what is a chemical?
lithium perchlorate
alcohol - ethanol
water
What are the origins of chem?
technology
alchemy
natural philosophy
modern science
what is science?
observation, identification, description, experimental investigation, and theoretical explanation of natural phenomena.
chemistry?
science of the composition, structure, properties and reactions of matter, especially of atomic and molecular systems.
hypothesis?
trial explanation of certain facts that provides a basis for further experimentation.
Theory?
well established hypothesis.
an explanation of the general principles of certain phenomena w/ considerable evidence or facts to support it.
Law?
STATEMENT!
statement of natural phenomena to which no exceptions are known under the given conditions. A law is not an explanation.
what types of research exists?
applied research
basic research
Matter?
anything that has mass and occupies space
Mass?
quantity of amount of matter that an object possesses.
- fixed
- independent of the objects location
weight?
measure of the earths gravitational attraction for an object
- not fixed
- depends on objects location!
Properties of substances?
property = ?
property = characteristic of a substance
each substance has a unique set of .....that no other substance has.
properties
Physical properties?
taste
color
physical state
melting point
boiling point
chemical properties
ability of a substance to form new substances.
chemical properties do what?
they:
react
decompose
ex. gasoline burns, acid can corrode, iron can rust.
chemical change = ?
new substances are formed that have different properties and composition from the original material.
example of chemical change?
copper oxide from
-> copper & oxygen!
what is composed of discrete, tiny fundamental particles called atoms?
Matter
what are elements?
elements contain only one kind of atom!
what are compounds?
compounds contain two or more kinds of atoms.
matter exists in how many states?
three.
solid, liquid and gas
rigid substance with a definite shape?
solid
has a definite volume but takes the shape of its container
liquid
takes shape and volume of container?
gas
essentially incompressible?
solids
indefinite shape/ definite volume
liquids
particles are mobile, able to move around each other
liquid
indefinite shape and volume?
gas
compressible
gas
particles far apart and small compared to the volume they occupy
gas
has a definite, fixed composition?
Substance
examples of substances?
Na, Cl2, Al
aka pure substance!
element can or cannot be broken down into a simper substance?
cannot!
substances can or cannot be decomposed into two or more simpler substances?
they can...example:
water - can decompose into hydrogen and oxygen
table salt - sodium and chlorine
elements can or cannot be decomposed into simpler substances?
cannot!
smallest particle of an element that can exist?
Atom
smallest unit of an element that can enter into chemical reaction?
atom
how many symbols do elements have?
give an ex.
one or two
ex.
C for Carbon
Ba for Barium
For exam!
Memorize first 36 elements &
Ag, Sn, I, Xe, Ba, Au, Hg, Pb, U, Pu
...
what cannot be decomposed into simpler substances?
elements
what can be decomposed chemically into simpler substances?
compounds
2 types of compounds?
molecular and ionic
mixture has a composition that can be ?
varied
solutions are...?
mixtures
matter that is uniform in appearance and has the same properties throughout?
homogenous
pure substance?
water
mixture?
sugar and water
classification of matter
what is a pure substance?
what is a mixture?
always homogenous in composition
mixture - two or more substances and may be either homogenous or heterogenous
SCIENTIFIC NOTATIONS
...
scientific notation=?
6.022 x 10 (23)
length ?
meter
mass
kg
temp
kelvin K
time
seconds
substance
mole
electric current
ampere
luminous intensity
candela
what is mega?
10^6
kilo
10^3
deca
10^1
deci
10^-1
centi
10^-2
milli
10^-3
micro
10^-6
nano
10^-9
1 meter is how many inches?
39.37 inches
1 meter longer or shorter than a yard?
longer
how many millimeters in 2.5 meters?
...
1 inch = how many cm?
2.54
1 kg = pounds?
