Classification of Matter Unit 3.3: Classification of Matter Vocabulary: matter, mass, volume, substance, chemical change, physical change, state, particle, gas, liquid, solid, attract

Vocabulary: system phase atom molecule compound ion mixture homogeneous substance heterogeneous substance solution solvent solute

2.3: Classification of matter System: the entire “universe” being studied Phase: any part of the system that is uniform in composition and properties ex: oil and water You can see the boundary between the oil and water. This is a 2 phase system

2.3: Classification of matter Atom: the smallest unit of an element Cannot be broken down into a simpler type of matter Ex: Ag (silver), C (carbon) Molecule: 2 or more atoms held together Ex: H2O, NaCl, H2

2.3: Classification of matter Ion: an atom or molecule with a charge Ex: Na+, Cl-, NO3-, NH4+ Atoms gain or lose electrons to form an ion

DESCRIBING MATTER:

Classifying Matter Matter

Classifying Matter Matter Pure Substances

Classifying Matter Matter Pure Substances Mixtures

Pure Substance  A substance that is homogeneous and has an unchangeable composition Examples: sugar, water, copper, iron Mixture  A system made up of two or more substances, such as the relative amounts can be VARIED (different) Examples: Salt dissolved in water

2.1 Elements - The Most Simple Kind of Matter Pure Substance: “Something that with a uniform, fixed composition at the submicroscopic level” Recognized by the unchanging nature of their properties Element: “A pure substance composed of only one kind of atom” Atom: “The smallest particle of an element” Atoms of different elements are different and are shown on the periodic table Each element has a one or two letter abbreviation Hydrogen - H Helium - He Sodium - Na Lithium - Li S 2.0 The Chemical View of Matter

Classifying Matter Matter Pure Substances Mixtures Elements Compounds/molecules

2.3: Classification of matter Mixture: a group of 2 or more substances that are physically mixed there are homogeneous and heterogeneous mixtures

Examples: Air, water, salt water, a piece of iron Homogeneous: A substance consisting of only ONE PHASE (gas, liquid, or solid) Examples: Air, water, salt water, a piece of iron Heterogeneous: A substance consisting of MORE THAN one phase (gas, liquid, and/or solid) Examples: A human being, a pencil

2.3 Mixtures and Pure Substances Homogeneous Sample: “ Matter that has a uniform appearance and composition throughout “ A mixture of water and alcohol Sugar dissolved in water Gold blended with silver (18 karat gold) The air we breathe - a mixture of oxygen and nitrogen Solutions: “Homogeneous mixtures, either liquid, solid or gaseous” continue….. S 2.0 The Chemical View of Matter

Homogeneous Mixtures Homo means “same” Looks like one substance 1 phase Called solutions  ex: milk tea, water and salt

Heterogeneous Mixtures Hetero means “different” You can see all the different parts of the mixture Called mechanical mixtures  ex: m&m’s, sand and water

Sand and water do not mix to form a uniform mixture Copyright 1999, PRENTICE HALL Chapter 1

3.3 Mixtures: The substances are mixed together but are not chemically combined mixtures can be separated into their parts by physical changes

Solution: homogeneous mixtures of 2 or more substances Solvent: dissolves things (usually bigger quantity) Solute: gets dissolved (usually smaller quantity) Example: salt and water Solvent = Solute =

NaCl(s) + H2O(l)  NaCl(aq) Aqueous solutions are solutions where the solvent is water. NaCl(s) + H2O(l)  NaCl(aq) (aq) = aqueous

Types of Solutions Type of Solution Example Gas-in-Gas solution Air (Nitrogen, Oxygen) Gas-in-Liquid solution Soda Pop (Coke Zero…MMMMM!) Liquid-in-Liquid solution Water and alcohol Solid-in-Liquid solution Salt water Solid-in-Solid solution Alloys (Metals melted together)

Classifying Matter Matter Pure Substances Mixtures Elements Compounds/molecules Classify followings as pure substances and mixtures? a. Sugar b. dirt c. air

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous

2.3: Classification of matter Compound: pure substance made up of 2 or more different atoms Ex: H2O, NaCl, C6H12O6 All compounds are also molecules Not all molecules are compounds (ex: H2, O2) are molecules NOT compounds

2.2 Chemical Compounds (cont) Compound: “ Any pure substance that can be decomposed by a chemical change into two or more pure substances is a compound “ - (another definition) Compounds are made up of elements Examples of Compounds: Water - H2O Ethanol - C2H6O Salt - NaCl Sugar - C6H12O6 Examples of Mixtures of Compounds: Pepper Beer, Wine & Soda Pop Milk Cheese continue….. S 2.0 The Chemical View of Matter

2.2 Chemical Compounds - Atoms in Combination Chemical Compounds: “ Pure substances made of atoms of different elements combined in definite ways” Examples: H2O Water NaCl Sodium Chloride C2H6O Ethanol C6H12O6 Sugar S 2.0 The Chemical View of Matter

