Atoms-and-the-Periodic-Table inorganic chemistry.pptx

ATOMS AND THE
PERIODIC TABLE
1 BSED – SCIENCE
TOPIC 1

ATOMS, SUBATOMIC
PARTICLES, AND
ATOMIC STRUCTURE

Inorganic vs. Organic
Question: Is it under inorganic chemistry or
organic chemistry?

Video link:
https://youtu.be
/v48u8hjqNBU?
si=YhFlGGzXHrT
Tux36

ATOMIC THEORY
It is the scientific concept that matter
is composed of small fundamental
particles called atoms.

HISTORY OF ATOMS
Before 1800s - Democritus
“ATOMOS”
- Ancient Greek word meaning “indivisible”
Along with Leucippus, they outlined the idea
that everything is made of atoms

HISTORY OF ATOMS
1803 - John Dalton: Solid Sphere Model
English chemist
- atoms are indivisible
- atoms of the same
element are identical
- compounds are
combinations of different
types of atoms

HISTORY OF ATOMS
1803 - John Dalton: Solid Sphere Model

HISTORY OF ATOMS
1897 - Joseph John (JJ.) Thomson:
Electron
English physicist
- proved that something smaller
than atoms existed: “corpuscle”

HISTORY OF ATOMS
1904 - Joseph John (JJ.) Thomson:
Plum Pudding Model

HISTORY OF ATOMS
1911 – Ernest Rutherford: Nucleus and
Proton
Physicist
- discovered the small, dense,
positively-charged center: “nucleus”

HISTORY OF ATOMS
1911 – Ernest Rutherford: Nuclear
Model

HISTORY OF ATOMS
1913 – Niels Bohr: Planetary Model
Danish physicist
- Modified Rutherford’s model
- electrons
- Electrons move around the
nucleus in orbits of fixed
sizes and energies.
- The energy in this model
was quantized

HISTORY OF ATOMS
1913 – Niels Bohr: Planetary Model

HISTORY OF ATOMS
1926 – Erwin Schrodinger: Quantum
Model
Australian physicist
- electrons behave as waves
rather than the electrons
moving in fixed orbits or
shells
- electron cloud or “cloud of
probability”

HISTORY OF ATOMS
1926 – Erwin Schrodinger: Quantum
Model

HISTORY OF ATOMS
1932 – James Chadwick: Neutron
- performed beryllium bombardment
experiments and discovered particles with
mass approximately equal to a proton but
without charge: neutron

SUBATOMIC PARTICLES
PROTON (p+
) - positively charged
- found in the nucleus, mass: 1.6726 x 10-27
kg
ELECTRON (e-
) - negatively charged
- orbits the nucleus, mass: 9.11 x 10-31
kg
NEUTRON (n0
) - no charge
- found in the nucleus, mass: 1.6749 x 10-27
kg

ATOMIC STRUCTURE
An atom consists
of a nucleus and
the associated
electrons that are
called orbital
electrons.

Video link:
https://youtu.be
/vxuBcOoGoD4?
si=VAgri8ZCzg_R
IM_s

CLASSIFICATIONS OF MATTER
Pure Substance Mixture
Element Compound

Choose the letter of the correct answer.
1. What subatomic particles are within an
atom's nucleus?
A. Neutron and electron
B. Electron and proton
C. Proton and neutron
D. Proton, neutron, and electron

2. What subatomic particles orbit around the
nucleus?
A. Protons
B. Neutrons
C. Electrons
D. Protons and neutrons

3. What do you call the outermost electrons?
A. Electrons
B. Nuclear model
C. Atomic structure
D. Valence electrons

4. What is the charge of an atom?
A. Electrically neutral
B. Electrically positive
C. Electrically negative
D. Sometimes positive, sometimes negative

5. The atomic number is unique for each atom,
therefore, there are no other atoms with the same
atomic number. True or false?
A. True, the atomic number is different with every atom.
B. True, the atomic number represents the atom's
electrons.
C. False, there are some that have the same atomic
numbers.
D. Both true and false, depending on the atom.

