Science 20F

Unit: Chemistry in Action

Student Notes

Name: __________

Unit Checklist

HERE ARE THE ITEMS YOU NEED TO KNOW FOR THE CHEMISTRY UNIT IN GR.10 UNDERSTAND HOW TO READ THE PERIODIC TABLE BASED ON THE ELEMENTS

FAMILY, PERIOD AND VALENCY (Valence electrons) BE ABLE TO UNDERSTAND HOW ELEMENTS COMBINE BASED ON THE POSITION OF

THE ELEMENT FROM THE PERIODIC TABLE. EX. ALKALI METALS WITH HALOGENS EXPLAIN USING THE PERIODIC TABLE HOW AND WHY ELEMENTS COMBINE IN

SPECIFIC RATIOS. WRITE FORMULAS AND NAMES OF BINARY IONIC COMPOUNDS FOR BOTH

COVALENT AND IONIC MOLECULES AND COMPOUNDS WRITE FORMULAS FOR COVALENT MOLECULES USING PREFIXES

INVESTIGATE THE LAW OF CONSERVATION OF MASS AND RECOGNIZE THAT MASS

IS CONSERVED (DID NOT CHANGE) IN A CHEMICAL REACTION BALANCE CHEMICAL EQUATIONS

BE ABLE TO CLASSIFY THE TYPES OF CHEMICAL REACTIONS

BE ABLE TO EXPLAIN ACIDS AND BASES PROPERTIES INVOLVING pH, REACTIVITY,

AND INDICATORS NEUTRALIZATION REACTIONS FROM AN ACID AND BASE REACTION

TECHNOLOGIES INVOLVED IN REDUCING EMISSIONS OF POTENTIAL AIR

POLLUTANTS

ATOMS REVIEW

• Everything is made _____________________________. • When we _______________ everything (cells, protein, tables, fuel, gasoline, breath of

air, nails, hormones etc…), we get a _______________ of _______________ joined together.

• There are different “_______________” of atoms that form the _______________ _______________ we have in our entire _______________.

WHAT ARE ELEMENTS

• Elements are the different “_______________” or “flavours” that atoms can have. • Think of _______________ as a _______________ _______________ piece • Think of _______________ as the _______________ types of pieces

• When _______________ atoms are _______________ together, they form _______________.

• That something can be made up of _______________ joined together or a _______________ of _______________ kinds joined together

Every element has their own unique characteristic or properties

1 Kind of Lego pieces or 1 kind of Element joined together forming a pure substance

Different kinds of Lego pieces joined together, or different kinds of elements combined with each other forming compounds or molecules.

EXAMPLES OF ELEMENTS

• Oxygen, Carbon, Lead, Hydrogen, Lithium, Gold, Silver, Platinum, etc…

• Everything _______________ on your _______________ ARE _______________ hence the “Periodic Table of Elements”!

• Elements _______________ be _______________ down any further. They are the _______________ broken down type of matter.

• If we were to _______________ down a bar of _______________, you would have all _______________ atoms.

• Chlorine? • Aluminum? • Water? • Carbon dioxide? • Tin? • Nitrogen? • DNA? • Cell?

ELEMENT OR NOT AN EL EMENT?

• There are 3 _______________ particles:

1) _______________ 2) _______________ 3) _______________

• _______________: have a _______________ charge, are in the _______________, and

_______________ the _______________ number

• _______________: have a _______________ charge, are on orbits around the nucleus,

and equals the _______________ number (in pure atoms, not ions)

• _______________: have _______________ charge, are in the nucleus, and equals the

_______________ number minus the _______________ number

• This is the periodic table of elements • All elements known to man are

arranged in this chart. • Elements are a substance that cannot be

broken down further, so elements are atoms.

• Examples: Oxygen, Aluminum, Calcium are all elements

STRUCTURE OF AN ATOM

• The _______________ is the big number in the top of each element box • The _______________ is the small number _______________ the element’s symbol

ex: Protons = Electrons = 7 Neutrons = _______________

Nucleus has Protons and Neutrons

Electrons on outside

N

7

14.01

There are _______________ on the periodic table.

_______________ are the columns (up and down).

_______________ are the rows (left and right).

_______________ are the elements in the _______________ column.

_______________ are the elements in the _______________ column.

_______________ are the elements in the _______________ column.

_______________ are the elements in the _______________ column.

_______________ are the elements in the last (_______________ column.

HOW IS THE PERIODIC TABLE ARRANGED?

