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Pressure ​ ​ The force applied per unit area.

STP (Standard Temperature and Pressure) Grade 10 SABIS SABIS A set of conditions (0°C and 1 atm) used as a reference for gas laws and other calculations.

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Law of Conservation of Mass Grade 10 SABIS SABIS Same as Conservation of Mass.

Vaporization of ethanol Grade 10 SABIS SABIS Endothermic

Collision Theory: SABIS Grade 10 SABIS ​ 1) For a reaction to proceed, particles of reactants must collide with one another.2) Particles must collide with the minimum amount of energy needed to react called the activation energy. Such collisions are called effective or successful collisions.3) To increase the rate of a chemical reaction, it is required to increase the frequency of effective collisions, i.e increase the number of successful collisions per unit time.

< Back Chapter 4: Electrochemistry Learn about the study of chemical reactions involving the transfer of electrons and their applications in various fields. Chapter 4: Electrochemistry - This chapter explores the relationship between electricity and chemical reactions. Students will learn about oxidation-reduction reactions, electrochemical cells, and the Nernst equation. The chapter also covers the applications of electrochemistry, including batteries and electrolysis. Previous Next

Chapter 7 PDF Grade 10 SABIS ​ Elements Monoatomic Gaseous Elements Diatomic Gaseous Elements Liquid Elements Inert Elements Halogens Alkali Metals Transition Metals Properties of Elements Physical Properties Metals Non-Metals Specific Properties Graphite Iodine Potassium Properties of Group I Elements Physical Properties Chemical Properties Periodic Table Structure Rows and Columns Position of Metals and Non-Metals Chemical Reactions Alkali Metals with Various Elements Halogens with Various Elements Displacement Reactions Compounds Types of Compounds Ionic Compounds Molecular Compounds Isoelectronic Species Specific Compounds Alkali Metal Hydrides Alkali Metal Halides Hydrogen Halides Chemical Tests Flame Test for Alkali Metals Identification of Halide Ions Identification of Unknown Alkali Halide Chemistry of Third-Row Elements Hydrides Chlorides Oxides Chemical Reactivity in the Periodic Table Reactivity of Various Groups Additional Exercises and Notes 1819 Level L Chemistry Chapter 7 Notes (2) .pdf Download PDF • 682KB

Alkali metals are very unstable: they react vigorously with O2, Cl2, H2 and water forming stable compounds. Grade 10 SABIS ​

Stoichiometric Calculations Grade 10 SABIS SABIS These calculations involve using the coefficients from a balanced chemical equation to calculate the amounts of reactants or products involved in the reaction.

Know the meaning of bond energy of the hydrogen molecule Grade 10 SABIS ​ The bond energy of the hydrogen molecule refers to the amount of energy required to break the bond between two hydrogen atoms and separate them completely. It represents the strength of the chemical bond holding the hydrogen atoms together in a molecule. In a hydrogen molecule (H2), the two hydrogen atoms are bonded together by a covalent bond. This bond forms when the two hydrogen atoms share their electrons, resulting in a stable molecule. The bond energy is a measure of the stability of the hydrogen molecule. It quantifies the energy needed to overcome the attractive forces between the positively charged nuclei and the negatively charged electrons in order to separate the hydrogen atoms. To break the bond and separate the hydrogen atoms, energy must be supplied to overcome the attractive forces and pull the atoms apart. The bond energy is the minimum energy required to achieve this separation. The bond energy of the hydrogen molecule is typically expressed in units of energy per mole (kJ/mol). It represents the average bond energy over a large number of molecules and can vary slightly depending on the specific conditions and molecular environment. The bond energy of the hydrogen molecule is relatively high, indicating a strong covalent bond between the hydrogen atoms. It reflects the stability and strength of the bond, which influences the reactivity and physical properties of hydrogen compounds. Knowing the bond energy of the hydrogen molecule allows us to understand and predict various chemical reactions involving hydrogen. Reactions that involve breaking or forming hydrogen bonds can be analyzed based on the energy difference between the bond energies of the reactants and products. For example, if a chemical reaction involves breaking the hydrogen molecule into individual hydrogen atoms, the bond energy represents the energy released when the bond is broken. On the other hand, if the reaction involves forming a hydrogen molecule, the bond energy represents the energy required to form the bond. The bond energy of the hydrogen molecule is an essential concept in understanding chemical bonding, thermodynamics, and reaction kinetics. It provides insights into the energy changes associated with chemical reactions and plays a crucial role in various fields, including chemistry, biochemistry, and material science. In summary, the bond energy of the hydrogen molecule refers to the energy required to break the bond between two hydrogen atoms and separate them completely. It represents the strength and stability of the covalent bond holding the hydrogen atoms together. Understanding the bond energy of the hydrogen molecule is important in analyzing chemical reactions and predicting the energy changes involved.

Calculate H of a reaction as Σbonds broken − Σbonds formed Grade 10 SABIS ​ Calculating ΔH (enthalpy change) of a reaction using the sum of bonds broken minus the sum of bonds formed is a fundamental concept in thermochemistry. This method is based on the idea that the enthalpy change of a reaction is determined by the energy required to break the existing bonds in the reactants and the energy released when new bonds are formed in the products. To calculate ΔH using this approach, we start by identifying the bonds present in the reactants and the products. Each bond is associated with a specific bond energy, which represents the energy required to break that bond. The sum of bonds broken refers to the total energy required to break all the bonds in the reactants. This is determined by adding up the bond energies of all the bonds in the reactant molecules. Similarly, the sum of bonds formed refers to the total energy released when new bonds are formed in the products. This is determined by adding up the bond energies of all the bonds in the product molecules. Once the bond energies for the bonds broken and formed are determined, we subtract the sum of the bond energies of the bonds formed from the sum of the bond energies of the bonds broken. The resulting value represents the enthalpy change of the reaction, ΔH. For example, let's consider the combustion of methane (CH4) to form carbon dioxide (CO2) and water (H2O). We know the bond energies for the C-H, C=O, and O-H bonds involved in this reaction. By subtracting the sum of the bond energies for the bonds formed (C=O and O-H) from the sum of the bond energies for the bonds broken (C-H), we can calculate the enthalpy change, ΔH, for this reaction. It's important to note that the bond energies used in these calculations are typically average values and can vary depending on the specific molecular environment and conditions. Additionally, bond energy calculations assume that all bonds in a molecule have equal energy, neglecting any effects of neighboring atoms or functional groups. Calculating ΔH as the sum of bonds broken minus the sum of bonds formed provides a valuable approach to estimate the enthalpy change of a reaction without relying on direct experimental measurements. It allows us to understand the energy changes associated with the breaking and forming of chemical bonds during a reaction. In summary, calculating ΔH of a reaction as the sum of bonds broken minus the sum of bonds formed involves determining the bond energies for the bonds broken and formed in the reactants and products. By subtracting the sum of the bond energies for the bonds formed from the sum of the bond energies for the bonds broken, we can calculate the enthalpy change of the reaction. This approach provides insights into the energy transformations occurring in chemical reactions and aids in understanding the thermodynamic behavior of systems.