Physical and Chemical Changes Quiz
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Questions and Answers

What type of reaction is represented by the equation 2HCl + Na2CO3 → CO2 + 2NaCl + H2O?

  • Single Replacement
  • Double Replacement (correct)
  • Decomposition
  • Synthesis

A combustion reaction involves a metal reacting with a non-metal to form a compound.

False (B)

What is the product of the decomposition of sodium bicarbonate (NaHCO3)?

Sodium carbonate (Na2CO3), water (H2O), and carbon dioxide (CO2)

The type of reaction where one reactant is broken down into two or more products is called _____ reaction.

<p>Decomposition</p> Signup and view all the answers

Match the chemical reaction types with their definitions:

<p>Decomposition = One reactant is broken down into two or more products. Combustion = A fuel is combined with oxygen to produce carbon dioxide and water. Synthesis = Two or more reactants combine to form one product. Single Replacement = A compound reacts with an element to form a new compound. Double Replacement = Two compounds react to form two different compounds.</p> Signup and view all the answers

What is the chemical formula for Beryllium Sulfide?

<p>BeS (B)</p> Signup and view all the answers

The cation in aluminum oxide is Al²⁺.

<p>False (B)</p> Signup and view all the answers

What is the name of the compound with the formula Ca(BrO₃)₂?

<p>Calcium Bromate</p> Signup and view all the answers

The compound formed from the oxide ion and potassium ion is K______.

<p>₂O</p> Signup and view all the answers

Match the following compounds with their corresponding names:

<p>NH₄Cl = Ammonium Chloride Ca(BrO₃)₂ = Calcium Bromate HClO₂ = Hydrogen Chlorite BeSO₄ = Beryllium Sulfate</p> Signup and view all the answers

Which ion is represented by Cu²⁺?

<p>Copper(II) ion (C)</p> Signup and view all the answers

Calcium phosphate has the formula Ca₃(PO₄)₂.

<p>True (A)</p> Signup and view all the answers

Write the chemical formula for Ammonium sulfate.

<p>(NH₄)₂SO₄</p> Signup and view all the answers

The formula for Lithium Selenide is Li______.

<p>₂Se</p> Signup and view all the answers

What happens when salt is heated in a test tube?

<p>It melts and forms a liquid. (D)</p> Signup and view all the answers

How many atoms are found in one molecule of hydrogen (H₂)?

<p>2 (C)</p> Signup and view all the answers

The chemical equation H2 + O2 → H2O is balanced.

<p>False (B)</p> Signup and view all the answers

What is the balanced equation for the reaction of hydrogen and oxygen to form water?

<p>2 H2 + 1 O2 → 2 H2O</p> Signup and view all the answers

A molecule of oxygen (O2) contains ______ atoms.

<p>2</p> Signup and view all the answers

Match the following chemical equations with their balanced forms:

<p>A. 2 Na + 1 Cl2 = A. 2 NaCl B. 2 Na + 2 H2O = B. 2 NaOH + H₂ C. 2 Mg + 1 O2 = C. 2 MgO D. 2 KClO₃ = D. 2 KCl + 3 O₂</p> Signup and view all the answers

What does a subscript indicate in a chemical formula?

<p>The number of atoms of that element in a molecule (B)</p> Signup and view all the answers

Changing the structure of a molecule is allowed when balancing a chemical equation.

<p>False (B)</p> Signup and view all the answers

What type of reaction occurs when hydrogen reacts with oxygen?

<p>Synthesis reaction</p> Signup and view all the answers

In the reaction 3 Mg + 1 P4 → ______, Mg₃P₂ is produced.

<p>Mg₃P₂</p> Signup and view all the answers

What is the purpose of coefficients in a chemical equation?

<p>Specify the number of molecules involved in the reaction (D)</p> Signup and view all the answers

Which of the following is a chemical change?

<p>Baking a cake (A)</p> Signup and view all the answers

A physical change can be reversed.

<p>True (A)</p> Signup and view all the answers

What evidence indicates that a chemical change has occurred?

<p>Formation of gas, color change, or temperature change.</p> Signup and view all the answers

The process of __________ involves a change in state from liquid to solid.

<p>freezing</p> Signup and view all the answers

Match each change with its type (Physical or Chemical):

<p>Dissolving sugar = Physical Burning toast = Chemical Frying an egg = Chemical Popping corn = Chemical</p> Signup and view all the answers

What is the evidence that indicates a physical change has occurred?

<p>Change in state (B)</p> Signup and view all the answers

Describe the change that occurs when food is chewed.

<p>It is a physical change as it breaks food into smaller pieces without changing its chemical composition.</p> Signup and view all the answers

Which formula unit represents Magnesium Chloride?

<p>MgCl2 (A)</p> Signup and view all the answers

An ionic compound forms when atoms share electrons.

