If you have never heard it before write down what you

(1)

(2)

Have you ever heard the word bonding before?

If you have never heard it before write down what you

think it means?

If so, where did you hear it and what

does it mean?

(3)

Bonding is what keeps

elements and ions of

compounds together!!!

(4)

What’s the difference between an Element and a Compound?

Give an example of each and

explain why.

(5)

Elements

An element is a substance that cannot be broken down into different

substances.

It is the smallest form of matter that has the same characteristics of that substance.

Examples: Au (gold), Na (sodium) etc.

(6)

COMPOUNDS

Define what a compound is?

Two or more DIFFERENT atoms

(elements) that are chemically bonded together because of a chemical

reaction.

We use chemical formulas to

represent compounds. Can you think of any…?

H ₂ O (Wudder) CO ₂ (Carbon Dioxide)

CH ₃ COOH + NaHCO ₃ ===> CH ₃ COONa + H ₂ O + CO ₂

(7)

A Element

A Elements C Mix of

Elements

D Mixture of Compounds

E Mix of Elements/

Compounds

B Compounds

1 6 5

4

3

2

(8)

A New Language

Let’s do the Vial Lab!

(9)

We will talk about

4 TYPES OF BONDS

IONIC

COVALENT METALLIC HYDROGEN

(Ions)

(Sharing

valence electrons) (Metals)

(Ions)

(10)

IONIC BONDS

• Form between ions with opposite

charges: + and -. (a metal and a

non-metal)

• They bond because the opposite charges are attracted to

each other. (Think

magnets!!!)

(11)

IONIC BONDS

Like charges repel each other!

Ions and ionic bonds form because

electrons are

transferred from

one atom to the

other

(12)

Properties of IONIC BONDS

• Ionic compounds have high melting and boiling points.

• These are very strong bonds.

• An example is Na ⁺¹ + Cl ^-1

= NaCl (salt)

NaCl Melting point 801 °C NaCl Boiling point1465 °C

(13)

IONIC BONDS

Only certain ratios (combinations) of elements result in the formation of Ionic compounds.

For ex: Lithium (Li) will react with Fluorine (F) to form LiF.

BUT, it will NOT form LiF ₂ , LiF ₃ , etc.

Magnesium (Mg) will react with Fluorine to form MgF ₂ .

BUT, it will NOT form MgF, MgF ₃ , etc.

(14)

IONIC BONDS

• When writing a chemical formula for an ionic compound:

*The charges have to balance

to create a neutral compound.*

(15)

IONIC BONDS

• For example:

- With salt the charges are both 1: Na ⁺¹ and Cl ^-1

So we just need one of each ion to make the compound neutral

= the ratio is 1:1

= NaCl

(16)

IONIC BONDS

• What if the charges are not the same number???

- Like Li ⁺¹ + O ^-2

Here you will not have a 1:1 ratio. You

need to balance the chemical formula…

(17)

IONIC BONDS

• What could you do to get the charges to cancel out if you wanted to form this

ionic compound???

Li ⁺¹ + O ^-2

ANSWER: You would need to use 2 Li ⁺¹ for every O ^-2 !!!

= Li ₂ O

(18)

IONIC BONDS

Let’s Practice!!! Write chemical formulas for:

1.) K and N 2.) Ca and F 3.) Li and Cl 4.) Mg and Si 5.) Al and O

1.) K ₃ N 2.) CaF ₂ 3.) LiCl

4.) Mg ₂ Si

5.) Al ₂ O ₃

(19)

IONIC BONDS

6.) Ca and Cl 7.) K and P

8.) Mg and Cl 9.) Li and P 10.) K and O

6.) CaCl ₂ 7.) K ₃ P

8.) MgCl ₂

9.) Li ₃ P

10.) K ₂ O

(20)

Metal Nonmetal Chemical Formula

Compound Name

Chemical Formulas

Rb ând Cl Na ând S Li ând P

1. Hints: The metal comes first, the non-metal comes second Change the end of the name of the second element to “ide”

Copy down this table for your answers.

