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Starter
Use your Polyatomic Sheet/Flash Cards to write the chemical formula of each polyatomic below:
1. Phosphate
2. Nitrite
3. Hydrogen Carbonate
4. Ammonium
5. Perchlorate
Name the following polyatomic ion: SO4
2-
A.) sulfur tetraoxide
B.) sulfur oxite
C.) sulfite
D.) sulfate
E.) sulfete
Name the following polyatomic ion: ClO4
-
A.) hypochlorite
B.) chlorite
C.) chlorate
D.) perchlorate
E.) chloroxite
Write the formula for the following polyatomic ion: hydroxide
A.) HO
B.) HO-
C.) OH
D.) OH-
E.) H2O
Unit Four: Bonding/Nomenclature
GPS SC1: Students will analyze the nature of matter and its classifications.
Classification of Matter
Mixtures
Elements
MetalCation
NonmetalAnion
Ionic
Nonmetal Nonmetal
Covalent
Compounds
Pure Substances
Matter
Formation of Ionic Bonds
Opposites _____________________.
A metal loses an electron(s), and the nonmetal gains an electron(s).
Cation and anions form as a result.
The two ions are electrostatically-attracted, and form an ionic bond.
Ionic Bond
Ionic bond: the electrostatic force that holds oppositely charged particles together in an ionic compound
Compounds that contain ionic bonds are called ionic compounds.
Ionic compounds form between metals and nonmetals.
Writing Ionic Compound Names from the Formulas
When given a formula, analyze the ions.
Identify the two ORIGINAL ions that were used.
Name the cation first (Transition dilemma – CRISS CROSS METHOD)!
Name the anion last (Use -ide for non-polyatomic atoms)!
Practice Writing Names from Chemical Formulas
Write the name of the compound that is represented by the following formula:
– MgCl2
Magnesium Chloride
Name the following compound: CrPO4
A.) chromium phosphate
B.) chromium (I) phosphate
C.) chromium (II) phosphate
D.) chromium (III) phosphate
E.) chromium (IV) phosphate
What is the name of MnO4-?
A.) permanganate
B.) manganate
C.) manganite
D.) hypomanganite
Name the following compound: PbS
A.) lead sulfur
B.) lead sulfide
C.) lead (I) sulfide
D.) lead (II) sulfide
E.) lead sulfate
Name the following compound: Al2(SO4)3
A.) aluminum (III) sulfate
B.) aluminum sulfate
C.) aluminum (II) sulfate
D.) aluminum sulfite
E.) aluminum sulfide
Name the following compound: Cu2CO3
A.) copper carbonate
B.) copper (I) carbonate
C.) copper (II) carbonate
D.) copper (II) carbonate (III)
E.) copper carbontrioxide
Name the following compound: NiSO4
A.) nickel sulfate
B.) nickel (I) sulfate
C.) nickel (II) sulfate
D.) nickel (III) sulfate
E.) nickel (IV) sulfate
Name the following compound: KBr
A.) potassium bromide
B.) potassium (I) bromide
C.) potassium bromite
D.) potassium bromate
Name the following compound: TiO2
A.) titanium oxide
B.) titanium (II) oxide
C.) titanium (IV) oxide
D.) titanium oxide (II)
Starter:
How can you determine if a compound is Ionic?
Examine the formula to name the following Ionic Compounds:
1.MgO 3. KOH
2.V(ClO)2 4. CuSO4
Criss-Cross Method for Writing Chemical FormulasLet’s predict the formula for the stable ionic compound that contains:
–calcium ion and phosphide
–aluminum ion and sulfate
–tin(II) and carbonate
Valence Electrons & Stability Review
Questions to ALWAYS ask yourself:• What is the charge on the ions (how
would they change their electrons to become more stable)?
• Are transition metals involved?• How many of the cations/anions are in
the compound? (CRISS-CROSS METHOD)
• Is the ratio (AKA formula unit) reduced?
What is the chemical formula for sodium hypochlorite?
A.) NaCl
B.) NaClO
C.) NaClO2
D.) NaClO3
E.) Na(ClO)
What is the chemical formula for titanium (IV) oxide?
A.) Ti4O
B.) Ti4O2
C.) Ti2O
D.) Ti2O4
E.) TiO2
What is the chemical formula for magnesium oxide?
A.) MnO
B.) MnO2
C.) MgO
D.) Mg2O2
E.) MgO2
What is the chemical formula for nickel(II) nitrate?
