21 what type of bonds will form between a mg and o atom? ionic or covalent. 11 22 draw the electron movement and lewis structure of the compound formed between mg and o. i use arrows for electron movement in ionic bonds and circles for covalent bonds. electron movement /2 lewis structure /1

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Accepted Answer

### Part 1: Bond Type (Ionic or Covalent)
# Brief Explanations:
Magnesium (Mg) is a metal, and Oxygen (O) is a non - metal. Ionic bonds typically form between metals and non - metals due to the transfer of electrons from the metal to the non - metal. Covalent bonds form between non - metals through electron sharing. So, the bond between Mg and O is ionic.
# Answer:
The bond formed between a Mg and O atom is an IONIC bond.

### Part 2: Electron Movement and Lewis Structure
# Brief Explanations:
1. **Electron Configuration and Transfer**: Magnesium has an electron configuration of $[Ne]3s^{2}$. It tends to lose its 2 valence electrons to achieve a stable noble - gas configuration (like Ne). Oxygen has an electron configuration of $[He]2s^{2}2p^{4}$ and needs 2 more electrons to achieve a stable octet (like Ne). So, Mg will transfer its 2 valence electrons to O.
2. **Lewis Structure Representation**:
   - For Mg: Initially, Mg has 2 valence electrons (represented as dots around the Mg symbol). After losing 2 electrons, it becomes $Mg^{2 + }$, so the Lewis structure for $Mg^{2+}$ has no valence electrons (since it lost them).
   - For O: Initially, O has 6 valence electrons. After gaining 2 electrons from Mg, it has 8 valence electrons (a stable octet) and becomes $O^{2 - }$. The Lewis structure for $O^{2 - }$ has 8 electrons (dots) around the O symbol, and we can represent the electron transfer with arrows: from the 2 valence electrons of Mg to the valence shell of O. The compound formed is MgO. The Lewis structure of MgO (ionic compound) can be represented as $[Mg]^{2+}[:\ddot{O}:]^{2 - }$, where the square brackets are used to show the ions, and the dots around O represent the 8 valence electrons (6 original + 2 gained from Mg). The electron movement is shown by arrows from Mg's valence electrons to O's valence shell.
# Answer:
- **Electron Movement**: Magnesium (Mg) loses its 2 valence electrons (shown with arrows pointing from Mg to O), and Oxygen (O) gains these 2 electrons.
- **Lewis Structure of MgO**: The Lewis structure is $[Mg]^{2+}[:\ddot{O}:]^{2 - }$, where $Mg^{2+}$ is the magnesium cation (with no valence electrons shown as it lost its 2 valence electrons) and $[:\ddot{O}:]^{2 - }$ is the oxide anion (with 8 valence electrons, 6 original and 2 gained from Mg).

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Question

Explanation:

Part 1: Bond Type (Ionic or Covalent)

Answer:

Part 2: Electron Movement and Lewis Structure