This document discusses different types of chemical bonds including ionic, covalent, and metallic bonding. It explains how ionic bonds form through the transfer of electrons between metals and nonmetals, resulting in ions. Covalent bonds form through the sharing of electron pairs between nonmetals. Metallic bonding occurs through the interaction of positively charged metal ions in a "sea" of delocalized electrons. The properties of compounds formed by different bonding types are also summarized.
This document provides information on covalent bonding including:
1) Covalent bonds form when atoms share pairs of electrons, with each atom contributing one electron to the bond. This holds the atoms together due to attraction between the nuclei and shared electrons.
2) Covalent bonds can form between atoms of the same element or different elements. Exceptions include cases where atoms don't achieve a full octet or share all electrons to exceed the octet limit.
3) Multiple bonds are stronger and shorter than single bonds due to greater orbital overlap in the bonding region. Bond polarity increases with difference in electronegativity between atoms.
The document discusses ionic bonding. Ionic bonds form between elements when one atom loses electrons to become a positively charged cation and another atom gains those electrons to become a negatively charged anion. This transfer of electrons allows both atoms to achieve a stable noble gas electron configuration. The resulting ions are held together by electrostatic attraction in a crystal lattice structure. Ionic compounds have high melting points, are brittle, and do not conduct electricity as solids since the ions are tightly bound. They dissolve in water, allowing the ions to separate and move, making the solutions electrically conductive.
The document discusses chemical bonds and the formation of compounds from atoms. It begins by describing how the atoms in vitamin C bond together in a very specific orientation to form the molecule's shape. It then provides an outline of the chapter sections, which include topics like periodic trends in atomic properties, Lewis structures of atoms and compounds, and molecular shape. The chapter examines various types of bonds like ionic bonds formed through the transfer of electrons between atoms and covalent bonds formed by the sharing of electrons between atoms. It discusses concepts such as electronegativity and how molecular shape is influenced by bond polarity.
This document provides an overview of chemical bonding and the properties of ionic and covalent compounds. It discusses the following key points:
1. Chemical bonds form due to the attraction between atoms and involve the transfer or sharing of valence electrons. Ionic bonds form through electron transfer between metals and nonmetals, while covalent bonds involve electron sharing.
2. Lewis symbols represent atoms and their valence electrons and are used to predict bonding patterns. Electronegativity determines bond polarity.
3. Ionic compounds have high melting and boiling points due to strong electrostatic attractions in the crystal lattice. Covalent compounds can be solids, liquids or gases.
We will be going over information for Exam 2. Talking a lot about naming of compounds and learning electron domain geometries with molecular geometries.
An electrochemical cell consists of two different metals submerged in an electrolyte such as an acid or salt solution. Electrons flow from the more reactive metal, creating a voltage. For example, in a zinc-copper cell, zinc releases electrons into the electrolyte more readily than copper, becoming the negative electrode. The electrons flow to the copper electrode.
Electrolysis is the process of using a direct electric current to drive nonspontaneous chemical reactions. It involves the decomposition of an electrolyte into its constituent ions by the removal or addition of electrons to the ions. During electrolysis, ions migrate to the electrodes where they undergo oxidation or reduction reactions. In the electrolysis of molten lead bromide, lead ions are reduced to metallic lead at the cathode, while bromide ions are oxidized to bromine gas at the anode. When an aqueous solution of copper sulfate is electrolyzed using copper electrodes, copper ions are reduced at the cathode to form metallic copper while oxygen gas forms at the anode. Electrolysis requires an electrolyte, electrodes, and a direct current power
The document discusses electrochemistry and electrolysis. It defines electrolytes and non-electrolytes, and explains how electrolytes can conduct electricity in molten or aqueous states through the movement of ions. Examples are given of electrolysis processes and how electrolysis can be used for metal extraction, purification, and electroplating.
This document provides information on covalent bonding including:
1) Covalent bonds form when atoms share pairs of electrons, with each atom contributing one electron to the bond. This holds the atoms together due to attraction between the nuclei and shared electrons.
2) Covalent bonds can form between atoms of the same element or different elements. Exceptions include cases where atoms don't achieve a full octet or share all electrons to exceed the octet limit.
3) Multiple bonds are stronger and shorter than single bonds due to greater orbital overlap in the bonding region. Bond polarity increases with difference in electronegativity between atoms.
