This document provides an overview of key concepts from a chemistry textbook chapter on matter, including its properties, changes, mixtures, and elements/compounds. It discusses the three states of matter and defines physical and chemical properties. It also describes two types of changes matter can undergo (physical vs. chemical) and techniques for separating mixtures. Finally, it defines elements and compounds, and explains how they are organized in the periodic table according to atomic structure. The chapter assessments cover identifying properties, states of matter, and distinguishing between mixtures, elements and compounds.
This document provides a summary of sections from a chemistry textbook chapter on properties and changes in matter. It summarizes key concepts from sections on properties of matter, changes in matter, mixtures of matter, and elements and compounds. The sections define states of matter, physical and chemical properties, physical and chemical changes, mixtures, elements, compounds, and laws of chemistry such as definite and multiple proportions.
This document summarizes key concepts from a chemistry chapter about matter, its properties, and changes. It discusses the three common states of matter, physical and chemical properties, and physical and chemical changes. It also covers mixtures and their separation techniques, elements and compounds, and the laws of definite and multiple proportions.
This document defines key terms related to states of matter and the classification of matter. It describes the four fundamental states of matter - solid, liquid, gas, and plasma. It also defines properties of solids, liquids and gases. The document outlines that matter can be classified as elements, compounds or mixtures. It defines physical and chemical properties and explains intensive and extensive properties. Laws of conservation of mass, energy and mass-energy are also summarized.
This document provides an overview of some basic concepts in chemistry. It discusses the classification of matter as either pure substances or mixtures. Pure substances are further classified as elements or compounds. Mixtures can be either homogeneous, containing a uniform composition throughout, or heterogeneous, with a non-uniform composition. The three common states of matter - solid, liquid, and gas - are also introduced based on how closely or loosely packed the particles are. Key concepts like physical and chemical properties of matter and the differences between physical and chemical changes are summarized.
This document defines key concepts about the properties of matter. It explains that matter is anything that has mass and takes up space, and can exist in solid, liquid, or gas states. Physical properties can be observed without changing a substance's identity, while chemical properties involve chemical changes forming new substances. Matter can also be classified as pure substances like elements and compounds, or mixtures that are either homogeneous solutions or heterogeneous mixtures of different phases.
This document provides an overview of chemistry, including:
1. Chemistry is the study of matter, its properties, and the changes it undergoes during chemical reactions. It is a central science essential to many other fields like biology and physics.
2. Studying chemistry allows us to explain natural phenomena and can prepare students for careers in fields like medicine, environmental science, and more.
3. The scientific method involves making observations, developing hypotheses, designing experiments to test hypotheses, and using results to modify hypotheses or develop theories to explain phenomena.
This document provides an overview of basic chemistry concepts including:
- Matter can be classified as mixtures or pure substances. Pure substances have a definite composition while mixtures do not.
- Elements are pure substances that cannot be broken down further, and are classified as metals, nonmetals, and metalloids. Compounds are also pure substances but have elements combined in fixed proportions.
- Chemical properties describe reactions that change a substance's composition, while physical properties can be observed without chemical changes.
Chemistry - Chapter 2 matter and changeMr. Walajtys
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.
This document provides a summary of sections from a chemistry textbook chapter on properties and changes in matter. It summarizes key concepts from sections on properties of matter, changes in matter, mixtures of matter, and elements and compounds. The sections define states of matter, physical and chemical properties, physical and chemical changes, mixtures, elements, compounds, and laws of chemistry such as definite and multiple proportions.
This document summarizes key concepts from a chemistry chapter about matter, its properties, and changes. It discusses the three common states of matter, physical and chemical properties, and physical and chemical changes. It also covers mixtures and their separation techniques, elements and compounds, and the laws of definite and multiple proportions.
This document defines key terms related to states of matter and the classification of matter. It describes the four fundamental states of matter - solid, liquid, gas, and plasma. It also defines properties of solids, liquids and gases. The document outlines that matter can be classified as elements, compounds or mixtures. It defines physical and chemical properties and explains intensive and extensive properties. Laws of conservation of mass, energy and mass-energy are also summarized.
This document provides an overview of some basic concepts in chemistry. It discusses the classification of matter as either pure substances or mixtures. Pure substances are further classified as elements or compounds. Mixtures can be either homogeneous, containing a uniform composition throughout, or heterogeneous, with a non-uniform composition. The three common states of matter - solid, liquid, and gas - are also introduced based on how closely or loosely packed the particles are. Key concepts like physical and chemical properties of matter and the differences between physical and chemical changes are summarized.
This document defines key concepts about the properties of matter. It explains that matter is anything that has mass and takes up space, and can exist in solid, liquid, or gas states. Physical properties can be observed without changing a substance's identity, while chemical properties involve chemical changes forming new substances. Matter can also be classified as pure substances like elements and compounds, or mixtures that are either homogeneous solutions or heterogeneous mixtures of different phases.
This document provides an overview of chemistry, including:
1. Chemistry is the study of matter, its properties, and the changes it undergoes during chemical reactions. It is a central science essential to many other fields like biology and physics.
2. Studying chemistry allows us to explain natural phenomena and can prepare students for careers in fields like medicine, environmental science, and more.
3. The scientific method involves making observations, developing hypotheses, designing experiments to test hypotheses, and using results to modify hypotheses or develop theories to explain phenomena.
This document provides an overview of basic chemistry concepts including:
- Matter can be classified as mixtures or pure substances. Pure substances have a definite composition while mixtures do not.
- Elements are pure substances that cannot be broken down further, and are classified as metals, nonmetals, and metalloids. Compounds are also pure substances but have elements combined in fixed proportions.
- Chemical properties describe reactions that change a substance's composition, while physical properties can be observed without chemical changes.
Chemistry - Chapter 2 matter and changeMr. Walajtys
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.
This document summarizes key concepts from a chapter on matter, including:
- Distinguishing between physical and chemical properties and changes
- Defining the three physical states of matter
- Explaining conservation of mass in chemical reactions
- Contrasting mixtures and pure substances
- Describing techniques to separate mixtures
- Distinguishing between elements and compounds
- Explaining the organization of the periodic table and laws of definite and multiple proportions governing compounds
This document provides an overview of organic chemistry and organic medicinal chemistry. It discusses general chemistry topics including the definition of chemistry, classification of matter, physical and chemical properties, and acid-base properties. It also covers organic chemistry topics such as the difference between inorganic and organic chemistry, functional groups, isomerism, and reactions. The document is intended to serve as a refresher course on these fundamental concepts.
