Properties of Solids, Liquids, and Gases

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

<p>Solids have fixed shape while liquids do not (A)</p> Signup and view all the answers

<p>To make objects more resistant to corrosion (C)</p> Signup and view all the answers

<p>It results in higher energy products than reactants. (C)</p> Signup and view all the answers

<p>Higher than the products. (B)</p> Signup and view all the answers

<p>Making of bonds is exothermic. (C)</p> Signup and view all the answers

<p>By comparing the amount of heat absorbed against the heat released. (B)</p> Signup and view all the answers

<p>To oxidize the pure metal. (A)</p> Signup and view all the answers

<p>Endothermic process (D)</p> Signup and view all the answers

<p>The volume of X required must be half that of Y (C)</p> Signup and view all the answers

<p>Divide the mass of each element by its atomic mass (A)</p> Signup and view all the answers

<p>The reaction is endothermic. (C)</p> Signup and view all the answers

<p>By multiplying the empirical ratio by the molar mass (A)</p> Signup and view all the answers

<p>The enthalpy change (ΔH) is negative. (A)</p> Signup and view all the answers

<p>The production of a new substance. (A)</p> Signup and view all the answers

<p>Actual yield / expected yield x 100 (D)</p> Signup and view all the answers

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

<p>The ions are produced at both electrodes (D)</p> Signup and view all the answers

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

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

<p>It is where reduction occurs (B)</p> Signup and view all the answers

<p>They form water at the anode (A)</p> Signup and view all the answers

<p>The oxidation state of iron in the compound (D)</p> Signup and view all the answers

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

<p>They ionise completely in water (C)</p> Signup and view all the answers

<p>Salt and water are formed (D)</p> Signup and view all the answers

<p>7 (B)</p> Signup and view all the answers

<p>Neutralizer for acidic soil (B)</p> Signup and view all the answers

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

<p>Partial ionization in water (B)</p> Signup and view all the answers

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

<p>They react with both acids and bases (D)</p> Signup and view all the answers

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

<p>Lead chloride (D)</p> Signup and view all the answers

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

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

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

<p>Boiling point (D)</p> Signup and view all the answers

<p>CnH2n+2 (C)</p> Signup and view all the answers

<p>Different general formula (D)</p> Signup and view all the answers

<p>Hydration (D)</p> Signup and view all the answers

<p>Gasoline/Petrol (D)</p> Signup and view all the answers

<p>At the bottom of the fractionating column (C)</p> Signup and view all the answers

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

<p>Boiling point increases with increasing chain length (A)</p> Signup and view all the answers

<p>-OH (D)</p> Signup and view all the answers

<p>Carbon dioxide (D)</p> Signup and view all the answers

<p>Ethanol (D)</p> Signup and view all the answers

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

<p>To provide sacrificial protection (B)</p> Signup and view all the answers

<p>Sodium and Potassium (D)</p> Signup and view all the answers

<p>By combining calcium oxide with acidic oxides (D)</p> Signup and view all the answers

<p>Using anhydrous cobalt (II) chloride (C)</p> Signup and view all the answers

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

<p>78% nitrogen (C)</p> Signup and view all the answers

<p>Carbon monoxide (D)</p> Signup and view all the answers

<p>Leads to acid rain formation (B)</p> Signup and view all the answers

<p>Convert harmful gases into harmless emissions (A)</p> Signup and view all the answers

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

<p>Trapping of radiation by greenhouse gases (B)</p> Signup and view all the answers

<p>Activated carbon treatment (B)</p> Signup and view all the answers

<p>Displaces ammonia from fertilizers (A)</p> Signup and view all the answers

<p>Harmful algal blooms (B)</p> Signup and view all the answers

Solids have strong attractive forces between particles, fixed positions, and vibrate. They have a fixed volume, shape, and high density.

Liquids have weaker attractive forces than solids. Particles are further apart, move freely, and take the shape of their container. Liquids maintain a fixed volume.

Gases have little to no attractive forces between particles. Particles are far apart, move randomly in all directions, and take the shape and volume of their container.

The random movement of particles in a fluid, caused by collisions with other faster-moving particles.

Particles in solids are arranged in an orderly, fixed manner.

The reactant that is completely consumed in a chemical reaction, determining the maximum amount of product that can be formed.

The simplest whole-number ratio of atoms of each element in a compound.

The actual number of atoms of each element present in a molecule of a compound.

The percentage of the theoretical yield that is actually obtained in a chemical reaction.

The percentage of a substance that is pure, calculated from the mass of the pure substance divided by the total mass, then multiplied by 100.

The process of using an electric current to drive a non-spontaneous chemical reaction.

An ionic compound in aqueous or molten state that can conduct electricity.

The products formed during electrolysis of dilute aqueous solutions depend on the reactivity of ions, and oxygen is always formed at the anode.

In concentrated solutions, the anion determines the anode product, while the cathode product depends on reactivity.

The positive electrode in an electrolytic cell.

A technique used to coat an object with a thin layer of another metal for corrosion resistance or improved appearance. It involves using electrolysis with a pure metal anode, the object as the cathode, and an electrolyte solution containing the metal ions.

