These slides consist of information about the formation molecules by sharing of electrons between two or more non metals also known as covalent bonding. The slides describes the properties of covalent compounds.
This chapter discusses chemical bonds and mixtures. It introduces electron-dot structures to show valence electrons and how they are involved in bonding. Ionic bonds form when ions with opposite charges are attracted to each other. Covalent bonds form when atoms share electrons. Polar covalent bonds result when electrons are shared unevenly. Molecular polarity arises if the polar bonds in a molecule do not cancel out. Most materials are mixtures that can be separated into pure substances. Solutions are homogeneous mixtures where a solute dissolves evenly throughout a solvent. Concentration, molarity, and solubility are measures used to describe solutions.
This chapter discusses chemical bonds and mixtures. It introduces electron-dot structures to show valence electrons and how they are involved in bonding. Ionic bonds form when ions with opposite charges are attracted to each other. Covalent bonds form when atoms share electrons. Polar covalent bonds result when electrons are shared unevenly. Molecular polarity arises if the polar bonds in a molecule do not cancel out. Most materials are mixtures that can be separated into pure substances. Solutions are homogeneous mixtures where one substance dissolves evenly throughout another. Concentration, molarity, and solubility are measures used to describe solutions.
This chapter discusses chemical bonds and mixtures. It introduces electron-dot structures to show valence electrons and how they are involved in bonding. Ionic bonds form when ions with opposite charges are attracted to each other. Covalent bonds form when atoms share electrons. Polar covalent bonds result when electrons are shared unevenly. Molecular polarity arises if the polar bonds in a molecule do not cancel out. Most materials are mixtures that can be separated into pure substances. Solutions are homogeneous mixtures where one substance dissolves evenly throughout another. Concentration, molarity, and solubility are discussed in relation to solutions.
CHAPTER 11 L2 covalent bonds.ppt chemical bondsAmelHanafi3
Atoms form covalent bonds by sharing valence electrons. This allows atoms to gain stability and form molecules. Covalent bonds can be single, double, or triple depending on how many electron pairs are shared. Molecules like H2O are polar if one atom attracts the shared electrons more strongly, affecting their properties. Covalent compounds have low melting and boiling points and are usually gases, liquids, or solids. A chemical formula shows the types of atoms in a molecule but not its shape, which can be modeled differently.
1. The document discusses molecular shapes and intermolecular forces. It explains that molecular shape is determined by valence shell electron pair repulsion (VSEPR) theory, where electron pairs around an atom repel each other and take up positions as far apart as possible.
2. The most common molecular shapes are linear, trigonal planar, tetrahedral, trigonal pyramidal, and bent. Molecular polarity depends on bond polarity and symmetry. Polar molecules have an uneven distribution of charge while nonpolar molecules have symmetrical charge distributions.
3. Intermolecular forces include hydrogen bonding, dipole-dipole interactions, and dispersion forces. Hydrogen bonding is the strongest and occurs between molecules with hydrogen bonded to fluorine,
This document provides an introduction to biochemistry by discussing basic chemical principles like atomic structure, subatomic particles, isotopes, ionic bonds, covalent bonds, and molecular properties of water. It explains that biochemistry relies on an understanding of the chemistry of living systems, which are composed of chemical elements consisting of protons, neutrons, and electrons. The chemical properties of elements, including their ability to form ionic and covalent bonds, are determined by their electron configuration and electronegativity.
This document discusses the chemical level of organization in living things. It describes the structure of atoms and the six main elements found in biological molecules. Atoms contain protons, neutrons and electrons. Elements are substances made of one type of atom. There are three main types of chemical bonds: ionic bonds form when atoms gain or lose electrons to become ions; covalent bonds form when atoms share electrons; and hydrogen bonds form weak attractions between molecules. These bonds allow atoms to combine into molecules and compounds that make up living things.
This chapter discusses chemical bonds and mixtures. It introduces electron-dot structures to show valence electrons and how they are involved in bonding. Ionic bonds form when ions with opposite charges are attracted to each other. Covalent bonds form when atoms share electrons. Polar covalent bonds result when electrons are shared unevenly. Molecular polarity arises if the polar bonds in a molecule do not cancel out. Most materials are mixtures that can be separated into pure substances. Solutions are homogeneous mixtures where a solute dissolves evenly throughout a solvent. Concentration, molarity, and solubility are measures used to describe solutions.
