Skip over navigation

Contents

Review of Chemical Bonding

Review Test

Table of Contents

Further Reading

Which of the following has the longest bond?

Which of the following is the shortest bond?

Which of the following bonds is the longest?

Which of the following is the strongest bond?

Which of the following is the strongest covalent bond?

Which of the following is the weakest ionic bond?

Which of the following has the smallest bond dipole?

Which of the following molecules has a net dipole?

What is the relationship between bond dipole and bond strength?

What is electronegativity?

What type of bond is formed when a highly electronegative element and an electropositive element form a bond?

Which of the following atoms has the highest electronegativity?

Which of the following is the largest?

Why do ionic compounds form crystal lattices instead of isolated molecules?

Which of the following has a noble gas configuration?

Why does MgO exist as Mg2+ O2- not Mg+ O- ?

Predict the formula of lithium nitride.

Predict the formula of magnesium argonide.

Why do atoms share their electrons?

If two atoms are bonded together, one with six valence electrons, the other with four, how many electrons must they share for both to achieve a full octet?

Why does sharing an electron pair between nuclei create a bond?

How many resonance structures are possible for SO3 2-?

How much charge resides on each oxygen in SO3 2-?

Which of the following molecules has more than one resonance structure?

What is the formal charge on boron in BF4 -?

Lewis structures with less formal charge are more stable. Given this statement, determine which structure is more stable, the octet or non-octet structure of BCl3. (Hint: the octet structure places a double bond between the B and a Cl atom.)

What is the formal charge on each hydrogen in CH3 +?

What is the formal charge on a triply-bonded oxygen?

How many lone pairs are present in the Lewis structure for NF3?

Explain why the Lewis structure for SF6 has twelve electrons around sulfur instead of eight.

How many lone pairs are present on iodine in IF4 -

Which of the following is a correct explanation of why it is difficult to draw the Lewis structure for NO.

How many different types of oxygen atoms are present in the molecule CH2OHCO2 -?

What is the molecular geometry of oxygen in H3O+?

Why is it reasonable for VSEPR to assume that electron pairs are oriented as far away as possible from one another?

What is the molecular geometry of I3 -?

Which has a smaller bond angle between oxygen atoms, SO3 2- or CO3 2-?

Which of the following ions produces unreasonable Lewis structures?

How many different types of bonding overlap are possible for a homonuclear diatomic molecule like W2 when only considering bonding through the p orbitals?

What property of B2 would change if the energy of its p bonds were raised above its s bond formed from the overlap of its 2p orbitals?

The Lewis structure of NO is difficult to draw due to its odd number of electrons. Use molecular orbital theory to predict which atom has the odd electron.

Light can be used to excite electrons enough to remove an electron from a molecule. When light of an appropriate frequency is shined on oxygen, the O-O bond becomes stronger despite the loss of an electron. Explain.

Is molecular nitrogen paramagnetic or diamagnetic? Why?

How does the molecular orbital diagram for LiF account for the fact that LiF is an ionic compound?

What determines the heights of the orbitals for each single atom in a correlation diagram?

Which atom's 2s orbital would be lower on the orbital correlation diagram, B or C?

What is the hybridization of oxygen in CH2OH+?

What is the hybridization of the central nitrogen in N2O?

Which of the following statements contrasts hybridization and molecular orbital theory for polyatomic molecules?

Photoelectron spectroscopy can be used to determine the energy levels in molecules. The photoelectron spectrum for silane reveals two different low energy peaks indicating the two distinct energy levels for the bonded electrons. Which of the following bonding descriptions is not consistent with the experimental results?

Follow Us