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< Back A level Organic chemistry ​ ​ Previous Next

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< Back Atomic Structure Lesson 2 ⚛️ Lesson 2 ⚛️ This section delves into the mass and charge distributions within the atom, emphasizing the nucleus as the center of mass and the dance of electrostatic attraction that holds the atom together, while also highlighting the distinct movements of electrons, protons, and neutrons in an electric field. Previous Next ⚛️ 1.1.2 Mass, Charge & Subatomic Particles ⚛️ ✨🔬 Unmasking the Atom: Unveiling Mass & Charge Distributions 🔬✨ 1️⃣ The Mighty Nucleus: A Mass Reservoir 🏋️‍♀️🎯 Like a dense treasure chest in the heart of the atom, the nucleus is where the hefty subatomic heroes reside—the mighty protons and neutrons. They hoard nearly all of the atom's mass, with their combined weight making the nucleus the weightlifting champion of the atomic world. 🏆🌍 2️⃣ Electrons: The Lightweight Performers 💃⚡ Flirting around this massive nucleus, you'll find the feathery electrons. Their mass is so negligible, they're like tiny dancers pirouetting around a grand stage. Despite their lightness, they wear cloaks of negative charge, creating a bustling 'cloud' of negativity around the positive heart of the atom. ⛅💨 3️⃣ The Atom's Secret Glue: Electrostatic Attraction 🔗🧲 And what stops these nimble electrons from flitting away? The invisible ties of electrostatic attraction! The positive nucleus and negative electrons are drawn to each other, a captivating dance of opposite charges that keeps the atom together. 💖 ✨🎢 Subatomic Particles: Performers in an Electric Field 🎢✨ 1️⃣ The Electron's Graceful Waltz 🩰🌀 Imagine our subatomic performers, each moving at the same pace, but through a charged, electric stage. The electron, wearing its negative charge, is deflected away from the negative plate and is lured towards the positive plate with ease. This behavior not only proves its negative charge but also showcases its incredibly small mass as it pirouettes nimbly in the electric field. 🎭💫 2️⃣ The Proton's Powerful Stride 🏃‍♂️⚡ In contrast, the proton, with its positive charge, displays a different performance. It strides away from the positive plate and towards the negative one, asserting its positive nature. But compared to the electron's swift deflection, the proton's move is less pronounced, hinting at its greater mass. 💪🎖️ 3️⃣ The Neutron's Neutral Stand 🧍‍♂️🎭 What about the neutron? Well, the neutron, true to its neutral character, remains unaffected by the charged plates. It does not veer towards or shy away from either plate, simply continuing its journey unaffected—an applause-worthy performance proving its neutral nature. 👏🎭 So, there you have it—our subatomic performers illuminating the atom's inner workings through their mesmerizing dance in the atomic world and electric field! 🌠🌌 Quiz: Mass, Charge & Subatomic Particles ✨🔬 Unmasking the Atom: Unveiling Mass & Charge Distributions 🔬✨ Complete the missing words in the following questions: What resides in the nucleus and holds nearly all of the atom's mass? Answer: 🌟 Protons and neutrons Electrons have __________ mass compared to protons and neutrons. Answer: 🌌 Negligible/lightweight What creates an electric field that influences the movement of charged particles? Answer: 🔋 Charged plates Electrons are ____________ to the positive nucleus due to electrostatic attraction. Answer: 💞 Attracted In an electric field, electrons are deflected ____________ from the negative plate and toward the positive plate. Answer: 🌪 Away The proton, with its positive charge, moves ____________ from the positive plate and toward the negative plate in an electric field. Answer: 💥 Away Neutrons remain ____________ by the charged plates in an electric field due to their neutral nature. Answer: 🌟 Unaffected Protons have a ____________ mass compared to electrons. Answer: 💪 Greater The electron's movement in an electric field showcases its ____________ charge and small mass. Answer: 💫 Negative Neutrons demonstrate their ____________ nature by not veering towards or away from the charged plates in an electric field. Answer: 👏 Neutral Keep up the great work in understanding the mesmerizing dance of subatomic particles and their role in the atom's mass and charge distributions! 🎉🌠

Physical Change Grade 10 SABIS SABIS Produces no new kind of matter, is generally easily reversible, is not accompanied by great heat change, produces no observable change in mass

The process of cooling liquid paradichlorobenzene until it solidifies Grade 10 SABIS SABIS Exothermic

< Back Alkanes Alkanes may seem difficult at first. The nomenclature, the structures, the reactions - it can all be overwhelming. But don't let that discourage you. Because every great organic chemist started where you are. They faced the same challenges and setbacks, but they never gave up. They never let the complexity defeat them. Files Download DAY 12 Notes Alkanes The IGCSE Organic Chemistry Challenge 2 .pdf Download PDF • 6.14MB Notes Topic Exercise Answers DAY 13 .14 HW part 1 and 2 Alkanes The IGCSE Organic Chemistry Challenge .pdf Download PDF • 14.40MB answers DAY 13 .14 HW part 1 and 2 Alkanes The IGCSE Organic Chemistry Challenge .pdf Download PDF • 17.28MB Videos Previous Next

