This document provides information on ionic compounds and metals. It discusses how ions are formed through the gain or loss of valence electrons to achieve stable octet configurations. Ionic compounds contain oppositely charged ions that are attracted to each other. Their crystal lattices give them high melting and boiling points. Metals form lattices with cations surrounded by a sea of delocalized electrons, giving them malleability, ductility, and high conductivity.
Ionic compounds form when oppositely charged ions attract each other, forming ionic bonds. Ions are formed when atoms gain or lose valence electrons to achieve a stable electron configuration. In ionic compounds, the cation is written first followed by the anion in chemical formulas. Metals form metallic bonds where metal atoms donate their valence electrons, which are free to move throughout the crystal lattice structure.
Ionic compounds form when atoms gain or lose valence electrons to achieve stable electron configurations, forming oppositely charged ions that attract each other. Ions are arranged in repeating crystal lattices that give ionic compounds high melting and boiling points and make them brittle solids. Metals form metallic bonds through delocalized electrons that allow metal atoms to bond without transferring or sharing electrons.
This document contains an overview of several sections from a chemistry textbook chapter on ionic compounds and metals. Section 7.1 discusses how ions are formed when atoms gain or lose electrons to achieve a stable octet configuration. Section 7.2 describes how ionic bonds form between oppositely charged ions, resulting in ionic compounds with a crystalline lattice structure. Section 7.3 covers writing formulas and naming conventions for ionic compounds and polyatomic ions. Section 7.4 explains metallic bonding and how metal atoms share delocalized electrons in a "sea" of electrons, giving metals their characteristic physical properties.
This document summarizes key concepts from Chapter 7 on ionic and metallic bonding. It discusses how ions form as atoms gain or lose electrons to achieve stable noble gas electron configurations. Cations are positive ions that form when metals lose electrons, while anions are negative ions that form when nonmetals gain electrons. Ionic compounds consist of cations and anions bonded through electrostatic attraction. Their properties include being crystalline solids with high melting points that conduct electricity when molten or dissolved. Metallic bonding is described as a "sea of electrons" where metal atoms are positively charged cations floating in a sea of delocalized electrons that are free to move, explaining metals' malleability and conductivity. Alloys are mixtures of
This document discusses the formation of ions from elements. It begins by defining valence electrons as the electrons in the outermost energy level of an atom. The number of valence electrons determines an element's chemical properties and usually matches the element's group number on the periodic table. Atoms form ions by gaining or losing valence electrons to achieve stable noble gas configurations. Cations are positively charged ions that form when metals lose electrons. Anions are negatively charged ions that form when nonmetals gain electrons. Common cations include Na+ and Mg2+; common anions include Cl- and O2-.
Chapter 6.3 : Ionic Bonding and Ionic CompoundsChris Foltz
Ionic compounds are composed of positive and negative ions in ratios that balance the charges. They form crystalline lattices with ions arranged in an orderly pattern. The ions are held together by strong electrostatic forces called lattice energy. Ionic compounds have high melting and boiling points, are hard and brittle, and conduct electricity when molten or dissolved but not in the solid state. Polyatomic ions are charged groups of covalently bonded atoms that behave as single ions in ionic compounds.
There are three main types of chemical bonds: ionic bonds, covalent bonds, and hydrogen bonds. Ionic bonds involve the transfer of electrons between atoms, covalent bonds involve the sharing of electrons between atoms, and hydrogen bonds are weak attractions between polar molecules containing hydrogen, such as water molecules. Chemical bonds are crucial as they hold atoms and molecules together, allowing for the formation of larger biological compounds like proteins.
This document discusses metallic bonding and the properties of metals. It explains that metals consist of positively charged metal cations bonded to a "sea" of delocalized valence electrons. This metallic bonding allows the cations to slide past one another, giving metals properties like malleability, ductility, and high thermal and electrical conductivity. Alloys are also discussed, which are mixtures of metals that can have superior properties to the pure metals. An important alloy example given is steel, an iron-carbon alloy with various other elements added to control its properties for different applications.
Ionic compounds form when oppositely charged ions attract each other, forming ionic bonds. Ions are formed when atoms gain or lose valence electrons to achieve a stable electron configuration. In ionic compounds, the cation is written first followed by the anion in chemical formulas. Metals form metallic bonds where metal atoms donate their valence electrons, which are free to move throughout the crystal lattice structure.
Ionic compounds form when atoms gain or lose valence electrons to achieve stable electron configurations, forming oppositely charged ions that attract each other. Ions are arranged in repeating crystal lattices that give ionic compounds high melting and boiling points and make them brittle solids. Metals form metallic bonds through delocalized electrons that allow metal atoms to bond without transferring or sharing electrons.
This document contains an overview of several sections from a chemistry textbook chapter on ionic compounds and metals. Section 7.1 discusses how ions are formed when atoms gain or lose electrons to achieve a stable octet configuration. Section 7.2 describes how ionic bonds form between oppositely charged ions, resulting in ionic compounds with a crystalline lattice structure. Section 7.3 covers writing formulas and naming conventions for ionic compounds and polyatomic ions. Section 7.4 explains metallic bonding and how metal atoms share delocalized electrons in a "sea" of electrons, giving metals their characteristic physical properties.
This document summarizes key concepts from Chapter 7 on ionic and metallic bonding. It discusses how ions form as atoms gain or lose electrons to achieve stable noble gas electron configurations. Cations are positive ions that form when metals lose electrons, while anions are negative ions that form when nonmetals gain electrons. Ionic compounds consist of cations and anions bonded through electrostatic attraction. Their properties include being crystalline solids with high melting points that conduct electricity when molten or dissolved. Metallic bonding is described as a "sea of electrons" where metal atoms are positively charged cations floating in a sea of delocalized electrons that are free to move, explaining metals' malleability and conductivity. Alloys are mixtures of
This document discusses the formation of ions from elements. It begins by defining valence electrons as the electrons in the outermost energy level of an atom. The number of valence electrons determines an element's chemical properties and usually matches the element's group number on the periodic table. Atoms form ions by gaining or losing valence electrons to achieve stable noble gas configurations. Cations are positively charged ions that form when metals lose electrons. Anions are negatively charged ions that form when nonmetals gain electrons. Common cations include Na+ and Mg2+; common anions include Cl- and O2-.
