UNIT 1Matter and Measuring

Ch. 2,3,4

WHAT IS MATTER??

Examples: color shape density temperature

A. Matter: Anything that has and B. Physical Property: is a quality or condition of a

that can be observed or measured

matter

volumesubstance without attempting to chemically

change it..

Physical Properties of three States of Matter

Solid Liquid Gas

Picture

Properties of Water(H2O)

•Definite shape•Definite Volume•Not compressible•Close together•Vibrating

•Indefinite shape•Conforms to container•Definite volume•Not compressible•Flowing •Low energy

•Indefinite shape•Always fills containers•Indefinite Volume•Easily Compressible•Far apart•Flying•High energy

C. Physical Change alters the material without changing it’s identity

Section Review 2.1

2.

3. (include an explanation for how you now it’s a physical change)

a. c.

b. d.

2-2 MixturesA. A mixture is a that are not a. mixtures are i.e. b. Homogeneous mixture are also called

c. mixtures are i.e.

multiple substance

chemically bonded togetherHomogeneo

us exactly the same composition through out.

Kool aid, liquid cleaners

solutions

Some Common Types of Solutions

System (States of Matter)

Examples

Gas → GasLiquid → GasGas → LiquidLiquid → LiquidSolid → LiquidSolid → Solid

Nitrogen is out air, CO2, O2 are dissolved inHumidityCarbonated BevGasoline mixturesSalt into waterMetal alloys Heterogeneous two or more distinctly different compositions

sand, Oreo cookies, sandwich

B. Separating Mixturesa. Mixtures can be separated by This means

youdo no actuallyb. The composition of a mixture i.e. lotions, drinks, cleaners, concrete. i. Some common physical properties that allow you to

separate mixtures. ( Magnetism, boiling point, solubility) ii. Study figure 2.5, ph 34. Then check out the distillation

demo. Explain how it works by describing the physical properties and physical change of the substance.

physical means.create new substances

varies.

Section Review 2.26. (pg. 34, explain each answer such as: Air = homogeneous bc it is the same color, odorless, gas throughout.) a) b) c) d) e)

7.

9.

10.

11.

Hetero or Homo Mixture Why?

1. Dish Soap:2. A Rock:3. Stainless Steel:4. Brewed Coffee:5. Carbonated Pop:6. An Egg:7. Dust Free Air:8. Rusty Nail:

Same green, slimy, liquidDifferent colorsSame shiny solid

Gas and liquidWhite, yoke, shellMixture of dissolve gasesRust and Iron

2-3 Elements and CompoundsA. Pure substances can be classified into two groups:

&

a. Pure substances have . i.e. B. The simplest form of . be broken

down by i.e.

C. that combine chemically to form a larger substance called a In general, the properties of a are quite different from those of their

a. Homogenous looking?? Be careful. Of the four types of matter (list them below)

circle the three that always look homogeneous(the same throughout)? The only way to tell is if you know what is in it, or if you test it by

elements compounds.

definite compositions

sugarElements :

matter Cannotany means. Hg, Ag, Au, O2

Compound :Different elements compound.

compoundcomponent elements.

element compoundheterogeneous mix

homogeneous mix

chem and phys props

D. Symbols and Formulas a. ______________All matter is ultimately composed of

Each is represented by a one or two letter Notice on theperiodic table that each symbol has only capitol letter.

List any elements names and symbols you already know:

b. When two or more elements are bonded together they form a In a compound formula, are used to represent the number of each element in the compound. Compounds always have capitol letter.

• Water is made of two hydrogen atoms and one Oxygen atom, the formula is

atoms (elements).

element symbol.one

Compounds:

differentcompound.

subscripts

more than one

H2O

2 H2 + 1 O2 → 2 H2O

Demo

• Sugar is made of six carbon atoms, twelve hydrogen atoms, and six oxygen atoms. The chemical formula is

•Table salt (Sodium Chloride, NaCl) = Sodium = Chorine =

Hydrogen: H2 = Elem./Comp

Physical Properties:

Chemical Properties:

Oxygen: O2 = Elem./Comp

Physical Properties:

Chemical Properties:

Water: H2O = Elem./Comp

Physical Properties:

Chemical Properties:

Less dense than airOdorlessClear

FlammableReacts with O2

ClearOdorless

Reacts with H2, L, Mg, Na, wax

Clear, 1g/mL = Densityroom temp liquidF.P. = 0 ˚CB.P = 100 ˚C

8H12 O6

Required for life, white, solidexplosive, metal dangerousGas @ room temp, poisonous, yellow

Matter

Section Review 2.3

14.

