Name: Class: Date:---------- -------- -----

MATTER

Everything is made of matter. Matter has two fundamental properties: it has weight(mass) and it takes up space (volume).

All matter has a variety of properties, some of which are characteristic of thesubstance. Characteristic properties do not depend on the amount of the substance (asmass and volume do). Properties such as magnetic attraction, conductivity, density, pH,boiling point and solubility are characteristic properties that can be used to identifysubstances.

Definitions

Matter: Anything that has mass and occupies space (volume). Every form of matter hasphysical and chemical properties.

Physical properties: can be observed without changing into another substance, no chemicalbonding:

Examples: size, shape, hardness, solubility, magnetism, texture,color, and density.

Chemical properties: the ability of a substance to change into different substances,chemical bonds formed or broken.

Examples: the abi lity to burn or rust

Mass: the amount of matter in an object (basic unit of measure is grams)

Volume: the amount of space that an object takes up (basic unit of measure is liter)

Density: Relates the mass of a substance to its volume. The more matter in a set volume,the more dense it is.

Expressed as units of mass per unit of volume (example: grams/liter)

Formula:Density = Mass

Volume

~~

~~

More dense f------------------------------------------------------------------------~Less dense

I

Name: Class: Date:-------- -----

Calculate the density of the following matter:

1. What is the density of a substance that has a volume of 3 ml and a mass of 9 grams?

2. Calculate the density of a substance that has a mass of 500 grams and a volume of50 liters.

3. What is the density of a substance that has a volume of 10 ml and a mass of 90grams?

2

Name: Class: Date:---------- -------- -----

MIXTURES

Solids, liquids or gases can be combined to form mixtures. In a mixture, eachsubstance keeps its individual properties. In some mixtures, each of the componentscan be seen (for example, rocks, twigs, insects and leaves are visible components ofsoil); in other mixtures, the individual substances blend so well that they appear to bea single substance (for example, oxygen, nitrogen and carbon dioxide are mixedtogether to form air).

Mixtures can be separated using different methods, depending on the physicalproperties of the component substances. Fi Itering, evaporating, floating/settling,dissolving, and using magnets are all methods for separating mixtures based on theproperties of their components.

Solutions are mixtures that appear to be single substances because particles havedissolved and spread evenly throughout the mixture. Not all separation methods areeffective for separating the components of solutions.

Lab Activity to Separate Mixtures

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Narne.: Class.: _

13-2 Changes in Matter

Date: _

Key Concepts

~ What is a physical change?

I}--T What is a chemical change?

....,. How are changes in matter related to changesin energy?

Key Terms

• physical change • chemical ch,mge • energy

• thermal energy • endothermic change

• exothermic change • law of (On~rvationof mass

Physical and Chemical Changes Matter can undergo physicalor chemical changes. In a physical change, a substance does notchange its identity. Only a physical characteristic, such as shape or vol­ume, changes.~ A substance that undergoes a physical change isstill the same substance after the change. One example of a physicalchange is a change in state. Changing from a solid to a liquid or from aliquid to a gas is a dlangt' in state. If you place water in an ice tray andfreeze it, the water experiences a physical change. Other kinds of phys­ical changes are dissolving, bending, crushing, and filtering.

The other way that matter can change is by a chemical change, inwhich one or more substances combine or break apart to fonn one ormore new substances. h Unlike a physi.cal change, a chemicalchange produces new substances with different properties fromthose of the original substances. Combustion, or burning, is onechemical change. When natural gas burns, it combines with oxygen inthe air to produce carbon dioxide gas and water. Other examples ofchemical change are electrolysis, oridation (rusting), and tarnishing.

Energy Changes Energy is the ability to do work or causechange. h Every chemical or physical change in matter includes achange in energy. "When ice melts, it absorbs energy from the sur­rounding matter. When water freezes, energy is released.

One kind of energy is thennal energy. Thermal energy is the totalenergy of all the particles in an object. Thermal energy always movesfrom matter at a higher temperature to matter at a lower temperature.Thermal energy is different from temperature. Recall that temperatureis a measure of the average kinetic energy, or energy of motion, of theparticles in an object. Temperature depends on the amount of thermalenergy an object has. A change in thermal energy often causes achange in the energy of motion of the particles. Thus, a change inthermal energy may change the temperature ofa substance.

