U3 Matter and Energy

7/30/2019 U3 Matter and Energy

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Unit 3: Matter and Energy

Part I: Classifying Matter


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2

Matter is anything that has mass andvolume.

Volume is the amount of threedimensional space an object occupies.

Mass is a measure of the amount ofmatter.

Matter


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3

Which of the following are examples of matter?

a. Sand

b. Paperc. Heat

d. Air

e. Sound

f. Light

g. Chalk

h. Smoke

f. Water Vapor

Pause for a Cause

Learning Activity 1


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Building matter

An element is a pure substance that cannot be

broken down into simpler, stable substances

and is made of one type of atom.

An atom is the

smallest unit of an

element thatmaintains the

chemical identity of

that element.


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Elements

How many known elements are there in the

universe?

117


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The Periodic Table

Period

Group or

family

PeriodProperties varyTotal of 7 periods

GroupHave similar properties

Total of 18 groups

Metals


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Groups

The vertical columns on the periodic table are calledgroups or families.

Groups are numbered 1-18 on the periodic table

Elements belonging to the same group have similar properties


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Periods

The horizontal row of elements on the periodic table are

called periods or series.

Periods are numbered 1-7.

The closer two elements are to one another in a period, the more

similar their properties.


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Pause for a Cause

Learning Activity #1Identify the element located in:

a) Group 2 Period 4b) Group 17 Period 6

c) Group 13 Period 2

d) Group 10 Period 4

e) Group 1 Period 1


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Metals, nonmetals, and metalloids can be located on the

periodic table by knowing where to find the metalloid line!


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Properties of Metals

Conductive- metals aregood conductors of heat andelectricity

Malleable- metals can be

hammered into thin sheets

Ductile- can be drawn intothin wire

Tenacious- metals havehigh tensile strength andresist being pulled apart

Lustery- metals are

recognized by their shine


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Examples of Metals

Potassium, Kreacts with

water and must

be stored in

kerosene Copper, Cu, is a relatively soft metal, and

a very good electrical conductor.

Mercury, Hg, is the only metal that

exists as a liquid at room

temperature


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Propertiesof NonmetalsCarbon, the graphite in pencil lead is a great example of a

nonmetallic element.

Nonmetals are poor conductors of heat and electricity

Nonmetals tend to be brittle

Many nonmetals are gases at room temperature


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Examples of NonmetalsSulfur, S, was once

known as

brimstoneMicrospheres of

phosphorus, P, a

reactive nonmetal

Graphite is not the only pure form

of carbon, C. Diamond is also

carbon; the color comes fromimpurities caught within the

crystal structure


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Metalloids straddle the

border between metals

and nonmetals on the

periodic table.

They have properties of both metals and nonmetals.

Metalloids are more brittle than metals, less brittle

than most nonmetallic solids Metalloids are semiconductors of electricity

Some metalloids possess metallic luster

Properties of Metalloids


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Silicon, Si A Metalloid

Silicon has metallic luster

Silicon is brittle like a nonmetal

Silicon is a semiconductor of electricity

Other metalloids include: Boron, B

Germanium, Ge Arsenic, As

Antimony, Sb

Tellurium, Te


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Noble Gases

Unreactive

Gases at room

temperature

Neon, argon, krypton

and xenon are used in

lighting

Helium is used in

balloons


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Pause for a Cause

Learning Activity #2Tell whether each of the following elements is a

metal, nonmetal, metalloid or noble gas:

a) Silicon

b) Chlorinec) Sodium

d) Iron

e) Antimony

f) Radon

g) Cesium

h) Sulfur


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Have a silvery appearanceand are soft enough to cut

with a knife.Not found in nature as

free elements.

React violently with waterReact with halogens toform salts

The Properties of a Group:the Alkali Metals


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Harder, denser, andstronger than alkali metals.

Higher melting points thanalkali metals.

Not found in nature as

free elements.

The Properties of a Group:

the Alkaline-Earth Metals


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Good conductors of electricity andhave a higher luster.

