Chem Test 3 Study Set

Choose the molecule that is incorrectly matched with the electronic geometry about the central atom. (a) CF4 - tetrahedral (b) BeBr2 - linear (c) H2O - tetrahedral (d) PF3 - pyramidal

(d) PF3-pyramidal

A (pi) bond is the result of the (a) overlap of two s orbitals. (b) overlap of an s and a p orbital. (c) overlap of two p orbitals along their axes. (d) sidewise overlap of two parallel p orbitals.

(d) sidewise overlap of two parallel p orbitals.

C-O bond length is minimum in (a) CO2 (b) CO32- (c) HCOO- (d) CO

(d)CO

Which of the molecules does not have a permanent dipole moment? (a) SO3 (b) SO2 (c) H2S (d) CS2

(d)CS2

Which of these elements is mostly to form ions with a 2+ charge? 1.Ca 2.P 3.O 4.Li

1. Ca

The effective nuclear charge is ____ for electrons in an atom that are _____ the nucleus. 1.Largest, closest to 2.Smallest, closest to 3.The same, anywhere with respect to 4.largest, away from

1. Largest, closest to

Which of these molecules has a Lewis structure with a central atom having no nonbonding electron pairs? 1.CO2 2.PF3 3.Both CO2 and H2S 4.H2S

1.CO2

As you go ______ in the periodic table, ______ decreases. 1.From bottom to top up a column, the charge of most common ion for each element 2.From left to right across a row, atomic size 3.More than one of a, b, c, d 4.From left to right across a row, radius of most common ion for each element

2. From left to right across a row, atomic size

Arrange these electrons in order of decreasing effective nuclear charge: a 1s electron in carbon, a 3s electron in silicon, a 3s electron in germanium, and a 1s electron in tin. 1.Sn 1s > Ge 3s > Si 3s > C 1s 2.Sn 1s > Ge 3s > C 1s > Si 3s 3.Ge 3s > Si 3s > Sn 1s > C 1s 4.C 1s > Si 3s > Ge 3s > Sn 1s

2. Sn 1s>Ge 3s> C 1s>Si 3s

What is the expected electron configuration of a Co3+ ion? 1.[Ar] 4s2 3d4 2.[Ar] 3d6 3.[Ar] 4s1 3d5 4.[Ar] 4s2 3d7

2. [Ar]3d6

Which of the following statements about multiple bonds is false? 1.The formation of multiple bonds allows atoms to satisfy the octet rule. 2.A triple bond involves the sharing of three electrons between the two atoms. 3.A double bond is shorter than a single bond. 4.A molecule can have more than one multiple bonds in it.

2.A triple bond involves the sharing of three electrons between the two atoms.

For how many of the following molecules is it not possible to write a Lewis Structure that Satisfies the octet rule: NH4+, NO, NO2, N2O? a) 2 b) 1 c) 3 d) 4

a) 2

Which process corresponds to the second ionization energy of generic element A? a) A+ (g)---> A^2+ (g) + e b) A (g) --->A^2+ (g) + 2e c) 2A (g) --->A2^2+ (g) + 2e d) A (g)---> A+ (g) + e

a) A+(g)--->A^2+ (g) + e

How many of the following molecules are hypervalent: PF3, PF5, XeF2, XeF4? a) 4 b) 3 c) 2 d) 1

b) 3

Which element has the highest first ionization energy? a) B b) C c) N d) O

b) C

A typical bond length is approximately how long? a) 1 x 10-6 m b) 1 x 10-12 m c) 1 x 10-10 m d) 1 x 10-8 m

c) 1 x10-10 m

Which one of the following violates the octet rule? (a) PCl3 (b) CBr4 (c) NF3 (d) AsF5

(d) AsF5

When an electron is added in valence shell then A) Energy is absorbed B) Energy is released C) Energy remains same D) Force of attraction increases

B) Energy is released

The molecular geometry of __________ is square planar. A) CCl4 B) XeF4 C) PH3 D) XeF2

