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Chemical ReactionsSpecific Learning Outcomes (SLO's; these incorporate knowledge, scientific and other essential skills and attitudes). At the end of this unit students will be able to: Explain safe ways of storing chemicals and cleaning chemical spills Recall the first 20 elements in order and draw any of them as a neutral atom

labelling the two particles and their charges in the atom’s nucleus (proton-positive charge, neutron-no charge) with the correct number of electrons orbiting (negative charge).

Recall the names and formulas for common mineral acids (HCl, H2SO4, HNO3) and an organic acid (acetic/ethanoic: CH3COOH)

Recall the names and formulas for common bases (NaOH, NH3, Ca(OH)2) Recognise that a base that is soluble in water is called an alkali. Give everyday examples of acids and bases (HCl in stomach, CH3COOH in vinegar,

H2SO4 in car batteries, NaOH in oven cleaner, NH3 in general household cleaners) Observe and recall colour changes of indicators (litmus, universal) and pH with acids,

bases and water. Recall and use the pH scale to indicate the relative positions of acids, bases and neutral

substances on the scale. Carry out experiments to investigate the pH of household substances (bleach, stain

remover, white vinegar, antacid, cream of tartar, baking soda, sugar, soap, NaCl salt) Carry out experiments to observe the reaction between acids and bases. Recall that the general neutralisation reaction is Acid + Base --> Salt + Water Write word equations for the neutralisation reaction

e.g. hydrochloric acid + sodium hydroxide --> sodium chloride + water Carry out experiments to observe the reaction between acids and metal. Recall the general reaction Acid + Metal --> Salt + Hydrogen gas (H2) Observe and recall that hydrogen gas is produced when an acid reacts with a metal, explodes

when ignited in air (the 'squeaky pop test') and is less dense than air Write word equations for the reaction between acids and metals

e.g. hydrochloric acid + magnesium --> magnesium + hydrogen gas Carry out experiments to observe the reaction between acids and carbonates. Recall the general reaction: Acid + Carbonate --> Salt + Water + Carbon Dioxide gas (CO2) Observe and recall that the carbon dioxide produced in the reaction between an acid and

a carbonate, extinguishes a burning splint, turns limewater milky and is denser than air. Write word equations for the reaction between acids and carbonates e.g.

hydrochloric acid + calcium carbonate --> calcium chloride + water + carbon dioxide gas Describe simple properties of acids (taste sour, turn blue litmus red, fizz with magnesium

and fizz with marble chips and contain the element hydrogen) and bases (turn red litmus blue, react with acids and feel soapy)

Observe and recall that oxygen causes a glowing splint to relight and is approximately the same density as air . Recall the names, formulae, preparation and tests for the hydrogen, carbon dioxide and

oxygen and draw a molecule of these gases. Recall that an ion is a neutral atom that has lost or gained electrons and that

positively charged ions attract negatively charged ions. Use a table of ions to find formulas of salts from their names (and vice versa) Recognise that for a reaction to occur we need an effective collision Investigate factors that affect the rate of a reaction (ie temperature, concentration, surface

area and catalysts) through experimentation. Use the collision theory to explain how temperature, concentration and surface area affect

the rate of reaction. Identify exothermic and endothermic reactions through experimentation (sodium

hydroxide in water and ammonium nitrate in water) Recall everyday examples such as combustion (exothermic), respiration (exothermic) and

photosynthesis (endothermic).

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Unit Word ListAcetic Acid denser than air manganese dioxide redacetic/ethanoic acid density metal relightsAcid DNA