2.205lb
what is volume?
amount of space occupied by matter.
what is heat?
form of energy that is associated with the motion of small particles of matter
what is density
d= mass/ volume
~~~~CHAPTER 2~~~~~
...
law of conservation of mass
matter is neither created nor destroyed during a chemical change
atoms are rearranged instead.
what has a unique number of elements?
a compound.
what contains two or more elements combined in a definite proportion of mass?
a compound.
each element has what exactly?
an atomic number.
every atom w/ an atomic number of 1 is what kind of atom?
an hydrogen atom.
every hydrogen atom contains what?
1 proton in its nucleus.
every atom w/ an atomic number of 92 is what kind of atom?
a uranium atom.
atomic mass units
...
what is the mass of an hydrogen atom?
1.673 x 10 ^ -24
AMU?
atomic mass units
what is the atomic mass?
sum of p + n
(protons + neutrons)
~~~~Chapter 3~~~~~
...
Atomic structures
...
-> The discovery of ions <-
...
cathode?
negative electrode
anode
positive electrode
cathodes and anodes=?
ions
an ion always carries
a positive or negative electrical charge.
what are smaller particles than atoms?
subatomic particles
subatomic particles are...?
electrons
protons
neutrons
electrons have a ?
negative charge
form shell of atom
small mass
protons have a ?
positive charge
in of nucleus of atom
large mass
neutrons?
no charge
neutral
slightly more mass than proton
Ions?
...
general arrangement of subatomic particles
...
atomic number is equal to the number of ?
protons
AMU?
protons + neutrons
What are isotopes?
Same # of protons but different number of neutrons.
Isotopes of the same element have?
equal number of protons.
different number of neutrons.
hydrogen has three isotopes
1 proton, 0 neutron
1 proton, 1 neutron
1 proton, 2 neutron
mass number
protons and neutrons
Atomic number
number of protons
Atomic mass summary
...
elements do / do not have different isotopes?
elements do have different isotopes
each element does have/ doesn't have same # of protons?
has the same # of protons.
elements can/ cannot have different # neutrons
they can have different number of elements.
different number of neutrons make what?
different atomic masses.
amu (atomic mass) = ?
isotopic mass x abundance
for example?
62.9298 x 69.09 = 43.48 amu
mass number - atomic number=?
number of neutrons!
ex. (mass number = 109, atomic number 47)
109-47 = 62 -> number of neutrons
modern periodic table
...
chemical bonds (Ch.4)
...
what is chemical nomenclature?
system of naming chemicals
two classes of chemical names. what are they?
common names
systematic names
formula for the element is based on what?
based on the symbol of the element
sodium?
Na
Potassium?
K
Zinc
Zn
Argon
Ar
Mercury
Hg
Lead
Pb
Calcium
Ca
Naming cations
Na - Sodium - Na+
Ca- Calcium - Ca+
Lithium - Li+
Magnesium - Mg2+
Strontium - Sr2+
Naming anions
fluorine (F) - F- = Fluoride ion
chlorine (Cl) - Cl- = chloride ion
Bromine (Br) - Br- = bromide ion
anions ?
....ide ending!
brom(ide)
ox(ide)
...
when are ions formed?
metals combine w/ nonmetals!
H3PO4 - Indicate:
1. the elements
2. the atoms
1. elements: H - hydrogen,
P - phosphorus
O - Oxygen
2. Atoms: 3 H atoms
- 4 O atoms!
a chemical compound must have a net charge of?
0
what are binary compounds?
binary compounds contain two different elements
metal and non-metal
so what is a binary compound exactly? name three examples?
metal + non-metal + (ide ending)
Examples:
1. aluminum chloride AlCl3
2. aluminum oxide Al2 O3
3. hydrogen chloride HCl
what is:
NaCl
MgCl2
K2O
Na3P
NaCl - sodium chloride
MgCl2 - Magnesium chloride
K20 - Potassium oxide
Na3P - Sodium Phosphide
classical system!
...
metals suffixes are usually?
-ous and -ic
-ous = higher or lower charge?
lower
study tip: -lo = low
- ic
higher charge!
nonmetal names end w/?