The document discusses ionic bonding. Ionic bonds form between elements when one atom loses electrons to become a positively charged cation and another atom gains those electrons to become a negatively charged anion. This transfer of electrons allows both atoms to achieve a stable noble gas electron configuration. The resulting ions are held together by electrostatic attraction in a crystal lattice structure. Ionic compounds have high melting points, are brittle, and do not conduct electricity as solids since the ions are tightly bound. They dissolve in water, allowing the ions to separate and move, making the solutions electrically conductive.
The document discusses chemical bonds and the formation of compounds from atoms. It begins by describing how the atoms in vitamin C bond together in a very specific orientation to form the molecule's shape. It then provides an outline of the chapter sections, which include topics like periodic trends in atomic properties, Lewis structures of atoms and compounds, and molecular shape. The chapter examines various types of bonds like ionic bonds formed through the transfer of electrons between atoms and covalent bonds formed by the sharing of electrons between atoms. It discusses concepts such as electronegativity and how molecular shape is influenced by bond polarity.
This document provides an overview of chemical bonding and the properties of ionic and covalent compounds. It discusses the following key points:
1. Chemical bonds form due to the attraction between atoms and involve the transfer or sharing of valence electrons. Ionic bonds form through electron transfer between metals and nonmetals, while covalent bonds involve electron sharing.
2. Lewis symbols represent atoms and their valence electrons and are used to predict bonding patterns. Electronegativity determines bond polarity.
3. Ionic compounds have high melting and boiling points due to strong electrostatic attractions in the crystal lattice. Covalent compounds can be solids, liquids or gases.
We will be going over information for Exam 2. Talking a lot about naming of compounds and learning electron domain geometries with molecular geometries.
An electrochemical cell consists of two different metals submerged in an electrolyte such as an acid or salt solution. Electrons flow from the more reactive metal, creating a voltage. For example, in a zinc-copper cell, zinc releases electrons into the electrolyte more readily than copper, becoming the negative electrode. The electrons flow to the copper electrode.
Electrolysis is the process of using a direct electric current to drive nonspontaneous chemical reactions. It involves the decomposition of an electrolyte into its constituent ions by the removal or addition of electrons to the ions. During electrolysis, ions migrate to the electrodes where they undergo oxidation or reduction reactions. In the electrolysis of molten lead bromide, lead ions are reduced to metallic lead at the cathode, while bromide ions are oxidized to bromine gas at the anode. When an aqueous solution of copper sulfate is electrolyzed using copper electrodes, copper ions are reduced at the cathode to form metallic copper while oxygen gas forms at the anode. Electrolysis requires an electrolyte, electrodes, and a direct current power
The document discusses electrochemistry and electrolysis. It defines electrolytes and non-electrolytes, and explains how electrolytes can conduct electricity in molten or aqueous states through the movement of ions. Examples are given of electrolysis processes and how electrolysis can be used for metal extraction, purification, and electroplating.
The document discusses topics related to chemical reactions and the periodic table. It provides information on:
- Mendeleev's creation of the periodic table and how he arranged elements based on their properties.
- The structure of atoms consisting of protons, neutrons, and electrons located in electron shells around the nucleus.
- The modern periodic table including atomic number and mass number.
- Ionic bonding forming between metals and non-metals through the transfer of electrons. Ionic compounds have high melting/boiling points and conduct electricity when molten or dissolved.
- Covalent bonding forming when atoms share electrons in covalent molecules. Simple covalent substances have low melting/boiling points while giant
Chemical bonds form between atoms in different ways depending on electron configuration. Ionic bonds form when electrons are transferred between metals and nonmetals, creating positively and negatively charged ions. Covalent bonds form when electrons are shared between nonmetals. Metallic bonds form between metal atoms through a "sea of electrons" that holds the atoms together.
Chemical bonds form between atoms in order to fill their outer electron shells. Ionic bonds form when electrons are transferred between metals and nonmetals, creating positively and negatively charged ions. Covalent bonds form when electrons are shared between nonmetals. Metallic bonds form between metal atoms through a "sea of electrons".
The document provides information about electrolysis, including:
1) Electrolysis is the chemical effect of electricity on ionic compounds, causing them to break up into simpler substances like elements.
2) During electrolysis, ions move to electrodes of opposite charge where chemical reactions occur - non-metals form at the anode and metals or hydrogen form at the cathode.
3) Examples of electrolysis include molten lead(II) bromide producing lead at the cathode and bromine at the anode, and aqueous copper(II) chloride producing copper at the cathode and chlorine at the anode.
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.
The document discusses key concepts in electrochemistry including electrolytes, conductors, electrolysis, and cations and anions. It defines an electrolyte as a substance that can conduct electricity due to the presence of freely moving ions. Conductors are able to conduct electricity but do not undergo chemical reactions. Electrolysis is the process of using a direct electric current to drive nonspontaneous chemical reactions through an electrolyte. During electrolysis, cations migrate to the cathode and anions migrate to the anode.