Chapter 6.3 : Ionic Bonding and Ionic CompoundsChris Foltz
Ionic compounds are composed of positive and negative ions in ratios that balance the charges. They form crystalline lattices with ions arranged in an orderly pattern. The ions are held together by strong electrostatic forces called lattice energy. Ionic compounds have high melting and boiling points, are hard and brittle, and conduct electricity when molten or dissolved but not in the solid state. Polyatomic ions are charged groups of covalently bonded atoms that behave as single ions in ionic compounds.
There are three main types of chemical bonds: ionic bonds, covalent bonds, and hydrogen bonds. Ionic bonds involve the transfer of electrons between atoms, covalent bonds involve the sharing of electrons between atoms, and hydrogen bonds are weak attractions between polar molecules containing hydrogen, such as water molecules. Chemical bonds are crucial as they hold atoms and molecules together, allowing for the formation of larger biological compounds like proteins.
This document discusses metallic bonding and the properties of metals. It explains that metals consist of positively charged metal cations bonded to a "sea" of delocalized valence electrons. This metallic bonding allows the cations to slide past one another, giving metals properties like malleability, ductility, and high thermal and electrical conductivity. Alloys are also discussed, which are mixtures of metals that can have superior properties to the pure metals. An important alloy example given is steel, an iron-carbon alloy with various other elements added to control its properties for different applications.
The document discusses ionic bonds and ionic compounds. It explains that ionic compounds form when oppositely charged ions attract via electrostatic forces called ionic bonds. Ionic compounds are crystalline solids that are electrically neutral, have high melting points, and can conduct electricity when molten or dissolved in water as the ions are free to move. Sodium chloride is given as a common example of an ionic compound composed of sodium and chloride ions.
Ionic compounds form when a metal transfers electrons to a nonmetal, resulting in oppositely charged ions that are attracted in a crystal lattice structure. The ratio of cations to anions must result in an overall neutral charge. Ionic compounds are named by writing the cation first followed by the anion. Polyatomic ions are named based on the nonmetal and number of oxygen atoms. Metallic bonds form a "sea of electrons" that are delocalized and allow metal atoms to strongly attract each other.
Ionic compounds form giant lattice structures when oppositely charged ions bond via electrostatic forces. This ionic bonding results in high melting points and the ability to conduct electricity when molten or dissolved. Covalent bonds involve electron sharing and can form either simple molecules with weak intermolecular forces or giant covalent structures with very high melting points due to numerous strong covalent bonds. Metallic bonding involves delocalized electrons that act as glue between positive metal ions, allowing them to slide past one another.
Ionic compounds are formed when ions bond via ionic bonds. Ions form when atoms gain or lose electrons to achieve a stable electron configuration. Ionic bonds result from the electrostatic attraction between oppositely charged ions. Ionic compounds consist of a crystal lattice structure where ions are arranged in a repeating pattern. Metals form metallic bonds where delocalized electrons are attracted to metallic cations. Alloys are mixtures of metals or metals with other elements that have distinct properties from their components.
This document discusses chemical bonding and macromolecular structures. It begins by explaining the different types of bonds - ionic bonds formed between metals and non-metals by electron transfer, and covalent bonds formed between non-metals by electron sharing. It describes the properties of ionic and covalent compounds. It then discusses macromolecular structures found in substances like diamond, graphite and metals. It explains metallic bonding and compares the structures and properties of diamond and graphite. In the end, it discusses the different uses of diamond and graphite based on their properties.
The document outlines key learning outcomes and concepts about atomic structure, including describing the structure of atoms with atomic numbers 1 to 20, defining terms like atomic number and mass number, explaining electron configuration and outer electrons, and distinguishing between isotopes, ions, and molecules of elements and compounds. It also provides illustrations of atomic structure and examples of applying atomic structure concepts.
Substances with simple molecular, giant ionic and giant covalent structures have very different properties. Ionic, covalent and metallic bonds are strong, while forces between molecules are weaker. Nanomaterials have new properties due to their small size on the scale of 10 atoms. The structures of substances influence their properties and uses.
Ionic compounds are formed through ionic bonding between metals and nonmetals. Electrons are transferred from the metal atoms to the nonmetal atoms, resulting in cations with positive charges and anions with negative charges. The electrostatic forces between the oppositely charged ions hold the compound together in a crystalline lattice structure. Common polyatomic ions like nitrate, sulfate, and phosphate are also present in ionic compounds. Ionic compounds have properties like being solid at room temperature, having high melting points, and being good conductors of electricity when molten or dissolved in water.
This document discusses chemical bonding and intramolecular bonding. It begins by introducing ionic and covalent bonds as the two major types of intramolecular bonding that hold atoms together to form molecules. Ionic bonds form between ions through the transfer of electrons from metals to nonmetals. Covalent bonds form between nonmetals by the sharing of electrons. The document then goes into further detail about the formation of ions, ionic compounds through electron transfers, and the naming of ionic compounds according to IUPAC nomenclature rules.
The document discusses different types of chemical bonds and macromolecular structures. It explains that ionic bonds form between metals and non-metals via the transfer of electrons, giving ionic compounds high melting points and the ability to conduct electricity when molten or dissolved. Covalent bonds form between non-metals by the sharing of electrons, resulting in covalent compounds having low melting points and the inability to conduct electricity. Some covalent substances exist as macromolecules or giant molecular structures like diamond and graphite. These have very high melting points and different properties compared to simple molecules. Metallic bonding is also described, involving positive metal ions in a "sea of electrons" giving metals properties like malleability and high conductivity
Ionic bonding occurs when atoms of metals and non-metals combine to form ionic compounds. Atoms of metals will donate electrons to form cations, while atoms of non-metals will accept electrons to form anions. This transfer of electrons allows the atoms to achieve stable electron configurations similar to noble gases. Common examples are sodium chloride, which forms when sodium donates an electron to chlorine, and magnesium oxide, which forms when magnesium donates two electrons to oxygen. The chemical formulas of ionic compounds are written to balance the charges of the cation and anion.
We will be going over information for Exam 2. Talking a lot about naming of compounds and learning electron domain geometries with molecular geometries.
