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Starter. Use your Polyatomic Sheet/Flash Cards to write the chemical formula of each polyatomic below: Phosphate Nitrite Hydrogen Carbonate Ammonium Perchlorate. Name the following polyatomic ion: SO 4 2-. iRespond Question. Multiple Choice. F. 897876E2-BC56-0344-B8E9-5E892C40C40F.

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Starter
Starter

  • Use your Polyatomic Sheet/Flash Cards to write the chemical formula of each polyatomic below:

  • Phosphate

  • Nitrite

  • Hydrogen Carbonate

  • Ammonium

  • Perchlorate


Name the following polyatomic ion: SO42-

iRespond Question

Multiple Choice

F

897876E2-BC56-0344-B8E9-5E892C40C40F

A.) sulfur tetraoxide

B.) sulfur oxite

C.) sulfite

D.) sulfate

E.) sulfete


Name the following polyatomic ion: ClO4-

iRespond Question

Multiple Choice

F

8EF4B52F-0321-824D-A11A-E3B932C44068

A.) hypochlorite

B.) chlorite

C.) chlorate

D.) perchlorate

E.) chloroxite


Write the formula for the following polyatomic ion: hydroxide

iRespond Question

Multiple Choice

F

0AD5553A-0A32-FC4C-9404-6B5B89DB5FCA

A.) HO

B.) HO-

C.) OH

D.) OH-

E.) H2O


Unit four bonding nomenclature

Unit Four: Bonding/Nomenclature hydroxide

GPS SC1: Students will analyze the nature of matter and its classifications.



Formation of ionic bonds
Formation of Ionic Bonds hydroxide

  • 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 hydroxide

  • 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
Writing Ionic Compound Names from the Formulas hydroxide

  • 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
Practice Writing Names from Chemical Formulas hydroxide

  • Write the name of the compound that is represented by the following formula:

    • MgCl2

       Magnesium Chloride


Name the following compound: CrPO hydroxide4

iRespond Question

Multiple Choice

F

BEBFB6B0-F26B-DC41-B427-42ADB2146B20

A.) chromium phosphate

B.) chromium (I) phosphate

C.) chromium (II) phosphate

D.) chromium (III) phosphate

E.) chromium (IV) phosphate


What is the name of MnO hydroxide4-?

iRespond Question

Multiple Choice

F

A47EC230-904D-CB4A-8729-D32196BA428A

A.) permanganate

B.) manganate

C.) manganite

D.) hypomanganite

E.)


Name the following compound: hydroxidePbS

iRespond Question

Multiple Choice

F

3FB364E5-C5F2-DA40-A9D8-FF54A1F547CC

A.) lead sulfur

B.) lead sulfide

C.) lead (I) sulfide

D.) lead (II) sulfide

E.) lead sulfate


Name the following compound: Al hydroxide2(SO4)3

iRespond Question

Multiple Choice

F

B940D1EE-6C72-7F4C-B327-4A0B1EBB9898

A.) aluminum (III) sulfate

B.) aluminum sulfate

C.) aluminum (II) sulfate

D.) aluminum sulfite

E.) aluminum sulfide


Name the following compound: Cu hydroxide2CO3

iRespond Question

Multiple Choice

F

1929127E-8E2A-8541-9E33-9E481F84296A

A.) copper carbonate

B.) copper (I) carbonate

C.) copper (II) carbonate

D.) copper (II) carbonate (III)

E.) copper carbontrioxide


Name the following compound: NiSO hydroxide4

iRespond Question

Multiple Choice

F

67C781D7-A40E-FD47-A890-319C139AB3FF

A.) nickel sulfate

B.) nickel (I) sulfate

C.) nickel (II) sulfate

D.) nickel (III) sulfate

E.) nickel (IV) sulfate


Name the following compound: KBr hydroxide

iRespond Question

Multiple Choice

F

7B74BE42-F826-854D-A49D-C1DDE7B776B9

A.) potassium bromide

B.) potassium (I) bromide

C.) potassium bromite

D.) potassium bromate


Name the following compound: TiO hydroxide2

iRespond Question

Multiple Choice

F

BF4E0959-7A7D-EF47-8421-4292A0A717D1

A.) titanium oxide

B.) titanium (II) oxide

C.) titanium (IV) oxide

D.) titanium oxide (II)


Starter1
Starter: hydroxide

  • How can you determine if a compound is Ionic?

