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Given a name, write a formula. Given a formula, write a name.

1. PCl₅
2. P₄O₁₀
3. SF₆
4. PCl₃
5. H₂O

6. trisilicon tetranitride
7. dioxygen difluoride
8. iodine heptafluoride
9. arsenic triiodide
10. carbon monoxide

Fill in the following table by calculating the total number of valence electrons, drawing a correct Lewis structure, and giving the name of the 3-D shape.

Assign the correct ionic charge to the following elements. The first one is done for you as an example.

1. Li⁺
2. Be
3. B

3. N
4. O
5. F

Build all possible compounds from the following ions and write their names. The first one is done for you.
K⁺, Ca²⁺, Al³⁺, P^3–, S^2–, I^–

1. K₃P potassium phosphide
2.  
3.  
4.  
5.  

6.   
7.   
8.   
9.   

Build all possible compounds from the following ions and write their names. Remember that some ions, those made from the transition elements in groups 3 – 12, can have more than one possible charge. The name must include the charge of the ion as a roman numeral. The first one is done for you.
Fe²⁺ (iron(II)), Fe³⁺ (iron(III)), N^3–, O^2–, F^–

1. Fe₃N₂ iron(II) nitride
2.  
3.  
4.  
5.  

6.  
7.  
8.  
9.  

Write the name of the compound given a formula or write the formula given the name. The Ions Reference will be helpful here. Remember that acids have formulas starting with the hydrogen ion (H⁺) like HCl orH₂SO₄.

1. Fe(NO₂)₂
2. Fe(NO₃)₃
3. CuOH
4. Cu(OH)₂
5. CaCO₃
6. Ni₂(CO₃)₃
7. NiCO₃
8. H₂SO₄

9. sodium sulfate 
10. aluminum sulfate 
11. cobalt(II) nitrite 
12. cobalt(III) sulfite 
13. magnesium phosphate 
14. chromium(III) chlorate 
15. barium chloride 
16. nitric acid 

Answer the following questions.

1. What makes the formula of an electrolyte different from the formula of a non-electrolyte? Give examples for the formulas of each type of compound.
2. Why do solutions of electrolytes in water conduct electricity?

Moles: Numbers and Masses

Molar Masses

Putting Molar Masses to Work

For each of the masses, convert to number of moles. For each quantity given in moles, convert to mass in grams. Express each answer with the correct number of significant figures.

Chemical Equations

Balancing Equations

Classifying Chemical Reactions

Stoichiometry with Limiting Reactants

1. Nitrogen Gas and Hydrogen Gas react to form Ammonia. (All reactants and products are gases).
   N₂ + 3H₂ → 2NH₃
   1. If you have 1 mol of nitrogen gas and 4 mol of hydrogen gas how many moles of ammonia form? If any reactant gases are leftover give the amount of each in moles that did not react.
   2. If you want to make 25 mol of ammonia, how much nitrogen and hydrogen gas do you need in moles?
   3. If you have 3 mol of nitrogen gas and 3 mol of hydrogen gas how many moles of ammonia form? If any reactant gases are leftover give the amount of each in moles that did not react.
   4. If you have 5.7 mol of nitrogen gas and 12.9 mol of hydrogen gas how many moles of ammonia form? If any reactant gases are leftover give the amount of each in moles that did not react.
   5. You have 12 mol nitrogen and an unlimited supply of hydrogen. How much ammonia can you make (in moles)?
2. Zinc and Hydrochloric Acid react to form Zinc Chloride and Hydrogen Gas.
   Zn + 2HCl → ZnCl₂ + H₂
   1. You want to make 0.75 mol of hydrogen gas. How many grams of zinc do you need to use?
   2. You have 10 mol zinc and 15 mol hydrochloric acid. How many moles of hydrogen gas can you make? If any reactants are leftover give the amount of each in moles that did not react.
   3. You have 130.8 g of zinc and 1 mol of hydrochloric acid. How many moles of hydrogen gas can you make? If any reactants are leftover give the amount in grams of each that did not react.

