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Presentation. 3 class 11 chemistry chapter .pptx
This document discusses electron gain enthalpy and the factors that affect it. It begins by defining electron gain enthalpy as the energy released when an isolated gaseous atom gains an electron. More negative electron gain enthalpy means an atom more easily gains electrons, while less negative or positive values mean an atom is not as likely or able to gain electrons. The main factors that affect electron gain enthalpy are an atom's size, shielding effects, electronic configuration, and penetration effect. Trends in the periodic table show that electron gain enthalpy becomes more negative from left to right in a period as atomic size decreases, and less negative from top to bottom in a group as atomic size increases. The document concludes
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The document discusses periodic trends in atomic properties including atomic radius, ionization energy, and electronegativity. It explains that as you move down a group in the periodic table, atomic radius increases while ionization energy and electronegativity decrease due to increased electron shielding. However, as you move across a period, atomic radius decreases while ionization energy and electronegativity increase due to the stronger effective nuclear charge pulling electrons in more tightly.
Periodic Trends
This document discusses periodic trends in properties such as ionization energy, atomic radius, electronegativity, and electron affinity. It explains that these properties generally increase or decrease predictably across periods and down groups on the periodic table due to factors like nuclear charge, electron shielding, and electron configuration. Predictable trends in properties can be understood and used to make inferences about elements based on their positions in the periodic table.
Electro negativity and electron affinity .pptx
Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. It increases across a period as the proton number and effective nuclear charge increases, making the nucleus more able to attract electrons. However, electronegativity decreases down a group as the energy level and shielding effect increases, weakening the attraction between the nucleus and valence electrons. Electron affinity is the energy change when an electron is added to a neutral atom to form a negative ion. It is measured as the electron attachment energy or electronegativity.
Periodic trends cca
This document discusses trends in atomic properties across the periodic table, including atomic radius, ionization energy, and electronegativity. It explains that atomic radius generally increases down groups and decreases across periods. Ionization energy follows the opposite trend, increasing across periods as the number of protons increases but decreasing down groups. Electronegativity tends to decrease down groups but increase left to right across periods, with metals having low values and nonmetals having high values.
Periodic trends detailed edit
Periodic Trends
This document discusses several periodic trends including ionization energy, electronegativity, atomic radius, and ionic radius. It notes that ionization energy generally decreases down a group and increases left to right in a period as the nuclear charge increases. Electronegativity also typically increases left to right and decreases down a group. Atomic radius decreases left to right in a period as the nuclear charge increases but increases down a group as the principal energy level increases. Ionic radius trends are similar, with positive ion size decreasing left to right and both positive and negative ion size increasing down a group.
Photon interaction with matter rahul
1. Photons interact with matter through various processes depending on their energy level. Low energy photons mainly undergo coherent scattering, while intermediate energies result in the Compton effect. Higher energy photons above 1.02 MeV can undergo pair production.
2. During interactions, photons may be deflected without energy loss, deflected with some energy loss, disappear by ejecting electrons, or pass through unchanged. Common interaction types include the photoelectric effect, Compton scattering, and pair production.
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Periodic Trends
1. The document discusses several periodic trends including atomic radius, ionization energy, and electronegativity. It explains that atomic radius decreases left to right within a period and increases down a group. Ionization energy generally increases left to right within a period and decreases down a group. Electronegativity increases left to right within a period and decreases down a group.
2. The document also discusses ionic radius trends, explaining that the size of positive ions decreases left to right within a period while the size of negative ions increases. Ionic radius increases down a group for both positive and negative ions.
3. The octet rule is mentioned as determining what types of ions atoms will form in order to acquire
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Presentation. 3 class 11 chemistry chapter .pptx
This document discusses electron gain enthalpy and the factors that affect it. It begins by defining electron gain enthalpy as the energy released when an isolated gaseous atom gains an electron. More negative electron gain enthalpy means an atom more easily gains electrons, while less negative or positive values mean an atom is not as likely or able to gain electrons. The main factors that affect electron gain enthalpy are an atom's size, shielding effects, electronic configuration, and penetration effect. Trends in the periodic table show that electron gain enthalpy becomes more negative from left to right in a period as atomic size decreases, and less negative from top to bottom in a group as atomic size increases. The document concludes
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The document discusses periodic trends in atomic properties including atomic radius, ionization energy, and electronegativity. It explains that as you move down a group in the periodic table, atomic radius increases while ionization energy and electronegativity decrease due to increased electron shielding. However, as you move across a period, atomic radius decreases while ionization energy and electronegativity increase due to the stronger effective nuclear charge pulling electrons in more tightly.
