matter, energy, and the environment unit copyright © 2010 ryan p. murphy

Part I

Matter and Phase Change

Matter, Energy, and the Environment Unit

Copyright © 2010 Ryan P. Murphy

First Area of Focus: Matter

Matter : Anything that has mass and takes up space.


• Important note: Mass and weight are different.


• Important note: Mass and weight are different.– Mass is a measurement of the amount of matter

something contains.



something contains.– Weight deals with the pull of gravity.



something contains.– Weight deals with the pull of gravity. – Even if you are weightless in space you still have

mass.


Characteristics of Matter- Can be a solid, liquid, gas or plasma

- Example: water, cereal, desk

- Non examples: light, love, gravity

PURE SUBSTANCE

Define- Matter that always has the same composition and properties

Characteristics- can be classified as elements and compounds, can not be broken down without breaking chemical bonds

Examples: all elements, sugar, salt, diamondNonexamples: dirt, pencil, soda

Element: A substance that is made entirely from one type of atom.


ELEMENT

Define- substance that is made up of entirely one type of atom

Characteristics: has a fixed composition and cannot be broken down into simpler substances

Examples: everything on the periodic table, gold, carbon, titanium, mercury

Non examples: steel, water, jello

Compound: Made up of two or more elements (atoms) chemically bonded together.


COMPOUNDSCharacteristics- can be broken down into individual elements. Properties of the compound differ from the substances from which it is made

Examples: silicon dioxide (SiO2) water (H2O), rust (FEO2)

Non examples: all elements on the periodic table

Homogeneous mixture: Same molecules throughout.




Solute



Homogeneous(Same throughout)

(Uniform)

HomogeneousDefine: Substances evenly distributed that you cannot distinguish them

Characteristics: uniform molecules- appears to contain only one substance but does not,

Examples: alloys like stainless steel, cake batter, coffee

• Alloys (combined metals) are homogeneous because each metal added changes the melting point of the whole.

Heterogeneous: A mixture of two or more compounds.




Mixture is not uniformthroughout.




Spoonful is Heterogeneous




Spoonful is Heterogeneous

Broth mightbe homogeneous

Heterogeneous

Define- made up of different material that remain physically separate

Characteristics: parts are noticeably different

Examples: sand, trail mix, beans and rice

Non examples: vinegar, coffee, soda

Which is… A

B C

D E F G

An untouched substance made of atoms or more elements chemically combined in fixed ratios. Example CO2

A substance made of the same type of atoms.Example - Hydrogen

Anything that has mass and takes up space.

An accumulation of molecules or atoms of different types.

A substance that is a form of matter that has a constant chemical composition and characteristic properties. It cannot be separated into its several components without breaking its chemical bonds.

A mixture is made of different materials that remain physically separate.

answer

A mixture that has the same uniform appearance and composition throughout.

SolutionDefine: when a substance dissolves

and forms a homogeneous mixture

Characteristics: particles too small to separate into layers, let light pass through, or be filtered

SOLUTION

Examples: windshield wiper fluid, tea

Nonexamples: orange juice with pulp, Muddy water

Suspension

Define: heterogeneous mixture that separates into layers over time

Characteristics: contains larger particles that can be filtered, scatter light making them cloudy

Suspension

Examples: muddy water, orange juice with pulp with pulp

Nonexamples: koolaid, coffee

COLLOID

Define: contains particles that are intermediate in size between the small particles in a solution and the larger particles in a suspension

Characteristics: do not separate in layers, cannot filter out particles, particles scatter light

COLLOID

Examples: homogenized milk (decreases size of fat molecule compared to fresh milk which is a suspension, fog

Nonexamples: fresh milk, salt water, sand and water

Solvent: A substance that does the dissolving (usually larger amount).


Solute: The substance that gets dissolved (usually lesser amount).


Solubility: How much solute can dissolve in a substance before it becomes saturated.


