Acids and BasesYear 11 100 Science

4 External CreditsAS90944

Ms Gibellini

https://play.kahoot.it/#/?quizId=248ce6a9-8476-4133-bf25-915462acb928

Where to find info on moodlehttp://learningon.theloop.school.nz/moodle/course/view.php?id=1336

Kahoots Introduction

Aspects of acids and bases will be selected from: Atomic structure

electron arrangement of atoms and monatomic ions of the first 20 elements (a periodic table will be provided)

ionic bonding names and formulae of ionic compounds using a given table of ions.

Properties acids release hydrogen ions in water reactions (of acids with bases) to form salts pH and effects on indicators.

Rates of reaction and particle theory.  Uses

neutralisation carbon dioxide formation salt formation.

Acids and bases are restricted to HCl, H2SO4, HNO3, metal oxides, hydroxides, carbonates and hydrogen carbonates. Other acids may be included in examination questions. The names and formulae of any such acids will be given in the question.

Achievement Standard

SLOs

A neutron walks into a restaurant and orders a couple of cokes.

As she is about to leave, she asks the waiter how much she owes. 

The waiter replies, "For you, No Charge!!!"

Neutrons

Describe the structure of an atom

Discuss the key differences between the three sub-atomic particles

SLO

All matter is made up of atoms

Chemistry involves the rearrangement of atoms or groups of atoms

Recall the structure of an atom

Atoms

http://www.bbc.co.uk/schools/gcsebitesize/science/add_aqa_pre_2011/atomic/atomstrucact.shtml

http://www.bbc.co.uk/schools/gcsebitesize/science/aqa/fundamentals/atomsact.shtml

Overview

Atoms are made up of the following sub atomic particles:

Electrons negative charge outside nucleus, in shells constant motion very very small (1/2000 of a proton) 

Neutron No charge, neutral Inside nucleus Same size as proton

Proton Positively charged Inside nucleus

Atomic Structure

Atoms have an overall neutral charge, therefore:

Number of protons = Number of electrons

Model of an AtomCriteria: • Different colour for each sub atomic particle• Electrons smaller than protons and neutrons• Labels – including charge of particles• Electron clouds – 2, 8

Complete worksheets provided

Compete Scipad page 10: Atoms

Describe the atomic structure of a lithium atom

Explain how the particles within an atom contribute to its overall mass.

Success Criteria

Describe the atomic structure of a lithium atom

Explain how the particles within an atom contribute to its overall mass.

Overall mass of an atom is made up of protons and neutrons, as the mass of electrons is negligible

Success Criteria

http://chemistry.about.com/library/weekly/blatomquiz.htm

http://ippex.pppl.gov/interactive/matter/elements.html

http://www.pbslearningmedia.org/asset/lsps07_int_theatom/

http://www.bbc.co.uk/education/guides/zt2hpv4/revision - read and complete the quiz at the end

http://phet.colorado.edu/en/simulation/build-an-atom

https://www.youtube.com/watch?v=wRNxrxXkCRQ – only watch the first section on atoms

Online Activities

Define the term ‘element’

Name and write symbols of common elements

Develop an understanding of the structure of the Periodic Table

SLO

Elements are made of only one kind of atom

◦Gold is made of gold atoms

◦Carbon is made of carbon atoms

◦Hydrogen is made of hydrogen atoms

Elements

Elements have been put in order of: Physical properties Chemical properties Atomic number Mass number Number of electrons in outer shell

  on the Periodic Table of Elements 

Atoms and Elements

https://www.youtube.com/watch?v=uPkEGAHo78o

1) Hydrogen2) Helium3) Lithium4) Beryllium5) Boron6) Carbon7) Nitrogen

8) Oxygen9) Fluorine10)Neon11)Magnesium12)Aluminium13)Silicon14)Phosphorus

HHeLiBeBCN

OFNeMgAlSiP

Elements to Learn

15)Sulphur16)Chlorine17)Argon

18) Calcium19) Zinc

The less obvious ones:1) Sodium2) Potassium3) Iron4) Copper5) Silver

6) Tin7) Gold8) Mercury9) Lead

SClAr

CaZn

NaKFeCuAg

SnAuHgPb

Element Song Daniel Radcliff

Learn your symbols: http://education.jlab.org/elementflashcards/

Online Activities

Periodic Table Video http://www.youtube.com/watch?v=1PSzSTil

u_

03/05/2023

Mendeleev

Periodic table

The periodic table arranges all the elements in groups according to their properties.

