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chem 2 final
both semester quizzes
| Question | Answer |
|---|---|
| Which of the following ideas helped John Dalton formulate his atomic theory? | the law of constant composition |
| Choose the response that includes all the items listed below that not pure substances, i.e. that are mixtures. i. orange juice ii. steam iii. wine iv. oxygen v. vegetable soup | i, iii, v |
| At "room temperature" most elements exist as | solids |
| The most common element in the Earth's crust, oceans and atmosphere is | oxygen |
| Which of the following is not a postulate of Dalton's atomic theory? | The nucleus contains most of the mass of an atom |
| All metals exist as solids at room temperature. | False |
| The law of multiple proportions says that mixtures can have varying compositions. | true |
| Distillation can be used to separate the elements of a chemical compound. | false |
| Filtration can not be used to separate the solute from the solvent of a solution. | true |
| Only a few elements can be found in nature in pure form (that is as the pure element). | true |
| The correct IUPAC name for CaI2is | calcium iodide |
| The correct IUPAC name for P2O5 is | diphosphorous pentoxide |
| The molecular mass of PbI2 calculated to 3 significant figures is | 461 |
| What is the mass percent of hydrogen in water H2O (use the atomic masses from the text, and 2 significant figures) | 11% |
| The 2 most abundant naturally occuring isotopes of potassium are potassium-39 and potassium-41, the difference between neutral atoms of these isotopes is: | K-41 has two more neutrons than K-39. |
| The listed atomic mass for potassium is 39.0983. If the 3 naturally occuring isotopes are K-39, K-40 and K-41, which is the most abundant isotope? | k-39 |
| Barium has an atomic number of 56, this means that: | Every atom of barium has 56 protons. |
| Every carbon-14 atom has: | 8 neutrons |
| Astintine(At) is a radioactive halogen that concentrates in the thyroid gland. From its position in the periodic table predict the formula of its sodium salt. i.) NaAt ii.) Na2At iii.) NaAt2 | i |
| Astintine(At) is a radioactive halogen that concentrates in the thyroid gland. From its position in the periodic table, predict its physical state at 25C. | solid |
| Astintine(At) is a radioactive halogen that concentrates in the thyroid gland. Predict from its position in the periodic table the color of its sodium salt. | white |
| One of the groups of the periodic table is commonly referred to as the "coinage metals" (not an IUPAC approved name) as they have been traditionally used to make coins. Which group is this? | 11 |
| Magnesium burns in a pure carbon dioxide atmosphere to form magnesium oxide (MgO) and elemental carbon. When balanced, the coefficients for the reactants and products from left to right are: ___Mg(s) + ___CO2® ___MgO(s) + ___C(s) | 2,1,2,1 |
| One of the as yet undiscovered elements that Mendeleev predicted based on his idea of periodicity is | gallium |
| The coefficients that we use to balance chemical equations lend themselves to many interpretations. One interpretation does not work is | grams |
| Group 17, the halogens are named from the Greek word meaning | salt formers |
| As we move down each group, elements become "more metalic". | true |
| Listing elements in order of atomic number gives exactly the same order as listing by atomic mass. | false |
| Which of the following has the smallest first ionization energy? | Be |
| The visible lines in the hydrogen emission spectrum all arise from transitions that end at the n=2 energy level. From which level does the transition that gives rise to the red line originate? | none of the above |
| The scientist who was first to propose that matter, like electrons, has wavelike properties is | De Broglie |
| Valence electrons are | all of the above |
| Compared to ultraviolet light, xrays have | shorter wavelength |
| The electromagnetic radiation that gives rise to photons with the greater energy is | visible light |
| Standard household electricity is either 50 or 60 cycles per second. Is this a wavelength or a frequency? | frequency |
| new element, the element is a "main group" element; the 1st 5 ionization energies r given below, 2 what group (group numbers periodic table in the txt) does ths element? I1 I2 I3 I4 I5 3.6 7.8 15.4 20.6 135 | 14 |
| The colors seen in flame tests for alkali metals arise from | "relaxation" i.e. transitions of excited atoms. |
| The Bohr theory of the hydrogen atom was somewhat successful; however, one problem with it is | it could not be extended to atoms with more than one electron. |
