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Questions and Answers
Which of the following compounds follows the naming rule that ends with –ide?
Which of the following compounds follows the naming rule that ends with –ide?
What must be true when writing a balanced chemical equation?
What must be true when writing a balanced chemical equation?
What suffix is generally used for compounds that contain three or more elements, one of which is oxygen?
What suffix is generally used for compounds that contain three or more elements, one of which is oxygen?
Which of the following statements is true regarding the conservation of mass in chemical reactions?
Which of the following statements is true regarding the conservation of mass in chemical reactions?
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In the naming of compounds, when two of the same element are present, what is the naming convention?
In the naming of compounds, when two of the same element are present, what is the naming convention?
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Which of the following represents a correctly balanced symbol equation?
Which of the following represents a correctly balanced symbol equation?
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Which compound is correctly named based on its formula Al(OH)3?
Which compound is correctly named based on its formula Al(OH)3?
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What does a state symbol of (s) indicate in a chemical equation?
What does a state symbol of (s) indicate in a chemical equation?
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What must be true for a chemical equation to be considered balanced?
What must be true for a chemical equation to be considered balanced?
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Which method is acceptable for balancing a chemical equation?
Which method is acceptable for balancing a chemical equation?
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In the reaction 2Mg + O2 → 2MgO, how many atoms of magnesium are present on the reactants side?
In the reaction 2Mg + O2 → 2MgO, how many atoms of magnesium are present on the reactants side?
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What is the state symbol for a gas in chemical equations?
What is the state symbol for a gas in chemical equations?
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Which of the following is NOT a step in writing a balanced equation?
Which of the following is NOT a step in writing a balanced equation?
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How do you indicate the physical state of a substance in a balanced equation?
How do you indicate the physical state of a substance in a balanced equation?
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What is the balanced form of the reaction for sodium and chlorine?
What is the balanced form of the reaction for sodium and chlorine?
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What is produced during a combustion reaction?
What is produced during a combustion reaction?
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Which type of reaction results in a solid precipitate?
Which type of reaction results in a solid precipitate?
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In a precipitation reaction, the substances being mixed are typically in what state?
In a precipitation reaction, the substances being mixed are typically in what state?
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What happens to the ionic compounds when a precipitate forms?
What happens to the ionic compounds when a precipitate forms?
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What is the role of solubility in precipitation reactions?
What is the role of solubility in precipitation reactions?
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In the reaction between calcium chloride and potassium carbonate, what are the reactants?
In the reaction between calcium chloride and potassium carbonate, what are the reactants?
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Which of the following defines a precipitate?
Which of the following defines a precipitate?
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Which of the following correctly illustrates the equation for a combustion reaction?
Which of the following correctly illustrates the equation for a combustion reaction?
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Which metal is known to turn black or tarnished when exposed to air over time?
Which metal is known to turn black or tarnished when exposed to air over time?
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Which of the following metals turns brown or red over time due to air exposure?
Which of the following metals turns brown or red over time due to air exposure?
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What do carbon reduction reactions typically result in?
What do carbon reduction reactions typically result in?
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Why can carbon not displace metals that are more reactive than itself?
Why can carbon not displace metals that are more reactive than itself?
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What property of solids allows reactions to occur at their surfaces?
What property of solids allows reactions to occur at their surfaces?
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Which scenario would likely result in the fastest rate of reaction?
Which scenario would likely result in the fastest rate of reaction?
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What does the term 'rate of reaction' refer to?
What does the term 'rate of reaction' refer to?
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Which factor can enhance the rate of a chemical reaction?
Which factor can enhance the rate of a chemical reaction?
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What are the essential components required for combustion to occur?
What are the essential components required for combustion to occur?
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What is the product of complete combustion of fuels?
What is the product of complete combustion of fuels?
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Which of the following fuels can be classified as an organic compound?
Which of the following fuels can be classified as an organic compound?
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Which equation correctly represents the combustion of propane gas with sufficient oxygen?
Which equation correctly represents the combustion of propane gas with sufficient oxygen?
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What might incomplete combustion produce?
What might incomplete combustion produce?
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How can the rate of reaction be calculated from a graph?
How can the rate of reaction be calculated from a graph?
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Which factor does NOT influence the rate of reaction?
Which factor does NOT influence the rate of reaction?
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What is the change in grams when the initial mass is 2.2g and the final mass is 3.7g?
What is the change in grams when the initial mass is 2.2g and the final mass is 3.7g?
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What is the primary product of complete combustion of hydrocarbons?
What is the primary product of complete combustion of hydrocarbons?
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What results from incomplete combustion in terms of carbon products?
What results from incomplete combustion in terms of carbon products?
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What is the definition of an acid in terms of pH?
What is the definition of an acid in terms of pH?
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During a neutralisation reaction, what indicates that the solution has been neutralized?