ATOMS AND THE
PERIODIC TABLE
1 BSED – SCIENCE
TOPIC 2

ACTIVITY: Element Rumble
Group yourselves into two (2)
groups and choose a representative to
represent your group, the participants
will participate in this activity with
similar rules to a gameshow named
Rainbow Rumble.

(Choose an element to uncover the hidden
questions)

ACTIVITY: Tongue Twister (QnA Edition)
The participants will read the tongue
twisters presented in front, depending on
how good he/she read the tongue twisters
the teacher will decide if the participant is
exempted to get questioned or not.

1.Periodic products promptly placed, prevent
perpetual perplexity.
2.Xenon and xenophilic xenonates exhibit
extraordinary, exotic electron exchanges.
3.Phosphorus and platinum playfully
participate, producing patterns.

Q. There are 5 types of metals, give me at least 2
Q. The atomic number of an element is the(?)
______________
Q. What type of element the elements are in the
last column?
Q. How many periods are there in the periodic
table?
Q. How many elements are currently found in
the Periodic Table?

Activity: Modified True / False
Identify whether the statements below are true or
false, if false underline the word that makes the
statement incorrect and write down the correct
answer.
_______1. I am Flourine and I am a Halogen
_______2. I am Lithium and I’m an alkaline
earth metals.

_______3. I am Zinc and my atomic
number is 31.
_______4. We are the group 18
known as the noble gas.
_______ 5. We are the Alkali metals
the most reactive of all groups.

PERIODIC TABLE
Most chemical elements are represented
symbolically by two letters, generally the
first two in their name. A very few
elements have symbols which appear to
have no relationship with their names. In
those cases, the origin of the symbol used
is given.
Basic Structure

e.g.
Au derived from the latin
word “Aurum”
Pb derived from the latin word
“Plumbum” meaning liquid
silver

Atomic Number
The atomic number of an
element is the number of protons in the
nucleus of an atom of that element. It
is a fundamental property that defines
the identity of the element.

Key Points
hydrogen has an atomic number of 1,
meaning it has one proton in its nucleus,
while carbon has an atomic number of 6,
meaning it has six protons.

The periodic table, organizes all
discovered chemical elements in rows
(called periods) and columns (called
groups) according to increasing atomic
number.

Periodic Trends
Periodic trends are specific patterns observed
in the periodic table that illustrate various
properties of elements. These trends arise
due to the arrangement of elements in the
periodic table and their atomic structure.

1. Atomic Radius: This is the distance
from the nucleus of an atom to its
outermost electron.
2. Electronegativity: This measures an
atom's ability to attract and bind
with electrons.

3. Ionization Energy: This is the energy
required to remove an electron from an atom.
4. Electron Affinity: This is the energy change
when an electron is added to a neutral atom.
5. Metallic Character: This refers to how
easily an element can lose electrons.

Types of Elements
1. Metals:
- Alkali Metals: Highly reactive, found in
Group 1 (e.g., Lithium, Sodium).
- Alkaline Earth Metals: Less reactive than alkali
metals, found in Group 2 (e.g., Magnesium,
Calcium).

- Transition Metals: Found in the center of
the table, known for their ability to form
various oxidation states (e.g., Iron, Copper).
- Post-Transition Metals: Softer and have
lower melting points than transition metals
(e.g., Aluminum, Tin).

2. Nonmetals:
- Halogens: Very reactive, found in Group 17
(e.g., Fluorine, Chlorine).
- Noble Gases: Inert and non-reactive, found
in Group 18 (e.g., Helium, Neon).
- Other Nonmetals: Include elements like
Carbon, Nitrogen, and Oxygen, which are
essential for life.

3. Metalloids:
- These elements have properties intermediate
between metals and nonmetals (e.g., Silicon, Boron).

ELECTRONIC CONFIGURATION
The electronic configuration of an atom
describes how its electrons are arranged in
different energy levels and orbitals, following
specific rules like the Aufbau principle, Pauli
exclusion principle, and Hund's rule.