This chapter discusses chemical bonds and mixtures. It introduces electron-dot structures to show valence electrons and how they are involved in bonding. Ionic bonds form when ions with opposite charges are attracted to each other. Covalent bonds form when atoms share electrons. Polar covalent bonds result when electrons are shared unevenly. Molecular polarity arises if the polar bonds in a molecule do not cancel out. Most materials are mixtures that can be separated into pure substances. Solutions are homogeneous mixtures where one substance dissolves evenly throughout another. Concentration, molarity, and solubility are measures used to describe solutions.
This chapter discusses chemical bonds and mixtures. It introduces electron-dot structures to show valence electrons and how they are involved in bonding. Ionic bonds form when ions with opposite charges are attracted to each other. Covalent bonds form when atoms share electrons. Polar covalent bonds result when electrons are shared unevenly. Molecular polarity arises if the polar bonds in a molecule do not cancel out. Most materials are mixtures that can be separated into pure substances. Solutions are homogeneous mixtures where one substance dissolves evenly throughout another. Concentration, molarity, and solubility are discussed in relation to solutions.
CHAPTER 11 L2 covalent bonds.ppt chemical bondsAmelHanafi3
Atoms form covalent bonds by sharing valence electrons. This allows atoms to gain stability and form molecules. Covalent bonds can be single, double, or triple depending on how many electron pairs are shared. Molecules like H2O are polar if one atom attracts the shared electrons more strongly, affecting their properties. Covalent compounds have low melting and boiling points and are usually gases, liquids, or solids. A chemical formula shows the types of atoms in a molecule but not its shape, which can be modeled differently.
1. The document discusses molecular shapes and intermolecular forces. It explains that molecular shape is determined by valence shell electron pair repulsion (VSEPR) theory, where electron pairs around an atom repel each other and take up positions as far apart as possible.
2. The most common molecular shapes are linear, trigonal planar, tetrahedral, trigonal pyramidal, and bent. Molecular polarity depends on bond polarity and symmetry. Polar molecules have an uneven distribution of charge while nonpolar molecules have symmetrical charge distributions.
3. Intermolecular forces include hydrogen bonding, dipole-dipole interactions, and dispersion forces. Hydrogen bonding is the strongest and occurs between molecules with hydrogen bonded to fluorine,
This document provides an introduction to biochemistry by discussing basic chemical principles like atomic structure, subatomic particles, isotopes, ionic bonds, covalent bonds, and molecular properties of water. It explains that biochemistry relies on an understanding of the chemistry of living systems, which are composed of chemical elements consisting of protons, neutrons, and electrons. The chemical properties of elements, including their ability to form ionic and covalent bonds, are determined by their electron configuration and electronegativity.
This document discusses the chemical level of organization in living things. It describes the structure of atoms and the six main elements found in biological molecules. Atoms contain protons, neutrons and electrons. Elements are substances made of one type of atom. There are three main types of chemical bonds: ionic bonds form when atoms gain or lose electrons to become ions; covalent bonds form when atoms share electrons; and hydrogen bonds form weak attractions between molecules. These bonds allow atoms to combine into molecules and compounds that make up living things.
The document discusses different types of chemical bonds including intramolecular and intermolecular forces. It defines ionic bonds as occurring between metal and non-metal atoms through the transfer of electrons, and covalent bonds as occurring between non-metal atoms through the sharing of electrons. The document also discusses metallic bonding, the octet rule, and provides examples of different ionic compounds.
Materials science and engineering involves the study of atomic structure and bonding in materials. There are three primary types of atomic bonding - ionic, covalent, and metallic. Crystalline solids can have face-centered cubic (FCC), body-centered cubic (BCC), or hexagonal close-packed (HCP) crystal structures which influence material properties. Crystalline materials can assemble into either crystalline or amorphous structures, and material properties depend on crystal orientation in single crystals but are isotropic in polycrystalline materials with randomly oriented grains.
An atom is the smallest unit of matter that retains the properties of an element. It consists of a nucleus containing protons and neutrons, surrounded by electrons. A molecule is made up of two or more atoms bonded together. Molecules exhibit the properties of their constituent elements and can be broken down into atoms. Atoms are the fundamental building blocks that make up all matter in the universe and were formed after the Big Bang. While once thought to be indivisible, atoms can undergo chemical reactions that separate, combine, or rearrange them.
