Day 2: Class Review AtomsIonsIsotopes, Periodic Table, Using the Bohr Model

Atomic Structure:1. How does changing the number of protons affect the atom?2. How does changing the number of electrons affect the atom?3. How does changing the number of neutrons affect the atom?

Atoms and Ions Finding P, E, N

Determine the Average Atomic Mass of Each of the Following:

Isotope % Abundance Mass Mass ContributedNitrogen-14

Nitrogen-15

99.634

0.366

14.003074

15.000108

(Answer)

Isotope % Abundance Mass Mass ContributedOxygen-16

Oxygen-18

99.762

0.200

15.994915

17.999160

(Answer)

Isotope % Abundance Mass Mass ContributedNeon-20

Neon-22

90.51

9.22

19.992435

21.991383

(Answer)

4. Identify the number of Protons, Neutrons, and Electrons in the following: a. Phosorus-33 b. Carbon-14

5. An isotope of phosphorus (phosphorus-32) has a half-life of 320 years. If 5.0 mg of phosphorus-32 disintegrates over a period of 960 years, how many mg of phosphorus-32 would remain?

6. The half-life of U-240 is 1.2 million years. How many years would it take for a 10.0 g sample of U-240 to decay and have only 0.3125 g of it remain?

Periodic Table1. How many protons do each of the following elements have?a. calcium ________ b. sodium ________ c. iodine ________ d. sulfur ________e. nitrogen ________ f. mercury ________ g. ununoctium _______ h. silver ________

2. How many occupied principal energy levels do elements in period 4 have? _____________________3. How many valence electrons do the elements in group 17 have? ___________________4. What are the oxidation states for: a. elements in group 1? _______ b. elements in group 2? ________5. Draw the electron dot diagram representing valence electrons for each of the following:

a. K B. Sr c. B d. Si e. N f. S g. Cl h. Ar

Periodic Trends1. As you go from left to right across a row of the Periodic Table:

a. What happens to the atomic number and the number of protons? ____________b. As a result, what happens to the pull on the electrons? __________c. Therefore what happens to the atomic radius? __________d. Finally, what does this mean about the likelihood of losing electrons? Do the elements become more or less metallic?

2. As you go from top to bottom down a column of the Periodic Table:a. What happens to the number of shells? ___________b. As a result, what happens to the atomic radius? __________c. Therefore, what happens to the pull on the electrons? _________d. Finally, what does this mean about the likelihood of losing electrons? Do the elements become more or less metallic?

3. What do the elements at the extreme right of the Periodic Table have in common? What affect does this haveon the chemical properties?

4. Which group in the periodic table contains the most reactive metals? _______________a. Which element in the group is the most reactive? __________b. Do they have high or low ionization energies?_________ Which within the group has the lowest?

_____c. Do they have high or low electronegativity? __________ d. Do they readily gain or lose electrons? _____________

5. Which group in the periodic table contains the most reactive nonmetals? ______________a. Which element in the group is the most reactive? __________b. Do they have high or low electronegativities?_________ Which within the group has the higehst?

____c. Do they have high or low ionization energies? __________ d. Do they readily gain or lose electrons? _____________

Draw arrows on the periodic table and tell what is happening to the 1. Electronegativity2. Atomic Radius3. Ionization Energy

Electron Configuration:Draw the Electron configuration pattern and include all orbitals? Make sure to write out the 1s, 2s, 2p, ect….

Electron Configurations1) Write the full electronic configuration (1s2s2, etc.) for each of the following elements. 2) Circle the Valence electrons. 3) Write the complete orbital diagram (that’s the little boxes) 

a.) silicon, z = 14

b.) argon, z = 18

c.) magnesium, z = 12

Waves and Bohr Model1. a. How are wavelength and frequency of electromagnetic radiation related?  

b. How are the energy and frequency of electromagnetic radiation related?  

c. How are the energy and wavelength of electromagnetic radiation related?

d. A beam of red light has higher or lower energy than blue light? ___________

2. In the line spectrum for hydrogen, 2 of the emission lines in the visible line spectrum are red and green. The electrons responsible for these lines had to “fall” closer to the nucleus to emit the light. Which electron “fell” farther, the one causing the red line or the one causing the green line? Explain.

3. An electron in a hydrogen atom falls from the 3rd energy level to the 2nd. What wavelength of light is produced?

4. An electron in a hydrogen atom falls from the 4th energy level to the 2nd. What wavelength of light is produced?

5. How do the waves in questions 3 and 4 compare in: State which wave contains the Larger and Smaller

a. wavelength?

b. frequency?

c. energy?

d. speed?