A.) Ni2NO3
B.) Ni1NO32
C.) NiNO3
D.) (Ni)(NO3)2
E.) Ni(NO3)2
What is the formula for hydrogen carbonate?
A.) H2CO3
B.) HCO3-
C.) HCO32-
D.) HCO3
What is the chemical formula for magnesium phosphate?
A.) MgP
B.) Mg3P2
C.) MgPO4
D.) Mg2(PO4)3
E.) Mg3(PO4)2
After the quick review,
NEW VOCAB: The formulas that you have written are called “formula units.”– The smallest whole number ratio of ions
that form a stable, neutral ionic compound
Do you suffer from:– Parenthesesitis
– Reduce-a-phobia
– Nomenclaturosis
Starter:
Name the following Ionic Compounds:
1.BaS
2.Pb(NO2)3
Write formulas for the following Ionic Compounds:
3. Aluminum Oxide
4. Thallium (III) Sulfite
5. Potassium Chlorate
Write the chemical formula for zinc selenide.
A.) ZnSe
B.) Zn2Se
C.) ZnSe2
D.) Zn2Se2
Write the chemical formula for calcium nitrate.
A.) CaNO3
B.) CaNO2
C.) Ca(NO3)2
D.) Ca(NO2)2
E.) Ca3N2
Write the chemical formula for cobalt(III) phosphide.
A.) Co3P
B.) Co3P3
C.) CoP
D.) CoPO3
E.) CoPO4
Formula unit ratios form beautiful crystals…Ionic compounds are crystals!
What You’ll See in Our Lab
Ionic compound solids that form when two solutions are mixed
“Snow Globe” effectSeparation
line Paint effect
Physical Properties of Ionic Compounds
Applying heat to melt sodium chloride
Applying a current to test conductivity of
sodium chloride
Forming Ionic Compounds Pre-Lab
Lab Purpose: To write formulas and names of 20 ionic compounds; to see ionic compounds formed in the lab
Lab Safety: Wear goggles and apron. Avoid contact with chemicals. Wash your hands after the lab. Do not mix up the pipettes.
Lab Procedure: Note the layout of the test tubes. Place 4-5 drops of each chemical into the well-plate.
Lab Report: Turn in your data table at the conclusion of the lab. We’ll pass them up when we return to our seats.
Post-Lab Clean-up: Place your well-plate on the table beneath the goggle cabinet. Wipe down your station.
Ionic Exit
Throughout this unit, there will be several quizzes on ionic and covalent compounds.
Correctly name or write the formula for as many of the following ionic compounds as you can to receive up to 5 extra credit points in this Unit
Indium Permanganate
ZnCl2
Palladium (III) Hydrogen Phosphate
MnI4
Lithium Chlorite
SrCr2O7
As you come in,
The Material:
– Paper and pencil for notes
– Remote control
– Paper, periodic table, and pencil for quiz
The Plan:
– Take the Ionic Compound Quiz
– Learn about COVALENT COMPOUNDS
The Assessment:
– Covalent & Acid Quiz – Thursday
– Combined Ionic, Covalent & Acid Quiz - Friday
Starter
Which of the following formulas is incorrect? Name the correct ionic compounds.
RaCl2 Ag(HSO3)2 Al(PO4)4
• When a CATION forms…which of the following actually happens?
- The # of protons changes- The atom gets lighter or weighs less- The atom loses electrons
Covalent Bonding
Why do atoms bond?
Remember that ionic compounds form by gaining and losing electrons.Covalent compounds form when 2 atoms both need electrons. They can both achieve the full octet by SHARING electrons.
What is a covalent bond?
Covalent bond: chemical bond that results from sharing electronsCovalent bonding generally occurs when elements are relatively close together on the periodic table.The majority of covalent bonds form between nonmetallic elements…often groups 4A to 7A.
Naming Covalent Compounds
First, you must be sure that the compound is COVALENT by analyzing the formula.
Second, you use prefixes to communicate the number of atoms of each element that form the compound.
Example: H2O = dihydrogen monoxide
Prefixes
One = mono
Two = di
Three = tri
Four = tetra
Five = penta
Six = hexa
Seven = hepta
Eight = octa
Nine = nona
Ten = decaNEVER USE MONO ON THE FIRST ELEMENT NAME.
ALWAYS USE THE -IDE ENDING ON THE SECOND ELEMENT NAME.
