CHEMISTRY
Chemistry
- Deals with the study of matter and
its properties, composition,
reactions, structure, energy, and
particles
Matter
-
Anything that occupies space
and has mass
Three states of matter
Solid
- Has definite shape and
volume
Liquid
- Has indefinite shape but has
definite volume
Gas
- Has no definite shape and
volume
Properties of a Matter
1. Physical Properties
- Can be observed without
changing the composition of
a substance
Intensive Properties
- Melting, boiling, and freezing
point, density, color, physical
state and thermal
conductivity
Extensive Properties
- Mass, length, size, and
volume
2. Chemical Properties
- Can be observed with an
accompanying change in the
chemical composition
Ex.:
Flamability, toxicity
Classification of Matter
1. Pure substance
-Contains only one type of particle and has
same elements all throughout
1.1 Element
-
Composed of only one kind
of atom
1.1.1. Metal
- Good conductor of heat and
electricity
Ex.:
Na, Ca, Mg
1.1.2.
Non-Metal
- Poor conductor of heat and
electricity
Ex.:
C,N,O,S
1.1.3. Semi Metal/ Metalloids
- Elements which have both
properties of metal and non
metal
1.2.
Compound
- Composed of two or more elements
1.2.1. acid
- donates the H+ion in an aqueous solution
Ex.:
Vinegar, citrus fruits
1.2.2. base
- accepts the H+ion in an aqueous solution
Ex.:
Baking soda (NaOH), soap
1.2.3. salt
- formed when acid and heat
2. Mixture
- Made up of two or more
substances that are not
chemically bounded together
2.1.
Homogenous mixture
- A mixture that has a uniform
solution
- Can be classified as solution
Ex.:
Sugar and water
2.2.
Heterogenous mixture
- A mixture that has two or
more phases
- It doesn’t have a uniform
composition
2.2.1. Colloid
- Particle are evenly
distributed throughout the
mixture
- Particles are larger than the
particles of solution but
smaller than the particles of a
suspension
Ex.:
Mayonnaise, blood, fog, milk
2.2.2. Suspension
- Particles are bigger than
those particles of colloid
- Solid particles are settle
down
Ex.:
Sand and water
Filtration
-
-
It used to separate water
soluble from water insoluble
components
It requires filtering medium
(cheese cloth or filter paper)
Residue
- Are solid components that
remains in the filtering
medium
Filtrate
- The clear liquid collected
Ex.:
Silver chloride and potassium
nitrate
Sedimentation
- Heavy suspended particles are allowed to
settle at the bottom of the container
- Followed by decantation
Decantation
-A process of seperating a solid from a
liquid by pouring off the liquid after
sedimentation
Ex.:
Sand and water
Dissolution
- It is another method in which
a moxture of a soluble and
insoluble solid substances
can be seperated by using
appropriate solvent
Ex.:
Salt and sand
-
The process of changing
solid to gas form without
passing through the liquid
state
Ex.:
Napthalene and salt mixture
Distillation
-
A process whereby a liquid is
converted into vapor by
boiling and the vapor is
converted back to liquid
cooling
It is used if the impurities are not
volatile and the liquid compound
does not decompose
Fractional distillation
- it is used to separate two or
more liquids with different
boiling points
Crystallization
- A method to separate a
soluble solid from its solution
based from the different
solubility of solid in water at
25 degree celcius
Chromatography
- A process which utilizing the strategy that
lets the mixture flow over the materials at
different speeds
- it has two components:
• The mobile phase
• The stationary phase
Centrifugation
- aprocess of separation
mixtures by applying
centripetal force to a mixture
using a centrifuge machine
Use of magnet
-
It is used when separating
metallic and non-metallic
substances
Use of Separatory Funel
Sublimation
-
it is used to facilitate the
separation of liquid to liquid
mixture that did not mix
-
Refers to the degree to which
several measurement are
very close to each other
Evaporation
-It involves the application of heat to the
solution to allow the solvent to evaporate
leaving behind the solid component as a
residue
Rules in Counting the Significant Figure
1. Every non zero digit in a reported
measurement are SIGNIFICANT
2. Left most zeros before the first non
zero digit are NOT SIGNIFICANT, they
only get as a placeholder to show the
position of decimal pount
3. Zeros in between non zero digits are
significant
4. Zeros to the right of a non zero digit
and to the right of the decimal point are
significant
5. Zeros at the right modt end of a
measurement that lie to the left of an
“understood decimal point” are not
significant if they serve as placeholders.
If such zeros were known measured
values then they would be significant
Ex.:
1. 791.22=5
2. 0.00356=3
3. 310.009=6
4. 1000=1
Rules in Operations involving significant
figures
For ADDITION and SUBTRACTION

Least decimal place
For MULTIPLICATION and DIVISION

Least significant figure
Precision and Accuracy
Accuracy
- Measurement refers to the
how close the measured
values is to the true value or
accepted value
Precise
Dalton’s Atomic Theory
1. Matter is made up of extremely small
indivisible particles called Atoms
2. Atoms of the same element are
identical and are different from those of
other elements
3. Compounds are formed when atoms
of different elements combine in certain
whole number ratios
4. Atoms rearrange only during a
chemical reaction to form new
compounds
Fundamental/ Basic Laws of Matter
1. Law of Conservation of Mass
- States that in a chemical
reaction, matter is neither
created nor destroyed, or
more accurately, there is no
detectable change in mass
during an ordinary chemical
reaction
2. Law of Definitie Proportions
- States that different samples
of any pure compound
contain the same elements in
the same proportion by
mass
3. Law of Multiple Proportion
- States that the mass of one
element that can combine
with a fixed mass of another
element are in a ratio of
small whole numbers
Antoinne Lavoisier
-
Proponent of law of
conservation of mass
French chemist
Isotopes
-Same atomic number but different number
of neutrons
Joseph Louis Roust
- Proponent of law of definite proportions
- French chemist
Jonh Dalton
-
Proponent of law of multiple
proportion
British scientist
Subatomic Particles
1. Electron (e-)
- Was discovered by J.J
Thomson
- Negatively charged
- Plum pudding model
2. Proton (p)
- Was discovered by Ernest
Rutherford (gold foil
experiment) and Eugene
Goldstein (cathode ray tube)
- Positiveley charged
3. Neutron (n)
- Was discovered by James
Chadwick
Determining the number of p, n, e, in a
nuetral atom
Atomic number= no. of p= no. of e
Mass no.= no. of p + no. of n
No. of n= mass no. – atomic no.
Quantum Numbers
- Gives an information about
the atomic orbital where and
electron may be found
1. Principal quantum numbers (n)
- It indicates the energy level
or shell where an atomic
orbital can be found
2. Azimuthal quantum numbers (r)
- It specifies the sublevel
within a particular energy
level
3. Magnetic quantum numbers
- It indicates the specific orbital
within the sublevel where the
electron is found
4. Spin quantum numbers
- According to the Pauli
Exclusion Principle, only a
maximum two electrons can
occupy an orbital and they
must have opposite spins to
minimize repulsion between
them
lower energies than those
with highes energies
Hund’s Rules of Maximum Multiplicity
- States that for degenerate
orbitals, the electrons will
singly occupy each orbital
and with parallel spins before
they pair up
Electron Configuration
- Shows the distribution of
electrons among the orbitals
in an atom
Aufbau Principle
- States that electrons must
first occupy the orbitals with