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The smallest unit of matter that retains all of the chemical properties of an element.

Atom

Are submicroscopic, meaning they are so small they cannot be seen with a microscope.

Atom

They are composed of smaller subatomic particles known as protons, neutrons, and electrons.

Atom

This number uniquely identifies: each chemical element.

Atomic Number

Negatively charged particle

Electron

positively charged particle found in the nucleus

Proton

particpe found in nucleus with no charge

Neutron

The basic building blocks of matter.

Atom

The smallest part of an element. The smallest unit of matter.

Atom

A pure substance consisting of one type of atom and can be identified by its atomic number.

Element

Formed when two or more atoms join together chemically. Can be the same atoms.

Molecule

Formed when two different elements join together.

Compound

consists of two different elements. Examples are water, salt, and Silicon Dioxide.

Binary Compound

Splits a larger atom into two or more smaller ones.

Fission

Joins two or more lighter atoms into a larger one.

Fusion

Is the emission of ionizing radiation from nuclear decay.

Radioactivity

A process involve in energetic particles of atom.

Radioactive Decay

5 Types of Nuclear Reaction

Alpha Decay, Beta Decay, Gamma Radiation, Positron Emission, Electron Capture

Loss of an alpha particle.

Alpha Decay

Loss of beta particle. A – unchanged Z – increase by 1

Beta Decay

Emission of gamma ray. A – unchanged Z – unchanged

Gamma Radiation

Conversion of a proton in a nucleus into a neutron, with the release of a positron. A – unchanged Z – decrease by 1

Positron Emission

Drawing on an electron into an atom’s nucleus. A - unchanged Z – decrease by 1

Electron Capture

Three Cosmic Origin of Elements (Universal Element Formation)

The Bigbang, Stellar Formation and Evolution, Stellar Explosion

Elements formed in Bigbang

H - Hydrogen, He - Helium, Li - Lithium, Be - Beryllium

The ______ of an evolved core of a high-mass star at the end of its red giant stage.

onion layers

Elements heavier than iron ______ be formed through ______ as tremendous amounts of energy are needed for the reaction to occur.

cannot, fusion

Where heavy elements are formed.

Supernova

A massive explosion of star.

Supernova

Example of an element formed in Supernova.

Uranium

Type I Supernova

Detonation

Type II Supernova

Explosion

Models of Matter

Empedocles

Believes that atter is made up of only 4 elements.

Empedocles

What are the 4 elements according to Empedocles?

Water, Air, Earth, Fire

Believes that the elements are arranged by gravity into perfect spheres.

Aristotle

Proper arrangement of elements based on Aristotle

Earth, Water, Air, Fire

A fifth element (quintessence) is found in the heavens.

Aether

He believed that teavenly bodies travel through the ether in perfect spheres.

Aristotle

One who deals with alchemy.

Alchemist

A medieval form of chemistry which focused on the transmutation of base metals into gold.

Alchemy

According to him, “To understand the very large, we must understand the very small"

Democritus

Greek Model / Greek Philosopher

Democritus

His idea of "atomos" derived from the word atom, in indestructable.

Democritus

Democritus have no experiments to support his idea.

True

Democritus's model of atom has no protons, electrons, or neutrons. It is solid and indestructable.

True

He made a book entitled "The Sceptical Chymist"

Robert Boyle

He is best kmown for introducing the Atomic Theory.

John Dalton

Another Frenchman a few years after Lavoisier

Joseph Proust

He proposed Law of Definite Proportions.

Joseph Proust

He roughly stated that a chemical could have only one ratio of atoms within it.

Joseph Proust

Samples of a given compound always contain the same proportion of elements by mass.

Law of Definite Proportions

Proust's Law of Definite Proportions is also called as _____?

Law of Constant Composition

Elements can form different compounds, the masses of the second element that can combine with a fixed mass of the first element are in a ratio of small whole numbers.

Law of Multiple Proportions

In chemical reaction, the mass of the substances produced is equal to the mass of the substances reacted.

Conservasion of Mass

Three Fundamental Particles of an Atom

Proton, Electron, Neutron

Three Types of Rays Emitted by Radioactive Materials

Alpha, Beta, Gamma

Plum Pudding Atomic Model

J.J. Thomson

Gold Foil Experiment

Rutherford

Discovery of Neutron

Sir James Chadwick

Discovered the elementary charge of an electron using the oil-drop experiment.

Robert Millikan

- Who discovered the Mass of Elenctron (9.109 × 10^-31 kg) - When was it discovered

Robert Millikan, 1909

Is the number of protons plus neutrons.

Mass number

Is the number of protons

Atomic Number

Elements which have the same atomic number but a different mass.

Isotopes

An isotope of a Carbon which is abundant in nature.

Carbon - 12

An isotope of Carbon that is found in space and used in experiments.

Carbon - 13

An isotope of a Carbon that is used to determine age/artefacts of an object.

Carbon - 14

Is a charge-carrying atom or molecule.

Ion

Is an atom or molecule with a net electrical charge.

Ion

Type of ion that is negatively charged.

Anion

Type of ion that is positively charged.

Cation

Is a process that produces an ion from an atom or a molecule.

Ionization

Type of ion which contains only one atom.

Monatomic Ion

Type of ion which contains two or more atoms.

Polyatomic Ion

It notes the number of missing or extra electrons.

Superscript

If there is a (+) superscript: that means that the ion is _____ electrons

missing

- If there is a (-) superscript: that means that the ion has _____ electrons

extra

It deals with a smallest particle.

Quantum Physics

The mallest unit of energy. Can be connected to other particles.

Quantum

Based on the picture, what model is it?

Quantum Mechanical Model

What model or whose model is shown in the picture?

Bohr’s Atomic Model

Enumerate the Four Quantum Numbers

Principal, Azimuthal, Magnetic, Spin

Distance of the electron from nucleus

Principal

It indicates the atomic size.

Principal

It indicates the shape of the subshell/orbital. It also defines shape of the electron.

Azimuthal

It indicates the orientation of the orbital.

Magnetic

It indicates the orientation of the electron spin.

Spin

Two types of notation that are used to show the distribution of electrons in the different orbitals in an atom.

Electron Configuration, Orbital Diagram

Uses the symbols of the orbitals and the number of electrons (written as superscripts) that occupy each orbital.

Electron Configuration

Consists of boxes and arrows that represent the orbitals and the electrons, respectively. The up and down orientation of the arrows represent the two magnetic spins of the electrons.

Orbital Diagram

2 Rules/Principle of Orbital Diagram

Pauli Exclusion Principle, Hund's Rule

When is the first periodic table presented?

March 6, 1869

Who is the father of the periodic table?

Dmitri Mendeleev

Atomic Structure Timeline

1707 - Newton, 1803 - Dalton, 1832 - Faraday, 1869 - Mendeleev, 1873 - Maxwell

Is a column in the periodic table.

Group

Elements based on groups have the same number of ________.

valence electrons

How many groups are there in a periodic table?

Is a row in the periodic table.

Period

100

Elements in a period/series have the same number of ________.

electron shells

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