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