Types of Compounds

Types of CompoundsTypes of Compounds

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There are two types of compounds

1. Ionic Compounds

These are compounds where electrons are transferred from one atom to another to give each atom full outer shells. This forms a (+) ion and a (-) ion. These oppositely charged ions are attracted to each other to form an ionic bond Eg Na = 2,8,1 Now Na+ is formed

Cl = 2,8,7 Now Cl- is formedThe Na+ and Cl- come together to form NaCl (now we don’t write the charges)

The Na electron is transferred to the Cl atom

Ionic compounds are always between a metal and a non metal

eg Na (metal) Cl (non metal) make NaCl

In year 11 you will be given a table of ions – you don’t have to remember them.

But you must know how to write balanced formula for ionic compounds using these ions

1+ 2+ 3+ 2-

Na+ Mg2+ Al 3+ O2-

Li+ Ca2+

K+ Fe2+

Cu2+

Zn2+

Pb2+

1+ 2+ 3+ 2- 1-

Na+

(Sodium)Mg2+

(magnesium)Al3+

(aluminium)O2-

(oxide)OH-

(hydroxide)

Li+

(Lithium)Ca2+

(calcium)

Fe3+

(ferric)

SO42-

(sulfate) Cl-

(chloride)

K+

PotassiumFe2+

(ferrous)

CO3 2-

(carbonate)

F-

(fluoride)

Cu2+

(copper)

NO3-

(nitrate)

Zn2+

(zinc)

Pb2+

(lead)

Task : write the chemical formula for sodium oxide in your book

Step one:

Write out the two ions from the chart with their charges ie Na+ and O2-

Step two :Step two :Make the two charges balanceMake the two charges balance(in other words are there the same number of (+) as (-) )(in other words are there the same number of (+) as (-) ) Na = +1 and O = -2 no they don’t balance.Na = +1 and O = -2 no they don’t balance.

Step three:Step three:

Now the seesaw doesn’t balance

You must add an extra Na+ ion to make the (+) and (-) balance You must add an extra Na+ ion to make the (+) and (-) balance which ion do you think you will need to add to the seesaw?which ion do you think you will need to add to the seesaw?

Yes you are correct you need to add one NaYes you are correct you need to add one Na+ + to the left to the left hand side of the seesawhand side of the seesaw

Now you write the formula for sodium oxide as NaNow you write the formula for sodium oxide as Na22OO

This tells us in each particle of sodium oxide (NaThis tells us in each particle of sodium oxide (Na22O) O)

There are two NaThere are two Na++ ions and one O ions and one O2-2- ion ion

Task : Find the formula for aluminium oxide

Step one

Write out the ions from your table ie Al 3+ and O 2-

Step two :Step two :Make the two charges balanceMake the two charges balance(in other words are there the same number of (+) as (-) )(in other words are there the same number of (+) as (-) ) Al = +3 and O = -2 Al = +3 and O = -2 no they don’t balance.no they don’t balance.

Step three: Step three:

Add ions to both sides until the charges balance Add ions to both sides until the charges balance

Al 3+ O 2-

Al 3+ O 2-

O 2-

Al2O3 Aluminium oxide

You try this one write out each step : Find the formula for magnesium nitrate

Step one

Write out the ions from your table

ie Mg2+ and NO3-

Step two :Step two :Make the two charges balanceMake the two charges balance(in other words are there the same number of (+) as (-) )(in other words are there the same number of (+) as (-) ) Mg = Mg = +2 +2 and NOand NO33

-- = = -1-1 no they don’t balance.no they don’t balance.

Step three: Step three:

Add ions to both sides until the charges balance Add ions to both sides until the charges balance Mg 2+

NO3-

Mg(NO3)2

NO3-

Then write formula

Starter Task : Write the chemical formula for Calcium hydroxide in your book

Step one:

Write out the two ions from the chart with their charges

Step two :Step two :Make the two charges balance by adding ions Make the two charges balance by adding ions

Step three:Step three:

Write the finished formula without the chargesWrite the finished formula without the charges

You can quietly read the following 6 slides or you can copy them down

Covalent bonds involve atoms sharing electrons to form molecules.

