Help
Options
Didn't know it?
click below
click below
Knew it?
click below
click below
Don't Know
Remaining cards (0)
Know
retry
shuffle
restart
0:00
Embed Code - If you would like this activity on your web page, copy the script below and paste it into your web page.
Normal Size Small Size show me how
Normal Size Small Size show me how
Gen Chem Errors
| Question | Answer |
|---|---|
| What is the pH of a 0.001 M solution of sulfuric acid? (pKa = -2.8), assuming complete dissociation? | Typically, the concentration of hydrogen ions [H+] is the same as the concentration of the acid [HA] in a solution. From the question we already know that [HA] = 0.001; therefore, we have to multiply the [HA] by 2 to determine [H+]. pH = -log(0.002) = 3 |
| Which of the following bonds is the most polar? C-H, O-F, C-C, C-N, O-H | O-H |
| Radioactive decay is the spontaneous breakdown of an atomic nucleus resulting in the release of energy and matter from the nucleus. What order kinetics does radioactive decay follow? | First-order kinetics |
| The distance separating two adjacent carbon nuclei is 1.54 Å and the bond length in F2 is 1.32 Å. Based on this data, which of the following is the length of the C-F bond in CF4? | Number of bond lengths: 2 Sum of the given bond lengths = 1.54 Å + 1.32 Å = 2.86 Å Resulting bond length = sum of given bond length/number of bond lengths -> 2.86/2 = 1.43 A |
| Electron Affinity and its trend | the amount of energy released or spent when an electron is added to a neutral atom or molecule in the gaseous state to form a negative ion. Electron affinity increases UPWARD for the groups and from LEFT to RIGHT across periods of the periodic table. |
| Which of the following elements has the lowest electron affinity? Li, B, O, F, Ne? | Ne, noble gases have an electron affinity of zero |
| Which of the following is true for a reaction that has a small negative ΔG value? | Products will be favored at equilibrium |
| At which point during a titration experiment does pH = pKa ? | Half-equivalence point |
| What is the ionic reaction for the neutralization of HCl with NaOH? | H+(aq) + Cl-(aq) + Na+(aq) + OH-(aq) ↔ H2O(l) + Na+(aq) + Cl-(aq) |
| How many equivalent resonance structures can be drawn for the nitrate ion, NO3-? | 3 |
| Which reaction has an equilibrium point affected by changes in pressure? | equilibrium is affected if moles of gas in the reactants is different than the products. An inc in pressure will cause the equilibrium to shift to the side that has fewer moles of gas, and a decrease in pressure shift to the side that has greater. |
| When go gases behave ideally? | They perform at high temperatures, low pressure |
| Each of the following are properties of transitional metals EXCEPT one. Which one is the EXCEPTION? | The classic characteristic property that most transition metals do not possess is having low melting and boiling points. Transition metals are widely known for having exceptionally high melting points and being dense, hard, and strong. |
| Each of the following are single-replacement reactions that occur EXCEPT one. Which one is the EXCEPTION? | CaF2(s)+ Br2(ℓ) → CaBr2(s) + F2(g). Halogens that are higher up on the periodic table are more reactive. Based on this reactivity order, fluorine is more reactive than bromine, so the following reaction will not occur. |
| Which type of glassware sits below the burette in an acid-base titration? | Erlenmeyer flask |
| What is the pH of a 0.001 M solution of a monoprotic acid with a Ka value of 9 × 10^-7? | -log[3 × 10^-4]. To tackle this equation, we must first realize that the monoprotic acid given to us is NOT a strong acid (due to the low Ka value). Ka = (X)^2 / HA -> X = sqrt of (1*10^-3)(9*10^-7) |
| What are the colligative properties of liquid? | Colligative properties are properties that can only be applied to solutions and they depend on the amount or concentration of the solute in a solution. (Boiling point, Freezing point, Osmotic pressure, and Vapor pressure) |
| Which of the following best describes nuclear binding energy? | The energy required to disassemble the nucleus of an atom into its components |
