Naming Compounds Writing Formulas Chapter 5. Systematic Naming l There are too many compounds to...
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Transcript of Naming Compounds Writing Formulas Chapter 5. Systematic Naming l There are too many compounds to...
Systematic Naming There are too many compounds to
remember the names of them all. Compound is made of two or more
elements. Put together atoms. Name should tell us how many and
what type of atoms.
Periodic Table More than a list of elements. Put in columns because of similar
properties. Each column is called a group.
Atoms and ions Atoms are electrically neutral. Same number of protons and electrons. Ions are atoms, or groups of atoms,
with a charge. Different numbers of protons and
electrons. Only electrons can move. Gain or lose electrons.
Anion A negative ion. Has gained electrons. Non metals can gain electrons. Charge is written as a superscript on
the right.
F1- Has gained one electron
O2- Has gained two electrons
Cations Positive ions. Formed by losing electrons. More protons than electrons. Metals form cations.
K1+ Has lost one electron
Ca2+ Has lost two electrons
Two Types of Compounds Molecular compounds Made of molecules. Made by joining nonmetal atoms
together into molecules.
Two Types of Compounds Ionic Compounds Made of cations and anions. Metals and nonmetals. The electrons lost by the cation are
gained by the anion. The cation and anions surround each
other. Smallest piece is a FORMULA UNIT.
Two Types of Compounds
Smallest piece
Melting Point
State
Types of elements
Formula Unit Molecule
Metal and Nonmetal
Nonmetals
solidSolid, liquid or gas
High >300ºC Low <300ºC
Ionic Molecular
Chemical Formulas Shows the kind and number of atoms in
the smallest piece of a substance. Molecular formula- number and kinds of
atoms in a molecule. CO2
C6H12O6
Formula Unit The smallest whole number ratio of
atoms in an ionic compound. Ions surround each other so you
can’t say which is hooked to which.
Charges on ions For most of Group A elements,
location on the Periodic Table can tell what kind of ion they form
Elements in the same group have similar properties.
Including the charge when they are ions.
2+
1+
3+ 3- 2- 1-
Charge in groups 1A, 2A and 3A is the group number
in 5A, 6A and 7A are different.
Can also use electron dots If it has a few
it loses them
If it has many, it gains enough for octet
K+
Al3+
F -N
3-
Naming ions
Cation- if the charge is always the same (Group A) just write the name of the metal.
Most transition metals can have more than one type of charge.
Indicate the charge with Roman numerals in parenthesis.
Co2+ Cobalt(II) ion
Naming ions
A few, like silver, zinc and cadmium only form one kind of ion
Don’t get roman numerals Ag+ silver ion Zn2+ zinc ion Cd2+ cadmium ion
Name theseNa1+ Sodium ionCa2+ Calcium ionAl3+ Aluminum ionFe3+ Iron(III) ionFe2+ Iron(II) ion
Li1+ Lithium ionPb2+ Lead(II) ion
Write Formulas for these
Potassium ion K1+
Magnesium ion Mg2+
Copper(II) ion Cu2+
Chromium(VI) ion Cr6+
Barium ion Ba2+
Mercury(II) ion Hg2+
Polyatomic ions Groups of atoms that stay together
and have a charge. Covalently bonded You must note these.
(pg 178 Table 2)
1- ions Acetate C2H3O2
1-
Nitrate NO31-
Nitrite NO21-
Hydroxide OH1-
Permanganate MnO41-
Cyanide CN1-
2- ions Sulfate SO4
2-
Sulfite SO32-
Carbonate CO32-
Chromate CrO42-
Dichromate Cr2O72-
Silicate SiO32-
Adding Hydrogen to Polyatomics Hydrogen ions are 1+ Attach to other polyatomic ions-
changes charge by one Sulfate SO4
2-
Hydrogen sulfate HSO41-
Phosphate PO43-
Hydrogen phosphate HPO42-
Dihydrogen phosphate H2PO41-
Naming Binary Ionic Compounds Binary Compounds - 2 elements. Ionic - a cation and an anion. The name is just the names of the ions. Cation first anion second Easy with Group A elements. NaCl = Na+ Cl- = sodium chloride
MgBr2 = Mg2+ Br- = magnesium bromide
Na2S
Naming Binary Ionic Compounds The problem comes with the transition
metals. Cation name includes the charge. The compound must be neutral. same number of + and – charges. Use the negative charge to find the
charge on the positive ion.