-ide
lower charge examples?
copper - cuprous - lower charge
iron - fe2+ - ferrous - lower charge
lead - pb2+ - plumbous
higher charge examples?
Cu2+ - cupric - higher charge = ic ending!
Pb4+ - plumbic - higher charge = ic ending
stannous = Sn4+ = stannic = ic ending!
poly =
two or more
polyatomic ions means?
two or more elements
example for polyatomic ion?
NO-3
when naming a compound, name what first?
cation first (positive), then anion (negative)
example?
Na2CO3
ite like nitrite = ?
-ite = more ions
-ate?
less oxygen
per short for what?
hyper = more
example for per?
perchlorare = CL0-4
hypo -
less
example
hypochlorite = ClO-
four ions do not the ate = less and ite (more) system. Name all four ions.
1. hydroxide
2. cyanide
3. hydrogen sulfide
4. peroxide
three common positively charged polyatomic ions?
mercury(I) - HG2/2
Hydronium - H3O+
ammonium NH +4
Remember all polyatomic ions!
Page 106
mono?
1
di?
2
tri?
3
tetra?
4
penta?
5
hexa
6
hepta
7
octa
8
nona
9
deca
10
name 5?
penta
name 10
deca
name 9
nona
name 8
octa
name 6
hexa
name 3
tri
name 2
di
dinitrogen trioxide
N2O3
PCl5
phosphorus pentachloride
dichlorine heptaoxide
Cl2O7
Cl2O3
dichlorine trioxide
N2O3
dinitrogen trioxide
CCl4
carbon tetrachloride
phosphorous triiodide
PI3
Mgl2
magnesium iodide
Lewis Structures of Atoms
...
valence electron structure
usually 8 electrons
valence electrons
the electrons that occupy the outermost energy level of an atom.
Review page 60 PPT chapter 4
...
what is an ionic bond?
transfer of electrons from one atom to another
covalent bond
sharing electrons
what is a chemical?
lithium perchlorate
alcohol - ethanol
water
What are the origins of chem?
technology
alchemy
natural philosophy
modern science
what is science?
observation, identification, description, experimental investigation, and theoretical explanation of natural phenomena.
chemistry?
science of the composition, structure, properties and reactions of matter, especially of atomic and molecular systems.
hypothesis?
trial explanation of certain facts that provides a basis for further experimentation.
Theory?
well established hypothesis.
an explanation of the general principles of certain phenomena w/ considerable evidence or facts to support it.
Law?
STATEMENT!
statement of natural phenomena to which no exceptions are known under the given conditions. A law is not an explanation.
what types of research exists?
applied research
basic research
Matter?
anything that has mass and occupies space
Mass?
quantity of amount of matter that an object possesses.
- fixed
- independent of the objects location
weight?
measure of the earths gravitational attraction for an object
- not fixed
- depends on objects location!
Properties of substances?
property = ?
property = characteristic of a substance
each substance has a unique set of .....that no other substance has.
properties
Physical properties?
taste
color
physical state
melting point
boiling point
chemical properties
ability of a substance to form new substances.
chemical properties do what?
they:
react
decompose
ex. gasoline burns, acid can corrode, iron can rust.
chemical change = ?
new substances are formed that have different properties and composition from the original material.
example of chemical change?
copper oxide from
-> copper & oxygen!
what is composed of discrete, tiny fundamental particles called atoms?
Matter
what are elements?
elements contain only one kind of atom!
what are compounds?
compounds contain two or more kinds of atoms.
matter exists in how many states?
three.
solid, liquid and gas
rigid substance with a definite shape?
solid
has a definite volume but takes the shape of its container
liquid
takes shape and volume of container?
gas
essentially incompressible?
solids
indefinite shape/ definite volume
liquids
particles are mobile, able to move around each other
liquid
indefinite shape and volume?
gas
compressible
gas
particles far apart and small compared to the volume they occupy
gas
has a definite, fixed composition?
