Category: Chemistry

Describe the role of intermolecular forces in electronic and molecular shapes. How does the presence of lone (unshared) electrons change the electronic shape in the formation of the molecular shape? Be sure to cite specific

Describe the role of intermolecular forces in electronic and molecular shapes. How does the presence of lone (unshared) electrons change the electronic shape in the formation of the molecular shape? Be sure to cite specific

What is the frequency of light (s-1 ) that has a wavelength of 1.23 X 10 -6 cm?What is the de Broglie wavelength (m) of a 2.0 kg object moving at a speed of 50 m/s?

 Exam Review CHM 111
Chapter 2

The energy of a photon of light is __________ proportional to its frequency and __________
proportional to its wavelength.
A. directly, directly
B. inversely, inversely
C. inversely, directly
D. directly, inversely
E. indirectly, not

What color of visible light has the longest wavelength?
A. blue
B. violet
C. red
D. yellow
E. green

What is the frequency of light (s-1 ) that has a wavelength of 1.23 X 10 -6 cm?
A. 3.69
B. 2.44 X 10 16
C. 4.10 X 10 12
D. 1.04 X 10-13

The energy of a photon that has a wavelength of 13.2 nm is __________ J.
A. 9.55 X 10-25
B. 1.62 X 10-17
C. 1.99 X 10-25
D. 1.51 X 10-17

A mole of yellow photons of wavelength 527 nm has __________ kJ of energy.
A. 165
B. 227
C. 2.74 X 10-19
D. 4.56 X 10-46
E. 6.05 X 10-3

It takes 254 kJ/mol to eject electrons from a certain metal surface. What is the longest wavelength of light (nm) that can be used to eject electrons from the surface of this metal via the photoelectric effect __________ ?
A. 472 B. 233 C. 165 D. 725 E. 552

What is the de Broglie wavelength (m) of a 2.0 kg object moving at a speed of 50 m/s?
A. 6.6 X 10 -36
B. 1.5 X 10 35
C. 5.3 X 10 -33
D. 2.6 X 10 -35
E. 3.8 X 10 34

At maximum, an f-subshell can hold __________ electrons, a d-subshell can hold __________
electrons, and a p-subshell can hold __________ electrons.
A. 2, 8, 6
B. 14, 10, 6
C. 2, 8, 18
D. 2, 12, 21
E. 14, 6, 10

The __________ quantum number defines the shape of an orbital.
A. spin
B. magnetic
C. principal
D. azimuthal
E. psi

The principal quantum number for the outermost electrons in a Br atom in the ground state is
__________.
A. 1
B. 2
C. 3
D. 4
E. 0

Which one of the quantum numbers does not result from the solution of the Schroedinger
equation?
A. spin
B. magnetic
C. principal
D. azimuthal
E. angular momentum
Chapter 3

The element that corresponds to the electron configuration1s22s2 2p6 3s2 3p 6 4s1 3d5 is
A. Titanium
B. Chromium
C. Vanadium
D. Manganese
E. Iron

Give the complete electronic configuration for Mn.
A. 1s2 2s2 2p 6 3s23p 6 4s2 4d5
B. 1s2 2s2 2p 6 3s23p 6 4s1 3d6
C. 1s2 2s2 2p 6 3s23p 6 4s2 3d5
D. 1s2 2s2 2p 6 3s23p 6 4s2 4p5

Choose the ground state electron configuration for Zn 2+
A. [Ar]4s23d 8
B. [Ar]3d 10
C. [Ar]4s23d 6
D. [Ar]
E. [Ar]3d 8

How many valence electrons do the halogens possess?
A. 5
B. 7
C. 6
D. 8
E. 1

Place the following in order of increasing atomic radius: As O Br
A. As < Br < O
B. O < As < Br
C. Br < As < O
D. As < O < Br
E. O < Br < As

Place the following in order of increasing IE. K Ca Rb
A. Ca < K < Rb
B. Rb < Ca < K
C. Ca < Rb < K
D. Rb < K < Ca
E. K < Ca < Rb

Which element is NOT paramagnetic? A. Li B. F C. Rb D. V E. Zn 8. Give the number of electrons in Na +1 . A. 10 B. 13 C. 9 D. 11 E. 12 9. Predict the charge of the most stable ion of magnesium. A. 3+ B. 1- C. 1+ D. 2- E. 2+ 10. Electrons add to orbitals from lowest to highest energy is known as the A. Pauli exclusion principle. B. Hund’s rule. C. Aufbau principle. D. Heisenberg uncertainty principle.

