matter chapter 3 1

Matter

Chapter 3

Why does soda fizz when you open the bottle?

Why is the sun hot? When iron rusts, what’s happening?

Objectives

• Observe and explain the difference between states of matter.

reserved.

3-1 Universe Classified

• Matter is the part of the universe that has mass and volume

- There are three states of matterSolid, liquid, and gas

• Chemistry is the study of matter– The properties of different types of matter– The way matter behaves when influenced by other

matter and/or energy

Some Criteria for the Classification of Matter

• Composition (elements and compounds)

• State (solid, liquid, gas)

• Properties

States of Matter

YES YES YES

YES YES

States of Matter

Figure 3.1: Liquid water takes the shape of its container.

• Teacher Website Select Interactive 1

Figure 3.11: In ice, the water molecules vibrate randomly about their positions in the solid. Their motions are represented by arrows.

Figure 3.12: Equal masses of hot water and cold water separated by a thin metal wall in an insulated box.

Figure 3.13: The H2O molecules in hot water have much greater random motions than the H2O molecules in cold water.

Figure 3.14: The water samples now have the same temperature (50°C) and have the same random motions.

Phase ChangesMelting solid liquidCondensation gas liquid

Freezing liquid solid

Deposition gas solid

Evaporation liquid gasSublimation solid gas

*Boiling: Evaporation occurring beneath the liquid’s surface.

Gallium metal has such a low melting point (30°C) that it melts from the heat of a hand.

NAME THAT PHASE CHANGE

Video - https://www.youtube.com/watch?v=wln6WSv-cro

Objectives

• Explain the difference between elements and compounds.

reserved.

3-3 Elements and Compounds

• a pure substance

• same composition throughout

• Contains only one type of atom

• Can not be broken down into simpler substances by ordinary chemical reactions (not a nuclear reaction)

Element

Chemical Symbols of Elements

• System started by Jons Berzelius (Sweden, 1779-1848)

• 90-91 naturally occurring elements• One or two first letters of name of the

element.

• Many elements names have roots from: Latin, Greek, mythology, geography, names of scientists.

Examples:• Americium, Am

• Einsteinium, Es

• Bromine, Br

• Helium, He

• Lead(Plumbum), Pb

• Niobium, Nb

• Iron (Ferrum), Fe

• Mendelevium, Md

Examples of other elements: O2, H2, I2

Compound – chemical combination of two or more elements

Have two properties in common with elements:

1. pure substance2. Homogeneous – same chemical composition at all times

Compound

Compounds cont.

Have two properties that differ from elements:

1.two or more elements that are chemically combined, in a definite ratio

2. Compounds can be broken down by chemical reactions using energy:

a) decomposition - uses heatb) electrolysis - uses electricity

> 10 million compounds

•elements are represented by symbols•compounds are represented by chemical formulas

•chemical formula1. symbol --> tells which elements are present in compounds2. subscript (little # lower right) --> tells the number of atoms of each element

When the elements sodium and chlorine combine chemically to form sodium chloride, there is a change in composition and a change in properties.

Properties of Compounds

• Sodium chloride (commonly known as table salt) is a white solid.

Distinguishing ElementsDistinguishing Elementsand Compoundsand Compounds

Compounds have different properties from their individual elements.

Breaking down Compounds

Breaking down NaCl

•Sodium is a soft gray metal.

Breaking down NaCl

Breaking down Compounds

• Chlorine is a pale yellow poisonous gas.

Classification of Matter(by composition)

Classification of Matter

P u re S ub s ta n ceC o n s tan t C o m p o s it ion

H o m o ge n e o us

M ix tu reV a ria b le C o m p o s it ion

M a tte r

3-4 Mixtures

Mixtures can be classified as:•Homogeneous Mixtures

•Heterogeneous Mixtures

• Homogeneous mixture = uniform throughout, appears to be one layer– Also called solutions

– Examples: olive oil, salt water, lemonade, coffee, air

The substances in the olive oil are evenly distributed throughout the mixture

Example: Stainless SteelA homogeneous

mixture of: -Iron (Fe) -Chromium (Cr)-Nickel (Ni)

• Heterogeneous mixture = non-uniform, contains regions with different properties than other regions

- Examples: oil and vinegar, salad, chicken soup

Pure Substances vs. Mixtures• Pure Substances

– All samples have the same physical and chemical properties– Constant Composition all samples have the same composition– Homogeneous– Separate into components based on chemical properties

• Mixtures– Different samples may show different properties– Variable composition– Homogeneous or Heterogeneous– Separate into components based on physical properties

• All mixtures are made of pure substances

Figure 3.4: When table salt is stirred into water (left), a homogeneous mixture called a solution forms (right).

reserved.