Groups go up and

down.

Tells you how many _______________ there are. • Valence electrons

• Found on the _______________ most _______________ of an atom • Only _______________ _______________ combine or _______________ into

_______________ atoms to _______________ bonds • In elements _______________ than _______________ metals, there can only be

a _______________ of _______________ valence electrons • _______________ has _______________ valence electron, _______________ has

2 _______________ electrons, etc…

• _______________ diagrams show electrons in _______________ shells • 1st shell has a _______________ of _______________ • 2nd and 3rd shells have _______________ of 8 electrons • The electron number on the _______________ shell are your ______________

electrons.

WHAT DO THESE COLUMNS TELL US?

BOHR DIAGRAMS

DRAW BOHR DIAGRAM OF BORON AND S IL ICON

An _______________ is “happy” when it has a _______________ shell of

_______________ (like the noble gases) Elements will try to _______________ 1 or _______________ 1 valence electron on its

valence shell. Ex. Sodium has _______________, so it will try lose electrons to form bonds. Ex. Cl has _______________ electrons, so it will try to gain 1.

The periodic table is _______________ into two basic types of elements, _______________ and _______________.

WHY ARE VALENCE ELEC TRONS IMPORTANT?

Periodic table

The _______________ are on the _______________ of the periodic table and the non-metals are on the _______________ of the periodic table.

The metals and non-metals are _______________ by the “_______________”. All elements along the stair-case are known as _______________ that have

_______________ of both metals and non-metals.

• These are bonds that occur _______________ two (or more) _______________. • We will have to _______________ them and also write the _______________ from

_______________

Covalent Bonding

Naming • _______________ bonds _______________ use _______________ when naming • The prefixes are _______________ (1), di (2), _______________ (3), tetra (4),

_______________ (5), and _______________ (6), septa (7), octa (8), nona (9), deca (10) • You name the _______________ normally adding a _______________ if there are

_______________ or more of that element • Then, you name the _______________ element ending in “-_______________” using a

_______________ no matter how many there are. ex: Name the following:

a) CCl4 b) N2O5 Writing Formulae from Names

When given a name, _______________ write the appropriate _______________ and number based on what the name says.

ex: Write the formulae for: a) dihydrogen monoxide

Try these

• 1. CO • 2. N2O3 • 3. SiF4 • 4. diarsenic trisulfide • 5. nitrogen tribromide • 6. diphosphorous pentoxide • 7. diboron hexahydride • 8. N2S3 • 9. Br2

Ionic Bonding

• These are bonds between _______________ and _______________ _______________. • For now, we will focus on the _______________ between one _______________ and

one _______________. • Again, we will both name and write _______________ for these types of bonds. • One major difference from covalent bonds is that ionic bonds _______________ use

prefixes!

Naming Ionic Bonds

• To start, you name the first _______________ _______________. • Then, you name the second element ending in “-_______________”.

**_______________ USE PREFIXES** ex: Name CaBr2

Writing Formulae for Ionic Bonds

• An _______________ is any charged particle.

• Basically any _______________ on the periodic table can be charged • The _______________ column metals will have a _______________ of +1, the

_______________ column +2, then +3, then +/- 4. • After the _______________ column, we get negative ions. • The fifth column is -3, then -2, then -1 and the _______________ gases have no charge

(they can’t be ions!)

• So, in order to write the formula for an _______________ bond, you have to first figure out the charges on each ion in the name.

• Then you _______________ the numbers (forget about the + and – signs). **Make sure after you switch the numbers, you put them below the letters**

• This will allow you to have a neutral compound (all the positives need to balance out the negatives).

ex: Write the formulae for: a) Calcium Fluoride

b) Aluminum sulfide Ionic bonding with transition metals

• These bonds involve metals from the _______________ metals family (_______________ of the periodic table)

• Some transition metals can carry _______________ than 1 charge, ex. Iron (Fe) can be Fe2+ or Fe3+

• To show the charge, _______________ _______________ are used. • Ex. Iron (II) Oxide

Because of the (II), Iron has a 2+ charge

Therefore, Fe2+ O2- FeO

• Ex. – Iron (III) oxide – Fe3+ O2- – Fe2O3 So the _______________ do play a big part!