2. If you mix Calcium Chloride (CaCl ₂ ) into a glass of water

until it dissolves, what is the chemical formula?

(21)

Metal Nonmetal Chemical Formula

Compound Name

Chemical Formulas

Rb ând Cl Na ând S Li ând P

1. Hints: The metal comes first, the non-metal comes second Change the end of the name of the second element to “ide”

2. If you mix Calcium Chloride (CaCl ₂ ) into a glass of water until it dissolves, what is the chemical formula?

Rb

Sodium Sulfide

Cl

Na S

Li P

RbCl Na ₂ S Li ₃ P

Rubidium Chloride Lithium Phosphide

CaCl ₂ (aq)

+1 -1

+1 -2

+1 -3

(22)

Ionic Bonds Practice

Write the chemical formulas for the compounds formed when these ions bond:

11.) Al & S 12.) Rb & O 13.) Be & F 14.) Al & Cl 15.) Ca & N 16.) Ga & Se

13.) BeF ₂ 11.) Al ₂ S ₃ 12.) Rb ₂ O

14.) AlCl ₃

15.) Ca ₃ N ₂

16.) Ga ₂ Se ₃

(23)

Questions

Without using your notes, answer the following questions.

Write the questions!

1. What is a compound?

Two or more DIFFERENT atoms (elements) that are chemically bonded together because of a chemical reaction.

2. Which formula is a compound and why?

C ₈ H ₁₀ N ₄ O ₂ or F ₂ C ₈ H ₁₀ N ₄ O ₂₌ compound

3. What are the element(s) that make up each chemical formula in question 2? How many are in each element?

8 Carbon, 10 Hydrogen, 4 Nitrogen, 2 Oxygen

2 Fluorine

(24)

COVALENT BONDS

• Form between two non-metals

• They bond because the outer electron rings

are not full so they share valence

electrons!

• (The atoms are NOT

stable.)

(25)

Properties of

COVALENT BONDS

• Covalent compounds will have low melting and boiling points.

• These are usually weak bonds.

• Some examples are H ₂ O (water/ wudder),

and CO ₂ (Carbon Dioxide)

(26)

COVALENT BONDS

• The reason H ₂ O is covalent:

Remember H can be a metal or a non-metal!!!

Here H is behaving like a non-metal.

Hydrogen is usually a non-metal!

(27)

Let’s Practice!

Write the following compounds and determine if they are Ionic or Covalent?

1.) NH ₃ 7.) AlCl ₃ 2.) NaCl 8.) P ₂ O ₅ 3.) CH ₄ 9.) Li ₃ P 4.) CO ₂ 10.) BN 5.) CaCl ₂ 11.) N ₂ O

6.) KBr 12.) MgS

(28)

ANSWERS ^…

1.) NH ₃ Covalent

2.) NaCl Ionic

3.) CH ₄ Covalent

4.) CO ₂ Covalent

5.) CaCl ₂ Ionic 6.) KBr Ionic

7.) AlCl ₃ Ionic

8.) P ₂ O ₅ Covalent 9.) Li ₃ P Ionic

10.) BN Covalent

11.) N ₂ O Covalent

12.) MgS Ionic

(29)

Lewis Structures

Electron Dot Diagrams

• We can show how the atoms share or transfer electrons by drawing electron dot diagrams.

• You will only use the valence e- for

dot diagrams.

(30)

Dot Diagrams

• Start the dot diagram by writing the atomic symbol for the atom.

Ex: Mg

The symbol has 4 sides…

(31)

Dot Diagrams

Each side can hold up to 2e-

You cannot pair the electrons until

there is one on each side.

(32)

Dot Diagrams

Mg

Mg only has 2 valence e-.

So it’s dot diagram looks like this:

Mg

Let’s try… Si

how about… S

(33)

Dot Diagrams Practice!!!

Draw the Dot Diagrams for:

1.) Cl

2.) Al

3.) Na

4.) Sn

5.) Ar

(34)

Dot Diagrams

Now we can put individual diagrams together to show whether atoms

transfer or share their valence e-!!!

Who donates their electrons, metals or non-metals?

Metals always donate their electrons!

