Proton Don
Your Guide for Success—Chemistry Unit Name: __________________________
Chemistry Outline I. Atoms A. Structure of an Atom 1. Subatomic Particles 2. Different Form b. Isotope II. Periodic Table 1. Arranging a. Mendeleev b. Mosely 2. Grouping the Elements III. Chemical Bonding A. Ionic Bonding 1. Forming Ionic Bonds 2. Forming Positive Ions 3. Forming Negative Ions 4. Properties B. Covalent and Metallic Bonds 1. Molecules 2. Movement of Electrons in Metallic Bonds 3. Properties of Metallic Bonds
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1V. Chemical Reactions A. Forming New Substances 14 B. Chemical Formulas and Equations 16 1. Chemical Formulas 2. Writing Formulas for Covalent and Ionic Compounds 3. Chemical Equations 4. Law of Conservation of Mass 5. Balancing Equations
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The Atom vs. The Isotope Chapter _4_ Section _2_ Pages _88-94_ Smallest unit of an _____________ that maintains the properties of that element. Contains subatomic particles: Protons, _______________, and Electrons
us
Nucleus:
Tiny, ________ core of an atom
Contains ____________ and neutrons
Most of an atom’s ___________.
Very small and ____________. Protons:
Most of an atom’s _______
Contains ______________
_____________ charged
MUCH _______________
VERY ________________
Neutrons
_________ charged
1 ________ = 1 amu
Atomic # = the number of ___________
Symbol: + or ____
Together: Protons + _____________ = atomic mass
Electron Cloud: _____________ the nucle-
1 ________ = 1 amu
Symbol: 0 or ____
# of Electrons = # of ________________ Symbol: - or _______
An ______________ that has the same number of _______________ (atomic number) but a __________________ number of ________________, therefore it has a different
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5
Arranging the Elements Chapter _5_ Section _1_ Pages _106-112_
History 101-The Periodic Table
Dmitri Mendeleev—______________ Chemist—____________
Discovered a ________________ in the elements properties.
His final arrangement—increasing atomic _____________.
He left gaps in the his table—for yet _______________ elements.
He could _________________ the properties of the undiscovered elements.
Our Current Periodic Table
Henry Mosely—___________________ Scientist—____________
Rearranged original table—Our current periodic table is by atomic ______________________.
This allowed all elements to fit the __________________________.
Classification of Elements on the Periodic Table
Metals __________ of zig-zag line
________ valence elec-
trons
Metalloids ____________ zig-zag line About _________ a complete set of valance electrons
Nonmetals __________ of zig-zag line
___________ or almost complete set of valence electrons
An element’s classification is determined by its number of _____________ electrons. The ____________ line helps you recognize where to locate each classification on the Periodic Table.
Decoding The Elements of the Periodic Table Periods
Direction =
Period # = __________
There are ______ periods.
Groups/Families
Direction = _____________ Each group has _____________ properties. If you know the group number you can determine the number of _______________ electrons. There are ______ groups. 6
7
Grouping the Elements Chapter _5_ Section _2_ Pages _114-120_ Group 2 (G2) —Alkaline-Earth Metals: ___________ reactive than G1
Group 1 (G1) —Alkali Metals: __________ reactive metals
1 ______________ electron
2 ________________ electrons
Often store in _____________
Found in nature in _________________
Physical Properties—Silver, ____________ density ring ct u a f than G1 anu _m ___ nt ___ _ me _ e _ c _ and ___ __ n_ i _ _ d ___ Use ___ n i nd Fou
Physical Properties — Soft, _______________, shiny, and low __________________
Groups 3-12 (G3-12)—Transition Metals: 1 or 2 ___________ electrons (Do not let them go as easily as G1 or G2) Less _____________ than G1 and G2
Good ___________________ __________ density, ______________ melting point than G1 and G2 Lanthanide Series:
Appears at the bottom of the table to keep it from being too wide.
