Transcript Bell Activity Chem II January 3, 2012

Bell Activity
Chem II
January 3, 2012
• Discuss the real differences (by your
understanding) in organic chemistry
and inorganic chemistry. Make it at
least two paragraphs (one on each
topic) (you can find all you need
starting in chapter 11 of the organic
(green) book).
CHEMISTRY II BELL
January 4, 2012
•Name 5 things that one should never do in a
laboratory setting.
•Name 5 things that would be considered
acceptable during a lab activity.
•List 5 (general) pieces of equipment and define
their purpose during lab activities.
Chemistry II Bell Activity
January 5, 2012
• Ingesting this causes blindness and then
death.
• This is found in nail polish remover.
• This causes impotence
• The most flammable of all the solvents
• This causes one to become intoxicated.
• The solvent used in dry cleaning
• Was one used as an anesthetic
Chemistry II Bell Work
January 6, 2012
• What is the purpose of the “tare” button on the
electronic balance?
• What is the advantage of having the shapes of
the Erlenmeyer flask and the graduated
cylinder?
• What does “denatured” mean?
• What happens if you don’t wear your goggles?
• If you boil alcohol and water, which one would
boil off first? (hint: alcohol = 650, water =
1000—both in Celsius)
CHEM II BELL ACTIVITY
January 10, 2012
• What is distillation?
• a process in which a liquid or vapor mixture
of two or more substances is separated into
its component fractions of desired purity, by
the application and removal of heat.
• List the pieces that you will be using in the
distillation process.
• Beaker, boiling flask, distillation head, hollow
stopper w/gray holder attached, thermometer,
condenser, rubber tubing, vacuum adapter, ring
stands (2), graduated cylinder, hot plate, ring
stand clamps (2).
Chem II Bell Activity
January 13, 2012
• From yesterday’s lab, answer the following
questions:
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What did you learn?
What did you do differently the second day?
How could you have made your lab activity safer?
What was the purpose of the food coloring?
How did you find your percent y?
Why do you think your boiling points differed from the
accepted values?
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Chem II Bell Work January17, 2012
Name each functional Group below:
CH3 – CH– CH2 – CH3
CH3 – C – CH2 – CH2 – CH3
CH3 – C – H
CH3 – CH2 – CH2 – C – OH
CH3 – CH2 – CH2 – C – CH2 – CH3
CH3 – CH2 – CH2 – CH2 – CH2 –NH2
CH3 – CH2 – O – CH3
CH3 – CH2 – C – NH2
CH3 – CH = CH – CH2 – CH2 – CH3
Chemistry II Bell Work
August 25, 2011
• Name at least six items you recognize to
be composed of organic compounds.
• Why were the compounds of carbon
originally called organic compounds?
Early scientists noted that organized (living) systems were the source of
these compounds, hence; the name “organic” was applied
• Describe what Wohler did that made the
vital force theory highly questionable.
• What is the unique structural feature
shared by all organic compounds?
They all contain carbon
CHEMISTRY II BELL ACTIVITY
January 18, 2012
• Define the terms and/or describe what the
following people contributed to organic
chemistry. Get this from your book:
– Friedrich Wohler
– Lewis Dot structures
– VSEPR theory
– Vital force (chapter 11)
– Covalent bond
– Ionic bond
Daily Purpose: To identify the 10 functional Groups we use in organic
chemistry.
Chem II Bell Activity August 26, 2011 (Put these in your notes)
The Functional Groups
Term/Definition
Alkane consists of only carbon to carbon single bonds
Alkene consists of at least one carbon to carbon double bond
Alkyne consists of at least one carbon to carbon triple bond
Alcohol contains an R-OH group
Aldehyde contains a terminal R- O=C-H group
Ketone contains an internal R-C=O-Rgroup
Carboxylic acid contains a terminal R-O=C-OH group
Ether contains an internal R-O-R
group
Ester contains an internal R-O=C-O-R group
Amine contains a terminal R-NH2 group
Amide contains a terminal o=C-NH2
Aromatic contains the benzene ring C6H6
CHEMISTRY II BELL ACTIVITY
August 26, 2011
• Define the following terms:
– Polar covalent bond shows bond polarization—bonding electrons are shared unequally
– Nonpolar Pair of electrons are shared equally by the bonded atoms
Shows the general arrangement of atoms
– Condensed structural formula but without showing all the covalent bonds
– Expanded structural formula Shows all the covalent bonds
combination of atoms that differentiates molecules of organic
– Functional group Acompounds
of one class from those of another
orbital produced from the combination of two or more nonequivalent
– Hybrid orbital An
orbital's of an atom
property in which two or more compounds have the same molecular formula but
– Isomerism Adifferent
arrangements of atoms
Chemistry II Bell Work
August 26, 2011
• What is one of the major differences in
organic and inorganic compounds?
• What is one of the major reasons why we
have so many organic molecules?
• What does “saturated” mean?
• Draw the structure belonging to C6H6.
• Yes or No! Can carbon tetrachloride be
made from reacting methane with
chlorine?
Chemistry II Bell Activity
January 27, 2011
• What causes all the different molecules to
form different shapes? Answer this based
on your knowledge of electrons, polarity,
charges, electronegativity, etc. (Use your
book to find this answer under the VSEPR
section)
• Draw the tetrahedral shape of the
methane molecule.
