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Chemistry > Ozone Story > Flashcards

Ozone Story Flashcards

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1
Q

What are the 3 types of intermolecular bonds

A

1) instantaneous dipole- induced dipole
2) permanent dipole-permanent dipole
3) hydrogen bonds

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2
Q

How do instantaneous dipole- inducer dipole bonds work?

A

1) electrons are always moving causing charge density to change making instantaneous dipoles
2) this can induce a dipole be attracted towards it creating an instantaneous- induced bond

(The bonds get broken and remade because electrons keep moving)

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3
Q

How does a molecules shape affect its intermolecular bonds?

A

More places for id-id bonds to form if it had a longer chain

Branch chains can’t get as close

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4
Q

Why does a molecules size and mass effect boiling point?

A

The bigger the molecule the larger electron cloud which means it forms stronger id-id bonds

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5
Q

What do bonds need to be in order to have a pd-pd bond?

A

Polar

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6
Q

When can hydrogen bonding happen and why?

A

When a hydrogen is attached to a fluorine, nitrogen, or oxygen.

Very electronegative with hydrogen - high charge density on the H

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7
Q

What does electronegative mean?

A

Tendency to attract electrons and form negative ions

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8
Q

Two ways hydrogen bonds affect how a substance behaves

A

1) hydrogen bonding is a very strong intermolecular bond giving the substance a high melting point as it’s hard to over come
2) soluble in water - can form bonds with the water making it soluble

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9
Q

How can an experiment show differences in bond strengths

A

Energy is absorbed to break bonds when a liquid evaporates

so you can measure the temperature change in order to see how easily a liquid evaporates

and what type of intermolecular bonds it’s likely to form

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10
Q

What is the collision theory

A

Particles must collide with:

  • correct orientation
  • enough kinetic energy to react (activation energy)
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11
Q

How would increased temp change the Boltzmann distribution graph?

A
  • moves it to the right
  • reduces hump
  • more molecules with enough activation energy to react
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12
Q

How do catalysts affect reaction rate?

A
  • lowers activation enthalpy by providing an alternative pathway (a different way for bonds to be broken and remade)
  • so more particles have enough energy to react
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13
Q

How does pressure and concentration affect reaction rate?

A
  • particles are closer together on average

- collide more often so have more chances to react

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14
Q

How does temperature affect reaction rate?

A
  • particles have more energy so more likely to react when they collide
  • move faster - collide more frequently
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15
Q

How can you use experiments to find out rate of reaction?

A

Measure loss of reactant of formation of product at regular intervals

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16
Q

What is a catalyst

A

A catalyst increases rate of reaction by providing and alternative reaction pathway with lower activation enthalpy
Catalyst is chemically unchanged at the end and reformed

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17
Q

Two types of catalyst

A

Homogeneous - same state heterogeneous - different state

18
Q

How do homogeneous catalysts work?

A
  • by forming intermediated
  • the activation enthalpy needed to make intermediates and form the product is lower than reactants straight to products
  • catalyst reformed again
19
Q

How many jumps does a homogeneous catalyst reaction have?

A

2 from making intermediates

20
Q

Do boiling points of haloalkanes increase or decrease down the group?

A

Increase

Stronger id-id bonds because molecules are bigger due to more electron levels

21
Q

Why are carbon-halogen bonds polar

How does this affect the molecule?

A

High difference in electronegativity

Carbon becomes electron deficient so it can be attacked by a nucleophile

22
Q

What is a nucleophile?

Give an example

A

An electron pair donor

OH-
NH3

23
Q

What is nucleophilic substitution

A

A functional group in a compound is replaced by another

Because a nucleophile attacked a partially positive carbon

24
Q

What do haloalkanes react with to form alcohols

A

OH-

25
Q

What do haloalkanes react with to form amines?

A

Ammonia (dissolved in ethanol)

26
Q

How is ozone formed and where?

A

Oxygen radicals and O2
UV radiation from sun breaks down oxygen into O radicals

  • stratosphere
27
Q

Equation for formation of ozone in the stratosphere

A

hv
O2 —> O + O
O2 + O —> O3

28
Q

Why is the ozone layer being constantly replaced

A

UC radiation can reverse formation of O3
O3—>O2 +O

O can react with O2 to replace it

Creates an equilibrium

29
Q

How does the ozone layer protect against UV radiation

A

When Ozone breaks down it absorbed high frequency radiation which can be dangerous to humans it reaches the troposphere

30
Q

What can Ozone in the troposphere cause? And why is it bad?

A
  • photochemical smog when mixed with pollutants such as NO2
  • this can cause respiratory problems
  • is toxic to humans and animals
  • can damage plants and materials
31
Q

What can breakdown to become catalysts in breaking down ozone?

A

CFCs (ChloroFloroCarbons)

32
Q

What order or bond strength are carbon-halogen bonds?

A

Stronger up the group because it has high bond enthalpy.

More reactive down group

33
Q

How is the ozone layer being destroyed by CFCs and homogenous catalysis?

A

More CFCs are being produced so chlorine radicals from CFCs act as catalysts in the break down resulting in more being broken down than being replaced.

Cl +O3—>O2+ClO
ClO+O3—>Cl+2O2

34
Q

What radicals destroy ozone?

A

Cl
NO
Halogen radicals from haloalkanes

35
Q

Equation for parts per million to percentage

A

Divide by 100

Times by 1 000 000

36
Q

What does visible light and ultra violet radiation do to electrons?

A

Electrons have fixed energy levels which when they are hit by the right amount of UV or visible light they can move up

Only specific frequencies if enough is absorbed bonds break forming radicals

37
Q

What makes a MOLECULE polar

A

Shape and polarity of bonds

Imagine the molecule like an atom

38
Q

What does a significant difference in electronegativity do to a covalent bond

A

Polarise it

39
Q

What is a dipole

A

Difference in charge between the two atoms caused by a shift in electron density in the bond

40
Q

What difference in electronegativity is significant enough for to make it polar?

A

Approx 0.4

Chemistry (8 decks)

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