Actinide Series: ______________/Unstable After element number _______________ made in laboratories. Group 13 (G13)—Boron Group: ____ metalloid and _____ metals
3 ______________ electrons
Group 14 (G14)—Carbon Group: _____ nonmetal, _____ metalloids, and ____ metals 4 _____________ electrons
_______________ at RT
Most common = _____________
Varying _________________ ______________ at RT
in sed
___
___ ___ _ _ ___ ___ _ _ _
ps
chi
U
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Grouping the Elements…..continued Chapter _5_ Section _2_ Pages _114-120_ Group 16 (G16)—Oxygen Group: _____ nonmetals, _____ metalloids, and _____ metals 6 ________________ electrons
Group 15 (G15)—Nitrogen Group: _____ nonmetals, _____ metalloids, and _____ metals 5 ______________ electrons . athe
o ___% _ _ _ _
f the
___ ____ _ _ _ _
e b re gas w
____
__ r ____
.
athe
b re s we a g the % of _ _ _ ____
ive eact
Groups 17 G(17)—Halogens: All _______________________
7 ____________________ electrons
Very ____________________
Need to gain only __________ valence electron
Forms compounds with ______________very easily.
Chemical properties _____________________
Physical properties _______________ different
Group 18 (G18)—Noble Gases: All _____________________
Hydrogen:
8 _______________ electrons— Exception is He—__________ valence electrons.
STABLE!
1 _________________ electron
Set a part because the _______________ do not ____________ any other group. Is placed above ___________ because the ______________ of valence electrons is the same. Most __________________ element 9
Ionic Bonding Chapter _1_ Section _2_ Pages _8-11_ Ionic Compounds
Forms when _______________ electrons are transferred (gained or lost) from one atom to
first.
another to _______________ each others outer energy level.
Forms between _________________ (+ ions) When formed, the # of _______________ lost equals the # of electrons ______________.
Therefore, ionic compounds are ____________.
The charges _____________ each other out.
Properties include; ______________ bond,
Write the ____ ion or the ____________ second. Polyatomic ion—an ion that is made up of more than one atom (2 capital letters—Ex
and nonmetals ( ____ ions)
Writing Ionic Formulas Always write the ____ ion or __________
(NH4)+
When written name remains the same.
Use parentheses
____________ numerals show _______________ number.
____________ melting and boiling points.
An oxidation number is the number of _________________ electrons an atom gains or loses to become ______________.
Make sure compounds are _______________.
Forming + Ions - Cation
Occurs when an atom __________ valence
Forming - Ions— Anion
electrons.
An atom now has ___________ protons than
lence electrons.
negative electrons. (Unbalanced + and -)
(Unbalanced + and -)
Only takes a small amount of ______________ to lose their few ___________________ elec______ and _______ are examples of atoms that form + ions.
___________________ form - ions because they have an almost full outer level.
trons.
An atom now has move ______________ electrons than positive protons.
_______________ form + ions because they have ________ valance electrons (1, 2, or 3)
Occurs when an atom ______________ va-
Ending of the elements name changes to ___________ (Ex. Fluorine —>Fluoride)
______ and _______ are examples that form - ions. 10
Section A: Complete the chart using a periodic table to help you.
Section B: Answer these questions: 1. An atom that gains one or more electrons will have a _________________ charge. 2. An atom that loses one or more electrons will have a __________________ charge. 3. At atom that gains or loses one or more electrons is called an ________________. 4. A positive ion is called a ___________________ and a negative ion is called a ________________. 5. Atoms will transfer one or more ______________ to another to form the bond. 6. Each atom is left with at ____________________ outer shell. 7. An ionic bond forms between a _________________ ion with a positive charge and a ___________________ ion with a negative charge. Section C: Draw the ionic compounds below. Show the transfer, give the name of the compound and give the formula. Example #1: Sodium + Chlorine
Example #2: Magnesium + Iodine
Example #3: Sodium + Oxygen
Example #4: Aluminum + Chlorine
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Covalent and Metallic Bonding Chapter _1_ Section _3_ Pages _12-17_
Covalent Molecules Forms when atoms _______________ valence
electrons to complete an atom’s outermost en-
_____________________ between positively
ergy level.
charged metal ions and the
Forms between 2 or more _______________.
__________________ in the metal.
May have ______________ bonds between the atoms.
The metals outermost energy levels _______________.
This overlapping allows the
Consist of individual particles called
________________ electrons to move
__________________.
throughout the metal.
Simplest type = ___________________
Example—Hydrogen H2 and Oxygen O2
Metallic Compounds This type of bond is formed by the
The _______________ ____ cancel the __________________ charge of the ions.
Properties: _______________ bond, ________ melting and boiling points.