Molecules can be compounds made of two or more different atoms eg CO2, H2O, C6H12O6 etc

Molecules can also be elements where 2 identical atoms are covalently bonded together eg H2, N2, O2, Cl2 etc

Types of CompoundsTypes of Compounds

2. Covalently bonded Compounds

Remember covalent bonds involve the sharing of electrons

This is how both carbon and hydrogen achieve full valence (or outer) shells in CH4.

When atoms form covalent bonds they form molecules.

First draw both atoms with their valence electrons

How to draw the bonding structure of a covalent molecule

1. In pairs use the model atoms to make a methane (CH4) molecule

C atoms are black H atoms are white

Use the long grey bonds to join them

2. Then make an H2O molecule

H = white O = red

3. Then make a SO2 molecule S = yellow O = red

4. Then make an H2 molecule

Show me when you have finished each one

Then make a carbon dioxide (CO2) molecule

Then make a glucose (C6H12O6) molecule (hint make a ring of 6 carbons)

Show me when you have finished each one

Covalent bonding in methane (CH4)

From the carbon atomic number we find:

C6

12

carbon has an electron arrangement of 2, 4

This means carbon has 4 electrons in its valence

(or outer) shell

We can draw the 4 valence electrons of carbon like this:

How many electrons does carbon need in its valence (or outer) shell?

Ans: 8 electrons

H1

1

hydrogen has an electron arrangement of 1

This means hydrogen has 1 electron in its valence (or outer) shell

From the hydrogen atomic number we find:

We can draw the valence electron of hydrogen like this:

How many electrons does hydrogen need in its valence (or outer) shell?

Ans: 2 electrons

Place 4 hydrogen atoms around the C atom so that each H shares an electron with a C electron

Each H atom shares one electron with one C electron to give each H a full valence shell of 2 electrons

This sharing of electrons between H and C also means the C atom has a full valence shell of 8 electrons

Can you see that both H and C atoms have full valence shells by sharing their electrons?

Ions and Molecules

IonsWrite down the following filling in the gaps.

Ions are atoms that have g_____ or l_____ electrons to form p_______ or n________ ions

3 examples of ions are _________ion symbol ( ) , ________ ion symbol ( ) and _________ ion symbol ( ).

Choose from : smallest, neutrons, covalent, electrons, gained, loss, negative, positive, valence, outer, protons, water, hydrogen gas, H2, CO2, H2O

Atoms, Ions and Molecules

AtomsWrite down the following filling in the gaps.

Atoms are the s________ particles that make up all things.They consist of ________ and _________ in the nucleus with e________ in shells around the nucleus.

3 examples of atoms are _________ symbol ( ) , ________ symbol ( ) and _________ symbol ( ).


Atoms, Ions and Molecules

MoleculesWrite down the following filling in the gaps.

Molecules are where two or more atoms share electrons in a c________ bond to give both atoms full v______ or o______ shells.

3 examples of molecules are w_______ formula ( ) , c________ d_______ formula ( ) and h______ g___ formula ( ).


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What is an ion?What is an ion?An anion is an atom that has gained An anion is an atom that has gained electron(s) to form a (-) ion electron(s) to form a (-) ion

e.g Cle.g Cl- - (Chloride) (Chloride) SS2- 2- (Sulfide) (Sulfide)

or a cation is an atom that has lost electron(s) or a cation is an atom that has lost electron(s) to form a (+) ionto form a (+) ion e.g Nae.g Na+ + (Sodium) (Sodium)

FeFe2+ 2+ (iron (ll) ion) (aka Ferric ion) (iron (ll) ion) (aka Ferric ion) FeFe3+ 3+ (iron(lll) ion ) (Ferrous)(iron(lll) ion ) (Ferrous)

Compounds can be two types – Copy this neatly into your book

1. Compounds can be Ionic

Ionic compounds form when atoms lose and gain electrons to form charged (+) and (-) .These oppositely charged ions are attracted together to form an ionic bond.Ionic bonds always occur between a metal and non metal.

Eg Na (+) and Cl (-) come together to form NaCl

Compounds can be two types – Copy this neatly into your book

2. Compounds can be Covalent

These atoms share electrons so that each atom has a full outer shell. This sharing of electrons is called a covalent bond.Covalently bonded atoms form molecules.Molecules are always between non metal atoms.

Examples of molecules are CH4 methane, H2O water, CO2 carbon dioxide

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Atoms and elements

A substance made of one type of atom is called an element

e.g. a piece of Aluminium (symbol Al) consists of only aluminium atoms bonded together and is called an element.

