
10 30
9
25
8
7
20
6
1st I.E (eV)
Zeff v1
Zeff
5 15
1st ionization energy (eV)
4
10
3
2
2p The third electron in
the p subshell
5
1 requires more
energy to remove
0 than the fourth
0
electron
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
Atomic Number
33. PERIODIC TRENDS AND Zeff
The third electron in the p subshell requires more energy
to remove than the fourth electron
vs
Removing the third electron produces this:
Having all three half-full orbitals is more stable than having one
orbital completely empty
vs
More stable
34. PERIODIC TRENDS AND Zeff
Stability: Rank the following from most to least stable
Most
stable
Increasing
stability
Least
stable
35. PERIODIC TRENDS AND Zeff
Zeff vs 1st I.E Elements 1-36
10 30
9
25
8
7
20
6
1st I.E (eV)
Zeff v1
Zeff
5 15
1st ionization energy (eV)
4
10
3
2
5
1 3s The same trend repeats for 3s
and 3p
0 0
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
Atomic Number
36. PERIODIC TRENDS AND Zeff
Zeff vs 1st I.E Elements 1-36
10 30
9
25
8
7
20
6
1st I.E (eV)
Zeff v1
Zeff
5 15
1st ionization energy (eV)
4
10
3
2
5
1 The same trend repeats for 3s
3p
and 3p
0 0
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
Atomic Number
37. PERIODIC TRENDS AND Zeff
Zeff vs 1st I.E Elements 1-36
10 30
9 4s and 3d are close in energy, so
there is no great change in 25
8 ionization energy in between
7
20
6
1st I.E (eV)
Zeff v1
Zeff
5 15
1st ionization energy (eV)
4
10
3
2
3d 5
1
4s
0 0
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
Atomic Number
38. PERIODIC TRENDS AND Zeff
Zeff vs 1st I.E Elements 1-36
10 30
9
4p repeats the ionization energy
8 trend of 2p and 3p
25
7
20
6
1st I.E (eV)
Zeff v1
Zeff
5 15
1st ionization energy (eV)
4
10
3
2
5
1
4p
0 0
1
2
3
4
5
6
7
8
9
10
11
12
13
14
15
16
17
18
19
20
21
22
23
24
25
26
27
28
29
30
31
32
33
34
35
36
Atomic Number
39. PERIODIC TRENDS AND Zeff
4s and 3d are close in energy, so there is no great change in
ionization energy in between.
RECALL:
Zeff vs 1st I.E Elements 1-36
10 30
9
25
8
7
20
6
Zeff
5 15
4
10
3
2
3d
5
1
0
4s 0
1
2
3
4
5
6
7
8
9
10
17
20
29
36
11
12
13
14
15
16
18
19
21
22
23
24
25
26
27
28
30
31
32
33
34
35
Atomic Number
40. PERIODIC TRENDS AND Zeff
Zeff Vs. Atomic Radius Elements 1-36
10 TREND: As Zeff increases, the nuclear attraction 250 the
for
outermost electron increases, and thus the electrons are
9
pulled closer to the nucleus. This results in a smaller
atomic radius
8 200
7
Atomic Radium (pm)
6 150
Zeff v1
Zeff
5
Atomic Radius (pm)
4 100
3
2 50
1
0 0
1 2 3 4 5 6 7 8 9 10 11 12 13 14 15 16 17 18 19 20 21 22 23 24 25 26 27 28 29 30 31 32 33 34 35 36
Atomic Number
41. PERIODIC TRENDS AND Zeff
TREND: As Zeff increases, the nuclear attraction for the outermost
electron increases, and thus the electrons are pulled closer to the
nucleus. This results in a smaller atomic radius
O F
Weaker Zeff Stronger Zeff
.: weaker attraction to nucleus .: stronger attraction to nucleus