Structure 2.2.1—A covalent bond is formed by the electrostatic attraction between a shared pair of electrons and the positively charged nuclei. The octet rule refers to the tendency of atoms to gain a valence shell with a total of 8 electrons. Deduce the Lewis formula of molecules and ions for up to four electron pairs on each atom.
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[N/A]Directly related questions
- 19M.1A.HL.TZ1.12: Which species has delocalized electrons? A. OH− B. H2CO C. CO2 D. CO32−
- 19M.1A.HL.TZ1.12: Which species has delocalized electrons? A. OH− B. H2CO C. CO2 D. CO32−
- 19M.1A.HL.TZ1.12: Which species has delocalized electrons? A. OH− B. H2CO C. CO2 D. CO32−
- 19M.1A.HL.TZ1.12: Which species has delocalized electrons? A. OH− B. H2CO C. CO2 D. CO32−
- 19M.1A.SL.TZ2.11: Which molecule contains an incomplete octet of electrons? A. NF3 B. BF3 C. BrF D. SF2
- 19M.1A.SL.TZ2.11: Which molecule contains an incomplete octet of electrons? A. NF3 B. BF3 C. BrF D. SF2
- 19M.1A.SL.TZ2.11: Which molecule contains an incomplete octet of electrons? A. NF3 B. BF3 C. BrF D. SF2
- 19M.1A.SL.TZ2.11: Which molecule contains an incomplete octet of electrons? A. NF3 B. BF3 C. BrF D. SF2
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19M.2.SL.TZ2.5d(i):
Identify the type of bonding in sodium hydrogencarbonate.
Between sodium and hydrogencarbonate:
Between hydrogen and oxygen in hydrogencarbonate:
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19M.2.SL.TZ2.5d(i):
Identify the type of bonding in sodium hydrogencarbonate.
Between sodium and hydrogencarbonate:
Between hydrogen and oxygen in hydrogencarbonate:
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19M.2.SL.TZ2.d(i):
Identify the type of bonding in sodium hydrogencarbonate.
Between sodium and hydrogencarbonate:
Between hydrogen and oxygen in hydrogencarbonate:
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19M.2.SL.TZ1.5c(i):
Draw a Lewis (electron dot) structure of chloramine.
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19M.2.SL.TZ1.5c(i):
Draw a Lewis (electron dot) structure of chloramine.
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19M.2.SL.TZ1.c(i):
Draw a Lewis (electron dot) structure of chloramine.
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19M.2.SL.TZ1.5c(i):
Draw a Lewis (electron dot) structure of chloramine.
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19M.2.SL.TZ1.5c(i):
Draw a Lewis (electron dot) structure of chloramine.
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19M.2.SL.TZ1.c(i):
Draw a Lewis (electron dot) structure of chloramine.
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19M.2.SL.TZ2.5b(iii):
Identify the type of bonding in sodium hydrogencarbonate.
Between sodium and hydrogencarbonate:
Between hydrogen and oxygen in hydrogencarbonate:
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19M.2.SL.TZ2.5b(iii):
Identify the type of bonding in sodium hydrogencarbonate.
Between sodium and hydrogencarbonate:
Between hydrogen and oxygen in hydrogencarbonate:
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19M.2.SL.TZ2.b(iii):
Identify the type of bonding in sodium hydrogencarbonate.
Between sodium and hydrogencarbonate:
Between hydrogen and oxygen in hydrogencarbonate:
- 19N.1A.SL.TZ0.13: Which atom does not obey the octet rule? A. C in CO2 B. F in BF3 C. O in H2O D. S in SF6
- 19N.1A.SL.TZ0.13: Which atom does not obey the octet rule? A. C in CO2 B. F in BF3 C. O in H2O D. S in SF6
- 19N.1A.SL.TZ0.13: Which atom does not obey the octet rule? A. C in CO2 B. F in BF3 C. O in H2O D. S in SF6
- 19N.1A.SL.TZ0.13: Which atom does not obey the octet rule? A. C in CO2 B. F in BF3 C. O in H2O D. S in SF6
- 21M.2.SL.TZ1.1d(v): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
- 21M.2.SL.TZ1.1d(v): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
- 21M.2.SL.TZ1.d(v): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
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21M.2.HL.TZ1.7a(i):
Draw a Lewis (electron dot) structure for ozone.
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21M.2.HL.TZ1.7a(i):
Draw a Lewis (electron dot) structure for ozone.
