Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Chemistry > Ozone Story > Flashcards

Ozone Story Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

What are the units for electronegativity

A

Has no units

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What scale is electronegativity measured on

A

Pauling scale as Linus Pauling suggested this method

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What happens to electronegativity across a period

A

Increases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What happens to electronegativity down a group

A

Decreases

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

What two factors effect how strongly an atom attracts its shared electrons

A

Atom size and closeness to nucleus

Size of core charge

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

How does the atom size effect electronegativity

A

Smaller can get closer to electrons

Has a larger attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How does the size of core charge effect electronegativity

A

Higher nuclear charge has more attraction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How does a permanent dipole occur

A

When two atoms in a bond have very different electronegativities

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What happens if two atoms do not have a very big electronegativity difference

A

No overall dipole even though bonds can still be polar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

Why does CCl4 have no overall dipole due to its shape

A

Is tetrahedral
Chlorine carries small negative charge, central car in positive
Centre of negative charge midway between all chlorines
Centre molecule, positive charge put on carbon
Dipoles cancel due to molecule symmetry, no overall dipole so is non-polar

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

How is a permanent dipole-permanent dipole bond made

A

Not made it is molecule attraction e.g hydrogen chloride attract each other quite strong

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

Can a dipole form without a permanent droplets

A

Yes from electronegativity similarities

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

How is a permanent dipole - induced dipole bond made

A

If add a molecule with a permanent dipole next to a non-polar molecule the permanent dipole induces a dipole.

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

How does an instantaneous dipole - induced dipole bond form

A

Instantaneous dipole forms due to an unequal distribution of electrons in induced dipole molecule, has a temporary dipole (lasts short time)
Can effect molecule with no dipole

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What must molecules have for hydrogen bonding

A

Large dipole between hydrogen atom and highly electronegative atom
Small hydrogen atom that can get very close to atoms in nearby molecules
Lone pair of electrons that positive hydrogen can line up with

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Dipole-dipole bonds in all hydrogen halides, which has the highest boiling point and why

A

Hydrogen fluoride highest as has hydrogen bonding

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

What happens to electronegativity of halogens down group

A

Decreases as get bigger down group as more electrons

18
Q

What is different about waters structure of bonding

A

Oxygen has two lone pairs for can form twice as many hydrogen bonds

19
Q

why do liquids with hydrogen bonding have a higher viscosity

A

To flow past each other need to break binds, stronger the bond - hydrogen bonding, more difficult

20
Q

Why are substances with hydrogen bonds often more soluble in water

A

Hydrogen bonds form between water and substance

21
Q

How does ice have an open structure

A

Has four groups round each oxygen atom, maximises hydrogen bonds between them

22
Q

What is viscosity

A

How easily liquid flows

23
Q

What is collision theory

A

Reactions occur when particles react with minimum kinetic energy
Not all collisions cause reaction
Existing bonds stretch, new bonds form
Only pairs with enough energy to overcome activation energy react

24
Q

What is an enthalpy profile

A

Shows the energy of reacting particles before, during and after reaction

25
Q

What is activation enthalpy

A

Minimum kinetic energy of particles need to react

26
Q

What methods are there if measuring rate of reaction

A

Collecting gas - use volume of gas made
Mass change - lose mass, gas made
Colour - colorimeter, light percentage pass through substance
pH - titration/neutralisation
Chemical analysis- sample reaction moisture at regular intervals, stop reaction (quench) before analysis

27
Q

How does temperature effect rate of a reaction

A

Increase temperature on average particles have more kinetic energy so move faster
More molecules will have activation energy, reaction faster

28
Q

What happens to Boltzmann distribution curve when increase temperature

A

Pushes it to right

29
Q

What happens to the total number of molecules in area under curve when increase temperature

A

Stays same

30
Q

Why are not all collisions successful

A

Particles must have activation energy of more to react

Particles must approach in correct orientation for reaction to take place on collision - steric factor

31
Q

How does a catalyst effect a reaction

A

Spreads yo reaction, provides alternative route from reactants to products with lower activation energy
Chemically unchanged at end of reaction

32
Q

What is homogenous catalysis

A

Catalyst and other reactants all in gaseous state in atmosphere

33
Q

How does homogenous catalysis work

A

Form an intermediate in first step, changed back to catalyst in second step

34
Q

How is percentage changed into parts per million (ppm)

A

x 10000

35
Q

How is parts per million changed into percentage

A

Divide by 10000

36
Q

How are haloalkanes named

A

Start from end of chain that will give smallest numbers
Alphabetical order if more than one halogen
Use e.g ‘di-‘ if two

37
Q

What is a primary haloalkane

A

Halogen on end of chain

38
Q

What is a secondary haloalkane

A

Halogen atom attached to carbon atom in middle of hydrocarbon chain

39
Q

What is a tertiary haloalkane

A

Halogen attached to carbon on atom which carry no hydrogen atoms

40
Q

What is electronegativity

A

Ability of an atom in a covalent bond to attract shared electrons to itself

Chemistry (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions