Matter and Its Properties: GEN Examples Of Chemical Property – Heat

CHEM of combustion, stability, reactivity,

relative activity, ionization, toxicity,
Matter flammability.
- Is anything that has mass and occupies • Sodium burns in oxygen to form sodium
space. peroxide Na2O2
- Everything on earth has a mass and takes • Alkaline earth metal dissolves in liquid
up space ammonia form a deep blue solution.
- Everything you see is matter.
Classification Of Matter
Properties of Matter ➢ Pure Substance
• Physical Property - A matter that has a definite composition
- Are those that can be measured and and distinct properties.
observed without changing the - Can be either an element or compound
composition of the substance.
- Divided into 2 Classification: • Element – simplest form of matter,
Intensive Physical Property composed of only one kind of atom. (H,
- Intrinsic property He, Li, Be)
- It does not depend on the size or amount • Compound – containing 2 or more
of the sample. kinds of atom chemically combined in
- Ex. Color, melting point, boiling point, a definite proportion by mass.
density, solubility, conductivity,
malleability, luster, and viscosity. ➢ Mixtures
- Composed two or more substances
Extensive Physical Properties
combined physically in variable
- Extrinsic Property proportions.
- Is those that can be affected by the size - Classified as Homogenous or
Heterogenous.
and amount of space
- Ex. Mass, volume, length, and shape Homogenous Mixture – “solution”, is
relatively uniform in composition; every
• Chemical Property portion of mixture is like every other
portion.
- Is the ability of a substance to react with Heterogeneous Mixture – varies from
other substance such as air, water, acid one position to another. Can be either
and base. suspension or a colloid.
• Suspension – consists of coarse particles 5. Decantation
which are visible to naked eye. Particles - Solid particles can settle first at the
are unstable since they settle down after a bottom.
short period of time. - The liquid which is called “supernatant”
• Colloids – consist of a dispersed phase or is poured into another container leaving
the substance that is dissolved or behind the solid particles.
scattered. Dispersing medium in which
the dispersed phase is spread. It exhibits 6. Centrifugation
the Tyndall Effect. - Mixture is poured into a special tube in
the centrifuge apparatus and can spin
Ways of Separating Mixture using centrifugal force.
1. Filtration - The spinning motion forces the
- Separating suspended solid matter from sediments to settle at the bottom.
a liquid.
- Causing the latter to pass through the 7. Chromatography
pores of substance called “Filter” - Separating of mixture by passing it in
- The liquid which has passed through the solution or suspension or as a vapor
filter is called “Filtrate” through a medium in which the
components move at different rates.
2. Magnetic Separation - Thin-Layer Chromatography – used
- Separating elemental metals from other for separating and identifying mixtures
particles in a mixture. that are or can be colored, especially
- This process makes use of magnet which pigments.
exerts magnetic force to attract metallic
particles and sets them apart from a Atoms, Molecules, And Ions
certain mixture.