3. Benzene (C₆H₆) burns in oxygen to form carbon dioxide and water.
   2C₆H₆ + 15O₂ → 12CO₂ + 6H₂O
   1. If you burn 2 mol of benzene how much oxygen (in moles) is required to burn all of the benzene?
   2. How many moles of carbon dioxide result from the burning of 2 mol of benzene?
   3. How many moles of water result from the burning of 78.1 g of benzene?
   4. How many grams of carbon dioxide result from the burning of 156.2 g of benzene?
4. Elemental sulfur (S₈) reacts with fluorine gas to form sulfur hexafluoride.
   S₈ + 24F₂ → 8SF₆
   1. How many moles of fluorine gas are required to react with each mole of elemental sulfur?
   2. If you have 12 mol of fluorine gas and 2 mol elemental sulfur then how many moles of sulfur hexafluoride can you make? If any reactants are leftover give the amount of each in moles that did not react.
   3. If you have 2.4 mol of fluorine gas and 0.05 mol elemental sulfur then how many moles of sulfur hexafluoride can you make? If any reactants are leftover give the amount of each in moles that did not react.
   4. You have 128.25 g of elemental sulfur. How many grams of fluorine gas are required to react with all of the sulfur?
   5. You have 384.8 g of elemental sulfur. If you have more than enough fluorine gas to react with all of the sulfur then how many grams of sulfur hexafluoride can you make?

Light and Atoms

1. Draw a simple wave and label wavelength and amplitude.
2. Draw two waves with different frequencies. How can the drawing tell you about the frequency of the wave?
3. Fill in the blanks with the word ‘increases’ or ‘decreases’.
   As wavelength increases, frequency __________________.
   As frequency increases, wavelength __________________.
   As frequency increases, energy per photon __________________.
   As frequency decreases, energy per photon __________________.
4. What is meant by the ground state and excited state of an atom?
5. An electron must gain energy to move farther away from the nucleus. According to your reading how do electrons gain energy to move to higher energy levels?
6. Just as a ball naturally rolls downhill (and not uphill) an electron naturally falls down to lower energy levels, eventually reaching the ground state. How is the excess energy released when this happens?
7. Why do different elements have different bright line spectrums?
8. What are the different regions of the electromagnetic spectrum called? List them in order from longest to shortest wavelength.
9. What are the different regions of the electromagnetic spectrum called? List them in order from largest to smallest energy.

Use the Speed Formula to find wavelength (λ) given frequency or to find frequency (f) given wavelength. For each problem identify what part of the electromagnetic spectrum each problem refers to by using the spectrum reference sheet you have received.

Sometimes wavelengths of light are given in nanometers (nm, 1 m = 1 × 10⁹ nm) or micrometers (μm, 1 m = 1 × 10⁶ μm). Visible and ultraviolet light are measured using nanometers (nm) and infrared and some microwave wavelengths are are measured using micrometers (μm).

For each of the following problems find the wavelength in meters and then decide whether the light is in the ultraviolet (UV) (10 nm – 400 nm), Visible (400 nm – 700 nm) or the infrared (IR) range (0.7 μm – 1000 μm). If it is in the UV or visible range convert meters to nanometers. If it is in the IR range convert meters to micrometers.

Frequencies, too, are sometimes given in units other than Hz (1/s). The only proper unit to use in c = λf is 1/s (which is the same as Hz). So when frequencies are given in kHz, MHz, or GHz it is necessary to convert them first.
1 GHz = 1 × 10⁹ Hz           1 MHz = 1 × 10⁶ Hz          1 kHz = 1,000 Hz.

Find the wavelength in meters for each of the following frequencies.

Use Planck’s Formula (E = hf) to find energy per photon (E) given frequency (f) or to find frequency given energy per photon. For each problem identify what part of the electromagnetic spectrum each problem refers to by using the spectrum reference sheet you have received.

Often it is important to be able to use a wavelength (λ) to find the energy per photon (E). This is a two-step calculation in which you must first use c = λf to find frequency (f) and second use E = hf to find energy per photon (E). For each of the following, perform the indicated calculation. For each problem identify what part of the electromagnetic spectrum each problem refers to by using the spectrum reference sheet you have received.