Q: What is the correct formula to calculate the formal charge on an atom in a Lewis structure?

$$\text{Formal charge} = (\text{number of valence electrons}) - [(\text{number of nonbonding electrons}) + (1/2 \times \text{number of bonding electrons})]$$

Question 1

Which of the following best describes the type of bonding and electron behavior in a compound formed between sodium (Na) and chlorine (Cl)?

Accepted Answer

Ionic bonding; electrons are transferred from sodium to chlorine.

Question 2

Which of the following molecules will align with an external electric field due to its molecular properties?

Accepted Answer

HF

Question 3

Given the Lewis structure for OCl$$_2$$, which of the following is the best representation?

Accepted Answer

O is the central atom, with two single bonds to Cl atoms and two lone pairs on O.

Question 4

Which of the following statements about electronegativity trends in the periodic table is correct?

Accepted Answer

Electronegativity decreases down a group and increases across a period.

Question 5

Which bond type is expected for a molecule with an electronegativity difference ($$\Delta EN) of 1.0$$?

Accepted Answer

Polar covalent

Question 6

Which molecule below is expected to have the largest dipole moment?

Accepted Answer

LiF

Question 7

Which of the following best explains why the HCl molecule is polar?

Accepted Answer

The bond is polar because Cl is more electronegative than H, creating a dipole.

Question 8

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

Accepted Answer

CO$$_2$$

Question 9

What is the correct formula to calculate the formal charge on an atom in a Lewis structure?

Accepted Answer

$$	ext{Formal charge} = (	ext{number of valence electrons}) - [(	ext{number of nonbonding electrons}) + (1/2 	imes 	ext{number of bonding electrons})]$$

Question 10

Which of the following molecules is an example of a free radical?

Accepted Answer

ClO

Question 11

Which of the following molecules can have an expanded octet?

Accepted Answer

H$$_3PO$_4$$

Question 12

Which of the following bonds is the shortest?

Accepted Answer

Triple covalent bond

Question 13

Which of the following best describes the molecular geometry of NO$$_3^- ($$nitrate ion)?

Accepted Answer

Trigonal planar

Question 14

What is the bond angle in a molecule with tetrahedral electron geometry?

Accepted Answer

$$109.5^\circ$$

Question 15

Which of the following best describes the effect of lone pairs on bond angles in a molecule?

Accepted Answer

Lone pairs decrease bond angles due to increased repulsion.

Question 16

Which of the following is the correct order of increasing electronegativity for the elements P, Na, N, Al?

Accepted Answer

Na \u003c Al \u003c P \u003c N

Question 17

Which of the following best describes the molecular geometry and bond angle of ICl$$_4^-$$?

Accepted Answer

Square planar, $$90^\circ$$

Question 18

Which of the following statements about molecular polarity is correct?

Accepted Answer

A molecule is nonpolar if the vector sum of its bond dipoles is zero.

Question 19

Which of the following best describes the bond type and example for a $$\Delta EN of 2.1$$?

Accepted Answer

Ionic; NaCl

Question 20

Which of the following is the correct formula for calculating the dipole moment ($$\mu) of a $$bond?

Accepted Answer

$$\mu = q 	imes r$$

Chemical Bonding I: Bond Types, Polarity, and Electronegativity

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