During a neutralisation reaction, what indicates that the solution has been neutralized?
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What colour change would you expect as an acid is added to a base in a titration?
What colour change would you expect as an acid is added to a base in a titration?
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Which statement correctly describes a base in terms of smell and feel?
Which statement correctly describes a base in terms of smell and feel?
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What happens to the pH of a solution when excess acid is added during a neutralisation process?
What happens to the pH of a solution when excess acid is added during a neutralisation process?
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What is a common use of hydrochloric acid?
What is a common use of hydrochloric acid?
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Study Notes
Chemical Reactions - Year 10 Science Semester Two 2023
- Unit covers chemical reactions, types, rates, equations, states, predicting products, rates and changing conditions, titration procedures, assessment (SIS task, unit test)
- Starter activity from Lesson 1 includes identifying the type of compound (Cu(NO3)2), number of elements, naming the compound, and predicting the outcome if iron is added to the copper nitrate solution.
Word and Chemical Equations
- Learning intentions: writing word equations, balancing chemical compounds
- Word equations show the names of reactants and products; chemical changes are indicated with an arrow.
- Example: Magnesium + oxygen → magnesium oxide
- Example uses: MgO is magnesium oxide, KCl is potassium chloride. MgCO3 is magnesium carbonate
Conservation of Mass
- In chemical equations, mass cannot be created or destroyed
- Atoms rearrange to form new bonds and products
- Mass in reactants must equal mass in products
Combination Reactions
- Two reactants join to form one product.
- Example: magnesium + oxygen → magnesium oxide
- Your teacher will demonstrate the reaction of zinc and sulphur
Chemical Formulae
- Students need to recognize cations (positive ions) and anions (negative ions) in chemical formulae.
- A list of common cations and anions is given.
- Examples shown on the slide include: ammonium (NH4+), barium (Ba2+), calcium (Ca2+), sodium (Na+), copper (II) (Cu2+), potassium (K+), lead (II) (Pb2+), silver (Ag+), magnesium (Mg2+), bromide (Br-), carbonate (CO32-), chloride (Cl-), iodide (I-), oxide (O2-), hydroxide (OH-), sulphate (SO42-), phosphate (PO43-), nitride (N3-)
What's the formula? (Examples of reactions)
- Questions and examples on determining formulas from ions
- Method for calculating formulas explained: drop the charges from each ion, and write it down.
Naming Compounds
- General naming rules for compounds
- Two atoms of the same element: name stays the same (N₂) - nitrogen
- Two elements joined together: name ends in -ide (MgO) - magnesium oxide
- More than two elements, one of which is oxygen: name usually ends in -ate (MgCO3) - magnesium carbonate
- Ion sheet used to help name compounds by joining ion names.
Chemical Formulae Worksheet Tasks
- Tasks to complete on naming ionic formulae and creating balanced ionic formulae.
Lesson 2-3 - Learning Intentions
- Students need to learn to write and balance symbol equations for chemical reactions including state symbols.
Lesson Starter: Name these Compounds
- A list of compounds are provided for practice, including KBr, AlBr3, MgSO4, NaNO3, K2CO3, and Al(OH)3
Balanced Equations
- Reactants on the left side of the arrow, products on the right side.
- Illustrated by the example of methane + oxygen → carbon dioxide + water (CH4 + 2 O2 → CO2 + 2 H2O)
Balancing Chemical Equations
- Equations must have equal numbers of atoms on both sides.
- Example using glucose and oxygen producing carbon dioxide and water (C6H12O6 + 6O2 → 6CO2 + 6H2O) and atoms count.
- Balancing is done by adding coefficients in front of formulas, not by changing subscripts.
Worked Example
- Example steps shown to balance an equation (Na + O2 → Na2O) by adjusting coefficients until equal numbers of atoms is achieved on both sides of the equation.
Combination Reactions - Students Complete in Booklet
- Examples for students to complete in their booklet using ion table:
- Magnesium + oxygen → magnesium oxide (2Mg + O2 → 2MgO)
- Oxygen + carbon → carbon dioxide (O2 + C → CO2)
- Calcium oxide + water → calcium hydroxide (CaO + H2O → Ca(OH)2)
- Sodium + chlorine → sodium chloride (2Na + Cl2 → 2NaCl)
State Symbols
- State symbols (s, l, g, aq) must be written in brackets after the formula, indicating the physical state of substances.
- s = solid
- l = liquid
- g = gas
- aq = aqueous (dissolved in water)
Writing Equations
- Step-by-step process for writing chemical equations from word equations.
- Checking for balance of atoms and adding coefficients.
Worksheets 1-3 - Balancing Symbol Equations
- Students are instructed to complete worksheets for balancing symbol equations.
Knowledge Check (example)
- Specific example reaction provided: magnesium + hydrochloric acid.
