Unit 1 Flashcards
Bond Formations
Ionic transferred from metal to nonmetal
Covalent shared between two nonmetals
Metal delocalized among metal atoms
Physical States
Ionic solid
Covalent solid, liquid, or gas
Metal solid
Melting Points
Ionic high
Covalent low
Metal very high
Solubility
Ionic yes
Covalent usually not
Metal no
Electrical Conductivity
Ionic yes solution or liquid
Covalent not
Metal yes any form
Other Properties
Ionic no
Covalent odorous
Metal malleable, ductile, lustrous
Salts
Product of ionic bonding
Oppositely charged ions
Metal Alloys
Formed when metal atoms replace other metal atoms
Or when larger metal atoms occupy small spaces between larger atoms
True Molecule
A group of two or more atoms held together by chemical bonds
Forming the smallest identifiable unit of substance
Properties of Ionic Compounds
Bonds are very strong
High melting and boiling point
Does not conduct electricity in solid state but aqueous state
Solids at room temperature
Made of metal and nonmetal
Aqueous
Dissolved in water
Changes properties
Crystalline Solid
Three dimensional network of positive and negative ions
Mutually attracted to one another
Crystal Lattice
The orderly three dimensional arrangement
Ions
Electron Dot Diagrams
Place one dot on each side before pairing up
Besides helium which uses two dots on same side
Electron Dot Diagram Cation
Zero dots to represent losing level
Brackets and charge
Electron Dot Diagram Anion
Eight dots to represent octet
Brackets and charge
Formation of Ionic Compounds
Write metal first
Then nonmetal
Lattice Energy
Higher
Means stronger bond
Polyatomic Ions
Group of covalently bonded atoms that bond in such a way that the group has a net charge
Covalent Naming Rules
Name first element fully using prefix besides one
Second element always change to -ide and ad prefix
Acid Naming Rules
Start with hydrogen
No oxygen use hydro-
Find number of hydrogen based on charge of anion
Use other element or polyatomic ion name
-ate to -ic
-ite to -ous
Binary Acid
Second element nonmetal
Root of second elements name follows prefix
Ends with -ic acid
Writing Acidic Formulas
No hydro- tells oxyacid
Change -ic to -ate and -ite to -ous
Write symbol with their charges
All begin with H+1
Add the nonmetal
Crossover and reduce
Incomplete Octet
Hydrogen only forms one bond
Boron only forms three bonds
Beryllium only forms two bonds
Expanded Octets
P
S
Xe
Can Form Covalent Bonds
Beryllium
Yuh
Can Form With Expanded Octets
Periods 3
And below
Valence Electrons
Across
Yuh
Lewis Structure Rules
Count
Find middle
Set up
Add to middle then ends
Create bonds
Count again
HONC
Hydrogen and halogens form one bond never central atom
Oxygen forms two bonds
Nitrogen forms three bonds
Carbon forms four bonds
Lone Pairs
Repel more strongly because they take up more space
Reduce bond angle
REMEMBER
Don’t forget to check diatomic
Ionic can’t share bonds
Dipoles
Polar bonds constitute
Polarity of individual polar bond between atoms
Or he net polarity of a polar molecule that may have several polar covalent bonds within it
Or the polar molecule itself
Polarity of Molecules Can Affect
Many of their other properties
Such as their solubility, boiling and melting points, and their odor
Electronegativity Symbol
∆EN
Yuh
Determining Molecular Polarity One Central Atom
Lone pairs means polar
No lone pairs but terminal atoms on same element means nonpolar
No lone pairs and no terminal atoms means polar
Determining Molecular Polarity Two or More Central Atoms
Lone pairs means polar
No lone pairs but central and terminal atoms on same element means nonpolar
No lone pairs but central atoms on same element and no terminal atoms on same element means polarity depends on symmetry
No lone pairs and no central atoms means polar
Molecule Can Still Be Nonpolar If
Overall pull still cancels out
Bonds are still evenly spaced
Magnitude is what matters
Less Electronegative
Named first
Yuh
Bent Shape Ensures
Dipole moments don’t cancel out
Yuh
Resonance Structure
Set of two or more electron dot diagrams of a single polyatomic Including fractional bonds and fractional charges
Molecular/Geometric Structure
Three dimensional arrangement of atoms within a molecule
Including the bond lengths, angles, and relative positions of each atom
Type I Binary Compound
Has cation that has only one charge
Metals in group one and group two and aluminum in group thirteen
Type II Binary Compound
Has cation that has multiple charges
All other metals that are not type one
Type I Ternary Compound
Contains a metal with fixed oxidation Bonded to polyatomic ion
Type II Ternary Compound
Contains a multivalent metal
Bonded to a polyatomic ion
Oxyanion
A negatively charged polyatomic ion
That contains oxygen
