I.e and electroneg
•Download as PPT, PDF•
0 likes•77 views
1. Ionization energy is the amount of energy required to remove an electron from an atom or ion. The first ionization energy is the amount required to remove the outermost electron from a neutral atom. 2. Ionization energies generally increase as each successive electron is removed from an atom. They decrease down a group and increase across a period on the periodic table. Noble gases have the highest ionization energies due to their stable electron configuration. 3. Electronegativity is a measure of how strongly an element attracts electrons in a bond. It shows similar trends to ionization energy, decreasing down groups and increasing across periods. Electronegativity values are used to determine if molecules are polar or non
Report
Share
Report
Share
Recommended
Electron affinity
Electron affinity is the energy released when an electron is added to an isolated gaseous atom. Electron affinity increases with increasing atomic number and decreasing size, as effective nuclear charge increases. Electron affinity decreases with increasing size and number of electron shells, as effective nuclear charge decreases. Electron affinity also increases with greater effective nuclear charge and decreases with greater screening effects and stability of half or completely filled orbitals.
ELECTRONEGATIVITY
Pauling was the first to propose a scale of electronegativity in 1932 based on the difference in the measured energy of an AB bond and the expected energy of a purely covalent AB bond. Mulliken suggested an approach to electronegativity in 1934 based on ionization enthalpy and electron affinity, defining electronegativity as the arithmetic mean of ionization energy and electron affinity. Electronegativity is influenced by factors such as charge on the atom, hybridization state, ionization energy, electron affinity, and effective nuclear charge. It is used to determine bond polarity, percent ionic character, and enthalpy of formation.
Ionization Energy...
The document discusses ionization energy and atomic and ionic radii. It defines an ion as a charged atom or molecule resulting from an imbalance of protons and electrons. The first ionization energy is the amount of energy required to remove an electron from the outermost shell of an atom. Each subsequent ionization energy is greater than the preceding one. Atomic radius decreases left to right on the periodic table as nuclear charge increases, while it increases down a group as electron shells expand. Positive ions have smaller radii than their parent atoms due to their increased nuclear charge.
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.
Ionization Potential
This document discusses ionization potential and the factors that affect it. Ionization potential is the amount of energy required to remove an electron from an isolated atom, forming a cation. The first ionization energy is removing the outermost electron, and subsequent ionization energies increase with each additional electron removed. Factors that affect ionization potential include effective nuclear charge, atomic size, shielding effects, and full or half-filled orbitals. Ionization energy generally increases left to right across a period and decreases down a group on the periodic table.
Periodic trends
This document discusses several key trends seen in the periodic table including atomic radius, ionization energy, electronegativity, and electron shielding. It defines these terms and explains how they vary depending on an element's location in the periodic table, such as atomic radius generally increasing down a group and decreasing left to right across a period. The document also provides examples of comparing atomic radii of different elements and assessing trends in ionization energy and electronegativity.
Periodic Relationships
There are observable trends in the physical and chemical properties of elements across periods and down groups in the periodic table. As you move across a period, atomic radius decreases due to the increasing effective nuclear charge pulling the valence electrons closer. Down groups, atomic radius increases as each successive energy level is farther from the nucleus. Ionization energy generally increases across periods as effective nuclear charge increases, and decreases down groups as the valence electrons are farther from the nucleus. Electron affinity increases across periods but decreases down groups. Oxidation states can be used to keep track of electrons in compounds and ions.
Periodic trends
Here are the answers to your questions:
1. Shielding of nuclear charge remains constant as you move across a period or down a group since the number of electron shells remains the same.
2. Atomic size decreases as you move across a period due to increased nuclear charge, and increases as you move down a group due to additional electron shells providing more shielding.
3. Ions form when atoms gain or lose electrons. Cations form when atoms lose electrons, becoming positively charged. Anions form when atoms gain electrons, becoming negatively charged.
4. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom.
5. Ionization energy increases
Recommended
Electron affinity
Electron affinity is the energy released when an electron is added to an isolated gaseous atom. Electron affinity increases with increasing atomic number and decreasing size, as effective nuclear charge increases. Electron affinity decreases with increasing size and number of electron shells, as effective nuclear charge decreases. Electron affinity also increases with greater effective nuclear charge and decreases with greater screening effects and stability of half or completely filled orbitals.
ELECTRONEGATIVITY
Pauling was the first to propose a scale of electronegativity in 1932 based on the difference in the measured energy of an AB bond and the expected energy of a purely covalent AB bond. Mulliken suggested an approach to electronegativity in 1934 based on ionization enthalpy and electron affinity, defining electronegativity as the arithmetic mean of ionization energy and electron affinity. Electronegativity is influenced by factors such as charge on the atom, hybridization state, ionization energy, electron affinity, and effective nuclear charge. It is used to determine bond polarity, percent ionic character, and enthalpy of formation.
Ionization Energy...
The document discusses ionization energy and atomic and ionic radii. It defines an ion as a charged atom or molecule resulting from an imbalance of protons and electrons. The first ionization energy is the amount of energy required to remove an electron from the outermost shell of an atom. Each subsequent ionization energy is greater than the preceding one. Atomic radius decreases left to right on the periodic table as nuclear charge increases, while it increases down a group as electron shells expand. Positive ions have smaller radii than their parent atoms due to their increased nuclear charge.
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.
Ionization Potential
This document discusses ionization potential and the factors that affect it. Ionization potential is the amount of energy required to remove an electron from an isolated atom, forming a cation. The first ionization energy is removing the outermost electron, and subsequent ionization energies increase with each additional electron removed. Factors that affect ionization potential include effective nuclear charge, atomic size, shielding effects, and full or half-filled orbitals. Ionization energy generally increases left to right across a period and decreases down a group on the periodic table.
