5.1 The Gaseous State Kinetic theory of gases Assumptions made in the kinetic theory of gases as applied to ideal gases: The gas particles have zero intermolecular forces between them The gas particles behave as point particles which have negligible volume. The gas...
4.6 Metallic Bonding Metallic bonds Metallic bond is the electrostatic force of attraction between the delocalised electrons and the positive metal ions Take sodium as an example, in the solid state, sodium atoms are packed so closely together that the 3s...
4.7 Bonding and Physical Properties of Substances Physical state at room temperature 1) Ionic compounds - Ionic compounds are solids at room temperature, this is because the ionic bond holding the oppositely-charged ions is very strong, a lot of energy is...
CHAPTER 5: States of Matter The Gaseous State The Liquid State The Solid State Ceramics Conserving Materials Learning outcomes: state the basic assumptions of the kinetic theory as applied to an ideal gas explain qualitatively in terms of intermolecular forces...
4.5 Intermolecular Forces Intermolecular and intramolecular forces Intramolecular force is the force of attraction that hold individual atoms together in a molecule. Commonly referred to as covalent bonds. Intermolecular force is the force of attraction...
4.4 Electronegativity, Bond Polarity, Bond Length and Bond Energy Electronegativity Electronegativity is the ability of an atom which is covalently bonded to the other atom to attract the bond pair of electrons towards itself The more electronegative an atom is,...
4.3 Shapes of Molecules Valence shell electron pair repulsion(VSEPR) theory All electrons are negatively-charged, so they will repel each other when they are close together So, a pair of electrons in the bonds surrounding the central atom in a molecule will repel...
4.2 Covalent Bonding Formation of covalent bond Covalent bond is the electrostatic force of attraction that two neighbouring nuclei have for a localised pair of electrons shared between them Covalent bond is formed without transferring electrons, instead, the...
4.1 Ionic Bonding Formation of ionic bond Ionic bond is the electrostatic force of attraction between oppositely-charged ions formed by the complete transfer of electrons from an atom to another atom. Ionic bond is also called electrovalent bond 1. An...
3.3 Ionisation Energy What is ionisation energy? The 1st ionisation energy, ΔHi1 is the energy needed to remove one electron from each atom in one mole of the atoms of the element in the gaseous state to form one mole of gaseous 1+ ions The general...
CHAPTER 4: Chemical Bonding Ionic Bonding Covalent Bonding Shapes of Molecules Electronegativity, Bond Polarity, Bond Length and Bond Energy Intermolecular Forces Metallic Bonding Bonding and Physical Properties of Substances Learning outcomes: describe ionic...
3.2 Electronic Configuration Ways to represent electronic configuration Electronic configuration describes how the electrons in an atom/ion are arranged in their shells, sub-shells and orbitals. Using 'electrons-in-boxes': . Using energy levels: Using...
3.1 Sub-shells and Atomic Orbitals Principle quantum shell Electrons are arranged outside the nucleus in energy levels or principle quantum shell, n. The principal quantum shells are numbered according how far are they from the nucleus ...
2.5 Stoichiometry and Equations Stoichiometry Stoichiometry is the proportion of things either reacting or combining In compounds, it refers to the ratio in which the atoms are combined For example, water, H2O has a stoichiometry of 2 hydrogen to 1 oxygen. It also...
CHAPTER 3: Electrons in Atoms Sub-shells and Atomic Orbitals Electronic Configuration Ionisation Energy Learning outcomes: describe the number and relative energies of the s, p and d orbitals for the principal quantum numbers 1, 2 and 3 and also the 4s...
2.3 Amount of Substance The mole and the Avogadro's constant A mole of a substance is the amount of substance that contains the same amount of stated elementary units as there are atoms in 12 g of C-12. The number of atoms is 12 g of C-12 is 6.02 x 10²³...
2.4 Empirical Formula and Molecular Formula Percentage composition by mass Empirical formula Empirical formula is a chemical formula that shows the simplest ratio of the atoms that combine to form a molecule Steps to find empirical formula: Find the mass of...
2.2 Mass Spectrometer What is mass spectrometer? A mass spectrometer is used to determine: relative isotopic mass relative abundance of isotopes relative atomic mass relative molecular mass structural formula of compounds Determination of relative atomic...
2.1 Mass of Atoms and Molecules Concept of relative mass Relative mass is an indication of how heavy is an atom compared to another atom which is used as a standard Relative mass is expressed in atomic mass unit(a.m.u). C-12 was chosen to be the standard model...
Mass of Atoms and Molecules Mass Spectrometer Amount of Substance Empirical Formula and Molecular Formula Stoichiometry and Equations Learning outcomes: define and use the terms relative atomic, isotopic, molecular and formula masses, based on the C-12 define and...
1.1 Inside the Atom Sub-atomic particles Electrons revolve around in region of space called Electrons do not move in fixed The nucleus is made up of protons and neutrons which contains almost all the mass of the atom. This is because the mass of...
1.2 Isotopes Isotopes Isotopes are atoms of the same element with the same number of proton but different number of Example: Isotopes have the same: number of protons and electrons electronic configuration chemical properties(because they have the...