| If you halve the pressure of a gas at constant temperature, what happens to the volume? | Volume will double. Use P1V1/n1T1 = P2V2/n2T2 |
| What is the value of E° for the following reaction? | Identify what's being reduced and what's being oxidized, if there's an oxidation, the sign should be neg and reduction should have a pos. Then add. |
| Under what conditions can a supercritical fluid be changed back into a liquid or gas? | Decrease temperature only (temp is the x axis and pressure is the y axis) |
| Given that self-ionization of water is an endothermic process, what is the value of pH + pOH at 350 K? | Higher than 25 C, both pH and pOH will decrease and give a sum that is less than 14 |
| What is the Ka of an acid HA, if a 0.001 M solution of HA has a pH of 4? | [H3O]+ = [A-] = 10^-4. [10^-4][10^-4] / [0.001] = 10^(-8+3) = Ka = 10^-5 |
| What is the pH of a 1.5 M solution of hypochlorous acid with a Ka of 3.5 x 10^-8? | You can set up an ICE table. Since HClO is a reactant and on the bottom, it would have 1.5-x while the others would just be x. Do 3.5 * 10^-8 = (x^2)/(1.5) -> x = sqrt ((1.5)(3.5 * 10^-8)) |
| Which of the following best explains why HF is a weaker acid than HCl, HBr, and HI? | Fluorine has the fewest number of electron shells. Since fluoride ions are smaller than other halide ions (fewer valence shells), they are less stable in solution, thus making their conjugate acids weak. |
| Which of the following best explains why H2SO4 is more acidic than H2SO3? | O4^2- has a greater resonance stabilization than SO3^2- |
| concentration of titrant = | moles of titrant / volume of titrant |
| During the titration of a weak acid using a strong base, the buffering zone ends when | the concentration of the weak acid is significantly less than its conjugate base. |
| A weak base, NH3, is being titrated with a strong acid, H+. Which point on the titration curve represents when the pH of the solution is the most dependent on NH4+? | approximately at the equivalence point of the titration curve. At this point, the predominant compound in the solution is NH4+ since the strong acid has neutralized all of NH3 to form it conjugate acid NH4+. |
| During the titration of a weak diprotic acid, the pH increases more rapidly after the second equivalence point than after the first equivalence point. Which of the following best explains this phenomenon? | The first equivalence point results in a weaker conjugate base than the second equivalence point |
| Which statement best describes heat transfer through convection? | Convection refers to heat transfer by the movement of a medium. Conduction also needs a medium, but radiation does not. |
| As temperature increases, the water dissociation constant | increases, because the autoionization equilibrium shifts to produce more H3O+ and OH-. |
| Which of the following describes a key characteristic that makes a compound amphoteric? | Presence of both acidic hydrogen and basic lone pairs |
| Which of the following changes to the dissociation of HNO2 will increase the pH of the solution? | Increasing the number of NO2- molecules |
| As temperature increases, the water dissociation constant | increases, because the autoionization equilibrium shifts to produce more H3O+ and OH-. |
| Each of the following compounds are amphoteric EXCEPT one. Which one is the EXCEPTION? | NH4+ can act as an acid by donating a proton to form NH3. However, it is unable to act as a base since it does not have a free electron lone pair to accept a proton. Therefore NH4+ is not an amphoteric compound. |
| If HBr is added to a solution containing NH3 at equilibrium depicted in the equation below, in which direction will the equilibrium of NH3 shift? NH3 + H2O ⇌ NH4+ + OH- | Shift right, due to a decrease in OH- ions |
| Given that humans maintain an internal body temperature of 37C, which of the following statements correctly characterizes the effect that body temperature has on the Ka and Kb of water, compared to room temperature? | Both Ka and Kb values of water is greater in the human body |
