chemical bonding: part 1 - ionic

Chemical Bonding: PART 1

- IONICYou know you LOVE notes because they

help you learn!

Chemical bonding is the way atoms are attracted to each other to form compounds.

Chemical bonding determines nearly all of the chemical

properties we see in life. And as we know, the number “8” is

very important to chemical bonding!

8

Bonding Basics• All atoms want to have a

FULL outer energy level – just like the Noble Gases – because this means stability!

• Atoms want 8 valence electrons (except H & He who want 2 because 2 electrons mean FULL)

Compound• a pure substance formed

by two or more elementsExamples: FeO2 – Rust HCl – An acid found in your

stomach CH4 – A gas produced in your

body (methane) CO2 – Soda pop bubbles

(carbon dioxide)


by two or more elementsExamples: NH3 – You’ll know this when you smell it

(ammonia) C12H22O11 – It will make your life sweeter

(table sugar) NaHCO3 – Something you’ll need to

make good cakes and cookies (baking soda)

C8H10N4O2 – This will give you some pep! (caffeine)


by two or more elementsExamples: CO – A dangerous gas (carbon

monoxide) H2SO4 – Acid found in car batteries CaCO3 – Used to write on a

blackboard (calcium carbonate)

H2O2 – Used to disinfect wounds (hydrogen

peroxide)

Valence Electrons

• How many valence electrons?

• What group number?

• What family?

All in the Family…• Group 1: Alkali Metals• Group 2: Alkaline Earth Metals• Groups 3-12: Transition Metals• Group 13: Boron Group• Group 14: Carbon Group• Group 15: Nitrogen Group• Group 16: Oxygen Group• Group 17: Halogens• Group 18: Noble Gases

Electron Dot Diagrams…

Mg B

O

H

Cl

NC

Ne

Ionic Bonding• In an Ionic Bond,

electrons are lost or gained in order to reach a FULL outer energy level which results in the formation of Ions

• METAL elements LOSE electrons to form positive ions: cations

• It is easier to lose 1-2 electrons than gain 6-7

• Groups 1,2,13

Positive Ions

Group 1

Group 2

Group 13

• NON-METAL elements GAIN electrons to become negative ions: anions

• It is easier to gain 1-2 electrons than lose 6-7

• Groups 15,16,17

Negative Ions

Na + Cl Na+ + Cl-

NaCl

1. Metal + Non-metal (Metal always listed

first)2. Opposite charges must

balance

3. + and - charges hold ions together

How to Ionic Bond…

Opposites Attract!

Becoming Potassium Fluoride:

FK

FK


• The ionic bond is the attraction between the ________ ion (K+) and the ________ ion (F-)

F _K+

POSITIVENEGATIVE


Positive Ions

NEXT SLIDE

ADVANCED

STUDENTS ONLY

Electromagnetic Attraction

The + and – ions have

an electromagn

etic attraction (similar to

static electricity).

Electron Dot Diagram for Positive Ions (EDD

for + Ions)1. Metals have few valence

electrons

Mg

1. Metals have few valence electrons


for + Ions)

Mg

2. Electrons are given away

1. Metals have few valence electrons


for + Ions)

2. Electrons are given away3. Positive Ions are formed

Mg2+

Examples of Positive Ions :

Mg

Li Li+

Mg+2

Group 1

Group 2

Al Al+3Group 13

Electron Dot Diagram for Negative Ions (EDD

for - Ions)1. Non-Metals have more

valence electrons

P



valence electrons2. Electrons are gained to fill

outer energy shell

PP



valence electrons2. Electrons are gained to fill

outer energy shell3. Negative Ions are formed

P -3

Examples of Negative Ions :

S

N N-3

S-2

Group 15

Group 16

I I-Group 17

What about group 18?

They rarely bond because they are

already happy and stable with 8

valence electrons!

Putting Ions Together1 to 1 ratios:1. Groups 1 & 17 (Alkali

Metals & Halogens)

Na+ + Cl- NaCl

Putting Ions Together

2.Groups 2 & 16 (Alkaline-Earth Metals & Oxygen Family)Ca+2 + O-2 CaO

Putting Ions Together2 to 1 ratios:1. Groups 1 & 16 (Alkali

Metals & Oxygen Family)

2. Groups 2 & 17 (Alkaline-Earth Metals & Halogens)

Na+ + O-2

Ca+2 + Cl-

Na2O

CaCl2


AlI3

MgF2

KCl

LiBr

Mg+2 + F-

Al+3 + I-

K+ + Cl-

Li+ + Br-

Potassium + Chlorine Potassium Chloride

Lithium + Bromine Lithium Bromide

Magnesium + Fluorine Magnesium Fluoride

Aluminum + Iodine Aluminum Iodide


Na2O

CaCl2

CaO

NaCl

Ca+2 + Cl-

Na+ + O-2

Ca+2 + O-2

Na+ + Cl-

Calcium + Oxygen Calcium Oxide

Sodium + Chlorine Sodium Chloride

Calcium + Chlorine Calcium Chloride

Sodium + Oxygen Sodium Oxide

SnF2Na+2 + F-


Sodium + Fluorine Tin Fluoride

FINAL SLIDES

ADVANCED

STUDENTS ONLY

Electron Energy

• The energy level relates to the amount of energy electrons have within the atom.

What are the characteristics of electrons closer to the nucleus??Farther away??How does that affect bonding??

Electron Energy

Electron EnergyElectrons FARTHEST

from Nucleus

Electrons

CLOSEST to

Nucleus


from Nucleus

Electrons

CLOSEST to

NucleusPull on

electrons by positive nucleus


from Nucleus

Electrons

CLOSEST to

NucleusPull on


LESS


from Nucleus

Electrons

CLOSEST to

NucleusPull on


LESS MORE


from Nucleus

Electrons

CLOSEST to

NucleusPull on


LESS MORE

Ability to remove

electrons


from Nucleus

Electrons

CLOSEST to

NucleusPull on


LESS MORE

Ability to remove

electronsEASIER


from Nucleus

Electrons

CLOSEST to

NucleusPull on


LESS MORE

Ability to remove

electronsEASIER HARDER


from Nucleus

Electrons

CLOSEST to

NucleusPull on


LESS MORE

Ability to remove


Amount of electron energy

available for bonding


from Nucleus

Electrons

CLOSEST to

NucleusPull on


LESS MORE

Ability to remove




MORE


from Nucleus

Electrons

CLOSEST to

NucleusPull on


LESS MORE

Ability to remove




MORE LESS

BONDING REACTIVITYMETALS NONMETALS

• More reactive with MORE energy levels

because WEAKER force pulling electrons into

the nucleus• More reactive the

LOWER the element is in the group

• Group 1 MORE reactive than Group 2 because it is easier to

remove 1 electron than 2

• More reactive with FEWER energy levels because STRONGER

force pulling electrons into the nucleus

• More reactive the HIGHER the element is

in the group• Group 17 MORE

reactive than Group 16 because it is easier to gain 1 electron than 2

Electron Energy

Quote of the Day:“Equipped with his five

senses, man explores the universe around him and calls

the adventure Science.” ~Edwin Powell Hubble,

The Nature of Science, 1954

And Remember

:

Name (first AND last)Date

Period

chemical bonding: part 1 - ionic

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