Chemistry chapter 7
Mercury (I) ion (Mercurous ion)
*Hg2 2+
Hydrogen combined with a nonmetal
+1
Hydrogen combined with a metal
-1
only charge on Ag
1+
typical charge on group 1 metals
1+
Binary Ionic Compound Formulas
1. Metal written first Nonmetal written second 2. Use criss-cross method and subscripts to insure sum of charges = 0
only charge on Zn
2+
typical charge on group 2A metals
2+
only charge on Al
3+
empirical formula
A formula showing the lowest whole number ratio of atoms in a compound; (symbols for elements combined in a compound; subscripts show smallest whole-number mole ratio of different atoms in a compound)
Binary acids
Acids that consist of two elements, usually hydrogen and 1 halogen
Oxyacids
Acids that contain hydrogen, oxygen, and a third element (usually a nonmetal )
Molecular formula
Actual formula of a molecular compound
AlH₃
Aluminium Hydride
AlP
Aluminium Phosphide
Al(HSO₃)₃
Aluminum Bisulfite
Al₂(CO₃)₃
Aluminum Carbonate
Al3+
Aluminum ion
NH₄NO₃
Ammonium Nitrate
(NH₄)₂O₂
Ammonium Peroxide
(NH₄)PO₄
Ammonium Phosphate
(NH₄)₂S
Ammonium Sulfide
salt
An ionic compound composed of a cation and the anion from an acid
Binary Acids
Are acids that consist of two elements, usually hydrogen, and one of the halogens.
Oxyacids
Are acids that contain hydrogen, oxygen, and a third element usually a nonmetal.
AsCl₃
Arsenic Trichloride
Ions with greater number of oxygen atoms ends in
Ate
Covalent-network compounds
Atoms covalently bonded in a 3-D network
write the empirical formula for Ba²⁺ + Cl⁻
BaCl₂
Ba(ClO)₂
Barium Hypochlorite
Ba2+
Barium ion
BeI₂
Beryllium Iodide
Be2+
Beryllium ion
Bi(HSO₄)₃
Bismuth(III) Bisulfate
Br-
Bromide
Cd(NO₃)₂
Cadmium Nitrate
Ca(HSO₄)₂
Calcium Bisulfate
Ca2+
Calcium ion
CsBrO₃
Cesium Bromate
CsCN
Cesium Cyanide
CsNO₂
Cesium Nitrite
Cs+
Cesium ion
Cl-
Chloride
Cr(NO₃)₃
Chromium(III) Nitrate
Cr₂(SO₄)₃
Chromium(III) Sulfate
Cobalt (II) ion (Cobaltous ion)
Co2+
Cobalt (III) ion (Cobaltic ion)
Co3+
Co(ClO₃)₂
Cobalt(I) Chlorate
CoCl₂
Cobalt(II) Chloride
Co(HSO₃)₄
Cobalt(IV) Bisulfite
CoF₄
Cobalt(IV) Fluoride
Co3+
Cobaltic Cobalt(I II)
Binary ionic compound
Compounds of 2 elements
CuBr
Copper(I) Bromide
Cu₂CO₃
Copper(I) Carbonate
CuCl₂
Copper(II) Chloride
CuSO₄
Copper(II) Sulfate
Chromium (II) ion (Chromous ion)
Cr2+
Chromium (III) ion (Chromic ion)
Cr3+
Copper (I) ion (Cuprous ion)
Cu+
Copper (II) ion (Cupric ion)
Cu2+
Cu2+
Cupric
Cu(ClO₄)₂
Cupric Perchlorate
Cu+
Cuprous copper1
Iron (II) ion (Ferrous ion)
Fe2+
Iron (III) ion (Ferric ion)
Fe3+
Fe3-
Ferric
Fe2-
Ferrous
F-
Floride
C and Si
Form covalent bonds
Do Transition Metals for Cations or Anions?
Form positive ions (cations), but not always with the same charge.
Au(ClO₄)₃
Gold(III) Perchlorate
mono
Greek prefix for 1 with covalent bonding
deca
Greek prefix for 10 with covalent bonding
di
Greek prefix for 2 with covalent bonding
tri
Greek prefix for 3 with covalent bonding
tetra
Greek prefix for 4 with covalent bonding
penta
Greek prefix for 5 with covalent bonding
hexa
Greek prefix for 6 with covalent bonding
hepta
Greek prefix for 7 with covalent bonding
octa
Greek prefix for 8 with covalent bonding
nona
Greek prefix for 9 with covalent bonding
Mercury (II) ion (Mercuric ion)
Hg2+
H-
Hydride
H₂O₂
Hydrogen Peroxide
H₂SO₄(aq)
Hydrogen Sulfate
H+
Hydrogen ion
H₃PO₄(aq)
Hydrogen phosphate
Ion with 1 fewer oxygen atom than ite has the prefix
Hypo
-ite (tiny like a mite)
In oxyanions: The ion with less oxygen is given the ending: -
-ate (I ate too much; more)
In oxyanions: The ion with more oxygen is given this ending: -
hypo-
In oxyanions: The ion with one less less oxygen is given the beginning: ____-
per-
In oxyanions: The ion with one more more oxygen is given the beginning:
I-
Iodide
Oxidation Number =
Ion Charge - number of electrons transferred to or away from an atom when it becomes an ion.