(35)

Dot Diagrams for Ionic Bonds

In an Ionic Bond, atoms are transferring their valence e- …

To show this “transferring” , we draw arrows between the Atomic Symbols to represent the transferring of e-.

We can show this w/ dot diagrams.

For Ex: (Li + Cl = LiCl) Cl

Li

(36)

Dot Diagram Practice for Ionic Bonds

1. BeO 2. NaCl 3. MgS 4. CaCl ₂ 5. LiP

6. AlCl

(37)

Dot Diagram Practice for Ionic Bonds

2. NaCl

3. MgS

(38)

Dot Diagram Practice for Ionic Bonds

5. LiP

6. AlCl

(39)

Dot Diagrams for Covalent Bonds

In a Covalent Bond, atoms are sharing their valence e- …

To show this “sharing”, we draw a BAR

between the Atomic Symbols to represent the sharing of e-.

One bar = 2 e-.

For Ex: H ₂ O

(40)

Dot Diagrams for Covalent Bonds

One bar = 2 e-.

For Ex: H ₂ O (draw out the individual dot diagrams first.)

H O H

***H’s ALWAYS have to go on the ENDS.

(41)

(42)

Dot Diagram Practice for Covalent Bonds

1. CO

2. CH

3. SO

4. NH

5. SiO

6. CF

(43)

(44)

Bonding Dot Diagram Steps

1 .) Identify the type of bond you have.

(Covalent or Ionic)

2.) Separate the individual elements and put

them in a line. Put the atomic symbol w/ least amount of valance electrons in CENTER!!!

3.) Except the Hydrogen’s!!!! Remember H’s have to be on ENDS!!!

4.) Draw the “dots” for each atomic symbol.

(45)

Bonding Dot Diagram Steps

5.) Show either the transferring or sharing of e- with arrows or bars.

6.) If sharing (covalent bonds)…connect the “lonely” dots between DIFFERENT symbols!!!

7.) Count the e- around each atomic symbol to make sure there are 8!!!

(ONLY 2 for H!)

(46)

1234 HONC

Based on your prior knowledge of atoms and their valance electrons, what in the world does

1234 HONC mean?

Hydrogen, Oxygen, Nitrogen, Carbon Based on their valance electrons, how many atoms can bond to each of them?

1 2 3 4 H O N C

H= can form one bond.

O= can form two bonds.

N= can form three bonds.

C= can form four bonds.

This works for COVALENT bonds only

(47)

Dot Diagram Practice

1.) NF ₃ 2.) Sr ₃ N ₂

(48)

Dot Diagram Practice

1.) NF ₃ 2.) Sr ₃ N ₂

3.) Rb ₂ O

4.) CH ₃ Cl

5.) Al ₂ S ₃

6.) Na ₃ N

(49)

Dot Diagram Practice

3.) Rb ₂ O 4.) CH ₃ Cl

(50)

Dot Diagram Practice

5.) Al ₂ S ₃ 6.) Na ₃ N

(51)

Dot Diagram Practice

7.) CH ₃ Br

8.) NH ₂ Cl

9.) PCl ₃

10.) CH ₄

11.) Br ₂ O

12. IBr

(52)

Dot Diagram Practice

7.) CH ₃ Br 8.) NH ₂ Cl

(53)

Dot Diagram Practice

9.) PCl ₃ 10.) CH ₄

(54)

Dot Diagram Practice

11.) Br ₂ O 12. IBr

(55)

Quick Quiz

Covalent bonds form because…

A. They share valence electrons

B. Like charges attract C. They gain neutrons

D. Opposite charges attract

E. They share protons

(56)

The compound C ₆ H ₁₂ O ₆ has

A. Ionic bonds

B. Covalent bonds C. Nuclear bonds D. Metallic bonds

E. Hydrogen bonds

(57)

Covalent bonds mostly occur with atoms on the right side of the

periodic table.

