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chemistryyyy > Unit 3 Test Mcq Focused > Flashcards

Unit 3 Test Mcq Focused Flashcards

(71 cards)

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1
Q

Which if the following best describes how the model is limited in its depiction of the phenomenon

A

It doesn’t show how the temporary fluctuating dipoles of the molecular electron cloud results in a net force of attraction between the molecules

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2
Q

If the substance is an ionic compound what must be true about the aqueous solutions

A

Test the electric conductivity of the aqueous solutions to see if it’s ionic

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3
Q

At room temp why is I2(s) a molecular solid

A

It is not a good conductor of electricity because it’s VE are localized in bonding and non bonding pairs

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4
Q

When there is fewer molecules of product than reactant what happens

A

The pressure decreases

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5
Q

When absolute temperature is doubled what is also doubled

A

Pressure

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6
Q

Measurements that must be made to calculate the molar mass of gas(like they fire experiment we did) must include all EXCEPT

A

Mass of the water in the apparatus

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7
Q

When comparing flasks use what formula

A

PV=nRT

Usually in this situation V is a constant however

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8
Q

If the partial pressure elf each has is half its initial pressure then wha happens to the final total pressure

A

The final total pressure is half the sum fo the initial pressure of the 2 gases

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9
Q

Liters of sample can affect what

A

The total pressure

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10
Q

Equal masses of three different ideal gases depends on

A

The relative molecular masses of X Y and Z

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11
Q

Atoms will escape faster for, a container if they have

A

A higher average speed which is due to the weight of the atom

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12
Q

When gas is added to a rigid container at a constant temp the average speed of the gas molecule…

A

Stays the same

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13
Q

If a sample of a gas ic cooled the average speed of the molecule

A

Decreases

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14
Q

At standard temp and pressure, various # of mol samples still have the same

A

Average molecular kinetic energy

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15
Q

If area under the graph is the same for all gases in maxwell distribution graph that means that

A

The molecular masses of the gases have the same average KE

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16
Q

If the temperature is held constant what happens to the KE

A

The KE stays the same

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17
Q

If 2 flexible containers are held at the same temp and gas the volume of the one gas container is not

A

The same as the volume of the other gas container

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18
Q

A gas deviates more from ideal behavior at high temperatures than another gas because

A

The particle volume of a gas is greater than the other gas

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19
Q

The ideal gas law does not include a factor for molecular

A

Volume

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20
Q

When the average distance between molecules is greater

A

The behavior of a sample is more like an ideal gas

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21
Q

Less force in collisions means what about the ideality of a gas?

A

That it’s more ideal

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22
Q

Low pressure can be a result of what with IMF

A

Strong IMF

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23
Q

The ideal gas law best describes what type of gas molecules

A

A diatomic gas

No polar

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24
Q

Molarity equation

A

Moles of solute/ moles of volume

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25
Concentration is with what variable
M | Molarity
26
What is a concentration
Molarity, what is said in the original solution, does not change
27
When volumes are additive it is saying
You can’t simply add the moles you have to multiply by the mL sample
28
Which chem tool has the greatest accuracy for measuring L
The 100 mL volumetric flask
29
When solving concentration or molarity problems PAY ATTENTION TO
of moles of the element you are solving for!!
30
If a molecule is np and another is polar, are there IMF between the two?
Yes there are definitely LDF and possibly also dip-dip
31
Is nacl np
No it’s polar
32
What gas can be collected by a displacement of water
H2
33
When asked about ions present in significant concentrations don’t include
The ions that are in both molecules
34
Which of the following techniques is most appropriate for the recovery of solid molecules from an aqueous solution of a molecule
Evaporation to dryness
35
I’m looking at a graph to find the greatest percentage of which compound can be recovered by look at what
look at the slopes of the molecules
36
for paper chromatography if the solvent is polar and stationary what’s products will travel up deplete the fastest(np or p)
polar product will travel the furthest up the paper
37
The substance that would be initially present in higher concentration in the distal it is because(identify bonds and what needs to happen to them)
it has more C-C bonds to break
38
When asked to identify X and Y in paper chromatography don’t pay attention to the polarity of the paper pay attention to…?
The polarity of the solution at the bottom | hexane for example
39
Why would one guest be able to absorb ultraviolet light but not visible light in the other gas be able to absorb both
because visible light may produce transitions between energy levels in one gas but not the other
40
The band in the region corresponding to shorter wavelength shows what(think about absorbance in comparison to longer wavelengths)
A lower absorbance than the band in the region corresponding to longer wavelengths
41
what is h in frequency equations
planks constant | 6.626*10^-34 J
42
nano is to what power?
-9
43
speed of light
3*10^8 m/s
44
A gas mixture at 0°C and one atm contains .01 moles of H2, space .015 moles of O2, space and .025 moles of N2. Space assuming ideal behavior what is the partial pressure of hydrogen gas H2 in the mixture
about .20 atm because each to comprises i20% of the total number of moles of gases
45
Doubling the number of moles does want to partial pressure
doubling the number of moles doubles it’s partial pressure
46
What can polar H2O molecules do to the electron clouds of O2 molecules
they can induce temporary dipoles on the electron clouds
47
Molecules dissolve in a solution if
they are like substances for example it is a polar solution and there’s a polar solvent or vice versa (with nonpolar)
48
What do molecular models not show that results in a net force of attraction between molecules
it does not show how the temporary fluctuating dipoles of the molecular electron clouds result in a net force
49
When considering boiling point consider
more polarizable more electrons the most importantly the IMF
50
Which of the following is not shown in a model of flasks with particles but explains why a flask must contain certain gas
The strength of the IMF between the particles in the liquids
51
What is the order of the IMF
strongest is hydrogen bonding then dipole dipole forces then London dispersion forces
52
Which one has a higher melting points MgS or NaCl
MgS | because it has charges of +2 in -2 while NaCl has charges of +1 and -1
53
what does lower melting point mean | in relation to IMF
lower melting point aligns with higher boiling points meaning it has stronger IMF
54
what is boron nitride | type of solid
a covalent network
55
what so a covalent network
a network solid of atoms connected by covalent bonds w fixed bond angles
56
is ionic bonding soluble in water
yes
57
are dipole dipole forces soluble in water
yes
58
is ionic bonding soluble in hexane(polar)
no
59
will a solid ionic compound conduct electricity why or why not
no becuase the particles aren’t free to move
60
will an aqueous ionic compound conduct electricity
yes because the electrons are now free to move
61
what happens to the temps of different gases at thermal equilibrium
they stay the same
62
when considering the greatest average speed of the particles consider
the lowest molar mass and highest temp
63
greatest MM is determined by what
most # of particles
64
when asked about which molecule will have the largest dipole consider
electronegativit and polarity
65
when asked which molecule will form h bonds with other molecules consider
if there is an h bond in that molecule itself
66
which is the IMF exhibited by a pure sample of Cs2
LDF only
67
which molecule would have the largest dispersion forces
look for strongest IMF
68
when ranking the lattice energy of the following formulas consider
identify bond strength so identify ion charges
69
which do you do first when identifying bond strength | identity charge first or ion size
charge first
70
when charges are equal what do you sue to break the tie when identifying bond strength
use ion size
71
if considering highest vapor pressure look for
strongest IMF

chemistryyyy (40 decks)

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