The document defines matter and describes its three common states: solid, liquid, and gas. It distinguishes between physical and chemical properties of matter, and between physical and chemical changes. It defines mixtures and pure substances, and classifies matter as homogeneous or heterogeneous. Key terms include the various states of matter, physical and chemical properties, and the classification of matter.
This document provides an overview of chemistry unit 2 which covers how matter changes. It discusses the three common states of matter - solids, liquids and gases. It defines physical and chemical properties and changes. It also defines mixtures and how they are combinations of substances that can be separated. It introduces elements and compounds, explaining how compounds are combinations of elements that have different properties. It covers the laws of definite and multiple proportions for compounds.
Some basic concepts of chemistry
chapter 1 of class 11.
N.B : This is for reference only. Students are advised not to copy, but to take ideas and do the work in their own style-it builds your imagination.
This document provides an overview of properties of matter. It begins by defining the three states of matter - solids, liquids, and gases. It describes the properties of each state, such as solids having a fixed shape and volume while gases have no fixed shape or volume. The document then discusses physical and chemical properties and changes, defining the difference between physical and chemical changes. It provides examples of each. Density is also covered, defining concepts such as mass, volume, and density and providing practice problems. The document concludes by discussing elements, compounds, and mixtures.
General Chemistry and Inorganic Pharmaceutical Chemistry Module 1 Pharmacist ...Senyora Ouf'ra
This document provides an overview of Module 1 of the pharmacist licensure exam, which covers various topics in pharmaceutical chemistry. It will be the first module administered on the first day of the exam from 8-10 AM. The module will include questions from general chemistry, inorganic and organic medicinal chemistry, analytical chemistry, and other related chemical topics. The document emphasizes that Module 1 will be the most difficult and important module to study for. It then provides examples of key topics covered, such as atomic structure, types of chemical bonds, gas laws, and thermodynamics.
This unit discusses how matter changes states and undergoes physical and chemical transformations. It introduces the key concepts of physical and chemical properties, the three common states of matter (solid, liquid, gas), mixtures and their separation techniques. It also covers the basic definitions and principles of elements, compounds, the periodic table, and the laws of definite and multiple proportions that govern chemical combinations. The unit provides objectives and outlines the main topics to help students understand the fundamental composition and behavior of matter.
Pharmaceutical chemistry of inorganic medicinalsEnter Exit
This document provides an introduction to chemical kinetics and equilibrium. It defines chemical kinetics as the study of reaction rates and mechanisms. It describes factors that influence reaction rates, such as the nature of reactants, physical state, concentration, temperature, catalysts and pressure. It then discusses collision theory and activation energy. The document also explains chemical equilibrium, including the law of mass action and Le Chatelier's principle. Finally, it covers pH, pOH, pKa and pKb calculations and their relationships to acid/base ionization constants.
Matter is anything that has mass and takes up space. It is composed of atoms, which contain protons, neutrons, and electrons. Elements are pure substances made of only one type of atom, while compounds are made of two or more elements chemically bonded together. Mixtures contain different substances mixed together but not chemically combined. The three main states of matter are solids, liquids, and gases. Chemical and physical properties can be used to describe and identify matter.
Matter can be described by physical and chemical properties. Matter is capable of undergoing physical and chemical changes based on these properties.
Chapter 15:1, 10:1
1. The document provides an overview of an advanced physical chemistry course taught by Dr. Fateh Eltaboni.
2. The course covers topics such as thermodynamics, kinetics, quantum mechanics, and spectroscopy.
3. Key concepts from the kinetic molecular theory are discussed, including how the random motion of gas molecules relates to measurable properties like pressure, temperature, and volume.
+ Neet ug, iseet chemistry mc qs ( pdfdrive )SaranyaS920998
This document provides information about a chemistry textbook titled "Chemistry MCQs for XI (Science) + NEET UG/ISEET". It was written by Professors Santosh B. Yadav and Anil Thomas. The book contains multiple choice questions organized by chapter and section, with the sections progressing from easier to more competitive questions. It is designed to help students prepare for exams like NEET and ISEET in addition to their class exams. The book is published by Target Publications Pvt. Ltd. in Mumbai, India.
The document discusses the different states of matter and phases. It explains that matter can exist in solid, liquid, gas, and plasma phases. The solid phase occurs when molecules are tightly bound, while the liquid phase allows molecules to flow freely but maintain a shape defined by their container. Gas molecules exhibit random motion and the least intermolecular forces. Plasma is an ionized gas that conducts electricity. The document also briefly discusses Bose-Einstein condensates, an exotic state of matter.
This document discusses the classification of matter. It defines mixtures as combinations of two or more substances that are not chemically bonded and can be separated by mechanical means. Mixtures can be heterogeneous, with visible components, or homogeneous, appearing uniform. Pure substances cannot be broken down and include elements, which cannot be broken down further, and compounds, made of two or more elements joined in a fixed ratio. Elements are found on the periodic table and compounds are named according to the elements present and their ratios. The properties of materials, such as their conductivity, magnetism, and position on the periodic table, determine whether they are classified as metals, nonmetals, or metalloids.
This document discusses the properties and states of matter. It defines matter as anything that has mass and takes up space, and explains that matter is made up of atoms. It then describes the three main states of matter - solids, liquids, and gases - and how their properties differ based on factors like the arrangement and movement of particles. The document also briefly introduces plasma and Bose-Einstein condensates as more advanced states of matter. It concludes by contrasting physical and chemical properties and changes in matter.
This document is a chapter summary covering key topics in analyzing scientific data, including units and measurements, scientific notation, uncertainty in data, and representing data graphically. It discusses the SI system of units, derived vs base units, accuracy vs precision, significant figures, error analysis, and types of graphs like line graphs, bar graphs and pie charts. Key points covered include the SI base units, dimensional analysis using conversion factors, expressing numbers in scientific notation, and interpreting graphs to identify patterns and trends in data.