• Draw the two isomers of C2H6O
Chemistry II Bell Activity
January 31, 2011
• What does the term “Like dissolves like”
mean?
• What is the difference in polar and
nonpolar molecules?
• What does it mean for something to be
“hydrophobic” or “hydrophilic”?
Chemistry II Bell Activity
January 31, 2011
• Explain how the structure and
bonding of carbon lead to the
diversity and number of organic
compounds.
• Tell me how many covalent bonds
each of the 10 elements we use in
organic can form. Ex. Carbon can
form 4, etc.
Chem II Bell Activity
September 1, 2010
• Discuss 5 reasons why a pharmacists or
doctor would need to have a good
understanding of organic chemistry.
• Why is carbon so important to the medical
field as well as to each of us?
CHEMISTRY II BELL ACTIVITY
August 30, 2011
• Do learning check 11.1 and 11.2 on page
344 (green book)
• Define the following terms:
– Hydrocarbons
– Saturated hydrocarbons
– Normal alkane
•List the prefixes for the first 10 alkanes and name the
alkyl group associated with them. (Page 357) (top of page
in first paragraph)
CHEMISTRY II BELL ACTIVITY
August 31, 2011
• Do learning check 11.4 on page 350.
• Look at the story on “petroleum” on page
367. Pick out 5 key words in the 3
paragraphs, then write a summary
statement using those five key words.
(**Remember a summary statement
consists of 2-3 sentences only using
key words you have picked out of the
paragraphs)
Chemistry II Bell Activity
September 1, 2011
• Name the first 10 alkanes.
• State the first 3 rules in naming alkanes.
• What is the naming system we use in
naming organic compounds?
Chem II Bell Activity
September 2, 2011
• List the prefixes (from memory) for the
alkyl groups (1-5)
• List the first ten alkanes (from memory)
• Are the following (1)parents or (2)groups
and give the name the parent or group:
– C6H14
– C10H21
– C7H15
– C8H18
C2H5
C4H9
C3H8
C5H11
CHEMISTRY II BELL ACTIVITY
September 6, 2011
• Write a molecular formula for the following
structures: (remember: CnH2n + 2)
– Methane
– Methyl
– Ethane
– Ethyl
– Propane
– Propyl
-hexane
-hexyl
-pentane
-pentyl
-butane
-butyl
Chemistry II Bell Activity
September 7, 2011
• What is the term given to a carbon that is
connected to 4 other carbons?
• Which functional group does benzene belong
to?
• How do you write an alkyl halide?
• What is a continuous chain of carbons called?
• Define isomer.
• Go to page 374 and complete problem 11.42.
Chem II Bell Activity
September 8, 2011
• Turn to page 369 and read “Carbon
Monoxide, Silent and Deadly” and write a
3-5 sentence summary of the topic
discussed.
• Why are there NO 1-methyl groups?
• What is the difference in a primary carbon
and a tertiary carbon group?
Chemistry II Bell Activity
September 12, 2011
• Are the following structures possible? If not,
then write the correct answer
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1,2-dimethylpropane
3,4-dimethylpentane
2-ethyl-4-methylpentane
2-bromo-3-ethylbutane
2-methylhexane
2,4-methylhexane
1,1,1-triethylcyclopentane
2-propylcyclobutane
Chemistry II Bell Activity
September 13, 2011
• Which functional group contains at least
one double bond and is unsaturated?
• Is “COKE” found in nature or is it
synthetic?
• Do alkanes undergo oxidation? And if they
do what is produced?
• Where is natural gas found?
Chemistry II Bell Activity
September 14, 2011
• How is methane transported?
• What color are the tankers that transport
propane and butane? Why?
• What is another name for Isopropyl
Iodide?
• Which alkanes are more cost efficient for
tractor fuels?
Chem II Bell Work
September 15,2011
Are the following molecules possible?
– 1,2,2,2-tetrabromobutane
– 3,3-dimethyl-4-ethyloctane
– 1-methylcyclobutane
– Dimethylpropane
• Draw the following:
•3,4,4-trimethyloctane
•3-ethyl-2-methylhexane
4-ethyl-3,3-dimethylhexane
2,2,6-trimethyloctane
•1,1,4—trimethylcyclohexane
methylcycloheptane
Chem II Bell Work
September 16, 2011
• This is used as a refrigerant
• Can an alkyl halide be produced when alkanes
undergo substitution?
• Does the blood hemoglobin like CO or CO2
better?
• Is “Iso” a prefix or does it go by the alphabetizing
rule?
• What are the 4 products of petroleum refining?
• Which process is used for petroleum refining?
Chemistry II Bell Activity
September 19, 2011
• Define the following terms:
– Hydration
polyunsaturated
– Polymerization
carbocation
– Markovnikov’s rule
phenyl group
– Addition reaction
– Aromatic hydrocarbons
– Alkenes
– Alkynes
– Alkyl halide
Chem II Bell Activity
September 21, 2011
• Name the following alkenes:
– CH3CH2CH=CHCH2CH2CH3
– CH2(Br)CH2CH(Br)CH2CH2CH=CH2
– CH3CH2CH(CH(CH3)2)CH=CHCH2CH2CH3
– CH3CH2C CCH2CH2CH(Br)CH3
CH2CH3
CH3
Chemistry II Bell Activity
September 23 , 2010
• What are cis and trans isomers?
