front 1 How do you know if something is an isotope? | back 1 they have the same atomic number but not necessarily the same atomic mass |
front 2 If the density of nitrogen in air is 0.870 g/L, what mass (in kg) of nitrogen is contained in a room with dimensions of 13.3 m × 4.58 m × 2.43 m? | back 2 129kg |
front 3 What is the correct answer to the following expression: (765.0 + 36.0) × 0.81150? | back 3 650 |
front 4 Express 0.00735 in scientific notation | back 4 7.35E-3 |
front 5 What is the percent mass of carbon, hydrogen and oxygen in acrolein, C3H4O? | back 5 C 64.26, H 7.2, O 28.54 |
front 6 Which element is most likely to form a 2+ ion? N Mg Na S Al | back 6 Mg |
front 7 What are the respective coefficients when the equation is balanced with the smallest whole numbers? __ Al + __ FeO → __ Fe + __Al2O3 | back 7 2 3 3 1 |
front 8 If 13.0 g N2 and 2.46 g H2 react to produce 1.30 g NH3, what is the percent yield of the reaction? N2(g) + 3 H2(g) → 2 NH3(g) | back 8 9.4 |
front 9 Select the ions present in Ca3(PO4)2 | back 9 Ca2+ PO4 3- |
front 10 Which of the following observations is/are examples of chemical change? 1. Sodium chloride melts at 801 0C. | back 10 only 3 |
front 11 Which of the following formulas correctly match the given names? 1. dinitrogen tetroxide, NO4 | back 11 3 |
front 12 Which of the following are covalent compounds? 1. CO2 | back 12 1 2 |
front 13 Which of the following compounds are named correctly? 1. Ca(NO3)2, calcium(II) nitrate | back 13 2 3 |
front 14 You have 5.67 g of each of the following elements: Na, Ca, Pb, Ti and Zn. Which sample contains the largest number of moles? | back 14 Na |
front 15 A compound containing nitrogen and oxygen is 69.55% by mass oxygen with a molecular weight of 92.02. What is the molecular formula for this compound? | back 15 N2O4 |
front 16 How many atoms of fluorine are present in 4.00 moles of NF3? | back 16 7.23E24 |
front 17 Which of the following statements concerning atomic structure is/are correct? 1- Neutrons and electrons are found in the nucleus. | back 17 3 |
front 18 How many protons, electrons and neutrons are present in 40Ca2+? | back 18 20 P 18 e 20 N |
front 19 Two students independently determine the volume of ethanol delivered
by a 50.00-mL pipet. Each student takes 10 measurements, then
calculates the average volume delivered and the standard deviation.
The results are tabulated below. | back 19 A: good precision, good accuracy. B: poor precision, poor accuracy |
front 20 Iron reacts with oxygen to produce iron(III) oxide. 4 Fe(s) + 3 O2(g) → 2 Fe2O3(s) If 6.96 moles of Fe react with excess O2, how many moles of Fe2O3 can be formed? | back 20 3.48 |
front 21 Which statements below are true about homogeneous mixtures? | back 21 2 |
front 22 Helium has 2 naturally occurring isotopes, He-4 (4.003 u) and He-3 (3.016 u). In an unusual sample of helium taken from a natural gas well the abundance of He-4 is 95.78%. What is the average atomic mass of this sample of helium? | back 22 3.961 |
front 23 For the following reaction 0.224 moles of nitrogen are allowed to
react 0.416 moles of hydrogen. What is the limiting reagent and how
much ammonia can be produced? | back 23 H2 0.277 |
front 24 Which have the same mass? | back 24 2 3 |
front 25 What is the ground state electron configuration for P3-? | back 25 [Ne]3s23p6 |
front 26 What are the oxidation numbers of sulfur in each of the following compounds SF6, S2F10 and SF4, respectively? | back 26 +6 +5 +4 |
