CH 101 Final
What is the maximum number of d orbitals that are possible in a given shell?
9
The de Broglie wavelength of an electron with a velocity of 7.40 × 106 m/s is ________ m. The mass of the electron is 9.11 × g.
9.83 x 10^-11
What is the volume (in cm3) of a 9.37 g piece of metal with a density of 4.66 g/cm3?
2.01
When 8.00 × 1023 molecules of ammonia react with 7.00 × 1022 molecules of oxygen according to the chemical equation shown below, how many grams of nitrogen gas are produced? 4 NH3(g) + 3 O2(g) → 2 N2(g) + 6 H2O(g)
2.17 g
What is the bond order of N21+?
2.5
Draw the best Lewis structure for the nitrate ion. What is the formal charge on the N?
+1
What is the oxidation number for nitrogen in the nitrite ion?
+3
The temperature rises from 25.00°C to 29.00°C in a bomb calorimeter when 3.50 g of sucrose undergoes combustion in a bomb calorimeter. Calculate ΔErxn for the combustion of sucrose in kJ/mol sucrose. The heat capacity of the calorimeter is 4.09 kJ/°C. The molar mass of sugar is 342.3 g/mol.
-1.60 × 103 kJ/mole
Give the possible values for ml for a d orbital.
-2, -1, 0, 1, 2
Calculate the change in internal energy (ΔE) for a system that is giving off 25.0 kJ of heat and is changing from 12.00 L to 4.00 L in volume at 1.50 atm pressure. (Remember that 101.3 J = 1 L∙atm)
-23.8 kJ
A sample of NI3 is contained in a piston and cylinder. The samples rapidly decomposes to form nitrogen gas and iodine gas, and releases 3.30 kJ of heat and does 590 J of work. What is ∆E?
-3890 J
Calculate the work, w, gained or lost by the system when a gas expands from 15 L to 40 L against a constant external pressure of 2.5 atm. 1 L ∙ atm = 101 J
-6.3 kJ
Give the theoretical yield, in moles, of CO2 from the reaction of 4.00 moles of C6H14 with 4.00 moles of O2. 2 C6H14 + 19 O2 → 12 CO2 + 14 H2O
2.52 moles
Give the number of valence electrons for XeF2.
22
Calculate the wavelength (in nm) of the blue light emitted by a mercury lamp with a frequency of 6.88 × 1014 Hz.
436 nm
According to the following reaction, what volume of 0.244 M KCl solution is required to react exactly with 50.0 mL of 0.120 M Pb(NO3)2 solution? 2 KCl(aq) + Pb(NO3)2(aq) → PbCl2(s) + 2 KNO3(aq)
49.2 mL
How many significant figures are in the measurement, 20.300 m?
5
Draw the Lewis structure for SO42⁻. How many equivalent resonance structures can be drawn?
6
Identify the number of electron groups around a molecule with sp3d2 hybridization
6
What is the mass of 6.78 × 1024 molecules of SO2? The molar mass of SO2 is 64.06 g?
721 g
Identify the number of valence electrons in Cl-.
8
Give the mass percent of hydrogen in C14H19NO2
8.21%
If an object has a density of 8.65 g/cm3, what is its density in units of kg/m3?
8.65 × 103 kg/m3
How many molecules of sucrose (C12H22O11, molar mass = 342.30 g/mol) are contained in 14.3 mL of 0.104 M sucrose solution?
8.96 × 1020 molecules C12H22O11
All of the following compounds are soluble EXCEPT
PbCl2
The atomic number (Z) is the number of ________ found in the nucleus of an atom.
Protons
Place the following in order of decreasing XO bond length, where "X" represents the central atom in each of the following compounds or ions. SiO32⁻ CO2 CO32⁻
SiO32⁻ > CO32⁻ > CO2
What does "X" represent in the following symbol? 28 X 14
Silicon
Which reaction below represents the second ionization of Sr?
Sr⁺(g) → Sr2⁺(g) + e⁻
Which element would most likely form an ion with a charge of -2?
Te
Rutherford's Gold Foil Experiment helped prove
That the mass of an atom is concentrated in a very small space.
Which of the following statements is FALSE?
The alkali metals are fairly unreactive.
Which of the following statements is FALSE?
The halogens tend to form 1+ ions.
The mass number is equal to
The sum of the number of protons and neutrons.
Which of the following occur as the energy of a photon increases?
The wavelength gets shorter.
Which element is diamagnetic?
V
Choose the ground state electron configuration for Zn2⁺.
[Ar]3d10
Give the ground state electron configuration for I.
[Kr]5s24d105p5
Give the ground state electron configuration for Pb
[Xe]6s24f145d106p2
Write the name for Ba3(PO4)2.
barium phosphate
Choose the pure substance from the list below.
carbon dioxide
The compound, Cu(NO3)2, is named
copper(II) nitrate.
