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Chemistry > Ozone > Flashcards

Ozone Flashcards

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1
Q

What is electronegativity?

A

The ability of an atom in a molecule to attract electrons in a chemical bond to itself.

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2
Q

What is the trend of electronegativity across a period?

A

Electronegativity increases across a period.

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3
Q

What is the trend of electronegativity down a group?

A

Electronegativity decreases down a group (excluding noble gases).

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4
Q

Which element is the most electronegative?

A

Fluorine, with an electronegativity of 4.0.

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5
Q

What creates a polar covalent bond?

A

A difference in electronegativity between two bonding atoms.

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6
Q

What is the polarity of a C-F bond?

A

C δ+ — F δ-, where carbon is partially positive and fluorine is partially negative.

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7
Q

What is a dipole?

A

A molecule with a positive end and a negative end due to charge difference.

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8
Q

What are instantaneous dipoles?

A

Temporary dipoles formed when electrons are unevenly distributed in a molecule.

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9
Q

What are instantaneous dipole-induced dipole bonds?

A

Weak intermolecular bonds formed when an instantaneous dipole polarises a nearby molecule.

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10
Q

What is a permanent dipole?

A

A dipole formed when two atoms in a bond have different electronegativities and charges don’t cancel.

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11
Q

What is the trend in boiling points for halogens?

A

Boiling points increase down the group due to stronger instantaneous dipole-induced dipole bonds.

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12
Q

What causes stronger intermolecular forces in alkanes?

A

Longer carbon chains and larger molecular surface areas.

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13
Q

What is the experimental test for permanent dipoles in a liquid?

A

Use a charged rod near a liquid jet; deflection indicates permanent dipoles.

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14
Q

What are hydrogen bonds?

A

The strongest type of intermolecular bond, formed when H is covalently bonded to F, N, or O.

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15
Q

Why does ice float on water?

A

Ice has an open lattice structure, making it less dense than liquid water.

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16
Q

What properties do liquids with hydrogen bonds have?

A

High viscosity, high melting/boiling points, and solubility in water.

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17
Q

What is activation enthalpy?

A

The minimum energy required for particles to react upon collision.

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18
Q

What do catalysts do in a reaction?

A

Provide an alternate pathway with lower activation enthalpy.

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19
Q

What happens to the rate of reaction as concentration increases?

A

It increases due to more frequent collisions.

20
Q

What is the effect of increasing temperature on reaction rate?

A

Increases rate by raising particle energy and frequency of collisions.

21
Q

What does a Maxwell-Boltzmann distribution show?

A

The spread of kinetic energy among particles in a gas.

22
Q

How do catalysts affect the Maxwell-Boltzmann distribution?

A

Lower the activation energy, allowing more particles to react.

23
Q

What is the formula for the speed of light?

A

c = λ × ν, where λ is wavelength and ν is frequency.

24
Q

How is photon energy calculated?

A

E = h × ν, where h is Planck’s constant and ν is frequency.

25
Q

What are haloalkanes?

A

Alkanes with at least one hydrogen atom replaced by a halogen atom.

26
Q

What makes a haloalkane reactive?

A

The polar carbon-halogen bond, where the carbon is electron-deficient.

27
Q

What is nucleophilic substitution?

A

A reaction where a nucleophile replaces an atom or group in a molecule.

28
Q

What happens when water acts as a nucleophile?

A

It hydrolyses haloalkanes, forming alcohols and H⁺ ions.

29
Q

What happens to C-X bond reactivity down group 7?

A

Reactivity increases due to decreasing bond enthalpy.

30
Q

What is a radical?

A

A molecule with an unpaired electron.

31
Q

What is homolytic fission?

A

A bond breaks evenly, with each atom receiving one electron.

32
Q

What is heterolytic fission?

A

A bond breaks unevenly, with one atom receiving both bonding electrons.

33
Q

What are the three stages of a radical chain reaction?

A

Initiation, propagation, and termination.

34
Q

What is the role of chlorine radicals in ozone depletion?

A

They catalyse the breakdown of ozone into oxygen.

35
Q

What is the overall reaction for ozone breakdown?

A

O₃ + O● → 2O₂.

36
Q

What are the effects of ozone in the stratosphere?

A

Absorbs UV radiation, reducing its harmful effects on Earth’s surface.

37
Q

What are the effects of ozone in the troposphere?

A

It is a pollutant that causes photochemical smog and respiratory problems.

38
Q

What is the role of UV radiation in ozone formation?

A

UV dissociates O₂ molecules, forming radicals that create ozone.

39
Q

What is photodissociation?

A

The breaking of a chemical bond due to absorption of light energy.

40
Q

What is the electromagnetic spectrum?

A

Radio waves, microwaves, infrared, visible light, ultraviolet, X-rays, and gamma rays.

41
Q

How is ozone both formed and destroyed?

A

O₂ + UV → O●, O● + O₂ → O₃; UV can also split O₃ into O₂ + O●.

42
Q

What does the speed of light in a vacuum equal?

A

3.00 × 10⁸ m/s.

43
Q

Why is ozone depletion concerning?

A

It allows more harmful UV radiation to reach Earth’s surface, increasing health risks.

44
Q

What is the effect of radicals like NO● on ozone?

A

They catalyse the destruction of ozone, similar to chlorine radicals.

45
Q

Why is C-F less likely to break than C-I?

A

C-F has the highest bond enthalpy, while C-I has the lowest.

46
Q

What happens when haloalkanes reach the stratosphere?

A

They release radicals that deplete ozone.

Chemistry (8 decks)

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