  • Examine the formula to name the following Ionic Compounds:

  • MgO 3. KOH

  • V(ClO)2 4. CuSO4


Criss cross method for writing chemical formulas
Criss-Cross Method for Writing Chemical Formulas hydroxide

  • Let’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
Valence Electrons & Stability Review hydroxide

  • 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? hydroxide

iRespond Question

Multiple Choice

F

FAAB3991-5386-AC4B-BB47-A52F5D8AAEA0

A.) NaCl

B.) NaClO

C.) NaClO2

D.) NaClO3

E.) Na(ClO)


What is the chemical formula for titanium (IV) oxide? hydroxide

iRespond Question

Multiple Choice

F

82F2CB0B-1B3B-DF49-B135-7B93A3EF7994

A.) Ti4O

B.) Ti4O2

C.) Ti2O

D.) Ti2O4

E.) TiO2


What is the chemical formula for magnesium oxide? hydroxide

iRespond Question

Multiple Choice

F

E1CC6316-9ACB-F044-BFC3-1EDE379323F4

A.) MnO

B.) MnO2

C.) MgO

D.) Mg2O2

E.) MgO2


What is the chemical formula for nickel(II) nitrate? hydroxide

iRespond Question

Multiple Choice

F

6A4727B6-E917-C645-BCF1-0671B166C95D

A.) Ni2NO3

B.) Ni1NO32

C.) NiNO3

D.) (Ni)(NO3)2

E.) Ni(NO3)2


What is the formula for hydrogen carbonate? hydroxide

iRespond Question

Multiple Choice

F

12DFBEDD-67D1-0E45-8BAB-1A5736E8FBFE

A.) H2CO3

B.) HCO3-

C.) HCO32-

D.) HCO3

E.)


What is the chemical formula for magnesium phosphate? hydroxide

iRespond Question

Multiple Choice

F

5165E0D9-45FB-EF40-9EB8-77B068200690

A.) MgP

B.) Mg3P2

C.) MgPO4

D.) Mg2(PO4)3

E.) Mg3(PO4)2


After the quick review
After the quick review, hydroxide

  • 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


Starter2
Starter: hydroxide

  • Name the following Ionic Compounds:

  • BaS

  • 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. hydroxide

iRespond Question

Multiple Choice

F

22E75BC6-684F-4C4C-810A-AD6391DDD620

A.) ZnSe

B.) Zn2Se

C.) ZnSe2

D.) Zn2Se2

E.)


Write the chemical formula for calcium nitrate. hydroxide

iRespond Question

Multiple Choice

F

34AFBE46-B89D-1540-AD53-D98E2973D59C

A.) CaNO3

B.) CaNO2

C.) Ca(NO3)2

D.) Ca(NO2)2

E.) Ca3N2


Write the chemical formula for cobalt(III) phosphide. hydroxide

iRespond Question

Multiple Choice

F

08C9ACB3-CE5D-C24A-9A8A-949F076DC8CB

A.) Co3P

B.) Co3P3

C.) CoP

D.) CoPO3

E.) CoPO4


Formula unit ratios form beautiful crystals…Ionic compounds are crystals!

In Nature


What You’ll See in Our Lab compounds are crystals!

Ionic compound solids that form when two solutions are mixed

precipitate

Separation line

“Snow Globe” effect

Paint effect


Physical Properties of Ionic Compounds compounds are crystals!

WHY?

Applying heat to melt sodium chloride

Applying a current to test conductivity of sodium chloride


Forming ionic compounds pre lab
Forming Ionic Compounds Pre-Lab compounds are crystals!

  • 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
Ionic Exit compounds are crystals!

