Question 1

In the gaseous phase,which of the following diatomic molecules would be the most polar?
A)CsF
B)CsCl
C)NaCl
D)NaF
E)LiF

Accepted Answer

A

Question 2

In which case is the bond polarity incorrect? A)(^$\delta$+H-F^$\delta$-) B)(^$\delta$+K-O^$\delta$-) C)(^$\delta$+Mg-H^$\delta$-) D)(^$\delta$+Cl-I^$\delta$-) E)(^$\delta$+Si-S^$\delta$-)

Accepted Answer

In option D, the bond polarity is incorrect because chlorine (Cl) is more electronegative than iodine (I), so the delta negative (δ-) should be on the chlorine atom, not on the iodine atom.

Question 3

A nonpolar covalent bond results from the unequal sharing of a pair of electrons between atoms in a molecule.

Accepted Answer

A nonpolar covalent bond results from the equal sharing of a pair of electrons between atoms in a molecule. Polar covalent bonds result from the unequal sharing of electrons.

Question 4

In which pair do both compounds exhibit predominantly ionic bonding? A)SCl₆ and HF B)Na₂SO₃ and NH₃ C)KI and O₃ D)LiF and H₂O E)LiBr and MgO

Accepted Answer

Ionic bonding occurs predominantly in compounds formed between metals and nonmetals, where there is a significant difference in electronegativity between the atoms, leading to the transfer of electrons. In option E, LiBr is composed of lithium (a metal) and bromine (a nonmetal), and MgO is composed of magnesium (a metal) and oxygen (a nonmetal), both of which exhibit predominantly ionic bonding due to the significant electronegativity differences and the transfer of electrons from the metal to the nonmetal.

Question 5

Which of the following groups contains no ionic compounds? A)HCN,NO₂,Ca(NO₃)₂ B)PCl₅,LiBr,Zn(OH)₂ C)KOH,CCl₄,SF₄ D)NaH,CaF₂,NaNH₂ E)CH₂O,H₂S,NH₃

Accepted Answer

All the compounds in choices A, B, C, and D contain at least one ionic compound. However, all the compounds in choice E are covalent compounds.

Question 6

The force between two bodies having identical electric charges
A)is a force of repulsion
B)is a force of repulsion if the charges are negative,and one of attraction if they are positive
C)increases as the bodies are moved further apart
D)is independent of the distance between them
E)is directly proportional to the distance between them

Accepted Answer

Like charges repel each other, so the force between two bodies having identical electric charges is a force of repulsion.

Question 7

For the elements Cs,F,and Cl,the order of increasing electronegativity is:
A)F < Cl < Cs
B)Cs < Cl < F
C)Cl < Cs < F
D)F < Cs < Cl
E)none of these

Accepted Answer

Electronegativity increases across a period from left to right and decreases down a group in the periodic table. Cesium (Cs) is a member of the alkali metals and is found in the bottom left corner of the periodic table, making it one of the least electronegative elements. Chlorine (Cl) and fluorine (F) are halogens, with fluorine being the most electronegative element in the periodic table. Therefore, the correct order of increasing electronegativity is Cs < Cl < F.

Question 8

What is the correct order of the following bonds in terms of decreasing polarity?
A)N-Cl,P-Cl,As-Cl
B)P-Cl,N-Cl,As-Cl
C)As-Cl,N-Cl,P-Cl
D)P-Cl,As-Cl,N-Cl
E)As-Cl,P-Cl,N-Cl

Accepted Answer

The answer of What is the correct order of the...

Question 9

Which of the following bonds is least polar?
A)C-O
B)H-C
C)S-Cl
D)Br-Br
E)They are all nonpolar.

Accepted Answer

The Br-Br bond is the least polar because both Br atoms have the same electronegativity value (2.8), so the electron pair is shared equally between them, resulting in a nonpolar covalent bond. The other bonds listed have different electronegativity values, resulting in varying degrees of polarity.

Question 10

When a metal reacts with a nonmetal a covalent bond is formed.

Accepted Answer

When a metal reacts with a nonmetal, an ionic bond is formed, not a covalent bond. Covalent bonds occur when two nonmetals bond together.

Question 11

Choose the compound with the most ionic bond.
A)LiCl
B)KF
C)NaCl
D)LiF
E)KCl

Accepted Answer

KF has the most ionic bond because the difference in electronegativity between potassium (K) and fluorine (F) is the greatest among the given options, leading to a more ionic character.

Question 12

Which of the following bonds would be the least polar,yet still be considered polar covalent?
A)Mg-O
B)C-O
C)O-O
D)Si-O
E)N-O

Accepted Answer

The answer of Which of the following bonds would be...