- Tasks to complete tasks: word equation, chemical equation, and state symbols
Extra Practice
- Offers Jefferson option for difficulty levels in balancing equations games. Link to balancing equation practice videos.
- Worksheets are in portal "extension" area.
Success Criteria
- Summary of understanding level for neutralisation reactions, combustion and other reactions.
Lesson 3 - Different Types of Reactions
- Lesson starter involving balancing chemical equations.
Answers (for Lesson 3 different types of reactions)
- Balaced equations provided for the lesson starter.
Lesson 3 - Different Types of Reactions
- Learning intentions: recognizing different types of reactions, constructing reactions equations with relevant state symbols.
A World of Reactions
- Key point: matter is constantly changing in reactions but does not change the substances
- Different types of reactions happening constantly.
Types of Reactions
- Awareness of safety precautions when carrying out investigations using symbols.
- Recognizing type of reaction from knowing reactants/products
- Writing word equations for reaction types
- Constructing symbol equations (ions list included for reference)
- Balancing equations to ensure equal atoms on both sides
- Adding state symbols to equations
Types of Reactions Table
- Table indicating different chemical reactions and their types: (Combination, Decomposition, Displacement, Precipitation, Neutralisation, Combustion)
Combination
- Two elements combining to form a new compound (A + B → AB)
- Example: 4Ag + O₂ → 2Ag₂O
Decomposition
- One reactant breaking down into multiple products (AB → A + B)
Displacement
- One element replacing another in a compound (AB + C → AC + B). Explanation of single vs double displacement reactions are provided
Precipitation
- A type of displacement reaction where a solid is formed; usually with colour change
Neutralisation
- Reaction between an acid and a base producing water and salt
Combustion
- Fuel reacting with oxygen to produce carbon dioxide and water; generally involves heat/light production
Lesson 5 - Pyrophoric Iron Practical
- Instructions to carry out the decomposition reaction.
Lesson 6-7 Precipitation Reactions
- Lesson starter: Identify the types of reactions by provided equation examples
Answers (for Lesson 6-7 Precipitation Reactions)
- Balanced equations provided for the reactions.
Lesson 6-7 - Precipitation Reactions Learning Objectives
- Learning objectives includes identifying precipitation reactions, writing chemical equations for precipitation reactions including relevant state symbols .
Precipitation Reactions
- Special type of displacement reaction where one compound is a solid
- Two aqueous solutions reacting to form one soluble and one insoluble components
Precipitation Reactions
- Two aqueous solutions combine to produce a solid (precipitate)
Neutralisation
- Reaction between an acid and base producing water and salt.
- Acids and bases reacting to produce water, their taste, corrosiveness and pH are mentioned.
- Examples, like vinegar, citric juice, and hydrochloric acid are provided
pH Scale
- Universal indicator colors used to show acidity.
- A substance with low pH is a hydrogen donor, a substance with high pH is a hydrogen acceptor.
Neutralization Reactions
- Explained for acid and alkali (dissolved base).
- pH decrease when acid is added to alkali. pH of 7 indicates neutral solution. If excess acid added, produced low pH.
- Titration explained: approaching pH7 endpoint where the indicator changes color, should add one drop at a time until the neutral endpoint is achieved.
Titration
- Procedure for acid-base titrations.
- The procedure for how to perform titration and measuring the volume is explained.
Burette
- Explanation of burette measurement; scale reads downwards and small divisions equal 0.1 mL to make it accurate. Reading the bottom meniscus of solution in the burette is shown to measure volume
Teacher Demonstration – Acid-Base Reaction Steps
- Steps for performing a teacher demonstrated acid-base reactions.
Neutralization
- Post demonstration, activity sheet (on portal)
Success Criteria (Neutralisation)
- Learning outcome for neutralization reactions.
Lesson 14 - Products of Neutralisation
- Learning intent: identifying different types of reactions; determining names of salts.
Neutralisation - Naming Salts
- Instructions on how to name salts based on the acid and base.
Naming salts – click to reveal
- Instruction to complete word equations and provide the products of neutralisation reactions involving carbon containing components or not. (Example: sodium hydroxide + sulphuric acid → Sodium sulphate + water ; Calcium carbonate + hydrochloric acid → Calcium chloride + carbon dioxide + water)
Knowledge Check (neutralisation)
- Exercise to complete a word reaction, symbol equation and providing state symbols for the reaction with bicarbonate.
Success Criteria
- Learning outcome for naming salts.
Revision Activities
- Instructions to ensure booklet completeness, A3 Revision sheet completion and practice tests/revision worksheets from the portal .
Lesson 8 - Extracting Metals
- Lesson starter questions - identification of common metals based on their appearance when exposed to air
- Answers for A, B, and C) are provided (Silver, Iron, Copper)
Lesson 8 - Extracting Metals - Learning Intention
- To use reactivity to explain why different extraction techniques
Carbon Reduction
- A type of displacement reaction.
