Starter
This presentation is the property of its rightful owner.
Sponsored Links
1 / 106

Starter PowerPoint PPT Presentation


  • 70 Views
  • Uploaded on
  • Presentation posted in: General

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.

Download Presentation

Starter

An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -

Presentation Transcript


Starter

Starter

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

  • Phosphate

  • Nitrite

  • Hydrogen Carbonate

  • Ammonium

  • Perchlorate


Starter

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


Starter

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


Starter

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

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


Classification of matter

Classification of Matter


Formation of ionic bonds

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

  • 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

  • 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

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

    • MgCl2

       Magnesium Chloride


Starter

Name the following compound: CrPO4

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


Starter

What is the name of MnO4-?

iRespond Question

Multiple Choice

F

A47EC230-904D-CB4A-8729-D32196BA428A

A.) permanganate

B.) manganate

C.) manganite

D.) hypomanganite

E.)


Starter

Name the following compound: PbS

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


Starter

Name the following compound: Al2(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


Starter

Name the following compound: Cu2CO3

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


Starter

Name the following compound: NiSO4

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


Starter

Name the following compound: KBr

iRespond Question

Multiple Choice

F

7B74BE42-F826-854D-A49D-C1DDE7B776B9

A.) potassium bromide

B.) potassium (I) bromide

C.) potassium bromite

D.) potassium bromate


Starter

Name the following compound: TiO2

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:

  • 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

  • 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

  • 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?


Starter

What is the chemical formula for sodium hypochlorite?

iRespond Question

Multiple Choice

F

FAAB3991-5386-AC4B-BB47-A52F5D8AAEA0

A.) NaCl

B.) NaClO

C.) NaClO2

D.) NaClO3

E.) Na(ClO)


Starter

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

iRespond Question

Multiple Choice

F

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

A.) Ti4O

B.) Ti4O2

C.) Ti2O

D.) Ti2O4

E.) TiO2


Starter

What is the chemical formula for magnesium oxide?

iRespond Question

Multiple Choice

F

E1CC6316-9ACB-F044-BFC3-1EDE379323F4

A.) MnO

B.) MnO2

C.) MgO

D.) Mg2O2

E.) MgO2


Starter

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

iRespond Question

Multiple Choice

F

6A4727B6-E917-C645-BCF1-0671B166C95D

A.) Ni2NO3

B.) Ni1NO32

C.) NiNO3

D.) (Ni)(NO3)2

E.) Ni(NO3)2


Starter

What is the formula for hydrogen carbonate?

iRespond Question

Multiple Choice

F

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

A.) H2CO3

B.) HCO3-

C.) HCO32-

D.) HCO3

E.)


Starter

What is the chemical formula for magnesium phosphate?

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,

  • 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:

  • 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


Starter

Write the chemical formula for zinc selenide.

iRespond Question

Multiple Choice

F

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

A.) ZnSe

B.) Zn2Se

C.) ZnSe2

D.) Zn2Se2

E.)


Starter

Write the chemical formula for calcium nitrate.

iRespond Question

Multiple Choice

F

34AFBE46-B89D-1540-AD53-D98E2973D59C

A.) CaNO3

B.) CaNO2

C.) Ca(NO3)2

D.) Ca(NO2)2

E.) Ca3N2


Starter

Write the chemical formula for cobalt(III) phosphide.

iRespond Question

Multiple Choice

F

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

A.) Co3P

B.) Co3P3

C.) CoP

D.) CoPO3

E.) CoPO4


Starter

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

In Nature


Starter

What You’ll See in Our Lab

Ionic compound solids that form when two solutions are mixed

precipitate

Separation line

“Snow Globe” effect

Paint effect


Starter

Physical Properties of Ionic Compounds

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

  • 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

  • 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


Starter

  • Indium Permanganate


Starter

  • ZnCl2


Starter

  • Palladium (III) Hydrogen Phosphate


Starter

  • MnI4


Starter

  • Lithium Chlorite


Starter

  • SrCr2O7


As you come in

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


Starter3

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

Covalent Bonding


Why do atoms bond

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

What is a covalent bond?

  • 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

  • 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

  • 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.


Starter

Name the following compound: P4S5

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


Starter

Name the following compound: SeF6

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


Starter

What is the chemical formula for dinitrogen trioxide?

iRespond Question

Multiple Choice

F

FC671842-660B-AD4D-BA78-86341802C10B

A.) NO

B.) N2O

C.) N2O2

D.) N2O3

E.) N3O2


Starter4

Starter:

  • 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

  • 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


Starter

Give the correct formula for sulfurous acid.

iRespond Question

Multiple Choice

F

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

A.) HS

B.) H2S

C.) H2SO3

D.) H2SO4

E.) HS2


Starter

Give the formula for hydrophosphoric acid.

iRespond Question

Multiple Choice

F

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

A.) HP

B.) H3P

C.) H3PO3

D.) H3PO4

E.) HP3


Starter

Name the following compound: H3N

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


Starter

Name the following compound: HClO3

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


Starter

Write the formula for vanadium (III) selenide.

iRespond Question

Multiple Choice

F

A.) V3Se

B.) V3Se2

C.) V3Se3

D.) V2Se3

E.)


Starter

Name the following ionic compound: ZnSO3

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

  • 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


Starter

  • Barium Iodide


Starter

  • Dicarbon hexahydride


Starter

  • SCl4


Starter

  • Be3As2


Starter

  • Iodine pentafluoride


Starter

  • VBr5


Starter5

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:

  • SiO2

  • H2Te

  • H2CrO4

  • SnSe2


Lewis structures

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 structures1

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 structures2

Lewis Structures

  • Tips:

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


Example 1 ch 4

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 nh 3

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 o 2

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 co 2

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

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

Resonance Structures

  • 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

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

  • Examples: NO3-, CO3-2


Resonance structures2

Resonance Structures


Electronegativity

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

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

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

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 br 2

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

Advanced Lewis Structures

  • Draw the Lewis structure for CH3Cl.

    • Check the polarity of the overall molecule.

    • Will this molecule mix with water?


Starter6

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 structures1

Advanced Lewis Structures

  • 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

  • Draw the Lewis structure for CH3OH.

    • Check the polarity of the overall molecule.

    • Will this molecule mix with water?


Starter7

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


Inter molecular forces

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

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

Electric Lab: Discussion Questions

  • 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:

  • 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 - 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- Density


Making molecular models activity

Making Molecular Models Activity

  • 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

  • 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…

  • 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

  • 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…

  • 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

  • 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

  • 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,

  • 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,

  • 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!


Starter

Tests MUST be turned in by 3:24 pm.

  • 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!


  • Login