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Flashcards

1. Atomic Structure and the Periodic Table

JR HN Chemistry GCSE English 49 cards

Cards in this deck (49)

  1. 1What size are atoms?Atoms are 0.1 nanometres (1x10⁻¹⁰m)
  2. 2What are the relative masses of protons, neutrons and electrons?1, 1 and very small
  3. 3Do atoms or ions have an overall charge?Atoms don't, ions do.
  4. 4Why do ions have an overall charge?The numbers of protons and electrons are not equal like in an atom.
  5. 5What do the mass number and atomic number symbolise?Mass = total number of protons and neutrons
    Number = number of protons = number of electrons
  6. 6What are isotopes?Isotopes are different forms of the same element with different numbers of neutrons.
  7. 7What determines what element an atom is?The number of protons.
  8. 8What is the relative atomic mass and why is it used as opposed to mass?Aᵣ is the average mass of all isotopes used because many elements have more than one.
  9. 9What are elements?Elements are substances containing only one type of atom.
  10. 10What is a compound and its properties?Compounds are substances containing two or more types of atom. Its properties are totally different from those of the original elements and they are inseperable by physical processes.
  11. 11What is ionic bonding?When a metal and a non-metal form a compound, the metal atoms lose electrons to form positive ions and the non-metal atoms gain them, forming negative ions. The opposite charges means they are strongly attracted.
  12. 12What is the formula for ammonia?NH₃
  13. 13How do you find the formula for an ionic compound?Find which groups the elements are in and the ions they respectively form, then ensure the charges in the compound total 0.
  14. 14How do you balance equations?1. Find the element that doesn't have the same number of atoms on each side of the equation.
    2. Pencil in a larger number to the left of it and continue until all imbalances are removed.
  15. 15What is a mixture and its properties?A mixture is made up of seperate elements or compounds mixed together with no chemical bonds between them. Its properties are consequently a mixture of the components' properties.
  16. 16What are the 5 methods used to separate mixtures?Filtration, crystallisation, simple distillation, fractional distillation and chromatography.
  17. 17What is the pattern of spots resulting from chromatography called?A chromatogram.
  18. 18What method is used to separate an insoluble solid from a liquid?Filtration.
  19. 19What is the name for a liquid something had been or will be dissolved in?A solvent e.g water, ethanol.
  20. 20What methods are used to separate a soluble solid and a solution and what is the difference?Crystallisation and evaporation; crystallisation takes longer but forms crystals that would decompose if heated.
  21. 21What method is used to separate a mixture of different coloured liquids?Chromatography.
  22. 22What method is used to separate a mixture of liquids with a significant difference in boiling point?Simple distillation.
  23. 23What method is used to separate a mixture of liquids without a significant difference in boiling point?Fractional distillation.
  24. 24What were the atomic models leading to and including the plum pudding model, and when and by who were they devised?1. (1800s) John Dalton thought atoms were solid spheres, diffferent spheres composing different elements.
    2. (1897) JJ Thomson discovered electrons using measurements of charge and mass, concluding atoms were a ball of positive charge with electrons stuck in it.
  25. 25What was the first version of the nuclear model, and when and by who was it devised?3. (1909) Ernest Rutherford did sent alpha particles at a thin sheet of gold and discovered many were deflected. Him and his student thought most would pass through due to the spread out nature of positive mass in the plum pudding model. Rutherford devised the model of a positively charged nucleus surrounded by a cloud of electrons.
  26. 26What were the second and third versions of the nuclear model, and when and by who was it devised?4. (1913) Niels Bohr suggested electrons were contained in shells, upon realising a cloud of electrons would be attracted to the nucleus and cause the atom to collapse.
    5. (1932) James Chadwick provided evidence for neutrons from his own experiments and updated this model.
  27. 27What are the maximum electron numbers for each shell?2, 8, 8, 18
  28. 28Which group's elements are least reactive?Group 0, the noble gases, because they have full outer shells.
  29. 29Why did early periodic tables have some elements in the wrong group?Elements were in order of relative atomic mass because it was all early scientists could record, the table was incomplete and their properties were not taken into account so were in the wrong groups.