Horizontal rows are called PERIODS

Vertical columns are called GROUPS

03/05/2023

H He

Li Be B C N O F Ne

Na Mg Al Si P S Cl Ar

K Ca Fe Ni Cu Zn Br Kr

Ag I Xe

Pt Au Hg

The Periodic TableFact 1: Elements in the same group have the same number of electrons in the outer shell (this corresponds to their group

number)

E.g. all group 1 metals have __ electron in their outer shell

These elements have __ electrons in their outer shell

These elements have __ electrons in their outer shells

03/05/2023

H He

Li Be B C N O F Ne

Na Mg Al Si P S Cl Ar

K Ca Fe Ni Cu Zn Br Kr

Ag I Xe

Pt Au Hg

The Periodic TableFact 2: As you move down through the periods an extra electron shell is added:

E.g. Lithium has 3 electron in the configuration 2,1

Potassium has 19 electrons in the configuration __,__,__,__

Sodium has 11 electrons in the configuration 2,8,1

03/05/2023

H He

Li Be B C N O F Ne

Na Mg Al Si P S Cl Ar

K Ca Fe Ni Cu Zn Br Kr

Ag I Xe

Pt Au Hg

The Periodic TableFact 3: Most of the elements are metals:

These elements are metals

This line divides metals from non-metals

These elements are non-metals

03/05/2023

H He

Li Be B C N O F Ne

Na Mg Al Si P S Cl Ar

K Ca Fe Ni Cu Zn Br Kr

Ag I Xe

Pt Au Hg

The Periodic TableFact 4: (Most important) All of the elements in the same group have similar PROPERTIES. This is how I thought of the periodic table in the first place. This is called PERIODICITY.

E.g. consider the group 1 metals. They all:

1) Are soft2) Can be easily cut with a knife3) React with water

Metals on the _____ Non Metals on the ______

Rows tell us the number of electron shells an element has

Groups tell us the number of electrons in the outer shell

Patterns on the Periodic Table

https://play.kahoot.it/#/?quizId=6dcc49a4-465e-4829-add4-115f06d2e8e4&user=ngibellini&token=3888d935-6c6c-456b-a1eb-6c979d632e41

https://play.kahoot.it/#/?quizId=992e0aa6-2451-4a92-af04-c088951ea18f

Kahoots

Complete Scipad page 11and 13

http://www.bbc.co.uk/education/guides/z84wjxs/revision - read information, complete activity and quiz

http://inteleducationresources.intel.co.uk/content/keystage4/chemistry/pc/lessons/uk_ks4_elements_periodic_table/h-frame-ns6.htm

http://inteleducationresources.intel.co.uk/content/keystage4/chemistry/pc/lessons/uk_ks4_atoms_periodic_table/h-frame-ns6.htm

http://preparatorychemistry.com/Element_name_symbol_Flash1.htm

http://lessons.e-learningforkids.org/efk/Courses/EN/Science_Elements/base.htm

Success Criteria

Determine the structure of an atom based on data from the periodic table

Draw the arrangement of electrons around any given atom

Use the electron arrangement of an atom to identify which group on the periodic table it belongs too.

SLO

What is the difference between Gold and Oxygen?

Elements are made up of one kind of atom only Elements have been put in order of:

Physical properties Chemical properties Atomic number Mass number Number of electrons in outer shell

  on the Periodic Table of Elements 

Atoms and Elements

http://www.youtube.com/watch?v=pV822HfqT44&feature=fvwrel

https://play.kahoot.it/#/?quizId=6bee131c-b3e1-4180-b3ba-53db2256ed0e

Introduction to Atomic Structure

Atomic Number:

Smaller number Number of protons Number of electrons

Atomic Mass or Mass Number:

Bigger number of the two Total number of sub atomic particles Number of protons + neutrons.

Atom Information

How do we work out the number of:

Protons = Atomic number

Electrons = Atomic number

Neutrons = Mass number – atomic number

Fill in first 5 columns of Elemental information sheet

http://learningon.theloop.school.nz/moodle/mod/quiz/view.php?id=78647

Atomic Information

Electrons arrange themselves in regular order around the nucleus depending on their energy.

Each energy level holds a different number of electrons:

◦ Level 1 – 2 electrons◦ Level 2 – 8 electrons◦ Level 3 – 8 electrons

Electrons fill from Level 1 shell, or the closet to the nucleus first.

Electron Shell Configuration

Calculating electron arrangement using the periodic table:

Row/Period gives us the number of electron shells

Group tells us the number of electrons in outside shell

Eg Sodium – row 3 – three shells - group 1 – 1 electron in outside shell - electron arrangement = 2,8,1

The Periodic Table

Fill in columns 9, 10, 11 on elemental information sheet.

