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chemistryyyy > Unit 3 Test > Flashcards

Unit 3 Test Flashcards

1
Q

Wha si true for “ideal gases”(3)

A

Collisions between particles are elastic
No attractive or repulsive forces between particles
Particle volume is negligible
Gas particles are in constant random motion

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2
Q

Real gas behavior(2)

A

All gases are able to condense- there are attractive forces

Molecules vary in size and have volume

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3
Q

If particles are larger they have a better chance of …

A

Colliding

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4
Q

Why is gas non ideal at high pressures

A

Because the particle volume becomes significant

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5
Q

What is a solvent

A

The liquid

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6
Q

What is a solute

A

The solid

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7
Q

Which have larger radius and why(anions or cations)

A

Anions because they have more e-

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8
Q

Chromatography used to separate IMF based on

A

Polarity

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9
Q

Suspension

A

A polar and no polar substance won’t mix

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10
Q

Type of level?

Microwave radiation

A

Molecular rotational level

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11
Q

Type of level?

Infrared radiation

A

Molecular vibrational energy

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12
Q

Type of level?

Ultraviolet/ visible radiation

A

Electric energy levels

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13
Q

What is the kinetic energy formula

A

KE=1/2mv^2

Kinetic energy is mass times velocity squared

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14
Q

Describe cold gas maxwell distribution graph

A

High tall peak in the beginning of the graph

High on y axis and short on x axis

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15
Q

Describe room temperature graph

A

Regular graph in middle of both x and y axis

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16
Q

Describe hot gas maxwell distribution graph

A

Short flat wide graph

Short on y axis
Long on x axis

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17
Q

If equimolar samples are both at standard conditons(1 atm 273 K)
Which sample has more KE

A

Same KE since they are at the same temperatures

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18
Q

When considering which sample has higher average molecular speeds consider

A

The atomic radius because if the atom is lighter then it’s speed is faster

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19
Q

If there is a tube, one end has a substance that’s np and one that’s polar which side will the precipitate be closer to?

A

The polar side because it has dipole dipole and/or possibly hydrogen bonding so it has a stronger pull, pulling the precipitate closer to it

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20
Q

If NO is placed in a sealed rigid container and it is heated what will happen to NO

A

The pressure will increase because the # of collisions will increase and because he kinetic energy increases that leads to friction causing the temp to increase

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21
Q

Which has do you predict to deviate from ideal gas

Choosing from a polar and a np gas

A

The polar one because the IMF is stronger so it is less likely for the forces to be stable

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22
Q

If the volume of a gas is greater than expected that is because

A

The particle volume is great

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23
Q

Of the volume of a gas is less than expected based on the ideal gas law that is because

A

The IMFs are stronger

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24
Q

Equation for the molarity of a solution

A

M = moles of solute divided by the total liters of the solution

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25
Q

When looking for an image of the best representation of a solution consider

A

What should en repelling and attracting( look at the charges of the atoms in the molecule and the way they are facing)

26
Q

Intermolecular forces occur where

A

Between 2 separate molecules

27
Q

Drawing particulate models

A

Consider how molecules connect (negative with positive side and vice versa)

28
Q

How to find the retention factor unique pee solute(the total dye)

A

Rf=ddye/dsolvent

29
Q

In paper chromatography with polar water how will the polar sample travel and how will the np sample travel

A

Polar samples will travel far and np samples will travel short

30
Q

For paper chromatography the sample travels further when(did in class)

A

They are like or similar polarities

31
Q

For colum chromatography how do polar parts of mixture travel and how do least polar parts or mixture travel(never did in class)

A

Polar parts travel slow esta no elastic polar parts travel fastest

32
Q

To find colum chromatography once use same ratios

A

Divide final position of dye by the leading edge

33
Q

What is a leading edge

A

Highest value on paper that is possible(up to clip where paper is held)

34
Q

Solubility

A

The extent where a solute will dissolve into a solvent to from a solution

35
Q

Is water a good solvent (why or why not)

A

Yes because water is very polar

36
Q

Hydration

A

Process where molecules surround ions to dissolve them

37
Q

3 steps for a solution to form

A

The solute particles must selarate(energy is required)
The solvent particles must separate(energy required)
The solute and solvent particles must come back together (energy released)

38
Q

When will more energy be involved in a solution

A

When the IMFs are stronger

39
Q

What does like dissolve

A

Like

40
Q

When determining which is more strongly hydrated consider what first and what second

A

First consider charge than consider size

41
Q

When considering hydration, what does higher charge mean

A

More strongly hydrated

42
Q

When considering hydration, what radius is more strongly hydrated(smaller or larger and why)

A

The smaller radius is stronger because it has more electrons

43
Q

When considering which pairs are miscible consider

A

Pairs of substances that are both polar or non polar

44
Q

What does aqueous mean?

A

Dissolves in water

45
Q

What si spectroscopy

A

Study of how matter interacts with electromagnetic radiation

46
Q

In ultraviolet visible light spectroscopy what do the electrons do

A

They move from their ground state to a higher energy “excited” state

47
Q

For visible light spectroscopy to work solutions need. ..o

A

To be colored

48
Q

To determine the functional group of a formula

A

Match its graph to the other examples- choose the one that matches the most

49
Q

What sina known fact about alcohols and their chemical formulas

A

They always have an -OH group attached

50
Q

The wavelength of the electromagnetic wave is related to its frequency and the speed of light by the equation

A

C= λv

51
Q

The energy of a photon is related to the frequency of the electromagnetic wave through Plancks equation

A

E=hv

52
Q

When light shines ont he surface of the road, what happens to the electrons

A

The electrons can be ejected from the surface

53
Q

What is E(E=hv)

A

Energy in joules

54
Q

what is h

E=hv

A

Plancks constant

55
Q

What is Plancks constant

A

6.626x10^-34

56
Q

What is v

E=hv

A

Frequency in Hz s^-1

57
Q

What is c

C= λv

A

Speed of light: 3.00x10^8 m/s

58
Q

What is λ

C= λv

A

Wavelength(m)

59
Q

As wavelength increases what happens to the energy

A

The energy decreases

Less energy as wavelength increases

60
Q

As wavelength decreases what happens to the energy

A

The energy increases

The shorter the wavelength the higher the energy

61
Q

What is r in PV=nRT

A

0.0821

chemistryyyy (40 decks)

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