< Back Chemical Thermodynamics Prerequisites ​ Prerequisite Previous Next 🌟📘 Prerequisites for Chapter 6: Chemical Thermodynamics 📘🌟 Before diving into Chapter 6, which deals with chemical thermodynamics, students must have a solid understanding of the following concepts: 🔬 1. Basic Chemistry Concepts 🧪 Understand atoms, molecules, and chemical reactions. 🔬 2. Energy and Heat 🔥 Understand the concept of energy and the difference between heat and temperature. 🔬 3. Chemical Bonds 💪 Understand the energy involved in the formation and breaking of chemical bonds. 🔬 4. The Mole Concept 🐾 Understand the concept of moles and Avogadro's number. 🔬 5. Basic Mathematics 🧮 Be comfortable with algebra and solving equations. 🌟 20 Multiple Choice Questions to Check Mastery of Prerequisites 🌟 What is the smallest unit of an element that retains the properties of that element? a) Molecule b) Atom c) Electron d) Compound What is the energy called that is needed to break a chemical bond? a) Activation energy b) Bond energy c) Kinetic energy d) Potential energy How many atoms are in one mole of a substance? a) 6.022 x 10²³ b) 12 c) 1000 d) 1 What is the standard unit of temperature? a) Kelvin b) Celsius c) Fahrenheit d) Rankine What is the energy change of a system called? a) Enthalpy b) Entropy c) Heat d) Work What is the heat absorbed or released at constant pressure called? a) Internal energy b) Entropy c) Enthalpy d) Work What is the standard unit of energy? a) Joule b) Calorie c) Watt d) Newton What is the term for a reaction that absorbs heat from the surroundings? a) Exothermic b) Endothermic c) Isothermal d) Adiabatic What is the term for the average kinetic energy of particles in a substance? a) Heat b) Temperature c) Enthalpy d) Entropy Which law states that energy cannot be created or destroyed? a) First Law of Thermodynamics b) Second Law of Thermodynamics c) Hess's Law d) Law of Conservation of Mass What is the heat content of a system at constant pressure called? a) Internal energy b) Entropy c) Enthalpy d) Work What type of reaction releases heat to the surroundings? a) Exothermic b) Endothermic c) Isothermal d) Adiabatic What is the heat transfer into or out of a system called? a) Internal energy b) Entropy c) Enthalpy d) Heat What is the standard unit of pressure? a) Pascal b) Atmosphere c) Torr d) Bar What is the term for the heat transfer that occurs with no change in temperature? a) Latent heat b) Specific heat c) Enthalpy d) Entropy What is the term for the disorder or randomness of a system? a) Internal energy b) Entropy c) Enthalpy d) Heat In an exothermic reaction, the energy of the products is _______ than the energy of the reactants. a) Higher b) Lower c) The same d) Cannot be determined What is the heat required to raise the temperature of 1 gram of a substance by 1 degree Celsius called? a) Latent heat b) Specific heat c) Enthalpy d) Entropy What is the term for a reaction where the reactants and products are in equilibrium with each other? a) Dynamic equilibrium b) Static equilibrium c) Chemical equilibrium d) Physical equilibrium What is the term for the minimum energy required for a chemical reaction to occur? a) Activation energy b) Bond energy c) Kinetic energy d) Potential energy 🌟 Answers 🌟 b) Atom b) Bond energy a) 6.022 x 10²³ a) Kelvin a) Enthalpy c) Enthalpy a) Joule b) Endothermic b) Temperature a) First Law of Thermodynamics c) Enthalpy a) Exothermic d) Heat a) Pascal a) Latent heat b) Entropy b) Lower b) Specific heat a) Dynamic equilibrium a) Activation energy