This document provides an overview of chemical bonding concepts covered in Chapter 6, including:
1) Valence electrons and how to determine them from the periodic table.
2) The main types of chemical bonds - ionic, covalent, and metallic. Ionic bonds form between metals and nonmetals, covalent between nonmetals, and metallic within metals.
3) Key characteristics of ionic and covalent bonds such as crystal structure, conductivity, and bond strength. Lewis structures are used to represent covalent bonds.
Electrolysis is the process of using direct electrical current to cause a non-spontaneous chemical reaction. During electrolysis, ions conduct electricity and move towards the electrode that attracts them. The key factors that determine the products of electrolysis include:
1) The type of electrolyte, whether it is a molten salt or aqueous solution, determines which ions are present and can be reduced or oxidized.
2) An ion's position in the electrochemical series indicates its tendency to gain or lose electrons. Ions lower in the series are more readily reduced or oxidized.
3) The concentration of the electrolyte solution can allow ions higher in the electrochemical series to also be reduced or
This document provides an overview of modern atomic theory and the periodic table. It discusses:
1) The history of atomic models including the Bohr model and wave-mechanical model.
2) How electrons are organized into principal energy levels, sublevels, and orbitals. The document defines s, p, d, and f orbitals.
3) Rules for distributing electrons including the Pauli exclusion principle and Hund's rule.
4) How the periodic table is organized by periods and groups based on electron configurations. Groups contain elements with similar properties.
5) How to write electron configurations using noble gas notation and determine an element's valence electrons based on its position in the periodic table
The document provides an overview of electrolysis, including what it is, how it works, and key factors that affect the products formed. Electrolysis is the separation of an ionic compound using direct current, where ions move to electrodes and gain or lose electrons. The type of electrolyte, position of ions in the electrochemical series, concentration of the solution, and type of electrodes used can impact what substances are produced during electrolysis.
Includes a discussion of Voltaic and electrolytic cells, the Nernst equation and the relationship between electrochemical processes, chemical equilibrium and free energy.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Covalent bonds form when atoms share electrons to complete their outer electron shells. Covalent compounds are typically made of nonmetal atoms. Binary covalent compounds contain only two elements. Their names follow specific rules based on element position in the periodic table. Molecular shape is determined by VSEPR theory, which predicts the geometry that minimizes electron pair repulsions. Polar covalent bonds result from unequal electron sharing between atoms of different electronegativity. Molecular polarity depends on both bond polarity and molecular geometry.
Electrolysis is the process of using electric current to cause non-spontaneous chemical changes. During electrolysis, ions are discharged at the electrodes. The key factors that determine which ions are discharged include the position of ions in the electrochemical series, concentration of ions, and type of electrode. Electrolysis has important industrial applications such as electroplating, metal purification, and metal extraction.
This document provides an overview of chemical bonding models including ionic bonding, covalent bonding, and metallic bonding. Ionic bonding involves the transfer of electrons between metals and nonmetals. Covalent bonding involves the sharing of electron pairs between two nonmetals. Metallic bonding occurs between metals and involves delocalized electrons within an electron sea. Lewis electron dot structures are used to represent electron arrangements around atoms and how they bond. Electronegativity differences between atoms determine bond polarity. Multiple bonding and resonance structures are also discussed.
Electrolysis is the decomposition of a substance by an electric current, where electrolytes carry current as ions in solution. During electrolysis, ions move to the electrodes and undergo oxidation or reduction reactions. At the cathode, electrons are gained and reduction occurs. At the anode, electrons are lost and oxidation occurs. The amount of substance deposited or gas produced can be calculated using Faraday's law, relating current, time, and moles of electrons in the electrode reactions.
This document provides information on electron configurations and quantum numbers:
- It defines the principal quantum number n, which describes the main energy level of an electron. It also defines the subsidiary quantum number l, which describes the shape of an orbital, and the magnetic quantum number m, which describes the orientation of an orbital in space.
- It discusses the four quantum numbers that describe each electron in an atom: n, l, m, and spin quantum number s.
- It provides examples of writing the four quantum numbers for the last electron in different atoms like Li, Cl, B, O, and Ar.
- It includes sample exam questions that test understanding of electron configurations, ion formations, bonding definitions
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.
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.
The document discusses topics related to chemical reactions and the periodic table. It provides information on:
- Mendeleev's creation of the periodic table and how he arranged elements based on their properties.
