BASIC REVIEW CH.1-8
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Question 1
How many protons does copper have?
Explanation
Question 2
How many electrons does copper have? Remember atoms are neutral.
Question 3
How many neutrons does copper-63 have? Help given in feedback.
Explanation
Remember the protons and neutrons constitute most of the mass of an atom. For example, iron-56 has an approximate mass of 56 g per mol. Per atom, there are 26 protons and 56-26 = 30 neutrons.
Question 4
What is the mass of 1 mol of CO2 in g?
Molar mass example
Explanation
Molar Mass of CO2 = 44 g
1 mol of CO2 = x g / 44 (g/ mol)
Question 5
What is the mass of 39 molecules of SO3 in g?
Explanation
39 molecules / (6.022*10^23) * 80.066 = 5.18e-21
(molecules/ Avogadro’s #) * MolarMass(g)
Question 6
Correctly match the element with the property.
Periodic Table and Group IA and IIA metals
Metal that reacts with cold water to produce OH- and H2(g)Choose…CrNaSSiHe Metal (all conduct electricity)–no reaction with water, but reacts with acid to produce H2 gasChoose…CrNaSSiHe
Non-metal–does not conduct electricityChoose…CrNaSSiHe
Noble gas–inert, stable electron configurationChoose…CrNaSSiHe
Semimetal–poor conductor of electricityChoose…CrNaSSiHe
Question 7
What is the correct formula for aluminum sulfide?
Oxidation states
Select one:
Explanation
Al 3+; S2-
Al2S3
Question 8
Which compound is the most ionic?
Select one:
Explanation
Ionic compounds-
Question 9
Match properties correctly
Indicates energy and size of orbitalChoose…pnfd2s l=0Choose…pnfd2s
l=1Choose…pnfd2s
l=2Choose…pnfd2s
l=3Choose…pnfd2s
Number of possible electron spins for each orbitalChoose…pnfd2s
Explanation
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Question 10
Select the correct set of quantum mechanical numbers for an electron in an s, p, d, and f orbital. (4 correct answers.)
Allowed Combination of Quantum Numbers
Select one or more:
Explanation
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Question 11
Correctly match the information for the angular momentum quantum number (l) which gives the shape of the orbital. A nodal plane is a region where the electron density is zero, that is, the probability of finding the electron there is zero.
The maximum number of electrons in an electron orbital.Choose…dspf2 Spherically symmetric orbital–no nodal planesChoose…dspf2
Orbital shaped like a peanut or dumbbell–one nodal planeChoose…dspf2
4 of the 5 orbital shaped like a double peanut–2 nodal planesChoose…dspf2
Orbital shaped like flower or fancy–3 nodal planesChoose…dspf2
Explanation
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Question 12
What is the ground-state electron configuration for S?
Select one:
Explanation
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Question 13
What is the electron configuration for S2-?
Electron Configurations Negative Ions
Select one:
Explanation
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Question 14
What is the electron configuration for K1+?
Electron Configurations Positive Ions
Select one:
Explanation
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Question 15
Match atomic radius from largest to smallest.
KChoose…Second largest atomic radiusThird largest atomic radiusFourth largest atomic radiusLargest atomic radiusSmallest atomic radius AlChoose…Second largest atomic radiusThird largest atomic radiusFourth largest atomic radiusLargest atomic radiusSmallest atomic radius
NaChoose…Second largest atomic radiusThird largest atomic radiusFourth largest atomic radiusLargest atomic radiusSmallest atomic radius
ArChoose…Second largest atomic radiusThird largest atomic radiusFourth largest atomic radiusLargest atomic radiusSmallest atomic radius
SChoose…Second largest atomic radiusThird largest atomic radiusFourth largest atomic radiusLargest atomic radiusSmallest atomic radius
Explanation
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Question 16
Match ionization energies from smallest to largest.
KChoose…Third smallest ionization energyFourth smallest ionization energyLargest ionization energySmallest ionization energySecond smallest ionization energy AlChoose…Third smallest ionization energyFourth smallest ionization energyLargest ionization energySmallest ionization energySecond smallest ionization energy
NaChoose…Third smallest ionization energyFourth smallest ionization energyLargest ionization energySmallest ionization energySecond smallest ionization energy
ArChoose…Third smallest ionization energyFourth smallest ionization energyLargest ionization energySmallest ionization energySecond smallest ionization energy
SChoose…Third smallest ionization energyFourth smallest ionization energyLargest ionization energySmallest ionization energySecond smallest ionization energy
Explanation
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Question 17
What is the correct formula for iron (III) oxide?
Multiple oxidation states
Select one:
Explanation
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Question 18
Which of the following tin (IV) compounds makes sense using oxidation states and conservation of charge?
Oxidation State and Polyatomic Ions
Select one:
Explanation
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Question 19
Warmup question. How many moles of Ca(OH)2 are required to neutralize (react completely with) 0.89 moles of HCl? The balanced reaction is:
2HCl(aq) + Ca(OH)2(aq) → 2H2O(l) + CaCl2(aq)
Explanation
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Question 20
What volume in L of 0.35 M Ca(OH)2 is required neutralize 0.39 moles of HCl? The balanced reaction is:
2HCl(aq) + Ca(OH)2(aq) → 2H2O(l) + CaCl2(aq)
Explanation
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Question 21
What volume in L of chlorine at 30oC and 611 torr is required to react completely with 3.72 g aluminum:
2Al(s) + 3Cl2(g) → 2AlCl3(s)
Calculate the moles chlorine needed (as in the previous problem), then use the ideal gas law–PV = nRT. Additional help is given in the feedback.
Explanation
Procedure: g Al –> mol Al –> mol Cl2. Next solve for V in PV = nRT. Did you remember to convert torr to atm and oC to K?
Question 22
The following reaction takes place at a certain elevated temperature:
Fe2O3(s) + 3CO(g) → 2Fe(l) + 3CO2(s)
What is the percent yield of iron if 41.1 g Fe2O3 in excess CO produces 25.0 g Fe? The M.W. of Fe2O3 is 159.7 g/mol and the M.W. of CO is 28.01 g/mol.
Recall that the percent yield is the actual yield divided by the theoretical yield times 100%. Additional help is given in the feedback.
Explanation
Procedure: g Fe2O3 –> mol Fe2O3 –> mol Fe –> g Fe (This is the theoretical yield. Note M.W. CO is not used.) Take actual yield, 25.0, and divide by the theoretical yield and then multiply by 100 (to change to percent yield).
Question 23
What is the mass percent of carbon in sugar, C12H22O11? M.W. sugar = 342 g/mol.
Help is given in the feedback.
Explanation
Mass percent C = (mass C/ total mass) x 100%. Pick 1 mol sugar. What is the mass? How many mol C in 1 mol sugar? What is the mass C?
Question 24
Analysis of 3.500 g sample of an unknown compound shows that it contains 1.400 g C, 0.235 g H, and the rest O. What is the empirical formula of this compound?
Hint, given in feedback.
Select one:
Explanation
Because total mass is conserved, the mass of O can be found. Convert each mass to moles. Convert moles to smallest whole numbers. Sometimes it is sufficient to divide each by the smallest number of moles. Compare the number of moles of each element in the compound.
Question 25
Hemoglobin has a mass of about 67,000 g/mol. It is 0.3335% iron by mass. How many iron atoms are in a molecule of hemoglobin?
Help is given in the feedback.
Explanation
Find mass of iron in 1 mole of hemoglobin. Divide by M.W. of iron. This gives moles of iron in 1 mole of hemoglobin. It equals the atoms of iron in 1 molecule of hemoglobin.