Periodic trends
This document discusses several key trends seen in the periodic table including atomic radius, ionization energy, electronegativity, and electron shielding. It defines these terms and explains how they vary depending on an element's location in the periodic table, such as atomic radius generally increasing down a group and decreasing left to right across a period. The document also provides examples of comparing atomic radii of different elements and assessing trends in ionization energy and electronegativity.
Periodic Relationships
There are observable trends in the physical and chemical properties of elements across periods and down groups in the periodic table. As you move across a period, atomic radius decreases due to the increasing effective nuclear charge pulling the valence electrons closer. Down groups, atomic radius increases as each successive energy level is farther from the nucleus. Ionization energy generally increases across periods as effective nuclear charge increases, and decreases down groups as the valence electrons are farther from the nucleus. Electron affinity increases across periods but decreases down groups. Oxidation states can be used to keep track of electrons in compounds and ions.
Periodic trends
Here are the answers to your questions:
1. Shielding of nuclear charge remains constant as you move across a period or down a group since the number of electron shells remains the same.
2. Atomic size decreases as you move across a period due to increased nuclear charge, and increases as you move down a group due to additional electron shells providing more shielding.
3. Ions form when atoms gain or lose electrons. Cations form when atoms lose electrons, becoming positively charged. Anions form when atoms gain electrons, becoming negatively charged.
4. Ionization energy is the minimum amount of energy required to remove an electron from a neutral gaseous atom.
5. Ionization energy increases
04 periodic trends v2
- 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
Tang 02 wave quantum mechanic model
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.
Electronegativity
Linus Pauling introduced the concept of electronegativity in 1932 to help explain the nature of chemical bonds. Electronegativity is a property that reflects an atom's ability to attract electrons in a bond. Atoms with high electronegativity strongly attract electrons, while atoms with low electronegativity attract electrons weakly. Whether a bond is ionic or covalent depends on the difference in electronegativity between the bonded atoms - a large difference leads to ionic bonds where one atom takes the electrons, while a small difference leads to covalent bonds where electrons are shared. Electronegativity values help predict bond type based on this principle.
Atomic radius ppt for chem
The document discusses several atomic properties including atomic radius, ionic radius, ionization energy, electronegativity, nuclear charge, and shielding effect. It provides trends within the periodic table, noting that atomic radius increases down a group and decreases left to right across a period. Ionic radius also decreases left to right within a period and increases down a group. Ionization energy 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. The document also examines nuclear charge and shielding effect.
9/25 What is the trend for electronegativity?
The document is a chemistry class lecture on trends in the periodic table, specifically electronegativity. It defines electronegativity as an atom's ability to attract electrons in a chemical bond. It then explains that electronegativity increases from left to right across periods due to more protons, but decreases down groups because more electron shells shield the nucleus from outer electrons. Practice problems are assigned for students to study these trends.
Chemistry
Chemistry topics:
1) Atom
2) Electron Configuration
3) Ions
4) Metals
5) Factors affecting solvation
6) Colligative Properties of Solution
7) Stoichiometry
Chemistry grade 10
1) Atom
2) Electron Configuration
3) Ions
4) Metals
5) Factors affecting solvation
6) Colligative Properties of Solution
7) Stoichiometry
Tang 01 light and atomic structure
The teacher will be preparing spectroscopes and gas tubes to revisit atomic structure with students. The document discusses how light and atomic structure are related, including that electrons move between discrete energy levels and absorb or emit photons of specific wavelengths when changing levels. Different elements have unique emission spectra due to variations in electron configuration.
PERIODIC TABLE
This document discusses ionization energy, electronegativity, and melting/boiling points across period 3 elements. It defines ionization energy as the minimum energy required to remove electrons from atoms or ions. Electronegativity increases across a period as atomic size decreases and effective nuclear charge increases, but decreases down a group as atomic size increases. Melting and boiling points depend on bond strength and type of intermolecular forces. Larger molecules with stronger van der Waals forces, like S8, have higher melting and boiling points than smaller molecules like Ar.
5 nuclear stability and radioactive decay
The document discusses nuclear stability and radioactive decay. It explains that stable nuclei have a balance of protons and neutrons, while unstable nuclei decay through processes like alpha decay, beta decay, and gamma emission to become more stable. Alpha decay involves emitting a helium nucleus, beta decay changes the number of protons or neutrons by converting between the two, and gamma emission releases energy without changing the nucleus. Unstable nuclei may undergo several types of decay until becoming a stable isotope. The various types of decay are illustrated with nuclear equations and examples.
Effective nuclear charge
Effective nuclear charge increases across a period due to increasing shielding. As you move from left to right, protons and electrons are added but shielding increases by less than one, so effective nuclear charge felt by electrons increases. Effective nuclear charge is most useful for comparing electrons in the same shell and subshell of different atoms. It is less useful comparing electrons in different periods.
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.
What is an ion? - Chemistry presentation
An ion is an atom or molecule that has gained or lost electrons, giving it a positive or negative charge. Atoms can become ions through ionization, where metals typically lose electrons to form cations and nonmetals gain electrons to form anions. Ionic compounds are formed when oppositely charged ions bond via ionic bonds, while covalent bonds involve the sharing of electron pairs between nonmetal atoms.
Tang 04 periodic trends
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.
04 periodic trends and effective nuclear charge supplement
This document discusses periodic trends in atomic radius and effective nuclear charge (Zeff). It begins by listing elements in order of decreasing atomic radius and noting errors in the predicted order. It then provides the actual order and atomic radii data. It explains that alkali and alkaline earth metals generally have significantly larger atomic radii than nonmetals. The document also discusses how ionic radii change for metals versus nonmetals upon forming ions. Finally, it explains how Zeff relates to atomic radius, noting that a higher Zeff results in a smaller atomic radius due to a stronger attraction between the nucleus and outer electrons.
