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Chemistry Core Lesson 1

Chemistry Core Lesson 1. http://www.privatehand.com/flash/elements.html All must Know that all substances are made of atoms. know and define the term element . be able to name several elements be able to find several elements in the Periodic Table . Most should

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Chemistry Core Lesson 1

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  1. Chemistry Core Lesson 1 • http://www.privatehand.com/flash/elements.html • All must • Know that all substances are made of atoms. • know and define the term element. • be able to name several elements • be able to find several elements in the Periodic Table . • Most should • Know the layout of the Periodic Table • Be able to use chemical symbols. • http://clipbank/espresso/clipbank/servlet/link?macro=setresource&template=vid&resourceID=1618&taxonomyNodeID=731

  2. Chemistry Core • What is an element? • An element is a single pure substance which cannot be broken down into anything simpler. • An element is made of identical atoms. • What is an atom? • Atoms are small spheres. • The atoms of one element are different from the atoms of every other element.

  3. Where are all elements listed? • In the Periodic Table – a list of all known elements. • Why use symbols? • It’s simpler than writing long names! • Symbols are known all over the world even in different languages. • E.g. S is always sulphur, even though the Japanese for sulphur is iwo, the Spanish is azufre and the French is soufre • Rules For Symbols: • Either one capital letter e.g. C carbon • OR one capital letter and one lower case letter • E.g. Zn zinc

  4. The Periodic Table • The Periodic Table is divided up: • Into metal and non metals – where? • Metals and non metals are separated by a zigzag starting to the LEFT of Boron – where is this? • Into Groups – where and why? • Groups are VERTICAL COLUMNS of similar elements. • Into Periods where? • Periods are HORIZONTAL ROWS.

  5. Chemistry and Our Earth

  6. Interactive Periodic Table • http://www.absorblearning.com/media/attachment.action?quick=tf&att=2108 • http://www.bbc.co.uk/learningzone/clips/groups-and-periods-in-the-periodic-table/10623.html

  7. Structure of the Atom • All must • know that atoms are made up of smaller sub atomic particles. • know the mass, charge and position in the atom of protons, neutrons and electrons and the charge on an atom. • Most • should be able to use element symbols in the Periodic Table to work out the numbers of sub atomic particles in atoms of any element • Work out the electron arrangement for any element for the first 20 elements in the Periodic Table.

  8. Atomic Structure • http://clipbank/espresso/clipbank/servlet/link?macro=setresource&template=vid&resourceID=3495&taxonomyNodeID=731

  9. Structure of an Atom • Atoms have a small central nucleus containing protons and neutrons • Electrons orbit the nucleus • Protons, neutrons and electrons have different masses and charges Structure of an Atoms

  10. Atomic structure Atomic Structure

  11. Atomic structure Atomic Structure

  12. Atomic number • The atomic number is the number of protons in the nucleus • In an atom, the number of electrons always equals the number of protons • Atoms do not have an overall electrical charge Atomic Number

  13. Atomic number Atomic Number

  14. Mass number • The mass number is the total number of protons and neutrons in an atom • The number of neutrons can be calculated by subtracting the atomic number from the mass number Mass Number

  15. Mass number Mass Number

  16. Calculations Calculations

  17. Electron arrangements • Electrons move around the outside of the atom in an ‘electron cloud.’ • In the cloud are shells or energy levels where electrons have similar energy. • Electron shells fill from the nucleus out. • Each shell holds a maximum number of electrons. • When it is full the next shell out starts to fill. • http://www.btinternet.com/~chemistry.diagrams/electron_adding.htm • http://www.footprints-science.co.uk/flash/periodic.swf

  18. What is the Electron Cloud Model?

  19. Electron Arrangement • http://clipbank/espresso/clipbank/servlet/link?macro=setresource&template=vid&resourceID=2056&taxonomyNodeID=731 • 1st shell = up to 2 electrons (nearest to the nucleus) • 2nd shell up to 8 electrons • 3rd and subsequent shells APPEAR full at 8 electrons.

  20. Electron Arrangement • Work out the electron arrangement for the following: • Li • Na • K • F • Cl • He • Ne • Ar

  21. Electron Arrangement • Elements in the same GROUP of the Periodic Table have the SAME number of electrons in their outer electron shell. • How does this affect the properties of the elements? • Some groups have names. • E.g. Group 1 contains the Alkali Metals

  22. The Alkali Metals • Physical Properties • http://www.rsc.org/Education/Teachers/Resources/Practical-Chemistry/video-clips/physical-properties-of-group-1-elements.asp • Chemical Properties • Reaction with Water • Burning in Oxygen • Word and Formula Equations

  23. Reaction with Water Conclusion? Elements in the same group of the Periodic Table have similar reactions because they have the same number of electrons in their outer shell.

