classification of matter
DESCRIPTION
Science Explorer Chapter 13TRANSCRIPT
PROPERTIES OF MATTER
Objectives Define matter.
Explain the gas, liquid, and solid states of matter in terms of particles.
Distinguish between the physical properties and chemical properties of matter.
Classify Changes of matter as physical or chemical.
Distinguish between a mixture and a pure substance.
Identify the chemical symbols of elements, and name elements, given their symbols.
Identify important families of elements on the periodic table.
TEKS: 2A,2D,2E,3B,3C,3D,3E,4A,4B,4C,4D,5A,11A,11B
Definition of MatterThe two properties of matter are:
• Mass – amount of matter
• Volume – amount of space occupied
• Therefore…matter is anything that has mass and takes up space.
• The study of Matter is Chemistry.
• Density = Mass (m)/ Volume (V)
• D= m/V or g/mL
Density
Density is the mass of an object divided by its volume.
Density = mass/volumeMass calculated on scale.Measure in SI (Systeme
International) grams
Volume = l x w x h (regular)Cm3 or CC or mL
Volume of an Irregular shape
Volume of sample = final water level − initial water level.
86 mL – 80 mL = 6 mL
Identify Unknown Substances Using density you can identify
substances
Water density is 1.0 g/mL
States of Matter Solid – definite shape and volume ice
Liquid – definite volume, and takes the shape of the container
water
Gas – takes the shape and volume of the container steam
Plasma – a collection of high energy ions and electrons.
Sun• Only place on earth in arc of arc welder
Physical Changes Physical change alters the substance
without changing its composition or chemical identity.
From a solid to a liquid, boil, melt cut break, split , grind crush , bend, condense freeze , dissolve and crack are examples of physical changes.
Physical Properties
A physical property is a condition that can be measured or observed without changing the identity of the substance.
Examples of physical properties include color, solubility, odor, hardness, density, melting point and boiling point, etc.
Chemical Properties
The ability of a substance to undergo a chemical reaction to form a new substance is called a chemical property. Chemical properties are observed when a substance undergoes a chemical change.
Chemical Change A change in which one or more
substances are converted into different substances is called a chemical change or chemical reaction\
Yields
C + O2 CO2
(reactants) (product)
Usually light or heat producedBubbles producedForms a percipitant
Look for terms such as . . .
burn rot rust decompose ferment explode oxidize corrode grow precipitate gas formation digest
Classifying Properties
Both physical and chemical properties can be classified as being either extensive or intensive properties.
Extensive vs. IntensiveExtensive Properties
Depend on the amount of matter present
Mass, volume, length, height, amount of energy, etc.
Intensive Properties
Do not depend on the amount of matter present
Density, boiling point, melting point, color, ability to conduct electricity, etc.
Classifying Matter Matter is classified by the number of
phases it contains.
Any part of a system with uniform composition and properties is called a phase.
Matter can be classified as either Homogeneous or Heterogeneous.
Homogeneous & Heterogeneous
Homo = same Hetero = different• Homogeneous materials exist in only one phase.
• Heterogeneous materials contain more than one phase.• Includes
solutions, compound & elements
• Example:milkshake
• Separate by filter, magnet, distill, evaproration
• Heterogeneous materials are all mixtures
• Example:Salad
• Separate by picking out different particles
Mixtures Mixtures are a physical blend of 2 or
more kinds of matter.
Mixtures can be either homogeneous (solutions) or heterogeneous.
Separation of mixtures is done by physical means such as magnets, distillation, chromatography and filtration.
Pure Substances• A pure substance has a fixed
composition . Elements and compounds are pure substances.
• Unlike mixtures, every sample of a pure substance has exactly the same characteristic properties and composition.
Elements and CompoundsAn element is a collection of the same
type of atom. They are the simplest form of matter that can exist under normal lab conditions.
Atoms are the smallest particle of an element
Compounds consist of two or more elements that are chemically combined. They can be separated only by a chemical change.
Reactants Products Na + Cl(g) NaClSodium + Chlorine Yeilds Sodium Chloride (table
Salt)
Law of Conservation of Mass
“What you start with you have to end with” Matter is neither created or destroyed but
changed from one form to another.Chemical Formula
Coefficient(Reactants)2H2 + O2 2H2O (Product)
Subscript
Forms of EnergyThermal is Heat Energy
Temperature is the measure of average energy.
Endotherimic
Taking in heat Example: ice takes
in heat and melts
Exothermic
Release energy Example: Wood fire
Forms of Energy
Kinetic (motion) Potential (stored) Chemical (battery Li) Electromagnetic (light waves) Electrical (electrically charged particles) Thermal (heat)
You can change from one form to another.
Classification of Matter
Mixtures Pure Substances
Heterogeneous Mixtures
Solutions Compounds
Elements
Homogeneous Matter