ISN IV: Bonding Chemicals
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Cover & Things 2 Know
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Text
Pages 119-129
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3-4
Notes & Ions List
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Ionic Bonding Chips
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Text
Pages 130-135
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6-7
LAB: IONIC COMPOUNDS SAMPLER
Text
Pages 136-7
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Review of Ionic Bonding
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Text
138-142
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9-11
Bonding & Electron Dot Diagrams
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Formula Review
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13-14
Lab: Compounds & Bonding
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15-16
LAB: Molecular Models
10
Parent signature and Date
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12
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Parent signature ___________________________________date_______________
name:________________________________________per_____
Updated Things 2 Know
1. SAFETY FIRST!!
2. You are required to have a pencil or erasable pen, ISN with
cover, and calculator everyday.
3. Any missed labs or in class work should be made up during
lunch or X-Block or tutorial
4. Stout’s email address: [email protected]
5. Stout’s web site: www1.northbrook28.net/~cstout
6. Matter is anything with mass and volume
7. Matter is made of tiny particles that are always in some
motion.
8. Matter can exist in several states(or phases), the most
common are solid, liquid, gas and plasma.
9. Temperature is how fast the particles are vibrating
10. Matter can be described by physical and chemical properties
11. The Metric System is used to measure matter. Some common
measurements are length, mass, volume and density.
12. An element is the most basic type of matter that is still unique.
13. Atoms are composed of protons, neutrons and electrons.
14. The number of protons(atomic number) determines the identity
of an element
15. The periodic table is organized on several levels, including by:
atomic number, electron arrangement, and similar properties.
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NOTES
• # of valence electrons determines chemical properties of
an element/atom
• valence electrons involved in chemical bonding
• valence electrons located in highest energy level
• chemical bond: force of attraction that holds atoms
together
• Valence electrons: group 1 = 1, group 2= 2, groups
3-12= varies, group 13=3, group 14=4, group 15 = 5,
group 16=6, group 17=7, group 18= 8
• Group 18 (Noble Gases) most stable group on table it
has all 8 valence electrons (octet)
• Metals left side of staircase (Cu and Zn) & non metals
right side of staircase
Ionic Bonds
• ion: atoms that have a + or - charge
• Polyatomic ions: ions made of more than 1 atom
• Example: HCO3- (bicarbonate)
—-> Big clue: 2 capital letters next to each other
• Metal + Non Metal
• “Opposites Attract”
• Metal lose valence electrons = + ions
• Non metals gain valence electrons = - ions
• Ionic bonds form ionic compounds
• Valence electrons are transferred
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Positive & Negative Ions List
Positive 1+
Potassium Lithium
Silver
Sodium
Copper (I) Mercury(I) Hydrogen Cesium
Ammonium Negative 1K
Li
Ag
Na
Cu
Hg
H
Cs
NH4
Hydronium H3O
Positive 2+
Barium
Beryllium Cadmium Calcium
Cobalt(II) Copper(II) Iron(II)
Lead(II)
Magnesium Mercury(II)
Nickel(II) Strontium Tin(II)
Zinc Positive 3+
Ba
Be
Cd
Ca
Co
Cu
Fe
Pb
Mg
Hg
Ni
Sr
Sn
Zn
Aluminum Chromium(III)
Iron(III) Boron
Al
Cr
Fe
B
Acetate
Bicarbonate
Bisulfate
HCO3
HSO4
Bromide
Chloride
Chlorate
Br
Cl
ClO3
Chlorite
ClO2
Cyanide
Fluoride
Hydroxide
Hydride
Iodide
Nitrate
CN
F
OH
H
I
NO3
Nitrite
NO2
Permanganate
Negative 2CO3
Chromate
CrO4
Dichromate Cr2O7
Oxide
O
Sulfate
SO4
Sulfide
S
Nitride
Negative 3
Phosphate Diatomic Molecules: H2 O2 I2
!4
MnO4
Carbonate Positive 4+
Tin(IV)
Sn
Manganese Mn
C2H3O2
N
PO4
N2 Cl2
F2 Br2
Ionic Bonds
Write the chemical formula for each compound:
1. potassium hydroxide ___________________
2. potassium chloride _____________________
3. potassium oxide _____________________
4. potassium sulfate___________________
5. potassium nitride_____________________
6. potassium phosphate___________________
7. sodium hydroxide _____________________
8. sodium chloride _____________________
9. sodium oxide_____________________
10. sodium sulfate_____________________
11. sodium nitride_____________________
12. sodium phosphate_____________________
13. calcium hydroxide_____________________
14. calcium chloride_____________________
15. calcium oxide____________________
16. iron (II) hydroxide_____________________
17. iron (III) hydroxide_____________________
18. aluminum oxide_____________________
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LAB: Ionic Compounds Sampler
Nightingale:
1.Describe copper(II) sulfate:
color, state (s-l-g)
Name and Describe each of the three elements that make up copper sulfate
(HINT: look up sulfate on the IONS LIST on ISN page 4)
2.
