Preexam 3 NAME:…………………………………………………………..
Fill the scantron
1) In which set of elements would all members be expected to have very similar chemical
properties?
A) P, Se, I
B) Cl, Br, Na
C) Si, As, Te
D) Ne, Na, Mg
E) Br, I, At
2 ) Screening of the nuclear charge by core electrons in atoms is __________.
A) less efficient than that by valence electrons
B) more efficient than that by valence electrons
C) essentially identical to that by valence electrons
D) responsible for a general decrease in atomic radius going down a group
E) both essentially identical to that by valence electrons and responsible for a general decrease in
atomic radius going down a group
3) Of the following, which gives the correct order for atomic radius for Mg, Na, P, Si and Ar?
A) Mg > Na > P > Si > Ar
B) Ar > Si > P > Na > Mg
C) Si > P > Ar > Na > Mg
D) Na > Mg > Si > P > Ar
E) Ar > P > Si > Mg > Na
4) Which of the following correctly represents the second ionization of aluminum?
A) Al+ (g) + e- → Al (g)
B) Al (g) → Al+ (g) + eC) Al- (g) + e- → Al2- (g)
D) Al+ (g) + e- → Al2+ (g)
E) Al+ (g) → Al2+ (g) + e-
5-intro) Consider the following electron configurations to answer the questions that follow:
(i) 1s22s22p63s1
(ii) 1s22s22p63s2
(iii) 1s22s22p63s23p1
(iv) 1s22s22p63s23p4
(v) 1s22s22p63s23p5
The electron configuration belonging to the atom with the highest second ionization energy is
__________.
A) (i)
B) (ii)
C) (iii)
D) (iv)
E) (v)
6) Of the elements below, __________ has the highest melting point.
A) Ca
B) K
C) Fe
D) Na
E) Ba
7) Transition metals within a period differ mainly in the number of ________ electrons.
A) s
B) p
C) d
D) f
E) all of the above
8) Which one of the following compounds would produce an acidic solution when dissolved in
water?
A) Na2O
B) CaO
C) MgO
D) CO2
E) SrO
9) Which of the following has eight valence electrons?
A) Ti4+
B) Kr
C) ClD) Na+
E) all of the above
10) In ionic bond formation, the lattice energy of ions ________ as the magnitude of the ion
charges _______ and the radii __________.
A) increases, decrease, increase
B) increases, increase, increase
C) decreases, increase, increase
D) increases, increase, decrease
E) increases, decrease, decrease
11) In which of the molecules below is the carbon-carbon distance the shortest?
A) H2C CH2
B) H–C≡C–H
C) H3C–CH3
D) H2C C CH2
E) H3C–CH2–C H3
12) Of the atoms below, __________ is the most electronegative.
A) Si
B) Cl
C) Rb
D) Ca
E) S
13) Which of the following has the bonds correctly arranged in order of increasing polarity?
A) Be F, Mg F, N F, O F
B) O F, N F, Be F, Mg F
C) O F, Be F, Mg F, N F
D) N F, Be F, Mg F, O F
E) Mg F, Be F, N F, O F
14) In the nitrite ion (NO2-), __________.
A) both bonds are single bonds
B) both bonds are double bonds
C) one bond is a double bond and the other is a single bond
D) both bonds are the same
E) there are 20 valence electrons
15) A valid Lewis structure of __________ cannot be drawn without violating the octet rule.
A) NF3
B) IF3
C) PF3
D) SbF3
E) SO42-
16) Why don't we draw double bonds between the Be atom and the Cl atoms in BeCl2?
A) That would give positive formal charges to the chlorine atoms and a negative formal charge
to the beryllium atom.
B) There aren't enough electrons.
C) That would result in more than eight electrons around beryllium.
D) That would result in more than eight electrons around each chlorine atom.
E) That would result in the formal charges not adding up to zero.
17) The ion PO43- has __________ valence electrons.
A) 14
B) 24
C) 27
D) 29
E) 32
18) The Lewis structure of HCN (H bonded to C) shows that __________ has __________
nonbonding electron pairs.
A) C, 1
B) N, 1
C) H, 1
D) N, 2
E) C, 2
19) The formal charge on nitrogen in NO3- is __________.
A) -1
B) 0
C) +1
D) +2
E) -2
20) The formal charge on sulfur in SO42- is __________, where the Lewis structure of the ion is:
A) -2
B) 0
C) +2
D) +4
E) -4
21) Using the table of average bond energies below, the △H for the reaction is __________ kJ.