Name the following compound: P4S5
A.) phosphorus sulfide
B.) tetraphosphorus pentasulfur
C.) tetraphosphorus pentasulfide
D.) tetraphosphide pentasulfide
E.) phosphorus (IV) sulfide
Name the following compound: SeF6
A.) selenide fluoride
B.) selenium fluorine
C.) monoselenium hexafluoride
D.) selenium hexafluoride
E.) monoselenide hexafluoride
What is the chemical formula for dinitrogen trioxide?
A.) NO
B.) N2O
C.) N2O2
D.) N2O3
E.) N3O2
Starter:
Name the following Compounds:
1.CO
2.Sn(C2O4)2
3.NH3
Write formulas for the following Compounds:
3. Rubidium Nitride
4. Carbon Tetrahydride
5. Lead (II) Silicate
Naming Acids
Acids are compounds that contain hydrogen ion bonded to an anion, except water.
Two types of acids:– Binary Acids - “Hydro + root + ic acid”
• Examples: HCl, HBr, H2S,
– Oxyacids - “root + ic acid” OR “root + ous acid”
• Examples: H2SO4, HNO3, HC2H3O2
• ic = ate anion; ous = ite anion
Give the correct formula for sulfurous acid.
A.) HS
B.) H2S
C.) H2SO3
D.) H2SO4
E.) HS2
Give the formula for hydrophosphoric acid.
A.) HP
B.) H3P
C.) H3PO3
D.) H3PO4
E.) HP3
Name the following compound: H3N
A.) hydrogen nitride
B.) hydrogen (III) nitride
C.) hydronitric acid
D.) nitric acid
E.) nitrous acid
Name the following compound: HClO3
A.) hydrogen chloroxide
B.) hydrogen chlorite
C.) hydrogen chlorate
D.) chloric acid
E.) chlorous acid
Write the formula for vanadium (III) selenide.
A.) V3Se
B.) V3Se2
C.) V3Se3
D.) V2Se3
Name the following ionic compound: ZnSO3
A.) zinc sulfate
B.) zinc (II) sulfate
C.) zinc sulfide
D.) zinc sulfite
E.) zinc (II) sulfite
Mixed Compound Exit
Throughout this unit, there will be several quizzes on ionic and covalent compounds.
Correctly name or write the formula for as many of the following compounds as you can to receive up to 5 extra credit points in this Unit
Barium Iodide
Dicarbon hexahydride
SCl4
Be3As2
Iodine pentafluoride
VBr5
Starter
What is a formula unit?
SrSCN is an incorrect formula. If a student mixes Ca3(SCN)2 with SrCl2, what would be the correct formula unit for SrSCN?
Name the following compounds:
1.SiO2
2.H2Te
3.H2CrO4
4.SnSe2
Lewis Structures
Lewis structures: electron-dot diagrams show how electrons are arranged in molecules (AKA covalent compounds)– Draw electron dot diagrams for atoms showing
ONLY valence electrons.– Dashes represent “bonding pairs” and dots
represent “lone pairs”.
Lewis Structures
Steps:– Find the total # of valence electrons in the molecule.– Divide this number by 2. This is the number of bonding pairs.– Arrange the elements to show a clear central atom and
surrounding atoms. The central atom is usually farther to the left on the periodic table.
– Place one of the bonding pairs between the central atom and each terminal atom.
– Place the remaining pairs around the terminal atoms…if they need more electrons. Put the rest around the central atom.
– Check to be sure that multiple bonds don’t exist.
Lewis Structures
Tips:– Hydrogen is always terminal, on an end of
the molecule.
Example #1: CH4– Name the compound
• Carbon tetrahydride– Total valence electrons
• 4 + 1 + 1 + 1 + 1 = 8– Bonding pairs
• 8/2 = 4 bonding pairs– Arrange the atoms
• Remember the H is always terminal.– Place bonding pairs between the C & each H– How many pairs remain?
• O remaining pairs– Check for multiple bonds. (Does each atom have 8 valence
electrons?)• Yes, so there are no multiple bonds needed.
Example #2: NH3– Name the compound
• Nitrogen trihydride (AKA ammonia)– Total valence electrons
• 5 + 1 + 1 + 1 = 8– Bonding pairs
• 8/2 = 4 bonding pairs– Arrange the atoms
• Remember the H is always terminal.– Place bonding pairs between the N & each H– How many pairs remain?
• 4 pairs - 3 pairs used = 1 remaining pair• Add the remaining pair to the terminal first...then the central.
– Check for multiple bonds. (Does each atom have 8 valence electrons?)
