... Topics 2 Chapter 1 Topics Matter and its Classification Physical and Chemical Changes and Properties of Matter Energy and Energy Changes (skip) Scientific Inquiry Chapter 1 Math Toolboxes Scientific Notation (exponential notation) Significant Figures Units and Conversions Chem 100 Spring 2014 Classification of Matter Chemistry is a branch of physical science, concerned with the study of the composition, properties and behavior of matter. Matter is anything that occupies space and has mass. Forms of energy are NOT matter. Heat and light, for example, do not occupy space and have no mass. Consider the different forms of matter and energy in this picture. 3 Chem 100 Spring 2014 Classification of Matter We classify matter so that we can understand it better. One way to classify matter is as pure substances or mixtures. 4 Matter Pure Substances Mixtures Chem 100 Spring 2014 Classification of Matter – Pure Substances Pure Substances: have the same composition throughout, and from sample to sample. can be further classified as either elements or compounds. 5 Pure Substances Elements Compounds Chem 100 Spring 2014 Pure Substances - Elements An element is a substance that cannot be broken down into simpler substances even by a chemical reaction. 6 Chem 100 Spring 2014 Elements and their Symbols Element symbols often consist of one or two letters of the element’s name. Examples:...
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...Chapter 5: Properties of Matter Matter is anything that has a mass and takes up space. The particle theory of matter is a theory that describes the composition and behavior. Matter can be many up of many different particles or only one. A pure substance is a type of matter that consists of only one type of particle. Then there are mixtures that are made up of at least two different types of particles. There are two different types of mixtures; mechanical mixtures and solutions. A mechanical mixture is a mixture in which the substances in it are distinguishable from each other, either with the unaided eye or a microscope. A solution looks like a pure substance but it contains more than one type of particle. Alloys are when two or more metals are mixed together. A physical property is a characteristic of a substance that can be determined without changing the composition of that substance. A qualitative physical property is not measured and includes hardness, malleability and electrical conductivity. Quantitative physical properties are measured and include temperature, height and mass. A physical change is a change is which the composition of the substance remains unaltered and no new substances are produced Examples of physical change are a change of size or shape, a change of state, and dissolving. A chemical property is a property of a substance that describes its ability to undergo changes to its composition to produce one or more new substances. A chemical; change is a...
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...Food and Agriculture • Genetically modified crops • “Natural” pesticides • Specialized fertilizers • • • Classification of Matter A substance is a form of matter that has a definite composition and distinct properties. An element is a substance that is composed of tiny particles called atoms. A compound is a substance composed of atoms of two or more elements chemically united in fixed proportions. Compounds can only be separated into their pure components (elements) by chemical means. A mixture is a combination of two or more substances in which the substances retain their distinct identities. Physical means can be used to separate a mixture into its pure components. Homogenous mixture – composition of the mixture is the same throughout. Heterogeneous mixture – composition is not uniform throughout. 1 |P a g e _____________________________________________________________________CHEM 100 LECTURE PROPERTIES OF MATTER Physical properties: readily observable/measurable without altering the composition or identity of a substance. (mass, color, density, boiling point) Chemical properties: can only be observed by altering the composition or identity of the substance(s) involved. (combustibility, flammability, oxidizability) An extensive property of a material depends upon how much matter is being...
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...CHEMISTRY CHEMISTRY (CLASSES XI–XII) Rationale Higher Secondary Stage is the most crucial stage of school education because at this stage specialised discipline based, content oriented courses are introduced. Students reach this stage after 10 years of general education and opt for Chemistry with a purpose of mostly for pursuing their career in basic sciences or professional courses like medicines, engineering, technology and studying courses in applied areas of science and technology at tertiary level. Therefore, at this stage, there is a need to provide learners with sufficient conceptual background of Chemistry, which will make them competent to meet the challenges of academic and professional courses after the higher secondary stage. National Curriculum Framework for School Education – 2005 recommends a disciplinary approach with appropriate rigour and depth with the care that syllabus is not heavy and at the same time it is comparable to the international level. It emphasizes a coherent focus on important ideas within the discipline that are properly sequenced to optimize learning. It recommends that theoretical component of Higher Secondary Science should emphasize on problem solving methods and the awareness of Syllabus for Secondary and Higher Secondary Levels 22 historical development of key concepts of science be judiciously integrated into content. The present exercise of syllabus development in Chemistry at Higher Secondary Stage is based on this framework...
