Physical Science 1.3 : Chemical Properties
•
3 likes•1,264 views
This document discusses chemical properties and the differences between physical and chemical changes. It explains that chemical changes alter the composition and identity of a substance, often resulting in a new substance through signs like a change in color, odor, heat production or fizzing. In contrast, physical changes do not alter the composition of a substance and are more easily reversible than chemical changes.
Report
Share
Report
Share
Recommended
Chemical and Physical Change Practice
The document contains questions about physical and chemical changes. It defines physical changes as changes that alter the form or appearance of a substance without changing its chemical makeup, such as evaporation, melting, and freezing. Chemical changes result in new substances with different chemical properties, as occurs during burning or corrosion. A physical change also maintains the original substances, while a chemical change creates new ones.
Chemistry Unit 2 Part 2 - Changes in Matter
This document discusses physical and chemical changes in matter and provides examples to help students understand the key differences:
- Physical changes alter the physical properties of a substance without changing its chemical composition, such as changes of state between solid, liquid and gas, or cutting and crushing.
- Chemical changes involve chemical reactions that alter the molecular structure and create new substances, like rusting, burning, or digestion.
- The rock cycle and digestion process involve both physical changes (breaking rocks or movement through the digestive system) and chemical changes (chemical weathering or digestion of food).
Investigation 2 2 vocab
The document defines key chemistry terms and their relationships:
Elements are fundamental substances that cannot be broken down further. All matter is made up of combinations of elements, which can change and form new substances through chemical reactions. Matter is anything that has mass and takes up space, and a substance is a unique form of matter that is distinct from other forms.
Investigation 2 2 vocab
The document defines key chemistry terms and their relationships:
Elements are fundamental substances that cannot be broken down further. All matter is made up of combinations of elements, which can change and form new substances through chemical reactions. Matter is anything that has mass and takes up space, and a substance is a unique form of matter that is different from other forms.
What Are Chemical Changes In Matter 1
There are two types of properties that describe substances: physical properties and chemical properties. Physical properties involve the substance itself and include characteristics like color, size, and state of matter. Chemical properties involve how a substance interacts with other substances through chemical reactions. A chemical change results in one or more new substances forming through a chemical reaction. Compounds are substances made up of two or more elements that have chemically combined. There are clues that indicate a chemical change has occurred, such as gas bubbles, color changes, smells, or new properties forming in the substance. The law of conservation of mass states that the mass of products equals the mass of reactants in a chemical reaction.
03 Chemical Reactions
This document provides an overview of chemical reactions and changes. It defines a chemical reaction as a process that changes one set of chemicals into another. It discusses reagents (reactants) and products. It distinguishes between physical and chemical changes, providing examples of each. Signs of a chemical change are described as the formation of a precipitate, color change, bubbles, temperature change, or new odor. The law of conservation of mass is explained. Chemical equations are introduced and the importance of balancing equations is described through an example. Finally, practice problems are provided to test understanding of these concepts.
7. Chemical Changes
This document is an outline for a chemistry unit that discusses chemical changes in matter. It covers the differences between physical and chemical changes, how to identify a chemical reaction through changes in a substance's nature, representing chemical reactions with symbols and formulas, the law of conservation of mass in chemical reactions, John Dalton's atomic model, balancing chemical equations, mass balance in chemical reactions, energy and rates of reactions, industrial chemistry and its impact on the environment. The outline also includes activities and videos to supplement the topics.
Chapter 12 Lesssons
The document summarizes key concepts from Chapter 12 on changes in matter. It discusses physical and chemical changes, types of chemical reactions including decomposition, combination, and replacement. It also describes how chemical properties can be used to separate mixtures and identify substances. Finally, it gives examples of how chemistry is applied in health, materials, transportation, and technology to improve lives.
Recommended
Chemical and Physical Change Practice
The document contains questions about physical and chemical changes. It defines physical changes as changes that alter the form or appearance of a substance without changing its chemical makeup, such as evaporation, melting, and freezing. Chemical changes result in new substances with different chemical properties, as occurs during burning or corrosion. A physical change also maintains the original substances, while a chemical change creates new ones.
Chemistry Unit 2 Part 2 - Changes in Matter
This document discusses physical and chemical changes in matter and provides examples to help students understand the key differences:
- Physical changes alter the physical properties of a substance without changing its chemical composition, such as changes of state between solid, liquid and gas, or cutting and crushing.
- Chemical changes involve chemical reactions that alter the molecular structure and create new substances, like rusting, burning, or digestion.
- The rock cycle and digestion process involve both physical changes (breaking rocks or movement through the digestive system) and chemical changes (chemical weathering or digestion of food).
Investigation 2 2 vocab
The document defines key chemistry terms and their relationships:
Elements are fundamental substances that cannot be broken down further. All matter is made up of combinations of elements, which can change and form new substances through chemical reactions. Matter is anything that has mass and takes up space, and a substance is a unique form of matter that is distinct from other forms.
Investigation 2 2 vocab
The document defines key chemistry terms and their relationships:
Elements are fundamental substances that cannot be broken down further. All matter is made up of combinations of elements, which can change and form new substances through chemical reactions. Matter is anything that has mass and takes up space, and a substance is a unique form of matter that is different from other forms.
What Are Chemical Changes In Matter 1
There are two types of properties that describe substances: physical properties and chemical properties. Physical properties involve the substance itself and include characteristics like color, size, and state of matter. Chemical properties involve how a substance interacts with other substances through chemical reactions. A chemical change results in one or more new substances forming through a chemical reaction. Compounds are substances made up of two or more elements that have chemically combined. There are clues that indicate a chemical change has occurred, such as gas bubbles, color changes, smells, or new properties forming in the substance. The law of conservation of mass states that the mass of products equals the mass of reactants in a chemical reaction.
03 Chemical Reactions
This document provides an overview of chemical reactions and changes. It defines a chemical reaction as a process that changes one set of chemicals into another. It discusses reagents (reactants) and products. It distinguishes between physical and chemical changes, providing examples of each. Signs of a chemical change are described as the formation of a precipitate, color change, bubbles, temperature change, or new odor. The law of conservation of mass is explained. Chemical equations are introduced and the importance of balancing equations is described through an example. Finally, practice problems are provided to test understanding of these concepts.
7. Chemical Changes
This document is an outline for a chemistry unit that discusses chemical changes in matter. It covers the differences between physical and chemical changes, how to identify a chemical reaction through changes in a substance's nature, representing chemical reactions with symbols and formulas, the law of conservation of mass in chemical reactions, John Dalton's atomic model, balancing chemical equations, mass balance in chemical reactions, energy and rates of reactions, industrial chemistry and its impact on the environment. The outline also includes activities and videos to supplement the topics.
Chapter 12 Lesssons
The document summarizes key concepts from Chapter 12 on changes in matter. It discusses physical and chemical changes, types of chemical reactions including decomposition, combination, and replacement. It also describes how chemical properties can be used to separate mixtures and identify substances. Finally, it gives examples of how chemistry is applied in health, materials, transportation, and technology to improve lives.
