Q: Which of the following best describes the bond dipole moment ($$\mu$$)?

$$\mu = q \times r$$, where $$q is $$the magnitude of partial charges and $$r is $$the bond distance.

Question 1

Which of the following statements best explains why sodium (Na) and chlorine (Cl) form an ionic compound?

Accepted Answer

Sodium loses an electron to achieve a filled valence shell, while chlorine gains an electron to achieve a filled valence shell, resulting in oppositely charged ions that attract each other.

Question 2

Which of the following ions is isoelectronic with argon ($$\mathrm{Ar}$$)?

Accepted Answer

$$\mathrm{K^+}$$

Question 3

What is the formal charge on the oxygen atom in the hydroxide ion ($$\mathrm{OH^-}$$)?

Accepted Answer

$$-1$$

Question 4

Which of the following molecules violates the octet rule by being electron deficient?

Accepted Answer

$$\mathrm{BF_3$}$$

Question 5

Which statement about resonance structures is correct?

Accepted Answer

The true structure of the molecule is a resonance hybrid, which is an average of all valid resonance forms.

Question 6

What is the electron pair geometry and molecular structure of ammonia ($$\mathrm{NH_3$}$$)?

Accepted Answer

Electron pair geometry: tetrahedral; Molecular structure: trigonal pyramidal

Question 7

Which of the following molecules is nonpolar despite having polar bonds?

Accepted Answer

$$\mathrm{CO_2$}$$

Question 8

What is the bond angle in a molecule with a trigonal planar geometry?

Accepted Answer

$$120^\circ$$

Question 9

Which of the following best describes the difference between pure covalent and polar covalent bonds?

Accepted Answer

Pure covalent bonds involve equal sharing of electrons, while polar covalent bonds involve unequal sharing due to differences in electronegativity.

Question 10

Which molecule is hypervalent?

Accepted Answer

$$\mathrm{SF_6$}$$

Question 11

What is the formal charge on the central nitrogen atom in the nitrate ion ($$\mathrm{NO_3$^-}) $$using the following formula: $$\mathrm{FC = \#VE - \#lone\ pair\ electrons - \frac{1}{2}(\#bonding\ electrons)}$$?

Accepted Answer

$$+1$$

Question 12

Which of the following statements about the VSEPR model is correct?

Accepted Answer

Electron pairs around a central atom arrange themselves as far apart as possible to minimize repulsion.

Question 13

Which of the following molecules has a bent molecular structure?

Accepted Answer

$$\mathrm{H_2O}$$

Question 14

A molecule has the formula $$\mathrm{AX_2E_2}. $$What is its molecular structure and approximate bond angle?

Accepted Answer

Bent; $$104.5^\circ$$

Question 15

Which of the following best explains why lone pairs cause deviations from ideal bond angles?

Accepted Answer

Lone pairs occupy more space than bonding pairs, pushing bonded atoms closer together and decreasing bond angles.

Question 16

Which molecule has a trigonal bipyramidal electron pair geometry?

Accepted Answer

$$\mathrm{PF_5$}$$

Question 17

Which of the following is true about molecular polarity?

Accepted Answer

A molecule is polar if it has at least one polar bond and an overall dipole moment.

Question 18

Which of the following best describes the bond dipole moment ($$\mu$$)?

Accepted Answer

$$\mu = q 	imes r$$, where $$q is $$the magnitude of partial charges and $$r is $$the bond distance.

Question 19

Which of the following molecules is expected to have the largest bond angle?

Accepted Answer

$$\mathrm{BF_3$}$$

Question 20

Which of the following is a correct step in drawing a Lewis structure for a polyatomic ion?

Accepted Answer

Add one electron for each negative charge to the total number of valence electrons.

Chemical Bonding and Molecular Geometry (Chapter 4 Study Notes)

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