Year of discovery of the periodic table

Made a table of atomic weights and introduced letters to symbolize elements.

Made an extensive list containing 33 elements; made a distinction between metals and non-metals.

Introduced triads.

The average atomic weights of the 1^st and 3^rd number of this gave the atomic weight of the 2^nd number.

Law of octaves.

Formulated the first periodic law.

Horizontal row of elements in the periodic table.

Vertical column of elements in the periodic table.

Alkali Metals

Alkaline Earth Metals

Noble Gas

Halogen

Formula: 2n² n=3

Designated using the letters s, p, d, f.

Can accommodate 2 electrons.

can accommodate 6 electrons.

can accommodate 14 electrons.

Electron moves within an orbital.

Set of numbers used to describe electrons

Determines the overall energy of the electrons.

Determines the angular momentum and shape of the orbital.

Determines the number of orbitals and their orientation within a subshell.

Determines the direction of rotation of electron. Downward: - Upward: +

Statement of how many electrons an atom has in each of its electron subshells.

½ of the distance between two nuclei in 2 adjacent atoms.

The amount of energy needed to remove an electron from a neutral atom to convert it to a positively charged atom.

The amount of energy released when a neutral atom accepts an electron from its outermost shell to convert it to a negatively charged atom.

Tendency of an atom to attract electrons to itself when it is chemically combined with another atom.

Symbol for Oxygen

Symbol for Silicon

Element #15

Symbol for Tin

Branch of science that deals with the study of composition and properties of matter

Can be described broadly as the “Chemistry of everything else.”

1st metals used in 3000 BC

He made gunpowder (1214-1294)

He discovered radioactivity on 1896

A measure of the quantity of matter in a sample of any material

Intrinsic/Intensive

Extrinsic/Extensive

Characteristics which describe physical appearance; perceived by our senses; can be observed without causing any change in chemical composition.

Example of chemical property:

Simplest form of matter; made up of only one type of atom; cannot be broken down into simpler forms by ordinary chemical and physical means or change.

Conductors of electricity; Examples are: Copper, Lead, Tin, Nickel, and Zinc

Tend to ACCEPT electrons.

Example of a Metalloid/Amphoteric Element

Made up of 2 or more elements that are chemically combined

sour in taste, yield hydrogen ion (H+) in water solution

bitter in taste, yield hydroxide (OH-) in water solution

made up of a positive ion other than the H+ and negative ion other than OH-

Made up of 2 or more elements or compounds.

"solution"; uniform in appearance; single/one phase

"suspensions"; not uniform in appearance; distinct phases (2 or more layers)

Evidence of Physical Change:

Formation of new substance

Rotting of Fruit

Splitting of atom under nuclear change.

The Ability or Capacity to do work

Energy possessed by a body by virtue of its position.

Energy possessed by a body by virtue of its motion.

Energy associated with light, x-rays, radio waves.

Energy associated with machines, pumps.

Energy associated with the passage of electrons.

Energy cannot be created or destroyed in a chemical reaction or in a physical change. It can only be converted from one form to another.

In 1900, Max Plank proposed the Quantum theory of Radiant Energy. Plank suggested that radiant energy could be absorbed or given in definite quantities called?

In 1905, Albert Einstein proposed that Plank's quanta are discontinuous bits of energy, which were later called?

Concluded that matter is consisted of various combinations of the four “elements”—fire, earth, air, and water—and could be infinitely divided.

He developed the theory of atomism.

Models of an atom: Billiard Ball Model

Models of an atom: Plum Pudding Model

Models of an atom: Planetary Model

Models of an atom: Nuclear Model

Atoms with the same mass number (A)

Atoms with the same number of neutrons

Atoms of the same element of the same atomic number (contain same number of protons) but different mass number.