Physical & Chemical Changes
This document contains notes from a science class discussing physical and chemical properties and changes. It includes definitions of physical properties, physical changes, chemical properties, and chemical changes. There are descriptions of 5 clues that indicate a chemical change may have occurred. The document outlines several mini labs and demonstrations for students to observe physical and chemical changes, including reactions involving magnesium and hydrochloric acid, milk and vinegar, baking soda and vinegar, and a mystery substance in a test tube.
Chemical equations
The document discusses chemical reactions and how to write chemical equations. It explains that chemical reactions involve rearranging bonds and atoms to form new compounds that are different than the starting materials. It provides examples of word and formula equations and shows the parts of a chemical equation including reactants, products, and physical states. It also instructs how to write chemical equations by converting word equations to symbolic equations using chemical formulas and reaction arrows.
Chem II Day VIII
This document provides an agenda for a chemistry class. It includes topics like reaction types, potential energy diagrams, stoichiometry, final project presentations, solubility rules, and types of chemical reactions like synthesis, decomposition, single replacement, and double replacement reactions. Students are asked to complete worksheets, turn in chapter reviews, and prepare questions for tutorials to earn extra credit.
simple chemical reactions - chemistry
This document provides an overview of simple chemical reactions, including:
1. It defines chemical reactions and gives examples of reactions that occur in everyday life like cooking and rusting.
2. It explains the difference between physical and chemical changes and identifies signs that a chemical reaction is occurring.
3. It describes reactants and products, explaining that reactants change into products in a chemical reaction.
Topic 1
Chemical and physical changes can be distinguished based on whether changes occur at the molecular level or involve energy and states of matter. Physical changes alter the shape or state of matter of a substance without changing its chemical composition, such as crushing a can or melting ice. Chemical changes involve transformations of molecular structure and composition through breaking and forming of chemical bonds, such as rusting of iron or burning of sugar. While some changes are obvious, others occur at the microscopic level of molecular structure and bonding.
CHEMICAL EQUATION
This document discusses chemical reactions and equations. It defines chemical equations as a method to represent chemical reactions using symbols and formulas. It explains the key components of a chemical equation including reactants, products, and balancing equations. It then describes several types of chemical reactions - combination, decomposition, displacement, double displacement, oxidation, and reduction reactions - and provides an example of each. Finally, it discusses two common effects of oxidation reactions: corrosion of metals and rancidity of food.
Changing matter
There are two types of matter changes: physical changes and chemical changes. Physical changes alter the physical properties of matter without changing its chemical composition, such as changes in state from solid to liquid to gas. Chemical changes form new chemical substances through rearrangement of atoms, such as burning or rusting. Chemical changes are identified through evidence like gas formation, color change, or energy transfer, and matter is conserved before and after the reaction according to the law of conservation of mass.
February 25
The document provides an agenda and lesson plan for a chemistry class on the topic of conservation of mass. The agenda includes a warm-up, setting up notes, a candle demonstration, a conservation of mass activity, and finishing with notes and answering focus questions. The demonstration shows how atoms are conserved in a chemical reaction by rearranging to form new substances, as seen in the burning of a candle. Students then do a hands-on modeling activity and learn that the atoms in the reactants are the source of the atoms in the products.
Chemical reactions
This document discusses simple chemical reactions including reactions with acids, metals, carbonates, and oxygen. It provides examples of physical and chemical changes and explains the differences between them. Word equations are given for common chemical reactions like metals reacting with acids and carbon reacting with oxygen. The key reactants and products are identified for these reactions.
Reactions20082
The document describes different types of chemical reactions: synthesis reactions occur when two substances combine to form a compound; decomposition reactions occur when a single substance breaks down into simpler parts upon heating; single replacement reactions involve one metal displacing another from a compound; double replacement reactions involve the exchange of ions between two compounds to form new compounds. The document also notes that a chemical equation represents the reactants on the left and products on the right, and that the law of conservation of mass means the mass of reactants equals the mass of products in a chemical reaction.
Physical and chemical changes:chemical equations
This document discusses physical and chemical changes, providing definitions and examples of each. A physical change alters a substance's physical properties but not its chemical composition, and can be reversed. A chemical change produces new substances with different properties than the original, through rearrangement of atoms, and cannot be reversed. The document also discusses the importance of balanced chemical equations in showing reactants, products, and mole ratios in chemical reactions. Four main types of chemical reactions are defined: combination, decomposition, displacement, and double decomposition.
Changes in Matter
Physical changes alter the state or form of a substance without changing its chemical identity, and are reversible. Chemical changes transform one or more substances into new substances with different properties, are indicated by color changes, formation of precipitates or gas bubbles, production of heat or light, and are not easily reversible. Physical and chemical changes can be distinguished by whether the identity of the substance is conserved and if the change is reversible.
Reactions2010
The document discusses chemical reactions and the four main types: synthesis, decomposition, single replacement, and double replacement. It defines key terms like reactants and products. Synthesis reactions combine two elements to form a compound. Decomposition reactions involve a single reactant breaking down into simpler products. Single replacement reactions involve one element replacing another in a compound. Double replacement reactions swap ions between two compounds. The law of conservation of mass is also mentioned.
Chemical Changes
A chemical change is a change where one or more new types of matter form as the original materials react and combine in new ways. Some signs that a chemical change has occurred include a change in color, gases being given off, or a change in temperature without external heating or cooling. Common examples of chemical changes provided are burning, rusting, wood ash being left after burning, and fruits or metals oxidizing and changing color when exposed to air.
Grade
This document provides key notes on chemical reactions and equations from a 10th grade chemistry textbook. It defines chemical reactions as processes that form new substances with different properties than the reactants. Chemical equations are used to represent chemical reactions symbolically and show the physical states of reactants and products. For equations to be balanced, the number of atoms of each element must be the same on both sides of the reaction. The document also describes several types of chemical reactions including combination reactions, decomposition reactions, displacement reactions, and double displacement reactions. Thermal, electrolytic, and photolytic decomposition reactions are given as examples.
Physical change or chemical change
A physical change can be reversed and only alters the shape or form of the material, while a chemical change produces new substances that cannot be reversed back to the original forms. Toasting bread and burning wood are examples of chemical changes, as the original substances cannot be recovered, while shaping clay into pots is a physical change since it remains clay just in a different shape. Determining if a change is physical or chemical is not always clear cut and may require microscopic examination in some cases.
Chem change
This document discusses chemical and physical changes in matter. It defines chemical properties as those that describe a substance's ability to change into a different substance through a chemical reaction. Physical properties can be observed without a chemical change. Chemical changes result in new substances, while physical changes only alter the form or appearance. Evidence of a chemical change includes a change in properties or energy, with energy either absorbed or released. Chemical equations are used to represent chemical reactions and their reactants and products. The mass of reactants and products is conserved in any chemical change.
