ion formation an atom there are the same number of protons and electrons it is electrically neutral

ION FORMATIONION FORMATION

an atom there are the same an atom there are the same number of protons and electronsnumber of protons and electrons

it is electrically neutral.it is electrically neutral.


An ion is an atom that has lost or An ion is an atom that has lost or gained electrons and now has an gained electrons and now has an electric chargeelectric charge


The net charge of an ion that has The net charge of an ion that has lost or gained electrons is shown lost or gained electrons is shown as a superscript to the right of the as a superscript to the right of the atomic symbolatomic symbol

It is also called the oxidation It is also called the oxidation numbernumber


Na = Na+1

Bi = Bi-3

Bismuth will gain 3 electrons and have a negative 3 charge

Sodium will lose its electron and become positively charged

Oxidation number


The number of electrons that an The number of electrons that an atom will gain or lose depends on atom will gain or lose depends on its position on the periodic table its position on the periodic table (group number)(group number)

Na =

Ca+ionCa+ion

An atom that has lost electrons and An atom that has lost electrons and now has a net positively chargednow has a net positively charged

Na+1

Sodium will lose its electron and become positively charged

AnionAnion

An atom that has gained an An atom that has gained an electron and now has a net electron and now has a net negative chargenegative charge

Bi = Bi -3

Bismuth will gain 3 electrons and have a negative 3 charge


Metals, elements to the left of the Metals, elements to the left of the staircase, will form cations (+ staircase, will form cations (+ charge)charge)

Nonmetals, elements to the right of Nonmetals, elements to the right of the staircase will form anions (- the staircase will form anions (- negative)negative)

ION FORMATION ION FORMATION group “B” elementsgroup “B” elements

The oxidation numbers of the “B” The oxidation numbers of the “B” group elements are variable. group elements are variable.

They do not follow a pattern like They do not follow a pattern like the Group “A” elements.the Group “A” elements.


Oxidation numbers will be given to Oxidation numbers will be given to you as a Roman Numeral in you as a Roman Numeral in parentheses following the name parentheses following the name of the element.of the element.

Practice1. Write the ion formed by these

element.a. iodine I-1 d. cobalt (II) Co+2

b. potassium K+1 e. gallium Ga+3

c. sulfur S-2 f. chromium (III) Cr+3



Writing Ions Writing Ions PracticePractice

IONION OxidationOxidationCationCation

NumberNumber or Anion or Anion

BromineBromine 11 AnionAnion

RubidiumRubidium 11 CationCation

BariumBarium 22 CationCation

SulfurSulfur 22 AnionAnion

Tin (IV)Tin (IV) 44 CationCation

IodineIodine 11 AnionAnion

ArgonArgon 00 NeitherNeither

AluminumAluminum 33 CationCation

MagnesiumMagnesium 22 CationCation

IONION OxidationOxidationCationCation

NumberNumber or Anion or Anion

StrontiumStrontium 22 AnionAnion

Lead (II)Lead (II) 22CationCation

Antimony (V)Antimony (V) 55CationCation

PhosphorusPhosphorus 33 AnionAnion

Copper (I)Copper (I) 11 CationCation

SeleniumSelenium 22 AnionAnion

BONDINGBONDING

Remember that a compound Remember that a compound consist of two or more elements consist of two or more elements chemically combined togetherchemically combined together

HH22O, NaCl, SbO, NaCl, Sb33(PO(PO44))55

BONDINGBONDING

The smallest unit of a compound is The smallest unit of a compound is a moleculea molecule

Only electrons move during bondingOnly electrons move during bonding

It is the movement of valence It is the movement of valence electrons that determines how electrons that determines how one atom will bond with anotherone atom will bond with another

BONDINGBONDING

Octet Rule- all atoms need 8 Octet Rule- all atoms need 8 valence electrons to be stablevalence electrons to be stable

BONDING, FOUR TYPESBONDING, FOUR TYPES

IONIC- Transfer of electronsIONIC- Transfer of electrons

COVALENT- sharing of electronsCOVALENT- sharing of electrons

POLAR COVALENT- uneven sharing of electronsPOLAR COVALENT- uneven sharing of electrons

METALLIC- bonds between cations and free METALLIC- bonds between cations and free electronselectrons

