s3 chemistry atomic structure, bonding & properties...s3 chemistry atomic structure, bonding...

S3 ChemistryAtomic Structure, Bonding &

Properties

NEW LEARNING

Through gaining an Understanding of the structure of atoms and how they join, Ican begin to connect theproperties of substances withtheir possible structuresSCN 4-15a

Atomic structure and bonding related to properties of materialsNational 4

REVISION

I have developed my knowledge of the Periodic Table by considering the properties and uses of a variety of elements relativeto their positionsSCN 3-15a

S3 ChemistryAtomic Structure, Bonding & Properties

NEW LEARNING



Lessons 1 & 2 – History of the Atom

REVISION


Learning Objectives & Success Criteria

Today we will learn …

We will do this by …

We will have succeeded if…

About the scientific history of the discovery of the atom.

Researching the different scientists involved in atomic science and presenting a poster based on their work. Using each other’s posters as a learning tool and peer assessing.

All members of the class can complete a summary table on the key scientists involved in the scientific history of the discovery of the atom using the information extracted from classmates posters.

https://www.twigonglow.com/film/factpack-structure-of-the-atom-1353/

https://www.twigonglow.com/film/factpack-structure-of-the-atom-1353/

Atomic Theory Scientists

Your scientist will be one of the following:

You will team up with the classmates who have part of the same photo as you.

• Ernest Rutherford

• Neils Bohr

• John Dalton

• JJ Thomson

• Werner Heisenberg

Sources of Information

Your poster must include the following:

1.Name of scientist

2.Date of proposed theory

3.What did they think an atom looked like? Include a picture if available.

4.Were they correct (or did other scientists improve upon their model)?

Poster – Key Features

If you want to add more information you can but be sure to include the above first of all!

Tell me three things...

1. One thing you have done well

2. One thing you would like to find out more about

3. One thing you know now that you didn’t know 50

minutes ago

Lesson 1 - Exit Task – 3 Things

Lesson 2 StarterWhat were the 4 key features you were asked to include on your poster?Name of scientist, date of proposed theory, what they think an atom looked like (pictureif available) & if they were correct?

Tick each of the features you have already finished on your poster. You now have only 20 minutes to complete the rest of your poster. We will then be placing our posters up for classmates to learn from. Do your best for each other!

NEW LEARNING



Lessons 1 & 2 – History of the Atom


REVISION


Lesson 2 - Exit Task – Match Up

Match the atomic theory model to the scientist.

Solid sphere modelRutherford

Dalton

Bohr Plum pudding model

Planetary model - electrons in

specific energy levelsThomson

Planetary model – discovered the

nucleus

NEW LEARNING



Lesson 3 – Structure of the Atom


REVISION



Today we will learn to …



Identify the properties and locations of protons, electrons and neutrons in an atom.

Hearing about what an atom is made of and drawing our own atoms.

We can state the mass, charge and location of the 3 subatomic particles. We can draw atom diagrams which include the correct electron arrangement.

++

The electrons are always found outside the nucleus in electron shells.

Most of the atom is empty space! Imagine a Helium atom the size of Wembley stadium. The nucleus would be the size of a football on the centre spot. The electrons would be the size of two peas flying around the whole stadium. The rest of it is emptiness!

Copy & complete the following table to summarise the key features about the 3 subatomic particles.

Write the electron arrangement for the following atoms:

-

+

++

-

-


Today we will learn to …



Identify the properties and locations of protons, electrons and neutrons in an atom.

Hearing about what an atom is made of and drawing our own atoms.

We can state the mass, charge and location of the 3 subatomic particles. We can draw atom diagrams which include the correct electron arrangement.

Fist to Five

Rate your understanding of today’s lesson using your fingers.

NEW LEARNING



Lesson 4 – Nuclide Notation


REVISION






What is meant by the terms Atomic Number and Mass Number and how to use these two numbers to work out the numbers of each subatomic particle in an atom.

Carrying out simple calculations using Atomic number and Mass Number. Using the periodic table and data book to help find these two numbers.

We can work out the number of protons, electrons and neutrons from the nuclide notation or when given the Atomic and Mass numbers.

11

23 56 119

5026





What is meant by the terms Atomic Number and Mass Number and how to use these two numbers to work out the numbers of each subatomic particle in an atom.

Carrying out simple calculations using Atomic number and Mass Number. Using the periodic table and data book to help find these two numbers.