Question 13

Which of the following bonds would be the most polar without being considered ionic?
A)Mg-O
B)C-O
C)O-O
D)Si-O
E)N-O

Accepted Answer

The Si-O bond is highly polar due to the significant difference in electronegativity between silicon and oxygen, but it is not considered ionic.

Question 14

For the elements Cs,F,and P,the order of increasing electronegativity is:
A)Cs < F < P
B)Cs < P < F
C)P < F < Cs
D)F < Cs < P
E)none of these

Accepted Answer

Electronegativity increases as we move from left to right across a period and decreases as we move down a group. Cs is in Group 1 (alkali metals) and has the lowest electronegativity among the three elements. F is in Group 17 (halogens) and has the highest electronegativity among the three elements. P is in Group 15 and has a higher electronegativity than Cs but lower than F. Therefore, Cs < P < F in terms of increasing electronegativity.

Question 15

Metals typically have _______ electronegativity values.
A)high
B)low
C)negative
D)no
E)two of these

Accepted Answer

Metals usually have low electronegativity values because they tend to lose electrons rather than gain them in chemical reactions.

Question 16

Based on electronegativity differences,which of the following is most likely to be ionic? A)CaF₂ B)Br₂ C)BH₃ D)NO E)CF₄

Accepted Answer

Ionic bonds typically form between elements with large electronegativity differences. Ca has a relatively low electronegativity and F has a relatively high electronegativity, therefore CaF2 is most likely to be ionic.

Question 17

Atoms with greatly different electronegativity values are expected to form
A)no bonds
B)covalent bonds
C)triple bonds
D)ionic bonds
E)none of these

Accepted Answer

Atoms with greatly different electronegativity values (usually more than 1.7 difference) are expected to form ionic bonds, as one atom will donate an electron to the other to form a positively charged cation and a negatively charged anion, which are held together by electrostatic attraction. Covalent bonds are formed by atoms with similar electronegativity values sharing electrons, while triple bonds are a type of covalent bond characterized by sharing three pairs of electrons. Thus, the best choice is ionic bonds (D).

Question 18

The electron pair in a C-F bond could be considered
A)closer to C because carbon has a larger radius and thus exerts greater control over the shared electron pair
B)closer to F because fluorine has a higher electronegativity than carbon
C)closer to C because carbon has a lower electronegativity than fluorine
D)an inadequate model since the bond is ionic
E)centrally located directly between the C and F

Accepted Answer

Fluorine has a higher electronegativity than carbon, which means it attracts electrons towards itself more strongly. Therefore, the electrons in the C-F bond are closer to F.

Question 19

Atoms having equal or nearly equal electronegativities are expected to form
A)no bonds
B)polar covalent bonds
C)nonpolar covalent bonds
D)ionic bonds
E)covalent bonds

Accepted Answer

When atoms have equal or nearly equal electronegativities, they will share electrons equally, resulting in a nonpolar covalent bond. Polar covalent bonds occur when atoms have different electronegativities, and ionic bonds occur when electrons are transferred completely from one atom to another, resulting in ions with opposite charges attracting each other. No bonds and covalent bonds are too broad and do not accurately describe the behavior of atoms with nearly equal electronegativities.

Question 20

Based on electronegativities,which of the following would you expect to be most ionic? A)N₂ B)CaF₂ C)CO₂ D)CH₄ E)CF₄

Accepted Answer

To determine which compound is most ionic, we need to look at the difference in electronegativity between the two elements in each compound. The greater the difference, the more ionic the bond.
Using electronegativity values from the periodic table:
Ca = 1.00
F = 3.98
∆EN = |3.98 – 1.00| = 2.98
This is the greatest electronegativity difference among the options. Therefore, CaF2 is the most ionic compound.

Quiz 8: Bonding: General Concepts

In the gaseous phase,which of the following diatomic molecules would be the most polar?

In which case is the bond polarity incorrect?

A nonpolar covalent bond results from the unequal sharing of a pair of electrons between atoms in a molecule.

In which pair do both compounds exhibit predominantly ionic bonding?

Which of the following groups contains no ionic compounds?

The force between two bodies having identical electric charges

For the elements Cs,F,and Cl,the order of increasing electronegativity is:

What is the correct order of the following bonds in terms of decreasing polarity?

Which of the following bonds is least polar?

When a metal reacts with a nonmetal a covalent bond is formed.

Choose the compound with the most ionic bond.

Which of the following bonds would be the least polar,yet still be considered polar covalent?

Which of the following bonds would be the most polar without being considered ionic?

For the elements Cs,F,and P,the order of increasing electronegativity is:

Metals typically have _______ electronegativity values.

Based on electronegativity differences,which of the following is most likely to be ionic?

Atoms with greatly different electronegativity values are expected to form

The electron pair in a C-F bond could be considered

Atoms having equal or nearly equal electronegativities are expected to form

Based on electronegativities,which of the following would you expect to be most ionic?