IONSIONShttps://

www.youtube.com/watch?v=WWc3k2723IM

UNIT 1B.10UNIT 1B.10Ionic BondingIonic Bonding

https://www.youtube.com/watch?v=hiyTfhjeF_U

The Bohr Model of the AtomThe Bohr Model of the Atom

A.A. Electrons of hydrogen circle the Electrons of hydrogen circle the nucleus in orbitsnucleus in orbits

1. 1. orbitsorbits have a fixed amount of ______ have a fixed amount of ______

in the ground statein the ground state

2. 2. orbitsorbits are a fixed ________ from the are a fixed ________ from the

nucleusnucleus

3.3. orbitsorbits furthest from the nucleus have furthest from the nucleus have

the ________ energythe ________ energy

Niels Bohr Niels Bohr (1885 – 1962) Bohr Model of the Atom(1885 – 1962) Bohr Model of the Atom

Bohr’s ModelBohr’s Model

Nucleus

Electron

Orbit

Energy Levels

Bohr’s ModelBohr’s ModelIn

crea

sing

ene

rgy

Nucleus

First

Second

Third

Fourth

Fifth

}

Further away from Further away from the nucleus the nucleus means more means more ________.________.

There is no “in There is no “in between” energybetween” energy

Energy LevelsEnergy Levels

IONSIONS

An atom usually has a An atom usually has a ____________charge. That charge. That means it has the same number of _____ as means it has the same number of _____ as ________________

Remember, a proton has a positive charge and an Remember, a proton has a positive charge and an electron has a negative chargeelectron has a negative charge

ION ION – an atom that has lost or _____ one or – an atom that has lost or _____ one or more electrons and has become charged more electrons and has become charged either ______ or ________either ______ or ________

Positive IonsPositive Ions

When an atom When an atom LOSESLOSES electrons, it electrons, it becomes more becomes more __________________– Why?Why?

If you are getting rid of ______ particles If you are getting rid of ______ particles (electrons) but your number of positive (electrons) but your number of positive particles (______) are staying the same.particles (______) are staying the same.– In other words, you are subtracting negative In other words, you are subtracting negative

numbersnumbers

ExamplesExamples

What would the charge be if:What would the charge be if:

The neutral form of Gold (Au) lost 4 of its 79 The neutral form of Gold (Au) lost 4 of its 79 electrons. It now has 79 protons and electrons. It now has 79 protons and _____electrons_____electrons

The neutral form of Mg lost 2 of its 12 The neutral form of Mg lost 2 of its 12 electrons. It now has __ protons and 10 electrons. It now has __ protons and 10 electrons.electrons.

Negative IonsNegative Ions

When an atom When an atom GAINSGAINS electrons it becomes electrons it becomes more more __________________– Why?Why?

Electrons have a _______ charge, so the Electrons have a _______ charge, so the more you have, the more negative you more you have, the more negative you becomebecome

Representing IonsRepresenting Ions

Ions are represented by placing a Ions are represented by placing a “superscript” charge number next to the “superscript” charge number next to the atomic symbol.atomic symbol.

Ex. Ex. – OO-2-2 = oxygen with a negative __charge = oxygen with a negative __charge– KK++ = potassium with a ______ 1 charge = potassium with a ______ 1 charge– NN-3-3 = nitrogen with a _______ 3 charge = nitrogen with a _______ 3 charge– And so onAnd so on

Keeping Track of ElectronsKeeping Track of Electrons

2. Atoms in the same column2. Atoms in the same columna. Have the same outer _______ configuration.a. Have the same outer _______ configuration.

b. Have the same ________ electrons.b. Have the same ________ electrons.

c. Easily found by looking up the group number c. Easily found by looking up the group number on the ________ table.on the ________ table.

d. Group 2A - Be, Mg, Ca, etc.-d. Group 2A - Be, Mg, Ca, etc.-

2 ________ electrons2 ________ electrons

List the number of valence shell electrons List the number of valence shell electrons are in each of the elements in groupsare in each of the elements in groups

1-2 13-181-2 13-18

B. Electron Dot Diagrams: Lewis B. Electron Dot Diagrams: Lewis StructuresStructures

1. A way of keeping track of 1. A way of keeping track of _______ electrons._______ electrons.

2. How to write them2. How to write them3. Write the symbol.3. Write the symbol.4. Put one ___ for each valence 4. Put one ___ for each valence

electronelectron5. Don’t pair up until they have to5. Don’t pair up until they have to

X

The Electron Dot diagram for Nitrogen

Nitrogen has __ valence electrons.

