Structure 2.1.1—When metal atoms lose electrons, they form positive ions called cations. When non-metal atoms gain electrons, they form negative ions called anions. Predict the charge of an ion from the electron configuration of the atom.
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[N/A]Directly related questions
- 19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
- 19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
- 19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
- 19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
- 19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
- 19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
- 19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
- 19M.1A.SL.TZ2.9: How does a lithium atom form the most stable ion? A. The atom gains a proton to form a positive...
- 21M.2.SL.TZ1.1d(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.1d(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.d(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.1d(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.1d(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.d(i): Describe the bonding in this type of solid.
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21M.2.SL.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.1d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.d(iv):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
- 21M.2.SL.TZ1.1c(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.1c(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.c(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.1c(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.1c(i): Describe the bonding in this type of solid.
- 21M.2.SL.TZ1.c(i): Describe the bonding in this type of solid.
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21M.2.SL.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.1c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
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21M.2.SL.TZ1.c(iii):
Outline, in terms of their electronic structures, why the ionic radius of the sulfide ion is greater than that of the oxide ion.
- 21M.2.SL.TZ2.2a(ii): Explain the decrease in radius from Na to Na+.
- 21M.2.SL.TZ2.2a(ii): Explain the decrease in radius from Na to Na+.
- 21M.2.SL.TZ2.a(ii): Explain the decrease in radius from Na to Na+.
- 21M.2.SL.TZ2.2a(ii): Explain the decrease in radius from Na to Na+.
- 21M.2.SL.TZ2.2a(ii): Explain the decrease in radius from Na to Na+.
- 21M.2.SL.TZ2.a(ii): Explain the decrease in radius from Na to Na+.
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22M.2.SL.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
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22M.2.SL.TZ1.1e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
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22M.2.SL.TZ1.e(iii):
The nitride ion and the magnesium ion are isoelectronic (they have the same electron configuration). Determine, giving a reason, which has the greater ionic radius.
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22M.2.SL.TZ1.1g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.
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22M.2.SL.TZ1.1g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.
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22M.2.SL.TZ1.g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.
-
22M.2.SL.TZ1.1g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.
-
22M.2.SL.TZ1.1g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.
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22M.2.SL.TZ1.g:
State the types of bonding in magnesium, oxygen and magnesium oxide, and how the valence electrons produce these types of bonding.