Chemical bonds hold atoms together in compounds and determine compounds' properties. Compounds have definite compositions and properties unlike their constituent elements. Ionic bonds form when atoms transfer electrons to become ions of opposite charge, binding in crystalline structures. Covalent bonds form when atoms share electron pairs, binding as individual molecules with properties depending on size and shape. Metallic bonds allow electron delocalization in metal crystals. Different bonding structures give compounds distinctive physical and chemical characteristics.
Bonding and structure - ionic compounds, covalent compounds and metals. Relationship between intermolecular forces and physical properties. Allotropes.
Ionic bonding results from the electrostatic attraction between oppositely charged ions. When a metal atom reacts with a nonmetal, the metal typically loses electrons to form a cation while the nonmetal gains electrons to form an anion. These oppositely charged ions are then attracted to each other, forming an ionic bond. Ionic compounds have crystalline structures where the ions are arranged in repeating patterns. Their strong ionic bonds make them brittle with high melting points. Many ionic compounds dissolve in water to form electrolyte solutions where the ions are free to move.
The document summarizes key aspects of the periodic table, including:
1) It describes the historical development of the periodic table by scientists like Lavoisier, Dobereiner, Newlands, Meyer, and Mendeleev.
2) It explains the modern arrangement of elements in the periodic table based on proton number and discusses the properties of elements in the same group and period.
3) It provides examples of properties and reactions of representative elements from groups 1, 17, 18 and period 3 of the periodic table. Transition elements and semimetals are also discussed.
1. The document discusses different types of chemical bonding including ionic bonding, covalent bonding, and metallic bonding.
2. Ionic bonding involves the transfer of electrons between atoms to form ions with opposite charges that are attracted in a giant lattice structure.
3. Covalent bonding can form either simple molecules held together by shared electron pairs or giant covalent structures with thousands of atoms bonded together.
1. Chemical bonds are invisible forces that hold atoms together in compounds. They form when atoms undergo changes and combine with each other.
2. There are two main types of chemical bonds - ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between atoms to form ions, while covalent bonds involve the sharing of electrons between atoms.
3. The shape and properties of molecules can be predicted using Lewis structures, the valence shell electron pair repulsion (VSEPR) model, and by determining the hybridization of the atoms' orbitals. This allows for determining important characteristics like molecular geometry.
Ionic bonds form when oppositely charged ions attract each other, forming ionic compounds. Cations form when atoms lose electrons to achieve a stable electron configuration, while anions form when atoms gain electrons. Ionic compounds consist of a crystal lattice structure where cations are surrounded by anions. They have properties like high melting points and boiling points since energy is required to overcome the strong electrostatic attractions between ions.
I. Ionic compounds form when oppositely charged ions bond via ionic bonds. When atoms gain or lose electrons to achieve stable octet configurations, they form cations or anions that bond in a crystalline lattice.
II. Ionic bonds are strong electrostatic attractions between cations and anions. Ionic compounds have high melting and boiling points and are brittle solids that do not conduct electricity well.
III. Formulas and names of ionic compounds follow conventions where the cation is written first followed by the anion. Polyatomic ions are also considered when writing formulas and names.
This document covers ionic compounds and metals. It discusses:
1) How ions form when atoms gain or lose electrons to achieve stable octet configurations, and how ionic bonds form between oppositely charged ions in ionic compounds.
2) Ionic compounds consist of a crystalline lattice of ions with strong electrostatic attractions that give them high melting points and make them brittle and poor conductors.
3) Metals bond through delocalized electrons that form a "sea" of electrons, giving metals malleability, ductility, and high heat and electrical conductivity.
The document discusses ionic bonds and ionic compounds. It explains that ionic compounds form when oppositely charged ions attract via electrostatic forces called ionic bonds. Ionic compounds are crystalline solids that are electrically neutral, have high melting points, and can conduct electricity when molten or dissolved in water as the ions are free to move. Sodium chloride is given as a common example of an ionic compound composed of sodium and chloride ions.
Ionic compounds form when a metal transfers electrons to a nonmetal, resulting in oppositely charged ions that are attracted in a crystal lattice structure. The ratio of cations to anions must result in an overall neutral charge. Ionic compounds are named by writing the cation first followed by the anion. Polyatomic ions are named based on the nonmetal and number of oxygen atoms. Metallic bonds form a "sea of electrons" that are delocalized and allow metal atoms to strongly attract each other.
Ionic compounds form giant lattice structures when oppositely charged ions bond via electrostatic forces. This ionic bonding results in high melting points and the ability to conduct electricity when molten or dissolved. Covalent bonds involve electron sharing and can form either simple molecules with weak intermolecular forces or giant covalent structures with very high melting points due to numerous strong covalent bonds. Metallic bonding involves delocalized electrons that act as glue between positive metal ions, allowing them to slide past one another.
Ionic compounds are formed when ions bond via ionic bonds. Ions form when atoms gain or lose electrons to achieve a stable electron configuration. Ionic bonds result from the electrostatic attraction between oppositely charged ions. Ionic compounds consist of a crystal lattice structure where ions are arranged in a repeating pattern. Metals form metallic bonds where delocalized electrons are attracted to metallic cations. Alloys are mixtures of metals or metals with other elements that have distinct properties from their components.
This document discusses chemical bonding and macromolecular structures. It begins by explaining the different types of bonds - ionic bonds formed between metals and non-metals by electron transfer, and covalent bonds formed between non-metals by electron sharing. It describes the properties of ionic and covalent compounds. It then discusses macromolecular structures found in substances like diamond, graphite and metals. It explains metallic bonding and compares the structures and properties of diamond and graphite. In the end, it discusses the different uses of diamond and graphite based on their properties.
The document outlines key learning outcomes and concepts about atomic structure, including describing the structure of atoms with atomic numbers 1 to 20, defining terms like atomic number and mass number, explaining electron configuration and outer electrons, and distinguishing between isotopes, ions, and molecules of elements and compounds. It also provides illustrations of atomic structure and examples of applying atomic structure concepts.
Substances with simple molecular, giant ionic and giant covalent structures have very different properties. Ionic, covalent and metallic bonds are strong, while forces between molecules are weaker. Nanomaterials have new properties due to their small size on the scale of 10 atoms. The structures of substances influence their properties and uses.
Ionic compounds are formed through ionic bonding between metals and nonmetals. Electrons are transferred from the metal atoms to the nonmetal atoms, resulting in cations with positive charges and anions with negative charges. The electrostatic forces between the oppositely charged ions hold the compound together in a crystalline lattice structure. Common polyatomic ions like nitrate, sulfate, and phosphate are also present in ionic compounds. Ionic compounds have properties like being solid at room temperature, having high melting points, and being good conductors of electricity when molten or dissolved in water.
