GCSE Chemistry 2
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| Elements in Group 1 of the periodic table, including lithium, sodium, potassium, rubidium, caesium, and francium. | Alkali Metals |
| The elements belonging to the first group of the periodic table, characterized by similar properties and chemical behavior. | Group 1 Elements |
| Caesium, being highly reactive, exhibits an explosive reaction when coming into contact with water, demonstrating the extreme reactivity of some alkali metals. | Explosive Reaction with Caesium |
| What role does shielding play in alkali metal reactivity? | Shielding by inner electron shells reduces the attraction between the outer electron and the nucleus in alkali metals, making the outer electron more easily lost and contributing to increased reactivity down the group. |
| Name the 6 alkali metals in order of increasing reactivity | Lithium Sodium Potassium Rubidium Caesium Francium |
| Which group do alkali metals belong to in the periodic table? | Alkali metals belong to Group 1 in the periodic table. |
| Caesium, being highly reactive, exhibits an explosive reaction when coming into contact with water, demonstrating the extreme reactivity of some alkali metals. | Explosive Reaction with Caesium |
| NA | NA |
| Name the 4 characteristics of the alkali metals | Low densities Soft enough to cut through with a knife Relatively low melting points (e.g., sodium: 98°C, potassium: 63°C) Highly reactive |
| What is a common physical property of alkali metals? | Alkali metals have low densities and are soft enough to be cut with a knife. |
| Explain why alkali metals are highly reactive | Have 1 electron in outer shell Easily form positive ions by losing this electron |
| Alkali metals have relatively low melting points for metals. For example, sodium has a melting point of 98°C, and potassium has a melting point of 63°C. | Melting Points of Alkali Metals |
| Compare the melting point of sodium with that of iron. | Sodium has a melting point of 98°C, while iron has a much higher melting point of 1538°C. |
| Alkali metals are highly reactive due to having only 1 electron in their outer shell. | Reactivity of Alkali Metals |
| Why are alkali metals highly reactive? | Alkali metals are highly reactive because they have just 1 electron in their outer shell, making it easy for them to lose this electron and form a positive ion. |
| The observed pattern that the reactivity of alkali metals increases as you move down the group in the periodic table. | Alkali Metal Reactivity Trend |
| Name 4 Alkali Metal Properties. | Low densities Softness Low melting points High reactivity due to having only one electron in their outer shell |
| Why does the reactivity of alkali metals increase down the group? | The reactivity increases because the number of electron shells in each atom increases. As the outer electron moves further from the nucleus and becomes more shielded by inner electron shells, its attraction to the nucleus decreases, making it more easily lost. |
| The count of electron shells in an atom, which increases down the alkali metal group, contributing to changes in reactivity. | Number of Electron Shells (contributing to reactivity) |
| How does the distance from the nucleus affect reactivity in alkali metals? | As the number of electron shells increases, the outer electron in alkali metals moves further from the nucleus, reducing its attraction to the nucleus and making it more easily lost, leading to increased reactivity. |
| What role does shielding play in alkali metal reactivity? | Shielding by inner electron shells reduces the attraction between the outer electron and the nucleus in alkali metals, making the outer electron more easily lost and contributing to increased reactivity down the group. |
| Compounds formed when alkali metals react with water, resulting in the production of hydrogen gas and salts that dissolve in water. | Metal Hydroxides |
| What happens when alkali metals react with water? | Alkali metals react vigorously with water, producing hydrogen gas and forming metal hydroxides. |
| Solutions produced when metal hydroxides dissolve in water, giving a basic pH and contributing to the characteristic alkaline properties. | Alkaline Solutions |
| What is the result of metal hydroxides dissolving in water? | The dissolution of metal hydroxides in water produces alkaline solutions with characteristic basic properties. |
| The level of activity or violence with which alkali metals react with water, where more reactive alkali metals lead to more vigorous reactions. | Reaction Vigor in Alkali Metals |
| How does the reactivity of alkali metals affect their reaction with water? | The more reactive an alkali metal is, the more vigorous its reaction with water. This is evident in the production of hydrogen gas and metal hydroxides. |
