Chemistry Yr 10 2025

Atoms and Matter

In Our Classroom

• Classroom Expectations:

  • Try our best.

  • Respect each other.

  • Are a team.

  • Learn from mistakes.

  • Celebrate each other's success.

  • Create.

Google Classroom

• Class code provided to join class.

Learning Intentions

• Recall that all matter is composed of atoms and has mass.

• Classify compounds into groups based on common chemical characteristics.

Success Criteria

• Explain what a compound is.

• Classify compounds into groups based on common chemical characteristics.

SMART Goals

• Specific: What do you want to do?

• Measurable: How will you know when you've reached it?

• Achievable: Is it in your power to accomplish it?

• Realistic: Can you realistically achieve it?

• Timely: When exactly do you want to accomplish it?

Glossary

• Atom: The smallest possible particle of an element.
  *Example: Carbon atom (6 protons + 6 neutrons).

• Compound: A substance made up of two or more types of atoms bonded together in fixed ratios. *Example: Water (H₂O).

• Element: A pure substance made up of only one type of atom. *Examples: Helium (He), Oxygen (O₂).

• Electron

• Proton

• Neutron

Isotopes

• Atoms of the same element with the same number of protons but different numbers of neutrons.
  *Examples: Hydrogen-1, Hydrogen-2 (Deuterium), Hydrogen-3 (Tritium).

Mass

• The amount of matter in an object.

Matter

• Physical substance that has mass and takes up space.

Formula for Sulfuric Acid

• $H₂SO₄$: 2 Hydrogen atoms, 1 Sulfur atom, 4 Oxygen atoms.

Matter Composition

• Matter is made up of different types of atoms.

• Atoms of identical size, mass, and similar properties are called elements.

  • Listed in the periodic table of elements.

• Atoms consist of a positive nucleus containing protons and neutrons surrounded by electrons orbiting the nucleus.

• The mass of the atom is concentrated inside its nucleus and is the sum of the mass of the protons and neutrons.

Atom Components

• Proton (+): positive charge, mass of 1 atomic mass unit (amu), located in the nucleus.

• Neutron: no charge (neutral), mass of 1 amu, located in the nucleus.

• Electron (-): negative charge, mass of 0 amu, located in orbitals.

Literacy - Subject-Verb Agreement

• All things in the universe are made from atoms.

• An atom is a very tiny piece of matter.

• When scientists look through a regular microscope, it is impossible to see an atom.

• Millions of atoms fit into the space of the full stop at the end of this sentence.

• All the objects we touch, see and feel, and even the air and our own bodies consist of atoms.

Pure Substances

• Every element and every pure compound is a different and distinct substance.

• Seawater is a mixture of substances rather than a substance itself.

Elements vs. Compounds

• Elements:

  • Pure substances that contain the same type of atoms.

  • Example: Sodium contains only sodium atoms, each with 11 protons, 11 electrons and 12 neutrons.

  • Listed in the periodic table of elements.

  • Most are formed naturally, but some (technetium, californium, neptunium) are made by scientists in nuclear reactors or particle accelerators.

• Compounds:

  • Chemical substance made up of atoms of two or more elements held together in fixed ratios by chemical bonds.
    *Examples: Water ($H₂O$), carbon dioxide ($CO₂$), glucose ($C₆H₁₂O₆$), and salt ($NaCl$).

Elements vs Compound (Visual)

• Elements: Contains only one kind of atom (e.g., Helium - He, Oxygen - $O₂$)

• Compounds: Contains two or more kinds of atoms (e.g., Water - $H₂O$)

Elements vs Compound (Capital Letters)

• Elements:

  • First letter of element symbol is always capitalized

  • Only have one capitalized letter
    *Examples: Fe, $O₂$, K

• Compounds

  • Combination of elements

  • Recognizable by how many capital letters (2 or more)
    *Examples: $H₂O$, $NaCl$, $Ba(OH)₂$

Examples of compounds/elements

• Water: $H₂O$ (2 Hydrogen, 1 Oxygen)

• Carbon Dioxide: 1 Carbon, 2 Oxygen

• Glucose: $C₆H₁₂O₆$ (6 Carbon, 12 Hydrogen, 6 Oxygen)

• Salt: $NaCl$

• Fool's Gold: 1 Iron, 2 Sulfur

• Baking Soda: $NaHCO₃$

• Silicate: $SiO₄$

• Dioxide: 2 Oxygen

Matter Flowchart

• Matter can be either a pure substance or a mixture.

• Pure substances can be elements or compounds.

• Mixtures can be heterogeneous or homogeneous (solution).

