ch. 3: matter and energy
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Ch. 3: Matter and Energy. Dr. Namphol Sinkaset Chem 152: Introduction to General Chemistry. I. Chapter Outline. Introduction Classifying Matter Physical/Chemical Properties/Changes Conservation of Matter Energy Temperature Heat Capacity. I. Introduction. - PowerPoint PPT PresentationTRANSCRIPT
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Ch. 3: Matter and EnergyCh. 3: Matter and Energy
Dr. Namphol Sinkaset
Chem 152: Introduction to General Chemistry
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I. Chapter OutlineI. Chapter Outline
I. Introduction
II. Classifying Matter
III. Physical/Chemical Properties/Changes
IV. Conservation of Matter
V. Energy
VI. Temperature
VII. Heat Capacity
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I. IntroductionI. Introduction
• Everything around you is composed of matter.
• Besides matter, energy is the other major component of our universe.
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II. MatterII. Matter
• Matter is anything that occupies space and has mass.
• Some matter is easy to see (water, wood), others are difficult (air, dust).
• The most basic building block of matter is the atom.
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II. Atoms and MoleculesII. Atoms and Molecules
• atoms: submicroscopic particles that are the fundamental building blocks of all matter.
• Sometimes, atoms are bonded together to form molecules.
• molecules: two or more atoms joined to one another in specific geometric arrangements.
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II. Atomic and Molecular II. Atomic and Molecular MatterMatter
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II. Actual Images of Atoms II. Actual Images of Atoms and Moleculesand Molecules
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II. States of MatterII. States of Matter
• Matter can be classified by its state.• solid: closely-packed particles with fixed
locations• liquid: closely-packed particles, but free to
move around• gas: great distances between particles with
free movement
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II. States of MatterII. States of Matter
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II. The Solid StateII. The Solid State
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II. Properties of Different StatesII. Properties of Different States
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II. Pure Substances and II. Pure Substances and MixturesMixtures
• Matter can be classified by its composition.
• pure substance: matter composed of only one type of atom or molecule
• mixture: matter composed of two or more different types of atoms or molecules which may vary in proportion
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II. ElementsII. Elements
• element: a pure substance that cannot be broken down into simpler substances
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II. CompoundsII. Compounds
• compound: a pure substance composed of two or more elements in fixed definite proportions.
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II. MixturesII. Mixtures• Most matter exists in this form.• heterogeneous: varied composition from one
region to another• homogeneous: uniform composition throughout
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II. Classification by II. Classification by CompositionComposition
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II. Sample ProblemII. Sample Problem
• Classify the following as a pure substance or mixture. Further classify them as an element, compound, homogeneous, or heterogeneous.a) blood
b) sugar
c) mercury in a thermometer
d) chicken noodle soup
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III. Distinguishing MatterIII. Distinguishing Matter
• We use physical and chemical properties to tell the difference between samples of matter.
• physical property: a property a substance displays without changing its composition
• chemical property: a property a substance displays only by changing its composition
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III. Boiling Point of WaterIII. Boiling Point of Water
• At the boiling point, water is converted to steam, but steam is just a different form of water.
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III. An Iron Nail RustsIII. An Iron Nail Rusts• When iron rusts, it must react and incorporate
oxygen to become a new compound.
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III. Sample ProblemIII. Sample Problem
• Identify the following as physical or chemical properties.a) Hydrogen gas is explosive.
b) Silver has a shiny appearance.
c) Dry ice sublimes (goes from solid directly to vapor).
d) Copper turns green when exposed to air.
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III. Physical/Chemical ChangesIII. Physical/Chemical Changes
• Physical/chemical changes are closely related to definitions of physical/chemical properties.
• physical change: matter changes its appearance, but not its composition
• chemical change: matter changes its composition
• Chemical changes occur through chemical reactions in which reactants become products.