Ionic compounds are formed between a metal and nonmetal where electrons are transferred, creating oppositely charged ions held together by ionic bonds. Covalent molecular compounds are formed between two or more nonmetals where atoms share electrons through covalent bonds to form electrically neutral molecules like table sugar. Both compound types exhibit distinct physical properties depending on their bonding such as ionic compounds having high melting points and being brittle while covalent compounds have low melting points and are soft and flexible.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
Human physiology involves the study of molecules, cells, tissues, organs and organ systems that make up the human body. At the most basic level, atoms combine through chemical bonds like ionic and covalent bonds to form molecules, which then organize into cells. Cells further organize into tissues and organs to carry out specific functions and form organ systems that allow the human body to function as a whole.
This document discusses how researchers used chemical bonding theories and models to develop drugs that treat HIV/AIDS. It explains that:
1) In the 1980s, researchers discovered the structure of the HIV protease protein and used bonding models to simulate how potential drugs might interact with it.
2) This allowed drug companies to design protease inhibitor molecules that disable the protease protein, preventing HIV from spreading.
3) Clinical trials showed these protease inhibitors, taken in combination with other drugs, reduced viral levels in HIV patients to undetectable amounts. While not a cure, the drugs allow those treated to have near-normal lifespans.
1) Researchers used bonding theories to simulate how potential AIDS drug molecules would interact with the HIV protease molecule. This led to the development of protease inhibitor drugs.
2) Protease inhibitors disable the HIV protease enzyme, preventing the virus from spreading. When taken in combination with other drugs, protease inhibitors have reduced viral levels in patients to undetectable levels.
3) While not a cure for AIDS, protease inhibitor drugs allow those infected with HIV to live nearly normal lifespans when the drugs are taken regularly.
This document discusses different types of chemical bonds, including ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between metals and nonmetals, forming oppositely charged ions that are attracted in a crystal lattice. Covalent bonds involve the sharing of electrons between nonmetal atoms. Lewis structures can represent electron and bond arrangements in molecules and ions using dots and lines. The octet rule describes atoms' tendency to bond so they have eight electrons in their valence shell, like noble gases. Exceptions include hydrogen following the duet rule and structures with underfilled or overfilled octets.
The document discusses the basic chemistry concepts that are essential for life, including the structure of atoms and molecules, chemical bonds, and chemical reactions. It also examines the organic compounds that are important for living things like carbohydrates, lipids, proteins, and nucleic acids. Furthermore, the document explains how enzymes are important biological catalysts that allow chemical reactions to occur efficiently in living cells.
This document provides an overview of elements, compounds, and how they relate. It defines elements as pure substances made of single atom types, while compounds are formed when two or more different elements bond together. Elements are represented by symbols on the periodic table and have distinct properties based on their atomic structure. Compounds have new properties and are represented by formulas showing the elements present and their ratios. The document explains how ionic and covalent bonds form compounds from elements and provides examples of common elements, compounds, and how to determine compound formulas from their constituent ions.
Chemistry
Chemistry is the branch of science that deals with the composition, structure and properties of matter.
Chemistry is also called the science of atoms and molecules.
Chemistry is the study of matter and the changes it undergoes.
Nursing
Nursing is a profession within the healthcare sector focused on the care of individuals, families and communities so they may attain, maintain or recover optimal health and quality of life.
Nurses may be differentiated from the other healthcare providers by their approach to patient care, training and scope of practice.
Chemistry in nursing is very important, as it sets the basis for understanding the medications that are being administered to certain patients
Nurses must understand how particular medicines will react in different patients. This helps to avoid wrong combinations of drugs that can lead to adverse effects.
Nursing programs feature different chemistry courses, including biochemistry, pharmacology, general level chemistry and organic chemistry. All of these courses play an important role in helping nurses understand different organic compounds, chemical equations, chemical reactions and chemical processes.
Therefore, chemistry knowledge allows nurses to understand the effects of different medicines when used alone or in combination with others.
