chemical bonds. a.compounds 1.are made from more than one type of atom (element) 2.are made during a...
Post on 26-Dec-2015
216 Views
Preview:
TRANSCRIPT
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
B. Chemical Formulas1.Use symbols to
represent the ratios of elements in a particular compound. • Element symbols • Subscripts
I. Chemical Compounds
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
I. Chemical Compounds
C. Atoms Combine3. Noble gases
– Are inert– do not react because
they already have a full valence energy level
(stable octet)
I. Chemical Compounds
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
A. Ions are atoms which
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)
A. Ions are atoms which
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
B. Formulas for Ionic Cmpds
Be3
P2
Example #3: Ba and S
B. Formulas for Ionic Cmpds
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
C. Naming Binary Cmpds
calcium chloride
Example #2:
What is the formula name for Mg3P2?
Step 1: magnesiumStep 2: magnesium
phosphorus Step 3: magnesium
phosphide
C. Naming Binary Cmpds
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.
D. Formulas for Polyatomic Ionic Cmpds
3.Rules for Writing Formulas
D. Formulas for Polyatomic Ionic Cmpds
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
D. Formulas for Polyatomic Ionic Cmpds
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.
G. Special case ionic bonds: ACIDS
Examples of binary acids would include things like:
HF, HI, H2S and HCl
Examples of ternary acids would include things like:
H2SO4 and HNO3
G. Special case ionic bonds: ACIDS
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
G. Special case ionic bonds: ACIDS
“flourine” becomes
Example #1: HF
G. Special case ionic bonds: ACIDS
“flouric” becomes
“flourine” becomes
Example #2: HF
G. Special case ionic bonds: ACIDS
“hydroflouric” becomes
“flouric” becomes
“flourine” becomes
Example #1: HF
G. Special case ionic bonds: ACIDS
“hydroflouric acid”
“hydrochloric” becomes
“chloric” becomes
“chlorine” becomes
Example #1: HF
G. Special case ionic bonds: ACIDS
Example #2: HCl
G. Special case ionic bonds: ACIDS
“chlorine” becomes
Example #2: HCl
G. Special case ionic bonds: ACIDS
“chloric” becomes
“chlorine” becomes
Example #2: HCl
G. Special case ionic bonds: ACIDS
“hydrochloric” becomes
“chloric” becomes
“chlorine” becomes
Example #2: HCl
G. Special case ionic bonds: ACIDS
“hydrochloric acid”
“hydrochloric” becomes
“chloric” becomes
“chlorine” becomes
Example #2: HCl
G. Special case ionic bonds: ACIDS
G. Special case ionic bonds: ACIDS
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
G. Special case ionic bonds: ACIDS
Example #1: H2SO4
G. Special case ionic bonds: ACIDS
“sulfate” becomes
Example #1: H2SO4
G. Special case ionic bonds: ACIDS
“sulfuric” becomes
“sulfate” becomes
Example #1: H2SO4
G. Special case ionic bonds: ACIDS
“sulfuric acid”
“sulfuric” becomes
“sulfate” becomes
Example #1: H2SO4
G. Special case ionic bonds: ACIDS
Example #1: HNO2
G. Special case ionic bonds: ACIDS
“nitrite” becomes
Example #1: HNO2
G. Special case ionic bonds: ACIDS
“nitrous” becomes
“nitrite” becomes
Example #1: HNO2
G. Special case ionic bonds: ACIDS
“nitrous acid”
“nitrous” becomes
“nitrite” becomes
Example #1: HNO2
G. Special case ionic bonds: ACIDS
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: 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.
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Example: hydrosulfuric acid
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Example: hydrosulfuric acid
H+1 S-2
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Example: hydrosulfuric acid
H+1 S-2
H+1 S-2
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Example: hydrosulfuric acid
H+1 S-2
H+1 S-2
H2S
Rules for Writing Formulas for ternary acids
G. Special case ionic bonds: 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.
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Example: sulfuric acid
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Example: sulfuric acid
H+1 SO4-2
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Example: sulfuric acid
H+1 SO4-2
H+1 SO4-2
Rules for Writing Formulas for binary acids
G. Special case ionic bonds: ACIDS
Example: sulfuric acid
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
G. Special case ionic bonds: ACIDS
hydroiodic acid
1.
2. phosphoric acid
3. hydrobromic acid
4. H2SO3
Name the chemical or write the symbol
G. Special case ionic bonds: ACIDS
H3PO4
hydroiodic acid
1.
2.
3. hydrobromic acid
4. H2SO3
Name the chemical or write the symbol
G. Special case ionic bonds: ACIDS
HBr
H3PO4
hydroiodic acid
1.