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This document discusses periodic trends in properties such as ionization energy, atomic radius, electronegativity, and electron affinity. It explains that these properties generally increase or decrease predictably across periods and down groups on the periodic table due to factors like nuclear charge, electron shielding, and electron configuration. Predictable trends in properties can be understood and used to make inferences about elements based on their positions in the periodic table.
Electro negativity and electron affinity .pptx
Electronegativity is a measure of an atom's ability to attract electrons in a chemical bond. It increases across a period as the proton number and effective nuclear charge increases, making the nucleus more able to attract electrons. However, electronegativity decreases down a group as the energy level and shielding effect increases, weakening the attraction between the nucleus and valence electrons. Electron affinity is the energy change when an electron is added to a neutral atom to form a negative ion. It is measured as the electron attachment energy or electronegativity.
Periodic trends cca
This document discusses trends in atomic properties across the periodic table, including atomic radius, ionization energy, and electronegativity. It explains that atomic radius generally increases down groups and decreases across periods. Ionization energy follows the opposite trend, increasing across periods as the number of protons increases but decreasing down groups. Electronegativity tends to decrease down groups but increase left to right across periods, with metals having low values and nonmetals having high values.
Periodic trends detailed edit
Periodic Trends
This document discusses several periodic trends including ionization energy, electronegativity, atomic radius, and ionic radius. It notes that ionization energy generally decreases down a group and increases left to right in a period as the nuclear charge increases. Electronegativity also typically increases left to right and decreases down a group. Atomic radius decreases left to right in a period as the nuclear charge increases but increases down a group as the principal energy level increases. Ionic radius trends are similar, with positive ion size decreasing left to right and both positive and negative ion size increasing down a group.
Photon interaction with matter rahul
1. Photons interact with matter through various processes depending on their energy level. Low energy photons mainly undergo coherent scattering, while intermediate energies result in the Compton effect. Higher energy photons above 1.02 MeV can undergo pair production.
2. During interactions, photons may be deflected without energy loss, deflected with some energy loss, disappear by ejecting electrons, or pass through unchanged. Common interaction types include the photoelectric effect, Compton scattering, and pair production.
3. The dominant interaction mechanism depends on photon energy and the atomic number of the absorber. Low energies favor photoelectric effect in high Z materials, while Compton scattering does not depend strongly on Z. Pair production rises with both energy
Periodic Trends
1. The document discusses several periodic trends including atomic radius, ionization energy, and electronegativity. It explains that atomic radius decreases left to right within a period and increases down a group. Ionization energy generally increases left to right within a period and decreases down a group. Electronegativity increases left to right within a period and decreases down a group.
2. The document also discusses ionic radius trends, explaining that the size of positive ions decreases left to right within a period while the size of negative ions increases. Ionic radius increases down a group for both positive and negative ions.
3. The octet rule is mentioned as determining what types of ions atoms will form in order to acquire
Periodic Trends
The document discusses periodic trends in chemical and physical properties revealed by the periodic table. It examines six key trends: atomic number, atomic mass, atomic radius, electronegativity, ionization energy, and reactivity. For each trend, it describes how the property changes as you move down groups or across periods on the periodic table, enabling predictions about an element's chemical behavior.
periodic table trends
The Periodic Table and Periodic Law SECTION 3 Periodic Trends
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The document summarizes trends in properties of elements as you move through the periodic table, including atomic radius, ionic radii, ionization energy, electron affinity, and electronegativity. It explains that atomic radius increases down a family due to increasing energy levels, while decreasing left to right due to more protons. Ionic radii decrease when gaining electrons and increase when losing electrons. Ionization energy increases when removing electrons due to stronger nuclear attraction and decreases down a family and increases left to right. Electron affinity and electronegativity both increase left to right and decrease top to bottom.
Inorganic Chemistry: Period 2 and 3
The document summarizes trends in atomic properties across periods 2 and 3 of the periodic table. Atomic radius decreases across periods due to increasing nuclear charge, while it increases down groups due to greater screening effect. Ionic radius, melting/boiling points, and enthalpy of vaporization follow similar trends. Electrical conductivity increases with more delocalized electrons. Electronegativity increases across periods but decreases down groups.
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The document discusses several periodic trends:
1. Atomic radius generally increases moving down a group and decreases moving across a period, due to shielding and nuclear charge effects.
2. Ionization energy increases moving across a period as the effective nuclear charge increases, and decreases moving down a group as the distance from the nucleus increases.
3. Electronegativity increases moving across a period as it is easier to gain than lose electrons, and decreases moving down a group with increased atomic radius.
Periodic trends lecture notes a.k
The document discusses several periodic trends, including how atomic radius, ionic radius, ionization energy, and electronegativity change across periods and down groups in the periodic table.