• Distinction depends on whether it can be physically separated/chemically decomposed and whether the composition is uniform.

Mass vs. Weight

• Mass: the amount of matter in an object. Constant; can only be changed by physically altering the object.

• Weight: a measure of gravity's pull on an object.

Isotopes

• Different forms of the same element with different numbers of neutrons in the nuclei of their atoms.

• Different mass numbers and some different properties (e.g., radioactivity).

• Same atomic number and occupy the same space on the periodic table.

• Hydrogen isotopes: Protium, Deuterium, Tritium.

Worksheet 14.1 Atoms and Matter

• Worksheet and questions regarding atoms and matter

Atoms & Molecules

• An atom is a tiny particle made up of even tinier particles.

• In the center of each atom, there is a nucleus.

• Inside the nucleus, there are protons and neutrons.

• Electrons whiz around the nucleus, like planets orbiting the sun.

• There are even smaller particles inside the nucleus.

• A neutron is made up of tiny particles called quarks held together with other particles called gluons.

Challenge Questions

• Explain what matter is.

• Describe the difference between an element and a compound.

• Identify two elements and two compounds.

• Identify the different parts of an atom.

• Draw the atomic structure of an atom and label the nucleus, protons, electron and neutrons.

• What is an isotope, and how do isotopes of the same element differ?

• Identify the isotopes of hydrogen.

• State the number of protons, electrons and neutrons in the carbon isotopes C-12, C-13 and C-14.

• Research to find out why scientists made technetium.

Bonds Between Atoms

Learning Intentions

• Classify compounds into groups based on their bonding type.

Glossary

• Covalent Bond: A bond in which two atoms share one or more pairs of electrons.

• Ionic Bond: A bond in which some atoms gain and some lose electrons, becoming ions.

• Molecule: The smallest unit of a covalent compound that can take part in a chemical reaction.

• Lattice: An interlaced structure or pattern.

• Metallic Bond: A bond in which free electrons move around metal ions.

• Valency: An element's power to combine with other atoms.

• Ion: A charged atom. Cation (+) has less electrons than protons. Anion (-) has more electrons than protons.

Elements, Molecules and Compounds Classification

• Atomic: Atoms of an element, e.g., helium (He).

• Molecular (Element): Molecules of an element, e.g., oxygen (O₂).

• Molecular (Compound): Molecules of a compound, e.g., water (H₂O).

• Ionic: Lattice of a compound, e.g., salt (NaCl).

Elements, Compounds, Atoms and Molecules

• Atoms are the simplest form of matter (single particle).

• Molecules are made up of two or more atoms joined together by chemical bonds.

• Elements are substances made up of one kind of atom only.

• Compounds are substances made up of at least two different kinds of atoms joined together by chemical bonds.

Explain the Meanings

• Explain the meanings of the terms molecule and compound and use examples to show the difference between them.

Atoms and Bonding

• All matter is made up of atoms.

• In order for atoms to stick together to make a compound, they need to form bonds with other atoms.

• These bonds are formed by the atoms' electrons, and there are three different types of bonds that can form.

Covalent Bonding

• Occurs between non-metal atoms.

• The number of bonds depends on how many electrons are in the outer shell.

• Chlorine is only short of one electron so can only form one covalent bond.

• Oxygen is short of two electrons. It can bond with two hydrogen atoms to become water.
  Interactive simulation explaining covalent bonds

Covalent Compounds

• Electrons in the outermost shell, called the valence shell, move around to bond atoms together.

• When two or more non-metallic atoms bond, they share electrons in their valence shells, producing a molecule.

• Few non-metallic elements (helium) naturally occur as single atoms; most appear as molecules containing two or more atoms.

Covalent Bond Formation

• Unpaired valence electrons shared between two nonmetal atoms or a nonmetal and a metalloid to form a covalent molecule.

Covalent molecules and their formulas

• Ammonia: $NH₃$

• Carbon Dioxide: $CO₂$

• Chlorine: $Cl₂$

• Glucose: $C₆H₁₂O₆$

• Hydrogen: $H₂$

Ionic Bonding

• An electrically charged atom is called an ion.

• Ionic bonds are very strong.

• Ions are formed when electrons are added or removed from the outer shell.

• Ionic compounds have high melting and boiling points.
  Interactive simulation explaining ionic bonds

Ionic Compounds

• Some atoms gain or lose electrons when they bond, creating ions.

• Atoms lose electrons: positively charged ions.

• Atoms gain electrons: negatively charged ions.

• Metal atom bonds with a non-metal atom, the metal loses electrons and the non-metal gains them, creating an ionic compound.

• Ions arrange themselves into a lattice rather than individual molecules.

