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Solutions, Mixtures, Photoelectric Effect

Total questions: 53

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

A student combines a solution of NaCl(aq) with a solution of AgNO3(aq), and a precipitate forms.

Which of the following is evidence that ionic bonds formed during the precipitation?

a)

The resulting solution is colorless.

b)

The resulting solution conducts electricity.

c)

The precipitate has a high melting point.

d)

The temperature of the solution did not change significantly during the precipitation.

2.

The range of IR radiation is....

a)

200-400 nm

b)

400-800 nm

c)

700 nm - 1 mm

d)

0.1 - 10 mm

3.

The basis of IR absorption is .................

a)

Electronic transition

b)

Vibrational transition

c)

Nuclear spin

d)

Rotational transition

4.

This method separates dissolved substances based on differences in how well they dissolve in a solvent.

a)

Filtration

b)

Evaporation

c)

Distilation

d)

Chromatography

5.

Which method(s) separate substances based on them having different boiling points? (Select all that apply)

a)

Filtration

b)

Evaporation

c)

Distilation

d)

Chromatography

6.

Distillation is used to separate ______.

a)

a liquid from its solution.

b)

an insoluble solid from its solution.

c)

a soluble solid from its solution.

7.
A pure substance shows ------------------ spot on chromat gram
a)
0
b)
1
c)
2
d)
3
8.

Polar organic compound is

a)

CCl4

b)

C3H8

c)

C2H6O

d)

CH3OH

9.

If the brightness of a beam of light increases without changing its color, the ______ will increase.

a)

number of photons

b)

frequency of the light

c)

energy of the photons

d)

wavelength of the photons

10.

Light of a given wavelength is used to illuminate the surface of a metal. However, no photoelectrons are emitted. In order to cause electrons to be ejected, light of __________ should be used.

a)

lower energy

b)

higher intensity

c)

shorter frequency

d)

higher frequency

11.

The energy of a photon is directly proportional to its _____ and inversely proportional to its ______.

a)

intensity - speed

b)

wavelength - frequency

c)

frequency - wavelength

d)

intensity - wavelength

12.

In the photoelectric effect, if the incident photons have a wavelength that is larger than the threshold wavelength, _______.

a)

electrons will be ejected from the metal surface

b)

there will be photoelectric current

c)

no electrons will be emitted from the metal surface

d)

the kinetic energy of the ejected electrons increases

13.

What color of light has the greatest energy per photon?

a)

Red

b)

Green

c)

Blue

d)

Violet

14.

What is the best description of 'threshold frequency'?

a)

The minimum energy needed for electrons to escape a surface.

b)

The maximum kinetic energy that an emitted electron has.

c)

The minimum frequency of a photon that will cause an electron to be emitted.

d)

The frequency that an emitted electron will have.

15.

When light of specific frequencies is shined on a surface, electrons are ejected from the surface. This is the idea behind...

a)

Quantization of Energy

b)

Photoelectric Effect

c)

Compton Effect

d)

deBroglie Waves

e)

Uncertainty Principle

16.

A photon with frequency of 1.5 x 10^15 Hz is incident on a piece of metal in the standard photoelectric experimental setup. What is the wavelength of this photon?

a)

20 nm

b)

150nm

c)

200nm

d)

500nm

17.
Which drawing represents the process by which an absorption line is formed?
a)
A
b)
B
c)
C
d)
D
18.

What is the electron configuration for this PES graph?

a)

1s22s22p63s23p2

b)

1s22s22p63s23p1

c)

1s22s22p63s23p3

d)

1s22s22p63s2

19.

The complete photoelectron spectrum for an element is shown above. Which of the following observations would provide evidence that the spectrum is consistent with the atomic model of the element?

a)

A neutral atom of the element contains exactly two electrons.

b)

The element does not react with other elements to form compounds.

c)

In its compounds, the element tends to form ions with a charge of +1.

d)

In its compounds, the element tends to form ions with a charge of +3.

20.

The energy in joules of a photon of wavelength 355 nm is

a)

5.596 x 1019 J

b)

5.596 x 1028 J

21.
What is the frequency of UV light that has an energy of 2.39 × 10 -18 J? 
a)
2.32 x 109 Hz
b)
3.60 x 1015 Hz
c)
1.58 x 10-51 Hz
d)
3 x 108  m/s
22.
Find the energy, in joules per photon, of microwave radiation with a frequency of 7.91 × 10 10 1/s.
a)
6.63 x 10-34 J
b)
5.25 x 1014 J
c)
5.24 x 10-23 J
d)
1.19 x 1044 J
23.