Ionic bonding
This document discusses the nature of ionic bonds and properties of ionic compounds. It explains that ionic bonding occurs when there is a large difference in electronegativity (>1.7) between a metal and non-metal atom. The metal atom donates electrons to become a positively charged cation, while the non-metal atom gains electrons to become a negatively charged anion. These oppositely charged ions are arranged in a regular crystal lattice structure held together by electrostatic forces. Ionic compounds have properties stemming from this lattice structure such as being crystalline solids, brittle, and able to conduct electricity when in solution but not in solid form.
Periodic trends
The document discusses periodic trends in elemental properties, including atomic radius, ionization energy, electron affinity, electronegativity, and reactivity. It explains that Dmitri Mendeleev was the first to organize elements into a periodic table based on their properties and predicted undiscovered elements. The trends are due to changes in atomic structure and the effective nuclear charge as protons and electrons are added. Atomic radius generally decreases left to right and increases top to bottom. Ionization energy and electronegativity increase as you move up and to the left on the periodic table.
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.
Periodic trend in properties
Periodic properties refer to properties that repeat at regular intervals in the periodic table. These include atomic radius, ionic radius, ionization enthalpy, electron gain enthalpy, electronegativity, and valency. The document discusses the trends in these periodic properties across periods and down groups in the periodic table. For example, ionization enthalpy generally increases as you move left to right across a period as nuclear charge increases, while metallic character decreases as you move left to right but increases as you move down a group.
Periodic properties of the elements
periodic properties of the elements for class 11th and 12th science students..go and copy all the stuff
Chapter 8 notes
The document discusses the periodic classification of elements and periodic trends in their physical properties. Elements are arranged in the periodic table according to increasing atomic number and are classified based on their electron configurations. Representative elements have incompletely filled s or p subshells, transition metals have incompletely filled d subshells, and lanthanides and actinides have incompletely filled f subshells. Periodic trends include decreases in atomic radius and increases in ionization energy and electron affinity across a period as effective nuclear charge increases. Down a group, atomic radius increases as nuclear charge remains constant but principal quantum number increases.
Periodicity
Periodicity refers to the recurring trends in properties seen when elements are arranged in order of increasing atomic number in the periodic table. Elements within the same group have similar properties. The periodic table is organized into rows and columns, with elements in the same period having electron shells filling in a similar way.
Some key periodic properties that were discussed include atomic radius, ionization energy, electron affinity, and electronegativity. Atomic radius decreases left to right within a period as protons increase, but increases down a group as electron shielding effects occur. Ionization energy generally increases left to right as it takes more energy to remove electrons from smaller atoms. Electron affinity values increase left to right and decrease down a group. Electrone
More Related Content
What's hot
04 periodic trends v2
- 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
Tang 02 wave quantum mechanic model
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.
Electronegativity
Linus Pauling introduced the concept of electronegativity in 1932 to help explain the nature of chemical bonds. Electronegativity is a property that reflects an atom's ability to attract electrons in a bond. Atoms with high electronegativity strongly attract electrons, while atoms with low electronegativity attract electrons weakly. Whether a bond is ionic or covalent depends on the difference in electronegativity between the bonded atoms - a large difference leads to ionic bonds where one atom takes the electrons, while a small difference leads to covalent bonds where electrons are shared. Electronegativity values help predict bond type based on this principle.
Atomic radius ppt for chem
The document discusses several atomic properties including atomic radius, ionic radius, ionization energy, electronegativity, nuclear charge, and shielding effect. It provides trends within the periodic table, noting that atomic radius increases down a group and decreases left to right across a period. Ionic radius also decreases left to right within a period and increases down a group. Ionization energy 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. The document also examines nuclear charge and shielding effect.
9/25 What is the trend for electronegativity?
The document is a chemistry class lecture on trends in the periodic table, specifically electronegativity. It defines electronegativity as an atom's ability to attract electrons in a chemical bond. It then explains that electronegativity increases from left to right across periods due to more protons, but decreases down groups because more electron shells shield the nucleus from outer electrons. Practice problems are assigned for students to study these trends.
Chemistry
Chemistry topics:
1) Atom
2) Electron Configuration
3) Ions
4) Metals
5) Factors affecting solvation
6) Colligative Properties of Solution
7) Stoichiometry
Chemistry grade 10
1) Atom
2) Electron Configuration
3) Ions
4) Metals
5) Factors affecting solvation
6) Colligative Properties of Solution
7) Stoichiometry
Tang 01 light and atomic structure
The teacher will be preparing spectroscopes and gas tubes to revisit atomic structure with students. The document discusses how light and atomic structure are related, including that electrons move between discrete energy levels and absorb or emit photons of specific wavelengths when changing levels. Different elements have unique emission spectra due to variations in electron configuration.
PERIODIC TABLE
This document discusses ionization energy, electronegativity, and melting/boiling points across period 3 elements. It defines ionization energy as the minimum energy required to remove electrons from atoms or ions. Electronegativity increases across a period as atomic size decreases and effective nuclear charge increases, but decreases down a group as atomic size increases. Melting and boiling points depend on bond strength and type of intermolecular forces. Larger molecules with stronger van der Waals forces, like S8, have higher melting and boiling points than smaller molecules like Ar.
