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Chem Notes Part 1
Title
Unit 2: Chemical Reactions
Oct 1310:33 AM
Review Activity 1
Chemistry Review Activity: 29 Brains are better than 1...
1. At your first station, brainstorm with your group and try to write down as much information about chemistry from Science 9 as you can (matter, atoms, elements, periodic table, safety, etc). When the timer goes off, stop and look to the front for directions. (15mins)
2. Move clockwise to the next station & bring your markers. Edit the info listed by the first group if needed, and add anything you feel is missing. When the timer goes off, stop and look to the front for directions. (10mins)
3. Move clockwise to the next station & bring your markers. Edit the info listed by the first two groups if needed, and add anything you feel is missing. When the timer goes off, stop and look to the front for directions. (5mins)
4. Move clockwise to the next station. We'll take turns sharing info and use it to make review notes together. I'll help you decide if each piece is important enough to write down. If a group shares something that you have on your chart paper too, put an X by it so we don't write it down twice.
Review Activity 2
Chemistry Review Activity ‐ Throw down Showdown
1. Come up with a science‐themed team name. Write it at the top of your flip chart paper.
2. Brainstorm with your team ‐ write down anything and everything you can remember about the Atoms and Elements unit in Science 9 IN POINT FORM. Hide your work from the other teams!!
3. When the timer goes off, stop writing! Turn to face the front of the room. Keep one marker, and have one team member return the rest.
4. Taking turns, each team will offer one piece of information, while the other teams check their lists to see if they have the same idea written down. If you have something another team shares, put an X by it so you don't use that same fact again.
5. The only way your team scores a point is if you had something written down that no other team recorded!
Mon Oct 17
Monday, October 17th
• Chemical Compounds• Octet Rule• 3 Main Types• Ions & Ionic Compounds• Practice: p.189 #1‐4
• Gr 9 Review Quiz Tomorrow• I expect you to practice & study
Periodic Table
0.1 Chem Intro + Ionic Comp.notebook
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Chem Notes Part 1
Octet Rule
Compounds• 2+ different elements bonded in a fixed proportion• Atoms want to have a complete valence shell (like the noble gases)• They achieve this by sharing or transferring electrons:• Ex: H2O
• This is called the octet rule because most elements want 8 valence electrons. (Exceptions: Hydrogen and Helium only want 2).oNoble gases do not easily form compounds because their electron arrangements are already stable all by themselves.
3 Types of Compounds
Compounds• There are 3 main types of compounds:
• Ionic Compounds• Elements:• Electrons:• Example:
• Molecular Compounds• Elements:• Electrons:• Example:
• Metallic Compounds• Elements:• Electrons:• Example:
Atom to Ion
Ionic Compounds• Atoms become ions when they transfer (gain/lose) valence electrons.• ionic charge is the # value of the charge (+/‐). • Write as a superscript on the right of the symbol (ex. Ba2+).• Families tend to form ions with similar charges.• Look on the back of your Periodic Table!
(Cation) (Anion)
Periodic Table of Ions
Hydrogen fits on the left with the Alkali Metals because it has one valence electron that it can give away.
Hydrogen also fits on the right with the Halogens because it could gain one more electron and have a full valence shell.
Tues Oct 18
Tuesday, October 18th
• Gr 9 Review Quiz > MUST be written in pencil > MUST be marked in pen
• Ionic Compounds
• Practice: p.189 #1‐4
Ionic Compounds
Ionic Compounds• Made up of a metal and a nonmetal • Metals lose electrons & become positively charged• (they are conductors, so they don't hold them well) • Nonmetals gain electrons & become negatively charged• (they are insulators, so they do hold them well)
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Chem Notes Part 1
Ionic Bonding
Ionic Compounds• Ionic Bonding: oppositely charged ions are attracted to each other• Result = electrically neutral compound
Try it!
Beryllium & chlorine
Potassium & oxygen
p. 189 #14
p. 189 #1‐4
(or Lewis Dot)
p. 189 #12 ANS
p. 189 #1‐41. (a) How do metals form ionic compounds with nonmetals?
(b) Describe the process with an example.
2. Beryllium and fluorine react to form an ionic compound.(a) Which element is the metal and which is the nonmetal?
(b) Draw Bohr diagrams of beryllium and fluorine.
(c) How many electrons must each element gain or lose to form stable ions?
(d) Draw sketches to show how this compound forms by transfer of electrons.
(e) Indicate the ionic charges on the ions.
(f) Which is the overall charge on the compound?
(g) What is the chemical formula of the compound?
p. 189 #34 ANS
p. 189 #1‐43. Repeat question 2 for the compound formed by aluminum and
fluorine.(a) Which element is the metal and which is the nonmetal?
(b) Draw Bohr diagrams of aluminum and fluorine.
(c) How many electrons must each element gain or lose to form stable ions?
(d) Draw sketches to show how this compound forms by transfer of electrons.
(e) Indicate the ionic charges on the ions.
(f) Which is the overall charge on the compound?
(g) What is the chemical formula of the compound?