(deoxyribonucleic acid)

milky respiration

Acidic effective collision mineral acids Saltalkali electrons molecule salt (NaCl)Ammonium Hydroxide

element negative charge soapy feel

antacid tablets endothermic reactions

neutral atom Sodium ( Na)

atom equation neutral solution Sodium Hydroxidebaking soda exothermic reactions neutral substances solublebases experiment neutralisation solutionBasic explodes neutron splintbleach extinguishes nitrate squeaky pop testBlue faster Nitric Acid stain removerburning splint gas no charge stomach acidcalcium ( Ca ) glowing splint nucleus sugar soapCalcium Hydroxide green one sulfatecar battery acid Hydrochloric Acid orbiting Sulfuric Acidcarbon dioxide gas Hydrogen Carbonate organic acid surface areacarbonates hydrogen gas orientation Tannic Acidcatalysts hydrogen peroxide oven cleaner taste sourchemical equation Hydroxide oxygen gas temperaturechemical formulas ignited particles test tubechemical names indicators pH scale theorychemicals ions phosphate universal indicatorchloride iron ( Fe ) photosynthesis vinegarCitric Acid less dense than air pop Watercollision lichen positive charge white vinegarcollision theory lighted ( lit ) Potassium

permangenatezinc ( Zn )

colour changes limewater properties of acids combustion litmus indicator protonconcentration magnesium ( Mg ) Pure water corrosive Magnesium

Hydroxiderate of a reaction

cream of tartar Magnesium ribbon reaction


Knowing Atoms and Elements- (the first 20 anyway)

1/ How many types of atom does an element have ?

_______________________________________________

2/ Name the particles and give the charge for A, B, C in the diagram of the sodium atom shown below

Letter Name of particle Charge typeA

B

C

3/ Find the Periodic Table in your science manual.

a) About how many elements are there ?________________________________

b) Name 6 elements that exist as gases

1 3 5

2 4 6

c) Name one element (of the two) that is a liquid.____________________________

d) Fill in the symbols and names for the first 20 Elements from the Periodic Table in order. The first two are done for you.( You are expected to learn this and be able to fill this in from memory.)

1 2 13 14 15 16 17 18H

HydrogenHe

Helium

P

Valency Number _____ _____ _____ _____ _____ _____ _____ _____


Safe ways of storing chemicals and cleaning up chemical spills

Acids and bases can be very corrosive and can ‘eat away” or corrode objects such as metals, clothing and your skin. They must always be handled with care.

Most schools have laboratory rules for the protection of students. Here are a fewof the more important ones relating to the handling of chemicals. Think of a reason for each of these rules.Rule ReasonStudents must wait outside a lab until a teacher is present.

Food must not be eaten in a lab and glassware must not be used for drinking.Any accident, no matter how unimportant it may appear at the time, should be reported to the teacher.Split chemicals must be wiped up immediately.

Acids or bases split on skin or clothing must be washed off immediately under running water.Take care not to bump anyone who is using chemicals.

Always check the label on the bottle before using the contents.

Look at the four pictures A to D below. Write down the lab rule that is being broken in each case in the space provided.

A B C D

A

B

C

D


Report even minor accidents.

Gas Test RevisionComplete the table below to summarise the gas tests you learnt in Year 9.

Name of gas Formula Drawing of a molecule

Density(compared to air – more/less/same)

Test and Observation:

Complete the sentences

OxygenO______ gas r________ a g________ splint.

H2

H_________ gas e__________ when ignited with a l_____ splint. This test is known as the squeaky p___ test.

Carbon dioxide

C_______ d________ gas turns l____________ milky and e__________ a l___ splint.

Testing Oxygen Gas

The following diagram shows four steps in the test for oxygen however they are not in the correct order. Number the diagrams from 1 to 4 in the space provided to put them in the correct order

Making Oxygen Gas

What would the “chemicals making oxygen” shown in the diagram above be?

Oxygen can be made by heating purple p__________ p_______________ in a dry t _____

t_____ or adding black m_____________ d__________ to hy_________ p___________ in

a t_____ t______. The o_________ gas produced r_______________ a g__________

splint.


Common Acids and Alkalis

AcidsAll acids contain the element H___________ and release the H__________ ion (H+) which is

the part that makes them an a_______. The acids that you use in the lab are called

mi________ acids and are very co_________. The acids that we find in plants or animals are

called o___________ acids and are not as corrosive.

Complete the table below for the names and formulae of common acids.

Formula:

HCl H2SO4

CH3COOH

Name: Nitric acid

BasesAll bases release the H__________ ion (OH-) which is the part that makes them a base.

Soluble bases are called al_________. Bases are described as the opposites of a_______.

Complete the table below for the names and formulae of common alkalis.