- The structure of atoms consisting of protons, neutrons, and electrons located in electron shells around the nucleus.
- The modern periodic table including atomic number and mass number.
- Ionic bonding forming between metals and non-metals through the transfer of electrons. Ionic compounds have high melting/boiling points and conduct electricity when molten or dissolved.
- Covalent bonding forming when atoms share electrons in covalent molecules. Simple covalent substances have low melting/boiling points while giant
Chemical bonds form between atoms in different ways depending on electron configuration. Ionic bonds form when electrons are transferred between metals and nonmetals, creating positively and negatively charged ions. Covalent bonds form when electrons are shared between nonmetals. Metallic bonds form between metal atoms through a "sea of electrons" that holds the atoms together.
Chemical bonds form between atoms in order to fill their outer electron shells. Ionic bonds form when electrons are transferred between metals and nonmetals, creating positively and negatively charged ions. Covalent bonds form when electrons are shared between nonmetals. Metallic bonds form between metal atoms through a "sea of electrons".
The document provides information about electrolysis, including:
1) Electrolysis is the chemical effect of electricity on ionic compounds, causing them to break up into simpler substances like elements.
2) During electrolysis, ions move to electrodes of opposite charge where chemical reactions occur - non-metals form at the anode and metals or hydrogen form at the cathode.
3) Examples of electrolysis include molten lead(II) bromide producing lead at the cathode and bromine at the anode, and aqueous copper(II) chloride producing copper at the cathode and chlorine at the anode.
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.
The document discusses key concepts in electrochemistry including electrolytes, conductors, electrolysis, and cations and anions. It defines an electrolyte as a substance that can conduct electricity due to the presence of freely moving ions. Conductors are able to conduct electricity but do not undergo chemical reactions. Electrolysis is the process of using a direct electric current to drive nonspontaneous chemical reactions through an electrolyte. During electrolysis, cations migrate to the cathode and anions migrate to the anode.
This document provides an overview of chemical bonding concepts covered in Chapter 6, including:
1) Valence electrons and how to determine them from the periodic table.
2) The main types of chemical bonds - ionic, covalent, and metallic. Ionic bonds form between metals and nonmetals, covalent between nonmetals, and metallic within metals.
3) Key characteristics of ionic and covalent bonds such as crystal structure, conductivity, and bond strength. Lewis structures are used to represent covalent bonds.
Electrolysis is the process of using direct electrical current to cause a non-spontaneous chemical reaction. During electrolysis, ions conduct electricity and move towards the electrode that attracts them. The key factors that determine the products of electrolysis include:
1) The type of electrolyte, whether it is a molten salt or aqueous solution, determines which ions are present and can be reduced or oxidized.
2) An ion's position in the electrochemical series indicates its tendency to gain or lose electrons. Ions lower in the series are more readily reduced or oxidized.
3) The concentration of the electrolyte solution can allow ions higher in the electrochemical series to also be reduced or
This document provides an overview of modern atomic theory and the periodic table. It discusses:
1) The history of atomic models including the Bohr model and wave-mechanical model.
2) How electrons are organized into principal energy levels, sublevels, and orbitals. The document defines s, p, d, and f orbitals.
3) Rules for distributing electrons including the Pauli exclusion principle and Hund's rule.
4) How the periodic table is organized by periods and groups based on electron configurations. Groups contain elements with similar properties.
5) How to write electron configurations using noble gas notation and determine an element's valence electrons based on its position in the periodic table
The document provides an overview of electrolysis, including what it is, how it works, and key factors that affect the products formed. Electrolysis is the separation of an ionic compound using direct current, where ions move to electrodes and gain or lose electrons. The type of electrolyte, position of ions in the electrochemical series, concentration of the solution, and type of electrodes used can impact what substances are produced during electrolysis.
Includes a discussion of Voltaic and electrolytic cells, the Nernst equation and the relationship between electrochemical processes, chemical equilibrium and free energy.
**More good stuff available at:
www.wsautter.com
and
http://www.youtube.com/results?search_query=wnsautter&aq=f
Covalent bonds form when atoms share electrons to complete their outer electron shells. Covalent compounds are typically made of nonmetal atoms. Binary covalent compounds contain only two elements. Their names follow specific rules based on element position in the periodic table. Molecular shape is determined by VSEPR theory, which predicts the geometry that minimizes electron pair repulsions. Polar covalent bonds result from unequal electron sharing between atoms of different electronegativity. Molecular polarity depends on both bond polarity and molecular geometry.
