IPS1: Inorganic Chemistry Part 1 - Fundamentals - (A4) Quantum Numbers, Electron Configuration, Periodic Table

Proverbs 16:3

Quantum numbers

1. Principal QN (n)

2. Orbital QN (l)

3. Magnetic QN (ml)

4. Spin QN (ms) - for individual electrons

1. Principal Quantum Number

n = 1, 2, 3, ... (n)

orbital = shell or energy level

distance of electron from the nucleus; the higher the n, the higher the energy

2. Angular Momentum Quantum Number (l)

aka Azimuthal or Orbital Angular momentum Quantum number

l = 0, 1, 2, 3, ... (n-1)

orbital = subshell/sublevel

Shape of the orbital

2. Angular Momentum Quantum Number (l)

3. Magnetic Quantum Number

ml = -l ... 0 ... +l

orbital = specific orbital

orientation in space of the orbital

4. Spin Quantum Number (ms)

for each individual electron only

ms = +1/2 (upward; clockwise) or -1/2 (downward; counterclockwise)

Quantum Number and Electron Configuration

Electron Configuration

distribution electrons

describes the number and arrangement of electrons in orbitals, sub shells, and shells in an atom

Ground state

atom in its lowest energy or unexcited, state

Aufbau principle

orbitals fill in order of increasing energy, from lowest to highest

Pauli Exclusion Principle

No more than two electrons can occupy each orbital, and if two electrons are present, they must have opposite spins

Orbital Diagrams

Noble Gas Configuration

an atom consists of the elemental symbol if the last noble gas prior to that atom followed by configuration of the remaining electrons

Hund's Rule

the order of fill is the same but as you can see from above the electrons are placed singly into the boxes before filling them with both electrons

a single electron will occupy an empty orbital first before pairing

Dimitri Mendeleev

concepts on periodic table based on chemical properties

Lothar Meyer

concepts on periodic table based on physical properties

Dimitri Mendeleev

Lothar Meyer

both emphasized the periodicity, or regular periodic repetition of properties with increasing atomic weight

Increasing atomic number

Elements are now arranged in the periodic table in order of

Periodic Law

the properties of the elements are periodic functions of their atomic numbers

Vertical columns

group or families

Horizontal rows

periods

Group 1 (IA): Lithium group

H and Alkali metals

Group IIA: Beryllium group

Alkaline earth metals

1) Group IIIA

2) Group IVA

3) Group VA

4) Group VIA

5) Group VIIA

1. Scandium group

2. Titanium group

3. Vanadium group

4. Chromium group

5. Manganese group

Group 8,9,10 (VIIIB)

Iron group

Cobalt group

Nickel group

Group 11 (IB)

Coinage metals

Group 12 (IIB)

Zinc group

Group 13 (IIIA): Boron group

Triels; 3 valence electrons

Group 14 (IVA): Carbon group

Tetrels; 4 valence electrons

Group 15 (VA): Nitrogen group

Pnictogens; "to choke"

Group 16 (VIA)

Chalcogens; "ore"

Group 17 (VIIA)

Halogens: "salt"

Group 18 (8A): Helium or neon group

Noble gases

Properties of metals

forms cations by losing electrons

form ionic compounds with non metals

solid state characterized by metallic bonding

Properties of metals

high electrical conductivity that decreases with increasing temperature

high thermal conductivity

almost all are solids

malleable (can be hammered into sheets)

ductile (can be drawn into wires)

metallic gray or silver luster

Mercury (Hg)

Cesium (Cs)

Gallium (Ga)

liquid metals; melt at body temperature

Malleability

property to be hammered into sheets

Ductility

property to be drawn into wires

Copper (Cu)

Gold (Au)

metals that are not metallic gray or silver luster

Properties of non metals

poor electrical conductivity

good heat insulators (except C)

solid, liquid or gases

brittle in solid state

non ductile

non metallic luster

Properties of non metals

form anions by gaining electron

form ionic compounds with metals and molecular (covalent) compounds with nonmetals

covalently bonding molecules

Graphite (Carbon)

non metal that is good electrical conductor

Carbon

non metal that is not good heat insulator

Metalloid

show properties of both metals and non-metals

semiconductors

Lower

Metalloids are insulators at _____ temperature

Conductors

Metalloids are ______ at higher temperature

Metalloids

Boron (B)

Silicon (Si)

Arsenic (As)

Tellurium (Te)

Germanium (Ge)

Antimony (Sb)

Polonium (Po)

Astatine (At)

Atomic radii

half of the distance between the nuclei of neighboring atoms in the pure element

express in Angstroms (1Å = 10^-10 m)

Ionization Energy (IE)

the energy required to remove an electron from a gas-phase atom

Electron Affinity (AE)

the energy change that occurs when an electron is attached to an atom in the gas phase to form negative ion

Electronegativity

measure of the relative tendency of an atom to attract electrons to itself when it is chemically combined with another atom

H and noble gases

excluded in the periodic trends

Periodic Trends

Increasing from left to right and down to top

Periodic trend: Ionization energy

Increasing from left to right and down to top

Periodic trend: Electron affinity

Increasing from left to right and down to top

Periodic trend: Electronegativity

Increasing from top to down and right to left

Periodic trend: Atomic radius

increasing from lower left to upper right

Periodic trend: Nonmetallic character

increasing from upper right to lower left

Periodic trend: Metallic character