Draw dot diagrams for the first 5 elements H, He, Li, Be, B) (use dots for electrons, and draw shell lines in pencil, use blue pen for protons and red for neutrons)

Complete Scipad pages 12, 15, 16

Success Criteria

http://lgfl.skoool.co.uk/content/keystage4/chemistry/pc/lessons/uk_ks4_atoms_periodic_table/h-frame-ns6.htm

http://phet.colorado.edu/en/simulation/build-an-atom http://www.pbs.org/wgbh/aso/tryit/atom/ http://

www.learner.org/interactives/periodic/elementary_interactive.html http://

www.sciencequiz.net/jcscience/jcchemistry/atomstruct/atomicstmc1a.htm

http://science.widener.edu/svb/tutorial/protons.html http://www.pbs.org/wgbh/aso/tryit/atom/builder.html http://

www.classzone.com/books/earth_science/terc/content/investigations/es0501/es0501page05.cfm?chapter_no=investigation

http://www.bbc.co.uk/schools/gcsebitesize/science/add_edexcel/atomic_structure/electronsrev3.shtml - read and complete test bite

Online Activities

Describe the role of electrons in chemical reactions

Describe how positive and negative ions are formed

Write the name and formula of common ions

SLO

What’s the Answer?

Two atoms are walking down the street.

Says one atom to the other, "Hey! I think I lost an electron!"

The other says, "Are you sure??"

"Yes, I'm positive!"

Atoms

Chemical reactions occur when atoms gain or lose electrons

The fewer electrons that are gained or lost the more reactive atoms are.

Chemical Reactions

Atoms require their outer shells to be full in order to be chemically stable

Atoms either lose or gain electrons to get a full outer shell (2,8,8)

When atoms lose or gain electrons they become electrically charged and are then called ions

Gaining electrons (-ve) results in a ________ ion

Losing electrons results in a __________ ion The number of protons (+ve) stays the

same

Ions

E.g Na Na+ + e-

Sodium atom sodium ion Free electron2, 8, 1 2, 8,  Cl + e- Cl-Chlorine atom electron Chlorine ion 2, 8, 7 2, 8, 8 The charge on an ion is called its valency.  Valency always has a sign (+ or -) and a numerical value. (although we don’t write 1)

Complete ion information on elemental sheet

How do you know if an atom will gain or lose electrons?

Eg. Na 2,8,1 is it easier to lose one electron or gain 7? Hence Na looses a negative electron to become: Na+

Eg. Cl 2,8,7 is it easier to gain one electron or lose 7? Hence Cl gains a negative electron to become: Cl-

Calculating Ion Formation

Information Na Be ClAtomic NumberMass NumberProtonsNeutronsElectronsElectron Config.Gain/Lose Electrons+ve/-ve chargeIon FormedIon electron config.Protons: Electrons in Ion

Atom and Ion Information

Complete Scipad pages 17-19

Magnesium and calcium atoms both form ions with a charge of +2. Magnesium atoms form Mg2+ ions, and calcium atoms form Ca2+ ions.

Explain why magnesium and calcium atoms form ions with the same charge of +2. In your answer, you should: define an ion explain why atoms form ions identify the group on the periodic table where the two

atoms are found explain why both magnesium and calcium ions have a

charge of +2.

Success Criteria

Definition of an ion:

An ion is an atom or group of atoms that have lost or gained an electron and therefore carry a charge.

Explanation of formation of ions:

If the outer shell (valence) of an atom is not filled, the atom is unstable. It will react to gain a full outer shell to become more stable, by either losing or gaining electrons and making it into an ion.

Identification of Group: Magnesium and calcium are in the same group on the periodic table Group 2 – both have two electrons in outside shell.

Explanation of why both form+2 ions:

The atoms have the same number of electrons (two) in their outer shell. 2,8,2 and 2,8,8,2

Both Mg and Ca need to lose two outer electrons to become stable by having a full outer shell.

Each ion (Mg2+ and Ca2+) ends up with two less electrons(negative) than there are protons(positive) in its nucleus, so the ion has a charge of +2.

http://learningon.theloop.school.nz/moodle/mod/quiz/view.php?id=78656

http://education-portal.com/academy/lesson/ions-predicting-formation-charge-and-formulas-of-ions.html#lesson

Kahoots - https://play.kahoot.it/#/?quizId=2cac1ec6-82e3-4ba2-b5e2-70de7c141537&user=ngibellini&token=3888d935-6c6c-456b-a1eb-6c979d632e41

Online Activities

Describe ionic bonding

Use ions to write the name and formula of compounds

A sign outside the chemistry hotel reads "Great Day Rates,  Even Better NO3

-'s"