2.
3.
4. H2SO3
Name the chemical or write the symbol
G. Special case ionic bonds: ACIDS
sulfurous acid
HBr
H3PO4
hydroiodic acid
1.
2.
3.
4.
Name the chemical or write the symbol
G. Special case ionic bonds: ACIDS
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!
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3
Your Turn!
covalent
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3
Your Turn!
covalentionic
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3
Your Turn!
covalentionic ionic
State if each of the following compounds is ionic or covalent
1. CO2
2. MgS
3. Na2O
4. PI3
Your Turn!
covalentionic ionic covalent
B.Writing Covalent Formulas1.Greek Prefixes
IV.Cmpds with Covalent Bonds
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
B. Writing Covalent Formulas
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
B. Writing Covalent Formulas
Write the formula for carbon dioxide
C
3.Practice problem #1
B. Writing Covalent Formulas
Write the formula for carbon dioxide
CO
3.Practice problem #1
B. Writing Covalent Formulas
Write the formula for carbon dioxide
CO2
3.Practice problem #1
B. Writing Covalent Formulas
Write the formula for carbon dioxide
CO2
No Prefix = No Subscript
3.Practice problem #2
B. Writing Covalent Formulas
Write the formula for dinitrogen trioxide
3.Practice problem #2
B. Writing Covalent Formulas
Write the formula for dinitrogen trioxide
N
3.Practice problem #2
B. Writing Covalent Formulas
Write the formula for dinitrogen trioxide
N O
3.Practice problem #2
B. Writing Covalent Formulas
Write the formula for dinitrogen trioxide
N2O3
3.Practice problem #3
B. Writing Covalent Formulas
Write the formula for dichlorine hexabromide
3.Practice problem #3
B. Writing Covalent Formulas
Write the formula for dichlorine hexabromide
Cl
3.Practice problem #3
B. Writing Covalent Formulas
Write the formula for dichlorine hexabromide
Cl
Br
3.Practice problem #3
B. Writing Covalent Formulas
Write the formula for dichlorine hexabromide
Cl
2Br6
3.Practice problem #3
B. Writing Covalent Formulas
Write the formula for dichlorine hexabromide
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!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
Your Turn!
CCl4
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
Your Turn!
Cl3Br7
CCl4
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
Your Turn!
Cl3Br7
N2O
CCl4
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
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
IV.Cmpds with Covalent Bonds
Note: Do not use mono on the first element!
2.Practice problem #1
C. Naming Covalent Cmpds
Write the name for CO
2.Practice problem #1
C. Naming Covalent Cmpds
Write the name for CO
Carbon
2.Practice problem #1
C. Naming Covalent Cmpds
Write the name for CO
Carbonoxygen
2.Practice problem #1
C. Naming Covalent Cmpds
Write the name for CO
Carbonoxygenoxide
2.Practice problem #1
C. Naming Covalent Cmpds
Write the name for CO
CarbonMonoxide
2.Practice problem #1
C. Naming Covalent Cmpds
Write the name for CO
Carbon
Carbon Monoxide
Monoxide
2.Practice problem #2
C. Naming Covalent Cmpds
Write the name for Cl2O3
2.Practice problem #2
C. Naming Covalent Cmpds
Write the name for Cl2O3
chlorine
2.Practice problem #2
C. Naming Covalent Cmpds
Write the name for Cl2O3
chlorine
oxygen
2.Practice problem #2
C. Naming Covalent Cmpds
Write the name for Cl2O3
chlorine
oxide
2.Practice problem #2
C. Naming Covalent Cmpds
Write the name for Cl2O3
chlorine
oxygenoxidetrioxideDichlorine
trioxide
2.Practice problem #2
C. Naming Covalent Cmpds
Write the name for Cl2O3
chlorine
oxygen
Dichlorine trioxide
oxidetrioxideDichlorine
trioxide
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
Your Turn!
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
Your Turn!
CCl4
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
Your Turn!
Cl3Br7
CCl4
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
Your Turn!
Cl3Br7
N2O
CCl4
Write formulas for the following compounds
1. Carbon tetrachloride
2. Trichlorine heptabromide
3. Dinitrogen monoxide
4. Carbon monoxide
Your Turn!
Cl3Br7
N2O
CO
CCl4
Name the following compounds
1. PBr5
2. NO
3. S2I3
Your Turn!
Name the following compounds
1. phosphorus pentabromide
2. NO
3. S2I3
Your Turn!
Name the following compounds
1. phosphorus pentabromide
2. nitrogen monoxide
3. S2I3
Your Turn!
Name the following compounds
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!!!
top related