9/23 - Which parts of the lab do you NOT need to do? Do you still need to do observations for those parts?
9/25 - Give an example of a chemical change, and what evidence you would see from it.
9/30 - What is a significant digit? Why is it important? How do you know if a digit is significant?
10/2 - What are the rules for math with significant digits? What is the sum of 3.5 and 11? What is the product of those two?
10/8 - Why do we use Kelvin? What is the conversion from celsius to Kelvin? What is 20.5°C in Kelvin?
10/9 - How many inches are in a foot? What would that be as a conversion factor? How many feet are in 39 inches?
10/10 - How many cm are in a m? What would be the conversion factor? So, how many meters are in 655 cm?
10/11 - A Taco Bell box is 5.3cm by 20.8cm by 20.9 cm. What is the volume in cubic meters?
10/14 - What is 3.51x10² m³ in mm³?
10/15 - What is density? Is it intensive or extensive? What is the density equation? What is the density of an object of 36g and 6.0mL?
10/16 - What is the volume of an object with a mass of 117g and a density of 11.2 g/cm³?
10/17 - You have a beaker with a mass of 36.10g, then you add water, and it now has a mass of 42.23g. What is the mass of the water?
10/18 - What is the percent error calculation? What is the percent error if you measure the density of aluminum to be 2.56 g/mL?
10/21 - Convert 3.1x10³ mL to m³. Answer in scientific notation with correct significant digits.
10/22 - What is the first step in doing a conversion? How do you convert celsius to Kelvin?
10/23 - What do you know about atoms?
10/24 - How was the atom first described by Democritus then Dalton?
10/25 - What did Thomson add to the idea of the atom? What did he use?
10/28 - What was new in the Rutherford Model of the atom? What did he do to make his discovery?
10/29 - What is atomic number? What is mass number? How do you use these to determine number of neutrons?
10/30 - What is the number of protons, electroncs and neutrons in barium-138.
10/31 - How do you calculate average atomic mass? What is the average atomic mass if 33% has a mass of 5.9 amu and 67% has a mass of 5.0 amu?
11/1 - What is the difference between atomic number, mass number, and atomic mass?
11/4 - Where are the electrons in the atom? What else do we know about them?
11/5 - What was wrong with the Rutherford model of the electron? How did Bohr try to solve it?
11/6 - How did Schrodinger try to fix Bohr's model? What did he keep? What did he add?
11/7 - What are the 3 rules of electron configurations?
11/8 - Do the orbital diagram and electron configuration for arsenic.
11/11 - No School. Veteran's Day.
11/12 - What do you know about light and color?
11/13 - What happens to frequency when wavelength goes up? What happens to energy when wavelength goes up? What is this called?
11/14 - Draw the orbital drawing and electron configuration of silver. Should it be an exception to the aufbau principle? Why or why not?
11/15 - No journal.
11/18 - What information is on the periodic table?
11/19 - How do we organize the elements? How did they? (pg 155)
11/20 - What are the 3 classes of elements?
11/21 - What element is on energy level 2, and is in group 3? What about level 4, group 2?
11/22 - What direction does atomic size trend? What is larger: Al or N?
11/25 - What is electronegativity? Which direction does it trend? What has a higher electronegativity, Br or Be?
11/26 - What would have a higher first ionization energy, He or H? Why?
11/27 - Draw the directions of atomic trends for atomic size (radius), electronegativity, and ionization energy.
12/2 - How do ions form? What is the "goal" of forming ions?
12/3 - What is a valence electron? Why are only s and p electrons counted? What does that have to do with the octet rule?
12/4 - How do cations form? How do anions form? How would sulfide form? How would aluminum ion form?
12/5 - How would barium form an ion with nitrogen? Draw the starting atoms and the ending ions.
12/6 - What are the properties of metallic bonds? What causes each?
12/9 - What are the rules for naming monatomic cations? What about naming anions? What about transition metals?
12/10 - What suffixes do most polyatomic ions end in?
12/11 - What are the rules for writing ionic compounds? What is the formula of barium nitride? What about iron (III) chloride?
12/12 - What is the formula for copper (I) biphosphate? What about ammonium carbonate?
12/13 - What is an acid? What is a base? Was the formula for chloric acid? What about chlorous acid? What is the name of KOH?
12/16 - How is an ionic bond different from a metallic bond?
12/17 - Draw how the ionic compound between calcium and phosphide would form. Include the atoms and ions.
12/18 - What is the name and the formula for the combination of hydrogen and bromide ions?
12/19 - Write the acid naming rules.
12/20 - When do ions have roman numerals?
1/6 - How does an ionic compound follow the law of the octet?
1/7 - What is the difference between an ionic bond and a covalent bond?
1/8 - What are some properties of molecular compounds?
1/9 - What is a single covalent bond? A double covalent bond? A triple?
1/10 - Draw the bonds formed in F2. CO2. CH4. N2.
1/13 - Draw the structure of phosphate. It is a polyatomic ion that violates the octet rule.
1/14 - SNOW DAY!
1/15 - What is the VSEPR Theory? What does it mean? What shapes do you get?
1/16 - Draw nitrite. What VSEPR shape and angle does it have?
1/17 - Why are some bonds polar? How do you know whether or not they will be polar?
1/20 - Martin Luther King Jr. Day.
1/21 - What is the name of CF4? What about CO? What about P2O4?
1/22 - Draw water. Include the correct shape and polarity of the bond and molecule.
1/23 - How do you know if a bond is polar? How do you know if a molecule is polar?
1/24 - Have a classmate count your journals from 11/12 to 1/23 and binder items on a half-sheet.
- Start of Semester 2 -
1/27 - How many are in a pair? A dozen? A Sagan? Halvtred? A score?
1/28 - How many are in a mole? Why?
1/29 - How many molecules are in 2.00 moles of CO2? How many atoms is that?
1/30 - What is the molar mass of water? Carbon dioxide? Oxygen gas?
1/31 - Find the mass of 3.11 mol of water.
2/3 - How many liters is 0.791 mol. of N2 gas at STP? What would be the mass?
2/4 - What is STP? Be specific.
2/5 - What is the molar mass of magnesium?
2/6 - What is the equation for percent compositon? What percent of water is hydrogen, by mass?
2/7 - How do you determine empirical formula? What is the empirical formula of 7.75% H and 92.25% C?
2/10 - You are a CSI who has a white crystal found at a crime scene that could be strychnine (C21H22O2N2) or caffeine (C8H10O2N4). You find it is 49.5% carbon. What is it?
2/11 - Is C4H10 an empirical formula? If not, what would it's empirical formula be?
2/12 - How many moles, liters, and molecules would be in 12.1g of O2?
2/13 - Write the molar conversion map, and add density. Then also draw the map to determine formula.
2/14 - What is STP? What happens if you are above STP in temperature? What about pressure?
2/19 - What chemicals did we use in order to do our molar conversions lab. What was the result?
2/20 - Write the skeleton equation for the reation of glucose with oxygen to make carbon dioxide and water.
2/21 - No journal.