First we write the symbol.

NThen add __electron at a time to each side.Until they are forced to pair up.

Write the electron dot diagram Write the electron dot diagram forfor

NaNa

MgMg

CC

OO

FF

NeNe

HeHe

C. Ion Formation in Representative C. Ion Formation in Representative ElementsElements

GroupGroup Gain or Lose Gain or Lose Charge of Ion Charge of Ion1 (1A) lose 1 +11 (1A) lose 1 +12 (2A) lose 2 +2 2 (2A) lose 2 +2 13 (3A) lose 3 +313 (3A) lose 3 +314 (4A) lose or gain 4* +4,-4*14 (4A) lose or gain 4* +4,-4*15 (5A) gain 3 -315 (5A) gain 3 -316 (6A) gain 2 -216 (6A) gain 2 -217 (7A) gain 1 -117 (7A) gain 1 -1

Electron Dots For CationsElectron Dots For Cations

Metals will have few valence electronsMetals will have few valence electrons

Ca

Electron Dots For CationsElectron Dots For Cations

Metals will have few valence electronsMetals will have few valence electrons These will come ____These will come ____

Ca

Electron Dots For CationsElectron Dots For Cations

Metals will have few valence electronsMetals will have few valence electrons These will come offThese will come off Forming _______ionsForming _______ions

Ca+2

D. Electron Configurations for D. Electron Configurations for AnionsAnions

1. Nonmetals gain _______ to attain noble 1. Nonmetals gain _______ to attain noble gas configuration.gas configuration.

2. They make ______ ions.2. They make ______ ions.

Electron Dots For AnionsElectron Dots For Anions

Nonmetals will have many Nonmetals will have many ______ .electrons.______ .electrons.

They will gain electrons to fill _____ shell.They will gain electrons to fill _____ shell.

P P-3

E. Stable Electron ConfigurationE. Stable Electron Configuration

1.All atoms react to achieve noble gas configuration.1.All atoms react to achieve noble gas configuration.

2. 8 valence electrons .2. 8 valence electrons .

3. Also called the octet rule.3. Also called the octet rule.

Ar

Write the electron Write the electron configuration diagram label as configuration diagram label as

anion or cation anion or cation NaNa MgMg PP OO FF ClCl KK

quizquiz

I. Properties of Ionic CompoundsI. Properties of Ionic Compounds

View Ionic videoView Ionic video

a. Crystalline structure.a. Crystalline structure.

b. A regular ________ arrangement of ions b. A regular ________ arrangement of ions in the solid.in the solid.

c. Structure is rigid.c. Structure is rigid.

Ionic_Bonds.asf

I. Chemical BondsI. Chemical Bonds

A. The force that holds two atoms together.A. The force that holds two atoms together. 1. Why do atoms form bonds?1. Why do atoms form bonds? a. to acquire ___electrons in thea. to acquire ___electrons in the valence shell (like noble gases valence shell (like noble gases

2. How do atoms form bonds? 2. How do atoms form bonds? a. atoms may lose, ____ or sharea. atoms may lose, ____ or share electrons to get 8 in the ______electrons to get 8 in the ______ shellshell

A. Chemical Bond and A. Chemical Bond and valence electron valence electron

1.The electrons responsible for the chemical 1.The electrons responsible for the chemical properties of atoms are those in the outer properties of atoms are those in the outer energy level: energy level: ____________________.____________________.

a.Valence electrons - The electrons in a.Valence electrons - The electrons in the outer _______ level.the outer _______ level.

b.Inner electrons -those in the energy b.Inner electrons -those in the energy _______ below. _______ below.

