CH. 3Matter- Properties

and Changes

Monday

• Physical and Chemical Change Lab ???

Tuesday

• Explain properties of matter notes

TEKS

• (4) Science concepts. The student knows the characteristics of matter and can analyze the relationships between chemical and physical changes and properties.

• The student is expected to: • (A) differentiate between physical and chemical

changes and properties; • (B) identify extensive and intensive properties;

3.1 Properties of Matter• Substance - composition is uniform, does

not change between samples and is “pure”.

• Pure substances:1. Elements – Na, H, He

2. Compounds – NaCl (salt) H2O (water)

Elements and Compounds• Element- Pure substance that

can not be separated into simpler substances by physical or chemical means

• Examples: Copper, Oxygen, Iodine

Compounds• Compound- a pure substance

that is a combination of two or more elements that are combined chemically.

3.2 Changes in MatterTEKS

• (8) Science concepts. The student can quantify the changes that occur during chemical reactions. The student is expected to:

• E. Determine mass relationships between reactants and products

3.2 Changes in Matter

• Physical Change- changes which alter a substance without changing the composition.

• (Does not change the identity of the substance)–Ex: ice to water

Examples of Physical Changes

• Change in Size or Shape such as:Bend, break, cut, grind, crumple, split, or crush

• Change in State such as:Melting, freezing, vaporization, boiling, condensation, or sublimation

• Chemical Change- involves one or more substances changing into another substance

• (also called a Chemical Reaction)Ex: steel to rust

Examples of Chemical Changes

• Fermentation, • rusting, • explode, • oxidize, • corrode, • tarnish, • burn, • or rot.

• Chemical Property- the ability of a substance to combine with or change into one or more substances

• Na + Cl = NaCl (Salt)

Examples of Chemical Properties

– Ability to rust– Formation of precipitate– Reacts with water, oxygen,

acids, bases, or other substances– Flammability

Physical Properties of Matter

• Physical property- characteristic that can be observed or measured without changing the sample’s composition

• Qualitative!!

Examples of Physical Properties

–Density–Color–Odor–Taste–Hardness–Melting Point–Boiling Point

Extensive Properties–Dependent upon amount of

substance present–Mass, Length, Volume–It changes if you take away

some of the substance.

Intensive propertiesIndependent of amount of

substance presentExamples: Density, color, odor,

boiling point.Intensive properties Don’t change

and can be used to identify the substance.

Miners often got Pyrite (fool’s gold) and real gold mixed up. But Density could be used to correct the error.

The density of gold is 19.3 g/mL and the density of pyrite is 5 g/mL

Pyrite – fools gold Gold

Properties of CopperPhysical Properties Chemical Properties

Reddish brown, shiny Forms green copper carbonate compound

Malleable, ductile Forms new substances with nitric acid and sulfuric acid.

Good conductor Forms a deep blue solution with ammonia.

Density = 8.92 g/mL

Melting pt = 1085 oC

Boiling pt = 2570 oCSo changing States of Matter are PHYSICAL properties!!

Both are copper

Properties of Matter

Chemical Properties

Reactions in the presence of

Water, Air, Acid, Base

What happens when heated

Physical Properties

Intensive PropertiesDo NOT depend on the

amount________________

E.G Color, Taste, Melting/Boiling Point, Luster, Hardness

Extensive Properties Depends on the

amount_______________Mass, Volume, Length, Shape

http://www.roomd113.com/TAKS%20PP/matterclass_pres.ppt

Evidence of a Chemical Reaction

• The observation that the product has different properties than the reactant(s).

• Clues:• If something can burn• Production of energy, such as light, heat, or sound• Formation of a gas • Formation of a solid – called a precipitate • Change in odor• Change in color

Wednesday

Chemical Reactions• The new substances formed in the

reaction have different compositions and different properties from the substances present before the reaction occurred.

• Reactant – starting material in a reaction

• Product – ending material in a reaction

Reactant(s) turn into Product(s)• Na + Cl = NaCl (Salt)

• C. Conservation of Mass – By carefully measuring the mass before and after many chemical reactions, it was observed that the total mass involved in the reaction stayed the same.

• Law of Conservation of Mass- states that matter is neither created nor destroyed during a reaction– it is conserved

Total mass of the reactants must equal the total mass of the products.

Massreactants = Massproducts

4. According to the law of conservation of mass, how much zinc was present in the zinc carbonate?

A 40 g B 88 gC 104 D 256 g

• Antoine Lavoisier used an analytical balance to help prove this law.

Conservation of Mass problems

• Ex: 23 g of Na reacts with 35 g of Cl, what is the mass of the product, sodium chloride?

• 23 g Na+ 35 g Cl = ______ g NaCl

Ex: #2• 10 g HgO = 9.26 g Hg + _____ g of O

Properties of Matter

Chemical Properties

Physical Properties

Intensive properties

Extensive properties

MATTER

Can it be physically separated?

Homogeneous Mixture

Heterogeneous Mixture Compound Element

MIXTURE PURE SUBSTANCE

yes no

Can it be chemically decomposed?

noyesIs the composition uniform?

noyes

Colloids

SuspensionsSolutions

Thursday

• States of matter and card sorting activity

Friday

• 10 bottle demo

Monday

• Mixtures

3.3 Mixtures of Matter

TEKS• 2.(E) plan and implement investigative

procedures, including asking questions, formulating testable hypotheses, and selecting equipment and technology

• 4. (D) Classify matter as pure substances or mixtures through investigation of their properties.

