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Questions and Answers
Which type of chemical reaction involves one element replacing another element in a compound?
Which type of chemical reaction involves one element replacing another element in a compound?
- Synthesis
- Decomposition
- Single replacement (correct)
- Double replacement
Balancing chemical equations ensures that the number of atoms of each element is the same on both sides of the equation, adhering to the law of conservation of mass.
Balancing chemical equations ensures that the number of atoms of each element is the same on both sides of the equation, adhering to the law of conservation of mass.
True (A)
What type of reaction is represented by the general equation $A + B \rightarrow AB$?
What type of reaction is represented by the general equation $A + B \rightarrow AB$?
Synthesis
A reaction in which a substance combines with oxygen and releases energy in the form of heat and light is known as ______.
A reaction in which a substance combines with oxygen and releases energy in the form of heat and light is known as ______.
Match the following reaction types with their correct descriptions:
Match the following reaction types with their correct descriptions:
Using the activity series, which metal will displace copper ($Cu$) from a solution of copper(II) sulfate ($CuSO_4$)?
Using the activity series, which metal will displace copper ($Cu$) from a solution of copper(II) sulfate ($CuSO_4$)?
A precipitate is formed when all products of a double replacement reaction are aqueous, according to solubility rules.
A precipitate is formed when all products of a double replacement reaction are aqueous, according to solubility rules.
In a balanced chemical equation, what do coefficients represent?
In a balanced chemical equation, what do coefficients represent?
The symbol '(aq)' after a chemical formula in a chemical equation indicates that the substance is ______.
The symbol '(aq)' after a chemical formula in a chemical equation indicates that the substance is ______.
Match each reactant with its product in the following single replacement reactions:
Match each reactant with its product in the following single replacement reactions:
Which set of coefficients correctly balances the following equation: $C_2H_6 + O_2 \rightarrow CO_2 + H_2O$?
Which set of coefficients correctly balances the following equation: $C_2H_6 + O_2 \rightarrow CO_2 + H_2O$?
The activity series is used to predict the products of decomposition reactions.
The activity series is used to predict the products of decomposition reactions.
Provide the chemical formula for iron(II) sulfide.
Provide the chemical formula for iron(II) sulfide.
In the reaction $BaCl_2(aq) + Na_2SO_4(aq) \rightarrow ______ + 2NaCl(aq)$, the missing product is $BaSO_4(s)$.
In the reaction $BaCl_2(aq) + Na_2SO_4(aq) \rightarrow ______ + 2NaCl(aq)$, the missing product is $BaSO_4(s)$.
Match the following chemical equations with their reaction types:
Match the following chemical equations with their reaction types:
Given the reaction: Aluminum + Oxygen -> Aluminum Oxide. What is the correctly balanced equation?
Given the reaction: Aluminum + Oxygen -> Aluminum Oxide. What is the correctly balanced equation?
In the reaction of acetic acid and copper, hydrogen gas will be produced.
In the reaction of acetic acid and copper, hydrogen gas will be produced.
What are the products of the following reaction: silver nitrate + sodium bromide?
What are the products of the following reaction: silver nitrate + sodium bromide?
In a chemical equation, the substances on the left side of the arrow are called ______.
In a chemical equation, the substances on the left side of the arrow are called ______.
Match the state symbols with their meaning in a chemical equation:
Match the state symbols with their meaning in a chemical equation:
Flashcards
Combination Reaction
Combination Reaction
A reaction where two or more substances combine to form a single product.
Decomposition Reaction
Decomposition Reaction
A reaction where a single compound breaks down into two or more simpler substances.
Combustion Reaction
Combustion Reaction
A reaction involving rapid oxidation that produces heat and light.
Single Replacement Reaction
Single Replacement Reaction
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Double Replacement Reaction
Double Replacement Reaction
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Activity Series
Activity Series
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Solubility Chart
Solubility Chart
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Chemical Equation
Chemical Equation
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Coefficients
Coefficients
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State Symbols
State Symbols
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Study Notes
- Know the different reaction types and how to recognize them.
- Be able to place coefficients to balance given equations.
- Be able to write word equations into balanced chemical equations, including state symbols.
- Know how to use the activity series and a solubility chart.
- Be able to predict products and complete reactions, and identify when no reaction will occur.
Balancing Chemical Equations
- Classified as combination, decomposition, combustion, single replacement, or double replacement.
- Balance the equations by ensuring the number of atoms for each element is the same on both sides.
- Word equations must be correctly translated into chemical formulas, including proper state symbols such as (s) for solid, (l) for liquid, (g) for gas, and (aq) for aqueous (dissolved in water).
Predicting Products
- Requires knowing the reactants, predicting the products based on reaction type and applying the rules of chemical formulas and nomenclature.
- After predicting the products, the equation must be balanced to satisfy the law of conservation of mass.
- Reactions may be combination (synthesis), decomposition, single replacement, double replacement (metathesis), or combustion reactions.
Example Reactions
- Iron reacting with sulfur to form iron (II) sulfide, silver nitrate reacting with sodium bromide to form sodium nitrate and silver bromide, and potassium chlorate (when heated) decomposing into potassium chloride and oxygen.
- Additional reactions include mercury (II) oxide (when heated) decomposing into mercury and oxygen, aluminum reacting with oxygen to form aluminum oxide, and iron (III) chloride reacting with ammonium hydroxide to form iron (III) hydroxide and ammonium chloride.
- More examples are iron (III) oxide reacting with carbon to form iron and carbon monoxide, and aluminum reacting with sulfuric acid to form aluminum sulfate and hydrogen.
- Predict the products for reactions like magnesium bromide with chlorine, aluminum with iron (III) oxide, silver nitrate with zinc chloride, zinc with hydrochloric acid, sulfuric acid with sodium hydroxide, sodium with hydrogen, and acetic acid with copper.
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