<p>False (B)</p> Signup and view all the answers

What is the Lewis structure for Calcium in the formation of Calcium Iodide?

<p>[Ca] ^2+</p> Signup and view all the answers

The formula unit for Beryllium Nitride is _______.

<p>Be₃N₂</p> Signup and view all the answers

Match the following compounds with their corresponding formula units:

<p>Magnesium Chloride = MgCl2 Aluminum Fluoride = AlF3 Calcium Phosphate = Ca3P2 Rubidium Oxide = Rb2O</p> Signup and view all the answers

Which of the following is the correct Lewis structure for Potassium?

<p>[K] ^+ (A)</p> Signup and view all the answers

In a formation of an ionic compound, both atoms lose electrons.

<p>False (B)</p> Signup and view all the answers

Identify the compound formed between Magnesium and Sulfur.

<p>Magnesium Sulfide</p> Signup and view all the answers

The formula unit for Strontium Fluoride is _______.

<p>SrF₂</p> Signup and view all the answers

Flashcards

Physical Change

A change in the appearance or form of a substance, but not its chemical composition. The change is usually reversible.

Chemical Change

A change where a new substance is formed with different properties. This change is typically irreversible.

Evidence of a Chemical Change

Indicators that a chemical change has occurred, such as the formation of bubbles, a change in color, a change in temperature, or the release of a gas.

Evidence of a Physical Change

Indicators that a physical change has occurred, such as a change in state (solid, liquid, gas), a change in shape, or a change in size.

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Reversible Change

A change that can be reversed back to its original state.

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Irreversible Change

A change that is permanent and cannot be reversed back to its original state.

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Examples of Physical Changes

Examples of physical changes include melting ice, freezing water, cutting paper, dissolving sugar in water, boiling water, and stretching a rubber band.

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Ionic Bonding

A type of chemical bond formed when one atom gives up one or more electrons to another atom, resulting in oppositely charged ions that attract each other.

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Lewis Structure

A diagram that shows the valence electrons of an atom, using dots to represent the electrons, and helps visualize how atoms bond.

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Formula Unit

The smallest repeating unit in an ionic compound, representing the ratio of ions in the compound.

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Cation

A positively charged ion formed when an atom loses one or more electrons.

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Anion

A negatively charged ion formed when an atom gains one or more electrons.

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Magnesium Chloride (MgCl₂)

An ionic compound formed by the transfer of two electrons from a magnesium (Mg) atom to two chlorine (Cl) atoms, resulting in the formation of Mg²⁺ and Cl⁻ ions.

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Magnesium Sulfide (MgS)

An ionic compound formed by the transfer of two electrons from a magnesium (Mg) atom to a sulfur (S) atom, resulting in Mg²⁺ and S²⁻ ions.

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Potassium Fluoride (KF)

An ionic compound formed by the transfer of one electron from a potassium (K) atom to a fluorine (F) atom, resulting in K⁺ and F⁻ ions.

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Potassium Oxide (K₂O)

An ionic compound formed by the transfer of one electron from two potassium (K) atoms to one oxygen (O) atom, resulting in K⁺ and O²⁻ ions.

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Ionic compound formula

Represents the simplest ratio of ions in a compound, ensuring electrical neutrality.

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Lewis Structure of BeS

Be (2 valence electrons) loses 2 electrons to form Be²⁺. S (6 valence electrons) gains 2 electrons to form S²⁻. The ionic bond forms due to electrostatic attraction between oppositely charged ions.

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Aluminum Oxide Formula

Al³⁺ (3+ charge) and O²⁻ (2- charge) combine to form Al₂O₃, balancing the charges.

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Ionic Compound Naming

Name the cation first, followed by the anion, using roman numerals for transition metal cations if needed.

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Polyatomic Ions

Groups of atoms with a net charge, acting as a single unit in ionic compounds.

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Ammonium Chloride Formula

NH₄⁺ (ammonium ion) combines with Cl⁻ (chloride ion) to form NH₄Cl, simple 1:1 ratio.

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Sodium Chromate Formula

Na⁺ (sodium ion) combines with CrO₄²⁻ (chromate ion) to form Na₂CrO₄, balancing charges.

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Ionic Compound Properties

High melting points, solubility in water, good electrical conductivity when dissolved or melted.

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Observation 1 - Salt under microscope

Salt crystals reveal a regular, repeating structure under the microscope, demonstrating their ionic nature.

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Observation 2 - Heating Salt

Heating salt causes it to melt and potentially decompose, demonstrating its high melting point and potential for chemical change.

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What is a chemical reaction?

A process where atoms rearrange to form new substances with different properties.

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What are the four main types of chemical reactions?

Synthesis, decomposition, single replacement, and double replacement.

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What is a synthesis reaction?

Two or more reactants combine to form a single product.

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What is a decomposition reaction?

One reactant breaks down into two or more products.

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What is a single replacement reaction?

One element replaces another element in a compound.

