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

Energy is the part of the universe that has the ability to do work

Chemistry is the study of matterThe properties of different types of matterThe way matter behaves when influenced by

other matter and/or energy

Physical Properties are the characteristics of matter that can be changed without changing its composition.Characteristics that are directly observableExamples: odor, color, volume, state of

matter, density, boiling point and melting point .

Extensive property – depend on the amount of matter present (length, mass, and volume).

Intensive property – do not depend on the amount of matter present (melting point, boiling point, density).

Chemical Properties are the characteristics that determine how the composition of matter changes as a result of contact with other matter or the influence of energy

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)

Digesting your breakfast or lunch- Chemical property – describes behavior of food –

forming a new substance (depends on what you ate)

solid, liquid, gas

State Shape Volume Compress Flow

Solid Keeps Shape

Keeps Volume

No No

Liquid Takes Shape of Container

Keeps Volume

No Yes

Gas Takes Shape of Container

Takes Volume of Container

Yes Yes

Physical Changes are changes to matter that do not result in a change the fundamental components that make that substanceState Changes – boiling, melting, condensing

Chemical Changes involve a change in the fundamental components of the substanceProduce a new substanceChemical reactionReactants ProductsExamples: burning, digesting, fermentation, decomposition.

1. Color change2. Gas is formed (bubbles are produced).3. Heat and light are produced.4. A precipitate forms.

A precipitate is a solid that is produced when two liquids are combined. Often a color change will occur as well.

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)A hot dog is cooked.

Source: Jim Pickerell/Stone/Getty Images

Substances which can not be broken down into simpler substances by chemical reactions are called elements

Most substances are chemical combinations of elements. These are called compounds.Compounds are made of elementsCompounds can be broken down into elementsProperties of the compound are not related to

the properties of the individual elements that in it.

Same chemical composition at all times

Homogeneous = uniform throughout, appears to be one thing pure substances solutions (homogeneous mixtures)

Heterogeneous = non-uniform, contains regions with different properties than other regions or phases

Phase - any part of a system with uniform composition and properties.

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

H o m o g e ne o us

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

M a tte r

Pure SubstancesAll samples have the same physical and

chemical propertiesConstant Composition all samples have the

same compositionHomogeneousSeparate into components based on chemical

properties

MixturesDifferent samples may show different

propertiesVariable compositionHomogeneous or HeterogeneousSeparate into components based on physical

propertiesAll mixtures are made of pure substances

Gasoline a homogenous mixture

A stream with gravel on the bottoma heterogeneous mixture

Copper metalA pure substance (all elements are pure

substances)

Separate mixtures based on different physical properties of the componentsPhysical change

Different Physical Property Separation TechniqueBoiling Point Distillation

State of Matter (solid/liquid/gas) FiltrationAdherence to a SurfaceChromatographyVolatility Evaporation

Distillation – liquid is boiled to produce a vapor that is then condensed again to a liquid.

Filtration – pouring a mixture through a filter that will allow the smaller part of the mixture to flow through while collecting the larger particles.

Chromatography – separation of a mixture into colors.

Magnets – if one component of the mixture is magnetic but another is not, the magnetic substance can easily be separated.

Decanting – pouring the liquid off the top of the mixture while leaving the solid at the bottom undisturbed.

Source: Photo by James Scherer.

Source: Photo by James Scherer.

Source: Photo by James Scherer.

Capacity to do workchemical, mechanical, thermal,

electrical, radiant, sound, nuclear

Energy may affect mattere.g. raise its temperature, eventually

causing a state changeAll physical changes and chemical

changes involve energy changes

Heat - flow of energy due to a temperature difference1. Exothermic = A process that results in the

evolution of heat. Gas Liquid Solid are changes of state

that are all exothermic processes Heat is exiting the system and going

into the surroundings. It feels warm or hot to the touch.

2. Endothermic = A process that absorbs energy. Solid Liquid Gas are changes of

state that are all endothermic processes.

Heat is being put into the system from the surroundings. It feels cool or cold to the touch.

One calorie (cal) is the amount of energy needed to raise the temperature of one gram of water by 1°C.kcal = energy needed to raise the temperature of

1000 g of water 1°Cjoule (J)

4.184 J = 1 cal, 4.184 kJ = 1 kcalIn nutrition, calories are capitalized

1 Cal = 1 kcal

Convert 60.1 joules to calories

How many kilojoules are there in 4.80 x 103 calories of energy?

The amount the temperature of an object increases depends on the amount of heat added (q).If you double the added heat energy

the temperature will increase twice as much.

The amount the temperature of an object increases depends on its massIf you double the mass it will take

twice as much heat energy to raise the temperature the same amount.

Specific Heat (Cp) is the amount of energy required to raise the temperature of one gram of a substance by one Celsius degree

C gJ

4.184 is water ofheat specific the,definitionBy

Amount of Heat = Mass x Temperature Change x Specific Heat

q = mTCpT = final temp. - initial temp.

What is the final temperature of aluminum (Cp = 0.90 J/goC) that absorbs 425 J of energy when a 10.0 gram sample of aluminum is initially at 25oC?

Calorimetry – an accurate and precise measurement of heat change for chemical and physical processes.

If any reaction heat gained by the system or the surroundings equals heat lost by the system or the surroundings.

q lost = - q gained

A 19.6-gram sample of a metal was heated to 61.7oC. When the metal was placed into 26.7 grams of water in a calorimeter, the temperature of the water increased from 25.0oC to 30.0oC. What is the specific heat of the metal assuming that all of the heat lost by the metal was gained by the water?

A 50.0 gram sample of water at 100.oC was placed in an insulated cup. Then a sample of iron metal (Cp = 0.449 J/goC) at 25.0oC was added to the water. The temperature of the water dropped to 96.7oC. What is the mass of the iron assuming that all of the heat lost by the iron was gained by the water?