II. Ionic BondingII. Ionic Bonding

A. Anions and cations are held together by A. Anions and cations are held together by _________ charges._________ charges.

B. Ionic _________ are called salts.B. Ionic _________ are called salts.

C. Simplest ratio is called the formula unit.C. Simplest ratio is called the formula unit.

D.The bond is formed through the transfer of D.The bond is formed through the transfer of __________.__________.

E. Electrons are transferred to achieve _____ E. Electrons are transferred to achieve _____ gas configuration.gas configuration.

II.II. Formation and Nature of Ionic BondsFormation and Nature of Ionic Bonds

FF. 1. atom “M” loses electron(s) . 1. atom “M” loses electron(s) ____________

2. atom “N” gains electron(s) 2. atom “N” gains electron(s) anionanion

3. cation and ______ attract each other3. cation and ______ attract each other

a. electrostatic attractiona. electrostatic attraction

4. the 4. the electrostatic forceelectrostatic force that holds the that holds the

oppositely charged ____ together isoppositely charged ____ together is

the ______ bondthe ______ bond

Sodium loses an electron forming a (+) ion. Sodium loses an electron forming a (+) ion. Chlorine gains an electron forming a ( - ) ion.Chlorine gains an electron forming a ( - ) ion.

________ attraction between the (-) and (+) ion forms ________ attraction between the (-) and (+) ion forms the ______bond between sodium and chlorinethe ______bond between sodium and chlorine

B. Ionic CompoundsB. Ionic Compounds 1. compounds containing ______ bonds1. compounds containing ______ bonds 2. types of ionic compounds2. types of ionic compounds a. a. oxidesoxides – metal + ________– metal + ________

NaNa22O, CaO, AlO, CaO, Al22OO33, Fe, Fe22OO33

b. b. salt salt – metal + _________– metal + _________ NaCl CaF AgCl KINaCl CaF AgCl KI c. c. binary compoundsbinary compounds – two elements – two elements 1)all of the compounds in a and b 1)all of the compounds in a and b

are binary compoundsare binary compounds

D. D. monoatomicmonoatomic ionion - ____atom - ____atom

1) ex. K1) ex. K+ + FeFe3+3+ O O2-2- N N3- 3-

EE. . polyatomic ionpolyatomic ion – ion with more than – ion with more than

one atom that acts as a _____ ionone atom that acts as a _____ ion

NONO33-- OH OH-- SO SO44

2-2- NH NH44++

III. Names and FormulasIII. Names and FormulasA.A. Formulas for Ionic CompoundsFormulas for Ionic Compounds 1. vocabulary 1. vocabulary a. a. formula unitformula unit – simplest _____ of – simplest _____ of ions in a compound ions in a compound

1) ex. NaCl MgBr1) ex. NaCl MgBr22 AlCl AlCl33

b.b. monoatomicmonoatomic ion - ___ atomion - ___ atom 1) ex. K1) ex. K+ + FeFe3+3+ O O2-2- N N3- 3-

BB. . Formulas For Ionic CompoundsFormulas For Ionic Compounds 1. write formula for the 1. write formula for the ____________ first, then first, then the the ____________ 2. use 2. use ________________ to indicate number of to indicate number of ions (criss-cross the charges)ions (criss-cross the charges) a. sum of charges should equal 0a. sum of charges should equal 0 b. never change subscripts inb. never change subscripts in ____________________

Sodium Chloride CrystalSodium Chloride Crystal

Ionic BondingIonic Bonding

Na Cl

Ionic Bonding: Lewis StructureIonic Bonding: Lewis Structure

Na+ Cl -

Ionic BondingIonic Bonding

All the electrons must be accounted for!All the electrons must be accounted for!