| If the pH of pure water at 40C is 6.75, what is the Kw of neutral water at this temperature? | pH + pOH = pKw In pure water, the concentration of hydronium molecules is equal to the concentration of hydroxide molecules. pH = pOH 6.75 + 6.75 = 13.5 Kw = 10^-13.5 |
| If the percent dissolution of NH3 (Kb = 1.8 × 10-5) is 10%, what was the initial concentration of NH3? | You would set up your ICE table with (0.1x)(0.1x)/0.9x = Kb |
| Tip about galvanic cells | Another word for them is voltaic |
| The following exothermic reaction is at equilibrium. Which of the following shifts the reaction towards the reactants? 2NO (g) -> N2(g) + O2(g) | Endothermic reaction – increases in temperature favors the products so that heat in the system is reduced. Exothermic reaction – increases in temperature favors the reactants so that heat in the system is reduced. |
| Pressure Changes | Compression of gases (increased pressure, decreased volume)— reaction favors the side containing fewer moles of gas Expansion of gases (decreased pressure, increased volume)— reaction favors the side containing more moles of gas |
| Aqueous NH3 was titrated with HBr until the endpoint. The resulting solution underwent testing using four pH indicators, and the table below provides information about the indicators and the colors observed during the test. | The color change one that produces a color not previously included would be the correct indicator of the pH |
| Which of the following best describe bond energy? | Energy required to break a bond |
| Given 5 moles of oxygen gas are present in a 5 L container at 25oC, what is the pressure of the oxygen gas? (R = 8.314 L•kPa•K-1•mol-1) | 2500 kPa. Use PV = nRT, make sure that you use the numbers AS CLOSE AS POSSIBLE |
| Each of the following are ionic compounds EXCEPT one. Which one is the EXCEPTION? NH4NO2 KH LiNO3 CH3NH2 NaOH | It is formed from the covalent bonding of the three hydrogen molecules to carbon and nitrogen, with carbon as the central atom. SO NO OPPOSITE CHARGES |
| Given methanol has a density of 0.792 g•cm-3 at 273 K, what volume of container is needed to hold 0.060 kg of methanol at 273 K? | 75 cm3, you could round 0.792 to 0.8 in calculations or multiply by 1.25, which would be the same thing |
| Which of the following represents the highest value of pressure? 100 kPa 1 atm 780 mmHg 25 torr 96,000 Pa | 1 atm = 101,325 Pascals = 760 mmHg = 760 torr So 780 mmHg is the largest |
| N2(g) + 3 H2(g) → 2 NH3(g) If the pressure at equilibrium was more than the initial pressure, what can be said about the reaction quotient and the direction of reaction as the reaction progressed toward equilibrium? | Qc > Kc ; backward reaction. The only way for pressure to increase is if the reaction went backwards (making more moles of gas). |
| How to solve titration graph problems | Quantity of acid or base delivered = (volume of titrant added) × (titrant concentration). Find how much volume (mL) was needed to reach the equivalent point via the graph and then multiply that by the M value. |
| How many moles of oxygen are in a 190 g solution of KNO3 at a temperature of 28C ? | 5.7. Find moles of KNO3, multiply by 3 for moles of oxygen. |
| In a fission reaction, uranium-235 is bombarded with a neutron and decays into two main radioactive fragments and 3 neutrons: 235U + 1n → 141Ba + X + 31n What is the element and the atomic mass of radioactive fragment X? | 92Kr, remember that the original X should always change! |
| Using an incorrectly calibrated pipette will result in | systematic error (always in one direction) |
| Random errors | skewed in a different way each time, a stopwatch used to time a runner or pendulum might be started slightly early or late on each trial. |
| Principal Number (n) | n, positive integers (1,2,3) represents orbital size and energy level |
| Azimuthal quantum number (ℓ) | Integers from 0 to n-1, represents orbital size (sublevels/subshells) |
| Magnetic quantum number (mℓ) | Integers -l to +l, represents orbital orientation |