Formula:

NaOH Ca(OH)2

Name: Ammonia(Ammonium hydroxide)

Neutral SubstancesBetween acids and alkalis there are many substances which are n__________. Pure water is a common example.

‘Everyday’ Acids and Alkalis:Match the name of the acid or alkali with where it is found. (Use lines or colour code your answers)

Name of acid/alkali Where it is foundhydrochloric acid lemon juicecitric acid car batteriestannic acid nucleus of cellsDNA (deoxyribonucleic acid) teamagnesium hydroxide (an alkali) in the stomachsulfuric acid antacid tablets

SummaryUse the information on this page to write a sentence to explain each of the following terms:Acid _____________________________________________________________________

Base _____________________________________________________________________

Alkali _____________________________________________________________________

Neutral ___________________________________________________________________


Antacid TabletsContains citric acid

Indicators and the pH scale

1. The pH scaleSome acids are weak enough for us to eat eg. v__________. However, other acids such as s____________ acid can be strong. The strength of an acid is measured by its p__.Every acid contains H___________ (H+) ions. The stronger the acid, the more h_______ i______ there are in it. pH is a symbol that shows the ‘strength of acids and bases’.Pure water is n______________ and has a pH of ____.The pH scale ranges from __ to __ and is shown below:

3. IndicatorsAn i___________ is a dye that changes c________ when it is put into an a_______ or a b__________. There are a number of different indicators but you only need to learn two: L__________ and U___________ i___________. Many are made from plant extracts. L_________ is made from lichen.

Colour changes of Universal Indicator

5. Use the information on this page to answer the questions below:a. Which is more acidic, pH 3 or pH 6?________

b. Would a pH of 2 be suitable for a shampoo? Explain. __________________________

____________________________________________________________________

c. Which is more acidic – human or cow’s milk? ________________________________

d. What colour would Universal indicator turn when added to lemon juice? ___________

e. What colour would Red Litmus turn when added to sodium hydroxide?____________

f. What colour would an antacid tablet turn Universal Indicator? ___________________


strongstrong weak weak

2. pH of common substances. Complete the table below.SubstancepHAcidic, basic or neutral?Human milk7HCl1acidicNaOH13Lemon juice2.3Pure

waterneutralBaking soda8.4Stomach juices2Vinegar3Antacid tablet11Cow’s

milk6.5Skin and hair6.6Human blood7.4

4. Complete the table below to summarise the colours of indicatorsColour in acidColour in waterColour in baseBlue Litmus

Red LitmusUniversalIndicator

Neutralisation Reactions: Acid + Base Salt + Water1. What is neutralisation?Definition: Neutralisation occurs when an a_______ is added to a b______ to make a

n____________ solution. This solution contains a s_______ plus w________.During a neutralisation reaction, the H_________ (H+) ions of the acid combine with the H___________ (OH-) of the base to make water (H2O) which would turn Universal Indicator g_______.

Example:

General Equation: ACID + BASE SALT + WATER

Word Equation:Hydrochloric acid + Sodium hydroxide Sodium chloride + Water

2. Complete the following sentences:a. When hydrochloric acid is added to a base, a c_____________ salt is produced.b. When sulfuric acid is added to a base, a s_____________ salt is produced.c. When nitric acid is added to a base, a n____________ salt is produced.

3. Complete the following word equations for neutralisation reactions:a. Sodium hydroxide + Sulfuric acid S_________ s__________ + w_______

b. Calcium hydroxide + Sulfuric acid C_________ s__________ + ________

c. Sodium hydroxide + Nitric acid S_________ n__________ + ________

d. Calcium hydroxide + Hydrochloric acid C_________c__________ + ________

4. Useful neutralisation reactionsTaking the sting out. Bees have an acid sting while wasps have a basic sting. To treat the sting we need to neutralise it. What could you use from the list below to treat a bee sting? ____________ or a wasp sting? ________________. (List: vinegar, lemon juice, water, baking soda)

Cleaning your teeth. During the day your teeth become coated in sugars and acids from the food you eat. Toothpaste helps to neutralise the effect of acids formed when microbes in your mouth feed on sugar. Would toothpaste be acidic, neutral or basic? _____________