Chemical reactions
This document discusses chemical reactions and properties of matter. It defines physical and chemical properties, and explains that a chemical change produces new substances while a physical change does not. It also outlines how to identify chemical reactions through observation of properties like color change, gas production, or precipitate formation. The document then explains how to write and balance chemical equations, and categorizes three main types of chemical reactions: synthesis, decomposition, and replacement. Finally, it discusses factors that affect the rate of chemical reactions like surface area, temperature, concentration, and catalysts.
Chemical reactions
This document summarizes key concepts about chemical reactions and properties. It defines chemical properties as the ability of a substance to change into a new substance, and physical properties as observable characteristics that do not change the substance. Chemical changes result in new substances, while physical changes alter appearance but not substance. For a chemical reaction to occur, bonds must be broken and reformed, allowing atoms to rearrange. Signs that a chemical reaction has taken place include formation of a precipitate, release of heat or light, and changes in color, temperature or gas formation. Chemical equations balance reactants and products to obey the law of conservation of matter, where mass and atoms are conserved despite rearrangement during bonding changes. Reaction rates depend on factors like activation energy
Physical and chemical change
The document discusses physical and chemical changes in matter. A physical change alters the form of matter but not its identity, and can be reversed. A chemical change produces new substances through chemical reactions, with the mass and number of atoms conserved but molecules changing. Chemical changes involve more energy and are not easily reversible. The document also outlines laws of conservation of mass and constant composition, and Gay-Lussac's law regarding gas reactions.
Physical Science 1.2 : Physical Properties
Physical properties can be observed or measured without changing the identity of matter and include density, which is the amount of matter in a given volume. Density can be used to identify substances and is calculated by dividing an object's mass by its volume. Examples of physical changes include melting, freezing, boiling, and condensing, which change a substance's state but do not form new substances.
Structure Of The Ecosystem
The document discusses key concepts in ecosystems including abiotic and biotic factors, trophic levels, food chains and webs, and energy pyramids. It explains that abiotic factors are non-living elements that affect organisms, while biotic factors are living components. It outlines the trophic levels of primary producers, primary consumers, secondary consumers, and decomposers. Food chains represent the transfer of energy between trophic levels, while food webs show a more complex network of interactions. Energy and biomass pyramids illustrate how the amount of energy and matter decreases at higher trophic levels due to inefficiencies in energy transfer between levels.
More Related Content
What's hot
Physical & Chemical Changes
This document contains notes from a science class discussing physical and chemical properties and changes. It includes definitions of physical properties, physical changes, chemical properties, and chemical changes. There are descriptions of 5 clues that indicate a chemical change may have occurred. The document outlines several mini labs and demonstrations for students to observe physical and chemical changes, including reactions involving magnesium and hydrochloric acid, milk and vinegar, baking soda and vinegar, and a mystery substance in a test tube.
Chemical equations
The document discusses chemical reactions and how to write chemical equations. It explains that chemical reactions involve rearranging bonds and atoms to form new compounds that are different than the starting materials. It provides examples of word and formula equations and shows the parts of a chemical equation including reactants, products, and physical states. It also instructs how to write chemical equations by converting word equations to symbolic equations using chemical formulas and reaction arrows.
Chem II Day VIII
This document provides an agenda for a chemistry class. It includes topics like reaction types, potential energy diagrams, stoichiometry, final project presentations, solubility rules, and types of chemical reactions like synthesis, decomposition, single replacement, and double replacement reactions. Students are asked to complete worksheets, turn in chapter reviews, and prepare questions for tutorials to earn extra credit.
simple chemical reactions - chemistry
This document provides an overview of simple chemical reactions, including:
1. It defines chemical reactions and gives examples of reactions that occur in everyday life like cooking and rusting.
2. It explains the difference between physical and chemical changes and identifies signs that a chemical reaction is occurring.
3. It describes reactants and products, explaining that reactants change into products in a chemical reaction.
Topic 1
Chemical and physical changes can be distinguished based on whether changes occur at the molecular level or involve energy and states of matter. Physical changes alter the shape or state of matter of a substance without changing its chemical composition, such as crushing a can or melting ice. Chemical changes involve transformations of molecular structure and composition through breaking and forming of chemical bonds, such as rusting of iron or burning of sugar. While some changes are obvious, others occur at the microscopic level of molecular structure and bonding.
CHEMICAL EQUATION
This document discusses chemical reactions and equations. It defines chemical equations as a method to represent chemical reactions using symbols and formulas. It explains the key components of a chemical equation including reactants, products, and balancing equations. It then describes several types of chemical reactions - combination, decomposition, displacement, double displacement, oxidation, and reduction reactions - and provides an example of each. Finally, it discusses two common effects of oxidation reactions: corrosion of metals and rancidity of food.
Changing matter
There are two types of matter changes: physical changes and chemical changes. Physical changes alter the physical properties of matter without changing its chemical composition, such as changes in state from solid to liquid to gas. Chemical changes form new chemical substances through rearrangement of atoms, such as burning or rusting. Chemical changes are identified through evidence like gas formation, color change, or energy transfer, and matter is conserved before and after the reaction according to the law of conservation of mass.
February 25
The document provides an agenda and lesson plan for a chemistry class on the topic of conservation of mass. The agenda includes a warm-up, setting up notes, a candle demonstration, a conservation of mass activity, and finishing with notes and answering focus questions. The demonstration shows how atoms are conserved in a chemical reaction by rearranging to form new substances, as seen in the burning of a candle. Students then do a hands-on modeling activity and learn that the atoms in the reactants are the source of the atoms in the products.
Chemical reactions
This document discusses simple chemical reactions including reactions with acids, metals, carbonates, and oxygen. It provides examples of physical and chemical changes and explains the differences between them. Word equations are given for common chemical reactions like metals reacting with acids and carbon reacting with oxygen. The key reactants and products are identified for these reactions.
Reactions20082
The document describes different types of chemical reactions: synthesis reactions occur when two substances combine to form a compound; decomposition reactions occur when a single substance breaks down into simpler parts upon heating; single replacement reactions involve one metal displacing another from a compound; double replacement reactions involve the exchange of ions between two compounds to form new compounds. The document also notes that a chemical equation represents the reactants on the left and products on the right, and that the law of conservation of mass means the mass of reactants equals the mass of products in a chemical reaction.
Physical and chemical changes:chemical equations
This document discusses physical and chemical changes, providing definitions and examples of each. A physical change alters a substance's physical properties but not its chemical composition, and can be reversed. A chemical change produces new substances with different properties than the original, through rearrangement of atoms, and cannot be reversed. The document also discusses the importance of balanced chemical equations in showing reactants, products, and mole ratios in chemical reactions. Four main types of chemical reactions are defined: combination, decomposition, displacement, and double decomposition.
Changes in Matter
Physical changes alter the state or form of a substance without changing its chemical identity, and are reversible. Chemical changes transform one or more substances into new substances with different properties, are indicated by color changes, formation of precipitates or gas bubbles, production of heat or light, and are not easily reversible. Physical and chemical changes can be distinguished by whether the identity of the substance is conserved and if the change is reversible.