  • 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



  • ZnCl compounds are crystals!2



  • MnI compounds are crystals!4



  • SrCr compounds are crystals!2O7


As you come in
As you come in, compounds are crystals!

  • 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


Starter3
Starter compounds are crystals!

  • 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

Covalent Bonding compounds are crystals!


Why do atoms bond
Why do atoms bond? compounds are crystals!

  • 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
What is a covalent bond? compounds are crystals!

  • Covalent bond: chemical bond that results from sharing electrons

  • Covalent 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
Naming Covalent Compounds compounds are crystals!

  • 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
Prefixes compounds are crystals!

  • Six = hexa

  • Seven = hepta

  • Eight = octa

  • Nine = nona

  • Ten = deca

  • One = mono

  • Two = di

  • Three = tri

  • Four = tetra

  • Five = penta

NEVER USE MONO ON THE FIRST ELEMENT NAME. ALWAYS USE THE -IDE ENDING ON THE SECOND ELEMENT NAME.


Name the following compound: P compounds are crystals!4S5

iRespond Question

Multiple Choice

F

C908769F-99E7-5C40-8BB8-7E708DAE4525

A.) phosphorus sulfide

B.) tetraphosphorus pentasulfur

C.) tetraphosphorus pentasulfide

D.) tetraphosphide pentasulfide

E.) phosphorus (IV) sulfide


Name the following compound: SeF compounds are crystals!6

iRespond Question

Multiple Choice

F

3DA7319B-5C50-9C40-B50C-1C83BD029A3E

A.) selenide fluoride

B.) selenium fluorine

C.) monoselenium hexafluoride

D.) selenium hexafluoride

E.) monoselenide hexafluoride


What is the chemical formula for dinitrogen trioxide? compounds are crystals!

iRespond Question

Multiple Choice

F

FC671842-660B-AD4D-BA78-86341802C10B

A.) NO

B.) N2O

C.) N2O2

D.) N2O3

E.) N3O2


Starter4
Starter: compounds are crystals!

  • Name the following Compounds:

  • CO

  • Sn(C2O4)2

  • NH3

  • Write formulas for the following Compounds:

    3. Rubidium Nitride

    4. Carbon Tetrahydride

    5. Lead (II) Silicate


Naming acids
Naming Acids compounds are crystals!

  • 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. compounds are crystals!

iRespond Question

Multiple Choice

F

524237E3-3EAF-8A43-8B1B-62F25EBFB5EE

A.) HS

B.) H2S

C.) H2SO3

D.) H2SO4

E.) HS2


Give the formula for hydrophosphoric acid. compounds are crystals!

iRespond Question

Multiple Choice

F

157FCEB7-BD61-0C4F-96B4-4139A464ADFF

A.) HP

B.) H3P

C.) H3PO3

D.) H3PO4

E.) HP3


Name the following compound: H compounds are crystals!3N

iRespond Question

Multiple Choice

F

4B49FE19-7090-D54B-BB6E-CE073CCCC329

A.) hydrogen nitride

B.) hydrogen (III) nitride

C.) hydronitric acid

D.) nitric acid

E.) nitrous acid


Name the following compound: HClO compounds are crystals!3

iRespond Question

Multiple Choice

F

AB2AD2FC-E3E4-A849-8D85-4A7A2316E926

A.) hydrogen chloroxide

B.) hydrogen chlorite

C.) hydrogen chlorate

D.) chloric acid

E.) chlorous acid


Write the formula for vanadium (III) compounds are crystals!selenide.

iRespond Question

Multiple Choice

F

A.) V3Se

B.) V3Se2

C.) V3Se3

D.) V2Se3

E.)


Name the following ionic compound: ZnSO compounds are crystals!3

iRespond Question

Multiple Choice

F

A.) zinc sulfate

B.) zinc (II) sulfate

C.) zinc sulfide

D.) zinc sulfite

E.) zinc (II) sulfite


Mixed compound exit
Mixed Compound Exit compounds are crystals!

  • 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




  • SCl compounds are crystals!4


  • Be compounds are crystals!3As2



  • VBr compounds are crystals!5


Starter5
Starter compounds are crystals!

