GOOD DAY!
☺
OBJECTIVES:
▪ Perform simple nomenclature & illustration of
compounds & chemical reactions.
▪ List & categorize common everyday events &
their associated biochemical reactions.
▪ Generalize & apply the principles learned in
biochemistry by solving biochemical reactions.
BASICS
OF
BIOCHEMISTRY
C6H12O6 + 6O2 6CO2 + 6H2O + ATP
PHYSICAL SCIENCE
➢ They deal with properties of matter and the
interaction of energy to it.
LIFE SCIENCE
➢ They deal with the chemical processes related to
life processes, as well as the essential elements
and compounds necessary to life.
SPACE SCIENCE
➢ Allows astronomers to know more about the creation
of the Universe by tracing every element formed by
stars and galaxies, as well as the atomic and sub
atomic processes related to both fields.
EARTH SCIENCE
➢It has components of both Space and Life sciences, as
well as the development of the Earth itself and how it
has manifested itself through the years.
CHEMISTRY – first began as the study
of nature, and how these came to be.
Four (4) Classical Elements:
1.Fire
2.Air
3.Water
4.Earth
SOLID – is the
state of matter with a
defined appearance.
- It has its own
shape, and has very
little to no molecular
movement. Ex.
Diamond.
LIQUID – is the state of
matter with molecular
movement.
- Its movement is dictated
by how fast the liquid flows.
- It has no shape of its
own due to its loose
molecular structure. Ex.
Glass of lemon juice.
GAS – is the state of
matter with high molecular
movement.
- Its molecular structure
is looser than liquid.
- It behaves the same way
as a liquid. Ex. The air we
breathe.
PLASMA – is the state of
matter with a very high
molecular movement.
- Due to heat, a gas
becomes plasma due to the
energy it absorbs and
releases, making its
molecules move even faster.
- Ex. Is the neon light
fixture seen in restaurants.
THE ORGANIZATIONAL CHART OF MATTER
PURE SUBSTANCE – are substances that
are made up of only one kind of particles and
has a fixed or constant structure.
MIXTURES - is a material made up of two or
more different Chemical substance/substances
which are not chemically combined.
COLLOID - is a mixture with a distinct
formation. It has two substances:
1. MEDIUM – the substance responsible for
holding the dispersed material.
2. DISPERSED MATERIAL – the substance
mixed into the medium.
HETEROGENOUS MIXTURE - is a mixture
with poorly mixed composition. Its components are
easy to recognize.
HOMOGENOUS
MIXTURE – better
known as a solution.
- is a mixture with even
composition between
substances.
- This may start as a
heterogenous mixture, but
in time, it will turn into a
homogenous mixture.
ELEMENT- is a substance made up of one kind
of atom.
COMPOUND - is a substance made up of one
kind of molecule, which is made up of 2 or more
different elements.
- An example is carbonic acid, found in soft
drinks (H2CO3)
THE PERIODIC TABLE OF ELEMENTS
- The periodic table is divided
mainly by Families.
- Families - elements in a
column in the periodic table.
THE PERIODIC TABLE OF ELEMENTS
- The older International Union of
Pure & Applied Chemistry (IUPAC)
system would use Roman numerals &
letters to differentiate the families.
However the modern IUPAC makes use
Arabic numbers which simply numbers
the columns 1 to 18.
However the modern IUPAC makes use of ARABIC
NUMBERS which simply numbers the columns 1 to 18.
GROUPS in the periodic table.
- Same group have similar properties,
Two (2) main parts of a Periodic Table
1.Period / Series – horizontal row
- Horizontal rows on the periodic table which
corresponds to the number of valence electrons.
2.Group / Families – Column
- Vertical columns on the periodic table which shares
similar chemical properties.
Horizontal - H
Vertical - V
POLAR COVALENT BOND - >0.5
Ex. HCl
3.0-2.1=0.9
NON-POLAR COVALENT BOND – <0.5
Ex. Cl2
3.0-3.0=0
BIOCHEMICAL REACTIONS
Chemical Equation – written to see
which elements were transformed &
affected.