[1] Atomic radius decreases and ionization energy increases when moving across a period as nuclear charge increases, while trends are opposite when moving down a group as additional energy levels are added.
[2] Ionic radius follows the same trends as atomic radius, decreasing across periods and increasing down groups.
[3] Electronegativity also decreases down groups as the distance between nucleus and electrons increases, but increases across periods as nuclear charge rises.
Chapter 16 8th grade
The document discusses atomic structure and chemical bonds. It explains that atoms are made up of protons and neutrons in the nucleus surrounded by electrons in energy levels. The number and arrangement of electrons determines an element's properties. Electrons closer to the nucleus have lower energy than those farther away. Elements in the same family on the periodic table have similar properties because they have the same number of electrons in their outer energy level, which determines how they bond with other elements.
Interaction of radiation with matter
The document discusses various interactions between radiation and matter, including excitation, ionization, and radiative losses. It describes the processes of excitation, ionization, specific ionization, linear energy transfer, scattering, bremsstrahlung, and the four main interactions of x-rays and gamma rays with matter: Rayleigh scattering, Compton scattering, photoelectric absorption, and pair production. The probability and characteristics of each interaction depends on factors like the atomic number of the absorbing material and the energy of the incident radiation. These interactions are important in diagnostic imaging and radiation therapy.
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basic concepts of inorganic and analytical chemistry.pptx.pdf
The document summarizes key periodic properties including atomic radius, ionization energy, electron affinity, and electronegativity. It explains that atomic radius decreases and ionization energy increases moving left to right within a period due to increasing nuclear charge. Down a group, atomic radius increases and properties like ionization energy decrease as the number of shells increases. Fluorine generally has the highest values for electron affinity and electronegativity due to its small size.
3b. The periodic table and trends.pptx 11
1. This document provides an overview of trends in the periodic table, including atomic size, ionization energy, electronegativity, and metallic/non-metallic character. It explains that these properties trend both across periods, from left to right as atomic number increases, and down groups as additional shells are filled.
2. Specifically, it notes that atomic size decreases across periods as nuclear charge increases, while increasing down groups as additional shells are added. Ionization energy and electronegativity both increase from left to right as nuclear charge increases, while decreasing down groups as electrons are farther from the nucleus. Metallic character increases down groups and decreases across periods.
3. The document aims to explain these
Trends of periodic atomic properties
1) Atomic radius decreases across a period as atomic number increases, leading to higher effective nuclear charge and stronger attraction of the nucleus. Atomic radius increases down a group as shielding electrons increase.
2) Ionization energy increases across a period as effective nuclear charge increases, making it harder to remove electrons. Ionization energy decreases down a group as shielding increases and atomic radius gets larger.
3) Electronegativity increases across a period for the same reasons as ionization energy, and decreases down a group as shielding increases and attraction decreases.
Basic electronics
This document provides information about atomic structure and bonding. It discusses:
- The basic components of atoms (protons, neutrons, electrons) and their properties.
- Electron orbitals and energy levels within atoms. Electrons occupy discrete shells and energy levels.
- Covalent bonding between atoms, where valence electrons are shared. This forms crystalline structures.
- Semiconductors like silicon and germanium have incomplete valence shells, so their atoms form covalent bonds to share electrons until each has a full outer shell. This tightly binds electrons.
- Doping semiconductors with impurities introduces extra electrons or holes, increasing conductivity and making the material n-type or p-
1st leacture
Semiconductors are materials that conduct electricity between conductors and insulators. Silicon is a commonly used semiconductor that has four valence electrons. When energy is supplied to silicon, some electrons jump from the valence band to the conduction band, leaving holes behind. This creates electron-hole pairs that allow current to flow through the semiconductor when a voltage is applied. The movement of free electrons is called electron current, while the movement of holes acts as another type of current flow in semiconductors.
Ionization potential and electron affinity
1) The document discusses trends in ionization potential and electron affinity across the periodic table. Ionization potential generally increases from left to right in a period as nuclear charge increases and atomic radius decreases. It also decreases down a group as atomic size increases.
2) Electron affinity generally increases from left to right as nuclear charge increases but decreases down a group as atomic size increases. Elements in the lower left of the periodic table tend to have lower ionization potentials and are more metallic.
3) Factors that influence ionization potential and electron affinity include effective nuclear charge, atomic size, shielding effects, and stability of electron configurations.