Which electron configuration represents a violation of the Aufbau principle?

No two electrons can have the same four quantum numbers is known as the A. Pauli exclusion principle. B. Hund’s rule. C. Aufbau principle. D. Heisenberg uncertainty principle. A) B) C) D) E)

Which electron configuration represents a violation of the Pauli exclusion principle?

When filling degenerate orbitals, electrons fill them singly first, with parallel spins is known as A. Pauli exclusion principle. B. Hund’s rule. C. Aufbau principle. D. Heisenberg uncertainty principle.

Which electron configuration represents a violation of Hund’s Rule?

Which element on the Periodic Table has the highest electronegativity? A. Francium B. Radon C. Fluorine D. Helium E. Hydrogen 17. Repulsions that cause a net reduction in the attraction of electrons to the nucleus. A. core B. valence C. effective nuclear charge D. shielding E. electron affinity A) B) C) D) E) A) B) C) D) E) 18. The Outer transition metals form the A. f-block B. d-block C. p-block D. s-block E. solitary confinement 19. Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar? A) Mg > Na > P > Si > Ar
B) Ar > Si > P > Na > Mg
C) Si > P > Ar > Na > Mg
D) Na > Mg > Si > P > Ar
E) Ar > P > Si > Mg > Na

Of the following atoms, which has the largest first ionization energy?
A) Br
B) O
C) C
D) P
E)

Briefly describe the positive ion. What kind of element is it? Does it have more than one positive ion? If so, list these. What are the real-world applications for your ionic compound?

Chemistry of Compounds and Chemical Reactions

Research your ionic compound using at least two different websites, and in your own words describe:

Write out the name, provide the cation and anion, and write out the correct formula. (describe the steps for how you did this)

Briefly describe the positive ion. What kind of element is it? Does it have more than one positive ion? If so, list these.

Briefly describe your ionic compound. What are some of its physical and chemical properties?

Does it react to other molecules? If so, which ones? Write out the equation for at least one example.

What are the real-world applications for your ionic compound?

Pick two out of the four types of Chemical Reactions (Combination, Decomposition, Replacement (single or double), and Combustion). For your two selections answer the below questions:

Compare and contrast your selections. How are they similar or different.

Go out to the internet and find an example of each.

Write out the related formulas and verbally describe what is happening in that reaction.

Pick a real life example of a chemical change. Here is a good website to get you started: chemical change examples. For the example you pick answer the following questions:

Do you have first-hand experience with this chemical change? If so, describe what you saw or experienced.

Describe which of the chemical reactions may be involved in this situation.

Research and completely describe the process of the change. Include any chemical formulas and write out the formulas associated with them.

How would you explain it to someone who is new to chemistry?Which principle do you think is most useful in impacting percent yield?

Synthesis
https://www.acs.org/content/acs/en/greenchemistry/principles/12-principles-of-green-chemistry.html

1 Read about the 12 principles of green chemistry from this website.

2 Pick one of those principles and explain it in detail.  put the principle within your Subject heading. First come first serve, if your principle has already been discussed make sure to explain it from a different perspective. How would you explain it to someone who is new to chemistry?

Give an example of how that principle is used or can be used. Be specific and cite your sources.

Which principle do you think is most useful in impacting percent yield?

Which principle do you think is the most important? Why?

 Explain how the law works in your example, noting the relationships of, say, pressure, volume, temperature, etc.

Gas Laws

Pick one of the gas laws covered in our textbook: Boyle’s Law, Charles’s Law, Gay-Lussac’s Law, The Ideal Gas Law, and Dalton’s Law. Find a real-life example of where your chosen law comes into play and claim this in your Subject heading (e.g. XXX Law, real-life example). Provide the following information.

1 Remind us what your law is in a sentence or two,
2 And then explain your real-life example, try to be as specific as possible, (do try to have it relate to chemistry when possible)

Explain how the law works in your example, noting the relationships of, say, pressure, volume, temperature, etc.

Describe what that career is and how one gets trained for it. Describe how the chemical principle you have identified is used by the individual in that career. Give some examples.

Solution chemistry

Describe what that career is and how one gets trained for it. Describe how the chemical principle you have identified is used by the individual in that career. Give some examples.

How do we as a society benefit from equilibrium-driven processes? Sample contexts may include nutritional, medicinal, agricultural, industrial, commercial, or any other relevant application of your choice. Be sure to cite your sources.