- In writing a chemical equation, the
reactants are written on the left-hand side
while the products are written on the right-
hand side.
CHEMICAL REACTION
- is a process through which one (1) or more
substances are changed into different substances.
- The original substances are known
as reactants, and the resulting substances are
known as products.
Examples of Chemical Reactions
REACTANTS PRODUCTS
COEFFICIENT
# OF ATOMS
SYMBOLS IN CHEMICAL EQUATIONS
Here are some ways to see that
chemical reactions occur:
1. Bubble formation – indicates gas formation
2. Visual changes from transparent (or
translucent) to cloudy (or opaque) - indicates
formation of solid substance
3. Changes in temperature - sometimes
accompanied by the formation of light (or fire),
indicates chemical reaction
CHEMICAL EQUATIONS
1. can also be written in word format.
2. In this case, the chemical symbols are instead
replaced by their word counterparts.
3. This format only represents the qualitative
meaning of the reaction, identifying only the
reactants and the products -- without their quantities.
TYPES OF REACTION
Composition/Synthesis Reactions – multiple
reactants, such as element A and B, interact with
each other to form element a single product,
compound AB.
Ex. A + B → AB.
TYPES OF REACTION
Displacement Reactions – where the reactants
are have more than one (1) element, such as
element A and BC, interact with each other by
swapping one (1) of the elements.
- The general formula for composition
reactions is: A + BC = AB + C
TYPES OF REACTION
Reduction-Oxidation (Red-ox) Reactions –
- Transfer of electrons between two species.
- An oxidation-reduction reaction - which
the oxidation number of a molecule, atom, or ion
changes by gaining or losing an electron.
Fe2O3(s)+2Al(s)→Al2O3(s)+2Fe(l)
TYPES OF REACTION
Decomposition Reactions – where one (1)
compound undergoes changes due to an
external factor that initiates the reaction
(temperature).
- It is broken down into its constituents &
releases energy as the bonds broken.
SODIUM Chlorine
(Na) (Cl)
SODIUM Chlorine
(Na) (Cl)
SODIUM Chlorine
(Na1+) (Cl-1)
(Na1+) (Cl-1)
Cl
Ca
Cl
Cl Cl1-
Ca Ca2+
Cl Cl1-
Cl
Ca
Cl
NAMING &
WRITING BINARY
IONIC COMPOUNDS
Binary IONIC Compound
- Compound formed from just “two (2)
elements”.
- the first element named is the metal –
cation followed by the non-metal-anion.
In naming Binary Ionic Compounds:
Rule: Write Cation as it is, followed by the
Anion with the suffix –ide.
Sodium & Chlorine Lithium & Bromine
Sodium & Chloride Lithium & Bromide
Take note: Do not put prefixes!
KBr
Potassium & Bromine
Potassium Bromide
The “ide” Nomenclature
Grp 4A
C – Carbon – Carbide (C4-)
Si – Silicon – Silicide (Si4-)
Grp 5A
N – Nitrogen – Nitride (N3-)
P – Phosphorus – Phosphide (P3-)
The “ide” Nomenclature
Grp 6A
O – Oxygen – Oxide (O2-)
S – Sulfur – Sulfide (S2-)
Se – Selenium – Selenide (Se2-)
Te – Tellurium – (Te2-)
Grp 7A
F – Flourine – Flouride (F1-)
Cl – Chlorine – Chloride (Cl1-)
Br – Bromine – Bromide (Br1-)
I – Iodine – Iodide (I1-)
Li3N
- Lithium Nitride
BaO
- Barium Oxide
TERNARY IONIC
COMPOUND
- consisting of three (3) elements.