• Draw the following molecules:
– 1-ethyl-3-methylcyclobutene
– 2-bromo-1,3-pentadiene
– 2,5-dichloro-2,4-hexadiene
– 4-isopropylcyclopentene
– 5,5-diIsobutylcycloheptene
– 1,2-dimethyl-4-propylcyclohexene
Chemistry II Bell Activity
September 29, 2011
• Draw the following alkenes:
– 2-pentene
– Ethyne
– 3,4,4-trimethyl-1-pentene
– 1,2,3-tribromocyclo butene
– 1-chloro-3-methyl-3-hexene
– 2,5-diethyl-1,3,3-trimethylcyclopentene
– 1-butyl-2-isopropylcyclopropene
– 2,2,5-trichloro-3-heptyne
Chemistry II Bell Activity
September 27, 2010
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Which kind of rubber is bouncy? cis
Which kind of rubber is not bouncy? trans
Cis-retinal
Another name for vitamin A is _____. or opsin
Which kind of fatty acid is bad for you? trans
What is the pheromone secreted by the
female gypsy moth? Cis-glyplure
Chemistry II Bell Activity
September 28, 2010
• What is the IUPAC name for acetylene?
• What is the common name for propene?
• What is the chemical that ripens fruits and
vegetables?
• What is the process that changes the cis
fatty acid to trans fatty acid?
• The rule that states that the carbon that is
“poor” (of hydrogens) will produce the
major product.
Chem II Bell Activity
September 12, 2008
• Look on page 407 and do the following
exercises:
– 12.1
– 12.2
– 12.3
Define the following terms:
– carbocation
-hydration
– hydrogenation
-Markovnikov’s rule
– phenyl group
-polyunsaturated
Chemistry II Bell Activity
October 4, 2010
• What do you dehydrate in order to make
an alkene?
• In an alkyl halide-RX-what does the X
stand for? The R?
• What agent is used in
dehydrohalogenation?
• In a dehydration reaction, what is
produced other than an alkene?
Chemistry II Bell Activity
Alkene test info 2008
• Things to remember for the test
– Read the wording carefully.
– Name all HC products
– If you have a major—then you will have a minor—
draw them both
– If you have a cis—there is a trans— draw them both
– Don’t put a major/ minor if you can’t use one of the
rules
– Put your lines representing the hydrogens.
– Remember the difference in hydration and
hydrogenation.
Chemistry II Bell Activity
October 21, 2011
• Who was Michael Faraday?
He discovered the benzene structure in 1825
• Who was Freidrich Kekule’ and his
contribution to the benzene structure?
He was the one who suggested that the benzene molecule might be
represented by a ring arrangement of carbon atoms with alternating
single and double bonds between the carbon atoms.
• Name 9 ways of lowering your cancer rate
and give an explanation of each of the 9.
(Next slide)
1. Do not smoke: increases ones risk of mouth, throat, pancreatic,
kidney, stomach, bladder, breast, and colon cancers.
2. Increase your consumption of fruits, vegetables, and whole grains:
High fruit/vegetable intake have the lowest rate of most cancers.
3. Reduce your intake of animal fat: red meat—risk of prostate and colon
cancer & sometimes breast cancer.
4. Don’t grill meats at high temperatures: open flames cause cancerpromoting compounds to form in the meat.
5. Reduce your alcohol intake: excessive use can cause cirrhosis and
cancer to the liver.
6. Be active: exercise has shown that it reduces breast cancer in women
and prostate cancer in males
7. Maintain a proper weight: obesity increases the risk of heart disease,
strokes, diabetes, and development of cancer.
8. Don’t sunbathe: limit your exposure to the sun
9. Avoid exposure to known hazardous materials or conditions: Be
aware of and use appropriate precautions and protective equipment.
Chemistry II Bell Activity
March 28, 2011
• Describe the chief physical properties of
aromatic hydrocarbons. Nonpolar & insoluble in water
• Why does benzene not readily undergo
addition reactions characteristic of other
unsaturated compounds?
B/c benzene rings are relatively stable chemically & b/c of this,
benzene often reacts in such a way that the aromatic ring remains
intact.
• Compare the chemical behavior of
benzene and cyclohexene.
Cyclohexene undergoes addition reactions. Benzene resists addition
reactions. Both undergo combustion.
Chemistry II Bell Activity
October 24, 2011
• What is another name for 2,4,6trinitrotoluene? TNT
• What is DDT’s greatest drawback?
It is very stable
• What does DDT stand for?
dichlorodiphenyltrichloroethane
• What did DDT do the egg shells of birds?
It upset the bird’s estrogen level
Chemistry II Bell Activity
October 24, 2011
• Why will DDT become less effective in the
future? Insects are becoming immune to it
• What is the compound that smells like
mothballs? naphthalene
• What type of reaction does benzene go
through? substitution
• Do all aromatics smell good? No
• Is chlordane synthetic or naturally
produced? synthetic
Chemistry II Bell Activity
March 30, 2011
• What is a major drawback for DDT?
• Name three advantages of using DDT.
