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3A- The Periodic Table

pareya English 32 cards

Cards in this deck (32)

  1. 1Properties with Water 1) Lithium?2) 2)Sodium?2) 3) Potassium?2) 4) What occurs between Sodium and the law of 'triads'?3)1) Fizzes gently- hydrogen given off
    2) Fizzes- hydrogen given off
    3) Fizzes violently- hydrogen given off
    4) The RAM of Sodium is the mean of Lithium and Potassium, the rate of reaction is also in between the other two, this also occurs for the other 'triads' of elements.
  2. 21) What happens with Newlands Law of Octaves?2)1) Newlands was the first to notice that if you arrange the elements in order of RAM every 8th element exhibited similar physical and chemical properties.
    This only worked for the first 16 elements and other elements were missing.
  3. 3Mendeleev's Periodic Table 1) What did Mendeleev do?2) 2) What did he do about the 'gaps' on the periodic table?1)1) He was the first to put the 60 known elements in the arrangement that they are in today. Mendeleev arranged the elements in increasing mass order but left gaps for elements that had not been discovered yet.
    2) he made it possible to predict the properties of elements that had not yet ben discovered
  4. 41) What did Henry Mosley do about the Periodic Table?2) 2) How is the modern periodic table arranged?2)1) Moseley showed that the real order of the elements in the Periodic Table is based on atomic number and not RAM, the sequence is close but not exactly the same.
    2) The elements are arranged in increasing atomic number, elements with similar properties appear in a regular pattern in the list
  5. 51) What are groups?1) 2) what are periods?1) 3) what is periodicity?1)1) A vertical column is called a group
    2) a horizontal row is called a period
    3) a regular periodic variation of properties of elements with atomic number and the position in the periodic table
  6. 6Variation in electron structure 1) what are chemical reactions due to?1) 2) what does ths mean?3)1) outer shell electrons only
    2) elements with the same number of electrons in the outer shell will react in similar ways, the vigour of the similarities will depend on shielding and the number of protons in the nucleus, this is what causes periodicity- the regular repeating patterns.
  7. 7Periodicity: Ionisation energy and atomic radii- trends across a period 1) what happens to periodic patterns as you go across a period ?5)1) the nuclear charge increases
    2) and the shielding between nucleus and outer electron shell remains the same.
    3) The increased nuclear charge pulls the electron shell closer to the nuclei.
    4) This means there is a slightly greater attraction between the nucleus and the other shell electrons.
    5) The increase in nuclear charge is the most important factor.
  8. 81) what happens as the atomic radius decreases?1 2) what are the factors affecting ionisation energies?3)1) first ionisation energy increases overall
    2) the distance of the electron from the nucleus, size of the positive nuclear charge, the shielding affect by full inner shells
  9. 9why does the decrease in atomic radius increase the first ionistion energy?5)1) As you go across a period, the nuclear charge increases
    2) As the distance between the nucleus and outer shell remains the same
    3) and as shielding between nucleus and outer electron shell remains the same
    4) The increased nuclear charge pulls the electron shell closer to the nuclei
    5) this means there is a slightly greater attraction between the nucleus and the outer shell electrons.
  10. 101) What happens as you go down a group?5)1) as you go down a group the nuclear charge increases
    2) there are more electron shells which increases shielding between nucleus and outer electron shell
    3) as there are more electron shells the distance between nucleus and outer shell increases.