Ca P

Ionic BondingIonic Bonding

Ca P

Ionic BondingIonic Bonding

Ca+2 P

Ionic Bonding

Ca+2 P

Ca

Ionic Bonding

Ca+2 P-3

Ca

Ionic Bonding

Ca+2 P-3

Ca P

Ionic Bonding

Ca+2 P-3

Ca+2 P

Ionic Bonding

Ca+2 P-3

Ca+2 P

Ca

Ionic Bonding

Ca+2 P-3

Ca+2 P

Ca

Ionic Bonding

Ca+2 P-3

Ca+2P

-3

Ca+2

Ionic Bonding

Ca3P2

Formula Unit

Ionic_Bonds.asf

ShortcutShortcut

CaCa+2 +2 PP-3-3

CaCa33PP22

Crisscross the charges to become Crisscross the charges to become the subscript!!!!!!!!!!!!!!!!!!!!!!!!!the subscript!!!!!!!!!!!!!!!!!!!!!!!!!

I. Properties of Ionic CompoundsI. Properties of Ionic Compounds

a. Crystalline structure.a. Crystalline structure.

b. A regular repeating arrangement of b. A regular repeating arrangement of ions in the solid.ions in the solid.

c. Structure is rigid.c. Structure is rigid.

Crystalline structureCrystalline structure

Ionic CompoundsIonic Compounds

Ionic compounds Ionic compounds consist ofconsist of

a a ____________

of positiveof positive

and _______ ions.and _______ ions.

Lattice: three Lattice: three dimensional array of dimensional array of ____________

NaCl:

Ionic propertiesIonic properties

d. Ions are strongly bonded- because of d. Ions are strongly bonded- because of strong forces between ions they havestrong forces between ions they have

1.______melting points1.______melting points 2. high _______ point2. high _______ point

3. high hardness _______3. high hardness _______4. very ______4. very ______5. _______ brittle5. _______ brittle

Ionic solids are brittleIonic solids are brittle

+ - + -+- +-

+ - + -+- +-

Ionic solids are brittleIonic solids are brittle

+ - + -

+- +-+ - + -

+- +-

Strong Repulsion breaks crystal apart.Strong Repulsion breaks crystal apart.

E. ConductivityE. Conductivity

1.Conducting electricity is allowing charges 1.Conducting electricity is allowing charges to move.to move.

2.In a solid, the ions are locked in place.2.In a solid, the ions are locked in place.3. Ionic solids are insulators.3. Ionic solids are insulators.4. When melted, the ions can move around.4. When melted, the ions can move around.5. Melted ionic compounds conduct.5. Melted ionic compounds conduct.6. First get them to 800ºC.6. First get them to 800ºC.7. ELECTROLYTE-Dissolved in water they 7. ELECTROLYTE-Dissolved in water they

conduct. (aqueous solution)conduct. (aqueous solution)

Building Ionic CompoundsBuilding Ionic Compounds

Binary compound - metallic cation bonded to nonmetallic anion 1. Oxide- When a metal is ionically bonded to

OxygenSalt - Metal + Non-metal

Polyatomic IonsPolyatomic Ions

An ion made up of two or more atoms bonded An ion made up of two or more atoms bonded together that acts as a single unit with a net together that acts as a single unit with a net charge.charge.

Build with tabs NHBuild with tabs NH4 ,4 ,OH, Write the polyatomic ion OH, Write the polyatomic ion

and the charge it has.and the charge it has.

Na(OH)- a balance compoundNa(OH)- a balance compound

MgMg+2+2(OH(OH) –1) –1

Mg(0H)Mg(0H)2 2 a balanced compounda balanced compound

ACTIVITY:

MAKE TAB CUTOUTS OF THE VALENCE SHELL OF AL, O, Na, Cl, Mg, Ca

Bond Al O Mg O Na Cl

Build just one formula unit- remember it doesn’t exist as Build just one formula unit- remember it doesn’t exist as oneone i in nature – it is a crystal of many formula units where each – is surrounded by a +

ActivityActivity

Demo- Burn to Create Mg+O=MgODemo- Burn to Create Mg+O=MgO Check the conductivity of:Check the conductivity of: 1. NaCl- solid1. NaCl- solid 2. NaCl-aqueous solution2. NaCl-aqueous solution 3. Distilled water3. Distilled water 4. Tap4. Tap 5. MgO-solid5. MgO-solid 6. MgO-aqueous solution6. MgO-aqueous solution 7. use magnifying glass to view NaCl7. use magnifying glass to view NaCl

I. Metallic BondsI. Metallic Bonds

How atoms are held together in the solid How atoms are held together in the solid form.form.

