UNIT 1

1.1

100

Write the Atomic Symbol for this element. 

Protons - 14

Neutrons - 10

Electrons - 13

Si is the symbol, 14 is the bottom number, 24 is the top number, and there is a negative one charge on the atom

200

What is the mass in grams of 3.25 x 10^22 Krypton atoms?

3.25E22 x (1 mol Kr / 6.022E23) x (83.798 g Kr / 1 mol Kr) --> 4.522475922 grams

300

Write the nuclide symbol of two isotopes for a -1 ion with 13 electrons.

I will determine if they are correct

400

What mass of phosphorus contains the same number of atoms as 16.5 grams of Bromine? Explain why your answer makes sense logically.

16.5 g Br x (1 mol Br / 79.904 g Br) x (1 Mol Br / 1 Mol P) x (30.973762 g P / 1 mol P) --> 6.40 grams

1.2

100

Write the chemical symbol of Zinc Hydroxide

ZN(OH)₂

200

Name this compound SF₆

Sulfur Hexafluoride

300

DRAWING:

Draw the difference between the molecules HBr and Li₂S - Explain the difference between the drawings

I will determine if it is correct

400

A polyatomic compound has Na, O, and S. The sample contains 52.8% sodium, 20.2% oxygen, and 27% sulfur. Using this information find the empirical formula for the compound. (FOR THIS YOU DO NOT NEED WHOLE NUMBERS IN YOUR EMPIRCAL)

Na_2.7O_1.5S

1.3

100

2NaCl + H₂SO₄ --> NaHSO₄ + HCl

2.5 moles of sodium chloride react with excess sulfuric acid if 1.8 moles of NaHSO₄ is produced what is the percent yield?

144%

200

Balance this chemical equation: 

__ C₄H₁₀ + __ O₂ --> __ CO₂ + __ H₂O 

How many grams of water are produced from 3.2 moles of C₄H₁₀ burned in excess oxygen?

2, 13, 8, 10

288.3 Grams

300

4NH₃(g)+3O₂(g)→2N₂(g)+6H₂O(g)

If you start with:

• 5.0 moles of NH₃

• 6.0 moles of O₂

1. Identify the limiting reagent.

2. Determine the theoretical yield of nitrogen monoxide (N₂) in moles.

3. Calculate how many moles of excess reactant remain after the reaction is complete.

• Limiting Reagent: NH₃ (ammonia)
• Theoretical Yield of N₂: 2.5 moles of N₂
• Excess Reactant Remaining: 2.25 moles of O₂

400

4NH₃ + 3O₂ --> 2N₂ + 6H₂O

If you start with:

• 8.0 moles of NH₃
• 12.0 moles of O₂

1. Identify the limiting reagent.
2. Determine the theoretical yield of nitrogen monoxide (N₂) in moles.
3. Calculate the mass of the excess reactant remaining after the reaction is complete.

• Limiting Reagent: NH₃ (ammonia)
• Theoretical Yield of N₂: 4.0 moles of N₂
• Mass of Excess Reactant (O₂) Remaining: 192.0 grams of O₂

Conceptual

100

How would you find the average atomic mass given two isotopes and their percentage of prevalence? 

You would make the percentages into decimals and then multiply the molar weights of each one by their abundance rate. Then add them together. 

200

What is the difference between molecular and ionic bonds? Explain in terms of their naming. 

Molecular - non metals - Greek Pre-Fixes

Ionic - 1 Metal and 1 Non-Metal - Fixed charge no RN if variable charge include RN

300

Whats the difference between saying molecule vs atoms?

Molecules is the entire compound while atoms are the individual parts of each of the compounds.

400

What equation would you use if you were given 2 volumes and 1 molarity? What is the equation for molarity? 

M₁V₁ = M₂V₂

_mol/L