Very stable
Kills lice/ticks, mosquitoes, control of bird population
• Which animals would most likely have the
highest levels of DDT? Fish or minnows
• What does DDT stand for? dichlorodiphenyltrichloroethane
• Why did DDT become less effective? Insects became resistant
• What made bird egg shells to become thin?
Birds estrogen levels were upset
Chemistry II Bell Activity
October 26, 2011
• What are the terms given to the OH
group? Hydroxy, hydroxyl, and hydrid
• What is the source for making wine? grapes
• What is tetrahydrofuran used for?
PVC coating &
laboratory solvents
• How are alcohols similar to water?
They are both polar molecules & they contain the OH
grouping
• What are two ways to make ethanol?
Fermentation and hydration of ethene
Chemistry II Bell Activity
April 5, 2011
Apple Lab Questions
• If oxygen is lacking what will be the product of
fermentation? If present?
• Write a balanced equation illustrating the
process of fermentation.
• What is one way you can determine whether the
product is alcohol or vinegar?
• Differentiate between beers and wine.
• What causes dough to rise?
• What gas is produced in fermentation?
• What is the purpose of the balloon on top of the
apparatus used to distill the alcohol?
Chemistry II Bell Acitivity
April 6, 2011
• Why are the boiling points of alcohols much higher
than the boiling points of alkanes with similar
molecular weights.
• Arrange the compounds of each group in order of increasing
boiling points
– Ethanol, 1-propanol, methanol
– Butane, ethylene glycol, 1-propanol
• Which member of each of the following pairs would you expect to be more
soluble in water?
•Butane or 2-butanol
•2-propanol or 2-pentanol
•2-butanol or 2,3-butanediol
Chemistry II Bell Activity
October 27, 2011
• What is the irritant in poison ivy? tetrahydrourushiol
• What is the aqueous form of phenol? Carbolic acid
• Which of the solvents causes you to go
blind if you drink it? methanol
• This is also called grain alcohol? ethanol
• The antifreeze that is safe for pets. Propylene glycol
• What is the common name for 2-propanol?
Isopropyl alcohol
Chemistry II Bell Activity
October 28, 2011
• This is used in mouthwash and also treats
4-n-hexylrescorcinol
hookworms
• The antifreeze that is safe around pets and
animals
Propylene glycol
• This lowers the cholesterol and found in red
wine
resveratol
• This is a powerful explosive and is used to treat
angina pectoris (heart conditions)
nitroglycerin
• This is known as wood alcohol
methanol
Chemistry II Bell Activity
October 31, 2011
• One of the earliest antiseptics but no longer
used b/c it burns the skin. Carbolic acid
• What is the sticky black stuff on railroad ties and
telephone poles?
creosote
• A moisturizing agent used to help babies poop.
glycerin
• This is now used as a germicide for cleaning
(floors). Lysol
• This was added to mouthwash to make it taste
bad b/c we all know that if it tastes bad it works
better.
menthol
Chemistry II Bell Activity
November 15, 2011
• Is the carbonyl group polar or nonpolar?
• Can secondary alcohols oxidize into
ketones?
• Can we have cyclic ketones?
• Is formalin is a gas at room temperature?
• Does a ketone end in “anal” or “one”?
• What is the IUPAC name for acetone?
polar
yes
yes
“one”
2-propanone
no
Chemistry II Bell Activity
November 9, 2011
• Draw the following aldehydes/ ketones:
– 2-ene-pentanal
– CycloOctanone
– 3,4-dichloro-2-ene-butanal
– 2,3-dimethylcyclopropanone
– 4-ene-2-hexanone
– Cyclobutanone
– Acetone
Chemistry II Bell Activity
November 15, 2011
1. What is the term associated with the carbon
next to the carbonyl group? Alpha carbon
2. What is the reaction called when an aldehyde
changes into a carboxylic acid? oxidation
3. What is the name of the simplest ketone? acetone
4. Which of the test produces the silver mirror? Tollens
5. What was once used to embalm cadavers and
transport specimens to schools? formaldehyde
6. What is now used to transport specimens to
school systems? formalin
Chemistry II Bell Activity
November 16, 2011
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This has a musky aroma muscone
Used in margarine and foods butyraldehyde
Used in candy, toothpaste, and foods carvone
Part of the nut family acetophenone
Has a buttery odor butyraldehyde
Has a spearmint odor carvone
Known as a lachrymator chloroacetophenone
Chem II Bell Activity
November 17, 2011
• Is formalin a liquid or gas at room
temperature? gas
• What is the “suffix” in naming aldehydes?
Ketones? “anal” and “one”
• What is another name for acetone?(can be
two different names) 2-propanone & dimethyl ketone
• This is usually green in color and can be
found in ice cream. acetophenone
Chem II Bell Activity
April 28, 2010
• This kills bacteria and used to sterilize
surgical instruments. formalin
• What is the chemical that will turn your
skin black that we do in lab? Silver nitrate
• What is electronegativity? Refers to the attraction of
electrons to an atom
• Acetaldehyde is often converted into this,
which is easier to handle. paraldehyde
• This is used in liniments and inhalants.
camphor
Bell Activity
November 29, 2011
IUPAC Name
Common Name
Methanoic acid
Formic acid
Ethanoic acid
Acetic acid
Propanoic acid
Propionic acid
Butanoic acid
Butyric acid
Pentanoic acid
Valeric acid
Hexanoic acid
Caproic acid
Heptanoic acid
Heptylic acid
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Octanoic acid
Caprylic acid
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Nonanoic acid
Pelargonic acid
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Decanoic acid
Capric acid
Chapter 15
Chemistry II Bell Activity
November 29, 2011
• What is the structure of the carboxylic acid
functional group? How does it differ from the
structure of an alcohol and from that of an
aldehyde or a ketone?
