Bonding Basics
Reaction Types
Naming Compounds
Lewis Structures
Balancing Equations
Stoichiometry
Percent Yield
100
What type of bond involves the transfer of electrons?
ionic
100
What type of reaction is: A + B → AB?
synthesis
100
Name: CO₂
carbon dioxide
100
What do Lewis dot structures show?
Valence electrons
100
What law requires equations to be balanced?
law of conservation of matter/mass
100
What is the mole used for?
counting extremely large amounts (usually atoms/particles/molecules)
100
What is percent yield?
actual amount of substance produced compared to theoretical amount
200
What type of bond forms between two nonmetals?
covalent
200
What type of reaction is: AB → A + B?
decomposition
200
Name: NaCl
sodium chloride
200
How many valence electrons does oxygen have?
6
200
Balance: H₂ + O₂ → H₂O
2H₂ + O₂ → 2H₂O
200
How many moles are in 18.0 g of H₂O?
1 mol
200
Write the percent yield formula
300
Why do atoms form bonds? (Be specific about energy/stability)
to fill their valence shells/to fulfill the octet rule/to become stable
300
Identify the reaction type:
Zn + CuCl₂ → ZnCl₂ + Cu
single replacement
300
Write the formula: dinitrogen tetroxide
N2O4
300
Draw the Lewis structure for H₂O
300
Balance: Fe + O₂ → Fe₂O₃
4Fe + 3O₂ → 2Fe₂O₃
300
What is the mole ratio in:
2H₂ + O₂ → 2H₂O
2 mol of H2 : 1 mol of O2 : 2 mol of H2O
300
Calculate percent yield: actual = 40g, theoretical =50g
80%
400
Explain the difference between ionic and covalent bonding in terms of electrons/electronegativity
ionic - electrons transferred bc large differences in electronegativity (one atom pulls all valence electrons very close to its nucleus)
Covalent - electrons shared bc smaller differences in electronegativity (one atom may pull all valence electrons closer to its nucleus, or atoms may have same electronegativity and electrons remain at equal distances between nuclei)
400
Explain the difference between single and double replacement reactions.
single: one single element swaps places with an element in a compound
double: two compounds; one element from each compound swaps places to create two new compounds
400
Write the formula: Iron (III) oxide
Fe2O3
400
Explain the octet rule and why it matters
number of electrons required to fill valence shell of all elements (except H and He) and make atoms stable
400
Explain why subscripts cannot be changed when balancing equations
bc that would be creating a new substance out of thin air i.e. creating matter which breaks the law of conservation of matter
400
H2 + O2 --> H2O
What is the limiting reagent/reactant given 2 g of H2 and 3 g of O2?
O2
400
Why is percent yield rarely 100%?
Loss, incomplete reaction
500
Predict the bond type between magnesium and oxygen and justify your answer.
ionic bc metal and nonmetal
500
Write a combustion reaction.
CxHy + O2 --> CO2 + H2O
500
Explain the difference between naming ionic vs covalent compounds (rules + reasoning)
ionic: no greek prefixes; change ending to -ide of second element; include roman numerals for charges of transition metals ONLY
covalent: greek prefixes (except for mono- for first element); change ending to -ide of second element; NO roman numerals
500
Draw and explain the Lewis structure for CO₂ (include bonding explanation)
double bonds in order for carbon to fulfill octet rule
500
Balance: C₃H₈ + O₂ → CO₂ + H₂O
C₃H₈ + 5O₂ → 3CO₂ + 4H₂O
500
H2 + O2 --> H2O
How many grams of H₂O are produced from 10.0 g H₂?
89.1 g H₂O
500
A chemist is synthesizing ammonia (NH3) by reacting nitrogen gas with hydrogen gas. Based on the amount of starting materials used, the theoretical yield of ammonia for this reaction is calculated to be 25.0 grams.
Upon completing the experiment in the lab, the chemist weighs the final product and finds that only 18.2 grams of ammonia were actually produced.
Calculate the percent yield for this reaction.
72.8%