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Get a piece of paper and title it “UNIT 1 TEST CORRECTIONS”
Total Score out of 70 Add up the score on your MC with score on short answer to
calculate full score/70 Retakes mandatory for 70% and below You can retake just MC or just FR
Averages1st = 81.0%3rd = 83.4%4th = 82.4%5th = 82.5%6th = 79.9%
For each MC you missed, write the correct letter and explain why your answer was wrong.
For free response, completely re-answer the question Ex: 1a. Correct Answer = Schrodinger. My answer, Bohr,
was incorrect because Bohr described electrons as having specific energy levels, not traveling in waves.Retakes start today or by appointment through next
Wednesday!
Scientists/Atomic Theory
Periodic Trends Atomic Numbers, Isotopes, Ions
Electron Configurations
Bonding/Electronegativity
Phys/Chem/Nuclear Changes
As you correct your answers, categorize your
wrong answers to determine your areas of weakness for the retake.
After determining your top two areas of weakness, go to my website and find the document titled “Test One Content Revisit”
Complete the two short assignments for your two areas of weakness and turn in by Wednesday.
There will be no late work. No areas of weakness? Complete the enrichment
assignment on the same document. (Nuclear Reading and Questions)
Simple Ionic Compounds, Type II Ionic Compounds, Polyatomics
KCl – Potassium Chloride◦ In fertilizers◦ Alternate to NaCl, in water softeners and table salt◦ Lethal Injection (in high concentrations)
KClO3 – Potassium Chlorate◦ Pesticides◦ Generate oxygen on air & space craft◦ Propellant for gun power/explosives
Compounds like to be neutral, so the combined charges of the two elements must be neutral (ex: Na + and Cl-)
This determines how many of each atom goes into each ionic compounds (ex: 1 Na and 1 Cl)
BaO – Barium Oxide
Na2O – Sodium Oxide
2 of THAT atom
Al2S3 – Aluminum Sulfide
Hint: To make the compound neutral….
Look for the least common multiple and make the overall charge of each ion equal to this 6+ vs 6-
2 aluminum
3 sulfur
If making a compound from Al 3+ and S 2-, for example, “switch” the charges and make them subscripts.
Al2S3
There have to be 3 sulfur’s for every 2 aluminums to have a neutral compound (= # of + and -)
On the white grid, fill in the chemical formulas in the first 5 columns (there are little numbers in the boxes)
Write small! We will be adding a chemical name too!
Metals =Losers Positive = Ca+ions
Non-Metals =Thieves (Takers)
Neg = Anions
Many metals and non-metals have predictable charges- let’s label our periodic tables now!
A bond formed because e- transferred Electronegativity Difference =LARGE!!!
Or more simply put…between a metal & non-metal
Why does one Na bond with just one Cl?
How many Cl would bond with one Ca?
1) Metal first and keep their name2) Non-metal is 2nd and ends in –ide(POLYATOMIC ION NAMES DO NOT CHANGE!)3) Total charge must = Ø4) Subscripts = number of atoms5) Reduce subscripts
Example:Sodium & Oxygen
Na2OSodium Oxide
1. Potassium & phosphorus 2. Calcium and Bromine K3P CaBr2
Potassium Phosphide Calcium Bromide
You try writing the formula and name :NaI - Sodium Iodide Mg3N2 – Magnesium Nitride
AlF3- Aluminum Fluoride BaS - Barium Sulfide
Sodium & Iodine Magnesium & Nitrogen
Aluminum & Fluorine Barium & Sulfur