SLO

Ionic compounds: Have equal numbers of + and – charges

Made up of metal and non metal

Named by the ions they contain

Metal part goes first, then non metal

If non metal ion is made up of two or more elements change end to ate,

SO4 – sulphate

only 1 element in non metal ion it ends in ide NaCl = sodium chloride

Ionic Compounds

Positive Ions Negative Ions+1 +2 +3 -3 -2 -1H+

Hydrogen Ion

Mg 2+

Magnesium Ion

Al3+

Aluminium Ion

N3-

Nitrite IonO2-

Oxygen ionCl-Chloride ion

Li+Lithium Ion

Ca2+

Calcium IonFe3+

Iron III ionP3-

Phosphide ion

S2-

Sulphide ionBr-

Bromide ion

Na+

Sodium IonFe2+

Iron II ionPO3-

4Phosphate Ion

CO2-3

Carbonate ion

I-Iodide ion

K+

Potassium Ion

Cu2+ SO2-4

Sulphate IonNO-

3Nitrate ion

Ag+ Silver Ion

Zn2+ HCO-

Hydrogen carbonate ion

NH+4

Ammonium Ion

Pb2+ OH-

Hydroxide ion

Table of Ions

Ionic compounds have an overall neutral charge. Therefore there must be equal numbers of positive and negative charges. 

◦ Magnesium Nitrate Mg2+NO3-1

 Mg+ Mg+ NO3

-1

   

◦ 2 positives and one negativewhat is needed to balance the charges?

 ◦ Another negative or (NO3

-1)2  Mg2+(NO3

-1)2 - we need another whole anion so use brackets

Ionic Formulae

Write out symbols from table Put brackets around ions with two elements (two capitals) eg SO2-

4 Count the number of positives and negatives

Balance charges by multiplying ion Check it balances Rewrite without charges

Balancing Formula

Cross and Drop

Formulas show how many atoms of each type are in a compound The bottom right hand number tells us

how many of the atoms directly before it there are.◦ H20 = 2 hydrogen atoms, one oxygen atom

We don’t write 1 in as we are lazy!

Counting Atoms

The number directly outside a bracket is a multiplier of everything inside the bracket.◦ Al(OH)3 = 1 Al, 3 O, 3 H

◦ (NH4)3PO4 = 3N, 12 (3x4) H , 1P, 4 O

To get the total number of atoms we work out how many of each atoms there are and then add them

◦ (NH4)3PO4 = 3N, 12 (3x4) H , 1P, 4 O◦3+12(3x4)+1+4 = 20 atoms

A big number in front means two of the whole compound – so work out how many of each atom there is, add them up and then multiply this by the big number at the front.◦2(NH4)3PO4 = 3N, 12 (3x4) H , 1P, 4 O◦ 3+12+1+4 = 20 atoms◦ 20 x 2 = 40 atoms

Complete Scipad pages 20-27

Explain why the ions in sodium hydroxide combine to give the formula NaOH but the ions in beryllium hydroxide combine to give the formula Be(OH)2.

In your answer, you should: compare the charges on the individual ions found in

the compounds sodium hydroxide and beryllium hydroxide

explain why the ions combine in the ratios the way they do to form the compounds NaOH and Be(OH)2.

Success Criteria

Comparison of charges on ions:When these elements react, Na loses one electron and forms a +1 ion, while Be loses two electrons and forms a +2 ion in order to adopt the stable electron configuration. The hydroxide carries a charge of -1.

Explanation of formation of compounds: An ionic compound is electrically neutral

therefore all the positive charges must balance the negative charges.

Therefore it requires one OH-1 for each Na+ ion but two OH-1 ions for each Be2+ ion to form a neutral compound/ balance the charges.

Explain why the ions formed by sodium and oxygen both have the same electron arrangement. In your answer you should:• describe an ion• describe the atomic structures of a sodium ion and an oxide ion • state the charge on the sodium ion and the oxide ion• explain the charges on both ions in terms of electron arrangement and number of protons

Success Criteria

Element X is between numbers 11 and 18 on the Periodic Table. An atom of element X forms an ion. This ion combines with the hydroxide ion to form a neutral compound, X(OH)3.

Determine what element X is and justify your answer.

In your answer you should:• consider the ratio of X ions to hydroxide ions • use the formula X(OH)3 to determine the charge of the X ion • explain how you would use the Periodic Table in your Resource Booklet to find out which group element X is in • name element X.

http://www.learner.org/interactives/periodic/basics_interactive.html

http://www.sciencegeek.net/Chemistry/taters/Unit2IonicCompoundFormulas.htm

http://preparatorychemistry.com/Bishop_anion_nom_Flash1.htm

http://preparatorychemistry.com/Bishop_cation_nom_Flash1.htm

Online Activities

Write word equations for chemical reactions

Balance chemical equations

SLO

Reactant Product There has to be the same number and type

of each atom on both sides of the arrow – this is how you check you have balanced the equation correctly!