We can work out the number of protons, electrons and neutrons from the nuclide notation or when given the Atomic and Mass numbers.

What? How?

Explain what you have learnt today and how you have learnt it

?

NEW LEARNING



Lesson 5 – The Properties of Elements


REVISION


Lesson Starter

1. What do you think we mean when we say“a property of an element”?

A property is any characteristic of an element.

2. Give some examples of properties of elements.

Physical properties (what they are like: colour, size, density, melting point, boiling point, odour).

Chemical properties (what they can react with).





About the properties of elements and how electron arrangement links to properties of elements.

Carrying out conductivity tests on elements. Watching video clips about certain groups of elements and using the data book to learn about the electron arrangements within groups.

We can use the position of an element in the periodic table to predict it’s properties.

**REMINDER**

All metals conduct electricity.

All non-metals except carbon (graphite) are non-conductors (insulators).

Mercury, the only metal which is a liquid at room temperature, can conduct electricity. All metals in the liquid state can conduct electricity.

Non-Metals

Metals

1

2 3 4 5 6 7

8/0

_ _ _ _ _ _

_ _ _ _ _ _ _

Periodic Table - Important Areas Summary

Group 1 – Alkali Metals - very reactive metals (stored in oil). React violently with water to produce an alkali and hydrogen gas. Soft and can be cut with a knife. Members become more reactive as you move down the group.

Group 7 - Halogens - very reactive non-metals. All colouredelements. Members become less reactive as you move down the group.

Group 8/0 - Noble Gases - extremely unreactive gases. They do not readily combine with other elements to form compounds.

Transition Metals – middle block elements – Form brightly coloured compounds. Variable valency. Several are used as catalysts to speed up chemical reactions.

Same group, ends in same number

Crossing a period group by group, the last number increases by 1 each time.

0/8

Elements in the same group have similar chemical properties. This is because elements in the same group have the same number of outer electrons.

The number of outer electrons an element has is responsible for how it reacts.

When an element has an incomplete outer shell of electrons it is unstable and it reacts with (forms bonds with) other elements to achieve stability.

Outer Electrons & Chemical Properties

Elements in group 8 (0) each have a full outer electron shell giving the noble gases a special stability.

This means noble gases do not need to form bonds with other elements i.e. do not form compounds.





About the properties of elements and how electron arrangement links to properties of elements.

Carrying out conductivity tests on elements. Watching video clips about certain groups of elements and using the data book to learn about the electron arrangements within groups.

We can use the position of an element in the periodic table to predict it’s properties.

Mind MapProduce a mind map to summarise the

lesson today.

http://images.google.co.uk/imgres?imgurl=http://ccat.sas.upenn.edu/~rs143/map1.jpg&imgrefurl=http://www.fordham.edu/HALSALL/sbookmap.html&usg=__D0Trzr9Drtr1e3fxYpwb5kAjOb8=&h=715&w=952&sz=189&hl=en&start=8&tbnid=6Ag99PXFd51WpM:&tbnh=111&tbnw=148&prev=/images?q=map&gbv=2&hl=en&sa=G

http://images.google.co.uk/imgres?imgurl=http://ccat.sas.upenn.edu/~rs143/map1.jpg&imgrefurl=http://www.fordham.edu/HALSALL/sbookmap.html&usg=__D0Trzr9Drtr1e3fxYpwb5kAjOb8=&h=715&w=952&sz=189&hl=en&start=8&tbnid=6Ag99PXFd51WpM:&tbnh=111&tbnw=148&prev=/images?q=map&gbv=2&hl=en&sa=G

http://images.google.co.uk/imgres?imgurl=http://www.defensetech.org/archives/mind_control.gif&imgrefurl=http://www.defensetech.org/archives/cat_bizarro.html&usg=__FiujKzjTVRrh8ShQDb1sTyONvR0=&h=374&w=381&sz=14&hl=en&start=1&tbnid=P4Gt6LLZAmsj2M:&tbnh=121&tbnw=123&prev=/images?q=mind&gbv=2&hl=en

http://images.google.co.uk/imgres?imgurl=http://www.defensetech.org/archives/mind_control.gif&imgrefurl=http://www.defensetech.org/archives/cat_bizarro.html&usg=__FiujKzjTVRrh8ShQDb1sTyONvR0=&h=374&w=381&sz=14&hl=en&start=1&tbnid=P4Gt6LLZAmsj2M:&tbnh=121&tbnw=123&prev=/images?q=mind&gbv=2&hl=en

NEW LEARNING



Lesson 6 – Lose, Gain, Share: Making Compounds


REVISION


Lesson Starter

Name all the elements present in the following 5 compounds.