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MoleculesMoleculesSome elements are unstable as Some elements are unstable as single atoms and only exist as 2 single atoms and only exist as 2 atoms atoms covalentlycovalently bonded together to bonded together to form a form a molecule. molecule.

These are usually gasesThese are usually gases

e.g He.g H22 , N , N22, Cl, Cl22, O, O22

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Compounds and MoleculesCompounds and Molecules

Some compounds are molecules that Some compounds are molecules that contain 2 or more contain 2 or more differentdifferent atoms atoms covalently bondedcovalently bonded together. Some together. Some common molecular compounds are:common molecular compounds are:

COCO2 2 (carbon dioxide) (carbon dioxide)

HH22O (water)O (water)

CHCH44 (methane) (methane)

CC66HH12 12 OO6 6 (glucose) (glucose)

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Balancing Reactions Balancing Reactions Mg + O2

Zn + HCl

Fe + Cl2

NaOH + HCl

CH4 + O2

Ca + H2O

NaOH + H2SO4

CH3OH + O2

MgO

ZnCl2 + H2

FeCl3

NaCl + H2O

CO2 + H2O

Ca(OH)2 + H2

Na2SO4 + H2O

CO2 + H2O

2

2

2 3

2

2

2

2 3

2

2

2

2

2 4

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Simple formulae to learnSimple formulae to learn

H2O

CO2

NH3

H2

O2

N2

SO2

Water

Carbon dioxide

Ammonia

Hydrogen

Oxygen

Nitrogen

Sulphur dioxide

NaCl

CaCl2

MgO

HCl

H2SO4

HNO3

NaOH

Ca(OH)2

CaCO3

Al2O3

Fe2O3

Sodium chloride

Calcium chloride

Magnesium oxide

Hydrochloric acid

Sulphuric acid

Nitric acid

Sodium hydroxide

Calcium hydroxide

Calcium carbonate

Aluminium oxide

Iron oxide

Acids Acids release hydrogen ions (H+) in water to give acidic solutions

Common Lab Acids are:

Sulfuric acid (formula H2SO4 )

Nitric acid (formula HNO3)

Hydrochloric acid (formula HCl)

These are strong acids because they form a lot of H+ ions in water

Eg HCl (l) H+ (aq) + Cl- (aq)

Eg H2SO4 (l) 2H+ (aq) + SO42- (aq)

Acids

Other Acids found around the home are:

ethanoic acid (formula CH3COOH )

this is the acid found in vinegar.

Tartaric acid (formula C4H6O6 )used in cooking

Citric acid ( formula C6H8O7) this is the acid found in

oranges and other fruits.

ascorbic acid is another acid known as vitamin C.

These acids are called weak acids because they form a small number of H+ ions in water

BasesBases are substances that release hydroxide ions (OH-) in water.

Eg NaOH (s) Na+ (aq) + OH- (aq)

Eg KOH (s) K+ (aq) + OH- (aq) Strong bases give off lots of OH- ions and weak base give off less OH-

ions

Common strong bases are:Sodium hydroxide (NaOH)Potassium hydroxide (KOH)Ammonium hydroxide (NH4OH)

Many cleaning agents are bases eg oven cleaners, window cleaners

The pH Scale

The amount of H+ ions given off by an acid are measured by the pH scale

1 on the pH scale means there are a lot of H+ ions in the water and the solution is said to be acidic

14 on the pH scale means there are very few H+ ions in the water but a lot of OH- ions creating a basic solution

1 2 3 4 5 6 7 8 9 10 11 12 13 14

Draw the pH scale below your book

1 2 3 4 5 6 7 8 9 10 11 12 13 14

acidNeutralEg water

base

The colours below are the colours for the different pH numbers with universal indicator this indicates how acidic or basic a solution is

Task – gently shade your pH scale these colours

1 2 3 4 5 6 7 8 9 10 11 12 13 14

1 2 3 4 5 6 7 8 9 10 11 12 13 14

acid neutral basic

Anything less than 7 on the pH scale is called an acid

Weakacid

Strong

acid

neutral

1 2 3 4 5 6 7 8 9 10 11 12 13 14

acid neutral basic

Indicators can also tell us how many OH- ions a base will give off and this gives us an indication of how basic a solution is.