• Ex. – Copper (II) Fluoride

Going backwards… • Au2O3

• What kind of bond? Ionic bond

• Au is Gold • F is Fluorine

• Gold is a transition metal so we need roman numerals.

• The roman numerals will be the number found on the opposite element.

Gold(III) Oxide

Complex Ionic Bonds

• These involve the reaction between one _______________ and a _______________ ion

_______________ of 2 or more non-metals • Naming is the same as before but the _______________ part _______________ end in

“-ide” but rather it’s named using the _______________ ion chart. • Writing _______________ works the same but you should always put a complex ion in

_______________ before you criss-cross. ex: Name CaSO4

ex 2: Name Al(CH3COO)3 ex 3: What’s the formula for sodium carbonate? ex 4: What’s the formula for aluminum chromate?

Chemical reaction

How do we write a chemical reaction? Say we react vinegar with baking soda.

Vinegar is CH3COOH 2 Carbon, 2 Oxygen, 4 Hydrogens

Baking soda is NaHCO3

The reaction:

CH3COOH + NaHCO3 NaCH3COO + H2CO3

Questions to consider When we reacted the vinegar with baking soda, what happened to the power? And the

liquid?

Did I lose the vinegar and the baking soda?

Did they just vanish into thin air?

After the reaction, was my mass the same as before?

What do you think happened to them?

Law of conservation of mass The _______________ of substances produced (products) by a chemical reaction is _______________ equal to the _______________ of the _______________ substances (reactants).

What does this mean?

The _______________ of the reactants is the _______________ as the mass of the _______________

Also… The _______________ of atoms in the reactants has to _______________ the

number of atoms in the _______________

Types of Reactions There are 6 basic types of reactions that can occur when reactants are reacted with

each other.

These are:

1. _______________

2. _______________

3. _______________

4. _______________

5. _______________

6. _______________ (neutralization)

Types of Chemical reactions Complete the following Info on the various types of chemical reactions

1. Synthesis: General formula: __________________________________________________________ Chemical reaction: _________________________________________________________ Illustration of a synthesis reaction

A short analogy or story of a synthesis reaction: _____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

___________________________________

Balance the synthesis reaction only:

CuO Cu + O2

__________________________________________________________________

Mg + Cl2 MgCl2

___________________________________________________________________

PbCO3 PbO + CO2

_________________________________________________________________

2. Decomposition: General formula: __________________________________________________________ Chemical reaction: _________________________________________________________ Illustration of a decomposition reaction

A short analogy or story of a decomposition reaction: _____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

Balance the decomposition reaction only:

CuO Cu + O2

__________________________________________________________________

Mg + Cl2 MgCl2

___________________________________________________________________

PbCO3 PbO + CO2

_________________________________________________________________

NO + O2 NO2

_________________________________________________________________

Ag2CO3 Ag2O + CO2

_________________________________________________________________

3. Combustion:

General formula: __________________________________________________________ Chemical reaction: _________________________________________________________ Illustration of a combustion reaction

A short analogy or story of a combustion reaction: _____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

Balance the combustion reaction only:

NaHCO3 Na2CO3 + CO2 + H2O

_______________________________________________________

FeCl3 Fe + Cl

___________________________________________________________

C2H6 + O2 H2O + CO2

______________________________________________________________

CH3OH + O2 CO2 + H2O

________________________________________________________________

Ag2CO3 Ag2O + CO2

_________________________________________________________________

What are the products of all combustion reaction?

__________________________________________

4. Single Dispalcement: General formula: __________________________________________________________ Chemical reaction: ________________________________________________________ Illustration of a single displacement reaction

A short analogy or story of a single displacement reaction: _____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

___________________________________

Balance the single displacement reactions only:

KOH + HNO3 H2O + KNO3

_______________________________________________________

BaCl2 + H2SO4 BaSO4 + HCl

_____________________________________________________

F2 + 2KI I2 + 2KF

______________________________________________________________

Li + H2O H2 + LiOH

________________________________________________________________

Ag2CO3 Ag2O + CO2

_________________________________________________________________

5. Double displacement: General formula: __________________________________________________________ Chemical reaction: _________________________________________________________ Illustration of a double displacement reaction

A short analogy or story of a double displacement reaction: _____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

_____________________________________________________________________________

___________________________________

Balance the double displacement reactions only:

KOH + HNO3 H2O + KNO3

__________________________________________________________

BaCl2 + H2SO4 BaSO4 + HCl

__________________________________________________________

F2 + 2KI I2 + 2KF

______________________________________________________________

Li + H2O H2 + LiOH

________________________________________________________________

BaCl2 + Na2SO4 BaSO4 + NaCl

________________________________________________________

Balancing chemical equations Example:

Al + O2 Al2O3 How many of each do I have? How does that make sense? They are not equal! Let’s make them equal: If I have 1 Al atom on the left, and 2 Al on the products side, let’s make 2 Al on the reactants side to balance with the 2 on the right.