1.Aluminium bromide2.Hydrogen oxide3.Sodium hydroxide4.Nitrogen hydride5.Nickel sulfate

Aluminium & bromineHydrogen & oxygenSodium & hydrogen & oxygenNitrogen & hydrogenNickel & sulfur & oxygen





About the types of bonding which exist.

Considering which types of elements are joining together in compounds and learning the rules about when atoms LOSE, GAIN or SHARE electrons.

We can use the name of a compound to predict the type of bonding within it. We will also use the name to predict whether the bond is formed by loss & gain of electrons or by sharing electrons.

**REMINDER**

A compound is a substance made up of two or more types of atom joined.

A mixture is a substance made up of two or more types of substances (atoms/elements/compounds) NOT JOINED

Compound names are recognisable because they have 2 parts e.g. sodium chloride (sodium & chlorine).

If a compound name ends in -IDE that compound only contains the 2 elements obvious from it’s name.

Except where the second part of the compound name is hydroxide or cyanide.

e.g. sodium hydroxide = sodium, hydrogen and oxygen

sodium cyanide = sodium, carbon and nitrogen

If a compound name ends in -ATE or -ITE that compound contains the 2 elements obvious from it’s name PLUS OXYGEN e.g. sodium carbonate (sodium, carbon & oxygen).

**REMINDER**

Naming Compounds

When elements bond they are able to achieve a full outer shell of electrons like a noble gas by LOSING, GAINING or SHARING electrons.

Achieving A Noble Gas Arrangement

We learned in the last lesson that all elements except the noble gases have an incomplete outer electron shell and must form bonds to achieve stability.

Lithium

Electron Arrangement =

Closest Noble Gas electron arrangement =

Change to electrons =


2,1

2 (He)

Lose 1

Fluorine





2,7

2, 8 (Ne)

Gain 1

Oxygen





2,6

2, 8 (Ne)

Gain 2

Aluminium





2,8,3

2,8 (Ne)

Lose 3

Calcium





2, 8, 8, 2

2, 8, 8 (Ar)

Lose 2

HINT – Use the data book p4 to help you decide (remember the zig-zag line)

• Ionic compounds form by a metal atom losing electrons and a non-metal atom gaining electrons to form ions.

• Covalent compounds form by two or more non-metal atoms sharing electrons

Now reconsider the compounds from the last 2 slides & state whether they would LOSE/GAIN or SHARE electrons.

Lose, Gain, Share

Lose, Gain, Share

Lose/Gain

Share

Lose/Gain

Lose/Gain

Share

Lose, Gain, Share

Lose/Gain

Share

Share

Share

Lose/Gain

Mr Wrong

Explain why this student statement is wrong…

“Sodium chloride, like other covalent compounds, bonds by sharing electrons”

Exit Task

NEW LEARNING



Lesson 7 – Covalent Bonding


REVISION


Lesson Starter

1. Name the type of bonding in the following compounds:

A Phosphorus chloride

B Copper chloride

2. What would happen to the electrons in the above compounds as they bond (i.e. lose/gain OR share)?:

A Share

B Lose/Gain

covalent

ionic





How non-metal atoms join together via covalent bonds to form covalent compounds.

Hearing about what a covalent bond is. Drawing covalent molecules and building them using molecular model kits.

We can state the definitions of the terms covalent bond, covalent molecule and diatomic. We can use our periodic table to find and name the 7 diatomic elements.

element).

chlorinechlorine

Covalent Elements

compound).

hydrogen chlorinehydrogen chloride

elements (forming a compound).

atoms of different

Covalent Compounds

Using Molecular Models – Building Molecules

oxygen

hydrogen

chlorine

nitrogen

Using the molecular model kits (molymods) and the colour key shown opposite build a diatomic molecule of the 4 elements shown in the key.Remember diatomic means 2 atoms.

How many bonds does each molecule have joining the 2 atoms?Remember that where there is a hole in the model atom a bond must be inserted and all bonds must be joined to something (except with Nitrogen).

Brief slide/note on covalent network?

Covalent Networks

Covalent networks are giant structures with no fixed number of atoms. In covalent network structures all atoms are non-metals and are joined by covalent bonds. Covalent network substances can be elements or compounds.

