6. what was your charge after you gained/lost electrons? why?

7. what kind of atom did you
eact\ with? explain what happened!

8. draw the electron dot diagram for your ion. an example of the electron dot diagrams for the calcium and chloride ions is shown below:

image of electron dot diagram for calcium and chloride ions

9. why do metals form chemical bonds with nonmetals?

Question

6. what was your charge after you gained/lost electrons? why?

7. what kind of atom did you
eact\ with? explain what happened!

8. draw the electron dot diagram for your ion. an example of the electron dot diagrams for the calcium and chloride ions is shown below:

image of electron dot diagram for calcium and chloride ions

9. why do metals form chemical bonds with nonmetals?

Accepted Answer

### Question 6
# Brief Explanations:
If an atom loses electrons, it has more protons (positive charge) than electrons (negative charge), so it becomes positively charged (cation). If it gains electrons, it has more electrons than protons, so it becomes negatively charged (anion). For example, a sodium atom (Na) has 11 protons and 11 electrons. If it loses 1 electron, it has 11 protons and 10 electrons, so its charge is $ +1 $ (since $ 11 - 10 = +1 $). The reason is that electrons have a negative charge, so losing them reduces the negative charge, making the overall charge positive, and gaining them increases the negative charge, making the overall charge negative.
# Answer:
If I lost electrons, my charge was positive (cation) because I had more protons than electrons. If I gained electrons, my charge was negative (anion) because I had more electrons than protons. (The specific charge depends on the number of electrons gained or lost. For example, losing 1 electron gives a $ +1 $ charge, losing 2 gives $ +2 $, gaining 1 gives $ -1 $, etc.)

### Question 7
# Brief Explanations:
Typically, metals (like Na, Mg, Ca) react with non - metals (like Cl, O, S). For example, in the case of sodium (Na, a metal) and chlorine (Cl, a non - metal), sodium has 1 valence electron and chlorine has 7 valence electrons. Sodium loses its 1 valence electron to achieve a stable octet (like the noble gas Ne), and chlorine gains that 1 electron to achieve a stable octet (like the noble gas Ar). The transfer of electrons forms ions ( $ \text{Na}^+ $ and $ \text{Cl}^- $) which are then attracted to each other by electrostatic forces, forming an ionic bond.
# Answer:
I likely reacted with a non - metal atom (if I was a metal) or a metal atom (if I was a non - metal). For example, if I was a metal like calcium (Ca), I would react with a non - metal like chlorine (Cl). Calcium has 2 valence electrons. It loses these 2 electrons to achieve a stable electron configuration (like Ar). Chlorine atoms (each with 7 valence electrons) gain 1 electron each. So one calcium atom can react with two chlorine atoms: $ \text{Ca} $ loses 2 electrons (becomes $ \text{Ca}^{2+} $) and each $ \text{Cl} $ gains 1 electron (becomes $ \text{Cl}^- $), and the ions are held together by ionic bonds.

### Question 8
# Brief Explanations:
Let's assume we have a sodium ion ($ \text{Na}^+ $) as an example. A sodium atom has 11 electrons, with an electron configuration of $ 1s^2 2s^2 2p^6 3s^1 $. When it loses 1 electron (from the 3s orbital), the sodium ion ($ \text{Na}^+ $) has an electron configuration of $ 1s^2 2s^2 2p^6 $. The electron dot diagram (Lewis dot structure) for $ \text{Na}^+ $ would show the symbol $ \text{Na} $ with a superscript $ + $ and no valence electrons (since it lost its 3s electron). For a chloride ion ($ \text{Cl}^- $), a chlorine atom has 7 valence electrons. When it gains 1 electron, it has 8 valence electrons. The electron dot diagram would show $ \text{Cl} $ surrounded by 8 dots (representing the 8 valence electrons) and a superscript $ - $.
# Answer:
For example, if the ion is $ \text{Na}^+ $ (sodium ion): The Lewis dot structure is $ \text{Na}^+ $ (no valence electrons shown as it lost its single valence electron). If the ion is $ \text{Cl}^- $ (chloride ion): The Lewis dot structure is $ [\text{Cl}:]^- $ (with 8 dots around the Cl, representing the 8 valence electrons after gaining 1 electron). (The specific diagram depends on the ion in question. If it's a metal ion like $ \text{Ca}^{2+} $, the dot diagram would be $ \text{Ca}^{2+} $ with no valence electrons shown, as calcium loses its 2 valence electrons.)

### Question 9
# Brief Explanations:
Metals have few valence electrons (usually 1 - 3) and tend to lose these electrons to achieve a stable electron configuration (like a noble gas configuration). Non - metals have more valence electrons (usually 4 - 7) and tend to gain electrons to achieve a stable electron configuration. When a metal loses electrons, it forms a positive ion (cation), and when a non - metal gains electrons, it forms a negative ion (anion). The opposite charges of these ions (positive and negative) attract each other, forming an ionic bond. This bond allows both the metal and non - metal to achieve a stable electron configuration, which is a lower - energy, more stable state. For example, in sodium chloride (NaCl), sodium (a metal) loses 1 electron to become $ \text{Na}^+ $, and chlorine (a non - metal) gains 1 electron to become $ \text{Cl}^- $. The electrostatic attraction between $ \text{Na}^+ $ and $ \text{Cl}^- $ forms the ionic bond in NaCl.
# Answer:
Metals form chemical bonds with nonmetals because metals tend to lose valence electrons (to achieve a stable electron configuration) and nonmetals tend to gain electrons (to achieve a stable electron configuration). The metal becomes a positive ion (cation) and the nonmetal becomes a negative ion (anion), and the opposite charges of these ions attract each other, forming an ionic bond, which stabilizes both atoms.

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