• What is the latin term given to acetic acid?
• Why are carboxylic acids generally called fatty
acids?
• What is a familiar physical property
characteristic of carboxylic acids? Give an
example and tell where it comes from.
Chemistry II Bell Activity
November 30, 2011
• What is the reason why the common names are
They were discovered
used more often that IUPAC naming? before IUPAC came into
existence.
• What was formic acid isolated from? Red ants
• What was caproic, caprylic, and capric acids first
isolated from? Goat fat secretions (perspiration)
• What ending is used in naming a CA with more
than one double bond present?
Dieneoic acid
• Describe the boiling points of CA’s.
They have the highest b.p. of any functional group studied
Chemistry II Bell Activity
December 1, 2011
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List the common names for CA’s #’s 1-5
A species made of two identical units
What is a dimer?
Where does “locker room odor” come from?
What is the most important commercial CA?
Show the equation for producing vinegar.
Sugar -----------> acetic acid
+
Butyric acid
Acetic acid
carbon dioxide
• Where is most industrial acetic acid produced from and
show the equation for producing it?
Acetylene; acetylene -------------> acetaldehyde -------------> acetic acid
• What is the simplest dicarboxylic acid? What is its
IUPAC name?
Oxalic acid; ethanedioic acid
Chemistry II Bell Activity
December 8, 2011
• What
is the most characteristic property of CA’s?
Sour taste
• What is the simplest dicarboxylic acid? Oxalic acid
• This is used to cauterize gums when going to
the dentist. Trichloroacetic acid
• The term associated with the feeling of ants
crawling all over you. formication
• The acid that is produced in the muscles after
doing heavy exercise. Lactic acid
• The strongest organic acid Oxalic acid
Chemistry II Bell Activities
December 12, 2011
• This is an important preservative used to
inhibit the growth of mold and bacteria.
• Used as a preservative in cheese, bread,
and cakes
• Used to treat athlete’s foot
• Used for minor skin irritations such as
diaper rash, insect bites, acne, etc.
• Formed from a reaction between a CA and
an alcohol.
Sodium
benzoate
Ca/Na propionate
Zinc-10-Undecylenate
Aluminum Acetate
Ester
Chemistry II Bell Activity
December 13, 2011
• Give the name of the ester for the
following flavors:
– Rum Ethyl formate
– Banana Isopentyl acetate
– Orange Octyl acetate
– Pineapple Ethyl butyrate
– Apple Methyl butyrate
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What is esterification?
The synthesis of an alcohol and CA
• The great pain reliever with major drawbacks.
• The acid used to form aspirin.
Salicylic acid
aspirin
Chemistry II Bell Activity
December 14, 2011
• What is the disorder in children that is
caused by taking aspirin?
• What is the chemical name for aspirin?
• What is an acyl chloride?
• What is saponification?
• What are vasodilators?
• How is saponification(the process) carried
out?
Reye Syndrome
Acetylsalicylic
acid
Compound with a carbonyl group connected to
a chlorine
Soap making process
They enter the bloodstream and cause the smooth
muscles that line blood vessels to relax, which
lowers blood pressure
Carried out by the hydrolysis of glycerides which yields salts of the CA’s
and glycerol
Chemistry II Bell Activity
December 1, 2008
• Give the IUPAC or common name for the
ones listed:
– Methanoic acid
– Heptanoic acid
– Acetic acid
2-hydroxypropanoic acid
octanoic acid
valeric acid
• Which of the following groups would have the lowest
boiling point:
•Alkenes
esters
CA’s
• Draw the following structures:
•Lactic acid
acetylsalicylic acid ethanedioic acid
Chemistry II Bell Activity
December 14, 2011
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Define a syndet. Synthetic detergents
NaOH
What is another name for lye?
Is soap an organic or inorganic salt? organic
What does dialate mean? Make larger
Is saponification a base-catalyzed or acid
catalyzed reaction? Base-catalyzed
• In a detergent, which end would be considered
hydrophilic and which end would be
hydrophobic? Carbonyl end (hydrophilic) HC end (hydrophobic
• From what language are the common names of
CA’s derived? Latin
Chemistry II Bell Activity
December 3, 2008
• What is the other name for each of the
following: Do not use notes on this
– Acetic acid
-formic acid
– Formic acid
-oxalic acid
– Methanoic acid -heptanoic acid
– 2-hydroxypropanoic acid
– Caprylic acid
-pentanoic acid
– Butanoic acid
hexanoic acid
Chemistry I Bell Activity
March 7, 2008
The energy released when 1 mol of
an ionic crystalline compound is
formed from gaseous ions
• What is lattice energy?
• What are some properties of ionic compounds?
high melting/boiling points, conduct electricity, soluble in water
• What does the term “crystal” have to do with
ions in an ionic compound are organized
ionic compounds? The
into a crystal
• What are some properties of molecular
melting/boiling points, do not conduct
compounds? low
electricity, not soluble in water
• As light strikes the surface of a metal, what do
the electrons in the electron sea do?