B) XeF4

In order to produce sp3 hybrid orbitals, __________ s atomic orbital(s) and __________ p atomic orbital(s) must be mixed. A) one, two B) one, three C) one, one D) two, two

B) one, three

According to VSEPR theory, if there are five electron domains in the valence shell of an atom, they will be arranged in a(n) __________ geometry. A) octahedral B) trigonal bipyramidal C) tetrahedral D) trigonal planar

B) trigonal bipyramidal

The horizontal lines in the modern periodic table are called— A) Metal B) Group C) Period D) None of the above

C) Period

In counting the electron domains around the central atom in VSEPR theory, a __________ is not included. A) nonbonding pair of electrons B) single covalent bond C) core level electron pair D) double covalent bond

C) core level electron pair

The electron-domain geometry and the molecular geometry of a molecule of the general formula ABn are __________. A) never the same B) always the same C) sometimes the same D) not related

C) sometimes the same

The angles between sp2 orbitals are __________. A) 45° B) 180° C) 90° D) 120°

D) 120°

How many element groups are there? A) 7 B) 11 C) 16 D) 18

D) 18

According to valence bond theory, which orbitals on bromine atoms overlap in the formation of the bond in Br2? A) 3s B) 3p C) 4s D) 4p

D) 4p

There are __________ σ and __________ π bonds in the H2C=C=CH2 molecule. A) 4, 2 B) 6, 4 C) 2, 2 D) 6, 2

D) 6, 2

The basis of the VSEPR model of molecular bonding is __________. A) regions of electron density on an atom will organize themselves so as to maximize s-character B) regions of electron density in the valence shell of an atom will arrange themselves so as to maximize overlap C) atomic orbitals of the bonding atoms must overlap for a bond to form D) electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions

D) electron domains in the valence shell of an atom will arrange themselves so as to minimize repulsions

Which of the following pairs of molecules and their molecular geometries is WRONG? (a) NF3 - trigonal planar (b) H2O - bent (c) BF3 - trigonal planar (d) AsF5 - trigonal bipyramidal

(a) NF3 - trigonal planar

Select the term best describing the series of elements: Mn, Fe, Co, Ni, Cu. (a) d-transition metals (b) representative elements (c) metalloids (d) alkaline earth metals

(a) d-transition metals

Draw one of the resonance structures of SO3. The formal charge of S is (a) +2 (b) +1 (c) 0 (d) -1

(a)+2

Which molecule is nonpolar? (a) H2Se (b) BeH2 (c) PF3 (d) CHCl3

(b) BeH2

Find the molecule with the maximum dipole moment (a) CH4 (b) NH3 (c) CO2 (d) NF3

(b) NH3

Which one of the compounds below is most likely to be ionic? (a) GaAs (b) ScCl3 (c) NO2 (d) CCl4

(b) ScCl3

Which of these isoelectronic species has the smallest radius? (a) Br- (b) Sr2+ (c) Rb+ (d) Se2-

(b) Sr2+

The valence electrons of representative elements are (a) in s orbitals only. (b) located in the outermost occupied major energy level. (c) located closest to the nucleus. (d) located in d orbitals.

(b) located in the outermost occupied major energy level

What is the total number of electrons in the correct Lewis dot formula of the sulfite ion? (a) 8 (b) 24 (c) 26 (d) 30

(c) 26

The species that contains 24 protons, 26 neutrons and 22 electrons would be represented by the symbol: (a) 50V3+ (b) 26Cr2+ (c) 50Cr2+ (d) 50Mn2+

(c) 50Cr2+

Which molecule has a linear arrangement of all component atoms? (a) CH4 (b) H2O (c) CO2 (d) NH3

(c) CO2

Which element has the largest atomic radius? (a) Li (b) Na (c) Rb (d) F

(c) Rb

What hybridization is predicted for sulfur in the HSO3- ion? (a) sp (b) sp2 (c) sp3 (d) sp3d

(c) sp3

MX6 is a molecule with octahedral geometry. How many X - M - X bonds are at 180°? (a) four (b) two (c) three (d) six

