Matter and Its Properties Quiz

Matter and Its Properties

• Substances are composed of atoms.
• Elements consist of only one type of atom.
• Compounds are formed from two or more different types of atoms chemically bonded, like water (H₂O).
• Chemical reactions involve atoms bonding and creating new substances.
• Word equations utilize substance names to represent reactions.
• Chemical equations use symbols for reactions, including state symbols (s, l, g, aq) for solids, liquids, gases, and aqueous solutions.
• Conservation of mass dictates equal numbers of each atom type on both sides of a balanced chemical equation.
• Mixtures are combinations of substances not chemically bonded, like air.
• Solutions are mixtures where one substance dissolves in another, e.g., salt water.
• Filtration separates insoluble solids from liquids.
• Crystallization separates a dissolved solid (solute) from a liquid (solvent) via evaporation.
• Distillation separates liquids with different boiling points by heating, collecting vapor, and cooling.
• Fractional distillation separates miscible liquids with different boiling points.
• Matter exists in three states: solids (particles vibrate, fixed positions), liquids (particles touch, move freely), and gases (particles far apart, move rapidly).
• Melting and evaporation necessitate energy input to overcome interparticle forces; no new substances form during these physical changes.

Atomic Structure & The Periodic Table

• Early atomic models included the Plum Pudding Model (J.J. Thomson).
• Rutherford's gold foil experiment revealed atoms are mostly empty space with a dense nucleus.
• Bohr proposed electron shells as specific orbitals around the nucleus.
• Chadwick discovered neutrons, neutral particles in the nucleus alongside protons.
• Atomic number defines an element, representing the number of protons.
• Mass number (relative atomic mass, RAM) is the total protons and neutrons.
• Isotopes are atoms of the same element with different neutron counts, thus different mass numbers.
• Relative abundance indicates the proportion of each isotope in a natural sample.
• Average relative atomic mass is calculated considering the abundance of each isotope.

Periodic Table and Reactivity

• The periodic table organizes elements by increasing atomic number, showing patterns in reactivity and properties.
• Groups (vertical columns) have similar properties, sharing the same number of valence electrons.
• Periods (horizontal rows) have elements with the same number of electron shells.
• Metals readily donate electrons, forming positive ions.
• Nonmetals readily accept electrons, forming negative ions.
• Group 1 (Alkali Metals) donate one valence electron, making them highly reactive with water.
• Group 7 (Halogens) accept one electron, and reactivity decreases down the group.
• Group 0 (Noble Gases) have full outer electron shells, resulting in low reactivity.
• Transition Metals exhibit variable electron donation and can form multiple charged ions. They're typically harder and less reactive than alkali metals, and often form colored compounds.

Bonding

• Metallic bonds involve a "sea" of delocalized electrons around metal ions, explaining conductivity.
• Ionic bonds form between metals and nonmetals due to electron transfer, creating ions held by electrostatic attraction.
• Covalent bonds form between nonmetals via electron sharing to achieve full outer electron shells.
• Giant covalent structures form extensive networks of covalent bonds, resulting in high melting points.

Key Examples

• Diamond, a giant covalent structure, consists of carbon atoms with four covalent bonds.
• Graphite, another allotrope of carbon, has layered structures with delocalized electrons, leading to conductivity.
• Graphene is a single layer of graphite.
• Fullerenes are 3D carbon structures, including buckminsterfullerenes and nanotubes.
• Nanoparticles exhibit a high surface area to volume ratio.

Quantitative Chemistry

• Conservation of mass states the total reactant mass equals the total product mass in a reaction.
• Relative formula mass (RFM) is the sum of atomic masses in a compound.
• The mole is the unit for amounts of substance, containing Avogadro's number of particles (6.022 x 10²³).
• Moles = mass (g) / RFM (g/mol).
• Limiting reactant is the reactant that's completely used up first, determining product yield.
• Solution concentrations are often expressed in g/dm³ or mol/dm³ (molarity).
• Reversible reactions can proceed in both directions.

Percentage Yield

• Percentage yield measures the actual product yield compared to the theoretical maximum.
• % Yield = (Actual mass of product / Theoretical mass of product) x 100%.

Atom Economy

• Atom economy assesses efficiency by comparing the mass of desired product to total reactant mass.
• % Atom Economy = (Mass of desired product / Total mass of reactants) x 100%.

Gas Volumes

• One mole of any gas occupies 24 dm³ at room temperature and pressure (RTP).
• RTP is defined as 20°C and 1 atmosphere pressure.

Reactivity Series

• The reactivity series lists metals in order of decreasing reactivity.
• More reactive metals displace less reactive metals from their compounds.
• Metals more reactive than hydrogen can displace hydrogen from acids.

Metals

• Alkali metals react vigorously with water to produce hydrogen gas and a metal hydroxide.
• Smelting extracts less reactive metals from ores by displacement with carbon, a reduction reaction.
• Reactive metals react with acids (HCl, H₂SO₄) producing a salt and hydrogen gas.

Acids and Alkalis

• Acids have pH values less than 7, containing H⁺ ions.
• Alkalis have pH values greater than 7, containing OH⁻ ions.
• Acids and alkalis neutralize to form a salt and water.
• The pH scale is logarithmic, each unit change represents a tenfold change in H⁺ or OH⁻ concentration.
• Strong acids fully dissociate in solution, whereas weak acids do not.

Titration

• Titration determines the concentration of an unknown acid or alkali.
• A known volume and concentration solution is carefully added to a measured volume of the unknown solution until the reaction is complete.
• An indicator signals the neutralisation point.

Electrolysis

• Electrolysis uses an electric current to decompose an ionic compound.
• Molten or dissolved compounds are used, in an apparatus with inert electrodes.
• Cations (positive ions) are reduced at the cathode, while anions (negative ions) are oxidized at the anode.

Energy Changes in Chemical Reactions

• Bond formation releases energy.
• Bond breaking requires energy.
• Exothermic reactions release more energy than absorbed.
• Endothermic reactions absorb more energy than released.

Fuel Cells

• Fuel cells convert chemical energy to electrical energy.
• Hydrogen and oxygen react to form water, releasing energy.

Test your knowledge on the fundamental concepts of matter and its properties. This quiz covers substances, elements, compounds, chemical reactions, and the principles of conservation of mass. Prepare to balance chemical equations and understand the differences between mixtures and solutions.