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49 Cards in this Set
- Front
- Back
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Soulution |
homogeneous mixture of two or more substances |
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solvent |
solution component present in greatest amount |
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solute(s) |
soulution component(S0 present in lesser amount. |
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bronsted acid |
is a proton donor |
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bronsted base |
is a proton acceptor |
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Electorlytes |
are soluble compounds that conduct current when dissolved in a solvent, usually water. |
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Strong electrolytes |
dissociate completely into ions i soulution |
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Weak electrolytes |
dissociate partially into ions in soulution |
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Non electrolytes |
do not dissociate into a soulution |
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dissociate reaction |
When and ionic solid dissloves in wate, it breaks into its constituents ions. Conduct electric current and are electrolytes. |
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Monprotic Acids |
an acid that donates only one proton or hydrogen atom per molecule to an aqueous solution. This is in contrast to acids capable of donating more than one proton or hydrogen, which are called polyprotic acids. |
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Diprotic acids |
a class of Arrhenius acids which are capable of donating two protons or hydrogen cations per molecule when dissociating in aqueous solutions. |
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Triprotic |
the one which release three hydrogen ions in aqueous solution. |
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Netralization |
Mixing and acid and a base leads to a reaction known as_______, In which the resulting solutions is neither acdici nor basic |
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Net Ionic equatins |
for neutralization of strong acid and strong base in water |
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strong acids and bases |
completely dissociate in water |
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Oxidation |
a chemical process causing electron loss; the atom or molecule losing one or more electrons is oxidized |
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Reduction |
a chemical process causing electron gain; the atom or molecule gaining one or more electrons is reduced; its charge is reduced |
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Oxidizing agent |
the atom or molecule taking up electrons: the species being reduced. |
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reducing agent |
the atom or molecule giving up electrons the species being oxidized |
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Free elements |
have and oxidatin number of zero Na,Be, K, Pb, H2, o2, P4=0 |
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double arrows |
the reacation doesnt go into one area. |
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Monatomic Ions |
the oxidatin number is equal to the chrage on the ion |
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Oxidation Number of oxygen |
-2. In H2O2 and O2 2- it is -1 |
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oxidation number of hydrogen |
+1 except when it is bonded to metals in binary compounds. In these cases it oxidation number is -1 |
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conjugate base |
within the Brønsted–Lowry acid–base theory, is a species formed by the reception of a proton (H+) by a base—in other words, it is a base with a hydrogen ion added to it. On the other hand, a conjugate base is merely what is left after an acid has donated a proton in a chemical reaction. |
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Group IA metals are IIA etals are Flurine is always |
+1, +2. -1 |
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Hydrogen displacement |
Reactions in which hydrogen ion is reduced to hydrogen gas |
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Molarity or molar concentration, |
is the number of moles of solute per liter of solution Molarity(M)+ Moles of solute/ liter of solution |
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Dilution |
process in which solvent is added to a solution to decrease the concentration of the solution. The number of moles of solute is the same before and after dilution. SInce the number of moles of solute equals the product of molarity and volume (MxV), we can write the following equation where the subscripts denote Intial and final values Mi x Vi= Mf x Vf |
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Molality |
+ moles of solute/ kg of solution |
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Covalently bonded Material |
Dissolves in water the molecules remain intact, they do not conduct current. These compounds are nonelctrolytes |
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Chemical Equations for Aqueous Reactions |
When and Ionic solid dissolves in water, it breaks into its constituents ions. This is called a dissociation reactions. These compounds conduct electric current and electrolytes. NaCL(2)---> |
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Flourides of the Alkaline Earths |
(Mg+, Ca+,..Ba+..) are insoluble |
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Metals |
_____ are cations there for they have a postive charge. |
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Groups |
When elements are in the same group as each other they will have the same reaction. |
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Zn---> ZN++ + 2e- oxidations |
Cu++ +2e- ----> Cu 0 Reduction |
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Oxidation |
a chemical process causing electron loss; theatom or molecule losing one or more electrons is oxidized. |
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reductions |
a chemical process causing electron gain; theatom or molecule gaining one or more electrons is reduced;its charge is reduced. |
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Oxidizing agent: |
the atom or molecule taking up electrons;the species being reduced. |
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Reducing agent: |
the atom or molecule giving up electrons;the species being oxidized. |
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Free elements (uncombined state) have an oxidation number of zero(Oxidation Number) |
Na, Be, K, Pb, H2, O2, P4 = 0 |
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In monatomic ions, the oxidation number is equal to the charge on theion. |
Li+, Li = +1; Fe3+, Fe = +3; O2-, O = -2 |
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The oxidation number of oxygen is usually In H2O2 and O22-it is |
-2, -1 |
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The oxidation number of hydrogen is__except when it isbonded to metals in binary compounds. In these cases, itsoxidation number is__ |
+1, -1 |
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Group IA metals are__ IIA metals are__and fluorine is always |
+1, +2,-1 |
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Oxidation Number |
The sum of the oxidation numbers of all the atoms in a moleculeor ion is equal to the charge on the molecule or ion. |
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What are the oxidationnumbers of all the elementsin HCO3- ? |
HCO3-O = -2 H = +13x(-2) + 1 +-5 = -1C = +4 |
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halogen oxidation |
when a halogen is with oxygen in an oxidiation state besuppicious it may not be and -1 |