5 nuclear stability and radioactive decay
The document discusses nuclear stability and radioactive decay. It explains that stable nuclei have a balance of protons and neutrons, while unstable nuclei decay through processes like alpha decay, beta decay, and gamma emission to become more stable. Alpha decay involves emitting a helium nucleus, beta decay changes the number of protons or neutrons by converting between the two, and gamma emission releases energy without changing the nucleus. Unstable nuclei may undergo several types of decay until becoming a stable isotope. The various types of decay are illustrated with nuclear equations and examples.
Effective nuclear charge
Effective nuclear charge increases across a period due to increasing shielding. As you move from left to right, protons and electrons are added but shielding increases by less than one, so effective nuclear charge felt by electrons increases. Effective nuclear charge is most useful for comparing electrons in the same shell and subshell of different atoms. It is less useful comparing electrons in different periods.
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.
What is an ion? - Chemistry presentation
An ion is an atom or molecule that has gained or lost electrons, giving it a positive or negative charge. Atoms can become ions through ionization, where metals typically lose electrons to form cations and nonmetals gain electrons to form anions. Ionic compounds are formed when oppositely charged ions bond via ionic bonds, while covalent bonds involve the sharing of electron pairs between nonmetal atoms.
Tang 04 periodic trends
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.
04 periodic trends and effective nuclear charge supplement
This document discusses periodic trends in atomic radius and effective nuclear charge (Zeff). It begins by listing elements in order of decreasing atomic radius and noting errors in the predicted order. It then provides the actual order and atomic radii data. It explains that alkali and alkaline earth metals generally have significantly larger atomic radii than nonmetals. The document also discusses how ionic radii change for metals versus nonmetals upon forming ions. Finally, it explains how Zeff relates to atomic radius, noting that a higher Zeff results in a smaller atomic radius due to a stronger attraction between the nucleus and outer electrons.
Ionic bonding
This document discusses the nature of ionic bonds and properties of ionic compounds. It explains that ionic bonding occurs when there is a large difference in electronegativity (>1.7) between a metal and non-metal atom. The metal atom donates electrons to become a positively charged cation, while the non-metal atom gains electrons to become a negatively charged anion. These oppositely charged ions are arranged in a regular crystal lattice structure held together by electrostatic forces. Ionic compounds have properties stemming from this lattice structure such as being crystalline solids, brittle, and able to conduct electricity when in solution but not in solid form.
Periodic trends
The document discusses periodic trends in elemental properties, including atomic radius, ionization energy, electron affinity, electronegativity, and reactivity. It explains that Dmitri Mendeleev was the first to organize elements into a periodic table based on their properties and predicted undiscovered elements. The trends are due to changes in atomic structure and the effective nuclear charge as protons and electrons are added. Atomic radius generally decreases left to right and increases top to bottom. Ionization energy and electronegativity increase as you move up and to the left on the periodic table.
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.
Periodic trend in properties
Periodic properties refer to properties that repeat at regular intervals in the periodic table. These include atomic radius, ionic radius, ionization enthalpy, electron gain enthalpy, electronegativity, and valency. The document discusses the trends in these periodic properties across periods and down groups in the periodic table. For example, ionization enthalpy generally increases as you move left to right across a period as nuclear charge increases, while metallic character decreases as you move left to right but increases as you move down a group.
What's hot (19)
04 periodic trends and effective nuclear charge supplement
04 periodic trends and effective nuclear charge supplement
Similar to I.e and electroneg
Periodic properties of the elements
periodic properties of the elements for class 11th and 12th science students..go and copy all the stuff
Chapter 8 notes
The document discusses the periodic classification of elements and periodic trends in their physical properties. Elements are arranged in the periodic table according to increasing atomic number and are classified based on their electron configurations. Representative elements have incompletely filled s or p subshells, transition metals have incompletely filled d subshells, and lanthanides and actinides have incompletely filled f subshells. Periodic trends include decreases in atomic radius and increases in ionization energy and electron affinity across a period as effective nuclear charge increases. Down a group, atomic radius increases as nuclear charge remains constant but principal quantum number increases.
Periodicity
Periodicity refers to the recurring trends in properties seen when elements are arranged in order of increasing atomic number in the periodic table. Elements within the same group have similar properties. The periodic table is organized into rows and columns, with elements in the same period having electron shells filling in a similar way.
Some key periodic properties that were discussed include atomic radius, ionization energy, electron affinity, and electronegativity. Atomic radius decreases left to right within a period as protons increase, but increases down a group as electron shielding effects occur. Ionization energy generally increases left to right as it takes more energy to remove electrons from smaller atoms. Electron affinity values increase left to right and decrease down a group. Electrone
Classification of elements & periodicity in properties
The document discusses periodic trends in properties such as atomic radius, ionization energy, and electronegativity. It explains Mendeleev's periodic table and how modern periodic law arranges elements based on atomic number instead of atomic mass. Periodicity in properties occurs because similar electronic configurations repeat at regular intervals as atomic number increases. Atomic radius generally decreases across a period as nuclear charge increases, and increases down a group as more shells are added. Ionization energy is the energy required to remove an electron from an atom, and is directly proportional to nuclear charge and inversely proportional to size and shielding effects.
periodic table trends
The Periodic Table and Periodic Law SECTION 3 Periodic Trends
ionization energy
atomic radius
electronegativity
classification of elements ppt 11.pptx
1) The document discusses the classification of elements and periodic trends in properties according to the periodic table. It explains early classification systems like Newlands' Law of Octaves and Mendeleev's periodic table. (Sentence 1)
2) Key periodic trends discussed include how atomic radius decreases across a period but increases down a group, how ionization enthalpy generally increases across a period but decreases down a group, and how shielding effects influence these trends. (Sentence 2)
3) The document also outlines the different blocks of the periodic table (s, p, d, f blocks) and describes general electronic configurations and properties of elements in each block. (Sentence 3)
L5theperiodictable 130906000951-
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.
