Ionic Compounds and Such Flashcards
2 types of ions
Cation
Anion
Ion
Atom that has an electrical charge
Electrical charge caused by loss or gain of electron
Cation
Ion with a positive charge
Lost electron
Anion
Negative charge
Gained electron
Ionic bonds
Attraction between ions of opposite charge
Why do atoms lose or gain electrons
To become more stable
What electrons to atoms lose first
Electrons farthest from the nucleus
Outermost electrons
Valence electrons
Electrons in outer energy level
Core notation
Nearest noble gas before it + everything else that comes after
Atomic stability
Nobel gases
In outer energy level
Octet rule
Atoms lose or gain electrons to match noble gas configuration
Isoelectronic
Having the same electron configuration as another atom
Ex: Ne is the same as F- O2- N3-
Oxidation number (charge)
Share a monotomic ion
Li+ = +1
P3- = -3
How do metals become stable
Lose electron
Cations
How do nonmetals become more stable
Gain electrons
Anions
Binary ionic compounds
Cation+anion
Write cation first anion second
Binary ionic compounds must
Balance out
Ex
Na+ Cl-= 1+-1=0
Naming compounds
Cation+anion+ide
More than one oxidation state use to an numeral
Polyatomic ions
Any Ion made up of more than one atom
Platonic ions can bond to
Other polytonal ions
Monotomic ions
When is the only time you ever change the name for anything
When monoatomic comes second
Properties of covalent bonds
Occurs between two nonmetals Electrons are shared Tells number of atoms Nonmetals Not soluble in h20 Low melting point Low boiling point Gas liquid or solid at room temp
Diatomic molecule
Simples form of covalent bond
Atoms of the same element
7 diatomic elements + hydrogen
H2 N2 O2 F2 Cl2 Br2 I2
Prefix system
Mono Di Tri Tetra Penta Hexa Hepta Octa Nana Deca
Properties of ionic compounds
Tells ratio of atoms
Metal nonmetal section of table
Soluble in H2O
High melting pint and boiling point
Doesn’t conduct electricity in solid form
Conducts in liquid form or when dissolved in water
Solid at room temp
Electro negativity
Tendency of an atom to ATTRACT BONDING ELECTRONS TO ITSELF when it bonds with another atom
When moving across a table electronegativity
Increases
When moving down a period electronegativity
Decreases
When naming covalent compounds ____ electronegative go first
Least
The type of bond (ionic or covalent) is determined by
Electronegativity differences between to elements
When a compound has no electronegativity difference
All diatomic molecules
Non polar COVALENT
Intermediate electro negativity difference
Polar molecules have positive (delta+) and negative (delta-) ends
Large electro negativity difference
Ionic
Polar molecules are separated
