Nomenclature
- Acids and Bases
- Acids -
molecules that can lose H+ (proton donors) in
water making H3O+(aq) in water. Note H+(aq)
is really just short hand for H3O+(aq). Also
note that (aq) means dissolved and surrounded by water. If there are H+(aq)
ions called hydronium ions present, then the solution is acidic.
- Know
these acids: HCl, HNO3 and H2SO4.
Hydrochloric, nitric and sulfuric.
- Reactions
looks like this: HCl(g) +H2O(l) g H3O+(aq) + Cl-(aq)
- Remember
people that take acid are losers - so acids LOSE H+
- Bases -
molecules than can gain H+ (proton acceptors) and/or make OH-
in water. If there are OH-(aq) ions present called
hydroxide ions, then the solution is basic.
- Know
these bases: NaOH, KOH, Ba(OH)2 which are all solids
- Reactions
looks like this when put in water: NaOH(s) g Na+(aq) + OH-(aq)
- Why are
these dissolving in water in the first place? Well because the sum
of all the ion-dipole forces created by having the ions surrounded by
water are greater than the original ionic or covalent bond. Not all acids
and bases dissolve in water so easily! You'll learn a lot more in
second semester.
- Nomenclature SUPER IMPORTANT
- Ionic Compounds
- Why do
they form in the first place? Well remember that each atom's goal
is to be s2p6 and to get there they must lose or
gain electrons (except the Noble Gases) and then they are cations or
anions with an oxidation state. Review it
here! IMPORTANT
- You MUST
be able to put ionic formulas together so that the charges sum to
zero. Practice
is below this outline. DO IT!
- name of
metal cation + name of nonmetal anion + ide
- Examples
- NH4Cl
- ammonium chloride
- CaCO3
- calcium carbonate
- NaOH -
sodium hydroxide
- MgO -
magnesium oxide
- Li3P
- lithium phosphide
- CaBr2
calcium bromide
- Na2S
- sodium sulfide
- Mg3(PO4)2
- magnesium phosphate
- Na2SO4
- sodium sulfate
- Variable charge metal
compounds
- name of
transition metal, (charge in Roman numerals) + name of nonmetal + ide
- Why the
Roman numeral? Well the oxidation state of most transition metals
varies - so we have to indicate what it is.
- Examples
- Fe2O3
- iron(III) oxide
- AgCl -
silver(I) chloride
- CuS -
copper(II) sulfide
- Co(NO3)3
- cobalt(III) nitrate
- FeSO4
- iron(II) sulfate
- Zn(OH)2
- zinc(II) hydroxide
- iron(III)
flouride - FeF3
- iron(II)
phosphate - Fe3(PO4)2
- Remember
you are supposed to know all these atom's names: H, He, Li, Be, B, C, N,
O, F, Ne, Na, Mg, Al, Si, P, S, Cl, Ar, K, Ca, Cr, Mn, Fe, Co, Ni, Cu,
Zn, Br, Kr, Sr, Ag, Sn, I, Ba, Au, Hg, Pb and U IMPORTANT
- Hey - Ag is always +1, Zinc and Cadmium are
always +2 so you don't need to use a Roman Numeral with them: AgCl
is silver chloride, Zinc fluoride is ZnF2, Ag2S is
silver sulfide
- Covalent Compounds
- prefix
name of least electronegative nonmetal + prefix name of most
electronegative nonmetal
- prefixes
are mono, di, tri, tetra, penta, hexa, hepta, octa (mono is ommitted
from the first element)
- Examples
- CO2
- carbon dioxide
- CO -
carbon monoxide
- PCl5
- phosphorus pentachloride
- SF4
- sulfur tetraflouride
- P2O5
- diphosphorus pentoxide
- SiO2
- silicon dioxide
- H2O2
- dihydrogen dioxide
- nitrogen
monoxide - NO
- carbon
tetrachloride - CCl4
- nitrogen
trihydride - NH3
- iodine
heptaflouride - IF7
- Ionic
compounds with polyatomic ions
- treat
polyatomic ions as groups that always stay together
- never
change the name of the polyatomic ion, otherwise name as ionic compounds
- Memorize
these: NH4+, CH3COO-,
CN-, HCO3-, OH-,
MnO4-, NO2-, NO3-,
CO32-, SO42-, SO32-,
PO43- IMPORTANT
- NaOH is
sodium hydroxide, Ca(NO3)2 is calcium nitrate,
MgSO4 is magnesium sulfate
- ammonium
sulfide is (NH4)2 S, calcium carbonate is CaCO3,
magnesium phosphate is Mg3(PO4)2
- Oxoanions
- different numbers of oxygens
- Know
hypochlorite, chlorite, chlorate, perchlorate
- Try
example 2.14 and 2.15. Try problems 2.27-29.
- Oxoacids
- Know
hypochlorous, chlorous, chloric, and perchloric acids
- Know
nitrous and nitric acids
Final Notes - At this point in time you should be able to:
- Given any
covalent molecule, name the molecule.