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...vibrate, move about, and slide past each other. * solid vibrate (jiggle) but generally do not move from place to place. Liquids and solids are often referred to as condensed phases because the particles are very close together. The following table summarizes properties of gases, liquids, and solids and identifies the microscopic behavior responsible for each property. Some Characteristics of Gases, Liquids and Solids and the Microscopic Explanation for the Behavior | gas | liquid | solid | assumes the shape and volume of its container particles can move past one another | assumes the shape of the part of the container which it occupies particles can move/slide past one another | retains a fixed volume and shape rigid - particles locked into place | compressible lots of free space between particles | not easily compressible little free space between particles | not easily compressible little free space between particles | flows easily particles can move past one another | flows easily particles can move/slide past one another | does not flow easily rigid - particles cannot move/slide past one another | ------------------------------------------------- Chemical or Physical? Physical changes do not cause a...
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...PHYSICAL CHANGE Physical changes are changes affecting the form of a chemical substance, but not its chemical composition. Physical changes are used to separate mixtures into their component compounds, but cannot usually be used to separate compounds into chemical elements or simpler compounds.[1] Physical changes occur when objects or substances undergo a change that does not change their chemical composition. This contrasts with the concept of chemical change in which the composition of a substance changes or one or more substances combine or break up to form new substances. In general a physical change is reversible using physical means. For example salt dissolved in water can be recovered by allowing the water to evaporate. A physical change involves a change in physical properties. Examples of physical properties include melting, transition to a gas, change of strength, change of durability, changes to crystal form, textural change, shape, size, colour, volume and density. An example of a physical change is the process of tempering steel to form a knife blade. A steel blank is repeatedly heated and hammered which changes the hardness of the steel, its flexibility and its ability to maintain a sharp edge. Methods Heating and cooling Many elements and some compounds change from solids to liquids and from liquids to gases when heated and the reverse when cooled. Some substances such as iodine and carbon dioxide go directly from solid to gas in a process called sublimation...
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...solution.This crystallised slat contains much less of the impurity than before. The salt can then be filtered and dried.Sugar cane industry. | Assess separation techniques for their suitability in separating examples of earth materials, identifying the differences in properties which enable these separations Yes, fractional distillation can separate a mixture of oxygen and nitrogen because they have similar (but not the same) boiling points. Could filtration successfully separate sand from a sand-salt mixture? No. Without water the salts in the sand and salt mixture will not separate out via filtration because filtration requires an insoluble solid plus a liquid mixture, which in this case would be salt + water Describe situations in which gravimetric analysis supplies useful data for chemists and other scientists * the process of determining the % by mass of one substance in a mixture * It is used to determine whether mining is economically feasible * to determine the composition of compounds in soil to determine whether the soil is appropriate for growing certain crops * to determine the percentage of particular pollutants in water Apply systematic naming of inorganic compounds as they are...
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...they can no longer hold each other, this forms the liquid state * if they are continued to be heated the particles literally fly apart 3. The difference between pure substances and mixtures: * pure substance: contains only one type of particle * element: a pure substance that can not be broken down into a simpler chemical substance by any physical or chemical means * compound: a pure substance composed of 2 or more different elements that are chemically joined * mixture: contains 2 or more types of particles * mechanical mixture: a mixture in which you can distinguish between different types of matter * solution: a uniform mixture of 2 or more substances 4. Difference between quantitative and qualitative properties: * quantitative property: a property of a substance that is measured and has a numerical value, such as temperature, heat and mass * qualitative property: a property of a substance that is not measured and does not have a numerical value such as colour, odour and texture 5. Physical properties vs. chemical properties: * physical property: a characteristic of a substance that can be determined without changing the composition of that substance * chemical property: a characteristic of a substance that is determined when the composition of the substance is...