Reactions2010
The document discusses chemical reactions and the four main types: synthesis, decomposition, single replacement, and double replacement. It defines key terms like reactants and products. Synthesis reactions combine two elements to form a compound. Decomposition reactions involve a single reactant breaking down into simpler products. Single replacement reactions involve one element replacing another in a compound. Double replacement reactions swap ions between two compounds. The law of conservation of mass is also mentioned.
Chemical Changes
A chemical change is a change where one or more new types of matter form as the original materials react and combine in new ways. Some signs that a chemical change has occurred include a change in color, gases being given off, or a change in temperature without external heating or cooling. Common examples of chemical changes provided are burning, rusting, wood ash being left after burning, and fruits or metals oxidizing and changing color when exposed to air.
Grade
This document provides key notes on chemical reactions and equations from a 10th grade chemistry textbook. It defines chemical reactions as processes that form new substances with different properties than the reactants. Chemical equations are used to represent chemical reactions symbolically and show the physical states of reactants and products. For equations to be balanced, the number of atoms of each element must be the same on both sides of the reaction. The document also describes several types of chemical reactions including combination reactions, decomposition reactions, displacement reactions, and double displacement reactions. Thermal, electrolytic, and photolytic decomposition reactions are given as examples.
Physical change or chemical change
A physical change can be reversed and only alters the shape or form of the material, while a chemical change produces new substances that cannot be reversed back to the original forms. Toasting bread and burning wood are examples of chemical changes, as the original substances cannot be recovered, while shaping clay into pots is a physical change since it remains clay just in a different shape. Determining if a change is physical or chemical is not always clear cut and may require microscopic examination in some cases.
Chem change
This document discusses chemical and physical changes in matter. It defines chemical properties as those that describe a substance's ability to change into a different substance through a chemical reaction. Physical properties can be observed without a chemical change. Chemical changes result in new substances, while physical changes only alter the form or appearance. Evidence of a chemical change includes a change in properties or energy, with energy either absorbed or released. Chemical equations are used to represent chemical reactions and their reactants and products. The mass of reactants and products is conserved in any chemical change.
Chemical reactions
This document discusses chemical reactions and properties of matter. It defines physical and chemical properties, and explains that a chemical change produces new substances while a physical change does not. It also outlines how to identify chemical reactions through observation of properties like color change, gas production, or precipitate formation. The document then explains how to write and balance chemical equations, and categorizes three main types of chemical reactions: synthesis, decomposition, and replacement. Finally, it discusses factors that affect the rate of chemical reactions like surface area, temperature, concentration, and catalysts.
Chemical reactions
This document summarizes key concepts about chemical reactions and properties. It defines chemical properties as the ability of a substance to change into a new substance, and physical properties as observable characteristics that do not change the substance. Chemical changes result in new substances, while physical changes alter appearance but not substance. For a chemical reaction to occur, bonds must be broken and reformed, allowing atoms to rearrange. Signs that a chemical reaction has taken place include formation of a precipitate, release of heat or light, and changes in color, temperature or gas formation. Chemical equations balance reactants and products to obey the law of conservation of matter, where mass and atoms are conserved despite rearrangement during bonding changes. Reaction rates depend on factors like activation energy
Physical and chemical change
The document discusses physical and chemical changes in matter. A physical change alters the form of matter but not its identity, and can be reversed. A chemical change produces new substances through chemical reactions, with the mass and number of atoms conserved but molecules changing. Chemical changes involve more energy and are not easily reversible. The document also outlines laws of conservation of mass and constant composition, and Gay-Lussac's law regarding gas reactions.
What's hot (20)
Viewers also liked
Physical Science 1.2 : Physical Properties
Physical properties can be observed or measured without changing the identity of matter and include density, which is the amount of matter in a given volume. Density can be used to identify substances and is calculated by dividing an object's mass by its volume. Examples of physical changes include melting, freezing, boiling, and condensing, which change a substance's state but do not form new substances.
Structure Of The Ecosystem
The document discusses key concepts in ecosystems including abiotic and biotic factors, trophic levels, food chains and webs, and energy pyramids. It explains that abiotic factors are non-living elements that affect organisms, while biotic factors are living components. It outlines the trophic levels of primary producers, primary consumers, secondary consumers, and decomposers. Food chains represent the transfer of energy between trophic levels, while food webs show a more complex network of interactions. Energy and biomass pyramids illustrate how the amount of energy and matter decreases at higher trophic levels due to inefficiencies in energy transfer between levels.
Chemical Properties And Changes
The document discusses the differences between physical and chemical changes, noting that physical changes alter a substance's appearance but not its chemical composition, while chemical changes produce new substances with different properties. Examples of physical changes include cutting, cracking, chopping, bending, and tearing materials, while chemical changes include burning wood, frying an egg, digesting food, and rusting metal. Signs that a chemical change occurred include a new color, odor, gas/smoke production, or temperature change.
Physical and Chemical Properties
This document discusses the physical and chemical properties of substances. Physical properties can be observed without changing the substance's identity and include properties like state, colour, odour, and hardness. Chemical properties describe a substance's ability to change into new substances through chemical reactions like combustibility, solubility, and reaction with acids. Both qualitative properties observable by the senses and quantitative properties measured with numbers are discussed.
Peace education
The document discusses several aspects of peace education, including its goals, key figures who advocated for non-violence like Gandhi and Martin Luther King Jr., and how peace is developed at different levels from personal to global. It also outlines indicators of peace and strategies for peacemaking, including cultivating peaceful thoughts, cultural sensitivity, and non-violent actions. Global education is presented as a way to promote understanding between all people.
Physical & chemical changes
This document discusses physical and chemical changes. It defines physical changes as changes that affect physical properties but do not form new substances, while chemical changes form new substances with different properties and identities. Examples of physical changes given include state changes like melting and dissolving, while chemical changes include cooking, burning, and rusting. Signs that a chemical change is occurring include changes in color, odor, production of heat, fizzing or bubbling, sound, and light. The document asks readers to identify examples as physical or chemical changes.
Physical Or Chemical Change Qz
Physical changes are changes that do not result in a new substance and can sometimes be reversed, such as melting, freezing, breaking, and cutting. Chemical changes result in new substances through chemical reactions, such as burning, digestion, and rusting, and cannot be reversed. The document provides examples of both physical and chemical changes and discusses their distinguishing properties.
Physical & chemical change
This document discusses the difference between physical and chemical changes in matter. A physical change alters the form or properties of a substance without changing its chemical composition, such as cutting, crushing, dissolving, or changes in state. A chemical change results in one or more new substances being formed through chemical reactions, evidenced by signs like color change, bubbling, gas production or temperature change. Examples of physical changes given are melting ice, sawing wood, and evaporating a puddle. Chemical change examples include burning fuels, baking a cake, and dissolving sugar in tea.