Rank these in order of strength (#1 = strongest)

a)

UV

b)

Blue Light

c)

Red Light

d)

Infrared

e)

microwaves

1)
2)
3)
4)
5)
24.

Match the following

a)

Microwave radiation

1.

molecular rotation

b)

Infrared Radiation

2.

molecular vibration

c)

Ultraviolet - Visible Light

3.

Transition in electronic energy levels

25.

Spectroscopy can only be used on solutions that have a color.

a)

True

b)

False

26.
This image is an illustration of
a)
photoelectric effect
b)
Dalton's atomic theory
c)
Bohr model
d)
Quantum mechanical model
27.

To gravimetrically analyze the silver content of a piece of jewelry made from an alloy of Ag and Cu, a student dissolves a small pre-weighed sample in HNO3(aq). Ag+(aq)and Cu2+(aq) ions form in the solution. Which of the following should be the next step in the analytical process?

a)

Centrifuging the solution to isolate the heavier ions

b)

Evaporating the solution to recover the dissolved nitrates

c)

Adding enough base solution to bring the pH up to 7.0

d)

Adding a solution containing an anion that forms an insoluble salt with only one of the metal ions

28.

Why are ionic compounds soluble in water?

a)

They form between nonmetals, are nonpolar and so water is repelled and dissolves them

b)

They form between nonmetals, are polar and so water is attracted and dissolves them

c)

They form between a metal and a nonmetal, are polar and so water is attracted and dissolves them

d)

They form between a metal and a nonmetal, are polar and so water is repelled and dissolves them

29.

If you have 34 mL of a 0.50 M NaBr solution, what will the concentration be if 56 mL of water is added to it?

a)

.188 M

b)

3.78 M

c)

.389 M

d)

1.76 M

30.

What is the acetate ion concentration [C2H3O21-] of a 100. mL of Calcium Acetate solution Ca(C2H3O2)2 with 25.0 g dissolved of the compound?

MM of Calcium Acetate = 158.17 g/mol

a)

1.58 M

b)

0.812

c)

3.16 M

d)

4.50 M

31.

The solvent used was water, rank the following colors from Most Polar (#1) to Least Polar (#5)

a)

Yellow

b)

Green

c)

Blue

d)

Pink

e)

Red

1)
2)
3)
4)
5)
32.

Which of the following laboratory setups is most appropriate for the student to use in order to separate and collect a substantial sample of each of the two pigments?

a)

b)

c)

d)

33.

Which of the following diatomic molecules would be MOST soluble in Water?

a)

F2

b)

Cl2

c)

I2

d)

Br2

34.

Polarizability is a term to describe the ability of a nonpolar (or polar) molecule to become polar (or more polar). Which of these nonpolar particles would be most polarizable? Why?

a)

CF4; because it has a larger electron cloud

b)

CH4; because it has a larger electron cloud

c)

SiF4; because it has a larger electron cloud

d)

SiH4; because it has a larger electron cloud

35.
Question Image

Match the following particles to their type of IMF

a)

NaF

1.

Ionic

b)

Au/Cu

2.

Metallic

c)

C2H4

3.

LDF

d)

NH4Cl (pictured)

4.

Ionic and molecular

e)

CF4

5.

Molecular

36.

Both of the following particles have polar covalent bonds and liquid at room temperature: HCN and HCP.

Which would have a greater boiling point?

a)

HCN; it has a stronger dipole since N is more EN

b)

HCN; it has a stronger dipole since N is less EN

c)

HCP; it has a stronger dipole since P is more EN

d)

HCP; it has a stronger dipole since P is less EN

37.

Q. chromatography separates the mixture of dyes on the basis of their ----------------------------

a)

solubility

b)

boiling point

c)

boiling point

d)

boiling point

38.

How to calculate Rf?

a)

Rf = distance travelled by sample / distance travelled by solvent

b)

Rf = distance travelled by solvent / distance travelled by sample

39.

A student performed a (fractional) distillation of a mixture of two straight-chain hydrocarbons, C7H16 and C8H18.