The nurse must understand the present condition of the patient, importance and difference in sodium, potassium, chloride, bicarbonate, oxygen and many other elements and electrolytes in the body. This understanding will guide the nurse to identify if there is an electrolyte imbalance.
Thus, it is vital for nurses to have the skills to take care of their patients emotionally, but it is also important that the nurse have the necessary knowledge to interpret data regarding the patient condition to treat physically accurately and in a timely manner.
The term matter refers to anything that occupies space and has mass. All matter is made up of substances called elements, which have specific chemical and physical properties and cannot be broken down into other substances through ordinary chemical reactions.
There are two ways of classifying the matter:
(A) Physical Classification
Matter can exist in three physical states:
Solids
Liquids
Gases.
(B) Chemical classification
Based upon the composition, matter can be divided into two main types:
Pure Substances
Mixtures.
1. Solids
The solid state is one of the fundamental states of matter.
Solids differ from liquids and gases by the characteristic of rigidity.
The molecules of solids are tightly packed because of strong intermolecular forces; they only oscillate about their mean positions.
Whereas, liquids and gases possess the property of fluidity and can easily flow.
Solids can be defined as the state of matter which has definite shape and volume and has a rigid structure.
Solids possess the least compressibility and thermal expansion.Example: Iron (Fe)
2. Liquid
The molecules in a liquid are
Organic chemistry is the study of carbon-containing compounds, excluding simple substances like carbonates. Carbon forms diverse structures due to its ability to form four covalent bonds and its position in the periodic table. The simplest organic compounds are hydrocarbons consisting of carbon and hydrogen. Organic compounds can form covalent, metallic, or ionic bonds depending on the atoms involved. Covalent bonds are formed by the sharing of electron pairs between atoms. Polarity, melting/boiling points, and solubility are determined by bond polarity within molecules. Functional groups are common bonding patterns that determine a molecule's reactivity.
All matter is composed of basic building blocks called atoms and molecules. Atoms are the smallest units that make up elements, and molecules are formed when atoms combine. Atoms contain protons, neutrons, and electrons. Protons and neutrons are located in the central nucleus, while electrons orbit around the nucleus in defined energy shells. Elements are pure substances made of only one type of atom, while compounds are made of two or more different elements bonded together. Atoms can bond through ionic bonds by transferring electrons or covalent bonds by sharing electrons to form molecules. The periodic table organizes the known elements based on their atomic structure.
This document discusses chemical bonds and how they form compounds. It explains that ionic bonds form between metals and nonmetals when electrons are transferred, creating oppositely charged ions. Covalent bonds form when atoms share electrons. There are different types of covalent bonds depending on how electrons are shared. The document provides examples of naming simple ionic compounds and covalent molecules, and discusses more complex compounds involving polyatomic ions or water of hydration.
Properties of Ionic compounds and Covalent BondsLelGuatz1
Ionic compounds:
1. Form crystals and conduct electricity when dissolved in water or molten but do not conduct in solid state.
2. Are hard, brittle, and have high melting and boiling points.
3. Are good electrical insulators.
Covalent bonds:
1. Result from the sharing of electron pairs between two atoms.
2. Occur when electron pairs are shared by atoms, as seen in single, double and triple bonds between similar or dissimilar atoms.
3. Differ from ionic bonds which form through the transfer of electrons between metals and nonmetals.
1) Covalent bonding occurs when two nonmetal atoms share electrons in their outer shells to achieve a stable full outer shell.
2) Atoms that cannot gain or lose electrons, like carbon, must share electrons through covalent bonds rather than forming ions. They share electrons tightly in molecular compounds.
3) Double and triple covalent bonds form when two or three pairs of electrons are shared between two atoms, as seen in carbon dioxide and nitrogen molecules.
The document discusses different types of chemical bonds including intramolecular and intermolecular forces. It defines ionic bonds as occurring between metal and non-metal atoms through the transfer of electrons, and covalent bonds as occurring between non-metal atoms through the sharing of electrons. The document also discusses metallic bonding, the octet rule, and provides examples of different ionic compounds.
Materials science and engineering involves the study of atomic structure and bonding in materials. There are three primary types of atomic bonding - ionic, covalent, and metallic. Crystalline solids can have face-centered cubic (FCC), body-centered cubic (BCC), or hexagonal close-packed (HCP) crystal structures which influence material properties. Crystalline materials can assemble into either crystalline or amorphous structures, and material properties depend on crystal orientation in single crystals but are isotropic in polycrystalline materials with randomly oriented grains.