• lonic bonds in an ionic compound are very strong due to electrostatic attraction.

Ionic Bond Formation

• Metal atom transfers electrons to a nonmetal atom, creating an ionic molecule.

Ions

• Atoms lose electrons: positively charged ions (e.g., $Na^+$

• Atoms gain electrons: negatively charged ions (e.g., $Cl^−$).

• Gaining or losing more than one electron is indicated by a number in front of the + or - (e.g., $O^{2−}$ or $Hg^{2+}$).

Metallic Bonding

• Metal atoms bond together and create giant lattice structures.

• Electrons de-localise into a sea that moves through the lattice.

• Metals are good conductors of electricity and heat.

• Metals are very strong and malleable.

Metalic Bonds

• All of the metal atoms lose electrons, rather than gain or share them.

• Lost electrons form a 'sea' of free electrons that surrounds the positive metal ions.

• Metal ions are closely packed together and are held in place by their attraction to the sea of electrons.

• Metallic bonds tend to be weaker than ionic bonds, but the large numbers of free electrons make metallic compounds good conductors of heat and electricity.

Bonding in Metals

• Free electrons move easily around metal ions in a metal.

Worksheet 14.2: Bonds between atoms

Ionic Compounds

• Ionic compound questions and worksheets. Includes covalent bonding diagram for chlorine, hydrogen, water; and movement electron diagrams for Lithium Fluorine, and Sodium Chloride

Key Concepts

• How are covalent compounds formed?

• How are ionic compounds formed?

• How are metals formed?

Challenge Questions

• Explain the difference between elements and compounds.

• Explain what a compound is.

• Name three compounds.

• Draw a table that shows three molecules found in air and write the formula of each next to them.

• How are ions formed?

• Glucose has the formula $C₆H₁₂O₆$. How many atoms of carbon, hydrogen and oxygen are there in one molecule of glucose?

• How are covalent bonds formed?

• Which are stronger - ionic bonds or covalent bonds?

• Do metals form positive or negative ions when they lose electrons?

• Compare and contrast ionic, metallic and covalent bonds.

Identifying Chemical Compounds

Learning Intentions

• Identify a range of compounds using their common names and chemical formulae.

Success Criteria

• Identify a range of compounds using their names and chemical formulas.

• Use rules to name chemical compounds.

Glossary

• Chemical formula: Chemical symbols showing the ratio of elements to one another.

• Polyatomic ion: Two or more ions bonded together and acting as a single charged unit.
  *Example: Hydrogen

• Prefix: A word or number placed before another word.
  *Example: Oxygen, Nitrogen, Carbon

Chemical Formula

• Shorthand way of writing the name of an element or compound that tells you the number and type of atoms in a compound.

• Used to write chemical equations that model reactions.

Rules for Naming Covalent Compounds

• Determine whether the compound is ionic or covalent.

  • If it contains a metal, it is ionic.

  • If it contains two or more non-metals, it is covalent.

• Name the element that comes first in the formula.

• Name the second element, making sure it ends with 'ide'
  *Example: carbon fluoride (CF), hydrogen chloride (HCl).

• If there is more than one of each type of atom in the formula, add a prefix to the element's name
  *Example: phosphorus pentoxide ($P2O5$), carbon dioxide ($CO₂$).

• Water ($H₂O$)'s scientific name is dihydrogen monoxide.

lonic Compounds

• The metal atom in the compound is always named first.

• If it has more than two elements, there is a group of elements bonded together into a polyatomic ion. The metal is named first, then the polyatomic ion, which has its own name
  *Example: sodium sulfate ($Na₂SO₄$), copper hydroxide ($Cu(OH)₂$).

Common Polyatomic Ions

• Ammonium ($NH₄$)

• Carbonate ($CO₃^{2-}$

• Hydroxide ($OH^−$

• Nitrate ($NO₃$)

• Nitrite ($NO₂$)

• Phosphate ($PO₄^{3-}$

• Sulfate ($SO₄^{2-}$

• Hydrogen sulfate ($HSO₄$)

• Sulfite ($SO₃^{2-}$

Swap-and-Drop Method

• Used to determine the chemical formula for an ionic compound.

  • Step 1: Write the ions (positive ion on the left, negative ion on the right).

  • Step 2: Swap the charge number on the left-hand side to become a subscript on the right-hand side.

  • Step 3: Swap the charge number on the right-hand side to become a subscript on the left-hand side.

  • Step 4: Simplify, using brackets and the lowest common factor.

• Example: Calcium carbonate ($CaCO_3$)

Transition Metals

• Some metals have different ionic forms, and Roman numerals are added after the name of the metal to show the ionic form.