Naming Binary Ionic Compounds Write the name of CuO Need the charge of Cu O is 2- copper must be 2+ Copper(II) oxide Name CoCl3 Cl is 1- and there are three of them = 3- Co must be 3+ Cobalt(III) chloride
Naming Binary Ionic Compounds Write the name of Cu2S. Since S is 2-, the Cu2 must be 2+, so
each one is 1+. copper(I) sulfide Fe2O3 Each O is 2- 3 x 2- = 6- 2 Fe must = 6+, so each is 3+. iron(III) oxide
Ternary Ionic Compounds Will have polyatomic ions At least three elements (3 capital letters) Still just name the ions
NaNO3
CaSO4
CuSO3
Writing Formulas The charges have to add up to zero. Get charges on pieces. Cations from name or periodic table. Anions from periodic table or polyatomic. Balance the charges by adding subscripts. Put polyatomics in parenthesis if there is
more than one of them
Writing Formulas Write the formula for calcium chloride. Calcium is Ca2+
Chloride is Cl1- Ca2+ Cl1- would have a 1+ charge. Need another Cl1- Ca2+ Cl2
1-
Write the formulas for these Lithium sulfide tin (II) oxide tin (IV) oxide Copper (II) sulfate Iron (III) phosphide gallium nitrate Iron (III) sulfide ammonium sulfide
Yes
Charge from name
Charge from table
No
Formula and
charge from
memory
Charge from table
Yes No
M+X Nm-Y
MYNmX
Ionic
Roman Numeral?
Polyatomic?
Things to look for If cations have (), the number is their
charge. Not how many. If anions end in -ide they are probably off
the periodic table (Monoatomic) If anion ends in -ate or -ite it is polyatomic The positive piece always gets written first Hydrogen- it depends on where it’s at
– If it is second, it’s a nonmetal -hydride
Molecular compounds made of just nonmetals smallest piece is a molecule can’t be held together because of
opposite charges. can’t use charges to figure out how
many of each atom
Easier Ionic compounds use charges to
determine how many of each.
– Have to figure out charges.
– Have to figure out numbers. Molecular compounds name tells you
the number of atoms. Uses prefixes to tell you the number
Naming
Exception - we don’t write mono- if there is only one of the first element.
No ao oo double vowels when writing name, io, oi, and ai are okay.
Prefix name Prefix name -ide
To write the name write two words
Write formulas for these diphosphorus pentoxide tetraiodine nonoxide sulfur hexaflouride nitrogen trioxide Carbon tetrahydride phosphorus trifluoride aluminum chloride diagram
Acids Compounds that give off hydrogen ions
when dissolved in water. Must have H in them. will always be some H next to an anion. The anion determines the name.
Naming acids If the anion attached to hydrogen is
ends in -ide, put the prefix hydro- and change -ide to -ic acid
HCl - hydrogen ion and chloride ion hydrochloric acid H2S hydrogen ion and sulfide ion hydrosulfuric acid
Naming Acids If the anion has oxygen in it it ends in -ate or -ite change the suffix -ate to -ic acid HNO3 Hydrogen and nitrate ions
Nitric acid change the suffix -ite to -ous acid HNO2 Hydrogen and nitrite ions
Nitrous acid
Writing Formulas Hydrogen will always be first name will tell you the anion make the charges cancel out. Starts with hydro- no oxygen, -ide no hydro, -ate comes from -ic, -ite
comes from -ous
Write formulas for these hydroiodic acid acetic acid carbonic acid phosphorous acid hydrobromic acid diagram
38.Name these acidsa) H2C2O4 b) HF c) HClO2 d)
H2CO3
39.Write formulas for these compoundsa) nitrous acid b) hydroselenic acidc) phosphoric acid d) acetic acid
43. Name these compoundsa) AlF3 b) SnO2 c) Fe(C2H3O2)3
d) KHSO4 e) CaH2 f) HClO3
g) Hg2Br2 h) H2CrO4
44. Write formulas for thesea) Phosphorus pentabromideb) Carbon chloridec) potassium permanganate
43. Name these compoundsa) AlF3 b) SnO2 c) Fe(C2H3O2)3
d) KHSO4 e) CaH2 f) HClO3
g) Hg2Br2 h) H2CrO4
44. Write formulas for thesea) Phosphorus pentabromideb) Carbon chloridec) potassium permanganated) Calcium hydrogen carbonatee) dichlorine heptoxidef) trisilicon tetrahydrideg) sodium dihydrogen phosphate
Summary Periodic table
– Grouped by properties Metals- make cations
– 2 types those with () and those without Nonmetals make anions
– Three types• Without O -ide• With O -ite and -ate
Only electrons can move to make ions