Less reactive than the alkali metalsand the alkaline-earth metalsSome exist as free elements


the Transition Elements


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Most reactive nonmetals.React with most metals to

form salts.


the Halogens


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Noble GasesGroup 18 Elements

Unreactive

Gases at room

temperature

Neon, argon, krypton

and xenon are used in

lighting

Helium is used in

balloons


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Learning Activity #3The following questions refer to the following

elements

A. Sodium

B. Fluorine

C. Boron

D. Argon

1. Does not interact readily with other elements

2. Reacts explosively with water

3. Is classified as a halogen


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Pure substances

Element

Made of the same types of

atom

Can be just one atom

Chemically bonded

Compound

Made of different types of

atoms

Must be more than one

Chemically bonded


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Building blocks of matter

Elements and compounds can combine to

create mixtures.

Mixtures are combinations of two or more

substances in which each substance maintains

its own chemical identity.


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Types of mixtures

Homogeneous (solutions) Heterogeneous


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Pause for a Cause

Learning Activity #4

Identify each of the following as eitherhomogeneous or heterogeneous:

a) Paper

b) Sweetened Teac) Pencil Lead

d) Fresh-squeezed Lemonade

e) Goldf) Chocolate Chip Cookies

g) Oil and Vinegar Salad Dressing


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Classifying matter



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Classify each of the following as an element,

compound, heterogeneous or

homogeneous mixture.

Chex Mix

Gold ring

Sea water (salt and water)

C6H12O6


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Colloid

Colloids are solutions.They can be described asa substance trappedinside another substance.They can be identified bytheir characteristicscattering of light.

For example: air trappedinside the fat molecules inwhipped cream.


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Suspension

Mixture that contains

solid particles

These particles will fall

out of solution overtime (sedimentation)

Muddy water

Dust particles in the air

Paint


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So you say

Mixtures are combinations in which each part

maintains its own chemical identity.

We can use these identities to separate the

components.


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How would you separate the following?

Have them move! They

will all go at different

speeds.


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What about these?

Iron

Gold


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What about these?

Sand

Water


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Filtration

Used for theseparation ofsolids from fluids(liquids or gases)

by interjecting amedium which thefluid can pass, butthe solids (or at

least part of thesolids) in the fluidare retained.

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http://upload.wikimedia.org/wikipedia/commons/8/86/Filtration_diagram.svg


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And these?

Purple dye

Pink dye

Yellow dye


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Chromatography


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And these?

Salt

Water

Distillation

A

B


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Lab intro

Mixture contains

Salt

Sand

Iron fillings Poppy seeds

All in water

Available equipment

Cotton balls

Filter funnels

Filter paper

Forceps Magnet

Paperclips

Paper towels

Petri dish

Pipettes

Rubber stoppers

Test tubes

Tissue paper

Experiment 1; Modern Chemistry pg 26


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Matter and Energy

Part II: Properties and Changes


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Same, samebut different?

P f M


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Properties of Matter

Extensive properties

Intensive properties

Volume

Mass

Energy Content (think Calories!)

depend on theamount of matter that is present.

do not dependon the amount of matter present.

Melting point

Boiling point

Density

Ability to conduct electricity

Ability to transfer energy as heat


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Tell whether each of the following represents an

extensive or intensive property:a. volume

b. density

c. boiling point

d. ability to conduct heat

e. mass

Pause for a Cause

Learning Activity 7


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Properties of matter can

also either bechemical or physical.


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Physical properties

Characteristics that can be observed

or measured without changing the

identity of the substance.

Melting pointBoiling point

Ch i l P ti


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Relates to a

substances ability to

undergo changes thattransform it into

different substances.

Chemical reactivity

Combusts or Rusts

Chemical Properties

C i f Ph i l d Ch i l


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Comparison of Physical and Chemical

Properties


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Pause for a Cause


Classify each of the following properties as

either chemical or physical properties:

a. color i. tarnishing

b. reactivity j. decay c. flammability k. texture

d. odor l. density

e. ductility

f. solubility

g. length

h. melting point/boiling point


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Physical ChangeA change in a substance that does not involve a

change in the identity of the substance.Example:

Phase Changes(Change of State):

A change of a

substance from one

state of matter toanother.