Covalent Network ElementDiamond

Covalent Network CompoundSilicon Dioxide (sand)





How non-metal atoms join together via covalent bonds to form covalent compounds.

Hearing about what a covalent bond is. Drawing covalent molecules and building them using molecular model kits.

We can state the definitions of the terms covalent bond, covalent molecule and diatomic. We can use our periodic table to find and name the 7 diatomic elements.

Definition

Choose three new words you have learnt today and write

dictionary definitions.

NEW LEARNING



Lesson 8 – Ionic Bonding


REVISION


Lesson Starter

1. What is a covalent bond?

A shared pair of electrons between 2 non-metal atoms.

2. Why do the atoms of some elements form bonds?To achieve stability by obtaining a full outer electron shell like a noble gas.

3. What are the 7 diatomic elements (hint – use your periodic table to help)?Hydrogen, Oxygen, Nitrogen, Fluorine, Chlorine, Bromine, Iodine (remember HON 7).

Learning Objectives & Success CriteriaToday we will learn …



Reflecting on what we learned in our lose, gain, share lesson. Learning about the changes which arise in electron arrangement when electrons are transferred and how these changes link with the exact charge of the ion formed.

We can use the electron arrangement of an element to predict the charge on the ion it forms to achieve stability like a noble gas.

How metal and non-metal atoms are altered to become ions and how they subsequently join together via ionic bonding to form ionic compounds.

Li

Li+

ClCl-

Ionic Lattice

More Ionic Bonding

Mg -> Mg2+ 2 F -> 2 F-

Writing Ion SymbolsUsing the electron arrangement information from the data booklet we can work out the symbol for an ion of an element which has achieved stability by electron transfer (i.e. has a full outer electron shell like a noble gas). We do this by the following steps:

1. Write the symbol for an atom of the element.

2. Write the electron arrangement for that atom.

3. Consider what change to electron numbers would result in a full outer shell.

4. Consider what this change to electron numbers would mean in terms of ion charge and add the charge as a superscript.

Ion Name Atom electron arrangement

Closest Noble Gas electron arrangement

Change to electrons

Ion symbol

Aluminium

Chloride

Oxygen

Lithium

Calcium

Nitride

Phosphide

Sodium

Writing Ion Symbols

Al3+

Cl-

O2-

Li+

Ca2+

N3-

P3-

Na+

2,8,3

2,8,7

2,6

2,1

2,8,8,2

2,5

2,8,5

2,8,1

2,8 (Ne)

2,8,8 (Ar)

2 (He)

2,8 (Ne)

2,8,8 (Ar)

2,8,8 (Ar)

2,8 (Ne)

2,8 (Ne)

Lose 3

Gain 1

Gain 2

Gain 3

Gain 3

Lose 1

Lose 2

Lose 1

Learning Objectives & Success CriteriaToday we will learn …



Reflecting on what we learned in our lose, gain, share lesson. Learning about the changes which arise in electron arrangement when electrons are transferred and how these changes link with the exact charge of the ion formed.

We can use the electron arrangement of an element to predict the charge on the ion it forms to achieve stability like a noble gas.

How metal and non-metal atoms are altered to become ions and how they subsequently join together via ionic bonding to form ionic compounds.

Exit Task – Summary TableCopy & complete the summary table. It outlines the key

differences between ionic and covalent bonding.

Covalent Bonding Ionic Bonding

Element types involved in this bonding.

What happens to the electronsduring this bonding?

Named example

Non-metals only.One metal and one non-metal.

Electrons are shared.

Electrons are lost by the metal and gained by the non-metal.

Carbon dioxide. Sodium chloride.

NEW LEARNING



Lesson 9 – Writing Formulae (Prefixes & Diagrams)


REVISION


Lesson Starter

For the following elements write the symbol of the ion which would be formed when that element achieves a full outer electron shell like a noble gas:

1 Magnesium atom : MgElectron arrangement: 2, 8, 2

2 Fluorine atom: FElectron arrangement: 2, 7

3 Aluminium atom: AlElectron arrangement: 2, 8, 3

Mg2+

F-

Al3+





How to write simple chemical formulae.

Using diagrams to work out formulae.Using prefixes to work out formulae.Using valency rules / visual aids to work out formulae.

We can select the most appropriate method of writing formulae for a compound and apply it in order to write down the formula correctly.

