Kinetic Particle Theory Quiz

<p>Lighter gases diffuse faster than heavier gases. (A)</p> Signup and view all the answers

<p>Particles lose energy and come closer together. (B)</p> Signup and view all the answers

<p>A strong attraction between oppositely charged ions (D)</p> Signup and view all the answers

<p>Atoms with the same number of protons but different numbers of neutrons (C)</p> Signup and view all the answers

<p>Electrons are found in shells around the nucleus (C)</p> Signup and view all the answers

<p>They have a full outer electron shell (C)</p> Signup and view all the answers

<p>2,8,2 (B)</p> Signup and view all the answers

<p>Formed by the sharing of a pair of electrons (A)</p> Signup and view all the answers

<p>The total number of protons and neutrons (A)</p> Signup and view all the answers

<p>They form regular lattices (C)</p> Signup and view all the answers

<p>Electronegativity typically increases (A)</p> Signup and view all the answers

<p>Loss of electrons (D)</p> Signup and view all the answers

<p>They are oxidized when they reduce another substance. (B)</p> Signup and view all the answers

<p>By simultaneous oxidation and reduction (C)</p> Signup and view all the answers

<p>Water is produced along with salt. (B)</p> Signup and view all the answers

<p>Al2O3 (B)</p> Signup and view all the answers

<p>When it reacts with a base. (C)</p> Signup and view all the answers

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

<p>Lower pH means higher concentration of H+ ions. (B)</p> Signup and view all the answers

<p>Acids turn litmus paper red. (A)</p> Signup and view all the answers

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

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

<p>They have a full external electron shell. (B)</p> Signup and view all the answers

<p>Metals are more conductive than non-metals. (B)</p> Signup and view all the answers

<p>They form coloured compounds. (B)</p> Signup and view all the answers

<p>They exist as diatomic molecules. (C)</p> Signup and view all the answers

<p>The different sized atoms prevent layers from sliding. (A)</p> Signup and view all the answers

<p>It decreases. (B)</p> Signup and view all the answers

<p>Red-brown liquid (D)</p> Signup and view all the answers

<p>It has good electrical conductivity and ductility. (C)</p> Signup and view all the answers

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

<p>The paper turns blue (A)</p> Signup and view all the answers

<p>Carbon dioxide (CO2) (C)</p> Signup and view all the answers

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

<p>Using a lighted splint that produces a 'pop' sound (D)</p> Signup and view all the answers

<p>Copper(II) (Cu2+) (A)</p> Signup and view all the answers

<p>potassium, sodium, calcium, magnesium (D)</p> Signup and view all the answers

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

<p>It forms magnesium oxide and water vapor. (A)</p> Signup and view all the answers

<p>Covering with plastic paint (C)</p> Signup and view all the answers

<p>Dissolving NaCl in water (A)</p> Signup and view all the answers

<p>Minimum energy for reactants to collide (A)</p> Signup and view all the answers

<p>It lowers the melting point of aluminium oxide. (A)</p> Signup and view all the answers

<p>Connecting a metal to a more reactive metal to protect it. (C)</p> Signup and view all the answers

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

<p>Boiling to remove all contaminants (B)</p> Signup and view all the answers

<p>Color of reactants (D)</p> Signup and view all the answers

<p>To remove offensive tastes and odours (D)</p> Signup and view all the answers

<p>The rate of the forward reaction equals the rate of the reverse reaction (B)</p> Signup and view all the answers

<p>Decreases the activation energy (B)</p> Signup and view all the answers

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

<p>It increases the frequency of particle collisions (B)</p> Signup and view all the answers

<p>Iron(III) oxide (C)</p> Signup and view all the answers

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

<p>N2(g) + 3H2(g) ⇌ 2NH3(g) (D)</p> Signup and view all the answers

<p>450 °C and 200 kPa are commonly used (D)</p> Signup and view all the answers

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

<p>Chemical changes involve the formation of new substances, while physical changes do not (D)</p> Signup and view all the answers

<p>It shifts the equilibrium toward the side with fewer moles of gas (B)</p> Signup and view all the answers

<p>Color of the reactants (D)</p> Signup and view all the answers

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

<p>Double carbon-carbon covalent bonds (C)</p> Signup and view all the answers

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

<p>Separation into useful fractions based on boiling points (B)</p> Signup and view all the answers

