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Comparing guided inquiry with open inquiry strategies. Investigating exothermic and endothermic reactions for #CW9 #science #edutwitter @JctScience @pascoscientific 
Students preferred open inquiry method.

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Comparing guided inquiry with open inquiry strategies. Investigating exothermic and endothermic reactions for #CW9 #science #edutwitter @JctScience @pascoscientific 
Students preferred open inquiry method. https://t.co/ak4R0UDXQq

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Comparing guided inquiry with open inquiry strategies. Investigating exothermic and endothermic reactions for #CW9 #science #edutwitter @JctScience @pascoscientific
Students preferred open inquiry method. pic.twitter.com/ak4R0UDXQq
— Mike Kavanagh (@Mikekav66) November 29, 2019

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Comparing guided inquiry with open inquiry strategies. Investigating exothermic and endothermic reactions for #CW9 #science #edutwitter @JctScience @pascoscientific 
Students preferred open inquiry method. https://t.co/ak4R0UDXQq

# data[].attributes.attachment_link.metadata.attachment_props.original_text
Comparing guided inquiry with open inquiry strategies. Investigating exothermic and endothermic reactions for #CW9 #science #edutwitter @JctScience @pascoscientific 
Students preferred open inquiry method. https://t.co/ak4R0UDXQq

# data[].attributes.attachment_link.metadata.attachment_props.text
Comparing guided inquiry with open inquiry strategies. Investigating exothermic and endothermic reactions for #CW9 #science #edutwitter @JctScience @pascoscientific 
Students preferred open inquiry method.

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Activation energy

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Multiple choice questions appear throughout both exam papers, and at both foundation tier and higher tier. Multiple choice questions are usually asked as questions, often starting with 'what is...' or 'why...'.

You have three or four options to choose from in a multiple choice question. You must choose the number of options asked for in the question by placing ticks in boxes. Most multiple choice questions require just one tick, but a few ask for two ticks. You will not get a mark if you leave all the boxes blank, or if you put a tick in more than the required number of boxes.

Multiple choice questions often have two answers that could, at first glance, be correct. It is important to check all the answers before deciding which box to tick. It is also important to check that your chosen statement answers the question - some questions might include an option that is a correct statement, but that does not answer the question.

Sample question 1 - Foundation

The diagram shows the reaction profile of an exothermic reaction.

What does the energy value of 1370 kJ represent?
[1 mark] This question is AQA material which is reproduced by permission of AQA.

Sample question 2 - Foundation

Magnesium needs to be heated before it reacts with oxygen in the air. What conclusion can you draw from this?
[1 mark] This question is AQA material which is reproduced by permission of AQA.

Sample question 3 - Higher

Which of the following statements correctly explains why a reaction is endothermic?
[1 mark] This question has been written by a Bitesize consultant as a suggestion to the type of question that may appear in an exam paper.

Sample question 4 - Higher

Which of the following reactions releases most energy to the surroundings?
[1 mark] This question has been written by a Bitesize consultant as a suggestion to the type of question that may appear in an exam paper.

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Sample exam questions - Energy changes - AQA - Revision 1 - GCSE Chemistry (Single Science) - BBC Bitesize

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Multiple choice questions appear throughout both exam papers, and at both foundation tier and higher tier. Multiple choice questions are usually asked as questions, often starting with 'what is...' or 'why...'. You have three or four options to choose from in a multiple choice question.

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Exothermic and endothermic open inquiry

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Exothermic and endothermic guided inquiry

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Vinegar and magnesium ribbon Exothermic

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Exothermic Reaction - Magnesium in Vinegar | ThinkTac

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Vinegar and baking soda Endothermic

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Endothermic Reaction Baking Soda and Vinegar

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Activation Energy Analogy///Homemade Science with Bruce Yeany

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In this investigation, students classify chemical reactions as exothermic or endothermic. Next, students explore the relationship between an observed change in temperature and the classification of a change as chemical or physical.

Students will explore energy changes during chemical reactions, heat of reaction (ΔH), and the connection between energy changes and chemical changes.

Be sure you and the students wear properly fitting goggles.

Acetic acid (vinegar) vapors can be irritating. Work in a well-ventilated area. In the event of eye contact, flush with water. The concentration of acetic acid in this experiment does not present any significant hazards.

Calcium chloride can be an irritant to body tissues. In the event of contact, wash affected areas with water. Dispose of calcium chloride solutions according to local regulations.

Materials for Each Group

Vinegar

Baking soda

Calcium chloride

Water

Thermometer

4 small clear plastic cups

1 cup measuring cup

Measuring spoons (1 tablespoon, ½ teaspoon)

Time Required

One class period, approximately 45-50 minutes.

After students explore one example of an endothermic change and one example of an exothermic change, they are then asked to explore the connection between energy changes and chemical reactions. To do this, students may need some guidance to arrive at the idea that temperature changes may also accompany dissolving.

Students will have an easier time devising a fair test if they are well versed in the definitions of physical changes and chemical changes. Students should propose an experiment to you before they test their hypothesis. To observe a temperature change during a physical change, students should devise a procedure such as:

Add 10 mL of water to a small plastic cup and place a thermometer in the water. Record the initial temperature (Ti).

Add ½ teaspoon of calcium chloride to the water and swirl the cup. After it has stopped changing, record the final temperature (Tf).

Pre-Lab Discussion

This investigation introduces the concepts of enthalpy (heat) of ΔH in the context of exothermic and endothermic reactions. To give students a deeper grounding in the basics and reinforce basic concepts covered previously, you may wish to review the mechanics of chemical changes, how to write balanced chemical equations, and the law of conservation of energy.

Incorporating into the Curriculum

This investigation could be incorporated into a unit on chemical changes or thermochemistry.

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Exothermic, Endothermic, & Chemical Change

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In this investigation, students classify chemical reactions as exothermic or endothermic. Next, students explore the relationship between an observed change in temperature and the classification of a change as chemical or physical. Students will explore energy changes during chemical reactions, heat of reaction (ΔH), and the connection between energy changes and chemical changes.

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Activitation Energy

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Endothermic Reactions

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PowerSchool Learning : 8th Grade Science : Endothermic reactions

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Exothermic Reactions

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Energy is conserved in chemical reactions, so the total amount of in the universe at the end of a reaction is the same as it was before the reaction.

When a chemical reaction happens, energy is transferred to or from the surroundings. When energy is transferred to the surroundings, this is called an reaction, and the temperature of the surroundings increases. Examples of exothermic reactions include:

Everyday uses of exothermic reactions include self-heating cans and hand warmers.

When energy is taken in from the surroundings, this is called an reaction and the temperature of the surroundings decreases. Examples of endothermic reactions include:

Everyday uses of endothermic reactions include instant ice packs which can be used to treat sports injuries.

The slideshow describes an exothermic reaction between dilute sodium hydroxide and hydrochloric acid and an endothermic reaction between sodium carbonate and ethanoic acid.

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Exothermic and endothermic reactions - AQA - Revision 1 - GCSE Combined Science - BBC Bitesize

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Energy is conserved in chemical reactions, so the total amount of in the universe at the end of a reaction is the same as it was before the reaction. When a chemical reaction happens, energy is transferred to or from the surroundings.