This document discusses chemical bonding and intramolecular bonding. It begins by introducing ionic and covalent bonds as the two major types of intramolecular bonding that hold atoms together to form molecules. Ionic bonds form between ions through the transfer of electrons from metals to nonmetals. Covalent bonds form between nonmetals by the sharing of electrons. The document then goes into further detail about the formation of ions, ionic compounds through electron transfers, and the naming of ionic compounds according to IUPAC nomenclature rules.
The document discusses different types of chemical bonds and macromolecular structures. It explains that ionic bonds form between metals and non-metals via the transfer of electrons, giving ionic compounds high melting points and the ability to conduct electricity when molten or dissolved. Covalent bonds form between non-metals by the sharing of electrons, resulting in covalent compounds having low melting points and the inability to conduct electricity. Some covalent substances exist as macromolecules or giant molecular structures like diamond and graphite. These have very high melting points and different properties compared to simple molecules. Metallic bonding is also described, involving positive metal ions in a "sea of electrons" giving metals properties like malleability and high conductivity
Ionic bonding occurs when atoms of metals and non-metals combine to form ionic compounds. Atoms of metals will donate electrons to form cations, while atoms of non-metals will accept electrons to form anions. This transfer of electrons allows the atoms to achieve stable electron configurations similar to noble gases. Common examples are sodium chloride, which forms when sodium donates an electron to chlorine, and magnesium oxide, which forms when magnesium donates two electrons to oxygen. The chemical formulas of ionic compounds are written to balance the charges of the cation and anion.
We will be going over information for Exam 2. Talking a lot about naming of compounds and learning electron domain geometries with molecular geometries.
Chemical bonds hold atoms together in compounds and determine compounds' properties. Compounds have definite compositions and properties unlike their constituent elements. Ionic bonds form when atoms transfer electrons to become ions of opposite charge, binding in crystalline structures. Covalent bonds form when atoms share electron pairs, binding as individual molecules with properties depending on size and shape. Metallic bonds allow electron delocalization in metal crystals. Different bonding structures give compounds distinctive physical and chemical characteristics.
Bonding and structure - ionic compounds, covalent compounds and metals. Relationship between intermolecular forces and physical properties. Allotropes.
Ionic bonding results from the electrostatic attraction between oppositely charged ions. When a metal atom reacts with a nonmetal, the metal typically loses electrons to form a cation while the nonmetal gains electrons to form an anion. These oppositely charged ions are then attracted to each other, forming an ionic bond. Ionic compounds have crystalline structures where the ions are arranged in repeating patterns. Their strong ionic bonds make them brittle with high melting points. Many ionic compounds dissolve in water to form electrolyte solutions where the ions are free to move.
The document summarizes key aspects of the periodic table, including:
1) It describes the historical development of the periodic table by scientists like Lavoisier, Dobereiner, Newlands, Meyer, and Mendeleev.
2) It explains the modern arrangement of elements in the periodic table based on proton number and discusses the properties of elements in the same group and period.
3) It provides examples of properties and reactions of representative elements from groups 1, 17, 18 and period 3 of the periodic table. Transition elements and semimetals are also discussed.
1. The document discusses different types of chemical bonding including ionic bonding, covalent bonding, and metallic bonding.
2. Ionic bonding involves the transfer of electrons between atoms to form ions with opposite charges that are attracted in a giant lattice structure.
3. Covalent bonding can form either simple molecules held together by shared electron pairs or giant covalent structures with thousands of atoms bonded together.
1. Chemical bonds are invisible forces that hold atoms together in compounds. They form when atoms undergo changes and combine with each other.
2. There are two main types of chemical bonds - ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between atoms to form ions, while covalent bonds involve the sharing of electrons between atoms.
3. The shape and properties of molecules can be predicted using Lewis structures, the valence shell electron pair repulsion (VSEPR) model, and by determining the hybridization of the atoms' orbitals. This allows for determining important characteristics like molecular geometry.
Ionic bonds form when oppositely charged ions attract each other, forming ionic compounds. Cations form when atoms lose electrons to achieve a stable electron configuration, while anions form when atoms gain electrons. Ionic compounds consist of a crystal lattice structure where cations are surrounded by anions. They have properties like high melting points and boiling points since energy is required to overcome the strong electrostatic attractions between ions.
I. Ionic compounds form when oppositely charged ions bond via ionic bonds. When atoms gain or lose electrons to achieve stable octet configurations, they form cations or anions that bond in a crystalline lattice.
II. Ionic bonds are strong electrostatic attractions between cations and anions. Ionic compounds have high melting and boiling points and are brittle solids that do not conduct electricity well.
III. Formulas and names of ionic compounds follow conventions where the cation is written first followed by the anion. Polyatomic ions are also considered when writing formulas and names.
This document covers ionic compounds and metals. It discusses:
1) How ions form when atoms gain or lose electrons to achieve stable octet configurations, and how ionic bonds form between oppositely charged ions in ionic compounds.
2) Ionic compounds consist of a crystalline lattice of ions with strong electrostatic attractions that give them high melting points and make them brittle and poor conductors.
3) Metals bond through delocalized electrons that form a "sea" of electrons, giving metals malleability, ductility, and high heat and electrical conductivity.
This document describes the formation and properties of ionic compounds. Ionic bonds form when oppositely charged ions attract each other to form electrically neutral compounds. Ionic compounds have high melting and boiling points because the ionic bonds between ions require a large amount of energy to overcome. The ions are tightly packed in a crystal lattice structure. Physical properties like conductivity depend on whether the ions are free to move or locked in place. Smaller or more highly charged ions result in stronger ionic bonds and higher lattice energies.
This document provides instructions for navigating a presentation on chemical bonding. It describes how to view the presentation as a slideshow, advance through slides, access resources and lessons, and exit the slideshow. The presentation covers topics like electrons and chemical bonding, ionic bonds, and covalent and metallic bonds. It includes bellringer questions, learning objectives, content on topics like ion formation and crystal lattices, and a concept map to summarize the key topics.
