Adv Chem Unit 04: The Periodic Table fixed

Where are representative elements located?

On the s-block (Groups 1 and 2) and the p-block (Groups 13-18)

Where are the transition metals located?

Groups 3 through 12 (the d-block) of the periodic table

Where are Lanthanoids and Actinoids located?

two separate rows at the bottom of the periodic table (the f-block)

Where are the Alkali metals located?

Group 1 of the periodic table (except Hydrogen)

Where are the Alkaline Earth Metals located?

Group 2 of the periodic table

Where are the post-transition metals located?

Groups 13, 14, and 15 of the periodic table

Where are the halogens located?

Group 17 of the periodic table

Where are the noble gases located?

Group 18 of the periodic table

What are the 7 diatomic elements?

BrINCl HOF (Hydrogen, Nitrogen, Oxygen, Fluorine, Chlorine, Bromine, Iodine)

What are some characteristics of Alkai metals?

• 1+ ions

• Most reactive metals

• Can react with water

• Not found in nature as pure elements

• form basic (high pH) compounds

What are some characteristics of Alkaline Earth metals?

• 2+ ions

• Rarely found in nature as pure elements

• Less reactive than group 1 neighbors

What are some characteristics of Transition metals?

• Often 2+ or 3+ ions, however charge is variable

• Common useful metals

What are some characteristics of Post-Transition metals?

• Decreasing metallic characters

What are some characteristics of Lathanoids and Actinoids?

• Many actinoids are synthetic

• The actinoids are mostly radioactive

What are some characteristics of Halogens?

• 1- ions

• Most reactive nonmetals

• Diatomic elements

What are some characteristics of Noble Gases?

• Full octet

• Inert (unreactive)

• Rarely from compounds

• Monoatomic gases

Where are metals located on the periodic table?

Group 1 to 12 (except hydrogen) and to the left of the staircase

Where are metalloids on the periodic table?

B, S, Ge, As, Sb, Te, Po, At

Where are nonmetals located on the periodic table?

Group 14 to 18 ( + Hydrogen) right of staircase

What are some characteristics of metals?

Conductors, Malleability (moldable), Lustrous (shiny), Ductile (flexible/wires), and high melting points

What are some characteristics of metalloids?

Semiconductors, properties of both metals and nonmetals, usually have a metallic appearance but "behave" like nonmetals.

What are some characteristics of nonmetals?

Insolators, brittle (cracking into pieces), non-lustrous (not shiny), with a low melting point; most are gases at room temperature.

Who created the first attempt at the periodic table?

Antoine Lavoisier

Who organized the periodic table by atomic mass?

Dmitri Mendeleev

Who organized the periodic table by atomic number?

Henry Moseley

Coulomb's law

Like charges repel and opposite charges attract

1.) The greater the charge of particles, the greater the attraction between them (directly proportional)

2.) The greater the distance between particles, the lesser the attraction between them (inversely proportional)

Atomic Radius

The half distance between the nuclei (center of an atom) of 2 bonded atoms

1.) The greater the nuclear charge, the greater the attraction, which means the smaller the atomic radius

2.) The greater the distance between the outermost electrons and the nucleus, the lesser the attraction, and the greater the atomic radius

Ionic radius

• An atom that LOSES an electron(s) is a cation

• An atom that GAINS an electron(s) is an anion

• When an atom gains an electron, its radius increases, which means an atom is smaller than its corresponding anion

• When an atom loses electrons, its radius decreases, which means an atom is larger than its corresponding cation

Remember that an ion is an element that has either lost or gained an electron

Ionization energy

the minimum energy required to remove an electron from an atom

Electronegativity

The tendency for an atom of an element to attract shared electrons when forming a chemical bond, or the 'desire' for electrons

• the greater the electronegativity, the greater the tendency to attract electrons in a chemical bond

• the greater the electronegativity, the greater the tendency to attract electrons in a chemical bond