  30. 30When was Mendeleev's periodic table designed and what did it look like?- 1869. They were in order of atomic mass but switched if the properties prompted it.
    - There were 50 known elements in it.
    - Gaps were left to ensure property-group relation, some of which indicated undiscovered elements and allowed Mendeleev to predict their properties.
  31. 31Why was Mendeleev correct not to put elements in a strict order of atomic mass?Isotopes of the same element have different masses but similar properties so occupy the same position on the current periodic table.
  32. 32Where are metals on the periodic table?Metals are from the centre-right to the left.
  33. 33Where are non-metals on the periodic table?Non-metals are on the far right at the top.
  34. 34In what group does reactivity increase going down and why?Group 1, atom size increases down the table and the single electron in its outer shell is further from the attraction of the positive nucleus, and is therefore easier to lose.
  35. 35In what group does reactivity decrease going down and why?Group 7, atom size increases down the table and the incomplete outer shell is further from the attraction of the positive nucleus, and the single electron needed is therefore harder to gain.
  36. 36What type of element doesn't normally form positive ions and why?Non-metals, because their atoms would have to lose a lot of electrons and it's easier to gain some to fill the outer shell.
  37. 37What type of element can form positive ions and why?Metals, because the larger atoms only have to lose one or a few electrons to have a full outer shell, and the smaller atoms' outer electrons have a strong attraction to the nucleus.
  38. 38What are the physical properties of the transition metals?Metals are...
    - Often shiny
    - Strong and malleable (bendable)
    - High boiling and melting points
    - Solid at room temp (except mercury)
    - Usually higher density
    - Good conductors.
  39. 39What are the physical properties of non-metals?Non-metals are...
    - Dull-looking
    - More brittle
    - Not always solid at room temperature
    - Usually lower density
    - Poor conductors.
  40. 40What are additional properties only transition metals have?Transition metals...
    - Can form more than one type of ion.
    - Often have colourful ions.
    - Can make good catalysts as elements or in compounds.
  41. 41What are the properties of the group 1 elements?Group 1 elements...
    - Are the alkali metals.
    - Are soft, silvery solids with a low density.
    - Have to be handled with forceps as they can cause chemical burns.
    - Decrease in melting/boiling point going down the group.
    - Form ionic compounds with non-metals.
    - Form 1+ ions.
  42. 42What are the properties of the group 7 elements?Group 7 elements...
    - Are halogens.
    - Are non-metals with coloured vapours.
    - Decrease in melting/boiling point going down the group.
    - Form ionic bonds with metals or covalent bonds with non-metals.
    - Form 1- ions.
    - More reactive halogens will displace a less reactive one.
  43. 43What are the properties of the group 0 elements?Group 0 elements...
    - Are the noble gases.
    - Are motionless, colourless gases.
    - Are unreactive and non-flammable.
    - Boiling points increase going down the group.
  44. 44How do group 1 elements (the alkali metals) react with water?They react vigorously to produce hydrogen gas and metal hydroxides, energy release increasing down the group.
  45. 45How do group 1 elements (the alkali metals) react with chlorine?They react vigorously when heated in chlorine gas to form white metal chloride salts.
  46. 46How do group 1 elements (the alkali metals) react with oxygen?If reacted with pure oxygen a metal oxide will form, which is why these metals tarnish in the air to form a metal oxide layer.
  47. 47What is a displacement reaction and in which group do the relevant elements reside?A displacement reaction is where one element replaces a less reactive one from an aqueous solution of its salt. Group 7 elements (the halogens) do this.
  48. 48How do you identify a hydroxide formed from an alkali metal and water?The hydroxide will dissolve in water to give an alkaline solution.
  49. 49What is the mnemonic for the reactivity series?Please - Potassium, Stop - Sodium, Calling - Calcium, Me - Magnesium, A - Aluminium, (Cute - Carbon), Zebra - Zinc, I - Iron, Like - Lithium, (Her - Hydrogen), Call - Copper, Smart - Silver, Goat - Gold

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GCSE Chemistry Flashcards on 1. Atomic Structure and the Periodic Table, created by JR HN on 25/09/2018.
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JR HN
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