| Spin quantum number (ms) | +1/2 or -1/2, represents electron spin direction |
| A Lewis acid is | an electron acceptor |
| A Lewis base is | an electron donor |
| Bronsted-Lowry acid | chemical species that donates a proton |
| Bronsted-Lowry base | chemical species that accepts a proton |
| Arrhenius Acid | a compound that increases the H+ ion concentration in aqueous solution |
| Arrhenius Base | accept H+ in aqueous solution |
| Which pair of equipment is used in acid-base titration? | Burette and Erlenmeyer flask |
| A 24.5 mL acid solution was added to 120 mL of water. What is the final volume of the mixed solution, rounded and expressed in the correct number of significant digits? | 140 |
| Which of the following factors is most likely to affect the general shape of the meniscus? | Intermolecular forces, Whether a liquid appears concave or convex depends on whether the liquid inside the container is more strongly attracted to the container or the other liquid molecules. |
| How does metallic character change across the periodic table? | Increases going right to left across a period, and increases going down a group. |
| How does Zeff change across the periodic table? | Increases left → right across a period (more protons, no new shells). Increases slightly going down a group (nuclear charge increase outweighs added shielding). |
| How to determine the amount of sheilding electrons? | They're the same amount as the protons of the last noble gas |
| Which of the following is the most prominent oxidation state for transition metals? | +2 |
| Which of the following is responsible for the observation that chlorine (Cl) has a smaller atomic radius than magnesium (Mg)? | Chlorine has more protons than magnesium. |
| Given the following standard reduction potentials below, what can be said about the reaction and standard cell potential for a galvanic cell consisting of Zinc and Copper? EoreductionCu = + 0.339 V EoreductionZn = - 0.762 V | Spontaneous and has an E value of +1.101, Among two or more elements, elements with lower potentials tend to be oxidized (reducing agent), while elements with higher potentials tend to be reduced (oxidizing agent). |
| Calcium metal reacts with water at standard temperature and pressure to form hydrogen gas and calcium hydroxide. Using this process, what mass of water is needed to generate 11.2 L of hydrogen gas? | 18 g (11.2 L H2) / (22.4 L/mol) = 0.500 mol H2 because the problem mentioned standard Then write the balanced equation (0.500 moles H2) × (2 mol H2O) / (1 mol H2) = 1.00 mol H2O 1.00 * 18 g/mol = 18 |
| Which of the following represents the electron configuration of the transition metal Mo? | 1s22s22p63s23p64s23d104p65s14d5 There are certain elements that have special exceptions, molybdenum being one of them since it is a transition metal. |
| Which molecules have electric configuration exceptions? | Cr, Cu, Mo, Ru, Rh, Pd, Ag, Pt, Au |
| First Law of Thermodynamics | Energy cannot be created or destroyed, only transferred |
| Second Law of Thermodynamics | The total entropy of an isolated system always increases over time. |
| Third Law of Thermodynamics | as the temperature of a system drops to absolute zero, its disorder (entropy) approaches zero. |
| Which of the following occurs during deposition? | ΔH < 0, ΔS < 0. Deposition is the change from a gaseous state to a solid, while sublimation is solid to gas. |
| 75 g of Mg(Cl)2 is dissolved in 150 g of water. What is the molality of this solution? | 5 mol•kg-1 moles of Mg(Cl)2 = (75g) / (95g/mol) = ~0.75 150g = 0.15kg m = (0.75) / (0.15) = ~5 moles/kg |
| The concentration of a stock solution is 1 g•mL-1. What volume of the stock solution is required to make a 0.5 L sample with a concentration of 400 mg•mL-1? | (400 mg/mL)(1 g/1000 mg) = 0.4 g/mL (0.5 L)(1000 mL/L) = 500 mL C1V1 = C2V2 X = 200 mL |
| Which of the following is expected to be insoluble in water? AgNO3 Mg(ClO4)2 NH4C2H3O2 CsOH HgCO3 | HgCO3 |
| Tip for soluble and insoluble | Soluble = NAG SAG (nitrates, acetate, group 1 ions, sulphates, ammonium, group 17 ions) Insoluble = PMS (lead, mercury, silver) |
