Chapter 7
1) The atomic radius of main-group elements generally increases down a group because ______.
A) effective nuclear charge increases down a group
B) effective nuclear charge decreases down a group
C) effective nuclear charge zigzags down a group
D) the principal quantum number of the valence orbitals increases
E) both effective nuclear charge increases down a group and the principal quantum number of the valence orbitals increases
2) 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
3) Atomic radius generally decreases 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
4) 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
5) Of the following, which gives the correct order for atomic radius for Ca, K, As, Ge and Kr?
A) Ca > K > As > Ge > Kr
B) Kr > Ge > As > K > Ca
C) Ge > As > Kr > K > Ca
D) K > Ca > Ge > As > Kr
E) Kr > As > Ge > Ca > K
6) Which one of the following atoms has the largest radius?
A) O
B) F
C) S
D) Cl
E) Ne
7) 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
8) Of the choices below, which gives the order for first ionization energies?
A) Kr > Se > Br > Ga > Ge
B) Kr > Br > Se > Ge > Ga
C) Ga > Br > Ge > Kr > Se
D) Ga > Ge > Se > Br > Kr
E) Br > Se > Ga > Kr > Ge
9) ______have the lowest first ionization energies of the groups listed.
A) Alkali metals
B) Transition elements
C) Halogens
D) Alkaline earth metals
E) Noble gases
10) Which equation correctly represents the first ionization of phosphorus?
A) P (g) + e- → P- (g)
B) P (g) → P- (g) + e-
C) P (g) → P+ (g) + e-
D) P- (g) → P (g) + e-
E) P+ (g) + e- → P (g)
11) Which equation correctly represents the first ionization of calcium?
A) Ca (g) → Ca+ (g) + e-
B) Ca (g) → Ca- (g) + e-
C) Ca (g) + e- → Ca- (g)
D) Ca- (g) → Ca (g) + e-
E) Ca+ (g) + e- → Ca (g)
12) Which equation correctly represents the first ionization of copper?
A) Cu (g) → Cu+ (g) + e-
B) Cu (g) → Cu- (g) + e-
C) Cu (g) + e- → Cu- (g)
D) Cu- (g) → Cu (g) + e-
E) Cu+ (g) + e- → Cu (g)
13) Sodium is much more apt to exist as a cation than is chlorine. This is because ______.
A) chlorine is a gas and sodium is a solid
B) chlorine has a greater electron affinity than sodium does
C) chlorine is bigger than sodium
D) chlorine has a greater ionization energy than sodium does
E) chlorine is more metallic than sodium
14) Which equation correctly represents the electron affinity of calcium?
A) Ca (g) + e- → Ca- (g)
B) Ca (g) → Ca+ (g) + e-
C) Ca (g) → Ca- (g) + e-
D) Ca- (g) → Ca (g) + e-
E) Ca+ (g) + e- → Ca (g)
15) Which of the following correctly represents the electron affinity of bromine?
A) Br (g) → Br+ (g) + e-
B) Br (g) + e- → Br- (g)
C) Br2 (g) + e- → Br- (g)
D) Br2 (g) + 2 e- → 2 Br- (g)
E) Br+ (g) + e- → Br (g)
16) Which of the following correctly represents the electron affinity of phosphorus?
A) P (g) → P+ (g) + e-
B) P (g) + e- → P (g)
C) P4 (g) + e- → P (g)
D) P4 (g) + 4 e- → 4 P- (g)
E) P+ (g) + e- → P (g)
17) Of the elements below, ______is the most metallic.
A) sodium
B) barium
C) magnesium
D) calcium
E) cesium
18) Which one of the following is a metalloid?
A) Ge
B) S
C) Br
D) Pb
E) C
19) Which one of the following is a metal?
A) Ge
B) S
C) Br
D) Pb
E) C
20) The list that correctly indicates the order of metallic character is ______.
A) B > N > C
B) F > Cl > S
C) Si > P > S
D) P > S > Se
E) Na > K > Rb
21) The list that correctly indicates the order of metallic character is ______.
A) Sr > Ca > Mg
B) F > Cl > Br
C) C > Ge > Si
D) Li > Na > K
E) O > Se > S
22) The element in the periodic table that looks like a metal, is a poor thermal conductor, and acts as an electrical semiconductor is ______.
A) Sn
B) B
C) As
D) Si
E) Ge
23) Nonmetals can be ______at room temperature.
A) solid, liquid, or gas
B) solid or liquid
C) solid only
D) liquid only
E) liquid or gas
24) Which of the following is not a characteristic of metals?
A) acidic oxides
B) low ionization energies
C) malleability
D) ductility
E) These are all characteristics of metals.
25) Consider the general valence electron configuration of ns2np5 and the following statements:
(i) Elements with this electron configuration are expected to form -1 anions.
(ii) Elements with this electron configuration are expected to have large
positive electron affinities.
(iii) Elements with this electron configuration are nonmetals.
(iv) Elements with this electron configuration form acidic oxides.
Which statements are true?
A) (i) and (ii)
B) (i), (ii), and (iii)
C) (ii) and (iii)
D) (i), (iii,) and (iv)
E) All statements are true.
26) Which of the following traits characterizes the alkali metals?
A) very high melting point
B) existence as diatomic molecules
C) formation of dianions
D) the lowest first ionization energies in a period
E) the smallest atomic radius in a period
27) This element is more reactive than lithium and magnesium but less reactive than potassium. This element is ______.
A) Na
B) Rb
C) Ca
D) Be
E) Fr
28) Alkali metals tend to be more reactive than alkaline earth metals because ______.
