Announcements Exam #1: Tonight!, 7:00-8:30pm, locations posted on website, bring ID Conflict Exam: 5:00-6:30pm, 161 Noyes, bring ID No Lab this week! No book homework due Friday! Lecture on Thursday! (New Material) Exam scores posted late Wednesday evening. Get graded exams back on Friday. Liquid nitrogen ice cream winner = highest section average!!!

Chemistry Joke of the Day Q: What do chemists call a benzene ring with iron atoms replacing the carbon atoms? A: A ferrous wheel.

Exam Format – 90 minutes total 15 Multiple Choice Questions 2 Free Response Questions 5 possible choices 50% of test grade ~3 minutes to answer each (~45 min on this half of exam) Write in answers – both qualitative and quantitative 50% of test grade ~45 minutes on this half of exam ***A periodic table & cover sheet with equations will be attached.***

Most Requested Topics Polyatomics help please! Partial pressure Ideal gas law Empirical & molecular formula Finding “unknown” elements Please no more lighting things on fire 

Clicker #1 What is the molar mass of nickel(II) carbonate?   a) 74.02 g/mol b) 118.7 g/mol c) 134.7 g/mol d) 178.71 g/mol e) 296.09 g/mol

Clicker #2 A 88.02 g of carbon dioxide and 92.02 g of dinitrogen tetroxide are mixed in a rigid steel container. Which of the following is true regarding the partial pressures of the two gases? The partial pressure of carbon dioxide is half that of dinitrogen tetroxide. The partial pressure of the gases is the same. The partial pressure of carbon dioxide is twice that of dinitrogen tetroxide. The partial pressure of carbon dioxide is four times that of dinitrogen tetroxide. Without knowing either the temperature or the volume of the gases, it is impossible to draw any conclusions about the partial pressures of the two gases. Follow up: Explain based on kinetic molecular theory – why does CO2 have a higher partial pressure than N2O4?

Clicker #3 If a gaseous mixture is made of 3.50 g of He and 5.75 g of Ar in an evacuated 2.05-L container at 25°C, what will be the partial pressure of Ar in the container? a) 1.72 atm b) 5.75 atm c) 10.4 atm d) 11.9 atm e) 12.1 atm Follow up: What is the total pressure in the container?

Clicker #4 A compound consists of silicon and 8.23% by mass of hydrogen. The molar mass of the compound is approximately 122 g/mol. What is the molecular formula of this compound?   a) Si4H10 b) SiH2 c) SiH3 d) Si2H5 e) Si4H12

Clicker #5 A member of the alkaline earth metal family whose most stable ion contains 36 electrons forms a compound with bromine. What is the correct formula for this compound?   CaBr2 BaBrO3 KrBr RbBr SrBr2

Clicker #6 A flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level, where the temperature is 25oC and the barometric pressure is 0.947 atm. The balloon then rises to an altitude of 6000 ft, where the pressure is 0.796 atm and the temperature is 15oC. What is the change in the volume of the balloon as it ascends from sea level to 6000 ft?   128 L b) 373 L c) 610. L d) 983 L e) none of these?

Clicker #7 You are given 0.785 lbs. of magnesium phosphate. How many moles does this represent? (1 kg = 2.205 lbs, 1 kg = 1000 g)   a) 1.35 mol b) 1.54 mol c) 2.98 mol d) 93.6 mol e) 206 mol

Clicker #8 A gas sample containing 2.50 mol at 25°C exerts a pressure of 1.00 atm. Some gas is added to the same container and the temperature is increased to 50.°C. If the pressure increases to 2.00 atm, how many moles of gas were added to the container? Assume a constant-volume container.   1.25 mol b) 2.11 mol c) 2.50 mol d) 4.61 mol e) 5.00 mol

Clicker #9 15. If you have equal mole samples of each of the following compounds, which compound contains the greatest number of oxygen atoms?   magnesium nitrate dinitrogen pentoxide iron(III) phosphate barium oxide potassium acetate

Clicker #10 Which of the following is true regarding ? # protons # electrons # neutrons mass number a) 26 29 30 56 b) 26 30 23 49 c) 26 23 30 56 d) 30 29 26 56 e) 26 26 23 49

Clicker #11 Which sample contains the greatest number of atoms? 10.0 g Na 10.0 g Fe 10.0 g Ag 10.0 g Cu 10.0 g Ba

Clicker #12 Which of the following statements is true?   An 18.02-g sample of water contains 6.022 × 1023 molecules of water. The mass of one nitrogen atom is 14.01 g. If five “units” of iron(III) nitrate is dissolved, there will be 65 particles in solution. One mole of sodium (Na) is equal to 22.99 atomic mass units (amu). For every one mole of magnesium phosphate, there are six moles of oxygen atoms present.