This document outlines the key topics covered in a course on scientific measurement:
1. It introduces different types of measurements and SI units.
2. It discusses derived units, and measuring mass, weight, and temperature.
3. It distinguishes between accuracy and precision in measurements.
4. It covers converting measurements to scientific notation and the importance of significant figures.
This document discusses significant figures and how to determine the number of significant figures in measurements and calculations. It provides examples of counting significant figures in given values. It also summarizes the rules for determining significant figures in addition, subtraction, multiplication and division calculations. Specifically, for multiplication and division the number of significant figures in the result equals the number in the least precise measurement. For addition and subtraction, the number of decimal places in the result equals the number in the least precise measurement.
The document is a series of slides covering different sections of a biology textbook chapter on the chemistry of life. It begins with an outline listing the section topics: proteins, carbohydrates, lipids, nucleic acids, and metabolism. The following sections then provide more details on the structures and functions of these key biomolecules.
The document discusses various topics in science including derived units, percent error, scientific notation, significant figures, rounding numbers, and graphing. It defines key terms such as derived units, density, error, scientific notation, and significant figures. Rules are provided for determining significant figures, rounding numbers, and ensuring calculations maintain the appropriate number of significant figures. Graphs are described as a way to visually display data and relationships between variables.
This document summarizes key concepts from a chapter on matter, including:
- Distinguishing between physical and chemical properties and changes
- Defining the three physical states of matter
- Explaining conservation of mass in chemical reactions
- Contrasting mixtures and pure substances
- Describing techniques to separate mixtures
- Distinguishing between elements and compounds
- Explaining the organization of the periodic table and laws of definite and multiple proportions governing compounds
This document provides an overview of organic chemistry and organic medicinal chemistry. It discusses general chemistry topics including the definition of chemistry, classification of matter, physical and chemical properties, and acid-base properties. It also covers organic chemistry topics such as the difference between inorganic and organic chemistry, functional groups, isomerism, and reactions. The document is intended to serve as a refresher course on these fundamental concepts.
The document defines matter and describes its three common states: solid, liquid, and gas. It distinguishes between physical and chemical properties of matter, and between physical and chemical changes. It defines mixtures and pure substances, and classifies matter as homogeneous or heterogeneous. Key terms include the various states of matter, physical and chemical properties, and the classification of matter.
This document provides an overview of chemistry unit 2 which covers how matter changes. It discusses the three common states of matter - solids, liquids and gases. It defines physical and chemical properties and changes. It also defines mixtures and how they are combinations of substances that can be separated. It introduces elements and compounds, explaining how compounds are combinations of elements that have different properties. It covers the laws of definite and multiple proportions for compounds.
Some basic concepts of chemistry
chapter 1 of class 11.
N.B : This is for reference only. Students are advised not to copy, but to take ideas and do the work in their own style-it builds your imagination.
This document provides an overview of properties of matter. It begins by defining the three states of matter - solids, liquids, and gases. It describes the properties of each state, such as solids having a fixed shape and volume while gases have no fixed shape or volume. The document then discusses physical and chemical properties and changes, defining the difference between physical and chemical changes. It provides examples of each. Density is also covered, defining concepts such as mass, volume, and density and providing practice problems. The document concludes by discussing elements, compounds, and mixtures.
General Chemistry and Inorganic Pharmaceutical Chemistry Module 1 Pharmacist ...Senyora Ouf'ra
This document provides an overview of Module 1 of the pharmacist licensure exam, which covers various topics in pharmaceutical chemistry. It will be the first module administered on the first day of the exam from 8-10 AM. The module will include questions from general chemistry, inorganic and organic medicinal chemistry, analytical chemistry, and other related chemical topics. The document emphasizes that Module 1 will be the most difficult and important module to study for. It then provides examples of key topics covered, such as atomic structure, types of chemical bonds, gas laws, and thermodynamics.
This unit discusses how matter changes states and undergoes physical and chemical transformations. It introduces the key concepts of physical and chemical properties, the three common states of matter (solid, liquid, gas), mixtures and their separation techniques. It also covers the basic definitions and principles of elements, compounds, the periodic table, and the laws of definite and multiple proportions that govern chemical combinations. The unit provides objectives and outlines the main topics to help students understand the fundamental composition and behavior of matter.
Pharmaceutical chemistry of inorganic medicinalsEnter Exit
This document provides an introduction to chemical kinetics and equilibrium. It defines chemical kinetics as the study of reaction rates and mechanisms. It describes factors that influence reaction rates, such as the nature of reactants, physical state, concentration, temperature, catalysts and pressure. It then discusses collision theory and activation energy. The document also explains chemical equilibrium, including the law of mass action and Le Chatelier's principle. Finally, it covers pH, pOH, pKa and pKb calculations and their relationships to acid/base ionization constants.
Matter is anything that has mass and takes up space. It is composed of atoms, which contain protons, neutrons, and electrons. Elements are pure substances made of only one type of atom, while compounds are made of two or more elements chemically bonded together. Mixtures contain different substances mixed together but not chemically combined. The three main states of matter are solids, liquids, and gases. Chemical and physical properties can be used to describe and identify matter.
Matter can be described by physical and chemical properties. Matter is capable of undergoing physical and chemical changes based on these properties.
Chapter 15:1, 10:1
1. The document provides an overview of an advanced physical chemistry course taught by Dr. Fateh Eltaboni.
2. The course covers topics such as thermodynamics, kinetics, quantum mechanics, and spectroscopy.
3. Key concepts from the kinetic molecular theory are discussed, including how the random motion of gas molecules relates to measurable properties like pressure, temperature, and volume.
+ Neet ug, iseet chemistry mc qs ( pdfdrive )SaranyaS920998
This document provides information about a chemistry textbook titled "Chemistry MCQs for XI (Science) + NEET UG/ISEET". It was written by Professors Santosh B. Yadav and Anil Thomas. The book contains multiple choice questions organized by chapter and section, with the sections progressing from easier to more competitive questions. It is designed to help students prepare for exams like NEET and ISEET in addition to their class exams. The book is published by Target Publications Pvt. Ltd. in Mumbai, India.
The document discusses the different states of matter and phases. It explains that matter can exist in solid, liquid, gas, and plasma phases. The solid phase occurs when molecules are tightly bound, while the liquid phase allows molecules to flow freely but maintain a shape defined by their container. Gas molecules exhibit random motion and the least intermolecular forces. Plasma is an ionized gas that conducts electricity. The document also briefly discusses Bose-Einstein condensates, an exotic state of matter.
