Final ReviewFinal ReviewPhysical SciencePhysical Science

1. 1. 1. Protons – positive2. Neutrons - neutral3. Electrons - negative

2. 2. 1. Protons – nucleus2. Neutrons – nucleus3. Electrons – electron cloud

3. 3. 1. Protons2. NeutronsCharge – positive

4. 4. Protons and neutrons. Not based on electrons because the

mass of the electron is too small to count.

5. 5. Stable isotope – same number of

protons but different number of neutrons. Does not break down

Unstable isotope – radioactive isotope used for nuclear weapons, nuclear power plants, and biomedicine. Highly radioactive,Unpredictable in breaking down.

6. 6. Atomic numberYes, because the number of protons

never change

7. 7. Oxidation number – number of

electrons an atom can gain, lose, or share (based on group #)

O: 2-Ba: 2+Li: 1+N: 3-C: 4+

8. 8. They have 8 valence electrons and are

stable . They do not need to react with another group to become stable.

9. 9. Atomic number

10 - 12. 10 - 12. • Metals – left of stair step line• Nonmetals – right of stair step line• Metalloids – on stair step line

13. # of valence electrons

Element Atomic Mass

Atomic #

# of protons

# of electrons

# of neutrons

H 1.01 1 1 1 0

He 4.00 2 2 2 2

C 12.01 6 6 6 6

Cl 35.45 17 17 17 19

O 16.00 8 8 8 8

20. 20. Group 1 has one valence electron and

has to give it away. Group 17 has 7 valence electrons and needs one more to be stable.

21. 21. Halogens - Group 17: 1-Alkali Metals - Group 1: 1+Alkaline earth – Group 2: 2+Nobel Gases – Group 18: 0

22. 22. Physical properties:

Color, shape, size, odor, melting Color, shape, size, odor, melting point, boiling point, state of point, boiling point, state of matter, viscosity, density, matter, viscosity, density, solubilitysolubility

Chemical properties:Flammability, sensitivity to light,

oxidation, tarnishing, corrosion of metals

23. 23. Physical change: Change in a Change in a

substance’s size, shape, or state substance’s size, shape, or state of matterof matter

Chemical changeChemical change: A change of one : A change of one substance into a substance into a differentdifferent substancesubstance

Do you still have the same Do you still have the same substance or is it a new substance or is it a new substance?substance?

24. 24. Iron Rusts: ChemicalIce Melting: PhysicalMilk Sours: ChemicalFood is digested: ChemicalEvaporation: PhysicalSugar dissolves in water: Physical

25. 25. 1. Physical2. Density = mass / volume (d=m/v)3. D = 30g / 12cm3

d = 2.5 g/cm3

26. 26. • Organic compounds always contain

carbon and hydrogen atoms.

27. 27. Atom: smallest part of an element

that can be identified as that element.

Molecule: neutral particle that results from a covalent bond. Can also be polar or nonpolar.

28. 28. Element: Substance that cannot be chemically

broken down into a simpler substance.

Compound:Two or more elements chemically

combined.Differences: Element is by itself where

a compound is two or more elements.

29. 29. Compounds are chemically combined

while mixtures are physically combined.

1.Hetergeneous – unevenly mixed ex: suspension, salad, chocolate chip cookie, granite

2.Homogeneous – evenly mixedex: soda, vinegar, saltwater

30. 30. Ionic:Metal and nonmetalCovalent:2 or more nonmetalsDifference: Ionic – gain and loses electronsCovalent – share electrons

31. 31. H and O: H1+ O 2- H2O

Na and Cl: Na 1+ Cl 1- NaCl

Na and O: Na 1+ O2- Na2O

Be and O: Be 2+ O2- BeO

32. 32. • Boiling Point: Covalent - low

• Melting Point: Ionic - high (does not easily break down) Covalent – low (comes apart easily)

• Conductivity: Ionic – conducts electricity; covalent does not

33.33.• Stirring• Temperature• Pressure• Surface Area

34.

•Solids – tightly packed particles vibrating in place

•Liquids – particles are close, but can move around each other and are not in one place

•Gases – particles bounce off of each other and are as far apart as possible

35. 35. • S to L: particles start slipping and

sliding past each other. The bond holding the particles together is broken

• L to G: particles move fast throughout container and are colliding with one another

36.36.• A. Solid• B. Melting Pt• C. Liquid• D. Boiling Pt• E. Gas• F. Condensation Pt• G. Freezing Pt

37. 37.

