Unit 3-1 The Periodic Table and Periodic Law Development of the Modern Periodic Table Classification of the Elements Periodic Trends s, p, d, & f-block elements

Early History ____________ was the first to discover that when elements were arranged by mass, their properties repeated every eight element (Periodic Law, Law of Octaves) _____________ was first to publish a periodic table arranged by atomic mass _____________ published modern periodic table where elements are arranged by atomic number

Classification of the Elements A __________ (B, Si, Ge, As, Sb, Te, Po, At) separates metals from non-metals _________ are good conductors, malleable, have luster, and are ductile _________ are poor conductors, and generally dull-looking _________ have properties of both metals and nonmetals

Modern Periodic Table Vertical columns are called ________ or __________. Horizontal rows are called __________. Groups labeled with an A are ___________ elements; those labeled with a B are ___________ elements.

Classification of the Elements Elements can be classified into 4 categories according to their ____________________. 1.The _____________ 2.The ___________________ 3.The ________________ 4.The ________________

Noble gases Elements in which the outermost __ or __ sublevel is filled.  Group 8A  Also known as ___________. The representative elements Usually called the _______ elements Elements in which the outermost __ or __ sublevel is only partially filled  Group 1A elements are the _______________  Group 2A elements are the _______________ The transition metals Called the _________ elements Outermost orbitals are ___ and ___ sublevel The inner transition metals Outermost orbitals are ___and ___ sublevel

Valence Electrons A representative element’s ___________ and _____________ are the same The energy level of an element’s valence electrons is represented by the _______________ s, p, d, f Block Elements The periodic table can further be divided by blocks (s, p, d, f) which show _______________________  s block: __________ and ______  p block: ____________________ and ______ (except for _______)  d block: ____________ (________)  f block: ___________________

Properties of s, p, d, f block elements s-block  group 1A:  group 2A: p-block  Group 3A:  Group 4A:  Group 5A:  Group 6A:  Group 7A:  Group 8A: d-block  ______________ f-block  ______________

Periodic Trends Because of the nature of electron arrangement, and chemical reactivity is dependent upon ____________________, there are several trends that are built into the periodic table. These trends include __________, _____________, _____________, and ___________________.

Atomic Radius Define: _______________________________ ______________________________________. Atomic radius _____________ as you go down a group because you are adding electron shells. Atomic radius _____________ as you go across a group due to the increased positive charge of the nucleus.

Formation of Ions The _______________ states that all atoms want to have eight valence electrons to be stable. Ions are often formed when an atom gains electrons (______, ____________) or loses electrons (______, __________).

Ionic Radius Define:__________________________________ _______________________________________.  Atoms of _________ elements have low ionization energies and they form _____ ions.  Atoms of _________ elements readily form _________ ions. The loss or gain of electrons affects the _____ of the ions formed.  Ionic radii for non-metals tend to be __________ as a negative ion is formed  the same is true for metals that tend to be ___________.

Ionization Energy Define: _______________________________ ______________________________________. _______________ as you go across a period because due to the increased nuclear charge. _______________ as you go down a group because you keep adding electron shells which allow the valence electrons to be further away from the positively charged nucleus.

Electronegativity Define ___________________________ _________________________________. Electronegativity ___________ as you move across a period Electronegativity ___________ as you move down a group

Reference /electrons/ 101/electrons/ act/c120/periodtb.html act/c120/periodtb.html