Salt
Ionic compound composed of a cation and the anion from an acid
Fe₂O₃
Iron (III) Oxide
FeBr₂
Iron(II) Bromide
FeCO₃
Iron(II) Carobonate
FeCrO₄
Iron(II) Cromate
Fe(PO₄)₂
Iron(II) Phosphate
Fe₂(Cr₂O₇)₂
Iron(III) Dichromate
Ion with smaller number of oxygen atoms end in
Ite
Pb(HCO₃)₂
Lead(II) Bicarbonate
Pb(ClO₄)₂
Lead(II) Perchlorate
PbO₂
Lead(II) Peroxide
LiClO₃
Lithium Chlorate
LiH
Lithium Hydride
LiOH
Lithium Hydroxide
Li₃PO₄
Lithium Phosphate
Li+
Lithium ion
Mg(HSO₃)₂
Magnesium Bisulfite
Mg(ClO₂)₂
Magnesium Chlorite
MgCr₂O₇
Magnesium Dichromate
Mg₃N₂
Magnesium Nitride
Mg2+
Magnesium ion
Hg2+
Mercuric
Hg1+
Mercurous
Hg₂(C₂H₃O₂)₂
Mercury(I) Acetate
Hg₂CrO₄
Mercury(I) Chromate
Hg₂SO₄
Mercury(I) Sulfate
HgCL₂
Mercury(II) Chloride
Criss-Cross Method
Method used to insure that there is a balance between the number of electrons transferred by the metal to the nonmetal.
Manganese (II) ion (Manganous ion)
Mn2+
Manganese (III) ion (Manganic ion)
Mn3+
write the formula for Na⁺ + Cl⁻
NaCl
Anions
Negative ions
Ni(ClO₃)₂
Nickel(II) Chlorate
NiSO₃
Nickel(II) Sulfite
Nonmetal Anion Names end in __________
Nitride (N³⁻), Phosphide (P³⁻), Oxide (O²⁻), Sulfide (S²⁻),Fluoride (F¹⁻), Chloride (Cl¹⁻), , Bromide (Br¹⁻), , Iodide (I¹⁻)
Negative Ion (anion) Formation
Nonmetals tend to gain valence electrons to become stable and form negative ions called anions.
Oxidation numbers
Number of electrons that must be added to or removed from an atom in a combined state to convert the atom into the elemental form
In order to become stable, atoms will either gain or lose valence electrons in order to acquire an _________. (like a Noble Gas)
Octet.
O2-
Oxide
Lead (II) ion (Plumbous ion)
Pb2+
Lead (IV) ion (Plumbic ion)
Pb4+
Ion with 1 or more oxygen atoms than -ate has the prefix
Per
Percentage composition
Percentage by mass of each element in a compound
Pt(CN)₄
Platinum(IV) Cyanide
Pb4+
Plumbic Lead(IV)
Pb2+
Plumbous Lead (II)
Oxyanions
Polyatomic anions that contain oxygen
Common Polyatomic Ions
Polyatomic ions have their own names and charges and must either be memorized or looked up on a chart
Cations
Positive ions
KClO₃
Potassium Chlorate
KMnO₄
Potassium Permanganate
K+
Potassium ion
Rb₂CrO₄
Rubidium Chromate
Chemical formulas
Show relative number of atoms in a chemical compound
AgI
Silver Iodide
Ag₂SO₃
Silver Sulfite
Ag+
Silver ion
Tin (II) ion (Stannous ion)
Sn2+
Tin (IV) ion (Stannic ion)
Sn4+
NaHSO₄
Sodium Bisulfate
Na₂Cr₂O₇
Sodium Dichromate
Na₂SO₄
Sodium Sulfate
Sn4+
Stannic Tin(IV)
Sn2+
Stanous Tin(II)
Sr₃(PO₄)₂
Strontium Phosphate
SrS
Strontium Sulfide
S2-
Sulfide
Formula mass
Sum of the average atomic mass of all atoms represented in a formula
Molar mass
Sum of the masses of the element in one mole molecules or formula units that make up a compound
Empirical formula
The symbol of element in a compound with subscripts showing the smallest whole number mole ratio of the atom in the compound
SnF₄
Tin (IV) Fluoride
Sn₃(PO₄)₂
Tin Phosphate
SnBr₂
Tin(II) Brimide
SnO
Tin(II) Oxide
Sn(MnO₄)₄
Tin(IV) Permanganate
Sn(SO₄)₂
Tin(IV) Sulfate
Ionic Compound Formation
Total number of electrons transferred by the metal must equal the total number of electrons accepted by the nonmetal.
