Question 1:

The correct answer is:

C. transfer of electrons from metal to non-metal atoms

Here's why:

• Ionic bonding occurs when electrons are transferred from one atom to another (not shared).

• Metals tend to lose electrons (forming positive ions, or cations).

• Non-metals tend to gain electrons (forming negative ions, or anions).

• The electrostatic attraction between the oppositely charged ions forms the ionic bond.

So the transfer is from metal to non-metal.

Quick distinction:

• Covalent bonding = sharing of electrons between non-metal atoms (option B).

• Option A is incorrect because metals do not share electrons with each other in ionic bonding (they form metallic bonds instead).

• Option D is incorrect because electrons are transferred from the metal to the non-metal, not the other way around.

*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:

The correct answer is:

B. sharing of electrons between non-metal atoms

Here's why:

• Covalent bonding occurs when atoms share pairs of electrons to achieve a full outer shell (stable electron configuration).

• This type of bonding typically happens between non-metal atoms (e.g., H₂, O₂, H₂O, CH₄).

Quick recap of the other options:

• A is incorrect — metal atoms usually form metallic bonds (sharing delocalized electrons) or ionic bonds with non-metals, not covalent bonds.

• C and D describe ionic bonding (transfer of electrons between metals and non-metals), not covalent 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 3:

The correct answer is:

A. loses one electron and forms a positive ion with a 1+ charge

Here's why:

• Sodium (Na) is a metal in Group 1 of the periodic table. It has 1 electron in its outermost shell.

• To achieve a stable noble gas configuration (like neon), it is easier for sodium to lose that 1 electron than to gain 7.

• Losing a negatively charged electron leaves the sodium atom with more protons than electrons, giving it a positive charge of 1+ (Na⁺).

• This is the basis of ionic bonding — sodium transfers its outer electron to oxygen (a non-metal), forming sodium oxide (Na₂O).

Quick elimination of others:

• B is wrong because losing an electron creates a positive ion, not a negative one.

• C is wrong because sodium loses (not gains) an electron, and gaining would make it negative, not positive.

• D is wrong for both reasons — sodium loses, not gains, and forms a positive ion.

*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 correct answer is:

C. gains two electrons

Here's why:

• Oxygen (O) is a non-metal in Group 6 of the periodic table. It has 6 electrons in its outermost shell.

• To achieve a stable noble gas configuration (like neon), oxygen needs to gain 2 electrons to complete its outer shell (8 electrons total).

• Gaining 2 negatively charged electrons gives the oxygen atom a 2– charge (O²⁻), forming an oxide ion.

• In the reaction with sodium, each oxygen atom gains 2 electrons from sodium atoms (two sodium atoms each lose 1 electron to form Na⁺, and one oxygen atom gains both to form O²⁻), resulting in sodium oxide (Na₂O).

*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 correct answer is:

C. chlorine atom shares one pair of electrons with the hydrogen atom

Here's why:

• Hydrogen (H) is a non-metal, and chlorine (Cl) is also a non-metal.

• When two non-metals bond, they form a covalent bond by sharing electrons (not transferring them).

• Hydrogen has 1 electron in its outer shell and needs 1 more to achieve a full shell (like helium).
  Chlorine has 7 electrons in its outer shell and needs 1 more to achieve a full shell (like argon).

• Therefore, they share one pair of electrons (one from hydrogen and one from chlorine) to form a single covalent bond, creating the molecule HCl (hydrogen chloride).

Quick elimination:

• A and B describe ionic bonding (transfer of electrons), which happens between a metal and a non-metal. Both H and Cl are non-metals, so this does not apply.

• D is wrong because a single covalent bond involves one shared pair of electrons, not two. Two pairs would be a double bond (e.g., O₂), which is not the case here.

*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:

Electron Transfer:

Magnesium (Mg) is a metal with 2 outer electrons. Fluorine (F) is a non-metal with 7 outer electrons.

- Magnesium Ion: Mg loses its 2 outer valence electrons to achieve a stable full inner shell. This forms an Mg²⁺ ion with 0 outer valence electrons.