Thermal energy is the most common form of energy released orabsorbed when matter changes. lee melts when it absorbs thermalenergy from its surroundings. The melting of ice is an endothermicchange, in which energy is taken in, or absorbed. When wood burns,energy is given off in the form of heat and light. Burning is an exampleof an exothennic change. which releases, or gives off, energy.

4

physical mange

chemical change

energy

thermal energy

endothermic change ___

Name: Class: Date: _

A.600§1;~500

Volume {mU ;:

200'00

600500

2i,~~~;:.~~'00 ~~·~:a~:;O~..aJ

Figure 13-1As the for(~ (weight) on the particles increases, density increases because theparticles are forced into a smaller spoKe.

Law of Conservation of Mass Matter is not created ordestroyed in any chemical or ph~ical change. This important state­ment is the law of conservation of mass. The application of this prin­ciple is often easy to Stt in physical changes. When an object is dividedinto two parts, for example. the sum of the masses of the parts equalsthe mass of the original object. Matter sometimes seems to disappearduring a reaction, but that is not what is really happening. When paperis burned, for example, the mass of the ashes is less than the mass of thepaper. Howevcr, if you include the mass of the gasn released duringburning. you Stt that the law of conservation of mass is not violatro.

Figtm 13·1 shows how the raw or consavation ofmassapplies to achange in de-:nsity. A gas-fill~ jar is covewl. by a movable top. Placingweights on the top pushes the gas into a smaller volume_ The densityof the gas increases. because thi volume is reduced but its m~ssremains the same.

Section 13-2 Assessment1. CllUsifying Which of the following processes is a chemical

change: drying wet clothes, cutting snowflakes out of paper, light­ing a m.atch from a matchbook?

2. Applying Concepts Name some types of evidence that you couldlook for to determine whether a chemical change has occurredduring an experiment.

3. Inferring If your teacher ~ets two chemicals in a jar and the jarfeels warm, is this an endothermic or an exothermic reaction?

5

DEfINE ,uotMnnic cNnge ___

law of conservallon of mass

Name: Class: Date:---------- --=-cc------- -----Phases of Matter

- definite shapeSOLID

•- definite volume ICE

- atoms are locked into somekind of structure

- takes the shape of containerLIQUID - definite volume WATER

~· . .- atoms roll over, under, and· . .. ..· .....· ......· . .· . . .

around each other· . . .

GAS

~- takes the shape of container STEAM

<'< .<. - does not have definite volume· .......· ......··,(··st··......· ....· .......· ......- atoms push away from

each other

6

STRUCTURE OF THE ATOM

rtfeu'ron~

Pr:olone

M

......... -.... LI .... ~ _. .......\ " I• .... K .... /\ /- - - "-\.. / e -,-Ii

~ / /",,.....- /,~ /~. ,. - - -... ..I ......" ..."I' •. ~ .., \

\- '.- Ji

~ Electron SheIIS)-

Atom

Nucleus

electron shells

or levels

Numbervaries

All elementsin the same

period havethe samenumber oflevels

tiny particle thatmakes upeverything in theworld

the center of theatom

the outer cloudaround the nucleus

orbits or energylevels of electronsflying around thenucleus

Atom

Nucleus

Neutro ProtonElectron

electrons

protons

Neutrons

negativecharge

positivecharge+

no charge

very tiny particleorbiting the

nucleusEquals the numberof protons

larger particle innucleus

# of protonsdetermine the kind

of atom

Equals the numberof electronslarger particle innucleus

Name: Class: Date:---------c-- --=----=:------ -----Arranging the Elements

Dmitiri Mendeleev designed the first periodic table in 1869. He organized the 63elements that were known at the time into rows according to their atomic mass. Theelements were grouped in columns. All elements in a column had similar physical and chemicalproperties.

In the modern periodic table of over 100 elements, the known elements arearranged in order of increasing atomic number. When the elements were arranged by theiratomic number, it was found that the elements periodically (at regular intervals) had thesame properties. This is called the periodic law.

Each vertical column of the periodic table is called a group. All of the elements inthe same vertical column have similar chemical properties because they have the samenumber of electrons (-) in their outer electron shell.

Each horizontal row of the periodic table is called a period. All of the elements in aperiod have the same number of energy levels.