IONIC BONDSIONIC BONDS

Electrons are transferred from one Electrons are transferred from one atom to anotheratom to another

This creates a Cation (+) and anThis creates a Cation (+) and an

Anion (-)Anion (-)

Opposite charges attract Opposite charges attract

IONIC BONDINGIONIC BONDING

Cl

Cl

-1

Na

Na+1

Cl-1

Na+1

The Cation (Na) is attracted to the Anion (Cl)

IONIC BONDINGIONIC BONDING

Ionic Bonds are the strongest bondsIonic Bonds are the strongest bonds

Form between Metals and Non-Form between Metals and Non-MetalsMetals

BONDINGBONDINGThe stair case separates Metals (Left) from Non-Metals (Right)

IONIC BONDINGIONIC BONDINGLewis DotLewis Dot

Cl

Cl

-1

Na

Na+1

BONDINGBONDINGEnergy LevelsEnergy Levels

Na

Na

Cl

Cl

+1-1

Writing Formulas for Writing Formulas for Ionic CompoundsIonic Compounds

Ion- an atom that has lost or gained Ion- an atom that has lost or gained electronselectrons

Cation- Lost electrons positive Cation- Lost electrons positive chargecharge

Anion- Gained electrons negative Anion- Gained electrons negative chargecharge


Oxidation number- indicates the Oxidation number- indicates the number of electrons lost or number of electrons lost or gained during bondinggained during bonding

To be stable- oxidation number To be stable- oxidation number must be zero (no charge)must be zero (no charge)

Binary Compound– formed between Binary Compound– formed between metal and non-metalmetal and non-metal


1.1. Write the ion of the Cation – MgWrite the ion of the Cation – Mg+2+2

2.2. Write the ion of the Anion – OWrite the ion of the Anion – O-2-2

3.3. Write the subscripts (bottom Write the subscripts (bottom numbers) to indicate how many numbers) to indicate how many ions of each element is needed ions of each element is needed to make the sum of the oxidation to make the sum of the oxidation numbers zero (do not write 1’s)numbers zero (do not write 1’s)


Magnesium (Mg)Magnesium (Mg)

Group IIGroup II

Loses two Loses two electronselectrons

MgMg+2+2

Oxygen (O)Oxygen (O)

Group VIGroup VI

Gains two Gains two electronselectrons

OO-2-2


MgMg+2 +2 + O + O -2 -2 = net charge of 0 = net charge of 0

Formula = MgOFormula = MgO


Magnesium (Mg)Magnesium (Mg)

Group IIGroup II


MgMg+2+2

Bromine (Br)Bromine (Br)

Group IIVGroup IIV

Gains one Gains one electronselectrons

Br Br -1-1


MgMg+2 +2 + Br + Br -1 -1 = net charge of +1 = net charge of +1We need 2 Br We need 2 Br -1 -1 ions to even out the ions to even out the

chargecharge

MgMg+2 +2 + Br + Br22 -1 -1 = net charge of 0 = net charge of 0(Mg(Mg+2 +2 + Br + Br -1 -1 + Br + Br -1-1 = net charge of 0) = net charge of 0)

Formula = MgBrFormula = MgBr22


Sodium (Na)Sodium (Na)

Group IGroup I

Loses one Loses one electronselectrons

NaNa+1+1


Group VIGroup VI


O O -2-2

Combine Sodium and Oxygen


NaNa+1 +1 + O + O -2 -2 = net charge of -1 = net charge of -1We need 2 Na We need 2 Na +1 +1 ions to even out the ions to even out the

chargecharge

NaNa22+2 +2 + O + O -2 -2 = net charge of 0 = net charge of 0(Na(Na+1 +1 + Na+ Na+1 +1 + O + O -2-2 = net charge of 0) = net charge of 0)

Formula = NaFormula = Na22OO


Calcium (Ca)Calcium (Ca)

Group IIGroup II


CaCa+2+2

Fluorine (F)Fluorine (F)

Group VIIGroup VII


F F -1-1

Combine Calcium and Fluorine


CaCa+2 +2 + F + F -1 -1 = net charge of +1 = net charge of +1We need 2 F We need 2 F -1 -1 ions to even out the ions to even out the

chargecharge

CaCa+2 +2 + F + F22 -1 -1 = net charge of 0 = net charge of 0(Ca(Ca+2 +2 + F+ F-1 -1 + F + F -1-1 = net charge of 0) = net charge of 0)