Chemical properties
Chemical properties describe how a substance reacts or changes during a chemical reaction. Some key chemical properties include flammability, reactivity, and the ability to undergo chemical changes that alter the composition of the substance. Common signs that a chemical change has occurred include a change in color, production of a gas, or formation of a precipitate. However, physical changes can sometimes exhibit similar signs, so the only definitive way to identify a chemical change is if the composition of the substance changes to form new substances.
Physical and chemical changes
The document discusses physical and chemical changes. Physical changes alter the state of a substance but do not create a new substance, such as melting, freezing, or breaking something into smaller pieces. Chemical changes form an entirely new substance, evidenced by a change in color, gas release, or new solid forming. Examples of physical changes include shattering a plate or melting wax, while examples of chemical changes include burning wood or rusting metal.
Peace and conflict
Subject: Global Perspectives:
Background for Peace and Conflict and a group/paired activity for the students.
Peace education
Peace has traditionally been defined as the absence of war or direct violence. However, in the 1960s an alternative view emerged that peace also requires the absence of structural violence in societies. Structural violence refers to indirect ways that people suffer due to social, political, and economic injustices built into systems. Johan Galtung argued for defining peace positively as both the absence of direct and structural violence, and the presence of social justice. Educating for peace is now seen as an ethical imperative and a way to challenge beliefs that war cannot be avoided, with the goal of cultivating non-violent and just societies.
Peace education presentation
The document discusses the importance and goals of peace education around the world. Peace education aims to foster positive social change through teaching democracy, human rights, nonviolence, and addressing issues like poverty, war, prejudice, and environmental problems. The document provides examples of how peace education is implemented in different countries and regions, highlighting issues specific to their contexts, from challenging militarism in Japan to addressing inequality in South America. It also outlines the role of educators and how schools can incorporate peace education into their curriculums and extracurricular activities to work towards building a more just and peaceful society.
Peace Presentation
The document discusses different symbols and representatives of peace, including Ned Flanders, Miley Cyrus giving a peace sign, and Woodstock 1969. It then provides details about Martin Luther King Jr. and Mahatma Gandhi, two peaceful representatives who led movements for civil rights and Indian independence, respectively, through non-violent protests and fasting. Both MLK and Gandhi are praised for effectively using peaceful means to achieve their goals and end discrimination.
Peace Education
Social Dimensions of Education
Chapter 4: Peace Education: A Transformative Response to Major Societal Challenges by Loreta N. Castro
Viewers also liked (15)
Similar to Physical Science 1.3 : Chemical Properties
Properties of matter
The document discusses the properties of matter at the molecular level. It defines matter as anything that has volume and mass, and describes physical properties like color, size, and state that can be observed without changing a substance's identity. Chemical properties describe a substance's ability to change into a new substance and are not as easy to observe. The document also distinguishes between physical changes like melting that do not form new substances, and chemical changes like baking or rusting that produce entirely new substances.
Matter ii 7th grade
Here are the answers:
1. blue color (P)
2. melting point (P)
3. density (P)
4. reacts with water (C)
5. flammability (burns) (C)
6. hardness (P)
Fe (Iron) rusts. (C)
A tire is inflated. (P)
Alcohol evaporates (P)
Food is digested. (C)
Ice melts. (P)
Paper towel absorbs water. (P)
BEd SCIENCE FILE COMPLETE FULL TOPIC OF CLASS 8TH
Physical changes alter a substance's physical properties like state, color, or odor without changing its chemical makeup. Examples include melting ice and blowing up a balloon. Chemical changes create new substances through irreversible reactions, such as ripening fruit that transforms its chemical structure. The document aims to differentiate and provide examples of physical and chemical changes.
U2L2 - Physical and Chemical Changes
This document discusses the differences between physical and chemical changes. It defines physical changes as changes that affect a substance's physical properties, like state, shape or size, without changing its chemical identity. Chemical changes form new substances with different properties than the reactants. The document also outlines signs that indicate a chemical change occurred, like gas production or color change. It explains that the law of conservation of mass states that mass is never created or destroyed in chemical or physical changes, only rearranged into different substances.
Matter
1. The document discusses classifying matter and describes the differences between elements, compounds, mixtures and pure substances.
2. It explains that elements are the simplest substances that cannot be broken down further, while compounds are formed by combining two or more elements.
3. Mixtures contain combinations of substances that are not chemically bonded, and can be separated using physical properties, whereas compounds require chemical changes to separate.
Properties of matter
There are two types of changes that matter can undergo: physical changes and chemical changes. Physical changes alter the physical properties of a substance without changing its chemical identity, such as ice melting or a metal being bent. Chemical changes occur when new substances are formed with different chemical properties than the original substances, like a log burning or food being digested. Some signs that a chemical change has taken place include a color change, gas production, energy release or absorption, light or sound production, or formation of a precipitate. Chemical changes form entirely new substances and are generally not reversible.
Density Common Chemical Changes Q And A
This document discusses physical and chemical properties and changes in matter. It provides examples of physical properties including state, size, mass, density, and magnetic properties. Examples of physical changes include changes in state, dissolving, and changes in shape. Chemical properties include ability to burn and examples of chemical changes are burning and rusting. The document also discusses signs that a chemical change has occurred such as release of energy, change in odor or color, and formation of gases or solids.
The propierties of matter
This document discusses the differences between physical and chemical properties of matter. It defines physical properties as characteristics that do not involve chemical changes, such as density, color, and hardness. Physical properties can be observed without changing the identity of the substance. Chemical properties describe a substance's ability to undergo chemical reactions and change into new substances. The document provides examples of physical properties like density and chemical properties like flammability. It also distinguishes between physical changes that do not alter a substance's identity and chemical changes that form new substances.
physical and chemical property and physical and chemical change
The document defines physical and chemical properties and changes. It states that physical properties can be observed without changing the substance's composition, and includes intensive properties that do not depend on amount and extensive properties that do. Chemical properties describe a substance's ability to change into a new substance through a chemical reaction. The document distinguishes between physical changes, which alter a substance's state or form without creating a new substance, and chemical changes, which produce new substances and are generally not reversible through physical processes alone.
Chemistry Unit 2 Part 1
This document discusses different types of properties and changes in matter. It defines extensive and intensive properties, with examples like mass and density. Physical properties can be observed without changing a substance's identity, while chemical properties involve changes in a substance's composition or structure. Physical changes alter a substance's state or form without changing its chemical makeup, like phase changes between solid, liquid and gas. Chemical changes form new substances through chemical reactions. All changes require a transfer of energy.
Good Presentation
The document discusses various topics related to matter and chemical changes. It defines elements and compounds, explains that compounds can undergo chemical changes while elements cannot, and states that the law of conservation of mass means the mass of reactants equals the mass of products in a chemical reaction. It also distinguishes physical and chemical changes, noting that only chemical changes alter the composition of matter.