This document discusses the classification of matter. It defines mixtures as combinations of two or more substances that are not chemically bonded and can be separated by mechanical means. Mixtures can be heterogeneous, with visible components, or homogeneous, appearing uniform. Pure substances cannot be broken down and include elements, which cannot be broken down further, and compounds, made of two or more elements joined in a fixed ratio. Elements are found on the periodic table and compounds are named according to the elements present and their ratios. The properties of materials, such as their conductivity, magnetism, and position on the periodic table, determine whether they are classified as metals, nonmetals, or metalloids.
This document discusses the properties and states of matter. It defines matter as anything that has mass and takes up space, and explains that matter is made up of atoms. It then describes the three main states of matter - solids, liquids, and gases - and how their properties differ based on factors like the arrangement and movement of particles. The document also briefly introduces plasma and Bose-Einstein condensates as more advanced states of matter. It concludes by contrasting physical and chemical properties and changes in matter.
This document is a chapter summary covering key topics in analyzing scientific data, including units and measurements, scientific notation, uncertainty in data, and representing data graphically. It discusses the SI system of units, derived vs base units, accuracy vs precision, significant figures, error analysis, and types of graphs like line graphs, bar graphs and pie charts. Key points covered include the SI base units, dimensional analysis using conversion factors, expressing numbers in scientific notation, and interpreting graphs to identify patterns and trends in data.
This document outlines the key topics covered in a course on scientific measurement:
1. It introduces different types of measurements and SI units.
2. It discusses derived units, and measuring mass, weight, and temperature.
3. It distinguishes between accuracy and precision in measurements.
4. It covers converting measurements to scientific notation and the importance of significant figures.
This document discusses significant figures and how to determine the number of significant figures in measurements and calculations. It provides examples of counting significant figures in given values. It also summarizes the rules for determining significant figures in addition, subtraction, multiplication and division calculations. Specifically, for multiplication and division the number of significant figures in the result equals the number in the least precise measurement. For addition and subtraction, the number of decimal places in the result equals the number in the least precise measurement.
The document is a series of slides covering different sections of a biology textbook chapter on the chemistry of life. It begins with an outline listing the section topics: proteins, carbohydrates, lipids, nucleic acids, and metabolism. The following sections then provide more details on the structures and functions of these key biomolecules.
The document discusses various topics in science including derived units, percent error, scientific notation, significant figures, rounding numbers, and graphing. It defines key terms such as derived units, density, error, scientific notation, and significant figures. Rules are provided for determining significant figures, rounding numbers, and ensuring calculations maintain the appropriate number of significant figures. Graphs are described as a way to visually display data and relationships between variables.
This presentation explores the many uses of mathematics in daily life. It is divided into nine areas focusing on different aspects of mathematics such as arithmetic progressions, trigonometry, Fibonacci sequences, and the golden section. Some key examples provided include using arithmetic progressions to predict the eruptions of Old Faithful geyser, applying trigonometry in fields like architecture, astronomy, and geology, finding Fibonacci sequences and the golden section in nature, architecture, art, and music, and learning about the origins and properties of Fibonacci sequences and the golden section.
This document provides an overview of stoichiometry concepts covered in 11 sections. It defines stoichiometry and discusses mole ratios from balanced equations. It describes how to perform stoichiometric calculations using mole-to-mole, mole-to-mass, and mass-to-mass conversions. It also covers limiting reactants, excess reactants, and calculating products. Finally, it defines theoretical yield, actual yield, and percent yield for chemical reactions. The document provides learning objectives, examples, and self-assessment questions for each section.
This document provides an overview of sections from a chapter on the periodic table and periodic law. It discusses the development of the modern periodic table, including the early work of scientists like Lavoisier, Newlands, Meyer and Mendeleev. It describes the key features of the periodic table such as periods, groups, representative elements and transition metals. It also summarizes periodic trends in properties like atomic radius, ionization energy and electronegativity that relate to an element's position on the periodic table.
The document is a chapter menu for organic chemistry covering substituted hydrocarbons and their reactions. It outlines 5 main sections that discuss alkyl and aryl halides, alcohols/ethers/amines, carbonyl compounds, other organic reactions, and polymers. Each section defines functional groups, draws structures, and discusses properties and reactions for different compound classes.
This document provides an overview of three sections on chemical equilibrium from a chemistry textbook. Section 17.1 discusses the definition of chemical equilibrium as a state where forward and reverse reactions occur at equal rates. It also defines equilibrium constants and expressions. Section 17.2 explains how temperature, pressure, and concentration changes affect equilibrium based on Le Châtelier's principle. Section 17.3 discusses using equilibrium constants to determine concentrations and solubility products, and how the common ion effect impacts solubility.
This document contains an outline for a chapter on redox reactions with the following sections:
1. Section 19.1 covers oxidation and reduction processes, defining oxidation numbers and identifying oxidizing and reducing agents.
2. Section 19.2 discusses balancing redox equations using the oxidation-number method and splitting reactions into half-reactions.
3. The document provides assessment questions to test understanding and links to additional resources like study guides, concept illustrations, and standardized test practice questions.
This document provides an overview of key concepts about acids and bases from sections 18.1 through 18.4. It introduces the Arrhenius, Brønsted-Lowry, and Lewis models of acids and bases. It describes the properties of acids and bases and how pH and pKa/pKb values relate to acid and base strength. Neutralization reactions between acids and bases are discussed along with acid-base titrations and buffered solutions.
This document contains a chapter menu and outline for a chapter on reaction rates. The chapter is divided into 4 main sections:
1) A Model for Reaction Rates - discusses calculating reaction rates from data and relating rates to collisions between particles.
2) Factors Affecting Reaction Rates - identifies factors like concentration, temperature, surface area, and catalysts that affect reaction rates.
3) Reaction Rate Laws - expresses the relationship between reaction rate and concentration, and how to determine reaction orders.
4) Instantaneous Reaction Rates and Reaction Mechanisms - discusses calculating instantaneous rates, complex reactions having multiple steps, and relating rates to reaction mechanisms.