Periodic classification
The document discusses periodic trends in elemental properties according to the periodic table. It explains that atomic radius generally increases moving left to right within a period and increases moving down within a family. Ionization energy decreases moving left to right within a period and decreases moving down within a family, while electron affinity shows the opposite trends. Metallic character decreases and electronegativity increases moving from left to right across the periodic table. Overall reactivity of metals increases with increasing size while reactivity of nonmetals increases with decreasing size. The document also discusses ion formation and how cations are smaller than the original atom while anions are larger.
Periodicity
The document discusses periodicity and how properties vary across periods and down groups in the periodic table. It specifically focuses on Period 3 elements (Na to Ar). Key points:
1) Atomic radius decreases across Period 3 as nuclear charge increases, attracting electrons more strongly. Radius increases down groups as atomic size increases.
2) Ionization energy generally increases across Period 3 as nuclear charge increases, requiring more energy to remove electrons. It decreases down groups as distance from nucleus increases.
3) Melting/boiling points are highest for metals/covalent networks and lower for weak molecular bonds. Electrical conductivity is highest for metals and lowest for nonmetals.
Periodic Table 5
The document discusses several periodic properties of elements including atomic radius, ionization energy, and electronegativity. It explains that atomic radius decreases across a period as nuclear charge increases but increases down a group as electron shielding increases. Ionization energy generally increases across a period as it becomes harder to remove electrons but decreases down a group as electrons are farther from the nucleus. Electronegativity also increases across a period as nuclear attraction increases.
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.
Classification of elements and periodicity in properties class 11th chapter 3...
The document discusses the classification of elements and periodic trends in properties according to the periodic table. It summarizes Mendeleev's periodic law and how he arranged elements in a table based on increasing atomic weight and similar properties in vertical columns. It discusses modern revisions to the periodic table based on atomic number. The document then explains trends in various physical and chemical properties across the periodic table, including atomic radius, ionization energy, electronegativity, and oxidation states. It discusses how properties vary periodically based on an element's position in the s, p, d, and f blocks of the periodic table.
Chemistry- JIB Topic 7 Periodicity
The document discusses several key concepts in chemistry including periodic trends in properties, ionization energy, electron affinity, and the behavior of cations, anions, and oxides. Specifically, it explains that ionization energy increases across a period as nuclear charge increases but decreases down a group as electrons experience more shielding. It also describes how cations are smaller than their parent atoms while anions are larger due to electron repulsion. Finally, it summarizes periodic trends in physical and chemical properties within and across periods.
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.
APChem- Chapter 7 Lecture- Periodic Trends
The document discusses trends in the properties of elements in the periodic table. It describes how elements in the same group generally have similar chemical properties, though properties are not identical. It discusses how Mendeleev and Meyer independently organized the elements into the first periodic tables based on recurring trends in properties. Elements in the inner transition metals block were later added.
Chem 101 week 9 ch8
The document summarizes periodic trends among elements including atomic and ionic sizes, ionization energies, and electron affinities. It explains that atomic size decreases left to right across a period as effective nuclear charge increases, while size increases down a group as principal quantum number increases. Ionization energy generally increases left to right as effective nuclear charge increases, with exceptions between groups IIA-IIIA and VA-VIA. Electron affinity becomes more exothermic left to right with exceptions between groups IA-IIA and IVA-VA. The document also describes trends and properties of representative elements and families including alkali metals, alkaline earth metals, halogens, and noble gases.
Advchemchapt8 101015121750-phpapp02
- Ionic bonds form when a metal reacts with a nonmetal, resulting in the transfer of electrons from the metal to the nonmetal. The ions achieve noble gas electron configurations.
- Covalent bonds form when two nonmetals share electrons between their nuclei. Polar covalent bonds result in unequal sharing of electrons between the atoms.
- Electronegativity describes an atom's ability to attract shared electrons. It increases left to right and decreases top to bottom on the periodic table. Unequal electronegativity between bonded atoms results in bond polarity.
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.
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-
Chapters6 121207125912-phpapp02
This document provides an overview of chemical bonding. It discusses valence electrons and how to determine the number for each element using the periodic table. It describes the different types of chemical bonds - ionic bonds formed by the transfer of electrons between atoms, and covalent bonds formed by the sharing of electron pairs. It also discusses concepts like electronegativity and how it relates to bond type and strength.
Similar to I.e and electroneg (20)
Classification of elements & periodicity in properties
Classification of elements & periodicity in properties
Classification of elements and periodicity in properties class 11th chapter 3...
Classification of elements and periodicity in properties class 11th chapter 3...
More from jawad ali yousafzai
Thomas Edison ppt
Thomas Alva Edison was an American inventor who developed many pioneering devices, including the phonograph, the motion picture camera, and a long-lasting practical electric light bulb. According to a story, when Edison was a child his teacher deemed him addled and told his mother he could no longer attend school, but his mother recognized his genius and taught him herself at home. Later in life, Edison discovered a note from the teacher calling him addled, and cried for hours realizing how much his mother had done for him. Edison held over 1,000 patents and won many awards for his inventions, leaving a significant impact on technology and daily life around the world.
prime minister of pakistan 2018
This short document provides limited information about an individual named Nasirul Mulk, born on May 28, 2018. It also mentions that more information will be coming soon and expresses gratitude to unspecified people.
Sentence
The document discusses the five kinds of sentences: assertive, negative, interrogative, exclamatory, and imperative. Assertive sentences make statements, negative sentences express negation, interrogative sentences ask questions, exclamatory sentences express strong feelings, and imperative sentences give commands or requests. Examples of each kind of sentence are provided.
