Exam 2 notes Flashcards
Ionic compound
held together by the attraction between the positive and negative ions.
F-
Floride ion
Cl-
cloride ion
Br-
bromine ion
I
iodide ion
O2
oxide ion
S2
sulfide ion
P3
phosphide ion
N3
nitride ion
Naming Ions
Add ion (for cation) to the element name.
Ex. Li+ = lithium ion or lithium cation
For elements that can form multiple ions
Add the magnitude of the charge to the name
Ex. Fe2+ ion (II) Fe3+(II) Fe1+ (I)
Naming ions anions
Add -ide to element name stems.
Ex. Br- = bromide ion
O2 = oxide ion
Ionic formula
chem formula for the ionic compound
writing ionic formula
Cation goes 1st; anion goes last
total number of positive charges = total number of negative charges in an uncharged compound.
Ex. LiBr = Li+1 Br-1
NaCl = Na+ Cl-
Mg + O = Mgo
Li+ O2- = Li2O-2
Mg2+ Br1- = MgBr2
Naming ionic compounds
- The cation name goes 1st omit “ion” or “cation.”
- Anion’s name goes next or last.
Ex. LiBr2 = Lithium chloride, CaBr2 = Calcium Bromine - For cation with more than 1 positive charge.
Put the charge in (Roman numerals) in parentheses after the cation name.
Ex. FeCl2
= iron (II) chloride, FeCl3 = iron (III) chloride,
Polyatomic ion
Poly = many
Atomic = atoms
Ion = Charge
What she wants us to know:
Ammonium = NH4+
Acetate = C2H3O2- or CH3COO-
Bicarbonate (hydrogen carbonate) = HCO3
Carbonate = CO3^2-
Cyanide = CN-
Hydroxide = OH-
Nitrate = NO3-
Phosphate = PO4^3-
Sulfate = SO3^2-
How to find the molar mass formula
Pb3(PO4)
Ex. 1(107.868)= 107.868
2(12.011) = 24.022
2(12.0067) = 28.013
——————————
15.9903
Reminder = ionic bonding
Occurs between metals & non-metals
“Thru electrons transfer between atoms forms ions.
Fill outer octet/duet.
Oppositely charged ions attract each other.
Electron sharing
Atoms can also fill octets or duets by sharing electrons.
Covalent Bond
It occurs when two atoms share electrons to fill outer octets/duets.
NaCl
No charge - when they are from different sides/ think ionic.
Bonding pair of electron pairs of electrons involved in a covalent bond.
A molecule group of atoms held together by covalent bonds.
Look in a notebook, for example.
Each hydrogen has two electrons to fill. Its subshell (duet)
Single Bond
Covalent bond - consists of two shared electrons (1 pair)
Bonding electron pairs that form a covalent bond
Look in a notebook, for example.
It is between two atoms only, but a molecule can have multiple covalent bonds.
Covalent bond
Central atoms
atom in the center of a molecule
Surrounding atoms
That covalently bonds to the central atoms.
How to draw Luis diagrams for molecules (covalent) + ions.
- Draw Lewis structures of all the atoms
- Identify the central atom + the surrounding atoms.
- Add each surrounding atom to the central atom individually.
- IF THE MOLECULE IS AN ION
ADD ONE ELECTRON FOR EACH NEGATIVE CHARGE
REMOVE ONE ELECTRON FOR EACH POSITIVE CHARGE
Look in your notebook for examples.
Double Bond
A covalent bond is composed of two pairs of bonding electrons.
Look in a notebook, for example.
Triple Bond
A covalent bond is composed of three pairs of bonding electrons.
Covalent typically form between two non-metals. They form by sharing electrons.
Present in polyatomic ions.
Can form ionic bonds between outer charged species.
Look in my notebook for an example.
