Chapter 6 Flashcards
Steps in balancing an equation
1) ID the number and type of atom on each side
constructing tables on each side helps
2) Add coefficients to balance the atoms (to have the same number and type of atoms of each on both sides)
3) DONT touch the subscripts
balance elemental forms last
Law of conservation of mass
matter is neither created nor destroyed in a chemical reaction
Subscripts
show the number of atoms w/in each molecule or formula unit (H2)
In a balanced equation:
the number and type of each atom are the same on both sides of the equation
properly balanced, smallest whole number ratio
Balancing polyatomic ions
do not break them apart into their elements, keep them as they are and balance them as such
4 Phase notations
(s) - solid
(l) - liquid
(g) - gas
(aq) - aqueous solution (dissolved in water)
Classifying reactions: Decomposition reaction
A single reactant forms two or more products
“one forms two or more”
(CaCO3 —-> CaO+CO2)
Classifying reactions: Synthesis (combination) reactions
Two reactants join together to form a single product
“two form one”
(CaO +H2O —-> Ca(OH)2)
Classifying reactions: Single displacement reaction
One element replaces another element in a compound
“one element replaces another”
(Zn+CuSO4 —->ZnSO4+Cu)
Classifying reactions: Double displacement reaction
two compounds rearrange to form two new compounds (involve a “swap” of cation-anion pairs)
“two ions replace each other”
(KCl+AgNO3——>KNO3+AgCl)
what type of reaction produces an iconic compound
a synthesis reaction of a metal cation and a nonmetal anion element
when an atom is oxidized it
looses electrons
when an atom is reduced (reduction) it
gains electrons
OIL RIG
Oxidation Is Loss Reduction Is Gain
Combustion reactions
Reactions in which oxygen gas combines with elements or compounds to produce oxides
Hydrocarbons
compounds composed of hydrogen and carbon
Combustion of hydrocarbons
Hydrocarbon+ oxygen —–> carbon dioxide + water
Ionic compounds dissociating
when dissolved in water the cations and anions of the compound are pulled apart and surrounded by water molecules
Molecular equation
shows ions together as neutral compounds
only thing that changes is the phase symbol?
(shown as molecules)
ionic equation
shows dissociated ions as separate species
shows individual ions
Factors that effect solubility
charge on ions
size of ions
how tightly ions are packed together
Usually soluble
ionic compounds containing halogens (unless bonded to Ag^+ or Pb^2+)
Sulfate (except when bonded with Ag^+ or Pb^2+, Ba^2+, Ca^2+)
Usually not soluble
compounds composed of ions w/ a charge of 2 or 3 three
most other ions
Compounds containing [ ] are always soluble
Alkali metals
ammonium
Large 1- oxyanions
compounds composed of ions w a charge of 1
Precipitation reaction
Two aqueous solutions produce an insoluble product
(double displacement reactions)
the driving force is the formation of a solid
The precipitate
the insoluble solid formed from a precipitate reaction
spectator ions
the ions that are present in a precipitation reaction but not directly involved
Complete ionic equation
shows all ions present (including the spectator ions)
precipitate shown as a compound bc its no longer separate ions
Net ionic equation
only includes ions included in the precipitation
omit spectator ions and only include the ions directly involved in the precipitation
Acids
Compounds that produce H+ ions in aqueous solutions
Bases
Compounds that produce OH- ions in aqueous solutions
Neutralization reactions
Acid + base —> water + “salt”
a double displacement reaction
formation of water is the driving force of the reaction
an H+ and a OH- forms water
A “salt”
the ionic compound formed from the spectator ions (of a neutralization reaction)?