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21M.2.HL.TZ1.a(i):
Draw a Lewis (electron dot) structure for ozone.
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21M.2.HL.TZ1.7a(i):
Draw a Lewis (electron dot) structure for ozone.
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21M.2.HL.TZ1.7a(i):
Draw a Lewis (electron dot) structure for ozone.
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21M.2.HL.TZ1.a(i):
Draw a Lewis (electron dot) structure for ozone.
- 21M.2.SL.TZ1.1c(iv): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
- 21M.2.SL.TZ1.1c(iv): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
- 21M.2.SL.TZ1.c(iv): Suggest why chemists find it convenient to classify bonding into ionic, covalent and metallic.
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21M.2.SL.TZ1.2a(i):
Draw the Lewis (electron dot) structure of hydrogen sulfide.
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21M.2.SL.TZ1.2a(i):
Draw the Lewis (electron dot) structure of hydrogen sulfide.
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21M.2.SL.TZ1.a(i):
Draw the Lewis (electron dot) structure of hydrogen sulfide.
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21M.2.SL.TZ1.2a(i):
Draw the Lewis (electron dot) structure of hydrogen sulfide.
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21M.2.SL.TZ1.2a(i):
Draw the Lewis (electron dot) structure of hydrogen sulfide.
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21M.2.SL.TZ1.a(i):
Draw the Lewis (electron dot) structure of hydrogen sulfide.
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21M.2.SL.TZ2.2c:
Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl2.
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21M.2.SL.TZ2.2c:
Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl2.
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21M.2.SL.TZ2.c:
Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl2.
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21M.2.SL.TZ2.2c:
Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl2.
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21M.2.SL.TZ2.2c:
Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl2.
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21M.2.SL.TZ2.c:
Deduce the Lewis (electron dot) structure and molecular geometry of sulfur dichloride, SCl2.
- 21N.1A.SL.TZ0.11: Which compound contains both ionic and covalent bonds? A. CH3COONa B. CH3COOH C. K2O D. ...
- 21N.1A.SL.TZ0.11: Which compound contains both ionic and covalent bonds? A. CH3COONa B. CH3COOH C. K2O D. ...
- 22M.1A.SL.TZ1.10: What is the explanation for the high melting point of sodium chloride? A. The covalent bond...
- 22M.1A.SL.TZ1.10: What is the explanation for the high melting point of sodium chloride? A. The covalent bond...
- 22M.1A.SL.TZ2.10: What is the type of bonding in a compound that has high boiling and melting points, poor...
- 22M.1A.SL.TZ2.10: What is the type of bonding in a compound that has high boiling and melting points, poor...
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22M.1A.SL.TZ2.9:
Which statement best describes the intramolecular bonding in HCN (l)?
A. Electrostatic attractions between H+ and CN− ions
B. Hydrogen bonding
C. Van der Waals forces and hydrogen bonding
D. Electrostatic attractions between pairs of electrons and positively charged nuclei
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22M.1A.SL.TZ2.9:
Which statement best describes the intramolecular bonding in HCN (l)?
A. Electrostatic attractions between H+ and CN− ions
B. Hydrogen bonding
C. Van der Waals forces and hydrogen bonding
D. Electrostatic attractions between pairs of electrons and positively charged nuclei
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22M.1A.SL.TZ2.9:
Which statement best describes the intramolecular bonding in HCN (l)?
A. Electrostatic attractions between H+ and CN− ions
B. Hydrogen bonding
C. Van der Waals forces and hydrogen bonding
D. Electrostatic attractions between pairs of electrons and positively charged nuclei
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22M.1A.SL.TZ2.9:
Which statement best describes the intramolecular bonding in HCN (l)?
A. Electrostatic attractions between H+ and CN− ions
B. Hydrogen bonding
C. Van der Waals forces and hydrogen bonding
D. Electrostatic attractions between pairs of electrons and positively charged nuclei
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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.HL.TZ2.3d(i): Draw the Lewis structure of NO3−.
- 22M.2.HL.TZ2.3d(i): Draw the Lewis structure of NO3−.
- 22M.2.HL.TZ2.d(i): Draw the Lewis structure of NO3−.
- 22M.2.HL.TZ2.3d(i): Draw the Lewis structure of NO3−.
- 22M.2.HL.TZ2.3d(i): Draw the Lewis structure of NO3−.
- 22M.2.HL.TZ2.d(i): Draw the Lewis structure of NO3−.