3.
4.
5. What is the formula for copper(II) sulfate?________________________
Newton
6. Describe ammonium dichromate
7. What four elements make up ammonium dichromate?
______________________
_______________________
______________________
_______________________
8. Describe ammonia
9. Describe chromium
10. What is the formula for ammonium dichromate?___________________
Curie
11. Describe calcium carbonate:
12. Name and Describe each of the three elements that make up calcium
carbonate. (HINT: look up sulfate on the IONS LIST on ISN page 7)
12313. What is the formula for calcium carbonate? _______________________
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LAB: Ionic Compounds continued
Galileo
14. Describe lead oxide
15.Name and Describe each of the two elements that make up lead oxide?
1216. What is the formula for lead oxide?____________________________
Goodall
17.What two elements make up hydrogen hydroxide?
_________________&___________________
18.What is the formula for hydrogen hydroxide?
____________________________
19. Figure out the common name of hydrogen hydroxide?
__________________(hint:use your brain)
20. What is the common way to write the formula for hydrogen hydroxide?
________________
Einstein’s Questions:
21. What are some common characteristics of ionic compounds due to their crystal
structure? (see Text 136-137)
22. What happens to electrons in ionic compounds?
23. What is the overall charge of an ionic compound?
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REVIEW of IONIC BONDING
Use your Ions List to answer these questions & textbook p. 84-85 1. How many electrons does sodium lose in a chemical reaction? ______
2. How many electrons does phosphorous gain in a chemical reaction? _______
3. Name two metals that do not always lose the same number of electrons.
4. How can you tell that those two do not always lose the same number of
electrons? 5. Name four nonmetals that could take the electron(s) that lithium loses in a
chemical reaction. 6. In a chemical compound, would you expect an oxide ion to be joined with one
atom of calcium or one atom of potassium? 7. A compound of sodium nitride would contain how many sodium ions? 8. Predict the number of atoms of each element that would be needed to form a
compound of cadmium sulfide. 9. What is the formula for hydronium carbonate?
!8
Determining Ionic,Covalent or Metallic Bonding
From the name of a compound, can we determine whether it
is ionic or covalent or metallic Bonding?
Yes, from the name of the compound, you have to be able to figure out
whether you have metal bonding with metal, non-metal with non-metal, or
metal and non-metal. Remember, metals are on the left side of the “staircase” non-metals are on the right.
Fe (Iron), the metal iron with metal iron so it is metallic bonding
H2O (water), is non-metal hydrogen with non-metal oxygen is covalent bonding
Na2O (sodium), metal sodium with non-metal oxygen so it is ionic bonding
There are some exceptions to those rules. The exceptions involve the
polyatomic ion ammonium. Ammonium(NH4) is a polyatomic positive ion
and contains only non-metals. So it is possible to have nonmetals that are
found in ammonium(nitrogen and hydrogen) in the form of NH4 with a
positive charge. When combined with negatively charged non-metal you
get an ionic compound but you have no metal atoms contained in it!
QUESTIONS: Which of the following compounds are ionic and which are covalent?
1. ammonia(NH3)
________________
3. tin(IV) oxide
_________________
2. potassium nitrate ________________
4. hydrogen (H2)
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_______________
Electron
Dot
Diagrams
Almost all chemical reactions occur between electrons in the outer energy level
of atoms. For that reason, the outer energy level will be the only one considered
here.
1. In the most stable atoms, the noble gases- their outer energy level is full
2. In somewhat stable atoms - the sub-levels of their outer energy level are about
half-filled, like Carbon
3. Octet Rule -the maximum number of electrons in the outer energy level is 8.
(a)Atoms will combine to form compounds in order to reach eight electrons
in their outer energy level.
(b)Atoms with less than 4 electrons in their outer level tend to lose electrons
to form compounds.