Role of nitrogen (n) (2)
The process of nutrition allows living organisms to obtain food and use it for growth, metabolism, and repair. Both plants and animals require nutrition throughout their lives. Plants can produce their own food through photosynthesis and are autotrophic. They require macronutrients like carbon, hydrogen, and nitrogen, as well as micronutrients like iron and copper. Nitrogen is a vital substance that is a major component of proteins, hormones, chlorophyll, vitamins, and enzymes essential for plant life. Nitrogen metabolism also plays a major role in stem and leaf growth.
Quaid e-azam
The document does not contain any substantive content to summarize. It appears to be blank or contain only formatting characters. In 3 sentences or less, a summary is not possible due to the lack of information in the provided text.
Population
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help alleviate symptoms of mental illness and boost overall mental well-being.
Part os speech
This document discusses different parts of speech in English including nouns, pronouns, adjectives, adverbs, prepositions, and conjunctions. It provides examples for each part of speech. Nouns are classified as common, proper, countable, or uncountable. Pronouns are used instead of nouns to avoid repetition. Adjectives are used to describe or modify nouns. Prepositions show relationships between nouns and pronouns. Conjunctions join words and sentences.
Noun
This document provides information about nouns, including the definition of a noun and different types of nouns. It defines nouns as words that name people, places, things, or ideas. There are several types of nouns discussed, including proper nouns, common nouns, concrete nouns, abstract nouns, collective nouns, and compound nouns. The document also covers singular and plural nouns, including rules for making nouns plural and some irregular plural forms. Examples are provided throughout to illustrate each noun concept.
New discovery
1. Astronomers detected a planet orbiting Proxima Centauri, the star closest to our sun, that is 1.3 times the mass of Earth and sits within the star's habitable zone.
2. Scientists from LIGO detected gravitational waves from the collision of two black holes over a billion years ago, confirming Einstein's theory of relativity.
3. Archaeological discoveries in Australia have shown that humans have inhabited the continent's interior for at least 49,000 years, 10,000 years longer than previously thought.
Mullah nasiruddin
Mullah Nasiruddin was a famous comedic character from folktales. Stories about his funny situations and life have been published in several languages around the world. In one tale, when asked why the moon is more useful than the sun, Mullah Nasiruddin replied that light is needed more at night than during the day. In another, when a friend pointed out that Mullah Nasiruddin had said he was forty years old two years ago, Mullah Nasiruddin insisted that he always stands by what he says.
Metals and its prop's
The document discusses the properties and classification of metals. It defines metals as elements in groups I, II, III (except boron), some elements of groups IV, V, and VI. Metals are malleable, ductile, good conductors of heat and electricity, and solid at room temperature (except mercury). It then provides specific details on the uses of sodium and magnesium, two common metals, including in synthetic rubber production, lighting, desulfurization, and lightweight alloys.
Medina charter
This document summarizes the key points of the Medina Charter signed after the migration of the Prophet Muhammad (PBUH) to Medina. The charter established an agreement between different communities in Medina, including Jews, pagans, and Muslims, to form a united community. It outlined principles of cooperation in defense against outside enemies, dispute resolution, protection of religious freedom, and blood money payments according to community customs. The charter established Medina as a sanctuary for signatories and prohibited fighting between or against believers on behalf of non-believers.
Lipid soluble vitamins
This document summarizes key information about lipid soluble vitamins, including vitamin A, D, E, K, and F. It describes the biological functions and roles of each vitamin, such as vitamin A's role in vision and cell growth. Sources of each vitamin are provided, along with symptoms of deficiency. The document also discusses hypervitaminosis and clinical uses of certain vitamins.
Kinds of-nouns
This document provides a lesson on types of nouns, including:
1. Common nouns name general people, places, things, or ideas while proper nouns name specific ones.
2. Concrete nouns can be seen, touched, etc. while abstract nouns are ideas, qualities, and feelings that cannot be seen or touched.
3. Examples are provided to demonstrate common vs. proper and concrete vs. abstract nouns, and students practice identifying and classifying different nouns.
Islam
Muhammad proclaimed a new monotheistic faith called Islam and established the religious and political principles that united diverse Arabian tribes into a militant civilization. After enduring years of exile in Medina, Muhammad and his followers triumphantly returned to Mecca in 630 CE where he had received his first revelations from God. The key figures and events that shaped early Islam included Muhammad's revelations which were recorded as the Quran, the migration from Mecca to Medina in 622 CE, and the establishment of the Five Pillars of Islam including daily prayer, which unified the early Muslim community.
Ionization energy
- Ionization energy is the amount of energy required to remove an electron from an atom. The first ionization energy is the amount required to remove the outermost electron.
- More energy is required to remove the second electron compared to the first, and even more for the third electron.
- Ionization energy decreases down a group as the atomic number increases since electrons are farther from the nucleus and more shielded.
- There is a general trend of increasing ionization energy when moving left to right across a period as protons are added making electrons more tightly bound.
I . e energy
The document discusses the benefits of exercise for mental health. Regular physical activity can help reduce anxiety and depression and improve mood and cognitive function. Exercise causes chemical changes in the brain that may help protect against mental illness and improve symptoms.
How to write_an_essay_(psy)
Writing an essay requires planning, researching, drafting, and revising. The writer should start by choosing a topic and developing a thesis statement. Research should involve finding credible sources to support the thesis. The essay is then written and revised to clearly communicate the key points and arguments.
Discovery
This document contains 3 summaries of separate topics:
1) New surveys in the Republic of Congo found the population of western lowland gorillas to be much higher than previously estimated, at 125,000. However, war in a neighboring country threatens the smaller population of mountain gorillas.
2) China has made impressive progress in its space program, launching 3 crewed missions between 2003-2008 and completing a spacewalk. China aims to land humans on the moon by 2020.
