FridayFun: 8 Holt Chemical Reactions Overview

A chemical reaction where two or more reactants combine to form a single product.

The chemical formula for the product formed from potassium reacting with chlorine is KCl.

The correct balanced equation is 2K + Cl2 → 2KCl.

In the product KCl, the potassium ion has a charge of 1+.

In KCl, the chloride ion has a charge of 1-.

The coefficient '2' in 2KCl indicates two units of potassium chloride are formed.

A reaction that involves only one reactant breaking down into two or more products.

Indicates that a substance is dissolved in water.

Represents that a substance is in a gaseous state.

The double arrow ⇋ shows that a reaction can proceed in both forward and reverse directions.

Represents a liquid substance in a chemical equation.

A catalyst speeds up the reaction rate without being consumed in the process.

Represents the pressure at which the chemical reaction occurs.

Indicates that a substance is a solid in a chemical equation.

This reaction proceeds in both forward and reverse directions, requiring specific conditions.

Change in color can suggest a chemical change but is not direct evidence of it.

Conducting a chemical analysis to confirm a new substance has formed is the most conclusive proof.

Boiling water is a physical change where gas forms without a new substance.

Indirect evidence of a chemical change can be observed, such as the operation of a battery.

Gas formation often indicates a strong chemical change but requires further proof.

Energy is a reactant that needs to be absorbed for the decomposition reaction to occur.

Molecules and atoms of reactants must come into contact for a chemical reaction to proceed.

Potassium chlorate and phosphorus are involved in igniting a safety match.

Reactants are physically separated, preventing ignition under normal conditions.

To show the chemical formulas and relative amounts of all reactants and products.

A match igniting when rubbed against a striking surface exemplifies that reactants must interact.

Some reactions, like dinitrogen tetroxide decomposition, require energy as a reactant.

Physical contact between reactants facilitates interactions and rearrangements of molecules and atoms.

The correct word equation is potassium chlorate → potassium chloride + oxygen.

The unbalanced formula equation for silver and sulfur forming silver sulfide is Ag + S8 → Ag2S.

Coefficients in front of formulas can be adjusted to balance chemical equations.

The balanced equation for forming water is 2H2 + O2 → 2H2O.

The student's error in writing Fe(s) + Cl3(g) → FeCl3(s) is that chlorine should be Cl2 instead of Cl3.

The balanced equation for iron(III) oxide and carbon monoxide producing iron and carbon dioxide is Fe2O3 + 3CO → 2Fe + 3CO2.

The coefficient of hydrogen in Fe2O3 + 3H2 → 2Fe + H2O is 3.

When balancing a chemical equation, coefficients in front of formulas can be adjusted.

The first step in balancing the equation Fe2O3 + H2 -> Fe + H2O is to balance the iron atoms.

If 4 hydrogen atoms are on the reactant side and 6 on the product side, add a coefficient of 1.5 before the reactant hydrogen to balance it.

In a balanced chemical equation, the number of atoms of each element must be the same on both sides.

There are 3 oxygen atoms on the reactant side of the equation Fe2O3 + 3H2 -> 2Fe + 3H2O.

The coefficient required to balance hydrogen atoms in the combustion of propane C3H8 + O2 -> CO2 + H2O is 4 before H2O.

In balancing Ca2Si + Cl2 -> CaCl2 + SiCl4, the first step is balancing the calcium atoms.

An equation where the number of atoms differ on each side.

Making the number of atoms equal on both sides without changing formulas.

Numbers placed before formulas to indicate amount of molecules.

H2O has 2 hydrogen atoms and 1 oxygen atom per molecule.

Inferring reactants or products when not all details are given.

Identify reactants/products, count atoms, adjust coefficients.

The process of tallying all atoms in a chemical equation.

2H2O indicates the presence of 4 hydrogen and 2 oxygen atoms.

A representation of a chemical reaction using the names of reactants and products.

An equation that uses chemical formulas and symbols to represent a chemical reaction.

An equation that uses chemical symbols to represent the reactants and products in a reaction.

The substances that undergo a chemical change in a reaction, written on the left side of the arrow.

The new substances formed in a chemical reaction, written on the right side of the arrow.

The principle stating that mass is neither created nor destroyed in a chemical reaction; atoms are conserved.

Occurs when three different elements combine in a reaction.

Products are usually two elements when a binary compound reacts.

Synthesis combines reactants; decomposition breaks them down.

Produces carbon dioxide and water when hydrocarbons burn completely.

A list that predicts the reactivity of elements in reactions.

Elements at the top of the activity series are more reactive.

Use prior knowledge to foresee if a reaction will happen.

A method using odd/even numbers to balance chemical equations.

Substances that undergo change in a chemical reaction.

Substances formed as a result of a chemical reaction.

The process to ensure atoms are equal in reactants and products.

Numbers placed before compounds to show how many molecules are involved.

A product formed when combustion or certain reactions occur with hydrogen.

A reaction where two compounds exchange ions, forming new compounds.

One product must be a solid, gas, or molecular compound like water.

A simpler representation highlighting only the ions involved in a reaction.

HCl and NaOH produce water (HOH) and NaCl when mixed.

A solution where a substance is dissolved in water.

The formation of a solid that separates from a liquid solution during a reaction.

A compound consisting of three elements that splits into its constituent elements.

A reaction where a compound made of two elements breaks into those two elements.

The reaction produces Hg(NO3)2 and AgCl from HgCl2 and AgNO3.

Aluminum reacts with mercury acetate to form Al(CH3COO)3 and mercury.

Calcium hydroxide reacts with phosphoric acid to produce calcium phosphate and water.

Balancing equations ensures mass conservation during a reaction.

A balanced equation has equal numbers of each type of atom on both sides.

Coefficients are adjusted to balance equations, not subscripts.