This document provides an overview of three sections (13.1, 13.2, 13.3) from a chemistry textbook chapter on gases. Section 13.1 describes gas laws including Boyle's law, Charles' law, Gay-Lussac's law, and the combined gas law. Section 13.2 introduces the ideal gas law, Avogadro's principle, and compares real and ideal gases. Section 13.3 explains how to use gas laws and stoichiometry to solve problems involving gaseous reactants and products in chemical equations.
The document discusses arithmetic and geometric sequences. It provides examples and explanations of key concepts such as common difference, common ratio, formulas for finding specific terms, and calculating series sums. Formulas are derived for finding the nth term in an arithmetic sequence as an = a1 + d(n-1) and the nth term in a geometric sequence as an = a1rn-1. Examples are worked through to demonstrate how to use the formulas and calculate sequence terms and series sums.
The document discusses different types of instruments used to measure temperature, volume, length, circumference, mass, and how to read them correctly. It explains that a clinical thermometer measures body temperature, a digital thermometer measures surrounding temperature, and a laboratory thermometer measures temperature in science experiments. It also describes how to use a string and ruler to measure the circumference of an object, and that mass can be measured using a lever balance, electronic balance, or weighing scale in grams or kilograms.
This document describes common laboratory equipment used in chemistry experiments. It provides brief descriptions of the purpose and use of various pieces of apparatus including beakers, conical flasks, measuring cylinders, test tubes, test tube racks, rubber bungs, watch glasses, stirring rods, funnels, pipettes, spatulas, forceps, scalpels, burettes, Bunsen burners, tripods, gauze, heatproof mats, clay triangles, evaporating dishes, crucibles, crucible tongs, clamp stands, and litmus and universal indicator paper.
The document contains multiple word problems describing situations that follow arithmetic sequences. Each situation provides the first few terms of the sequence and asks the reader to determine the total or sum based on a given number of terms. The solutions show setting up the arithmetic sequence formula to determine the general nth term and then applying this to calculate the requested total.
The document summarizes the main parts of a compound microscope and their functions. It describes the base, light source, stage, stage clips, arm, coarse and fine adjustments, eyepiece, body tube, nosepiece, high power objective, low power objective, scanning lens, and disk diaphragm. Each part has a specific role in allowing magnification and viewing of specimens.
I split the presentation for the unit into two, as I added so many slides to help with student questions and misconceptions. This one focuses on mathematical aspects of the unit.
This document provides an overview of sections from a chemistry textbook on matter and its properties. Section 3.1 discusses the states of matter and physical and chemical properties. Section 3.2 covers physical and chemical changes and the law of conservation of mass. Section 3.3 defines mixtures and different techniques for separating mixtures. Section 3.4 distinguishes between elements and compounds and explains the periodic table and laws of definite and multiple proportions.
This chapter discusses the properties and changes of matter. It introduces the three common states of matter - solids, liquids, and gases. Matter can undergo physical changes that alter its properties without changing its composition, or chemical changes that result in new substances. The law of conservation of mass states that mass is conserved in chemical reactions. Compounds are combinations of elements that can be broken down, while elements cannot be further broken down.
The document discusses key concepts from a chemistry chapter about matter, including its three common states as solids, liquids, and gases. It explains that matter can undergo physical changes that do not alter its chemical makeup or chemical changes that result in new substances forming. Most everyday matter is made of mixtures of different substances, and a compound is a pure substance consisting of two or more chemically bonded elements.
This document provides an overview of chemistry unit 2 which covers how matter changes. It discusses the three common states of matter, physical and chemical properties, and how matter undergoes physical and chemical changes. It also addresses mixtures as combinations of substances and how mixtures can be separated. The document defines elements and compounds, and explains the organization of elements in the periodic table. It describes how all compounds obey the laws of definite and multiple proportions.
This document defines and classifies various properties of matter. It discusses intensive and extensive properties, with intensive properties not depending on system size and extensive properties being proportional to amount of material. Physical properties can be observed without changing composition and include properties like density, color, and conductivity. Chemical properties describe how matter reacts with other substances and alters composition. The document provides examples of physical changes like changes in state and separation of mixtures, as well as chemical changes like corrosion and acid reactions. It concludes with a recap question to classify changes as physical or chemical.
This document provides an introduction to general chemistry, including why chemistry is studied, its central role in understanding matter, and learning goals for the course. Chemistry involves understanding the properties and behavior of matter, which exists as elements, compounds, and mixtures. The three states of matter - solid, liquid, and gas - are classified based on molecular motion and energy. Physical and chemical properties help characterize different types of pure substances and mixtures. Changes in matter can involve physical changes of state or chemical reactions that alter chemical identity. Energy also plays a key role in these transformations.
The document discusses the nature of matter. It describes matter as being composed of tiny particles called atoms that can be arranged into elements or compounds. Matter exists in three states - solid, liquid, and gas - which are distinguished by how tightly or loosely packed the particles are and how freely they can move. Mixtures are substances made of two or more materials mixed together, while pure substances have a consistent composition and can be either elements or compounds. The document outlines several methods for separating mixtures, including filtration, distillation, centrifugation, and chromatography.
PS CH 10 matter properties and changes editedEsther Herrera
The document discusses the properties and types of matter, including the three states of matter (solid, liquid, gas), mixtures and their separation, physical and chemical properties, physical and chemical changes, and the laws of conservation of mass, definite proportions, and multiple proportions as they relate to matter and chemical reactions. Elements are pure substances that cannot be broken down further, while compounds are combinations of two or more elements that have properties different from their component elements. Matter is anything that has mass and takes up space.
The document provides an overview of key concepts related to the mole unit from sections 10.1 to 10.5 of a chemistry textbook. Section 10.1 defines the mole and explains how it can be used to indirectly count particles. Section 10.2 relates the mass of a mole to atomic mass and molar mass. Section 10.3 discusses calculating molar mass for compounds and converting between moles, mass, and particles for compounds. Section 10.4 explains empirical and molecular formulas. Section 10.5 defines hydrates and how to determine the formula of a hydrate.
The document discusses atoms and elements. It defines key concepts like atoms, elements, compounds, mixtures, isotopes and subatomic particles. It explains Dalton's atomic theory and how it led to the concept of atomic mass and mass spectrometry. The periodic table is introduced as a way to organize and classify elements based on their atomic structure of protons, neutrons and electrons. Elements are classified as metals, nonmetals and metalloids based on their physical properties.