Physical & chemical changes oh my
Here are the answers:
1) Cutting Grass - Physical
2) Burning Toast - Chemical
3) Wadding up Homework - Physical
4) Ice Cream Melting - Physical
5) Frying an Egg - Chemical
6) Gasoline Combustion - Chemical
7) Sweat Evaporating - Physical
1.1&1.2
1. Chemistry is the study of matter and its properties. Matter is anything that has mass and occupies space.
2. There are three main states of matter: solids, liquids, and gases. Solids have a fixed shape and volume, liquids have a fixed volume but not shape, and gases have no fixed shape or volume. Changes between these states are physical changes.
3. Chemical changes involve changes in the identities of substances and the formation of new substances with different properties. Evidence of chemical changes includes bubbles, color changes, and energy transfers.
Chemistry - Chapter 2 matter and change
This document provides an overview of chapter 2 which covers properties of matter, states of matter, mixtures, elements and compounds, and chemical reactions. It defines key terms including physical and chemical properties, extensive and intensive properties, elements, compounds, mixtures, homogeneous and heterogeneous mixtures, physical and chemical changes, reactants and products. It also outlines the key objectives covered in each section and provides examples to illustrate important concepts such as the three states of matter, separating mixtures, symbols and formulas of elements, and the law of conservation of mass.
Physchem
The document discusses the differences between physical and chemical changes. A physical change alters a substance's properties like shape, size or state but does not change its chemical makeup. A chemical change creates new substances through molecular rearrangement. Examples of physical changes include cutting paper or crushing aspirin while chemical changes include burning logs or breaking down water into hydrogen and oxygen.
Chapter 2 matter and change
This chapter discusses the fundamental concepts of matter and chemical changes. It defines matter as anything that has mass and takes up space, and describes its three main states as solid, liquid, and gas. Properties of matter are classified as either intensive or extensive. Physical and chemical properties are distinguished. Mixtures and compounds are introduced, where mixtures maintain the properties of the individual components and compounds exhibit new properties. Elements are defined as pure substances made of only one type of atom that cannot be broken down further by chemical means. Chemical changes, in which the reactants are converted into products with different compositions, are described along with clues that indicate a chemical change has occurred. The law of conservation of mass, whereby the mass of the reactants equals the mass
Matter: Chemical Properties & Changes
Matter can be described by physical and chemical properties. Matter is capable of undergoing physical and chemical changes based on these properties.
Physical and chemical properties ppt
Physical properties describe a substance without changing its chemical makeup, such as state of matter, shape, or texture. Chemical properties describe a substance's reactivity and ability to change into different substances through chemical reactions like burning or corrosion. Some key physical properties include melting, freezing, and breaking, while important chemical properties involve flammability and reactivity with other materials through combustion or other reactions.
Arya pratheesh
This document discusses physical and chemical changes of matter. It defines a physical change as a change that alters a substance's appearance, shape, or size but not its chemical identity. Chemical changes create new substances by rearranging particles and bonds. The document provides examples of physical changes like boiling water and cutting paper and chemical changes like burning and rusting. It also describes signs that indicate a chemical reaction has occurred, such as gas production, color change, and temperature change.
Chemicall change
This document discusses observing and describing chemical changes. It defines chemical and physical properties and changes. A chemical change results in a new substance, while a physical change only changes the appearance or form of a substance. Chemical changes involve reactants changing into products and can be represented by chemical equations. They involve breaking and forming bonds. Evidence of a chemical change includes new properties, energy changes, and conservation of mass, with the same number and types of atoms in the reactants and products. A system can be open or closed to matter flow during chemical reactions.
Similar to Physical Science 1.3 : Chemical Properties (20)
physical and chemical property and physical and chemical change
physical and chemical property and physical and chemical change
More from Chris Foltz
Life Science 6.1 : Disease
This document discusses infectious diseases and how they spread. It explains that infectious diseases, also called pathogens, can be passed from one living thing to another through various pathways, including the air, contaminated objects, direct contact between people or animals, and through food and water. It notes that while some diseases like cancer are noninfectious, infectious diseases are caused by pathogens. It also outlines four methods that have helped reduce disease spread: pasteurization, vaccines and immunity, antibiotics, and improved sanitation.
Life Science 6.2 : Your Body Defenses
The document summarizes the body's defenses against pathogens and how the immune system works. It describes how the skin, platelets, macrophages, T cells, B cells, antibodies, fevers, and memory cells provide lines of defense and response. It also outlines four challenges to the immune system: allergies where it overreacts; autoimmune diseases where it attacks the body's own cells; cancer where cells divide uncontrollably; and AIDS where HIV infects and disables the immune system.
Life Science 4.2 : Responding to the Environment
The document describes several human senses and how they work. It discusses how touch is detected by receptors in the skin that respond to different stimuli. It explains how sight works through the pupil controlling light entering the eye, light traveling through the lens and being focused on the retina where it is converted to electrical signals. It outlines how hearing functions with sound waves being collected by the outer and middle ear and converted to signals in the inner ear.
Life Science 4.3 : The Endocrine System
The endocrine system is made up of glands that secrete hormones to regulate various bodily functions. The main glands include the adrenal glands, which release epinephrine during the fight or flight response; the thyroid gland, which controls growth hormone secretion; and the thymus gland, which produces immune cells. These glands utilize feedback mechanisms to control hormone release and ensure balance, though imbalances can occur if a gland produces too much or too little of a certain hormone.
Life Science 4.1: The Nervous System
The document summarizes key aspects of the nervous system, including its central and peripheral components. The central nervous system includes the brain and spinal cord, which process and respond to messages from the peripheral nervous system. The peripheral nervous system connects all body parts to the central nervous system using neurons, sensory neurons that gather information and motor neurons that send signals. The nervous system also has somatic and autonomic divisions, with the somatic controlling voluntary movement and the autonomic regulating involuntary functions like digestion. The brain acts as the main control center and is comprised of the cerebrum, cerebellum and medulla, each with distinct roles in thinking, movement and involuntary processes.
Life Science 3.2 : The Urinary System
The urinary system works to clean waste from the blood through the kidneys and excrete it as urine. The kidneys contain over 1 million nephrons that act as filters to clean the blood. When the body becomes dehydrated from sweating or other fluid loss, the kidneys respond by reabsorbing more water from urine with antidiuretic hormone to maintain water balance in the blood. Common disorders of the urinary system include bacterial infections, kidney stones, and kidney disease.
Life Science 3.1 : The Digestive System
The digestive system breaks down food into nutrients that the body can use. It includes the mouth, esophagus, stomach, small intestine, large intestine, liver, gallbladder and pancreas. Mechanical digestion breaks down food physically while chemical digestion uses enzymes to break down molecules. Digestion begins in the mouth and food travels through the esophagus to the stomach where it is further broken down. Nutrients are then absorbed in the small intestine before waste is passed into the large intestine and eliminated from the body.
