Question of the Day

Name for H3PO4 =

Formula for magnesium hydroxide =

Day 1 9-12

How do I name chemicals?

How do I determine a chemical’s formula?

Day 6 9-11

Practicing formulas:

Barium Sulfide

Ferric Chloride

Cobalt II oxide

Ionic Compounds & Polyatomic Ions

Oxyanions – polyatomic ions that contain oxygen

ate = ending for most common ion (ClO3- Chlorate)

ite = ending for one less oxygen (ClO2- Chlorite)

hypo = prefix for another less oxygen (ClO - Hypochlorite)

per = prefix for one more than most common (ClO4-

Perchlorate)

Binary Molecular CompoundsBased on Prefixes

1. Less electronegative first – prefix only if more than one atom

2. Second element – prefix, root of name, ending ide (if only two elements)

3.o or a @ the end of prefix is dropped if name begins with a vowel (monooxide, monoxide)

PAGE 281

Mono 1

Di 2

Tri 3

Tetra 4

Penta 5

Hexa 6

Hepta 7

Octa 8

Nona 9

Deca 10

Binary Molecular

Compounds – prefix system

Write the Formula:

Germanium tetraiodide

diphosphorous trioxide

Write the Name:N2O5

SbF3

GeI4

P2O3

Dinitrogen pentoxide

Antimony trifluoride

Binary Molecular Compounds

Binary Molecular CompoundsWrite the Formula:

carbon tetraiodide

dinitrogen trioxide

Write the Name:As2O5

ICl3

CI4

N2O3

diarsenic pentoxide

iodine trichloride

Molecular Element – molecule of atoms of same element – NOT a compound -like O2, Cl2, O3

allotrope – single element, different structure

Day 2 9-13

1. Name Cu2CO3

2. What are the formulas for sulfurous acid and Ferric nitrite?

1. How

do I use an equation to

represent a chemical reaction?

H2(g) + F2(g) 2HF(g)

Chemical equation

reactants products

Describing Chemical Reactions

Reactions are represented by chemical equations

H2(g) + F2(g) 2HF(g)

reactants products

Describing Chemical Reactions

State of matter: g = gas, l = liquid, s = solid, aq = aqueous solution

H2(g) + F2(g) 2HF(g)

reactants products

Describing Chemical Reactions

Coefficients – how many mols of each element react with each other – mol ratio

H2(g) + F2(g) 2HF(g)

Describing Chemical Reactions

1 mol of hydrogen gas reacts with 1 mol of fluorine gas to produce 2 mols of hydrogen fluoride gas

For now think of a mol as a piece:

1 piece of hydrogen gas reacts with 1 piece of fluorine gas to produce 2 pieces of hydrogen fluoride gas

Atoms are neither created nor

destroyed in ordinary chem. rxns.

Describing Chemical Reactions

Conservation of matter -

Chemical Reactions –

What’d We Just Do?

Bonds …

a process in which one or more substances are converted into new substances with different physical and chemical properties

Balancing Equations

Writing a chemical equation:Hydrogen gas reacts with chlorine to produce liquid hydrochloric acid.

Reactants =

Product =

H2(g) + Cl2(g) HCl(l)

Balancing Equations

Atoms are neither created nor destroyed in ordinary chem. rxns.

- Sum of atoms on each side must be equal

- Use coefficients to help

Balancing Equations

H2(g) + Cl2(g) HCl(l)

Solid magnesium reacts with fluorine gas to produce solid magnesium fluoride.

Equation:

Balancing Equations

Chemicals equations are not always balanced, sometimes we will have to balance them …

1. Balance different types of atoms one at a time

2. Start with atoms that appear only once on each side

1. Balance different types of atoms one at a time

2. Start with atoms that appear only once on each side

3. Balance polyatomic ions that appear on both sides of the equation as a single unit

4. Balance H and O atoms last

Balancing Equations

If it’s not working…1. Deep breathe

2. Check your chemical formulas

3. NEVER change subscripts this changes the compounds!!!

4. It’s ok to start over if you get frustrated

Balancing Equations

Balancing Equations

Al(s) + O2(g) Al2O3(s)

Balancing Equations

Na + Mg3(PO4)2 → Mg + Na3PO4 Polyatomic Example:

1. Name the following: CoPO4

and HC2H3O2.