• Yes, so there are no multiple bonds needed.
When the central atom has a lone pair
of electrons, the molecule bends.
Lone pairs of electrons take up
lots of space.
Example #3: O2– Name the compound
• Oxygen gas– Total valence electrons
• 6 + 6 = 12– Bonding pairs
• 12/2 = 6 bonding pairs– Arrange the atoms
• Two atoms are arranged next to each other.– Place bonding pairs between the two O atoms– How many pairs remain?
• 6 pairs - 1 pair used = 5 remaining pairs• Add the remaining pair to the terminal first...then the central.
– Check for multiple bonds. (Does each atom have 8 valence electrons?)
• No, so there ARE multiple bonds needed.
Example #4: CO2– Name the compound
• Carbon dioxide– Total valence electrons
• 4 + 6 + 6 = 16– Bonding pairs
• 16/2 = 8 bonding pairs– Arrange the atoms
• C should be central with an O on each side. (symmetrical)– Place bonding pairs between the C and each O atom– How many pairs remain?
• 8 pairs - 2 pairs used = 6 remaining pairs• Add the remaining pairs to the terminal first...then the central.
– Check for multiple bonds. (Does each atom have 8 valence electrons?)
• No, so there ARE multiple bonds needed.
Example #5: CO– Name the compound
• Carbon monoxide– Total valence electrons
• 4 + 6 = 10– Bonding pairs
• 10/2 = 5 bonding pairs– Arrange the atoms
• Two atoms are arranged side by side.– Place a bonding pair between the C and O atom– How many pairs remain?
• 5 pairs - 1 pair used = 4 remaining pairs• Add the remaining pairs to the terminal first...then the central.
– Check for multiple bonds. (Does each atom have 8 valence electrons?)
• No, so there ARE multiple bonds needed.
Resonance Structures
The Lewis Dot Structures for some covalent compounds can be written different ways
The different structures (versions) are called RESONANCE STRUCTURES
Resonance Structures
When writing Lewis Dot Structures, always consider if your structure is the ONLY possibility
Examples: NO3-, CO3
-2
Resonance Structures
Electronegativity
The difference in electronegativity of the atoms participating in a bond is IMPORTANT to notice.– Metals have a ______ electronegativity.– Nonmetals have a ___ electronegativity.– Atoms in an ionic compound have a ____
difference in electronegativity.– Atoms in a covalent compound have ___
difference in electronegativity.
Electronegativity Difference
What is electronegativity?
What is the trend?
There are two kinds of covalent bonds:
1. Polar covalent (one is greedy) – electrons are NOT shared equally
2. Nonpolar covalent (they play fair) - electrons are shared evenly
Polarity
Draw the Lewis Structure.Look at the central atom.– Does it have a surrounding atom that differs from
the others?– Does it have a lone pair of electrons?
If yes to either, then the molecule is polar.Polar molecules WILL dissolve in water; have one end that is slightly more negative.
Nomenclature/Lewis Stations
You must correctly answer questions at the 6 stations.
Label each station on your own sheet of paper and use your notes as a reference.
This assignment is graded!
Be sure to ask if you have any questions.
Extra Example: Br2– Name the compound
• Bromine– Total valence electrons
• 7 + 7 = 14– Bonding pairs
• 14/2 = 7 bonding pairs– Arrange the atoms
• Two atoms are arranged next to each other.– Place bonding pairs between the two Br atoms– How many pairs remain?
• 7 pairs - 1 pairs used = 6 remaining pairs• Add the remaining pair to the terminal first...then the central.
– Check for multiple bonds. (Does each atom have 8 valence electrons?)
• Yes, so there are no multiple bonds needed.
Advanced Lewis Structures
Draw the Lewis structure for CH3Cl.
– Check the polarity of the overall molecule.– Will this molecule mix with water?
Starter
What does a Lewis Dot Structure show you?
How many electrons are shared in a triple bond?
All resonance structures of a compound should have the same number of ________ __________.
Draw the Lewis Dot Structures for the following:
1. CH3F 2. SiO2
Advanced Lewis Structures
Draw the Lewis structure for PO3-.
– Check the polarity of the overall molecule.– Will this molecule mix with water?
Advanced Lewis Structures
Draw the Lewis structure for CH3OH.
– Check the polarity of the overall molecule.– Will this molecule mix with water?
Starter
Draw the Lewis Structures for the following compounds. Determine which of the following will dissolve in water and why: (Check for resonance structures!)
