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General- Chemistry-1- Reviewer
Dentistry (Iloilo Doctors' College)
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CHEM 1
GENERAL CHEMISTRY 1 REVIEWER
1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
CHEMISTRY
EXTENSIVE PROPERTY
EXAMPLE
Depend on the amount
of matter
Mass - the
measure of the
amount of matter
in an object. ∙
Volume - the
amount of space
occupied by an
object.
Weight - a
measure of force
that is equal to
the gravitational
pull on an object.
The study of matter, its properties, the changes
that matter undergoes, and energy associated
with these changes.
STATE OF MATTER
SOLID – has a fixed shape and volume. Solids may
be hard or soft, rigid or flexible.
ice cube, diamond, iron bar
LIQUID – has a varying shape that conforms to the
shape of the container, but a fixed volume.
gasoline, water, alcohol, blood
GAS – has no fixed shape or volume.
air, helium, oxygen
PROPERTIES OF MATTER
PHYSICAL PROPERTIES
PHYSICAL AND CHEMICAL CHANGE
it can be observed or measured without changing
the identity of the substance.
INTENSIVE
PROPERTY
EXAMPLE
Do not depend
on the amount of
matter.
Density - it is the mass of a
unit volume of a material
substance.
Boiling point - the
temperature at which the
vapor pressure of a liquid
equals the pressure
surrounding the liquid and
the liquid changes into a
vapor.
Other examples:
color, luster, odor,
hardness, malleability,
conductivity, ductility,
and melting point
CHEM 1
PHYSICAL CHANGE
changes in which no bonds are broken or formed
changes of state (changes from a solid to a
liquid or a gas and vice versa).
separation of a mixture.
physical deformation (cutting, denting,
stretching).
making solutions (special kinds of mixtures).
CHEMICAL CHANGE
occur when bonds are broken and/or formed
between molecules or atoms
Temperature changes
Light given off.
Unexpected color changes
Bubbles are formed
Different smell or taste
A solid forms if two clear liquids are mixed
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CHEM 1
GENERAL CHEMISTRY 1 REVIEWER
1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
PURE SUBSTANCE
matter with a definite chemical composition
CLASSIFICATION OF PURE SUBSTANCE
CHEMICAL FORMULAS
consists of chemical symbols of the elements present
in a substance with their respective quantities.
STEPS IN WRITING CHEMICAL FORMULAS:
ELEMENTS
COMPOUNDS
the simplest form of
pure substances.
It cannot be broken
down into simpler
substances.
made up of only one
atom type
composed of two or
more types of atom.
can be broken
down into simpler
substances by
chemical methods
Step 1: Convert each element to its corresponding
symbol.
Step 2: If there is only one atom for an element,
just write the symbol as it is. If there are two or
more atoms for that atom type, write the number
of atoms as a subscript of the symbol.
MIXTURES
matter with a definite chemical composition
Step 3: Combine the symbols and their subscript
(if applicable), without spacing.
CLASSIFICATION OF MIXTURES
HOMOGENEOUS
HETEROGENOUS
uniform throughout
Saltwater
Air
Sweet tea
not uniform in
appearance
rice pudding
rock and sand
oil water
CHEMICAL SYMBOLS
is a one or two-letter
representation of elements.
It must be written with the
first letter capitalized
CHEM 1
Substances and their Chemical Formulas
Sucrose
C12H22O11
Bleach (Sodium
hypochlorite)
NaOCl (or NaClO)
Agua oxinada
(Hydrogen peroxide)
H2O2
Rubbing alcohol
(Isopropyl alcohol)
C3H8O
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CHEM 1
GENERAL CHEMISTRY 1 REVIEWER
1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
SEPARATION TECHNIQUES
TECHNIQUES
DEFINITION
the insoluble matter
is separated from
the liquid with the
aid of a porous
material (e.g. filter
paper), while
allowing the liquid
to pass through it.
The separated
liquid is called the
filtrate, while the
separated materials
are called the
residue
FILTRATION
DECANTATION
The solids are
allowed to settle in
the container
before the liquid
(called decantate)
is slowly and
carefully poured
off, leaving the
residue in the
container
CENTRIFUGATION
CHEM 1
MAGNETIC
SEPARATION
SEPARATION USING
A SEPARATORY
FUNNEL
DISTILLATION
a heterogeneous
mixture is spun in a
machine, causing
the residue to
settle. After the
process, the liquid,
or the centrifugate,
can be removed by
simple decantation.
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the use of a
magnet to remove
selected metals like
iron, nickel, and
cobalt from a
mixture.
an apparatus used
to separate liquids
that do not mix
(immiscible liquids).
The liquid with the
higher density is at
the lower layer
while the liquid with
lower density floats.