Let’s make them equal: If I have 1 Al atom on the left, and 2 Al on the products side, let’s make 2 Al on the reactants side to balance with the 2 on the right. Now we have 2 oxygen on the left and 3 oxygen on the right… we need to make them equal. How about we make them both equal to 6 Multiply Oxygen from reactants by 3 Multiply Oxygen from products by 2

Can we balance the aluminum? YES WE CAN! Multiply the Aluminum by 4 Instead! Examples 1. __NaCl + __BeF2 --> __NaF + __BeCl2 2. __FeCl3 + __Be3(PO4)2 --> __BeCl2 + __FePO4 3. __AgNO3 + __LiOH --> __AgOH + __LiNO3 4. __CH4 + __O2 --> __CO2 + __H2O 5. __Mg + __Mn2O3 --> __MgO + __Mn

Al + O2 Al

2O

3

Is it balanced now? Let’s try it…

The numbers we multiplied are to be put IN FRONT of the elements/compounds

2Al + 3O2 2Al

2O

3

4Al + 3O2 2Al

2O

3

Acids and Bases

Student Ver. Notes and work booklet Brainstorm with your neighbor or in a small group the following:

True or False Quiz *Note: This activity is not for marks! Directions: After each statement, indicate whether you think it is True (T) or False (F). Be truthful and answer to the best of your knowledge. Good luck! 1. All acids will or dissolve many materials or substances. 2. All acids should be considered dangerous because they will burn your skin. 3. There is only one test for an acid: to see if it will dissolve something. 4. Strong acids react with metals faster than weak acids. 5. Acids are made using bases. 6. Acids typically taste sour, while bases typically taste bitter. 7. All chemicals with ‘H’ atoms in their formula are acids, and all chemicals with ‘OH’ in their formula are bases. 8. Acids are stronger than bases. 9. The strength of acids and bases can be recorded using the pH scale. 10. Acids have a lower pH than bases. 11. The concentration of an acid or a base tells you how strong that acid or base is. 12. Acids and bases always cancel each other out.

Introduction: What is an ACID? An acid is a substance (compound) that contains an ____________________to it. Examples: HCl –Hydrochloric acid HNO3 – Nitric acid HBr – Bromic acid CH3COOH – Acetic Acid Properties of acids

Acid reacts with ____________________

Have ____________________taste

Acids neutralize ____________________ What does that mean?

Whenever an acid is placed into a ____________________ (in water), the ____________________ released. See the diagram below.

The more H+ that is released, the ____________________the acid.

What does “releasing” or “dissociating” a H+ ion mean? It means that when the Acid is ____________________in water to form a ____________________, the H+ will be separated and found as an ion. The H+ is separated from the ___________ion ( )See diagram below. The example below is an example of HCl in water. The H+ ____________________from the Cl-.

Here are some common examples of ACIDS – notice the “alone” H+ that is attached to the acid. HCl – hydrochloric acid

o This is your ____________________acid o It has a pH of 1

HNO3 – nitric acid

o Used in making fertilizers o Can be used in ____________________ o Can be used in wood working o Extremely corrosive as it reacts with protein (basically what you are made of!)

H2SO4 – Sulfuric acid

o Drain cleaner o Found in car ____________________ (carries electrons) o Other cleaning agents and fertilizers

HF – Hydro fluoric acid

o Highly corrosive that can dissolve through metals and glass o Reactive with metals but not plastics o Can cause painless burns that will eat up the calcium inside your body causing cardiac arrest

CH3COOH – Acetic acid (Household vinegar)

o “Weak” acid o Used in cooking o Not very reactive but will react with base (baking soda)

What is a BASE? Instead of having a H+ that can be given off as in an ACID, a BASE is one that gives off a ____________________ Bases usually contain a OH- Just like an acid, a base releases a OH-

Properties of bases

Neutralizes acids

Feels ____________________and tastes ____________________ (soap)

Just like an acid, a base releases a OH-

Here are some common examples of bases – notice the “alone” OH- that is attached to the base. Sodium hydroxide (NaOH) or ____________________

Is a solid until dissolve to make a solution

Slippery when touched

Found in most ____________________

Very caustic (causes burns)

Used in paper making industries, paint stripping, food preparation

Potassium hydroxide (KOH) Calcium hydroxide Ca(OH)2

Found in _____________ to __________________.