A reaction in which heat energy is absorbed from the surroundings, resulting in a decrease in surrounding temperature. The products have higher energy than the reactants.

A reaction that releases heat energy into the surroundings, increasing the surrounding temperature. The products have lower energy than the reactants.

The process of breaking chemical bonds between atoms in molecules, requiring energy input and making it an endothermic process.

The formation of new chemical bonds between atoms, releasing energy and making it an exothermic process.

The difference in energy between the reactants and products of a reaction. A positive ΔH indicates an endothermic reaction, while a negative ΔH indicates an exothermic reaction.

A visual representation of energy changes during a chemical reaction, showing the activation energy and relative energy levels of reactants and products.

The minimum amount of energy required to start a chemical reaction. Reactant particles must possess this energy to react effectively.

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

A change in the chemical composition of a substance, resulting in the formation of new substances. They often involve breaking and forming bonds.

The number of electrons an atom gains or loses when forming a chemical bond. It's represented by Roman numerals for elements with multiple oxidation states, like transition metals.

A method to produce sulfuric acid (H2SO4) using sulfur, water, and concentrated sulfuric acid as raw materials.

A method to produce ammonia (NH3) using nitrogen and hydrogen as reactants.

Sulfuric acid has many applications, including preparation of fertilizers, electrolyte in car batteries, and production of detergents.

Sulfur dioxide, a gas, is used to sterilize baby bottles, preserve jams and jellies, and bleach wood pulp.

Acids are substances that can donate hydrogen ions (H+) in a solution.

Acids have a pH below 7, taste sour, are corrosive, and turn blue litmus paper red.

Bases are substances that can accept hydrogen ions (H+) in a solution.

Bases have a pH above 7, are metal oxides or hydroxides, and soluble bases are called alkalis.

A scale used to measure the acidity or alkalinity of a solution, ranging from 0 to 14, with 7 being neutral.

Substances that change color in the presence of acids or bases, allowing us to determine pH.

Acids that ionize completely in water, releasing all their hydrogen ions (H+), resulting in a very low pH.

Acids that only partially ionize in water, releasing some hydrogen ions (H+), resulting in a higher pH than strong acids.

Oxides of non-metals, which react with bases to form salts and water, and produce acidic solutions in water.

Oxides of metals, which react with acids to form salts and water, making basic solutions in water.

Compounds containing carbon atoms.

Organic compounds made up of only carbon and hydrogen.

A formula showing the ratio of elements in a specific series of compounds.

A diagram showing how atoms are connected in a molecule.

Burning with enough oxygen to produce carbon dioxide and water.

Burning with limited oxygen, producing carbon monoxide and water.

A mixture of hydrocarbons, a raw material for fuels.

Separating crude oil into fractions based on their boiling points.

A group of similar organic compounds sharing a functional group.

Hydrocarbons with single carbon-carbon bonds.

Hydrocarbons with a carbon-carbon double bond.

Reaction where simple molecules add across the double bond of an alkene.

Organic compounds containing the -OH functional group.

Anaerobic respiration by yeast, converting sugar to alcohol.

Breaking down large alkane molecules into smaller molecules like alkenes.

The process of coating iron or steel with a layer of zinc to prevent corrosion. This provides sacrificial protection, meaning the zinc corrodes first, protecting the iron.

A method of corrosion prevention where a more reactive metal is used to protect a less reactive one. The more reactive metal corrodes first, sacrificing itself to protect the other metal.

Sodium and potassium are too reactive, reacting violently and explosively with the environment. They would be consumed quickly, requiring frequent replacement.

Molten iron is brittle because it contains impurities like carbon, phosphorus, and silicon.

Molten iron is purified by adding oxygen and calcium oxide. The oxygen removes impurities as oxides, and the calcium oxide reacts with acidic silicon and phosphorus oxides to form slag. The slag then floats on the molten iron and is removed.

Metals higher in the reactivity series (above carbon) are extracted using electrolysis, while metals lower in the series (below carbon) are extracted by heating with carbon.

Aluminium is used for overhead electrical cables because of its low density (lightweight) and good electrical conductivity.

Copper is used in electrical wiring because it has good electrical conductivity and is ductile, meaning it can be drawn into thin wires.

Anhydrous cobalt(II) chloride turns from blue to pink when water is present, and copper(II) sulfate turns from white to blue.

Untreated water can contain dissolved oxygen, metal compounds, plastics, sewage, harmful microbes, nitrates and phosphates from fertilizers, and detergents.

Distilled water is used in chemistry because it has fewer chemical impurities, providing reliable results in experiments.

Large insoluble particles are removed from water through filtration, passing the water through layers of sand and gravel filters.

Chlorine is passed through water to disinfect it by chlorination, killing harmful bacteria.

Carbon monoxide is poisonous. It combines with blood and prevents oxygen from being carried by the blood, potentially leading to death.

Sulfur dioxide contributes to acid rain, damaging the environment and impacting ecosystems.

Catalytic converters use platinum and rhodium as catalysts to convert harmful gases, like carbon monoxide and oxides of nitrogen, into less harmful gases like nitrogen (N2) and carbon dioxide (CO2).