Polyatomic Ion
LiOH
- Lithium Hydroxide
KCN
- Potassium Cyanide
KClO3
- Potassium Chlorate
K2CO3
- Potassium Carbonate
K2CO3
K + CO3 2-
K2CO3
Potassium Carbonate
AlPO4
- Aluminum Phosphate
Ca(ClO3)2
- Calcium Chlorate
Na2SO4
- Sodium Sulfate
WRITING CHEMICAL
FORMULA(Transition Metal):
1. Get the charge of all the atoms
involved.
2. Criss-cross the charges of the two atoms
to become the subscript of the other atom. If
the new subscript is 1, do not write anymore.
3. Keep the subscripts to the lowest
possible ratio.
EXAMPLES:
Iron (II) Chloride
- FeCl2
Fe2+ -
Cl + Cl -
FeCl2
EXAMPLES:
Iron (II) Phosphate
- Fe3(PO4)2
EXAMPLES:
Iron (II) Phosphate
- Fe3(PO4)2
EXAMPLES:
Iron (II) Nitrite
- Fe(NO2)2
EXAMPLES:
Tin (II) Cyanide
- Sn(CN)2
EXAMPLES:
Lead (II) Phosphate
-Pb3(PO4)2
Writing Ionic Formulas with Transition
Elements
Basic Concept of Writing Ionic Formulas
1. Iron (III) bromide
2. Aluminum (III) oxide
3. Copper (I) chloride
4. Zinc (II) oxide
Writing Ionic Formulas with Transition Elements
Basic Concept of Writing Ionic Formulas
1. Iron (III) bromide – FeBr3
2. Aluminum (III) oxide – Al2O3
3. Copper (I) chloride - CuCl
4. Zinc (II) oxide – Zn2O2 → ZnO
NAMING COMPOUNDS:
1. Write the Cation as it is. If your
cation is a transition metal, use the
suffix –ous for lower charge & -ic for
higher charge.
2. Write the Anion with the suffix –
ide regardless if the Cation is a
transition metal or not.
In naming Binary Ionic Compound (When
involving Transition metals, the only difference is the
Cation, the Anion remains with the suffix –ide.
Concept: Transition metal used as Cations can
have multiple charges.
Rule: Write the charge as Roman Numerals (called
stock system).
Copper1+ = Copper (I) Copper2+ = Copper (II)
Rule: lower charge = suffix -ous Rule: higher charge = suffix -ic
Cuprous Cupric
In writing chemical formula:
1. Get the charge of the two elements
involved.
2. Criss-cross the charges to become the
subscript of the other.
Sodium Chloride Potassium Oxide
1+
Na Cl 1- 1+
K O 2-
NaCl K2 O
If subscript is 1, do not write anymore
WRITING CHEMICAL FORMULA:
(When involving transition metals)
Ferric Oxide or Iron Ferrous Oxide or Iron
(III) Oxide (II) Oxide
3+ 2-
Fe O Fe2+O2-
Fe2O3 FeO
Let’s Try this! ☺
Basic Concept of Writing Ionic Formulas
1. Sodium Chloride
2. Magnesium Bromide
3. Potassium Oxide
4. Calcium Iodide
5. Lithium Sulfide
Let’s Try this! ☺ (ANSWERS)
Basic Concept of Writing Ionic
Formulas
1. Sodium Chloride - NaCl
2. Magnesium Bromide – MgBr2
3. Potassium Oxide – K2O
4. Calcium Iodide – CaI2
5. Lithium Sulfide – Li2S
COVALENT /MOLECULAR COMPOUND
- occurs two non-metal elements.
- Greek prefixes used in naming molecular compound.
Prefix Meaning
Mono 1
Di 2
Tri 3
Tetra 4
Penta 5
Hexa 6
Hepta 7
Oct 8
Nona 9
Deca 10
EXAMPLES:
CO2
- Carbon Dioxide
CO
- Carbon Monoxide
SO3
- Sulfur Trioxide
CCl4
- is called carbon tetrachloride
EXAMPLES:
Nitrogen Dioxide
- NO2
Dioxygen Difluoride
- O2F2
Sulfur Hexafluoride
- SF6
Selenium Monoxide
- SeO
