Download notes fill in File

Unit I -- Families of Chemical Compounds
Section-1
Compounds can be classified into ______________ based on their physical and
chemical properties
One such classification is _________ versus _______________
Acids
 ____________ taste - but DON’T use taste for ID of chemicals
 Affect the __________ of indicators (an indicator is a compound that
shows a definite color change when mixed with an acid or a base)
 Turns blue litmus paper to _______ (acid)
 Phenolphthalein is ______________ in acid
 React with ________ metals to form hydrogen gas and a metal compound
 Contain hydrogen  produces H+ ions when dissolved in _________
Therefore defined as a proton (H+) donor
The H+ ion reacts with water to form the hydronium ion H3O+
Not all hydrogen containing compounds produce H+ ions therefore not all
are acids
 3 most common acids are (know these formulas!)
These three are all STRONG acids
H2SO4 = __________ acid
HNO3 = ___________ acid
HCl = ___________________ acid
The more ionization occurring, the stronger the acid
Strong acids make good _______________ (substance whose water
solution conducts electricity)
These are all WEAK acids
HC2H3O2 = ____________ acid
H2CO3 = _______________ acid
H3BO3 = ______________ acid
Weak acids are ________________ electrolytes because they release
only a few H+ ions
Bases
 __________ taste - again do not ID chemicals by taste or touch
 _____________ to the touch
 Can be ______________ or corrosive
 Turns red litmus paper ____________ (base)
 Phenolphthalein turns from colorless to BRIGHT __________ in a base
 Emulsify (dissolve) fats and oils to form a ___________
 Produces OH- ion (______________ ion) when dissolved in water
The OH- ion combines with H+ ion to form ______________
Therefore bases are defined as a _______________ (H+) acceptor

Know the common bases…
These are ____________ bases
KOH = ____________ hydroxide
NaOH = ____________ hydroxide
Strong bases are ____________ electrolytes
These are _____________ bases
NH4OH = ________________ hydroxide
Al(OH)3 = _________________ hydroxide
Weak bases are ___________ electrolytes
When water is ionized, here is the reaction:
2H2O  H3O+ + OH-
Section-2
Solutions can be ___________, basic, or neutral
The pH scale is used to measure ____________ of a solution
The _______ of solution is a measure of the hydronium (H3O+) concentration
pH indicates how _________ a solution is
pH scale goes from 0 to 14
_____ is neutral (neither an acid or a base)
pH  7 = acid
The lower the number, the more _________
pH  7 = base
The higher the number, the more _________
An indicator is used to determine pH (litmus paper/phenolphthalein…. Other
indicators are pH paper, methyl orange, bromothymol blue, red cabbage juice,
and tea
The most accurate measurements are done with a pH ________
When acids react with bases, they form _________ compounds
A salt is a compound formed from the positive ion of a base and the negative ion
of an acid
Example H+Cl- + Na+OH-  H2O +
NaCl (Double replacement reaction)
Acid
base H+ and OH- salt
This is called a ____________________ reaction
Many salts formed this way are only slightly soluble in water or insoluble in water
They __________________ out of solution and remain in the solid phase (they
precipitate out of solution…. Therefore they are called ___________________)
__________________ = a solid substance that crystallizes out of solution and
remains in the solid phase
The process of forming of a precipitate is called _______________
Section-3
__________________ is in more than 15 million compounds
Compounds containing carbon are called ________________ compounds
All organic compounds contain carbon
Organic means "____________ _________ ___________" because scientists
once thought only "living" organisms could produce organic compounds (they
were wrong -- _________________ made urea in 1828…. It is an organic
compound)
All organic compounds contain carbon but not all carbon containing compounds
are organic -- some are __________________
(Examples: calcium carbonate, carbon dioxide, carbon monoxide (have carbon
but are not organic…. These are inorganic)
There are so many carbon compounds because of its ability to bond with
__________ and ___________ elements
Carbon forms ____________ bonds which occur in chains (straight or branched)
and rings (single or joined together)
The bonds can be ___________ (one pair of electrons), ___________ (two pair
of electrons), or _______________ (three pair of electrons) covalent bonds
The simplest organic compound contains just hydrogen and carbon (H and C)
These are called ____________________
_______________ compounds usually exist as gases, liquids, or low melting
point solids
They have _______________ odors and low boiling points
They do not conduct electricity (nonelectrolytes) and generally do not
___________ in water
_______________ formula = shows the elements in the compound and the # of
atoms of elements in the compound but does not show the arrangement
Example: H2O 1 molecule (2 H atoms and 1 O atom)
______________ formula = shows the kind, #, and arrangement of atoms in a
molecule (model of a molecule)
In a structural formula a dash (-) is used to represent the pair of electrons shared
forming the covalent bond
= is a double bond
= is a triple bond
Carbon has ___ valence electrons and needs ___ to fill the shell
When writing a structural formula you cannot have dangling bonds (dangling
dashes)… all must be filled!
H
Example: methane (the carbon has single bonds)