1 2 3 4 5 6 7 8 9 10 11 12 13 14

Weakbase

Strongbase

neutral

Which beaker contains the acid and which one contains the base?

Beaker 1Blue litmus

Beaker 2Red litmus

BaseAcid

Which beaker has more OH- ions?

Which beaker has more H+ ions?

(H+) (OH-)

Litmus paper is another indicator

Remember blue litmus paper tests for acids

Red litmus tests for bases

Litmus paper can also tell us Whether we Have an Acid or a base.

Litmus paper can be red or blue

Acids turn blue litmus paper red

Bases turn red litmus paper blue

Neutralisation hydroxide (OH-) ions are the opposite to H+

When there are equal amounts of H+ and OH- ions in a solution they will react to form pure water (H2O) in a neutralisation reaction – the neutralisation reaction is below

H+ + OH- H2O (water is neutral and has a pH of 7)

So bases eg NaOH, KOH can neutralise acids!

and acids eg HCl,H2SO4 can neutralise bases!

From acid

From base

Gas tests

All carbonates eg _______ react with any acid to from CO2 (carbon dioxide) gas.

The limewater test bubbled CO2 through limewater

How do you test for CO2?

CaCO3

Give a balanced equation for an acid/carbonate reaction

CaCO3 + 2HCl CaCl2 + CO2 + H2O

CO2 + Ca(OH)2 CaCO3 + 2H2O

How do you test for O2? (Oxygen)

The glowing splint test

KMnO4 MnO2 + O2

Finally how do you test for H2 (hydrogen)?

The pop test

Give a balanced reaction for the magnesium and hydrochloric acid reaction

Mg + 2HCl MgCl2 + H2

Give a balanced reaction for the combustion of the hydrogen

Physical Property of metal

Meaning

malleable Means the metal can be bent

ductile Means the metal can be made into wires

Conductivity Conducts both heat and electricity

lustrous Shinysolid All are solid except

Hg

Physical Properties of metals

Metal Structure Metal Structure

A metal consists of a regular arrangement of A metal consists of a regular arrangement of positive ions held together by a 'sea' of positive ions held together by a 'sea' of electrons. electrons.

Metal structure StarterMetal structure StarterMetals consist of p______ metal ions surrounded by n______ electrons.The attraction of the e_______ for thep_____ ions acts like a glue that holds metals atoms together

Activity Activity

On the periodic table in your book colour the On the periodic table in your book colour the metals red and nonmetals blue metals red and nonmetals blue

leave the metalliods (these are elements found on leave the metalliods (these are elements found on the border line between the metals and non the border line between the metals and non metals) white.metals) white.

Give names to the following metal symbols:

Al - Zn - Ag -

Ni - Ca - Cu –

Fe - Li - Mg –

Pb - Na - Au -

Aluminium

Nickel

Iron

Lead

Calcium

Zinc

LithiumSodium

Silver

CopperMagnesiumGold

Metal Structure Metal Structure A metal consists of positive A metal consists of positive ions held together by a 'sea' ions held together by a 'sea' of electrons. of electrons.

The electrons account for the The electrons account for the lustrous appearance of lustrous appearance of metalsmetals

Because the electrons can Because the electrons can move freely they conduct move freely they conduct electricity, however the electricity, however the positive ions can only vibrate positive ions can only vibrate in the one spot. This means in the one spot. This means metals also conduct heat as metals also conduct heat as wellwell

Note

This type of metal bonding between positive ions and electrons in metals is strong giving metals high melting points.

Why metals conduct heatWhy metals conduct heat

Demo by heating spatula with paper clips attached by vasoline

The word particle in this passage refers to the metal ions.

As the metallic bonds do not act in a particular direction, the rows of positive ions can slide over one another easily. This allows the metal to be bent or shaped. This structure allows metals to be bent (malleable) or made into wires (ductile)

Why most metals can be bent or Why most metals can be bent or shapedshaped

Metal structure StarterMetal structure StarterMetals consist of p______ metal ions surrounded by n______ electrons.The attraction of the e_______ for thep_____ ions acts like a glue that holds metals atoms together

Isotopes

An isotope is an atom with a different number of neutrons

The above are all naturally occurring isotopes of hydrogen

electron) 1 neutrons, 2 proton, (1 TritiumH

elctron) 1 neutron, 1 proton, (1 Deuterium H

electron) 1 proton, (1 Hydrogen H

31

21

11

Metals and oxygen What is Metals and oxygen What is Rust?Rust?