There are three types of equations◦ Word equations (don’t need atoms balanced)◦ Symbol equations◦ Ionic equations (not need for level 1)

Balancing Equations

Step 1: Write out word equation Magnesium + oxygen Magnesium oxide 

Step 2: Write out symbol formula Mg + O2 MgO  Step 3: Count atoms of each kind on each side 1 Mg 2 O 1 Mg 1O

Step 4: Identify the atoms with different numbers 2 oxygen atoms on left one on right

Step 5: Increase atoms by putting number:

in front of compound (2H2O) – makes 4 H & 2 O after an ion (Mg2) – makes 2 Mg brackets and a subscript around polyatomic ions

(SO4)2 –makes 2 S & 8 O

Do hydrogen then oxygen atoms first Mg + O2 2MgO

Step 6: Count atoms of each kind on each side – they will have changed as a result of step 5!!!!  1 Mg 2 O 2 Mg 2O  Step 7: Identify the atoms with different numbers 1 Mg on left & 2 on right  Step 8: Increase atoms numbers 2Mg + O2 2MgO

 Step 1: Write out word equation 

Sodium + Water Sodium Hydroxide + Hydrogen

Step 2: Write out symbol formula   Na + H2O NaOH + H2

 Step 3: Count atoms of each kind on each side   1 Na, 2 H, 1 O 1 Na, 1 O, 3 H Step 4: Identify the atoms with different numbers   2 H 3 H Step 5: Increase atoms by putting number: 

Na + 2H2O 2NaOH + H2

Step 6: Count atoms of each kind on each side  1 Na 4H 2 O 2 Na 2 O 4H  Step 7: Identify the atoms with different numbers 1 Na on left and 2 on right  Step 8: Increase atoms numbers 2Na + 2H2O 2NaOH + H2

 

Step 12: Count atoms of each kind on each side  

2 Na 4H 2 O 2 Na 2 O 4H Same type of atoms and same number of atoms on both sides – DONE! Nobody said it’d be easy but it does get easier, and remember practice makes perfect!

http://misterguch.brinkster.net/eqnbalance.html

http://www.files.chem.vt.edu/RVGS/ACT/notes/scripts/bal_eq1.html

http://www.sciencegeek.net/Chemistry/taters/EquationBalancing.htm

http://preparatorychemistry.com/Bishop_bal_eq_Flash1.htm

http://education.jlab.org/elementbalancing/ http://funbasedlearning.com/chemistry/chemBalancer/default.htm http://phet.colorado.edu/sims/html/balancing-chemical-equations/latest/balancing-che

mical-equations_en.html http://www.creative-chemistry.org.uk/gcse/revision/equations/02.htm

Kahoots: https://play.kahoot.it/#/?quizId=891a4988-2b62-4650-a6ad-2448a3185aa4&user=ngib

ellini&token=3888d935-6c6c-456b-a1eb-6c979d632e41 https://play.kahoot.it/#/?

quizId=b9a2e1f9-e174-4a17-904f-772c3d8ca5d7&user=ngibellini&token=3888d935-6c6c-456b-a1eb-6c979d632e41

https://play.kahoot.it/#/?quizId=a12c2b2d-859b-49cf-a878-10344ebc6639

Complete Sci pad pages 28-31

Online Practice and Help

Complete Scipad pages 8-9, 32-35 http://

www.nobraintoosmall.co.nz/students/science/NCEA_Level1/pdfs/90944_collated_atom_questions.pdf#zoom=100

Complete purple book pages:

Complete worksheets:

Revise Section 1: Basics

SLOs

Particle theory

http://www.youtube.com/watch?v=_rsqBNhFG1Y

http://inteleducationresources.intel.co.uk/content/keystage3/chemistry/pc/learningsteps/particle_theory/launch.html

http://www.bbc.co.uk/bitesize/ks3/science/chemical_material_behaviour/particle_model/activity/

https://www.youtube.com/watch?v=eSInI1xHvh4

Videos

In order for a reaction to occur particles need to collide

Particles need to collide with enough force to break bonds and form new ones

The more successful collisions the faster a reaction occurs

Complete Rates of Reaction Experiments

Collusion Theory

More successful collisions can be caused by: 

◦ Increasing the temperature (particles move faster so collide more)

◦ Increasing the concentration (more particles to collide)

◦ Increasing surface area (small particles have greater surfaces for collisions to occur)

◦ Use a catalyst (holds chemicals so collisions can occur, lowers activation energy needed to break bonds)

◦ Increase pressure (particles are closer together therefore collide more often)

 Increasing collisions increases rate of reaction!

