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Periodic Trends
Solubility
Kinetics
Bonding
Acids and Bases
100
Which element is larger? a) carrbon; 6 b) francium; 87 c) nitrogen; 7 d) oxygen; 8
b) francium; 87
100
Which of the following is not soluble in water? a) silver nitrate b) sodium chloride c) lithium carbonate d) lead(II) bromide
d) lead(II) bromide
100
Predict the overall rate law for the following single elementary step? 2NO+Br2 -> 2NOBr a) rate=k[NO2][Br2] b) rate=k[NO]^2[Br]^2 c) rate=k[NO]^2[Br2] d) rate=k[NO]^2[Br2]^2
c) rate=k[NO]^2[Br2]
100
What is the name of the model used in chemistry to predict the 2D geometry of individual molecules from the number of electron pairs surrounding their central atoms? a) Kepert Model b) VSEPR Theory c) Atomic Theory d) Hund's Rule
b) VSEPR Theory
100
What is the hydroxide ion concentration for a solution with a pH of 10 at 25^oC? a) 10^-14M b) 10^-5M c) 10^-4M d) 10^-10M
c) 10^-4M
200
Electron Affinity describes- a) the change in energy due to the removal of an electron b) the change in energy due to the addition of an electron c) the difference between the amount of protons and electrons d) the difference in energy between protons and electrons
b) the change in energy due to the addition of an electron
200
Which of these ions make sulfate insoluble? a) Ba^2+ b) Li^+ c) NH4^+ d) Br^-
a) Ba^2+
200
You are attempting to calculate the half life for a second order reaction. Which equation should you use? a) t(1/2)=[A]0/2k b) t(1/2)=ln(2)/k c) t(1/2)=1/([A]0)2k
c) t(1/2)=1/([A]0)2k
200
How many lone pairs does a square pyramidal shaped molecule have? a) 0 b) 1 c) 2 d) 3
b) 1
200
Where is the equivalence point for the titration of a strong acid and a weak base? a) above 7 b) below 7 c) 14 d) 7
b) below 7
300
What causes the ionization energy to decrease? a) an increase in shielding b) more electrons added c) less protons in an element d) a and c
d) a and c
300
How do you know if you have correctly written a neutralization reaction? a) if the weak bases and acids ionize 100% b) if strong bases and acids remain together c) if strong bases and acids ionize 100% d) if nothing precipitates from it
c) if strong bases and acids ionize 100%
300
Which units are used for a first order rate constant a) L/mol*s b) 1/s c) 1/M*s d) mol/L
b) 1/s
300
What is the molecular geometry of NH3? a) bent b) trigonal planar c) see-saw d) trigonal pyramidal
d) trigonal pyramidal
300
What is the major difference between a strong and weak acid? a) Strong acids dissociate completely while weak acids dissociate somewhat b) Strong acids dissociate completely while weak acids don't dissociate at all c) Strong acids dissociate somewhat while weak acids don't dissociate at all d) Strong acids contain carbon while weak acids do not
a) Strong acids dissociate completely while weak acids dissociate somewhat
400
Why is it harder to remove the first electron from nitrogen than from carbon? a) nitrogen is larger than carbon b) carbon is less electronegative c) nitrogen has an electron in all 1p orbitals d) it's harder to remove the first electron from carbon
c) nitrogen has an electron in all 1p orbitals
400
When a solution of silver nitrate is mixed with magnesium bromide, which of the following precipitate is formed? a) MgBr2 b) AgBr c) Mg(NO3)2 d) AgNO3
b) AgBr
400
Which of the following is matched correctly? a) Zero Order: [A]=-kt+[A]0 First Order: ln[A]=-kt+ln[A]0 Second Order: 1/[A]=kt+1/[A] b) Zero Order: ln[A]=-kt+ln[A]0 First Order: [A]=-kt+[A]0 Second Order: 1/[A]=kt+1/[A] c) Zero Order: [A]=-kt+[A]0 First Order: 1/[A]=kt+1/[A] Second Order: ln[A]=-kt+ln[A]0
a) Zero Order: [A]=-kt+[A]0 First Order: ln[A]=-kt+ln[A]0 Second Order: 1/[A]=kt+1/[A]
400
How many areas of electron density does SF4 have? a) 3 b) 4 c) 5 d) 6
c) 5
400
Which one of the following acids is the weakest? a) HNO3 b) HCl c) H2SO4 d) H3PO4
d) H3PO4
500
Joe has an unknown compound. How can he tell if the compound is ionic? a) react it with oxygen b) dissolve it in water to see if it's conductive c) see if it stretches d) burn it to see what color it makes
b) dissolve it in water to see if it's conductive
500
When is Ca(OH)2 soluble? a) When its molarity is 20M or greater b) When its molarity is less than 1M c) It's never soluble d) It's always soluble
b) When its molarity is less than 1M
500
In a first order chemical reaction which is true at constant temperature? a) Half-Life and k are both constant b) Neither half-life nor k is constant c) Half-Life is constant, but k changes d) Half-Life changes, but k is constant
d) Half-Life changes, but k is constant
500
What are the bond angles in a ClF3? a) 90/120 b) <120 c) 90/180 d) 90/<120
c) 90/180
500
Which molecule/ion has the greatest potential to act as a Lewis acid? a) CH3^+ b) CN^- c) CO2 d) BF4
a) CH3^+