FORMING

Day 1 - ionic

THE ATOM

▪Protons (+)

▪Neutrons (0)

▪Electrons (-)▪Notice the size

VALENCE ELECTRONS

(ELECTRONS ON THE OUTER LAST “SHELL” RING)

WHY ARE VALENCE ELECTRONS IMPORTANT?

•They determine a majority of the reactions that

we see in daily life

• Atoms will steal or share valence electrons to

have a full valence shell like a noble gas ( “stable”

and “unreactive”)

•Octet rule (Full valence shell): atoms would like

to have 8 valence electrons to become stable

DO YOU GET IT?

Using your periodic table, find out how many valence electrons each of the following has:

Element Group NumberValence Electron

Number

How many e- to be

stable

(full valence shell) ?

Magnesium (Mg)

Silicon (Si)

Chlorine (Cl) 17 7 1

Iodine (I)

Calcium (Ca)

FUNDAMENTALS OF CHEMICAL BONDING• What is a chemical bond?

attraction between atoms that allows for the formation of compounds

WHAT ARE IONS?

A charged atom that results from it losing or gaining an electron

Once the electron is lost / gained (respectively), these atoms become IONS

CATION

+

(lose)

ANION

-

(gain)

WHAT ARE IONS?

A charged atom that results from it losing or gaining an electron

❑Elements in groups 1, 2, and 3 will form cations (lose

electrons).

❑Elements in GROUP 4 can form both cations and

anions depending on its partner element.

❑Elements in groups 5, 6, or 7 will form anions (gain

electrons).

❑What about group 8?

OXIDATION NUMBERS

CFU: DO YOU GET IT?

ElementWhat will it form?

Cation or AnionIon Symbol

F

K

Al

N

Anion

Cation

Cation

Anion

F-

K+

Al3+

N3-

IONIC BONDING• An Ionic Bond is a chemical bond formed

when one atom gains and another loses valence electrons then bond together to become stable (have a full valence shell).

• Ionic bonds form between metals and non-metals ONLY

LEWIS DOT DIAGRAM

• Valence electrons can be easily represented through a Lewis Dot Diagram

• Model that represents only the valence shell electrons of an element.

P

EXAMPLE 1: SODIUM (Na) AND CHLORIDE (Cl)

Na Cl Na Cl NaCl

1. Lewis Dot Diagram

2. Draw electron transfer arrows3. Determine the cation and anion 4. Write out the end result

FORMING IONIC COMPOUNDS

EXAMPLE 2: ALUMINUM (Al) AND PHOSPHORUS (P)

Al + P

Forming Ionic bonds can be straightforward

Al + P Al3+ P3-

Li + O

EXAMPLE 3: LITHIUM (Li) AND OXYGEN (O)

Forming Ionic bonds may NOT be straightforward

Li + O

Oxygen’s Valence shell is not full. Any ideas

about what we could do?

Add another Lithium to the equation!

Li + O

Li

Li + O

Li

Li 1+ O2-

The #2 below an

element indicates that

you used 2 of them

Li2 O

Li 1+

FORMING

Day 2 - covalent

IONIC BONDS

Cation(s) Anion Li2 OLi +1

Li +1

O -2

(one headed arrow represents TRANSFER)

COVALENT BOND PRACTICE CO 2

• STEP 1: Draw the Lewis Dot Diagram of each element

C OO

COVALENT BOND PRACTICE CO 2

• STEP 2: Show the sharing of electrons by drawing double-headed arrows

C OO

(double headed arrow represents SHARING)

COVALENT BOND PRACTICE CO 2

• STEP 3: Draw the Lewis Dot Structure to make sure all elements satisfy

the Octet Rule (show multiple bonds if necessary)

O C OEach line represents

2 e- being shared

DIATOMIC ATOMS

Pure elements that form molecules consisting of two atoms bonded together

CFU WHICH WILL FORM AN IONIC BOND? WHICH WOULD FORM A COVALENT BOND?

What type of bonds will form:

Ionic or Covalent

Nitrogen and Oxygen

Carbon and Sulfur

Sodium and Fluorine

Lithium and Aluminum

DIOXIDE – O2

dioxide

AMMONIA - NH3

METHANE - CH4

methane

FORMING & NAMING

Type 1 & 2 IONIC

Includes: metal & non-metal

Naming Rules:

1. The metal ion's name does not change regardless of charge

2. The non-metal's name ends in -ide.

For example: AlCl3 = aluminum chloride

Na2S = sodium sulfide

K2O = potassium oxide

MgH2 = magnesium hydride

Notice how the little numbers (subscripts) do not affect the way we name them.