15.(write both the name and symbol)

16. (write both the name and symbol)

17. (copy the word, then identify as element, compound, Homogeneous or Heterogeneous Mixture)

2-4 Chemical ReactionsA. In chemical reaction, one or more substances are changed into that have a) Common observations of chemical changes are:

B. Chemical Properties. The to undergo a to form new substances.

1. Can only be measured bya. Common reactions test for:

C. Chemical express the chemical change using symbols and formulas. a. Starting substances in a chemical reaction are called

because they are the ones that

b. The new substance that form after the chemical change are called the because they are

I.e: right nowo you are burning sugar with oxygen gas. In turn, you are producing carbon dioxide gas and water. This is expressed in a chemical equation below.

entirely new substances new chemical & physical properties.

reacts with oxygen ( slow= rust; med= flammable; fast= explosive) color change, heat change.

ability(or lack of)chemical reaction

trying the reaction out.

reacts with oxygen, acids, bases, water, salt.

equations

reactantreact.

products produced.

Chemical or Physical Property?

1. Tarnishes in Rain:2. Bends easily:3. Decomposes:4. Reusable/Recyclable:5. Shiny:6. Not Flammable: 7. Perishable:8. Freezable Food:

Chemical or Physical Change?

1. Lighting a firework:2. Boiling Pasta:3. Chewing gum:4. Running your car:5. Rolling your bike:6. Melting a crayon:7. Rusting a nail:8. Opening a can of pop:

ChemicalPhysicalChemical

PhysPhys

ChemChem

Phys

ChemPhysPhys

ChemPhys

PhysChem

phys

D. Law of the of Mass. a. In a chemical or physical matter is never or

b. In a chemical reactions, the mass of the must always the mass of the

Conservationchange

created destroyedproducts

equal reactant.

Section Review 2.420. (do all, copy the change before you anwer)

21.

22.a.

d.

23.

3-1 MeasurementsA. Measureable with our senses, or with non number

descriptions = data.a.

B. Measurable with numbers = data:b.

C. Scientific Notation: A number written as the product of two numbers: a and raised to a power.

c. 3.6 x 104 = d. 8.1 x 10 -3 = e. Try to express 0.000 000 000 000 000 000 000 327 in scientific notation.f. Try to express 2.3 x 107 as a whole number =g. Multiplication: Multiply the coefficients, then add the exponents.

i. (3.0 x 104 ) x (2.0 x 102 ) =ii. (4.0 x 10-6 ) x (2.0 x 102) =iii. (3.0 x 109) x (9.0 x 10-5) =

h. Division: Divide the coefficients, then subtract the exponent in the from the exponent in the

Qualitative Hot or Cold, Dark or Light, Soft or Hard

Quantitative Temp, length, density, mass

coefficient 10

3.6000.008

3.27 x 10-

22 23000000

6.0 x 1068.0 x 10-3

2.7 x 105

denominator numerator

i. =

i. Addition and Subtraction: Simple, you can only or subtract if the exponents are identical. If they are the same, you simply add or subtract the coefficients.

i. 5.4 x 103 + 0.6 x 103 =

1.5 x 102

6.0 x 103

Section Review 3.11a.

b.

3. all, copy problem then give an answer

4. all, copy the problem then give an answer

3-2 International Measurement UnitsA. Basic Units (also called standard international units = metric system

Quantity Unit Symbol Example

Length

Mass( call it weight)

Volume

Density (Heaviness)

*Temperature

Time

Pressure

Engery

meter mavg human = 1.6 m

Joules

Atmosphere

Seconds

Grams

Liters

Kelvin

g

L

K

s

atm

J

1 penny = 2.5g

2 Liters Pop

Water =

0˚C= 273K

1 atm = Sea level @ 0˚C4184J = 1000cal= 1 cal

1 min = 60 sec

*Temperature: Basic Units is . It is found by

• is actually 273 degrees Kelvin. Lots of energy still there.