(c) three

In the Lewis structure for the OF2 molecule, the number of lone pairs of electrons around the central oxygen atom is (a) 0 (b) 1 (c) 2 (d) 3

(c)2

Choose the species that is incorrectly matched with the electronic geometry about the central atom. (a) NO2- - trigonal planar (b) ClO4- - tetrahedral (c) SO32- - pyramidal (d) ClO3- - tetrahedral

(c)SO32- - pyramidal

The F-S-F bond angles in SF6 are ______. (a) 109o28' (b) 120o only (c) 90o and 120o (d) 90o and 180o

(d) 90o and 180o

Arrange following bonds in order of increasing polarity: B-Cl, P-S, Al-F, Br-Br 1.P-S < Br-Br < Al-F < B-Cl 2.Br-Br < P-S < B-Cl < Al-F 3.B-Cl < Br-Br < P-S < Al-F 4.Br-Br < P-S < Al-F < B-Cl

2.Br-Br < P-S < B-Cl < Al-F

The SO2 molecule, which has a central S atom bonded to two O atoms, has ___ equivalent resonance structures, and the two S-O bonds are _____. 1.One, different lengths 2.Two, the same length 3.One, the same length 4.Two, different length

2.Two, the same length

Which of these statements about first ionization energy is true? 1. Magnesium has a smaller first ionization energy than calcium. 2. The alkali metals have relatively large first ionization energies. 3. In comparing "early" (left of Fe/Ru/Os) transition metals to "late" (right of Fe/Ru/Os) transition metals, we would predict that the first ionization energy of the early transition metals is smaller than those of the late transition metals in the same period. 4.The noble gases have relatively low first ionization energies.

3. In comparing "early"(left of Fe/Ru/Os) transition metals to "late"(right of Fe/Ru/Os) transition. metals, we would predict that the first ionization energy of the early transition metals is smaller than those of the late transition metals in the same period.

Which of the following statements about ionic bonding is false? 1.The attraction between cations and anions increases as the charges on the ions increase. 2.Ionic bonds are found in compounds formed from metals combined with nonmetals. 3.The attraction between cations and anions increases as the radii of the ions increase. 4.Lattice energy is the energy needed to break an ionic compound into gaseous ions.

3. The attraction between cations and anions increases as the radii of the ions increase

As you go from left to right across a row in the periodic table, atomic size_____ and atomic number____. 1.Increases, decreases 2.Increases, increases 3.Decreases, increases 4.Decreases, decreases

3.Decreases, increases

Which of the following compounds has the largest lattice energy? 1.NaCl 2.RbCl 3.CaCl2 4.MgCl2

4. MgCl2

Which ionic compound consists of ions with the most extreme difference in ionic size? 1.NaF 2.KCl 3.RbBr 4.CsF

4.CsF

Which of the following ions has an electron configuration that differs from the others? 1.S^2- 2.Ca^2+ 3.K+ 4.Mg^2+

4.Mg^2+

The central iodine atom in IF5 has __________ unbonded electron pairs and __________ bonded electron pairs in its valence shell. A) 1, 5 B) 0, 5 C) 5, 1 D) 4, 1

A) 1, 5

Of the molecules below, only __________ is nonpolar. A) CO2 B) H2O C) NH3 D) HCl

A) CO2

What is the symbol for tin? A) Sn B) Se C) Sg D) Sr

A) Sn

As we go from left to right across period, electron affinity A) Increases B) Decreases C) Remains same D) None of above

A) increases

For a molecule with the formula AB2 the molecular shape is __________ A) linear or bent B) linear or trigonal planar C) linear or T-shaped D) T-shaped

A) linear or bent

The electron affinity for an element is written as _____, which is generally an ____ process. a) X(g) + e X-(g) , endothermic b) X(g) X+(g) + e, exothermic c) X(g) X+(g) + e, endothermic d) X(g) + e X-(g) , exothermic

d)X(g) + e ---> X-(g) , exothermic