| Which of the following compounds has the highest melting point? CH4 CH3Br CH2Br2 CHBr3 CBr4 | CBr4 the molecular weight can also play an important role in determining the melting point. When the molecular weight of a molecule increases, the number of electrons within the molecule also increases. |
| Which of the following is diamagnetic? K H- Li O2 Cu2+ | H-, all atoms or molecules with any paired electrons will exhibit diamagnetism. |
| Paramagnetism | results when an atom or molecule has any unpaired electrons. |
| What is the shape, bond angle, and lone pairs for Linear geometry? | 2 electron domains, 0 lone pairs, 180°. Example: CO₂. |
| What is the shape, bond angle, and lone pairs for Trigonal Planar geometry? | 3 electron domains, 0 lone pairs, 120°. Example: BF₃. |
| What is the shape, bond angle, and lone pairs for Bent/V-shaped (from 3 domains)? | 3 electron domains, 1 lone pair, <120°. Example: SO₂. |
| What is the shape, bond angle, and lone pairs for Tetrahedral geometry? | 4 electron domains, 0 lone pairs, 109.5°. Example: CH₄. |
| What is the shape, bond angle, and lone pairs for Trigonal Pyramidal geometry? | 4 electron domains, 1 lone pair, 107.5°. Example: NH₃. |
| What is the shape, bond angle, and lone pairs for Bent/V-shaped (from 4 domains)? | 4 electron domains, 2 lone pairs, 104.5°. Example: H₂O. |
| What is the shape, bond angle, and lone pairs for Trigonal Bipyramidal geometry? | 5 electron domains, 0 lone pairs, 90°/120°/180°. Example: PCl₅. |
| What is the shape, bond angle, and lone pairs for Seesaw geometry? | 5 electron domains, 1 lone pair, <90° and <120°. Example: SF₄. |
| What is the shape, bond angle, and lone pairs for T-Shaped geometry? | 5 electron domains, 2 lone pairs, <90°. Example: ClF₃. |
| What is the shape, bond angle, and lone pairs for Linear (from 5 domains)? | 5 electron domains, 3 lone pairs, 180°. Example: XeF₂. |
| What is the shape, bond angle, and lone pairs for Octahedral geometry? | 6 electron domains, 0 lone pairs, 90°. Example: SF₆. |
| What is the shape, bond angle, and lone pairs for Square Pyramidal geometry? | 6 electron domains, 1 lone pair, <90°. Example: ClF₅. |
| What is the shape, bond angle, and lone pairs for Square Planar geometry? | 6 electron domains, 2 lone pairs, 90°. Example: XeF₄. |
| What intramolecular forces are present in baking soda, NaHCO3? | Polar covalent and ionic bonds only |
| Seven strong acids | HCl, HBr, HI, HNO3, H2SO4, HClO3, HClO4 |
| Eight strong bases | LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2 |
| How to find the strongest acid between polyatomic acids? | When approached with polyatomic acids, only consider the first dissociation, because subsequent acid strength will always decrease. |
| Pos H, pos S | spontaneous at high temperature |
| Neg H, pos S | spontaneous at any temperature |
| Neg S, pos H | process is non-spontaneous at any temperature |
| Neg S, neg H | process is spontaneous at low temperature |
| What happens if the temperature is lowered for a liquid in a sealed container? | There are less gas molecules |
| Based on the following reduction potential data below, which of the following is most likely to occur? Ag+(aq) + e- → Ag(s) Eo = +0.80 V Cu2+(aq) + 2e- → Cu(s) Eo = +0.34 V | Remember that, in galvanic, the smaller Eo will be made negative (oxidized), so if Cu is being oxidized, it has to reduce the other thing. Cu(s) reduces Ag+(aq). |
| Reading a meniscus, concave up and down | Read the most bottom part when it's concave up and the most top part when it's concave down |
| Alpha Decay | A: decrease by 4 Z: decrease by 2 |
| Beta-Plus Decay (B+ Decay) | A: unchanged Z; decrease by 1 |
| Beta-Minus Decay (B- Decay) | A: unchanged Z: increase by 1 |
| Electron Capture | A: unchanged Z: decrease by 1 |
| Gamma Decay | A: unchanged Z: unchanged |
| In isoelectric series, which has the largest radius? | Anions > Regular > Cations |
| Which of the following is the correct list of elements in order of increasing electronegativity? He, O, F, Cl, N | He, N, Cl, O, F |