  24. Alkali Metals + Water • http://clipbank/espresso/clipbank/servlet/link?macro=setresource&template=vid&resourceID=1503&taxonomyNodeID=735 • http://www.bbc.co.uk/learningzone/clips/alkali-metals/4407.html • http://www.rsc.org/Education/Teachers/Resources/Practical-Chemistry/video-clips/caesium-with-water-longer.asp • http://www.rsc.org/Education/Teachers/Resources/Practical-Chemistry/video-clips/rubidium-with-water-longer.asp

  25. Reaction with oxygen Gas jar Burning metal Heat the metal on the burning spoon. Plunge into gas jar of oxygen as shown. Record observations. http://clipbank/espresso/clipbank/servlet/link?template=vid&macro=setResource&resourceID=1489

  26. Equations for the Reactions • Example equations: • All group 1 elements behave in the same way so have the same equations. • Sodium + oxygen sodium oxide • 4Na +O2  2Na2O • Potassium + water  potassium hydroxide + hydrogen • 2K +2H2O  2KOH + H2 • http://www.chemistryhelp.net/basic-chemistry/word-equations

  27. Noble Gases Group 8 or 0 Full outer electron shells. Do not form compounds. Uses reflect lack of reactivity. e.g. Argon in light bulbs prevents metal filament from burning. Do glow when electric current is forced through gas at low pressure.

  28. Equations Unit 1: Chemistry and Our Earth

  29. products reactants Reactants and products Inachemicalreaction,oneormorenewsubstancesareformed. The starting substances used in a reaction are reactants. The newsubstances formed in a reaction are products. The arrow means change into. In a chemical reaction, all the reactants change into the products. It is difficult to reverse a chemical reaction and change the products back into the reactants.

  30. S O2  SO2 +  + What is a symbol equation? A symbol equation uses the formulae of the reactants and products to show what happens in a chemical reaction. A symbol equation must be balanced to give the correct ratio of reactants and products. This equation shows that one atom of sulfur (S) reacts with one molecule of oxygen (O2) to make one molecule of sulfur dioxide (SO2).

  31. Balancing equations activity

  32. Symbol equations – balanced or not?

  33. Interactive Equation Balancing • http://www.files.chem.vt.edu/RVGS/ACT/notes/scripts/bal_eq1.html • http://education.jlab.org/elementbalancing/index.html • http://funbasedlearning.com/chemistry/chemBalancer/default.htm

  34. What is a chemical reaction? • All must know that elements react when atoms join with other atoms to form compounds. • Most should know how atoms combine and the names given to different types of bonding. • Some could EXPLAIN how bonding occurs in different types of materials.

  35. Chemical Bonds

  36. Reaction with chlorine Gas jar Burning metal Heat the metal on the burning spoon. Plunge into gas jar of chlorine as shown. Record observations. http://www.youtube.com/watch?v=2mzDwgyk6QM

  37. Chemical Reaction • Takes place by • GIVING • TAKING • Or SHARING electrons.

  38. Metal + Non metal • Metals GIVE electrons to non metals. • Atoms become charged IONS. • These attract each other. • http://www.absorblearning.com/media/attachment.action?quick=sn&att=2052

  39. Ionic Bonding • An ionic bond is formed when a metal atom and a non-metal atom combine • The metal atom donates an electron to the non-metal atom • The metal atom becomes a positively charged ion, the non-metal atom becomes a negatively charged ion • The positive ion attracts the negative ion – an ionic bond Ionic Bonding

  40. Ionic Bonding Ionic Bonding

  41. Ionic Bonding Ionic Bonding

  42. Ionic bonding Ionic Bonding

  43. IONIC BONDbond formed between two ions by the transfer of electrons

  44. 1). Ionic bond– electron from Na is transferred to Cl, this causes a charge imbalance in each atom. The Na becomes(Na+) and the Cl becomes(Cl-), charged particles or ions.

  45. COVALENT BONDbond formed by the sharing of electrons http://www.absorblearning.com/media/attachment.action?quick=sw&att=2070

  46. Non metal +Non metal - Element Non metal atoms SHARE ELECTRONS to gain FULL OUTER SHELLS. e.g. Cl2 Shared pair of electrons = covalent bond.

  47. Covalent Bonds

  48. Non metal + Non metal - Compound Hydrogen chloride formation Shared pair of electrons = covalent bond

  49. Molecules of Covalent Materials

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