Absorbs and re-emits light
Chemistry I Bell Activity
March 6, 2008
• How do you indicate resonance
structures? (hint: show the arrows)
With double-headed arrows
• What does the chemical formula for an
Simplest ratio of the combined
ionic compound represent? ions that balances total charges.
What is a molecular formula?
A formula that shows the types and numbers of atoms
combined in a single molecule
• What is a formula unit?
The simplest ratio of ions that balances
total charge.
Chemistry I Bell Activity
March 4, 2008
• What is the key to drawing a Lewis Dot
the number of valence electrons
structure? Knowing
in each atom
• How many valence electrons does the
ammonium ion contain? 8 valance electrons
• Which elements will most likely form
multiple bonds? Carbon, nitrogen, or oxygen
• What do the charges tell us about the
polyatomic ions? They tell us how many electrons the
ion has lost or gained
Chemistry I Bell Activity
March 3, 2008
• Which of the groups of atoms do not need to
Noble gases
satisfy the octet rule?
• When the octet rule is satisfied, which of the
sublevels are filled.
s and p orbitals
• When drawing the Lewis structures, which atom
would be the central atom?
Least
electronegative
• What determination can you make if there are
too many valance electrons to be used?
There will be one or more multiple covalent bonds
Chemistry I Bell Activity
February 26, 2008
•
•
•
•
group of atoms held together by covalent
Define a molecule. Neutral
bonds
Give an example of a molecular formula.
separation for which potential energy
What is bond length. The
is at a minimum.
How many electrons are needed in the
outermost energy level in order for a
compound to become stable? 8
• What does the octet rule state?
States that chemical compounds tend to form so that each atom has
an octet of eletrons in its highest occupied energy level.
H2O
Chemistry I Bell Activity
February 25, 2008
• What is an ionic bond?
• What is the difference in polar and
nonpolar molecules?
• What is shared in a covalent bond?
• Describe how you would determine
whether a compound is ionic or covalently
bonded?
• What is a molecule?
Attraction between positive & negative ions
Polar-shared electrons having an unequal attraction for
the electrons. .Non-polar—two covalently bonded
atoms are identical.
electrons
Take the chart on page 161 and subtract the elements, in the compound,
differences
A neutral group of atoms held together by covalent bonds.
Chemistry I Bell Activity
February 21, 2008
• What happens to the potential energy as
atoms bond to each other?
• Why do atoms form bonds?
• Before an atom combines with another
atom, what type of energy is present?
The potential energy
decreases making a more
stable arrangement of
matter.
To become more stable
A relatively high potential energy
• Why are valence electrons important in the
bonding process?
Because the way they are redistributed will determine the stability of the atom
Chem I Bell Activity
February 20, 2008
• A chemical bond results from the mutual
attraction of the nuclei for
•
A.
electrons.
•
B.
neutrons.
•
C.
protons.
•
D.
dipoles.
Ans. (A)
Chemistry I Bell Activity
January 30, 2008
• What is the mass (in grams) of each of the
following:
– 1.00 mol Li
6.022 x 1023 atoms C
How many moles of atoms are there in each of
the following:
– 3.011 x 1023 atoms Mg
– 3.25 x 105 g Pb
Chem I Bell Activity
January 31, 2008
• What is the mass in grams of each of the
following:
– A.
– B.
– C.
– D.
– E.
– F.
a) 9.500 g
3.011 x 1023 atoms F
1.50 x 1023 atoms Mg (b) 6.05 g
4.50 x 1012 atoms Cl (c) 2.65 x 10-10 g
8.42 x 1018 atoms Br (d) 1.12 x 10-3 g
25 atoms W (e) 7.6 x 10-21 g
(f) 3 x 10-22 g
1 atom Au
Chemistry I Bell Activity
February 4, 2008
•
•
•
•
•
Ans:
5.00 mole Zn = _____atoms Zn
20.0 X 1046 molecules H2O = ___mol HOH
1.50 mol Ca = ___ g Ca
6.75 mol Cu = ___atoms Cu
1.75 x 1015 atoms K = ___ g K
Chemistry I Bell Activity
February 5, 2008
•
•
•
•
•
•
15.0 x 1023 atoms Zn = ___ g Zn
878 g O = ___ atoms O
125 g Cr = ___ atoms Cr
4.75 x 106 atoms Al = ___ g Al
5.88 moles Na = ___ atoms Na
3.01 x 1023 molecules CO2 = ___ mole
CO2
Bell Activity
January 14, 2008
•Scientific and technological advances
are constantly changing how people
live and work. Discuss a change that
you have observed in your lifetime and
that has made life easier or more
enjoyable for you.
Chem I Bell Activity
1-15-08
• If you find an element in nature in its pure
elemental state, what can you infer about
the element’s chemical reactivity? How
can you tell whether that element is a
metal or a nonmetal.
Possible answer: The element is relatively un-reactive. If it
were reactive, it would have combined with other elements,
such as oxygen in the air, to form compounds. If it is shiny,
malleable, and ductile, a good conductor of electrical energy,
and can transfer energy as heat well, it is probably a metal. If
it is a nonconductor, it is probably a nonmetal
Chem I Bell Activity
January 18, 2008
• 1. Calculate the density of a substance
with a mass of 24.3 grams and a volume
of 32.9 ml
• 2. What is the volume of an object with a
density of 1.25 g/ml and a mass of 281
grams?