Formula = CaFFormula = CaF22


Iron (II) (Fe II)Iron (II) (Fe II)

Fe Fe (II)(II)


FeFe+2+2

Sulfur (S)Sulfur (S)

Group VIGroup VI


S S -2-2

Combine Iron (II) and Sulfur


FeFe+2 +2 + S + S -2 -2 = net charge of 0 = net charge of 0

Formula = FeSFormula = FeS

Writing Formulas for Writing Formulas for Ionic Compounds: Ionic Compounds: CrisscrossCrisscrossA SHORTCUT to figure out then A SHORTCUT to figure out then

number of each ion needed to number of each ion needed to form a neutral compoundform a neutral compound

Writing Formulas for Writing Formulas for Ionic Compounds: Ionic Compounds: CrisscrossCrisscross1.1. Write each Cation first followed Write each Cation first followed

by the Anionby the Anion2.2. Cross the oxidation numbers Cross the oxidation numbers

(superscript) to be the subscript (superscript) to be the subscript of the other of the other

3.3. Reduce the subscripts if they Reduce the subscripts if they aren’t alreadyaren’t already

Writing Formulas for Writing Formulas for Ionic Compounds: Ionic Compounds: CrisscrossCrisscrossMagnesium (Mg)Magnesium (Mg)

Group IIGroup II


MgMg+2+2

Bromine (Br)Bromine (Br)

Group IIVGroup IIV


Br Br -1-1

Writing Formulas for Writing Formulas for Ionic Compounds: Ionic Compounds: CrisscrossCrisscross

MgMg+2 +2 Br Br -1-1

MgMg 11 Br Br22

Formula = MgBrFormula = MgBr22

Writing Formulas for Writing Formulas for Ionic Compounds: Ionic Compounds: CrisscrossCrisscrossMagnesium (Mg)Magnesium (Mg)

Group IIGroup II


MgMg+2+2


Group VIGroup VI


OO-2-2


MgMg+2 +2 + O + O -2-2

MgMg+2+2 + O + O-2-2

Formula = MgFormula = Mg22 O O22

(REDUCE) (REDUCE)

=MgO

Writing Formulas for Writing Formulas for Ionic Compounds: Ionic Compounds: CrisscrossCrisscross

Sodium (Na)Sodium (Na)

Group IGroup I

Loses one electronLoses one electron

NaNa+1+1


Group VIGroup VI


O O -2-2

Combine Sodium and Oxygen


NaNa+1 +1 + O + O -2 -2

NaNa22 + O + O11

Formula = NaFormula = Na22OO


Iron (II) (Fe II)Iron (II) (Fe II)

Fe Fe (II)(II)


FeFe+2+2

Sulfur (S)Sulfur (S)

Group VIGroup VI


S S -2-2

Combine Iron (II) and Sulfur


FeFe+2 +2 + S + S -2-2

FeFe2 2 + S + S22

FeFe22SS2 2

REDUCE to REDUCE to FeSFeS

Naming Ionic Naming Ionic CompoundsCompounds

1.1. Write the name of the cation Write the name of the cation firstfirst


2. If the cation is a transition metal 2. If the cation is a transition metal add a Roman Numeral in add a Roman Numeral in parentheses to indicate parentheses to indicate oxidation number oxidation number

a)a) Use crisscross method in reverseUse crisscross method in reverse

FeS = FeFeS = Fe+1+1 S S-1 -1

Naming Ionic Naming Ionic CompoundsCompoundsb) Check negative ion to see if it b) Check negative ion to see if it

has correct oxidation number; has correct oxidation number; multiply the charges by the multiply the charges by the correct number till it doescorrect number till it does

FeS = FeFeS = Fe+1+1 SS-1-1 should be Sshould be S-2-2

2 x (Fe2 x (Fe+1+1 S S-1-1 ) = Fe ) = Fe+2+2 S S+2+2

Naming Ionic Naming Ionic CompoundsCompoundsc) Remember the Roman numeral c) Remember the Roman numeral

only goes in the name, not the only goes in the name, not the formula formula

(TRANSITON METAL ONLY)(TRANSITON METAL ONLY)

