[RAD101] Module 1.1

Atom

Smalles part of an element with all properties of that elemet

Matter

An atom is the basic unit of _______

0.1 to 0.5 nanometers

Atom's diameter in nm

Atomic Structure

The atom consists of three component parts: Protons

Nucleus

In an atom

Electrons

Particles that surround the nuclues

Electrically Neutral

Atoms are usually E______ N_____. They have 0 electric charge

Electron

Proton

Electron

Negative electrical charge that moves outside the nucleus

Joseph John Thomson

Discovered the electron

1897

Year JJ Thompson discovered the electron

9.110 x 10^-28 g

Mass of electron

0.000549 amu

Amu of an electron

Proton

Large and heavier than electrons with positive charge that are located in the nucleus of an atom

Ernest Rutherford

Discovered the nucleus and proton

Element

The number of protons determines what?

1.6727 x 10 ^-24 g

Mass of a proton

1.007316 amu

Amu of a proton

Neutron

Large and heavier than protons with no electrical charge and also located in nucleus.

Greater

Number of neutron is always (greater/lesser) than protons

1.6750 x 10-24 g

Mass of a neutron

1.008701 amu

Amu of a neutron

Nucleus

Center of an atom which contains the protons and neutronss

Late 1919

Year Rutherford discovered the proton

James Chadwick

Discovered neutron

1932

Year Chadwick discovered neutron

Nucleons

The collective term for protons and neutrons

Force

A push or pull upon an object that results to an interaction with anothre object

Grand Unified Theory

Is a vision of a physics theory that can combine three of the four fundamental forces into one single equation

Strong Nuclear Force

The force that holds nucleons together and is the strongest of all forces.

Short

Strong nuclear force acts only on a (short/long) range.

Pions and Gluons

Present in strong nuclear forces.

Electromagnetic Force

Combination of all electrical and magnetic forces

Electrons

Electromagnetic Force holds (protons

Electromagnetic Force

Holds atoms together

Infinite

Electromagnetic Force has an ______ range

Photons

A particle of light that is used by Electromagnetic Force.

0.7%

Electromagnetic Force is _____% as strong as the Strong Nuclear Force.

Weak Nuclear Force

Responsible for decay of radioactive atoms and emission of particles from the nucleaus.

Nuclear Fusion

Caused by Weak Nuclear Force (sun and stars)

One million

Weak Nuclear Force is _____ _______ as strong as the Strong Nucler Force

Shorter

Weak Nuclear Force has even (shorter/longer) range

Proton's Diameter

Range of a Weak Nuclear Force

W and Z bosons

Carry the weak nuclear force.

Gravitational Force

The pull between two objects directly related to their masses and inversely related to the distance between them (Newton)

Gravitational Force

The force that is the most powerful for massive and slow objects such as the Earth and Stars.

TRUE

TRUE OR FALSE:

Gravitational force has little effect at atomic level.

Gravitational Force

The weakes of all forces

6 x 10^-29

Gravitational Force is the weakest of all forces

Infinite

Gravitational Force has an ________ range.

Graviton

Particle that carries the gravitational force. Not yet observed

Four Fundamental Forces of Nature

Strong Nuclear

Dmitri Mendeleev (1869)

Created the periodic table

Periodic Table of Elements

Tabular display of the chemical elements arranged by atomic number

118

Number of elements in the periodic table as of 2019.

Oganesson

Og

Atomic Number (Z)

The number of protons in the nucleus of an atom

Atomic Number

Determine the chemical properties of an element and its place in the table.

Z

Atomic Number

Atomic Mass (A)

The mass of an atom of a chemical element expressin in atomic mass units (amu).

A

Atomic Mass

Atomic Mass

Approximately equal to the number of protons and neturons and the average number allowing for the relative abundances of different isotopes.

18

Number of groups/families on the periodic table

Alkali Metals

Group 1 elements

Alkaline-Earth Metals

Group 2 which are highly reactive but have slower reactions than Alkali. It is rarely found alone in nature.

Lanthanides

The 14 elements with atomic numbers from 58 to 71.

Group 3

Silvery white metals that tarnish when contacted with air.

Actinides

A group of elements in the second row of the rare earth elements.

Group 3 - Bottom

All are radioactive

Inner-transition Metals

Lanthanides and actinides

Thorium and Uranium

Part of the Actinides which occur naturally on Earth in substantial amount

Transition Metals

Groups 3-12

Transition Metals

Hard

Conductors

Materials that transfer energy easily

Post-Transition Metals

Group 13-17

Tend to be softer and poor conductors

Metalloids

Group 13-17

Represents transition from metals to nonmetals

Semiconductors

Semi-metals

Poor Metals

Metals that have low melting points

Also called semi-metals

Non-Metals

Group 14-16

Mostly gases which includes hydrogen

Halogen

Group 17

Highly reactive

Combine with alkaline to form salts

Noble Gases

Group 18

Colorless

Odorless

7

Number of periods in a periodic table

Periods

Tell the energy level of the element's valence electrons

Horizontal

Periods

Vertical

Groups

Groups

Vertical column of the periodic table that signifies the number of valence electrons in an element.

Families

Elements that have the same number of valence electrons and therefore similar properties.

Periods

The horizontal rows in the periodic table that signify the number of electron shells in an elemen

Electron Configuration

The arrangement of electrons in the orbitals of an atom

Shell

Sub-shell

Shell

Specific distance from the nucleus with a letter or a number

Absorb

If electrons ?? energy from a photon

Lower

Closer to the nucleus means electron shell has a ?? energy level

Release

If an electron drops back down to a lower-energy level

Increases

Maximum number of electrons in a shell ???? with the distance of the shell from the nucleus

n

The shell number or the principal quantum number

Principal Quantum Number

Symbolized by n

2n^2

Formula to calculate the maximum number of electrons within a shell

Sub-shell

A group of the same type of atomic orbitals (s

Sub-energy Levels

Also called the sub-shell

Orbitals

Complex-shaped high probability regions of space around the nucleus

Orbitals

Specific number of orbitals contained in each sub-shell