Historical Development
Dmitri Mendeleev's
development of the periodic
table is a remarkable story
of scientific insight and
innovation.
In the mid-19th century,
many elements had been
discovered, but there was
no systematic way to
organize them.

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One of Mendeleev's key insights was
leaving gaps in his table for elements
that had not yet been discovered. He
predicted the existence and properties of
these elements with remarkable
accuracy.

Activity: Pass the Ball
In this activity, you can randomly pass the ball to
anyone until the music stops, the last person who have
hold the ball in time when the music stop is the person
who will answer the questions prepared.
(The music that will be played is the Periodic Table
Song)

Questions:
1. Based on Mendeleev’s amazing predictions
about the existence of some undiscovered
elements, do you think there is a possibility that
the current total of elements found can increase?
2. How useful the periodic table is? In your own
point of view.
3. What is the importance of familiarizing the
periodic trends?

Activity: Review
Answer the following questions.
1-3. What are the three principles applied in
identifying the electronic configuration of
an element?
4. Au is derived of what Latin word?
5. The specific patterns observed in the
periodic table that illustrates the elements.

ATOMS AND THE
PERIODIC TABLE
1 BSED – SCIENCE
TOPIC 3

ATOMIC NUMBER,
MASS NUMBER
AND ISOTOPES
TOPIC :

Activity 1: Let us remember
•What have you learned about the
topic periodic table?

Activity: Guess me! (charades for 7 minutes)
Objectives: Guess the words and phrases based on
the acting of a player.
Rules:
•Divide the class into 2 groups
•Per group must choose a best player to act, and
for members they will guess what is being act.
•The first group to guess 3 correct answer will
be declared as a winner.

Activity 3: “Name that thing (pictures and emoji
edition)”
+ 🎤 +
1.

EXPLORE
Activity 4: Get to know more
a) How did you find the activity?
b) What have you observed while doing the
activity?
c) Based on the information you have
gathered in the activity called “Name that
thing” what do you think is our topic for
today’s discussion

ATOMIC NUMBER
atomic number, the number of a
chemical element in the periodic system
and on the periodic table that equals the
number of protons in the nucleus of the
atom.

MASS NUMBER
The mass number is defined as the
total number of protons and neutrons
in an atom. It can be calculated by
adding the number of neutrons and the
number of protons (atomic number)
together.

(Mass number = atomic number + number of neutrons)
(atomic number-mass number = neutrons)

(Mass number = atomic number + number of neutrons)
(atomic number-mass number = neutrons)
4 = 2 + 2
2 - 4 = 2

ISOTOPES
A family of people often consists of related
but not identical individuals. Elements have
families as well, known as isotopes. Isotopes
are members of a family of an element that
all have the same number of protons but
different numbers of neutrons.

oxygen -16
8 protons and 8 neutrons
Oxygen -17
Oxygen -18

Two types of Isotopes:
1.Stable isotopes are non-radioactive forms of
atoms.
ex.
HYDROGEN
•Protium
•Deuterium

2. Unstable isotopes, also known as radioactive
isotopes, are atoms that have an unstable nucleus,
leading to the emission of radiation as they attempt
to reach a more stable state.
ex.
HYDROGEN
tritium

EVALUATE
In this application activity, students will
answer the following elements by finding it’s
atomic number, protons, neutrons and mass
number. Then don’t forget to write the
symbols of each element

1.Manganese
2. Arsenic
3.Titanium
4.Aluminum
5.Antimony
6.Lithium
7.Neon
8.Iodine
9.Tantalum
10.Barium

EXTEND
Multiple Choice (5 Points)
Instruction: Write the letter of the correct
answer.
1. The number of protons in an atom is
called?
A.Subatomic number B. Atoms
C.Atomic Mass D. Atomic Number
2. Protons + neutrons=?
A.Electrons B. Atomic Number
C.Mass number D. Isotopes

3. A family of people often consists of related
but not identical individuals.
A.Isotopes B. Carbon dioxide
C.Nuclei. D. Subatomic particles
4. Are atoms of the same element that have a
different number of neutrons in their nucleus?
A.Radioactive Isotopes B. nuclei
C.Stable Isotopes D. electrons