NH3 – Ammonia – contains no –OH but is still considered as a base

Is a “____________________” base

Found in our urine – Ammonia was thought to be a “life” compound that cannot be man-made as it was produced by living things until Joseph Presley (1774) isolated it and revolutionized chemistry as now it is believed that “life” compounds can be synthesized.

The 6th type of chemical reaction - Mixing acids and bases Mixing an acid and a base will give a ____________________reaction.

o A neutralization reaction is a ____________________reaction. o Salt and water are the products of a neutralization reaction.

Salt is NOT just NaCl!!!!

Ex. HCl + NaOH ____________________ (or just H2O)

Salt

Ex. HCl + KOH ____________________ (or just H2O) Salt Measuring the “acidity” or “base-ness” of acids and bases

Since acids mainly contain H+ ion, a pH scale is developed

A pH scale was developed to rate the ____________________________ in a solution

pH stands for “____________________” where each step is ____________________ more powerful than the previous.

pH Scale ranges from 0 – 14 where ____________________ is the ____________________middle point (where water is found).

Any pH reading that is greater than 7 is considered ____________________or alkaline and any reading below 7 is considered ____________________

Example of pH scale with various substances The ____________________the number on the pH scale, the more ____________________it is. The ____________________the number on the pH scale, the more ____________________it is. How do we test the acidity of a substance? There are various ____________________such as ____________________, ____________________, Universal indicator and others.

Phenolphthalein

Phenolphthalein is ____________________when PINK but turns colourless when it becomes an acid.

P A C - Phenolphthalein is Acid when clear

Litmus Papers

Review:

1. How is an acid defined as in terms of chemistry? What about Base? 2. List all the characteristics of an acid and of a base 3. What does it mean when a H+ or OH- ion is “dissociated”? 4. What are always the products of a neutralization reaction? 5. What type of reaction (single displacement, double displacement, synthesis,

decomposition) is a neutralization reaction? 6. Complete the reactions

Pink Litmus Paper Blue Litmus Paper

Turns Blue when Basic

Notice the first letters of BLUE and BASIC

Turns Red when Basic

Or Blue for Basic

Contains phenolphthalein with water

Contains phenolphthalein with acid (HCl)

Contains phenolphthalein with base (NaOH)

a. Ca(OH)2 + HCl b. HF + NaOH c. HCl + NaOH d. Mg(OH)2 + HBr e. HNO3 + NaOH

7. Describe how to read a pH scale 8. Which of the following would have a higher pH?

a. NaOH or HCl b. Vinegar or milk c. Drano or lemon juice d. Car battery or blood e. HF or Ca(OH)2

9. You placed a drop of phenolphthalein indicator in an unknown solution. The solution turns pink, what can you conclude about the pH of the solution?

10. You dipped a red litmus paper in lemon juice. What colour should you expect the paper to turn?

11. You dipped a blue litmus paper in lemon juice. What colour should you expect the paper to turn?

12. You dipped a red litmus paper in Drano (with NaOH). What colour should you expect the paper to turn?

13. A solution with phenolphthalein and 50ml HCl has turned the solution colourless. What type of solution can you put in to change the colour back into pink? How much?

Answer Keys: Review Key

1. Acid releases H+ while a base releases OH- in solution (with water) 2. Review the notes above

3. H+ is released into solution when it is dissolved in water for acids while OH- is released into solution when it is dissolved in water

4. Salt and water 5. Double displacement 6.

a. CaCl2 + H2O b. NaF + H2O c. NaCl + H2O d. MgBr2 + H2O e. NaNO3 + H2O

7. Review the notes 8. High pH means it is more basic

a. NaOH b. Milk c. Drano since it is NaOH d. Blood (pH of about 8.0) e. Ca(OH)2

9. It is basic 10. Stays the same 11. Turns red 12. Turns blue 13. A strong base such as NaOH and exceed 50ml since 50ml will just neutralize it completely, having over

50ml will make it basic.