Ch. 1-3
Ch. 4-6
Ch.7-9
Ch.10-11
You get what you get
100
What is the correct name for covalent substance N2O?
dinitrogen monoxide
100
Which of the following metals will most likely react with water? a) K b) Ag c) Cr d) Co
K
100
Which period 2 element would be most likely to have the following successive ionization energies IE1=1,100 IE2=1,300 IE3=1,500 IE4 = 11,000 IE5=12,000
B
100
Under what conditions is the molecular shape the same as the electron-group arrangement? a) When the central atom has only single bonds b) When the central atom obeys the octet rule c) When the lone pairs on the central atom symmetrically arranged around d) When there are no lone pairs on the central atom
d) When there are no lone pairs on the central atom
100
Who was the scientist to propose that each electron in an atom travels in an orbit, similar to a planet in the solar system?
Bohr
200
Consider the following balanced reaction: 2 S2 + 3 O2 --> 2 S2O3 (MM S2 = 64.14) (MM O2 = 32.00) (MM S2O3 = 112.1) How many grams of S2O3 will excess S2 plus 44.0g O2 produce?
44g x (1 mol/32) = 1.375 mol x (2 mol S2O3 / 3 mol O2) = .917 mol x (112.1g/mol S2O2) = 102.8g
200
Which of the following ionic substances is most soluble? a) CoCO3 b) Ag3PO4 c) CaCl2 d) Pb(OH)2
CaCl2
200
Select a full set of quantum numbers for the last electron added to form the N atom (according to convention): a) n=2, l=1, ml=0, ms=-1/2 b) n=2, l=1, ml=-1, ms=-1/2 c) n=3, l=0, ml=-1, ms=+1/2 d) n=2, l=1, ml=+1, ms=+1/2
d) n=2, l=1, ml=+1, ms=+1/2
200
How many lone-pairs of electrons are on Cl in the ClF3 molecule?
2
200
Order the following elements by increasing atomic size: Ge, P, As
P < As < Ge
300
Which of the following does NOT match the name provided? A. SO42- Sulfate B. NO3– Nitrate C. ClO4– Chlorate D. PO43- Phosphate
ClO4– Chlorate
300
A system receives 200J of heat from the surroundings, and the surroundings does 800J of work on the system. Calculate the change in the internal energy, DeltaE, of the system.
+ 200J +800J +1000J
300
What is the correct "letter" designation for the "n=4, l=0" sub level?
S
300
Which of the following molecular shapes does not belong to the trigonal bi-pyramid electron group arrangement? a) T-shaped b) linear c) tetrahedral d) see-saw
c) tetrahedral
300
The octahedral hybrid configuration is composed of which orbital combination?
sp3d2
400
Suppose the [imaginary] element Saturnium (St) has two isotopes: 64^St 63.77g 30.00 abundant 67^St 67.03g 70.00 abundant
63.77g x .3 = 19.13 67.03g x .7 = 46.92 _____ 66.05
400
Which of the following statements is TRUE regarding thermochemical processes? a) DeltaH is typically measured using a content volume process b) in a constant volume process, heat flow into the system is always zero c) in a constant volume process, work done on the system is always zero d) DeltaE is best measured using a constant pressure process
c) in a constant volume process, work done on the system is always zero
400
What is the electron configuration of Pb2+ and Pb4+
Pb2+ [Xe] 6s2 4f14 5d10 Pb 4+ [Xe] 4f14 5d10
400
Describe the type(s) of bond(s) connecting the two carbon atoms in HC---CH. --- stands for triple bond in this question.
one sigma and two pi bonds.
400
According to molecular orbital theory, which statement is incorrect for neutral B2? a) the bond order is 2 b) The pi2p orbitals each have one electron c) the molecule is paramagnetic d) there are 10 electrons in molecular orbitals
a) the bond order is 2
500
Who used oil droplets to determine the charge of the electron?
Millikan
500
What is the oxidation number of P in the polyatomic ion P2O7 ^ 4-
+5
500
What is the energy difference between n = 5 and n =7 states of the H atom (in J)? B=2.18×10-18 J R=1.096776×107 m-1 h=6.626×10-34 J·s
-2.18E-18 x (1/49 - 1/25) = 4.27E-20
500
Which type of molecular orbital does the last electron go into in the molecular ion N2-
Pi*
500
Which one of the metric prefixes below correctly matches the multiplier beside it? a) deci 10^-2 b) pico 10^-12 c) micro 10^-3 d) nano 10^9
b) pico 10^-12
M
e
n
u