5. An isotopes that do not undergo nuclear
decay?
A. Unstable isotope B. Atomic number
C.Stable Isotopes D. mass number

ATOMS AND THE
PERIODIC TABLE
1 BSED – SCIENCE
TOPIC 4

• Explain what is meant by the atomic mass
of an element;
• Calculate the atomic mass of an element
from the masses and relative percentages of
the isotopes of the element; and,
• Appreciate the importance of obtaining the
average atomic mass.
Objectives

ACTIVITY: My Mass is...
Using your periodic table, identify the
atomic mass of the given elements below.
1.Helium
2.Carbon
3.Potassium
4.Manganese
5.Copper

ACTIVITY: 4 Pics, 1 Word
Guess the word that is being described or
portrayed by the pictures.
__ __ __ __ __ __ __

__ __ __ __
2.
__ __ __ __ __ __
__

Given below are the two (2) isotopes of
Chlorine

Video link:
https://youtu.be/dagoITYfEX0?si=cqJTyjx
mchLteshn

AVERAGE ATOMIC MASS
The average atomic mass of an
element is the weighted average of the
masses of its naturally occurring
isotopes. The average atomic mass of an
element can be determined from the
relative amounts of each isotope.

CALCULATING THE AVERAGE
ATOMIC MASS
Average atomic mass = (fractional
abundance of isotope 1)(atomic
mass of isotope 1) + (fractional
abundance of isotope 2)(atomic
mass of isotope 2) + …

Isotopes Abundance
(%)
Atomic
mass (amu)
Chlorine-35 75.76% 34.969
Chlorine-37 24.24% 36.366
Example:
Given below are the isotopes of chlorine.
Average atomic mass = (0.7576)(34.969) +
(0.2424)(36.366)
Average atomic mass = 35.453

Sample problem 1:
About 19.9% of all boron atoms are B-
10 with a mass of 10.0129 amu, and the
remaining 80.1% are 8-11 with a mass
of 11.0093 amu.

Sample problem 2:
A meteorite found in central Indiana contains
traces of the noble gas neon picked up from the
solar wind during the meteorite's trip through
the solar system. Analysis of a sample of the gas
showed that it consisted of 91.84% Ne-20 (mass
19.9924 amu), 0.47% Ne-21 (mass 20.9940
amu), and 7.69% Ne-22 (mass 21.9914 amu).
What is the average mass of the neon in the
solar wind?

ACTIVITY
Calculate the average atomic mass of the
following given data. Write your answer on a
piece of paper.
Isotopes
Abundance
(%)
Atomic
mass (amu)
Lithium-6 7.59% 6.015
Lithium-7 92.41% 7.016
1.

Isotopes
Abundance
(%)
Atomic mass
(amu)
Iron-55 14.50% 54.876
Iron-56 85.50% 55.998
2. Isotopes
Abundance
(%)
Atomic mass
(amu)
Hydrogen-1 99% 0.98
Hydrogen-2 0.80% 1.97
Hydrogen-3 0.20% 2.98
3.

Isotopes
Abundance
(%)
Atomic mass
(amu)
Gold-197 50% 196.56
Gold-198 50% 197.96
Isotopes Abundance (%)
Atomic mass
(amu)
Magnesium-24 78.70% 23.985
Magnesium-25 10.13% 24.986
Magnesium-26 11.17% 25.983
4.
5.

EVALUATE
Answer the following questions.
1. It is the weighted average of the masses of its naturally occurring
isotopes.
A. Atomic mass
B. Mass number
C. Atomic number
D. Average atomic mass
2. It refers to the percentage of abundance written in decimal form
A. Mass number
B. Atomic structure
C. Fraction abundance
D. None of the above

3. The necessary information in calculating the average atomic
mass is/are _______.
A. Isotopes
B. Atomic mass
C. Fractional abundance
D. All of the above
4. The first thing to do in calculating the average atomic mass is
_______.
C. add the atomic masses of the isotopes
D. Add the fractional abundance of the isotopes
C. multiply the first isotope’s fractional abundance with the
atomic mass
D. multiply the first isotope’s atomic number with the fractional
abundance

