SCIENCE G8 3RD QUARTER REVIEWER

SCIENCE G8 3RD QUARTER REVIEWER

created by: Ms. Jesabeth Alfaro

Isotopes

The atoms of an element which have the same atomic number with different mass numbers.

Atomic number (Z)

corresponds to the total number of protons and electrons.

Mass number (A)

corresponds to the atom's total number of protons and neutrons.

Example: Arsenic

Z= 75

Chemical symbol

 a notation of one or two letters representing a chemical element. The exceptions to the one- to two-letter symbol are the temporary element symbols assigned to designate new or to-be-synthesized elements.

Robert Millikan

He determined the value of the charge of an electron.

qe = -1.6022 x 10 ^19 C

Joseph Thomson

Calculated the charge-to-mass ratio of an electron.

qe/me = -1.7588 x 10^8 C/g

James Chadwick

Identified the existence of the neutrons (uncharged particle).

Ernest Rutherford

Established the existence of the nucleus of an atom.

(gold foil experiment lead to the discovery of the atomic nucleus)

Eugen Goldstein

Identified the existence of the protons from his canal rays experiment.

Multiple Choice

He established the existence of the nucleus of an atom.

• Eugen Goldstein

• James Chadwick

• Ernest Rutherford

• Joseph Thomson

Multiple Choice

He identified the existence of the protons.

• Robert Millikan

• James Chadwick

• Joseph Thomson

• Eugen Goldstein

Multiple Choice

He determined the value of the charge-to-mass ratio of an atom.

• Joseph Thomson

• Ernest Rutherford

• James Chadwick

• Eugen Goldstein

Multiple Choice

He determined the value of the charge of an electron.

• Eugen Goldstein

• James Chadwick

• Robert Millikan

• Joseph Thomson

Multiple Choice

He identified the existence of the neutrons.

• Eugen Goldstein

• James Chadwick

• Geiger and Marsden

• Democritus

The belief of the early Greeks on the continuity of matter.

"It is impossible to continuously divide a sample of matter."

Coulomb

The SI unit of an electric charge.

average atomic mass

aam = (%abundance of isotope 1/ 100) x mass of isotope 1 + (%abundance of isotope 2/ 100) x mass of isotope 2...

EXAMPLE: What is the average atomic mass of Boron 10 and 11 if the percent abundance are 19.91 and 80.09 respectively.

Gold foil experiment

(Ernest Rutherford)

The experiment which validated the existence of the nucleus of an atom.

"Raisin pudding model of an atom"

JJ Thomson was the firsts who theorized a possible arrangement of the subatomic particles.

(raisin pudding or plum pudding)

JOHN DALTON

He originated the idea than an atom is neutral, tiny, indestructible, and the smallest particle of matter.

Atom of the same element

They have the same number of protons.

Both electrons and protons, their charges are of equal magnitude.

proton = electron charge

Mass of electron and proton

electron = -1.6022 x 10^-19 C

proton = +1.6022 x 10^-19 C

Cathode ray tube

The first apparatus used to established the existence of the electrons.

(William Crookes, an English chemist and physicist, carried out experiments ona gas discharge tube.)

Particulate drawings

Form of spheres in varied sizes to model the atoms and molecules.

State of Matter

• Solid

• Liquid

• Gas

• Plasma

• Bose- Einstein condensate

PARTICLE ACCELERATOR

The instrument used by scientists to study the particles of matter.

EARLY BELEIFS ON THE ULTIMATE COMPOSITION OF MATTER

• air (Anaximenes)

• earth

• fire (Heraclitus)

• water (Thales)

• Aristotle (air, earth, water, and fire)

BOSE- EINSTEIN CONDENSATE

The state of matter that exixts only at a temperature of near absolute zero.

ARISTOTLE

He proposed the idea that matter has NO ultimate particle.

DEMOCRITUS

Proposed the idea on the existence of an atom being the ultimate particle of matter.

BASIC PRINCIPLES OF THE PARTICULATE NATURE OF MATTER

• Matter is composed of discrete particles.

• Particles of matter are in constant motion.

• There are empty spaces between particles of matter.

• There are forces that act between the particles.

The particulate drawings