Classification of Matter Elements There are 114+ elements known. Each element is given a unique chemical symbol (one or two letters). They are building blocks of matter. The earth’s crust consists of 5 main elements (shown next slide). The human body consists mostly of 3 main elements (O, C, and H). Copyright 1999, PRENTICE HALL Chapter 1

The Periodic Table and the Elements Main Group Elements Main Group Elements Transition Metals Inner Transition Elements Copyright 1999, PRENTICE HALL Chapter 1

Classification of Matter Elements Copyright 1999, PRENTICE HALL Chapter 1

Classification of Matter Compounds Most elements interact to form compounds. The proportions of elements in compounds are the same irrespective of how the compound was formed. Law of Constant Composition (or Law of Definite Proportions): The composition of a pure compound is always the same. Therefore, if water is decomposed, then there will always be twice as much hydrogen gas formed as oxygen gas. Copyright 1999, PRENTICE HALL Chapter 1

2.5 Classification of Matter Matter - Anything that occupies space and has mass (solid, liquid or gas) Heterogeneous Mixture: Non-uniform composition Homogeneous Mixture: Uniform composition Physically Separable Into Pure Substances: Fixed composition; cannot be further purified Solution: Homogeneous mixture Physically Separable Into Chemically Separable Into Compounds: Elements united in fixed ratios Elements: Cannot be subdivided by chemical or physical changes Combine Chemically to

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous Classify following as Homogeneous and Heterogeneous Diamond b. Tree c. egg d. Coffee

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous A clear glass bottle contains white sand, some nails, slat water with some dye dissolved in it and a layer of gasoline on top, How many phases are present in the system, excluding the bottle and lid?

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent shiney dull

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent shiney dull conduct nonconductors

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent shiney dull conduct nonconductors ductile brittle

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent shiney dull conduct nonconductors ductile brittle maleable

Classifying Matter Matter Pure Substances Mixtures A Elements B Compounds C Homogenous D Heterogeneous metals nonmetals ionic covalent shiney dull conduct nonconductors ductile brittle maleable left right of periodic table Periodic Table

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2 NaCl(aq)

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2 NaCl(aq) granite

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2 NaCl(aq) granite Co

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2 NaCl(aq) granite Co O2

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2 NaCl(aq) granite Co O2 NH4Cl

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2 NaCl(aq) granite Co O2 NH4Cl C12H22O11

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2 NaCl(aq) granite Co O2 NH4Cl C12H22O11 tea

Classifying Matter Matter Pure Substances Mixtures Elements Compounds Homogenous Heterogeneous metals nonmetals ionic covalent Na Cl2 NaCl NO2 NaCl(aq) granite Co O2 NH4Cl C12H22O11 tea pineapple juice Atom Ion

Can it be physically separated? A. Matter Flowchart MATTER yes no Can it be physically separated? MIXTURE PURE SUBSTANCE Is the composition uniform? no yes Can it be chemically decomposed? no yes Homogeneous Mixture (solution) Heterogeneous Mixture Compound Element Mechanical Suspensions Atom Ions

A. Matter Flowchart element hetero. mixture compound solution Examples: graphite pepper sugar (sucrose) paint soda element hetero. mixture compound solution

Pure Substances (can NOT be separated by physical change) Matter Pure Substances (can NOT be separated by physical change) Elements Metal Na Nonmetal Cl2 Compounds Ionic NaCl Covalent H2O Impure substances (can be separated by physical change) Mixtures Homogeneous salt-in-water Heterogeneous Oil-in-water

Learning Check Classify the following as elements, compounds, or mixtures: a)   Methane  (CH4)                        b)   Pizza                                                         c)   Milkshake                                               d)   Zinc                                                         e)   Laughing gas (N2O)                           f)   Clean air                                                     g)   A chocolate cookie                                          

Learning Check Give an example to show each of the following terms: a)     Matter -                                                    .  b)    Solution -                                                    . c)     Suspension -                                              .  d)    Mechanical mixture -                     . e)     Compound -                                            .  f)     Solution -                                   .  g)     Element -                                 .   

What is the difference between an element and a compound? Reflection Page What is the difference between an element and a compound? Give 3 examples of each.

Explain the difference between heterogeneous and homogenous. Reflection Page Explain the difference between heterogeneous and homogenous.

Reflection Page What is the difference between a solution, and a suspension? Give an example of each.

Workbook page. 52 Question # 33-44 Assignment: Workbook page. 52 Question # 33-44

Assignment:

Assignment:

Assignment: Make 2 questions about todays Lab Unit 3 Topic 1 Make 1 questions (about vapour and vapour pressure) Unit 3 Topic 2 Lab due by Monday(one for group) Tomorrow : Vapour Pressure Lab