C≡O (g) + 2H2 (g) → H3C–O–H (g)
Bond: C–O C=O C≡O C–H H–H
D (kJ/mol): 358 799 1072 413
436
O–H
463
A) +276
B) -276
C) +735
D) -735
E) -116
22) The wavelength of a photon that has an energy of 5.25 1019 J is __________ m.
A) 3.79 107
B) 2.64 106
C) 2.38 1023
D) 4.211024
E) 3.79 107
23) Calculate the energy (J) change associated with an electron transition from n = 2 to n = 5 in a
Bohr hydrogen atom.
A) 6.5  1019
B) 5.5 1019
C) 8.7  10 20
D) 4.6  10 19
E) 5.8 1053
24) The lowest energy shell that contains f orbitals is the shell with n = __________.
A) 3
B) 2
C) 4
D) 1
E) 5
25) In a hydrogen atom, an electron in a __________ orbital can absorb a photon, but cannot
emit a photon.
A) 3s
B) 2s
C) 3p
D) 1s
E) 3f
26)
[Ar]4s2 3d10 4p3 is the electron configuration of a(n) __________ atom.
A) As
B) V
C) P
D) Sb
E) Sn
27) The lowest orbital energy is reached when the number of electrons with the same spin is
maximized. This statement describes __________.
A) Pauli Exclusion Principle
B) Planck's constant
C) deBroglie hypothesis
D) Heisenberg Uncertainty Principle
E) Hund's rule
28) Which set of three quantum numbers (n, l, ml) corresponds to a 3d orbital?
A) 3, 2, 2
B) 3, 3, 2
C) 3, 2, 3
D) 2, 1, 0
E) 2, 3, 3
29) Which one of the following represents an impossible set of quantum numbers for an electron
in an atom? (arranged as n, l, ml, and ms)
A) 2, 1, -1, -1/2
B) 1, 0, 0, 1/2
C) 3, 3, 3, 1/2
D) 5, 4, - 3, 1/2
E) 5, 4, -3, -1/2
30) Which electron configuration represents a violation of the Pauli exclusion principle?
A)
B)
C)
D)
E)
31) The valence shell of the element X contains 2 electrons in a 5s subshell. Below that shell,
element X has a partially filled 4d subshell. What type of element is X?
A) main group element
B) chalcogen
C) halogen
D) transition metal
E) alkali metal
32) An electron in a(n) __________ subshell experiences the smallest effective nuclear
charge in a many-electron atom.
A) 3f
B) 3p
C) 3d
D) 3s
E) 4s
33)A tin atom has 50 electrons. Electrons in the __________ subshell experience the higest
effective nuclear charge.
A) 1s
B) 3p
C) 3d
D) 5s
E) 5p
34) The first ionization energies of the elements __________ as you go from right to left across a
period of the periodic table, and __________ as you go from the top to the bottom of a group in
the table.
A) increase, increase
B) increase, decrease
C) decrease, increase
D) decrease, decrease
E) are completely unpredictable
35) In
which set of elements would all members be expected to have very similar chemical
properties?
A) Ca, Sr, Ba
B) N, O, F
C) Na, Mg, K
D) S, Se, Si
E) Ne, Na, Mg
36) Of the hydrogen halides, only __________ is a weak acid.
A) HCl (aq)
B) HBr (aq)
C) HF (aq)
D) HI (aq)
E) They are all weak acids.
37)Atomic radius generally increases as we move __________.
A) down a group and from right to left across a period
B) up a group and from left to right across a period
C) down a group and from left to right across a period
D) up a group and from right to left across a period
E) down a group; the period position has no effect
38) Which of the following correctly lists the five atoms in order of increasing size (smallest to
largest)?
A) O < F < S
B) F < O < S
C) F < O < S
D) O < F < S
E) F < S < O
<
<
<
<
<
Mg < Ba
Mg < Ba
Ba < Mg
Ba < Mg
Mg < Ba
39) Of the choices below, which gives the order for first ionization energies?
A) Cl > S > Al > Ar > Si
B) Ar > Cl > S > Si > Al
C) Al > Si > S > Cl > Ar
D) Cl > S > Al > Si > Ar
E) S > Si > Cl > Al > Ar
40)Which of the following has the largest second ionization energy?
A) Si
B) Mg
C) Al
D) Na
E) P