To release the
lower layer, the
stopper and the
stopcock are
opened until only
the upper layer
remains inside the
separatory funnel.
the process in
which a liquid is
heated in a vessel
to become a gas,
then this gas is
condensed into
liquid upon passing
through a cooling
tube called a
condenser
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CHEM 1
GENERAL CHEMISTRY 1 REVIEWER
1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
SEPARATION TECHNIQUES
EVAPORATION
involves heating of
a mixture in an
evaporating dish to
cause removal of
the liquid
substance.
An example is a
homogeneous
mixture of water
and table salt.
CHROMATOGRAPHY
a method in which
substances in a
solution can be
separated by
loading the solution
on a material that
stays in place
(stationary phase)
and allowing a
liquid or gas
(mobile phase) to
carry the
substances.
LAW OF CONSERVATION OF MASS
The total mass of the products must be equal to
the total mass of the reactant.
In other words, mass cannot be created or
destroyed during a chemical reaction but is always
conserved.
SAMPLE PROBLEM:
1. How many grams of water vapor will form if 25.0
grams of hydrogen gas mixes with 12.0 grams of
oxygen gas?
2H2 (g) + 1O2(g)
2H2O(g)
1. Predict the minimum amount of nitrogen that will
react with 50.0 grams of hydrogen to produce
92.5 grams of ammonia.
Nitrogen + Hydrogen
Ammonia
Ans. 42. 5 N
LAW OF CONSTANT COMPOSITION
Different samples of a pure chemical compound
always contain the same proportions of elements
by mass.
Originated: In 1799, French chemist Joseph L.
Proust
Referred to as the "Proust’s Law of
Constant" or "Definite Composition"
Mass ratio: Proportions of elements by mass.
SAMPLE PROBLEM:
1. A compound contains only calcium and fluorine.
A sample of the compound is determined to
contain 2.00 g calcium and 1.90 g of fluorine.
According to the Law of Definite Proportions, how
much calcium should another sample of this
compound contain if it possesses 2.85 g of
fluorine?
Ans. 3.0 g Ca
LAW OF MULTIPLE PROPORTION
When 2 elements (A&B) form different compounds,
the mass of Element B that combine with 1 g of A
are a ratio of whole numbers.
Originated: In 1804, English chemist John
Dalton,
based on his Atomic Theory.
Ans. 37 g of water
CHEM 1
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CHEM 1
GENERAL CHEMISTRY 1 REVIEWER
1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
SAMPLE
PROBLEM:
SEPARATION
TECHNIQUES
1. Illustrate how nitrogen monoxide, NO and
nitrogen dioxide, NO2, obey the Law of Multiple
Proportions.
Ans. 2.286/1.142 = 2
ATOMIC THEORY
Atom from the Greek atomos, which undivided.
Dalton was able to take portions of Democritus
and Lavoiser’s ideas to fashion his theory.
First: Democritus (400 B.C.)
Modernized: John Dalton in (1803)
Dalton’s Atomic
Theory Postulates
1. All of matter is made
of atoms, which are
the smallest particles
of matter.
2. Atoms are indivisible
and therefore cannot
be created or
destroyed.
3. All atoms of a given
element are identical in
mass, size, &
properties.
4. Compounds are
made of 2 or more
different types of atoms
in fixed, simple, whole
number ratios.
5. A chemical reaction
is a rearrangement of
atoms.
CHEM 1
Modern Atomic Theory
1. All of matter is made
of atoms, which can be
further broken into 3
subatomic particles.
2. --------------3. Not all atoms of a
given element are
identical and exist in the
same form.
can have different
masses and
densities.
can connect in
different ways to
give rise to different
compounds.
4. Atoms don’t always
combine in fixed, simple,
whole number ratios.
They can be complex.
5.--------------
NAMING COMPOUNDS AND WRITING
FORMULA
A. IONIC COMPOUNDS
An ion is an atom or group of atoms with a net
positive or negative charge.
lons of opposite charges interact to form an
ionic compound.
An ionic compound is electrically neutral-the
sum of all charges of the cations and anions is
zero.
CATION - a positively charged ion
ANION - a negatively charged ion
BINARY IONIC COMPOUNDS
an ionic compound
which is made up
of two elements:
metallic
nonmetallic.
suffix –ide is
added for anions
MONOATOMIC IONS
POSITION ELEMENTS OF CATIONS
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CHEM 1
GENERAL CHEMISTRY 1 REVIEWER
1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
POSITION ELEMENTS OF ANIONS
OLD SYSTEM – the name of the metal is changed
by adding a suffix, either –ous or –ic, to the root of
the original Latin name of the metal.
–ous indicates the lower charge,
–ic indicates the higher charge.
