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chemistryyyy > Unit 3 Test > Flashcards

Unit 3 Test Flashcards

(61 cards)

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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
When looking for an image of the best representation of a solution consider
What should en repelling and attracting( look at the charges of the atoms in the molecule and the way they are facing)
26
Intermolecular forces occur where
Between 2 separate molecules
27
Drawing particulate models
Consider how molecules connect (negative with positive side and vice versa)
28
How to find the retention factor unique pee solute(the total dye)
Rf=ddye/dsolvent
29
In paper chromatography with polar water how will the polar sample travel and how will the np sample travel
Polar samples will travel far and np samples will travel short
30
For paper chromatography the sample travels further when(did in class)
They are like or similar polarities
31
For colum chromatography how do polar parts of mixture travel and how do least polar parts or mixture travel(never did in class)
Polar parts travel slow esta no elastic polar parts travel fastest
32
To find colum chromatography once use same ratios
Divide final position of dye by the leading edge
33
What is a leading edge
Highest value on paper that is possible(up to clip where paper is held)
34
Solubility
The extent where a solute will dissolve into a solvent to from a solution
35
Is water a good solvent (why or why not)
Yes because water is very polar
36
Hydration
Process where molecules surround ions to dissolve them
37
3 steps for a solution to form
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
When will more energy be involved in a solution
When the IMFs are stronger
39
What does like dissolve
Like
40
When determining which is more strongly hydrated consider what first and what second
First consider charge than consider size
41
When considering hydration, what does higher charge mean
More strongly hydrated
42
When considering hydration, what radius is more strongly hydrated(smaller or larger and why)
The smaller radius is stronger because it has more electrons
43
When considering which pairs are miscible consider
Pairs of substances that are both polar or non polar
44
What does aqueous mean?
Dissolves in water
45
What si spectroscopy
Study of how matter interacts with electromagnetic radiation
46
In ultraviolet visible light spectroscopy what do the electrons do
They move from their ground state to a higher energy “excited” state
47
For visible light spectroscopy to work solutions need. ..o
To be colored
48
To determine the functional group of a formula
Match its graph to the other examples- choose the one that matches the most
49
What sina known fact about alcohols and their chemical formulas
They always have an -OH group attached
50
The wavelength of the electromagnetic wave is related to its frequency and the speed of light by the equation
C= λv
51
The energy of a photon is related to the frequency of the electromagnetic wave through Plancks equation
E=hv
52
When light shines ont he surface of the road, what happens to the electrons
The electrons can be ejected from the surface
53
What is E(E=hv)
Energy in joules
54
what is h | E=hv
Plancks constant
55
What is Plancks constant
6.626x10^-34
56
What is v E=hv
Frequency in Hz s^-1
57
What is c C= λv
Speed of light: 3.00x10^8 m/s
58
What is λ C= λv
Wavelength(m)
59
As wavelength increases what happens to the energy
The energy decreases Less energy as wavelength increases
60
As wavelength decreases what happens to the energy
The energy increases The shorter the wavelength the higher the energy
61
What is r in PV=nRT
0.0821

chemistryyyy (40 decks)

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