front 27 All of the following sets of quantum numbers are allowed EXCEPT n = 3, l= 0, ml = 0 n = 4, l = 2, ml = –1 n = 5, l = 3, ml = +2 n = 2, l = 1, ml = 0 | back 27 1 |
front 28 What is the ground state electron configuration for F? | back 28 [He]2s22p5 |
front 29 If 103 mL of 1.84 M HCl(aq) is diluted with water to a volume of 926 mL, what is the molarity of the diluted HCl(aq)? | back 29 .205 |
front 30 The pH of an aqueous HI solution is 4.08. What is the H3O+ concentration of the solution? | back 30 8.32E-5 |
front 31 Which of the following are diamagnetic? | back 31 2 |
front 32 If a cordless phone operates at a frequency of 46.7 MHz. What is the wavelength of this radiation? | back 32 6.4 m |
front 33 What is the net ionic equation for the reaction of copper(II) hydroxide and hydrochloric acid? | back 33 Cu(OH)2(s)+2H+(aq)Cu2+(aq)+2H2O(l) |
front 34 Which of the following compounds are soluble in
water? | back 34 2 |
front 35 What is the net ionic equation (NIE) for the reaction of aqueous sodium bromide and aqueous lead(II) nitrate? | back 35 Pb+2(aq)+ 2Br-(aq) PbBr2(s) |
front 36 What is the mass of potassium iodide in 112 mL of 4.61E-2 M KI(aq)? | back 36 .857 |
front 37 For a hydrogen atom, calculate the wavelength of an
emitted photon in the Lyman series that results from the transition
n = 6.00 to n =
1.00. Rydberg constant is 1.097E+7
m–1. | back 37 93.8 nm |
front 38 What is the net ionic equation for the reaction of potassium hydroxide and hydroiodic acid? | back 38 H+(aq)+OH-(aq)H2O(l) |
front 39 What is the ground state electron configuration for Co2+? | back 39 [Ar]sd7 |
front 40 Which species in the below reaction is the reducing agent? Zn(s)+ 2Ag+(aq)Zn2+(aq)+ 2Ag(s) | back 40 Zn(s) |
front 41 Which of the following sets of quantum numbers refers to a 3p orbital? | back 41 n=3, l=1, ml=-1 |
front 42 Which of the following statements about the atomic structure model
is/are correct? | back 42 2 3 |
front 43 A 21.46 mL sample of NaOH is titrated with 27.78 mL of 0.1591 M HCl(aq). What is the concentration of the NaOH solution | back 43 .2060 |
front 44 What is the net ionic equation (NIE) for the reaction of aqueous ammonium sulfide and aqueous calcium nitrate? | back 44 Ca2+(aq)+ S2-(aq) CaS(s) |
front 45 What are the spectator ions in the reaction between aqueous ZnCl2 and aqueous K3PO4? | back 45 K+ Cl- |
front 46 What is the ground state electron configuration for Si? | back 46 [Ne] 3s2 3p2 |
front 47 R | back 47 1.097E-7 |
front 48 h | back 48 6.626E-39 |
front 49 c | back 49 2.998E-10 |
front 50 average atomic mass | back 50 (% abundance/100)* mass plus any additional |
front 51 # orbitals in shell | back 51 n2 |
front 52 # orbitals in subshell | back 52 2L+1 |
front 53 Aufbau | back 53 lower levels filled first |
front 54 Pauli | back 54 only 2 e- per orbitals with opposite spins |
front 55 Hund | back 55 singly occupied before doubling up |
front 56 Long Wavelengths vs short wavelengths | back 56 long wavelength -> low frequency, low energy, short line short wavelength -> high frequency, high energy, long line |
front 57 formal charge | back 57 valence e- - (LPE + 1/2 BE) |
front 58 how many particles/atoms in 1 mole | back 58 6.022E23 |
front 59 bond order trend | back 59 single is longest and weakest triple is strongest but shortest |
front 60 atomic radius trend | back 60 increases going down and decreases going right |
front 61 Exothermic | back 61 Expansion system working ON surroundings H < 0 q < 0 w< 0 surroundings get warmer |
front 62 Endothermic | back 62 Compression surroundings effect system H > 0 q > 0 w > 0 surroundings get colder |