[THE ATOM AND SUBATOMIC PARTICLES] Atomic Model & Nuclear Chemistry

Proverbs 16:3

Atom

[ATOMIC MODEL]

______ is the smallest identifiable unit of matter - identifiable meaning one can assign names to it ( the name being the element , e.g copper, hydrogen, carbon, etc)

• Proton

• Electron

• Neutron

[ATOMIC MODEL]

Today, smaller particles (the subatomic particles such as the ______ [3] ) exist but those have no unique names and are called the same way across all elements

Democritus

[ATOMIC MODEL]

Coined the term “atom” for the smallest identifiable unit of matter

John Dalton

[ATOMIC MODEL]

Formed the atomic theory (founded on the 3 fundamental laws of chemistry)

John Dalton

[ATOMIC MODEL]

Introduced the Billiard Ball Model that matter is made up of atoms as its basic unit

JJ Thomson

[ATOMIC MODEL]

Discovered the negatively -charged electrons via cathode ray tube experiments and assumed there are positive -charged particles balancing them out → plum pudding model

JJ Thomson

[ATOMIC MODEL]

He is known for the plum pudding model

Ernest Rutherford (with Hans Geiger and Ernest Marsden)

[ATOMIC MODEL]

Confirmed the positively -charged protons through gold foil experiments and proposed them to be concentrated in a small area (the nucleus) → nuclear model

Ernest Rutherford (with Hans Geiger and Ernest Marsden)

[ATOMIC MODEL]

He is known for the nuclear model

James Chadwick

[ATOMIC MODEL]

Discovered the uncharged neutrons by bombarding beryllium with polonium

Robert Millikan

[ATOMIC MODEL]

Measured the elementary electric charge (I.e. the real value “-1” or “+1” in coloumbs through the oil drop experiment)

Robert Millikan

[ATOMIC MODEL]

He is known for the oil drop experiment

Neil Bohr

[ATOMIC MODEL]

Proposed that electrons reside in energy levels/shells outside the nucleus → planetary model

Neil Bohr

[ATOMIC MODEL]

He is known for the planetary model

Werner Heisenberg

[ATOMIC MODEL]

Formulated the uncertainty principle , stating that one cannot accurately determine both the momentum and position of an electron at the same time (as if arguing againts the idea of fixed energy levels)

Ewin Schrodinger

[ATOMIC MODEL]

Improved on Bohr’s ideas and devised the quantum model where electrons lie dynamically in electron clouds rather than in fixed energy levels.

Ewin Schrodinger

[ATOMIC MODEL]

He is known for the quantum model

Nucleons

[ATOMIC MODEL]

Since protons and neutrons both belong to the nucleus , they are sometimes called _____

• Atomic number

• Mass number (aka atomic mass)

[ATOMIC MODEL]

The nucleons give rise to the:

• ______ → protons

• ______ → neutrons + protons

Atomic Mass

[ATOMIC MODEL]

Mass number is also known as _____

Hindi daw sya Lumalabas sa Board Exam sabi ni Sir!!!

SUB-ATOMIC PARTICLES [DIAGRAM]:

• A= mass number

• Z = atomic number

NOTE: How to find the number of electrons?

Under the assumption that the element is neutral (no charge) it will only be neutralize if the number of protons and electrons are equivalent so # proton = # electron

[ATOMIC MODEL]

Figure 2.Element “X”

6

Atomic number = number of proton

Find the atomic number

a. 6

b. 12

c. 8

d. 10

12

Atomic Mass = Mass number

Find the atomic mass

a. 6

b. 12

c. 8

d. 10

6

Number of Proton (Atomic number) = Number of Electron

Find the number of electrons

a. 6

b. 12

c. 8

d. 10

6

Neutron = Atomic mass (mass number) - Electron

Find the number of neutrons

a. 6

b. 12

c. 8

d. 7

Nuclides

A term for atoms when they have similar nucleons

• Isotopes

• Isotones

• Isobars

Types of Nuclides [3]

Isotopes

[ATOMIC MODEL]

Same protons but different neutron and mass number

Isotones

[ATOMIC MODEL]

Same neutron but different proton and mass number

Example:

Isobar

[ATOMIC MODEL]

Same mass number but different proton and neutron

Example:

Radioactivity

[NUCLEAR CHEMISTRY]

____ is the property to perform radioactive decay ramdomly

Radioactive decay

[NUCLEAR CHEMISTRY]

_____ is the release of energy, which can be accompanied by change in the quantity of nucleons (either protons or neutrons)

• Alpha

• Beta

• Gamma

Types of Radioactive Decay [3]

Alpha

Example:

[TYPE OF RADIOACTIVE DECAY]

• Release of 2 proton and 2 neutrons

• Loss of 4 in mass number

a. Alpha

b. Beta

c. Gamma

Beta

Example:

[TYPE OF RADIOACTIVE DECAY]

• Release of 1e accompanied by conversion 1n to 1p

• No loss in mass number

a. Alpha

b. Beta

c. Gamma

Gamma

Example:

m = means metastable (unstable) it has a lot of energy that wants to release all we have to do is to erase the "m"

[TYPE OF RADIOACTIVE DECAY]

• Release of high energy protons

• No loss in mass number

a. Alpha

b. Beta

c. Gamma

• Penetration

• Ionization

[TYPE OF RADIOACTIVE DECAY]

The crucial properties of decays are their _____ (capabiity to pierce through berriers) and _____ (capability to damage things / cause death)

Alpha

[TYPE OF RADIOACTIVE DECAY]

Have the LEAST PENETRATION (stopped by skin or paper)

a. Alpha

b. Beta

c. Gamma

Beta

[TYPE OF RADIOACTIVE DECAY]

Have the MIDDLE PENETRATION (stopped by a sheet of alimunum)

a. Alpha

b. Beta

c. Gamma

Gamma

[TYPE OF RADIOACTIVE DECAY]

Have the MOST PENETRATION (stopped by thick layer of lead)

a. Alpha

b. Beta

c. Gamma

Alpha

[TYPE OF RADIOACTIVE DECAY]

Have the MOST IONIZATION

a. Alpha

b. Beta

c. Gamma

Beta

[TYPE OF RADIOACTIVE DECAY]

Have the MIDDLE IONIZATION

a. Alpha

b. Beta

c. Gamma

Gamma

[TYPE OF RADIOACTIVE DECAY]

Have the LEAST IONIZATION

a. Alpha

b. Beta

c. Gamma

Measurement Type	Common Unit	SI Unit
Radioactivity	Ci (Curie)	Bq (Becquerel)
Absorbed Dose	RAD (radiation absorbed dose)	Gy (Gray)
Effective Dose	REM (roentgen equivalent man)	Sv (Sievert)
Exposure	R (roentgen)	C/kg (Coulomb/kg of air)

Units For Radioactivity