FeS = FeFeS = Fe+2+2 S S+2+2


3.3. Write the name of the anionWrite the name of the anion

Take the root word of the element Take the root word of the element name and end it with –idename and end it with –ide

FeS = Iron (II) sulfideFeS = Iron (II) sulfide


NaFNaF

1.1. SodiumSodium

2.2. Sodium is not a Sodium is not a transition metaltransition metal

3.3. FluorideFluoride

Sodium FluorideSodium Fluoride

MgOMgO

1.1. MagnesiumMagnesium

2.2. Magnesium is Magnesium is not a transition not a transition metalmetal

3.3. OxideOxide

Magnesium OxideMagnesium Oxide


CuClCuCl221.1. CopperCopper2.2. Copper is a transition metalCopper is a transition metal

a)a) CuCl CuCl2 2 = Cu= Cu+2 +2 ClCl-1-1

b)b) Cu Cu+2 +2 ClCl-1 -1 is correctis correctc) Copper (II)c) Copper (II)

3. Chloride3. Chloride

Copper (II) ChlorideCopper (II) Chloride


PbOPbO1.1. LeadLead2.2. Lead is a transition metalLead is a transition metal

a)a) PbO PbO = Pb= Pb+1 +1 OO-1-1

b)b) Pb Pb+1 +1 OO-1 -1 is not correctis not correct2(Pb2(Pb+1+1 OO-1-1) = Pb) = Pb+2+2 OO-2-2

c) Lead (II)c) Lead (II)

3. Oxide3. Oxide

Lead(II) OxideLead(II) Oxide


ZnSZnS ZincZinc Zinc is a transition metalZinc is a transition metal

a)a) ZnS ZnS = Zn= Zn+1 +1 SS-1-1

b)b) Zn Zn+1 +1 SS-1 -1 is not correctis not correct2(Zn2(Zn+1+1 SS-1-1) = Zn) = Zn+2+2 SS-2-2

c) Zinc (II)c) Zinc (II)

3. Sulfide3. Sulfide

Zinc (II) sulfideZinc (II) sulfide


KK33NN PotassiumPotassium Potassium is not a transition metalPotassium is not a transition metal

3. Nitride3. Nitride

Potassium NitridePotassium Nitride


BaOBaO BarriumBarrium Barrium is not a transition metalBarrium is not a transition metal

3. Oxide3. Oxide

Barrium OxideBarrium Oxide


CaOCaO CalciumCalcium Calcium is not a transition metalCalcium is not a transition metal

3. Oxide3. Oxide

Calcium OxideCalcium Oxide


AlFAlF33

AluminumAluminum Zinc is not a transition metalZinc is not a transition metal

3. Fluoride3. Fluoride

Aluminum FluorideAluminum Fluoride


CuICuI22 CopperCopper Copper is a transition metalCopper is a transition metal

a)a) CuS CuS2 2 = Cu= Cu+2 +2 II-1-1

b)b) Cu Cu+2 +2 I I-1 -1 is correctis correct

c) Copper (II)c) Copper (II)

3. Iodide3. Iodide

Copper (II) IodideCopper (II) Iodide

Naming Polyatomic Naming Polyatomic CompoundsCompoundsPolyatomic compounds have more Polyatomic compounds have more

than 2 different types of elements than 2 different types of elements in the formula Ex. Hin the formula Ex. H22SOSO44

NHNH44+1 +1 is the only Polyatomic ion that is is the only Polyatomic ion that is

a Cation a Cation

All others will come after the metal All others will come after the metal ionion

Name Formula

Ammonium NH41+

Acetate C2H3O21-

Chlorate ClO31-

Hydroxide OH1-

Nitrate NO31-

Carbonate CO32-

Sulfate SO42-

Sulfite SO32-

Phosphate PO43-

Nitrite NO21-

Chlorite ClO21-

Cyanide CN1-

Naming Polyatomic Naming Polyatomic CompoundsCompounds

Name a polyatomic compound just Name a polyatomic compound just like you would an ionic like you would an ionic compound but you do not compound but you do not change the ending of the change the ending of the Polyatomic ionPolyatomic ion