| Complete this sentence: Atoms emit visible and ultraviolet light | as electrons jump from higher energy levels to lower levels. |
| What is the maximum number of electrons in one atom that can have the following set of four quantum numbers? n = 4 l = 3 ml = -2 ms = +1/2 | only 1 |
| Which of the following is a possible set of quantum numbers (n, l, ml, ms) for the last electron added to an atom of gallium (Ga) in its ground state? | 4, 1, -1, +1/2 |
| "No two electrons in an atom can have the same four quantum numbers" is a statement of | the Pauli exclusion principle. |
| Applying Pauli's exclusion princible and Hund's rule, how many unpaired electrons would a ground-state atom of sulfur have? | 2 |
| Which element has the following ground-state electron configuration? [Kr]5s24d105p3 | Sb |
| How many electrons are there in the 2nd principal energy level (n = 2) of a phosphorus atom (be careful here)? | 8 |
| How many electrons are there in the 3rd principal energy level (n = 3) of a phosphorus atom? | 5 |
| Which of these choices is a possible electron configuration for an excited state of an oxygen atom? | 1s22s22p33s1 |
| Which atom has the greater atomic radius, sodium or sulfur? | sodium |
| Mg+2, Na+1, Ne, F-1, O-2, N-3 are ions (except neon which is an atom) with 10 electrons. Which is the biggest? | N-3 |
| The Lewis dot formula for sulfur tetrafluoride, SF4, has one lone pair of electrons on the central sulfur atom; the shape of the SF4 molecule is | seesaw (distorted tetrahedron). |
| Which of the following molecular geometries is not possible for molecules with a tetrahedral electron geometry (i.e. a molecule that has 4 pair of valence electrons around the central atom). | trigonal planer |
| Complete this sentence: The PCl5 molecule has | polar bonds, but is a nonpolar molecule. |
| Which of the following molecules have the same geometries? i. SF4 and CH4 ii. CO2 and H2O iii. CO2 and SiO2 iv. N2O and NO2 | iii |
| Nitrous oxide, N2O, is sometimes called "laughing gas". What is the molecular geometry for nitrous oxide? (The atom connectivity is N-N-O.) | linear |
| Structural isomers are pairs of molecules that: | have the same chemical formula with a different arrangement of the atoms |
| There are two possible geometric isomers for SF4Cl2. What is true of this pair of isomers? | one is polar, the other is not. |
| The central atom of the formaldehyde molecule (CH2O) is the carbon atom. What is the geometry of this molecule? | trigonal planer |
| The bond angle in the water molecule is somewhat less than 109.5 degrees because | the two lone pair of electrons on the oxygen take up more space and "push" the hydrogen atoms closer together than they would be in a tetrahedral molecule. |
| Only linear and tetrahedral molecules can contain polar covalent bonds arranged such that the molecule is non-polar. | false |
| Indicate the type of hybrid orbitals used for bonding by the nitrogen atom in NI3. i. sp ii. sp2 iii. sp3 iv. sp3d. | iii |
| If a triatomic molecule, such as CO2, is linear, then the hybridization of the central atom will A. sp. B. sp2. C. sp3. | A |
| The number of pi bonds in an ethylene, C2H4 molecule is | 1 |
| Consider the species N2+, N2, and N2-. According to molecular orbital theory, which of these species will be paramagnetic? | both ions, not the neutral molecule. |
| Which of the following is not true of molecular orbitals? | Which of the following is not true of molecular orbitals? |
| The electrons in the delocalized pi orbitals predicted by hybrid orbital theory of benzene (C6H6) | are free to move within rings above and below the six-membered carbon ring. |
| The number of sigma bonds in a molecule acetylene, C2H2 is (count C-C and C-H sigma bonds). | 3 |
| One mole of iron | None of the above |
| Calculate the number of moles of xenon in 13.1 g of xenon. | 0.100 mol |
| How many moles of oxygen atoms are there in 10 moles of KClO3? | 30 mol |
| Vanadium(V) oxide reacts with calcium according to the chemical equation below. When 10.0 moles of V2O5 are mixed with 10.0 moles of Ca, which is the limiting reagent? V2O5(s) + 5Ca(l) ® 2V(l) + 5CaO(s) | Ca |
| Hydrochloric acid can be prepared by the following reaction: 2NaCl(s) + H2SO4(aq)®2HCl(g) + Na2SO4(s) How many grams of HCl can be prepared from 150 g NaCl and excess H2SO4? | 93.5 g |
| What is the theoretical yield of aluminum that can be produced by the reaction of 60.0 g of aluminum oxide with 30.0 g of carbon according to the following chemical equation? Al2O3+ 3C ® 2Al + 3CO | 31.8 grams |