Using Models/Diagrams

carbon

oxygen

hydrogen

chlorine

nitrogen

O2

O O

HH

H

H

Si

SiH4

orH4Si

C C C

HHH

H H H

HH

C3H8 or H8C3

Hydrogen oxide - water

Hydrogen chloride

Carbon hydride

O

H H

H2O or OH2

H Cl HCl or ClH

CH4 or H4CC

H

HHH

Chlorine Cl Cl Cl2

Hydrogen

Carbon chloride

H2

CCl4 or Cl4CC

Cl

ClClCl

Nitrogen hydride NH3 or H3N

H H

NH

H

H

Chemical Formula From Prefixes

Sometimes the name of a compound contains a prefix which allows us to write the formula.

Prefixes when present before the name of an element tell you how many atoms of that element are present in the formula of that compound.

e.g. sulfur dioxide

Contains 1 sulfur and 2oxygens e.g. SO2

Glue in the handout then complete the table on the right.

1. If given a diagram or model – simply count the atoms.

2. If given a name including a prefix – write down formula using prefix(es) to guide how many of each atom in the formula.

3. IF AND ONLY IF there is no diagram and no prefix present in the compound name then we have to use something called valency.

Selecting the Best Method of Writing Formulae

Valency is the combining power of an element i.e. how many bonds it can form. It is linked to the group number in the periodic table.

Valency

Note that the Noble gases do not have a valency because they are unreactive and do not form compounds.

Valency & Group Number

Use your data book and/or the table above to find out the valency of the following elements:

Step 1 – Use your data book (or the table copied from the last slide) to find the valency of each element in the compound. Hint: 1 2 3 4 3 2 1.

Add this number of pegs to the plate with the relevant symbol.

Step 2 – Combine as many copies of each peg plate as required in order to connect ALL peg bonds between the elements.

Step 3 – Use the picture created to write down your formula.

Valency Method Using Visual Aids

potassium bromide KBr

**Optional activity**

In covalent molecules the formula is the exact number of atoms in the compound. In covalent network and ionic substances the formula is the ratio of particles (ions in an ionic lattice and atoms in a covalent network).

Formulae & Bonding Type

The formula does not always represent the exact number of particles of each type in a compound. It can sometimes represent the ratio of different particles.





How to write simple chemical formulae.

Using diagrams to work out formulae.Using prefixes to work out formulae.Using valency rules / visual aids to work out formulae.

We can select the most appropriate method of writing formulae for a compound and apply it in order to write down the formula correctly.

Reach For The Stars - Rating Exercise

Rate your understanding of the 3 Key Areas covered today:A Writing Formulae from diagrams/modelsB Writing Formulae from names with a prefixC Writing Formulae from valency with visual aids

NEW LEARNING



Lesson 10 – Writing Formulae (SVSDF)


REVISION


Lesson Starter1. Write the formula for the following molecule:

CCl4 or Cl4C

NF3

SBr2S Br

3. Write the formula for sulfur bromide.

Hint – Would working out the valency help?

2. Write the formula for nitrogen trifluoride.

Hint – Does the name have a prefix?

Br

BrS


Today we will …



Practise writing simple chemical formulae for elements in the numbered groups of the periodic table as well as the transition metal block.

Using a method called SVSDF, involving the valency of elements. We will also find out how valency is indicated for transition metals.

We can write the chemical formula for simple two element compounds including those containing transition metals.

Objective Traffic Lights

How do you feel about the lesson objectives?

Red = don’t think I have grasped this

Amber = feeling OK about this, have just about got there

Green = Confident I have achieved this

NEW LEARNING



Lesson 11 – Word Equations


REVISION


Lesson Starter

SO2

CaF2

CuO

Mn3N2





How to write equations which summarise the chemicals involved and how they change in a chemical reaction.

Learning about what must be and what must not be included in word equations. Practising writing word equations from descriptions of chemical reactions.

We can write a word equation for any chemical reaction which is described for us.

Word Equations• A word equation describes what we start with

(reactants) during a chemical reaction and what we end up with (products).

• It is similar to a recipe with reactants being like the ingredients and the product(s) being what we have made using those ingredients.

• The ingredients or reactants appear on the left of the equation while the products appear on the right.

plus Changes into ORReacts to produce

Reactants appear on the left of the arrow and products appear on the right.

