3.1.1-3 - Atomic Structure, AoS + Bonding Flashcards

1
Q

what is meant by ‘electronegativity’?

A

ability of an atom to attract the electron density of a covalent bond towards itself

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2
Q

what happens to electronegativity down the group?

A

electronegativity decreases
- due to increased shielding, meaning the distance between the nucleus + outer electron is greater

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3
Q

what happens to electronegativity across the period?

A

electronegativity increases
- nuclear charge increases

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4
Q

what is meant by ‘polarity’?

A

unequal sharing of electrons in a bond

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5
Q

how do London forces arise?

A
  • uneven distribution of electrons within an atom. This results in a slightly negative and slightly positive
    charge on either side of the atom
  • induces a temporary dipole; temporary dipole induces other dipoles on a neighbouring atom/molecule
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6
Q

why is solid ice less dense than water?

A
  • lattice structure of hydrogen bonds (very rigid + more stable)
  • bonds push the water molecules further apart, which lowers the density
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7
Q

what’s the bond angle of a linear molecule and why?

A

180; 2 bonding pairs of electrons around the central atom which repel as far as possible equally

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8
Q

what’s the bond angle of a trigonal planar molecule and why?

A

120; 3 electron pairs around the central atom which repel as far apart as possible equally

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9
Q

what’s the bond angle of a tetrahedral molecule and why?

A

109.5; 4 electron pairs around the central atom which repel as far apart as possible equally

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10
Q

what’s the bond angle of a trigonal bipyramidal molecule and why?

A

120 + 90; 5 electron pairs around the central atom which repel as far apart as possible equally

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11
Q

what’s the bond angle of an octahedral molecule?

A

90; 6 electron pairs around the central atom which repel as far apart as possible equally

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12
Q

what’s the bond angle of a pyramidal molecule and why?

A

107; there are 3 bonding pairs and 1 lone pair of electrons around the central atom; lone pairs repel more than bonding pairs

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13
Q

what’s the bond angle of a non-linear molecule and why?

A

104.5; 2 bonding pairs and 2 lone pairs around the central atom - lone pairs repel more than bonding pairs

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14
Q

what is meant by ‘relative atomic mass’?

A

the weighted average mass of an atom of an element, relative to 1/12th the relative atomic mass of an atom of carbon-12

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15
Q

how do you prepare a standard solution?

A
  • weigh the required mass of solid in a weighing boat using a balance
  • transfer the solid into a beaker using distilled water to wash it out - preventing any solid remaining in the sample bottle
  • reweigh the sample bottle and work out the difference
  • add distilled water to the beaker to dissolve the solid (small volume of water) + use a stirring rod to stir
  • transfer the dissolved solution into a 250cm3 graduated volumetric flask using a funnel, rinsing contents of the beaker and stirring rod with distilled water into the flask
  • add more distilled water, fill up the solution to 250cm3, using a dropping pipette for the last few drops. making sure the bottom of the meniscus is touching the line marking 250cm3.
  • invert the volumetric flask several times
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16
Q

what are the stages of a time of flight mass spectrometer?

A
  1. ionisation
  2. acceleration
  3. ion drift
  4. magnetic field
  5. detection
17
Q

describe how electrospray ionisation works

A
  • sample dissolved in volatile substancce pushed through small needle at high pressure/voltage
  • each particle gains H+ ion; sample turned into gas
18
Q

what’s the equation for electrospray ionisation?

A

X(g) + H+ -> XH+(g)

19
Q

describe how electron impact ionisation works

A
  • sample is vapourised + high energy electrons are fired at it
  • knocks 1 electron off each particle and they become 1+ ions
20
Q

what’s the equation for electron impact ionisation?

A

X(g) + e -> X+(g) + 2e

21
Q

describe the acceleration step in TOF mass spectrometry

A
  • positive ions attracted to negatively charged plate + accelerated towards it, so they have the same KE
  • lighter ions move faster than heavier ions
22
Q

describe the detection step in TOF mass spectrometry

A
  • ions with same charge reach detector
  • lighter ions have higher velocity to reach detector first
  • positive ions pick up electron; electric current generated
23
Q

how do you find the mass of an ion

A

(RAM X10 to the -3)/AVC

24
Q

how does IE change across a period?

A
  • increases across the period because nuclear charge increases
  • causes atomic radius to fall as outer shell is pulled closer to the nucleus
  • distance between nucleus + outer electrons decreases
  • shielding remains similar
  • becomes harder to remove an electron so more energy is needed
25
Q

how does IE change down the group?

A
  • no. of protons in the atom inc, so nuclear charge increases
  • atomic radius inc. due to more shielding
  • distance between nucleus and outer electron inc.
  • meaning less energy is required to remove the outer electron
  • so IE DECREASES