Rust only occurs with iron (Fe) metal.

Rusting is where iron reacts with oxygen in the air to form rust (also known as iron oxide Fe2O3)

To from rust iron, water and oxygen must be present.

Rust is always noticed by a reddish brown layer occurring on the surface of the iron.

Summary – Metal Reactions

metal + oxygen metal oxide

aluminium + oxygen aluminium oxide

Metals and oxygen – general reaction

Example

metal + oxygen

Use the general reaction below to write both word equations then symbol equations for each of the metals reacting with oxygen

calcium

sodium

magnesium

+ oxygen sodium oxide

+ oxygen calcium oxide

+ oxygen magnesium oxide

metal oxide

4Na + O2 2Na2O

2Ca + O2 2CaO

2Mg + O2 2MgO

zinc

copper

iron

aluminium

+ oxygen zinc oxide

+ oxygen iron oxide

+ oxygen copper oxide

+ oxygen aluminium oxide

4Al + 3O2 2Al2O3

2Zn + O2 2ZnO

4Fe + 3O2 2Fe2O3

2Cu + O2 2CuO

Experiment: metals and waterExperiment: metals and water

Aim: to observe the reactions of metals Aim: to observe the reactions of metals with water and sort out which react faster with water and sort out which react faster than others page 129 yellow lab bookthan others page 129 yellow lab book

The general reaction for a metal reacting with water is:

metal + water metal hydroxide + hydrogen

eg Na + H2O NaOH + H2

reaction mixture starter reaction mixture starter complete the followingcomplete the following

Li + H2O Ca + H2O

Mg + H2O (steam)

Al + H2O (steam)

Cu + O2

Fe + O2 (rust forms)

2LiOH + H2

Ca(OH)2 + H2

2CuO

2Fe2O3

MgO + H2

Al2O3 + 3H2

2

2

4 3

2 3

2 2

Experiment: metals and acidExperiment: metals and acidAim: to observe the reactions of metals with Aim: to observe the reactions of metals with acid and sort out which react faster than others acid and sort out which react faster than others ((that is - which ones are more reactivethat is - which ones are more reactive))

The general reaction for a metal reacting with an acid is:

metal + acid metal salt + hydrogen

Summary Summary

Most metals will react with dilute acids to give off hydrogen gas and form a salt.

The general formula for a metal acid reaction is

Magnesium + hydrochloric acid

Magnesium + chloride

hydrogen gas

Iron + hydrochloric acid

Iron Chloride +

hydrogen gas

Zinc + hydrochloric acid

Zinc Chloride +

hydrogen gas

Metal + acid Metal salt + hydrogen gas

Write word and symbol equations for these acid metal reactions

Complete the following WORD equation.

(a) ACID + METAL

Give a balanced example of an acid/metal reaction Mg + 2HCl MgCl2 + H2

Metal salt + Hydrogen

Write a balanced equation for an sulfuric acid and Iron metal reaction

Then complete exercises writing balanced symbol equations on page 133

Fe + H2SO4 FeSO4 + H2

Write out the following

From the folowing metal list answer the questions below

Li , Cu, Zn, Al, Mg , Fe, Pb

1. List the metals in order from most reactive to least reactive?

2. ____ is a metal that reacts with cold water

3. _______ is the metal that does not react with sulfuric acid.

4. ______ is the most reactive metal on the list

Li, Mg, Al, Zn, Fe, Pb, Cu

Li

Cu

Li

5. ______ is the metal that rusts Fe

Most reactive least reactive

Metal oxides + water

Give a balanced reaction for CaO reacting with H2O

metal hydroxide

CaO + H2O Ca(OH)2

Give a balanced reaction for sodium reacting with oxygen

4Na + O2 2Na2O

Give a balanced reaction for H2SO4 reacting with Li

2Li + H2SO4 Li2 SO4 + H2

Starter Summary Reactions

Some metal oxides do not d _____ in water and _____ ___ produce alkaline solutions.

