FINAL CHEM FLASHCARDS!

Q1: What are the properties of solids

Solids have a fixed shape and volume. Their particles are tightly packed in a regular pattern and can only vibrate. Solids have the lowest energy.

Q2: What are the properties of liquids

Liquids have a fixed volume but take the shape of the container bottom. Particles are loosely packed and move by sliding past each other. They have more energy than solids.

Q3: What are the properties of gases

Gases have no fixed shape or volume and fill the entire container. Their particles move freely and rapidly in all directions. Gases have the highest energy.

Q4: What happens to particles when a solid melts

Particles absorb heat and gain kinetic energy. They vibrate more and break some bonds, changing the solid into a liquid at its melting point.

Q5: What is boiling

Boiling is when a liquid changes into a gas at its boiling point. Heat energy causes particles to move faster and form bubbles of gas throughout the liquid, allowing them to escape into the air.

Q6: What is evaporation

Evaporation is when a liquid turns into gas from its surface at any temperature. High-energy particles at the surface escape into the air. It happens faster with higher temperatures or a larger surface area.

Q7: What is condensation

Condensation is when a gas turns into a liquid as it cools. Cooling reduces kinetic energy, so particles move slower and stick together to form a liquid.

Q8: What causes gas pressure

Gas pressure is caused by particles colliding with the walls of a container. More heat means faster-moving particles, increasing collisions and pressure.

Q9: What happens if gas is compressed

The same number of particles occupy a smaller volume. This causes more frequent collisions with the walls, increasing pressure.

Q10: What is an element

A substance made of only one type of atom with the same number of protons. It cannot be broken down into simpler substances.

Q11: What is a compound

A substance made of two or more elements chemically joined together in fixed proportions. It can only be separated by chemical methods.

Q12: What is a mixture

A combination of two or more substances not chemically bonded. Mixtures can be separated by physical methods like filtration or evaporation.

Q13: What are protons, neutrons, and electrons

Protons have a +1 charge and mass of 1. Neutrons have no charge and mass of 1. Electrons have a -1 charge and a very small mass.

Q14: What is the proton number

Also called atomic number, it tells the number of protons in an atom's nucleus and defines the element.

Q15: What is the nucleon number

Also called mass number, it is the total number of protons and neutrons in an atom's nucleus.

Q16: What does the group number tell you

It tells you the number of electrons in the outer shell of atoms in that group.

Q17: What is an ion

An ion is an atom or group of atoms that has gained or lost electrons, giving it a charge.

Q18: What is a cation

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

Q19: What is an anion

An anion is a negatively charged ion formed when an atom gains one or more electrons.

Q20: What is an ionic bond

An ionic bond is a strong electrostatic attraction between oppositely charged ions.

Q21: What types of elements form ionic bonds

Metals (which lose electrons) and non-metals (which gain electrons) form ionic bonds.

Q22: Do ionic compounds conduct electricity

They conduct electricity when molten or dissolved in water because ions can move. In solid form, the ions are fixed and cannot conduct.

Q23: What is a covalent bond

A covalent bond forms when two non-metal atoms share a pair of electrons.

Q24: Which elements form covalent bonds

Only non-metal elements form covalent bonds, often creating small molecules like H2O and CO2.

Q25: Why do covalent compounds have low melting points

Covalent compounds have weak intermolecular forces, so less energy is needed to separate the molecules.

Q26: Why don't covalent compounds conduct electricity

They do not have free ions or electrons, so they cannot carry an electric current.

Q27: What is electrolysis

Electrolysis is the process of breaking down an ionic compound using electricity. It must be molten or dissolved in water so the ions can move.

Q28: What is an electrolyte

An electrolyte is a molten or aqueous ionic compound that conducts electricity by allowing ions to move.

Q29: What is an electrode

An electrode is a rod that conducts electricity into or out of the electrolyte, often made of graphite or metal.

Q30: What is the anode

The anode is the positive electrode in electrolysis. It attracts negatively charged ions (anions).

Q31: What is the cathode

The cathode is the negative electrode in electrolysis. It attracts positively charged ions (cations).

Q32: What happens during electrolysis of molten lead(II) bromide

Lead(II) bromide is heated until molten. Lead ions go to the cathode and gain electrons to form grey lead metal. Bromide ions go to the anode and lose electrons to form brown bromine gas.