What is the difference between particle theory and collision theory

Complete Rates of Reactions Experiments

Complete worksheets

Complete scipad pages 37-39, 48-53

Complete pages 40-47 (all the equipment you need is up the front)

http://www.kscience.co.uk/animations/collision.htm

Success Criteria

Particle theory – all matter is made up of particles which are in constant motion

Collision theory – particles need to collide with enough force and energy to break bonds and form new ones

More particles more collisions faster rate of reaction

More movement more collisions faster rate of reaction

Theories behind rates of reactions:

Calcium carbonate (marble chips) and hydrochloric acid react together in a conical flask.The word equation for this reaction is:

calcium carbonate + hydrochloric acid → calcium chloride + water + carbon dioxide gas

(a) Describe an observation you would make when this reaction occurs.

(b) Explain why the mass decreases with time.

When more concentrated hydrochloric acid is used, the reaction is faster.

© Explain the difference in the rate of reaction.

In your answer you should refer to: • particles • collisions • reaction rate.

Fizzing / bubbling occurs, marble chips decrease in size, heat is produced.

Why mass decreasesThe marble chips decreases as one of the products is CO2 gas. This gas escapes and so the mass of the flask and contents is reduced.

What’s happeningAs the reactant particles collide, they form product particles. As the reaction proceeds, there are fewer and fewer reactant particles left to collide and so the rate of reaction becomes slower. At the start (section X) of the reaction, more product particles are being formed, then more gas is being formed, therefore more gas escapes at first and so the mass of the flask and contents decreases more rapidly. At X, the rate of reaction is fast but decreasing with time.

In section Y there are now fewer (less) reactants and so there are fewer collisions per second (unit time) and so less product is formed, ie less gas being released, so the mass does not decrease as rapidly. At Y, the rate of reaction is slow and slowing.

In section Z the reaction has stopped, as one of the reactants (marble chips or HCl) has run out, so there are no particles left to react.

When more concentrated acid is used, there are more acid particles in the same volume of the acid. Because of this, there are more particles to collide with the calcium carbonate. Because there are more to collide, the rate of reaction is faster.

Explains why the reaction is faster, by linking the idea that there are more acid particles in the same unit volume available for collisions, and hence there will be more collisions, causing the faster reaction rate

http://lgfl.skoool.co.uk/content/keystage4/chemistry/pc/lessons/uk_ks4_rates_of_reaction/h-frame-ns6.htm

http://inteleducationresources.intel.co.uk/content/keystage4/chemistry/pc/lessons/uk_ks4_rates_of_reaction/h-frame-ns6.htm

SLOs

Define the terms acid, base and alkali

Name and write the formula of three common laboratory acids

Classify acids and alkalis as chemicals with distinct properties and uses.

SLO

Substance Acid (red/orange)

Base (purple/blue)

Neutral (green)

Acid or Base

Taste sour pH less than 7 Turn litmus red Contain hydrogen ion H+

Conduct electricity Acid rain (oxides of sulphur and nitrogen from

factories dissolve in water to form acid rain) citric juice, stomach acid (HCl), vinegar, battery

acid Acid reactions:

◦ Acid + base salt + water◦ Acid + metal salt + hydrogen gas◦ Acid + carbonate salt + water + carbon dioxide

Acids

Taste bitter, Feel slippery pH greater than 7 Turn litmus blue Alkali is a base that is soluble in water Metal oxides and metal hydroxides Most contain OH- ion, hydroxide ion Conduct electricity Soaps, oven cleaners (NaOH) Antacids (Mg(OH)2) – neutralise stomach acids Floor cleaners, bleach (ammonium hydroxide) Calcium hydroxide is limewater Calcium hydrogen carbonate – limestone caves Used to neutralise acids:

◦ Neutralisation ◦ HCl + NaOH NaCl + H2O = pH 7◦ Acid + Base salt + water

Bases and Alkalis

Common Name Chemical Name

Formula Acid Base

VinegarLemon juiceGrape juiceSoda WaterAntacidsFloor CleanerBattery AcidStomach AcidNitric AcidHydrochloric AcidMagnesium oxide

Formulae

Common Name Chemical Name Formula Acid Base

Vinegar Acetic Acid C2H4O2

Lemon juice Citric Acid C6H8O7

Grape juice Tartaric Acid C4H6O6

Soda Water Carbonic Acid H2CO3

Antacids Magnesium Hydroxide MgOHFloor Cleaner Ammonium Hydroxide NH4OHBattery Acid Sulphuric Acid H2SO4