3) NASA's Phoenix lander explored Mars' polar region in 2008, finding evidence the planet was once wet but reinforcing that Mars is currently a dead world. The lander functioned as planned until the harsh Martian winter
More from jawad ali yousafzai (20)
Recently uploaded
Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...
Andreas Schleicher, Director of Education and Skills at the OECD presents at the launch of PISA 2022 Volume III - Creative Minds, Creative Schools on 18 June 2024.
skeleton System.pdf (skeleton system wow)
🔥🔥🔥🔥🔥🔥🔥🔥🔥
إضغ بين إيديكم من أقوى الملازم التي صممتها
ملزمة تشريح الجهاز الهيكلي (نظري 3)
💀💀💀💀💀💀💀💀💀💀
تتميز هذهِ الملزمة بعِدة مُميزات :
1- مُترجمة ترجمة تُناسب جميع المستويات
2- تحتوي على 78 رسم توضيحي لكل كلمة موجودة بالملزمة (لكل كلمة !!!!)
#فهم_ماكو_درخ
3- دقة الكتابة والصور عالية جداً جداً جداً
4- هُنالك بعض المعلومات تم توضيحها بشكل تفصيلي جداً (تُعتبر لدى الطالب أو الطالبة بإنها معلومات مُبهمة ومع ذلك تم توضيح هذهِ المعلومات المُبهمة بشكل تفصيلي جداً
5- الملزمة تشرح نفسها ب نفسها بس تكلك تعال اقراني
6- تحتوي الملزمة في اول سلايد على خارطة تتضمن جميع تفرُعات معلومات الجهاز الهيكلي المذكورة في هذهِ الملزمة
واخيراً هذهِ الملزمة حلالٌ عليكم وإتمنى منكم إن تدعولي بالخير والصحة والعافية فقط
كل التوفيق زملائي وزميلاتي ، زميلكم محمد الذهبي 💊💊
🔥🔥🔥🔥🔥🔥🔥🔥🔥
A Visual Guide to 1 Samuel | A Tale of Two Hearts
These slides walk through the story of 1 Samuel. Samuel is the last judge of Israel. The people reject God and want a king. Saul is anointed as the first king, but he is not a good king. David, the shepherd boy is anointed and Saul is envious of him. David shows honor while Saul continues to self destruct.
How Barcodes Can Be Leveraged Within Odoo 17
In this presentation, we will explore how barcodes can be leveraged within Odoo 17 to streamline our manufacturing processes. We will cover the configuration steps, how to utilize barcodes in different manufacturing scenarios, and the overall benefits of implementing this technology.
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
The History of NZ 1870-1900.
Making of a Nation.
From the NZ Wars to Liberals,
Richard Seddon, George Grey,
Social Laboratory, New Zealand,
Confiscations, Kotahitanga, Kingitanga, Parliament, Suffrage, Repudiation, Economic Change, Agriculture, Gold Mining, Timber, Flax, Sheep, Dairying,
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...Nguyen Thanh Tu Collection
https://app.box.com/s/tacvl9ekroe9hqupdnjruiypvm9rdaneBIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
Practical manual for National Examination Council, Nigeria.
Contains guides on answering questions on the specimens provided
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Aberdeen
Educational Technology in the Health Sciences
Plenary presentation at the NTTC Inter-university Workshop, 18 June 2024, Manila Prince Hotel.
How to Setup Warehouse & Location in Odoo 17 Inventory
In this slide, we'll explore how to set up warehouses and locations in Odoo 17 Inventory. This will help us manage our stock effectively, track inventory levels, and streamline warehouse operations.
Lifelines of National Economy chapter for Class 10 STUDY MATERIAL PDF
The chapter Lifelines of National Economy in Class 10 Geography focuses on the various modes of transportation and communication that play a vital role in the economic development of a country. These lifelines are crucial for the movement of goods, services, and people, thereby connecting different regions and promoting economic activities.
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
Physical pharmaceutics notes for B.pharm students
How to Predict Vendor Bill Product in Odoo 17
This slide will guide us through the process of predicting vendor bill products based on previous purchases from the vendor in Odoo 17.
Temple of Asclepius in Thrace. Excavation results
The temple and the sanctuary around were dedicated to Asklepios Zmidrenus. This name has been known since 1875 when an inscription dedicated to him was discovered in Rome. The inscription is dated in 227 AD and was left by soldiers originating from the city of Philippopolis (modern Plovdiv).
HYPERTENSION - SLIDE SHARE PRESENTATION.
IT WILL BE HELPFULL FOR THE NUSING STUDENTS
IT FOCUSED ON MEDICAL MANAGEMENT AND NURSING MANAGEMENT.
HIGHLIGHTS ON HEALTH EDUCATION.
BBR 2024 Summer Sessions Interview Training
Qualitative research interview training by Professor Katrina Pritchard and Dr Helen Williams
Wound healing PPT
This document provides an overview of wound healing, its functions, stages, mechanisms, factors affecting it, and complications.
A wound is a break in the integrity of the skin or tissues, which may be associated with disruption of the structure and function.
Healing is the body’s response to injury in an attempt to restore normal structure and functions.
Healing can occur in two ways: Regeneration and Repair
There are 4 phases of wound healing: hemostasis, inflammation, proliferation, and remodeling. This document also describes the mechanism of wound healing. Factors that affect healing include infection, uncontrolled diabetes, poor nutrition, age, anemia, the presence of foreign bodies, etc.
Complications of wound healing like infection, hyperpigmentation of scar, contractures, and keloid formation.
Recently uploaded (20)
Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...
Andreas Schleicher presents PISA 2022 Volume III - Creative Thinking - 18 Jun...