ZnSOZnSO4 4

From the ion chart SOFrom the ion chart SO4 4 is an polyatomic is an polyatomic ionion

1.1. ZincZinc2.2. Zinc is a transition metalZinc is a transition metal

a) Zn(SOa) Zn(SO44)) = Zn= Zn+1 +1 (SO(SO44) ) -1-1

b) Znb) Zn+1 +1 (SO(SO44)) -1 -1 is not correctis not correct

From the ion chart (SOFrom the ion chart (SO44)) -2-2

2(Zn2(Zn+1+1 SOSO44-1-1) = Zn) = Zn+2+2 SOSO44

-2-2

c) Zinc (II)c) Zinc (II)

3. Sulfate… From the chart3. Sulfate… From the chart

Zinc(II) sulfateZinc(II) sulfate


NaOHNaOH

From the ion chart OHFrom the ion chart OH is an is an polyatomic ionpolyatomic ion

1.1. SodiumSodium

2.2. Sodium is not a transition metalSodium is not a transition metal

3.3. 3. OH… Hydroxide… From the chart3. OH… Hydroxide… From the chart

Sodium HydroxideSodium Hydroxide


CaCOCaCO33

From the ion chart COFrom the ion chart CO3 3 is an is an polyatomic ionpolyatomic ion

1.1. CalciumCalcium

2.2. Calcium is not a transition metalCalcium is not a transition metal

3.3. 3. CO3. CO3 3 from the chart = Carbonatefrom the chart = Carbonate

Calcium CarbonateCalcium Carbonate


KCl0KCl022

From the ion chart ClOFrom the ion chart ClO2 2 is an is an polyatomic ionpolyatomic ion

1.1. PotassiumPotassium

2.2. Potassium is not a transition metalPotassium is not a transition metal

3.3. 3. ClO3. ClO2 2 from the chart = Chloratefrom the chart = Chlorate

Potassium ChloratePotassium Chlorate


Al(OH)Al(OH)33

From the ion chart OHFrom the ion chart OH is an is an polyatomic ionpolyatomic ion

1.1. AluminumAluminum

2.2. Aluminum is not a transition metalAluminum is not a transition metal

3.3. OHOH from the chart = Hydroxidefrom the chart = Hydroxide

Aluminum HydroxideAluminum Hydroxide


MgMg33(PO(PO44))22

From the ion chart POFrom the ion chart PO4 4 is an is an polyatomic ionpolyatomic ion

1.1. MagnesiumMagnesium

2.2. MAgnesium is not a transition metalMAgnesium is not a transition metal

3.3. 3. PO3. PO4 4 from the chart = Phosphatefrom the chart = Phosphate

Magnesium PhosphateMagnesium Phosphate

Binary Compounds Binary Compounds with Polyatomic Ionswith Polyatomic Ions Covalently-bonded groups of Covalently-bonded groups of

atoms that behave as a unit and atoms that behave as a unit and carry a chargecarry a charge

NONO33-1-1

Binary Compounds Binary Compounds with Polyatomic Ionswith Polyatomic Ions The Charge that is shown is for The Charge that is shown is for

the whole group not just the last the whole group not just the last atomatom

(NO(NO33))-1-1

Binary Compounds Binary Compounds with Polyatomic Ionswith Polyatomic Ions

Polyatomic ions have very specific Polyatomic ions have very specific names. (LIST ON YOUR NOTES)names. (LIST ON YOUR NOTES)

Binary Compounds Binary Compounds with Polyatomic Ionswith Polyatomic Ions1.1. To write the formula, use the criss To write the formula, use the criss

cross method for Polyatomic ions cross method for Polyatomic ions just like you did for regular ions. just like you did for regular ions.

