chemical bonds. a.compounds 1.are made from more than one type of atom (element) 2.are made during a...

CHEMICAL BONDS

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A.Compounds1.Are made from

more than one type of atom (element)

2.Are made during a chemical chg

3.Have properties different from the elements they are made of

4.Have constant compositions

I. Chemical Compounds

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B. Chemical Formulas1.Use symbols to

represent the ratios of elements in a particular compound. • Element symbols • Subscripts


Fe2O3

B. Chemical Formulas

3. Practice Interpreting Formulas • NaCl

1 sodium atom; 1 chlorine atom

• H2O 2 hydrogen atoms; 1 oxygen

atom• Al2(SO4)3

– 2 aluminum atoms – 3 sulfur atoms – 12 oxygen atoms

Your Turn!

Interpret each of the following

Fe2O3 Pb(C2H3O2)2 2 iron atoms3 oxygen atoms

1 lead atom4 carbon atoms6 hydrogen atoms4 oxygen atoms

C. Atoms Combine3. To become Stable

a.Atoms are stable when they have a full valence energy level – Octet rule: Usually 8 e-

– Exception: He is stable w/ 2 e-

b.Atoms gain, lose or share e-

to achieve a full valence levelc. Atoms are held together by

a chemical bond


C. Atoms Combine3. Noble gases

– Are inert– do not react because

they already have a full valence energy level

(stable octet)


A. Ions are atoms which1. Have gained or lost e-

ELements to the Left of the Line Lose eLectrons

II. Ions

GAINLOSE

Neither

A. Ions are atoms which

1. Have gained or lost e-

II. Ions


1. Have gained or lost e- – You can predict the # of

e- which will be gained or lost by looking at the family

II. Ions

Lose 1 e-

Gain 1 e-

Lose 2 e-

Gain 2 e-

Gain 3 e-Lose 3 e-

Varies

Will P gain or lose electrons when forming an ion? How many?

Gains 3 e-

3.Another name for charge is oxidation number

4.The formula for an ion includes its charge (oxidation number)


Formula= Na1+

• Na ion Lost 1 e-

Formula= Cl1-• Cl ion Gained 1 e-

Review it Now!1. What is the difference

between an atom and an ion? 2. What is an oxidation number? 3.Write the oxidation

number for each of the following ions:a. Li f. Alb. K g. S c. Mg h. Cld. P i. Nee. B j. N

Ions have a charge, atoms do not

The charge on an ion

1+1+2+3-

3+

3+2-

1-03-

A.Ionic Bonds1.Are formed

a.between (+) and (-) ions

b.When one atom gains e- while the other loses e-

2.Compounds with ionic bonds are called ionic compounds

III.Compounds with Ionic Bonds

A.Ionic Bonds

3. Ionic bonds are formed between a metal and a

nonmetal!

III.Compounds with Ionic Bonds

Which of the following are ionic compounds?

1. KCl

2. CO2

3. LiF

4. CaCl2

Check Your Understanding!

IonicNot ionic

Ionic

Ionic

Step 1:Write the symbol of the (+) ion first, followed

by the symbol of the (-) ion

Step 2: Determine the ox.# for each ion and write it

above the symbols.Step 3: Crisscross the charges

and write them as subscripts.

Step 4: If the charges can be reduced, do so.

B. Formulas for Binary Cmpds

Example #1: Ba and Cl

B. Formulas for Ionic Cmpds

Example #2: Be and P


Be3

P2

Example #3: Ba and S


BaSBa2S2 note subscripts

can be reduced; do so!

Write the formula for each of the following compounds

1. calcium with chlorine

2. potassium with bromine

3. lithium with sulfur

4. magnesium with phosphorus

5. aluminum with nitrogen

Your Turn!

CaCl2

KBr

Li2S

AlN

Mg3P2

Step 1:Write the name of the positive element 1st.

Step 2:Write the name of the negative element 2nd.

Step 3:Add the ending -ide to the root of the second element.

C. Naming Binary Cmpds

Example #1:

What is the formula name for CaCl2?

Step 1: calciumStep 2: calcium chlorine Step 3: calcium chloride


calcium chloride

Example #2:

What is the formula name for Mg3P2?

Step 1: magnesiumStep 2: magnesium

phosphorus Step 3: magnesium

phosphide


Magnesium phosphide

Name each of the following

1. Li2S

2. KBr

3. BaS

4. Al2O3

5. Na3N

Your Turn!