<p>Generally unreactive except during combustion (B)</p> Signup and view all the answers

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

<p>Fermentation of aqueous glucose (A)</p> Signup and view all the answers

<p>Electrostatic attraction between positive ions and delocalised electrons (D)</p> Signup and view all the answers

<p>Only single covalent bonds (D)</p> Signup and view all the answers

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

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

<p>The simplest whole number ratio of different atoms or ions (A)</p> Signup and view all the answers

<p>Alkenes are more reactive due to the presence of a double bond (B)</p> Signup and view all the answers

<p>Average mass of isotopes to 1/12th of a carbon-12 atom (D)</p> Signup and view all the answers

<p>6.02 x 10^23 particles per mole (D)</p> Signup and view all the answers

<p>Decomposition of an ionic compound by electric current (D)</p> Signup and view all the answers

<p>Non-metal elements (C)</p> Signup and view all the answers

<p>It generates electricity with water as the only product (A)</p> Signup and view all the answers

<p>The volume occupied by one mole of gas at standard conditions (A)</p> Signup and view all the answers

<p>It identifies which reactant runs out first during a reaction (D)</p> Signup and view all the answers

<p>Lead is deposited at the cathode (C)</p> Signup and view all the answers

<p>They are generally poor conductors in solid state (C)</p> Signup and view all the answers

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

<p>Nitrogen, Phosphorus, and Potassium (D)</p> Signup and view all the answers

<p>Incomplete combustion of fuels (A)</p> Signup and view all the answers

<p>Carbon Dioxide (A), Methane (C)</p> Signup and view all the answers

<p>Oxidation of nitrogen at high temperatures (B)</p> Signup and view all the answers

<p>carbon dioxide + water → glucose + oxygen (D)</p> Signup and view all the answers

<p>Low-sulfur fuels and catalytic converters (A)</p> Signup and view all the answers

<p>Has only single carbon-carbon bonds (C)</p> Signup and view all the answers

<p>Compounds with the same molecular formula but different structural arrangements (A)</p> Signup and view all the answers

<p>CnH2n (A)</p> Signup and view all the answers

<p>Same functional group and similar properties (C)</p> Signup and view all the answers

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

<p>Increased risk of respiratory illnesses and cancer (C)</p> Signup and view all the answers

<p>2CO + 2NO → 2CO2 + N2 (A)</p> Signup and view all the answers

<p>Global warming and climate change (A)</p> Signup and view all the answers

<p>Large molecules made from numerous monomers (D)</p> Signup and view all the answers

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

<p>They contain repeating units identical to the monomer (A)</p> Signup and view all the answers

<p>C2H4 (C)</p> Signup and view all the answers

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

<p>Made from a diol and a dicarboxylic acid (D)</p> Signup and view all the answers

<p>Accumulation in oceans (A)</p> Signup and view all the answers

<p>They are monomers that build proteins (C)</p> Signup and view all the answers

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

<p>By examining melting and boiling points (C)</p> Signup and view all the answers

<p>To separate mixtures of substances (C)</p> Signup and view all the answers

<p>A solid left after a separation process (B)</p> Signup and view all the answers

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

<p>To identify when the end-point is reached (C)</p> Signup and view all the answers

The state of matter where particles are closely packed, have a fixed arrangement and only vibrate in fixed positions.

The state of matter where particles are close together but can move around each other. They have a fixed volume but can take the shape of the container.

The state of matter where particles are widely spaced, move freely and have no fixed shape or volume.

The process of a substance changing from a solid to a liquid.

The process of a substance changing from a liquid to a gas.

Pure substances that cannot be broken down into simpler substances by chemical means.

Substances formed when two or more elements chemically combine in a fixed ratio.

A mixture contains two or more substances that are not chemically bonded, and can be separated by physical means.

The central part of an atom, containing protons and neutrons.

Subatomic particles with a positive charge, found in the nucleus.

Subatomic particles with no charge (neutral), found in the nucleus.

Negatively charged subatomic particles that orbit the nucleus in electron shells.

The number of protons in the nucleus of an atom, also known as the atomic number.