A. True

B. False

(58)

Ionic bonds have…

A. Strong bonds, low boiling and melting points

B. Weak bonds, low boiling and melting points

C. Strong bonds, high boiling and melting points

D. Weak bonds, low boiling

points and high melting

points

(59)

Ionic bonds are formed because

A. Opposite charges attract B. Share valence electrons C. Electrons are transferred D. Protons are transferred

E. Both A & C

F. Both C & D

(60)

Which compound has ionic bonds? *

A. CO ₂

B. CuSO ₄ C. O ₂

D. CH ₄

(61)

The Law of Conservation of Mass

states that in a chemical reaction, mass cannot be created or destroyed, but it can change forms!

So this means that the mass before the

reaction has to be the same as the mass

after the reaction.

(62)

6CO ₂ + 6H ₂ O C ₆ H ₁₂ O ₆ + 6O ₂

Does this equation go against the Law of Conservation of Mass?

(count the atoms of each element)

Photosynthesis

Reactants Chemical Products

Reaction

(63)

6CO ₂ + 6H ₂ O C ₆ H ₁₂ O ₆ + 6O ₂

Now, Does this equation go against the Law of Conservation of Mass?

6C

12 O 12 H 6 O

6C

12 H 6 O 12 O

This does not violate the Law of Conservation of Mass

(64)

Balancing Equations

Due to the Law of Conservation of Mass each type of element needs the same amount before the reaction and after the reaction.

“reactant(s) = product(s)”

But, you can’t change the elements that

participate in the reaction, so you must write a number in front of (to the left of) each material in the reaction to make sure every type of

element has the same number on each side of

the reaction.

(65)

How molecules are symbolized

Cl ₂ 2Cl 2Cl ₂

Cl Cl Cl Cl Cl Cl Cl Cl

How is the middle picture

different from the other two?

(66)

Balancing Equations

CaCl ₂ Subscript

The little two tells you that there are 2 Cl. It only applies to the Cl.

But… 2CaCl ₂

When you have a Coefficient 2CaCl ₂ CaCl ₂

+CaCl ₂

The 2 tells you that there are 2Ca and 4Cl

It applies to everything behind it in the compound.

You will NEVER add a subscript

only Coefficients!

(67)

Understanding

Chemical Compounds

How many atoms are in each chemical compound?

C ₆ H ₁₂ O ₆ 2H ₂ O ₂ 6CuNO ₃

6 C

4 H 4 O

6 O 12 H

6 Cu 6 N 18 O

(68)

Understanding Chemical Compounds

How many atoms are in each chemical compound?

C ₂₀ H ₃₀ O ₂ 3C ₆ H ₁₂ S ₂ 2K ₃ PO ₄

2C ₃ H ₇ NO ₂ 2Al ₂ S ₃

4KClO ₃

20 C

4 O 2 N

6 C 14 H

6 S 4 Al

12 O 4 K 4 Cl

6 K

2 O 30 H

2 P

18 C 36 H 6 S

8 O

(69)

RFA 23

CaCl ₂ C ₆ H ₁₂ O ₆

H ₂ SO ₄ NH ₄ Cl 2NH ₄ NO ₃

3BaTiO ₃

Ca 2 Cl

6 C 12 H 6 O

2 H S 4 O

N 4 H Cl

2 N 6 O 8 H

2 N

9 0

3 Ba 3 Ti

(70)

4NaHCO ₃ 8Bi ₂ Te ₃ 5CaCrO ₄ 3SiH ₂ Cl ₂

6Fe ₂ O ₃ 5NaOH

16 Bi

20 0 24 Te

5 Cr 5 Ca

6 Cl 6 H

3 Si

18 O 12 Fe

5 H 5 O

5 Na

4 Na 4 H 4 C 12 O

(71)

(72)

Bonding

What is the chemical formula for each one and WHY?

1.) 2.) 3.)

1.) 3Na ₂ (3 pairs chemically bonded) 2.) Na ₂ (1 pair chemically bonded) 3.) 2Na (not chemically bonded)

N a

N a N

a N

a

N a N

a

N a

N

a

(73)

Balancing Equations

What’s the difference between…

A ₂ + B ₂ and A ₂ B ₂ ?

A ₂ + B ₂ = Not chemically bonded, so its not a compound! These are elements.

