|Ch.1 - Intro to General Chemistry||2hrs & 53mins||0% complete||WorksheetStart|
|Ch.2 - Atoms & Elements||2hrs & 49mins||0% complete||WorksheetStart|
|Ch.3 - Chemical Reactions||3hrs & 25mins||0% complete||WorksheetStart|
|BONUS: Lab Techniques and Procedures||1hr & 38mins||0% complete||WorksheetStart|
|BONUS: Mathematical Operations and Functions||47mins||0% complete||WorksheetStart|
|Ch.4 - Chemical Quantities & Aqueous Reactions||3hrs & 55mins||0% complete||WorksheetStart|
|Ch.5 - Gases||3hrs & 47mins||0% complete||WorksheetStart|
|Ch.6 - Thermochemistry||2hrs & 28mins||0% complete||WorksheetStart|
|Ch.7 - Quantum Mechanics||2hrs & 35mins||0% complete||WorksheetStart|
|Ch.8 - Periodic Properties of the Elements||1hr & 57mins||0% complete||WorksheetStart|
|Ch.9 - Bonding & Molecular Structure||2hrs & 5mins||0% complete||WorksheetStart|
|Ch.10 - Molecular Shapes & Valence Bond Theory||1hr & 31mins||0% complete||WorksheetStart|
|Ch.11 - Liquids, Solids & Intermolecular Forces||3hrs & 40mins||0% complete||WorksheetStart|
|Ch.12 - Solutions||2hrs & 17mins||0% complete||WorksheetStart|
|Ch.13 - Chemical Kinetics||2hrs & 22mins||0% complete||WorksheetStart|
|Ch.14 - Chemical Equilibrium||2hrs & 26mins||0% complete||WorksheetStart|
|Ch.15 - Acid and Base Equilibrium||4hrs & 42mins||0% complete||WorksheetStart|
|Ch.16 - Aqueous Equilibrium||3hrs & 48mins||0% complete||WorksheetStart|
|Ch. 17 - Chemical Thermodynamics||1hr & 44mins||0% complete||WorksheetStart|
|Ch.18 - Electrochemistry||2hrs & 58mins||0% complete||WorksheetStart|
|Ch.19 - Nuclear Chemistry||1hr & 33mins||0% complete||WorksheetStart|
|Ch.20 - Organic Chemistry||3hrs||0% complete||WorksheetStart|
|Ch.22 - Chemistry of the Nonmetals||2hrs & 1min||0% complete||WorksheetStart|
|Ch.23 - Transition Metals and Coordination Compounds||1hr & 54mins||0% complete||WorksheetStart|
|Metal Alloys||7 mins||0 completed|
|Polyatomic Ions||15 mins||0 completed|
|Naming Covalent Compounds||6 mins||0 completed|
|Naming Ionic Compounds||36 mins||0 completed|
|Naming Acids||14 mins||0 completed|
|Empirical Formula||14 mins||0 completed|
|Combustion Analysis||13 mins||0 completed|
|Mass Percent Formula||17 mins||0 completed|
|Balancing Chemical Equations||8 mins||0 completed|
|Functional Groups in Chemistry||13 mins||0 completed|
|Stoichiometry||61 mins||0 completed|
|Ionic and Covalent Bonds|
|Balancing Chemical Equations Worksheet|
The atomic number of sulfur is 16. Sulfur combines with hydrogen by covalent bonding to form a compound, hydrogen sulfide. Based on the number of valence electrons in a sulfur atom, predict the molecular formula of the compound.
We are being asked to determine the molecular formula for hydrogen sulfide based on the valence electrons of sulfur.
Sulfur is in Group 6A and has 6 valence electrons and would only need two electron groups/atoms to satisfy an octet.
Hydrogen on the other hand has 1 valence electron and would need to bond with a single atom to satisfy the octet.
Recall that the octet rule states that an element is surrounded by eight electrons in the Lewis structure.
Exceptions to this rule occur when:
• there is an odd number of electrons, like in radicals
• there are less than 8 electrons or incomplete octet
• there are more than 8 electrons or expanded octet. This occurs to nonmetals from Period 3 to 7.
For this problem, we are dealing with charged species that form ionic compounds.
Elements have common charges based on what group they belong to in the periodic table.
Elements gain and lose electrons so that they have the same number of electrons as the noble gases (Octet Rule).
•Metals → lose electrons and gain positive (+) charge to become more like their closest noble gas
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