Light the Bunsen burner – adjust it to get a roaring blue flame.You should see the continuous spectrum of visible light.This could result in permanent damage to your eyes. Hold the spectroscope up to a window which does not face the You must NEVER point the spectroscope directly at the sun.Switch on the lamp and look at the bulb through the Look for a series of colours, one running into the next.strontium chloride, SrCl 2 (s) ( IRRITANT).sodium chloride, NaCl (s) ( LOW HAZARD).potassium chloride, KCl (s) ( LOW HAZARD).calcium chloride, CaCl 2 (s) ( IRRITANT).hydrochloric acid, HCI, 1 mol dm -3 ( LOW HAZARD).electric lamp with tungsten filament or energy saving light bulb.You will be using a hand spectroscope to observe the difference between a continuous emission spectrum produced by a fluorescent and a line spectrum produced by the excitation of electrons in various elements. This experiment is designed to give you a qualitative introduction to the spectra emitted by some s-block elements when their atoms are excited by heating in a Bunsen flame. IBDP Chemistry Guide (2025 First Examination).Structure 1.5.4-The relationship between the pressure, volume, temperature and amount of an ideal gas is shown in the ideal gas equation PV = nRT and the combined gas law.Structure 1.5.3-The molar volume of an ideal gas is a constant at a specific temperature and pressure.Structure 1.5.2-Real gases deviate from the ideal gas model, particularly at low temperature andhigh pressure.All collisions between particles are considered elastic. Structure 1.5.1-An ideal gas consists of moving particles with negligible volume and no intermolecular forces.Structure 1.4.6-Avogadro’s law states that equal volumes of all gases measured under the same conditions of temperature and pressure contain equal numbers of molecules.Structure 1.4.5-The molar concentration is determined by the amount of solute and the volume of solution.The molecular formula gives the actual number of atoms of each element present in a molecule. Structure 1.4.4-The empirical formula of a compound gives the simplest ratio of atoms of each element present in that compound.Structure 1.4.3-Molar mass M has the units g mol^–1.Structure 1.4.2-Masses of atoms are compared on a scale relative to 12C and are expressed as relative atomic mass Ar and relative formula mass Mr.One mole contains exactly the number of elementary entities given by the Avogadro constant. Structure 1.4.1-The mole (mol) is the SI unit of amount of substance.Structure 1.4-Counting particles by mass: The mole.Structure 1.3.7-Successive ionization energy (IE) data for an element give information about its electron configuration.Structure 1.3.6-In an emission spectrum, the limit of convergence at higher frequency corresponds to ionization.Structure 1.3.5-Each orbital has a defined energy state for a given electron configuration and chemical environment, and can hold two electrons of opposite spin.Structure 1.3.4-A more detailed model of the atom describes the division of the main energy level into s, p, d and f sublevels of successively higher energies.Structure 1.3.3-The main energy level is given an integer number, n, and can hold a maximum of2n^2 electrons.Structure 1.3.2-The line emission spectrum of hydrogen provides evidence for the existence of electrons in discrete energy levels, which converge at higher energies. ![]() Structure 1.3.1-Emission spectra are produced by atoms emitting photons when electrons in excited states return to lower energy levels.Structure 1.2.3-Mass spectra are used to determine the relative atomic masses of elements from their isotopic composition.Structure 1.2.2-Isotopes are atoms of the same element with different numbers of neutrons.Negatively charged electrons occupy the space outside the nucleus Structure 1.2.1-Atoms contain a positively charged, dense nucleus composed of protons and neutrons (nucleons).Structure 1.1.3-The temperature, T, in Kelvin (K) is a measure of average kinetic energy Ek of particles.Structure 1.1.2-The kinetic molecular theory is a model to explain physical properties of matter (solids, liquids and gases) and changes of state.Structure 1.1.1 Elements are the primary constituents of matter, which cannot be chemically broken down into simpler substances.Structure 1.1-Introduction to the particulate nature of matter (SL/HL).Models of the particulate nature of matter IBDP Chemistry SL and HL (2025 Specification).Mastering the Art of Revision: Tips and Tricks to Boost Your Success.Demonstrating the IB Learner Profile Attributes in Science: Examples and Applications.IGCSE Edexcel Science Prescribed Practical Experiments: A Comprehensive Guide.2025 IBDP Biology, Chemistry and Physics Subject guides (specification).
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