Electrolysis is the process of using electric current to cause non-spontaneous chemical changes. During electrolysis, ions are discharged at the electrodes. The key factors that determine which ions are discharged include the position of ions in the electrochemical series, concentration of ions, and type of electrode. Electrolysis has important industrial applications such as electroplating, metal purification, and metal extraction.
This document provides an overview of chemical bonding models including ionic bonding, covalent bonding, and metallic bonding. Ionic bonding involves the transfer of electrons between metals and nonmetals. Covalent bonding involves the sharing of electron pairs between two nonmetals. Metallic bonding occurs between metals and involves delocalized electrons within an electron sea. Lewis electron dot structures are used to represent electron arrangements around atoms and how they bond. Electronegativity differences between atoms determine bond polarity. Multiple bonding and resonance structures are also discussed.
Electrolysis is the decomposition of a substance by an electric current, where electrolytes carry current as ions in solution. During electrolysis, ions move to the electrodes and undergo oxidation or reduction reactions. At the cathode, electrons are gained and reduction occurs. At the anode, electrons are lost and oxidation occurs. The amount of substance deposited or gas produced can be calculated using Faraday's law, relating current, time, and moles of electrons in the electrode reactions.
This document provides information on electron configurations and quantum numbers:
- It defines the principal quantum number n, which describes the main energy level of an electron. It also defines the subsidiary quantum number l, which describes the shape of an orbital, and the magnetic quantum number m, which describes the orientation of an orbital in space.
- It discusses the four quantum numbers that describe each electron in an atom: n, l, m, and spin quantum number s.
- It provides examples of writing the four quantum numbers for the last electron in different atoms like Li, Cl, B, O, and Ar.
- It includes sample exam questions that test understanding of electron configurations, ion formations, bonding definitions
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.
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.
The document discusses progress on a study to understand how to increase ethical consumption among young adults in southern Finland. Focus groups were conducted which led the researchers to modify their original research question. The new question focuses on urban Finland and how to increase ethical consumption. Individual interviews are now scheduled to be completed by week 42 to understand drivers of ethical consumption and how ethical businesses can differentiate themselves. Challenges included an irrelevant original research question and scheduling delays.
Agile teams - right communication and trust building techniquesAmoli Upadhye
This document summarizes an agile workshop focused on improving communication and trust between teams. It discusses why trust and communication are important for productivity, alignment, and working together effectively. The workshop also addresses typical conflict scenarios in agile projects, strategies for being assertive, and role plays demonstrating aggressive, passive, and assertive responses to conflicts. Participants learned an assertiveness strategy called DRiVeN that involves disagreeing assertively, responding to resistance, emphasizing value, and negotiating tradeoffs.
Dokumen tersebut membahas tentang mikrokontroler ATmega8535 dan sistem minimum yang dibutuhkannya. Sistem minimum mikrokontroler terdiri dari rangkaian tersederhana untuk memungkinkan operasi dan deprogram mikrokontroler. Dokumen ini juga menjelaskan tentang port input/output pada ATmega8535, instruksi-instruksi dasar I/O, operasi aritmatika dan logika, serta tugas pembuatan sistem minimum ATmega8535.
Chemical bonding results from the attraction between nuclei and electrons. There are three main types of bonding: ionic, covalent, and metallic. Ionic bonding involves the transfer of electrons between atoms to form ions. Covalent bonding involves the sharing of electrons between non-metal atoms to form molecules. Metallic bonding occurs between metal atoms due to delocalized valence electrons. The type and strength of bonding influences various macroscopic properties like melting and boiling points. Intermolecular forces between molecules, such as hydrogen bonding and van der Waals forces, also impact physical properties.
Chemical bonding results from the attraction between nuclei and electrons. There are three main types of bonding: ionic, covalent, and metallic. Ionic bonding involves the transfer of electrons between atoms to form ions. Covalent bonding involves the sharing of electron pairs between atoms. Metallic bonding occurs between metal atoms through delocalized valence electrons. The type of bonding determines the physical properties of the substance.
Chemical bonding results from the attraction between nuclei and electrons. There are three main types of bonding: ionic, covalent, and metallic. Ionic bonding involves the transfer of electrons between atoms to form ions. Covalent bonding involves the sharing of electron pairs between atoms to form molecules. Metallic bonding occurs between metal atoms through delocalized valence electrons. The type of bonding determines the physical properties of the substance such as melting/boiling points and conductivity.
Chemical bonding occurs through ionic, covalent, and metallic bonding. Ionic bonding involves the transfer of electrons between atoms to form ions. Covalent bonding involves the sharing of electron pairs between atoms to form molecules. Metallic bonding occurs through delocalized valence electrons that are shared between metal atoms. The type of bonding determines the physical properties of the resulting compounds or materials.