Chemists use the periodic table to predict how elements wi II react with one anotherand to find out information about each element. Each square on the periodic table containsinformation about the element in it. The following information may be included:

Atomic number8

Name of element

0-1---Oxygen

16 --+---

Chemical symbol

Atomic mass

Use the periodic table of elements to answer the following questions:1. How many periods are there in the main body of the periodic table? _

2. How many groups are there in the periodic table? _

3. What is the chemical symbol for Aluminum? _

4. What is the atomic number for Carbon (C)? _

5. What is the atomic weight of Iron (Fe)? _

6. Calcium (Ca) has 2 electrons in it's outer shell, how many electrons do youpredict Strontium (Sr) will have? Why? _

7. Iron has 4 energy levels. How many energy levels do you predict that potassium,calcium, and zinc will have? Why? _

8

Ir;===============;1The Periodic Table of elements

til-, ,Li Be~­,

f66-::===t-...-.-.,·~ ........_·~-...,,-c c_.._CARIlO,~_C__

12 . -_..__ ._'0'_'

11,NC#-ME'TALa '7'

,. • q fl'

BCNOFNe""" -... ..,..... ...- ~-- """

" ,N, M- METALS, ,

.~:I: " , ,

~<~~S, Ti V CrT~1nT"'e

~INi Cn

~.- - -- ~ - -" .. •" " , ,. " .. "'I lJ" "Rio S, Y Z, Nb 1,1\10/'1~ Ru

Rh Pd ~J,,~_. - - ... - -" • " " "- ,. " .. ,n

•C, Bn '" T. W R, 0, I, PI An_.~ .- _.

~_. -- ~ .- _.

I." I." ,.'"

,. ,. '''' " '" '".. •• ,. , I ,.... I "F, R. ~ R~,.J. Bh ~~Ds R.- - om, 0- , '," , "' '," " 'w

KEYl;l_ .....__.-_._-0- ,_

...~ , • "a~

" " , .. , " 0AI SI P S CI M "- ,~ - ~ - - "TI " " • ",

~~':': K;z.

*'G, '"- .... -".. .. ,. " • " ,.

Cd In Sn Sb T, I X,, ,

~li n~:!. ~ n~!'2.. ~ ~.. "~"~1'~""" m"""" "'~~ Uu .!l~Jl Uuh Uuo'",,"",,'",'" .

Name: Class: Date:-----

It All Adds UpYou can use the periodic table to find the number of protons, neutrons, andelectrons that the atoms of an element have.

All atoms of a particular element have the same number of protons (+), andelectrons (-), but the number of neutrons they have may be different.Atoms of the same element with different number of neutrons are calledisotopes. Isotopes have the same atomic number, but different atomicmasses. In nature, an element is found as a mixture of different isotopes.The atomic masses in the periodic table are the average for an elementsisotopes.

Atomic number =number of protons

(Number of protons = number of electrons)

70Ca

Calcium

Atomic mass =number of protons + number of neutrons_ ~40.08

SoAtomic mass - atomic number =number of neutrons

Use the information above to fill in information on TheAtoms Family Math Challenge

Example: Atomic number of Co =20

Atomic mass of Co =40.08

# of protons =20

# Neutrons =40.08 - 20 =20.08

# electrons =20

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Name: Class: Date:---------- -------- -----

Atoms Family Math Challenge Questions

1

HHydrogen

1.0079

6C

Carbon

12.011

13

AIAluminum

26.9815

26

FeIron

55.847

HAtomic number = _Atomic mass =# of protons =# Neutrons =# electrons = _

CAtomic number = _Atomic mass =# of protons =# Neutrons =# electrons = _

AIAtomic number = _Atomic mass =# of protons =# Neutrons =# electrons = _

FeAtomic number = _Atomic mass =# of protons =# Neutrons =# electrons = _

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Name: Class: Date:---------- -------- -----

Common Elements

Element Symbol Atomic Form at Occurs Uses General Informationname # Room

temp

hydrogen H 1 gas 90% ofthe universe combines with a to Non-metal ,Hydrogen is the most basic andmajor part of stars form water, common of all elements in the universe. Overextremely flammable combines with C to ninety percent of all the atoms in the universe are

form all life, hydrogen atoms and they are the lightest of allfuel cells elements.

carbon C 6 solid in all life forms, food for our bodies Non-metal, carbon is the magic element forcarbohydrates from fuel for our culture: everything on Earth. All life on Earth depends onthe sun's energy in gas, coal, oil carbon. It is in nearly every biological compoundplants that makes up our bodies, systems, organs, cells,

and organelles. When you breathe out, it's carboncombined with oxygen. Carbon has been knownand used for thousands ofyears.

