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chemistryyyy > Unit 3 Test Mcq Focused > Flashcards

Unit 3 Test Mcq Focused Flashcards

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
Q

Concentration is with what variable

A

M

Molarity

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26
Q

What is a concentration

A

Molarity, what is said in the original solution, does not change

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27
Q

When volumes are additive it is saying

A

You can’t simply add the moles you have to multiply by the mL sample

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28
Q

Which chem tool has the greatest accuracy for measuring L

A

The 100 mL volumetric flask

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29
Q

When solving concentration or molarity problems PAY ATTENTION TO

A

of moles of the element you are solving for!!

30
Q

If a molecule is np and another is polar, are there IMF between the two?

A

Yes there are definitely LDF and possibly also dip-dip

31
Q

Is nacl np

A

No it’s polar

32
Q

What gas can be collected by a displacement of water

A

H2

33
Q

When asked about ions present in significant concentrations don’t include

A

The ions that are in both molecules

34
Q

Which of the following techniques is most appropriate for the recovery of solid molecules from an aqueous solution of a molecule

A

Evaporation to dryness

35
Q

I’m looking at a graph to find the greatest percentage of which compound can be recovered by look at what

A

look at the slopes of the molecules

36
Q

for paper chromatography if the solvent is polar and stationary what’s products will travel up deplete the fastest(np or p)

A

polar product will travel the furthest up the paper

37
Q

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)

A

it has more C-C bonds to break

38
Q

When asked to identify X and Y in paper chromatography don’t pay attention to the polarity of the paper pay attention to…?

A

The polarity of the solution at the bottom

hexane for example

39
Q

Why would one guest be able to absorb ultraviolet light but not visible light in the other gas be able to absorb both

A

because visible light may produce transitions between energy levels in one gas but not the other

40
Q

The band in the region corresponding to shorter wavelength shows what(think about absorbance in comparison to longer wavelengths)

A

A lower absorbance than the band in the region corresponding to longer wavelengths

41
Q

what is h in frequency equations

A

planks constant

6.626*10^-34 J

42
Q

nano is to what power?

A

-9

43
Q

speed of light

A

3*10^8 m/s

44
Q

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

A

about .20 atm because each to comprises i20% of the total number of moles of gases

45
Q

Doubling the number of moles does want to partial pressure

A

doubling the number of moles doubles it’s partial pressure

46
Q

What can polar H2O molecules do to the electron clouds of O2 molecules

A

they can induce temporary dipoles on the electron clouds

47
Q

Molecules dissolve in a solution if

A

they are like substances for example it is a polar solution and there’s a polar solvent or vice versa (with nonpolar)

48
Q

What do molecular models not show that results in a net force of attraction between molecules

A

it does not show how the temporary fluctuating dipoles of the molecular electron clouds result in a net force

49
Q

When considering boiling point consider

A

more polarizable more electrons the most importantly the IMF

50
Q

Which of the following is not shown in a model of flasks with particles but explains why a flask must contain certain gas

A

The strength of the IMF between the particles in the liquids

51
Q

What is the order of the IMF

A

strongest is hydrogen bonding then dipole dipole forces then London dispersion forces

52
Q

Which one has a higher melting points MgS or NaCl

A

MgS

because it has charges of +2 in -2 while NaCl has charges of +1 and -1

53
Q

what does lower melting point mean

in relation to IMF

A

lower melting point aligns with higher boiling points meaning it has stronger IMF

54
Q

what is boron nitride

type of solid

A

a covalent network

55
Q

what so a covalent network

A

a network solid of atoms connected by covalent bonds w fixed bond angles

56
Q

is ionic bonding soluble in water

A

yes

57
Q

are dipole dipole forces soluble in water

A

yes

58
Q

is ionic bonding soluble in hexane(polar)

A

no

59
Q

will a solid ionic compound conduct electricity why or why not

A

no becuase the particles aren’t free to move

60
Q

will an aqueous ionic compound conduct electricity

A

yes because the electrons are now free to move

61
Q

what happens to the temps of different gases at thermal equilibrium

A

they stay the same

62
Q

when considering the greatest average speed of the particles consider

A

the lowest molar mass and highest temp

63
Q

greatest MM is determined by what

A

most # of particles

64
Q

when asked about which molecule will have the largest dipole consider

A

electronegativit and polarity

65
Q

when asked which molecule will form h bonds with other molecules consider

A

if there is an h bond in that molecule itself

66
Q

which is the IMF exhibited by a pure sample of Cs2

A

LDF only

67
Q

which molecule would have the largest dispersion forces

A

look for strongest IMF

68
Q

when ranking the lattice energy of the following formulas consider

A

identify bond strength so identify ion charges

69
Q

which do you do first when identifying bond strength

identity charge first or ion size

A

charge first

70
Q

when charges are equal what do you sue to break the tie when identifying bond strength

A

use ion size

71
Q

if considering highest vapor pressure look for

A

strongest IMF

chemistryyyy (40 decks)

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