Curing indigestion. Dilute hydrochloric acid is found in your stomach. When you suffer from indigestion, there is more acid in the stomach than is needed. People take indigestion tablets to help this problem. These tablets often contain magnesium hydroxide. How do these tablets fix the problem?______________________________________________


Sodium hydroxide

Hydrochloric acid

A salt – sodium chloride – dissolved in water

LEARN this general equation

Acids and Carbonates

1. Acids react with c______________ to produce a s_____ and c__________ d_________

and w________. To test for c_________ d___________, the gas is bubbled through l_____

w________. If the gas is c__________ d___________, the l_____ w________ will turn

m___________.

General Equation:ACID + CARBONATE SALT + WATER + CARBON DIOXIDE

Word equation:Hydrochloric acid + Calcium carbonate Calcium chloride + water +Carbon dioxide gas

2. Complete the following sentences:a. Zinc carbonate + Sulfuric acid Z____ s__________ + w_____ + c_______ d________

b. Magnesium carbonate + Hydrochloric acid M__________ c__________ + w_______

+ c__________ d____________

c. Sodium carbonate + Hydrochloric acid ________ _______________ + __________

+ ____________ _________

d. Calcium carbonate + Nitric acid __________ _____________ + ______________ +

+ ____________ _________

3. Limestone contains calcium carbonate. You can prove this by adding a few drops of hydrochloric acid to a sample of the rock. If calcium carbonate is present what would you observe? _________________________________________________________________

4. Hydrogen carbonates.Hydrogen carbonates react in the same way as c_____________ and when added to an acid will produce a s______, c__________ d____________ and w___________.The chemical name for baking soda is sodium hydrogen carbonate and the chemical name for vinegar is acetic acid. They are both commonly found in the kitchen. Complete the following equation for this reaction.Sodium h__________ carbonate + a________ acid sodium acetate + ___________

___________ + ____________


Making carbon dioxide gas

marble chip

hydrochloric acid

Carbon dioxide

gas

Testing carbon dioxide gas

Acid + carbonate

Clear lime water Cloudy

lime water


Acids and Metals

1. Acids react with metals to produce a s______ and h__________ gas. To test for h________ g___, a l___ s________ is held in the gas. If the gas is h__________ then it will ignite with a p____.

General Equation:

ACID + METAL SALT + HYDROGEN

Word equation:Hydrochloric acid + Magnesium Magnesium chloride + hydrogen gas

2. Complete the following sentences:a. Sulfuric acid + Zinc Z_________ s__________ + H_________

b. Sulfuric acid + Magnesium M_________ s__________ + __________

c. Hydrochloric acid + Zinc Z_________ c__________ + __________

d. Sulfuric acid + Iron __________ ___________ + __________

Properties of Acids and Bases3. Complete the table below to summarise the properties of acids and bases.

Properties of Acids Properties of Bases

Acids are s________ in water Soluble bases are called a___________

Acids turn blue l_______ r______. Bases turn red l_______ b________

Acids turn Universal indicator __________ Bases turn Universal indicator ___________

Acids contain H__________ and produce

H__________ (H+) ions in solution.

Bases release the H___________ (OH-) ion

when mixed with water

Acids have a s_______ taste Bases are s_______ to touch

Acids have a pH of less than ______ Bases have a pH of more than _______

Acids react with m_________ to produce

H__________ gas

Bases react with a_________ to produce

s_______ and w________.

Acids react with c___________ to produce

C_________ d__________ gas

The reaction between an acid and a base is

called a n____________________ reaction.



Hydrogen gas

Sulfuricacid

Making hydrogen gas Testing for hydrogen gas

Lit splint

Test-tube of gas

Pops when

lit

Magnesium ribbon

Writing Ionic Formulae Table of ions Positive ions Negative ions

+3 +2 +1 -1 -2Al3+

AluminiumCu2+

CopperH+

HydrogenCl-

ChlorideO2-

Oxide

Fe3+

Iron (III)Ca2+

CalciumLi+

LithiumOH-

HydroxideSOSulfate

Mg2+

MagnesiumNa+

SodiumNO

NitrateCO

CarbonateK+

PotassiumHCO

Hydrogen carbonate

NHAmmonium

1. Formula Speed Test Instructions: Use pencil to fill in the grid with the correct formulae as quickly as possible and record your time.

