Exam 2

Question 1

Mass Percentage Equation

Answer 1

(mass of component) / (mass of solution) x 100%

Question 2

Acid-Base Reactions

Answer 2

where a hydrogen ion (H+) is transferred from one chemical species to another

Question 3

Common Strong Acids

Answer 3

HBr (hydrobromic acid)
HCl (hydrochloric acid)
HI (hydroiodic acid)
HNO3 (nitric acid)
HClO4 (perchloric acid)
H2SO4 (sulfuric acid)

Question 4

Base

Answer 4

substance that will dissolve water to yield hydroxide ions (OH)-

most common are G1 and G2 combinations with hydroxide ions

Question 5

Strong Bases

Answer 5

same as mentioned in base definition

completely dissociate in water

Question 6

Neutralization Reaction

Answer 6

a specific type of acid-base reaction where the reactants are an acid and a base (but not water), and the products are often a salt and water

acid + base –> salt + water

Question 7

How to write an equation for an acid-base reaction (neutralization)

Answer 7

a lot like solving for net ionic equation but instead of ions, it’s strong bases

keep polyatomic ions together always
cancel out the strong bases

Question 8

Oxidation-Reduction Reactions are

Answer 8

electron transfer between reactants species to create ionic products

Ex. 2Na + Cl2 –> 2NaCl

Question 9

Half Reaction

Answer 9

view 2Na + Cl2 –> 2NaCl with regard to each individual reactant to represent their fate

Ex. 2Na –> 2Na+ 2e-
Cl2 + 2e- –> 2Cl-

shows that Na atoms lose electrons while Cl atoms gain

Question 10

Oxidation

Answer 10

loss of electrons

Question 11

Reduction

Answer 11

gain of electrons

Question 12

Reductant

Answer 12

Na gets oxidized and functions as a reducing agent

provides electrons for Cl

Question 13

Oxidant

Answer 13

Cl functions as oxidizing agent and receives electrons lost from Na in this case

Question 14

Oxidation Number

Answer 14

the charge atoms would possess if a compound were ionic

Question 15

4 Rules to Assign an Oxidation Number

Answer 15

1. O.N of atom in elemental substance is 0
2. ON of monatomic ion is = to ion charge
3. ON numbers for nonmetals are usually
   a. H: +1 when combined with nonmetals and -1 with
   metals
   b. O: -2
   c. halogens: F=-1 always and for other halogens when combo with O or other halogens
4. sum of ONs for all atoms in molecule or polyatomic ion = charge on molecule or ion

Question 16

Single Displacement (replacement) Reactions

Answer 16

redox reactions where an ion in a solution is replaced via oxidation of a metallic element

Ex. Zn(s) + 2HCl(aq) –> ZnCl2(aq) + H2(g)

Question 17

Titrations

Answer 17

think of the lab we did where our goal was to get the mixture to pink