Name: _______________________________________
Date: Dec. 4, 2015
Outcomes
Outcomes 17, 19, & 20 Study Packet
The work you will do today covers all the material that you will be held responsible for on the
Outcomes you take next class period. You will be working to complete this packet and ensure
that you understand the material. At each station, collect a handout, read the Directions, and
get to work.
Outcome 17B: Lewis Dot Structures (front teacher’s desk)
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Refer to Outcome 16A!
Draw Lewis dot structures for compounds with single, double, and triple bonds
Answer questions about drawn Lewis dot structures
Outcome 19A: Ions (student desks)
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Define ion, cation, anion
Charges on elements
Explanation of why elements form ions and the charges they have
Outcome 20A: Nomenclature (back of room/lab area)
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Differentiate between ionic and covalent formulas/compounds
Write formulas
Explanation of ionic formulas (not just the trick)
OUTCOME 19A: IONS
1. Define ion:
2. Why do atoms form ions?
Fill in this chart:
Element
Does it gain or lose
electrons? And how many?
Charge
Strontium (Sr)
Bromine (Br)
Sodium (Na)
Aluminum (Al)
Phosphorus (P)
3. Pick an element in the table above that has an ion that is a cation. Explain what makes it a cation.
4. Pick an element in the table above that has an ion that is an anion. Explain what makes it an anion.
5. How many total electrons does each of these ions have?
a. Strontium:
______
b. Bromine:
______
c. Aluminum:
______
6. An element has 19 protons, 18 electrons, and 17 neutrons. What is its charge? ____________
7. What best explains why strontium is in group 2?
These are all from students’ answers on a homework assignment. The question was “What is the charge
of sulfur. Why does it have that charge?” For each student answer, write what is missing or what is
wrong. You do NOT need to re-write them. Remember that answers should meet the three criteria we
learned in class.
Student Answer
1
2
3
Sulfur has a negative charge. Sulfur has
a negative charge because it’s a nonmetal element and it’s gaining electrons.
The charge of sulfur is 2-. It is 2 because
it has seven valence electrons so it
needs to gain two to have a full outer
energy level. It is negative because when
it gains two electrons, it will have more
electrons than protons.
The charge of sulfur is 2-. It’s 2 because
it needs two valence electrons to reach
its full outermost energy level, so it
gains 2 valence electrons. It’s negative
because it’s more electrons than
protons.
4
The charge of sulfur is 2-. Sulfur has that
charge because it has 6 valence
electrons so it needs to gain 2- electrons
to have the full outermost energy level.
5
The charge of sulfur is 2-. It is 2 because
it has two valence electrons, so it needs
to gain 2 to have a full outer energy
level.
6
The charge of sulfur is 2- because sulfur
has 6 valence electrons and to become
an ion, it would rather gain 2 electrons
than lose 6 because it’s easier so sulfur
gains 2 electrons making the charge 2-.
7
Sulfur’s charge is a cation.
Missing and/or Wrong
Your Turn! Write the completely correct explanation for sulfur – What is the charge of sulfur? Why does it
have that charge?
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OUTCOME 20A: NOMENCLATURE
For this outcome, you need to be able to write formulas for ionic and covalent compounds, but you ALSO
have to explain why a formula is what it is. To provide you practice, I have provided a sample question
and 2 correct responses. Read that one and then do your own.
Sample Question: Explain why the formula for calcium fluoride is CaF2 and not CaF. Where
does the 2 come from? (Do not use the criss-cross trick to explain.)
Sample Answer 1: All ionic compounds need to be neutral. Each calcium ion has a 2+
charge and each fluorine ion has a 1- charge. In order to be neutral, the compound needs to have
two fluorine ions, which will give it a 2- charge to balance out one calcium ion.
Sample Answer 2: All ionic compounds need to be neutral. This shows how one calcium ion and
two fluorine ions makes the compound neutral:
Ca
F
2+
112+
2-  No charge means neutral
Your Turn!
You can use either strategy shown in the sample answers – whichever you are more comfortable with.
You will need to be able to do this on the outcome.
Explain why the formula for beryllium phosphide is Be3P2. Where do the numbers come from? (Do not
use the criss-cross trick to explain.)
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Posted on the lab tables are names of 20 compounds total. Copy the names into this chart as you rotate
and then write the formulas for the compounds! Remember to first determine if they are ionic or
covalent!
Compound Name
1. copper (II) oxide
2. sodium hydroxide
3. dinitrogen trisulfide
4. gallium chromate
5. aluminum sulfide
6. Iron (II) sulfite
7. Disulfur dichloride
8. Silver (III) phosphide
9. Carbon monoxide
10. Calcium sulfate
11. Vanadium (III) hydroxide
12. Nitrogen tribromide
13. Potassium oxide
14. Calcium chlorate
15. Disulfur hexachloride
16. Beryllium nitrite
17. barium cyanide
18. dioxygen pentiodide
19. Magnesium phosphate
20. gallium bicarbonate
Formula