Halogens can react with each other to form
covalent bonds
Determine the electron geometry (eg) and molecular geometry (mg) around the underlined atom in (CH3)3N (three CH3 groups attached to nitrogen).
eg = tetrahedral, mg = trigonal pyramidal
Determine the electron geometry (eg), molecular geometry (mg) and polarity of XeO3
eg = tetrahedral, mg = trigonal pyramidal, polar
Determine the electron geometry (eg), molecular geometry (mg), and polarity of PF3.
eg = tetrahedral, mg = trigonal pyramidal, polar
Determine the electron geometry (eg) and molecular geometry (mg) of BrF3.
eg = trigonal bipyramidal, mg = T-shape
Determine the electron geometry (eg) and molecular geometry (mg) of XeF2
eg = trigonal bipyramidal, mg = linear
Determine the electron geometry (eg) and molecular geometry (mg) of CH3+1.
eg = trigonal planar, mg = trigonal planar
Determine the electron geometry (eg) and molecular geometry (mg) of CO32⁻.
eg = trigonal planar, mg = trigonal planar
Give the name for SnO
tin (II) oxide
Give the hybridization for the O in OCl2
zp3
Draw the best Lewis structure for BrO4⁻ and determine the formal charge on bromine.
0
For n = 3, what are the possible sublevels?
0, 1, 2
A beaker contains 0.25 mol of potassium bromide in 600 mL of water. An additional 600 mL of water is added. The number of moles of potassium bromide in the beaker is
0.25
The titration of 25.0 mL of an unknown concentration H2SO4 solution requires 83.6 mL of 0.21 M LiOH solution. What is the concentration of the H2SO4 solution (in M)?
0.35 M
What is the concentration of phosphate ions in a 0.250 M Mg3(PO4)2 solution?
0.500 M
According to the following reaction, what amount of Al2S3 remains when 2.00 g of Al2S3 and 1.00 g of H2O are reacted? A few of the molar masses are as follows: Al2S3 = 150.17 g/mol, H2O = 18.02 g/mol. Al2S3(s) + 6 H2O(l) → 2 Al(OH)3(s) + 3 H2S(g)
0.611 g
How many of the following molecules have sp3 hybridization on the central atom? XeCl4 CBr4 SF4 C2H2
1
How many moles of C6H8 contain 4.95 × 1024 hydrogen atoms?
1.03 moles C6H8
A piece of metal weighing 57.3 g is heated to a temperature of 88.0°C and is then immersed in 155 g of water at a temperature of 21.53°C. After equilibration the temperature is 27.42°C. If CH2O = 4.184 J/g°C, what is Cmetal?
1.10 J/g°C
What answer should be reported, with the correct number of significant figures, for the following calculation? (433.621 - 333.9) × 11.900
1.19 × 103
What mass (in mg) does 2.63 moles of nickel have?
1.54 × 105 mg
A 1.401 g sample of N2 reacts with 2.031 g of H2 to form ammonia (NH3). If ammonia is the only product, what mass of ammonia is formed?
1.70 g (N2 + 3H2 -> 2NH3)
Which of the following contains the fewest atoms? You shouldn't need to do a calculation here.
10.0 g Cs
Consider the following balanced reaction. How many grams of water are required to form 79.5 g of HNO3? Assume that there is excess NO2 present. The molar masses are as follows: H2O = 18.02 g/mol, HNO3 = 63.02 g/mol. 3 NO2(g) + H2O(l) → 2 HNO3(aq) + NO(g)
11.4 g H2O
Give the percent yield when 26.18 g of CO2 are formed from the reaction of 4.000 moles of C8H18 with 8.000 moles of O2. 2 C8H18 + 25 O2 → 16 CO2 + 18 H2O
11.62%
If the density of methanol, CH3OH, is 0.792 g/mL. How many milliliters of methanol are needed to produce 20.0 g of CO2 according to the following chemical equation? CH3OH(l) + 2 O2(g) → CO2(g) + 2 H2O(l)
18.4 mL
How many valence electrons do alkali earth metals possess?
2
What value of l is represented by a d orbital?
2
How many valence electrons does an atom of Al possess?
3
What is the charge on the Fe ions in Fe2O3?
3+
How many mm are in 3.20 cm?
3.20 × 101 mm
Calculate the energy of the orange light emitted, per photon, by a neon sign with a frequency of 4.89 × 1014 Hz
3.24 × 10-19 J
A new compound was recently discovered and found to have an atomic weight of 342.38 amu. This element has two isotopes, the lighter of which has a mass of 340.91 amu and an abundance of 68.322%. What is the mass of the heavier isotope?