• 3. A substance has a density of 0.876
g/ml and a volume of 25.6 ml. Find its
mass in grams.
Chemistry I Bell Activity
February 14, 2008
• What does Valentines Day mean to you
and who is that special person that you
need to tell “I Love You”. This could be a
parent, friend, sibling, etc.
Chemistry I Bell Activity
January 22, 2008
• Determine how many significant figures are in the
following numbers:
• 1.2080
• 35.8900
• 0.000000010
• 50000900
• 305.00009
• 0.00050304
• 10000
• 50000.
• 56.3234000
Chemistry I Bell Activity
January 23, 2008
•
•
•
•
•
•
•
•
•
Do the following problems:
4.271 g + 2 g + 10.0 g
8.35 m x 3.996 m
7 cm x 1.86 cm x .002 cm
4.6215 L / 0.0000150 L
0.4330 cm x 209,000 cm
6.078g + 0.3329g + 3.45g
94.20g / 3.16722g
18.623g – 0.75g
Chemistry I Bell Activity
February 6, 2008
•
1. How many grams are in 3.52 moles of sodium phosphate,
•
2. How many moles are in 225 g of potassium iodide, KI?
•
3. How many atoms are in 0.615 grams of sodium hydrogen carbonate
(sodium bicarbonate), NaHCO3.
•
4. 542 g of aluminum sulfate, Al2(SO4)3, is how many atoms?
•
5. Convert 2.56 moles of nickel chloride, NiCl2, to grams.
•
6. 2.50 moles of ethyl alcohol, C2H5OH, is how many grams?
•
7. Convert 1000 g of ammonium sulfate, (NH4)2SO4, to molecules.
•
8. You have 35.2 g of barium hydroxide, Ba(OH)2. How many moles is that?
Na3 PO4 ?
Chemistry I Bell Activity
February 7, 2008
• No bell activity due to test today.
• Are there any questions before we take
the test.
• Use a #2 pencil to work the problems
• Put all answers on the answer sheet
provided.
• Put a book bag between you and your
table buddy.
Chemistry I Bell Activity
February 8, 2008
1.
–
–
–
What is the principal quantum number?
How is it symbolized?
What are shells?
What are the sublevels or subshells?
2. How many orbital orientations are possible in
each of the s, p, d, & f sublevels?
3. List five examples of electromagnetic radiation.
Chemistry I Bell Activity
February 12, 2008
• We are going to do the following electron
configurations together. Write them down
so we can work on them.
– Carbon
– Magnesium
– Sulfur
– Chromium
– Bromine
– Lithium
potassium
calcium
nitrogen
gallium
neon
zinc
Chemistry I Bell Activity
January 24, 2008
• An object has a mass of 57.6 g. Find the
object’s density given that its volume is 40.25
cm3.
1.43 g/cm3
• A lab worker measures the mass of some
sucrose as 0.947 mg. Convert that quantity to
grams and to kilograms.
9.47 x 10-4 g;
9.47 x 10-7 kg
• A large office building is 1.07 x 102m long, 31m
wide, and 4.25 x 102m high. What is its
volume?
1.4 x 106m3
Chemistry I Bell Activity
January 28, 2008
• Consider the following statements:
– Young people should not smoke and;
– Smoking at an early age may make it more
difficult to quit smoking later.
Determine which statement is an opinion
(unsupported idea) and which is a theory
(uses reason to explain observations and
experimental data). Which is similar to
Aristotle’s statements? (Hint: read page 67)
Chemistry I Bell Activity
January 29, 2008
• Atomic mass of an element is a weighted
average of the masses of the naturally
occurring isotopes of that element.
Compare atomic mass with a weighted
average that you, as students, encounter
during your lifetime.
Chemistry I Bell Activity
March 10, 2008
• No Bell Activity today due to testing.
Chemistry I Bell Activity
March 11, 2008
• How many atoms are contained in the
formula Al2O3?
• List 3 formulas that would represent a
molecule?
• What would be the correct formula for the
compound containing potassium ions and
oxygen ions?
• What is the formula for aluminum
carbonate?
Chemistry I Bell Activity
March 12, 2008
• Name the following
compounds/molecules—use the correct
formula:
–
–
–
–
–
–
–
–
Iron II hydroxide
Ammonium sulfide
Antimony pentasulfide
Potassium permanganate
Lithium phosphate
Lead II acetate
Mercury I iodate
Potassium arsenate
aluminum nitride
nitrogen dioxide
zinc II sulfate
hydrogen acetate
nickel II chloride
gold III chloride
lithium oxide
strontium carbonate
Chemistry I Bell Activity
March 13, 2008
• Write the correct formulas for the following:
Chemistry I Bell Activity
March 24, 2008
Use the stock system to name the following compounds:
•CuCl2
•PbO
•SnI4
•PbO2
Write formulas with polyatomic ions for the following:
•Tin (IV) sulfate
•Sodium carbonate
•Potassium dichromate
•Ammonium hydroxide
Chemistry I Bell Activity
Quiz I, March 25, 2008
• Write the correct chemical formulas for the
following:
•
•
•
•
•
•
•
•
lead(II) carbonate PbCO
copper(I) sulfate Cu SO4
Fe S
iron(III) sulfide
dinitrogen trioxide N O
lithium carbonate Li CO
calcium nitrate Ca(NO )
ammonium sulfide (NH ) S
sodium sulfate Na SO
3
2
2 3
2
3
2
3
3 2
4 2
2
4
Chemistry I Bell Activity
Quiz II, March 26, 2008
•
•
•
•
•
•
•
•
•
•
•
•
•
•
•
1.