4. What part of the atom is involved in making chemical bonds?
Mon Nov 9
Monday, November 9th
• Ionic Compounds > Bonding > Naming > Formula Writing
– Practice: p.189 #1‐4
• Gr 9 Review Quiz Tomorrow > I expect you to practice & study
Binary Ionic Compounds
K2O potassium oxide
Ionic Compounds ‐ NAMING• Naming binary ionic compounds:• Normal metal name, then nonmetal name ending in “ide”• Tell you what elements are involved, but NOT how many of each
NaCl sodium chloride
CaF2 calcium fluoride
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Chem Notes Part 1
Chemical Formula
Compounds• A chemical formula is a combination of symbols that represent a particular compound. It indicates…o what elements are present, ando the number of each atom present
Formula Contains NameNaCl: ___ sodium, ___ chlorine
Mg2Se: ___ magnesium, ___ selenium
KF: ___ potassium, ___ fluorine
Fe3C: ___ iron, ___ carbon
Thurs Nov 12
Thursday, November 12th
• Chemical Formulas > Review > Short Cut > Practice p. 195 #1‐6
Notes
o NOTE…§ There are no spaces between symbols when writing chemical
formulas.§ Be sure to capitalize the first letter of a chemical symbol. If
there is a second letter, it is always lowercase.§ There is no need to write a subscript if there is only one atom of
that element present.
Ionic Compounds ‐ FORMULA WRITING
BaCl2
Nov 129:31 AM
Formula Writing
Ionic Compounds ‐ FORMULA WRITING1. Temporarily write the ionic charge above each symbol.2. Crisscross the ionic charges, using them as subscripts for the
opposite ions.3. Reduce the subscripts to the lowest numbers possible.
Calcium Phosphide
Practice
Ionic Compounds ‐ FORMULA WRITING
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Chem Notes Part 1
Oct 24
Monday Oct 24th
• Recap Friday• p. 195 #1‐9• Return a ton of work
• Quiz Monday on Ionic Compounds
p. 195 #19
p. 195 #1‐9
14 56
79 Oct 2411:02 AM
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Chem Notes Part 1
Polyvalent Ionic Compounds
Ionic Compounds ‐ NAMINGo Some metals can form more than one kind of ion – they are called
polyvalent metals.o Begin by writing the name of the metal and add a Roman numeral in
round brackets after it to indicate its ionic charge. Finish with the name of the nonmetal ending in “ide”.
Oct 25
Tuesday Oct 25th
• Ionic Compounds Practice Sheet
• Quiz Monday on Ionic Compounds
Oct 26
Wednesday Oct 26th
• Polyatomic Ions• Acids & Bases• More Practice!
• Quiz Monday on Ionic Compounds• Finish WHMIS Training TODAY!
Polyatomic Ionic Compounds
Polyatomic Ionic Compounds• Polyatomic ion: atoms that tend to stay together and carry an overall ionic charge (ex. Nitrate ion: NO3‐).
• Find this table on your Periodic Table of Ions.• Bond with metals to form a polyatomic ionic compound.
Polyatomic Ionic Compounds
o When writing the formula of a polyatomic ionic compound, add brackets around the ion before showing the number you need.§ Ex. Ba(NO3)2 – barium nitrate
o Write the name of the metal first, then the polyatomic ion's name.All other rules for formula writing and naming still apply!
Fe(NO3)3
Polyatomic Ionic Compounds
yttrium carbonate
Fe(NO3)2 zinc phosphate
p. 198 #14
1. In your own words, explain what is meant by "polyatomic ion." Give two examples.
3. Write the formulas for the following compounds: (a) sodium phosphate(b) calcium sulfate(c) potassium chlorate(d) aluminum hydroxide(e) beryllium nitrate(f) magnesium hydrogen carbonate(g) nickel carbonate
4. Write the names for the following compounds:(a) K2CO3
(b) Na2SO4
(c) Al(HCO3)2(d) AgNO3
p. 198 #1, 3, 4
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Chem Notes Part 1
p. 198 #14
1. In your own words, explain what is meant by "polyatomic ion." Give two examples.
3. Write the formulas for the following compounds: (a) sodium phosphate
(b) calcium sulfate
(c) potassium chlorate
(d) aluminum hydroxide
(e) beryllium nitrate
(f) magnesium hydrogen carbonate
(g) nickel (II) carbonate
4. Write the names for the following compounds:(a) K2CO3
(b) Na2SO4
(c) Al(HCO3)2
(d) AgNO3
p. 198 #1, 3, 4
Acids
AcidsAcids are special ionic compounds containing hydrogen. Hydrogen acts like the metal part of the compound (gives away its electron). Acids break apart into their ions in water.
Naming acids
hydrogen + nonmetal = hydro_______ic acid
hydrogen + _____ate = ________ic acid
hydrogen + ______ite = ________ous acid
Bases
BasesBases are special ionic compounds containing the polyatomic ion hydroxide. Bases break apart into their ions in water.
Bases have no special rules for naming ‐ just follow the normal instructions.