Chapters 4-6 Test Questions – Flashcards
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Unlock answersHClO4 Strong or weak acid? |
| Strong Acid |
HCl Strong or weak acid? |
| Strong Acid |
HBr strong or weak acid |
| strong |
HI strong or weak acid |
| strong acid |
HNO3 strong or weak acid |
| strong acid |
HCN strong or weak acid |
| weak acid |
H2SO3 strong or weak acid |
| weak acid |
HNO2 strong or weak acid |
| weak acid |
HCHO2 strong or weak acid |
| weak acid |
H2SO4 (Name) |
| Sulfuric Acid |
H2SO3 (Name) |
| sulfurous acid |
HNO3 (name) |
| Nitric acid |
HNO2 (name) |
| nitrous acid |
HClO4 (name) |
| perchloric acid |
HClO3 (name) |
| chloric acid |
HClO2 (name) |
| chlorous acid |
HClO (name) |
| hypochlorous acid |
| anion formed from acids with -ous suffix |
| -ite |
| anion formed from acids with -ic suffix |
| -ate |
| Four conditions which dictate whether a metathesis (double replacement) reaction will occur. |
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 |
| Soluble Compounds |
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+ |
| Insoluble Compounds |
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+ |
| Compounds of the alkali metals...soluble/insoluble? |
| soluble |
| Salts containing NH4+...soluble/insoluble? |
| Soluble |
| Salts containing NO3-...soluble/insoluble? |
| soluble |
| Salts containing ClO4-...soluble/insoluble? |
| soluble |
| Salts containing ClO3-...soluble/insoluble? |
| soluble |
| Salts containing C2H3O2...soluble/insoluble? |
| soluble |
| Chlorides...soluble/insoluble? |
| soluble except with Ag+, Pb2+ and Hg22+ |
| Bromides...soluble/insoluble? |
| Soluble except with Ag+, Pb2+ and Hg22+ |
| Iodides...soluble/insoluble? |
| Soluble, except with Ag+, Pb2+ and Hg22+ |
| Oxides...soluble/insoluble? |
| Insoluble, except with Group IA and with Ca2+, Sr2+, Ra2+ and Ba2+ |
| Hydroxides...soluble/insoluble? |
| Insoluble, except with Group IA and with Ca2+, Sr2+, Ra2+ and Ba2+ |
| Sulfates...soluble/insoluble? |
| Soluble, except with Pb2+, Hg22+,Ca2+, Sr2+ and Ba2+ |
| Gas is formed by acid reactions with which compounds... |
Sulfides S Sulfites SO3 cyanides CN carbonates CO3 bicarbonates HCO3 bisulfites HSO3 |
| Gas is formed by base reactions with... |
| Ammonium salts NH4 |
| Four circumstances that qualify a reaction as redox... |
1. Loss or gain of electrons 2. Loss or gain of oxygen 3. Loss or gain of hydrogen 4. Change in oxidation number |
| decomposition reaction |
| When one reactant breaks down to give 2 or more products. |
| Combination/synthesis |
| When 2 or more reactants combine to give 1 product. |
| Elements that exist as diatomic molecules |
H2 N2 O2
F2 Cl2 Br2 I2 |
| Oxidation number of free element |
| Zero |
| Oxidation number of F in compounds |
| -1 |
| Oxidation number of Hydrogen in compounds |
| +1 |
| Oxidation number of Oxygen in compounds |
| -2 |
| Oxidation number of any simple, monoatomic ion |
| Equal to the charge on the ion |
| Oxidation numbers of molecules or polyatomic ions |
| Sum of all oxidation numbers must be equal to the charge on the particle |
| Oxidation number of group IA (alkali metals) |
| +1 |
| Oxidation number of group II A (Alkaline Earth Metals) |
| +2 |
| Examples of oxidizing agents |
Oxygen Oxyacids Nonmetals Oxygen-containing compounds (hydrogen peroxide and bleach) |
| Examples of reducing agents |
hydrogen metals |
| [image] |
| Exothermic |
| [image] |
| Endothermic |
| Energy transferred between objects caused by differences in their temperatures until they reach thermal equilibrium. |
| Heat |
| Ability to do work or transfer heat |
| Energy |
| Kinetic energy |
| energy of motion |
| potential energy |
energy of position energy stored in matter |
| formula for finding kinetic energy |
| KE = 1/2 mv2 |
| Two ways potential energy increases |
1. Objects that attract move apart 2. Objects that repel move closer together |
| Things with high potential energy are _________(stable/unstable). |
| Unstable |
| S.I. Unit of Energy |
| Joules |
| formula for finding joules |
J = kg * m2 s2 |
| British unit of energy |
| calorie |
| 1 calorie = |
| 4.184 J |
| 1 kcal = |
| 4.184 kJ |
| Δ E for reactions that don't involve gases. |
| ; E;= q |
| Substances with ____(high/low) specific heats resist temperature changes. |
| high |
| Heat capacity |
| The ability of an object with constant mass to absorb heat. |
| Heat capacity is an ___________(extensive, intensive) property. |
| Extensive Property |
| Specific heat;is an ___________(extensive, intensive) property. |
| intensive |
| Specific heat |
| Ability of a substance to store heat. |
| Heat evolved/transferred |
q = ms;t ; q = C;t |
| Formula for Heat capacity |
| C = ms |
| Formula used in calorimetry problems. |
| q = ms;t |
| Hess's Law |
| The overall enthalpy change for a reaction is equal to the sum of the enthalpy changes for individual steps in the reaction. |
| Formula for finding ΔH for reactions |
| Δ H = sum(mol x ΔHf products)-sum(mol x ΔHf reactants) |