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Ph


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PhaseDifferences

Soliddefinite volume and shape; particlespacked in fixed positions.

Liquid definite volume but indefiniteshape; particles close together but not infixed positions.

Gasneither definite volume nor definite

shape; particles are at great distancesfrom one another.Plasma high temperature, atoms lose mostof their electrons (fluorescent).


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Heat can be used to change the state of matter.

Low Temperature= Low energy

High Temperature= High energy


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Pause for a Cause #9

a. How does a solid differ from a liquid?

b.How does a liquid differ from a gas?

c. How is a liquid similar to a gas?

d.What is a plasma?


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Chemical Change or Chemical Reaction

A change in which one or more substancesare converted into different substances.

Reactants the substance that react, usually

on the left side of the reactionProducts the substance that are formed,usually on the right side of the reaction

C2H5OH + 3O2 2 CO2 + 3 H2O + EnergyReactants Products

The arrow always points to the products!!


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Evidence of a Chemical Change


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Classify each of the following as a

chemical or physical change:1. Iron metal is melted.

2. Wood burns in air.

3. Milk turns sour.

4. A rock is broken.

5. Iron combines with oxygen to form rust.

6. Moth balls vaporize in a closet.

7. Grapes ferment.8. Salt dissolves in water.

9. Flashlight batteries corrode.

Pause for a Cause

Law of Conservation of Mass


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Law of Conservation of Mass

Energy and Changes in Matter


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Energy and Changes in Matter

Energy is always involved when physical or

chemical changes occur.

Energy can be in various forms.

heat

light

sound

Energy can be absorbed or released in a change,

it is not destroyed or created.

law of conservation of energy


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PART 3: ENERGY AND SPECIFIC HEAT

Matter and Energy


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Energy changes

Endothermicenergy flows into the system, so

the temperature of the surroundings

_______________

Exothermicenergy out of the system, so the

temperature of the surroundings

________________

Are the following processes


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Are the following processes

endothermic or exothermic?

1. Freezing ice

2. Sweat evaporating

3. Fuel burning


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Endothermic vs. Exothermic

In an endothermic reaction, heat is a

_____________ (reactant or product).

In an exothermic reaction, heat is a

_______________ (reactant or product).

The following reaction is _______________

(exothermic or endothermic):

O2 + 2H2 2H2O + heat

http://www learn360 com/ShowVi


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http://www.learn360.com/ShowVi

deo.aspx?SearchText=specific+heat

&ID=139937 Specific heat video

Specific Heat Capacity


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p p y

Also known simply as specific heat (c).

The measure of the heat energy required to

increase the temperature of a substance An intensive property.

Unique for each compound.

The specific heat for water is 4.184 J/gC


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Calculation with Specific Heat

q = mcT

q is the heat absorbed or released(When heat is absorbed the process is said to be endothermic, when heat is

released the process is said to be exothermic.)

m is mass

c is specific heat capacity

T is the change in temperature( means change in, to calculate take the final value initial value)


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A 4.0 g sample of glass was heated from 274 K to 314 K and

was found to have absorbed 32 J of energy as heat.

A. What is the specific heat of this type of glass?

B. How much energy will the same glass sample gain when it

is heated from 314 K to 344 K?

Specific Heat Problems


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Determine the specific heat of a material if a

35 g sample absorbed 96 J as it was heated

from 293 to 313 K.


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If 980 kJ of energy are added to 6.2 L of water

at 291 K, what will the final temperature of

the water be?

Specific Heat Problems (No


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Specific Heat Problems (No

calculator)

How many calories of energy are transferred

when 20 mL of water cool to a temperature of

30 C from a temperature of 90 C. Assume the

density of water is 1 g/mL and the specificheat capacity of water is 1 cal/g*C.


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11.8


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If you have a mixture of water and ice at 0 C and you add a

piece of metal that is 50 C, which of the following will

occur?

A. The temperature of the water will decrease.

B. The temperature of the water will increase

C More ice will form

U3 Matter and Energy

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