- Fluoride Ions: Each of the 2 electrons lost by Mg is transferred to a different F atom. Each F atom gains 1 electron to complete its octet, forming two F⁻ ions.

- Ratio: The chemical formula is MgF₂, meaning one Mg²⁺ ion bonds with two F⁻ ions, as shown accurately in option B.

*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 option is D.

Explanation:

- Bonding Type: Water (H₂O) is a covalent compound formed by non-metals sharing electrons, not an ionic compound with charges. This rules out A and B.

- Chemical Formula: A water molecule consists of two hydrogen atoms bonded to one oxygen atom (H-O-H). Option C only shows one hydrogen atom.

- Electron Sharing: In option D, each hydrogen atom shares one electron (represented by a cross ×) with the oxygen atom, which shares one of its electrons (represented by a dot •).

- Full Shells: This single covalent bond completes the outer shell of both hydrogen atoms (2 electrons) and the oxygen atom (8 electrons, including 4 unbonded lone pair electrons).

*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:

The correct answer is:

D. sulfur changes from 2,8,6 to 2,8,8 and an S²⁻ ion forms

Here's why:

• Magnesium (Mg) is a metal in Group 2. Its electronic configuration is 2,8,2. To achieve a stable noble gas configuration (like neon, 2,8), it loses 2 electrons and forms an Mg²⁺ ion (not Mg⁺). So options A and B are incorrect because:

  • A says Mg⁺ (wrong charge) and the configuration after losing electrons should be 2,8 (not 2,8).

  • B says Mg²⁺ but gives the wrong configuration (2,8,1) — after losing 2 electrons, it should be 2,8.

• Sulfur (S) is a non-metal in Group 6. Its electronic configuration is 2,8,6. To achieve a stable noble gas configuration (like argon, 2,8,8), it gains 2 electrons and forms an S²⁻ ion. This is exactly what option D states.

Overall reaction:
Mg loses 2 electrons → Mg²⁺
S gains 2 electrons → S²⁻
They form an ionic compound, MgS (magnesium sulfide).

Correct answer: 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 9:

The correct answer is:

B. sharing three pairs of electrons

Here's why:

• Nitrogen (N) is a non-metal, so it forms covalent bonds by sharing electrons (not transferring them). This rules out option A.

• Each nitrogen atom has 5 electrons in its outer shell (electronic configuration 2,5) and needs 3 more to achieve a stable noble gas configuration (like neon, 2,8).

• To achieve this, the two nitrogen atoms share three pairs of electrons (one pair from each atom for each bond), forming a triple covalent bond (N≡N).

*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 correct dot-and-cross diagram representing the bonding in a carbon dioxide (CO₂) molecule is B.

Key Rules for Covalent Bonding:

- Covalent Sharing: Carbon dioxide is a covalent molecule formed by sharing electrons between non-metal atoms.

- Valence Electrons: A neutral carbon (C) atom has 4 valence electrons. A neutral oxygen (O) atom has 6 valence electrons.

- The Octet Rule: Every atom aims to have 8 electrons in its outer shell to become stable.

Step-by-Step Breakdown:

- Carbon Needs 4 Electrons: Since carbon has 4 outer electrons, it must share 4 more to reach a full octet of 8.

- Oxygen Needs 2 Electrons: Each oxygen atom has 6 outer electrons, so each needs to share 2 more to reach 8.

Forming Double Bonds:

- Carbon shares 2 of its electrons with the left oxygen atom, and that oxygen shares 2 back. This forms a double covalent bond (4 shared electrons in total in the left intersection: 2 dots and 2 crosses).

- Carbon shares its remaining 2 electrons with the right oxygen atom, and that oxygen shares 2 back. This forms another double covalent bond (4 shared electrons in total in the right intersection: 2 dots and 2 crosses).

- Unshared Electrons (Lone Pairs): Each oxygen atom keeps 4 unshared electrons (2 pairs) on its outer side. Carbon has shared all 4 of its original valence electrons, leaving none unshared on the carbon atom itself.

*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.