AP Chem Catalyst AP Chem Catalyst Catalyst Questions To Do & Homework You will have 6 tabs: (Use...

AP Chem CatalystCatalyst Questions

① The following atoms in their neutral form are unstable (don’t have 8 valence electrons): Ca, F, N, and S. Find the charges that they would form to become stable Tell me whether they are cations or anions.

To Do & Homework

Homework: Complete Nomenclature Problems

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1.5 Nomenclature

Forming Chemical Bonds

• The force that holds two atoms together is called a chemical bond.

• There are three types of bonds:• Ionic bonds (Metal & Nonmetal)• Covalent bonds (Nonmetal &

Nonmetal)• Metallic bonds(Metal & Metal)

The Formation and Nature of Ionic Bonds

• Cations are atoms with a positive charge.• Anions are atoms with a negative charge.• The electrostatic force holds ions of opposite

charge together, forming an ionic bond.

Ionic BondsCharacteristics of ionic bonds:

Formed between metals and nonmetalsHigh melting point and boiling point.Able to conduct electricity when dissolved in water.Unable to conduct electricity in the solid phase.The strength of the bond depends on the charges,

and distance between ions Ionic bonds form a lattice structure

Covalent Bonds• Characteristics of covalent bonds:

o Formed between nonmetal pairso Electrons are shared between atomso Lower melting points, Lower Boiling Pointso Do not conduct electricityo Brittle solids

Metallic• Properties of metallic bonds:

o Delocalized electronso High electrical conductivityo High luster (shiny)o Remember that transitional metals have a varying

number of valence electrons.

Predict if the following bonds are ionic or covalent:

a) C-N

b) N-O

c) Na-F

d) Mg-S

e) C-H

f) Ca-F

The oxidation number of an ion can be

determined with the aid of the periodic

table.

+1

+2 -1-2-3+4+3

0For transitional metals below, charges vary so when naming ionic compounds with these elements, put the charge in parenthesis after the metal.

ExampleCopper can have a +2 or +3 charge so to know which it is you put parenthesis next to the transitional metal.

Cu (II) means copper with a positive 2 charge Cu2+

Cu (III) means copper with a positive 3 charge Cu3+

Predict the oxidation number of the

following elements:a) Al

b) Mg

c) Si

d) O

e) Cl

Predict the oxidation number of the

following elements:

a) Al +3

b) Mg +2

c) Si +4

d) O -2

e) Cl -1

Nomenclature for Ionic Formula Units

There are over 50 million substances!

We CANNOT have unique names for all these substances, that would be too

much!

That is why we have naming rules.

Nomenclature• Steps for writing ionic formulas:

1. Determine the symbol and oxidation number of the elements

2. If the charges are not the same, subscripts must be added to achieve equal number of positive and negative ions.

3. Criss-cross, ignore charge, write formula4. Metals always first, then nonmetal 5. NO prefixes needed. 6. Ionic formulas end in -ide

Show on Dry Erase:7. Example 1: calcium chloride8. Example 2: Potassium oxide

ExamplesWrite the formula of the following ionic compounds:• Magnesium chloride• Aluminum oxide• Iron (III) chloride• Chromium (III) oxide

You try first, then confirm with partners.

Write the formula of the following ionic compounds:

a) Cesium nitrideb) Barium sulfidec) Calcium oxided) Aluminum fluoridee) Sodium oxide

What if the charges are the same, then just ignore charges, and write the formula, no need for criss- crossing!

Write the formula of the following ionic compounds:1. Iron (II) oxide2. Iron (III) oxide3. Copper (II) chloride4. Lead (IV) iodide5. Iron (II) chloride6. Chromium (III) sulfide7. Titanium (II) oxide8. Lead (IV) sulfide9. Copper (I) nitride

Ionic compounds with polyatomic

ions

Memorize, will be using all year

• Polyatomic ions are groups of atoms with a charge:

1. Ammonium (NH4) +

2. Hydronium (H3O)+

3. Hydroxide (OH)-

4. Sulfate (SO42-)

5. Nitrate (NO31-)

6. Chromate (CrO42-)

7. Carbonate (CO32-)

8. Phosphate (PO43-)

9. Cyanide (CN-)

Review Ionic Formulas using polyatomic ions

Write the formula of the following ionic compounds. Use the flashcards:

a) Calcium nitrateb) Sodium sulfatec) Ammonium oxided) Lead (II) phosphatee) Lead (IV) phosphate

You TryWrite the formula of the following ionic compounds:

a) Chromium (III) hydroxideb) Nickel (II) nitratec) Ammonium sulfated) Silver (I) nitratee) Magnesium chlorate

You try one more timeWrite the formula of the following ionic compounds:a) Potassium carbonate b) Hydrogen carbonate

c) Iron (III) hydroxided) Ammonium phosphatee) Sodium sulfate

Now backwards – ionic no prefixes!

Write the names of each of the following formulas:

a) Na2Ob) CuCl2

c) Cr2O3

HINT: Cu and Cr are transitional metals, so they need roman numerals.

Nomenclature for Covalent Compounds

Molecules that are made from a combination of

two nonmetals (covalent?) require Greek

prefixes in their names

Mono- 1 Hexa- 6 Di- 2 Hepta- 7Tri- 3 Octa- 8Tetra- 4 Nona- 9Penta- 5 Deca- 10

ExamplesFind the formula of the following

a) Phosphorus trifluorideb) Nitrogen dioxidec) Carbon trioxide

Mono is not required for the first nonmetal in the covalent compound

You Trya) Sulfur dibromideb) Sulfur hexachloridec) Phosphorus pentafluoride d) Nitrogen trihydridee) Oxygen difluoride

Now backwards, you try

Name the following compounds:

a) SF2

b) NI3c) CF4

Name the following compounds:

a) PCl3b) N2O3

c) PF3

d) NF3

e) SCl2

Naming Organic Compounds

Organic Compounds containing carbon and hydrogens

• Hydrocarbons are named by counting the number of carbon atoms:

C1 – meth C6 – hex

C2 – eth C7 – hept

C3 – prop C8 – oct

C4 – but C9 – non

C5 – pent C10 – dec

3 types of hydrocarbons

• The ending depends on the type of bond formed:oSingle bond: -ane (Alkanes)oDouble bond: -ene (Alkenes)oTriple bond: -yne (Alkynes)

Is it a ring or a chain?• The number of carbon atoms in a compound is

calculated by the formulas:• CXH2X+2 for chains

• CXH2X for rings

ExamplesWrite the formula/name for each of the following:

a) methaneb) butanec) cyclopropaned) C5H12

e) C6H14

f) C10H20

You tryWrite the formula/name for each of the following:

a) heptaneb) cyclononanec) ethaned) C3H6

e) C5H12

f) C7H14

Nomenclature for Acids

Naming Acids• Binary acids are named using the prefix hydro- and

the suffix –ic acid.• No prefixes

• HCl hydrochloric acid• HBr hydrobromic acid• HI hydroiodic acid• H2SO4sulfuric acid (no hydro- needed)

• HCN hydrocyanic acid