• Example, iron can exist as $Fe^{2+}$ and $Fe^{3+}$ which form different compounds: iron(II) chloride is $FeCl<em>2$, while iron(III) chloride is $FeCl</em>3$.

Key Concepts

• Why do scientists follow rules when naming compounds?

• What is a polyatomic ion?

Worksheet: Identifying Chemical Compounds

Covalent Compounds: naming with naming conventions - Example:

• $SiF$ a. $N₂S₃$ b. $HBr$ c. $Br₂$ d. $CO$ e. $P₄$ f. $NH₃$ g. $CH$

Ionic compounds: naming with naming conventions - Example:

• $LiF$ a. $PbS$ b. $CuSO₄$ c. $NaCl$ d. $Fe₂O₃$ e. $H₂SO₄$ f. $NaOH$ g. $CaCO₃$

Questions

• Explain why chemical formulas are used instead of chemical names.

• When naming a compound, which element should you write first?

• Explain what a polyatomic ion is.

Acids and Bases

Learning Intentions

• Classify compounds into groups based on common chemical characteristics.

Success Criteria

• Explain what acids and bases are and give examples of each.

• Describe the pH scale, including the range for acids and bases.

Glossary

• Caustic: Able to burn or corrode organic tissue through chemical action.

• Concentration: The amount of a substance in a volume of solution.

• Corrosive: Highly reactive and damaging or destructive to another substance.

• Neutralise: To make something chemically neutral.

• pH: A figure expressing the acidity or alkalinity of a solution.

The pH Scale

• Goes from 1 to 14, where each number differs by a factor of 10.
  *For example, pH 2 is ten times more acidic than pH 3.

Acids and Bases

• Chemical compounds can be grouped according to their common characteristics.

• Two of the most common groups are acids and bases.

• They are used in cleaning products, swimming pools and kitchens.

• Many of the foods we eat are either acidic or basic, and acids and bases help digest food.

Acids and Alkalis Key Facts

• Bases neutralise acids, and if a base dissolves in water then the solution is an alkali.

• Weak acids are safe to consume, but stronger acids can be harmful, irritant or corrosive.

• Acids have a pH of less than 7 and alkalis have a pH greater than 7.

• Universal Indicator solution can test any liquid to see how acidic or alkaline it is.

Acids & Hydrogen ions

• An acid is a corrosive chemical substance that produces hydrogen ions ($H^+$) when mixed with water. The higher the concentration of hydrogen ions produced by an acid, the higher its acidity.

• Strong acids are very dangerous.

• Weak acids are much safer to use, and are important in our diet.

• Citrus fruits contain a weak acid, called citric acid, which contributes to their sour flavor.

Twig

*Common acids, formulas for acids, comments, strong or weak

Acids & hydroxide ions

• A base is a substance that reacts with an acid to neutralise it.

• Bases that dissolve in water are called alkalis.

• When mixed with water, bases produce hydroxide ions ($OH^−$).

• Bases are caustic and can be just as dangerous as acids.

• Household cleaning products are strong bases.

• Weak bases are found in toothpaste, conditioners, antacid tablets and baking powder.
  *Three types of bases:

• Metal hydroxides (e.g., potassium hydroxide) contain metals bonded with hydroxide. ($OH$)

• Metal oxides (e.g., zinc oxide) contain metals bonded with oxide ($O_2$)

• Metal carbonates (e.g., copper carbonate) contain metals bonded with carbonate ($CO₃^{2-}$

The pH scale

• Measures acidity.

• Acids have a low pH, while bases have a high pH.

• Solution with a pH of 7 is neutral.

• pH below 7 is an acid and a pH above 7 is a base.

The Effect of Indicators on Acids and Bases

Observe the Effect of Indicators on Acids and Bases.

Questions for thought:

• What happens when an acid is mixed with water?

• What are alkalis?

• What is the pH of a neutral substance?

Challenge Questions

• List three properties of acids.

• Identify three acids.

• List two properties of bases.

• Identify three bases.

• What is the pH scale?

• Identify the pH of water.

• -Acids have a pH range of
  Bases have a pH range of

• Explain why strong acids and bases can be dangerous.

Neutralization

Learning Intentions

• Investigate a range of important chemical reactions that occur in non-living systems and involve energy transfer, including neutralisation and the reaction of acids.

Success Criteria

• Describe what happens when an acid reacts with a base.

Glossary

• Carbonate: A substance containing the elements carbon and oxygen.

• Neutralisation Reaction: A reaction involving an acid and a base to produce water and a salt.

• Strong acid: An acid that ionises completely in water.