This document provides instructions for navigating a presentation on chemical bonding. It describes how to view the presentation as a slideshow, advance through slides, access resources and lessons, and exit the slideshow. The presentation contains sections on electrons and chemical bonding, ionic bonds, and covalent and metallic bonds. It includes objectives, content on topics like valence electrons and ionic compounds, and assessment questions.
There are three main types of chemical bonds: ionic bonds, covalent bonds, and metallic bonds. Ionic bonds form between oppositely charged ions, such as between sodium and chlorine atoms where sodium loses an electron to become positively charged and chlorine gains an electron to become negatively charged. Covalent bonds form when atoms share electrons, such as in water where oxygen and hydrogen share electron pairs. Metallic bonds form by the attraction of free-floating electrons within a lattice of positive metal ions.
This document summarizes key concepts about ionic and metallic bonding from chapter 7 of the textbook. It discusses how ions form as atoms gain or lose electrons to achieve stable noble gas electron configurations. It then explains how ionic compounds form as cations and anions are held together by electrostatic attraction between opposite charges. Metallic bonding is described as a "sea of electrons" model where the positively charged metal ions are held in place by attraction to delocalized valence electrons. Common properties of ionic and metallic materials like crystal structure and conductivity are also covered.
The document summarizes the key differences between ionic and covalent bonding. Ionic bonds form when a metal transfers electrons to a nonmetal, creating oppositely charged ions. Covalent bonds form when nonmetals share electrons to obtain a full outer shell. Ionic compounds have high melting points, are brittle solids, and dissolve well in water, while covalent compounds have lower melting points, are soft and pliable, and are generally insoluble in water.
The document provides an introduction to chemical bonding, including definitions of key terms like chemical bond, ionic bond, covalent bond, and coordinate bond. It describes the three main types of bonds: ionic formed by electron transfer, covalent formed by electron sharing, and coordinate bonds formed when one atom provides both electrons. Examples of bond formation are given for ionic compounds like NaCl and MgCl2 and covalent compounds like Cl2, CO2, and NH3. Characteristics of ionic and covalent compounds are also summarized.
This document provides an overview of chemical bonding. It defines a chemical bond as a force of attraction between atoms or ions that holds atoms together in molecules or compounds. Atoms form bonds to achieve stable electron configurations. There are three main types of bonds: ionic, covalent, and metallic. Ionic bonds form through the transfer of electrons between metals and nonmetals. Covalent bonds form through the sharing of electrons, usually between nonmetals. Metallic bonds involve the pooling of electrons between metal atoms. The document further explores bond formation and properties.
It's very good for SPM students . You have to learn the ionic bond thoroughly. If you understand well you can explain it vividly. For other chemistry notes can email me puterizamrud@gmail.com or facebook Pusat Tuisyen Zamrud .
According to Gilbert Lewis, atoms combine i order to achieve a more stable electron configuration. Maximum stability is obtained when an atom is isoelectronic with a noble gas. This presentation would enable students to relate lattice energy with physical properties such as melting point.
Class 11 Chemistry Revision Notes Chemical Bonding and Molecular Structure.pdfNadishaFathima
This document discusses chemical bonding and molecular structure. It begins by introducing atoms, molecules, and the forces that hold atoms together in molecules. It then defines chemical bonding and describes the main types of bonds: ionic, covalent, hydrogen, and polar bonds. The remainder of the document discusses these bond types in more detail, including how to represent bonds using Lewis structures, the characteristics of ionic compounds, factors that influence ionic bond formation, and more. It also introduces concepts like formal charge, valence shell electron pair repulsion theory (VSEPR) for predicting molecular geometry, and hybridization.
Subject: Chemical Bonding in physics....trueangel2022
This document discusses different types of chemical bonds:
- Ionic bonds form between metals and nonmetals through the transfer of electrons to create positively and negatively charged ions. Covalent bonds form between nonmetals through the sharing of electron pairs to create molecular compounds. Metallic bonds involve the pooling of electrons between metal atoms. Polar bonds occur when electrons are shared unevenly between atoms. Understanding chemical bonds is important because they join atoms in the materials used in everyday life.
This document summarizes key concepts about ions, ionic bonding, and covalent bonding from chemistry. It defines ions as atoms that have gained or lost electrons, and discusses how ions bond to form ionic compounds like sodium chloride. It also explains how atoms can bond by sharing electrons in covalent bonds, including how bond polarity and molecular shape are determined. Chemical formulas and naming conventions for ionic and covalent compounds are presented.
Chemical bonding xi , dr.mona srivastava , founder masterchemclassesDR MONA Srivastava
Viewers,
This ppt of chemical bonding is designed to give a complete idea and though conceptual extract of the topic for the students of XI to help them understand the basics of chemical bonding in chemistry. Hope it covers all important aspects and points .
Dr Mona Srivastava
Founder-
Masterchemclasses
This document provides an overview of the structure of matter and different types of bonds between atoms. It defines key terms like elements, compounds, and chemical bonds. It describes the three main types of bonds - covalent, ionic, and metallic - and explains how they form. Covalent bonds form when atoms share electrons. Ionic bonds form when electrons are transferred between atoms to form ions. Metallic bonds form due to attraction between positively charged metal ions and delocalized electrons. The document also discusses naming conventions for compounds and polyatomic ions.
Conditions for Formation of Ionic and Covalent BondsDamanpreet Singh
For Ionic Bond
1.It is generally formed of the metals and non-metals. The metal atom loses one or more electrons present in its valence shell and these electrons accept by the non-metallic atom.
2.One of the species is cation and the other is an anion.By losing electrons, the metal atom changes to (positive ion) cation.Similarly, the non-metal atom gaining the electrons, get change to (negative Ion) anion. The oppositely charged ions attract each other. Therefore, come closer resulting the formation of the ionic bond (Electrovalent Bond).
This document discusses ionic and metallic bonding. It explains that ions are formed when atoms gain or lose electrons to achieve stable noble gas electron configurations. Metals form cations by losing electrons while nonmetals form anions by gaining electrons. Ionic compounds contain cations and anions in ratios represented by chemical formulas. Metallic bonding occurs via delocalized valence electrons that are shared between metal atoms.
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This document discusses suffixes and terminology used in medicine. It begins by listing common combining forms used to build medical terms and their meanings. It then defines several noun, adjective, and shorter suffixes and provides their meanings. Examples are given of medical terms built using combining forms and suffixes. The document also examines specific medical concepts in more depth, such as hernias, blood cells, acromegaly, splenomegaly, and laparoscopy.