Solubility: How much solute can dissolve in a substance before it becomes saturated.


Solutegets

dissolved

Supersaturated: When no more solute will dissolve. (crystals become visible)


Learn more about solutions at…http://www.chem4kids.com/files/matter_solution.html

http://www.chem4kids.com/files/matter_solution.html

Video Link! Supersaturated with Sodium Acetate and some interesting students.http://www.youtube.com/watch?v=1y3bKIOk

cmk

http://www.youtube.com/watch?v=1y3bKIOkcmk

http://www.youtube.com/watch?v=1y3bKIOkcmk

The Tyndall Effect

Used to identify solutions from colloids

Colloids- light collides with particles and scatters causing the substance to appear cloudy. This effect was observed and described by John Tyndall as the Tyndall Effect.

Solutions- do not exhibit Tyndall effect, light passes cleanly through

Physical properties

Physical property- characteristic of a material that can be observed or changed without changing the composition

Types of physical properties viscosity- the tendency of a liquid to

keep from flowing, its resistance to flowex. Ketchup has more viscosity

then water Viscosity decreases when heated

Physical properties

Conductivity- materials ability to allow heat to flow

high conductivity materials (metals) are called conductors and are also a good conductors of electricity

Physical PropertiesMalleability- ability of a solid to be

hammered without shattering; most metals are malleable. Ex. Glass is not malleable but gold is.

Physical Properties Melting point- temperature

when a solid changes into a liquid; specific temperature for every known substance;

Ex. Gold will melt at 1064 C

Boiling point- temperature when substance boils (converts to a gas)

ex. Gold will boil at 2856 C

Using physical properties to separate mixtures

Evaporation Allowing the

liquid to evaporate, leaving the solid behind.

Example: heating sugar water. The water evaporates and the sugar crystals are left behind.

MAGNETISM

- separating mixtures using a magnet to attract magnetic objects away from the substance it is in.

- Not all metals are magnetic: gold, silver, and aluminum are examples of metals that are not magnetic.

MAGNETISM

Magnetic separators are used in factories. Materials are put on a conveyor belt that is spun by magnetic wheels. As the objects are moved upside down the non magnetic objects fall off and the magnetic ones stay on.

Filtration

physically separating a heterogeneous mixture of a liquid and a solid.

Carried out by pouring mixture into a funnel with filter paper in it.Filtrate (liquid) is collected in the beaker

below the funnel.Solid residue is collected in the filter

paper.

Distillationphysically separating a

homogeneous mixture by differences in their boiling points.

Carried out by heating up the solution until the first substance boils and goes to the gaseous state.Gas is collected and condensed back

into the liquid state in a separate container.

Solid residue (or a second liquid with a higher boiling point) is collected in the original container.

DISTILLATION

https://www.youtube.com/watch?v=Cz_jYx4dF0U



DECANTING

- A method of physically separating the top layer of a liquid from a mixture.

- Top layer is poured into new container.Bottom layer remains in original container

CHROMATOGRAPHY

A method of physically separating a mixture based on differences in solubility of the components.Types of chromatography include:

Paper chromatography.Gas-liquid chromatography.Thin-layer chromatography.

CHROMATOGRAPHY

TLC is a simple, quick, and inexpensive procedure that gives the chemist a quick answer as to how many components are in a mixture.

Gas chromatography separating and analyzing compounds that can be vaporized without decomposition. Typical uses of GC include testing the purity of a particular substance, or separating the different components of a mixture

https://www.google.com/url?sa=i&rct=j&q=&esrc=s&source=images&cd=&cad=rja&uact=8&ved=0CAcQjRxqFQoTCPP-5I3Sl8gCFcKNDQodCM4Lww&url=https://www.flickr.com/photos/jimmysmith/109228760&psig=AFQjCNGEFW64wl5lpjJfIkoExZ3CvaPJQw&ust=1443457947116685

https://www.google.com/url?sa=i&rct=j&q=&esrc=s&source=images&cd=&cad=rja&uact=8&ved=0CAcQjRxqFQoTCJ-Ai9DSl8gCFUzTgAodySwDcA&url=https://en.wikibooks.org/wiki/Structural_Biochemistry/Chromatography/Thin_Layer&psig=AFQjCNFbo0HV3HDCHKChGVI78zefRMhFdg&ust=1443458095531106

CENTRIFUGATION- physically separating a mixture based on differences in density.

