Notes 

Chapter 6(p. 136-164)

Read page 161 for the five facts.

Periodic Law=

This states that there is a repetition of chemical and physical properties of elements when they are arranged by increasing atomic number.

Groups or families:

Elements with similar properties that appear in vertical columns in the periodic table.

Periods or rows=

The horizontal rows of elements with increasing atomic numbers in the periodic table.

Representative elements:  (group A)

The elements in the s and the p shells.

Transition elements:  (d-shell or group B)

Elements between groups 2 A and 3 A of the periodic table.  Most transition elements have similar structures and properties. (The number of valance electrons varies and so does their charge.)

Inner transition metals=

Elements in the f shell.

A)                Lanthanide series=(Elements 57-70)

Elements in the 4 f shell that starts with the element, Lanthanum.

B)                Actinide series=(Elements 89-102)

Elements in the 5 f shell that starts with the element, Actinium. (Mostly synthetic and many are radioactive)

Metals=

Elements that are generally shiny, malleable, ductile, and good conductors.

Red print means it is a family!

A) Alkali metals=

Elements in group 1A, which are extremely reactive metals.

https://www.youtube.com/watch?v=m55kgyApYrY

B) Alkaline earth metals=

Elements in group 2 A, and are very reactive metals.

Nonmetals=

Elements that are gases or brittle, dull-looking, and do not conduct very well.

C)                Halogens=

Highly reactive nonmetals in group 7 A.  They form diatomic molecules.

D)                Noble gases=

Extremely unreactive elements in group 8 A.

Metalloids=(Semi-metals)=

Elements that have characteristics of metals and nonmetals.

Mixed families

A) Boron family: The family of elements in group 3 A of the periodic table. In some occasion they may only have 6 valance e-1. (3 valance electron and form a charge of +3)

B) Carbon family: The family of elements in group 4 A of the periodic table. (4 valance electron and form a charge of +4 or -4)

C) Nitrogen family: The family of elements in group 5 A of the periodic table. These substances contain a lot of energy in their bonds. In some occasion they may have 10 valance e-1 .(5 valance electron and form a charge of -3)

D) Chalcogens: (Oxygen family.) The family of elements in group 6 A of the periodic table. These substances readily combine with metals. (6 valance electron and form a charge of -2)

Ion=

Atom or group of atoms that has a charge.

Ionization energy=(trend)

Energy needed to remove an electron from an atom.

Octet Rule=

The tendency of an atom to gain or lose electrons to fill the outer shell. (8 e=s2 and p6)

*Duet Rule=

The tendency of an atom to gain or lose electrons to fill the outer shell. (2 e=s2)

Electronegativity=(trend)

The relative ability of an atom to attract electrons in a chemical bond.

Ionization energy=(trend)

The energy needed to remove electrons from an atom.

Atomic radii=(trend)

The distance from the nucleus to the outermost electrons in elements without a charge.

Ionic radii=(trend)

The distance from the nucleus to the outermost electrons in elements with a charge.

*Alchemists:

People who helped establish the scientific method as they systematically took matter apart to analyze it.

*Natural elements: (92)

Elements that are found in nature

Families on the periodic table

A) Alkali metal family: the family of very reactive elements in group 1A of the periodic table. (1 valance electron and form a charge of +1)

B) Alkaline earth metal family:  the family of elements in group 2 A of the periodic table. (2 valance electron and form a charge of +2)

C) Boron family: The family of elements in group 3 A of the periodic table. In some occasion they may only have 6 valance e-1. (3 valance electron and form a charge of +3)

D) Carbon family: The family of elements in group 4 A of the periodic table. (4 valance electron and form a charge of +4 or -4)

E) Nitrogen family: The family of elements in group 5 A of the periodic table. These substances contain a lot of energy in their bonds. (5 valance electron and form a charge of -3)

F) Chalcogens: (Oxygen family.) The family of elements in group 6 A of the periodic table. These substances readily combine with metals. (6 valance electron and form a charge of -2)

G) Halogen family:

The family of elements in group 7 A of the periodic table that react most readily with the alkali metals to form salts.  They also form diatomic molecules and are in the gaseous state. (7 valance electron and form a charge of -1)

H) Noble gas family: the family of elements in group 8 A of the periodic table that usually do not combine with other elements. (8 valance electron and form a charge of 0)

Group Questions

Three major divisions of the periodic table.

1.                  Metals: These are elements located to the left side of the “steps” on the periodic table, but NOT touching the “steps”.

2.                  Nonmetals:  These are elements located to the right side of the “steps” on the periodic table, but NOT touching the “steps”.

3.                  Metalloids: These are elements that are touching the “steps” on the periodic table.(NOT Al)

Metalloids have both properties of metals and nonmetals.

Group Questions Answers:

History of the periodic table.

John Newlands-

Arranged elements based on mass and noticed properties repeat every eighth element.

Lothar Meyer-

Demonstrated a connection between properties and atomic mass.(Arranged elements in increasing mass.)

Dmitri Mendeleev-

Predicted existence and properties of undiscovered elements.

Henry Moseley-

Arranged elements according to atomic number which resulted in periodic patterns.(current periodic table.)

Antoine Lavoisier-Defined chemical element, distinguished between metals and nonmetals, and made a list of all known elements.

Jon Jacob Berzelius-Proposed symbols for known elements.

Researchers in Berkeley, California synthesized the first element heavier than the Actinides.

         Metals usually possess the following characteristics:

1. Malleable: Able to be pounded into various shapes and NOT lose strength.

2. Ductility: Able to be drawn into a wire.

3. Luster: Reflect light/ shiny appearance.

4. Conductor: Able to transmit electricity and heat very readily.

5. Reactivity: Produce hydrogen gas when mixed with acids (oxidize (rust) in the presence of CuCl2 [copper(ll)chloride].)

Nonmetals usually possess the following characteristics:

1. Brittle: Break when hit with a hammer.

2. Dull: Most do NOT reflect light/ appear shiny.

3. No ductility: Can NOT be drawn into a wire.

4. Nonconductor: Do NOT transmit heat or electricity.

5. Reactivity: Do NOT react with acid or oxidize in CuCl2 [cupric chloride].