starter use your polyatomic sheet/flash cards to write the chemical formula of each polyatomic...

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.