UNIT 4 WRITING & NAMING CHEMICAL COMPOUNDS • What is the Periodic Table?

• Periodic Trends

• Metals and

• What is the Oxidation number?

• More on Ionic Compounds

• Binary Naming of Ionic Compounds

• Polyatomic

• Molecular Compounds

• Little bit of Organic (Hydrocarbons)

• Diatomic's PERIODIC TABLE

• Organization of elements in increasing atomic number/number of protons from left to right and from top to bottom

• The horizontal “rows” are called periods

• Vertical “rows” are called columns or families

• Three types of elements: Metals, Nonmetals, & Metaloids METALS AND NONMETALS

• There are many more metals then nonmetals

• Metaloids make up the “Stairs” METALS CHARACTERISTICS • Have luster (shiny)

• Can conduct electricity this is means that they are conductors

• Ductile- can be pulled out into a wire

• Malleable- can be hammered into thing sheets

• Always lose electrons from their Valance energy level to form positive Ions or Cations

• The Roman numeral or numbers with an “A” beside them at the top of the column on the periodic table are the number of electrons in the Valence electrons each element in the column has NONMETALS

• Do not have luster and are frequently powdery, liquid or gaseous

• do not conduct electricity

• not ductile or malleable

• Always gains electrons in there Valance energy level until they have 8 of electrons (octet rule) and for negative ions which are called Anions PERIODIC TABLE CONTINUED

• Each Family group has the same number of electrons and will either gain or lose electrons to have a fully filled valence shell (8 of Valance electrons), a halfway filled valence shell (4 of Valance electrons), or an empty valence shell (0 pairs of Valance electrons).

• Because of this, names were assigned to each family FAMILY 1: ALKALI METALS

• These elements have 1 single valance electron

• These elements what to have an empty valance shell so they tend to loose their electron when binding to nonmetals

• These elements are the most reactive

• https://youtu.be/I8tOtZKpi04 FAMILY 2: ALKALINE EARTH METALS • These elements tend to lose 2 valance Electrons they have an oxidation of +2 making them very reactive

FAMILY 3-12: TRANSITION METALS • 38 elements. The valence electrons are present in more then one shell this is why they have several oxidation states. FAMILY 17: HALOGENS • Nonmetals with 7 valence electrons in its outer shell. Oxidation number of -1 FAMILY18: NOBLE GASES

• These elements have a full valence shell making them very nonreactive, oxidation number is 0 WHICH FAMILY BELONGS TO THE NONMETALS?

• Alkaline

• Alkaline Earth

• Transitions

• Hallogens WHICH OF THESE ELEMENTS BELONG TO THE ALKALINE EARTH METALS?

• Li

• K

• Ca

• C

• Br WHAT FAMILY DOES FLORINE BELONG TO? NOT MULTIPLE CHOICE

HALLOGENS WHAT FAMILY (COLUMN) DOES THE NOBLE GASES MAKE UP? NOT MULTIPLE CHOICE PERIODIC TRENDS • Reactivity: how easily a metal atom loses its electron (ionization energy). The more reactive the metal the easier it bonds to a .

• The Chart below shows the reactivity trend for Metals. It is the opposite for Nonmetals. Decreases

Increases PERIODIC TRENDS • Electronegativity- Tendency of an atom to pull electrons which are bonded close to itself and add them to its valance orbit

• The most electro negative element is Fluorine Increases

Decreases PERIODIC TRENDS

• Electron Affinity- Amount of energy absorbed or given off when an atom is forced to accept an electron

• The more negative value the higher the affinity and vise versa Increase

Decreases PERIODIC TRENDS

• Ionization Energy- Amount of energy to remove 1 electron from an atom

Increases

Decreases PERIODIC TRENDS

• Atomic Radius- radius “across” an atom

Decreases

Increases PERIODIC TRENDS

• Shielding- a barrier made of inner-shell electrons which serves to decrease the pull of the nucleus on outer electrons

Constant

Increases WHAT IS THE MOST ELECTRONEGATIVE ELEMENT? WHICH ELEMENT HAS THE HIGHEST ELECTRON AFFINITY

• Li

• C

• O

• Fr WHICH METAL IS MOST REACTIVE?

• Rb

• Li

• Al

• O

• Ca WHICH ELEMENT HAS THE LEAST AMOUNT OF SHIELDING?

• K

• Te

• C

• He

• N WHICH NONMETAL IS THE MOST ELECTRONEGATIVE?