STRAND 1 MIXTURES ELEMENTS AND COMPOUNDS.pptxkimdan468
This document discusses elements, compounds, and their properties. It defines elements as pure substances made of one type of atom, while compounds are formed by combining two or more elements. Some common elements and their symbols are listed, such as hydrogen (H), carbon (C), oxygen (O), and nitrogen (N). Everyday applications of common elements like nitrogen, aluminum, gold, copper, oxygen, and hydrogen are described.
This document discusses states of matter and phase changes. It covers gases, liquids, solids, and the forces between particles in each state. Gases consist of freely moving particles with empty space between them. Liquids and solids have particles with limited motion that are held close together by intermolecular forces. Phase changes between solid, liquid and gas occur when energy is added or removed, breaking or forming bonds between particles.
This chapter introduces key concepts in chemistry including distinguishing science from technology, defining important terms like hypothesis and theory, and classifying types of matter. It outlines learning objectives related to the states and properties of matter, physical and chemical changes, and using units and calculations. Students will learn to differentiate elements, compounds, mixtures and various research types as well as manipulate matter concepts like density, heat, temperature and phases. Critical thinking skills will also be developed.
The document discusses physical and chemical changes, including the key differences between them. A physical change does not create new substances, while a chemical change involves atoms rearranging to form new substances. The document also examines signs that a chemical reaction has occurred, such as a change in color, odor, temperature, or the formation of a gas or precipitate. It introduces the concept of a chemical equation to represent a chemical reaction and explains that chemical equations must be balanced to satisfy the law of conservation of mass.
Chemistry is the study of matter and its composition, properties, and the changes it undergoes. There are several key points:
1) Matter is anything that has mass and takes up space, and can be either a pure substance or a mixture.
2) Chemical and physical properties are used to identify substances. Chemical properties involve changes in composition while physical properties do not.
3) Energy drives all chemical and physical changes. It is transferred and transformed during reactions but cannot be created or destroyed. Exothermic reactions release energy while endothermic reactions absorb energy.
CLASSIFICATIONA AND PROPERTIES OF MATTER.pptxGemreyBravo
This document provides an overview of matter, its properties, and classification. It begins by outlining learning objectives about differentiating physical and chemical properties, states of matter, and classifying matter. The document then defines key concepts such as atoms, elements, compounds, and mixtures. It describes the three states of matter and different types of particles that make up matter. The document classifies matter as either pure substances like elements and compounds, or mixtures that can be homogeneous or heterogeneous. It provides examples of solutions, suspensions, and colloids. Finally, the document distinguishes between physical and chemical properties and changes.
The document provides a review of key concepts for an 8th grade physical science exam, including different types of measurements, scientific experimentation, phases and changes of matter, the structure and properties of atoms and elements, and the differences between physical and chemical changes and mixtures and pure substances. It defines length, volume, mass, weight, time, temperature, and density and their standard units. It also outlines the key characteristics of plasma, phases of matter, changes in state, and physical and chemical properties.
This document provides a revision guide for the chemistry part of the IGCSE Coordinated Science course. It contains all the material needed to cover the syllabus and highlights supplementary material in dashed boxes. The guide alone is not sufficient for high-scoring students, who should use multiple resources to develop a deeper understanding. Some recommended websites provide additional practice questions, diagrams and explanations to aid further study.
Here are the key points about stoichiometry from the document:
- Stoichiometry is the calculation of relative quantities in chemical reactions based on molar ratios from chemical formulas and balanced equations.
- Chemical formulas show the elemental composition of compounds using symbols for the elements and subscripts to indicate the number of atoms (e.g. H2O for water, with 1 oxygen and 2 hydrogens).
- Balanced chemical equations show the reactants on the left and products on the right, with coefficients indicating relative quantities such that mass and atoms are conserved in the reaction.
- Molar mass is used to convert between masses of different substances using the relative atomic masses from the periodic table and the quantities indicated by chemical formulas
Similar to chemistry chapter 03 (all sections in one powerpoint) (20)
This document provides an overview of key concepts in chemistry. It discusses the differences between observations and inferences, and emphasizes recording observations rather than inferences in lab exercises. It also covers scientific methodology, including variables, controls, and the scientific method. Measurement concepts like accuracy, precision, error, and significant figures are defined. Formulas for calculating percent error are presented. Key terms like independent and dependent variables are introduced.
This document lists and describes common lab equipment used in chemistry including beakers, Erlenmeyer flasks, graduated cylinders, test tubes, burners, clamps, and more. It explains what each piece of equipment is used for, such as holding liquids (beakers), measuring volumes (graduated cylinders), heating substances (Bunsen burners), and securing items to ringstands (clamps). Safety notes are also provided about proper use and handling of some equipment.
This document outlines several important safety guidelines for working in a lab, including always wearing safety goggles to prevent eye injuries from chemicals or flying objects. Long hair and loose clothing must be secured, and food/drink, backpacks, and horseplay are prohibited in the lab. The location of safety equipment like eyewash stations and fire extinguishers should be known. Proper handling of chemicals, heating procedures, and cleaning of spills are also covered. Any injuries must immediately be reported to the instructor.
This document discusses uncertainty in measurement and significant figures. It explains that measurements have uncertainty due to limitations of instruments. Precision refers to the agreement between repeated measurements while accuracy is the agreement with the true value. There are two types of errors - random errors that can be high or low, and systematic errors that are always in the same direction. The document provides rules for determining the number of significant figures in measurements and calculations, including how significant figures are treated in addition, subtraction, multiplication and division.
The document discusses the SI system of measurement. It defines a measurement as having two parts - a number and a unit. The SI system establishes standard units for seven base quantities: meter (length), kilogram (mass), second (time), ampere (electric current), kelvin (temperature), mole (amount of substance), and candela (luminous intensity). SI prefixes are used to denote multiples and submultiples of units, such as kilo, centi, and milli. Conversions within the metric system involve moving the decimal place in the number to change the unit, as shown through examples converting between liters and milliliters, grams and milligrams, and kilograms and milligrams.
