Question 1:

The true statement for the formation of a covalent bond is:

C. Non-metal atoms share electrons with non-metal atoms.

Explanation:

• A is incorrect because metal atoms typically do not form covalent bonds; they usually form metallic bonds.
• B is incorrect as metal atoms transfer electrons to non-metal atoms in ionic bonding, not covalent bonding.
• C correctly describes covalent bonding, where non-metal atoms share electrons to achieve a full outer shell.
• D is also incorrect because non-metal atoms do not transfer electrons to metal atoms in covalent bonding; this describes ionic bonding.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 2:

A covalent bond is the electrostatic attraction between:

B. a shared pair of electrons and the positively charged nuclei.

Explanation:

• A describes metallic bonding, not covalent bonding.
• B correctly defines a covalent bond as the attraction between the shared electrons and the nuclei of the atoms involved.
• C refers to interactions between polar molecules, which do not define covalent bonds.
• D describes ionic bonding, which involves the attraction between oppositely charged ions.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 3:

The true statements in moving from S-O to S=O are:

B. I and III only.

Explanation:

• I. Bond strength increases: This is true because double bonds (S=O) are generally stronger than single bonds (S-O).
• II. Bond length increases: This is false; bond length decreases when moving from a single bond to a double bond.
• III. Number of shared electrons increases: This is true because a double bond involves the sharing of two pairs of electrons (four electrons total), compared to one pair in a single bond.

Thus, the correct answer is B. I and III only.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 4:

The true statement is:

B. C=C bonds are shorter than C-C bonds.

Explanation:

• A is false; C≡C bonds share more electron pairs (three pairs) than C=C bonds (two pairs).
• B is true; double bonds (C=C) are shorter than single bonds (C-C) due to increased electron density between the atoms.
• C is false; C=C bonds are generally nonpolar unless there are substituents that create polarity.
• D is false; C=C bonds require more energy to break than C-C bonds due to the increased number of shared electron pairs.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 5:

The species that contains a coordinate bond is:

C. CO (carbon monoxide).

Explanation:

• A. N₂ contains a triple bond (not a coordinate bond) formed by the sharing of electrons.
• B. NH₃ (ammonia) contains covalent bonds but no coordinate bonds.
• C. CO has a coordinate bond where the carbon atom donates a pair of electrons to the oxygen atom, forming a stable molecule.
• D. CO₂ contains double bonds between carbon and oxygen but no coordinate bonds.

Thus, the correct answer is C. CO.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 6:

The species that is trigonal planar in shape is:

C. BF₃.

Explanation:

• A. PH₃ has a trigonal pyramidal shape due to lone pair-bonding pair repulsion.
• B. CCl₄ is tetrahedral in shape because of the four bonding pairs around the central carbon atom.
• C. BF₃ is trigonal planar as it has three bonding pairs and no lone pairs on the boron atom, resulting in a flat, triangular shape.
• D. H₃O⁺ (hydronium ion) has a tetrahedral shape due to the four electron pairs (three bonding pairs and one lone pair).

Thus, the correct answer is C. BF₃.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 7:

The correct row for the NH^2- ion is:

D. tetrahedral (electron domain geometry) and bent V-shaped (molecular geometry).

Explanation:

• Electron Domain Geometry: NH₂⁻ has four electron domains (two bonding pairs and two lone pairs), which gives it a tetrahedral electron domain geometry.
• Molecular Geometry: The presence of two lone pairs causes the molecular geometry to be bent (or V-shaped).

Thus, the correct choice is D.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 8:

Let’s go through each option step by step.

A. The oxygen atom has 3 electron domains
In H₃O⁺, oxygen is bonded to 3 hydrogen atoms and has 1 lone pair.
Electron domains = bonding domains (3 O–H bonds) + 1 lone pair = 4 electron domains.
So this statement says “3 electron domains” — that’s false. It has 4.

B. It has a coordinate bond in its Lewis formula
Yes, one H⁺ (no electrons) bonded to O (in H₂O) by O donating both electrons — that’s a coordinate covalent bond.

C. It has a trigonal pyramidal shape
Yes, 4 electron domains with 1 lone pair → trigonal pyramidal, like NH₃.

D. The H–O–H bond angles are approximately 107°
Yes, close to NH₃ angle, slightly less than 109.5° due to lone pair-bond pair repulsion.

The NOT true statement is A.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 9:

I was unable to view the image you provided, but I can describe the correct Lewis (electron dot) formula for this molecule so you can identify the right option among the choices you see.

The correct Lewis structure must account for a total of 26 valence electrons and satisfy the octet rule for all atoms.

The correct structure will feature:

1. Central Atom: A Phosphorus (P) atom in the center.

2. Bonds: Three single bonds connecting the central P atom to the three Chlorine (Cl) atoms.

3. Lone Pairs on Cl: Each of the three Cl atoms must have three lone pairs of electrons (6 non-bonding electrons) to satisfy its octet.

4. Lone Pair on P: The central P atom must have one lone pair of electrons (2 non-bonding electrons) to satisfy its octet.

In summary, the correct Lewis structure for PCl₃ has a total of 3 bonding pairs and 10 lone pairs (1 on P and 3 on each Cl).

*This description corresponds to image D
The Silverback

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.

Question 10:

The number of electron domains on the carbon atom in carbon dioxide (CO₂) is:

A. 2.

Explanation:

• In CO₂, the carbon atom forms two double bonds with two oxygen atoms. Each double bond counts as one electron domain. Therefore, there are two electron domains around the carbon atom.

*These A.I. responses have been individually checked to ensure they match the accepted answer, but explanations may still be incorrect. Responses may give guidance but the A.I. might not be able to answer the question! This is particularly the case for questions based on diagrams, which the A.I. typically cannot interpret.
Grade Gorilla uses Gemini, Deepseek and a range of other A.I. chatbots to generate the saved responses. Some answers have had human intervention for clarity or where the A.I. has not been able to answer the question.