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IONIZATION ENERGY of period three elemen
The document discusses ionization energy, which is the energy required to remove an electron from an atom or ion. It explains that the first ionization energy is the energy needed to remove the first electron, and successive ionization energies increase as more electrons are removed. The factors that affect ionization energy are the size of the nuclear charge, size of the atom, and shielding effects of inner electrons. Graphs of ionization energies provide evidence of electron shell structure based on jumps in energy.
Lecture 6.3- Periodic Trends (Honors)
This document contains information about periodic trends in atomic properties such as size, ionization energy, and electronegativity. It explains that atomic size generally increases down a group and decreases left to right across a period as the number of protons increases. Ionization energy decreases down a group as outer electrons are more easily removed, and increases left to right as atoms get smaller. Electronegativity also increases left to right as atoms get smaller, allowing them to better attract electrons.
Ionic Trends
The document discusses ionic trends in atomic radius, ionization energy, and electronegativity across the periodic table. It explains that atomic radius generally decreases from left to right as more protons are added to the nucleus, attracting the electrons closer. Ionization energy decreases from right to left as the right side has more full valence shells, making them less likely to lose electrons. Electronegativity increases from left to right and decreases down groups as the distance from the valence electrons to the nucleus changes.
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The document discusses periodic trends in chemical and physical properties revealed by the periodic table. It examines six key trends: atomic number, atomic mass, atomic radius, electronegativity, ionization energy, and reactivity. For each trend, it describes how the property changes as you move down groups or across periods on the periodic table, enabling predictions about an element's chemical behavior.
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The document summarizes trends in atomic properties across periods 2 and 3 of the periodic table. Atomic radius decreases across periods due to increasing nuclear charge, while it increases down groups due to greater screening effect. Ionic radius, melting/boiling points, and enthalpy of vaporization follow similar trends. Electrical conductivity increases with more delocalized electrons. Electronegativity increases across periods but decreases down groups.
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The document discusses several periodic trends:
1. Atomic radius generally increases moving down a group and decreases moving across a period, due to shielding and nuclear charge effects.
2. Ionization energy increases moving across a period as the effective nuclear charge increases, and decreases moving down a group as the distance from the nucleus increases.
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The document discusses several periodic trends, including how atomic radius, ionic radius, ionization energy, and electronegativity change across periods and down groups in the periodic table.
[1] Atomic radius decreases and ionization energy increases when moving across a period as nuclear charge increases, while trends are opposite when moving down a group as additional energy levels are added.
[2] Ionic radius follows the same trends as atomic radius, decreasing across periods and increasing down groups.
[3] Electronegativity also decreases down groups as the distance between nucleus and electrons increases, but increases across periods as nuclear charge rises.
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The document discusses atomic structure and chemical bonds. It explains that atoms are made up of protons and neutrons in the nucleus surrounded by electrons in energy levels. The number and arrangement of electrons determines an element's properties. Electrons closer to the nucleus have lower energy than those farther away. Elements in the same family on the periodic table have similar properties because they have the same number of electrons in their outer energy level, which determines how they bond with other elements.
Interaction of radiation with matter
The document discusses various interactions between radiation and matter, including excitation, ionization, and radiative losses. It describes the processes of excitation, ionization, specific ionization, linear energy transfer, scattering, bremsstrahlung, and the four main interactions of x-rays and gamma rays with matter: Rayleigh scattering, Compton scattering, photoelectric absorption, and pair production. The probability and characteristics of each interaction depends on factors like the atomic number of the absorbing material and the energy of the incident radiation. These interactions are important in diagnostic imaging and radiation therapy.
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basic concepts of inorganic and analytical chemistry.pptx.pdf
The document summarizes key periodic properties including atomic radius, ionization energy, electron affinity, and electronegativity. It explains that atomic radius decreases and ionization energy increases moving left to right within a period due to increasing nuclear charge. Down a group, atomic radius increases and properties like ionization energy decrease as the number of shells increases. Fluorine generally has the highest values for electron affinity and electronegativity due to its small size.
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1. This document provides an overview of trends in the periodic table, including atomic size, ionization energy, electronegativity, and metallic/non-metallic character. It explains that these properties trend both across periods, from left to right as atomic number increases, and down groups as additional shells are filled.
2. Specifically, it notes that atomic size decreases across periods as nuclear charge increases, while increasing down groups as additional shells are added. Ionization energy and electronegativity both increase from left to right as nuclear charge increases, while decreasing down groups as electrons are farther from the nucleus. Metallic character increases down groups and decreases across periods.
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1) Atomic radius decreases across a period as atomic number increases, leading to higher effective nuclear charge and stronger attraction of the nucleus. Atomic radius increases down a group as shielding electrons increase.
2) Ionization energy increases across a period as effective nuclear charge increases, making it harder to remove electrons. Ionization energy decreases down a group as shielding increases and atomic radius gets larger.
