Overview of Matter. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE.

Slides:

Advertisements

Similar presentations

Matter: Properties & Change

Advertisements

I. Chemistry As a Physical Science

Ch. 1 - Matter II. Classification of Matter (p.15-17, )

Ch. 1 – Matter and Its Properties. Scientific Method  Steps  Ask a __________________________  Observe and collect data  Formulate a hypothesis (a.

 Matter- anything that has mass and volume  Atom- smallest unit of an element that keeps the properties of element  Element- pure substance made of.

Ch. 9 - Classification of Matter II. Composition of Matter ( p )  Matter Flowchart  Pure Substances  Mixtures MATTER.

States of Matter. Matter Matter – anything that has mass and takes up space Everything around us Mass: measurement that reflects the amount of matter.

UNIT 3. Targets (I CAN…) :  Utilize appropriate scientific vocabulary to explain scientific concepts in this unit.  Characterize matter by its chemical.

Instructional Focus for 9/3/13

I. States of Matter Kinetic Energy States of Matter

“STUFF” Matter and Energy. What is Matter? Matter is anything that has both mass and volume. Mass is a measurement of the amount of “stuff” in an object.

 Matter – anything that has mass and takes up space  Mass – the amount of matter the object contains  Everything is made up of matter  Substance contain.

Thursday, September 13, 2013 How Can Density Be Used to Identify A substance Lab.

Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno.

Matter – General Information Chem328 1 st Year Chemistry Revised 2015.

MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno Can it be chemically.

Physical and Chemical Changes Matter  Matter – anything that has volume or mass. Atoms are the smallest unit of matter!  Volume – anything that takes.

Chem 11. Indications of a chemical reaction Energy absorbed or released Color change Gas produced Precipitate- solid that separates from solution Not.

Chapter 3 Matter Properties and Changes. Atom: The smallest particle of an element that retains all the properties of that element –Comprised of protons,

Ch. 1 - Matter I. States of Matter  Kinetic Energy  States of Matter.

Ch. 1 - Matter I. States of Matter  Kinetic Energy  States of Matter.

Matter I. States of Matter  Kinetic Molecular Theory  States of Matter.

C. Johannesson Matter Anything that has mass and takes up space (volume) (What do you remember about mass and volume?)

UNIT 02 MATTER. A. CLASSIFYING MATTER Matter is anything that has a mass and volume. Mass is the amount of matter the object contains. Examples of things.

I. States of Matter (p.12) Kinetic Molecular Theory States of Matter

Starter: Write Down What Type of Change?     

Chapter 3 Matter I. Properties & Changes in Matter  Extensive vs. Intensive  Physical vs. Chemical.

III. Classification of Matter Matter Flowchart Pure Substances Mixtures Created by GBaker

Classification of Matter

1 Classification of Matter. 2 Classifying Matter by Composition Homogeneous – matter with a uniform composition Heterogeneous - matter without a uniform.

Ch Matter I. Classification of MatterClassification of Matter (p )  Matter Flowchart  Pure Substances  Mixtures.

Classification of Matter WORD:Matter DEF: anything that has mass and takes up space.

Matter: Properties & Change

Matter Classification  Matter Flowchart  Pure Substances  Mixtures.

Matter part 1 II. Classification of Matter  Pure Substances  Mixtures  Matter Flowchart.

Solid, Liquid and Gas Classification of Matter Separation Techniques

Bell Work According to the phase diagram below, what is the boiling point of this substance at a pressure of 30 atmospheres? C. Johannesson.

Classification of Matter Properties of Matter

Ch. 1 - Matter II. Classification of Matter (p.3-8) Matter Flowchart

Foldable Answers SolidLiquidGas Definite shapeIndefinite shape Definite volume Indefinite volume Low kinetic energyMedium kinetic energy High kinetic energy.

Ch. 2 - Classification of Matter I. Describing Matter  Physical Property  Physical Change  Chemical Change  Chemical Property MATTER.

Chp 2. MATTER & MATERIALS. 2.1 Chemistry A branch of science that deals with the composition, structure, properties and reactions (transformations) of.

Elements, Compounds or Mixtures. What is an Element? A pure substance made up of only one kind of atom.

Classification of Matter This well-known molecule is a compound because it contains more than one element. A molecule but not a compound Ozone, O 3, is.

Mixtures and Pure Substances. Pure Substance Pure Substance: a substance that contains only one type of material –Element- substance that contains only.

Matter: Properties & Change. Matter Matter – anything that has mass and takes up space Everything around us Chemistry – the study of matter and the changes.

Chapter 1: Matter and Change Chemistry is a Physical Science Matter and Its Properties Elements.

Matter Flowchart MATTER yes no MIXTURE PURE SUBSTANCE yes no yes no

Branches of Chemistry BranchArea of Emphasis Examples Organic chemistry most carbon-containing chemicalspharmaceuticals, plastics Inorganic chemistry in.

Introduction to Matter Matter: has mass & occupies space.

Do Now. Matter Classification of Matter A. Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture Heterogeneous MixtureCompoundElement.

Classification of Matter. Matter can be divided into pure and impure particle arrangement- A pure substance is anything that contains only one type of.

II. Classification of Matter Matter Flowchart Pure Substances Mixtures

Ch. 1 - Matter II. Classification of Matter (p.15-17, )

Classification of Matter

Ch. 1 - Matter II. Classification of Matter (p.15-17, )

I. States of Matter Kinetic Molecular Theory States of Matter

II. Classification of Matter Matter Flowchart Pure Substances Mixtures

Classification of Matter Matter Flowchart Pure Substances Mixtures

Classification of Matter Matter Flowchart Pure Substances Mixtures

Classification of Matter

Classification of Matter Matter Flowchart Pure Substances Mixtures

Classifying Matter.

Ch. 1 - Matter II. Classification of Matter (p.15-17, )

Matter and Its Properties

Ch. 1 - Matter II. Classification of Matter (p.15-17, )

Physical and Chemical Changes

II. Classification of Matter Matter Flowchart Pure Substances Mixtures

Classification of Matter

Classification of Matter

Presentation transcript:

Overview of Matter

Matter Flowchart MATTER Can it be physically separated? Homogeneous Mixture (solution) Heterogeneous MixtureCompoundElement MIXTUREPURE SUBSTANCE yesno Can it be chemically decomposed? noyes Is the composition uniform? noyes

Mixtures Variable combination of 2 or more pure substances. HeterogeneousHomogeneous

Pure Substances Element –composed of identical atoms –EX: copper wire, aluminum foil

Pure Substances Compound –composed of 2 or more elements in a fixed ratio –properties differ from those of individual elements –EX: table salt (NaCl)

Endothermic – energy absorbed Exothermic – energy released

Physical Properties of Matter Melting Points Boiling Points Density Solubility

Melting and Boiling Points Use the Reference Tables to determine the following: –Rank the following substances from smallest melting point to largest melting point: H 2 O, N 2, iron, lead, O 2, C 12 H 22 O 11

Reference Tables con’t What is the state of matter (solid, liquid, or gas) will each of the following substances at the given temperature? a. chlorine at -25 o C b. ethanol at 0 o C c. sodium chloride at 1500 o C d. methanol at -100 o C e. sulfur dioxide at 10 o C

Density Using the reference tables, determine the following: –Rank the following substances from greatest density to smallest density: H 2 O, Mg, C 6 H 14, Pb, methanol, NaCl

Reference Tables con’t What is the mass of 36.5 mL of ethanol? What is the volume of 50.0 g of molten lead? You have cm 3 of glucose and sucrose. Which sample has the greatest mass? Support answer with calculations.