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III. Physical/Chemical ChangesIII. Physical/Chemical Changes
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III. Sample ProblemIII. Sample Problem
• Categorize the following as either a physical or chemical change.a) Copper metal forming a blue solution
when dropped in concentrated nitric acid.
b) A train flattening a penny.
c) A match igniting a firework.
d) Ice melting into liquid water.
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IV. There is No New MatterIV. There is No New Matter
• In ordinary chemical reactions, matter is neither created nor destroyed.
• Known as Conservation of Mass.
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V. EnergyV. Energy
• Physical and chemical changes are accompanied by energy changes.
• energy: the capacity to do work• work: results from a force acting on a distance
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V. Two Types of EnergyV. Two Types of Energy
• potential energy (PE): energy due to the position or composition of the object
• kinetic energy (KE): energy due to motion of the object
• An object’s total energy is the sum of its PE and KE
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V. Energy ConversionsV. Energy Conversions
• The Law of Conservation of Energy states that energy is neither created nor destroyed.
• Energy can change from one form to another or transferred from one object to another.
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V. Specific Types of EnergyV. Specific Types of Energy• Electrical energy is the energy
associated with the flow of electrical charge.
• Thermal energy is the energy associated with motions of particles of matter.
• Chemical energy is a form of PE associated with positions of particles in a chemical system.
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V. Energy Unit ConversionsV. Energy Unit Conversions
• There are three common units for energy.
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V. Sample ProblemV. Sample Problem
• The complete combustion of a wooden match produces about 512 cal of heat. How many kilojoules are produced?
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V. System and SurroundingsV. System and Surroundings
• When describing energy changes, we need reference points.
• system: object of study
• surroundings: everything else
• Systems with high PE tend to change such that their PE is lowered.
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V. Energy DiagramsV. Energy Diagrams
• Chemical reactions can either be exothermic or endothermic.
• exothermic: release energy to surroundings
• endothermic: absorb energy from surroundings
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V. Sample ProblemV. Sample Problem
• Identify the following changes as exothermic or endothermic.a) Water freezing into ice.
b) Propane burning.
c) Isopropyl alcohol evaporating from skin.
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VI. Thermal EnergyVI. Thermal Energy
• Atoms and molecules of matter are in constant, random motion, which is the source of thermal energy.
• More motion = more thermal energy.
• Is there a way to easily measure this motion?
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VI. Temperature and HeatVI. Temperature and Heat
• Temperature is the measure of the thermal energy of a substance.
• The hotter an object, the greater the motion of its particles, and the greater the thermal energy.
• Heat is the transfer or exchange of thermal energy caused by a temperature difference.
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VI. Temperature ScalesVI. Temperature Scales
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VI. Temperature ConversionsVI. Temperature Conversions
• The formulas below allow conversion between different temperature units.
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VI. Sample ProblemVI. Sample Problem
• Convert 67 °F to kelvin and degrees Celsius.
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VII. Heating a SubstanceVII. Heating a Substance
• When you heat a substance, its temperature changes.
• The amount of change depends on the substance.
• heat capacity: quantity of heat needed to raise the temp of substance by 1 °C
• specific heat capacity: quantity of heat needed to raise temp of 1 g of substance by 1 °C
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VII. Specific Heat CapacitiesVII. Specific Heat Capacities
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VII. Energy and Heat CapacityVII. Energy and Heat Capacity
• Heat absorbed and temperature change are directly related as shown in the equation below.
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VII. Sample ProblemVII. Sample Problem
• Calculate the heat necessary to warm a 3.10 g sample of copper from -5.0 °C to 37.0 °C if the specific heat capacity of copper is 0.385 J/g °C.
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VII. Sample ProblemVII. Sample Problem
• A sample of lead (C = 0.128 J/g °C) absorbs 11.3 J of heat, rising in temperature from 26 °C to 38 °C. Find the mass of the sample in grams.
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VII. Sample ProblemVII. Sample Problem
• A 328-g sample of water absorbs 5.78 kJ of heat. If the water sample has an initial temperature of 35.3 °C, what will be its final temperature? Note that C = 4.18 J/g °C for water.