Chemical bonding occurs through ionic, covalent, and metallic bonding. Ionic bonding involves the transfer of electrons between atoms to form ions, while covalent bonding involves the sharing of electron pairs between atoms. Metallic bonding involves the mobile valence electrons that are shared between positively charged metal ions. The type of bonding determines the physical properties of the substance, with ionic compounds being hard solids and poor conductors, and metals being malleable and good conductors. Molecular shape is influenced by electron pair repulsion according to VSEPR theory. Intermolecular forces like hydrogen bonding and van der Waals forces are also important in determining a substance's melting and boiling points.
1. The document discusses different types of chemical formulas including molecular, empirical, and structural formulas. It provides examples of each type like H2O for water and C6H12 for hexene.
2. It also discusses ionic and covalent bonding. Ionic bonding involves the complete transfer of electrons from one atom to another, like from sodium to chlorine in NaCl. Covalent bonding involves the sharing of electron pairs between atoms.
3. The document describes electronegativity and how it relates to the polarity of covalent bonds. Polar covalent bonds form between atoms with an electronegativity difference of 0.5-1.6, while ionic bonds form between atoms with a difference above
This document provides a summary of key concepts in chemical bonding:
1. It defines different types of bonds including ionic bonds formed between ions, covalent bonds formed by shared electrons between nonmetals, and metallic bonds formed by pooled electrons between metal atoms.
2. It describes characteristics used to identify bond types such as solubility in water and conductivity. Electronegativity is also defined as an atom's pull on shared electrons.
3. Bond polarity is discussed in relation to differences in electronegativity, with polar bonds having an unequal sharing of electrons between atoms.
1. Covalent bonds form when two atoms share one or more pairs of valence electrons in order to achieve a stable octet of electrons.
2. Molecules are formed when atoms are bonded together by covalent bonds, and molecular compounds are composed of molecules.
3. Molecular compounds tend to have lower melting and boiling points than ionic compounds and many are gases or liquids at room temperature.
This document provides information about molecular and ionic compounds, including:
- Molecular compounds are formed by covalent bonds between nonmetal atoms, while ionic compounds involve metal and nonmetal atoms bonded by ionic bonds.
- Molecular formulas show the actual number and type of atoms in a molecule, while ionic formulas use the lowest whole number ratio.
- Covalent bonds are represented by electron dot structures that show how atoms share electrons to achieve stable configurations. Multiple and coordinate covalent bonds are also discussed.
- Polarity arises in polar covalent bonds due to unequal electron sharing. Polar molecules have dipole moments while intermolecular forces include hydrogen bonding, dipole-dipole interactions, and
This document discusses chemical bonding and Lewis dot structures. It explains that atoms combine to achieve stable electron configurations, often those of noble gases. Ionic bonds form when electrons are transferred between atoms, creating ions. Covalent bonds form through electron sharing between nonmetals. Lewis dot structures represent valence electrons and can show electron transfers in ion formation. Different bond types - ionic, covalent, and metallic - depend on differences in electronegativity between atoms. Practice problems are provided to determine bond type based on electronegativity values.
1). Chemical bonds form when atoms gain, lose, or share electrons to achieve stable noble gas configurations. Ionic bonds occur through electron transfer between metals and nonmetals, while covalent bonds form through electron sharing.
2). Lewis dot structures use dots to represent valence electrons and illustrate octet formations. Exceptions include expanded and incomplete octets. Molecular geometry is determined by minimizing electron pair repulsion using the VSEPR model.
3). Bond properties like length, energy, order, and angle are influenced by bonding type. Ionic compounds maximize lattice energy through opposite ion arrangements.
1). Chemical bonds form when atoms gain, lose, or share electrons to achieve stable electron configurations like the noble gas configuration. Lewis dot structures use dots to represent valence electrons and show electron sharing between atoms.
2). Ionic bonds form when a metal transfers an electron to a nonmetal, creating oppositely charged ions that are attracted to each other. Covalent bonds form when atoms share one or more pairs of electrons to achieve stable octets.
3). The VSEPR theory predicts molecular geometry based on electron pair-pair repulsion, treating bond pairs and lone pairs as electron domains around a central atom that arrange to maximize distance between each other. Common molecular geometries include linear, trigonal planar,
The document discusses chemical bonding, including:
1. Defining ionic and covalent bonding, and explaining how different types of bonds are formed through electron sharing or transfer.
