L4 Quantum numbers and significant
Page 1: Periodic Table and Quantum Numbers
Periodic Table of Elements
An organized chart that displays all known chemical elements arranged by increasing atomic number.
Quantum Numbers
Variables that describe the properties of atomic orbitals and the electrons in those orbitals.
Page 2: Arrangement of Elements in the Periodic Table
Chemical Elements
Examples include H (Hydrogen), He (Helium), Li (Lithium), Be (Beryllium).
Classification
Nonmetals, metals, and metalloids.
Categories include:
Alkali metals (IA)
Alkaline Earth metals (IIA)
Transition metals
Post-transition metals
Metalloids
Halogens
Noble gases
Periodic Table Organization
Elements are arranged in horizontal rows (periods) and vertical columns (groups).
Page 3: Historical Development of the Periodic Table
Discussion of how the periodic table has evolved over time with contributions from various scientists.
Page 4: The Structure of the Periodic Table
Periodic Table Basics
Each element is represented by its Atomic Number, Symbol, Name, and Average Atomic Mass.
Organized by increasing atomic number.
Page 5: Layout of Periodic Table
Periods and Groups
Rows represent periods; columns represent groups.
Page 6-7: Basic Information of Elements**
Elements such as H, He, Li, Be, Na, Mg, etc.
Information includes atomic numbers and average atomic mass.
Lists many elements and their properties (symbols, names, classification).
Page 8: Periods in the Periodic Table
There are 7 periods in the periodic table.
Each period corresponds to the number of electron shells.
Page 9: Arrangement of Periods
Definition of Period
Periods are defined as elements having the same number of valence electron shells.
Page 10: Details of Periods
Energy Levels
Each period corresponds to an increase in the number of energy levels: 1st period = 1 shell, 2nd = 2 shells, etc.
Page 11: Main-Group Elements
Configuration
The arrangement of electrons in an atom's orbital.
Split into s and p blocks, transition elements (d block), and inner transition elements (f block).
Page 12: Groups of the Periodic Table
Groups denoted by numbers 1-18 or as A and B groups distinguished based on the type of elements they are.
Page 13: Families in the Periodic Table
Definition of families as columns or groups with similar chemical properties due to the same number of valence electrons.
Page 14: Metals, Metalloids, Nonmetals
Classification based on element properties within the periodic table.
Page 15: Group Types
Representative Elements - partially filled outermost s and p.
Transition Elements - electrons present in d and f orbitals.
Page 16: Element Arrangement Properties
Discussion on how properties such as atomic size, metallic character, ionization energy, electron affinity, and electronegativity influence the arrangement.
Page 17: Atomic Size
Atomic radius increases from right to left across a period and from top to bottom within a group.
Page 18-19: Metallic Properties
Elements that can lose electrons easily; metallic property increases from right to left and top to bottom in the table.
Page 20: Ionization Property
Energy required to remove an electron from a neutral atom.
Page 21: Trends in Ionization Energy
Ionization energy increases from left to right and bottom to top.
Page 22-23: Electron Affinity
Energy change when an atom gains an electron; increases from left to right and bottom to top in the periodic table.
Page 24-25: Electronegativity
Trends in electronegativity similar to ionization energy, increases across a period and up a group.
Page 26: Summary of Periodic Trends
Overview of ionization energy, electronegativity, atomic radius, and electron affinity trends in the periodic table.
Page 27-30: Quantum Numbers
Quantum Numbers Overview
Principal (n), Angular (l), Magnetic (m), Electron Spin (s) numbers define electron arrangements in atoms.
Page 31-36: Principal Quantum Number (n) and Shell Designation
Each principal shell contains subshells, and the energy increases in the order s < p < d < f.
Shapes and orientations of orbitals defined.
Page 37-41: Orbital Types and Shapes
S, p, and d orbitals characterized by their shapes and orientations in space.
Page 42-44: Electron Spin Quantum Number (s)
The electron can spin either clockwise or counterclockwise with possible values of +1/2 or -1/2.
Page 45-54: Quantum Configuration Examples
Examples of quantum number configurations for specific elements and how to identify them.
Page 55-57: Significant Figures
Counting Significant Figures
Rules for determining the number of significant figures in a measurement based on the presence of non-zero digits and the location of zeros.