H-C-H

H
______________ = compounds with the same molecular formula but different
structural formulas
Example: Butane
and
Isobutane
H H H H
H HH
   
| | |
H-C-C -C-C-H
H-C-C-C - H
| |
|
|
/ | \
H H H H
C4H10
H C H
C4H10
/ | \
H HH
As the number of carbon atoms in a molecule ___________, the number of
isomers _____________
Section-4
__________________ = contain only H and C
Hydrocarbons are classified as ______________ and ______________
Saturated = all carbon bonds are ___________ covalent bonds
Unsaturated = one or more carbon bonds is a ___________ or _________
covalent bond
_____________ = straight chained or branched chain hydrocarbons where all
carbon bonds are single covalent bonds (saturated)
The simplest alkane is _____________ (CH4)
Each successive alkane has ___ more carbon and ___ more hydrogen
Example: ethane C2H6, propane C3H8… etc)
The general formula is CnH2n+2 where n=the # of carbons atoms in the alkane
All alkanes end in ______________
The __________ tells the # of carbon atoms
Meth = 1, Eth = 2, Prop = 3, But = 4, Pent = 5, Hex = 6, Hept = 7, Oct = 8,
Non = 9, Dec = 10
_______________ = hydrocarbons with at least one pair of carbon atoms joined
by a double covalent bond (unsaturated hydrocarbon)
The simplest alkene is ethene (C2H4) H
H
All alkenes end in -ene
\
/
The general formula is CnH2n
C=C
/
\
H
H
Alkenes are more _______________ than alkanes because a double bond is
more _____________ broken than a single bond
______________ = hydrocarbons with at least one pair of carbon atoms joined
by a triple covalent bond (unsaturated hydrocarbon)
The simplest alkyne is ethyne (C2H2) ethyne is also called acetylene
All alkynes end in -yne
The general formula is CnH2n-2
Alkynes are more reactive than alkenes because there is not much __________
needed to break a triple bond
Some hydrocarbons form _________ (instead of straight or branched chains)
These are called aromatic hydrocarbons
They have strong ___________ odors (aromas)
The basic structure is a ring of 6 carbon atoms joined by alternating single and
double bonds
The simplest aromatic hydrocarbon is benzene (C6H6)
H
|
C
// \
H-C C-H
/\
|
||
OR |O|
H-C C-H
\/
\\ /
C
|
H
Section-5
______________ hydrocarbon = formed when one or more hydrogen atoms in a
hydrocarbon chain or ring is ______________ by a different atom or group of
atoms
Example: alcohols, organic acids, esters, and halogen derivatives
________________ = (substituted hydrocarbons) have one or more hydrogen
atoms replaced by an
-OH group (hydroxyl group)
The simplest alcohol is methanol (CH3OH) (one of the Hydrogen atoms from
methane CH4 is replaced by OH)
_________________ is used to make plastic, synthetic fibers, gas de-icer, and
as a solvent
It is very _____________ (even externally)
All alcohols end in -ol
This ______________ is added to the name of the corresponding hydrocarbon
Example: ethanol C2H5OH is ethane C2H6  H to OH
Ethanol is produced by the action of _________ or _____________ on sugar
stored in grains
________________ is a good solvent for organic compounds that don't dissolve
in water
Ethanol is also used in ____________ and ___________ beverages
H H
| |
H-C - C-OH Ethanol
| |
H H
______________ alcohol = ethanol made unfit for beverage purposes by adding
____________ compounds such as methanol to it
Alcohols can be in rings or chains
___________ = alcohol formed by replacing one hydrogen atom in a benzene
ring with an -OH group
Phenol is used for preparation of _________ and as a _______________
___________ acids = (substituted hydrocarbon) one hydrogen is replaced by a
-COOH group (carboxyl group)
In the carboxyl group, one of the carbon oxygen bonds is a double bond C-OH
||
O
Examples of organic acids: formic acid (HCOOH) and acetic acid (CH3COOH)
_________ acid is the _________ organic acid
It is also called __________ acid and is found in _________ (in stinging nettle
plants and in some ants)
The ending -oic is added to the name of the corresponding hydrocarbon
However common names are used more frequently
__________ acid is also called ethanoic acid
It is found in ____________
__________ acid which is derived from propane (propanoic acid) is found in
________________ fruits
It is written C2H5COOH
Esters = formed when an ___________ and an ___________ acid combine
Esters have a pleasant ___________ and ______________
The sweet smell of __________ comes from esters (example: strawberries,
bananas, pineapples)
Many esters occur naturally but we can make synthetic esters too (for
_________ and ________________)
______________ derivatives = formed when the hydrogen in a hydrocarbon is
__________________ by a halogen (still a substituted hydrocarbon)
Example: methyl chloride CH3Cl, tetrachloroethane C2H2Cl4, and
dichlorodifluoromethane CCl2F2