NAMING IONIC COMPOUNDS
Separate the
formula into ions
Give the name of the
cation, followed by
the name of the
anions
NAMING POLYVALENT CATIONS
Write the formula for the cation and anion
For charges greater than 1, cross section the charges.
Reduce the subscripts of the cation and the anion to
their simplest whole number ratio
Separate the formula into ions
Give the name of the cation, followed by the name of
the anions
POLYVALENT IONS
two or more charge in cations (metals) and anions
(nonmetals)
POLYVALENT CATIONS
two or more charge in cations (metals)
STOCK SYSTEM – uses Roman numerals in
parentheses to indicate the charge.
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CHEM 1
GENERAL CHEMISTRY 1 REVIEWER
1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
COVALENT BOND
bond is formed by the sharing of electrons
between atoms
formed between two nonmetallic elements
NAMING COVALENT COMPOUNDS
1. Give the full name of the
first element.
NAMING POLYATOMIC IONS
Separate the formula into ions
Give the name of the cation, followed by the name of
the anions
WRITING FORMULAS FOR POLYATOMIC IONS
Write the formula for the cation and anion
For charges greater than 1, cross section the charges.
Reduce the subscripts of the cation and the anion to
their simplest whole number ratio
2. State the name of the
second element in which
the root word is retained
followed by suffix "-ide".
3. Add Greek prefix to both
names to indicate the
number of atoms. For the
first element, the prefix
"mono-" is no longer
written.
ACIDS
a compound that produces hydrogen ions (H+)
upon mixing with water
BINARY ACIDS
acids consisting of hydrogen attached to a
nonmetallic element
named with the prefix hydro- followed by the
stem of the nonmetal with suffix-ic and the word
acid attached.
For example, HCI is hydrochloric acid.
WRITING BINARY ACIDS
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CHEM 1
GENERAL CHEMISTRY 1 REVIEWER
1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
OXOACIDS BOND
RELATIVE ATOMIC MASS
acids consisting of hydrogen, oxygen, and another
element.
nonmetal that can form two oxyanions:
higher number of oxygen atoms = -ic ending + acid
fewer oxygens = -ous ending.
For example, HNO2 is nitrous acid and HNO3
is nitric acid.
the ratio of the mass of an element to the mass of
1/12 of a 12C isotope
NAMING OXOACIDS
being a ratio of masses, relative atomic mass is a
unitless quantity.
Separate hydrogen cation
from: the anion
Identify the name of the
anion
Follow this convention:
-ite = - ous
-ate = - ic
SAMPLE PROBLEM:
Given that the mass of an oxygen atom is
2.657 10-20 kg. what is its relative atomic
mass?
ATOMIC MASS
mass of an atom expressed in atomic mass units
(amu)
AVERAGE ATOMIC MASS
an element is the weighted average of the masses
of its naturally occurring isotopes.
It is so-called weighted average because the
relative abundance of each isotope is taken into
account
STOICHIOMETRY
SAMPLE PROBLEM:
area of study that deals with quantifying the
substances produced or consumed in a chemical
reaction
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FORMULA:
MOLE
the international system (SI) base unit for the
amount of substance
symbol = mol
atoms
1 mol Ar = 6.022 10^23
Ar atoms
molecule
1 mol H2O = 6.022 x
10^23 H₂O molecules
ions
1 mol Na= 6.022 10^23
Na+ ions
ionic compounds
1 mol NaCl = 6.022
1023 NaCl formula
units
other particles
1 mol e = 6.022 x 1023
e particles
The value 6.022 x 1023 is called the Avogadro's
number,
named after Amedeo Avogadro, an Italian
chemist,
postulated that two different gases at a given
temperature and pressure are equal in number
of molecules.
gram-mole (g-mol)
This unit is
normally used in
quantifying
relatively small
amounts of
substances
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CHEM 1
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1st SEMESTER 1st QUARTER 2023-2024 leomar ‘17 & Seuri
MOLAR MASS
the mass that an atom, or any substance, has in 1
mole
unit for molar mass = gram per mole (g/mol)
SAMPLE PROBLEM #2:
Calculate the molar mass of sodium
bicarbonate, NaHCO3
SAMPLE PROBLEM #2:
Calculate the molar mass of calcium
phosphate, Ca3(PO4)2
value of molar mass of an
atom in g/mole is EQUAL
to the atomic mass in amu
molar mass is the SUM of the molar
masses of all atoms presents
SAMPLE PROBLEM #1:
SUMMARY OF MOLAR MASS
Molar mass is the mass of 1 mole of a substance.
Calculate the molar mass of the elemental
nitrogen, N2
The molar mass of an atom in grams per mole is
the same as the value of atomic mass in atomic
mass units.
The molar mass of a substance with more than
one atom is the sum of the molar masses of all
atoms present.
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