Stomach Acid Hydrochloric Acid HClNitric Acid Nitric Acid HNO3

Hydrochloric Acid Hydrochloric Acid HClMagnesium oxide Magnesium oxide MgO

Formulae

Complete Scipad pages 58-59 What is an Acid, What is a Base

List three common household acids and their formulas

List three common household bases and their formulas

Success Criteria

http://inteleducationresources.intel.co.uk/content/keystage4/chemistry/pc/lessons/uk_ks4_acids_alkalis_salts/h-frame-ns6.htm

http://preparatorychemistry.com/Bishop_acid_base_Flash1.htm

http://preparatorychemistry.com/Bishop_type_sub_Flash1.htm

Online Interactives

Use the pH scale to compare the acidity and alkalinity of different solutions

http://inteleducationresources.intel.co.uk/content/keystage3/chemistry/pc/learningsteps/acids_alkalis/launch.html

http://inteleducationresources.intel.co.uk/content/keystage3/chemistry/pc/learningsteps/acid_base_reactions/launch.html

http://inteleducationresources.intel.co.uk/content/keystage3/chemistry/pc/learningsteps/neutral_react/launch.html

http://inteleducationresources.intel.co.uk/content/keystage3/chemistry/pc/learningsteps/ph_scale/launch.html

SLO

We use a pH scale to tell us how acidic, basic or neutral a substance is. Acids have a pH range from 1-6 Alkalis or bases have a pH range from 8-14 Neutral substances have a pH of 7 

pH

Strong acids contain more free H+ ions

Strong bases contain more free OH- ions

Most naturally occurring substances are weak eg. Citric acid in citrus fruit

Strong and Weak

Complete Scipad Investigations pages 61-62 Testing pH and Making Indicators

Complete Scipad page 63

Success Criteria

Name and write the formula for various metal oxides, metal hydroxides, metal carbonates and hydrogen carbonate

SLO

Metal oxides contain oxide ion O2-

Rust Iron oxide FeO, Zinc oxide (sunscreen) ZnO Basic Acid + Metal Oxide Metal Salt + Water

Metal Hydroxide Contain hydroxide ion OH-

Antacids Magnesium hydroxide MgOH Form when metal or metal oxide reacts with

water Acid + Metal Hydroxide Metal Salt + Water

Metals

Metal Carbonates Contain the carbonate ion CO3

-

Calcium carbonate CaCO3- marble chips

Release carbon dioxide when react with acids Acid + Metal Carbonate Metal Salt + Water + Carbon

Dioxide

Metal Hydrogen Carbonates Contain hydrogen carbonate ion HCO3

-

Neutralise acids Produce carbon dioxide when reacted with acids Calcium hydrogen carbonate CaHCO3 Acid + Metal Hydrogen Carbonate Metal Salt + Water +

Carbon Dioxide

Metals

Name Metal Type FormulaeCopper oxide

CuCO3Lithium hydroxide

FeOZinc carbonate

MgOHCalcium hydrogen

carbonate

Naming Metal Compounds

Describe neutralisation reactions

Identify the products of neutralisation reactions

SLO

When we add base to an acid, a chemical reaction takes place.

The acid and base are used up in the reaction.

We say they are neutralised. They make a salt and water.

When a substance has been neutralised or is neutral it has a pH of around 7.

Acid + Base Salt + Water

Neutralisation

Aim: To neutralise an acid using a base. Method: Step 1: Add four drops of sodium hydroxide to a test tube. Step 2: Add one drop of universal indicator to the test tube and shake.  Step 3: Stop when the solution is green, if the solution turns red or orange add a very small drop of NaOH until the liquid turns green. 

Neutralization Reaction

Complete Scipad practical page 64 Neutralisation

Complete scipad page 65

Tasks

What causes indigestion?-to much acid in the oesophagus

What do we need to add to neutralize that acid? Base! – Antacid, quickeze, mylanta,

gaviscon etc

Indigestion

   Iron

 Magnesiu

m

 Zinc

 Copper

 

 Lead

 Hydrochlori

cAcid

         

 Sulphuric

Acid

   Zinc

SulphateZnSO4

  

NoReaction

 

 NitricAcid

         

SaltSalts are named after the acids from which they are formed.• Hydrochloric acid forms chloride salts• Sulphuric acid forms sulphate salts• Nitric acid forms nitrate salts

http://lgfl.skoool.co.uk/content/keystage4/chemistry/pc/lessons/uk_ks4_acids_alkalis_salts/h-frame-ns6.htm

Complete pages 93, 94, 95

A student puts 5 mL of dilute hydrochloric acid into a boiling tube and adds five drops of universal indicator to the solution. The student then takes a solution of sodium hydroxide of the same concentration as the acid and adds it one drop at a time to the acid until the colour stops changing.  Describe the colour of the universal indicator solution: 

◦ in the hydrochloric acid before any sodium hydroxide was added.◦ when the sodium hydroxide was added and the colour of the solution stopped

changing. As the sodium hydroxide is added several colour changes occur.  Explain how the colour changes relate to pH AND what ions are present

in the solution colour changes. 