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Basic electronics
This document provides information about atomic structure and bonding. It discusses:
- The basic components of atoms (protons, neutrons, electrons) and their properties.
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- Semiconductors like silicon and germanium have incomplete valence shells, so their atoms form covalent bonds to share electrons until each has a full outer shell. This tightly binds electrons.
- Doping semiconductors with impurities introduces extra electrons or holes, increasing conductivity and making the material n-type or p-
1st leacture
Semiconductors are materials that conduct electricity between conductors and insulators. Silicon is a commonly used semiconductor that has four valence electrons. When energy is supplied to silicon, some electrons jump from the valence band to the conduction band, leaving holes behind. This creates electron-hole pairs that allow current to flow through the semiconductor when a voltage is applied. The movement of free electrons is called electron current, while the movement of holes acts as another type of current flow in semiconductors.
Ionization potential and electron affinity
1) The document discusses trends in ionization potential and electron affinity across the periodic table. Ionization potential generally increases from left to right in a period as nuclear charge increases and atomic radius decreases. It also decreases down a group as atomic size increases.
2) Electron affinity generally increases from left to right as nuclear charge increases but decreases down a group as atomic size increases. Elements in the lower left of the periodic table tend to have lower ionization potentials and are more metallic.
3) Factors that influence ionization potential and electron affinity include effective nuclear charge, atomic size, shielding effects, and stability of electron configurations.
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The document discusses ionization energy, which is the energy required to remove an electron from an atom or ion. It explains that the first ionization energy is the energy needed to remove the first electron, and successive ionization energies increase as more electrons are removed. The factors that affect ionization energy are the size of the nuclear charge, size of the atom, and shielding effects of inner electrons. Graphs of ionization energies provide evidence of electron shell structure based on jumps in energy.
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This document contains information about periodic trends in atomic properties such as size, ionization energy, and electronegativity. It explains that atomic size generally increases down a group and decreases left to right across a period as the number of protons increases. Ionization energy decreases down a group as outer electrons are more easily removed, and increases left to right as atoms get smaller. Electronegativity also increases left to right as atoms get smaller, allowing them to better attract electrons.
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The document discusses ionic trends in atomic radius, ionization energy, and electronegativity across the periodic table. It explains that atomic radius generally decreases from left to right as more protons are added to the nucleus, attracting the electrons closer. Ionization energy decreases from right to left as the right side has more full valence shells, making them less likely to lose electrons. Electronegativity increases from left to right and decreases down groups as the distance from the valence electrons to the nucleus changes.
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Call For Paper -3rd International Conference on Artificial Intelligence Advan...
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Call for Research Papers!!!
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3rd International Conference on Artificial Intelligence Advances (AIAD 2024)
July 13 ~ 14, 2024, Virtual Conference
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Use PyCharm for remote debugging of WSL on a Windo cf5c162d672e4e58b4dde5d797...
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The document further emphasizes on the importance of checking the connection between the Windows and WSL environments, providing instructions on how to ensure that the connection is optimal and ready for remote debugging.
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https://www.leewayhertz.com/generative-ai-use-cases-and-applications/
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Electron affinity chemistry engineering ppt
- 2. is defined as the energy process in which an electron is acquired by the atom in the gas phase Electron affinity...
- 3. More info... • The larger the affinity of an atom for an electron, the more negative the value • Electron affinity trends are related to the trends of ionization energy because both represent the energy involved in the gain or loss of an electron by an atom, respectively
- 4. The trend down the column... Electron affinity decreases as it goes down a column
- 5. This is because... • Electrons are added increasingly farther from the nucleus, so the attractive force between the nucleus and electrons decreases • The outer electrons experience less of a positive charge as you go up the periodic table (effective nuclear charge)
- 6. The trend across a period... Electron affinity increases as it goes across a period
- 7. This is because... • The octet rule states that atoms with close to full valence shells will tend to gain electrons. When they gain the electrons, they use energy, which allows the ion to become more stable • The outer electrons experience less of a positive charge as you go across a period (effective nuclear charge)
- 9. Units of EA KJ/Mol ** electron affinity is negative
- 10. Exceptions... • Nitrogen atoms have no affinity - in N- ions, electron-electron repulsion makes these ions unstable • Beryllium anion has no affinity - Be- is not stable, because the added electron is assigned to a higher energy subshell (2p) than the valence electrons (2s)
- 11. More Exceptions... • Noble gases have no affinity - they have full valence shells and by adding or taking away electrons, they become unstable • Fluorine has a low affinity - because it has a small amount of shells and when you add another electron, electron-electron repulsion happens, creating an unstable ion