| The chemical reaction where lithium reacts with water to produce lithium hydroxide and hydrogen gas, exemplifying the general behavior of alkali metals in water. | Example Reaction - Lithium with Water |
| How does potassium's reaction with water differ from lithium's? | The reaction of potassium with water is more vigorous, releasing enough energy to ignite hydrogen, (producing a lilac flame) showcasing the trend that more reactive alkali metals have more energetic reactions. |
| Caesium, being highly reactive, exhibits an explosive reaction when coming into contact with water, demonstrating the extreme reactivity of some alkali metals. | Explosive Reaction with Caesium |
| Where are Group 7 elements located on the periodic table? | Group 7 elements, also known as halogens, are found on the right side of the periodic table. |
| What is the molecular structure of halogens? | Halogens exist as molecules made of pairs of atoms that are covalently bonded together. An example is Cl2, where two chlorine atoms are covalently bonded. |
| Halogens achieve this by forming molecules through covalent bonding, ensuring both atoms in the molecule have a complete outer electron shell. | Stable Full Outer Shell |
| How many electrons do halogens have in their outer shell? | Halogens have 7 electrons in their outer shell, contributing to their similar chemical reactivity. |
| Due to having 7 electrons in their outer shell, halogens react in similar ways, exhibiting comparable chemical behaviors across the group. | Similar Reactivity of Halogens |
| Why do halogens all react in similar ways? | Halogens have 7 electrons in their outer shell, leading to similar reactivity patterns as they strive to achieve a stable full outer shell through chemical reactions. |
| The observed pattern where the melting and boiling points of halogens increase as you move down Group 7 of the periodic table. | Halogen Melting and Boiling Points Trend |
| What is the state of halogens at the top of Group 7 at room temperature? | Halogens at the top of Group 7 are gases at room temperature. |
| Halogens at the bottom of Group 7 are solids at room temperature. | State of Halogens at the Bottom of Group 7 |
| What factor influences the increase in melting and boiling points of halogens down the group? | The increase in melting and boiling points is influenced by the increasing relative atomic mass of halogens. |
| Larger halogen atoms have stronger intermolecular forces between them, contributing to higher melting and boiling points. | Intermolecular Forces in Larger Atoms |
| Why do larger atoms require more energy to change from a solid to a gas? | Larger atoms have stronger intermolecular forces, requiring more energy (higher temperature) to overcome these forces and transition from a solid to a gas. |
| The correlation between the increasing relative atomic mass of halogens and the corresponding rise in their melting and boiling points down Group 7. | Relationship between Atomic Mass and Melting/Boiling Points |
| How does the trend in melting and boiling points align with halogen size in Group 7? | The trend shows that as you move down Group 7, from smaller to larger halogens, the melting and boiling points increase due to stronger intermolecular forces in larger atoms. |
| Knowledge of the colors and physical states of chlorine, bromine, and iodine at room temperature. | Physical States and Colors of Halogens |
| Chlorine exists as a pale green gas at room temperature. | Chlorine Characteristics |
| What is the physical state and color of chlorine at room temperature? | Chlorine is a pale green gas at room temperature. |
| Bromine exists as a red-brown liquid at room temperature. | Bromine Characteristics |
| Describe the physical state and colour of bromine at room temperature. | Bromine is a red-brown liquid at room temperature. |
| Iodine is a dark grey solid at room temperature. | Iodine Properties |
| What is the physical state and color of iodine at room temperature? | Iodine is a dark grey solid at room temperature. |
| A specific test to identify the presence of chlorine (Cl2) involves placing damp litmus paper in a test tube of gas. | Chemical Test for Chlorine |
| How do you test for the presence of chlorine, and what is the result? | To test for chlorine (Cl2), place damp litmus paper in the test tube of gas. If chlorine is present, the litmus paper will be bleached white. |
| The observed pattern where the reactivity of halogens decreases as you move down Group 7 of the periodic table. | Halogen Reactivity Trend |
| Which halogen is at the top of Group 7 and is the most reactive? | Fluorine, positioned at the top of Group 7, is the most reactive halogen. |
| Astatine, located near the bottom of Group 7, is a much less reactive halogen. | Reactivity of Astatine |
| What influences the reactivity trend of halogens down the group? | The reactivity of halogens decreases with increasing relative atomic mass. |
| Halogens react by gaining 1 electron to fill their outer shells. | Electron Gain in Halogen Reactivity |