2.2. Never change anything within the Never change anything within the polyatomic ionpolyatomic ion

3.3. Add subscripts outside Add subscripts outside parentheses parentheses


Magnesium PhosphateMagnesium Phosphate

Mg Mg +2+2 POPO4 4 -3-3

MgMg33(PO(PO44))22

Binary Compounds Binary Compounds with Polyatomic Ionswith Polyatomic IonsMagnesium CarbonateMagnesium Carbonate

Mg Mg +2+2 COCO33-2-2

MgMg22(CO(CO33))2 Reduce 2 Reduce

Mg(COMg(CO33))


Calcium HydroxideCalcium Hydroxide

Ca Ca +2+2 OHOH -1-1

Ca(OH)Ca(OH)22


Manganese(IV) SulfiteManganese(IV) Sulfite

Mn Mn +4+4 SOSO3 3 -2-2

MnMn22(SO(SO33))44

Covalent BondsCovalent Bonds

Electrons are shared between Electrons are shared between atoms but not transferredatoms but not transferred

Electrons are located in the Electrons are located in the outermost energy levels of both outermost energy levels of both atoms at the same timeatoms at the same time

Form between nonmetalsForm between nonmetals


NHNH33

Lewis Dot Lewis Dot

NN

H

HH


NHNH33

Energy Level Energy Level H

H

H

N

Covalent BondsCovalent BondsIonic vs. Covalent Properties

Covalent Bonds Ionic Bonds

type of elements

Nonmetals only Metals and Nonmetals

type of bonding share electrons transfer electrons

structure not rigid – solid, liquid or gas

crystalline

melting point low high

hardness soft hard very hard

conduct electricity?

no yes (when dissolved in water)

Covalent Bonds: Covalent Bonds: Diatomic AtomsDiatomic Atoms

There are 7 elements that can form There are 7 elements that can form covalent bonds between its atomscovalent bonds between its atoms

HydrogenHydrogen

Atoms Atoms Molecule Molecule H·H· ·H ·H H:H H:H


NitrogenNitrogen

AtomsAtoms · ·· ·

: N · · N :: N · · N : · · · ·MoleculeMolecule Forms a triple bondForms a triple bond

: N : : : N :: N : : : N :


·· ··O : : O ·· ··

·· ··: F : F :

·· ··

·· ··:Cl : Cl :

·· ··

·· ··

: Br : Br: ·· ··

·· ··: I : I :·· ··

OXYGEN(Double bond

between atoms)

FLOURINE CHLORINE BROMINE IODINE

Determine ionic or Determine ionic or covalent bondscovalent bondsNN22OO55

A liquid at toom A liquid at toom temptemp

PbNOPbNO33

Covalent Covalent (nonmetals)(nonmetals)

Covalent (liquid)Covalent (liquid)

Ionic (Metal with Ionic (Metal with nonmetal)nonmetal)

Determine ionic or Determine ionic or covalent bondscovalent bondsA salt that conducts A salt that conducts

electricity in electricity in solutionsolution

KFKF

AgClAgCl

Ionic (conducts Ionic (conducts electricity)electricity)

Ionic (metal with Ionic (metal with nonmetal)nonmetal)

Ionic (Metal with Ionic (Metal with nonmetal)nonmetal)

Determine ionic or Determine ionic or covalent bondscovalent bondsGasolineGasoline

PClPCl33

OO22

Covalent (liquid)Covalent (liquid)

Covalent (metal to Covalent (metal to metal)metal)

Covalent (share Covalent (share electrons)electrons)

Naming Covalent Naming Covalent CompoundsCompoundsOxidation numbers are not used in Oxidation numbers are not used in

determining the formula unitdetermining the formula unit

Two nonmetals can combine in more Two nonmetals can combine in more than 1 waythan 1 way

We use prefixes to name and We use prefixes to name and indicate the number of atoms of indicate the number of atoms of each type each type

Naming Covalent Naming Covalent CompoundsCompounds

Prefix Number

mono 1

di 2

tri 3

tetra 4

penta 5

hexa 6

hepta 7

octa 8

nona 9

deca 10


Write the name of the element that Write the name of the element that is farthest left first is farthest left first

Write the other element second Write the other element second and change the ending to –ideand change the ending to –ide

Add prefixes to the two elementsAdd prefixes to the two elementsDo not use mono on first elementDo not use mono on first element

Naming Covalent Naming Covalent CompoundsCompoundsCOCO22

Element to left first, then the second element with Element to left first, then the second element with an –ide endingan –ide ending

Carbon OxideCarbon OxideAdd prefixesAdd prefixes

Monocarbon DioxideMonocarbon Dioxide

Drop Mono from first elementDrop Mono from first element

Carbon dioxideCarbon dioxide

Naming Covalent Naming Covalent CompoundsCompoundsCFCF44

Element to left first, then the second element with an –ide Element to left first, then the second element with an –ide endingending