• is equal to

• is equal to . This is called absolute Everything

Practice Problems!

1. Antarctica can get as cold as -100 °C.How many K is this?

2. If global warming continues, Earth could earn an average temperature of 423 K.

How many degrees Celsius would this be?

Kelvin °C + 273

0°C

100°C 373K

-273°C 0 K zero. stop

173 K

150˚C

Prefix Symbol

Meaning Factor Sci. Example

giga G Billion 1,000,000,000

x 109 computer

mega- M Million 1,000,000

x 106 mega millions

kilo K Thousand 1000 x 103 5K run =32 mi

Deci d thenth 1/10 x 10-

1

centi c hundreth 1/100 x10-2 dime = 1mm thick

mirco u millionth 1/1,000,000

x 10-

6

ind. cells

nano

pico

3-3 Density: Density is i.e. Water density = Cork density =

C. The formula for finding density is

Question: if you have two objects of the same size, and object A is more dense than object B, which one will have more mass?

how heavy for its size. 1 g/cm3 or 1g/mL

0.3 g/mL

mass / volume

Rectangular Solid exampleD=

Odd shaped Solid ExampleD =

Liquid Example D=

Practice Density calculations:

1. An object has a mass of 80 grams and a volume 40 mL. What is it’s density?

2. A liquid has a volume of 200mL and a mass of 150 grams. What is it’s density?

3. A rubber dog toy is perfectly square and measures 5 cm on each side. The package says is weighs 110 grams. What is the density of the toy? Can the person throw it in the water to play with the dog?   4. A clear liquid is poured into a graduated cylinder and reads 50 mL. The weight increased by 70 grams. What is the density? Is it water? 

D. Practice Lab with notes

4-1 & 4-2 Converting Units

A. You must always when converting units. This will pay huge dividends for your entire science future!

B. Math Review: a) Any number can be written over It will not

b) Any number divided by equals

c) If you multiply by , it will * so if you multiply by a conversion factor, you

are really multiplying by____________.

d) Any amount divided by the exact same amount equals *This is called a conversion factor (a fraction with equal amounts on top and bottom, but in different units)

show your work

one. change value

one itself.

one stay the same.

one

C. Dimensional Analysis: AKA showing your work1. Write down the given number, with units. 2. Choose a conversion factor that will get you away from

what you’re and get you to what you Remember, the and of the fraction must be an amount, so it really only equals

3. Place your conversion factor next to the given number so that it is using . Make sure what you is on top, and what your getting rid of is on

4. If multiple changes are needed, just multiply by multiple conversion factors.

5. Cross of units that appear on and . The only unit left should be the one you .

6. In your calculator, multiply all numbers, divide by any numbers.

given want. topbottom equal

one

multiplying brackets wantbottom.

top bottomwant

topbottom

Examples, step by step

1. One step problem: Convert 3 weeks to days-

2. Two step problem: Convert 3 weeks to hours-

3. Four step problems: Convert 3 weeks to seconds-

3 wks * = 21 days

3 wks * * = 504 hrs

3 wks * * * * = 806,400 sec

Practice Problems pgs. 93 – 95 (show all work for all problems)

9.

10.

11.

12.

13.

Section Review 4.2

15. (all)

16.(all, show work)

17. (show work)

18.(prove it by showing work)

19. (show work)

1. Record data in tables• Which info is the Independent Variable?

• Which info is the Dependent Variable

2. Graphing: Find a graph that will best describe your data. This should let a reader know exactly what trends and patterns your data reveals.

-1st: Decide what kind of graph will show what you need.

2nd: Independent variable (x-axis) Dependent variable (y-axis)

3rd: Make a 3:4 ratio graph

4th: Label the title, x-axis, y-axis (include units)

5th: Spread out our numbers using whole paper

Pasta length (cm)

Pasta mass(g)

Dependent Variable Title: ____________

________

Independent Variable Title:_____________________________

Title:________________________________