Scientific notation is a method used to write very large or small numbers in a standardized form. It expresses numbers as the product of a number between 1 and 10 and a power of 10. This allows easier calculations with numbers that would otherwise be difficult to work with in standard form due to the number of zeros. Some key points covered are:
- Scientific notation is written as M x 10n, where 1 ≤ M < 10 and n is an integer exponent.
- When adding or subtracting terms with the same exponent, we simply add or subtract the leading numbers and keep the exponent.
- For terms with different exponents, we move the decimal in the number with the smaller exponent to equalize the exponents
The blank periodic table of the elements is an image showing the layout of the periodic table without any element names or properties filled in. It contains the standard 18 columns and 7 rows that organize the 118 known elements based on their atomic structure and properties. This blank template can be used to learn or review the elements and their placement on the periodic table.
chemistry chapter 03 (all sections in one powerpoint)
1.
2. Matter—Properties and Change
Section 3.1 Properties of Matter
Section 3.2 Changes in Matter
Section 3.3 Mixtures of Matter
Section 3.4 Elements and
Compounds
Exit
Click a hyperlink or folder tab to view
the corresponding slides.
3. Section 3.1 Properties of Matter
• Identify the characteristics of a substance.
• Distinguish between physical and chemical
properties.
• Differentiate among the physical states of matter.
density: a ratio that compares the mass of an
object to its volume
4. Section 3.1 Properties of Matter (cont.)
states of matter
solid
liquid
gas
vapor
physical property
extensive property
intensive property
chemical property
Most common substances exist as
solids, liquids, and gases, which have
diverse physical and chemical
properties.
5. Substances
• Matter is anything that has mass and takes
up space.
• Matter is everything around us.
• Matter with a uniform and unchanging
composition is a substance.
6. States of Matter
• The physical forms of matter, either solid,
liquid, or gas, are called the states of
matter.
• Solids are a form of matter that
have their own definite shape and
volume.
• Liquids are a form of matter that
have a definite volume but take the
shape of the container.
7. States of Matter (cont.)
• Gases have no definite shape or
volume. They expand to fill their
container.
• Vapor refers to the gaseous state
of a substance that is a solid or
liquid at room temperature.
8. Physical Properties of Matter
• A physical property is a characteristic that
can be observed or measured without
changing the sample’s composition.
9. Physical Properties of Matter (cont.)
• Extensive properties are dependent on
the amount of substance present, such as
mass, length, or volume.
• Intensive properties are independent of the
amount of substance present, such as
density.
10. Chemical Properties of Matter
• The ability of a substance to combine with
or change into one or more other
substances is called a chemical property.
– Iron forming rust
– Copper turning green in the air
11. Observing Properties of Matter
• A substance can change form–an
important concept in chemistry.
• Chemical properties can change with specific
environmental conditions, such as
temperature and pressure.
12. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
Section 3.1 Assessment
Density is what kind of property?
A. atomic
B. intensive
C. extensive
D. dependent
13. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
Section 3.1 Assessment
What defines a gas?
A. Gases have a definite volume
and shape.
B. Gases have a definite volume but
take the shape of their container.
C. Gases have no definite volume
or shape.
D. Gases have a definite shape but
no definite volume.
14.
15. Section 3.2 Changes in Matter
• Define physical change and list several common
physical changes.
• Define chemical change and list several indications
that a chemical change has taken place.
• Apply the law of conservation of mass to chemical
reactions.
observation: orderly, direct information gathering
about a phenomenon
16. Section 3.2 Changes in Matter (cont.)
physical change
phase change
chemical change
law of conservation of mass
Matter can undergo physical and
chemical changes.
17. Physical Changes
• A change that alters a substance without
changing its composition is known as a
physical change.
• A phase change is a transition of matter from
one state to another.
• Boiling, freezing, melting, and condensing all
describe phase changes in chemistry.
18. Chemical Changes
• A change that involves one or more
substances turning into new substances is
called a chemical change.
• Decomposing, rusting, exploding, burning, or
oxidizing are all terms that describe chemical
changes.
19. Conservation of Mass
• The law of conservation of mass states
that mass is neither created nor destroyed
in a chemical reaction, it is conserved.
• The mass of the reactants equals the mass of
the products.
massreactants = massproducts
20. Section 3.2 Assessment
When one substances turns into another,
what kind of change has taken place?
A. chemical reaction
B. physical reaction
C. extensive reaction
D. nuclear reaction
A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
21. The law of conservation of mass states
that:
A. Matter can be created and destroyed.
B. Matter can be created but not destroyed.
C. The products of a reaction always
A. A
B. B
C. C
D. D
Section 3.2 Assessment
0% 0% 0% 0%
A
B
C
D
have a greater mass than the
reactants.
D. The products of a reaction must
have the same mass as the
reactants.
22.
23. Section 3.3 Mixtures of Matter
• Contrast mixtures and substances.
• Classify mixtures as homogeneous or
heterogeneous.
• List and describe several techniques used to
separate mixtures.
substance: a form of matter that has a uniform and
unchanging composition; also known as a pure
substance
24. Section 3.3 Mixtures of Matter (cont.)
mixture
heterogeneous mixture
homogeneous mixture
solution
filtration
distillation
crystallization
sublimation
chromatography
Most everyday matter occurs as
mixtures—combinations of two or
more substances.
25. Mixtures
• A mixture is a combination of two or more
pure substances in which each pure
substance retains its individual chemical
properties.
• A homogenous mixture is a mixture where
the composition is constant throughout.
26. Mixtures (cont.)
• Homogeneous mixtures are also called
solutions.
• A heterogeneous mixture is a mixture
where the individual substances remain
distinct.
28. Separating Mixtures
• Filtration is a technique that uses a porous
barrier to separate a solid from a liquid in a
heterogeneous mixture.
• Distillation is a separation technique for
homogeneous mixtures that is based on the
differences in boiling points of substances.
• Crystallization is a separation technique for
homogenous mixtures that results in the
formation of pure solid particles from a
solution containing the dissolved substance.
29. Separating Mixtures (cont.)
• Sublimation is the process of a solid
changing directly to a gas, which can be
used to separate mixtures of solids when
one sublimates and the other does not.
• Chromatography is a technique that
separates the components of a mixture on the
basis of tendency of each to travel across the
surface of another material.