A. SiH2(OH)2 B. CH3I C. O3
Intermolecular Forces
Abbreviated - IMF
Forces of attraction and repulsion that exist BETWEEN molecules
Three types of IMF:– London dispersion forces– Dipole-dipole forces– Hydrogen bonding
Strength Increasing
Three Types of IMF
London dispersion forces (LDF) - weakest of all intermolecular forces; temporarily exists between any two molecules; ONLY one that occurs in nonpolar molecules (low melting & boiling points)Dipole-dipole forces - forces of attraction/repulsion that exist between POLAR molecules as a result of the partial charges (high melting & boiling points)Hydrogen bonding - STRONGEST intermolecular force that occurs when H is bonded to FON creating REALLY strong partial charges (highest melting & boiling points)
Electric Lab: Discussion Questions
1. How are the compounds similar that caused the bulb to light?
2. True or False: The reason a compound did not light the bulb is because the substance did not dissolve in water.
3. Why did these compounds in particular light the bulb?
Starter:
Name or Write the formula for the following compounds:
1.SiAt4 2. Magnesium sulfide 3. H3N
2.Draw the Lewis Dot Structure for: (Will it dissolve in water?)
1. SCN- 2. AsH3
VSEPR Theory - Shape Matters
Three-dimensional representation of moleculesValence Shell Electron Pair Repulsion TheoryCounting areas of electron density around the central atom.Electron density repels!This bends the molecule into interesting shapes.
Arranging Areas of High E- Density
# regions of high electron
densitymolecular shape
bond angle
2 linear 180°
3 trigonal planar 120°
4 bent2
Types
4 tetrahedral109.5
°
4 trigonal pyramidal107.5
°
Making Molecular Models Activity
1. H2O
2. O2
3. HCl
4. CO2
5. NH3
6. CH4
7. NO3-
8. CH3CH3
Draw a data table of 7 columns.
Column 1 - Formula
Column 2 - Name
Column 3 - Lewis structure
Column 4 - Shape
Column 5 - Bond angle
Column 6 - Polarity
Column 7 - Type of Intermolecular Force
Starter
For the following compounds determine the if it will dissolve in water, intermolecular force, shape and bond angle:
1.PO3- 2. SiSe2
3. NF3 4. CI4
What’s going on today…
Complete the Making Models Activity to be turned in today
Work on the Unit 4 Bonding WebQuest Review
If you should finish the WebQuest… work on practice problems in the review packet and self assess
StarterWhich compound requires more Lithium ions in its formula unit? (LiF or Li3P)
Compare water, oxygen gas, and CH3I. Determine which:
- Has the most electron density sites
- Will NOT dissolve in water
- Hardest to boil
List in order of increasing IMF strength
What’s going on today…
Rotate through the Unit 4 Bonding and Nomenclature Review Stations
Answer Keys are on the blog and on the center desk
Work on the Unit 4 Bonding WebQuest Review or the Review Packet Practice Problems
Be sure to ask questions!
Review for Cumulative Quiz
Describe the 4 periodic table trends
Which trend has no value (=0) for an entire group? Why?
Which 2 trends determine how an atom will bond (form cations and anions)?
How do the trends change has you move down a group or across a period?
StarterA new compound has been found with an unknown polyatomic (ZeQRX). When mixed with solutions the ions form ZeS and Ra5(QRX)2. What is the correct formula unit for the ionic compound?
Compare cyanide and carbon dioxide. Determine which:
- Shares the most electrons- Has the weaker IMF- Harder to boil- Melts the Fastest/Easiest
As you come in,
The Materials:– Remote control– Paper for stations and cumulative quiz– Webquest answers
The Plan:– Cumulative Quiz– Answer questions about webquest– Review stations– Check station answers
The Assessment:– Unit Four Test tomorrow!
As you come in,
Get the periodic table out of your resource notebook.
Pick up a scantron sheet from the front of the room.
Put paper on your desk for the short answer questions.
Be prepared to start ASAP!
NOTE: YOU MUST TURN YOUR TEST IN BEFORE 10:00 AM!
A STATE-MANDATED DRILL WILL TAKE PLACE AT EXACTLY 10:00 AM, AND WE’LL NOT HAVE TIME TO
FINISH OR TURN THINGS IN AFTER THE DRILL!
Get the periodic table out of your resource notebook.
Pick up a scantron sheet from the front of the room.
Put paper on your desk for the short answer questions.
Be prepared to start ASAP!
Tests MUST be turned in by 3:24 pm.