Cl- SO NO CO HCOK+ KCl K2CO3

Ca2+

Al3+

Na+

NH

Cu2+

Fe3+

2.Complete the following tableFormula Name Number of

elementsName of the

elementsNumber of atoms of

each element

Total number of atoms in one

moleculeMgO Magnesium oxide 2 oxygen

magnesium11

2

SO2 ………………………….

NH3 ………………………….

MgSO4 ……………………………………….

NaOH ……………………………………….

NaHCO3 …………………………………………………….


Trial Time Errors Score12345

More Ionic Formulae1. Write Ionic Formulae for the following Word Equations. (Fill in the gaps).

Acid + Base Salt + Water

Hydrochloric acid + Magnesium hydroxide Magnesium chloride + Water

__________ + _____________ _______________ + H2O

Sulfuric acid + Calcium hydroxide Calcium sulfate + Water

__________ + ____________ _______________ + H2O

Acid + Metal Salt + Hydrogen

Hydrochloric acid + Zinc Zinc chloride + Hydrogen

______________ + Zn ____________ + H2

Sulfuric acid + Magnesium Magnesium sulfate + Hydrogen

_____________ Mg ______________ + H2

Acid + Carbonate Salt + Carbon dioxide + Water

Hydrochloric acid + Copper carbonate Copper chloride + Carbon dioxide + Water

_____________ + ______________ ____________ + ___________ + ________

2. Match the chemical formulae to the chemical name. (Use lines or colour code)Chemical formulae Chemical nameNaCl Hydrochloric acidCaCO3 Sodium hydroxideMg(OH)2 Acetic acidCH3COOH Calcium carbonateNaOH Sodium chlorideHCl Sodium hydrogen carbonateNaHCO3 Magnesium hydroxide

3. Chemical FamiliesPut the compounds below in the correct column(s). Some compounds may fit into more than one column.

Acids Bases Nitrates Sulfates Carbonates

HCl Na2CO3 H2SO4 CaSO4 NaNO3 HNO3

LiHCO3 Cu(NO3)2 NaOH Ca(OH)2


Acids and Base Puzzle: A Basic Problem

What do you get when you cross a jumbo jet with a kangaroo?

1. Substances which gives hydrogen ions in solution. ___ ___

___ ___ ___

2. Metal which does not react with dilute acids. ___ ___ ___ ___ ___

___

3. Soluble base. ___ ___ ___ ___ ___ ___

4. Changes colour in acid or alkaline solutions. ___ ___ ___ ___ ___ ___ ___

___ ___

5. Gas which dissolves in water to give an alkaline solution. ___ ___ ___ ___ ___ ___

___

6. Vinegar is a dilute solution of this acid. ___ ___ ___ ___

___ ___

7. Acid produced when milk sours. ___ ___ ___ ___ ___

___

8. Measure of acidity ___ ___

9. Neutral liquid ___ ___ ___

___ ___

10. You should never t___________ a chemical in a lab. ___ ___ ____ ___ ___

11. Body organ which produces hydrochloric acid ___ ___ ___ ___ ___

___ ___

12. Metamorphic rock which fizzes with HCl ___ ___ ___

___ ___ ___

13. Describes acids which give a low concentration of hydrogen ions ___ ___ ___ ___

14. Litmus turns this colour in basic solutions. ___ ___ ___ ___

15. React with acids to give a salt and water. ___ ___ ___ ___

16. Indicator which turns blue in basic solutions ___ ___ ___ ___ ___ ___

17. Chemical formula for sodium hydroxide Na___ ___

18. Positively charged particle in an atom ____ ____ ____ ___ ___ ___19. Acid which gives off a brown gas when it reacts with metals. ___ ___ ___ ___ ___

___

20. Acid found in oranges and lemons. ___ ___ ___ ___

___ ___

21. Reacts with acids to give off carbon dioxide. C H A

L K


22. Gas produced when metals react with dilute hydrochloric acid. ___ ___ ___ ___ ___ ___

___ ___

23. Sound made when hydrogen gas ignites. ___ ___

___

24. Produced when an acid reacts with an alkali ___ ___

___ ___

Endothermic and Endothermic ReactionsReactions that give out h________ are called e_______________ reactions.Reactions that absorb h_______ are called e_______________ reactions.