The total number of protons and neutrons in the nucleus of an atom.

Atoms of the same element that have the same number of protons but different numbers of neutrons.

A chemical reaction that involves the transfer of electrons between reactants, resulting in a change in oxidation states for at least two species.

The process of gaining oxygen or losing electrons, resulting in an increase in oxidation number.

The process of losing oxygen or gaining electrons, resulting in a decrease in oxidation number.

A substance that causes another substance to be oxidized while itself being reduced. It gains electrons.

A substance that causes another substance to be reduced while itself being oxidized. It loses electrons.

A substance that releases hydrogen ions (H+) when dissolved in water, resulting in a sour taste and the ability to react with metals, bases, and carbonates.

A base that is soluble in water.

A chemical reaction between an acid and a base, resulting in the formation of salt and water, with the neutralization of the acidic and basic properties.

A compound formed by the reaction between an acid and a base, containing a cation from the base and an anion from the acid.

The periodic table is a systematic arrangement of elements organized into horizontal rows called periods and vertical columns called groups, ordered by increasing atomic number (number of protons).

Across a period (row) from left to right, elements generally change from metallic to non-metallic properties.

The group number of an element often corresponds to the charge of the ion it forms. For example, elements in Group 1 form ions with a +1 charge.

Elements in the same group have similar chemical properties due to having the same number of valence electrons (electrons in the outermost shell).

The Periodic Table can predict an element's properties based on its position. For example, elements in the same period have similar atomic radii but differ in electronegativity.

Group 1 elements (alkali metals) are soft metals with decreasing melting points and increasing reactivity down the group. Density also increases.

Group 7 elements (halogens) are diatomic non-metals, meaning they exist as pairs of atoms. They show decreasing reactivity and increasing density down the group.

Transition metals are metals with high densities, high melting points, form colored compounds, and often act as catalysts. They can have multiple oxidation states (charges) in their ions.

Group 8 elements (noble gases) are unreactive, monatomic gases. Their unreactivity is due to their full outer electron shells, making them stable.

Metals are generally good conductors of heat and electricity, malleable (can be hammered into sheets), ductile (can be drawn into wires), and have high melting and boiling points. They react with acids, cold water, and oxygen.

A reaction that releases energy to its surroundings, causing the temperature to increase. This energy release is often in the form of heat.

A reaction that absorbs energy from its surroundings, causing the temperature to decrease. This energy absorption is often from heat.

The change in heat energy during a chemical reaction. It represents the difference between the enthalpy of the products and the enthalpy of the reactants. Exothermic reactions have a negative enthalpy change, while endothermic reactions have a positive enthalpy change.

The minimum amount of energy that colliding particles must possess to have a successful reaction. It is the energy barrier that needs to be overcome for a reaction to occur.

A diagram that shows the energy changes during a chemical reaction. It shows the energy of the reactants, products, the activation energy, and the enthalpy change.

The process of breaking chemical bonds. This process requires energy and is therefore endothermic.

The process of forming chemical bonds. This process releases energy and is therefore exothermic.

The enthalpy change of a reaction can be calculated by considering the energy required to break bonds in the reactants and the energy released when forming bonds in the products. The difference between these two values gives the enthalpy change.

Any change that alters the appearance or form of a substance, but does not change its chemical composition. The substance remains the same.

A change that involves the formation of new substances with different chemical properties. The original substances are chemically transformed.

The theory that explains how reactions happen. It states that for a reaction to occur, the reacting particles must collide with sufficient energy and in the correct orientation to break the bonds in the reactants and form new bonds in the products.

A substance that increases the rate of a reaction without being consumed in the reaction. It lowers the activation energy, providing an alternate pathway for the reaction.

A special type of biological catalyst that speeds up biochemical reactions in living organisms.

A reaction that can proceed in both directions, meaning the products can react to form the reactants and vice versa.

The state of a reversible reaction where the rate of the forward reaction is equal to the rate of the reverse reaction. The concentrations of the reactants and products remain constant.

Metallic bonding is a type of chemical bonding that occurs between metal atoms. In this type of bonding, the outermost electrons of the metal atoms are delocalized, forming a "sea" of electrons that move freely throughout the metal lattice. This 'sea' of electrons is held together by electrostatic attraction to the positively charged ions. This strong electrostatic attraction is the foundation of metallic bonding.