Lithium sulfide

Potassium bromide

Barium sulfide

Sodium nitride

Aluminum oxide

1.Binary compounds are made of two kinds of elements.– Example: BaCl2

2.Polyatomic (ternary) compounds are made of three or more elements.– Examples:

K2SO4 Mg(ClO3)2

D. Formulas for Polyatomic Ionic Cmpds

3.Polyatomic ions are a group of covalently bonded atoms that act as one atom with a charge.


3.Rules for Writing Formulas


Step 1:Write the symbol and ox. #Step 2: Crisscross the charges and

write them as subscripts.Step 3: Make sure you put

polyatomic ions in parentheses (if you need more than one).Step 4: Make sure the subscripts are

reduced.

Example #1: Calcium Nitrate

D. Formulas for Ionic Cmpds

Ca(NO3)2

Ca2+ and NO31-

Ca2+ and NO31-

Ca2+ and (NO3)2

2

Example #2: Calcium Phosphate


Ca3(PO4

)2

Ca2+ and PO43-

Ca2+ and PO43-

23

Ca3 and (PO4)2

Write the formula for each of the following compounds

1. Sodium sulfate

2. Calcium hydroxide

3. Beryllium phosphate

4. Aluminum nitrate

Your Turn!

Na2SO4

Ca(OH)2 Be3(PO4)2

Al(NO3)3

1.Rules for Naming Polyatomic Compounds

E. Naming Polyatomic Ionic Compounds

Step 1:Write the name of the positive ion.Step 2: Write the name of the negative ion .

Example #1: Ca(NO3)2

E. Naming Polyatomic Ionic Cmpds

Calcium nitrate

Calciumnitrate

Example #2: AlPO4

E. Naming Polyatomic Ionic Cmpds

Aluminum phosphate

Aluminumphosphate

Name each of the following compounds

1. K2SO4

2. CaCO3

3. NaOH

4. NH4C2H3O2

Your Turn!

Calcium carbonate

Sodium hydroxide Ammonium acetate

Potassium sulfate

G. Special case ionic bonds: ACIDS

Acids are easy to recognize as compounds as they begin with the element hydrogen. As with other ionic bonds, acids fall into 2 categories, binary and ternary.


Examples of binary acids would include things like:

HF, HI, H2S and HCl

Examples of ternary acids would include things like:

H2SO4 and HNO3


Naming of binary acidsStep 1:Name the anion, changing the ending to “-ic”Step 2: Add the prefix “hydro-”Step 3: Slap acid on the end

Example #1: HF


“flourine” becomes

Example #1: HF


“flouric” becomes


Example #2: HF


“hydroflouric” becomes

“flouric” becomes


Example #1: HF


“hydroflouric acid”

“hydrochloric” becomes

“chloric” becomes

“chlorine” becomes

Example #1: HF


Example #2: HCl


“hydrochloric acid”




Example #2: HCl



Naming of ternary acidsStep 1:Name the polyatomicStep 2: Change “-ate” to “-ic” or “-ite” to “-ous”Step 3: Slap acid on the end

“sulfuric acid”

“sulfuric” becomes

“sulfate” becomes

Example #1: H2SO4


Example #1: H2SO4


“sulfuric acid”



Example #1: H2SO4


Example #1: HNO2


“nitrite” becomes

Example #1: HNO2


“nitrous” becomes


Example #1: HNO2


“nitrous acid”

“nitrous” becomes


Example #1: HNO2


Rules for Writing Formulas for binary acids


Step 1: Does the name begin with “hydro-”? If yes, then…Step 2:Write the symbol for the hydrogen ion followed by the symbol for the second elementStep 3: Crisscross the charges and

write them as subscripts.



Example: hydrosulfuric acid




H+1 S-2




H+1 S-2

H+1 S-2




H+1 S-2

H+1 S-2

H2S

Rules for Writing Formulas for ternary acids


Step 1: Does the name begin with “hydro-”? If no, then…Step 2:Write the symbol for the hydrogen ion followed by the appropriate polyatomic ionStep 3: Crisscross the charges and

write them as subscripts.



Example: sulfuric acid




H+1 SO4-2




H+1 SO4-2

H+1 SO4-2




H+1 SO4-2

H+1 SO4-2

H2SO4

1. HI

2. phosphoric acid

3. hydrobromic acid

4. H2SO3

Name the chemical or write the symbol


hydroiodic acid

1.