    4) this means that attraction between the nucleus and outer electrons decreases
    5) distance and shielding are the most important factors , the atomic radii increases and FIE decreases
  11. 11why does the FBI decrease as you go down a group?4)1) as you go down a group the nuclear charge increases
    2) There are more electron shells which increases shielding between nucleus and outer shell
    3) as there are more electron shells the distance between nucleus and outer shell increases
    4) this means the attraction between the nucleus and outer electrons decreases
  12. 12Periodicity Bioling Points what are the general trends?3) 2) explanation?1) 3) Metallic Bonding?2)1) Increase in boiling point from Gp 1-4, Sharp drop from Gp 4-5, Low Boiling Points for Gp 5-0
    2) as you move from left to right there is a general pattern
    3) the boiling points increase as you move along group 1-3, this is due to an increase in outer electrons available to be part of the mobile sea of electrons
  13. 13Giant Covalent Structures Gp4 3) Molecular/ Atomic Groups 5-0 3)1) These are carbon and silicon, this is due to the strong covalent bonds making up a giant structure, for these to boil the strong covalent bonds must be broken by leaving single atoms
    2)these are elements that are diatomic molecules or single atoms, the intermolecular forces between these elements are Van Der Waals and therefore weak, these Van Der Waals are easily overcome separating the diatomic molecule or atoms from each other
  14. 14Group 2 1) What are there elements also called?1) 2) What happens to the reactivity as you go down group 2?1) 3) Physical properties?3) 4) Electron configuration?1)1) alkaline earth metals as their hydroxides are alkaline
    2) increases
    3) All light metals, compounds are white or colourless, reasonably high melting and boiling points.
    4) all in the s block sub shell and all have s2 electrons
  15. 15Reactivity of Group 2 elements 1) Group 2 metals are reactive, what is the general formula?1) 2) What do elements in group 2 give away durin reactions?2) 3) Gaining electrons is what type of reaction?1) 4) Why are group 2 elements good reducing agents?1) 5) Reactivity inreases as you go down grou 2 what does this mean?2)1) M -> M2+ + 2e-
    2) 2 electrons, so whatever they react with must gain electrons.
    3) Reduction
    4) as the group 2 elements cause the reduction of other compounds or elements
    5) This means they lose their electrons more readily, this means as you go down group 2 they become better reducing agents.
  16. 16Oxidation Numbers 1) What is it used to describe?1) 2) what is it used for and what does it mean?3)1) the number of electrons used to bond with another atom.
    2) it is used for combining powers of atoms, it is a type of book for keeping electrons, it is a number describing the movement of electrons and is found by the application of certain rules.
  17. 17Rules for assigning Oxidation Numbers 1) element?1) 2) atoms in a compound?1) 3)ionic element?1) 4) in a polyatomic ion?1) 5)hydrogen? except metals? 6) Gp7 Halogens? 7) oxygen?1) no. of an element =0
    2) no. of each atom in a compound counts separately they must all add up to 0.
    3) no. of an ionic element = charge on ion
    4) e.g. (SO4,2-) sum of the ox no.'s of the atoms =charge on ion.
    5) H= 1+ except with metals, metal hydrides = -1
    6) halogens = -1 except with oxygen
    7) o= -2 except in peroxides ( h2o2, o= -1)
  18. 18Oxidation numbers in chemical names 1) Some elements form compounds where they could have a different charge/oxidation?2) 2) What are oxyanions?2)1) Transition metals and Oxyanions
    2) These are negative molecules that contain an oxygen atom, Oxyanions usually end in 'ate' to indicate the presence of oxygen.
  19. 191) What is oxidation?1) 2) what is reduction?1) 3) reducing agent?1) 4) oxiding agent?1)1) addition of oxygen/ loss of hydrogen/ loss of e-
    2) loss of oxygen/ addition of hydrogen/ gain of e-
    3) loss of e-
    4) gain of e-
  20. 20Iron ions can exist a fe2+ and Fe3+ what are the colours of the solutions?2) 2) The total increase in oxidation numbers by one element is always equal to what?1) 3) What are spectator ions?1)1) fe 3+ brown and fe 2+ green
    2) equal to the total decrease in oxidation numbers by another element.
