How many types of acids are there?
2: containing oxygen & not containing oxygen
Why is are Roman numerals used?
Some metals can take more than one charge. The Roman numeral always indicates the charge on the metal in that compound. The Roman numeral does not tell you the number of metal atoms present in the compound.
Naming acids w/out oxygen
Ion Name: •per\_\_\_ate •\_\_\_ate •\_\_\_ite •hypo\_\_\_ite
Acid Name: •per\_\_\_ic •\_\_\_ic •\_\_\_ous •hypo\_\_\_ous
True or false: Electrons are almost never shared in pairs.
False: Electrons are almost always shared in pairs.
Covalent Bond
Two or more valence electrons are shared between two atoms
Single Bond
When one pair of electrons are shared between two atoms
The nucleus of the one is attracted to the _______ _________ of the other.
Valence electrons
Electronegativity
Attraction of one atom for the electrons of another atom (fluorine is the biggest); differences: The type of bond is found by determining the difference (subtract) of the electronegativities
Nonpolar covalent bond
When electrons are equally shared between two atoms
Polar covalent bond
When electrons are unequally shared
Dipole
When a bond or molecule has unequal sharing
Drawing Lewis structures for molecules
- Count up the number of valence electrons for each atom in the molecule
-can do this easily by using the group number for each atom in the periodic table
-adjust the valence electrons if you are drawing the structure for an ion - Draw the atoms bonded together
-usually the central atom is written first in a molecule, or the atoms in the molecule are written in the order in which they are
-each bond contains two electrons - Fill in the remaining valence electrons to give all atoms an octet of electrons. leaving the central atom for last
A. If there are not enough electrons to complete all octets, use multiple bonds.
B. If there are extra electrons, place them around
Exceptions to the Octet Rule
- Hydrogen and Helium- both can hold only two electrons
- Boron- often has only six electrons
- Free radicals- compounds with an odd number of electrons
- Atoms with “d” subshells- can hold more than eight electrons
True or False: each pair of bond electrons counts for both of the atoms in the bond
True
When an ion has a negative charge, what is required?
For this type of ion, surround the structure with brackets and write the charge on the ion outside.
What is VSEPR?
Valence shell electron pair repulsion (VSEPR) theory is a model used, in chemistry, to predict the geometry of individual molecules from the number of electron pairs surrounding their central atoms.
Carbonate
Percarbonate: CO4(charge of -2)
Carbonate: CO3(charge of -2)
Carbonite: CO2(charge of -2)
Hypocarbonite: CO(charge of -2)
Sulfate
Persulfate: SO5 (charge of -2)
Sulfate: SO4 (charge of -2)
Sulfite: SO3 (charge of -2)
Hyposulfite: SO2 (charge of -2)
Phosphate
Perphosphate: PO5(charge of -3)
Phosphate: PO4(charge of -3)
Phosphite: PO3(charge of -3)
Hypophosphite: PO2(charge of -3)
Chlorate
Perchlorate: ClO4(charge of -1)
Chlorate: ClO3(charge of -1)
Chlorite: ClO2(charge of -1)
Hypochlorite: ClO(charge of -1)
Iodate
Periodate: IO4(charge of -1)
Iodate: IO3(charge of -1)
Iodite: IO2(charge of -1)
Hypoiodite: IO(charge of -1)
Acetate
Peracetate: C2H3O3(charge of -1)
Acetate: C2H3O2(charge of -1)
Acetite: C2H3O(charge of -1)
Manganate
Permanganate: MnO4(charge of -1)
Manganate: MnO3(charge of -1)
Manganite: MnO2(charge of -1)
Hypomanganite: MnO(charge of -1)
Bromate
Perbromate: BrO4(charge of -1)
Bromate: BrO3(charge of -1)
Bromite: BrO2(charge of -1)
Hypobromite: BrO(charge of -1)