Life Science 2.2 : Blood
Blood has four main components - plasma, red blood cells, platelets, and white blood cells. It has three main functions - transporting oxygen and nutrients to cells, helping blood clot via platelets, and fighting pathogens with white blood cells. Blood pressure is measured as the force exerted by blood on artery walls. There are four main blood types - A, B, AB, and O - which are determined by antigens on red blood cells and must match between donor and recipient for safe blood transfusions.
Life Science 2.4 : The Respiratory System
The document describes the respiratory system and its functions. It explains that respiration involves breathing to intake oxygen and release carbon dioxide through two processes - breathing and cellular respiration. The respiratory system includes the nose, pharynx, larynx, trachea, bronchi, bronchioles and alveoli. Breathing is powered by the diaphragm and rib muscles to diffuse oxygen into red blood cells and transport it to tissues through cellular respiration. Some respiratory disorders mentioned are asthma, emphysema and SARS.
Life Science 1.3 : The Muscular System
The muscular system is made up of three types of muscle tissue: smooth muscle, cardiac muscle, and skeletal muscle. Skeletal muscle is attached to bones by tendons and works in pairs of flexor and extensor muscles to move the skeleton. There are two main types of exercise for the muscular system - resistance exercise works against resistance to strengthen muscles while aerobic exercise strengthens the heart and increases endurance. Common muscular injuries include muscle strains from overstretching and tendonitis which is the inflammation of tendons.
Life Science 1.2 : The Skeletal System
The skeletal system consists of bones, cartilage, and connective tissue that hold bones together. Bones have two types of tissue - compact bone that is solid and spongy bone that has many open spaces. Bones perform four key functions: providing structure, allowing movement, protecting organs, and storing minerals. There are three types of joints - fixed, slightly movable, and freely movable. Common injuries to the skeletal system include fractures and broken bones, while diseases include arthritis which causes joint swelling and stiffness and osteoporosis which reduces bone density.
Life Science 1.1 : Body Organization
The document discusses the organization and structure of the human body. It explains that cells form tissues, tissues form organs, and organs work together in organ systems to maintain homeostasis. It lists the 11 major organ systems - integumentary, skeletal, muscular, cardiovascular, respiratory, nervous, digestive, urinary, lymphatic, reproductive, and endocrine - and briefly describes the basic function of each system. Working together, the organ systems help regulate body functions and keep the internal environment stable.
Earth Science 6.3 : Causes of Volcanic Eruptions
Magma forms deep underground due to decreasing pressure and rising temperature, and volcanoes erupt when this magma reaches the surface. Most volcanoes are located along plate boundaries, where tectonic plates are moving apart or colliding. Scientists can predict volcanic eruptions by monitoring earthquake activity, volcanic gas emissions, changes in slope and surface temperature at volcanoes, all of which indicate rising magma.
Earth Science 6.2 : Effects of Volcanic Eruptions
Volcanic eruptions can profoundly impact climate and the Earth's surface. Large eruptions eject ash and gases into the atmosphere, which can block sunlight and cause global temperatures to drop. There are three main types of volcanoes: shield volcanoes formed from nonexplosive eruptions creating gentle slopes; cinder cone volcanoes from moderately explosive eruptions forming steep slopes; and composite volcanoes from alternating explosive and lava flows creating broad bases that steepen toward their summits. In addition to volcanoes, other volcanic landforms include craters at volcano tops, calderas which are large depressions formed when the magma chamber empties, and lava plateaus resulting from nonexplosive eruptions
Earth Science 6.1 : Volcanic Eruptions
This document discusses volcanic eruptions, describing the differences between nonexplosive and explosive eruptions. Nonexplosive eruptions produce slow lava flows while explosive eruptions blast debris into the air. The type of eruption depends on the composition of the magma, particularly its silica, water, and gas content. Magma erupts as either lava or pyroclastic material like volcanic ash, bombs, and blocks.
Earth Science 5.2 : Earthquake Measurement
Seismographs are used to detect earthquakes and locate their epicenters. Scientists use seismograms from multiple seismographs to determine the time an earthquake's waves arrived using the S-P Time Method, locating the epicenter above the focus where it began. The Richter scale measures an earthquake's magnitude based on the ground motion recorded, adjusted for distance to the seismograph. The Modified Mercalli Intensity Scale further describes earthquake impacts from I (not felt) to XII (total damage), with higher intensities nearer the epicenter.
Earth Science 5.3 : Earthquakes and Society
The document discusses earthquake hazards, forecasting, and safety. It explains that earthquake hazard level is determined by past and present seismic activity, with more activity indicating a higher hazard level. Two methods of earthquake forecasting are discussed: studying patterns of past seismic activity to make general predictions, and the gap hypothesis which predicts quakes in areas along faults that have not experienced recent activity. The document outlines five ways to safeguard buildings from earthquakes through techniques like retrofitting and using steel, and provides safety procedures for during and after an earthquake.
Earth Science 5.1: What are Earthquakes?
Most earthquakes occur along faults located near tectonic plate boundaries. As the plates move and stress increases in the crust, rock deforms in either a plastic or elastic manner. Elastic deformation can build up stress until the rock breaks, suddenly releasing energy in the form of seismic waves. There are three main types of faults that form at plate boundaries - transform faults at transform boundaries, reverse faults at convergent boundaries, and normal faults at divergent boundaries. These faults generate earthquakes as the blocks of crust slide past one another.
Earth Science 4.2 : Restless Continents
Wegener originally hypothesized that the continents were once joined together in a supercontinent called Pangaea before breaking apart and drifting to their current positions (continental drift hypothesis). Evidence for this comes from sea-floor spreading, where new oceanic lithosphere is formed at mid-ocean ridges as magma rises and cools. As the sea floor spreads away from the ridges, it records magnetic reversals in the Earth's magnetic field over time, providing strong evidence for sea-floor spreading and continental drift.
Earth Science 4.1 : Inside the Earth
The document summarizes the layers and structure of the Earth's interior. It discusses the three main layers - crust, mantle, and core - based on their chemical compositions. The crust is the outermost layer and thinnest, with continental crust thicker than oceanic crust. The mantle makes up most of the Earth's mass and lies between the crust and core. The core is the central part made mostly of iron. It then describes the physical structure, dividing the interior into lithosphere, asthenosphere, mesosphere, outer core, and inner core based on their properties. Tectonic plates consist of crust and the rigid upper mantle, floating on the asthenosphere. Scientists have mapped the interior using seismic waves from earth
More from Chris Foltz (20)
Recently uploaded
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh
ANATOMY AND BIOMECHANICS OF HIP JOINT.pdf
it describes the bony anatomy including the femoral head , acetabulum, labrum . also discusses the capsule , ligaments . muscle that act on the hip joint and the range of motion are outlined. factors affecting hip joint stability and weight transmission through the joint are summarized.
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
Iván Bornacelly, Policy Analyst at the OECD Centre for Skills, OECD, presents at the webinar 'Tackling job market gaps with a skills-first approach' on 12 June 2024
Main Java[All of the Base Concepts}.docx
This is part 1 of my Java Learning Journey. This Contains Custom methods, classes, constructors, packages, multithreading , try- catch block, finally block and more.