Writing Covalent Formulas Usually the name tells you the _____________________.
However, many molecules have
Metallic bonding is what gives ______________ their particular properties.
________________ names Example—dihydrogen monoxide = water
Properties of Metals
When metals are ______________________ electric current, the ___________________
Pay attention to __________________ used.
electrons are moving through the metal.
Because of the “__________________” elec-
Mono—
Hexa—
Di—
Hepta -
trons, metals may be
Tri—
Octa -
____________________. Malleability and
Tetra—
Nona-
______________________ describe how a
Penta—
Deca—
metal may be reshaped. 12
Section A: Answer these questions: 1. Atoms ________________ one or more electrons with each other to form the bond. 2. Each atom is left with a _______________________ outer shell. 3. A covalent bond form between two _________________________________. Section B: Draw the molecular compounds below. Show how they share, give the name of the molecule and give the formula. Example #1: Hydrogen + Hydrogen
Example #2: Hydrogen + Oxygen
Example #3: Chlorine + Chlorine
Example #4: Oxygen + Oxygen
Example #5: Carbon + 2 Oxygen gen
Example #6: Carbon + 4 Hydro-
Write the formulas for the following covalent compounds:
Write the names for the following covalent compounds:
1)
antimony tribromide ____________________
9)
P4S5- __________________________________
2)
hexaboron silicide ______________________
10)
O2 __________________________________
3)
chlorine dioxide ________________________
11)
SeF6 __________________________________
4)
hydrogen iodide ________________________
12)
Si2Br-6 __________________________________
5)
iodine pentafluoride _____________________
13)
SCl4 __________________________________
6)
dinitrogen trioxide ______________________
14)
CH4 __________________________________
7)
ammonia ______________________________
15)
B2Si __________________________________
8)
phosphorus triiodide _____________________
16)
NF3 __________________________________
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Forming New Substances Chapter _2_ Section _1_ Pages _28-31_ Chemical Reactions
A process in which one or more substances _______________ to make one or more _________ substances. The _____________ and physical properties ____________ from the original substances.
Some Signs of Chemical Reactions
Reactions often have more than one of these signs. And the more of these signs you see, the more likely that a chemical reaction is taking place. However there is NO guarantee. The MOST important sign is ___________________ of a ________ substance!
How do new substances form in a chemical reaction?
Chemical bonds in the original substances must ________________.
The _____________ rearrange.
New ______________ form to make ___________ substances.
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On your desk place the “Physical Change” card to your left and the “Chemical Change” card to your right. Using what you know about physical and chemical changes, place each card into the correct category. Record you data in the chart below.
Physical Change
Chemical Change
Were there any cards you had trouble classifying? Give an example of a physical change that was not listed above. Give an example of a chemical change that was not listed above.
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Chemical Equations Chapter _2_ Section _2_ Pages _32-36_
Use symbols and __________________ to describe a chemical reaction.
Starting materials = _____________________________
Ending materials = _____________________________
Accuracy is key when writing chemical equations!
Equations MUST BE Balanced!
Atoms are never ______________ or gained in a chemical reaction—just _______________.
The __________________ of reactants must equal the number of ____________________.
Based on the work of Antoine Lavoisier—Law of _______________________________ of ________________________.
Steps to balance a chemical equation. 1. Write symbols and ___________________ correctly. 2. Make 2 lists of ______________ - write it the __________ on both sides of the arrow. 3. Count 4. Use _____________________ to balance 5. Recount/ __________________ if necessary.