• C

• P

• Ca

• Na

• At WHAT IS THE MOST REACTIVE NONMETAL

• Cl

• Ga

• Se

• I

• At WHICH ELEMENT HAS THE HIGHER IONIZATION ENERGY?

• N

• P

• As

• Sb

• Bi • Positive Ions ace called Cations. They have more protons then they have electrons. Metals always lose electrons.

• Negative ions are called Anions. They have gained more electrons in their valance energy level and therefore have more electrons then protons. OXIDATION NUMBERS • Oxidation Number- The overall charge on an after It has lost electrons (metals) or gained electrons (nonmetals)

• It is easier to memorize the family trends for the oxidation numbers

• The oxidation number of an atom in a compound is the charge it would have if all shared electrons were assigned to that with the greatest attraction for electrons. +1 OXIDATION # TRENDS

+2 +3 +4 -3 -2 -1 RULES FOR ASSIGNING OXIDATION NUMBERS

• Oxidation number of an atom in its free Cu element for is “0” Oxidation number is “0”

• The oxidation stat of a monoatomic ion is Ca2+ equal to its charge “2+” ox #

• The sum of oxidation numbers in a neutral H2O is “0” and an Ion is equal to the H ox# “1+” O ox# “2-“ stated charge (so we needed 2 H to count for O’s charge) • Group 1 always have an oxidation number NaCl of 1+ Group 2 have a 2+ ect. Na ox# “1+” Cl ox# “1-“ COMPOUNDS WITH OXIDATION NUMBERS

• When ions (charged elements) are combined together forming compounds, the overall charge of the compound which results must be neutral or “0”

• In order to do this sometimes you might need to change the ratio of elements in the compound

Mg2+ Cl1-

MgCl2 WEIGHTING CHEMICAL FORMULAS

• Split the ions up into its components

• Assign Oxidation numbers to each individual element

• Cross your oxidation numbers and make note of ration

• Check if it “zero’s” out

• Wright compound formula Wright the metal ion FIRST and the nonmetal LAST WRIGHT THE CORRECT FORMULA FOR THE A COMPOUND BETWEEN THESE TWO ELEMENTS:

• Lithium and Florine

• Calcium and

• Cesium (#55) and

• Potassium and

• Sodium and Oxygen

• Calcium and Bromine IONIC COMPOUNDS

• Ionic compounds- compounds made of

• A Metal and Nonmetal

• Metal and Polyatomic Ion

• Ion (NH4) and Nonmetal

• Ammonium Ion (NH4) and a Polyatomic Ion BINARY NAMING OF IONIC COMPOUNDS

• Binary Naming is naming of 2 elements only

• First: call the entire name of the metal

• Then: shorten the name of the nonmetal and add “ide” as a suffix

KCl Potassium Chloride EXAMPLE OF “IDE” ENDINGS

• Fluorine- Fluoride • Oxygen-

• Sulfur- • Phosphorus- Phosphide

• Bromine- • Iodine-

• - Nitride • - Chloride NAME THE FOLLOWING IONIC COMPOUNDS:

• MgBr2

• NaF

• ZnS

• Na2O

• K3N

• Al2O3 TRANSITION METALS RULES

• Each transition metal has multiple oxidation numbers

• When naming these you must use the latin names and the “ic and ous” naming system

• Use the ic suffix for the highest oxidation number

• Use the ous suffix for the lowest oxidation number EXAMPLES

• Copper (+2 & +1) • Cupric and Cuprous

• Iron (+3 & +4) • Ferric and Ferrous

• Lead (+4 & +2) • Plumbic and Plumbous

• Tin (+4 & +2) • Stannic and Stannous

• (+2 & +1) • Mercuric and Mercurous IUPAC NAMING • IUPAC (International Union of Practical and Applied Chemistry)

• IUPAC came up with a naming system for these transition metals that included metals with more then 2 different charges they called it “Stock naming”

• Uses a metal’s name followed by a Roman numeral in parentheses which indicates its oxidations number 2+ Cu would be called copper (II) WRITE THE CORRECT FORMULA:

• Iron (III) Oxide

• Tin (IV) Chloride

• Lead (IV) Oxide

• Tin (II) Sulfide

• Mercury (II) Bromide

• Iron (II) iodide HOW DO YOU KNOW WHICH OXIDATION NUMBER TO USE IF YOU ARE GIVEN A FORMULA AND ASKED TO NAME THE COMPOUND?