Chemical equilibrium

Pick one of the above-mentioned topics and relate it to the below (claim it in your Subject heading), then provide the following information:

Research and briefly describe a real-life application of chemical equilibrium. How do we as a society benefit from equilibrium-driven processes? Sample contexts may include nutritional, medicinal, agricultural, industrial, commercial, or any other relevant application of your choice. Be sure to cite your sources.

Make sure to include any related formulas that you find. (You will want to use the D2L Chemistry equation editor when necessary)

Describe Radiation and Shielding Required. How the travel distance “Radioactive” Isotope in Air, Tissue, and what would be used for Shielding? Can it penetrate through the body?

Chemistry and measurement

What is natural radioactivity? Speak to the different types of radiation that an unstable nucleus may emit, and the different types of radiation involved.

Why is it important to be able to write a balanced nuclear equation for radioactive decay? Go into some of the specifics of what is involved in writing an equation.

What is a “half-life” and why is it important to know the half-life of a radioisotope? List a few applications of how scientists make use of having this knowledge. Why would it be so important to know the half-lives of radioisotopes when it comes to medical applications?

Briefly describe how we can make use our knowledge of radioactivity in medicine. Speak about the characteristics of the radioisotopes used in these types of applications. What might they have in common? What process(es) do we use to detect these radioisotopes?

Create a table like Table 4.7 in your eText, and seen below, of the Element’s “Normal” and “Radioactive” isotope. Describe atomic symbol, atomic number, number of protons, number of electrons, mass number, number of electrons, Mass of Isotope (amu) and Percent Abundance.

Describe Element’s “Normal” isotope’s properties (Review Section 4.8).

Where is the “Normal” isotope located on periodic table (for example, top right, bottom left, center)?

Is “Normal” Isotope Metallic, Non-Metallic, or Metalloid? What does it mean to have this characteristic?

What is “Normal” Isotope’s Atomic size and Ionization Energy? Describe how the “Normal” Isotope’s Atomic size and Ionization Energy affect its chemical properties?

Create two tables, one like Table 5.7 (Half-Life of Your Element Name Here) and one like Table 5.8 (Medical Applications of Your Radioisotope Name Here) from your eText of the Element’s “Radioactive” Isotope. In your Half-Life table describe your Element, Radioisotope’s Atomic Symbol, Half-Life, Type of Radiation. And then in your Medical Application table describe: Isotope, Half-Life, Radiation, Medical Application.

Describe and show how your isotope(s) decays? (for example, “it decays with the emission of an alpha-particle”). Give the specific chemical reaction and diagram it out, listing reactants and products. See image below for example

Describe the Radiation type that is emitted. Create table like Table 5.2 of “Radioactive” Isotope. Describe Type of Radiation, Symbol, Mass number and Charge.

Describe Radiation and Shielding Required. How the travel distance “Radioactive” Isotope in Air, Tissue, and what would be used for Shielding? Can it penetrate through the body?

Describe, in greater detail than above, all medical application(s) and how it is used.

Describe if there are any negative or hazards associated with element?

Calculate the amount of time needed to bring the radioactivity to 25%. Show math.

Nuclear Medicine and Medical Isotopes. (n.d.). Retrieved from https://www.acls-pals-bls.com/nuclear-medicine-and-medical-isotopes/

How much more of the Typical Energy Requirements for Adults you have left for the day based on your Gender, Age and Activity level.Are you currently on a diet now or have ever been on one? Add a description if so about the general type of diet.

Nutrition

Are you currently on a diet now or have ever been on one? Add a description if so about the general type of diet.

If you’ve been on a diet, did you do any calorie counting or take into consideration the energy of the food you were eating? If so, what was your method?

Did you ever take into account how much exercise you’d have to do to burn off a certain meal or indulgence? If so, how did you calculate that?a. What percentage of your typical energy requirements you consumed. (Show your full calculation)

How much more of the Typical Energy Requirements for Adults you have left for the day based on your Gender, Age and Activity level.

Summarize the major findings you found above. How did your Total Energy for this meal compared to Typical Energy? How long would it take you to burn off the energy you consumed – looking at how many hours of sleep and swimming was needed to burn off your Total Energy for this meal.

Discuss if the food items were a good energy source for you. If not, discuss why not. Foods differ in their density of a wide variety of nutrients as compared to just the calories they give you.

Explain why you chose each of these food sources and if you would select differently next time. If you were on a particular diet how would your meal fit into that diet.