Ionic Type 1 (metal only has one charge)

IONIC TYPE 1: FORMULA

Here, we have to consider the common charges for calcium and phosphorus, which are +2 and -3,

respectively. Calcium, if you recall, typically loses two electrons to get a noble gas electron arrangement,

and phosphorus needs three more electrons.

Ca+2 and P-3

So the answer is Ca3P2.

• Other examples: potassium oxide : K+1 and O-2 yields K2O

aluminum bromide: Al+3 and Br-1 yields AlBr3.

Work space

If necessary!

CFU

Example Formula Name

H + Cl

Li + Br

Mg + Si

Rb + P

Mg + O

Includes: transition metal & non-metal

Naming Rules:

1. Transition metal goes first

2. Use roman numerals to specify the metals charge

3. The non-metal's name ends in ide.

For example:

• FeO → Fe + O →

• Fe2O3 → Fe + O →

• To go backwards, we need to figure out the charge of the transition metal.

• Name it by writing the metal first, its charge in roman numerals, then the non-metal with the suffix -ide

Ionic Type 2 (metal only has two charges)

2-?Iron (11) Oxide

? 2-Iron (1I1) Oxide

IONIC TYPE 2: FORMULA

If necessary!

Work space

• Iron (II) Oxide

• Iron (III) Oxide

CFU

Example Formula Name

Iron (II) Sulfide

Cobalt (II) Nitride

Tin (IV) Oxide

Manganese (II)

Sulfide

FORMING & NAMING

Covalent and polyatomic

Includes: non-metal & non-metal

Naming Rules:

1. Name the element furthest left first

2. Write the name of the second non-metal ending in -ide

3. Use prefixes to specify how many of each element

For example:

• CO – moncarbon monoxide

• CO2 – carbon dioxide

• P2O3 – ?

• The only time we drop a prefix is if the mono is to appear at the beginning of the name.

CovalentPrefix Number of atoms

mono 1

di 2

tri 3

tetra 4

penta 5

hexa 6

COVALENT: FORMULA

• Write the formula based on the name:

• Carbon tetrachloride – CCl4

• diatomic oxygen – ?

• H2O – ?

Includes: compound & non-metal OR metal

Naming Rules:

1. Name the cation first

2. Add –ide to ending of the anion

For example:

• Na2CO3

• KNO3

Polyatomic

POLYATOMIC: FORMULA

• Example:

• Ammonium sulfide

• Aluminum sulfate

If necessary!

CFU

Example Formula

Sodium Nitrate

Aluminum Phosphate

*Silicon Sulfate

Formula Name

NaNO3

Na2SO4

REVIEW

Day 5 – review for test

VALENCE ELECTRONS

WHAT ARE IONS?

A charged atom that results from it losing or gaining an electron

Once the electron is lost / gained (respectively), these atoms become IONS

CFU!

Sodium (Na) becomes ……

CFU!

Fluorine (F) becomes ……

WHAT ARE IONS?

A charged atom that results from it losing or gaining an electron

IONIC VS COVALENT

CFU: DO YOU GET IT?

ElementWhat will it form?

Cation or AnionIon Symbol

F

K

Al

N

Anion

Cation

Cation

Anion

F-

K+

Al3+

N3-

FORMING IONIC COMPOUNDS

Al + P Al3+ P3-

Li + O

Li

Li 1+ O2-

The #2 below an

element indicates that

you used 2 of them

Li 1+

Li2 O

Al P

FORMING COVALENT COMPOUNDS

C OO

CO2

WRITING NAMES

1. Is it polyatomic or ?

3 or

more

elements1 or 2

element

s

Name the cation first (+)

Name the anion after (-)

4 MG(OH)2MgCl2

1. Is it polyatomic or ?

3 or

more

elements1 or 2

element

s

Name the cation first (+)

Name the anion after (-)

1) Na2CO3

2) NaOH

3) MgBr2

4) KCl

5) FeCl2

6) FeCl3

7) Zn(OH)2

8) Be2SO4

2. Is it Ionic or covalent?

Metal +

non-

metal

1) PCl3

2) MgBr2

3) BrF5

4) KCl

5) FeCl2

6) FeCl3

7) N2O3

3. Is it

Metal has

only 1

charge

EASY!

Name the metal

&

Change the non-metal ending to “ide”

Use roman numerals (I, II, III, IV) to

indicate the charge of the metal

&

Change the non-metal ending to “ide”

1) MgBr2

2) FeCl3

3) BrF5

4) KCl

5) FeCl2