Never Ever Balance by Changing a Subscript! 16
Balancing Equations Practice Part A: Identify the following parts of each chemical formula by circling the subscripts and drawing a square around the coefficients. H2
2HCl
4O2
CH4
3CO3
2NaOH
Part B: List the symbols for the atoms in each formula and give the number of each. C2H6
2MgO
4P4O10
NH3
3Al(OH)3
2H2O
Part C: Balance each of the following equations following the procedure described in class. Be sure to show your work. P + O2 → P4O10
Mg + O2 → MgO
P= O=
Mg = O=
P= O=
Mg = O=
HgO → Hg + O2
Al2O3 → Al + O2
Hg = O=
Al = O=
Hg = O=
Al = O=
BaCl2 + H2SO4 → BaSO4 + HCl Ba = Ba = Cl = Cl = H= H= S= S= O= O= 17
Chemistry Outline I. Atoms A. Structure of an Atom 1. Subatomic Particles 2. Different Form b. Isotope II. Periodic Table 1. Arranging a. Mendeleev b. Mosely 2. Grouping the Elements III. Chemical Bonding A. Ionic Bonding 1. Forming Ionic Bonds 2. Forming Positive Ions 3. Forming Negative Ions 4. Properties B. Covalent and Metallic Bonds 1. Molecules 2. Movement of Electrons in Metallic Bonds 3. Properties of Metallic Bonds
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10
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1V. Chemical Reactions A. Forming New Substances 14 B. Chemical Formulas and Equations 16 1. Chemical Formulas 2. Writing Formulas for Covalent and Ionic Compounds 3. Chemical Equations 4. Law of Conservation of Mass 5. Balancing Equations
2
3
The Atom vs. The Isotope Chapter _4_ Section _2_ Pages _88-94_ Smallest unit of an _____________ that maintains the properties of that element. Contains subatomic particles: Protons, _______________, and Electrons
us
Nucleus:
Tiny, ________ core of an atom
Contains ____________ and neutrons
Most of an atom’s ___________.
Very small and ____________. Protons:
Most of an atom’s _______
Contains ______________
_____________ charged
MUCH _______________
VERY ________________
Neutrons
_________ charged
1 ________ = 1 amu
Atomic # = the number of ___________
Symbol: + or ____
Together: Protons + _____________ = atomic mass
Electron Cloud: _____________ the nucle-
1 ________ = 1 amu
Symbol: 0 or ____
# of Electrons = # of ________________ Symbol: - or _______
An ______________ that has the same number of _______________ (atomic number) but a __________________ number of ________________, therefore it has a different
4
5
Arranging the Elements Chapter _5_ Section _1_ Pages _106-112_
History 101-The Periodic Table
Dmitri Mendeleev—______________ Chemist—____________
Discovered a ________________ in the elements properties.
His final arrangement—increasing atomic _____________.
He left gaps in the his table—for yet _______________ elements.
He could _________________ the properties of the undiscovered elements.
Our Current Periodic Table
Henry Mosely—___________________ Scientist—____________
Rearranged original table—Our current periodic table is by atomic ______________________.
This allowed all elements to fit the __________________________.
Classification of Elements on the Periodic Table
Metals __________ of zig-zag line
________ valence elec-
trons
Metalloids ____________ zig-zag line About _________ a complete set of valance electrons
Nonmetals __________ of zig-zag line
___________ or almost complete set of valence electrons
An element’s classification is determined by its number of _____________ electrons. The ____________ line helps you recognize where to locate each classification on the Periodic Table.
Decoding The Elements of the Periodic Table Periods
Direction =
Period # = __________
There are ______ periods.
Groups/Families
Direction = _____________ Each group has _____________ properties. If you know the group number you can determine the number of _______________ electrons. There are ______ groups. 6
7
Grouping the Elements Chapter _5_ Section _2_ Pages _114-120_ Group 2 (G2) —Alkaline-Earth Metals: ___________ reactive than G1
Group 1 (G1) —Alkali Metals: __________ reactive metals
1 ______________ electron
2 ________________ electrons
Often store in _____________
Found in nature in _________________
Physical Properties—Silver, ____________ density ring ct u a f than G1 anu _m ___ nt ___ _ me _ e _ c _ and ___ __ n_ i _ _ d ___ Use ___ n i nd Fou
Physical Properties — Soft, _______________, shiny, and low __________________
Groups 3-12 (G3-12)—Transition Metals: 1 or 2 ___________ electrons (Do not let them go as easily as G1 or G2) Less _____________ than G1 and G2
Good ___________________ __________ density, ______________ melting point than G1 and G2 Lanthanide Series:
Appears at the bottom of the table to keep it from being too wide.
