types of reactions

Question 1

• solubility
• soluble

Answer 1

• maximum concentration of a substance that can be achieved under specified conditions
• large solubility

Question 2

• precipitate
• insoluble

Answer 2

• solutions conditions are such that its concentration exceeds its solubility
• low solubility, readily precipitate from solution

Question 3

precipitation reaction

Answer 3

dissolved substances react to form one (or more) solid products

Question 4

acid based reactions

Answer 4

a hydrogen ion, H+, is transferred from one chemical species to another -example: HCI is a strong acid

HCI(aq) + H₂O(aq) →Cl^-(aq) + H₃O³(aq)

H+ ions are transferred from HCI molecules to H₂O molecules

Question 5

precipitation reactions

example one

Answer 5

-molecular equation:

2KI(aq)+Pb(NO₃)₂(aq)→Pbl₂(s)+2KNO₃(aq)

-Ionic equation

2K⁺(aq)+2l^-(aq)+Pb²⁺(aq)+2NO₃^-(aq)→Pbl₂(s)+2K⁺(aq)+2NO₃-(aq)

-Net Ionic Equation

Pb²⁺(aq)+2l^-(aq)→Pbl₂(s)

Question 6

arrhenius acids and bases

Answer 6

arrhenius acid, substance that increases the concentration of H⁺(aq)

arrhenius base, increases the concentration of OH^-(aq)

does not include:

• compounds, not in aqueous solution
• acids that do not contain H⁺
• baes that do not contain OH^-

Question 7

precipittion reaction

Answer 7

-Molecular equation:

NaCl(aq)+AgNO₃(aq)→AgCl(s)+NaNO₃(aq)

• AgCl precipitates from solution, which is consistent with solubility rules
• Net ionic equation:

Ag⁺(aq)+Cl^-(aq)→AgCl(s)

Question 8

Oxidation

Reduction

Answer 8

• loss of electrons
• gain of electrons

Question 9

reducing agent

oxidizing agent

Answer 9

• provides electrons for (or reduces) chlorine
• effectively removes electrons from (oxidizes) sodium

Question 10

strong acids

Answer 10

acids that dissociate - 100%

Question 11

neutralization reaction

Answer 11

• specific type of acid-base reaction in which the reactants are an acid and a base, the products are often a salt and water, and neither reactant is the water itself.
• Acid+base →salt + water
• example:

Mg(OH)₂(s)+2HCl(aq) →MgCl₂(aq) + 2H₂O(l)

-MgCl₂ is a salt

Question 12

oxidation number

Answer 12

the charge its atoms would possess if the compound was ionic

Question 13

rules for assigning oxidation numbers

Answer 13

1. oxidation number of an atom in an elemental substance is zero
2. oxidation number of a monatomic ion is equal to the ions charge
3. oxidation numbers, nonmetals
   - hydrogen:
   - +1 when combined with non metals
   - 1 when combined with metals
   - oxygen:
   - -2 in most compounds
   - sometimes -1(so called peroxides, O₂^2-)
   - very rarely -1/2 ( so called superoxides, O₂^-)
   - positive values when combined with F (values vary)
   - Halogens:
   - -1 for F always
   - -1 for other halogens except when combined with oxygen or other halogens (positve oxidation numbers in these cases, varying values)
4. the sum of the oxidation numbers for all atoms in a compound is zero, and in a polyatomic ion equals the charge on the ion.

Question 14

oxidation reduction (redox) reactions

redox

Answer 14

redox: electrons are transferred

2Na(s) + Cl₂(g)→2NaCl(s)

2Na(s)→2Na⁺(s) +2e^-

Cl₂(g) + 2e^-→2Cl^-(s)