- Given any
group 1 or 2 metal, and a nonmetal, you should be able to predict the
formula of the resulting ionic compound, know the oxidation states on the
ions, and name the compound.
- Be able to
name a transition metal compound.
- Predict
the most common oxidation state for the ions the following elements
form: Li, S, Cs, Al, Br, N, Mg, K, P, Bi, F, Ne, Ba, Pb, As, Te.
- How many
electrons total do the noble gases have?
- What will
the following atoms do in order to be like a noble gas? Ga, F, I,
Be, K
- Predict
the ionic compound formulas for the following pairs of elements.
(Assume they can make an ionic compound) Li and Cl, K and S, Na and
P, Mg and Br, Ca and S, Ba and N, Al and F, Ga and O, In and P, Pb and F,
Pb and O, Bi and Cl, Bi and S, Po and F
- What makes
the noble gases so stable?
- What is
the difference between an ionic and covalent bond?
- If an atom
has more protons than electrons what is it called?
- Ionic
compounds are held together by ionic bonds which are basically
____________ attractions between ions.
- Name all
the elements that form covalent bonds with themselves and give their
formulas.
- Why does
hydrogen occur naturally as H2?
- Name the
following ionic compounds: KI, AlBr3, MgSO4,
Na3PO4, LiCH3COOH, Fe(CN)2, Ni(HCO3)3,
KOH
- Give the
chemical formulas for the following ionic compounds: calcium
nitrate, lithium iodide, sodium carbonate, ammonium nitride
- Name the
following covalent compounds: CO, PI5, IF7,
SiF4
- Write
chemical formulas for the following covalent compounds: nitrogen
trihydride, silicon tetrabromide, sulfur dihydride
- Name the
following compounds: KNO3, N2O5
NaBr, PH3, MgS, Ca(OH)2, CS2, NH4I,
LiF, (NH4)2CO3, PCl5
- Write
chemical formulas for the following: dihydrogen disulfide, lithium
nitride, calcium phosphide, nitrogen tribromide, magnesium nitride, sodium
iodide, sulfur tetrahydride, potassium phosphate, silver permanganate,
zinc nitrite, sodium sulfite
Answers:
- Li is +1,
S is -2, Cs is +1, Al is +3, Br is -1, N is -3, Mg is +2, K is +1, P is
-3, Bi is +5, F is -1, Ne does not make ions, Ba is +2, Pb is +4, As is +5
or -3, Te is +6 or -2.
- 2, 10, 18,
36, 54 and 86.
- Ga will
lose 3 electrons to become Ga+3, F will gain one electron to
become F-, I will gain one electron to become I-, Be
will lose two electrons to become Be+2, K will lose one
electron to become K+.
- Li and Cl
make LiCl, K and S make K2S, Na and P make Na3P, Mg
and Br make MgBr2, Ca and S make CaS, Ba and N make Ba3N2
(Ba is +2 and N is -3 so we need three Ba's to make +6 and we need two N's
to make -6 because +6-6 = 0), Al and F make AlF3, Ga and O make
Ga2O3, In and P make InP, Pb and F make PbF4,
Pb and O make PbO2, Bi and Cl make BiCl5, Bi and S
make Bi2S5 (S is -2 while Bi is either +5 or
-3. Since S is already negative, Bi must be positive. We need
five S's to make -10 and we need 2 Bi's to make +10), Po and F make PoF6
(Here Po will be +6 instead of -2 since it is bonding with F which is
negative)
- The have
full outer s and p subshells = 8 electrons. Except helium which just
has the full 1s with 2 electrons.
- An ionic
bond involves the transfer of electrons from a metal to a nonmetal.
A covalent bond involves the sharing of electrons between 2 or more
nonmetals.
- cation
- electrostatic
- hydrogen
occurs naturally as H2, Nitrogen occurs naturally as N2,
Oxygen as O2, Fluorine as F2, Chlorine as Cl2, Bromine
as Br2, Iodine as I2, and just for fun Phosphorus as
P4, Sulfur as S8 and Selenium as Se8
- Each
hydrogen atom has only one electron so it is not stable. H wants to
have 2 electrons to be like helium. If two H atoms come together
they can share their electrons so that each H then has 2 electrons.
So then each H is stable and like a noble gas. H : H
- potassium
iodide, aluminum bromide, magnesium sulfate, sodium phosphate, lithium
acetate, iron(II) cyanide, nickel(III) bicarbonate, potassium hydroxide
- Ca(NO3)2,
LiI, Na2CO3, (NH4)3N
- carbon
monoxide, phosphorus pentaiodide, iodine heptafluoride, silicon
tetrafluoride
- NH3,
SiBr4, SH2
- potassium
nitrate, dinitrogen pentoxide, sodium bromide, phosphorus trihydride,
magnesium sulfide, calcium hydroxide, carbon disulfide, ammonium iodide,
lithium flouride, ammonium carbonate, phosphorus pentachloride
- H2S2,
Li3N, Ca3P2, NBr3, Mg3N2,
NaI, SH4, K3PO4, AgMnO4, Zn(NO2)2,
Na2SO3