3. Distillation Atoms – basic units of matter and the

- Separating a homogeneous mixture defining structure of elements.
composed of two substances with
different boiling points.
Dalton’s Atomic Theory
4. Evaporation 1. Each element is composed of extremely
- Converting liquid to gas.
small particles called “atoms”.
- A technique used to separate out
homogeneous mixture where there is 2. All atoms of given element are identical,
one or more dissolved salts. but the atoms of one element are different
- Separating technique that involves
from the atoms of all other elements.
heating the mixture until no more liquid
remains. 3. Atoms of one element cannot be changed
into atoms of a different element by
chemical reaction; atoms are neither
created nor destroyed in chemical
reactions.
4. Compound are formed when atoms of Atomic Number (Z) – is a number of protons
more than one element combine; a given in its nucleus. The atomic number also
compound always has the same relative specifies the number of electrons present.
number and kind of atoms. Atomic number – # of protons = # of
electrons
The Subatomic Particles
1. Electron Mass Number (A) – is the sum of the
- 1897, J.J Thomson investigated the numbers of protons and neutrons in its
nature of cathode rays, using cathode ray nucleus.
tube. Mass no. = # of protons + # of neutrons
- He concluded that the cathode rays No. of neutrons = Mass number - # of protons
consists of negatively charged particles
are called electron. Isotopes – are atoms with the same atomic
2. Proton number but different mass numbers.
- 1909, Ernest Rutherford worked on Elements with the same number of protons
the Gold foil Experiment but have a different number of neutrons. It
- He concluded that the central part of the forms through nuclear reactions.
atom (nucleus) has a very small volume,
yet massive and positively-charged Molecules – is a combination of at least two
particles called protons. atoms in a definite proportion, bound
together by covalent bonds. It can be either
3. Neutron diatomic or polyatomic.
- 1932
- James Chadwick • Diatomic – contains only two atoms ex:
- Set up and experiment of a thin sheet of H2 CO
beryllium with alpha particles. • Polyatomic – it contains more two than
- It was found out that the rays were two atoms ex: NH3
composed of the third subatomic
particle, the neutron. Ions – sometimes an atom can lose or gain
- Neutron is neutral charge and has a mass electrons. If this happens it becomes charged.
of almost equal to proton. These charged atoms are generally called
ions.
Letter/s symbolizes each Elements: H, He, • Cation – lose electrons becomes
Li, C, O, N positively charged ion.
• Anion – it becomes negatively charged
ion.
 Chemical Formulas and Naming of Lewis Dot Symbols
Compounds - Are diagrams that represent the valence
electrons of atoms within a molecule.
Chemical Formula
- Written chemical structure of a
compound.
- It is made up of the elements and its
corresponding relative number in a
compound.

• Examples:
Compound: Water
Chemical Formula: H2O

Compound: Glucose
Chemical Formula: C6H12O6
Example:
Chemical Formulas Compound: Ammonia
Chemical Formula: NH3
1. Molecular Formula
- Indicates the actual number of each
element in a compound

2. Empirical Formula Molecular Model

- Is the simplest chemical formula. - A scale model showing the arrangement
- It only shows he relative ratio between of atoms in a molecule
the number of atoms of different
Ball and stick Model
Compound Molecular Empirical - Shows the geometric arrangement of the
Formula Formula
Benzene C6H6 CH
atoms with atomic sizes
Glucose C6H12O6 CH2O
Ammonia NH3 NH3 Space-filling Model
- Shows the relative sizes of atoms, the
Structural Formula atoms are represented by connected balls.
- It gives the same information as its
molecular formula and shows how the
atoms are bonded to one another in a
molecule

Example:
Compound: Ammonia
Chem Formula: NH3
Structural formula: H-N-H
H
Naming of Compounds • Stock Method
- The metal ion with variable charge is
Nomenclature named using its English name followed
- Set of rules used for forming the names or by the value of charge (oxidation no.)
terms in a particular field of arts and written in Roman Numeral.
sciences. - Ide
- The way in which compounds are named,
is based on their formula Covalent compound
Ionic Compounds - Are form by the reaction of non metals
- Are made of cations (metal) and anion - The names of the elements are written in
(non-metal) the order in which they appear in the
- The name of cation appears first followed formula.
by the name of the anion.
The convention for naming covalent
1. Binary Compounds compound below:
- Contains only two elements
- The positive ion (cation) retains the same - Prefix indicating the number of each kind
name as the element while, the negative of atom found in the unit is placed before
ion (anion) is named by using stem of the the name of the element.
name of element joined to suffix – ide - If only one atom of a particular kind is
present in molecules, the prefix mono- is
• Criss-cross-rule omitted from the first element.
- The oxidation number of cation becomes - The stem name of the last element is used
the subscript of the anion and the with the suffix ide
oxidation number of the anion becomes
the subscript of cation. 1. Mono
2. Di
2. Ternary Compounds 3. Tri
- Contains three elements 4. Tetra
- The cation goes first in its name before 5. Penta
the polyatomic ion which usually ends 6. Hexa
with 7. Hepta
8. Octa
3. Compounds with metallic Ion of 9. Nona
Variable Charge 10. Deca
- Contains metal cation with variable 11. Undeca
charge and anion 12. Dodeca
- There are two method that can be used to
name this compound namely: the Ternary Compounds
classical method and stock method. - Contain hydrogen, oxygen, and other
element.
• Classical Method
- It used Latin name of some metal ions For oxyanions – ending: ate change to ic follow
with variable charge and modified by the word acid
For Oxyanions – ending: ite change to ous follow
adding the suffix
the word acid