An atom is the smallest unit of matter that retains the properties of an element. It consists of a nucleus containing protons and neutrons, surrounded by electrons. A molecule is made up of two or more atoms bonded together. Molecules exhibit the properties of their constituent elements and can be broken down into atoms. Atoms are the fundamental building blocks that make up all matter in the universe and were formed after the Big Bang. While once thought to be indivisible, atoms can undergo chemical reactions that separate, combine, or rearrange them.
Ionic compounds are formed between a metal and nonmetal where electrons are transferred, creating oppositely charged ions held together by ionic bonds. Covalent molecular compounds are formed between two or more nonmetals where atoms share electrons through covalent bonds to form electrically neutral molecules like table sugar. Both compound types exhibit distinct physical properties depending on their bonding such as ionic compounds having high melting points and being brittle while covalent compounds have low melting points and are soft and flexible.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
The attractive force which holds various constituents (atom, ions, etc.) together and stabilizes them by the overall loss of energy is known as chemical bonding. Therefore, it can be understood that chemical compounds are reliant on the strength of the chemical bonds between its constituents; The stronger the bonding between the constituents, the more stable the resulting compound would be.
Human physiology involves the study of molecules, cells, tissues, organs and organ systems that make up the human body. At the most basic level, atoms combine through chemical bonds like ionic and covalent bonds to form molecules, which then organize into cells. Cells further organize into tissues and organs to carry out specific functions and form organ systems that allow the human body to function as a whole.
This document discusses how researchers used chemical bonding theories and models to develop drugs that treat HIV/AIDS. It explains that:
1) In the 1980s, researchers discovered the structure of the HIV protease protein and used bonding models to simulate how potential drugs might interact with it.
2) This allowed drug companies to design protease inhibitor molecules that disable the protease protein, preventing HIV from spreading.
3) Clinical trials showed these protease inhibitors, taken in combination with other drugs, reduced viral levels in HIV patients to undetectable amounts. While not a cure, the drugs allow those treated to have near-normal lifespans.
1) Researchers used bonding theories to simulate how potential AIDS drug molecules would interact with the HIV protease molecule. This led to the development of protease inhibitor drugs.
2) Protease inhibitors disable the HIV protease enzyme, preventing the virus from spreading. When taken in combination with other drugs, protease inhibitors have reduced viral levels in patients to undetectable levels.
3) While not a cure for AIDS, protease inhibitor drugs allow those infected with HIV to live nearly normal lifespans when the drugs are taken regularly.
This document discusses different types of chemical bonds, including ionic bonds and covalent bonds. Ionic bonds involve the transfer of electrons between metals and nonmetals, forming oppositely charged ions that are attracted in a crystal lattice. Covalent bonds involve the sharing of electrons between nonmetal atoms. Lewis structures can represent electron and bond arrangements in molecules and ions using dots and lines. The octet rule describes atoms' tendency to bond so they have eight electrons in their valence shell, like noble gases. Exceptions include hydrogen following the duet rule and structures with underfilled or overfilled octets.
The document discusses the basic chemistry concepts that are essential for life, including the structure of atoms and molecules, chemical bonds, and chemical reactions. It also examines the organic compounds that are important for living things like carbohydrates, lipids, proteins, and nucleic acids. Furthermore, the document explains how enzymes are important biological catalysts that allow chemical reactions to occur efficiently in living cells.
This document provides an overview of elements, compounds, and how they relate. It defines elements as pure substances made of single atom types, while compounds are formed when two or more different elements bond together. Elements are represented by symbols on the periodic table and have distinct properties based on their atomic structure. Compounds have new properties and are represented by formulas showing the elements present and their ratios. The document explains how ionic and covalent bonds form compounds from elements and provides examples of common elements, compounds, and how to determine compound formulas from their constituent ions.
Chemistry
Chemistry is the branch of science that deals with the composition, structure and properties of matter.
Chemistry is also called the science of atoms and molecules.
Chemistry is the study of matter and the changes it undergoes.
Nursing
Nursing is a profession within the healthcare sector focused on the care of individuals, families and communities so they may attain, maintain or recover optimal health and quality of life.