Success Criteria

Description of colour changes: red / pink to start with blue / purple / violet at end.Explanation of colour changes:At the beginning the red indicated a low pH due to excess H+ ions in the solution.As the NaOH was added, a yellow / green colour indicates a pH of around 7, due to the OH - ions combining with the H+ ions to form a neutral solution. As more NaOH is added the blue / purple indicated a pH of 11 plus, due to excess OH - ions in the solution.Identification of reaction type:Acid-base (or acid-carbonate) neutralisation (the carbonate ions react with the H+ ions of the acidic solution and neutralise the solution).Description of observations: Bubbling in the solution / fizzing / effervescence / frothing / foaming Ca2CO3 disappears.Linking observations to products:The products are CO2, H2O and a salt. The CO2 gas causes the bubbles / fizzing / etc. Writing a word equation:Nitric acid + sodium carbonate sodium nitrate + water + carbon dioxideWriting a symbol equation:2HNO3 + Na2CO3 2NaNO3 + H2O + CO2

A student put 10 ml of dilute nitric acid in a boiling tube with five drops of universal indicator. Sodium hydroxide of the same concentration was then added. The following observations were recorded.

Discuss the reaction occurring as sodium hydroxide is added to the nitric acid.

In your answer you should:• explain the relationship between the colours observed and the pH of the solution• explain which ions cause the different colours of the solution • write a word equation for the reaction AND a balanced symbol equation for the reaction.

Write word and symbol equations for a range of reactions involving acids and bases

Describe some everyday uses of acids, alkalis and neutralisation

SLO

Acid + Base Salt + Water

Hydrochloric acid + sodium hydroxide

sodium chloride + water

Test to see if reaction is complete by using indicator – solution should turn

Green

Acids + Base

Complete scipad pages 66-68 Writing chemical equations

Complete Scipad practical Making Salts, page 69

Tasks

Acid + Carbonate Salt + Water + Carbon dioxide

Sulphuric Acid + Copper Carbonate Copper sulphate + water + Carbon dioxide

We test for Carbon dioxide by bubbling the gas into lime water which turns

milky

Acid + Carbonate

Limewater (calcium hydroxide) reacts with carbon dioxide to produce a precipitate of calcium carbonate:

Ca(OH)2 (aq) + CO2 (g) → CaCO3 (s) + H2O (l)Limewater + carbon dioxide calcium carbonate + water

If excess CO2 is added, the following reaction takes place:

CaCO3 + H2O + CO2 --> Ca(HCO3)2 (colourless)Calcium Carbonate + water + carbon dioxide calcium bicarbonate

Limewater

Complete Scipad practical page 70 Carbonates and Acids

Complete Scipad page 71-73

Tasks

Acid + Metal Salt + Hydrogen Gas

Nitric Acid + magnesium magnesium nitrate + hydrogen gas

We test for hydrogen gas by doing the POP test

Acid + Metal

Acid + Base Salt + Water

Acid + Carbonate Salt + Water + Carbon dioxide

Acid + Metal Salt + Hydrogen Gas

Acid Reactions

A student wanted to make the salt, magnesium chloride.

Discuss how the student would make magnesium chloride salt from hydrochloric acid and magnesium oxide.

In your answer you should:• state what type of reaction occurs• write a word equation AND a balanced symbol equation for the reaction between hydrochloric acid and magnesium oxide• explain how you would make magnesium chloride in a school lab from hydrochloric acid and solid magnesium oxide (this can be done by drawing labelled diagrams).

Success Criteria

Type of reactionAcid-Base reaction or neutralisation.

Word Equationhydrochloric acid + magnesium oxide → magnesium chloride + water.

Balanced Equation2HCl + MgO → MgCl2 + H2O

How to make itAdd magnesium oxide to hydrochloric acid in a beaker. Heat slightly and pour this into an evaporating dish and leave somewhere warm (e.g. window sill) for a few days or heat over Bunsen to speed up the reaction, so that the water can evaporate, leaving magnesium chloride salt. Safe lab procedure would include dealing appropriately with chemicals such as HCl or the wearing of safety glasses

Complete Scipad pages 74-79

Brainstorm connecting words

Read the question and answer on the sheet,◦ highlight the connecting terms, ◦ use the marking schedule to mark it.

Swap and complete one more question

Complete questions on worksheet ◦ Use connecting terms!

Complete Scipad practice NCEA exam under exam conditions pages 80-85, mark it!!

Revision

Online Tutorials and Quizzes◦ http://

inteleducationresources.intel.co.uk/keystage3.aspx?id=64

Online Activities

Atoms and ions◦ Structure of an atom, number of protons, neutrons, elections,

electron configuration◦ Isotopes◦ Ion formation ◦ Ionic compounds

Rates of reactions◦ Particle theory◦ Factors affecting rate◦ Observations and tests for gases

Acids reactions◦ Properties of acids and bases◦ Common acid equations◦ pH, indicators and neutralisation◦ Word equations and balanced equations

Revision