  • 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:

  • SiO2

  • H2Te

  • H2CrO4

  • SnSe2


Lewis structures
Lewis Structures compounds are crystals!

  • 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 structures1
Lewis Structures compounds are crystals!

  • 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 structures2
Lewis Structures compounds are crystals!

  • Tips:

    • Hydrogen is always terminal, on an end of the molecule.


Example 1 ch 4
Example #1: CH compounds are crystals!4

  • 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 nh 3
Example #2: NH compounds are crystals!3

  • 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 o 2
Example #3: O compounds are crystals!2

  • 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 co 2
Example #4: CO compounds are crystals!2

  • 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
Example #5: CO compounds are crystals!

  • 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
Resonance Structures compounds are crystals!

  • The Lewis Dot Structures for some covalent compounds can be written different ways

  • The different structures (versions) are called RESONANCE STRUCTURES


Resonance structures1
Resonance Structures compounds are crystals!

  • When writing Lewis Dot Structures, always consider if your structure is the ONLY possibility

  • Examples: NO3-, CO3-2


Resonance structures2
Resonance Structures compounds are crystals!


Electronegativity
Electronegativity compounds are crystals!

  • 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
Electronegativity Difference compounds are crystals!

  • 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
Polarity compounds are crystals!

  • 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
Nomenclature/Lewis Stations compounds are crystals!

  • 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 br 2
Extra Example: Br compounds are crystals!2

  • 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
Advanced Lewis Structures compounds are crystals!

  • Draw the Lewis structure for CH3Cl.

    • Check the polarity of the overall molecule.

    • Will this molecule mix with water?


Starter6
Starter compounds are crystals!

  • 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 structures1
Advanced Lewis Structures compounds are crystals!

  • Draw the Lewis structure for PO3-.

    • Check the polarity of the overall molecule.

    • Will this molecule mix with water?


Advanced lewis structures2
Advanced Lewis Structures compounds are crystals!

  • Draw the Lewis structure for CH3OH.

    • Check the polarity of the overall molecule.

    • Will this molecule mix with water?


Starter7
Starter compounds are crystals!

  • 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


Inter molecular forces
Inter compounds are crystals!molecular 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
Three Types of IMF compounds are crystals!

  • 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
Electric Lab: Discussion Questions compounds are crystals!

  • How are the compounds similar that caused the bulb to light?

  • True or False: The reason a compound did not light the bulb is because the substance did not dissolve in water.

  • Why did these compounds in particular light the bulb?


Starter8
Starter: compounds are crystals!

  • Name or Write the formula for the following compounds:

  • SiAt4 2. Magnesium sulfide 3. H3N

  • Draw the Lewis Dot Structure for: (Will it dissolve in water?)

    1. SCN- 2. AsH3


Vsepr theory shape matters
VSEPR Theory - compounds are crystals!Shape Matters

  • Three-dimensional representation of molecules

  • Valence Shell Electron Pair Repulsion Theory

  • Counting areas of electron density around the central atom.

  • Electron density repels!

  • This bends the molecule into interesting shapes.


Arranging areas of high e density
Arranging Areas of High E compounds are crystals!- Density


Making molecular models activity
Making Molecular Models Activity compounds are crystals!

  • H2O

  • O2

  • HCl

  • CO2

  • NH3

  • CH4

  • NO3-

  • 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


Starter9
Starter compounds are crystals!

  • For the following compounds determine the if it will dissolve in water, intermolecular force, shape and bond angle:

  • PO3- 2. SiSe2

    3. NF3 4. CI4


What s going on today
What’s going on today… compounds are crystals!

  • 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


Starter10
Starter compounds are crystals!

  • Which 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 today1
What’s going on today… compounds are crystals!

  • 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
Review for Cumulative Quiz compounds are crystals!

  • 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?


Starter11
Starter compounds are crystals!

  • A 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 in1
As you come in, compounds are crystals!

  • 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 in2
As you come in, compounds are crystals!

  • 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!


Tests MUST be turned in by 3:24 pm. compounds are crystals!

  • 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!


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