Q33: What happens in electrolysis of concentrated aqueous sodium chloride (brine)

At the cathode, hydrogen gas is formed because H+ is less reactive than Na+. At the anode, Cl- ions lose electrons to form chlorine gas. Na+ and OH- remain in the solution to form sodium hydroxide.

Q34: What happens during electrolysis of dilute sulfuric acid

H+ ions go to the cathode and form hydrogen gas. OH- ions go to the anode and form oxygen gas. The ratio of hydrogen to oxygen is 2:1.

Q35: What is the pH scale and what does it show

The pH scale ranges from 0-14. Acids have pH 0-6, neutral is 7, and alkalis have pH 8-14.

Q36: What ions do acids and alkalis produce in water

Acids produce hydrogen ions (H⁺) and alkalis produce hydroxide ions (OH⁻).

Q37: What happens in a neutralisation reaction

An acid reacts with a base to form a salt and water. The H⁺ from the acid and OH⁻ from the alkali combine to make H₂O.

Q38: What are the products when acids react with metals, bases, and carbonates

1. Acid + metal → salt + hydrogen gas 2. Acid + base → salt + water 3. Acid + carbonate → salt + carbon dioxide + water

Q39: What colour does litmus turn in acids and alkalis

Red in acids, blue in alkalis.

Q40: What colour does methyl orange turn in acids and alkalis

Red in acids, yellow in alkalis.

Q41: What is oxidation

Oxidation is the gain of oxygen or the loss of electrons.

Q42: What is reduction

Reduction is the loss of oxygen or the gain of electrons.

Q43: What is a redox reaction

A reaction where oxidation and reduction happen at the same time.

Q44: What does OIL RIG stand for

Oxidation Is Loss (of electrons), Reduction Is Gain (of electrons).

Q45: How is the Periodic Table arranged

In order of increasing atomic number. Groups are vertical and show the number of outer electrons; periods are horizontal and show the number of electron shells.

Q46: What are the properties of Group 1 alkali metals

Soft, low melting points, reactive with water, form alkaline hydroxides and hydrogen gas. Reactivity increases down the group.

Q47: What are the properties of Group 7 halogens

Poisonous, diatomic, form halide ions. Reactivity decreases down the group as atoms get larger and attraction for electrons weakens.

Q48: What are the trends in Group 1 and Group 7

Group 1: Reactivity increases down the group. Group 7: Reactivity decreases down the group.

Q49: What are transition metals

Elements in the centre of the Periodic Table. They are hard, have high melting points, form coloured compounds, and act as catalysts.

Q50: What factors affect the rate of reaction

Temperature, concentration, surface area, and catalysts.

Q51: How does temperature affect the rate of reaction

Higher temperature gives particles more kinetic energy, so they collide more often and with more energy.

Q52: How does concentration affect the rate

More particles in a given volume increases the chance of collisions, speeding up the reaction.

Q53: How does surface area affect the rate

Smaller pieces or powders expose more particles to collide, increasing the rate.

Q54: What is a catalyst

A substance that speeds up a reaction by lowering the activation energy, without being used up.

Q55: Name 3 ways to measure the rate of a reaction.Measure gas produced, mass lost, or time for colour change/disappearance of a cross.

Q56: What is an exothermic reaction

A reaction that releases heat to the surroundings. Temperature increases and the energy change is negative.

Q57: What is an endothermic reaction

A reaction that absorbs heat from the surroundings. Temperature decreases and the energy change is positive.

Q58: Give examples of exothermic and endothermic processes.Exothermic: combustion, neutralisation. Endothermic: electrolysis, photosynthesis, thermal decomposition.

Q59: What does a reaction profile show

The energy of reactants and products. Exothermic reactions have products with lower energy than reactants; endothermic is the opposite.

Q60: What is an oxide

A compound formed when an element reacts with oxygen.

Q61: What are acidic oxides

Non-metal oxides that dissolve in water to form acids. They react with bases to form salt and water. E.g. CO₂, SO₂.

Q62: What are basic oxides

Metal oxides that react with acids to form salt and water. E.g. CaO, MgO.

Q63: What are amphoteric oxides

Oxides that react with both acids and bases. E.g. ZnO, Al₂O₃.

Q64: What are neutral oxides

Oxides that do not react with either acids or bases. E.g. CO, N₂O.