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Flashcards

Ionic and Covalent Bonding

eimearkelly3 Chemistry Leaving Certificate Inglês 53 flashcards

Flashcards do conjunto (53)

  1. 1CompoundTwo or more elements chemically combined
  2. 2Give one way in which compounds can be broken down into their elements.Electrolysis
  3. 3Hydrated substances containmolecules of water in definite proportions
  4. 4How can water of crystallisation be driven off?Heating
  5. 5Water of crystallisationWater chemically combined in definite proportions in a crystalline compound.
  6. 6ValencyThe number of bonds an atom forms when it reacts.
  7. 7Octet ruleAtoms on reaction tend to a stable electron arrangement with eight electrons in its outer shell.
  8. 8Exceptions to the octet ruleBeryllium and boron
    Sulfur and phosphorous
    D-block elements
    Hydrogen, helium, lithium (2 in outer shell)
  9. 9Valency of group 1I
  10. 10Valency of group 2II
  11. 11Valency of group 3III
  12. 12Valency of group 4IV
  13. 13Valency of group 5III
  14. 14Valency of group 6II
  15. 15Valency of group 7I
  16. 16Valency of group 00
  17. 17Why is helium safer than hydrogen in balloons and blimps although they both have low densities?Helium is not flammable
  18. 18Why is argon added to light bulbs?To prevent the tungsten filament for melting or reacting
  19. 19Ionic bonding typically happens betweenMetals and non-metals
  20. 20Ionic bondThe electrostatic force of attraction between oppositely charged ions.
  21. 21Positively charged ionsCations
  22. 22Is the cation generally larger or smaller than the corresponding atom?Smaller
  23. 23Do the metals or the non-metals become cations?Metals
  24. 24Negatively charged ionsAnions
  25. 25Do metals or non-metals generally become anions?Non-metals
  26. 26Is the anion generally larger or smaller than the corresponding atom?Larger
  27. 27Electrons are ...... in ionic bondingTransferred
  28. 28Everyday examples of ionic substancesTable salt (food preservation and flavouring)
    Brine (a solution of sodium chloride used for curing bacon --> preservation)
    Salt tablets (taken to replace salt lost by the body through sweat)
    Fluoride compounds (sodium fluoride - prevents food decay - added to water and occasionally toothpaste)
  29. 29Characteristics of ionic substancesSolids - high melting and boiling points
    Conduct electricity when molten or in aqueous solution (electrolytes)
    Soluble in water
  30. 30Electrons in a covalent bond areShared
  31. 31Each shared pair isA covalent bond
  32. 32Electron pairs involved in bonding are calledBonding pairs
  33. 33Electron pairs not involved in bonding are calledLone pairs
  34. 34Ionic bonding results in the formation ofA rigid 3D crystal lattice
  35. 35Covalent bonding results in the formation ofMolecules
  36. 36Covalent bonds form betweenNon-metals
  37. 37Double covalent bonds form betweenoxygen atoms
  38. 38Triple covalent bonds form betweenNitrogen atoms
  39. 39Two s orbitals overlappingsigma bond
  40. 40Pi bondTwo p orbitals overlapping sideways
  41. 41The strength of covalent bonds can be measured byBond dissociation energies
  42. 42Electrons shared equallyNon-polar / pure covalent bond
  43. 43What two factors dictate the extent to which the shared electrons are attracted by different nucleiSize of the atom
    The nuclear charge
  44. 44Electrons shared unequallyPolar covalent
  45. 45Characteristics of covalent compoundsLiquids or gases at room temperature
    Low melting and boiling points
    Not soluble in water (except polar covalent)
    Do not conduct electricity (neutral molecules)
  46. 46Examples of covalent compoundsPolar solvent = water
    Polar = glucose
    Non-polar solvent = cyclohexane
    Non-polar = petrol or oil
  47. 47ElectronegativityA measure of the relative attraction an atom has for the shared pair of electrons in a covalent bond.
  48. 48What is the most common scale of electronegativity?Pauling scale
  49. 49The higher the electronegativity valueThe better it is at attracting the shared electrons towards itself
  50. 503 factors responsible for the variation in electronegativity valuesNuclear charge
    Atomic radius
    Screening effect of inner shell electrons
  51. 51Difference of more than 1.7Ionic
  52. 52Difference of 0 or very littlePure covalent / non-polar covalent
  53. 53less than 1.7polar covalent

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Leaving Certificate Chemistry (Ionic and Covalent Bonding) FlashCards sobre Ionic and Covalent Bonding, criado por eimearkelly3 em 24-07-2013.
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eimearkelly3
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