• Fe + O2 Fe2O3 No, more iron and oxygen on product side

CH4 + O2 CO2 + H2O

38. 38. • Exothermic: heat released; reaction

becomes hotEx: burning sugar

• Endothermic: heat absorbed; reaction becomes coldEx: ice pack

3939• Mass of a reaction is not created nor

destroyed but conserved.

4040• You have to have equal amounts of

each element on the reactant and product side of the equation

• This is why the equation must be BALANCED

Formulas Reactions with metals

pH

Acids All have H as first element in formula

Corrodes metals

0-7

Bases All have OH in end of formula

They can but generally do not react with metals

Above 7

4242• How quick or slow it takes for a

reaction to occur

43. 43. Ways to increase Ways to increase reaction ratereaction rate • Increase temp• Stir• Adding a catalysts• Increasing surface area (break

down particle size)• Increasing the concentration

28•Elements and compounds are both pure substances

•Elements are made of one type of atom

•Compounds are made of two or more types of atoms

Pg 90-93

•Ionic bond – metal + nonmetal and electrons are transferred

•Covalent bond – nonmetal + nonmetal and electrons are shared

Pg 90-93•Criss-Cross Method•H and O …H+1 O-2

• H2O•Remember – don’t write the charges, the 1’s, or if the numbers are the same -2 and +2

Pg 90-93•Covalent bonds are weak: 1. low melting point 2. low boiling point 3. will not conduct electricity

110-111.

•Temperature – faster if heated

•Surface area – faster if more surface area

•Stirring – faster if you stir it

Pg 110-111

High concentration = more conductivity, lower freezing point

Pg 111

•Polar – water is a polar substance, so if it will dissolve in water, it is polar…like vinegar

•Nonpolar – anything that will not dissolve in water is nonpolar…like oil

Pg 94

Compounds with a hydrogen and a carbon

•Pg 94 (See board)•Draw the following hydrocarbons bonded

•C2H6

•C8H18

Pg 96-99

•Polymer is a long chain of something

•Protein – polymer of amino acids

•Starch – polymer of sugar•Example –•Train – polymer of cars

Pg 96-99

Polymers provide the nutrients we need for daily function…we take in nutrients and our body breaks them down and rearranges them into things we can use.

Pg 96-99Proteins -

Carbohydrates – starches and sugars give us energy

Lipids – fats that

Pg 173 See Board

Fe + O2 Fe2O3

Pg 175.

•Exothermic – heat is given off – temperature goes up

•Endothermic – heat is taken in – temperature goes down

Pg 173

•Matter cannot be created nor destroyed

•The amount of mass you started with before the reaction is the same after the reaction.

•Ex: burning a log

Pg 173

An equation must be balanced to exhibit the above law – in an unbalanced equation, there would be mass being created or destroyed

•Acids have a sour taste

•Bases have a bitter taste and a slippery texture.

Pg 190-193

•pH is very common in a grocery store…

•Lemons – pH 2•Drain cleaner – pH 14•Apple juice – pH 3•Soap – pH 10

Pg 169-171

Reaction rate is how quickly a reaction will happen

Pg 169-171

You can speed up a reaction by raising the temperature, stirring it, adding catalysts or enzymes, increasing surface area, or increasing the concentration

Pg 168-169

•Change in color•Change in temperature•A precipitate forms (a solid glob forms at the bottom)

Acid rain is formed from the pollution and other gases emitted from the environment which is surrounded by dust and dirt in clouds….the dust and dirt fall as rain bringing with it the pollution which is usually acidic

d

t

d

t

v

t

v

t

No motion Constant speed

Constant speed

acceleration

Pg 272-273

Pg 428-431Static electricity is made when two things rub together…electrons jump from one object to another

Pg 462-465Pg 462-465

•Electricity can produce a magnetic field

•Magnets can make electricity flow faster

Pg 442-443Pg 442-443

•Voltage is how much electricity CAN flow

•Amperage (current) is how much actually DOES flow

Pg 292 - 293

PE = highKE = low

PE = low KE = high

PE = highKE = low

Pg 296-305 Energy Pg 296-305 Energy

•Energy is the ability to do work

•Work is using energy to do a task

•Power is how fast you do work

•Efficiency is how well you used the energy to do the work

Mechanical Advantage tells you how well a machine works

MA = resistance force

effort force

Ex. What is the MA of a lever that does 500N with 50N of effort?