A ₂ B ₂ = This is chemically bonded because

it is a compound.

(74)

Balancing Equations

Let’s look at an example:

Element Mg will bond with element O in the chemical reaction below:

Mg + O ₂ MgO

Are there the same amount of O’s on the left as there are on the right???

NO!!! We must balance this equation!!!

O

Mg + O → Mg O

(75)

Balancing Equations

How can we make there be the same # of each element on both sides???

Mg + O ₂ → MgO

“reactants = product”

By putting a coefficient in FRONT...

Mg + O ₂ → 2MgO

You multiply all of the elements in the compound by the coefficient in front.

Is it balanced yet???

NO!

O

Mg + O → Mg O

(76)

Balancing Equations

Where else could we put a coefficient to balance it?

Mg + O ₂ → 2MgO

“reactants = product”

We need to add a coefficient in the front on the other side…

2Mg + O ₂ → 2MgO

“reactants = product”

There are 2Mg’s and 2 O’s on the left AND there are 2Mg’s and 2 O’s on the right…NOW it’s

BALANCED!!! ☺

(77)

Balancing Equations

2Mg + O ₂ → 2MgO

I only added Coefficients!

So let’s practice with some real problems to see how you do!

Reactants = product

(78)

Balancing Equations Let’s practice…

1.) Al + Br ₂ AlBr ₃ 2.) H ₂ + O ₂ H ₂ O 3.) Na + Cl ₂ NaCl

3.) 2Na + Cl ₂ 2NaCl 4.) Fe + O ₂ Fe ₂ O ₃

4.) 4Fe + 3O ₂ 2Fe ₂ O ₃ 5.) P ₄ + O ₂ P ₂ O ₅

5.) P ₄ + 5O ₂ 2P ₂ O ₅

(79)

Balancing Equations…

6.) N ₂ + H ₂ NH ₃

7.) Mg + O ₂ MgO

8.) H ₂ + Cl ₂ HCl

9.) Ag + S Ag ₂ S

10.) S + O ₂ SO ₄

(80)

Balancing Equations…

Lets see how you did!

6.) N ₂ + 3H ₂ 2NH ₃

6a.) 2N ₂ + 6H ₂ 4NH ₃ Is this balanced?

7.) 2Mg + O ₂ 2MgO 8.) H ₂ + Cl ₂ 2HCl

9.) 2Ag + S Ag ₂ S

10.) S + 2O ₂ SO ₄

(81)

Explain what are three differences between a Covalent bond and an Ionic Bond?

Covalent Bonds

1. Share valence electrons 2. Non-metal and Non-metal

3. Weak bonds

4. Low Boiling Pts. and Melting pts.

Ionic Bonds

1. Opposite charges attract 2. Metal and Non-metal

3. Strong bonds

4. High Boiling Pts. and Melting pts.

Try this without using your notes

(82)

Metallic Bonds

• Form between 2 metal atoms. (metal and metal)

• The atoms are unstable – they do not have full electron rings.

• Bond by sharing very loosely held valence

electrons with each other. (The electrons “flow”

between the atoms.)

• Metallic bonds are NOT the strongest bonds though…

• Ionic Bonds are the strongest bonds!

(83)

Properties of Metallic Bonds

• Metallic compounds are highly

conductive. (They conduct heat &

electricity very easily!!!)

• They also have metallic luster (shine)

• They are malleable (able to be hammered into thin sheets.)

• They are ductile (can be rolled into wires.)

• Examples: CuZn, AlSb, GaSb, LaMg

(84)

What makes it easier for some atoms to bond better than other atoms?

When you think about atoms bonding, what do atoms need to gain or lose?

VALENCE ELECTRONS!!!

N ^-3 Li ⁺¹

Which atom will bond the easiest?

Li ⁺¹ Why?

The LESS electrons an atom needs to

gain or lose to have a full outer ring, the

EASIER it is for that atom to bond!!!

(85)

Which groups (1-18) on the periodic

table, will bond the easiest?

(86)

Which groups on the periodic table will share or transfer electrons the easiest?

