Chemistry Day 30 Tuesday, December 3rd – Wednesday,

December 4th, 2019

Do-Now: “Nomenclature Do-Now”

1.  Write down today’s FLT 2.  On a scale of 1-5, 5 being best, how do you

think you did on the test? 3.  Identify three things you could do to

effectively prepare for the next test. 4.  What is the name of:

a.  CaCl2 b.  H2O

5.  Why do you think it’s important for scientists to have a system for naming molecules and compounds?

Take out your planner and ToC

FLT •  I will be able to write the names and

formulas of molecules and compounds by completing Nomenclature Notes

Standard HS-PS1-1:Usetheperiodictableasamodeltopredicttherelativepropertiesofelementsbasedonthepatternsofelectronsintheoutermostenergylevelofatoms.

Nomenclature

Naming Rule #1 •  Identify if it is:

1.  Ionic (NaCl) 2.  Covalent (CO2) 3.  Acidic (HCl)

Naming Ionic Compounds (Salts)

Examples of Salts • NaCl • KBr

• CaF2 • NaNO3

• Al2(CO3)3

Formulas • Atoms gain or lose electrons to form

ions – Metals lose e-s to form cations – Cations have the same name as their

metal – Ex/ Ca2+ = Calcium

Formulas • Atoms gain or lose electrons to form

ions – Nonmetals gain e-s to form anions – Anions end in -ide – Ex/ F- = Fluoride

Name the following: 1.  Na+ 2.  Br-

3.  Be2+

4.  Al3+

5.  S2-

6.  O2-

Naming •  Ionic Compounds are usually named

as cation + anion – Ex/CaCl2 = calcium chloride

What would you name these? 1.  NaF 2.  KI

3.  Rb2S 4.  MgO 5.  Al2O3

Metals with Multiple Charges

Naming • Some metals (esp. transition metals)

have multiple possible charges. •  If metals have multiple possible

charges, use roman numerals to indicate charge of cation – Ex/ Fe2+ is Iron (II) and Fe3+ is Iron

(III)

Predicting Ionic Charges Group B elements: Many transition elements

have more than one possible oxidation state. Iron (II) = Fe2+

Iron (III) = Fe3+ Note the use of Roman numerals to show charges

Predicting Ionic Charges Some of the post-transition elements also have more than one possible oxidation state. Tin (II) = Sn2+ Lead (II) = Pb2+

Tin(IV)=Sn4+ Lead(IV)=Pb4+

Predicting Ionic Charges Group B elements: Some transition elements have only one possible oxidation state, such as these three:

Zinc = Zn2+ Silver = Ag1+ Cadmium=Cd2+

Exceptions: • Some of the transition metals

have only one ionic charge, and do not need roman numerals: – Silver is always Ag1+ – Cadmium is always Cd2+ – Zinc is always Zn2+

Example • What is the name of HgO?

Transition Metals •  If you have a transition metal

other than Ag, Cd, or Zn USE ROMAN NUMERALS

•  Include metals such as Sn and Pb in this category since they have multiple possible charges

What would the names be?

1.  KCl 2.  MgS 3.  CuS 4.  SnCl2 5.  FeF3

Polyatomic Ions

Polyatomic Ions •  Polyatomic Ions = a charged group of

atoms that stay together •  Usually end in –ate or –ite •  Acetate: C2H3O2

1- •  Nitrate: NO3

1- •  Nitrite: NO2

1- •  Permanganate: MnO4

1- •  Hydroxide: OH1- •  Cyanide: CN1-

Naming • Use the table for naming • Ex/ NaNO3 = sodium nitrate

What would the names be?

1.  KOH 2.  CaCO3 3.  MgSO4

Note: • When writing formulas, you must

balance the charge of the polyatomic ion as a whole

• Use parentheses

Note: • When writing formulas, you must

balance the charge of the polyatomic ion as a whole

• Ex/ calcium nitrate

Try One: • What would the formula be for

sodium sulfate?

• What about calcium hydroxide?

Covalent Bonding

Covalent Bonding • Use prefixes to indicate the number

of each atom

Prefixes •  To write the name: prefix + 1st element +

prefix + 2nd element–ide •  Note: do not use the prefix mono for the first

element – Ex/ – N2O = dinitrogen monoxide – NO2 = nitrogen dioxide

Practice by naming these: 1.  Cl2O3 2.  CBr4 3.  CO2 4.  BaCl2

Write formulas for these: 1.  diphosphorus pentoxide 2.  tetraiodine monoxide 3.  sulfur hexafluoride 4.  nitrogen trioxide 5.  phosphorus trifluoride 6.  aluminum chloride

Acids For now, understand that acids usually begin with “H” 1.  Binary acids are named:

•  Hydro-______-ic acid 2.  Oxyacids (polyatomic ions) are

named: •  ______ ic acid (-ate polyatomic ions) •  ______ous acid (-ite polyatomic ions)

Acids Binary acids are named:

•  Hydro-______-ic acid ü  Ex/ HBr = hydrobromic acid ü  HCl? ü  H2S?