Describe the relative concentration of H+ ions at different points of the pH scale.

issolve will not

ACID + CARBONATE

Give a balanced reaction for HCl reacting with CaCO3

Salt + carbon dioxide + water

CaCO3 + 2HCl CaCl2 + CO2 + H2O

Give a balanced reaction for HCl reacting with NaHCO3

(sodium bicarbonate)

NaHCO3 + HCl NaCl + CO2 + H2O

Give a balanced reaction for H2SO4 reacting with ZnCO3 ZnCO3 + H2SO4 ZnSO4 + CO2 +

H2O

Acid Carbonate Reactions

Complete the experiment on page 136 then questions

Homework for test on Friday

Check out the 1.4 Achievement standard page 103 -104 (yellow lab book)Look at Specific learning out comes page 104 -105 make sure you use to make headings for study notes and practise theseRead chapter 15 Basic Chemistry (NCEA level 1 Science text) complete all questionsRead Chapter 16 acids and bases and complete all questions Read Chapter 17 metals and complete all questions

AlloysAlloys

Remember alloys are mixtures of metals and other Remember alloys are mixtures of metals and other substancessubstances

Important alloys areImportant alloys are

Steel made of carbon and iron – used in many industries Steel made of carbon and iron – used in many industries including car bodiesincluding car bodies

Brass made of copper and zinc – used in plumbing fittingsBrass made of copper and zinc – used in plumbing fittings

Solder made of tin and lead – used in making circuitsSolder made of tin and lead – used in making circuits

Alloys are made to change the physical property of Alloys are made to change the physical property of the metal eg solder melts lower than lead or tinthe metal eg solder melts lower than lead or tin

Read page 63 in MW to find why metals conduct electricity.

The sea of negative electrons in metals allows electrical current to flow through the metal.

These electrons also account for the shiny appearance of metals.

Why do metals conduct Why do metals conduct electricity?electricity?

As the metallic bonds do not act in a particular direction, the rows of positive ions can slide over one another easily. This allows the metal to be bent or shaped. This structure allows metals to be bent (malleable) or made into wires (ductile)

Why most metals can be bent or Why most metals can be bent or shapedshaped

Neutralisation

HCl + NaOH H2O + NaCl

Refresher

Strong bases eg _____ have a pH of ___ and will turn universal indicator _____ common lab bases are potassium hydroxide (KOH), sodium hydroxide (NaOH) and ammonium

hydroxide (NH4OH)

Common household bases are:__________________________________

Window cleanerOven cleanerJiff

KOH

14purple

Universal indicator goes ____ with a strong acid and the pH will be around ____

Neutral solutions (eg pure water) go _____ with universal indicator and a pH of around _____

Strong bases go _______ with universal indicator and have a pH of around____

Refresher

Strong acids eg _____ have a pH of ___ and will turn universal indicator _____

Weak acids eg Lemon ___ have a pH of ___ and will turn universal indicator _____

Examples of common household acids are:_________________________________________

HCl 1red

juice 4-6orange

vinegartartariccitric

Experiment finding the pH of substances -

Draw the table below:

Place 2 cms of water in each tube (then two drops of the test solutions)

3 drops of universal indicator in them – write then fill in your chart

Solution name Colour of solutionpH of Solution

Experiment finding the pH of substances -

Draw the table below:

Place 2 cms of each of the solutions below in a test tube then place

3 drops of universal indicator in them – write the colour in the chart

Baking soda solution

bleach

milk

lemonade

Soft soap

Jiff

pH 1

pH 14 pH 3-5

pH 7

pH 10 - 12 pH 1-2

red violet/purple

red

green

violet

red

Colour of solutionpH of Solution

Strong and Weak Acids- Experiment

Place 2cms of each of the 3 acids in 3 test tubes in a test tube rack – copy this table into your book - use a ruler to draw it

Acid Colour with Universal indicator

Reaction with Mg metal

Sulfuric

Hydrochloric

Ethanoic

Acid Reactions Experiment

Place 2cms of each of the 3 acids in 3 test tubes in a test tube rack – copy this table into your book - use a ruler to draw it

Acid Observation with calcium carbonate

Sulfuric

Hydrochloric

Ethanoic

Using the white boards answer the questions:By being the first group to neatly show the correct answer

Give the chemical symbols for:

Give the type and number of atoms in

sodium carbon

copper

Potassium

heliumiron

mercury

Sulfur

NaCl NaNO3

H2SO4

PbCO3 Na2CO3

Al2(SO4)3 CH3COOH

What can you remember?

Documents

Types of Compounds