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homework: what type of bond is it? 1. calcium atom and an oxygen atom? …

Question

homework: what type of bond is it?

  1. calcium atom and an oxygen atom?
  2. copper atoms
  3. two oxygen atoms
  4. two nitrogen atoms
  5. magnesium and chlorine
  6. zinc atoms
  7. two nitrogen atoms
  8. potassium and chlorine
  9. copper atoms
  10. sodium and nitrogen
  11. fluorine atoms
  12. gold atoms
  13. iron and oxygen
  14. nickel and iodine
  15. nitrogen with nitrogen

Explanation:

Step1: Analyze Question 1 (Calcium and Oxygen)

Calcium is a metal (alkaline earth metal), Oxygen is a non - metal. Ionic bonds form between metals and non - metals due to transfer of electrons. Calcium (Ca) will lose 2 electrons to form \(Ca^{2+}\), Oxygen (O) will gain 2 electrons to form \(O^{2-}\). The electrostatic attraction between \(Ca^{2+}\) and \(O^{2-}\) forms an ionic bond.

Step2: Analyze Question 2 (Copper atoms)

Copper is a metal. In metals, atoms are held together by metallic bonds. Metallic bonds involve a sea of delocalized electrons surrounding positive metal ions. So copper atoms are held by metallic bonds.

Step3: Analyze Question 3 (Two Oxygen atoms)

Oxygen is a non - metal. Two non - metal atoms (same element here) share electrons. Each oxygen atom has 6 valence electrons. They share 2 electrons to form a double covalent bond (\(O = O\)) to achieve octet. So it's a covalent (non - polar) bond.

Step4: Analyze Question 4 (Two Nitrogen atoms)

Nitrogen is a non - metal. Each nitrogen atom has 5 valence electrons. They share 3 electrons (a triple covalent bond, \(N\equiv N\)) to achieve octet. So it's a covalent (non - polar) bond.

Step5: Analyze Question 5 (Magnesium and Chlorine)

Magnesium is a metal (alkaline earth metal), Chlorine is a non - metal (halogen). Magnesium loses 2 electrons to form \(Mg^{2+}\), each Chlorine atom gains 1 electron to form \(Cl^{-}\). The electrostatic attraction between \(Mg^{2+}\) and \(Cl^{-}\) (there will be two \(Cl^{-}\) for each \(Mg^{2+}\)) forms an ionic bond.

Step6: Analyze Question 6 (Zinc atoms)

Zinc is a metal. Metallic bonds hold zinc atoms together, with delocalized electrons in a sea around positive zinc ions.

Step7: Analyze Question 7 (Two Nitrogen atoms)

Same as question 4. Nitrogen atoms form a triple covalent bond (\(N\equiv N\)) by sharing 3 electrons each to achieve octet. So covalent (non - polar) bond.

Step8: Analyze Question 8 (Potassium and Chlorine)

Potassium is a metal (alkali metal), Chlorine is a non - metal (halogen). Potassium loses 1 electron to form \(K^{+}\), Chlorine gains 1 electron to form \(Cl^{-}\). The electrostatic attraction between \(K^{+}\) and \(Cl^{-}\) forms an ionic bond.

Step9: Analyze Question 9 (Copper atoms)

Copper is a metal, so metallic bonds hold copper atoms together (delocalized electrons and positive metal ions).

Step10: Analyze Question 10 (Sodium and Nitrogen)

Sodium is a metal (alkali metal), Nitrogen is a non - metal. Sodium loses 1 electron to form \(Na^{+}\), Nitrogen gains 3 electrons to form \(N^{3-}\). The electrostatic attraction between \(Na^{+}\) (three \(Na^{+}\) for each \(N^{3-}\)) forms an ionic bond.

Step11: Analyze Question 11 (Fluorine atoms)

Fluorine is a non - metal. Two fluorine atoms share 1 electron each (a single covalent bond, \(F - F\)) to achieve octet. So it's a covalent (non - polar) bond.

Step12: Analyze Question 12 (Gold atoms)

Gold is a metal. Metallic bonds hold gold atoms together, with delocalized electrons in a sea around positive gold ions.

Step13: Analyze Question 13 (Iron and Oxygen)

Iron is a metal, Oxygen is a non - metal. Iron can form ions (e.g., \(Fe^{2+}\), \(Fe^{3+}\)) and Oxygen forms \(O^{2-}\). The electrostatic attraction between iron ions and oxide ions forms an ionic bond (in compounds like \(FeO\), \(Fe_2O_3\) etc.).

Step14: Analyze Question 14 (Nickel and Iodine)

Nickel is a metal, Iodine is a non - metal. Nickel loses electrons (e.g., \(Ni^{2+}\) or \(Ni^{3+}\)), Iodine gains electrons (\(I^{-}\)). The electrostatic attraction between…

Answer:

s (for each question):

  1. Ionic Bond
  2. Metallic Bond
  3. Covalent (Non - Polar) Bond
  4. Covalent (Non - Polar) Bond (Triple)
  5. Ionic Bond
  6. Metallic Bond
  7. Covalent (Non - Polar) Bond (Triple)
  8. Ionic Bond
  9. Metallic Bond
  10. Ionic Bond
  11. Covalent (Non - Polar) Bond (Single)
  12. Metallic Bond
  13. Ionic Bond
  14. Ionic Bond
  15. Covalent (Non - Polar) Bond (Triple)