Carbon FlourideCarbon FlourideAdd prefixesAdd prefixes

Monocarbon Monocarbon TetraflourideTetraflouride


Carbon Carbon TetraflourideTetraflouride

Naming Covalent Naming Covalent CompoundsCompoundsSiClSiCl33Element to left first, then the second element Element to left first, then the second element

with an –ide endingwith an –ide ending

Silicone ChlorideSilicone ChlorideAdd prefixesAdd prefixes

Monosilicone Monosilicone trichloridetrichloride


Silicon TrichlorideSilicon Trichloride

Naming Covalent Naming Covalent CompoundsCompoundsCOCO22

Element to left first, then the second element with Element to left first, then the second element with an –ide endingan –ide ending

Carbon OxideCarbon OxideAdd prefixesAdd prefixes

Monocarbon DioxideMonocarbon Dioxide


Carbon dioxideCarbon dioxide

Naming Covalent Naming Covalent CompoundsCompoundsHH22OOElement to left first, then the second element with an –Element to left first, then the second element with an –

ide endingide ending

Hydrogen OxideHydrogen OxideAdd prefixesAdd prefixes

Dihydrogen oxideDihydrogen oxide


Dihydrogen Dihydrogen oxideoxide


Common names to rememberCommon names to remember

HH22O = WaterO = Water

NHNH3 3 = Ammonia= Ammonia

CHCH4 4 = Methane= Methane

Writing Formulas for Writing Formulas for Binary Covalent Binary Covalent CompoundsCompoundsList the symbol of the first element List the symbol of the first element

in the name first and then second in the name first and then second element nextelement next

Use the subscripts to identify the Use the subscripts to identify the prefix in the name for that atomprefix in the name for that atom

Writing Formulas for Writing Formulas for Binary Covalent Binary Covalent CompoundsCompoundsCarbon TetrachlorideCarbon Tetrachloride

C ClC Cl

Tetra= 4Tetra= 4

CClCCl44

Writing Formulas for Writing Formulas for Binary Covalent Binary Covalent CompoundsCompoundsDinitrogen TrioxideDinitrogen Trioxide

NN OO

Di = 2Di = 2 Tri = 3Tri = 3

NN22OO33

Writing Formulas for Writing Formulas for Binary Covalent Binary Covalent CompoundsCompoundsIodine PentaflourideIodine Pentaflouride

I FI F

Penta = 5Penta = 5

IFIF55

Writing Formulas for Writing Formulas for Binary Covalent Binary Covalent CompoundsCompoundsHexaboron SilicideHexaboron Silicide

B SiB Si

Hexa = 6 Hexa = 6

BB66SiSi

Writing Formulas for Writing Formulas for Binary Covalent Binary Covalent CompoundsCompoundsDiantomny PentoxideDiantomny Pentoxide

Sb OSb O

Di = 2Di = 2 Penta = 5Penta = 5

SbSb22OO55

Writing Formulas for Writing Formulas for Binary Covalent Binary Covalent CompoundsCompoundsAmmoniaAmmonia

NHNH33

Polar Covalent BondsPolar Covalent Bonds

A type of covalent bond where electrons A type of covalent bond where electrons are shared unequally between atomsare shared unequally between atoms

Electrons spend more time with one atom Electrons spend more time with one atom than the otherthan the other

The stronger atom will be slightly The stronger atom will be slightly negative and the other will be slightly negative and the other will be slightly positivepositive

Polar covalent BondsPolar covalent Bonds

Water: the electrons hang around Water: the electrons hang around the oxygen atom more than the the oxygen atom more than the hydrogen atomhydrogen atom

Example of Polar Covalent Bond in Action

O

Polar Covalent BondPolar Covalent Bond

Water Water

Lewis Dot Lewis Dot

H H

Metallic BondsMetallic Bonds

Bonds between positive ions and Bonds between positive ions and free-roaming electronsfree-roaming electrons

These are flexible and are good These are flexible and are good conductors as solids (electrons conductors as solids (electrons are free to moveare free to move

ion formation an atom there are the same number of protons and electrons it is electrically neutral

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