The document is a chapter from a medical textbook that discusses anatomical terminology pertaining to the body as a whole. It defines the structural organization of the body from cells to tissues to organs to systems. It also describes the body cavities and identifies the major organs contained within each cavity, as well as anatomical divisions of the abdomen and back.
This document is from a textbook on medical terminology. It discusses the basic structure of medical words and how they are built from prefixes, suffixes, and combining forms. Some key points:
- Medical terms are made up of elements including roots, suffixes, prefixes, and combining vowels. Understanding these elements is important for analyzing terms.
- Common prefixes include hypo-, epi-, and cis-. Common suffixes include -itis, -algia, and -ectomy.
- Dozens of combining forms are provided, such as gastro- meaning stomach, cardi- meaning heart, and aden- meaning gland.
- Rules are provided for analyzing terms, such as reading from the suffix backward and dropping combining vowels before suffixes starting with vowels
This document is the copyright information for Chapter 25 on Cancer from the 6th edition of the textbook Molecular Cell Biology published in 2008 by W. H. Freeman and Company. The chapter was authored by a team that includes Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 24 on Immunology from the 6th edition of the textbook Molecular Cell Biology published in 2008 by W. H. Freeman and Company. The chapter was authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
Nerve cells, also known as neurons, are highly specialized cells that process and transmit information through electrical and chemical signals. This chapter discusses the structure and function of neurons, how they communicate with each other via synapses, and how signals are propagated along neurons through changes in their membrane potentials. Neurons play a vital role in the nervous system by allowing organisms to process information and coordinate their responses.
This document is the copyright information for Chapter 22 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "The Molecular Cell Biology of Development" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 21 from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Cell Birth, Lineage, and Death" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright page for Chapter 20 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Regulating the Eukaryotic Cell Cycle" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This document is the copyright information for Chapter 19 from the 6th edition textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Integrating Cells into Tissues" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This chapter discusses microtubules and intermediate filaments, which are types of cytoskeletal filaments that help organize and move cellular components. Microtubules are involved in processes like cell division and intracellular transport, while intermediate filaments provide mechanical strength and help integrate the nucleus with the cytoplasm. Together, these filaments play important structural and functional roles in eukaryotic cells.
This chapter discusses microfilaments, which are one of the three main types of cytoskeletal filaments found in eukaryotic cells. Microfilaments are composed of actin filaments and play important roles in cell motility, structure, and intracellular transport. They allow cells to change shape and to move by contracting or extending parts of the cell surface.
This document is the copyright page for Chapter 16 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Signaling Pathways that Control Gene Activity" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This document is the copyright page for Chapter 15 of the 6th edition textbook "Molecular Cell Biology" by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira. It provides the chapter title "Cell Signaling I: Signal Transduction and Short-Term Cellular Responses" and notes the copyright is held by W. H. Freeman and Company in 2008.
This document is the copyright page for Chapter 14 from the 6th edition textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Vesicular Traffic, Secretion, and Endocytosis" and is authored by a group of scientists including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This chapter discusses how proteins are transported into membranes and organelles within cells. Proteins destined for membranes or organelles have targeting signals that are recognized by transport systems. The transport systems then direct the proteins to their proper destinations, such as inserting membrane proteins into membranes or delivering soluble proteins into organelles.
This document is the copyright information for Chapter 12 from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Cellular Energetics" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
This chapter discusses the transmembrane transport of ions and small molecules across cell membranes. It covers topics such as passive transport through membrane channels and pumps, as well as active transport using ATP. The chapter is from the 6th edition of the textbook Molecular Cell Biology and is copyrighted by W. H. Freeman and Company in 2008.
This document is the copyright information for Chapter 10, titled "Biomembrane Structure", from the sixth edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter was written by a team of authors including Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh and Matsudaira.
This document is the copyright information for Chapter 9 from the 6th edition of the textbook "Molecular Cell Biology" published in 2008 by W. H. Freeman and Company. The chapter is titled "Visualizing, Fractionating, and Culturing Cells" and is authored by Lodish, Berk, Kaiser, Krieger, Scott, Bretscher, Ploegh, and Matsudaira.
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.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
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This presentation was provided by Racquel Jemison, Ph.D., Christina MacLaughlin, Ph.D., and Paulomi Majumder. Ph.D., all of the American Chemical Society, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
LAND USE LAND COVER AND NDVI OF MIRZAPUR DISTRICT, UPRAHUL
This Dissertation explores the particular circumstances of Mirzapur, a region located in the
core of India. Mirzapur, with its varied terrains and abundant biodiversity, offers an optimal
environment for investigating the changes in vegetation cover dynamics. Our study utilizes
advanced technologies such as GIS (Geographic Information Systems) and Remote sensing to
analyze the transformations that have taken place over the course of a decade.
The complex relationship between human activities and the environment has been the focus
of extensive research and worry. As the global community grapples with swift urbanization,
population expansion, and economic progress, the effects on natural ecosystems are becoming
more evident. A crucial element of this impact is the alteration of vegetation cover, which plays a
significant role in maintaining the ecological equilibrium of our planet.Land serves as the foundation for all human activities and provides the necessary materials for
these activities. As the most crucial natural resource, its utilization by humans results in different
'Land uses,' which are determined by both human activities and the physical characteristics of the
land.
The utilization of land is impacted by human needs and environmental factors. In countries
like India, rapid population growth and the emphasis on extensive resource exploitation can lead
to significant land degradation, adversely affecting the region's land cover.
Therefore, human intervention has significantly influenced land use patterns over many
centuries, evolving its structure over time and space. In the present era, these changes have
accelerated due to factors such as agriculture and urbanization. Information regarding land use and
cover is essential for various planning and management tasks related to the Earth's surface,
providing crucial environmental data for scientific, resource management, policy purposes, and
diverse human activities.
Accurate understanding of land use and cover is imperative for the development planning
of any area. Consequently, a wide range of professionals, including earth system scientists, land
and water managers, and urban planners, are interested in obtaining data on land use and cover
changes, conversion trends, and other related patterns. The spatial dimensions of land use and
cover support policymakers and scientists in making well-informed decisions, as alterations in
these patterns indicate shifts in economic and social conditions. Monitoring such changes with the
help of Advanced technologies like Remote Sensing and Geographic Information Systems is
crucial for coordinated efforts across different administrative levels. Advanced technologies like
Remote Sensing and Geographic Information Systems
9
Changes in vegetation cover refer to variations in the distribution, composition, and overall
structure of plant communities across different temporal and spatial scales. These changes can
occur natural.