345.55
How many oxygen atoms are there in 3.00 g of sodium dichromate, Na2Cr2O7?
4.83 × 1022 oxygen atoms
How many photons are contained in a flash of green light (525 nm) that contains 189 kJ of energy?
4.99 × 1023 photons
Which of the following represent isotopes?
A and C
An atom that has lost an electron is
A cation
Calculate the mass (in ng) of 2.33 × 1020 atoms of oxygen
A) 6.19 × 106 ng
Determine the oxidizing agent in the following reaction. Ag(C2H3O2)(aq) + K(s) → KC2H3O2(aq) + Ag(s)
Ag
Which of the following statements is TRUE?
An orbital that penetrates into the region occupied by core electrons is less shielded from nuclear charge than an orbital that does not penetrate and therefore has a lower energy.
Place the following in order of increasing IE1. N F As
As < N < F
Which statement about electromagnetic radiation is correct?
As the energy decreases the frequency decreases.
Identify the compound with atoms that have an incomplete octet
BF3
The chemical formula for barium nitride is
Ba3N2.
Which of the following contains BOTH ionic and covalent bonds?
BaSO4
Which of the following visible colors of light has the highest frequency?
Blue
Which of the following contains an atom that does NOT obey the octet rule?
BrF3
Draw the Lewis structure for the molecule CH2CHCH3. How many sigma and pi bonds does it contain?
C) 8 sigma, 1 pi
What is the empirical formula of a substance that contains 5.28 g of C, 1.11 g of H, and 3.52 g of O?
C2H5O
Why does an electron found in a 2s orbital have a lower energy than an electron found in a 2p orbital in multielectron systems?
Electrons in the 2s orbital can penetrate the 1s orbital and be closer to the nucleus
Which of the following pairs of aqueous solutions will form a precipitate when mixed?
FeCl3 + KOH
What are the oxidation numbers for the atoms in the following compound? H2O2
H = + 1, O = -1
Give the net ionic equation for the reaction (if any) that occurs when aqueous solutions of sodium hydrogen carbonate and hydrobromic acid are mixed.
H+(aq) + HCO3-(aq) → H2O(l) + CO2(g)
Place the following in order of decreasing bond length. H-F H-I H-Br
H-I > H-Br > H-F
The chemical formula for phosphoric acid is
H3PO4(aq).
Which compound has the highest carbon-carbon bond strength?
HCCH
A student performs an experiment to determine the density of a sugar solution. The student obtains the following results: 1.11 g/mL, 1.10 g/mL, 1.12 g/mL, 1.13 g/mL. If the actual value for the density of the sugar solution is 1.91 g/mL, which statement below best describes her results?
Her results are precise, but not accurate.
What is the empirical formula for Hg2(NO3)2?
HgNO3
Determine the limiting reactant (LR) and the mass (in g) of nitrogen that can be formed from 55.0 g N2O4 and 50.0 g N2H4. Some possibly useful molar masses are as follows: N2O4 = 92.02 g/mol, N2H4 = 32.05 g/mol. N2O4(l) + 2 N2H4(l) → 3 N2(g) + 4 H2O(g)
LR = N2O4, 50.2 g N2 formed
All samples of a given compound, regardless of their source or how they were prepared, have the same proportions of their constituent elements. Which law does this refer to?
Law of Definite Proportions
Write the formula for the compound formed between lithium and sulfur.
Li2S
Identify the compound with the largest dipole moment in the gas phase.
LiF
What species is represented by the following information? p+ = 12 n° = 14 e- = 10
Mg2+
What element is undergoing reduction (if any) in the following reaction? 2 MnO4-(aq) + 3 NO2-(aq) + H2O(l) → 2 MnO2(s) + 3 NO3-(aq) + 2 OH-(aq)
Mn
Place the following in order of increasing metallic character. Rb Cs K Na
Na < K < Rb < Cs
lace the following in order of increasing radius. Br⁻ Na⁺ Rb⁺
Na⁺ < Rb⁺ < Br⁻
What element(s) is/are undergoing reduction (if any) in the following reaction? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(g)
O
Place the following in order of increasing atomic radius. As O Br
O < Br < As
Which of the following is a molecular compound?
P2O4
Identify glucose (C6H12O6)
nonelectrolyte
Which of the compounds, KH, NH3, C2H6, HF, are ionic compounds?
only KH
Give the name for P Cl3
phosphorus tri chloride
Which of the following signs on q and w represent a system that is doing work on the surroundings, as well as losing heat to the surroundings?
q = -, w = -
What are the possible orbitals for n = 3?
s, p, d
What bond angle would you predict in the molecule ClNO?
slightly less than 120°
Give the hybridization for the C in HCN
sp
Give the hybridization for the O in H3O+.
sp3
