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