5. The mass number of the _______ isotope has
the closest value to the average atomic mass.
A. first
B. last
C. least abundant
D. most abundant

ATOMS AND THE
PERIODIC TABLE
1 BSED – SCIENCE
TOPIC 5

MOLE AND MOLAR
MASS
1 BSED - SCIENCE

IDENTIFY WHERE IS THE ATOMIC MASS,
ATOMIC NUMBER, AND SYMBOL
4.00260

Video Link: https://youtu.be/4q2elWPfB6A

MOLE
Mole is a counting unit used for
measuring an amount of a
substance. Mole comes from the
Latin word which means heap or
pile.

MOLE
A German
chemist named
Wilhelm Ostwald
created the term
mole in 1893.

AVOGADRO’S NUMBER
It is the number of
particles found in one mole
of a substance.
1 mole = 6.022×10 23
particles

Avogadro’s
number is named
after the Italian
scientist Amadeo
Avogadro.

1 mole of C
weighs 12.01g,
so 12.01 g of C
contains 6.022
x 1023
molecules

MOLAR MASS
is the mass (in grams) of one mole
of a substance. The molar mass of
any element is numerically equal to
its atomic mass and has the units
of g/mol.

Sample Problem 1: How many grams are equivalent to 5 moles of H2O?
Given:
n=5 mol
molar mass of H2O = 18 g/mol
Required: mass = ?
Formula: mass = n x molar mass

Sample Problem 1: How many grams are equivalent to 5 moles of H2O?
Solution: mass = n x molar mass
mass = (5 mole) (18 g/ mole)
mass = 90 g of H2O

Sample problem 2: How many moles are in 64 grams of Mg?
Given:
mass of Mg = 64 g
molar mass of Mg= 24g/mol
Required: number of moles or n = ?
Formula: n = mass of Mg
molar mass of Mg

Sample problem 2: How many moles are in 64 grams of Mg?
Solution: n = mass of Mg
molar mass of Mg
n = 64g
24 g/mol
n = 2.67 mol Mg

Sample problem 3: How many atoms are in 3 moles of Mg?
Given: n = 3 moles
N= 6.02 x 1023
atoms/mole
Required: no. of atoms of Mg = ?
Formula: no. of atoms = no. of moles x
Avogadro’s number

Sample problem 3: How many atoms are in 3 moles of Mg?
Solution: no. of atoms = no. of moles x
Avogadro’s number
= (3 moles) ( 6.02 x 10 23
atoms/ mole)
= 1.806 x 10 23
atoms Mg

FIND THE MOLAR MASS
1. C6H12O6
2. CCl4
3. H2O

Perform each of the following
conversions:
1.12.04x1023
atoms He to moles He
2.10 moles Na to mass
3.24 grams C to moles of C

Direction: Choose the letter of the best answer.
1. It refers to the SI unit for measurement of number of
particles in a substance.
A. ampere B. candela C. kilogram D. mole
2. Who among these chemists and physicists created
the term mole?
A. Amedeo Avogadro C. John Dalton
B. Jacques Charles D. Wilhelm Ostwald

3. Which of these values represent the number of
particles in one mole of a substance?
A. 6.02x10^22 C. 6.02x10^24
B. 6.022x10^23 D. 6.02x10^25
4. It is the sum of the atomic weights or mass number
of all the atoms in the formula of the substance.
A. Mole C. Avogadro’s Number
B. Molar Mass D. Atom

5. What is the mass of 2.5 mol CaCl2?
A. 420 g
B. 720 g
C. 120 g
D. 277 g

ATOMS AND THE
PERIODIC TABLE
1 BSED – SCIENCE
TOPIC 6

“Pass the Message!”
• Divide the class into two teams. Each
team lines up with their teammates.
• The facilitator assigns a unique sentence
(related to the new lesson) each team.
• Representatives pass the sentence down
the line; points awarded for correct
delivery at the front.