3.3 Mixtures of Matter

• Mixture- combination of two or more pure substances in which each retains its individual chemical properties.

Examples of Mixtures

–Sand and water

–Salt and Water

–If the substances do not react and can be separated by physical means, it is a mixture.

Types of Mixtures

• Heterogeneous Mixture- does not blend smoothly and individual substances remain distinct. (can see the different parts)

• Ex: salad, pizza

• Homogeneous Mixture- constant composition throughout (looks the same throughout)–Also known as solutions–Ex: Koolaid, air, sea water, sodas,

vinegar, steel

Colloid

• A heterogeneous mixture with particles larger than those in a solution

• Example : milk

Suspension

• A heterogeneous mixture whose particles settle out over time and can be separated from the mixture by filtration

• Example lead paint

Types of Solution SystemsSYSTEM EXAMPLE

Gas-Gas Air is primarily an example of nitrogen, oxygen and argon gases.

Gas- Liquid Carbonated beverages contain carbon dioxide gas in solution.

Liquid- Gas Moist air contains water droplets in air.

Liquid- Liquid Vinegar contains acetic acid in water.

Solid- Liquid Sweetened powder drink contains sugar and other solid ingredients in water.

Solid- Solid Steel is an alloy of iron containing carbon.

Separating Mixtures

• Because mixtures are physically combined,

the processes are used to separate them arebased on the difference in physical properties of the substances.• 4 methods for separation

Filtration

• Uses a porous barrier to separate a solid from a liquid

Distillation• Based on differences in

boiling points of the substances

• Heat mixture until substance with lowest boiling point boils to a vapor which is then condensed into a liquid

Crystallization• Results in formation of

pure solid particles of a substance from a solution containing the dissolved substance

Chromatography• Separates the components

of a mixture (called the mobile phase) on the basis of the tendency of each to travel or be drawn across the surface of another material (called the stationary phase)

3.4 Elements and Compounds

TEKS• 4. (D) Classify matter as pure substances or

mixtures through investigation of their properties.

3.4 Elements and Compounds• Element- Pure substance that

can not be separated into simpler substances by physical or chemical means

• Examples: Copper, Oxygen, Iodine

• Each element has a unique chemical name and symbol.

• The first letter is always capitalized, the rest are lowercase.–Ex:

•Oxygen O•Carbon C• Iron Fe

Periodic Table

• In 1869 Dmitri Mendeleev devised a chart which organized all of the known elements into rows and columns based on their similarities and masses.

Rows are called periodsColumns are called groups or families

• Can be broken down into simpler substances by chemical means (ex: using heat or energy)

Compounds• Compound- a pure substance

that is a combination of two or more elements that are combined chemically.

Common Compounds• There are 10 MILLION known compounds!• Ex: Water, Sodium chloride (salt), sucrose

(sugar), aspirin, etc.• Chemical compounds are represented by

formulas.Ex: Water is H2O

Sodium chloride is NaClSucrose is C12H22O11

• Properties of a compound are different than the elements that make it up.

Monday

• States of Matter• http://www.youtube.com/watch?v=V9WYweB

A6vA&feature=related• Oobleck• http://www.youtube.com/watch?

v=V9WYweBA6vA&feature=related

• Ex: Hydrogen and Oxygen are tasteless, odorless gases. They make water which is a clear liquid

Hydrogen + Oxygen Water

– Ex: Chlorine is a poisonous green gas. Sodium is an explosive metal. They make sodium chloride which is a white crystal that tastes salty.

– Stop pg 74

• States of matter- physical forms of all matter on Earth.

States of Matter• Solid- definite shape and volume. • Particles vibrate in place.• Particles are tightly packed.• This make a solid incompressible – can’t be

pressed into a smaller volume.

• Liquid- form of matter that flows, has constant volume, and takes the shape of its container.

Liquids

• Particles can move past each other

• Particles are close together.

• virtually incompressible

• Gas- form of matter that flows to conform to the shape of its container and fills the entire volume of its container.

Gases

• Particles of gases move freely.• Particles are very far apart. • Easily compressed.• Is normally in the gaseous state at

room temperature.

Movement of particles

                               

                               

                               

Microscopic view of a gas.

Microscopic view of a liquid.

Microscopic view of a solid.

Characteristics of Gases, Liquids and Solids and the Microscopic Explanation for their Behavior

Gas Liquid Solidflows easily particles can move past one another

flows easily particles can move/slide past one another

does not flow easily rigid - locked into place particles cannot move/slide past one another

compressible lots of free space between particles

not easily compressible

little free space between particles

not easily compressible little free space between particles

assumes the shape and volume of its container

assumes the shape of its container, but volume is constant

retains a fixed volume and shape

• Vapor – refers to the gaseous state of a substance that is usually a solid or liquid at room temperature.

Plasma• Plasma - the fourthstate of matter and the most common one.

Found in Stars, and occurs naturally on the Earth in lightning bolts.