Walmart Business+ and Spark Good for Nonprofits.pdfTechSoup
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How to Setup Warehouse & Location in Odoo 17 InventoryCeline George
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.
How to Make a Field Mandatory in Odoo 17Celine George
In Odoo, making a field required can be done through both Python code and XML views. When you set the required attribute to True in Python code, it makes the field required across all views where it's used. Conversely, when you set the required attribute in XML views, it makes the field required only in the context of that particular view.
This presentation was provided by Rebecca Benner, Ph.D., of the American Society of Anesthesiologists, for the second session of NISO's 2024 Training Series "DEIA in the Scholarly Landscape." Session Two: 'Expanding Pathways to Publishing Careers,' was held June 13, 2024.
2. Main Ideas
Ions are formed when atoms gain or lose valence
electrons to achieve a stable octet electron
configuration.
Oppositely charged ion attract each other, forming
electrically neutral ionic compounds.
In written names and formulas for ionic
compounds, the cation appears first, followed by
the anion.
Metals form crystal lattices and can be modeled as
cations surrounded by a “sea’” of freely moving
valence electrons.
3. Ion Formation
Ions are formed when atoms gain or lose
valence electrons to achieve a stable octet
electron configuration.
Goals and Objectives:
Define a chemical bond.
Describe the formation of positive and
negative ions.
Relate ion formation to electron
configuration.
4. Valence Electrons and
Chemical Bonds
Chemical Bond – is a force that holds two
atoms together.
They can form between the positive nucleus
of one atom and the negative valence
electrons of another atom or between two
oppositely charged ions.
5. Valence Electrons and
Chemical Bonds
Atom’s try to form the octet – the stable
arrangement of eight valence electrons in the
outer energy level – by gaining or losing
valence electrons.
The transfer of valence electrons between
two atoms is based on the ionization energy
and electron affinity of the two atoms.
Noble gases- high ionization energy + low
electron affinity = little chemical reactivity.
7. Positive Ion Formation
Metal atoms are reactive because they lose
valence electrons easily.
Group 1: commonly form +1 ions
Group 2: commonly form +2 ions
Group 13: sometimes +3 ions
8. Positive Ion Formation
Transition metal ions have an outer shell of s2
They will lose their s electrons and
occasionally a d electron.
Typically form +2 or +3 ions but can form
greater than +3 ions
9. Positive Ion Formation
Other relatively stable electron arrangements
are referred to as pseudo-noble gas
configurations.
Groups 11-14 will lose electrons to form full
outer shells: s, p, and d.
10. Negative Ion Formation
An anion is a negatively charged ion. (Add “-ide”
to the end of the root atom name.)
Nonmetals easily gain electrons.
Example:
Chlorine atom:
1s2 2s2p6 3s2p5
Chlorine ion:
1s2 2s2p6 3s2p6 = Argon
11. Negative Ion Formation
Nonmetal ions gain the number of electrons
required to fill an octet.
Some nonmetals can gain or lose electrons to
complete an octet.
Phosphorus can gain 3 or lose 5
Group 15 usually gains 3 electrons
Group 16 usually gains 2 electrons
Group 17 usually gains 1 electron
14. Ionic Bonds and Ionic
Compounds
Oppositely charged ions attract each other, forming
electrically neutral ionic compounds.
Goals and Objectives:
Describe the formation of ionic bonds and the structure
of ionic compounds.
Generalize about the strength of ionic bonds based on
the physical properties of ionic compounds.
Categorize ionic bond formation as exothermic or
endothermic.
15. Ionic Bond
Ionic Bond is the electrostatic force that
holds oppositely charged particles together.
Ionic Compound is a compound that contains
an ionic bond.
Ionic bonds between metals and oxygen
are called oxides.
Most other ionic compounds are
considered salts.
16. Binary Ionic Compound
Binary Ionic compound is an ionic compound
that contains two different elements.
One metallic cation and a nonmetallic anion.
Examples: NaCl, MgO, KBr, LiF
17. Ionic Bond Formation
Electrons gained and lost in each element
must be equal. (conservation of electrons)
Calcium and Fluorine
Aluminum and Oxygen
Sodium and Chlorine
18. Properties of Ionic
Compounds
Compounds are organized such that a pattern
repeats to balance attraction and repulsion
Total charge of a compound is neutral
Often highly organized
Example: NaCl crystal
19. Crystal Lattice
A crystal lattice is a three dimensional
geometric arrangement of particles.
Each negative ion is surrounded by a
positive ion which results in strong
attractions between ions.
Size and shape are dependent on relative
numbers of ions.
20. Crystal Lattice
Physical Properties:
Characteristics of bond strength – ionic
bonds are relatively strong and take a large
amount of energy to break.
Melting point – high
Boiling point – high
Hardness of material is high: rigid and
brittle solids.
22. Crystal Lattice
Characteristics of the compound:
Conducts electricity, conditionally
Ions in solid state ionic compounds are locked
in place and they do not have free electrons
in order to conduct electricity.
Ionic compounds that are melted or dissolved
in aqueous solutions have ions that are free
to move and therefore do conduct electricity
Electrolyte – an ionic compound that
conducts electricity in an aqueous solution.
23. Energy and the Ionic
Bond
Formation of ionic compounds forms a
more stable system and therefore reduces
the energy required to sustain it.
Since the creating of bonds lowers energy,
energy is released in the process. The
creation of bonds is said to be Exothermic.
Exothermic – energy is released during a
chemical reaction.
24. Energy and the Ionic
Bond
Breaking of ionic compounds reduces the
stability of a system and therefore increases
the energy required to sustain it .
Since the creating of bonds lowers energy, the
breaking of bonds increases energy and
therefore it is required for the process.
Endothermic – energy is absorbed during a
chemical reaction.
25. Lattice Energy
Lattice energy is the energy required to separate 1
mole of the ions of an ionic compound.
higher the lattice energy the stronger the bond
strength.
Directly related to the size of the ions bonded.
smaller ions form compounds more closely
because attraction increases with decreased
distance.