2. What are the formulas for the following: cadmium borate and chloric acid?

Day 3 9-16

1. How do I prepare solutions?

2. How do I balance chemical equations?

C6H14 + O2 CO2 + H2O

C

O

H

C

O

H

6

2

14 2

3

1

C’s First

6

12

13

O’s Second

142 19

26

2828

38

12 12

38

6

Balancing Equations

C3H8(g) + O2(g) CO2(g) + H2O(g)

Molarity = desired concentration moles/liter so a 1M solution contains 1 mole for every 1 liter

Desired concentration X volume (L) X molar mass of solid = needed mass

Desired concentration X volume (L) X molar mass of solid = needed mass

Moles Liters

Liters grams Moles

grams X X =

Molarity = desired concentration moles/liter so a 1M solution contains 1 mole for every 1 liter

Desired conc. X Desired vol. (L) = Starting conc. X Starting vol. of acid (L)

Moles Liters

Liters Moles Liters

LitersX X

Desired conc. X Desired vol. (L) = Starting conc. X Starting vol. of acid (L)

=

350 mL 0.5 M CuCl2

50 mL 0.5 M KOH

300 mL 1 M CuCl2

200 mL 2 M H3PO4

Period 1 9-14

50 mL 0.5 M CuCl2

50 mL 1 M CuCl2

200 mL 4 M H2SO4

200 mL 1 M HCl

Period 3 9-17

Read and/or review section 11.1 AND complete #s 9 (part b only), 10, and

11 on the bottom of page 354

# 11 p. 273, # 13 p. 275, # 14 p. 277, #s 21, 23-26 p. 279

Due tomorrow (Day 3 9-14)

Day 3 9-14

Liquid water breaks apart into hydrogen gas and oxygen

gas (electrolysis).

Equation:

Balance:

Reaction Type:

– solid formed when two aqueous

solutions react – product that comes out of solution

4 . BalanceH2SO4 + NaOH Na2SO4 + H2O

Na

SO4

H

O

Na

SO4

H

O

Types of Chemical Reactions

Synthesis reaction – composition reaction – 2 or more substances combine to form a new compound

A + B AB

A and B = eles. Or cmpds.

AB = cmpd.

Example # 1: 2H2(g) + O2(g) 2H2O(g) A B AB

Synthesis Reactions

A and B = eles. Or cmpds.

AB = cmpd.

Example # 2: 2H2SO3(aq) + O2(g) 2H2SO4(aq)

A B AB

Example # 3: CaO(s) + SO2(g) CaSO3(s)

A B AB

Types of Chemical EquationsSynthesis Reactions

Types of Chemical EquationsSynthesis ReactionsExamples:

- an element reacts with oxygen to form an oxide

- most metals react with halogens to form cmpds.

- oxides of active metals react with water to produce metal hydroxides

- certain metal oxides and nonmetal oxides react to form salts

Types of Chemical EquationsSynthesis Reactions

Types of Chemical EquationsDecompostion Reactionsdecomposition reaction – single compound undergoes a reaction that produces 2 or more simpler subs. – usually require add. of energy (heat or electricity)

AB A + BA and B = eles. Or cmpds.

AB = cmpd.

Example: 2H2O(l) 2H2(g) + O2(g) AB A B

electricity

Types of Chemical EquationsDecompostion ReactionsExamples:

- electric current to a binary compound producing its elements

- heating the oxides of less active metals

- Metal carbonates produce metal oxide + CO2

Types of Chemical EquationsDecompostion Reactions

Electrolysis –

decpomposition of

a substance by an

electrical current

Types of Chemical EquationsDecompostion Reactions