Metals are excellent conductors of electricity because their delocalized electrons are free to move throughout the metal lattice. When an electrical potential is applied, these electrons can easily flow, carrying the electric current.

Malleability describes a metal's ability to be hammered or pressed into different shapes without breaking. Ductility is the ability to be drawn into wires. Both are possible because of the 'sea' of delocalized electrons. When a force is applied, the layers of metal atoms can slide past each other without breaking the metallic bonds, as the electrons continue to attract the positive ions.

A molecular formula shows the actual number and type of atoms present in a single molecule of a compound. For example, the molecular formula of glucose is C6H12O6. This means each molecule of glucose contains 6 carbon atoms, 12 hydrogen atoms and 6 oxygen atoms.

An empirical formula shows the simplest whole number ratio of atoms present in a compound. It is the most simplified version of a molecular formula. For example, the molecular formula of glucose is C6H12O6, but its empirical formula is CH2O.

The relative atomic mass, Ar, is the average mass of the isotopes of an element compared to 1/12th of the mass of an atom of carbon-12.

The relative molecular mass, Mr, is the sum of the relative atomic masses of all the atoms in a molecule. For ionic compounds, the term relative formula mass, Mr, is used.

The mole is the SI unit of amount of substance. It is defined as the amount of substance that contains the same number of elementary entities (atoms, ions, molecules etc.) as there are atoms in 0.012 kilogram of carbon-12. This number is known as Avogadro's constant and is approximately 6.02 x 10^23.

Electrolysis is the process of decomposing an ionic compound by passing an electric current through its molten or aqueous solution. This process results in the separation of the compound into its constituent elements.

The anode is the positive electrode in an electrolytic cell. It is where oxidation occurs, meaning electrons are lost by ions. It's where non-metals (other than hydrogen) are usually formed.

The cathode is the negative electrode in an electrolytic cell. It is where reduction occurs, meaning electrons are gained by ions. Metals or hydrogen are usually formed at this electrode.

Electroplating is a process where a thin layer of metal is deposited onto the surface of another metal object. This is achieved by electrolysis, using the object to be plated as the cathode and the desired metal as the anode.

A hydrogen-oxygen fuel cell is a device that converts chemical energy from the reaction of hydrogen and oxygen into electrical energy. Water is the only by-product of this process, making it a clean energy source.

Hydrogen-oxygen fuel cells offer several advantages over gasoline/petrol engines. Some benefits include: Clean energy production with water as the only by-product; High energy efficiency compared to traditional combustion engines; Reduced emissions and greenhouse gases. However, they also have some drawbacks. These include: Hydrogen storage and transportation challenges; High initial cost; Limited infrastructure for refueling.

Aqueous sodium hydroxide (NaOH) solution reacts with aluminium ions (Al3+) to form a white gelatinous precipitate, which dissolves in excess sodium hydroxide solution to form a colorless solution.

Aqueous sodium hydroxide (NaOH) solution reacts with ammonium ions (NH4+) to produce a colorless gas with a pungent ammonia-like odor.

Aqueous sodium hydroxide (NaOH) solution reacts with copper(II) ions (Cu2+) to form a pale blue precipitate.

Aqueous ammonia (NH3) reacts with copper(II) ions (Cu2+) to form a pale blue precipitate, which dissolves in excess ammonia to form a deep blue solution.

A flame test is used to identify the cations of certain elements based on the color they produce when heated in a flame.

A list of metals arranged in order of decreasing reactivity, with the most reactive metal at the top and the least reactive at the bottom.

A chemical reaction where a more reactive metal displaces a less reactive metal from its salt solution.

The tendency of a metal to lose electrons and form positive ions.

The process of iron or steel reacting with oxygen and water to form hydrated iron(III) oxide (rust).

Methods that prevent rusting by physically blocking oxygen or water from reaching the metal surface.

The use of a more reactive metal to protect a less reactive metal from corrosion, by preferentially corroding itself.

A process that involves extracting a metal from its ore, which is a naturally occurring solid containing the metal compound.

A chemical process used to extract iron from its ore, hematite, by reducing iron(III) oxide to iron using carbon monoxide.