Also affected by charge of ions
Higher ion charge typically has higher lattice
energy.
29. Names and Formulas
for Ionic Compounds
In written names and formulas for ionic compounds, the
cation appears first, followed by the anion.
Goals and Objectives:
Relate a formula unit of an ionic compound to its
composition.
Write formulas for ionic compounds and oxyanions.
Apply naming conventions to ionic compounds and
oxyanions.
30. Formulas for Ionic
Compounds
A standardized system for naming compounds
was developed for much the same reason as the
SI unit system. This serves as a universal naming
system for communication among the science
community.
31. Formula Unit
A formula unit is the chemical formula for an ionic
compound and represents the simplest ratio of
ions.
MgCl2 not Mg4Cl8
A monoatomic ion is a one atom ion.
33. Formulas for Ionic
Compounds
The symbol for the cation is written first with
the anion second.
Subscripts represent the number of atoms of
each element in a compound.
The total charge must equal zero in an ionic
compound.
34. Polyatomic Ions
Polyatomic ions are made up of more than one
atom.
Formulas for polyatomic ionic compounds
Charge applies to the entire group of atoms.
Parentheses are used if more than one
polyatomic ion is needed to balance a
compound.
Do not change subscripts within the ion group
Example (NH4)O
38. Names for Ions and
Ionic Compounds
1. Name the cation followed by the anion.
2. For monatomic cations, use the element
name.
3. For monatomic anions, use the root of the
element with the suffix –ide.
39. Names for Ions and
Ionic Compounds
4. Multiple oxidation states are represented by a
Roman numeral in paranthesis after the cation.
a) This applies to transition metals with more than
one oxidation state and not the Group 1 and 2
cations.
b) Example: FeO is Iron (II) oxide; Fe2O3 Iron (III)
oxide.
5. With a polyatomic ion, name the cation followed by
the name of the polyatomic ion.
a) Example: NaOH is sodium hydroxide.
43. Metallic Bonds and the
Properties of Metals
Metals form crystal lattices and can be modeled as
cations surrounded by a “sea” of freely moving valence
electrons.
Goals and Objectives:
Describe a metallic bond.
Relate the electron sea model to the physical
properties of metals.
Define alloys, and categorize them into two basic
types.
44. Metals
Metals are not ionic but share several properties
with ionic compounds.
Metals also form lattices in the solid state,
where 8 to 12 other atoms closely surround each
metal atom.
Within the crowded lattice, the outer energy
levels of metal atoms overlap.
45. Electron Sea Model
The electron sea model proposes that all metal
atoms in a metallic solid contribute their
valence electrons to form a "sea" of electron.
The electrons are free to move around and
are referred to as delocalized electrons,
forming a metallic cation.
47. Properties of Metals
Boiling points are much more extreme than
melting points because of the energy
required to separate atoms from the groups
of cations and electrons.
48. Properties of Metals
Metals are malleable because they can be
hammered into sheets.
Metals are ductile because they can be drawn
into wires.
49. Properties of Metals
Mobile electrons around cations make metals
good conductors of electricity and heat.
As the number of delocalized electrons
increases, so does hardness and strength.
50. Metal Alloys
An alloy is a mixture of elements that has
metallic properties.
The properties of alloys differ from the
elements they contain.
52. Metal Alloys
Substitutional alloys are formed when some
atoms in the original metallic solid are
replaced by other metals of similar atomic
structure.
Interstitial alloys are formed when small
holes in a metallic crystal are filled with
smaller atoms.
58. Key Concepts
A chemical bond is the force that holds two atoms
together.
Some atoms form ions to gain stability. This stable
configuration involves a complete outer energy
level, usually consisting of eight valence
electrons.
Ions are formed by the loss or gain of valence
electrons.
59. Key Concepts
The number of protons remains unchanged during
ion formation.
Ionic compounds contain ionic bonds formed by
the attraction of oppositely charged ions.
Ions in an ionic compound are arranged in a
repeating pattern known as a crystal lattice
60. Key Concepts
Ionic compound properties are related to
ionic bond strength.
Ionic compounds are electrolytes; they
conduct an electric current in the liquid phase
and in aqueous solution.
Lattice energy is the energy needed to
remove 1 mol of ions from its crystal lattice.
61. Key Concepts
A formula unit gives the ratio of cations to
anions in the ionic compound.
A monatomic ion is formed from one atom.
The charge of a monatomic ion is its
oxidation number.
Roman numerals indicate the oxidation
number of cations having multiple possible
oxidation states.
62. Key Concepts
Polyatomic ions consist of more than one
atom and act as a single unit.
To indicate more than one polyatomic ion in a
chemical formula, place parentheses around
the polyatomic ion and use a subscript.
A metallic bond forms when metal cations
attract freely moving, delocalized valence
electrons.
63. Key Concepts
In the electron sea model, electrons move
through the metallic crystal and are not held
by any particular atom.
The electron sea model explains the physical
properties of metallic solids.
Metal alloys are formed when a metal is
mixed with one or more other elements.
65. Questions
What is the repeating pattern of atoms in an ionic solid
called?
A. crystal lattice
B. ionic lattice
C. energy lattice
D. ionic bonding
66. Questions
Give the name of the following: NaClO4
A. sodium hypochlorite
B. sodium chlorite
C. sodium chlorate
D. sodium perchlorate
67. Questions
As the distance between ions in an ionic bond is shortened,
A. the energy to break the bond decreases.
B. the electrostatic attraction decreases.
C. the electrostatic attraction increases.
D. the ionic bond changes to a metallic bond.
68. Questions
An alloy is what type of substance?
A. heterogeneous mixture
B. compound
C. mixture of elements
D. element
69. Questions
Which is NOT true about metallic solids?
A. Metals are shiny.
B. Metals are good conductors of heat and electricity.
C. Metals are ductile.
D. Metals have relatively low boiling points.
70. Questions
Electrons in an atom’s outer most energy level are
referred to as what?
A. ions
B. cations
C. valence electrons
D. noble-gas electrons
71. Questions
What is the oxidation state of copper in Cu(II)Cl2?
A. 1+
B. 2+
C. 2–
D. unable to determine
72. Questions
Which elements naturally occur with a full octet of
valence electrons?
A. alkali metals
B. alkali earth metals
C. halogens
D. noble gases