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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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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
slide2
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

slide3
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

slide4
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.

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

slide11
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

slide12
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.)

slide13
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

slide14
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

slide15
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

slide16
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

slide17
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

slide18
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?
slide22
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)

slide23
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

slide24
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

slide25
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

slide26
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.)

slide27
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

slide30
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.)

slide31
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

slide32
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

slide34
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

slide35
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
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
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.

slide51
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

slide52
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

slide53
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
slide56
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

slide57
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

slide58
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

slide59
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

slide60
Write the formula for vanadium (III) selenide.

iRespond Question

Multiple Choice

F

A.) V3Se

B.) V3Se2

C.) V3Se3

D.) V2Se3

E.)

slide61
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
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
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.
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!

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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!
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