Question 1

Which of the following best describes the nature of the bonding in sodium chloride (NaCl), as illustrated in the first image?

Accepted Answer

A lattice of ions held together by electrostatic attractions

Question 2

When lithium reacts with fluorine to form lithium fluoride (LiF), what happens to the sizes of the lithium and fluorine atoms, as shown in the second image?

Accepted Answer

Lithium becomes smaller and fluorine becomes larger

Question 3

Based on the third image, which compound has the highest percent ionic character and why?

Accepted Answer

LiF, because it has the highest electronegativity difference

Question 4

Referencing Table 9.3, which property distinguishes ionic compounds from covalent compounds at room temperature?

Accepted Answer

Ionic compounds have high melting points and are solids at room temperature

Question 5

The fifth image shows a molecular geometry with bond angles of 109.5°. What is the name of this geometry and which hybridization corresponds to it?

Accepted Answer

Tetrahedral, sp3 hybridization

Question 6

Which of the following statements about the structure of NaCl, as shown in the first and sixth images, is correct?

Accepted Answer

NaCl forms a three-dimensional lattice of Na+ and Cl- ions

Question 7

The seventh image shows two representations of a tetrahedral molecule. Which molecule is most likely to have this geometry?

Accepted Answer

CH4

Question 8

The eighth image shows three different orbital arrangements. Which hybridization is represented by the middle diagram?

Accepted Answer

sp2 hybridization

Question 9

The ninth image shows the water molecule with a bond angle of 105°. What is the main reason for this bond angle being less than 109.5°?

Accepted Answer

The presence of two lone pairs on the oxygen atom

Question 10

The tenth image shows a simplified model of the water molecule. Which statement best describes the polarity of water?

Accepted Answer

Water is polar because the oxygen atom is more electronegative than hydrogen and the molecule is bent

Question 11

The eleventh image shows a section of the periodic table. Which elements are most likely to obey the octet rule in stable compounds?

Accepted Answer

Elements in the second period: C, N, O, and F

Question 12

The twelfth image shows the Lewis structure for ClF3. What is the repulsion number (number of regions of high electron density) around the central atom?

Accepted Answer

$$	ext{R.N.} = 5$$

Question 13

The thirteenth image shows the Lewis structure for SCl4. Which statement about the central atom is correct?

Accepted Answer

Sulfur has an expanded octet with five regions of electron density

Question 14

The fourteenth image shows the Lewis structure for XeF2. What is the molecular geometry of XeF2 according to the VSEPR model?

Accepted Answer

Linear

Question 15

The fifteenth image shows an electrostatic potential map for ozone (O3). What does this map indicate about the distribution of electron density?

Accepted Answer

Electron density is evenly distributed between the two peripheral oxygen atoms

Question 16

The sixteenth image shows a tetrahedral geometry. Which hybrid orbitals are used by the central atom to achieve this geometry?

Accepted Answer

$$	ext{sp}^3$$ hybrid orbitals

Question 17

The seventeenth image shows three different orbital arrangements. Which hybridization is represented by the leftmost diagram?

Accepted Answer

$$	ext{sp}$$ hybridization

Question 18

The eighteenth image shows two molecules with their dipole moments. Which molecule is more polar and why?

Accepted Answer

The molecule on the left is more polar because its dipole moments reinforce each other

Question 19

The nineteenth image shows a linear molecule with a colored electrostatic potential map. Which molecule is most likely represented, and what is its polarity?

Accepted Answer

CO2, which is non-polar due to its symmetry

Chemical Bonding: Ionic and Covalent Bonds, Lewis Structures, VSEPR, Resonance, and Hybridization

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