Substance
examples of substances?
Na, Cl2, Al
aka pure substance!
element can or cannot be broken down into a simper substance?
cannot!
substances can or cannot be decomposed into two or more simpler substances?
they can...example:
water - can decompose into hydrogen and oxygen
table salt - sodium and chlorine
elements can or cannot be decomposed into simpler substances?
cannot!
smallest particle of an element that can exist?
Atom
smallest unit of an element that can enter into chemical reaction?
atom
how many symbols do elements have?
give an ex.
one or two
ex.
C for Carbon
Ba for Barium
For exam!
Memorize first 36 elements &
Ag, Sn, I, Xe, Ba, Au, Hg, Pb, U, Pu
...
what cannot be decomposed into simpler substances?
elements
what can be decomposed chemically into simpler substances?
compounds
2 types of compounds?
molecular and ionic
mixture has a composition that can be ?
varied
solutions are...?
mixtures
matter that is uniform in appearance and has the same properties throughout?
homogenous
pure substance?
water
mixture?
sugar and water
classification of matter
what is a pure substance?
what is a mixture?
always homogenous in composition
mixture - two or more substances and may be either homogenous or heterogenous
SCIENTIFIC NOTATIONS
...
scientific notation=?
6.022 x 10 (23)
length ?
meter
mass
kg
temp
kelvin K
time
seconds
substance
mole
electric current
ampere
luminous intensity
candela
what is mega?
10^6
kilo
10^3
deca
10^1
deci
10^-1
centi
10^-2
milli
10^-3
micro
10^-6
nano
10^-9
1 meter is how many inches?
39.37 inches
1 meter longer or shorter than a yard?
longer
how many millimeters in 2.5 meters?
...
1 inch = how many cm?
2.54
1 kg = pounds?
2.205lb
what is volume?
amount of space occupied by matter.
what is heat?
form of energy that is associated with the motion of small particles of matter
what is density
d= mass/ volume
~~~~CHAPTER 2~~~~~
...
law of conservation of mass
matter is neither created nor destroyed during a chemical change
atoms are rearranged instead.
what has a unique number of elements?
a compound.
what contains two or more elements combined in a definite proportion of mass?
a compound.
each element has what exactly?
an atomic number.
every atom w/ an atomic number of 1 is what kind of atom?
an hydrogen atom.
every hydrogen atom contains what?
1 proton in its nucleus.
every atom w/ an atomic number of 92 is what kind of atom?
a uranium atom.
atomic mass units
...
what is the mass of an hydrogen atom?
1.673 x 10 ^ -24
AMU?
atomic mass units
what is the atomic mass?
sum of p + n
(protons + neutrons)
~~~~Chapter 3~~~~~
...
Atomic structures
...
-> The discovery of ions <-
...
cathode?
negative electrode
anode
positive electrode
cathodes and anodes=?
ions
an ion always carries
a positive or negative electrical charge.
what are smaller particles than atoms?
subatomic particles
subatomic particles are...?
electrons
protons
neutrons
electrons have a ?
negative charge
form shell of atom
small mass
protons have a ?
positive charge
in of nucleus of atom
large mass
neutrons?
no charge
neutral
slightly more mass than proton
Ions?
...
general arrangement of subatomic particles
...
atomic number is equal to the number of ?
protons
AMU?
protons + neutrons
What are isotopes?
Same # of protons but different number of neutrons.
Isotopes of the same element have?
equal number of protons.
different number of neutrons.
hydrogen has three isotopes
1 proton, 0 neutron
1 proton, 1 neutron
1 proton, 2 neutron
mass number
protons and neutrons
Atomic number
number of protons
Atomic mass summary
...
elements do / do not have different isotopes?
elements do have different isotopes
each element does have/ doesn't have same # of protons?
has the same # of protons.
elements can/ cannot have different # neutrons
they can have different number of elements.
different number of neutrons make what?
different atomic masses.
amu (atomic mass) = ?
isotopic mass x abundance
for example?
