Chapter 2: the Structure of the Atom
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1 Chapter 2: the Structure of the Atom exists in MATTER made of goes through Solid Liquid Gas differs in Melting Freezing Boiling Condensation Sublimation consists of Atoms Arrangement of particles Movement of particles Attraction forces between particles Energy content can be explained by Kinetic theory of matter Subatomic particles Isotopes Proton Electron Neutron Proton Number Electron Arrangement Nucleon Number Atomic Structure Ionic Formula Relative Atomic Mass Position in Periodic Table concept mole Chemical compound Chemical equation
2 A) Matter 1 Matter - Is anything that occupies space and has mass - Is made up of tiny and discrete particles - There are spaces between these particles - These particles may be atoms, molecules or ions - Matter exists in three states solid, liquid and gas 2 Element - Is a substance that consists of only one type of atom 3 Compou nd - Is a substance that contains two or more elements that are chemically bonded together - Molecule, Ion 4 Atom - An atom is the smallest particle of an element that can participate in a chemical reaction - Metals and some non metals such as carbon and helium exist as atoms - Fe, Al, Mg, Au 5 Molecule - Is a group of two or more atoms which are chemically bonded together - O 2, H 2, H 2 O, CO 2 6 Ion - Is a positively-charged or negatively-charged particle - Sodium Chloride, NaCl: Na +, Cl - 7 Diffusion - Occur when particles of a substance, move in between the particles of another substance - Occur most rapidly in gases, slower in liquids and slowest in solids 8 The Kinetic Theory of Matter i Solid - a solid has a fixed volume and shape - a solid cannot be compressed - the particles are packed closely together in an orderly manner - there are strong forces between the particles - the particles can only vibrate and rotate about their fixed positions ii Liquid - a liquid has fixed volume It does not have a fixed shape but takes the shape of the container - a liquid cannot be compressed easily - The particles are packed closely together but not in orderly arrangement - The particles are held together by strong forces but weaker that the forces in a solid - The particles can vibrate, rotate and move through the liquid They collide against each other
3 iii Gas - a gas does not gave a fixed shape or volume - a gas can be compressed easily - the particles are very far apart from each other and in a random motion - there are weak forces between the particles,the particles can vibrate, rotate and move freely The rate of collision is greater that the rate of collision in a liquid 9 The change in the state of matter 1 0 Sublimation Solid Gas Heat energy is absorbed Melting Solid Liquid Heat energy is absorbed Evaporation or Boiling Liquid Gas Heat energy is absorbed Freezing Liquid Solid Heat energy is released Sublimation Gas Solid Heat energy is released Condensation Gas Liquid Heat energy is released The kinetic theory of matter i when a solid is heated, - the particles in the solid gain kinetic energy and vibrate more vigorously - the particles vibrate faster as the temperature increases until the energy they gained is able to overcome the forces that hold them at their fixed positions - At this point, the solid becomes a liquid This process is called melting - Melting point is the temperature at which a solid changes into a liquid at a particular pressure - Example: Naphthalene C 10 H 8
4 - The curve shows the changes in temperature when solid naphthalene melts At point A - naphthalene exists as solid - When the solid is heated, heat energy is absorbed This cause the particles to gain kinetic energy and vibrate faster - This is why the temperature increases from point A to point B At point B - solid naphthalene begins to melt - during the melting process, the temperature 0 Cof naphthalene does not rise, even though heating continues - the temperature remains constant because the heat energy absorbed by the particles is used to overcome the forces between particles - the solid can turn into liquid - this constant temperature is the melting point of naphthalene - at this temperature, both solid and liquid are present At point C - all the solid naphthalene has melted - from point C to D, the particles in liquid naphthalene absorb heat energy and move faster - the temperature increases from point C to point D
5 ii When a liquid is cooled / freezing - the particles in the liquid lose energy and move slower - As the temperature continues to drop, the particles continue to lose more energy until they do not have enough energy to move freely - At this point, the liquid changes into solid This process is called freezing - Freezing point is the temperature at which a liquid changes into a solid at a particular pressure - Example: Naphthalene, acetamide
6 B) The Atomic Structure 1 John Dalton ( ) - Atom as a small, invisible ball similar to a very tiny ball 2 JJ Thomson ( ) - He discovered electron - He described the atom as sphere of positive charge which contains a few negatively charged particles called electron 3 Ernest Rutherford ( ) - He discovered proton, a positive charge in an atom - The positive charge and most of the mass of the atom are concentrated in a small, central region called nucleus - The electrons move in a space that is lager than the space occupied by the nucleus - 4 Neils Bohr ( ) - he proposed that the electrons in an atom move in shells around the nucleus 5 James Chadwick ( ) - He proved the existence of neutrons, the neutral particles in the nucleus - Neutrons contribute approximately to half the mass of an atom
7 Subatomic particles of an atom 1 Proton - Symbol: P Relative electric charge: +1 Relative mass: 1 2 Neutron - Symbol: N Relative electric charge: 0 Relative mass: 1 3 Electron - Symbol: e Relative electric charge: -1 Relative mass: Approximately 1 ~ Nucleus - Contain proton and neutron - Most of the mass of an atom is concentrated in the nucleus - The nucleus has an overall positive charge due to the positively-charged protons in it 5 Proton number - The number of proton in its atom 6 Nucleon number 7 Symbols of elements 8 Standard representati on for an atom - The total number of protons and neutrons in its atom - Nucleon number = number of proton + number of neutrons - Number of neutron = Nucleon number Proton number Element Symb ol Elemen t Symb ol Element Symbo l Elemen t Symb ol Hydrogen Carbon Sodium Sulphur Helium Nitroge n Magnesiu m Chlorin e Lithium Oxygen Aluminiu Argon m Beryllium Fluorin e Silicon Potassi um Boron Neon Phosphor Calciu us m - - number of proton = 9, number of neutron = 19 9 = 10, number of electron = 9
8 9 Isotopes 1 0 Number of proton Number of neuron Number of electron 12 6 C Ne K Br - Isotopes are atoms of the same element (same number of proton) with different number of neutrons - Examples: Hrogren-1, Hydrogen-2, Hydrogen-3, Chlorine-35, Chlorine-37 Uses of Isotopes Isotopes Cobalt-60 Gamma rays of cobalt-60 Carbon-14 Phosphorous-32 Sodium-24 Electron arrangement Uses used in radiotherapy for the treatment of cancer used to destroy bacteria in food without changing the quality of food - Also know as electronic configuration estimate the age of fossils and artefacts study the metabolism of phosphorus in plants Used to detect leaks in pipes carrying gas - For atoms with the proton numbers of 1 to 20, - First shell: 2 electrons - Second shell: 8 electrons - Third shell: 8 electrons - Example: Cl For atoms with more than 20 electrons, the third shell can accommodate up to 18 electrons - Example: Rubidium, Rb
9 11 Valence electrons - Valence electrons are electrons found in the outermost occupied shell of an atom - Example, Cl, 287 The valence electrons of a chlorine atom are 7 Important information based on the electron arrangement Element Mg Cl K O Ca Si Proton number Electron arrangement Number of valence electron Number of shells Position in periodic Group 2, Group Group 1 Group table Period 3 12, Period 3 Period 4 16 Period 2
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