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...------------------------------------------------- When elements are arranged in the order of increasing atomic number, their physical and chemical properties recur periodically. This periodicity stems from the valence electronic configurations of the elements. This arrangement of the elements on the order of increasing atomic number with the elements having similar properties placed in vertical columns is known as the periodic table. INTRODUCTION This Experiment is all about for determining the given compound. In this Experiment we try to observe the physical state, color, appearance and the reaction of a compound on a litmus paper. MATERIALS AND METHODS In this experiment, we use Test tubes to observe the difference between the elements. 10 ml graduated cylinder to measure the water. Spatula, we used this to put the elements on the test tubes. We used Litmus Paper to determine maybe acid or base the elements. On this Activity, We try to identify the Physical state, Color, and Appearance of different elements. Li2 CO3 K2CO3 CaCO3 Na2CO3 MGCO3 BaCO3 On the first Procedure, We put a small amount of a elements samples Li2CO3 , K2CO3, CaCO3, Na2CO3, MGCO3 and BaCO3 in the different test tubes. We put 10ml water on the different test tubes. After adding we stir it and observe. We use a Litmus Paper to determine the elements maybe acid or base. On the Second Procedure, We get also a small amount of other elements C, Sn, Si and Pb and we placed it also in different...
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...Introduction to Chemistry I (MAE1106) Chapter 1: Properties, Measurement and Units Matter: All things we can see, or touch, whether books, pencils, telephones, or people as they have some thing in common. They are all composed of matter which is defined as anything that takes up space and has mass. Matter is generally considered to be a substance (often a particle) that has rest mass and (usually) also volume. Mass and weight are not really the same. The mass of a body is a measure of its resistance to a change in its velocity. Weight refers to the force with which an object of a certain mass is attracted by gravity to the earth or other body that may be near such as moon. The volume is determined by the three-dimensional space it occupies, while the mass is defined by the usual ways that mass is measured. Matter is also a general term for the substance of which all observable physical objects consist Properties of Substances Physical (Properties and Changes) A physical property is one that is displayed without any change in composition. (Intensive or Extensive) 1. Intensive: A physical property that will be the same regardless of the amount of matter. density: m/v • color: The pigment or shade • conductivity: electricity to flow through the substance • malleability: if a substance can be flattened • luster: how shiny the substance looks 2. Extensive: A physical property that will change if the amount of matter changes. • mass: how much...
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...different areas in Medical Education. PHYSICS S.No. 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. CLASS XI Physical world and measurement Kinematics Laws of Motion Work, Energy and Power Motion of System of Particles and Rigid Body Gravitation Properties of Bulk Matter Thermodynamics Behaviour of Perfect Gas and Kinetic Theory Oscillations and Waves CLASS XII Electrostatics Current Electricity Magnetic Effects of Current and Magnetism Electromagnetic Induction and Alternating Currents Electromagnetic Waves Optics Dual Nature of Matter and Radiation Atoms and Nuclei Electronic Devices CHEMISTRY S.No. 1. 2. 3. 4. 5. 6. 7. 8. 9. 10. 11. 12. 13. 14. 15. 16. CLASS XI Some Basic Concepts of Chemistry Structure of Atom Classification of Elements and Periodicity in Properties Chemical Bonding and Molecular Structure States of Matter: Gases and Liquids Thermodynamics Equilibrium Redox Reactions Hydrogen s-Block Element (Alkali and Alkaline earth metals) Some p-Block Elements Organic Chemistry- Some Basic Principles and Techniques Hydrocarbons Environmental Chemistry CLASS XII Solid State Solutions Electrochemistry Chemical Kinetics Surface Chemistry General Principles and Processes of Isolation of Elements p- Block Elements d and f Block Elements Coordination Compounds Haloalkanes and Haloarenes Alcohols, Phenols and Ethers Aldehydes, Ketones and Carboxylic Acids Organic Compounds Containing Nitrogen Biomolecules Polymers...
