1 / 136

Investigating Metal Properties & Implications in Matter

Explore the atomic structure, electron shells, and properties of metals such as reactivity, conductivity, and uses in this science inquiry. Discover how metal properties relate to their behavior in reactions and their extraction from ores.

harrist
Download Presentation

Investigating Metal Properties & Implications in Matter

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Year 11 Science 1.7 Investigate the implication of metal properties.

  2. Matter? • Matter is simply what the universe is made of; atoms, subatomic particles, dark matter (and goodness knows what else). • This year we will focus on atoms and their subatomic particles.

  3. Matter has 3 states. • Matter comes in 3 main states; solid, liquid and gas. • From last year you will remember, the state depends on how close together the atoms are and how much kinetic energy they have. • Solid; close together, low kE. • Liquid; further apart, some kE. • Gas; really far apart, lots of kE.

  4. Atoms; the smallest unit of matter.

  5. What is an atom made of?

  6. Elements. • Elements are atoms with a fixed number of protons. • Elements can lose or gain electrons and become ions. • Elements can come in different forms which have a different number of neutrons, these are called isotopes.

  7. Working out what an element looks like (revision from Year 10) • Atomic mass; always the bigger number. Proton number + Neutron number • Atomic number; always the smaller number. Proton number and electron number • Electron shells are filled; 2,8,8 So 9Be4 has 4 electrons, 4 protons & 5 neutrons, with a shell arrangement of 2,2.

  8. Draw these elements. • 24 Mg 12 • 11 B 5 • 20Ne10

  9. Draw these isotopes. • 10 B 5 • 11 B 5 • 12 B 5 Why are all of these atoms still Boron?

  10. Electron shells. • When filling electron shells you must follow the 2,8,8 rule. • 2 in the first shell, 8 in the second and 8 in the third. • This will be important when we get to ions too. • Complete Pg 55.

  11. STOP; Glossary • Atomic mass- the number of protons and neutrons in the nucleus. • Atomic number- the number of protons or electrons • Electron- a negatively charged particle. • Electron shell- where electrons are found (2,8,8) • Neutron- a particle with no charge. • Proton- a positively charged particle.

  12. Elements. • An element is an atom with a set number of protons. They are found on the periodic table of the elements.

  13. Columns; similar properties The table tells you…lots! • Tim & Moby Rows; proton number increases

  14. On your periodic table shade in and Indicate vertical columns – groups Indicate horizontal columns – periods Alkali metals in group one Earth metals in group two Transition metals The zig-zag between the metals and the non-metal Non metals Inert gases

  15. Key Alkali metals Transition metals Noble gases Alkali Earth metals Non metals

  16. 1st 20…you gotta know them! • From last year you will remember the first 20 element names and symbols, in order. • NO?!?!? • Right lets play element bingo! • Pgs 33- 38

  17. Properties Elements in a group have the same number of outer electrons therefore have similar chemical properties. These groups have names and are normally coloured differently on the periodic table.

  18. Alkali Metals to the left Found in group one ,all shiny and light metals Doesn’t include Hydrogen They are very reactive They are one electron away from being happy (full shells) So a strong desire to bond means they are more reactive!! Watch what happens with Lithium and water

  19. Alkaline earth metals • Strongly basic • Tend to occur in nature as compounds. • Have 2 electrons to give away.

  20. Transition metals • Are in the middle • Often good conductor of electricity • Highly coloured and/or precious • E.g. copper, silver, gold They are special because the can have more than eight electrons in the shell one in from the outermost shell these are usually incomplete – variable valenacy

  21. Non metals to the right • Usually poor conductors. • Have low melting points and unreactive with acids • Only nine are solid at room temp

  22. Inert gases Sometimes called noble gases All have full outer shell so happy not to react with other elements. Not reactive which is why they are called inert

  23. Glossary • Nobel gas- found in column 18, these gases have a full outer shell and do not react. • Periodic table- a list of all the elements, in order of neutron number.

  24. Metal properties • Metals are to be selected from; Na, Ca, Mg, Al, Zn, Fe, Pb and Cu. • Physical properties – melting point, colour, hardness, electrical conductivity, thermal conductivity, density, ductility, lustre and malleability. • Reactions of metals – limited to reactions between metals and oxygen, metals and water, and metals with acids • Relating the properties of metals to their reactivity and uses.