Actinide Series: ______________/Unstable After element number _______________ made in laboratories. Group 13 (G13)—Boron Group: ____ metalloid and _____ metals
3 ______________ electrons
Group 14 (G14)—Carbon Group: _____ nonmetal, _____ metalloids, and ____ metals 4 _____________ electrons
_______________ at RT
Most common = _____________
Varying _________________ ______________ at RT
in sed
___
___ ___ _ _ ___ ___ _ _ _
ps
chi
U
8
Grouping the Elements…..continued Chapter _5_ Section _2_ Pages _114-120_ Group 16 (G16)—Oxygen Group: _____ nonmetals, _____ metalloids, and _____ metals 6 ________________ electrons
Group 15 (G15)—Nitrogen Group: _____ nonmetals, _____ metalloids, and _____ metals 5 ______________ electrons . athe
o ___% _ _ _ _
f the
___ ____ _ _ _ _
e b re gas w
____
__ r ____
.
athe
b re s we a g the % of _ _ _ ____
ive eact
Groups 17 G(17)—Halogens: All _______________________
7 ____________________ electrons
Very ____________________
Need to gain only __________ valence electron
Forms compounds with ______________very easily.
Chemical properties _____________________
Physical properties _______________ different
Group 18 (G18)—Noble Gases: All _____________________
Hydrogen:
8 _______________ electrons— Exception is He—__________ valence electrons.
STABLE!
1 _________________ electron
Set a part because the _______________ do not ____________ any other group. Is placed above ___________ because the ______________ of valence electrons is the same. Most __________________ element 9
Ionic Bonding Chapter _1_ Section _2_ Pages _8-11_ Ionic Compounds
Forms when _______________ electrons are transferred (gained or lost) from one atom to
first.
another to _______________ each others outer energy level.
Forms between _________________ (+ ions) When formed, the # of _______________ lost equals the # of electrons ______________.
Therefore, ionic compounds are ____________.
The charges _____________ each other out.
Properties include; ______________ bond,
Write the ____ ion or the ____________ second. Polyatomic ion—an ion that is made up of more than one atom (2 capital letters—Ex
and nonmetals ( ____ ions)
Writing Ionic Formulas Always write the ____ ion or __________
(NH4)+
When written name remains the same.
Use parentheses
____________ numerals show _______________ number.
____________ melting and boiling points.
An oxidation number is the number of _________________ electrons an atom gains or loses to become ______________.
Make sure compounds are _______________.
Forming + Ions - Cation
Occurs when an atom __________ valence
Forming - Ions— Anion
electrons.
An atom now has ___________ protons than
lence electrons.
negative electrons. (Unbalanced + and -)
(Unbalanced + and -)
Only takes a small amount of ______________ to lose their few ___________________ elec______ and _______ are examples of atoms that form + ions.
___________________ form - ions because they have an almost full outer level.
trons.
An atom now has move ______________ electrons than positive protons.
_______________ form + ions because they have ________ valance electrons (1, 2, or 3)
Occurs when an atom ______________ va-
Ending of the elements name changes to ___________ (Ex. Fluorine —>Fluoride)
______ and _______ are examples that form - ions. 10
Section A: Complete the chart using a periodic table to help you.
Section B: Answer these questions: 1. An atom that gains one or more electrons will have a _________________ charge. 2. An atom that loses one or more electrons will have a __________________ charge. 3. At atom that gains or loses one or more electrons is called an ________________. 4. A positive ion is called a ___________________ and a negative ion is called a ________________. 5. Atoms will transfer one or more ______________ to another to form the bond. 6. Each atom is left with at ____________________ outer shell. 7. An ionic bond forms between a _________________ ion with a positive charge and a ___________________ ion with a negative charge. Section C: Draw the ionic compounds below. Show the transfer, give the name of the compound and give the formula. Example #1: Sodium + Chlorine
Example #2: Magnesium + Iodine
Example #3: Sodium + Oxygen
Example #4: Aluminum + Chlorine
11
Covalent and Metallic Bonding Chapter _1_ Section _3_ Pages _12-17_
Covalent Molecules Forms when atoms _______________ valence
electrons to complete an atom’s outermost en-
_____________________ between positively
ergy level.
charged metal ions and the
Forms between 2 or more _______________.
__________________ in the metal.
May have ______________ bonds between the atoms.
The metals outermost energy levels _______________.
This overlapping allows the
Consist of individual particles called
________________ electrons to move
__________________.
throughout the metal.
Simplest type = ___________________
Example—Hydrogen H2 and Oxygen O2
Metallic Compounds This type of bond is formed by the
The _______________ ____ cancel the __________________ charge of the ions.
Properties: _______________ bond, ________ melting and boiling points.
Writing Covalent Formulas Usually the name tells you the _____________________.