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What is a coefficient in a chemical equation?

A number placed in front of a chemical formula in a balanced chemical equation. It indicates the relative number of moles of each reactant and product involved in the reaction.

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What is a subscript in a chemical equation?

A small number written below and to the right of an element's symbol in a chemical formula. It indicates the number of atoms of that element present in a molecule.

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What does it mean for a chemical equation to be balanced?

A chemical equation is balanced when the number of atoms of each element on the reactants side of the equation equals the number of atoms of that element on the products side.

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How do you balance a chemical equation?

You balance a chemical equation by adjusting the coefficients in front of each chemical formula. This changes the number of molecules involved in the reaction without changing the chemical formulas themselves.

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What is a reactant?

A substance that is consumed during a chemical reaction. They are usually written on the left side of a chemical equation.

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What is a product?

A substance formed as a result of a chemical reaction. They are usually written on the right side of a chemical equation.

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Why are chemical equations balanced?

Balancing chemical equations ensures that the law of conservation of mass is followed. This law states that mass cannot be created or destroyed in a chemical reaction, only rearranged.

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What is an element?

A substance consisting of only one type of atom.

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Study Notes

Physical and Chemical Changes

  • Starter Activity: Classify reactions as physical or chemical changes.
  • Physical Change: Dissolving sugar, melting chocolate, boiling water, and frying an egg.
  • Chemical Change: Baking a cake, burning toast, freezing milk, popping corn.
  • Lab Investigation: Physical and Chemical Change Stations.
  • Station 1 (Sugar and Water): Physical change, can be reversed.
  • Station 2 (Baking Soda and Vinegar): Chemical change, bubble formation.
  • Station 3 (Video of Fireworks): Chemical change, explosion.
  • Station 4 (HCl and NaOH): Chemical change, pH changes in state.
  • Station 5 (Ice Cream Melting): Physical change.
  • Station 6 (Oil and Water): Physical change, can be separated.

Homework

  • Scenarios: Analyze scenarios to determine whether it is a physical or chemical change.
  • Evidence: Identify evidence such as change in state, smoke, appearance changes, or smells.
  • Examples: Students should distinguish chemical (irreversible changes) from physical changes (reversible changes).

Introduction to Ionic Bonding

  • Ionic Bond Formation: Occurs when one atom donates its outermost electrons to another.
  • Attraction: The resulting ions are attracted due to their opposite charges.
  • Ionic Compounds: Composed of positively-charged metal ions (cations) and negatively-charged non-metal ions (anions).

Drawing Lewis Structures

  • Procedure: Draw Lewis structures for various combinations of elements.

Writing Chemical Formulas for Ionic Compounds

  • Main Group Metals: Write formulas for ionic compounds involving main group metals
  • Examples: Lithium bromide, magnesium fluoride, potassium oxide, calcium sulfide.

Properties of Ionic Compounds

  • Observation 1: Examine salt under a microscope to observe structure.
  • Challenge: Predict ionic arrangement based on observations and understanding of ionic bonding.
  • Observation 2: Observing changes when heating a salt.
  • Observation 3: Experimental setup to observe the conductivity of salt when mixed.
  • Observation 4: Adding water to salt
  • Ionic Compounds conduct electricity when melted or dissolved in water.
  • Ionic Compounds have high melting and boiling points.

Types of Chemical Reactions

  • Synthesis: Two or more substances combine to form a single product.
  • Decomposition: One substance breaks down to form two or more simpler substances.
  • Single Replacement: One element replaces another element in a compound.
  • Double Replacement: Positive ions in two compounds exchange places.
  • Combustion: A rapid chemical reaction that produces heat and light.
  • Examples of common types of chemical reactions: Combination, Decomposition, Single Replacement, Double Replacement, Combustion.

Balancing Chemical Equations

  • Importance: Both sides of the equation must have the same number of each element.
  • Coefficients: Use these to balance the number of atoms on each side.

Solubility Rules

  • Salts: Ionic compounds (excluding those containing only oxygen and hydrogen).
  • Solubility: Some salts are soluble in water, others partially soluble, and still others insoluble.
  • Precipitation Reactions: Reactions that produce an insoluble salt (precipitate).
  • States: Indicate the state of matter for each chemical (solid, liquid, or gas) in an equation with (s), (l), or (g).

Molecular Equation and Ionic Equations

  • Molecular Equations: Show all species as neutral molecules.
  • Complete Ionic Equations: Separate soluble ionic compounds into their respective ions.
  • Net Ionic Equations: Omit spectator ions; these are ions that appear on both the reactant side and the product side that cancel out to zero.
  • Examples: Reactions of ionic compounds and their net ionic equations.

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Description

Test your knowledge on physical and chemical changes through various activities and examples. Analyze different scenarios and identify evidence that distinguishes between the two types of changes. This quiz will enhance your understanding of how substances interact and transform.

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