Nurses may be differentiated from the other healthcare providers by their approach to patient care, training and scope of practice.
Chemistry in nursing is very important, as it sets the basis for understanding the medications that are being administered to certain patients
Nurses must understand how particular medicines will react in different patients. This helps to avoid wrong combinations of drugs that can lead to adverse effects.
Nursing programs feature different chemistry courses, including biochemistry, pharmacology, general level chemistry and organic chemistry. All of these courses play an important role in helping nurses understand different organic compounds, chemical equations, chemical reactions and chemical processes.
Therefore, chemistry knowledge allows nurses to understand the effects of different medicines when used alone or in combination with others.
The nurse must understand the present condition of the patient, importance and difference in sodium, potassium, chloride, bicarbonate, oxygen and many other elements and electrolytes in the body. This understanding will guide the nurse to identify if there is an electrolyte imbalance.
Thus, it is vital for nurses to have the skills to take care of their patients emotionally, but it is also important that the nurse have the necessary knowledge to interpret data regarding the patient condition to treat physically accurately and in a timely manner.
The term matter refers to anything that occupies space and has mass. All matter is made up of substances called elements, which have specific chemical and physical properties and cannot be broken down into other substances through ordinary chemical reactions.
There are two ways of classifying the matter:
(A) Physical Classification
Matter can exist in three physical states:
Solids
Liquids
Gases.
(B) Chemical classification
Based upon the composition, matter can be divided into two main types:
Pure Substances
Mixtures.
1. Solids
The solid state is one of the fundamental states of matter.
Solids differ from liquids and gases by the characteristic of rigidity.
The molecules of solids are tightly packed because of strong intermolecular forces; they only oscillate about their mean positions.
Whereas, liquids and gases possess the property of fluidity and can easily flow.
Solids can be defined as the state of matter which has definite shape and volume and has a rigid structure.
Solids possess the least compressibility and thermal expansion.Example: Iron (Fe)
2. Liquid
The molecules in a liquid are
Organic chemistry is the study of carbon-containing compounds, excluding simple substances like carbonates. Carbon forms diverse structures due to its ability to form four covalent bonds and its position in the periodic table. The simplest organic compounds are hydrocarbons consisting of carbon and hydrogen. Organic compounds can form covalent, metallic, or ionic bonds depending on the atoms involved. Covalent bonds are formed by the sharing of electron pairs between atoms. Polarity, melting/boiling points, and solubility are determined by bond polarity within molecules. Functional groups are common bonding patterns that determine a molecule's reactivity.
All matter is composed of basic building blocks called atoms and molecules. Atoms are the smallest units that make up elements, and molecules are formed when atoms combine. Atoms contain protons, neutrons, and electrons. Protons and neutrons are located in the central nucleus, while electrons orbit around the nucleus in defined energy shells. Elements are pure substances made of only one type of atom, while compounds are made of two or more different elements bonded together. Atoms can bond through ionic bonds by transferring electrons or covalent bonds by sharing electrons to form molecules. The periodic table organizes the known elements based on their atomic structure.
This document discusses chemical bonds and how they form compounds. It explains that ionic bonds form between metals and nonmetals when electrons are transferred, creating oppositely charged ions. Covalent bonds form when atoms share electrons. There are different types of covalent bonds depending on how electrons are shared. The document provides examples of naming simple ionic compounds and covalent molecules, and discusses more complex compounds involving polyatomic ions or water of hydration.
Properties of Ionic compounds and Covalent BondsLelGuatz1
Ionic compounds:
1. Form crystals and conduct electricity when dissolved in water or molten but do not conduct in solid state.
2. Are hard, brittle, and have high melting and boiling points.
3. Are good electrical insulators.
Covalent bonds:
1. Result from the sharing of electron pairs between two atoms.
2. Occur when electron pairs are shared by atoms, as seen in single, double and triple bonds between similar or dissimilar atoms.
3. Differ from ionic bonds which form through the transfer of electrons between metals and nonmetals.
1) Covalent bonding occurs when two nonmetal atoms share electrons in their outer shells to achieve a stable full outer shell.
2) Atoms that cannot gain or lose electrons, like carbon, must share electrons through covalent bonds rather than forming ions. They share electrons tightly in molecular compounds.