Photosynthesis is an example of an e______________ reaction because light e____________ is a_____________ by the plant leaf. If this plant could be eaten, eg. a lettuce ,e________ would be released during the process of r________________.Are the following reactions endothermic or exothermic?a. A burning candle. _____________________b. Solid NaOH dissolves in water ______________________c. Solid ammonium nitrate dissolves in water ______________________d. An egg is fried ______________________


Reaction Rates The r___________ r________ describes how fast a c___________ r_____________ occurs.Some chemical reactions occur rapidly, eg the explosion of dynamite. Others occur slowly, eg. the rusting of iron.The r______ of a r____________ can be measured by finding out how quickly the r____________ are used up or how quickly p_______________ are formed.

The collision theory states that for a r_____________ to occur:

a. There must be a c_____________ between reacting particles.

b. The p______________ must c__________ with enough e___________ to break the forces holding p___________ together.

c. The p__________ must c___________ in the correct o_______________ (or position)

The c_____________ t___________ also states that reactions go f____________ when there are more collisions between p____________.The r______ of r___________ can be speeded up by:

Increasing t_______________. When the t______________ increases, p__________ move faster and c________ more

often. Increasing the t____________ will ___________ (increase/decrease) the r___________ rate.

Increasing the c________________ of the dissolved reactants.When the c______________ is increased, there is a higher number of p_________ to react. More c______________can occur so the r_______ of r______________ will______________ (increase/decrease).

Increasing the s___________ a___________ of solid reactants.When the s___________ a_______ of a reactant is increased, more p____________ are exposed for c___________ to occur.The r_____ of r_____________ will ____________ (increase/decrease).

Using a c__________. A catalyst is a c________added to a reaction that increases the r_____ ofreaction without being used up. A c___________lowers the e_______ needed for p__________ toform.

Use the collision theory to explain these observations:a A fire is hard to start using large logs. Wood cut into small pieces of kindling allows a fire

to start easily. _________________________________________________________________________________________________________________________________________

b. Magnesium metal burns violently in a gas jar of oxygen. It reacts more slowly in air. _______________________________________________________________________

c. Lumps of coal can be safely stored in a coal bucket in the home, but fine coal dust has caused explosions in coal mines. _______________________________________________________________________


A B

Concentration

Surface Area

Definitions PracticeIn the space beside each of the words in the following list, select a definition from the list below and write it out.Acidalkalibasescatalystseffective collision

endothermic reactionsexothermic reactionsindicatorsionsneutral atom

neutral solution

neutralisation

pH scale

rate of a reaction

surface area

Definitions Lista This type of collision is required if two substances are going to successfully react to

form a product.b A corrosive chemical that contains free hydroxide ions that turns Litmus and

Universal indicator BLUE.c A soluble base containing hydroxide ions that turns Litmus and Universal indicator

BLUE.d A chemical reaction that requires energy (usually heat) to be supplied to it if the

reaction is going to continue.e A corrosive chemical that contains free hydrogen ions that turns Litmus and

Universal indicator RED.f A chemical reaction that gives off energy as heat.g The general chemical reaction name for reacting all of an acid with a base forming

neutral water and a salt.h A substance that speeds up a chemical reaction without being used up in the

process.i An atom or group of atoms that has lost or gained electrons and are therefore

charged.j The scale that measures how acidic or basic a solution is (measured on from 1 to 14)k A solution that does not contain any extra hydrogen ions or hydroxide ions.l An atom that has exactly the same numbers of positive protons in its nucleus as

there are negative electrons orbiting around it.m A substance that changes colour in the presence of an acid or a base.n A measure of the amount of surface a reactant has exposed to the substance it is

reacting with.o The speed that reactants involved in a reaction are used and products of a reaction

are produced.


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