A) alkali metals have lower densities
B) alkali metals have lower melting points
C) alkali metals have greater electron affinities
D) alkali metals have lower ionization energies
E) alkali metals are not more reactive than alkaline earth metals
29) All of the following are ionic compounds except ______.
A) K2O
B) Na2SO4
C) SiO2
D) Li3N
E) NaCl
Chapter 8 Basic Concepts of Chemical Bonding (part I)
1) The type of compound that is most likely to contain a covalent bond is ______.
A) one that is composed of a metal from the far left of the periodic table and a nonmetal from the far right of the periodic table
B) a solid metal
C) one that is composed of only nonmetals
D) held together by the electrostatic forces between oppositely charged ions
E) There is no general rule to predict covalency in bonds.
2) Of the atoms below, ______is the most electronegative.
A) Si
B) Cl
C) Rb
D) Ca
E) S
3) Of the molecules below, the bond in ______is the most polar.
A) HBr
B) HI
C) HCl
D) HF
E) H2
4) 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
5) The Lewis structure of N2H2 shows ______.
A) a nitrogen-nitrogen triple bond
B) a nitrogen-nitrogen single bond
C) each nitrogen has one nonbonding electron pair
D) each nitrogen has two nonbonding electron pairs
E) each hydrogen has one nonbonding electron pair
6) There are ______valence electrons in the Lewis structure of CH3CH2Cl.
A) 14
B) 12
C) 18
D) 20
E) 10
7) There are ______valence electrons in the Lewis structure of CH3OCH2CH3.
A) 18
B) 20
C) 26
D) 32
E) 36
8) In the Lewis symbol for a sulfur atom, there are ______paired and ______unpaired electrons.
A) 2, 2
B) 4, 2
C) 2, 4
D) 0, 6
E) 5, 1
9) The Lewis structure of the COH32- ion is ______.
A)
B)
C)
D)
E)
10) Resonance structures differ by ______.
A) number and placement of electrons
B) number of electrons only
C) placement of atoms only
D) number of atoms only
E) placement of electrons only
11) To convert from one resonance structure to another, ______.
A) only atoms can be moved
B) electrons and atoms can both be moved
C) only electrons can be moved
D) neither electrons nor atoms can be moved
E) electrons must be added
12) Which of the following does not have eight valence electrons?
A) Cl-
B) Xe
C) Ti+4
D) Rb+1
E) Sr+1
13) The central atom in ______does not violate the octet rule.
A) SF4
B) KrF2
C) CF4
D) XeF4
E) ICl4-
14) The central atom in ______violates the octet rule.
A) NH3
B) SeF2
C) BF3
D) AsF3
E) CF4
15) Which atom can accommodate an octet of electrons, but doesn't necessarily have to accommodate an octet?
A) N
B) C
C) H
D) O
E) B
16) Bond enthalpy is ______.
A) always positive
B) always negative
C) sometimes positive, sometimes negative
D) always zero
E) unpredictable
17) Given that the average bond energies for C-H and C-Br bonds are 413 and 276 kJ/mol, respectively, the heat of atomization of bromoform (CHBr3) is ______kJ/mol.
A) 1241
B) 689
C) -689
D) 1378
E) -1378
18) Of the bonds C–C, C=C, and C≡C, the C–C bond is ______.
A) strongest/shortest
B) strongest/longest
C) weakest/longest
D) weakest/shortest
E) intermediate in both strength and length
19) Of the bonds C–N, C=N, and C≡N, the C–N bond is ______.
A) strongest/shortest
B) strongest/longest
C) weakest/shortest
D) weakest/longest
E) intermediate in both strength and length
20) A double bond consists of ______pairs of electrons shared between two atoms.
A) 1
B) 2
C) 3
D) 4
E) 6
21) A triple bond consists of ______pairs of electrons shared between two atoms.
A) 1
B) 2
C) 3
D) 4
E) 6
22) In the molecule below, which atom has the largest partial negative charge?
Cl
|
F- C -Br
|
I
A) Cl
B) F
C) Br
D) I
E) C
23) The ability of an atom in a molecule to attract electrons is best quantified by the ______.
A) paramagnetism
B) diamagnetism
C) electronegativity
D) electron change-to-mass ratio
E) first ionization potential
24) Given the electronegativities below, which covalent single bond is most polar?
Element: H C N O
Electronegativity: 2.1 2.5 3.0 3.5
A) C-H
B) N-H
C) O-H
D) O-C
E) O-N
25) A nonpolar bond will form between two ______atoms of ______electronegativity.
A) different, opposite
B) identical, different
C) different, different
D) similar, different
E) identical, equal
26) The formal charge on nitrogen in NO3- is ______.
A) -1
B) 0
C) +1
D) +2
E) -2
27) 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
28) In the resonance form of ozone shown below, the formal charge on the central oxygen atom is ______.
A) 0
B) +1
C) -1
D) +2
E) -2
29) Using the table of average bond energies below, the ΔH for the reaction is ______kJ.
Bond: C≡C C–C H–I C–I C–H
D (kJ/mol): 839 348 299 240 413
A) +160
B) -160
C) -217
D) -63
E) +63
30) Using the table of average bond energies below, the ΔH for the reaction is ______kJ.
H–C≡C–H (g) + H–I (g) → H2C=CHI (g)
Bond: C≡C C=C H–I C–I C–H
D (kJ/mol): 839 614 299 240 413
A) +506
B) -931
C) -506
D) -129
E) +129
31) 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 O–H
D (kJ/mol): 358 799 1072 413 436 463
A) +276
B) -276
C) +735
D) -735
E) -116
Chapter 9 Molecular Geometry and Bonding Theories (Bonding Concepts II)
1) ClF3 has "T-shaped" geometry. There are ______non-bonding domains in this molecule.