If you have never heard it before write down what you

Have you ever heard the word bonding before?

If you have never heard it before write down what you

think it means?

If so, where did you hear it and what

does it mean?

Bonding is what keeps

elements and ions of

compounds together!!!

What’s the difference between an Element and a Compound?

Give an example of each and

explain why.

Elements

An element is a substance that cannot be broken down into different

substances.

It is the smallest form of matter that has the same characteristics of that substance.

Examples: Au (gold), Na (sodium) etc.

COMPOUNDS

Define what a compound is?

Two or more DIFFERENT atoms

(elements) that are chemically bonded together because of a chemical

reaction.

We use chemical formulas to

represent compounds. Can you think of any…?

H 2 O (Wudder) CO 2 (Carbon Dioxide)

CH 3 COOH + NaHCO 3 ===> CH 3 COONa + H 2 O + CO 2

A Element

A Elements C Mix of

Elements

D Mixture of Compounds

E Mix of Elements/

Compounds

B Compounds

1

6 5

4

3

2

A New Language

Let’s do the Vial Lab!

We will talk about

4 TYPES OF BONDS

IONIC

COVALENT METALLIC HYDROGEN

(Ions)

(Sharing

valence electrons) (Metals)

(Ions)

IONIC BONDS

• Form between ions with opposite

charges: + and -. (a metal and a

non-metal)

• They bond because the opposite charges are attracted to

each other. (Think

magnets!!!)

IONIC BONDS

Like charges repel each other!

Ions and ionic bonds form because

electrons are

transferred from

one atom to the

other

Properties of IONIC BONDS

• Ionic compounds have high melting and boiling points.

• These are very strong bonds.

• An example is Na +1 + Cl -1

= NaCl (salt)

NaCl Melting point 801 °C NaCl Boiling point1465 °C

IONIC BONDS

Only certain ratios (combinations) of elements result in the formation of Ionic compounds.

For ex: Lithium (Li) will react with Fluorine (F) to form LiF.

BUT, it will NOT form LiF 2 , LiF 3 , etc.

Magnesium (Mg) will react with Fluorine to form MgF 2 .

BUT, it will NOT form MgF, MgF 3 , etc.

IONIC BONDS

• When writing a chemical formula for an ionic compound:

*The charges have to balance

to create a neutral compound.*

IONIC BONDS

• For example:

H ₂ O (Wudder) CO ₂ (Carbon Dioxide)

CH ₃ COOH + NaHCO ₃ ===> CH ₃ COONa + H ₂ O + CO ₂

• An example is Na ⁺¹ + Cl ^-1

BUT, it will NOT form LiF ₂ , LiF ₃ , etc.

Magnesium (Mg) will react with Fluorine to form MgF ₂ .

BUT, it will NOT form MgF, MgF ₃ , etc.

- With salt the charges are both 1: Na ⁺¹ and Cl ^-1

- Like Li ⁺¹ + O ^-2

Li ⁺¹ + O ^-2

ANSWER: You would need to use 2 Li ⁺¹ for every O ^-2 !!!

= Li ₂ O

1.) K ₃ N 2.) CaF ₂ 3.) LiCl

4.) Mg ₂ Si

5.) Al ₂ O ₃

6.) CaCl ₂ 7.) K ₃ P

8.) MgCl ₂

9.) Li ₃ P

10.) K ₂ O

Rb ând Cl Na ând S Li ând P

2. If you mix Calcium Chloride (CaCl ₂ ) into a glass of water

Rb ând Cl Na ând S Li ând P

2. If you mix Calcium Chloride (CaCl ₂ ) into a glass of water until it dissolves, what is the chemical formula?

RbCl Na ₂ S Li ₃ P

CaCl ₂ (aq)

13.) BeF ₂ 11.) Al ₂ S ₃ 12.) Rb ₂ O

14.) AlCl ₃

15.) Ca ₃ N ₂

16.) Ga ₂ Se ₃

C ₈ H ₁₀ N ₄ O ₂ or F ₂ C ₈ H ₁₀ N ₄ O ₂₌ compound