< Back Chemical Bonding prerequisite ​ Prerequisite Previous Next 🌟📘 Prerequisites for Chapter 4: Chemical Bonding 📘🌟 Before diving into Chapter 4, which deals with chemical bonding, students must have a solid understanding of the following concepts: 🔬 1. Atomic Structure 🧪 Understand the structure of an atom including protons, neutrons, and electrons. Know the arrangement of electrons in energy levels or shells. 🔬 2. Periodic Table 📊 Understand the arrangement of elements in the periodic table. Know the trends in atomic size, electronegativity, and ionization energy across periods and down groups. 🔬 3. Ion Formation ⚛️ Understand how ions are formed by the loss or gain of electrons. Know the difference between cations and anions. 🔬 4. Electronegativity ⚡ Understand the concept of electronegativity and its role in bond formation. 🔬 5. Valence Electrons 🎯 Know how to determine the number of valence electrons in an atom. Understand the role of valence electrons in bond formation. 🔬 6. Basic Stoichiometry 🧮 Understand the law of conservation of mass. Be able to balance chemical equations. 🔬 7. Types of Chemical Bonds 💥 Have a basic understanding of ionic and covalent bonds. 🌟 20 Questions to Check Mastery of Prerequisites 🌟 What are the three subatomic particles of an atom? 🤔 How many electrons can the first and second energy levels hold? 🔄 What is the charge of a proton? ➕ Define electronegativity. 🧲 Which element has the highest electronegativity? 🏆 How does atomic size change as you move across a period? 📉 What is the difference between a cation and an anion? ⚖️ How many valence electrons does oxygen have? 🎱 Write the electron configuration of carbon. ✍️ What is the octet rule? 🎱 What type of bond is formed when electrons are shared between atoms? 🤝 What type of bond is formed when electrons are transferred from one atom to another? 🔄 What is the chemical formula for sodium chloride? 🧂 Balance the following chemical equation: H2 + O2 -> H2O ⚖️ What is ionization energy? 💥 How many valence electrons are in an atom of chlorine? 🍀 What is the role of valence electrons in chemical bonding? 🤔 Define covalent bond. 🌉 Define ionic bond. ⚡ Which group of elements in the periodic table is known as the noble gases? 👑 🌟 Answers 🌟 Protons, neutrons, and electrons. First can hold 2, second can hold 8. +1. Electronegativity is the ability of an atom to attract electrons in a chemical bond. Fluorine. It decreases. Cations are positively charged, and anions are negatively charged. 1s² 2s² 2p². Atoms tend to gain, lose, or share electrons to have a full outer shell of 8 electrons. Covalent bond. Ionic bond. NaCl. 2H₂ + O₂ -> 2H₂O. Ionization energy is the energy required to remove an electron from an atom. Valence electrons are involved in forming chemical bonds with other atoms. A covalent bond is a chemical bond formed by the sharing of electron pairs between atoms. An ionic bond is a chemical bond formed by the transfer of electrons from one atom to another, resulting in the formation of positively and negatively charged ions. Group 18.

Heating wax until it melts Grade 10 SABIS SABIS Physical

Group 1 metals (alkali metals): each has 1 more electron than the noble gas before it  they form stable 1+ ions which have a noble gas electron arrangement. Grade 10 SABIS ​

< Back The Periodic Table: chemical periodicity ​ ​ Previous Next 🔬 Chapter 10: Periodicity 🔬 Structure of the Periodic Table 📊: Elements are arranged in the Periodic Table in order of atomic number. There are 18 groups (vertical columns) and rows across the table are called periods. The recurrence of the same pattern across periods is called periodicity. Electronegativity increases across a period due to increasing positive nuclear charge. The greater the difference in electronegativity between the Period 3 element and oxygen, the more likely the oxide will have ionic bonding. Acidic/Basic Nature of Period 3 Oxides 🧪: Sodium oxide (Na2O) and magnesium oxide (MgO) are basic. Aluminum oxide (Al2O3) is amphoteric. Silicon dioxide (SiO2), phosphorus pentoxide (P4O10), and sulfur dioxide (SO2) are acidic.

< Back States of matter ​ ​ Previous Next 🔬 Chapter 5: States of Matter 🔬 Learning Outcomes 🎯: State the basic assumptions of the kinetic theory as applied to an ideal gas. Explain qualitatively in terms of intermolecular forces and molecular size, the conditions necessary for a gas to approach ideal behavior. State and use the general gas equation pV = nRT in calculations. Describe, using a kinetic-molecular model, the liquid state, melting, vaporization, and vapor pressure. Describe in simple terms the lattice structures of crystalline solids, including ionic, simple molecular, giant molecular, hydrogen bonded, or metallic. Discuss the finite nature of materials as a resource and the importance of recycling processes. Outline the importance of hydrogen bonding to the physical properties of substances, including ice and water. Recycling Materials ♻️: Recycling metals saves energy, conserves supplies of the ore, reduces waste, and is often cheaper than extracting metals from their ores. Recycling copper is important due to the low percentage of copper in most remaining ores and the energy savings in recycling compared to extraction. Recycling aluminum is much cheaper than extracting it from bauxite ore, and there is a 95% saving in energy by recycling aluminum compared to extracting it from its ore. The Gaseous State 💨: The kinetic theory of gases assumes that gas molecules move rapidly and randomly, the distance between gas molecules is much greater than the diameter of the molecules, there are no forces of attraction or repulsion between the molecules, and all collisions between particles are elastic. The Liquid State 💧: When a solid is heated, the energy transferred makes the particles vibrate more vigorously, the forces of attraction between the particles weaken, and the solid changes to a liquid (melting). In a liquid, particles are close together but have enough kinetic energy to slide past each other. Vaporization is the change from the liquid state to the gas state, and the energy required for this change is called the enthalpy change of vaporization. The Solid State 🧱: Solids have fixed shape and volume, with particles touching each other and usually arranged in a regular pattern. The state of a substance at room temperature and pressure depends on its structure and bonding, including simple atomic, simple molecular, giant ionic, giant metallic, and giant molecular structures.