Word Equations

Example 1

Sodium reacts with chlorine to produce

sodium chloride

Sodium + chlorine sodium chloride

When you are given a sentence telling you how a chemical reaction has taken place, you should be able to write a word equation from that.

reactants

products

Acid + Alkali Salt + Water

Example 2

Acid reacts with alkali to produce salt and water.

reactants

products

Example 3

Nitrogen and hydrogen combine to form nitrogen hydride.

reactants

products

nitrogen + hydrogen nitrogen hydride

Mercury oxide decomposes on heating to form mercury and oxygen.

Example 4reactants

products

mercury oxide mercury + oxygen

Calcium carbonate fizzes up when it is added to nitric acid. This is because carbon dioxide gas is being made. Calcium nitrate and water are left in the beaker at the end of the reaction.

Example 5reactants

products

calcium carbonate

nitric acid

calcium nitrate

water+ +

Your body uses food and oxygen to make carbon dioxide and water in a process called respiration.

Example 6reactants

products

food + oxygen carbon dioxide

+ water

Rusting happens when iron reacts with the oxygen in air to form iron oxide

Example 7reactants

products

iron + oxygen iron oxide

Try the 2 sheets of examples on writing word equations. The examples in the first sheet have been partially done for you.

DO NOT WRITE ON THE SHEETS

Copy and complete the word equations into your jotter for both exercises.

Word Equation Extension Task





How to write equations which summarise the chemicals involved and how they change in a chemical reaction.

Learning about what must be and what must not be included in word equations. Practising writing word equations from descriptions of chemical reactions.

We can write a word equation for any chemical reaction which is described for us.

State what is wrong with each of the following word equations.

1.carbon + oxygen gas carbon dioxide

2.zinc + hydrochloric acid = zinc chloride +

hydrogen

3.Lead iodide and potassium nitrate are produced when

lead nitrate and potassium iodide are reacted together

Exit Task – Spot the Blooper!

Lead iodide + potassium nitrate lead nitrate + potassium iodide

Reactants on products side (RHS) and vice versa

NEW LEARNING



Lesson 12 – Equations Using Symbols & Formulae


REVISION


Lesson Starter

Write word equations for the following 3 chemical reactions:

1

2

3





How to write equations using symbols and formulae (including symbols which indicate the state of substances).

Learning the different state symbols. Applying our knowledge of elements to write the appropriate symbol/formula for them. Using the prefix or valency method (as appropriate) to work out the formulae for compounds.

We can write an equation, including symbols and formulae for a chemical reaction which is described for us.

(l)(g)(aq)(s)(s)(l)

(g)

(s)

(aq)

(g)

NOTE -State symbols can be

worked out for the elements

using the melting

point/boiling point information

on NAT 5 data book p5

boron boronB F2+ BF3

(s) (g)

NOTE - State symbols can

be worked out for the

elements using the melting



Si Br2+ SiBr4(s) (g)

NOTE - State symbols can

be worked out for the

elements using the melting



Extra Examples

1. Hot magnesium ribbon reacts vigorously with steam. It glows very brightly and the products are magnesium oxide and hydrogen gas.

a. Write a word equation for the reaction.

b. Write an equation using symbols and formulae for the reaction.

magnesium + steam magnesium oxide + hydrogen

Mg (s) + H2O (g) MgO (s) + H2 (g)

2.

C4H10 + O2 CO2 + H2O

Extra Examples

Try the sheet of examples on writing equations using symbols and formulae.

DO NOT WRITE ON THE SHEETS

Copy and complete the equations into your jotter.

Symbol & Formulae Equation Extension Task





How to write equations using symbols and formulae (including symbols which indicate the state of substances).

Learning the different state symbols. Applying our knowledge of elements to write the appropriate symbol/formula for them. Using the prefix or valency method (as appropriate) to work out the formulae for compounds.

We can write an equation, including symbols and formulae for a chemical reaction which is described for us.

Exit Task Flow-Chart

Can you draw a

flowchart like the one

we used in today’s

lesson to help us write

equations using

symbols and formulae.

NEW LEARNING



Lesson 13 – Properties of Compounds: Physical State & Solubility


REVISION


Na (s) + Cl2 (g) NaCl (s)

CuO (s) + C (s) Cu (s) + CO2 (g)

HINT – Write word equation first to help you !!!





About the properties of compounds and how they link to the type of bonding in that compound.

Examining the state of different compounds at room temperature. Testing the solubility of various compounds. Spotting any patterns based on the type of bonding.

