Basics Of Chemistry

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Basics Of Chemistry

8 th Science 2012

Matter Defined

Matter – anything that has volume or mass.

Everything you see and don’t see.

Definitions

Element- pure substance that cannot be separated into simpler substances by physical or chemical means.

 Represented by a symbol – Au stands for what?

Definitions

Atom – Smallest particle into which an element can be divided and still be the same substance, retaining its properties

Evolution of the Atomic Theory

Democritis – 440 BC

Greek philosopher who said that if you cut a substance in half again and again and again eventually you would have an “uncuttable” piece said that all atoms made of a single material formed into different shapes and they join together to make different materials

Greek word atomos

“indivisible”

, which means

John Dalton - 1803

Studied the atmosphere and other gases and developed atomic theory.

Dalton demonstrated that elements combine in specific

proportions to make different substances

John Dalton’s Atomic Theory

1. All substances are made of atoms .

Dalton’s New System of Chemical Philosophy

2. Atoms are small particles that cannot be created, divided, or destroyed.

Dalton’s Atomic Theory, continued

3. Atoms of the same element are identical in size, mass and other properties.

4. Atoms of different elements combine to make chemical compounds.

5. In chemical reactions , atoms are combined, separated, or rearranged.

J.J. Thomson - 1897

► discovered that there are small particles inside the atom, so the atom can be divided into smaller parts

JJ Thomson, continued

Experimented, using a cathode-ray tube to discover negative

particles he called corpuscles

► these negatively charged particles found in all atoms are now called electrons

Thomson’s Model

Plum Pudding model

Described electrons as scattered all about the atom

Ernest Rutherford - 1908

Rutherford, continued

Discovered a tiny, extremely dense, positively charged region called a nucleus

Most of the atom’s

mass was in the nucleus and electrons traveled around the nucleus

Rutherford cont’d

► said the atom was mostly

empty space

Niels Bohr – 1913

► said the electrons

travel around the nucleus in definite paths

Erwin Schrödinger and

Werner Heisenberg - 1926

Said electrons travel in clouds, not definite paths but we still use the Bohr Model to represent atoms.

The Atom

Subatomic Particles

Protons

Determine the identity of the matter

positively charged particles found in the nucleus

Mass =1.67262158 × 10 -27 kilograms

0.000000000000000000000000017 kg

Each proton is 1 amu

 AMU stands for Atomic Mass Unit

Subatomic Particles

Neutrons

Neutrons are the glue that holds the protons together in the nucleus

► no charge found in the nucleus mass is 1 amu

Subatomic Particles

Electrons

Determine the reactivity

Negatively charged

Found around the nucleus within electron clouds

Mass is very small, almost zero

Atoms are NEUTRAL

Atoms are neutral because the number of protons equals the number of electrons.

How To Read a Square

8

O

Oxygen

15.9994

Elements are identified by their atomic number – the number of protons. Also equals the number of electrons.

Chemical Symbol

Element Name

Atomic Mass

PEN Method

SLIDE, SLIDE, ROUND

THE BOTTOM

SUBTRACT TOP

P = 8

E = 8

N = 8

8

O

Oxygen

15.9994

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