Identity Each of the following as a Pure Substance, Homogeneous Mixture or

Heterogeneous Mixture

Gasoline

A stream with gravel on the bottom

Copper metal

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Identity Each of the following as a Pure Substance, Homogeneous Mixture or

Heterogeneous MixtureGasoline

– a homogenous mixture

A stream with gravel on the bottom– a heterogeneous mixture

Copper metal– A pure substance (all elements are pure substances)

reserved.

3-5 Separation of Mixtures• Separate mixtures based on different

physical properties of the components

EvaporationVolatility

ChromatographyAdherence to a Surface

FiltrationState of Matter (solid/liquid/gas)

DistillationBoiling Point

TechniqueDifferent Physical Property

Example: Separate iron filings from sulfur using a magnet.

Filtration: separates a solid from a liquid in a heterogeneous mixture

Figure 3.6: Distillation of a solution consisting of salt dissolved in water.

-separate dissolved solids from a liquid in a homogeneous mixture

-uses boiling and condensation.

Distillation of Crude Oil (Refining)

• Crude Oil is a mixture of Hydrocarbons

Distillation of Crude Oil

Paper Chromatography

Chromatography separates mixtures of substances into their components.They all have:• a stationary phase (a solid, or a liquid supported on a solid) •and a mobile phase (a liquid or a gas).

Properties of Matter

reserved.

Extensive Propertiesmass –

Volume –

–The volume of a basketball is greater than the volume of a golf ball.

a measure of the amount of matter the object contains.

of an object is a measure of the space occupied by the object.

Who has a greater volume?

An extensive property is a property that depends on the amount of matter in a sample. Examples: mass and volume

Extensive Properties

Objectives

• Observe and explain the difference between states of matter.

• Explain the difference between physical and chemical changes.

reserved.

– An intensive property is a property that depends on the type of matter in a sample, not the amount of matter.

Examples include:

- Hardness of an object -Color- Softness -Boiling point- Absorbency -Odor

Intensive Properties

Is changing phase a physical or chemical change?

3-2 Physical and Chemical Properties and Changes

reserved.

Properties of Matter• Physical Properties are the characteristics

of matter that can be changed without changing its composition

– Characteristics that are directly observable

– Examples: Color, odor, hardness, density, melting point, boiling point, state, solubility.

Substance State Color Melting Point (C°)

Boiling Point (C°)

Density (g/cm3)

Oxygen O2 Gas Colorless -218 -183 0.0014

Mercury Hg Liquid Silvery-white

-39 357 13.5

Bromine Br2 Liquid Red-brown -7 59 3.12

Water H2O Liquid Colorless 0 100 1.00

Sodium Chloride

NaCl Solid White 801 1413 2.17

Example: Physical Properties

Properties of Matter• Chemical Properties are the characteristics

that determine how the composition of matter changes as a result of contact with other matter

- Examples: burning, decompose, reactivity, corrode, tarnish, explode, ferment

reserved.

Classify Each of the following as Physical or Chemical Properties

The boiling point of ethyl alcohol is 78°C.

Diamond is very hard.

Sugar ferments to form ethyl alcohol.

reserved.

Classify Each of the following as Physical or Chemical Properties

The boiling point of ethyl alcohol is 78°C.– Physical property – describes inherent characteristic of

alcohol – boiling pointDiamond is very hard.

– Physical property – describes inherent characteristic of diamond – hardness

Sugar ferments to form ethyl alcohol.– Chemical property – describes behavior of sugar –

forming a new substance (ethyl alcohol)

Changes in Matter• Physical Changes are changes to matter that do

not result in a change in the composition

– State Changes – boiling, melting, condensing– Breaking, splitting, grinding, cutting

• Chemical Changes involve a change in the composition of the substance– Produce a new substance– Chemical reaction– Reactants Products

Indications of a Chemical Reaction

• Color change• Solid forms (precipitate)• Gas bubbles• Odor• Temperature change• Fizzing

reserved.

Formation of a Precipitate

Cu(OH)2

Precipitate

reserved.

Classify Each of the following as Physical or Chemical Changes

Iron metal is melted.

Iron combines with oxygen to form rust.

Sugar ferments to form ethyl alcohol.

reserved.

Classify Each of the following as Physical or Chemical Changes

Iron is melted.– Physical change – describes a state change, but the

material is still ironIron combines with oxygen to form rust..

– Chemical change – describes how iron and oxygen react to make a new substance, rust

Sugar ferments to form ethyl alcohol.– Chemical change – describes how sugar forms a new

substance (ethyl alcohol)

Oxygen combines with the chemicals in wood to produce flames. Is a physical or chemical change taking place?

Source: Jim Pickerell/Stone/Getty Images

Burning of MethaneCH4 +2O2 CO2 + 2H2O

l_______________l l_________________l l l

reactants products

Burning of MethaneCH4 + 2O2 CO2 + 2H2O

In a chemical change, what happens to matter that appears

to be lost?

The Law of Conservation of Mass (Antoine Lavoisier)

• In any chemical or physical change, mass is neither created or destroyed

• Mass is CONSTANT

matter chapter 3 1

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