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
Physical pharmaceutics notes for B.pharm students
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering
Syllabus
Chapter-1
Introduction to objective, scope and outcome the subject
Chapter 2
Introduction: Scope and Specialization of Civil Engineering, Role of civil Engineer in Society, Impact of infrastructural development on economy of country.
Chapter 3
Surveying: Object Principles & Types of Surveying; Site Plans, Plans & Maps; Scales & Unit of different Measurements.
Linear Measurements: Instruments used. Linear Measurement by Tape, Ranging out Survey Lines and overcoming Obstructions; Measurements on sloping ground; Tape corrections, conventional symbols. Angular Measurements: Instruments used; Introduction to Compass Surveying, Bearings and Longitude & Latitude of a Line, Introduction to total station.
Levelling: Instrument used Object of levelling, Methods of levelling in brief, and Contour maps.
Chapter 4
Buildings: Selection of site for Buildings, Layout of Building Plan, Types of buildings, Plinth area, carpet area, floor space index, Introduction to building byelaws, concept of sun light & ventilation. Components of Buildings & their functions, Basic concept of R.C.C., Introduction to types of foundation
Chapter 5
Transportation: Introduction to Transportation Engineering; Traffic and Road Safety: Types and Characteristics of Various Modes of Transportation; Various Road Traffic Signs, Causes of Accidents and Road Safety Measures.
Chapter 6
Environmental Engineering: Environmental Pollution, Environmental Acts and Regulations, Functional Concepts of Ecology, Basics of Species, Biodiversity, Ecosystem, Hydrological Cycle; Chemical Cycles: Carbon, Nitrogen & Phosphorus; Energy Flow in Ecosystems.
Water Pollution: Water Quality standards, Introduction to Treatment & Disposal of Waste Water. Reuse and Saving of Water, Rain Water Harvesting. Solid Waste Management: Classification of Solid Waste, Collection, Transportation and Disposal of Solid. Recycling of Solid Waste: Energy Recovery, Sanitary Landfill, On-Site Sanitation. Air & Noise Pollution: Primary and Secondary air pollutants, Harmful effects of Air Pollution, Control of Air Pollution. . Noise Pollution Harmful Effects of noise pollution, control of noise pollution, Global warming & Climate Change, Ozone depletion, Greenhouse effect
Text Books:
1. Palancharmy, Basic Civil Engineering, McGraw Hill publishers.
2. Satheesh Gopi, Basic Civil Engineering, Pearson Publishers.
3. Ketki Rangwala Dalal, Essentials of Civil Engineering, Charotar Publishing House.
4. BCP, Surveying volume 1
The Diamonds of 2023-2024 in the IGRA collection
A review of the growth of the Israel Genealogy Research Association Database Collection for the last 12 months. Our collection is now passed the 3 million mark and still growing. See which archives have contributed the most. See the different types of records we have, and which years have had records added. You can also see what we have for the future.
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...Nguyen Thanh Tu Collection
https://app.box.com/s/qhtvq32h4ybf9t49ku85x0n3xl4jhr15Pengantar Penggunaan Flutter - Dart programming language1.pptx
Pengantar Penggunaan Flutter - Dart programming language1.pptx
Wound healing PPT
This document provides an overview of wound healing, its functions, stages, mechanisms, factors affecting it, and complications.
A wound is a break in the integrity of the skin or tissues, which may be associated with disruption of the structure and function.
Healing is the body’s response to injury in an attempt to restore normal structure and functions.
Healing can occur in two ways: Regeneration and Repair
There are 4 phases of wound healing: hemostasis, inflammation, proliferation, and remodeling. This document also describes the mechanism of wound healing. Factors that affect healing include infection, uncontrolled diabetes, poor nutrition, age, anemia, the presence of foreign bodies, etc.
Complications of wound healing like infection, hyperpigmentation of scar, contractures, and keloid formation.
How to Create a More Engaging and Human Online Learning Experience
How to Create a More Engaging and Human Online Learning Experience Wahiba Chair Training & Consulting
Wahiba Chair's Talk at the 2024 Learning Ideas Conference. BBR 2024 Summer Sessions Interview Training
Qualitative research interview training by Professor Katrina Pritchard and Dr Helen Williams
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Aberdeen
How to Setup Warehouse & Location in Odoo 17 Inventory
In this slide, we'll explore how to set up warehouses and locations in Odoo 17 Inventory. This will help us manage our stock effectively, track inventory levels, and streamline warehouse operations.
How to Manage Your Lost Opportunities in Odoo 17 CRM
Odoo 17 CRM allows us to track why we lose sales opportunities with "Lost Reasons." This helps analyze our sales process and identify areas for improvement. Here's how to configure lost reasons in Odoo 17 CRM
Recently uploaded (20)
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
Traditional Musical Instruments of Arunachal Pradesh and Uttar Pradesh - RAYH...
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
Beyond Degrees - Empowering the Workforce in the Context of Skills-First.pptx
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
RHEOLOGY Physical pharmaceutics-II notes for B.pharm 4th sem students
Chapter wise All Notes of First year Basic Civil Engineering.pptx
Chapter wise All Notes of First year Basic Civil Engineering.pptx
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
BÀI TẬP DẠY THÊM TIẾNG ANH LỚP 7 CẢ NĂM FRIENDS PLUS SÁCH CHÂN TRỜI SÁNG TẠO ...
Pengantar Penggunaan Flutter - Dart programming language1.pptx
Pengantar Penggunaan Flutter - Dart programming language1.pptx
Liberal Approach to the Study of Indian Politics.pdf
Liberal Approach to the Study of Indian Politics.pdf
How to Create a More Engaging and Human Online Learning Experience
How to Create a More Engaging and Human Online Learning Experience
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
What is Digital Literacy? A guest blog from Andy McLaughlin, University of Ab...
How to Setup Warehouse & Location in Odoo 17 Inventory
How to Setup Warehouse & Location in Odoo 17 Inventory
How to Manage Your Lost Opportunities in Odoo 17 CRM
How to Manage Your Lost Opportunities in Odoo 17 CRM
Physical Science 1.3 : Chemical Properties
- 1. Chemical Properties Physical Science Chapter 1.3
- 2. Objectives: Describe two examples of chemical properties. Explain what happens during a chemical change. Distinguish between physical and chemical changes.
- 3. Chemical Properties Comparing Physical and Chemical Properties You can observe physical properties without changing the identity of the substance. Chemicals properties are more difficult to observe. Characteristic Properties The properties that are most useful in identifying a substance are characteristic properties.
- 5. Chemical Changes and New Substances What Happens During a Chemical Change? A substance changes chemical properties. Signs of Chemical Changes Change in color Odor Production of heat Fizzing
- 7. Physical Versus Chemical Changes A Change in Composition Physical changes do not change the composition of a substance while chemical changes do. Reversing Changes Many physical changes are easily reversed But most chemical changes cannot easily be reversed.