A chemical process used to extract aluminium from its ore, bauxite, by electrolysis, which uses an electric current to break down aluminium oxide into aluminium.

The process of removing impurities from a solution by sedimentation, filtration, and chemical treatment like chlorination.

Hydrocarbons are compounds that are made up of only hydrogen and carbon atoms.

Fossil fuels are natural fuels formed over millions of years from the remains of ancient organisms.

Coal, natural gas, and petroleum are the three main types of fossil fuels.

Petroleum is a mixture of hydrocarbons.

Fractional distillation is the process of separating petroleum into different fractions based on their boiling points.

Natural gas is mainly composed of methane, a simple hydrocarbon.

The cracking process breaks down larger alkanes into smaller, more useful alkenes and hydrogen gas. It uses high temperatures and a catalyst.

Alkanes are saturated hydrocarbons, meaning they contain only single carbon-carbon bonds.

Alkenes are unsaturated hydrocarbons, meaning they contain at least one double carbon-carbon bond.

Ethanol can be produced by fermentation of glucose or by catalytic addition of steam to ethene.

Ammonium salts and nitrates are chemical compounds used to provide essential nutrients like nitrogen to plants, promoting healthy growth.

NPK fertilizers contain nitrogen (N), phosphorus (P), and potassium (K), which are crucial for plant growth and development. These nutrients are needed in different quantities for specific plant processes.

Clean, dry air is primarily composed of nitrogen (N2) (around 78%), oxygen (O2) (around 21%), and a small percentage of noble gases like argon and carbon dioxide (CO2).

Carbon dioxide is produced when carbon-containing fuels, like wood or fossil fuels, are completely burned in the presence of oxygen.

When carbon-containing fuels are burned incompletely, carbon monoxide (CO) and particulate matter (small particles) are released into the air.

Methane is produced from the decomposition of organic matter, such as vegetation and waste, as well as from the digestive processes of animals.

Oxides of nitrogen are primarily produced by internal combustion engines, particularly in cars, due to high temperatures and the reaction between nitrogen and oxygen in the air.

Sulfur dioxide is released when fossil fuels containing sulfur compounds, such as coal and oil, are burned.

High levels of carbon dioxide in the atmosphere trap heat, leading to an increase in global temperature and resulting in climate change.

Carbon monoxide is a toxic gas that can be fatal when inhaled in high concentrations, as it displaces oxygen in the blood, preventing red blood cells from carrying oxygen throughout the body.

Particulate matter can irritate the respiratory system, leading to respiratory problems such as asthma and bronchitis, and also increase the risk of developing lung cancer.

Elevated levels of methane in the atmosphere contribute to global warming, as methane is a potent greenhouse gas, trapping heat and leading to climate change.

Oxides of nitrogen contribute to acid rain, which damages buildings, forests, and aquatic ecosystems. They also contribute to photochemical smog, a type of air pollution that causes respiratory problems.

Sulfur dioxide is a major contributor to acid rain, which damages ecosystems, buildings, and infrastructure. It also leads to respiratory problems in humans.

Photosynthesis is the process by which plants use sunlight, water, and carbon dioxide to produce glucose (a type of sugar) and oxygen. This process is essential for life on Earth.

Large molecules made from many smaller repeating units called monomers.

The process of joining monomers to form a polymer without the loss of any atoms.

A polymer formed by adding monomers together, with no loss of atoms.

The basic repeating unit in a polymer.

A polymer formed by the reaction of monomers, where small molecules such as water are lost during the reaction.

A polymer formed by the reaction of monomers, where small molecules such as water are lost during the reaction.

Polymers that are often used to make plastics.

A type of condensation polymer formed from a dicarboxylic acid (two COOH groups) and a diamine (two NH2 groups).

A type of condensation polymer formed from a dicarboxylic acid (two COOH groups) and a diol (two OH groups).

The properties of plastics, such as their durability and non-biodegradability, make them a challenge to dispose of.

A natural polyamide made from amino acid monomers.

The process of separating substances with different solubilities in a solvent.

The ratio of the distance traveled by a substance to the distance traveled by the solvent.

Techniques used to separate and purify substances based on their physical properties.

Substances that dissolve in a solvent.