| What is the number of valence electrons in a Cu2+ion? | 9 |
| What is the correct number of unpaired electrons in cobalt? | 3 electrons. s has 2 e in 1 pair/orbital p has 6 e in 3 pairs/orbitals d has 10 e in 5 pairs/orbitals f has 14 e in 7 pairs/orbitals So Cobalt's 9 valence electrons fill 4s1 completely and 2 of 3d7, leaving 3 orbitals unfufilled. |
| Why is the slope of the line for the melting/freezing curve negatively sloped? | The liquid phase is denser than the solid phase |
| Which physical property is described when the vapor pressure of a liquid equals the atmospheric pressure? | Boiling point |
| Which of the following is a diatomic molecule that is solid at room temperature? F2 N2 Br2 He I2 | I2 |
| Compared to benzene, when naphthalene is placed under UV light using a prism block, the resulting mixture appears more opaque. Which physical property has changed to account for the difference in opacity between benzene and naphthalene? | Molar absorptivity |
| Consider a solution that consists of a weak acid [HA] and its conjugate base [A–]. If a small amount of strong base is added to the buffer, how will the pH change and why? | The pH will increase because the ratio of [A–]/[HA] is increased. Remember the Henderson Hasselbach equation is pH = pKa + log ([A–]/[HA]) |
| Which of the following must be true for a chemical reaction that has the same activation energy for the forward and reverse directions? | ΔG° = 0 |
| How many atoms of oxygen are in a 68 g sample of H2O2? (Avogadro’s number is 6.0 x 10^23) | 2.4 x 10^24. Don't forget to specifically multiply by the amount of moles of OXYGEN! |
| A cube with side lengths of 2 cm was filled with 5 moles of oxygen gas. Which of the following would be the resulting density? | 20 g•mL-1. Remember that for density, you'd need mass over volume, not moles! |
| All of the following are safe lab practices EXCEPT one. Which one is the EXCEPTION? Weighing calcium outside the fume hood Washing an Erlenmeyer flask in the sink Adding water to concentrated acid Pouring sodium bicarbonate on an acid spill | Adding water to concentrated acid |
| Which of the following describes why a proton and neutron weigh more separately than when they are bound together? | Mass is converted into nuclear binding energy |
| Why is fluorine-18 unstable? | Its N/Z ratio is too small. Atomic mass is 18, we get the number of neutrons in this isotope: 18-9 = 9 neutrons. We see that fluorine-18 has less neutrons than the stable fluorine-19 isotope so the F-18’s N/Z ratio must be less than F-19’s. |
| How many electrons can be held in each subshell? | s = 2 p = 6 d = 10 f = 14 |
| Which of the following is the correct number of non-bonding valence electrons in HCCl3? | 18 |
| Which of the following best describes the energy conversion process of a battery operating in a remote controller? | Chemical to electrical. A battery is an electrochemical (galvanic) cell with a positive terminal (cathode) and a negative terminal (anode) that supplies electric power (dependent on its voltage). |
| Electrolytic Cell | Convert electrical energy to chemical energy. Common examples include electroplating metals and the industrial production of elements. |
| The point above which a gas cannot be converted into a liquid is known as what? | Critical point |
| When one mole of each of the following solutes is dissolved, which molecule will result in the greatest increase in the boiling point of the solvent? | MgCl2, because i = 3. NOT NH4OH - i = 2. |
| What is acetone (CH3)2CO's i factor? | The van’t Hoff factor (i) is 1 because acetone dissolves as individual molecules but does not produce ions. |
| What is the final concentration of chloride ions when a 1 L solution of 0.100 M CaCl2 is mixed with 1 L of 0.100 M NaCl? | 0.150 M. |
| Which of the following molecules produces an acidic solution when placed in water? NaCl KBr NH4Cl LiF RbI | NH4Cl - NH4+ = Acidic (NH3) and Cl– = Neutral (HCl) → NH4Cl = Acidic |
| If both ions of salt are conjugate acid and conjugate base of a strong base and strong acid, respectively, then... | the salt will produce a neutral solution. |