UNSCRAMBLE
Direction: Students will rearrange the
letters to form the correct word.
1. rcauenl imsethrcy
2. mboddbear
3. palha inssemio
4. noisfsi dan ufnois
5. aamgm yras

Video Link: https://www.youtube.com/watch?
v=U2ZNP5c58Rs

NUCLEAR CHEMISTRY
- is the study of the physical
and chemical properties of
elements which are influenced
by changes in the structure of
the atomic nucleus.

NUCLEAR REACTIONS
- is a process in which the
nucleus of an atom undergoes a
change, resulting in the formation
of a different element or isotope.

NUCLEAR REACTIONS
This change can occur through
various processes, such as
nuclear fission, nuclear fusion, or
radioactive decay.

FISSION
Nuclear fission is the process
in nuclear physics in which the
nucleus of an atom splits into
two daughter nuclei.

FUSION
fusion is when two or more atomic
nuclei fuse to form a single heavier
nucleus. In the reaction, the matter is
not conserved because some of the
mass of the fusing nuclei is converted
to energy.

Modern nuclear weapons are
made possible by a
combination of chemical
explosives, nuclear fission,
and nuclear fusion.

Video Link: https://www.youtube.com/watch?v=-
0Mg8Bu07fI&t=49s

RADIOACTIVE DECAY
is the spontaneous nuclear
transformations of unstable
atoms that result in the
formation of new elements.

RADIOACTIVE DECAY
This decay or loss of energy,
results in an atom of one type,
called the parent nuclide
transforming to an atom of a
different type, called the daughter
nuclide.

3 COMMON MODES OF
RADIOACTIVE DECAY

a. Alpha emission (α)
is a low-penetrating emission. An
alpha particle is a highly energetic
helium nucleus that is emitted from
the nucleus of an unstable atom
when the neutron-to-proton ration is
too low.

b. Beta particles (ß-)
are emissions having medium level
penetration. The resulting atom will
have an increase in the atomic
number by 1. There is no change in
the mass number.

c. GAMMA RAYS
commonly referred to as
highly penetrating and
dangerous emissions.
Gamma rays travel at the
speed of light.

MULTIPLE CHOICE
CHOOSE THE APPROPRIATE ANSWER OF EACH
QUESTION.
1. It is a process in which the nucleus of an atom undergoes
a change, resulting in the formation of different element or
isotopes?
A. Fission and Fusion
B. Radioactive Decay
C. Nuclear Chemistry
D. Nuclear Reaction

2. Two or more atomic nuclei combine to form a
single heavier nucleus.
A. Nuclear Fission B. Nuclear Fusion
C. Reaction D. Radioactive Decay
3. Is the study of the physical and chemical
properties of elements which are influenced by
changes in structure of the atomic nucleus?
A. Nuclear chemistry B. Radioactive Decay
C. Alpha emission D. Electron capture

4. A process in nuclear physics in which
the nucleus of an atom splits into two
daughter nuclei?
A. Radioactive Decay B. Plutonium
C. Nuclear Fission D. Atomic
Mass

5. This change can occur through the
process of nuclear fission, fusion and
radioactive Decay?
A. Carbon Dating
B. Radioactive process
C. Nuclear chemistry
D. Nuclear Reaction

6. It is the process in which an unstable
atomic nucleus spontaneously loses
energy by emitting ionizing particles and
radiation.
A. Radioactive Decay
B. Alpha emission
C. Gamma rays
D. Nuclear Reactions

7. Radium-226 can undergo radioactive decay
to form Radon-222. Which of the following is
the most likely type of particle that is emitted?
226 88Ra → 222 86Rn + 4 2He
A. Alpha emission
B. Beta particle
C. Gamma rays
D. Positron emission

8. Which of the following emissions
travels at the speed of light?
A. Gamma ray B. Beta particle
C. Alpha particle D. Antineutrino
9. Is a low penetrating emission
A. Nuclear Chemistry B. Positron
C. Alpha emission D. Beta particle

10. These are emissions having medium
level penetration.
A. Nuclear Chemistry
B. Positron
C. Alpha emission
D. Beta particle

Atoms-and-the-Periodic-Table inorganic chemistry.pptx

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