Deck 7: Chemical Bonding and Molecular Structure

Question 1

Alkali metals tend to form cations that are smaller than the neutral metal atom.

Answer 1

True

Question 2

Which of the following electron configurations belongs to an atom that is most likely to be involved in an ionic bond?

A) 1s²2s²2p⁶3s²
B) 1s²2s²2p⁶
C) 1s²2s²2p⁶3s²3p³
D) 1s²2s²2p⁶3s²3p⁶

Answer 2

1s²2s²2p⁶3s²

Question 3

Halogens tend to form anions that are larger than the neutral atom.

Answer 3

True

Question 4

In a pi bond the overlap of s-orbitals is responsible for the formation of the pi-bond..

Question 5

The bond angles of a tetrahedron are 120 degrees.

Question 6

The valence shell electron pair repulsion (VSEPR) theory states that molecules assume a shape that minimizes the repulsion between electron pairs and bonded atoms in the valence shell of the central atom.

Question 7

In resonance structures, the positions of all electrons are identical; only the positions of the atoms are different.

Question 8

An ionic bond is formed by the electrostatic attraction of oppositely charged ions.

Question 9

CFCs are destructive because they undergo photo-catalyzed reactions that destroy O₂.

Question 10

Of the following substances which is most reactive?

A) SiO₂
B) Sr(NO₃)₂
C) Cl₂
D) glucose

Question 11

The attraction of an atom for the electrons in a covalent bond is referred to as ionization energy.

Question 12

Which of the following electron configurations belongs to an atom that is most likely to be involved in a covalent bond?

A) 1s²2s²2p⁶3s²
B) 1s²2s²2p⁶
C) 1s²2s²2p⁶3s²3p³
D) 1s²2s²2p⁶3s²3p⁶

Question 13

Which of the following atoms is likely to be involved in an ionic bond?

A) He
B) Na
C) Si
D) P

Question 14

Which of the following atoms is likely to be involved in a covalent bond?

A) Sr
B) K
C) C
D) Ca

Question 15

Large jumps in ionization energy tend to occur whenever the removal of that electron disrupts an electron configuration ending in:

A) ns²
B) ns¹
C) np⁶
D) np⁴

Question 16

In order to achieve an electron configuration that is isoelectric with a noble gas, non-metals tend to:

A) gain electrons
B) lose electrons
C) form stable free radicals
D) both gain electrons and form stable free radicals

Question 17

The rubidium cation has a correct charge of:

A) 3+
B) 2+
C) 1 −
D) 1+

Question 18

Widely separated atoms do not interact, but will reach an optimal separation distance called the bond distance and form a bond.

Question 19

Which of the following is the correct charge for a bromine anion?

A) 1+
B) 1 −
C) 0
D) 2 −

Question 20

The aluminum cation has a correct charge of:

A) 3+
B) 2+
C) 1 −
D) 1+

Question 21

What is the correct electron configuration of the calcium cation?

A) 1s²2s²2p⁶3s²3p⁶4s¹
B) 1s²2s²2p⁶3s¹3p⁶4s²
C) 1s²2s²2p⁶3s²3p⁶
D) 1s²2s²2p⁶3s²3p⁶3d¹⁰

Question 22

Which of the following molecules is non-polar?

A) KI
B) C₂H₆
C) Ce(NO₃)₃
D) H₂O

Question 23

Consider the formation of ammonia. Using VSEPR, which molecule shape best describes the shape of the molecule?

A) octahedral
B) square planar
C) trigonal planar
D) trigonal pyramidal

Question 24

In assembling a Lewis Dot diagram of NO₃ ⁻ , there are ____ total electrons to use in the model.

A) 23
B) 24
C) 27
D) 20

Question 25

Which of the following has the largest radius?

A) I ⁻
B) Br
C) Cl ⁻
D) F

Question 26

Which of the following compounds illustrates sp³ hybridization?

A) C₂H₄
B) CH₄
C) C₂H₂
D) V₂O₅

Question 27

The correct symbol for chloride is:

A) Cl ⁻
B) Cl₂
C) Cl₂^{2 −}
D) Cl₂ ⁻

Question 28

Which of the following has the largest ionic radius?

A) Al³⁺
B) I ⁻
C) S
D) K⁺

Question 29

Which hybridization best characterizes the C atom involved in a CH₄ molecule?

A) sp
B) sp²
C) sp³
D) sp⁴

Question 30

If the combined radii of each pair is assumed equal, which pair of atoms releases the most energy during formation of an ion pair?

A) Na and Br
B) Al and S
C) Rb and F
D) K and O

Question 31

Which of the following has the largest radius?

A) Na
B) K⁺
C) Rb
D) Cs⁺

Question 32

Covalent bonds involve:

A) mostly alkali metal-halide interactions
B) the transport of electrons from one atom to another
C) a cationic re-arrangement of atoms
D) a significant electron density between two nuclei

Question 33

The preferred oxidation state of Ca²⁺ is described by which electron configuration:

A) 1s²2s²2p⁶3s²3p⁶
B) 1s²2s²2p⁶3s²3p⁶4s²
C) 1s²2s²2p⁶3s²3p⁶3d¹⁰
D) 1s²2s²2p⁶

Question 34

Coulomb's Law states that as the charge on the cation and anion decreases, the force (and potential energy) of the system:

A) increases
B) decreases
C) remains the same
D) becomes quantum mechanically unstable

Question 35

What is the molecular geometry of PCl₃

A) trigonal pyramidal
B) see-saw
C) tetrahedral
D) T-shape

Question 36

Multiple bonding results from the sharing of more than one electron pair. An example of this phenomenon is the double bond. In this case, the second bond is characterized as:

A) a second single bond
B) a plasmodic state
C) a sigma bond
D) a pi bond

Question 37

Which of the following molecules is most polar?

A) NaCl
B) C₂H₆
C) HF
D) H₂O

Question 38

The assignment of electrons in Lewis Dot diagrams is limited to:

A) all electrons
B) valence electrons
C) the "d" sub-orbital
D) only those in the first group

Question 39

Draw the Lewis Dot diagram of nitrate. How many resonance states are possible?

A) 3
B) 2
C) 1
D) 0

Question 40

Consider the formation of SF₆. Using VSEPR, which molecule shape best describes the shape of the molecule?

A) octahedral
B) square planar
C) square pyramidal
D) tetrahedral