We can state how the physical state and solubility of compounds varies based on their type of bonding.

Compound Solid/liquid/gas Type of Bonding

Water, H2O

Sucrose, C12H22O11

Sodium chloride, NaCl

Methane, CH4

Paraffin Wax, C12H52

Calcium oxide, CaO

Silicon dioxide (sand), SiO2

Carbon dioxide, CO2

Acetone, C2H6O

Potassium iodide, KI

Physical State & Bonding TypeThe physical state of a compound at room temperature is an indication of the bonding type in that compound.View the compound display then complete the table indicating the state of each compound and the bonding type (ionic or covalent).

liquid

solidsolidgas

solidsolid

solid

gasliquidsolid

covalentcovalent

ioniccovalentcovalent

ionic

covalent

covalentcovalent

ionic

Physical State & Bonding Type

Physical State & Bonding Type Conclusions

All ionic substances are in the _________ state at room temperature.

Covalent substances can be _______, ________ or _______ at room temperatures.

solid

solid liquidgas

Compound Type of Bonding Soluble / Insoluble

Copper Chloride, CuCl2

Sucrose, C12H22O11

Sodium chloride, NaCl

Starch, (C6H10O5)n

Paraffin Wax, C12H52

Sodium thiosulfate, Na2S2O3

Silicon dioxide (sand), SiO2

Solubility & Bonding Type

Test the solubility of each of the substances listed below and try to spot any patterns based on bonding type.Remember only to use a tiny quantity of each sample.

ioniccovalent

ioniccovalentcovalent

ionic

covalent

soluble

insoluble

solublesoluble

insoluble

soluble

insoluble

Solubility & Bonding Type Conclusions

Ionic substances are usually _________ in water.

Covalent substances can vary in their solubility. Some are _________ in water (they do dissolve). and others are _________ in water (they do not dissolve).

Sometimes covalent compounds which do not dissolve in water do dissolve in other solvents.

soluble

solubleinsoluble






Examining the state of different compounds at room temperature. Testing the solubility of various compounds. Spotting any patterns based on the type of bonding.

We can state how the physical state and solubility of compounds varies based on their type of bonding.

Pyramid

Question you have about the lesson

Things you have been

reminded of today

Things you have learned

today

Exit Task

NEW LEARNING



Lesson 14 – Properties of Compounds: Electrical Conductivity


REVISION







Testing the conductivity of various compounds. Spotting any patterns based on the type of bonding.

We can state how the conductivity of compounds varies based on their type of bonding.

Electricity is a flow of charged particles.

Elements and compounds that conduct electricity are called ___________.

Elements and compounds that do not conduct electricity are called _____________ (or _________ ).

Electrical Conductivity

conductors

non-conductorsinsulators

What happens when a substance is included as part of an electrical circuit gives us information about the particles in the substance and the way they are held together.

The terminals through which the electrical current enters and leaves the substance under test are called the electrodes.

Testing Electrical Conductivity

Compound Type of Bonding Conductor / Non-conductor

Copper chloride (s), CuCl2

Copper chloride (aq), CuCl2

Sucrose (s), C12H22O11

Sucrose (aq), C12H22O11

Sodium chloride (s), NaCl

Sodium chloride (aq), NaCl

Sodium thiosulfate (s), Na2S2O3

Sodium thiosulfate (aq), Na2S2O3

Starch (s), (C6H10O5)n

Paraffin Wax (s), C12H52

Silicon dioxide (s), SiO2

Testing the Conductivity of Compounds

ionic

covalent

ionic

covalent

ionic

covalent

covalent

covalent

ionic

ionic

ionic

non-conductor

non-conductornon-conductornon-conductor

non-conductor

non-conductornon-conductor

non-conductor

conductor

conductor

conductor

Conductivity & Bonding Type

Conductivity & Bonding Type Conclusions

Covalent compounds ________ conduct electricity, no matter what the physical state.

The conductivity of ionic compounds varies dependent on the physical state. Solid ionic compounds _______conduct electricity but molten (liquid) and dissolved (aqueous) ionic compounds _______ do.

never

always

never






Testing the conductivity of various compounds. Spotting any patterns based on the type of bonding.

We can state how the conductivity of compounds varies based on their type of bonding.

1

2

3

4

5

6

7

8

Show Me Board - Exit TaskState whether each numbered label should say conductor or non-conductor on the diagram below.