- Examples: Iron oxide + carbon → Carbon dioxide + Iron; Copper oxide + carbon → Carbon dioxide + Copper
Reactivity Series
- List of metals in a reactivity order; which metal is most reactive
Complete – Worksheet 1 – Lesson 8
- Completing the relevant worksheet in the booklet
Success Criteria
- Criteria for metals extraction.
Lesson 9-10 - Rates of Reaction
- Learning intentions: explaining reaction occurrence by collision theory; identifying factors changing reaction rates
- Understanding reaction rates, factors affecting them, and measuring them.
Rates of Reaction
- Reactions can be fast or slow, illustrated by example of an apple turning brown
- Reaction rates are important, e.g., rate of apple (surface) browning
Rates of Reaction
- Identifying where a reaction occurs
Rates of Reaction
- What does reaction rate mean?
- Measuring reaction rates
- Factors that speed up rate of reaction
- Video provided for reference
What makes a reaction happen?
- YouTube video for reference
Fruitful Collisions
- Collisions must have sufficient energy and correct orientation for a reaction
Changing rate of reaction (factors affecting rates)
- Factors: changing temperature, surface area, and concentration.
- Catalyst also increases reaction rate, but is not used up.
Rate of Reaction
- Formula: Rate = change in reaction / time
Calculating rate at regular intervals
- Calculating rates at different times during a reaction is more informative than a single average speed. (useful in practical).
Rate of Reaction Graphs
- Graph interpretation; steep gradient indicates faster reactions
Finding the Rate of Reaction from a Curved Graph
- Visual guidance for identifying rate of reaction given a curve graph
From the booklet – find the rate of reaction at 40 seconds
- Instructions for calculating reaction rate from a graph at a specific time point
Rate of Reaction Practical
- Information on a rate of reaction practical
Post Practical – Worksheet/Homework
- Instructions to complete post practical worksheet on rates of reaction (calculating the gradient of a graph).
Success Criteria
- Learning outcomes for reaction rates
Lesson 11 - Combustion reactions
- Lesson starter: calculate rates from the graph at 30 seconds
Lesson 11 - Combustion reactions - Learning Intention
- To recognize combustion reactions, and work out what products these will be
Combustion Reactions
- What combustion reactions require
Combustion Reactions
- Products of complete combustion (carbon dioxide and water vapor)
- Potential product of incomplete combustion (soot, carbon monoxide)
Incomplete combustion
- Information, including possible dangers of incomplete combustion, in homes.
Corrosion and Combustion
- Worksheet 1-Lesson 11, Worksheet 5.6 complete (corrosion and combustion).
Success Criteria (Combustion)
- Learning outcomes focused on combustion reactions and their products
Lesson 12-13 - Neutralisation Reactions - Learning Intention
- Identify neutralisation reactions and determine products.
Acids & Bases
- Properties of acids and bases (taste, corrosiveness, pH, feel)
- Acids examples: vinegar, citrus juice, hydrochloric acid, sulfuric acid
- Uses for acids: cleaning agents, fertilizers, carbonated drinks
- Bases examples: sodium hydroxide, ammonia, sodium carbonate
- Uses for bases: cleaning products, soap-making, antacids
pH Scale
- Understanding pH scale with relevant colors for universal indicator.
Neutralization Reactions
- Understanding of neutralization reactions (between acid and base/alkali).
- Solution becomes neutral when pH reaches 7.
- Titration procedure for achieving the neutral end point (adding one drop of acid at a time).
Carrying out titrations
- Procedure for acid-base titrations
Burette
- Explanation of measuring volume with burette
Teacher demonstration - Acid-Base Reaction Steps
- Detailed procedure of teacher demonstration of acid-base experiment
Neutralization Reactions
- Post demonstration, relevant activity sheet (on portal).
Success Criteria (Neutralization)
- Learning outcomes focused on neutralization reactions, and determining products.
Lesson 14 - Products of Neutralisation
- Learning intent: recognizing different types of reaction; identifying names of salts formed.
Naming Salts
- Rules for naming salts produced in neutralisation reactions.
Naming salts - click to reveal
- Instructions to help name neutralization reaction products when salts are produced, including those with carbon dioxide, using examples.
Knowledge Check
- Exercise: to write a word equation, symbol equation, balance the equation, and add state symbols and rate themselves on the task.
Success Criteria (Naming Salts)
- Learning outcomes focused on naming salts.
Revision Activities
- Instructions, materials for comprehensive review.
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Description
Test your knowledge on chemical compounding and balancing equations with this quiz. You'll explore naming rules, conservation of mass, and the conventions for writing balanced chemical equations. Ideal for students studying general chemistry.