(c)Atoms with more than 4 electrons in their outer level tend to gain electrons
to form compounds.
4. Electron-dot diagram - a way of drawing the outer energy level electrons of an
Lewis Dot Diagrams
atom. of the Elements
5. The chemical symbol for the atom is placed in the center of an imaginary
rectangle. The symbol represents the nucleus and all electrons of the atom,
Lewis Dot Diagrams of Selected
symbol represents an electron energy sub-level.
Elements
"dots".
6. Electrons are represented by
except the valence electrons. Each side of the imaginary box around the
Examples of Electron-dot diagrams
Index
Chemical
concepts
Chemistry
of the
Elements
Periodic
Table
Lewis Symbols Electron!10Configuration into Shells
Go Back
Electron Dot Diagrams (continued)
1.
Draw the electron-dot diagram for calcium.
2.
Draw the electron-dot diagram for sodium.
3.
Draw the electron-dot diagram for chlorine.
4.
Draw the electron-dot diagram lithium fluoride
5.
Draw the electron-dot diagram for a water molecule.
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Formula Review
Instructions: Compounds that form Ionic bonds (metal+ non metal)
Use charges on the IONS LIST on ISN page 4 to give the formula and the name
for each of the following compounds. NOTE: if there is no reaction possible
between the ions indicate by writing “NR.” 1 problem No Reaction (NR)
Ions in Compound Formula
Name
1. Mg O
2. Al
Cl
3. Zn I
4. Li
CO3
5. Al
Ba
6. Fe(II)
7. Ca
N
PO4
8. K Cl
9. Na
HCO3
10. Mn O
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COMPOUNDS & BONDING REVIEW
COMPOUND- ions combine chemically in a specific ratio, the ratio is indicated by a
formula
CHEMICAL FORMULA - shows the ratio by using SUBSCRIPTS
examples:
H2O
CuCl2
Al(CO3)3
How atoms combine is determined by the electrons in the outer energy level (VALENCE
ELECTRONS). The goal is to be STABLE with 8 electrons in the outer energy level. The
exception to this is an atom that just has one energy level then the number would be 2.
Atoms will gain, lose, or share electrons with each other to do this.
BOND - the force that holds atoms together - this bond is electrical in nature (+ or -)
ION - is a charged particle - if an atom loses electrons it becomes a positive ion - if an
atom gains electrons it becomes a negative ion
IONIC BONDING - bonding that occurs between opposite charged ions this happens as
one atom transfers electron(s) to another atom forming ions. Ionic bonding usually occurs
between metals and nonmetals
COVALENT BONDING - bonding that occurs between atoms as the share electrons to
become stable. Covalent bonding usually occurs between nonmetals
Hydrogen always covalently bonds
METALLIC BONDING - Occurs between metals. Metallic Bonding has free moving
electrons or “sea of electrons”
MOLECULE - a name applied to substances that are formed with covalent bonding.
FORMULA WRITING
OXIDATION NUMBER = VALENCE=Charge number
This is the combining ability of an atom. It tells how many electrons an atom will gain, lose,
or share when forming a compound. This is usually determined by the number of electrons
in the outer energy level but it can vary.
The sum of the oxidation numbers in compounds must equal 0
All compounds are electrically neutral
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COMPOUNDS & BONDING REVIEW Part 2
When writing a formulas the metal or the element with the positive (+) oxidation number/
is always written first
example:
NaCl or table salt. Na is positive and Cl is negative
The “Old” FORMULA TRICK
1. write oxidation numbers above the symbols
2. check to see if you have a positive(+) and negative(-)
3. check to see if they already add to 0 - if not go to 4
4. cross oxidation numbers to determine subscripts.
note: the number 1 is always implied
disregard negative sign
2+
Mg
-1
Cl
2+
Mg
-1
Cl
MgCl2
NAMING COMPOUNDS
BINARY COMPOUNDS - compounds made of 2 elements
IDE - in a binary compound, end the name of the second element with the ide suffix
sodium and chlorine make sodium chloride
POLYATOMIC IONS
• a group of atoms which act together as one charged particle called an ion. They
have their own name and oxidation number
• when you name compounds that have polyatomic ions in them you just use the
name of the polyatomic ion
NOTE - you must use ( )when you have more than one in the formula
example: Al2(CO3)3
is correct.
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Al2CO33 is NOT correct
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