  25. Carrying out a range of reactions to observe the physical and chemical properties of metals • Gathering quality primary data; processing and interpreting primary or secondary data about conditions that affect the usefulness of metals (corrosion) • Making significant links between the properties of metals and their uses • Making significant links between the use of metals and their reactivity with oxygen, water and/or acid • Making significant links between the extraction of metals from their ores to the reactivity of the metal • Making significant links between the properties of alloys and their composition and/or application • Using a wide range of chemistry vocabulary, symbols and conventions writing balanced symbol equations for reactions

  26. Sodium- Na • Na1123 • Number protons; • Number neutrons; • Number electrons; • Arrangement; • Diagram;

  27. Physical properties- Na • Melting point; 98oC • Colour; silver, but quickly turns to grey. • Hardness; very soft. • Electrical conductivity; yes • Thermal conductivity; yes • Density; light 0.97g/cm3 • Ductility; not ductile, too soft • Lustre; very shiny, but dulls very quickly. • Malleability; malleable but soft & weak

  28. Reactions of metals- Na Sodium + Oxygen Sodium Oxide 2Na + O2  2Na2O Sodium + Water  Sodium hydroxide + Hydrogen 2Na + 2H2O  2NaOH + H2 Sodium + hydrochloric acid  Sodium chloride + Hydrogen 2Na + 2HCl  2NaCl + H2

  29. Uses- Na • Nuclear reactors; the heat produced can be used to boil water in reactors. • Extraction of titanium from its ore.

  30. Calcium- Ca • Ca2040 • Number protons; • Number neutrons; • Number electrons; • Arrangement; • Diagram;

  31. Physical properties- Ca • Melting point;  839.0 °C • Colour; silver, but quickly turns to grey. • Hardness; soft. • Electrical conductivity; yes • Thermal conductivity; yes • Density; light 1.55g/cm3 • Ductility; yes, but weakly • Lustre; very shiny, but dulls very quickly. • Malleability; malleable

  32. Reactions of metals- Ca Calcium + Oxygen Calcium Oxide Ca + O2  Calcium + Water  Calcium hydroxide + Hydrogen Ca + H2O  Calcium + hydrochloric acid  Calcium chloride + Hydrogen Ca + HCl 

  33. Uses- Ca • A reducing agent in the extraction of other metals, such as uranium, zirconium, and thorium. • A deoxidizer, desulfurizer, or decarbonizer for various ferrous and nonferrous alloys. • An alloying agent used in the production of aluminium, beryllium, copper, lead, and magnesium alloys. • In the making of cements and mortars to be used in construction. • In the making of cheese, where calcium ions influence the activity of rennin in bringing about the coagulation of milk.

  34. Magnesium- Mg • Mg1224 • Number protons; • Number neutrons; • Number electrons; • Arrangement; • Diagram;

  35. Physical properties- Mg • Melting point; 650oC • Colour; silver, but dulls to dark grey. • Hardness; soft. • Electrical conductivity; yes • Thermal conductivity; yes • Density; low 1.7g/cm3 • Ductility; yes • Lustre; very shiny, but dulls very quickly. • Malleability; malleable but soft.

  36. Reactions of metals- Mg Magnesium + Oxygen Magnesium Oxide Mg + O2  Magnesium + Water  Magnesium hydroxide + Hydrogen Mg + H2O  Magnesium + hydrochloric acid  Magnesium chloride + Hydrogen Mg + HCl 

  37. Uses- Mg • Fireworks, sparklers & flares. • As an alloying agent to make aluminium-magnesium alloys, sometimes called "magnalium" or "magnelium". Since magnesium is less dense than aluminium, these alloys are prized for their relative lightness and strength.

  38. Aluminium- Al • Al1327 • Number protons; • Number neutrons; • Number electrons; • Arrangement; • Diagram;

  39. Physical properties- Al • Melting point; 660oC • Colour; silver. • Hardness; relativity soft. • Electrical conductivity; a good conductor. • Thermal conductivity; excellent. • Density; 2.7g/cm3 • Ductility; it is ductile. • Lustre; very shiny, but dulls over time. • Malleability; highly malleable.

  40. Reactions of metals- Al Aluminium + Oxygen Aluminium Oxide Al + O2  Aluminium + Water  Aluminium hydroxide + Hydrogen Al + H2O  Aluminium + hydrochloric acid  Aluminium chloride + Hydrogen Al + HCl 

  41. Uses- Al • Soft drink cans. • Plane & car construction (light weight). • Foil for food storage & cooking. • Construction (windows, doors etc). • Power lines & poles, street lights. • Cases for electrical goods.

  42. Zinc-Zn • Zn 3065 • Number protons; • Number neutrons; • Number electrons; • Electron arrangement; 2, 8, 18, 2 As a transition metal, the electrons are highly mobile.

  43. Physical properties- Zn • Melting point; 420oC • Colour; blue-ish white. • Hardness; Relativity hard. • Electrical conductivity; yes • Thermal conductivity; yes • Density; 7.4g/cm3 • Ductility; yes • Lustre; very shiny. • Malleability; highly malleable.

  44. Reactions of metals- Zn Zinc + Oxygen Zinc Oxide Zn + O2  Zinc + Water  Zinc hydroxide + Hydrogen Zn + H2O  Zinc + hydrochloric acid  Zinc chloride + Hydrogen Zn + HCl 

  45. Uses- Zn • Galvanization, which is the coating of iron or steel to protect the metals against corrosion. • Brass, which is an alloy of copper and zinc, has been used since at least the 10th century BC. • Sacrificial metal on boats.

  46. Iron- Fe • Fe2656 • Number protons; • Number neutrons; • Number electrons; • Arrangement; 2, 8, 14, 2

More Related