It was never really discovered. Ancient peopleknew ofthe black soot left over after a fire. Thatwas carbon.

oxygen a 8 gas 1/5 of Earth's essential for Non-metal, oxygen is a colorless and odorlessatmosphere, breathing, compound that is a gas at room temperature.easily forms 2/3 of our bodiescompounds,plants exhale oxygen,creates energy we seeas light from stars,fuels fire

protects life fromthin layer around ultraviolet raysEarth's atmosphere

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Name: Class: Date:---------- -------- -----

Element Symbol Atomic Form at Occurs Uses General Informationname # Room

tempaluminum Al 13 solid does not exist soda cans to auto The metal aluminum is a silvery white color and

naturally in its pure engInes very reflective. Another great trait of aluminum isform- must be aircraft that it is not toxic. So cook and eat away, theseparated from ore aluminum foil will not get you sick.bauxite When aluminum is combined with other metals it

becomes very strong. It is so strong that engineersuse it to build planes and ships.Will not rust, not magnetic

Hon Fe 26 solid Earth's crust, black element for The metal iron is found all over the Earth and thesand maintaining blood Universe. You have iron in your computer, your

molecule desk, and even your body.does not exist hemoglobin,naturally in its pure machinery, When purified, iron is a grayish, shiny metal. Itform- must be steel alloy oxidizes easily and the resulting compound isseparated from known as rust (iron oxide). Rust is a reddish-hematite brown color. While you may think of iron as a

magnetic metal, not all forms of iron are magnetic.

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Name: Class: Date:---------- -------- -----

Compounds vs. Mixtures

Atoms can combine chemically to make a molecule of a new substance with newproperties called a compound. A molecule is the smallest part of a compound andis made of atoms of different elements in specific amounts. Unlike mixtures,compounds cannot be separated using the physical properties of the componentelements.

Compounds have different properties than the individual elements of which theyare made. For example, table salt (NaCI) is a compound with differentcharacteristic properties than the elements sodium and chlorine from which itis made; water (H 20) is a compound with different characteristic propertiesthan the elements hydrogen and oxygen from which it is made. Differentamounts of the same elements can produce compounds with different properties(for example, water (H 20) and hydrogen peroxide (H 20 2).

In a chemical reaction, atoms can rearrange to form different molecules of newcompounds. During photosynthesis, carbon dioxide (C02) is taken in by greenplants and combined with water (H 20). The carbon, hydrogen and oxygen atomsrearrange to make two new compounds: glucose (made of atoms of carbon,oxygen, and hydrogen) and oxygen gas (made of atoms of oxygen).

Questions:

1. Compare and contrast a mixture and a compound. A Venn diagram may be used.

2. Provide an example of a mixture: _

3. Provide an example of a compound: _

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Name: Class: Date:---------- -----

HOW DO YOU IDENTIFY A METAL?

What are the characteristics of metals? There are four traits that wi II help you

identify whether an element is a metal or not.

Conduction: Metals are good at conducting electricity. Si Iver (Ag) and copper (Cu)

are some of the most efficient metals and are often used in electronics.

Reactivity: Metals are very reactive, some more than others, but most form

compounds with other elements quite easily. Sodium (Na) and potassium (K) are

some of the most reactive metals.

Chemical: A little complex here. Metals usually make positive ions when the

compounds are dissolved in solution. Also, their metallic oxides make hydroxides

(bases) (OH-) and not acids when in solution. Think about this example. Sodium

chloride (NaCI), when dissolved in water, breaks apart into sodium (Na+) and

chlorine (CI-). See that sodium is the positive ion? Sodium is the metal. It works

that way for other metals. Potassium ch lorine (KCI) works the same way.

Alloys: Metals are easily combined. Mixtures of many elements are called alloys.

Examples of alloys are steel and bronze

Common Elements and Identifying Metals Questions

1. Refer to the Periodic Table and identify 6 metals on the periodic table, write theirname, chemical symbol, and atomic number:

2. Compare and contrast aluminum and iron.

15