The reactivity of an atom is related to its _________ electrons
Valence
ZnCr₂O₇
Zinc Chromate
Zn(CN)₂
Zinc Cyanide
ZnNO₂
Zinc Nitrite
crystal lattice
a 3-dimensional geometrical structure formed by the alternative arrangement of positive and negative ions Shown above: crystal lattice of NaCl.
Oxyanion
a polyatomic ion composed of an element, usually a nonmetal, bonded to one or more oxygen atoms
CH3COO-
acetate
NH4+
ammonium
what is an ion
an atom that has either gained/lost electrons
Monatomic ion
an ion formed by only one atom
monatomic ion
an ion formed from a single atom. (remember to change nonmetals to -ide ending)
Polyatomic ions
an ion made up of two or more atoms bonded together that acts as a single unit with a net charge
Anion
an ion with a negative charge
Cation
an ion with a positive charge
Electrolyte
an ionic compound whose aqueous solution conducts an electric current
name of ions with - charges
anions "a nEGATIVE ion"
ions
atoms that have acquired either a positive or a negative charge.
Formation of an Ionic Bond
between a metal that loses one or more valence electrons and a nonmetal that gains one or more valence electrons.
CO3-
carbonate
name of ions with + charges
cations "c a + ion"
Formula Unit
chemical formula for an ionic compound; simplest ratio of positive to negative ions; overall charge = 0
binary compounds
compounds composed of two different elements; (compounds of 2 elements between metal (positive, s-block and p-block) and nonmetal (negative); metal is always listed first; change nonmetal to -ide ending)
Acid
distinct type of molecular compound; would show up on pH scale as a value below 7
HcO3-
hydrogen carbonate ( bicarbonate )
OH-
hydroxide
Monatomic ions
ions formed from 1 atom
Polyatomic Ions
ions made up of more than one atom; acts as an individual ion in a compound; charge applies to entire group of atoms.
Stock system
it is a widely used system of chemical nomenclature developed by the german chemist Alfred Stock. In this system, the oxidation states of some or all the elements in a compound are indicated in parentheses by Roman numerals
Differentiate between molecular and ionic compounds
metal + non-metal = ionic compound non-metal + non-metal = molecular compound
Positive Ion (Cation) Formation
metals tend to lose valence electrons to become stable and form positive ions called cations
nomenclature
naming system
NO3-
nitrate
binary molecular compounds
nonmetal to nonmetal; covalent bonds; uses Greek prefixes
Monatomic Ions
one-atom ions
( PO4 )3-
phosphate
oxyanions
polyatomic ions that contain oxygen
Stock system
specifically used for d-block elements, use Roman numeral to describe charge of metal, use periodic charge to find charge of nonmetal
Properties of Ionic Compounds
strong attraction between oppositely charged ions means: high melting & boiling points ionic crystals are very hard but brittle conduct electricity when dissolved in solution or melted (ELECTROLYTES)
If the metal loses more electrons than the nonmetal gains,then __________ must be used to balance the charges
subscripts.
( SO4 )2-
sulfate
oxidation states
the condition of an atom expressed by the number of electrons that the atom needs to reach its elemental form
Ionic bond
the electrostatic force that holds oppositely charged particles together in an ionic compound
Lattice energy
the energy required to separate one mole of the ions of an ionic compound, which is directly related to the size of the ions bonded and is also affected by the charge of the ions
Chemical bond
the force that holds two atoms together; may form by the attraction of a positive ion for a negative ion or by sharing electrons
Alloy
the mixture of elements that has metallic properties; most commonly forms when the elements are either similar in size, or the atoms of one element are much smaller than the atoms of the other
Oxidation numbers
the number assigned to an element that shows how many electrons it gains, loses, or shares
percentage composition
the percentage by mass of each element in a compound
Oxidation number
the positive or negative charge of a monatomic ion
Formula unit
the simplest ratio of ions represented in an ionic compound
formula mass
the sum of the average atomic masses of all atoms represented in the formula of any molecule, formula unit, or ion
Greek prefixes
used to name molecules with covalent bonds