However, many molecules have
Metallic bonding is what gives ______________ their particular properties.
________________ names Example—dihydrogen monoxide = water
Properties of Metals
When metals are ______________________ electric current, the ___________________
Pay attention to __________________ used.
electrons are moving through the metal.
Because of the “__________________” elec-
Mono—
Hexa—
Di—
Hepta -
trons, metals may be
Tri—
Octa -
____________________. Malleability and
Tetra—
Nona-
______________________ describe how a
Penta—
Deca—
metal may be reshaped. 12
Section A: Answer these questions: 1. Atoms ________________ one or more electrons with each other to form the bond. 2. Each atom is left with a _______________________ outer shell. 3. A covalent bond form between two _________________________________. Section B: Draw the molecular compounds below. Show how they share, give the name of the molecule and give the formula. Example #1: Hydrogen + Hydrogen
Example #2: Hydrogen + Oxygen
Example #3: Chlorine + Chlorine
Example #4: Oxygen + Oxygen
Example #5: Carbon + 2 Oxygen gen
Example #6: Carbon + 4 Hydro-
Write the formulas for the following covalent compounds:
Write the names for the following covalent compounds:
1)
antimony tribromide ____________________
9)
P4S5- __________________________________
2)
hexaboron silicide ______________________
10)
O2 __________________________________
3)
chlorine dioxide ________________________
11)
SeF6 __________________________________
4)
hydrogen iodide ________________________
12)
Si2Br-6 __________________________________
5)
iodine pentafluoride _____________________
13)
SCl4 __________________________________
6)
dinitrogen trioxide ______________________
14)
CH4 __________________________________
7)
ammonia ______________________________
15)
B2Si __________________________________
8)
phosphorus triiodide _____________________
16)
NF3 __________________________________
13
Forming New Substances Chapter _2_ Section _1_ Pages _28-31_ Chemical Reactions
A process in which one or more substances _______________ to make one or more _________ substances. The _____________ and physical properties ____________ from the original substances.
Some Signs of Chemical Reactions
Reactions often have more than one of these signs. And the more of these signs you see, the more likely that a chemical reaction is taking place. However there is NO guarantee. The MOST important sign is ___________________ of a ________ substance!
How do new substances form in a chemical reaction?
Chemical bonds in the original substances must ________________.
The _____________ rearrange.
New ______________ form to make ___________ substances.
14
On your desk place the “Physical Change” card to your left and the “Chemical Change” card to your right. Using what you know about physical and chemical changes, place each card into the correct category. Record you data in the chart below.
Physical Change
Chemical Change
Were there any cards you had trouble classifying? Give an example of a physical change that was not listed above. Give an example of a chemical change that was not listed above.
15
Chemical Equations Chapter _2_ Section _2_ Pages _32-36_
Use symbols and __________________ to describe a chemical reaction.
Starting materials = _____________________________
Ending materials = _____________________________
Accuracy is key when writing chemical equations!
Equations MUST BE Balanced!
Atoms are never ______________ or gained in a chemical reaction—just _______________.
The __________________ of reactants must equal the number of ____________________.
Based on the work of Antoine Lavoisier—Law of _______________________________ of ________________________.
Steps to balance a chemical equation. 1. Write symbols and ___________________ correctly. 2. Make 2 lists of ______________ - write it the __________ on both sides of the arrow. 3. Count 4. Use _____________________ to balance 5. Recount/ __________________ if necessary.
Never Ever Balance by Changing a Subscript! 16
Balancing Equations Practice Part A: Identify the following parts of each chemical formula by circling the subscripts and drawing a square around the coefficients. H2
2HCl
4O2
CH4
3CO3
2NaOH
Part B: List the symbols for the atoms in each formula and give the number of each. C2H6
2MgO
4P4O10
NH3
3Al(OH)3
2H2O
Part C: Balance each of the following equations following the procedure described in class. Be sure to show your work. P + O2 → P4O10
Mg + O2 → MgO
P= O=
Mg = O=
P= O=
Mg = O=
HgO → Hg + O2
Al2O3 → Al + O2
Hg = O=
Al = O=
Hg = O=
Al = O=
BaCl2 + H2SO4 → BaSO4 + HCl Ba = Ba = Cl = Cl = H= H= S= S= O= O= 17