3) Double and triple covalent bonds form when two or three pairs of electrons are shared between two atoms, as seen in carbon dioxide and nitrogen molecules.
Communicating effectively and consistently with students can help them feel at ease during their learning experience and provide the instructor with a communication trail to track the course's progress. This workshop will take you through constructing an engaging course container to facilitate effective communication.
Philippine Edukasyong Pantahanan at Pangkabuhayan (EPP) CurriculumMJDuyan
(𝐓𝐋𝐄 𝟏𝟎𝟎) (𝐋𝐞𝐬𝐬𝐨𝐧 𝟏)-𝐏𝐫𝐞𝐥𝐢𝐦𝐬
𝐃𝐢𝐬𝐜𝐮𝐬𝐬 𝐭𝐡𝐞 𝐄𝐏𝐏 𝐂𝐮𝐫𝐫𝐢𝐜𝐮𝐥𝐮𝐦 𝐢𝐧 𝐭𝐡𝐞 𝐏𝐡𝐢𝐥𝐢𝐩𝐩𝐢𝐧𝐞𝐬:
- Understand the goals and objectives of the Edukasyong Pantahanan at Pangkabuhayan (EPP) curriculum, recognizing its importance in fostering practical life skills and values among students. Students will also be able to identify the key components and subjects covered, such as agriculture, home economics, industrial arts, and information and communication technology.
𝐄𝐱𝐩𝐥𝐚𝐢𝐧 𝐭𝐡𝐞 𝐍𝐚𝐭𝐮𝐫𝐞 𝐚𝐧𝐝 𝐒𝐜𝐨𝐩𝐞 𝐨𝐟 𝐚𝐧 𝐄𝐧𝐭𝐫𝐞𝐩𝐫𝐞𝐧𝐞𝐮𝐫:
-Define entrepreneurship, distinguishing it from general business activities by emphasizing its focus on innovation, risk-taking, and value creation. Students will describe the characteristics and traits of successful entrepreneurs, including their roles and responsibilities, and discuss the broader economic and social impacts of entrepreneurial activities on both local and global scales.
Leveraging Generative AI to Drive Nonprofit InnovationTechSoup
In this webinar, participants learned how to utilize Generative AI to streamline operations and elevate member engagement. Amazon Web Service experts provided a customer specific use cases and dived into low/no-code tools that are quick and easy to deploy through Amazon Web Service (AWS.)
हिंदी वर्णमाला पीपीटी, hindi alphabet PPT presentation, hindi varnamala PPT, Hindi Varnamala pdf, हिंदी स्वर, हिंदी व्यंजन, sikhiye hindi varnmala, dr. mulla adam ali, hindi language and literature, hindi alphabet with drawing, hindi alphabet pdf, hindi varnamala for childrens, hindi language, hindi varnamala practice for kids, https://www.drmullaadamali.com
Strategies for Effective Upskilling is a presentation by Chinwendu Peace in a Your Skill Boost Masterclass organisation by the Excellence Foundation for South Sudan on 08th and 09th June 2024 from 1 PM to 3 PM on each day.
This document provides an overview of wound healing, its functions, stages, mechanisms, factors affecting it, and complications.
A wound is a break in the integrity of the skin or tissues, which may be associated with disruption of the structure and function.
Healing is the body’s response to injury in an attempt to restore normal structure and functions.
Healing can occur in two ways: Regeneration and Repair
There are 4 phases of wound healing: hemostasis, inflammation, proliferation, and remodeling. This document also describes the mechanism of wound healing. Factors that affect healing include infection, uncontrolled diabetes, poor nutrition, age, anemia, the presence of foreign bodies, etc.
Complications of wound healing like infection, hyperpigmentation of scar, contractures, and keloid formation.
ISO/IEC 27001, ISO/IEC 42001, and GDPR: Best Practices for Implementation and...PECB
Denis is a dynamic and results-driven Chief Information Officer (CIO) with a distinguished career spanning information systems analysis and technical project management. With a proven track record of spearheading the design and delivery of cutting-edge Information Management solutions, he has consistently elevated business operations, streamlined reporting functions, and maximized process efficiency.