62.9298 x 69.09 = 43.48 amu
mass number - atomic number=?
number of neutrons!
ex. (mass number = 109, atomic number 47)
109-47 = 62 -> number of neutrons
modern periodic table
...
chemical bonds (Ch.4)
...
what is chemical nomenclature?
system of naming chemicals
two classes of chemical names. what are they?
common names
systematic names
formula for the element is based on what?
based on the symbol of the element
sodium?
Na
Potassium?
K
Zinc
Zn
Argon
Ar
Mercury
Hg
Lead
Pb
Calcium
Ca
Naming cations
Na - Sodium - Na+
Ca- Calcium - Ca+
Lithium - Li+
Magnesium - Mg2+
Strontium - Sr2+
Naming anions
fluorine (F) - F- = Fluoride ion
chlorine (Cl) - Cl- = chloride ion
Bromine (Br) - Br- = bromide ion
anions ?
....ide ending!
brom(ide)
ox(ide)
...
when are ions formed?
metals combine w/ nonmetals!
H3PO4 - Indicate:
1. the elements
2. the atoms
1. elements: H - hydrogen,
P - phosphorus
O - Oxygen
2. Atoms: 3 H atoms
- 4 O atoms!
a chemical compound must have a net charge of?
0
what are binary compounds?
binary compounds contain two different elements
metal and non-metal
so what is a binary compound exactly? name three examples?
metal + non-metal + (ide ending)
Examples:
1. aluminum chloride AlCl3
2. aluminum oxide Al2 O3
3. hydrogen chloride HCl
what is:
NaCl
MgCl2
K2O
Na3P
NaCl - sodium chloride
MgCl2 - Magnesium chloride
K20 - Potassium oxide
Na3P - Sodium Phosphide
classical system!
...
metals suffixes are usually?
-ous and -ic
-ous = higher or lower charge?
lower
study tip: -lo = low
- ic
higher charge!
nonmetal names end w/?
-ide
lower charge examples?
copper - cuprous - lower charge
iron - fe2+ - ferrous - lower charge
lead - pb2+ - plumbous
higher charge examples?
Cu2+ - cupric - higher charge = ic ending!
Pb4+ - plumbic - higher charge = ic ending
stannous = Sn4+ = stannic = ic ending!
poly =
two or more
polyatomic ions means?
two or more elements
example for polyatomic ion?
NO-3
when naming a compound, name what first?
cation first (positive), then anion (negative)
example?
Na2CO3
ite like nitrite = ?
-ite = more ions
-ate?
less oxygen
per short for what?
hyper = more
example for per?
perchlorare = CL0-4
hypo -
less
example
hypochlorite = ClO-
four ions do not the ate = less and ite (more) system. Name all four ions.
1. hydroxide
2. cyanide
3. hydrogen sulfide
4. peroxide
three common positively charged polyatomic ions?
mercury(I) - HG2/2
Hydronium - H3O+
ammonium NH +4
Remember all polyatomic ions!
Page 106
mono?
1
di?
2
tri?
3
tetra?
4
penta?
5
hexa
6
hepta
7
octa
8
nona
9
deca
10
name 5?
penta
name 10
deca
name 9
nona
name 8
octa
name 6
hexa
name 3
tri
name 2
di
dinitrogen trioxide
N2O3
PCl5
phosphorus pentachloride
dichlorine heptaoxide
Cl2O7
Cl2O3
dichlorine trioxide
N2O3
dinitrogen trioxide
CCl4
carbon tetrachloride
phosphorous triiodide
PI3
Mgl2
magnesium iodide
Lewis Structures of Atoms
...
valence electron structure
usually 8 electrons
valence electrons
the electrons that occupy the outermost energy level of an atom.
Review page 60 PPT chapter 4
...
what is an ionic bond?
transfer of electrons from one atom to another
covalent bond
sharing electrons