Metals hold onto their _______ electrons Metals hold onto their _______ electrons very weakly.very weakly.

Think of them as _______ ions floating in a Think of them as _______ ions floating in a sea of electrons.sea of electrons.

http://www.youtube.com/watch?v=c4udBSZfLHY

Sea of ElectronsSea of Electrons

+ + + ++ + + +

+ + + +

Electrons are ______to move through the Electrons are ______to move through the solid.solid.

Metals ________electricity.Metals ________electricity.

Metals are MalleableMetals are Malleable

__________ into shape (bend).__________ into shape (bend). ________ - drawn into wires.________ - drawn into wires.

MalleableMalleable

+ + + ++ + + +

+ + + +

MalleableMalleable

+ + + +

+ + + ++ + + +

_________allow atoms to _______ by._________allow atoms to _______ by.

VideoVideo

http://www.youtube.com/watch?v=Bjf9gMDP47s

ALLOYSALLOYS

Alloys are Alloys are ______________________made by made by dissolving metals in other metals. They dissolving metals in other metals. They are prepared by melting the metals are prepared by melting the metals together and cooling the mixture.together and cooling the mixture.

The properties of alloys differ from those The properties of alloys differ from those of their component metals. For example of their component metals. For example ________________________, an alloy of iron, carbon, , an alloy of iron, carbon, chromium and nickel is stronger than iron chromium and nickel is stronger than iron and more resistant to corrosion. and more resistant to corrosion.

Name of Alloy CompositionName of Alloy Composition

________________________________________________________________________________

Sterling silver silver, copperSterling silver silver, copper

Brass copper, zinc, tinBrass copper, zinc, tin

Cast iron iron, carbonCast iron iron, carbon

Steel iron, carbonSteel iron, carbon

Stainless steel iron, chromium, carbon, nickleStainless steel iron, chromium, carbon, nickle

18 Carat gold gold, silver, copper18 Carat gold gold, silver, copper

Pewter tin, copper, bismuth, antimonyPewter tin, copper, bismuth, antimony

Plumber’s solder lead, tin Plumber’s solder lead, tin

ALLOYALLOY

A combination of 2 metalsA combination of 2 metals

IV.IV. Metallic Bonds – Properties of MetalsMetallic Bonds – Properties of MetalsA.A. Metallic BondsMetallic Bonds

1. valence electrons are 1. valence electrons are __________________ a. free to move from atom to atoma. free to move from atom to atom 2. bond is formed by the attraction of2. bond is formed by the attraction of metal cations for the moving electronsmetal cations for the moving electrons 3. 3. ____________________________”” –atoms of –atoms of metals contribute a “sea” of free metals contribute a “sea” of free moving electrons that move from one moving electrons that move from one atom to anotheratom to another

Electron Sea Model for Metallic BondsElectron Sea Model for Metallic Bonds

Positive Ions Surrounded by Delocalized ElectronsPositive Ions Surrounded by Delocalized Electrons

B.B. Properties of MetalsProperties of Metals 1. moderately high melting points1. moderately high melting points 2. high boiling points2. high boiling points 3. 3. ______________________ a. can be hammered into sheetsa. can be hammered into sheets 4. 4. ______________________ a. can be drawn into wirea. can be drawn into wire 5. good conductors of heat and electricity5. good conductors of heat and electricity 6. 6. __________________ (good reflectors of light)(good reflectors of light) 7. hardness and strength varies7. hardness and strength varies a. greater in transition elementsa. greater in transition elements

C. AlloysC. Alloys

1. mixture of two or more elements with1. mixture of two or more elements with

metallic propertiesmetallic properties

2. types2. types

a. a. substitutionalsubstitutional – atoms of similar– atoms of similar

size (sterling silver, brass, pewter)size (sterling silver, brass, pewter)

b. b. interstitialinterstitial – small holes in the – small holes in the

crystal filled with smaller atomscrystal filled with smaller atoms

(carbon steel) (carbon steel)