2. Describing the properties of ionic and covalent compounds, such as high melting points for ionic solids and variable states of matter for covalent substances.
3. Illustrating examples of single, double, and triple covalent bonds through Lewis dot structures of molecules like H2, O2, and N2.
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.
New chm-151-unit-6-20power-points-140227172225-phpapp02Cleophas Rwemera
This document provides an overview of chemical bonding models including ionic bonding, covalent bonding, and metallic bonding. Ionic bonding involves the transfer of electrons between metals and nonmetals. Covalent bonding involves the sharing of electron pairs between two nonmetals. Metallic bonding occurs through delocalized electrons that are shared among metal atoms. The document discusses electronegativity and bond polarity, provides examples of writing Lewis electron dot structures, and introduces resonance structures. Key concepts are illustrated with figures and sample problems are provided for writing Lewis structures.
Chemical bonds form between atoms to achieve more stable arrangements with lower potential energy. The main types of bonds are ionic, covalent, and metallic. Ionic bonds form between oppositely charged ions, covalent bonds form when atoms share electrons, and metallic bonds result from delocalized electrons being shared among many atoms in a metal. The degree of ionic or covalent character in a bond depends on the electronegativity difference between the atoms. Molecular compounds are made of molecules held together by covalent bonds, while ionic compounds are made of ionic bonds between cations and anions.
Chemical bonds form between atoms to achieve more stable arrangements with lower potential energy. The type of bonding depends on differences in electronegativity between atoms. Ionic bonds form between ions, covalent bonds involve shared electron pairs, and metallic bonds result from delocalized electrons shared among many atoms in a lattice. Molecular geometry and intermolecular forces also influence molecular properties.
Chemical bonding occurs through either ionic bonds or covalent bonds. Ionic bonds result from the electrostatic attraction between oppositely charged ions, while covalent bonds form through the sharing of electrons between atoms. The octet rule states that atoms seek to attain a full outer shell of eight electrons to achieve stability. Covalent bonds form when atoms share electrons to attain stable electron configurations of eight electrons. Metallic bonding is characterized by positive metal ions embedded in a "sea" of delocalized valence electrons, giving rise to metallic properties such as conductivity, malleability, and luster.
4. BOND FORMATION
exothermic process
E
N Reactants
E
R Energy
G released
Y
Products
5. BREAKING BONDS
Endothermic reaction
energy must be put into the bond in order to break it
E
N Products
E
R Energy
G Absorbed
Y Reactants
6. BOND STRENGTH
Strong, STABLE bonds require lots of energy to be
formed or broken
weak bonds require little E
7. TWO MAJOR TYPES OF BONDING
Ionic Bonding
forms ionic compounds
transfer of e-
Covalent Bonding
forms molecules
sharing e-
8. ONE MINOR TYPE OF BONDING
Metallic bonding
Occurs between like atoms of a metal
in the free state
Valence e- are mobile (move freely
among all metal atoms)
Positive ions in a sea of electrons
Metallic characteristics
High mp temps, ductile, malleable, shiny
Hard substances
Good conductors of heat and electricity as
(s) and (l)
10. IONIC BONDING
electrons are transferred between valence shells of
atoms
ionic compounds are
made of ions
NOT MOLECULES
• ionic compounds are called Salts or
Crystals
11. IONIC BONDING
Always formed between metals and non-metals
+ -
[METALS ] [NON-METALS ]
Lost e- Gained e-
12. IONIC BONDING
Electronegativity difference > 2.0
Look up e-neg of the atoms in the bond and subtract
NaCl
CaCl2
Compounds with polyatomic ions
NaNO3
13.
14. PROPERTIES OF IONIC COMPOUNDS
SALTS
hard solid @ 22 C
o
Crystals
high mp temperatures
nonconductors of electricity in solid phase
good conductors in liquid phase or dissolved in
water (aq)
15. COVALENT BONDING
Pairs of e- are shared
molecules
between non-metal
atoms
electronegativity difference <
2.0
forms polyatomic ions
16. MOLECULAR
SUBSTANCES
Covalent
bonding
Low m.p. temp and b.p.
temps
relatively soft solids as
compared to ionic compounds
nonconductors of electricity
in any phase
17. COVALENT, IONIC, METALLIC
BONDING?
NO
2
NH + • CO
sodium 4
Aluminu
hydride • Co
Hg m
phosphate
H S
2 KH
sulfate Also study
KCl your
HF characteristics!
18. DRAWING IONIC COMPOUNDS
USING LEWIS DOT STRUCTURES
• Symbol represents the KERNEL of the
atom (nucleus and inner e-)
• dots represent valence e-
19. NACL
This is the finished Lewis Dot Structure
-
[Na] [ Cl ]
How did we get here?