    3) when an element has not lost/ gained any electrons, it has not changed in oxidation numbers
  21. 21Reaction with Oxygen 1) Group 2 metals react vigorously with oxygen to give what?1) Reaction with Water 2) Group 2 metals react with water to give what?2) 3) what are Group 2 oxides and hydroxides?1) 4) what do group 2 oxides produce when they react with water?1) 5) group 2 hydroxides?1)1) to give the oxide
    2) hydroxide and hydrogen gas
    3) these are bases as they neutralise acids to form salts and water
    4) metal hydroxide, these are soluble so dissolve in the water forming an alkali
    5) as these are soluble they dissolve in water forming alkaline solutions
  22. 22Group 2 Hydroxides solubility?3)1) The solubility of the group 2 hydroxides increases as you go down the group, this means that as you go down group 2 more hydroxide ions are formed, this mans that as you go down group 2 they become more alkaline.
  23. 23Group 2 Carbonates 1) What happens when they're heated?1) 2) What is thermal decomposition?1) 3)general equation? 4) What happens as you go down group 2 carbonates?1)1) decompose
    2) the breaking down of a chemical substance with heat into at least 2 chemical substances
    3) MgCO3(s) -> MgO(s) + CO2 (g)
    4) harder to decompose
  24. 24Properties of Group 2 elements and their compounds?5)1) Because of periodicity we only have to learn the chemistry for one of the elements in group 2
    2) all the elements in group 2 will react in the same way ( but with different vigour)
    3) as you go down group 2: the elements become more reactive
    4) the carbonates decompose at higher temperatures
    5) the hydroxides become more soluble in water making the solution more alkaline
  25. 25Group 7 Physical Propeties?3) electronic configuration?3)1) the melting and boiling point of the halogens increases with atomic number due to increased Van Der Waals, this can be seen by their physical states at room temperature, Iodine sublimes to a purple vapour
    2) each group 7 element has7 electrons in the outer shell, each have s2p5 configuration and known are p block elements, the require 1 electron to complete their outer shell
  26. 261)Halogens as oxidising agents?3) 2)why do we say group 7 are good oxdising agents?1) 3) reactivity?2)1) these elements gain 1 electron when they react, this means whatever they react with must lose electrons, losing electrons is an oxidisation reaction
    2) as the group 7 elements cause the oxidation of other compounds or elements
    3) decreases as you go down the group this means they gain their electrons less readily, this means as you go down group 7 their oxidising power decreases
  27. 27Halogens as oxidising agents? 3) reactivity?2)1) these elements gain 1 electron when they react, this means that what ever they react with must lose electrons, losing electrons is an oxidation reaction
    2) this means they gain their electrons less readily, this means as you go down group 7 their oxidising power decreases
  28. 28Explanation why does theiroxiding power decreases?4)1) there are more electron shells which increases shielding between nucleus and outer electron shell, as there are more electron shells, the distance between nucleus and outer shell increases, this means that attraction between the nucleus and outer electrons decreases, this means the incoming electron is not captured as easily.
  29. 29Redox reactions of the halogens?5)1) Redox reactions can show how the halogens ability to form ions reduces as you go down the group
    2) by competing the halogens with the halides
    3)Each halogen is mixed with halides
    4)the more reactive Halogen will oxidise and displace the halide of a less reactive halogen
    5) Halogens are coloured in solution this can indicate whether a redox reaction has occured
  30. 301) What is a disproportion reaction?1) Properties of group 7 elements and compounds 2)what do they all form?1) 3) how will they react?1) 4) forces of attraction?1) 5) What happens as you go down the group?3)1) a reaction when the same element has been both oxidised and reduced
    2) diatomic covalent molecules
    3) same way but diff vigour
    4) vdw - Increases down the group more e-
    5) less reactive, weaker oxidising agent, form ionic halides with metals.
  31. 311) Fluroine's reactivity?2)1) most reactive element on the periodic table, it burns virtually anything in its path
  32. 32Testing for Halide Ions?5)1) dissolve a small amount of the compound in water
    2) add sliver nitrate
    3) the silver ions ag+ combines with the halide ions to form a silver halide precipitate
    4) the silver halide precipitates are coloured depending on the halide present
    5) because it is sometimes difficult to judge the colour, ammonia can be added as the different silver halides have diff solubility's in ammonia

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Flashcards on 3A- The Periodic Table, created by pareya on 16/01/2015.
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