Using four clean, dry flasks, the student collected the distillate (the liquid boiled and condensed in the other container) over the volume ranges (A, B, C, and D) shown in the graph above. Over what volume range should the student collect the distillate of the compound with the stronger intermolecular forces?

a)

A

b)

B

c)

C

d)

D

40.
Question Image

A student performed a (fractional) distillation of a mixture of two straight-chain hydrocarbons, C7H16 and C8H18.

Using four clean, dry flasks, the student collected the distillate (the liquid boiled and condensed in the other container) over the volume ranges (A, B, C, and D) shown in the graph above.

What is happening in each part of the graph?

a)

A

1.

The mixture is being heated

b)

B

2.

The hydrocarbon with the lower BP boils

c)

C

3.

The remaining hydrocarbon continues to heat

d)

D

4.

The hydrocarbon with the higher BP boils

41.

Of the following organic compounds, which is LEAST soluble in water at 298 K?

a)

CH3OH, methanol

b)

CH3CH2CH2OH, l-propanol

c)

C6H12O6, glucose

d)

C6H14, hexane

e)

CH3COOH, ethanoic (acetic) acid

42.

A student prepared five solutions of CuSO4 with different concentrations, and then filled five cuvettes, each containing one of the solutions. The cuvettes were placed in a spectrophotometer set to the appropriate wavelength for maximum absorbance. The absorbance of each solution was measured and recorded. The student plotted absorbance versus concentration, as shown in the

figure above. Which of the following is the most likely explanation for the variance of the data point for the 0.600 M CuSO4 solution?

a)

The cuvette into which the 0.600 M solution was placed had some water droplets inside.

b)

The cuvette into which the 0.600 M solution was placed was filled slightly more than the other cuvettes.

c)

The wavelength setting was accidentally moved away from that of maximum absorbance.

d)

The cuvette used for the 0.600 M solution had not been wiped clean before being put in the spectrophotometer.

43.

M+ is an unknown metal cation with a +1 charge. A student dissolves the chloride of the unknown

metal, MCl, in enough water to make 100.0 mL of solution. The student then mixes the solution with

excess AgNO3 solution, causing AgCl to precipitate. Which of the following diagrams best represents the AgNO3 solution before the reaction occurs?

a)
b)
c)
d)
44.
Beer’s law works for ___ radiation passing through a ___ solution in which the absorbing species is ___ in a concentrationdependent equilibrium
a)
polychromatic ; dilute ; participating
b)
polychromatic ; dilute ; not participating
c)
monochromatic; concentrated; not participating
d)
monochromatic; concentrated; participating
e)
monochromatic; dilute; not participating
45.
A solution prepared by dissolving 25.8 mg of benzene (78.11 g/mol) in hexane (86.16 g/mol) and diluting to 250 mL had an absorption peak at 256 nm and an absorbance of 0.266 in a 1.000-cm cell. What is the concentration of benzene solution?
a)
1.32×10^-3 M
b)
1.20×10^-3 M
c)
1.20 M
d)
1.32 M
46.

In IR spectrophotometry, analyte concentration is quantified based on ........

a)

Wavenumber

b)

Frequency

c)

Absorbance

d)

Transmission

47.
The substance in the mixture that has the greatest affinity for the stationary phase will travel
a)
fastest
b)
slowest
48.
Which of the following factors would not affect an Rf value
a)
solvent used
b)
time taken
c)
temperature
d)
paper used
49.

What is a calibration curve?

a)

Graph of light versus absorbance

b)

Graph of absorbance versus concentration

c)

Graph of concentration versus light

d)

Graph of absorbance volume

50.

A calibration curve is used in colorimetry to

a)

visualise the inverse relationship between ion concentration and light absorbance

b)

determine the concentration of an ion with known absorbance of light

c)

visualise the proportional relationship between ion concentration and light absorbance

d)

determine the absorbance of an ionic solution with a known concentration

51.
On the chromatogram given -------------- is mixture.
a)
red
b)
orange
c)
green
d)
black
52.

The diagram below shows a chromatogram obtained when a sample X was analysed together with four other known dyes P, Q, R and S. Dye Q was known to cause cancer. Which of the following dye(s) is/are safe for use?

a)

P only

b)

S only

c)

P and S

d)

P and X

53.
The Rf value  for the blue component is 
a)
0.3
b)
0.7
c)
10
d)
3

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