Acids Oxyacids (polyatomic ions) are named:

•  ______ ic acid (-ate polyatomic ions) •  ______ous acid (-ite polyatomic ions)

ü  Ex/ HNO3 = nitric acid ü  Ex/ HNO2 = nitrous acid ü H2SO4?

CW1.   NamingWS

–  PeriodateisIO4-

–  BromiteisBrO2-

–  WewilltakeaKAHOOTtopracticeshortly

2.   Finished?WorkonToCorstudyquietly

Chemistry Day 31 Thursday, December 5th – Friday,

December 6th, 2019

Do-Now: “BrainPOP: Chemical Equations” 1.  Write down today’s FLT 2.  What do you think a chemical reaction is?

(Write what you think, even if you’re not sure) 3.  Write down an example of a chemical reaction

(it could be anything you think is an example) 4.  Sketch what you think a chemical reaction might

look like. 5.  Write down the formula for lead(II) nitride. Show

work. 6.  Write down the formula for hydrochloric acid. 7.  Number 1-10 underneath your do-now.

Take out your planner and ToC

BrainPOP:ChemicalEquations• WatchtheBrainPOPvideo• Afterthevideo,answerthequestionsinyourgroup–everymembermustcopydownthesameanswer

• Thegroupwiththemostcorrectanswersà+5dojopointseachhttps://www.brainpop.com/science/matterandchemistry/chemicalequations/

FLT •  I will be able to translate a word

equation into a chemical equation by completing Ch. 7 Notes A

Standard HS-PS1-7:Usemathematicalrepresentationstosupporttheclaimthatatoms,andthereforemass,areconservedduringachemicalreaction

Ch. 7: Chemical Reactions

Part A: Describing Chemical Reactions

Recall

Recall • We have nomenclature rules in

chemistry that allow us to write chemical formulas

MgCl2

FeCl2 NaNO3 CCl4

Recall • You must know your naming and

formula-writing rules to write equations correctly – Ionic

• Standard • Transition and post-transition metals • Polyatomic ions

– Covalent

Chemical Reactions

Chemical Equations • Chemical Equation = Shorthand

for a chemical rxn

Chemical Equations

•  There are two parts to a reaction: 1.  Reactants = substances you start

with 2.  Products = substances you end

up with

All Chemical Reactions… •  The reactants will turn into the

products Reactants à Products

- Page 321

Reactants Products

Which are the reactants, which are the products?

•  H2 + O2 à H2O

• Na + Cl2 à NaCl

• Ca3N2 + NaCl à CaCl2 + Na3N

Describing Chemical Rxns Word equations = words only Ex/ Copper reacts with chlorine to form copper (II) chloride

Describing Chemical Rxns Symbols may be used in equations Copper + chlorine à copper (II) chloride

Describing Chemical Rxns Chemical Equations = uses formulas and symbols

Ex/ Cu + Cl2 à CuCl2

Chemical Rxn Symbols

Symbols • à = “yields” or “reacts to form”

Reactants à Products

Symbols •  + = “and”

Cu + Cl2 à CuCl2

Symbols •  Statesofmatter=indicatedwithsubscripts(s),(l),(g),or(aq)

2H2(g)+O2(g)à2H2O(l)

Symbols •  aq = aqueous = dissolved in water

NaCl(aq) à Na+ + Cl-

Symbols • Double arrow = reversible rxn

(more later)

Symbols • Others: Heat (Δ), energy, and

catalysts can be indicated on arrows

Symbols • A catalyst is a substance that is

added to speed up a reaction, but is not used or consumed by the reaction

Writing Equations

Writing Equations • Ex 1/ Diatomic bromine and

potassium iodide react to form potassium bromide and diatomic iodine

***NOTE*** • Diatomic gases =

H, N, O, F, Cl, Br, I • Always write as

diatomic if they are by themselves in a chemical equation

Writing Equations • Ex 2/ Iron and oxygen react to form

iron (III) oxide

Try this one: • Ex 3/ Iron (III) sulfide and

hydrochloric acid react to form iron (III) chloride and gaseous hydrosulfuric acid

Now, read these equations:

Fe(s) + O2(g) → Fe2O3(s)

Cu(s) + AgNO3(aq) → Ag(s) + Cu(NO3)2(aq)

NO2(g) N2(g) + O2(g) →