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< 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

< 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.

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 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.

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