NEWSPAPERS - QUESTION 1 - REVISION POWERPOINT.pptx
NEWSPAPERS - QUESTION 1 - REVISION POWERPOINT.pptx
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
Level 3 NCEA - NZ: A Nation In the Making 1872 - 1900 SML.ppt
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BÀI TẬP BỔ TRỢ TIẾNG ANH LỚP 9 CẢ NĂM - GLOBAL SUCCESS - NĂM HỌC 2024-2025 - ...
BIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
BIOLOGY NATIONAL EXAMINATION COUNCIL (NECO) 2024 PRACTICAL MANUAL.pptx
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
How to Setup Warehouse & Location in Odoo 17 Inventory
How to Setup Warehouse & Location in Odoo 17 Inventory
Lifelines of National Economy chapter for Class 10 STUDY MATERIAL PDF
Lifelines of National Economy chapter for Class 10 STUDY MATERIAL PDF
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
I.e and electroneg
- 1. 1 Mr. Shields Regents Chemistry U08 L05
- 2. Ionization energy 2 Ionization Energy (IE) – The amount of energy needed to remove an electron from an atom or ion. Every electron in any atom or ion has a specific ionization energy. First Ionization Energy – The amount of energy needed to remove the 1st electron from the outermost shell of a neutral (uncharged) atom.
- 3. 3 Rb + energy Rb+ + 1e- Ionization energies are measured in KJ/mole 1 2 3
- 4. Ionization Energy 4Some atoms have 2 or more electrons in the valence Shell. For example, for example alkaline earth elements such as Mg or Sr Removing the 1st electron (first ionization energy) will always take less energy than the energy necessary to Remove the 2nd electron (second ionization energy). This trend continues. The energy necessary to remove a 3rd electron is greater than the energy necessary to Remove the 2nd and so on
- 5. Ionization Energy Trends 5The energy necessary to remove a valence electron Varies from atom to atom in predictable ways: ) Ionization energy increases as each successive electron is removed ) Ionization energy DECREASES going DOWN a GROUP ) Ionization energy INCREASES as you go ACROSS a PERIOD ) The noble gases have the highest Ionization energies ) The alkali metals have the lowest Ionization energies
- 6. 6
- 7. Ionization Energy - Groups 7So… Why do ionization energies display these trends in groups and periods? Let’s see … Ionization energies decrease going down a Group: Moving down a group the principle energy level increases - distance of electron from the positive nucleus increases and there are more electrons providing inner shell shielding of the nucleus Therefore the valence electrons are less strongly held Na 2-8-1 (IE = 496 KJ/Mol) Rb 2-8-18-8-1 (IE = 403 KJ/mol)
- 8. Ionization Energy - Periods 8Ionization energies across a Period increase: As we move across a period the principle energy level of the valence electron doesn’t change - However Nuclear charge increases across the period while the distance of the valence electron from nucleus remains the same - Therefore valence electrons feel the inc. nuclear charge more strongly and it takes more energy to remove them from the atom +37 n=5 +47 n=5 Rb 2-8-18-8-1 (IE=403 KJ/mol) Ag 2-8-18-18-1 (IE=731KJ/mol)
- 9. Ionization Energy – Noble Gases 9Noble Gases: The valence shell octet found in the NOBLE GASES is a particularly stable electron configuration. Any change from this config will take unusually high energy since the net result is “destabilizing” But the trend of decreasing ionization going down a group is also true even for the Noble Gases Ne: 2-8 IE: 2081 KJ/mol Kr: 2-8-18-8 1351 Rn: 2-8-18-32-18-8 1037
- 11. 11 2nd or 3rd IONIZATION ENERGY: Once an e- is removed the positive nuclear charge per electron is now stronger. So the I.E. to remove the next electron increases Secondly, enough electrons are lost to achieve an octet, removal the next electron would destroy the very stable octet and the I.E. necessary to remove the next electron jumps significantly 1st IE(KJ/Mol) 2nd IE 3rd IE Na: 2-8-1 496 4,560 Mg: 2-8-2 736 1,450 7,730
- 12. Electronegativity 12When we discussed Intermolecular forces we needed To be able to specify whether a molecule was polar or Non-polar. We had a set of guide lines we used to help determine Non-polarity. What are they? So… What is the definition of a polar and a non-polar molecule? Electronegativity is a property of an element that Will help us quantify how polar a molecule is.
- 13. 13 ELECTRONEGATIVITY: - A measure of how strongly an element pulls electrons towards it in a chemical bond Electronegativity (unlike I.E.) has no units: EN has an arbitrary scale that ranges from 0 – 4.0 Fluorine’s EN is the highest (4.0) Francium’s EN is the lowest (about 0.7) FCs F Fvs Low EN Hi EN Same or Simialar EN (polar) (non-polar) δ+ δ-
- 14. Electronegativity 14 ALL ELEMENTS have IE values even if they have negative Oxidation Numbers (gain electrons). The same is true for electronegativity. - elements that tend to lose electrons (metals) still have an electronegativity value (though smaller than the non-metals) IE(KJ/mol) Electronegativity Fr 393 (lowest) 0.7 (lowest) F 1681 (very hi) 4.0 (highest)
- 15. Electronegativity 15 Since all Elements have electronegativity values we can Use these values to: 1) Help determine what molecules are polar 2) What molecules are more polar than others For example: Consider these two molecules H-Cl and H-I … both are polar molecules. Now, which one is MORE polar? (Hint you’ll need to use EN values) We’ll talk more about this in the next unit!
- 16. Electronegativity Trends 16 When considering Electronegativity, the trends are Very similar to those observed for Ionization Energy hold true for Electronegativity - Electronegativity decreases down a Group - Electronegativity increases across Periods