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Flashcards

Atomic structure and the periodic table C1

Emily Piepgrass Chemistry Year 9 English 51 cards

How do you draw the electronic structure of an atom using the energy levels?

Cards in this deck (51)

  1. 1What is an atom?The smallest quantity of an element.
  2. 2What is an element?A single or multiple atom(s) of the same type.
  3. 3What is a compound?Multiple atoms bonded together.
  4. 4What is a mixture?Multiple atoms that are not bonded.
  5. 5What is the difference between a mixture and a compound?In a mixture the atoms are not bonded but in a compound they are.
  6. 6What are the five ways of separating mixtures?Filtration, crystallisation, chromatography, distillation and fractional distillation.
  7. 7When would you use each seperation methodFiltration - bigger sediments
    Crystallisation - when you are trying to separate a soluble solid from a solvent.
    Chromatography - to separate mixtures of soluble substances
    Distillation - to separate a solvent from a solution.
    Fractional Distillation - to separate multiple liquids from a solution
  8. 8What was the first model of the atom and why did it change?The plum pudding model was changed because it was discovered that an atom has shells.
  9. 9What is the plum pudding model and how does it describe an atom?It describes an atom as a ball of positive charge with electrons inside.
  10. 10What did the alpha scattering experiment conclude and why did it change the atomic model?It concluded that there is a magnetic field around the nucleus and that there are different shells that electrons stay in.
  11. 11What is the difference between the plum pudding model and the nuclear model of the atom?There are shells in the nuclear model and the electrons are organised.
  12. 12How did Neils Bohr adapt the model of the atom and how did he confirm his ideas?He used the alpha scattering experiment to prove the magnetic field around the nucleus and the shells.
  13. 13Where are the protons and how did this change the model of the atom?The protons are in the nucleus of the atom.
  14. 14What did James Chadwick discover and when this occur?He discovered protons and neutrons in 1932.
  15. 15What are the particles in an atom and what are their relatives electrical charges?Proton - +1
    Neutron - 0
    Electron - -1
  16. 16Why do atoms have no overall electrical charge?Because there is an equal amount of electrons and protons.
  17. 17What is the atomic number and what does it show?The atomic number is the number of protons.
  18. 18How do atoms of different elements differ in terms of protons?Different elements have different numbers of electrons and therefore different amount of protons because there are equal amounts of protons and electrons in an atom.
  19. 19How small are atoms? What is their radius?The radius of an atom = 1x10-20
  20. 20What is the size of an atoms nucleus?The diameter of an atoms nucleus
    = 1x10-14
  21. 21Where is most of the mass of the atom?Most of the mass of an atom is in the nucleus.
  22. 22What are the relative masses of protons, electrons and neutrons.Protons - 1
    Electrons - 0
    Neutrons - 1
  23. 23What is the mass number of an atom?It is the average number of nucleons in an atom = protons + neutrons
  24. 24What is an isotope?An atom that has a different number of neutrons.
  25. 25How do you calculate the number of protons, electrons and neutrons in an atom or ion?atomic mass number - the atomic number
  26. 26What is the relative atomic mass of an element?relative mass x the percentage, repeat for all isotopes, then add then together and divide by 100.
  27. 27How do you draw the electronic structure of an atom using the energy levels?How do you draw the electronic structure of an atom using the energy levels?
  28. 28How do write the electronic structure of an atom?NE = 2.8
  29. 29How does the position of an element in the modern day periodic table relate to the atomic number and the arrangement of electrons in its atom?The group position relates to how many electrons are in the outer shell and the period they are in relates to how many shells there are.
  30. 30How were elements arranged before the discovery of protons, neutrons and electrons?Elements were ordered by atomic mass.
  31. 31What were the problems with the early periodic tables?Elements with different properties were put into the same groups and metals and non-metals were mixed.
  32. 32How did Mendeleev overcome some of these problems?He left gaps for undiscovered elements.
  33. 33What happened to the elements that Mendeleev predicted the properties?They were later discovered with the properties that Mendeleev predicted.
  34. 34How did the knowledge of isotopes explain why the atomic weight order was incorrect?Because there are many different weights that the isotope could weigh differing the order of weight.
  35. 35Where are the metals and non-metals in the periodic table?The metals are on the left side of the periodic table and the non-metals are on the right side.
  36. 36What are the differences in physical properties of metals and non-metals?Metals - shiny, malleable, ductile, heat conductors
    Non-metals - brittle, poor heat conductors, not ductile, at room temperature normally solid or liquid.
  37. 37What are the differences in chemical the properties of metals and non-metals?Metals - electropositive (lose an electron) in chemical reactions.
    Non-metals - electronegative (gains an electron) in chemical reactions.
  38. 38Where are the noble gases and why are they unreactive?They are in group 0 and they are unreactive because they have full outer shells.
  39. 39How does the boiling points of the noble gases change down the group?The boiling points increase down the group because the mass increases.
  40. 40Where are the alkali metals in the periodic table and what causes their characteristic properties?The alkali metals are in group 1 and they have an unstable electronic structure.
  41. 41How do lithium, potassium and sodium react with oxygen?Li, K, Na oxidises when in contact with oxygen causing them to lose their shine.
  42. 42How does Li, K, Na react with chlorine?Li, K, Na bond with chlorine because they want to lose one electron and chlorine needs to gain one electron.
  43. 43How does Li, K, Na react with water?Li, K, Na release hydrogen when reacting with water.
  44. 44How does the reactivity of the elements in the group 1 change down the group?The elements get more reactive down the group.
  45. 45Where are the halogens in the periodic table and why do they react similarly?The halogens are in group 7 and they react similarly to group 1 because group 7 needs to gain 1 electron and group 1 needs to lose 1 electron.
  46. 46What are the halogens and how do they exist as elements?Halogens are in group 7 and they exist as diatomic-molecules meaning they go around in pairs.
  47. 47What is formed when chlorine, bromine and iodine react with metals?A salt is formed?
  48. 48What is formed when chlorine, bromine and iodine react with non-metals?A molecular compound.
  49. 49How does the relative molecular mass, melting point and boiling point of the halogens change down the group?The relative molecular mass and melting and boiling points increase down the group.
  50. 50How does the reactivity of the halogens change down the group?The reactivity decreases down the group.
  51. 51What occurs when a more reactive halogen reacts with a less reactive halide salt?A displacement reaction occurs.

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Year 9 Chemistry Flashcards on Atomic structure and the periodic table C1, created by Emily Piepgrass on 29/04/2018.
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Emily Piepgrass
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