- Sample is spun at high speeds in tubes placed in a machine called a centrifuge:

- The most dense substance falls to the bottom layer and the least dense goes to the top

CHEMICAL PROPERTIES

Chemical property- any ability to produce a change in the composition of matter

- observed when one substance is changing into a different substance

Flammability- materials ability to burn in the presence of oxygen

CHEMICAL PROPERTIES

Reactivity- describes how readily a substance combines chemically with other substances

ex- oxygen reacts easily with most other elements; rust is formed when it reacts with iron and water

CHEMICAL CHANGE VS PHYSICAL CHANGE

Chemical changes- occurs when a substance reacts and forms one or more new substances

In a physical change , the composition of the matter remains the same and nothing new is produced.

EVIDENCE OF CHEMICAL CHANGE

1) change in color- ex. Silver bracelet turning dark (tarnish)

2) production of a gas- ex. Baking soda and vinegar

produces carbon dioxide

http://www.google.com/url?sa=i&rct=j&q=&esrc=s&source=images&cd=&cad=rja&uact=8&ved=0CAcQjRxqFQoTCMuDkriJm8gCFYqVDQodftIEtQ&url=http://blog.goldeneaglecoin.com/silver-coins-tarnish/&psig=AFQjCNGbHeZTdAnJ82xuosFfHp36lta6HQ&ust=1443575894408860

http://www.google.com/url?sa=i&rct=j&q=&esrc=s&source=images&cd=&cad=rja&uact=8&ved=0CAcQjRxqFQoTCIOSpNyJm8gCFYXMgAodId8KvQ&url=http://www.tophdgallery.com/with-vinegar-and-baking-soda.html&bvm=bv.103388427,d.eXY&psig=AFQjCNF_RwDT-alySktnnnuLaDU2e0zTJQ&ust=1443575975046251

3) Formation of a precipitate(any solid that forms and separates from a liquid mixture)- ex. Put lemon juice (acid in milk will cause it to curdle due to a change in the protein molecules)

EVIDENCE OF CHEMICAL CHANGE

http://www.google.com/url?sa=i&rct=j&q=&esrc=s&source=images&cd=&cad=rja&uact=8&ved=0CAcQjRxqFQoTCJybjKeJm8gCFQjOgAod-mkNTA&url=http://www.foodfor7stagesoflife.com/2010/08/how-to-make-organic-and-fat-free-paneer-at-home.html&psig=AFQjCNHKlun-j_FWml87Nv7JlZ2uMCqvbg&ust=1443575843613948

EVIDENCE OF A CHEMIAL CHANGE

• Temperature or energy change- endothermic- a change

(chemical reaction) that absorbs requires (absorbs) heat

so the temperature decreases as energy is used

ex. Photosynthesisrequires input from the sun

EVIDENCE OF A CHEMICAL CHANGE

- exothermic- a change (chemical reaction) that releases heat; temperature increases as heat is given off

ex. Combustion of fuels(releases heat)

Law Conservation of Matter-


Law Conservation of Matter-


Same amount ofelements, just arranged

differently

In any physical or chemical change, matter is neither created nor destroyed


In any physical or chemical change, matter is neither created nor destroyed Matter can be changed from one form to

another.


matter, energy, and the environment unit copyright © 2010 ryan p. murphy

Documents

murphy mixture

murphy matter

matter matter

murphyhomogeneous mixture

environment unit copyright

murphy important note

murphy heterogeneous

uniform molecules