• Check your NEGATIVE ION’S oxidation number. These never change

• Once you've figured out the negative oxidation number you make the compound’s overall charge neutral unless specified otherwise.

• Pay attention to your ratios!!!!!

FeO Iron (II) Oxide WHAT IF YOUR RATIO IS NOT 1:1

SnS2 • Still Check the negative ion first, But keep in mind the ratio (stoichiometry) and multiply the OXIDATION NUMBER by the RATIO.

• Once you found the new total negative oxidation number then you can find the positive oxidation by making the compound neutral.

Sulfur -2 oxidation number The overall oxidation is SnS2 But there are 2 Sulfur Ions neutral. So in order to So the new oxidation number make -4 “0” the Tin (Sn) -2 x 2 = -4 +4. Tin (IV) Sulfide NAME THE FOLLOWING COMPOUNDS WITH STOCK NAMING:

• FeCl2

• SnO

• Hg2I2

• CuI

• PbO2 POLYATOMIC IONS

• Polyatomic Ions- Ions which are imposed of several different elements

• These elements stay together in a chemical reaction and the entire group has an oxidation number or charge

• I STRONGLY ADVISE YOU MEMORIZE THESE ASAP!!!!

• When writing a polyatomic ion in a compound if you have a subscript you must put your Polyatomic Ion in parenthesis then the subscript outside of it. Polyatomic Subscript Ion Al(NO3)3 POLY ATOMIC ION CHART WRITE THE CORRECT FORMULA FOR EACH OF THE FOLLOWING COMPOUNDS:

• Aluminum

• Copper (II)

• Zinc

• Silver

• Aluminum NAMING MOLECULAR COMPOUNDS

• These compounds are made up of 2 nonmetals

• When Naming these compounds use a prefix to indicate the number of atoms of each element presents

• Do not use prefixes in IONIC compounds

• Outside of Prefixes keep the first metals name the same then add the suffix “ide” onto the end of shortened second metal Prefixes: 1. No prefix needed or use mono 6. Hexa 2. Di 7. Hepta 3. Tri 8. Octa 4. Tetra 9. Nona 5. Penta 10.Deca NAME THE FOLLOWING MOLECULAR COMPOUNDS:

• N2O5

• SO3

• CO

• P4O10

• As2O3 HYDROCARBONS (A LITTLE ORGANIC CHEMISTRY)

• Organic Chemistry is basically the chemistry of Carbon

• Hydrocarbons are Carbon chains with attached to them

• There are 2 types of Hydrocarbon chains: Straight Chain: Pentane Cyclic Chain: Cyclopentane HYDROCARBONS STRAIGHT CHAINS NAMING

• General Formula for recognition: CxH2x + 2

• Once you've identified it as a straight chain: you count the number of Carbons

• Use the same prefixes as did in molecular compounds from 5-10 then add the suffix “ane” on the end

• For hydrocarbons with 1-4 carbons you will just have to memorize the prefix Carbons 1-4 1.Methane 3. Propane 2.Ethane 4. Butane C5H12 Pentane CYCLIC HYDROCARBONS

• Formula for Recognition: CxH2x

• The smallest Cyclic structure has 3 Carbons

• When naming theses structures you count the amount of Carbons and use the same name as the straight chain hydrocarbons

• EXCEPT: You add the prefix “cyclo”

C6H12 Cyclohexane

C8H16 Cyclooctane NAME THE HYDROCARBONS

Hint: remember to find out the equation for both straight chain and cyclic hydrocarbons

• C3H6

• C5H12

• C8H18

• C4H8

• C7H16

• C5H10 CxH2x + 2

CxH2x WRITE THE CHEMICAL EQUATION:

Hint: remember the equation for both straight chain and cyclic hydrocarbons

• Cyclohexane

• Ethane

• Cyclobutane

• Decane

CxH2x + 2

CxH2x DIATOMIC’S

• There are 7 elements that cannot exist by themselves as single atoms, these are known as the diatomic

• They occur naturally in the world just in pairs

• All these elements in their purest forms combine with each other (having a 2 subscript next to them).

• These elements conveniently make a 7 on the periodic table besides

Br2 H2 O2 DIATOMICS TRENDS REMEMBER WHEN NAMING COMPOUNDS

• First What kind of compound is it?

• Ionic (metal and nonmetal)

• Molecular (nonmetal and nonmetal)

• Polyatomic

• Hydrocarbons

• Then: Find out the ratio of atoms and/or oxidation number

• Then: follow rules for each set of compounds