Metal Element Non-metal Element Ionic Compound Covalent

compound

Sort the list of substance names under the appropriate heading.

Lesson Starter

Metal Element Non-metal Element Ionic Compound Covalent

compound

Sort the list of substance names under the appropriate heading.

Lesson Starter

solid iron molten wax (C12H52)

solid carbon (graphite)

solid copper chloride

liquid bromine

Sodium bromide solution

glucose solution (C6H12O6)

Liquid potassium sulphide

NEW LEARNING



Lesson 15 – Properties of Substances Summarised & Explained


REVISION



Today we will …



Summarise the key properties of different types of substances and explain conductivity and physical state at room temperature.

Practice using the name of a substance to decide what TYPE of substance it is, what type of BONDING it will have and what PROPERTIES it is likely to have from our experiments. Hearing about why only certain substances conduct.Using diagrams to understand state at room temperature.

We can state the key properties of different substance types and explain some of them.

Conductor Non-conductor

Sort the list of elements under the appropriate heading.

Elements: Conductors or Non-Conductors ?

solid copper Liquid nitrogen molten magnesium

solid iodine argon gasmolten iron chlorine gas

solid graphite liquid mercury solid sodium liquid bromine


Sort the list of elements under the appropriate heading.

solid copper Liquid nitrogen

molten magnesium solid iodine

argon gasmolten iron

chlorine gassolid graphite

liquid mercury

solid sodium

liquid bromine

Elements: Conductors or Non-Conductors ?


Sort the list of compounds under the appropriate heading.

Compounds: Conductors or Non-Conductors ?

liquid hexane (C6H12)

solid magnesium chloride

barium nitrate solution

sodium sulfate solution

solid carbon tetrachloride

molten sodium chloride

liquid ethanol (C2H5OH)

molten aluminium fluoride

liquid selenium chloride

solid silver bromide

Conductivity of Substances - ExplainedIn order for a substance to conduct electricity it must contain _________ particles which can _____.

Non-metal elements and covalent compounds do not contain any charged particles so do not _________ electricity.

Metal elements and carbon in the form of ________ do conduct because they contain ___________ __________ (charged particles which can flow).

Ionic compounds contain _____ (charged particles) but they are only free to flow when ionic compounds are _______ or in solution. So ionic compounds only conduct electricity in these states, not when ______.

charged

solidmolten

ions

electronsdelocalised

graphite

conduct

flow

Ionic SubstancesPhysical State- Explained

Ionic compounds are all ______ at room temperature because lots of very _____ ionic bonds hold together the ions in giant ionic lattices.

high

solidstrong

Very _____ temperature would be needed in order to have enough energy to break those bonds (melt the substance).

Covalent SubstancesPhysical State- Explained

Remember there are two types of covalent substance:

solidCovalent Networks are all ______ at room temperature because lots of very _____ covalent bonds hold together the atoms in giant networks.

Very _____ temperature would be needed in order to have enough energy to break those bonds (melt the substance).

high

strong

Covalent SubstancesPhysical State- Explained

Remember there are two types of covalent substance:

betweenweak

Covalent Molecules are all liquid or gas at room temperature because only very _____ attractive forces must be broken _______ molecules to make them melt/boil. We are not breaking the strong covalent bonds within the molecule. So only a very _____ temperature would be needed to have enough energy to do this.

low

Property Ionic Compounds Covalent Compounds

State(s) at room temperature.

Relative melting & boiling points

Solubility in water

Electrical conductivity when solid

Electrical conductivity when molten (liquid)

Electrical conductivity when in solution (aqueous)

solid

high

soluble

Properties of Compounds OVERALL SUMMARYComplete the table below using the information you have learned over the last few lessons:

solid, liquid or gas

soluble or insoluble

non-conductor non-conductor

high or low

conductor

conductor

non-conductor

non-conductor


Today we will …



Summarise the key properties of different types of substances and explain conductivity and physical state at room temperature.

Practice using the name of a substance to decide what TYPE of substance it is, what type of BONDING it will have and what PROPERTIES it is likely to have from our experiments. Hearing about why only certain substances conduct.Using diagrams to understand state at room temperature.

We can state the key properties of different substance types and explain some of them.

Consider the work you have done in this whole topic. Select two things you have done/understood well and one thing you still don’t understand/have to work on.

Two Stars & A Wish

Exit Task

s3 chemistry atomic structure, bonding & properties...s3 chemistry atomic structure, bonding...

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