| Why does it become harder for halogens to gain an extra electron down the group? | It becomes harder down the group because the number of electron shells in each atom increases, causing the outer shell to be further away from the positive nucleus. |
| The outer shell's increased distance from the positive nucleus down the halogen group makes it harder to gain an extra electron due to increased shielding. | Outer Shell and Positive Nucleus Relationship |
| How does the outer shell's distance impact the reactivity of halogens? | The outer shell's increased distance makes it more challenging for halogens to gain an extra electron as it becomes more shielded from the pull of the positive nucleus, contributing to the decreasing reactivity trend down the group. |
| Compounds formed by the reaction of halogens with hydrogen, resulting in substances like hydrogen chloride (HCl). | Hydrogen Halides |
| How do halogens react with other non-metals to form compounds? | Halogens react with other non-metals by sharing electrons, creating covalent bonds that allow both atoms to complete their outer shells. |
| What kind of structures do compounds formed by halogens and non-metals have? | Compounds formed by halogens and non-metals have simple molecular structures, consisting of just a few atoms joined together by covalent bonds. |
| Hydrogen halides, formed by halogens and hydrogen, are gases at room temperature. | Hydrogen Halides at Room Temperature |
| What happens when hydrogen halides dissolve in water? | Hydrogen halides dissolve in water to create acidic solutions; for example, hydrogen chloride solution is known as hydrochloric acid: HCl(aq). |
| Ionic compounds formed when halogens react with metals, resulting in substances like sodium chloride (NaCl). | Metal Halides |
| What type of compounds do halogens and metals form when they react? | Halogens and metals form ionic compounds known as metal halides when they react. |
| Halogens gain one electron from a metal atom during the reaction to complete their outer shell. | Electron Gain by Halogens |
| What charge does a halogen ion have after gaining an electron? | When a halogen gains an electron, it forms an ion with a charge of –1. |
| Describe the formation of sodium chloride (NaCl) from chlorine and sodium. | In the reaction, chlorine gains an electron to form Cl–, which is attracted to Na+ to create the ionic compound NaCl, known as sodium chloride. |
| Instances of metal halides formed by halogens reacting with metals, including KI (potassium iodide) and FeBr3 (iron(III) bromide). | Examples of Metal Halides |
| A chemical reaction where a more reactive halogen displaces a less reactive halogen from an aqueous solution of its salt. | Displacement Reaction |
| What is required for a halogen displacement reaction to occur? | A more reactive halogen to (be able to) displace a less reactive halogen from an aqueous solution of its salt. |
| A solution in which a salt is dissolved in water, allowing for chemical reactions to take place. | Aqueous Solution |
| Provide an example of a displacement reaction involving chlorine, iodine, potassium AND chlorine, bromine, potassium. | Chlorine can displace iodine from a solution of potassium iodide and can displace bromine from a solution of potassium bromide. |
| Displacement reactions can be recognized by a colour change, indicating the occurrence of the chemical reaction. | Recognition of Displacement Reactions |
| How can you identify a displacement reaction? | Displacement reactions can be identified by observing a colour change during the reaction. |
| Halogens with higher reactivity can displace halogens with lower reactivity in displacement reactions. | Reactive Halogens and Displacement |
| Why can chlorine displace both iodine and bromine in displacement reactions? | Chlorine is more reactive than both iodine and bromine, allowing it to displace them in displacement reactions. |
| Displacement reactions involve a transfer of electrons and are categorized as redox (oxidation-reduction) reactions. | Displacement Reactions as Redox Reactions |
| What is the key characteristic of displacement reactions that makes them redox reactions? | Displacement reactions involve a transfer of electrons, making them redox reactions. |
| In the reaction between chlorine and iodide ions, there is a transfer of electrons. | Electron Transfer in Chlorine-Iodide Reaction |
| What happens to iodide ions in the chlorine-iodide reaction? | Each iodide ion (I–) loses an electron, pairing up to form iodine (I2). |
| The principle that oxidation involves the loss of electrons, and reduction involves the gain of electrons, often remembered as OIL RIG. | Oxidation-Reduction (Redox) Reaction Principle |
| How do iodide ions exhibit oxidation in the chlorine-iodide reaction? | Iodide ions (I–) lose electrons in the reaction, undergoing oxidation to form iodine. |