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Chapters 4-6
Solubility Rules, Metathesis Reactions, Acids and Salts, Strong Acids
75
Chemistry
Undergraduate 2
10/18/2009

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Term

HClO4

Strong or weak acid?

Definition
Strong Acid
Term

HCl

Strong or weak acid?

Definition
Strong Acid
Term

HBr

strong or weak acid

Definition
strong
Term

HI

strong or weak acid

Definition
strong acid
Term

HNO3

strong or weak acid

Definition
strong acid
Term

HCN

strong or weak acid

Definition
weak acid
Term

H2SO3

strong or weak acid

Definition
weak acid
Term

HNO2

strong or weak acid

Definition
weak acid
Term

HCHO2

strong or weak acid

Definition
weak acid
Term

H2SO4

(Name)

Definition
Sulfuric Acid
Term

H2SO3

(Name)

Definition
sulfurous acid
Term

HNO3

(name)

Definition
Nitric acid
Term

HNO2

(name)

Definition
nitrous acid
Term

HClO4

(name)

Definition
perchloric acid
Term

HClO3

(name)

Definition
chloric acid
Term

HClO2

(name)

Definition
chlorous acid
Term

HClO

(name)

Definition
hypochlorous acid
Term
anion formed from acids with -ous suffix
Definition
-ite
Term
anion formed from acids with -ic suffix
Definition
-ate
Term
Four conditions which dictate whether a metathesis (double replacement) reaction will occur.
Definition

1. Precipitate forms from soluble reactants

2. Acid-base neutralization occurs (not when salts used)

3. Gas is formed

4. Weak electrolte forms from soluble strong electrolytes

Term
Soluble Compounds
Definition

1. All compounds of alkali metals

2. All salts with NH4+, NO3-, ClO4-, ClO3- and C2H3O2-

3. All salts containing Cl-, Br- or I- except when combined with Ag+, Pb2+ and Hg22+

4. All SO42-, except with Pb2+, Ca2+, Sr2+, Hg22+ and Ba2+ 

Term
Insoluble Compounds
Definition

1. Metal hydroxides (OH-) and metal oxides (O2-) except Group IA and Ca2+, Ba2+, Sr2+, Ra2+

 

2. All salts with PO43- CO32-, SO32-, and S2-, except those of Group IA and NH4+

Term
Compounds of the alkali metals...soluble/insoluble?
Definition
soluble
Term
Salts containing NH4+...soluble/insoluble?
Definition
Soluble
Term
Salts containing NO3-...soluble/insoluble?
Definition
soluble
Term
Salts containing ClO4-...soluble/insoluble?
Definition
soluble
Term
Salts containing ClO3-...soluble/insoluble?
Definition
soluble
Term
Salts containing C2H3O2...soluble/insoluble?
Definition
soluble
Term
Chlorides...soluble/insoluble?
Definition
soluble except with Ag+, Pb2+ and Hg22+
Term
Bromides...soluble/insoluble?
Definition
Soluble except with Ag+, Pb2+ and Hg22+
Term
Iodides...soluble/insoluble?
Definition
Soluble, except with Ag+, Pb2+ and Hg22+
Term
Oxides...soluble/insoluble?
Definition
Insoluble, except with Group IA and with Ca2+, Sr2+, Ra2+ and Ba2+
Term
Hydroxides...soluble/insoluble?
Definition
Insoluble, except with Group IA and with Ca2+, Sr2+, Ra2+ and Ba2+
Term
Sulfates...soluble/insoluble?
Definition
Soluble, except with Pb2+, Hg22+,Ca2+, Sr2+ and Ba2+
Term
Gas is formed by acid reactions with which compounds...
Definition

Sulfides                      S

Sulfites                      SO3  

cyanides                     CN

carbonates                  CO3

bicarbonates               HCO3

bisulfites                    HSO3

Term
Gas is formed by base reactions with...
Definition
Ammonium salts  NH4
Term
Four circumstances that qualify a reaction as redox...
Definition

1. Loss or gain of electrons

2. Loss or gain of oxygen

3. Loss or gain of hydrogen

4. Change in oxidation number

Term
decomposition reaction
Definition
When one reactant breaks down to give 2 or more products.
Term
Combination/synthesis
Definition
When 2 or more reactants combine to give 1 product.
Term
Elements that exist as diatomic molecules
Definition

H2   NO2

 

   F2   Cl2   Br2  I2    

Term
Oxidation number of free element
Definition
Zero
Term
Oxidation number of F in compounds
Definition
-1
Term
Oxidation number of Hydrogen in compounds
Definition
+1
Term
Oxidation number of Oxygen in compounds
Definition
-2
Term
Oxidation number of any simple, monoatomic ion
Definition
Equal to the charge on the ion
Term
Oxidation numbers of molecules or polyatomic ions
Definition
Sum of all oxidation numbers must be equal to the charge on the particle
Term
Oxidation number of group IA (alkali metals)
Definition
+1
Term
Oxidation number of group II A (Alkaline Earth Metals)
Definition
+2
Term
Examples of oxidizing agents
Definition

Oxygen

Oxyacids

Nonmetals

Oxygen-containing compounds (hydrogen peroxide and bleach)

Term
Examples of reducing agents
Definition

hydrogen

metals

Term
[image]
Definition
Exothermic
Term
[image]
Definition
Endothermic
Term
Energy transferred between objects caused by differences in their temperatures until they reach thermal equilibrium.
Definition
Heat
Term
Ability to do work or transfer heat
Definition
Energy
Term
Kinetic energy
Definition
energy of motion
Term
potential energy
Definition

energy of position

energy stored in matter

Term
formula for finding kinetic energy
Definition
KE = 1/2 mv2
Term
Two ways potential energy increases
Definition

1. Objects that attract move apart

2. Objects that repel move closer together

Term
Things with high potential energy are _________(stable/unstable).
Definition
Unstable
Term
S.I. Unit of Energy
Definition
Joules
Term
formula for finding joules
Definition

J = kg * m2

   s2

Term
British unit of energy
Definition
calorie
Term
1 calorie =
Definition
4.184 J
Term
1 kcal =
Definition
4.184 kJ
Term
Δ E for reactions that don't involve gases.
Definition
Δ E = q
Term
Substances with ____(high/low) specific heats resist temperature changes.
Definition
high
Term
Heat capacity
Definition
The ability of an object with constant mass to absorb heat.
Term
Heat capacity is an ___________(extensive, intensive) property.
Definition
Extensive Property
Term
Specific heat is an ___________(extensive, intensive) property.
Definition
intensive
Term
Specific heat
Definition
Ability of a substance to store heat.
Term
Heat evolved/transferred
Definition

q = msΔt

 

q = CΔt

Term
Formula for Heat capacity
Definition
C = ms
Term
Formula used in calorimetry problems.
Definition
q = msΔt
Term
Hess's Law
Definition
The overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for individual steps in the reaction.
Term
Formula for finding ΔH for reactions
Definition
Δ H = sum(mol x ΔHf products)-sum(mol x ΔHf reactants)
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