30. Section 3.3 Assessment
Which is NOT a technique for separating a
homogenous mixture?
A. crystallization
B. distillation
C. filtration
D. chromatography
A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
31. Which of the following is a heterogeneous
mixture?
A. seawater
B. silver mercury amalgam
C. atmosphere
D. salad dressing
A. A
B. B
C. C
D. D
Section 3.3 Assessment
0% 0% 0% 0%
A
B
C
D
32.
33. Section 3.4 Elements and Compounds
• Distinguish between elements and compounds.
• Describe the organization of elements in the periodic
table.
• Explain how all compounds obey the laws of definite
and multiple proportions.
proportion: the relation of one part to another or
to the whole with respect to quantity
34. Section 3.4 Elements and Compounds (cont.)
element
periodic table
compound
law of definite proportions
percent by mass
law of multiple proportions
A compound is a combination of two or
more elements.
35. Elements
• An element is a pure substance that cannot
be separated into simpler substances by
physical or chemical means.
• 92 elements occur naturally on Earth.
• Each element has a unique name and a one,
two, or three-letter symbol.
• The periodic table organizes the elements
into a grid of horizontal rows called periods
and vertical columns called groups.
36. Compounds
• A compound is a made up of two or more
elements combined chemically.
• Most of the matter in the universe exists as
compounds.
• Table salt, NaCl, and water, H2O, are
compounds.
37. Compounds (cont.)
• Elements can never be separated.
• Compounds can be broken into components
by chemical means.
38. Compounds (cont.)
• This figure shows
electrolysis of
water to form
hydrogen and
oxygen.
39. Compounds (cont.)
• The properties of a compound are different
from its component elements.
40. Law of Definite Proportions
• The law of definite proportions states
that a compound is always composed of
the same elements in the same proportion
by mass, no matter how large or small the
sample.
41. Law of Definite Proportions (cont.)
• The relative amounts are expressed as
percent by mass, the ratio of the mass of
each element to the total mass of the
compound expressed as a percentage.
42. Law of Definite Proportions (cont.)
• This table demonstrates that the percentages of
elements in sucrose remain the same despite
differences in sample amount.
43. Law of Multiple Proportions
• The law of multiple proportions states
that when different compounds are formed
by a combination of the same elements,
different masses of one element combine
with the same relative mass of the other
element in whole number ratios.
– H2O2 and H2O
– Copper(I) chloride and copper(II) chloride
45. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
Section 3.4 Assessment
What is a period on the periodic table of
the elements?
A. a vertical columns
B. even numbered elements only
C. horizontal rows
D. the last vertical column only
46. An element is a substance that cannot be
A. divided into simpler substances.
B. combined to form a mixture.
C. combined to form an element.
D. different phases.
A. A
B. B
C. C
D. D
Section 3.4 Assessment
0% 0% 0% 0%
A
B
C
D
47.
48. Chemistry Online
Study Guide
Chapter Assessment
Standardized Test Practice
Image Bank
Concepts in Motion
49. Section 3.1 Properties of Matter
Key Concepts
• The three common states of matter are solid, liquid,
and gas.
• Physical properties can be observed without altering a
substance’s composition.
• Chemical properties describe a substance’s ability to
combine with or change into one or more new
substances.
• External conditions can affect both physical and
chemical properties.
50. Section 3.2 Changes in Matter
Key Concepts
• A physical change alters the physical properties of a
substance without changing its composition.
• A chemical change, also known as a chemical reaction,
involves a change in a substance’s composition.
• In a chemical reaction, reactants form products.
• The law of conservation of mass states that mass is
neither created nor destroyed during a chemical
reaction; it is conserved.
massreactants = massproducts
51. Section 3.3 Mixtures of Matter
Key Concepts
• A mixture is a physical blend of two or more pure
substances in any proportion.
• Solutions are homogeneous mixtures.
• Mixtures can be separated by physical means.
Common separation techniques include filtration,
distillation, crystallization, sublimation, and
chromatography.
52. Section 3.4 Elements and Compounds
Key Concepts
• Elements cannot be broken down into simpler
substances.
• Elements are organized in the periodic table of the
elements.
• Compounds are chemical combinations of two or more
elements and their properties differ from the properties
of their component elements.
53. Section 3.4 Elements and Compounds
(cont.) Key Concepts
• The law of definite proportions states that a
compound is always composed of the same
elements in the same proportions.
• The law of multiple proportions states that if elements
form more than one compound, those compounds will
have compositions that are whole-number multiples of
each other.
54. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
Which of the following is NOT a physical
property of water?
A. Ice melts at 0°C.
B. Water boils at 100.
C. Water reacts violently with
pure sodium.
D. Water is a liquid at room
temperature.
55. 28.0 grams of nitrogen gas reacts
completely with 6.0 grams of hydrogen to
form 34.0 grams of ammonia. What does
this demonstrate?
A. the law of conservation of energy
B. sublimation
C. distillation
D. the law of conservation of mass
A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
56. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
What is the best way to separate salt
dissolved in water?
A. sublimation
B. crystallization
C. freezing
D. filtration
57. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
Two or more elements chemically joined
form what?
A. substance
B. heterogeneous mixture
C. homogenous solution
D. compound
58. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
What is the ratio of oxygen to carbon in
carbon dioxide (CO2)?
A. 2:1
B. 1:2
C. 1:1
D. 1:3
59. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
Which is NOT a chemical reaction?
A. a car rusting
B. dissolving sugar in water
C. wood burning
D. a banana ripening
60. Which describes a substance that is in the
liquid state?
A. It has a definite shape.
B. It has no definite volume.
C. It can be compressed into a
A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
smaller volume.
D. It has a definite volume.
61. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
Elements in the same period are likely to
have similar ____.
A. physical properties
B. densities
C. chemical properties
D. melting points
62. Filtration is an easy way to separate what?
A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
A. heterogeneous mixture
B. homogeneous mixture
C. compounds
D. solutions
63. A. A
B. B
C. C
D. D
0% 0% 0% 0%
A
B
C
D
Compounds can be broken into their
component elements by which of the
following?
A. crystallization
B. distillation
C. filtration
D. chemical reaction
73. 3.4 Three Common States of Matter
3.10 Conservation of Mass
3.3 Types of Solution Systems
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