+
20. Step 1 after checking that it is IONIC
Determine which atom will be the +ion
Determine which atom will be the - ion
Step 2
Write the symbol for the + ion first.
NO DOTS
Draw the e- dot diagram for the – ion
COMPLETE outer shell
Step 3
Enclose both in brackets and show each
charge
22. DRAWING MOLECULES USING
LEWIS DOT STRUCTURES
Symbol represents the KERNEL of the atom
(nucleus and inner e-)
dots represent valence e-
23. Always remember atoms
are trying to complete
their outer shell!
The number of electrons the atoms needs is the
total number of bonds they can make.
Ex. … H? O? F? N? Cl? C?
one two one three one four
24. METHANE CH4
This is the finished Lewis dot structure
How did we get here?
25. Step 1
count total valence e- involved
Step 2
connect the central atom (usually the
first in the formula) to the others
with single bonds
Step 3
complete valence shells of outer
atoms
Step 4
add any extra e- to central atom
IF the central atom has 8 valence e-
26. SOMETIMES . . .
You only have two atoms, so there is no central
atom, but follow the same rules.
Check & Share to make sure all the atoms are
“happy”.
Cl2 Br2 H2 O2 N2 HCl
27. DOUBLE bond
atoms that share two e- pairs (4 e-)
O O
TRIPLE bond
atoms that share three e- pairs (6 e-)
N N
28. DRAW LEWIS DOT STRUCTURES
You may represent valence electrons from different
atoms with the following symbols x, ,
CO2
NH3
29. DIAGRAM FOR
POLYATOMIC IONS
Count all valence e- needed for covalent bonding
Add or subtract other electrons based on the
charge
REMEMBER!
A positive charge means it
LOST electrons!!!!!
31. TYPES OF COVALENT
BONDS
NON-Polar bonds
Electrons shared evenly in the
bond
E-neg difference is zero
Between identical atoms
Diatomic molecules
32. TYPES OF COVALENT
BONDS
Polar bond
Electrons unevenly shared
E-neg difference greater than
zero but
less than 2.0
closer to 2.0 more polar
more “ionic character”
33. POLARITY
WHICH IS LEAST AND WHICH IS
MOST?
HCl
CH
4
CO a.k.a.
2
“ionic character”
NH
3
N
2
HF
34. NON-POLAR MOLECULES
Sometimes the bonds within
a molecule are polar and yet
the molecule is non-polar
because its shape is
symmetrical. H
H C H
Draw Lewis dot first and
see if equal on all sides
H
47. TETRAHEDRAL
Ball and stick Space filling
model model
48. INTERMOLECULAR ATTRACTIONS
Attractions between
molecules
van der Waals
forces
Weak attractive
forces between
non-polar
molecules
Hydrogen
“bonding”
Strong
attraction
between special
49. VAN DER WAALS
Non-polar molecules can exist in liquid and solid
phases
because van der Waals forces keep the molecules
attracted to each other
Exist between CO2, CH4, CCl4, CF4, diatomics and
monoatomics
50. VAN DER WAALS PERIODICITY
increase with molecular mass.
Greater van der Waals force?
F2 Cl2 Br2 I2
increase
with closer distance between
molecules
Decreases when particles are farther away
51. HYDROGEN “BONDING”
Strong polar
attraction
Like magnets
Occurs ONLY
between H of one
molecule and N,
O, F of another
H “bond”
52. WHY DOES H “BONDING” OCCUR?
Nitrogen, Oxygen and Fluorine
small atoms with strong nuclear charges
powerful atoms
very high electronegativities
53. INTERMOLECULAR FORCES
DICTATE CHEMICAL PROPERTIES
Strong intermolecular forces cause high b.p., m.p.
and slow evaporation (low vapor pressure) of a
substance.
54. WHICH SUBSTANCE HAS THE
HIGHEST BOILING POINT?
HF
NH Fluorine has the highest e-neg,
3
H 2O SO
HF will experience the
WHY? strongest H bonding and ∴
needs the most energy to
weaken the i.m.f. and boil
55. THE UNUSUAL PROPERTIES OF
WATER
Unusually
high
boiling
point
Compared
to other
compounds
in Group 16
57. H2O(S) IS LESS DENSE THAN H2O(L)
The hydrogen bonding in water(l)
molecules is random. The molecules
are closely packed.
Thehydrogen bonding in water(s)
molecules has a specific open lattice
pattern. The molecules are farther
apart.