2. phosphoric acid

3. hydrobromic acid

4. H2SO3



H3PO4

hydroiodic acid

1.

2.

3. hydrobromic acid

4. H2SO3



HBr

H3PO4

hydroiodic acid

1.

2.

3.

4. H2SO3



sulfurous acid

HBr

H3PO4

hydroiodic acid

1.

2.

3.

4.



A.Covalent Bonds1.Are formed when

atoms share e-

IV.Compounds with Covalent Bonds

A.Covalent Bonds2.Are formed

Between two nonmetals

IV.Cmpds with Covalent Bonds

State if each of the following compounds is ionic or covalent

1. CO2

2. MgS

3. Na2O

4. PI3

Your Turn!


1. CO2

2. MgS

3. Na2O

4. PI3

Your Turn!

covalent


1. CO2

2. MgS

3. Na2O

4. PI3

Your Turn!

covalentionic


1. CO2

2. MgS

3. Na2O

4. PI3

Your Turn!

covalentionic ionic


1. CO2

2. MgS

3. Na2O

4. PI3

Your Turn!

covalentionic ionic covalent

B.Writing Covalent Formulas1.Greek Prefixes


mono-one

di- two

tri-threetetra- fourpenta-five

hexa- sixhepta-sevenocta- eightnona- ninedeca- ten

2.Rules

B. Writing Covalent Formulas

Step 1: Write the symbol of the first nonmetal.Step 2: Use the nonmetal’s prefix as a subscript

2.Rules


Step 3: Write the symbol of the second nonmetal.Step 4: Use the nonmetal’s prefix as a subscript.Note: If there is no prefix,

there is no subscript.

3.Practice problem #1


Write the formula for carbon dioxide

C




CO




CO2




CO2

No Prefix = No Subscript



Write the formula for dinitrogen trioxide




N




N O




N2O3



Write the formula for dichlorine hexabromide




Cl




Cl

Br




Cl

2Br6




Cl

2Br6Note: Do Not Reduce subscripts!

Write formulas for the following compounds

1. Carbon tetrachloride

2. Trichlorine heptabromide

3. Dinitrogen monoxide

4. Carbon monoxide

Your Turn!





4. Carbon monoxide

Your Turn!

CCl4





4. Carbon monoxide

Your Turn!

Cl3Br7

CCl4





4. Carbon monoxide

Your Turn!

Cl3Br7

N2O

CCl4





4. Carbon monoxide

Your Turn!

Cl3Br7

N2O

CO

CCl4

C.Naming Covalent CmpdsStep 1: Name each

element.Step 2: Change the ending

of the 2nd element to -ide

Step 3: Add Greek prefixes to indicate the # ofatoms of each element


Note: Do not use mono on the first element!


C. Naming Covalent Cmpds

Write the name for CO




Carbon




Carbonoxygen




Carbonoxygenoxide




CarbonMonoxide




Carbon

Carbon Monoxide

Monoxide



Write the name for Cl2O3




chlorine




chlorine

oxygen




chlorine

oxide




chlorine

oxygenoxidetrioxideDichlorine

trioxide




chlorine

oxygen

Dichlorine trioxide

oxidetrioxideDichlorine

trioxide





4. Carbon monoxide

Your Turn!





4. Carbon monoxide

Your Turn!

CCl4





4. Carbon monoxide

Your Turn!

Cl3Br7

CCl4





4. Carbon monoxide

Your Turn!

Cl3Br7

N2O

CCl4





4. Carbon monoxide

Your Turn!

Cl3Br7

N2O

CO

CCl4

Name the following compounds

1. PBr5

2. NO

3. S2I3

Your Turn!


1. phosphorus pentabromide

2. NO

3. S2I3

Your Turn!


1. phosphorus pentabromide

2. nitrogen monoxide

3. S2I3

Your Turn!


1. PBr5

2. nitrogen monoxide

3. disulfur triiodide

Your Turn!

phosphorus pentabromide

THAT’S ALL FOLKS!!!

Now you can name not only covalent bonds but binary and ternary ionic bonds, including acids. That being said, now…

GO DO!!!

chemical bonds. a.compounds 1.are made from more than one type of atom (element) 2.are made during a...

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