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...Atoms are building blocks, all matter is composed of indivisible particles called atoms. All atoms consist of subatomic particles called; protons, neutrons and electrons. Atoms cannot be created or destroyed but can be rearranged to from different substances. Compounds and elements are composed of tiny particles known as molecules, molecules are specified as atoms that are affiliated (combined) by chemical bonds—the joining of two or more atoms. Compounds are molecules containing at least two or more different elements, all compounds are molecules but not all molecules are compounds. A mixture is a substance that combines two or more compounds and elements in a way where no chemical reaction occurs. The mixture can then be homogeneous or heterogeneous, a homogeneous mixture has components distributed consistently throughout the mixture and example of this would be air, vodka or rain water. Heterogeneous mixtures components are not consistent, they have restricted sections with...
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...Lab Report for Experiment #4 Physical and Chemical Properties and Changes Student's Name __________ __________ Date of Experiment ___ _________ Date Report Submitted _________________ Title: (copy from lab, 1 point) Purpose: (copy from lab, 1 point) Changes to the Procedure by Instructors: 1. Do not test the odor of the samples. 2. In this lab the test tubes can get very dirty and cleaning is difficult. Your test tube may break, but don’t worry about it you will not need them again this term. Dispose carefully in the trash. Have you made any changes to the procedure? Please explain: Fill out the data sheet (page 3) for the experiment and answer the questions. Note: read the lab introduction for clarification on the difference between physical and chemical changes. Remember that a physical change often occurs during a chemical change, but a chemical change does not always happen when a physical change occurs. If you still have questions ask your instructor. From experiment # 1 we learned that a chemical change results in a color change, the formation of bubbles, the formation of a precipitate, or a change of temperature. Keep that in mind when you are deciding whether a physical or chemical change has occurred. Data Table (8 points) Read carefully before you begin your experiment! Be complete when writing your observations. One word observations are not usually complete. If there is a color change, include the color before and after. For...
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...CHAPTER ONE INTRODUCTION: MATTER AND MEASUREMENT The Study of Chemistry Chemistry: • is the study of properties of materials and changes that they undergo. • can be applied to all aspects of life. The Atomic and Molecular Perspective of Chemistry Chemistry involves the study of the properties and the behavior of matter. Matter: • is the physical material of the universe. • has mass. • occupies space. Examples of matter: ~100 elements constitute all matter. A property is any characteristic that allows us to recognize a particular type of matter and to distinguish it from other types of matter. Elements: • are made up of unique atoms, the building blocks of matter. • approximately 116 elements. • names of the elements are derived from a wide variety of sources. Molecules: • are combinations of atoms held together in specific shapes. • Macroscopic (observable) propertied of matter relate to submicroscopic realms of atoms • Properties relate to composition (types of atoms present) and structure (arrangement of atoms present. [pic] • Combinations of atoms held together in specific shapes CH3CH2OH HOCH2CH2OH Ethyl alcohol ethylene glycol Why study Chemistry? We study chemistry because: • It has a considerable impact on society (health care, food, clothing, conservation of natural resources, environmental issues...
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...how Mendeleev arranged the elements, known at that time, in a periodic table by using properties of these elements and their compounds and used his table to predict the existence and properties of some elements not then discovered ● Classify elements as metals or non-metals according to their position in the periodic table ● Describe the structure of an atom as a nucleus containing protons and neutrons, surrounded by electrons in shells (energy levels) ● Demonstrate an understanding that the nucleus of an atom is very small compared to the overall size of the atom ● Describe atoms of a given element as having the same number of protons in the nucleus and that this number is unique to that element ● Recall the relative charge and relative mass of a proton, a neutron and an electron ● Demonstrate an understanding that atoms contain equal numbers of protons and electrons ● Explain the meaning of the terms, atomic number, mass number and relative atomic mass ● Describe the arrangement of elements in the periodic ● Demonstrate an understanding that the existence of isotopes results in some relative atomic masses not being whole numbers ● Calculate the relative atomic mass of an element from therelative masses and abundances of its isotopes ● Draw the electronic configurations of the first 20 elements in the periodic table as diagrams and in the form 2.8.1 ● Describe the connection between the number of outer electrons and the position of an element in the periodic table ...
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