Chapter 1 and 2 Problems Flashcards
incomplete 3 d shell
transition metal
complete 3 p shell
inert gas
uncompleted 3 p shell
halogen
completed 4 s shell
alkaline earth metal
incomplete 4 s shell
alkali metal
whats the conversion for nanometers to meters
10^9
Ionic Characteristics
electrostatic attraction between oppositely charged ions
(metal and non-metal)
Covalent Characteristics
electron sharing between 2 atoms to gain stableness
(non-metal and non-metal)
Metallic Characteristics
positive cores are shielded and glued together by a sea of valence electrons
(metal and metal)
hydrogen bonding requirements
- must be bonded to either oxygen or nitrogen
- fluorine is an exception
Melting point Hierarchy
primary bonding:
ionic > covalent > metallic
secondary bonding:
hydrogen > di-pole > van der waals
lower molecular weight = lower melting point?
Exceptions to filling s shell before d shell
Copper and chromium
amount of s, p, d and f spots
S: 1 spot (2 electrons)
P: 3 spots (6 electrons)
D: 5 spots (10 electrons)
F: 7 spots (14 electrons)
Left side vs Right side Periodic Table
Left Side: Electropositive
Right Side: Electronegative
What are attraction and repulsion forces dependent on?
r: separation of interatomic distance
FN Equation
FN = FA + FR
which means
FA = -FR
Energy Equation
E = EA + ER
Bonding Capacity depending on states
solid = large bonding capacity (high melting point)
liquid = intermediate bonding capacity ( mid melting point)
gaseous = low bonding capacity (low melting point)
Intermolecular vs Intramolecular
Intra = primary bonds (holds atoms together within a molecule)
Inter = secondary bonds (bond molecules together)
metals, ceramic and polymer bonding
Metals: metallic bonding
Ceramics: ionic bonding
Polymers: covalent bonding
Metal Characteristics
- good conductivity
- high strength
- high stiffness
- ductility
Ceramic Characteristics
Compounds of metallic and non-metallic elements
- non-conductive
- high hardness
- high strength
- high melting point
- very brittle
Wave-like Characteristics of electrons
- electrons are in orbitals defined by a probability
- each orbital at discrete energy levels is determined by quantum numbers
Energy Levels/Shells
K- Shell 1s
L - Shell 2s 2p
M - Shell 3s 3p 3d
N - Shell 4s
Valance Shell
If any level isnt filled, it makes the whole shell the valance shell.
(Example: 1s^2 2s^2 2p^2 L Shell is valance)
sp3 vs sp2
sp3
-s and p levels completely combine
sp2
- s and p shells don’t combine fully
VSEPR Theory
-double and triple bonds have stronger repulsive forces than single bonds
- lone pairs also distort angles