• Weak acid: An acid that partially ionises (loses or gains electrons) in water.

Acid-Base Reactions Key Facts

• A neutral solution is pH 7

• Sodium bicarbonate is an alkali that can neutralise stomach acid

• In every neutralisation reaction an acid and base combine to form a salt and water

• Scuba divers use neutralisation reactions to allow them to stay underwater for longer

Neutralization reactions

• In a neutralisation reaction, an acid and a base react to form a salt and water.
  *B/c acids are a source of hydrogen ions ($H^+$), while bases are a source of hydroxide ions ($OH^−$).

• In an acid-base neutralisation reaction, the $H^+$ from the acid and the $OH^−$ from the base combine to form pure water, which is neutral and has a pH of 7:
  $Hydrogen + hydroxide → water$
  H^+ + OH^− -> H₂O

• The other parts of the acid and base combine to produce a salt.

• The reaction of a strong acid with a strong base results in a neutral solution with a pH of 7 and a neutral salt.

• The reaction of a strong acid with a weak base produces a solution with pH < 7, containing water and an acidic salt. *The reaction of a strong base with a weak acid produces a solution with pH > 7, containing water and a basic salt.
  Acid + Metal

Reactions-Acids and Metal reactions

• Investigate a range of important chemical reactions that occur in non-living systems and involve energy transfer, including neutralisation and the reaction of acids.

Reaction Films

Film regarding action of acids when cleaning coins.

Acids Reacting with Metals

• Acids react with metals to form salt and hydrogen gas.

• More reactive metals react faster, indicated by the release of hydrogen gas bubbles.
  *Reaction:
  *Acid + metal → salt + hydrogen The salt formed depends on the acid the metal reacts with.
  $Hydrochloric +magnesium → magnesium chloride + hydrogen$
  $2HCl + Mg → MgCl + H₂$

Acids Reacting with Metal Carbonates

• A metal carbonate is a compound containing metal, carbon and oxygen.
  Acid + metal carbonate → salt + carbon dioxide + water
  *Acid + Metal Carbonate | Chemistry: Observing acid interacting with carbonate and generating bubbles

Reacting Hydrochloric Acid With Magnesium (Aim)

*To investigate the the products of the reaction of hydrochloric acid and magnesium.

Acids + Metal Carbonate

• To test gas released in a reaction, use limewater

• Carbon dioxide which turns the lime water milky.

• For example - calcium carbonate - a compound to stop Upset Stomach (reacts with acids) to produce calcium chloride, carbon
  dioxide and water

• 2HCl + CaCO3→ CaCl2 + CO₂ + H₂O

Questions

• What is a neutralisation reaction?

• Which metals are more reactive than magnesium?

• How can we test if a gas is carbon dioxide?

Check Questions

List some reactions of acid!
Explain the role when hydrochloric acid reacts with magnesium.

Combustion chemical relations

• Investigate a range of types of important chemical reactions that occur in non-living systems and involve energy transfer, including combustion.

Combustion relations key facts-Glossary

• Combustion, Corrosion; Hydrocarbon Oxidation; Soot; Transform:
  Biological reactions and chemical reactions involve energy transfer

Oxidation & Combustion

2 types - Combustion & Corrosion

• Combustion requires oxygen. combustion takes place between a compound and oxygen. - producing heat and new product
  metal + burnt in oxygen = metal oxide + Energy
  Magnesium+ oxygen = magnesium oxide

Incomplete reactions

*limited oxygen - will occur, instead of producing carbon dioxide and water, complete combustion produces carbon monoxide (toxic gas)
Propane+ oxygen =carbon monoxide+ water OR Carbon +water
The complete combustion reaction of propane ($CH$) requires five molecules of oxygen

2 General reactions

1*React strongly with metal carbonates (Acids and Metals).
2 Carbon dioxide turns limewater milky + metal carbonate à salt + carbon dioxide+ water

Key Notes + Decomposition

Types of : Combustion & Electrical
**Combustion reactions involve oxygen.
**Incomplete combustion reactions produce carbon monoxide (toxic gas) and metal.

Acids and bases:

Questions and key points:
Define these topics (Acid and or a base, what will be the role of Hydrogen and what will be PH when interacting

Corrosion

Corrosion - Is a gradual degradation of metal structures
Corrosion will occur as the metals will react with oxygen, forming compounds! In turn
will - Affect structure properties:

Corrosive process

• Rust - aka iron oxide $(Fe₂O₃)$

*needs to be prevent with barriers/ layers/coating:

Example layers

• (Painting, coating with plastic) + galvanic cells and using Passivating metals

Passivating - Is the creation of surface layer that prevent corrosion, like Aluminum