| If cation of salt is conjugate acid of weak base, then... | it will produce an acidic solution. |
| If anion of salt is conjugate base of a weak acid, then... | it will produce a basic solution. |
| Which substance reacts with water most violently to produce H2 gas? Be C N O Li | Li. It is important to know that elements that are highly reducing (i.e., alkali metals and alkaline earth metals) are ones that are highly reactive in water. |
| Which of the following is a state function? Enthalpy Work Speed Power Heat | Enthalpy. A state function is defined as a unit that depends only on the change between initial and final states of a system. A path function is defined as a unit that depends only on the process by which the change occurs. |
| The rate of the reaction is second-order with respect to A and zero-order with respect to B. How will the rate constant change if the concentration of A was doubled and the concentration of B was tripled? | Check what it's asking you! We can see that the rate constant (k) remains constant no matter what happens to the concentration. So, no change. |
| How to find activation energy from graph | The activation energy is the difference between the activated complex (peak of graph) and the reactants. |
| Exothermic reaction vs endothermic reaction on a graph | Exothermic: reactants are higher, products are lower Endothermic: reactants are lower, products are higher |
| Charge of CN | -1 |
| Which of the following molecules possesses a non-zero dipole moment? BF3 Si(CH3)4 CO2 NH3 C6H6 | NH3, |
| Charge of Si | +4 |
| Which of the following is the correct the hybridization of a central carbon in propene, C3H6? | sp2 |
| Samples analyzed from a variety of sources possess the same ratio of elements chemically bonded together within each sample. Which of the following describes these samples? Colloid Compound Heterogenous mixture Pure element Homogenous mixture | Compound |
| According to the following reaction, if the initial concentration of SO2 and O2 are 0.10 M and 0.02 M respectively, what is the equilibrium concentration of SO3? (Kp = 5.0 × 10-4) 2 SO2(g) + O2(g)⇌ 2 SO3(g) | 2 * ((sqrt (5.0*10-4)(2.0*10^-4)) / 4) You would use the coefficients as exponents, but for the topmost portion - the x you're solving for - you'd also multiply that by 2 at the start and end. |
| If a weak base is added to a buffer solution, how do the concentrations of the weak acid and conjugate base change? | The concentration of conjugate base will increase |
| Which of the following statements regarding the solubility of NO2 gas in water is correct? | Solubility increases when pressure increases. Gases are more soluble at lower temperatures and high pressures. |
| Tip for electrolytic cells and electrochemical calculations: | In electrolytic cells (unlike galvanic), you want to set things up so you get a negative (nonspontaneous) E value. Furthermore, what reduces or oxidizes what is determined by which equation you reverse. |
| A gaseous mixture of O2, N2, and F2 has a total pressure of 2 atm. If the mole fractions of the gases are 0.3, 0.5, and 0.2, respectively, what is the partial pressure of the gaseous element that is present in the greatest mass? | 1.0 atm. Pretend that there's 10 mol total and multiply each by the mol fraction, then by their molar mass. Shows that nitrogen has the greatest mass, so then multiply 0.5 * 2 atm. |
| oxidizing agent | a molecule that is reduced itself – it gains electrons from another species. |
| reducing agent | a molecule that is oxidized itself – it loses electrons to another species. |
| Have No Fear Of Ice Cold Beer | H = Hydrogen N = Nitrogen F = Fluorine O = Oxygen I = Iodine Cl = Chlorine Br = Bromine |
| Qsp< Ksp | unsaturated solution (no precipitate forms) |
| Qsp= Ksp | saturated solution (no precipitate forms) |
| Qsp> Ksp | supersaturated solution (precipitate forms) |
| What is the formal charge of the central atom in BrO3-? | 0 |
| E value in Galvanic cell | Positive |
| E value in Electrolytic cell | Negative |
Created by:
smurtab