Certified as an ISO/IEC 27001: Information Security Management Systems (ISMS) Lead Implementer, Data Protection Officer, and Cyber Risks Analyst, Denis brings a heightened focus on data security, privacy, and cyber resilience to every endeavor.
His expertise extends across a diverse spectrum of reporting, database, and web development applications, underpinned by an exceptional grasp of data storage and virtualization technologies. His proficiency in application testing, database administration, and data cleansing ensures seamless execution of complex projects.
What sets Denis apart is his comprehensive understanding of Business and Systems Analysis technologies, honed through involvement in all phases of the Software Development Lifecycle (SDLC). From meticulous requirements gathering to precise analysis, innovative design, rigorous development, thorough testing, and successful implementation, he has consistently delivered exceptional results.
Throughout his career, he has taken on multifaceted roles, from leading technical project management teams to owning solutions that drive operational excellence. His conscientious and proactive approach is unwavering, whether he is working independently or collaboratively within a team. His ability to connect with colleagues on a personal level underscores his commitment to fostering a harmonious and productive workplace environment.
Date: May 29, 2024
Tags: Information Security, ISO/IEC 27001, ISO/IEC 42001, Artificial Intelligence, GDPR
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Training: ISO/IEC 27001 Information Security Management System - EN | PECB
ISO/IEC 42001 Artificial Intelligence Management System - EN | PECB
General Data Protection Regulation (GDPR) - Training Courses - EN | PECB
Webinars: https://pecb.com/webinars
Article: https://pecb.com/article
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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.
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3. Learning Objectives
• State that non-metallic elements form simple molecules
with covalent bonds between atoms.
• Describe the formation of covalent bonds in some common
compounds.
4. What is a covalent bond?
• Covalent bonds are shared pairs of electrons between non-
metal atoms.
• They are the bonds that form molecules. A molecule is two
or more atoms held together by covalent bonds.
• Some non-metal elements like hydrogen, oxygen, nitrogen
and chlorine are diatomic. They are naturally found as
molecules made from two of the same atom.
5. Covalent bonds form between non-metal atoms.
To understand covalent bonds, we
need to know the structure of the
atom.
Let's RECAP the structure of an atom
6. Electrons orbit the nucleus in
shells.
• The protons and neutrons are found in the
center of the atom in the nucleus. The electrons
are found in shells around the nucleus, and
atoms always have equal numbers of protons
and electrons.
• The shell nearest the nucleus holds only two
electrons.
• The second shell and the ones after that hold 8
electrons.
• Shells are filled starting from the first one. The
electrons in the outermost shell that are
involved in bonding are called valency electrons
7. Covalent bonds are strong.
• The nucleus of the atom contains
the protons, which makes it
positively charged.
• The electrons orbiting the
nucleus are negatively charged.
• There is a strong electrostatic
attraction between the positively
charged nuclei and the negatively
charged pair of electrons. This is
what holds the atoms together in
the covalent bond.
10. Ozone (O3) is a gas found in the Earth's atmosphere.
• Describe the bonds that hold the atoms
together and explain how you know that
the molecule has these bonds.
• When you describe a person, object,
event, or situation, you say what they are
like or what happened. When
you explain something, you give details
about it or describe it so that it can be
understood.
11. Covalent compounds
By the end of this lesson, you should be
able to:
• Describe the differences in properties
between ionic and covalent compounds.
• Explain the differences in melting point
and boiling point of ionic and covalent
compounds.
12. What is a
simple
covalent
compound?
• Non-metallic elements form simple molecules
with covalent bonds between atoms. There are many
different compounds whose atoms are held together
by covalent bonds.
• Some covalent compounds form simple
molecules, while others form giant structures. Those
compounds which form simple molecular structures
are called simple covalent compounds. We will be
focussing on these during this lesson.
• Water, carbon dioxide, ammonia, and hydrogen
chloride are all examples of simple covalent
compounds because they form small, individual
molecules.
13. Covalent bonds
are strong, intramolecular bonds.
• A covalent bond is formed when two atoms each share an electron to
make a shared pair.
• There is a strong electrostatic attraction between the positively-
charged nuclei and the negatively charged electron pair, and this force
holds the atoms together and makes covalent bonds strong.
• We call these bonds intramolecular because they are within the
molecule. So covalent compounds have strong intramolecular
bonds holding the atoms together.