| A 0.8715 g sample of sorbic acid, a compound first obtained from the berries of a certain ash tree, is burned completely in oxygen to give 2.053 g of carbon dioxide and 0.5601 g of water. The empirical formula of sorbic acid is | C3H4O |
| Tells us how fast a reactant is consumed or how fast a product is formed. | Reaction rate |
| Describes the dependence of the rate of reaction on the concentrations of the various species involved. | Rate law |
| Relates the “initial” and “final” amounts of a reactant with a time interval. | integrated rate law |
| The time required for one-half of the amount of a reactant to react. | half life |
| What is the best estimate for the initial rate of reaction from the plot given? | 2X10-4M/s |
| For this same graph of kinetics data, what is the instantaneous rate at point B (600s, 0.03M)? | 6X10-5M/s |
| From this concentration vs. time graph, the reaction order can be determined (one need only compare values for points A and B). What is the reaction order for this reaction? | first order |
| The half-life for the radioactive decay of sodium-25 is 10 minutes. Radioactive decay is a first order process. What is the value for the rate constant, k, for the decay of sodium-25? | 0.0693min-1 |
| For the overall chemical reaction shown below, which one of the following statements can be rightly assumed? 2H2S(g) + O2(g) → 2S(s) + 2H2O(l) | The rate law cannot be determined from the information given. |
| A first-order reaction has a rate constant of 3.00 × 10-3 s-1. The time required for the reaction to be 75.0% complete is | 462 s |
| At 25 ° C the rate constant for the first-order decomposition of a pesticide solution is 6.40 × 10-3 min-1. If the starting concentration of pesticide is 0.0314 M, what concentration will remain after 62.0 min at 25 ° C? | 2.11 × 10-2 M |
| What is the expected pH of a 0.01M HNO3 solution? | pH = 2 |
| Calculate the pH of a 0.010M CsOH solution. | Calculate the pH of a 0.010M CsOH solution. |
| The pH of a 0.05M propanoic acid solution was measured to be 3.09. Calculated a value for Ka from this data. | 1.32×10-5 |
| The pKa for chlorous acid (HClO2) is 1.96. The value of Ka is: | 0.011 |
| Aspirin is an acid with a Ka=3.31×10-4. What is the expected pH of a 0.020M solution of aspirin (0.02M is the approximate concentration of 1 standard tablet in 100mL of water)? | 2.62 |
| When acid is added to pure water bringing the pH to exactly 5.0, the concentration of hydronium ions has been increased by a factor of..... | 100 |
| An increase in the hydronium ion concentration by a factor of 1000 is accompanied by what change in hydroxide ion concentration? | A 1000 fold decrease. |
| Consider the reaction of carbon dioxide with water shown below. Which change would cause an increase in the pH of the solution? CO2(aq) + H2O(l) = H3O+(aq) + HCO3- (aq) | removal of some of the carbon dioxide from solution. |
| The conjugate base of nitric acid is: | The nitrate ion, NO3- which is not acidic or basic. |
| The carboxylic acid, propanoic acid has a Ka=1.4×10-5. What is the value for Kb of the propanoate ion? | 7.14×10-10 |
| Phosphoric acid, H3PO4 is an acid with three ionizable protons the Ka values are listed on the bottom of table 20.9 of the text. From this data, which of the following solutions will have the highest pH, that is be the most basic? | 0.1M Na3PO4 |
| For the formation of water from hydrogen and oxygen gas, the hydrogen gas is....(it is more than one thing) | the reducing agent oxidized |
| The unbalanced half reaction: Mo3+(aq) → MoO22+(aq) is a(n) ___________ half reaction. Be careful here. | Oxidation |
| To balanced this half reaction: Mo3+(aq) → MoO22+(aq) requires _______ electrons. | 1 |
| When correctly balanced with a coefficient of 2 for the MnO(s), how many hydrogen ions (H+) are needed? ___H + (aq) + ___MnO(s) + ___PbO 2 (s) → ___MnO 4 - (aq) + ___Pb 2+ (aq) + ___H 2 O(l) | 4 |
| Consider an electrochemical cell constructed from the following half cells, linked by an external circuit and by a KCl salt bridge. an Al(s) electrode in 1.0 M Al(NO3)3solution a Pb(s) electrode in 1.0 M Pb(NO3)2solution Which electrode is the anode? | 2.46 V |
| Which statement is true for a spontaneous redox reaction carried out at standard-state conditions? | E°cell is always positive |
| Which one of the following reagents is capable of transforming Cu2+(1 M) to Cu(s)? | Ni(s) |
| HCl(aq) + H2O(l) → H3O+ + Cl- | false |
| 2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g) | true |
| Cu(s) + 4HNO3(aq) → Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l) | true |
| Pb2+(aq) + 2I-(aq) → PbI2(s) | false |
| NH3 | -3 |
| H4N2 | -2 |
| HNO3 | +5 |
| NH4+ | -3 |
| NaNO2 | +3 |
| N2 | 0 |
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