__________________ sodium chloride
2.
__________________ dinitrogen pentoxide
3.
__________________ potassium sulfate
4.
__________________ silver acetate
5.
__________________ chromium(III) nitrate
6.
__________________ ammonium carbonate
7. __________________ calcium hydroxide
8. __________________ mercury(II) nitrate
9. __________________ dinitrogen monoxide
10. __________________ ferric oxide
11. __________________ lead(II) chlorate
12. __________________ ammonium phosphate
13. __________________ zinc chloride
14. __________________ calcium phosphate
15. __________________ oxygen difluoride
Chemistry I Bell Activity
Quiz III March 27, 2008
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
__________________ iron(III) sulfate
__________________ chromium(III) oxide
__________________ dinitrogen tetroxide
__________________ ammonium nitrate
__________________ gold(III) bromide
__________________ carbon monoxide
__________________ potassium carbonate
__________________ cesium chloride
__________________ nickel(II) permanganate
__________________ aluminum sulfate
__________________ aluminum sulfite
__________________ barium acetate
__________________ manganese(III) hydroxide
Chemistry I Bell Activity
March 28, 2008
• Calculate the % Composition
•
•
•
•
HgO
Na2S
(NH4)2S
Sr(NO3)2
• Calculate the Empirical Formula
• Determine the empirical formula of a compound that
contains 36.5% sodium, 25.4% sulfur, and 38.1%
oxygen.
• A hydrated compound has an analysis of 18.29% Ca,
32.37% Cl, and 49.34% H2 O. What is the formula?
Chem I Bell Activity
March 31, 2008
• Define the first 10 vocabulary words from
chapter 8
Chemistry I Bell Activity
April 1, 2008
1. Fe +
H2S04
2. C2 H6 + O2
3. KOH
+
4. SnO2
+ H2
5. NH3 +
O2
Fe2 (SO4 )3
+
H2O +
CO2
H3PO4
K3PO4
Sn
NO
+
+
H2
+
H2O
H2O
H2 O
Chemistry I Bell Activity
April 2, 2008
6. KNO3
+
H2CO3
7. B2Br6 + HNO3
8. BF3 +
K2CO3 +
B(NO3)3
Li2 SO3
+
B2 (SO3)3
HNO3
HBr
+
LiF
9. (NH4)3PO4 + Pb(NO3)4
Pb3(PO4)4 +
NH4NO3
10. SeCl6
SeO2
Cl2
+
O2
+
Chemistry I Bell Activity
April 7, 2008
Complete & Balance the following:
1. Na2 SO4 + CaCl2 -->
2. C2 H6 + O2 -->
3. Fe + H2 O -->
4. Al2O3 -->
5. Ca(OH)2 + HF ----->
6. Pb(NO3)2 + K2CrO4 -------->
7. Zn + H2CO3 ---------->
Chemistry I Bell Activity
April 8, 2008
Use the Activity Series and predict whether of the possible reactions listed below
will occur. For the reactions that will occur, write the products and balance the
equation.
1. Cr + HOH --->
2. Pt + O2 ------->
3. Cd + 2HBr ----->
4. Mg + steam ----->
5. Ni + HOH ------>
6. Br2 + KI ------->
7. Au + HCl ------>
8. Cd + HCl ------>
9. Mg + Co(NO3)2 ------>
Chemistry I Bell Activity
April 9, 2008
• NO BELL ACTIVITY DUE TO TESTING
Chemistry I Bell Activity
April 10, 2008
• Write out the following equations from word form given—then
balance:
– Hydrogen and oxygen react under a specific set of conditions to
produce water.
– Ethane (C2H6) undergoes combustion.
– Sodium chloride is produced from its elements through a
synthesis reaction.
– As early as 1938, the use of NaOH was suggested as a means
of removing CO2 from the cabin of a spacecraft
Chemistry I Bell Activity
April 14, 2008
1. Given the following equation: 2 C4H10 + 13 O2 ---> 8 CO2 + 10 H2 O, show what the
following molar ratios should be.
a. C4H10 / O2
b. O2 / CO2
c. O2 / H2O
d. C4H10 / CO2
e. C4H10 / H2O
2. Given the following equation: 2 KClO3 ---> 2 KCl + 3 O2
How many moles of O2 can be produced by letting 12.00 moles of KClO3 react?
3. Given the following equation: 2 K + Cl2 ---> 2 KCl
How many grams of KCl is produced from 2.50 g of K and excess Cl2.
4. Given the following equation: Na2O + H2O ---> 2 NaOH
How many grams of NaOH is produced from 1.20 x 102 grams of Na2O?
5. Given the following equation: 8 Fe + S8 ---> 8 FeS
What mass of iron is needed to react with 16.0 grams of sulfur?